First, lets start with naming ionic compounds. .pdf
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First, let\'s start with naming ionic compounds. A binary ionic compound has one metal and one nonmetal present in the compound. Rubidium chloride, or RbCl, is a binary ionic compound. The metal here is Rb (rubidium, group 1A) and the nonmetal is Cl (chlorine, group 7A). When you name binary ionic compounds, you mention the cation (positively charged ion) first (usually metals, those elements that appear on the left side of the periodic table have the tendency to form positively-charged ions). Then mention the anion (negatively charged ion). The cation is rubidium (Rb). We mention it thus: Rubidium The anion is chlorine. When we write the name of the anion [alongside with the cation], we drop the ending -ine (or whatever ending it may have) and replace it with -ide. So chlorine now becomes chlor + ide = chloride. Therefore, the name of the compound is Rubidium Chloride. When you write the formulas of binary ionic compounds, you use the criss-cross method. Here\'s how it works: Rubidium has a charge of +1. Chlorine has a charge of -1. You interchange the charges of both ions. These charges, when interchanged, become the subscripts of the elements in the compound. Hence, the compound now looks Rb1Cl1. Since the subscripts are all 1, we can remove them and write the formula as RbCl. Here\'s another example: Give the formula of the compound magnesium chloride. Mg has a charge of +2. Chlorine has a charge of -1. When you interchange the respective charges of magnesium and chlorine, we get the following formula: Mg1Cl2 We simplify this as MgCl2. A list of the common cations and ions is found at the back page or on the chapter of naming chemical compounds of your chemistry book. Take time to know them by heart. But what if... you\'ve got a compound named sodium nitrate. Ok. The formula is NaNO3. How did I know? Sodium nitrate is an example of a ternary ionic compound. A ternary ionic compound has two or more elements present in it. In this case, there are 3 (Na, N and O). The naming system of ternary ionic compounds is the same as that of binary ionic compounds. Let\'s name the participating ions: Na+ NO3- NO3- is the formula for the polyatomic ion (two or more elements joined together sharing a common charge; they act as one unit when they combine with other elements) nitrate. We interchange the charges of sodium and nitrate. Interchanging them gives us the formula NaNO3 To name this formula, just combine the name of the cation and anion together. In this case, it is sodium nitrate. What if we have a formula like this? Ba(OH)2 Don\'t worry. This is just barium hydroxide. Let\'s analyze why this came about. The charge of Ba is +2 and hydroxide (OH-) is -1. When you combine them together by interchanging subscripts, we get the following: BaOH2 Wait. The formula doesn\'t make sense. H is not the only atom having two of its kind, but O too. So we put parentheses around hydroxide to indicate that there are two units of the hydroxide ion, each of which h.
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![First, let's start with naming ionic compounds. A binary ionic compound has one
metal and one nonmetal present in the compound. Rubidium chloride, or RbCl, is a binary ionic
compound. The metal here is Rb (rubidium, group 1A) and the nonmetal is Cl (chlorine, group
7A). When you name binary ionic compounds, you mention the cation (positively charged ion)
first (usually metals, those elements that appear on the left side of the periodic table have the
tendency to form positively-charged ions). Then mention the anion (negatively charged ion).
The cation is rubidium (Rb). We mention it thus: Rubidium The anion is chlorine. When we
write the name of the anion [alongside with the cation], we drop the ending -ine (or whatever
ending it may have) and replace it with -ide. So chlorine now becomes chlor + ide = chloride.
Therefore, the name of the compound is Rubidium Chloride. When you write the formulas of
binary ionic compounds, you use the criss-cross method. Here's how it works: Rubidium has a
charge of +1. Chlorine has a charge of -1. You interchange the charges of both ions. These
charges, when interchanged, become the subscripts of the elements in the compound. Hence, the
compound now looks Rb1Cl1. Since the subscripts are all 1, we can remove them and write the
formula as RbCl. Here's another example: Give the formula of the compound magnesium
chloride. Mg has a charge of +2. Chlorine has a charge of -1. When you interchange the
respective charges of magnesium and chlorine, we get the following formula: Mg1Cl2 We
simplify this as MgCl2. A list of the common cations and ions is found at the back page or on
the chapter of naming chemical compounds of your chemistry book. Take time to know them by
heart. But what if... you've got a compound named sodium nitrate. Ok. The formula is NaNO3.
How did I know? Sodium nitrate is an example of a ternary ionic compound. A ternary ionic
compound has two or more elements present in it. In this case, there are 3 (Na, N and O). The
naming system of ternary ionic compounds is the same as that of binary ionic compounds. Let's
name the participating ions: Na+ NO3- NO3- is the formula for the polyatomic ion (two or
more elements joined together sharing a common charge; they act as one unit when they
combine with other elements) nitrate. We interchange the charges of sodium and nitrate.
Interchanging them gives us the formula NaNO3 To name this formula, just combine the name
of the cation and anion together. In this case, it is sodium nitrate. What if we have a formula like
this? Ba(OH)2 Don't worry. This is just barium hydroxide. Let's analyze why this came about.
The charge of Ba is +2 and hydroxide (OH-) is -1. When you combine them together by
interchanging subscripts, we get the following: BaOH2 Wait. The formula doesn't make sense.
H is not the only atom having two of its kind, but O too. So we put parentheses around
hydroxide to indicate that there are two units of the hydroxide ion, each of which has two O and
H atoms respectively. We now have the formula Ba(OH)2. Again, review the list of common
polyatomic cations and anions. So far there are two polyatomic cations: hydronium (H3O+) and
ammonium (NH4+). This can be found in your chem book and in the net. There are still lots of](https://image.slidesharecdn.com/firstletsstartwithnamingioniccompounds-230412162037-a6ee8708/85/First-lets-start-with-naming-ionic-compounds-pdf-1-320.jpg)
![stuff related to this, most of which are very basic, and I don't have the space to tackle all of them
here. Read your chem book or surf the net for more info. You can ask your chem teacher and
friends for help, too.
Solution
First, let's start with naming ionic compounds. A binary ionic compound has one
metal and one nonmetal present in the compound. Rubidium chloride, or RbCl, is a binary ionic
compound. The metal here is Rb (rubidium, group 1A) and the nonmetal is Cl (chlorine, group
7A). When you name binary ionic compounds, you mention the cation (positively charged ion)
first (usually metals, those elements that appear on the left side of the periodic table have the
tendency to form positively-charged ions). Then mention the anion (negatively charged ion).
The cation is rubidium (Rb). We mention it thus: Rubidium The anion is chlorine. When we
write the name of the anion [alongside with the cation], we drop the ending -ine (or whatever
ending it may have) and replace it with -ide. So chlorine now becomes chlor + ide = chloride.
Therefore, the name of the compound is Rubidium Chloride. When you write the formulas of
binary ionic compounds, you use the criss-cross method. Here's how it works: Rubidium has a
charge of +1. Chlorine has a charge of -1. You interchange the charges of both ions. These
charges, when interchanged, become the subscripts of the elements in the compound. Hence, the
compound now looks Rb1Cl1. Since the subscripts are all 1, we can remove them and write the
formula as RbCl. Here's another example: Give the formula of the compound magnesium
chloride. Mg has a charge of +2. Chlorine has a charge of -1. When you interchange the
respective charges of magnesium and chlorine, we get the following formula: Mg1Cl2 We
simplify this as MgCl2. A list of the common cations and ions is found at the back page or on
the chapter of naming chemical compounds of your chemistry book. Take time to know them by
heart. But what if... you've got a compound named sodium nitrate. Ok. The formula is NaNO3.
How did I know? Sodium nitrate is an example of a ternary ionic compound. A ternary ionic
compound has two or more elements present in it. In this case, there are 3 (Na, N and O). The
naming system of ternary ionic compounds is the same as that of binary ionic compounds. Let's
name the participating ions: Na+ NO3- NO3- is the formula for the polyatomic ion (two or
more elements joined together sharing a common charge; they act as one unit when they
combine with other elements) nitrate. We interchange the charges of sodium and nitrate.
Interchanging them gives us the formula NaNO3 To name this formula, just combine the name
of the cation and anion together. In this case, it is sodium nitrate. What if we have a formula like
this? Ba(OH)2 Don't worry. This is just barium hydroxide. Let's analyze why this came about.
The charge of Ba is +2 and hydroxide (OH-) is -1. When you combine them together by
interchanging subscripts, we get the following: BaOH2 Wait. The formula doesn't make sense.](data:image/gif;base64,R0lGODlhAQABAIAAAAAAAP///yH5BAEAAAAALAAAAAABAAEAAAIBRAA7)
Recommended
First, lets start with naming binary ionic comp.pdf
First, let\'s start with naming binary ionic compounds. A binary ionic compound
has one metal and one nonmetal present in the compound. Let\'s consider my username
(rubidium.chloride) as an example. Rubidium chloride, or RbCl, is a binary ionic compound.
The metal here is Rb (rubidium, group 1A) and the nonmetal is Cl (chlorine, group 7A). When
you name binary ionic compounds, you mention the cation (positively charged ion) first (usually
metals, those elements that appear on the left side of the periodic table have the tendency to form
positively-charged ions). Then mention the anion (negatively charged ion). The cation is
rubidium (Rb). We mention it thus: Rubidium The anion is chlorine. When we write the name
of the anion [alongside with the cation], we drop the ending -ine (or whatever ending it may
have) and replace it with -ide. So chlorine now becomes chlor + ide = chloride. Therefore, the
name of the compound is Rubidium Chloride. When you write the formulas of binary ionic
compounds, you use the criss-cross method. Here\'s how it works: Rubidium has a charge of +1.
Chlorine has a charge of -1. You interchange the charges of both ions. These charges, when
interchanged, become the subscripts of the elements in the compound. Hence, the compound
now looks Rb1Cl1. Since the subscripts are all 1, we can remove them and write the formula as
RbCl. Here\'s another example: Give the formula of the compound magnesium chloride. Mg
has a charge of +2. Chlorine has a charge of -1. When you interchange the respective charges of
magnesium and chlorine, we get the following formula: Mg1Cl2 We simplify this as MgCl2. A
list of the common cations and ions is found at the back page or on the chapter of naming
chemical compounds of your chemistry book. Take time to know them by heart. But what if...
you\'ve got a compound named sodium nitrate. Ok. The formula is NaNO3. How did I know?
Sodium nitrate is an example of a ternary ionic compound. A ternary ionic compound has two or
more elements present in it. In this case, there are 3 (Na, N and O). The naming system of
ternary ionic compounds is the same as that of binary ionic compounds. Let\'s name the
participating ions: Na+ NO3- NO3- is the formula for the polyatomic ion (two or more
elements joined together sharing a common charge; they act as one unit when they combine with
other elements) nitrate. We interchange the charges of sodium and nitrate. Interchanging them
gives us the formula NaNO3 To name this formula, just combine the name of the cation and
anion together. In this case, it is sodium nitrate. What if we have a formula like this? Ba(OH)2
Don\'t worry. This is just barium hydroxide. Let\'s analyze why this came about. The charge of
Ba is +2 and hydroxide (OH-) is -1. When you combine them together by interchanging
subscripts, we get the following: BaOH2 Wait. The formula doesn\'t make sense. H is not the
only atom having two of its kind, but O too. So we put parentheses around hydroxide to i.
Nomenclature handout
This document discusses the nomenclature (naming systems) for inorganic compounds, which differ depending on whether the compound is ionic or molecular. For ionic compounds, the cation is named first followed by the anion. Binary ionic compounds consisting of a metal and nonmetal are generally named by removing the ending from the nonmetal and adding -ide. For transition metals that form multiple ions, the modern system uses Roman numerals in parentheses after the metal to indicate charge. Molecular compounds are named by identifying the number of atoms of each element present using prefixes, and adding -ide to the second element. Several elements exist as diatomic molecules like H2, N2, O2, F2, Cl2, Br
Chemical nomenclature and formulas
Chemistry is involved with various and diverse interactions of matter either around us or simply inside the laboratory. These are described using the language of chemistry which consists of symbols, formulas and equations.
Ch2 z53 particles
This document provides an overview of key concepts in atomic structure and chemical bonding:
- It describes early theories of atoms proposed by thinkers like Democritus, Dalton, and Thomson. Experiments by Thomson, Millikan, and Rutherford provided evidence for the atom's internal structure.
- The document defines subatomic particles like protons, neutrons, and electrons. It introduces concepts like isotopes, ions, ionic and covalent bonding.
- Naming conventions for ions, ionic compounds, acids, and hydrates are outlined. Rules for writing chemical formulas are also summarized.
- Key models and experiments that advanced understanding of atomic structure are highlighted, including Dalton's atomic theory and the discoveries of the
Names and formulas of ionic compounds
This document discusses writing formulas for ionic compounds and naming ionic compounds and oxyanions. It provides rules for determining the formula unit of ionic compounds based on the ratio of ions present. Cation symbols are always written first, followed by anion symbols. Subscripts indicate the number of each ion. Polyatomic ions act as individual units in formulas. Oxyanions contain nonmetals bonded to oxygen. Five rules are provided for naming ionic compounds based on cation and anion names and oxidation states.
Atoms and molecules
The convention of using 1/12 the mass of a carbon-12 atom as the atomic mass unit was adopted because:
1) Carbon-12 has 6 protons and 6 neutrons which have nearly equal mass and the mass of electrons is negligible.
2) Dividing the total mass of protons and neutrons in carbon-12 by 12 provides a whole number for atomic masses rather than fractions.
3) Carbon-12 is the most common isotope with an equal number of protons and neutrons, making it readily available as a standard.
You must be familiar with the fact that melting p.pdf
You must be familiar with the fact that melting point is essentially the same thing as
freezing point. What is meant by this is that the same temperature will melt something (if we\'re
considering an endothermic reaction) as it will freeze something (exothermic reaction). After
you\'ve reached this clarity, simply observe all of the compounds and check for which ones have
low melting points and then work your way up. Now the question is, how can we identify
compounds with low melting points? Remember, if a compound is polar (charged, or is a dipole,
like water), it will have a high boiling point (it will be very tough to boil). So compounds that
have a high boiling point will most likely have high melting points as well (generally, not
universally). For NaBr, Na+ and Br- and the constituents and they certainly have an
electronegativity difference (uneven charge distribution in the electron density implies a dipole).
We have to look at calcium nitrate next before determining the priority of NaBr. Ca(NO3)2 is
obviously going to have charged constituents. The Ca will be positively charged and the nitrate
groups which are oxyANIONs will be negatively charged. Since there are MORE oxygens in
calcium nitrate, this compound will be more electronegative and will form a stronger dipole
compared to NaBr (Br is NOT as electronegative as oxygen). Greater electronegativity implies
stronger dipole in a compound and this means higher boiling point, which means higher melting
point, which means higher freezing point compared to NaBr. HCl is an acid and although there
are H atoms, HCl CANNOT form Hydrogen bonds (h-bonding occurs only for N-H, O-H, and F-
H. Cl is obviously NOT one of the constituents that can form hydrogen bonding and therefore
will have a LOW boiling point, meaning low freezing point as well. HCl falls at the very bottom
of our list. Ethanol is polar (because of the free electrons from O--H from the sp3 orbital).
Hydrogen bonding IMMEDIATELY implies high boiling point, so EtOH will have a relatively
large melting point, and thus freezing point. Now that I\'ve laid out the information as
thoroughly as possible. Simply arrange them to form your freezing point trend list given the four
compounds. Should be rather straightforward.
Solution
You must be familiar with the fact that melting point is essentially the same thing as
freezing point. What is meant by this is that the same temperature will melt something (if we\'re
considering an endothermic reaction) as it will freeze something (exothermic reaction). After
you\'ve reached this clarity, simply observe all of the compounds and check for which ones have
low melting points and then work your way up. Now the question is, how can we identify
compounds with low melting points? Remember, if a compound is polar (charged, or is a dipole,
like water), it will have a high boiling point (it will be very tough to boil). So compounds that
have a high boiling point will most likely have high melting poin.
10) Ionic compounds are a combination of metals a.pdf
10) Ionic compounds are a combination of metals and non-metals. A covalent
compound is a combination of a non-metal and another non-metal An example of an ionic
compound would be Na2SO4. An example of a covalent compound would be CO2. 10b.) a.
Hydrochloric acid Anytime you have H-nameofanyhalogen and its aqueous (aq), you know it\'s
an acid. To name acids (of this type) you just say \"Hydro\" then the prefix name of halogen (ie.
chlor) and add \"ic\" to the end So HCL = Hydro chlor ic acid. If you had for instance HBr, it
would be Hydro brom ic acid... Hydrobromic Acid b. Hydrogen Chloride This is the same letters
as Hydrochloric acid but it\'s NOT (aq). It\'s a gas (g). That\'s how you know it\'s a regular
covalent compound and not an acid. And it\'s covalent because it\'s a mix of two non-metals. So
therefore it would just be the names Hydrogen, and then chloride. When you have a covalent
compound you always say the first element name, just spelled out normally, and then the prefix
of the next element with the suffix \"ide.\" So HCl would be Hydrogen Chlor ide. Hydrogen
Chloride. c. Methane Many compounds have everyday names that have been given to them.
This is an example of that. You just have to memorize them there is no easy way of determining
an everyday name for these compounds. d. Methanol Yet another example, you just have to
memorize what these formulas are according to their name. 10c.) a. 2H2 + O2 ===> 2H2O b.
CH4 + 2O2 ===> CO2 + 2H2O As you can see, for both of these reactions they have the same
number of elements on both sides of the equation. Now, remember, you NEVER add subscripts
to any of the elements on either side of the equation when you\'re balancing. The subscripts stay
the same. What you DO add are coefficients in front of a compound. For instance the
unbalanced equation in your question (question a.) \"Hydrogen gas and oxygen gas react to form
liquid water.\" would be: H2 + O2 ===> H2O As you can see, it\'s not balanced..... the
hydrogens are balanced on both sides (2 on each side) but the oxygens are not. There are 2
oxygens on the left and only 1 on the right. So add a coefficion of 2 to the \"H2O\" so that you
can have 2 oxygens. Now our new reaction is: H2 + 02 ===> 2H2O However this is still not
balanced. As you can see we have 2 hydrogens on the left, but now we have 4 hydrogens on the
right. So, in order to fix this, add 2 in front of H2 on the left, so now we have: 2H2 + O2 ===>
2H2O Now we have a balanced equation with 4 hydrogens on the right, and 4 hydrogens on the
left. As well as 2 oxygens on the right and 2 oxygens on the left. This same type of procedure is
how you balance any reaction. 10d.) Al2(SO4)3 = Aluminum Sulfate To calculate percent
aluminum by mass you first find the mass of the compound. Molar Mass Al2(SO4)3: Al =
27.0(2) = 54g/mol S = 32.1(3) = 96.3g/mol O = 16.0(12) = 192g/mol Add them all together to
get the molar mass of Al2(SO4)3 = 342.3g/mol Now, to get the % by mass of Al in Al2(SO4).
Recommended
First, lets start with naming binary ionic comp.pdf
First, let\'s start with naming binary ionic compounds. A binary ionic compound
has one metal and one nonmetal present in the compound. Let\'s consider my username
(rubidium.chloride) as an example. Rubidium chloride, or RbCl, is a binary ionic compound.
The metal here is Rb (rubidium, group 1A) and the nonmetal is Cl (chlorine, group 7A). When
you name binary ionic compounds, you mention the cation (positively charged ion) first (usually
metals, those elements that appear on the left side of the periodic table have the tendency to form
positively-charged ions). Then mention the anion (negatively charged ion). The cation is
rubidium (Rb). We mention it thus: Rubidium The anion is chlorine. When we write the name
of the anion [alongside with the cation], we drop the ending -ine (or whatever ending it may
have) and replace it with -ide. So chlorine now becomes chlor + ide = chloride. Therefore, the
name of the compound is Rubidium Chloride. When you write the formulas of binary ionic
compounds, you use the criss-cross method. Here\'s how it works: Rubidium has a charge of +1.
Chlorine has a charge of -1. You interchange the charges of both ions. These charges, when
interchanged, become the subscripts of the elements in the compound. Hence, the compound
now looks Rb1Cl1. Since the subscripts are all 1, we can remove them and write the formula as
RbCl. Here\'s another example: Give the formula of the compound magnesium chloride. Mg
has a charge of +2. Chlorine has a charge of -1. When you interchange the respective charges of
magnesium and chlorine, we get the following formula: Mg1Cl2 We simplify this as MgCl2. A
list of the common cations and ions is found at the back page or on the chapter of naming
chemical compounds of your chemistry book. Take time to know them by heart. But what if...
you\'ve got a compound named sodium nitrate. Ok. The formula is NaNO3. How did I know?
Sodium nitrate is an example of a ternary ionic compound. A ternary ionic compound has two or
more elements present in it. In this case, there are 3 (Na, N and O). The naming system of
ternary ionic compounds is the same as that of binary ionic compounds. Let\'s name the
participating ions: Na+ NO3- NO3- is the formula for the polyatomic ion (two or more
elements joined together sharing a common charge; they act as one unit when they combine with
other elements) nitrate. We interchange the charges of sodium and nitrate. Interchanging them
gives us the formula NaNO3 To name this formula, just combine the name of the cation and
anion together. In this case, it is sodium nitrate. What if we have a formula like this? Ba(OH)2
Don\'t worry. This is just barium hydroxide. Let\'s analyze why this came about. The charge of
Ba is +2 and hydroxide (OH-) is -1. When you combine them together by interchanging
subscripts, we get the following: BaOH2 Wait. The formula doesn\'t make sense. H is not the
only atom having two of its kind, but O too. So we put parentheses around hydroxide to i.
Nomenclature handout
This document discusses the nomenclature (naming systems) for inorganic compounds, which differ depending on whether the compound is ionic or molecular. For ionic compounds, the cation is named first followed by the anion. Binary ionic compounds consisting of a metal and nonmetal are generally named by removing the ending from the nonmetal and adding -ide. For transition metals that form multiple ions, the modern system uses Roman numerals in parentheses after the metal to indicate charge. Molecular compounds are named by identifying the number of atoms of each element present using prefixes, and adding -ide to the second element. Several elements exist as diatomic molecules like H2, N2, O2, F2, Cl2, Br
Chemical nomenclature and formulas
Chemistry is involved with various and diverse interactions of matter either around us or simply inside the laboratory. These are described using the language of chemistry which consists of symbols, formulas and equations.
Ch2 z53 particles
This document provides an overview of key concepts in atomic structure and chemical bonding:
- It describes early theories of atoms proposed by thinkers like Democritus, Dalton, and Thomson. Experiments by Thomson, Millikan, and Rutherford provided evidence for the atom's internal structure.
- The document defines subatomic particles like protons, neutrons, and electrons. It introduces concepts like isotopes, ions, ionic and covalent bonding.
- Naming conventions for ions, ionic compounds, acids, and hydrates are outlined. Rules for writing chemical formulas are also summarized.
- Key models and experiments that advanced understanding of atomic structure are highlighted, including Dalton's atomic theory and the discoveries of the
Names and formulas of ionic compounds
This document discusses writing formulas for ionic compounds and naming ionic compounds and oxyanions. It provides rules for determining the formula unit of ionic compounds based on the ratio of ions present. Cation symbols are always written first, followed by anion symbols. Subscripts indicate the number of each ion. Polyatomic ions act as individual units in formulas. Oxyanions contain nonmetals bonded to oxygen. Five rules are provided for naming ionic compounds based on cation and anion names and oxidation states.
Atoms and molecules
The convention of using 1/12 the mass of a carbon-12 atom as the atomic mass unit was adopted because:
1) Carbon-12 has 6 protons and 6 neutrons which have nearly equal mass and the mass of electrons is negligible.
2) Dividing the total mass of protons and neutrons in carbon-12 by 12 provides a whole number for atomic masses rather than fractions.
3) Carbon-12 is the most common isotope with an equal number of protons and neutrons, making it readily available as a standard.
You must be familiar with the fact that melting p.pdf
You must be familiar with the fact that melting point is essentially the same thing as
freezing point. What is meant by this is that the same temperature will melt something (if we\'re
considering an endothermic reaction) as it will freeze something (exothermic reaction). After
you\'ve reached this clarity, simply observe all of the compounds and check for which ones have
low melting points and then work your way up. Now the question is, how can we identify
compounds with low melting points? Remember, if a compound is polar (charged, or is a dipole,
like water), it will have a high boiling point (it will be very tough to boil). So compounds that
have a high boiling point will most likely have high melting points as well (generally, not
universally). For NaBr, Na+ and Br- and the constituents and they certainly have an
electronegativity difference (uneven charge distribution in the electron density implies a dipole).
We have to look at calcium nitrate next before determining the priority of NaBr. Ca(NO3)2 is
obviously going to have charged constituents. The Ca will be positively charged and the nitrate
groups which are oxyANIONs will be negatively charged. Since there are MORE oxygens in
calcium nitrate, this compound will be more electronegative and will form a stronger dipole
compared to NaBr (Br is NOT as electronegative as oxygen). Greater electronegativity implies
stronger dipole in a compound and this means higher boiling point, which means higher melting
point, which means higher freezing point compared to NaBr. HCl is an acid and although there
are H atoms, HCl CANNOT form Hydrogen bonds (h-bonding occurs only for N-H, O-H, and F-
H. Cl is obviously NOT one of the constituents that can form hydrogen bonding and therefore
will have a LOW boiling point, meaning low freezing point as well. HCl falls at the very bottom
of our list. Ethanol is polar (because of the free electrons from O--H from the sp3 orbital).
Hydrogen bonding IMMEDIATELY implies high boiling point, so EtOH will have a relatively
large melting point, and thus freezing point. Now that I\'ve laid out the information as
thoroughly as possible. Simply arrange them to form your freezing point trend list given the four
compounds. Should be rather straightforward.
Solution
You must be familiar with the fact that melting point is essentially the same thing as
freezing point. What is meant by this is that the same temperature will melt something (if we\'re
considering an endothermic reaction) as it will freeze something (exothermic reaction). After
you\'ve reached this clarity, simply observe all of the compounds and check for which ones have
low melting points and then work your way up. Now the question is, how can we identify
compounds with low melting points? Remember, if a compound is polar (charged, or is a dipole,
like water), it will have a high boiling point (it will be very tough to boil). So compounds that
have a high boiling point will most likely have high melting poin.
10) Ionic compounds are a combination of metals a.pdf
10) Ionic compounds are a combination of metals and non-metals. A covalent
compound is a combination of a non-metal and another non-metal An example of an ionic
compound would be Na2SO4. An example of a covalent compound would be CO2. 10b.) a.
Hydrochloric acid Anytime you have H-nameofanyhalogen and its aqueous (aq), you know it\'s
an acid. To name acids (of this type) you just say \"Hydro\" then the prefix name of halogen (ie.
chlor) and add \"ic\" to the end So HCL = Hydro chlor ic acid. If you had for instance HBr, it
would be Hydro brom ic acid... Hydrobromic Acid b. Hydrogen Chloride This is the same letters
as Hydrochloric acid but it\'s NOT (aq). It\'s a gas (g). That\'s how you know it\'s a regular
covalent compound and not an acid. And it\'s covalent because it\'s a mix of two non-metals. So
therefore it would just be the names Hydrogen, and then chloride. When you have a covalent
compound you always say the first element name, just spelled out normally, and then the prefix
of the next element with the suffix \"ide.\" So HCl would be Hydrogen Chlor ide. Hydrogen
Chloride. c. Methane Many compounds have everyday names that have been given to them.
This is an example of that. You just have to memorize them there is no easy way of determining
an everyday name for these compounds. d. Methanol Yet another example, you just have to
memorize what these formulas are according to their name. 10c.) a. 2H2 + O2 ===> 2H2O b.
CH4 + 2O2 ===> CO2 + 2H2O As you can see, for both of these reactions they have the same
number of elements on both sides of the equation. Now, remember, you NEVER add subscripts
to any of the elements on either side of the equation when you\'re balancing. The subscripts stay
the same. What you DO add are coefficients in front of a compound. For instance the
unbalanced equation in your question (question a.) \"Hydrogen gas and oxygen gas react to form
liquid water.\" would be: H2 + O2 ===> H2O As you can see, it\'s not balanced..... the
hydrogens are balanced on both sides (2 on each side) but the oxygens are not. There are 2
oxygens on the left and only 1 on the right. So add a coefficion of 2 to the \"H2O\" so that you
can have 2 oxygens. Now our new reaction is: H2 + 02 ===> 2H2O However this is still not
balanced. As you can see we have 2 hydrogens on the left, but now we have 4 hydrogens on the
right. So, in order to fix this, add 2 in front of H2 on the left, so now we have: 2H2 + O2 ===>
2H2O Now we have a balanced equation with 4 hydrogens on the right, and 4 hydrogens on the
left. As well as 2 oxygens on the right and 2 oxygens on the left. This same type of procedure is
how you balance any reaction. 10d.) Al2(SO4)3 = Aluminum Sulfate To calculate percent
aluminum by mass you first find the mass of the compound. Molar Mass Al2(SO4)3: Al =
27.0(2) = 54g/mol S = 32.1(3) = 96.3g/mol O = 16.0(12) = 192g/mol Add them all together to
get the molar mass of Al2(SO4)3 = 342.3g/mol Now, to get the % by mass of Al in Al2(SO4).
Unit 3 lecture s2015
This document provides objectives and content for a chemistry unit on ionic and molecular compounds. The objectives include describing how ions combine to form compounds, writing formulas, determining compound types, naming compounds, writing formulas for compounds containing polyatomic ions, determining ion charges, naming compounds from formulas, and testing ions in solutions. The content reviews ionic bonding, writing formulas, naming binary ionic compounds and those containing polyatomic ions, determining ion charges, acid and base naming, and molecular compound naming. It also outlines labs to identify common ions and practice these skills.
Chapter 7 Notes
This document discusses chemical formulas and compounds. It covers:
- The importance of chemical formulas in showing elemental composition compared to common names.
- How to write formulas for binary compounds and name them.
- Charges of transition metals and how they are represented in names using Roman numerals.
- Writing formulas for compounds containing polyatomic ions by treating them as whole units.
- Naming molecular compounds using prefixes to indicate number of atoms.
- Common acids and how to name salts containing acid anions.
- Oxidation numbers and how to determine them based on element properties and charge balance.
chem 1.docx
1. Atoms consist of a positively charged nucleus surrounded by negatively charged electrons. The positive and negative charges are equal, making the overall atom electrically neutral.
2. Isotopes are variants of the same chemical element that contain equal numbers of protons but different numbers of neutrons, differing in relative atomic mass but not chemical properties.
3. Isobars are atoms of different elements that have the same number of nucleons but differ in atomic number and mass number.
Atoms and Molecules
This document discusses the history and development of atomic theory. It describes how ancient Indian and Greek philosophers first proposed that matter is divisible into smaller particles. Democritus named these indivisible particles "atoms." Later, scientists like John Dalton and Antoine Lavoisier established laws of chemistry, including the law of conservation of mass and the law of constant proportions, which supported the atomic theory. Dalton further proposed that elements are made of atoms that combine in whole number ratios. The document defines key concepts like molecules, ions, chemical formulas, and moles. It provides examples of atomic structure and molecular formulas of common compounds.
GCSE Chemistry [C3]
The document provides information on the structure of atoms, ionic and covalent bonding, the periodic table, properties of metals and non-metals, and chemical reactions. It discusses how atoms are composed of protons, neutrons and electrons, and how electrons are arranged in shells. It also explains how ionic bonding occurs through transfer of electrons between metals and non-metals, while covalent bonding involves sharing of electrons between non-metals.
Grade 9 chemistry, ions and writing chemical formulae
This document provides information on writing chemical formulas for ionic compounds. It discusses how ions are formed by elements gaining or losing electrons to achieve stability like the nearest noble gas. The charge on simple ions relates to the number of electrons gained or lost. Polyatomic ions contain two or more combined atoms and usually have a negative charge except for ammonium. To write formulas for ionic compounds, the numbers of positive and negative ions must balance to give an electrically neutral compound. The names of ionic compounds consist of the cation name followed by the anion name changed to end in "-ide".
AP Chem Chapter 2 Outline
This document provides an overview of atomic theory and basic concepts in chemistry including:
1) Dalton's atomic theory which states that matter is made of extremely small indivisible particles called atoms.
2) Atoms of different elements have different properties and atoms of the same element are identical.
3) Chemical reactions involve changes in how atoms are combined but atoms themselves are neither created nor destroyed.
4) The discovery of subatomic particles like electrons, protons and neutrons led to Rutherford's nuclear model of the atom.
5) Isotopes are atoms of the same element with different numbers of neutrons. The periodic table organizes elements by atomic number.
Ch02 outline
This document provides an overview of atomic theory and basic concepts in chemistry including:
1) Dalton's atomic theory which states that matter is made of extremely small indivisible particles called atoms.
2) Atoms of different elements have different properties and atoms of the same element are identical.
3) Chemical reactions involve changes in how atoms are combined, not in the atoms themselves.
4) The discovery of subatomic particles like electrons, protons and neutrons led to Rutherford's nuclear model of the atom with a small, dense nucleus.
5) The periodic table organizes elements based on atomic structure including atomic number and recurring trends in properties.
Metals, Non Metals And Oxidation
This document provides information about the periodic table, including the location and properties of metals, non-metals, and metalloids. It discusses periodic trends such as atomic radius and ionic charge. Various topics are covered, including oxidation-reduction reactions, ionic and covalent bonding, naming ionic and covalent compounds, and common polyatomic ions.
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This chapter discusses chemical reactions, including:
- The difference between physical and chemical changes.
- Writing and balancing word equations and chemical equations.
- Types of chemical reactions such as combustion, displacement, neutralization, synthesis, and decomposition.
- Stoichiometry deals with calculating quantities in chemical reactions based on mole ratios in balanced equations.
Naming_compounds.ppt
This document provides information on naming and writing formulas for different types of chemical compounds. It discusses binary ionic compounds composed of a metal and nonmetal, where the metal takes a Roman numeral charge and the nonmetal suffix is changed to "-ide". Ternary ionic compounds containing a polyatomic ion are also described. Polyatomic ions are groups of atoms that behave as a unit with a charge. The document outlines steps for writing formulas and uses examples like calcium phosphate and aluminum nitrate to illustrate the process. Finally, it defines binary molecular compounds as those containing two nonmetals covalently bonded, requiring the use of numerical prefixes in the naming.
Reaction intermediates
A reaction intermediate or an intermediate is a molecular entity that is formed from the reactants (or preceding intermediates) and reacts further to give the directly observed products of a chemical reaction.
AQA Chemistry C2 Revision
This document provides an overview of key concepts in chemistry including:
1) The structure of atoms including protons, neutrons, and electrons. It also discusses isotopes and electron configuration.
2) The periodic table is introduced including periodic trends in properties and how elements are arranged in groups and periods. Metals, nonmetals, and chemical properties are also covered.
3) Bonding including ionic bonding between metals and nonmetals and covalent bonding between nonmetals is explained through examples like sodium chloride and water. Dot and cross diagrams are used to represent covalent bonds.
4) Compounds and chemical equations are discussed including balancing equations and calculating relative formula mass. Giant ionic structures
CCCCCCCCHHHHHHHHH.docx
C
C
C
C
C
C
C
C
H
H
H
HH
HH
HH
HH
HH
HH
H
H
H
C
C
C
C
C
C
C
C
H
H
H
HH
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CH
HH
CH
H
H
H
H H H HH C H
HH
C C
C
CC
C C
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H
H
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H HH
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H
H
H
octane - unbranched (straight-chain)
4-ethyl-2-methyloctane - branched
ethylcyclohexane - cyclic
Figure 1 - Unbranched, branched, and
cyclic hydrocarbons.
Experiment #3 - Hydrocarbons
Introduction
Organic chemistry is the chemistry of the
compounds of carbon. Currently over twenty
million compounds have been reported in the
chemical literature; about 90% of them are
organic, ie they contain carbon. The remaining
compounds are called inorganic and are formed
from the other elements, of which there are
about 100. That carbon so dominates
compound formation is a result of the fact that it
is almost unique in its ability to form long
chains with other carbon atoms. [Carbon’s
neighbor in the periodic table, silicon, can do
this but rarely does.] These chains with one
carbon joined to a second and the second
joined to a third, etc., can be branched, ie,
chains of carbon atoms can be attached to
carbons in the original chain. It is also possible
for one carbon in a chain to become bonded to
another carbon in that chain, resulting in a
closed ring of atoms. We call these compounds
cyclic.
Since there are so many organic
compounds it is fortunate that we can organize
them into various groups that have some
similarity to each other. For example, one large
group of organic compounds is known as the
hydrocarbons because members of this group
contain only carbon and hydrogen and no other
elements. Figure 1 shows examples of branched, unbranched and cyclic hydrocarbons.
It is possible to subdivide the hydrocarbon group of compounds based on the
bonding between the carbons. If all the carbon-carbon bonds are single, the compound
is an alkane. If at least one of the carbon-carbon bonds in the compound is a double
bond, and the remaining carbon-carbon bonds are single, the compound is an alkene. If
at least one of the carbon-carbon bonds in the compound is a triple bond, and the
remaining carbon-carbon bonds are single, the compound is an alkyne. If the compound
contains a six carbon ring that has alternating double and single bonds around the ring
(three double and three single), we say that ring, and the compound, is aromatic. An
aromatic ring looks like an alkene with three double bonds because that’s the way we
draw it using Lewis structures. However, the actual bonding in such a ring is
considerably different from that in alkenes and, consequently, many of the chemical
properties are different also. Therefore, we place these compounds in a separate family.
By the way, the term aromatic as used here has nothing to do with fragrance.
Experiment #3 Hydrocarbons Page 2
Hydrocarbons may be saturated or unsaturated. A saturated hydrocarbon is one
that is maxed out in terms of the number of hydrogens that can be present given the
nu ...
Chapter 9
This document provides information on naming and writing formulas for different types of chemical compounds including:
1. Ionic compounds consisting of monatomic and polyatomic ions are named by writing the cation first followed by the anion. Transition metal ions have stock and classical naming systems.
2. Molecular compounds consisting of two nonmetals are named using prefixes to indicate the number of atoms of each element followed by the "-ide" suffix.
3. Acids are named based on the anion present, using prefixes like "hydro-", "-ous", or "-ic" depending on the anion suffix. Their formulas are written with hydrogen and the anion.
4. Bases are named by writing the cation
Blb12 ch02 lecture
- The document discusses atomic theory and the development of models of the atom over time, from Dalton's atomic theory to Thomson's "plum pudding" model to Rutherford's nuclear model.
- It also covers the discovery of subatomic particles like electrons, protons, and neutrons as well as radioactive decay.
- Additional topics include atomic structure, isotopes, ions, chemical formulas and nomenclature of compounds and acids.
Ch04 lecpptchem1012011f
The document provides an overview of key topics in chemical bonding covered in Chapter 4, including:
- Electron configurations and valence electrons and how they relate to chemical bonding and stability.
- Drawing electron-dot structures to represent atoms, ions, and molecules.
- The two main types of chemical bonds - ionic bonds formed between ions and covalent bonds formed by shared electron pairs.
- Nomenclature rules for naming ionic and covalent compounds from their formulas and writing formulas from compound names.
- Electronegativity and how it determines if bonds are nonpolar, polar, or ionic.
- The different molecular geometries that result from electron pair repulsion in covalent
Chemistry Grade 11 Basic
This presentation is designed for the students of grades 11 and 12. You can know about the importance and scope of chemistry. Atomic mass, the process of naming compounds, acids, the chemical name of substances, and so on.
Mot of coordination field theory
The document discusses ligand field theory, which examines how ligands affect the energies of d orbitals in metal complexes. It explains that for an octahedral complex:
1) Ligands raise the dx2-y2 and dz2 orbitals significantly due to strong interactions, forming an "eg" set of orbitals.
2) Ligands interact weakly with the dxy, dxz, and dyz orbitals, forming a lower "t2g" set of orbitals.
3) The splitting of orbitals into eg and t2g sets can lead to high-spin or low-spin electron configurations, influencing magnetic and chemical properties.
GC1.pptx
The document discusses several laws of chemical changes and principles of naming chemical compounds. It describes the law of conservation of mass, law of definite proportions, and law of multiple proportions. It also discusses Dalton's atomic theory and how it can explain these laws. The document provides rules for naming binary, ternary, molecular, and acidic compounds based on their composition and oxidation states. Examples of naming ionic compounds, acids, and writing chemical formulas from compound names are also presented.
steps are as follows Dissolve the (pressumably.pdf
steps are as follows : Dissolve the (pressumably solid) mixture in an organic
solven,,,,,,, Then, in a seperating funnel, add an (Aqueous) solution of sodium hydroxide. The
Phenol, and benzoic acid, as acids, will react with the base to form phenolate and benzenoate
ions, which will dissolve into the water layer. Collect this layer, and re-precipitate the organic
molecules by adding concentrated Hydrochloric acid. The phenol and Benzoic acid can be
seperated via their varying solubilities, (8.3g/100ml vs 0.34g/100ml. respectively) by heating the
mixture in water to dissolve the phenol, and then filtering of the (practically) insoluble benzoic
acid. The solution can then be acidified (with HCl) to return the phenol..,,,,,,,,,,,,, Now add a
solution of hydrochloric acid to the seperating funnel, which (as before) will react with the basic
anniline dossilving it into the water. Collect the aqueous layer and re-precipitate the anniline
with excess sodium hydroxide. ,,,,,,,,,,,,,,, finally boil off the remaining organic solvent to obtain
the napthalene, which was left untouched by all the acids and bases.,,,,,,,,, Flow chart : Mixture
+ xs HCl ----> anilinium(aq) Mixture - aniline + weak base (Na2CO3) ---> benzoate(aq)
Mixture - aniline - benzoic acid + base (NaOH) ---> p-bromophenoxide(aq) Mixture - aniline -
benzoic acid - p-bromophenol = naphthalene
Solution
steps are as follows : Dissolve the (pressumably solid) mixture in an organic
solven,,,,,,, Then, in a seperating funnel, add an (Aqueous) solution of sodium hydroxide. The
Phenol, and benzoic acid, as acids, will react with the base to form phenolate and benzenoate
ions, which will dissolve into the water layer. Collect this layer, and re-precipitate the organic
molecules by adding concentrated Hydrochloric acid. The phenol and Benzoic acid can be
seperated via their varying solubilities, (8.3g/100ml vs 0.34g/100ml. respectively) by heating the
mixture in water to dissolve the phenol, and then filtering of the (practically) insoluble benzoic
acid. The solution can then be acidified (with HCl) to return the phenol..,,,,,,,,,,,,, Now add a
solution of hydrochloric acid to the seperating funnel, which (as before) will react with the basic
anniline dossilving it into the water. Collect the aqueous layer and re-precipitate the anniline
with excess sodium hydroxide. ,,,,,,,,,,,,,,, finally boil off the remaining organic solvent to obtain
the napthalene, which was left untouched by all the acids and bases.,,,,,,,,, Flow chart : Mixture
+ xs HCl ----> anilinium(aq) Mixture - aniline + weak base (Na2CO3) ---> benzoate(aq)
Mixture - aniline - benzoic acid + base (NaOH) ---> p-bromophenoxide(aq) Mixture - aniline -
benzoic acid - p-bromophenol = naphthalene.
the two features of the asynchronus connection that allow the receiv.pdf
the two features of the asynchronus connection that allow the receiver to stay in sync with the
incoming data stream are the start bit and short frame connections . asynchronus connection are
asynchronus serial communications in which the communicating end points interfaces are not
continously synchronized by common clock signal and the data stream contains synchronization
in the form of start and stop signals before and after each unit of transmission .asynchronus start
and stop signals was widley used for dial up modem sources to time sharing computers and bbs
systems asynchronus start stop is the physical layer is used to connect computers to modems for
many dial up internet access applications using data link frame protocol such as ppp to create
packets made upto out of asynchronous serial characters .the examples that would benefit from
asynchronous connection are modems and usb that are connectedd to interfaces
Solution
the two features of the asynchronus connection that allow the receiver to stay in sync with the
incoming data stream are the start bit and short frame connections . asynchronus connection are
asynchronus serial communications in which the communicating end points interfaces are not
continously synchronized by common clock signal and the data stream contains synchronization
in the form of start and stop signals before and after each unit of transmission .asynchronus start
and stop signals was widley used for dial up modem sources to time sharing computers and bbs
systems asynchronus start stop is the physical layer is used to connect computers to modems for
many dial up internet access applications using data link frame protocol such as ppp to create
packets made upto out of asynchronous serial characters .the examples that would benefit from
asynchronous connection are modems and usb that are connectedd to interfaces.
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CCCCCCCCHHHHHHHHH.docx
C
C
C
C
C
C
C
C
H
H
H
HH
HH
HH
HH
HH
HH
H
H
H
C
C
C
C
C
C
C
C
H
H
H
HH
HH
HH
CH
HH
CH
H
H
H
H H H HH C H
HH
C C
C
CC
C C
H
H
C
H
H
H
H
H HH
H
H
H
H
H
H
H
octane - unbranched (straight-chain)
4-ethyl-2-methyloctane - branched
ethylcyclohexane - cyclic
Figure 1 - Unbranched, branched, and
cyclic hydrocarbons.
Experiment #3 - Hydrocarbons
Introduction
Organic chemistry is the chemistry of the
compounds of carbon. Currently over twenty
million compounds have been reported in the
chemical literature; about 90% of them are
organic, ie they contain carbon. The remaining
compounds are called inorganic and are formed
from the other elements, of which there are
about 100. That carbon so dominates
compound formation is a result of the fact that it
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neighbor in the periodic table, silicon, can do
this but rarely does.] These chains with one
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carbons in the original chain. It is also possible
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Since there are so many organic
compounds it is fortunate that we can organize
them into various groups that have some
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group of organic compounds is known as the
hydrocarbons because members of this group
contain only carbon and hydrogen and no other
elements. Figure 1 shows examples of branched, unbranched and cyclic hydrocarbons.
It is possible to subdivide the hydrocarbon group of compounds based on the
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at least one of the carbon-carbon bonds in the compound is a triple bond, and the
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Hydrocarbons may be saturated or unsaturated. A saturated hydrocarbon is one
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nu ...
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This document provides information on naming and writing formulas for different types of chemical compounds including:
1. Ionic compounds consisting of monatomic and polyatomic ions are named by writing the cation first followed by the anion. Transition metal ions have stock and classical naming systems.
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4. Bases are named by writing the cation
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1) Ligands raise the dx2-y2 and dz2 orbitals significantly due to strong interactions, forming an "eg" set of orbitals.
2) Ligands interact weakly with the dxy, dxz, and dyz orbitals, forming a lower "t2g" set of orbitals.
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The document discusses several laws of chemical changes and principles of naming chemical compounds. It describes the law of conservation of mass, law of definite proportions, and law of multiple proportions. It also discusses Dalton's atomic theory and how it can explain these laws. The document provides rules for naming binary, ternary, molecular, and acidic compounds based on their composition and oxidation states. Examples of naming ionic compounds, acids, and writing chemical formulas from compound names are also presented.
Similar to First, lets start with naming ionic compounds. .pdf (20)
Grade 9 chemistry, ions and writing chemical formulae
Grade 9 chemistry, ions and writing chemical formulae
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steps are as follows Dissolve the (pressumably.pdf
steps are as follows : Dissolve the (pressumably solid) mixture in an organic
solven,,,,,,, Then, in a seperating funnel, add an (Aqueous) solution of sodium hydroxide. The
Phenol, and benzoic acid, as acids, will react with the base to form phenolate and benzenoate
ions, which will dissolve into the water layer. Collect this layer, and re-precipitate the organic
molecules by adding concentrated Hydrochloric acid. The phenol and Benzoic acid can be
seperated via their varying solubilities, (8.3g/100ml vs 0.34g/100ml. respectively) by heating the
mixture in water to dissolve the phenol, and then filtering of the (practically) insoluble benzoic
acid. The solution can then be acidified (with HCl) to return the phenol..,,,,,,,,,,,,, Now add a
solution of hydrochloric acid to the seperating funnel, which (as before) will react with the basic
anniline dossilving it into the water. Collect the aqueous layer and re-precipitate the anniline
with excess sodium hydroxide. ,,,,,,,,,,,,,,, finally boil off the remaining organic solvent to obtain
the napthalene, which was left untouched by all the acids and bases.,,,,,,,,, Flow chart : Mixture
+ xs HCl ----> anilinium(aq) Mixture - aniline + weak base (Na2CO3) ---> benzoate(aq)
Mixture - aniline - benzoic acid + base (NaOH) ---> p-bromophenoxide(aq) Mixture - aniline -
benzoic acid - p-bromophenol = naphthalene
Solution
steps are as follows : Dissolve the (pressumably solid) mixture in an organic
solven,,,,,,, Then, in a seperating funnel, add an (Aqueous) solution of sodium hydroxide. The
Phenol, and benzoic acid, as acids, will react with the base to form phenolate and benzenoate
ions, which will dissolve into the water layer. Collect this layer, and re-precipitate the organic
molecules by adding concentrated Hydrochloric acid. The phenol and Benzoic acid can be
seperated via their varying solubilities, (8.3g/100ml vs 0.34g/100ml. respectively) by heating the
mixture in water to dissolve the phenol, and then filtering of the (practically) insoluble benzoic
acid. The solution can then be acidified (with HCl) to return the phenol..,,,,,,,,,,,,, Now add a
solution of hydrochloric acid to the seperating funnel, which (as before) will react with the basic
anniline dossilving it into the water. Collect the aqueous layer and re-precipitate the anniline
with excess sodium hydroxide. ,,,,,,,,,,,,,,, finally boil off the remaining organic solvent to obtain
the napthalene, which was left untouched by all the acids and bases.,,,,,,,,, Flow chart : Mixture
+ xs HCl ----> anilinium(aq) Mixture - aniline + weak base (Na2CO3) ---> benzoate(aq)
Mixture - aniline - benzoic acid + base (NaOH) ---> p-bromophenoxide(aq) Mixture - aniline -
benzoic acid - p-bromophenol = naphthalene.
the two features of the asynchronus connection that allow the receiv.pdf
the two features of the asynchronus connection that allow the receiver to stay in sync with the
incoming data stream are the start bit and short frame connections . asynchronus connection are
asynchronus serial communications in which the communicating end points interfaces are not
continously synchronized by common clock signal and the data stream contains synchronization
in the form of start and stop signals before and after each unit of transmission .asynchronus start
and stop signals was widley used for dial up modem sources to time sharing computers and bbs
systems asynchronus start stop is the physical layer is used to connect computers to modems for
many dial up internet access applications using data link frame protocol such as ppp to create
packets made upto out of asynchronous serial characters .the examples that would benefit from
asynchronous connection are modems and usb that are connectedd to interfaces
Solution
the two features of the asynchronus connection that allow the receiver to stay in sync with the
incoming data stream are the start bit and short frame connections . asynchronus connection are
asynchronus serial communications in which the communicating end points interfaces are not
continously synchronized by common clock signal and the data stream contains synchronization
in the form of start and stop signals before and after each unit of transmission .asynchronus start
and stop signals was widley used for dial up modem sources to time sharing computers and bbs
systems asynchronus start stop is the physical layer is used to connect computers to modems for
many dial up internet access applications using data link frame protocol such as ppp to create
packets made upto out of asynchronous serial characters .the examples that would benefit from
asynchronous connection are modems and usb that are connectedd to interfaces.
Telomerase is the enzyme responsible for maintenance of the length o.pdf
Telomerase is the enzyme responsible for maintenance of the length of telomeres by addition of
guanine-rich repetitive sequences, (Zvereva, 2010). Thus Telomerase, is a Specialized
Polymerase That Carries Its Own RNA Template. Thus it accounts for a faithful replication of
chromosomal ends as theTelomerase contains an RNA molecule that acts as a template for
extending the leading strand.
Solution
Telomerase is the enzyme responsible for maintenance of the length of telomeres by addition of
guanine-rich repetitive sequences, (Zvereva, 2010). Thus Telomerase, is a Specialized
Polymerase That Carries Its Own RNA Template. Thus it accounts for a faithful replication of
chromosomal ends as theTelomerase contains an RNA molecule that acts as a template for
extending the leading strand..
Suppose Bob sends an encrypted document to Alice. To be verifiable, .pdf
Suppose Bob sends an encrypted document to Alice. To be verifiable, Alice must be able to
convince herself that Bob sent the encrypted document. To be non-forgeable, Alice must be able
to convince herself that only Bob could have sent the encrypted document Alice must be able to
convince someone else that only Bob could have sent the document. To illustrate the latter
distinction, suppose Bob and Alice share a secret key, and they are the only ones in the world
who know the key. If Alice receives a document that was encrypted with the key, and knows that
she did not encrypt the document herself, then the document is known to be verifiable and non-
forgeable (assuming a suitably strong encryption system was used). However, Alice can not
convince someone else that Bob must have sent the document, since in fact Alice knew the key
herself and could have encrypted/sent the document.
Solution
Suppose Bob sends an encrypted document to Alice. To be verifiable, Alice must be able to
convince herself that Bob sent the encrypted document. To be non-forgeable, Alice must be able
to convince herself that only Bob could have sent the encrypted document Alice must be able to
convince someone else that only Bob could have sent the document. To illustrate the latter
distinction, suppose Bob and Alice share a secret key, and they are the only ones in the world
who know the key. If Alice receives a document that was encrypted with the key, and knows that
she did not encrypt the document herself, then the document is known to be verifiable and non-
forgeable (assuming a suitably strong encryption system was used). However, Alice can not
convince someone else that Bob must have sent the document, since in fact Alice knew the key
herself and could have encrypted/sent the document..
probablity = 212 100 = 16.6 Solutionprobablity = 212 10.pdf
The document calculates a probability as 2 out of 12 possibilities, which equals 16.6% when expressed as a percentage. It shows the work to calculate the probability as 2/12 and then multiplying that fraction by 100 to express it as a percentage.
Platinum complexes like Asplastin are powerful antitumor medications.pdf
Platinum complexes like Asplastin are powerful antitumor medications and they are having
ability to cross the cell membrane and then reaches the nucleus and will attach to DNA and stop
cell growth. The transfer of this Asplastin is facilitated by a copper transporter (Ctr1-membrane-
dwelling protein which main function is to bring copper into cells). The |Ctr1 structure has of
three helical segments which appears to sit in the membrane, and one end can be seen protruding
into the cell, while the other end will be seen on the outside and a channel like structure will be
formed when three such molecules assemble together.
When Asplastin is injected in the body of a cancer patient, the Asplastin which have a central
platinum ion and four ligands (which includes two neighboring chloride ions and two
neighboring amino groups). The Ctr1 will displaces these four ligands from Asplastin and will
bind to the platinum ion itself and it will transfer it through the channel and released in the
cytosol of the cell. In addition to this few amount of Asplastin molecules will interact with the
methionine-rich extracellular end of the copper transporter to form a trimeric channel structure to
get transported as a little interior bubble filled with the outer medium and will released into
various organelles including nucleus.
How it acts on cancer cells: The 4 steps how Asplastin will act is (i) Cellular uptake of drug, (ii)
aquation/activation of Asplastin, (iii) Drug binding to DNA and (iv) Lesions formed on DNA
will make the cell to opt for apoptosis.
N7 sites of deoxyguanosine residues on the DNA are the most nucleophilic positions and are
preferentially platinated. Asplastin will form a monofunctional adducts on DNA (You can see
only one covalent bond to the genomic polymer). Like in second reaction second guanine base
will get substituted by chloride ligand, thus forming a cross-link on the DNA (either on the same
strand or it may be on different strands). The most common lesion are formed from 1,2-d(GpG)
intrastrand cross-links and finally due to drug action we can see bending and unwinding of the
double helix and cells with damaged DNA will be arrested at the G2/M transition of the cell
cycle and undergoes apoptosis.
Solution
Platinum complexes like Asplastin are powerful antitumor medications and they are having
ability to cross the cell membrane and then reaches the nucleus and will attach to DNA and stop
cell growth. The transfer of this Asplastin is facilitated by a copper transporter (Ctr1-membrane-
dwelling protein which main function is to bring copper into cells). The |Ctr1 structure has of
three helical segments which appears to sit in the membrane, and one end can be seen protruding
into the cell, while the other end will be seen on the outside and a channel like structure will be
formed when three such molecules assemble together.
When Asplastin is injected in the body of a cancer patient, the Asplastin which have a central
platinum ion and f.
Part 1 1)#include stdio.hint testWhileLoop() ; int testFo.pdf
Part 1:
1)
#include
int testWhileLoop() ;
int testForLoop() ;
int main()
{
printf(\"While loop test \ \");
testWhileLoop();
printf(\"For loop test \ \");
testForLoop();
return 0;
}
Part 2:
1)
#include
int testWhileLoop() ;
int main()
{
printf(\"While loop test \ \");
testWhileLoop();
return 0;
}
int testWhileLoop()
{
int count=0;
int n;
while (count<10)
{
printf(\"Enter an integer: \");
scanf(\"%d\",&n);
printf(\"You Entered: %d\ \",n);
count++;
}
}
2)
#include
int testWhileLoop() ;
int main()
{
printf(\"While loop test \ \");
testWhileLoop();
return 0;
}
int testWhileLoop()
{
int count=0;
int n;
int sum=0;
while (count<10)
{
printf(\"Enter an integer: \");
scanf(\"%d\",&n);
printf(\"You Entered: %d\ \",n);
count++;
sum=sum+n;
}
printf(\"Total sum of integers is: %d\ \",sum);
}
3)
#include
int testWhileLoop() ;
int main()
{
printf(\"While loop test \ \");
testWhileLoop();
return 0;
}
int testWhileLoop()
{
int count=0;
int n;
int sum=0;
while (count<10)
{
printf(\"Enter an integer between 5 and 20: \");
scanf(\"%d\",&n);
while(n<5 || n>20)
{
printf(\"Error: You must enter a value between 5 and 20: please renter: \");
scanf(\"%d\",&n);
}
printf(\"You Entered: %d\ \",n);
count++;
sum=sum+n;
}
printf(\"Total sum of integers is: %d\ \",sum);
}
Part 3:
#include
int testForLoop() ;
int main()
{
printf(\"For loop test \ \");
testForLoop();
return 0;
}
int testForLoop()
{
int count=0;
int n;
int sum=0;
for (count=0;count<10;count++)
{
printf(\"Enter an integer: \");
scanf(\"%d\",&n);
printf(\"You Entered: %d\ \",n);
sum=sum+n;
}
printf(\"Total sum of integers is: %d\ \",sum);
}
Solution
Part 1:
1)
#include
int testWhileLoop() ;
int testForLoop() ;
int main()
{
printf(\"While loop test \ \");
testWhileLoop();
printf(\"For loop test \ \");
testForLoop();
return 0;
}
Part 2:
1)
#include
int testWhileLoop() ;
int main()
{
printf(\"While loop test \ \");
testWhileLoop();
return 0;
}
int testWhileLoop()
{
int count=0;
int n;
while (count<10)
{
printf(\"Enter an integer: \");
scanf(\"%d\",&n);
printf(\"You Entered: %d\ \",n);
count++;
}
}
2)
#include
int testWhileLoop() ;
int main()
{
printf(\"While loop test \ \");
testWhileLoop();
return 0;
}
int testWhileLoop()
{
int count=0;
int n;
int sum=0;
while (count<10)
{
printf(\"Enter an integer: \");
scanf(\"%d\",&n);
printf(\"You Entered: %d\ \",n);
count++;
sum=sum+n;
}
printf(\"Total sum of integers is: %d\ \",sum);
}
3)
#include
int testWhileLoop() ;
int main()
{
printf(\"While loop test \ \");
testWhileLoop();
return 0;
}
int testWhileLoop()
{
int count=0;
int n;
int sum=0;
while (count<10)
{
printf(\"Enter an integer between 5 and 20: \");
scanf(\"%d\",&n);
while(n<5 || n>20)
{
printf(\"Error: You must enter a value between 5 and 20: please renter: \");
scanf(\"%d\",&n);
}
printf(\"You Entered: %d\ \",n);
count++;
sum=sum+n;
}
printf(\"Total sum of integers is: %d\ \",sum);
}
Part 3:
#include
int testForLoop() ;
int main()
{
printf(\"For loop test \ \");
testForLoop();
return 0;
}
int testForLoop()
{
int c.
none of them are correct!Solutionnone of them are correct!.pdf
This 1 sentence document states that none of the potential solutions or answers are correct. It provides a concise but incomplete message without further context or explanation.
Negative control plate with no DNA transforms competent cells withou.pdf
Negative control plate with no DNA transforms competent cells without any DNA on selection
media. , If more colonies are produced, shows the problem with antibiotic in the agar plate.
No ligase control plates provide information about digestion efficiency. it transform competent
cells withdigested plasmid or DNA. If several colonies are found, it shows that digestion did not
completed properly.
Solution
Negative control plate with no DNA transforms competent cells without any DNA on selection
media. , If more colonies are produced, shows the problem with antibiotic in the agar plate.
No ligase control plates provide information about digestion efficiency. it transform competent
cells withdigested plasmid or DNA. If several colonies are found, it shows that digestion did not
completed properly..
Modifications highlighted in bold lettersDropOutStack.javaim.pdf
//Modifications highlighted in bold letters
//DropOutStack.java
import java.util.Arrays;
public class DropOutStack {
/**
* Defines the interface to a stack collection.
*
* @author Java Foundations
* @version 4.0
*/
public interface StackADT {
/**
* Adds the specified element to the top of this stack.
*
* @param element
* element to be pushed onto the stack
*/
public void push(T element);
/**
* Removes and returns the top element from this stack.
*
* @return the element removed from the stack
*/
public T pop();
/**
* Returns without removing the top element of this stack.
*
* @return the element on top of the stack
*/
public T peek();
/**
* Returns true if this stack contains no elements.
*
* @return true if the stack is empty
*/
public boolean isEmpty();
/**
* Returns the number of elements in this stack.
*
* @return the number of elements in the stack
*/
public int size();
/**
* Returns a string representation of this stack.
*
* @return a string representation of the stack
*/
public String toString();
}
/**
* Represents the situation in which a collection is empty.
*
* @author Java Foundations
* @version 4.0
*/
public static class EmptyCollectionException extends RuntimeException {
/**
* Sets up this exception with an appropriate message.
*
* @param collection
* the name of the collection
*/
public EmptyCollectionException(String collection) {
super(\"The \" + collection + \" is empty.\");
}
}
/**
* Program entry point for stack testing.
*
* @param args
* Argument list.
*/
public static void main(String[] args) {
ArrayDropOutStack stack = new ArrayDropOutStack(4);
System.out.println(\"DROP-OUT STACK TESTING\");
stack.push(1);
stack.push(2);
stack.push(3);
stack.push(4);
System.out.println(\"Stack : \"+stack.toString());
System.out.println(\"pushing 5 element \");
stack.push(5);
System.out.println(\"Now stack elements\");
System.out.println(stack.toString());
System.out.println(\"The size of the stack is: \" + stack.size());
if (!stack.isEmpty())
System.out.println(\"The stack contains:\ \" + stack.toString());
stack.pop();
System.out.println(\"poping element 5\"+stack.toString());
System.out.println(\"The size of the stack is: \" + stack.size());
System.out.println(\"pushing 7 element \");
stack.push(7);
System.out.println(\"Now stack elements\");
System.out.println(stack.toString());
System.out.println(\"pushing 8 element \");
stack.push(8);
System.out.println(\"Now stack elements\");
System.out.println(stack.toString());
if (!stack.isEmpty())
System.out.println(\"The stack contains:\ \" + stack.toString());
}
/**
* An array implementation of a stack in which the bottom of the stack is
* fixed at index 0.
*
* @author Java Foundations
* @version 4.0
*/
public static class ArrayDropOutStack implements StackADT {
private final static int DEFAULT_CAPACITY = 100;
private int top;
private T[] stack;
/**
* Creates an empty stack using the default capacity.
*/
public ArrayDropOutStack() {
this(DEFAULT_CAPACITY);
}
/**
* Creates an empty stack using.
Message types used by the DHCP boot sequenceop Message type.h.pdf
Message types used by the DHCP boot sequence
op
: Message type.
htype
: Hardware address type defined at Internet Assigned Numbers Authority (IANA).
hlen
: Hardware address length, in octets.
hops
: Value set to zero by DHCP clients. Optionally used to count the number of relay agents that
forwarded the message.
xid
: A random number used to associate messages and responses between a client and a server.
secs
: Seconds elapsed since client began address acquisition or renewal process.
flags
: Flags set by client. The Broadcast flag is set if the client cannot receive unicast IP datagrams
(for example, before it is configured with an IP address).
ciaddr
: Used if the client has an IP address and can respond to Address Resolution Protocol (ARP)
requests.
yiaddr
: Address given to the DHCP client by the DHCP server.
siaddr
: IP address of the server that is offering a lease.
giaddr
: DHCP relay agent IP address.
chaddr
: Client hardware address.
sname
: Optional server host name. Not used in Windows Server 2008.
file
: The name of the file containing the boot image for a BOOTP client.
options
: Optional parameters field. In the DHCP protocol packet, each option begins with a single octet
tag, which holds the option code, and a second octet, which describes the option data length, in
bytes. For a complete list of the DHCP options available by default on a DHCP server running
on Windows Server 2008, see DHCP Tools and Options.
op
: Message type.
htype
: Hardware address type defined at Internet Assigned Numbers Authority (IANA).
hlen
: Hardware address length, in octets.
hops
: Value set to zero by DHCP clients. Optionally used to count the number of relay agents that
forwarded the message.
xid
: A random number used to associate messages and responses between a client and a server.
secs
: Seconds elapsed since client began address acquisition or renewal process.
flags
: Flags set by client. The Broadcast flag is set if the client cannot receive unicast IP datagrams
(for example, before it is configured with an IP address).
ciaddr
: Used if the client has an IP address and can respond to Address Resolution Protocol (ARP)
requests.
yiaddr
: Address given to the DHCP client by the DHCP server.
siaddr
: IP address of the server that is offering a lease.
giaddr
: DHCP relay agent IP address.
chaddr
: Client hardware address.
sname
: Optional server host name. Not used in Windows Server 2008.
file
: The name of the file containing the boot image for a BOOTP client.
options
: Optional parameters field. In the DHCP protocol packet, each option begins with a single octet
tag, which holds the option code, and a second octet, which describes the option data length, in
bytes. For a complete list of the DHCP options available by default on a DHCP server running
on Windows Server 2008, see DHCP Tools and Options.
Solution
Message types used by the DHCP boot sequence
op
: Message type.
htype
: Hardware address type defined at Internet Assigned Numbers Authority.
Law of conservation of matter(mass)In any closed system subjected .pdf
Law of conservation of matter(mass)
In any closed system subjected to no external forces,the mass is constant irrespective of its
changes in different form. Matter cannot be created or destroyed in an isolated system. It only
changes from one form into another.
Solution
Law of conservation of matter(mass)
In any closed system subjected to no external forces,the mass is constant irrespective of its
changes in different form. Matter cannot be created or destroyed in an isolated system. It only
changes from one form into another..
It is a unit of measurement for the amount of substance.The mole is .pdf
It is a unit of measurement for the amount of substance.The mole is defined as the amount of
substance that contains as many elementary entities (e.g., atoms, molecules, ions, electrons) as
there are atoms in 12 g of the isotope carbon-12. The experimentally determined value of a mole
as adopted 6.02 × 1023.
Solution
It is a unit of measurement for the amount of substance.The mole is defined as the amount of
substance that contains as many elementary entities (e.g., atoms, molecules, ions, electrons) as
there are atoms in 12 g of the isotope carbon-12. The experimentally determined value of a mole
as adopted 6.02 × 1023..
In insurance, the term risk pooling refers to the spreading of f.pdf
In insurance, the term \"risk pooling\" refers to the spreading of financial risks evenly among a
large number of contributors to the program. Insurance is the transference of risks from
individuals or corporations who cannot bear a possible unplanned financial catastrophe to the
capital markets, which can bear them easily -- at least in theory.
Pure risk is a category of risk in which loss is the only possible outcome, which is the opposite of
speculative risk. There are products that can be purchased to mitigate pure risk, such as home
insurance being used to protect homeowners against their homes being destroyed. Other
examples of pure risk events include premature death, identity theft and career-ending
disabilities.1) in cases of home insurance and health insurance risk pooling can be effectively
used as of all the individuals who invest in the insurance by the law of large number a miniscule
probability of the people actually suffer the real risk. 2) Risk pooling is an important concept in
supply chain management . It suggests that demand variability is reduced if one aggregates
demand across locations because, as demand is aggregated across different locations, it becomes
more likely that high demand from one customer will be offset by low demand from another.
However,consider the 1)\"high risk pools\", which simply means separating out the sickest, most
expensive people in the country and dumping them into a separate program.With the \"bad
apples\" (ie, human beings with terrible medical problems) safely tucked out of the way, the
average cost of treating everyone else supposedly suddenly becomes less pricey.This is the exact
opposite of the entire point of health insurance in the first place...spreading the risk and hence
risk pooling fails here.
2)Liability risk includes economic losses from being held responsible for harming others or their
property. This cannot be covered by risk pooling.
Solution
In insurance, the term \"risk pooling\" refers to the spreading of financial risks evenly among a
large number of contributors to the program. Insurance is the transference of risks from
individuals or corporations who cannot bear a possible unplanned financial catastrophe to the
capital markets, which can bear them easily -- at least in theory.
Pure risk is a category of risk in which loss is the only possible outcome, which is the opposite of
speculative risk. There are products that can be purchased to mitigate pure risk, such as home
insurance being used to protect homeowners against their homes being destroyed. Other
examples of pure risk events include premature death, identity theft and career-ending
disabilities.1) in cases of home insurance and health insurance risk pooling can be effectively
used as of all the individuals who invest in the insurance by the law of large number a miniscule
probability of the people actually suffer the real risk. 2) Risk pooling is an important concept in
supply chain management . It suggests that.
Some CO is Added The Pressure of CH4 and H2O will.pdf
Some CO is Added The Pressure of CH4 and H2O will Increase Equilibrium will
shift to the Left Some CH4 is Removed Pressure of H2O will Increase Pressure of CO will
Decrease Equilibrium will shift to the Left The Volume of Vessel is Reduced Pressure of CH4
will Increase Pressure of H2O will Increase Equilibrium will shift to the Left
Solution
Some CO is Added The Pressure of CH4 and H2O will Increase Equilibrium will
shift to the Left Some CH4 is Removed Pressure of H2O will Increase Pressure of CO will
Decrease Equilibrium will shift to the Left The Volume of Vessel is Reduced Pressure of CH4
will Increase Pressure of H2O will Increase Equilibrium will shift to the Left.
Comments Figures are not properly numbered. Further signal of figur.pdf
Comments: Figures are not properly numbered. Further signal of figure 1 is not shown and hence
the above figure (assumed to figure 2) can not be simulated.
Solution
Comments: Figures are not properly numbered. Further signal of figure 1 is not shown and hence
the above figure (assumed to figure 2) can not be simulated..
Change the value of jug1 and jug 2 accordingly. 1 File WaterJugBSF.j.pdf
Change the value of jug1 and jug 2 accordingly. 1 File WaterJugBSF.java
import java.util.*;
import java.util.LinkedList;
class Test {
HashSet uniqueStates;
void letsRoll() {
/*
* The capacity of jug1(jug1 capacity is greater than jug2 capacity)
*/
int jug1 = 3;
/*
* The capacity of jug two
*/
int jug2 = 2;
/*
* Final Amount needed in jug1
*/
int amtNeeded = 2;
State initialState = new State(0, 0);
State finalState = new State(amtNeeded, 0);
State finalPath = null;
uniqueStates = new HashSet();
/*
* Change queue to stack to convert to DFS
*/
LinkedList queue = new LinkedList();
queue.add(initialState);
while (!queue.isEmpty()) {
State currState = queue.poll();
if (currState.equals(finalState)) {
finalPath = currState;
break;
}
// if x is zero fill it
if (currState.x == 0) {
State nextState = new State(jug1, currState.y, currState);
//System.out.println(currState);
checkUniqueStates(uniqueStates, nextState, queue);
}
// if y is empty fill it
if (currState.y == 0) {
State nextState = new State(currState.x, jug2, currState);
checkUniqueStates(uniqueStates, nextState, queue);
}
// if x is not empty , empty it
if (currState.x > 0) {
State nextState = new State(0, currState.y, currState);
checkUniqueStates(uniqueStates, nextState, queue);
}
// if y is not empty, empty it
if (currState.y > 0) {
State nextState = new State(currState.x, 0, currState);
checkUniqueStates(uniqueStates, nextState, queue);
}
// transfer from x to y, when x non empty and y is not full
if (currState.x > 0 && currState.y < jug2) {
int amtToTransfer = Math.min(currState.x, jug2 - currState.y);
State nextState = new State(currState.x - amtToTransfer, currState.y
+ amtToTransfer,
currState);
checkUniqueStates(uniqueStates, nextState, queue);
}
// transfer from y to x, when y is not empty and x is not full
if (currState.y > 0 && currState.x < jug1) {
int amtToTransfer = Math.min(currState.y, jug1 - currState.x);
State nextState = new State(currState.x + amtToTransfer, currState.y
- amtToTransfer,
currState);
checkUniqueStates(uniqueStates, nextState, queue);
}
}
if (finalPath != null) {
System.out.println(\"Final Result\");
System.out.println(\"J1 J2\");
System.out.println(finalPath);
}
else{
System.out.println(\"Not Possible\");
}
}
/*
* Checks whether State toCheck has been generated before, if not it is
* added to queue and uniqueStates Set
*/
void checkUniqueStates(HashSet uniqueStates, State toCheck,
LinkedList queue) {
if (!uniqueStates.contains(toCheck)) {
uniqueStates.add(toCheck);
queue.add(toCheck);
}
}
public static void main(String[] args) {
new Test().letsRoll();
}
}
2 State.java
class State {
/*
* Amount in jug1 for current State
*/
int x;
/*
* Amount in jug2 for current State
*/
int y;
/*
* Parent of current State
*/
State pre;
public State(int x, int y) {
super();
this.x = x;
this.y = y;
}
public State(int x, int y, State pre) {
super();
this.x = x;
this.y = y;
this.pre = pre;
System.out.println(\"(\"+x+\",\"+y+\")\");
}
@Override
public int hashCode() {
final int .
Balance sheetBalance sheet is the statement of financial position .pdf
Balance sheet
Balance sheet is the statement of financial position which reports all the assets, liabilities and
equity held by the company at a specific date. It helps in telling about the investments, resources,
claims and owner’s equity of the company. It revolves around the equation i.e. Assets =
Liabilities + equity.
What is shown in balance sheet:
The balance sheet has three major categories which includes Assets, liabilities and equity. All
these are calssified on the basis of their nature.
Assets can be said as the resources of the company and are classified as: Current assets, long
term investment, property, plant and equipment, intangible assets and other assets
Assets includes:
•Current assets – Cash, accounts receivables, prepaid expenses, inventories
•Long term investments – investment in stock
•Plant property and equipment – Land, building, equipment
•Intangible assets – Goodwill, patents, trademarks
Liabilities are the claims and can be classified as current liabilities, long term liabilities
Liabilities includes:
•Current liabilities: Accounts payable, income tax payable. Salaries payable, accrued expenses,
unearned revenue, current portion of long term debt due
•Long term liabilities- bonds payable, notes payable
Owner;s equity can be classified as the Capital stock which includes common stock and
preferred stock
It also includes Additional paid in capital, Retained earnings
Retained earnings are the accumulated earnings of the company. It is calculated as Beginning
balance, Add: Net income less: Dividends
Importance:
Balance sheet is important in every business. Considering the hospitality firm, it is important to
analyze different aspects of teh firm to know its financial postion. As the hospitality firm
emphasize on services, it is important to know the financial position of the company through its
financial statements. the hospitality firms like hotel needs to report their assets (building) held by
the company along with other assets, liabilities and equity.
Balance sheet is the statement which helps in analysing the financial position of the company, it
can also help in predicting the cash flows and the financial position of the company. With the
help of the balance sheet we can help in analysing the ability of the firm to pay off its short term
and long term debts.
Balance sheet reports its assets and liabilities on historical basis and uses different estimates to
analyse the amounts like uncollectibles
Solution
Balance sheet
Balance sheet is the statement of financial position which reports all the assets, liabilities and
equity held by the company at a specific date. It helps in telling about the investments, resources,
claims and owner’s equity of the company. It revolves around the equation i.e. Assets =
Liabilities + equity.
What is shown in balance sheet:
The balance sheet has three major categories which includes Assets, liabilities and equity. All
these are calssified on the basis of their nature.
Assets can be .
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First, lets start with naming ionic compounds. .pdf
- 1. First, let's start with naming ionic compounds. A binary ionic compound has one metal and one nonmetal present in the compound. Rubidium chloride, or RbCl, is a binary ionic compound. The metal here is Rb (rubidium, group 1A) and the nonmetal is Cl (chlorine, group 7A). When you name binary ionic compounds, you mention the cation (positively charged ion) first (usually metals, those elements that appear on the left side of the periodic table have the tendency to form positively-charged ions). Then mention the anion (negatively charged ion). The cation is rubidium (Rb). We mention it thus: Rubidium The anion is chlorine. When we write the name of the anion [alongside with the cation], we drop the ending -ine (or whatever ending it may have) and replace it with -ide. So chlorine now becomes chlor + ide = chloride. Therefore, the name of the compound is Rubidium Chloride. When you write the formulas of binary ionic compounds, you use the criss-cross method. Here's how it works: Rubidium has a charge of +1. Chlorine has a charge of -1. You interchange the charges of both ions. These charges, when interchanged, become the subscripts of the elements in the compound. Hence, the compound now looks Rb1Cl1. Since the subscripts are all 1, we can remove them and write the formula as RbCl. Here's another example: Give the formula of the compound magnesium chloride. Mg has a charge of +2. Chlorine has a charge of -1. When you interchange the respective charges of magnesium and chlorine, we get the following formula: Mg1Cl2 We simplify this as MgCl2. A list of the common cations and ions is found at the back page or on the chapter of naming chemical compounds of your chemistry book. Take time to know them by heart. But what if... you've got a compound named sodium nitrate. Ok. The formula is NaNO3. How did I know? Sodium nitrate is an example of a ternary ionic compound. A ternary ionic compound has two or more elements present in it. In this case, there are 3 (Na, N and O). The naming system of ternary ionic compounds is the same as that of binary ionic compounds. Let's name the participating ions: Na+ NO3- NO3- is the formula for the polyatomic ion (two or more elements joined together sharing a common charge; they act as one unit when they combine with other elements) nitrate. We interchange the charges of sodium and nitrate. Interchanging them gives us the formula NaNO3 To name this formula, just combine the name of the cation and anion together. In this case, it is sodium nitrate. What if we have a formula like this? Ba(OH)2 Don't worry. This is just barium hydroxide. Let's analyze why this came about. The charge of Ba is +2 and hydroxide (OH-) is -1. When you combine them together by interchanging subscripts, we get the following: BaOH2 Wait. The formula doesn't make sense. H is not the only atom having two of its kind, but O too. So we put parentheses around hydroxide to indicate that there are two units of the hydroxide ion, each of which has two O and H atoms respectively. We now have the formula Ba(OH)2. Again, review the list of common polyatomic cations and anions. So far there are two polyatomic cations: hydronium (H3O+) and ammonium (NH4+). This can be found in your chem book and in the net. There are still lots of
- 2. stuff related to this, most of which are very basic, and I don't have the space to tackle all of them here. Read your chem book or surf the net for more info. You can ask your chem teacher and friends for help, too. Solution First, let's start with naming ionic compounds. A binary ionic compound has one metal and one nonmetal present in the compound. Rubidium chloride, or RbCl, is a binary ionic compound. The metal here is Rb (rubidium, group 1A) and the nonmetal is Cl (chlorine, group 7A). When you name binary ionic compounds, you mention the cation (positively charged ion) first (usually metals, those elements that appear on the left side of the periodic table have the tendency to form positively-charged ions). Then mention the anion (negatively charged ion). The cation is rubidium (Rb). We mention it thus: Rubidium The anion is chlorine. When we write the name of the anion [alongside with the cation], we drop the ending -ine (or whatever ending it may have) and replace it with -ide. So chlorine now becomes chlor + ide = chloride. Therefore, the name of the compound is Rubidium Chloride. When you write the formulas of binary ionic compounds, you use the criss-cross method. Here's how it works: Rubidium has a charge of +1. Chlorine has a charge of -1. You interchange the charges of both ions. These charges, when interchanged, become the subscripts of the elements in the compound. Hence, the compound now looks Rb1Cl1. Since the subscripts are all 1, we can remove them and write the formula as RbCl. Here's another example: Give the formula of the compound magnesium chloride. Mg has a charge of +2. Chlorine has a charge of -1. When you interchange the respective charges of magnesium and chlorine, we get the following formula: Mg1Cl2 We simplify this as MgCl2. A list of the common cations and ions is found at the back page or on the chapter of naming chemical compounds of your chemistry book. Take time to know them by heart. But what if... you've got a compound named sodium nitrate. Ok. The formula is NaNO3. How did I know? Sodium nitrate is an example of a ternary ionic compound. A ternary ionic compound has two or more elements present in it. In this case, there are 3 (Na, N and O). The naming system of ternary ionic compounds is the same as that of binary ionic compounds. Let's name the participating ions: Na+ NO3- NO3- is the formula for the polyatomic ion (two or more elements joined together sharing a common charge; they act as one unit when they combine with other elements) nitrate. We interchange the charges of sodium and nitrate. Interchanging them gives us the formula NaNO3 To name this formula, just combine the name of the cation and anion together. In this case, it is sodium nitrate. What if we have a formula like this? Ba(OH)2 Don't worry. This is just barium hydroxide. Let's analyze why this came about. The charge of Ba is +2 and hydroxide (OH-) is -1. When you combine them together by interchanging subscripts, we get the following: BaOH2 Wait. The formula doesn't make sense.
- 3. H is not the only atom having two of its kind, but O too. So we put parentheses around hydroxide to indicate that there are two units of the hydroxide ion, each of which has two O and H atoms respectively. We now have the formula Ba(OH)2. Again, review the list of common polyatomic cations and anions. So far there are two polyatomic cations: hydronium (H3O+) and ammonium (NH4+). This can be found in your chem book and in the net. There are still lots of stuff related to this, most of which are very basic, and I don't have the space to tackle all of them here. Read your chem book or surf the net for more info. You can ask your chem teacher and friends for help, too.