Chemistry Bonding Assignment

Chemistry Bonding Assignment
Chemistry 30
Chemical Bonding – Properties of Molecules
1. For the following molecules determine which atoms are bonded (write the symbols with a bond
between them), the electronegativity difference between them, and the type of chemical bond it
represents. If the bond is ionic, state what ions are produced. If the bond is polar covalent, indicate
the direction of the dipole on the symbols from the first part.
a) KCl Electronegativity difference = K – Cl = 0.8 – 3.0 = 2.2 ionic bond K1+ Cl1– b) LiBr
Electronegativity difference = Li – Br = 1.0 – 2.8 = 1.8 ionic bond Li1+ Br1– [pic] c) HI
Electronegativity difference = H – I = 2.1 – 2.5 = 0.4 polar covalent bond ... Show more content on
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Both have London dispersion force drawing them together.
These two are isoelectronic so the London force should be the same. This is manifested in similar
boiling temperatures.
5. Why does liquid propane (C3H8) boil at a much lower temperature than gasoline (C8H18)?
Both are pure hydrocarbons and are non–polar (symmetry causes dipoles to cancel). Both have
london dispersion force. Propane has 26 electrons, gasoline has 66. Since gasoline has more
electrons, it has a higher london dispersion force and so has a higher boiling temperature than
propane.
6. Given the following molecules:
i) methane iii) butane ii) propane iv) methyl propane
a) Draw each structure
[pic] [pic] [pic] [pic]
b) Predict the order of increasing melting point. Give reasons for your answer.
methane, propane, butane, methyl propane.

fewest electrons, lowest melting point. methyl propane is more compact than butane so it packs
better in the solid phase and has the highest melting point.
c) Predict the order of increasing boiling point. Give reasons for your answer.
methane, propane, methyl propane, butane
fewest electrons, lowest boiling point. butane has more surface area in the liquid phase so more
interactions with surrounding molecules give it a higher boiling point.
7. Both krypton (b.p. –152°C) and
... Get more on HelpWriting.net ...

Separation Of Ionic Molecules Lab Report
In chemistry, an ionic compound is a type of chemical bond where the ions are fixed together via an
ionic bond. An ionic bond is formed when a metal reacts with non–metal; in the reaction, electrons
are transferred from the metal atoms to the non–metal atoms forming negatively and positively
charged ions. The electrostatic attraction, one of the strongest force in the universe which is caused
by electric charges between the positive and negative ions, holds the ionic compounds tightly
together. Consider the reaction between the metal calcium oxide (〖Ca〗^(2+)) and the non–metal
water (H_2 O), which react together to yield the ionic compound calcium hydroxide (Ca(〖OH)〗
_2).
In this reaction, calcium oxide donated its electron which was a negatively ... Show more content on
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Meaning, compounds with the same type of bonding tend to be soluble with one another. Polar
substances would dissolve in polar solvents such as water, however, would not dissolve in non–polar
solvents. Non–polar substances dissolve in non–polar solvents but do not dissolve in polar ones.
Most ionic compounds are able to be dissolved in water as the water molecules hydrate ions. For an
ionic compound to be dissolved, the water molecules must stabilize the ions, which thus would result
in the separation of the ionic bond to form a solution. Water is a polar molecule, it has a permanent
dipole. The oxygen atom has a partial negative charge whilst the hydrogen atom has a partial positive
charge. When an ionic substance is placed in to the water, the water molecules would quickly attract
the charged ions from the substance. They then become free to move about. However, this only
occurs when the attractive forces between the water molecules and ions are stronger than the
attractive forces within the ionic compound. CaOH is a slightly insoluble compound, the solubility of
CaOH is approximately 0.189 g/100 mL of water at 20. A more soluble ionic compounds solubility
such as NaCl is only 35.7 g/100 mL of water at 20°C. CaOH is only slightly insoluble as calcium and
oxygen are +2 and –2 ions in

Types Of Enthalpy Changes In Chemical And Chemical Changes
Enthalpy changes in chemical and physical processes– M1 and D1
By sharing electrons, atoms within a molecule that are attracted to one another is called an
intramolecular force. Between the molecules intermolecular force, the physical properties for
example the melting points and boiling points, relate to the solubility and the strength of these force.
Protons are positive components and electrons are negative components. The attractive force that
exists between the two is known as an intermolecular force due to the atoms and molecules of the
substance. Intermolecular forces have four types:
Ionic forces – This is like the dipole–dipole interaction but it differs slightly as ions are used as well
as polar molecules. ions are held together by electrostatic forces in ionic solids. The charges in an ion
are attracted to each other because they are opposites. "This force is the strongest intermolecular
force." In a crystal lattice structure, the ion forces hold the ions together.
https://www.nature.com/articles/srep35684 Dipole Forces – When a molecule has two poles they are
called dipoles or polar covalent molecules. The molecule will have a partial positive charge on one
pole whilst the other pole will have a different charge that is partially negative. Therefore, the
molecules will rearrange themselves so the charges are attracted to the opposite charge so it works.
Hydrogen Bonds– "when the hydrogen of an electronegative atom of one molecules is attached to an

Ionic Bond: Table Sodium Chloride (Nacl)
Ionic Bond:
Sodium Chloride (NaCl), also referred to as table salt, is an example of an ionic bond (Daempfle,
2016). Its compound includes the positive–charged atom named before the negatively charged atom.
In this case, the element symbol for the metal, sodium chloride is written before the symbol for the
nonmetal (Daempfle, 2016). This is a good example of an ionic bond because it consists of a metal
bonded to a nonmetal and formed between two atoms that have different electronegativity values. As
a result, its ability to attract electrons differs between the atoms.
Overall, sodium chloride molecules form by ionization of sodium and chlorine atoms, and the
attraction of the resulting ions. The ionic relationship occurs because one atom is an anion and the
other is a cation (Daempfle, 2016). In this example, sodium is a cation because it gives one of its
electrons and chlorine is an anion because it takes the electron given by sodium (Daempfle, 2016).
As a result, the molecule loses electrons because the cation becomes positive. As Na then loses an
electron, it becomes oxidized in the ionic formation of the bond (Daempfle, 2016). Next, Cl becomes
reduced because it receives an electron from Na, therefore forming NaCl, table salt.
Non–polar Covalent Bond: ... Show more content on Helpwriting.net ...
The molecule methane has a total of four Carbon–Hydrogen single covalent bonds. These bonds are
non–polar because the electrons shared by the adjacent atoms in the bonds are shared equally.
Because of this equal sharing of electrons, there is no charge separation. As a result, this molecule
cannot enter into a charge interaction with water (Nonpolar Covalent Bonds, n.d.). Overall, Methane
is considered a highly symmetric molecule that is made up of atoms with similar electronegativities
(Nonpolar Covalent Bonds, n.d.). Consequently, methane has an evenly distributed electron cloud
and no regions consisting of a significant

Essay on Ionic and Covalent Bonds Lab
Lab Report
Ionic and Covalent Bonds
Lab: Ionic and Covalent Bonds
Introduction:
The purpose of this experiment was to explore the properties of chemical substances that can be used
to identify the types of bonds in a chemical substance using a laboratory procedure. The two types of
bonds being identified were ionic and covalent. Based on a substance's properties, how can you
determine whether its bonds are ionic or covalent? This is the question I posed before starting the
experiment. An ionic bond is a bond that results from the attraction between oppositely charges ions;
one atom "gives" another atom an electron. Combinations of metals and nonmetals typically form
ionic bonds. A covalent bond is a bond that results from ... Show more content on Helpwriting.net ...
There were no controlled variables used in this experiment.
Materials and Procedure:
Materials
five 25 mL beakers – 5 mL of oil stirring rod – 2 g cornstarch
10 mL graduated cylinder – 2 g sodium chloride spoon – 2 g sodium bicarbonate conductivity
apparatus distilled water in a wash bottle
Lab Procedure
Step 1: Gather materials.
***Repeat steps 2–4 for each of the following: 5 mL of oil and 2 g each of cornstarch, sodium
chloride, and sodium bicarbonate.
Step 2: Note State and Appearance.
a) Put the substance in a 25 mL beaker.
b) Observe and record data in the data table on its state of matter, appearance, and texture and
whether it has a crystalline structure.
Step 3: Determine Solubility in Water.
a) Add distilled water to the beaker until the volume totals 15 mL.
b) Use the stirring rod to stir for 3 minutes.
c) Record the amount of substance that dissolved – all, some, a little, or none.
Step 4: Determine Conductivity.

a) Prepare the conductivity apparatus. The electricity should be turned off.
b) Spray a small amount of distilled water on the electrical leads of the conductivity apparatus. Insert
the electrical leads of the conductivity apparatus into the beaker.
c) Turn on the electricity. Record whether you observe conductivity.
d) Turn off electricity. Clean the electrical leads with soap and

Chemical Bonds Are An Attraction Between Two Or More Atoms
Chemical Bonds are an attraction between two or more atoms that occur because of an attraction or
force that occurs between the two. Three forms of chemical bonding exist, Ionic and covalent
bonding. In addition, polarity is the electronegativity of two atoms being transferred along the bond.
Some forms of polarity that exist are hydrogen bonds, interstitial forces and vanderwaals reactions.
In the realm of chemical bonding, the strongest form of bonding is covalent bonding. Covalent
bonding is a form of chemical bonding in which two or more atoms share their electrons with each
other for the sake of forming a close centered strong bond. This form of bonding is very important in
that it helps form bonds that are very hard to break to form ... Show more content on Helpwriting.net
...
The other form of bonding is nonpolar covalent bonding in which two atoms, usually the same ones,
bond and create a bond with less than 1 electronegativity difference. This difference is due to the
electron amount in each atom being either very similar or the size of the atom being very similar.
Some examples of non–polar bonds are H2, I2 and Cl2.
The next form of bonding is Ionic bonding. Ionic bonds are bonds formed when a nonmetal and a
metal come together to form a bond where the electrons are transferred. By transferred, it is meant
that the electrons are sent from the molecule with the less electrons to the molecule with the higher
amount in order to fill its octet. Here, both molecules have their octets filled when the atom with the
smaller amount of electrons loses the extra electrons it has and goes to the lower shell where its octet
becomes full. On the other hand, the atom with the larger amount of electrons has its octet filled
when the atom receives the needed electrons to fill its octet. This creates a bond between the two
atoms and leaves them in a state of ionic bonding. Ionic bonding is characterized by atoms with
extremely high boiling points and very low freezing points. Most ionic bonds form salts, such as the
common table salt known as NaCl. In addition, ionic bonds almost always form molecules that easily
dissociate in water. By dissociating in water, it is meant they separate

Physical Properties and Reactions of Period 3 Oxides
PHYSICAL PROPERTIES OF THE PERIOD 3 OXIDES
These pages explain the relationship between the physical properties of the oxides of Period 3
elements (sodium to chlorine) and their structures. Argon is obviously omitted because it doesn't
form an oxide.
A quick summary of the trends
The oxides
The oxides we'll be looking at are:
|Na2O |MgO |Al2O3 |SiO2 |P4O10 |SO3 |Cl2O7 |
| | | | |P4O6 |SO2 |Cl2O |
Those oxides in the top row are known as the highest oxides of the various elements. These are the
oxides where the Period 3 elements are in their highest oxidation states. In these oxides, all the outer
electrons in the Period 3 element are ... Show more content on Helpwriting.net ...
What you can safely say is that because the metallic oxides and silicon dioxide have giant structures,
the melting and boiling points are all high.
Electrical conductivity
Silicon dioxide doesn't have any mobile electrons or ions – so it doesn't conduct electricity either as a
solid or a liquid.
The molecular oxides
Phosphorus, sulphur and chlorine all form oxides which consist of molecules. Some of these
molecules are fairly simple – others are polymeric. We are just going to look at some of the simple
ones.
Melting and boiling points of these oxides will be much lower than those of the metal oxides or
silicon dioxide. The intermolecular forces holding one molecule to its neighbors' will be van der
Waals dispersion forces or dipole–dipole interactions. The strength of these will vary depending on
the size of the molecules.
None of these oxides conducts electricity either as solids or as liquids. None of them contains ions or
free electrons.
The phosphorus oxides
Phosphorus has two common oxides, phosphorus (III) oxide, P4O6, and phosphorus (V) oxide,
P4O10.
Phosphorus (III) oxide (tetraphosphorus hexoxide)
Phosphorus (III) oxide is a white solid, melting at 24°C and boiling at 173°C.
The phosphorus is using only three of its outer electrons (the 3 unpaired p electrons) to form bonds
with the oxygens.

Phosphorus (V) oxide (tetraphosphorus decoxide)
Phosphorus (V) oxide is also a white solid, subliming (turning straight

Categorization Of Intriguing Compounds Lab Report
The Categorization of Intriguing Substances An ionic compound is the electrostatic attraction
between protons and electrons that are transferred between two atoms. Ionic bonds occur with a
metal and a nonmetal atom. Metals lose electrons to create cations, while nonmetals gain electrons to
make anions. Covalent compounds occur only in nonmetals, which is characterized by the sharing of
pairs of electrons between atoms and other covalent bonds. Additionally, the melting and boiling
point of ionic bonds are high, whereas covalent bonds are low. Since electrons and ions are shared in
covalent compounds, it lacks moving electrons or ions. Therefore, electricity cannot be conducted;
on the other hand, ionic compounds move freely and will have ... Show more content on
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On the other hand, covalent compounds may take the form of either solid, liquid, or gas; moreover,
they are loose and molecular. Once the ions are dissolved, the presence of charged particles
distributed throughout the liquid allows the solution to conduct electricity. Therefore, ionic
compounds have higher melting and boiling points compared to covalent compounds. Similarly,
ionic compounds dissolved in water make an electrically conductive solution, which are able to
move freely through the solution carrying the charge and conducts an electric current.
Correspondingly, covalent compounds do not exhibit any electrical conductivity in either pure form
or when it is dissolved in water. Thus, ionic compounds dissolve in water and have higher melting
and boiling

Two Types of Solids
March 2, 2011
Lab Report
Physical Properties of Two Types of Solids
SCH3U0
Maggie Liu
Abstract
The purpose of this lab is to study some of the physical properties of two types of solids – ionic and
molecular. The samples used are sodium chloride (ionic) and camphor (molecular). The physical
properties studied are odour, hardness, melting point, solubility in water and solubility in 2–
propanol. It is observed that some of the physical properties of sodium chloride are no odours, hard,
a high melting point, soluble in water and insoluble in 2–propanol; some of the physical properties of
camphor are a strong odour, soft, a low melting point, insoluble in water and soluble in 2–propanol.
A few conclusions can be drawn from these ... Show more content on Helpwriting.net ...
Noted the observations for each solid in both water and 2–propanol.
Observations
|Physical property |Sodium chloride |camphor |
|Odour |No odour |Strong (mint) |
|Hardness |hard |soft |
|Melting point |high |low |
|Solubility in water |soluble |insoluble |
|Solubility in 2–propanol |insoluble |soluble |
Sodium chloride does not have any odours, whereas camphor has a strong mint–like smell. It is
found that ionic compounds usually do not have odours because they are solids and the particles are
all held tightly which makes the gas nearly impossible to be released into air and make the smell,
however, many molecular solids do have odours because their particles are not held very tightly and
there is space between the particles. Vapor or gas can be produced and released into air which causes
smell. Sodium chloride is harder than camphor.

Chem Lab Project 2 Essay
Investigating the Determining Characteristics of Cations and Anions
Chem 111 Sec 560
Introduction: The purpose of this lab was to study the specific characteristics of cations and anions,
and ultimately to be able to identify an unknown substance based on our studies and tests using the
logic trees developed through the experiment. A logic tree is a graphical display of the findings from
this lab which, through a series of yes/no questions, elimination tests, will help us to identify and
unknown sample. This lab will result in 2 logic trees, one for identifying cations and the other,
anions.
The lab was broken into three parts: Part 1 dealt with identifying a cation, Part 2 an ... Show more
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The resulting color flashes were recorded. The cation solutions were then disposed of in the
appropriate waste containers.
From the information in each of these tests, a Cation logic tree was formed for easy identification of
unknown cations.
Part 2: Anion Analysis: The experiment was performed on 4 anions: chloride (Cl
), sulfate (SO42
),
nitrate (NO3
), and carbonate (CO32
). A sample of each anion was prepared by placing 10 drops of
each anion solution into a centrifuge tube. The tubes were labeled accordingly. The original color of
the solution was recorded. The first test performed was an Anion Elimination Test, the Silver Nitrate
Test. 0.1 M AgNO3 was added dropwise to each tube until a precipitate was formed or 5 drops of 0.1
M AgNO3 were administered. First, 2 drops of 0.1 M AgNO3 was added to the tube containing Cl
‐
and the results recorded, noting the appearance (texture), color, and shape. This process was repeated
for all the anions as follows: SO42: 20 drops, NO3
: 20 drops, CO32
: 1 drop of 0.1 M AgNO3 was
added.
For each solution which formed a precipitate (Cl
,CO32
) the solution was centrifuged for 5 minutes
and the supernatant was decanted; 5 drops of distilled water were added to both

Ap Bio Work Essay
AP BIOLOGY PAK 1 HOMEWORK
Name: Jeremy Ng
Per:
3
Adv: Mr.Lee
Chapter 1: Introduction: Themes in the Study of Life
Begin your study of biology this year by reading Chapter 1. It will serve as a reminder about
biological concepts that you may have learned in an earlier course and give you an overview of what
you will study this year.
VOCABULARY– Should be completed in your notebook to be kept along with any notes taken for
the chapter.
eukaryotic cell genome prokaryotic cell negative feedback
DNA positive feedback
genes data 1. In the overview, Figure 1.3 recalls many of the properties of life. Label the seven
properties illustrated here, and give a different example of each.
Enter answer here
Evolutionary ... Show more content on Helpwriting.net ...
16. The text points out a common misconception about the term "controlled experiment". In the
snake mimicry experiment, what factors were held constant?
17. Explain what is meant by a scientific theory by giving the three ways your text separates a theory
from a hypothesis or mere speculation.
1.
__________________________________________________________________________________
2.
__________________________________________________________________________________
3.
__________________________________________________________________________________
Chapter 2: The Chemical Context of Life

This chapter covers the basics that you may have learned in your chemistry class. The questions that
follow should help you focus on the most important points.
VOCABULARY– Should be completed in your notebook to be kept along with any notes taken for
the chapter.
matter element trace element neutron atomic number atomic mass energy molecule polar covalent
bond anion van der Waals interactions
compound proton isotope electronegativity cation dynamic equilibrium
essential element electron electron shells nonpolar covalent bond hydrogen bond
Concept 2.1 Matter consists of chemical elements in pure form and in combinations called
compounds
1. What four elements make up 96% of all living matter?
_________________________________________
Concept 2.2 An element's properties depend on the structure of its atoms
2.

Cation and Amnion Lab Essay
Name: Lisa Brewer iLab, Week # 2 CATIONS AND ANION LAB Introduction The purpose of this
week's lab is to learn to demonstrate a double–replacement reaction of ionic compounds. To
accomplish this, two ionic compounds will be mixed together and the product will precipitate out of
solution. In this procedure, the product must be precipitated out of the solution and then weighed.
For this lab, lead (II) nitrate (Pb(NO3)2) and potassium chromate (K2CrO4) will be reacted together
to demonstrate double replacement reaction between 2 ionic compounds. This was shown when
chromate replaced the nitrate and formed lead (II) chromate, and when the nitrate replaced the
chromate and formed potassium nitrate, which is shown in the ... Show more content on
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This indicates a reaction occurred and precipitate has formed and settled on the bottom of the beaker.
Set up the Erlenmeyer flask with a Buchner funnel. Select equipment from toolbar, then from the
dropdown menu, select Erlenmeyer flask–250mL. Right click the Erlenmeyer flask, choose Buchner
funnel. The Buchner funnel will be added to your Erlenmeyer flask. Select the 100mL beaker and
right click on Pour/Decant. The flask will turn on its side so that you can move the beaker above the
Buchner funnel. The solution will pour into the funnel when positioned correctly. Note: When the
solution has been filtered, a white area will appear on the bottom of the flask. Right click the flask.
Select Buchner funnel. Message window appears with question. Select place solid into 50mL Test
tube. Click OK. Note: a test tube will appear with a small amount of precipitate on the bottom. To
measure the weight of the precipitate, right click the test tube. Select show weight. The weight of the
precipitate will appear below the test tube. Record this information in the Observations and Results
section of the lab report, including the weight and appearance of the precipitate. Observations and
Results The appearance of the precipitate was shown several ways during the experiment. In the
100mL beaker, after both chemicals were added, it was shown as a dotted solution. It was then
shown as a solid and a white color in

Ionic Bonds, Covalent Bonds, and Polymers
Ionic Bonds, Covalent Bonds, and Polymers An attraction between atoms that allows chemical
substances to form is commonly referred to as a chemical bond. Two of the most common types of
chemical bonds are ionic bonds and covalent bonds. Both ionic and covalent bonds can be mixed
together in order to form mixtures and compounds. While the two types of chemical bonds have
several similarities, they are also vastly different. Ionic and covalent bonds are formed when two or
more elements bond together. There are 117 elements known to date. An element is defined as a
substance that is made up of a single atom. While 94 of these elements are naturally occurring, 22 of
these elements are artificial. A complete list of elements can be found on the periodic table of the
elements, arranged by atomic number and by chemical property. When substances are formed
through ionic or covalent bonding, they can be combined with other substances to form mixtures or
compounds. A compound is a pure substance that is made up of two or more substances. A
compound is a homogenous mixture that requires all elements comprising the mixture to be present
in fixed proportions. When elements are combined to make a compound, they do not retain their
individual properties. Furthermore, in order to separate a compound into its individual elemental
components, a large amount of energy must be used. Compounds form naturally and have elemental
stability; stability depends on the number of electrons that

Ionic Bond Lab
Ionic bonds form by the nature of the atoms themselves. When the atoms chemically combine
together, the atoms create a compound that has different properties. The electronegativity between
the atoms in the bond determines what type it is. Atoms with higher electronegativity hold atoms
more tightly than those with a lower electronegativity. Therefore, when two elements bond, they
must fill each others orbitals to create a stable energy electron configuration. Each will have eight
electrons in their outer energy. The solubility and bond type lab was to use the compounds solubility
to predict the type of bond it contains. To determine so, I added sodium chloride to water in a test
tube and some of it dissolved. When the sodium chloride was put ... Show more content on
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"Stoichiometry." Encyclopedia of Physical Science. Science Online,
online.infobase.com/HRC/Search/Details/8?
articleId=299090&q=Balanced%20chemical%20equation. Accessed 6 May 2018.
Manning, Phillip. "Ionic Bonds." Chemical Bonds, Chelsea House, 2015. Science Online,
online.infobase.com/HRC/Search/Details/8?
articleId=368723&q=How%20Do%20ionic%20compounds%20form%3F. Accessed 2 May 2018.
Moscher, Karl F. "Molecular Modeling." Encyclopedia of Chemistry. Revised Edition. Science
Online, online.infobase.com/HRC/Search/Details/8?
articleId=299674&q=Models%20of%20Molecular%20Compounds. Accessed 3 May

Ionic and Covalent Bonding Essay
Ionic and Covalent Bonding
Ionic and covalent bonding is involved when the atoms of an element chemically combine to make
their outer shells full and to make the atoms stable.
The first type of bonding you can get is ionic bonding. Electrons are transferred from one atom to
another to try and create full outer shells, this gain and loss of electrons on the atoms results in
positive and negative ions. In these compounds you get electrostatic force, this is the force/attraction
that occurs between the positive and negative ions that hold the compound together. This type of
bonding takes place between metals and non–metals. The metals lose electrons and form cations,
whereas the non–metals gain ... Show more content on Helpwriting.net ...
As the size of the negative ion and the charge on the positive ion both increase and the size of the
positive ions decrease, the polarisation effect increases. This polar ionic bonding gives many of the
atoms covalent characters. Sometimes one of the atoms become so highly polarised that they share
the electrons and therefore can create covalent bonds.
Covalent bonding takes place where two atoms have a single, unpaired electron in an atomic orbital;
these orbitals will therefore overlap so that the two atoms are sharing a pair of electrons. The
attraction that holds the atoms together is the force between the electron and the nuclei in each of the
atoms. Before the atoms are bonded, the single, non–bonded pairs of electrons are called lone pairs
of electrons. When the atoms combine by means of covalent bonding they form molecules.
Simple covalent compounds consist of many small molecules. The covalent bonds within the
molecules are strong but the bondings between them to form the compounds are relatively weak, the
force that occurs between them is called the intermolecular force. It takes very little energy to break
these forces; therefore simple covalent compounds have very low melting points and generally
appear as gases.
You can also get multiple bonds; this is where atoms can share more than 2

Electrolytes: Ionic Bond and Sodium Chloride Essay
Week #2 Post Lab
1.) Define the following: electrolyte, nonelectrolyte
Electrolyte: A substance that dissolves in water to form solutions that conduct electricity.
Nonelectrolyte: A compound that doesn't dissociate into ions when dissolved in water.
2.) Using examples in the last link, draw beakers showing atomic scale representations of aqueous
solutions of the following compounds. Classify each as an electrolyte or nonelectrolyte. * Ba(OH)2
(aq)
* NH3 (aq)
* C3H7OH (aq)
* NaHCO3 (aq)
3.) Why would it be important to use de–ionized water when preparing the aqueous solutions in this
experiment?
It is important to use de–ionized water in this experiment because you don't want the electrolytes in
the water to ... Show more content on Helpwriting.net ...
7) Although water is a poor conductor of electricity, we are cautioned not to operate electrical
appliances around water. Why?
Water itself does not conduct electricity very efficiently, but contains trace elements (i.e. sodium)
that do contain electrolytes.
Week 2: Bright Ideas
1) Evidence: What is the evidence that leads to a claim?
This section focuses on the analysis of your data. Draw a copy of the flow chart you made in class
and attach it to your post laboratory assignments. 2) Claim: Based on the data, what is the answer to
the key question?
Write a sentence or two that answers the key question based on the evidence (it does not have to be
the "right answer" to get full credit but it does have to be supported by the data).
The reason the light bulb would light up was because of the strong electrolytes in the ionic bonds.
During the experiment, it was mostly the ionic compounds that were lighting up the light bulb while
the covalent compounds did not.

3) Reading: How do the ideas developed in the lab compare with other scientist' ideas? Start by
reading pgs 2–5 given to you in class as well one other source containing related information (like a
textbook or educational internet site). How does the flow chart you made during the experiment
compare and contrast to the flow chart on pg 5? The flow chart on page 5 was more in–depth than
mine. The chart

Task 1a Periodic Table Essay
TASK 1A Periodic table essay
Also you should organise into F blocks and S, P, D blocks.
Which groups and blocks belong too?
NA– Sodium
K– Potassium
CA– Calcium
MG– Magnesium
C– Carbon
O– Oxygen
N– Nitrogen
F– Fluorine
CL– Chorine
FE– Iron
H– Hydrogen
S– Sulphur
Groups
Group 1= Alkali metals
Group 2= Alkaline earth metals
Transition metals
Group 3 = Boron family
Group 4= Carbon family
Group 5= Nitrogen family
Group 6= Oxygen family
Group 7= Halogen family
Group 8= Noble gases
Rare earth materials
Some earth materials are radioactive. The earths that are rare are silvery white. Thirty rare earth
elements are unmoved in the actinide and lanthanide series. In the lanthanide series the one element
is the most of the elements in ... Show more content on Helpwriting.net ...
Families/ Groups
Columns of elements are called families or groups. Elements in the family have similar that are not
identical properties. For example, Lithium (LI) Sodium (NA), Potassium (K), and some other
members of group's family are soft with white shiny metals. The elements in the family have the
same amount of numbers of outer electrons.
Each horizontal row of the elements is called a period. The elements in the period are not like in

properties. In fact, the properties change greatly across even given row (periodicity). The first
element in the period is always an extremely solid that is active. The last element in the period is
always an inactive gas. Each new period will represent the next shell fall of electrons which will fill
the period.
Hydrogen group
Hydrogen rests at the summit of group yet it is not a representative of that family. Hydrogen is inside
a category of its own. Gas at free space temperature.
Alkali metals group 1
Never found while complimentary component within mature– repeatedly joined with another
section. 1 outer electron stability of clay, simply shaped with a knife. Conduct electricity. The most
reactive metals. They proceed dangerously with water. While you progress throughout the group
huge atoms (since there's only full shell. Outside for each row2 this is more react line although the
outer electron is further simply lost while it's further away from the cell. Higher thickness since the
atoms possess of

Research Paper On Benaldehyde
(4) Component Name: Benzaldehyde, Cherry flavoring/odor; C7H6O; 106.12g/mol–1
(5) Systematic Name: A) Bitter almond; B) Benzenecarbaldehyde; C) Phenylmethanal
(6) Structural Formula: General Description:
(7) Benzaldehyde is a compound since it contains of more than one element in its molecular formula.
(8) Benzaldehyde contains Covalent bonds and Polar Covalent bonds.
(9) Benzaldehyde is an Amino Acid and nucleotide. These are typically used as a Sodium or Calcium
Salt.
(10) Purpose: Benzaldehyde Flavoring is used when its difficulty taking a medication due to taste,
unable to swallow a capsule or battling a chronic illness; often, sweet flavors can become
unbearable, or bitter flavors' may cause nausea. In these instances, ... Show more content on
Helpwriting.net ...
(8) Purified water contains Covalent bonds and Polar Covalent bonds.
(9) Purified water is not an Acid, Base or Salt; it is just a regular compound.
(10) Purpose: Purified water has many uses, largely in the production of medications, in
Science and engineering laboratories and industries. Purified water is suitable for applications
including: autoclaves, hand–pieces, laboratory testing, laser cutting and automotive use. Large
productions are in the pharmaceutical industry. Water of this grade is widely used as a raw material,
ingredient, and solvent in the processing, formulation, and manufacture of pharmaceutical products.
(11) References:
(A) https://en.mwikipedia.org/wiki/Water
(B) https://pubchem.ncbi.nlm.nih.gov/compound/962
(4) Component Name: Sodium benzoate; C7H5O2Na; 144.11g/mol
(5) Systematic Name: A) Benzoic acid; B) sodium salt; and C) Sobenate
(6) Structural Formula: General Description:
(7) Sodium benzoate is a compound since it contains of more than one element in its molecular
formula.
(8) Sodium benzoate contains Ionic bonds, Covalent bonds and Polar Covalent

Ionic Compounds Lab Report
Background Ionic compounds and covalent compounds have many similarities and differences. Ionic
compounds are only formed with metals and non–metals. Covalent compounds are formed with non–
metals. Ionic compounds have an overall neutral charge, but covalent compounds don't have charge.
Ionic compounds are formed when non–metals take electrons from metals. This gives both of them
noble gas configuration. Covalent compounds are formed by two non–metals sharing their unpaired
electrons, so they can mutually have noble gas configuration. What properties do compounds form
when forming ionic and covalent bonds? Procedure The compounds are placed in a tray. Tin foil was
fit into an empty tray to make the same shape. The compounds were placed into the tinfoil tray with
a scoopula. The tinfoil tray was placed over the metal tray, which was positioned over the bunsen
burner. A timer was then started to time how long it took each compound to start melting. DI water
was then placed into a plastic tray. Each compound was placed into different holes, and stirred to test
its ... Show more content on Helpwriting.net ...
Salicylic acid, sucrose, paraffin, and sodium stearate are all covalent compounds. The ionic
compounds, on average, took much longer to melt than the covalent compounds did. For example,
sodium chloride did not melt at all, but paraffin melted, on average, in 28 seconds. The ionic
compounds also were more likely to dissolve in the water than the covalent compounds. Sodium
carbonate dissolved in the water, but the salicylic acid did not. The ionic compounds also were more
likely to conduct energy than the covalent compounds. Sodium bicarbonate conducted some
electricity, but sucrose did not. Some exceptions were calcium carbonate, which did not dissolve or
conduct electricity, sodium bicarbonate and copper (II) sulfate, which both melted, and copper (II)
sulfate which did not conduct

Chemistry Solubility
Jacinta Houng
Comparing the Solubility of Chemicals in Water
"Water is known as the "universal solvent" because so many different substances dissolve in it and
we rely on this for many of our daily needs."
Introduction: Water is known as the 'universal solvent' as it is capable of dissolving a variety of
different substances and dissolves more substances than any other liquid. However the ability to be
soluble depends on a substances polarity and bonding. This then contributes to the various ways that
different types of chemicals interact in water.
Solubility is crucial to every living thing on earth as water can carry along valuable chemicals,
minerals, and nutrients necessary for survival. In fact Water covers 70% of the Earths ... Show more
content on Helpwriting.net ...
However despite its name as the "universal solvent" there are many compounds that won't dissolve
or won't dissolve well in water. If the attraction is high between the opposite–charged ions in a
compound, then the solubility will be low. For example, most hydroxides exhibit low solubility in
water.
Polar molecule: H2O
Polar molecule: H2O
Aim: To investigate and compare the solubility of household chemicals in water to demonstrate the
various ways that the different types of chemicals interact in water.
Hypothesis: Substances with stronger bonds such as ionic bonds will have a low solubility whereas
substances with weaker bonds like covalent bonds will be highly soluble. Therefore sugar will have
the highest solubility followed by citric acid and then salt.
Materials: * Citric Acid * Salt * White Sugar * 600ml of water * 1 Thermometer * 1 Stirrer * 1
tablespoon * 3 transparent cups * 1 Measuring jug * Pen * Paper
Risk Assessment: A common laboratory risk is the handling of glass items. Items such as
thermometers and glass cups carry the risk of breakage, cuts and mercury poisoning. Ways to
minimize and handle this risk include: * Inspect glassware for defects or cracks before use. * Do not
handle broken glass with bare hands. Use appropriate cut–resistant gloves to handle broken glass. *
Use forceps, tongs, scoops, or other mechanical devices for removing

Atom And The Atoms Of Atoms
An atom is contained of a nucleus holding positively charged protons and neutrally charged
neutrons. Surrounding the nucleus of an atom are negatively charged electrons. In a neutral atom, the
number of electrons and protons are the same. However, the solidity of an atom, is the tendency for
the atom to gain or lose electrons, is directly proportional to the number of electrons located on the
valence of the atom, the outermost part of the shell. The stability of the electrons determines the
physical properties of a particular compound and can be used to determine if the bone is either an
ionic or covalent bond.
Introduction
The stability of an atom is determined by the number of electrons located on the valence (or outer
shell) of the atom. Electrons are located looping the nucleus in shells. The number and size of each
shell are determined by the number of electrons in an atom. The smaller shells are filled up first,
followed by the next shell. The number of electrons allowed in each shell are as followed: two
electrons in the first shell, eight electrons in the second shell, and 18 electrons in the third shell.
Some elements are more reactive than others varying on the number of electrons positioned on the
valence shell of the atoms involved. Atoms will attempt to create a full valence shell by either losing
excess electrons or by gaining the necessary electrons required to fill the atoms valence shell. This is
how ions are created.
An ion is an atom

Instructional Purpose : Venn Diagram
Instructional Purpose – Venn Diagram – Post Reading Strategy Instructional Purpose: The overall
goal of this activity is to provide the students with a diagram that can help them learn and memorize
the different characteristics associated with chemical bonding. If students have difficulties
differentiating the characteristics associated with covalent and ionic bonding, they will suffer with
future topics and other branches of chemistry. Ionic bonding is a crucial topic to understand within
general chemistry reactions. Covalent bonding is a root within Organic and Biochemistry that needs
to be understood in order to fully understand the theories and concepts discussed in both forms of
chemistry. What content in the reading may be used to ... Show more content on Helpwriting.net ...
Content Area Lesson Plan – Venn Diagram – Post Reading Strategy Introduction: Good morning
class! Yesterday we finished reading the section on chemical bonding. It is important that you all
understand the differences between the two major types of bonding, which are covalent and ionic
bonding. Both forms have specific characteristics that are important to memorize for future topics we
shall discuss in this class and in your college courses. In my opinion, the best way to learn and
memorize different characteristics between two different things is by completing a Venn Diagram.
Explain the Strategy: Most of you have completed many of these throughout your schooling
experience, but I shall provide you a nice refreshing reminder of how a Venn Diagram works. Start
by drawing two large circles, and the circles must overlap at the middle. This middle zone will
represent the characteristics that relate to both items being examined. Then the remaining zones will
contain characteristics that are associated with the term listed above. This creates a clean diagram
that makes studying easier because the characteristics are clearly separated, easy to read, and
associate with the term that is listed above. Model the Strategy: Now let me provide you all an
example of a Venn Diagram. I want to create a diagram between NASCAR and stock car racing. I
tend to start at the similarities when completing a Venn Diagram. Both are a form of racing, so I

What Happens When Glucose And Maltose Are Classified As...
1. If the pH of a solution is decreased from 7 to 6, it means the concentration of
a. H+ has decreased to 1/10 of what is was at pH 7
b. H+ has increased 10 times what it was at pH 7
c. OH– has increased 10 times what it was at pH 7
d. OH– has increased by 1/7 of what is was
2. The hydrogen bonds shown in this figure are each between
a. Two hydrogen atoms
b. Two oxygen atoms
c. An oxygen and a hydrogen atom of the same water molecule
d. An oxygen and a hydrogen atom of different water molecules
e. Between the atoms in each individual water molecule
3. How are amino acids attached together?
a. Between amino groups via dehydration synthesis
b. Between amino group and carboxylic acid group via dehydration synthesis
c. Between amino groups via ... Show more content on Helpwriting.net ...
Specific enzymes break down proteins into amino acids.
b. Specific hormones break down proteins into simple sugars.
c. Specific hormones break down proteins into complex sugars.
d. Specific enzymes break down proteins into simple sugars.
5. Which enzyme shows the greatest change in its rate of action with the least change in pH? 6.
Glucose and maltose are classified as organic compounds because they are both
a. Carbon– containing substances
b. Composed of simple elements
c. Waste products
d. Artificial sugars
7. The graph below shows the effect of temperature on relative rate of action of enzyme X on a
protein. Which change would not affect the relative rate of action of enzyme X?
a. An addition of cold water when the reaction is at 50 degrees Celsius
b. An increase in temperature from 70 to 80 degrees Celsius
c. The removal of the protein when the reaction is at 30 degrees Celsius
d. A decrease in temperature from 40 degrees Celsius to 10 degrees Celsius
8. The process represented by the equation show is known as a. Fermentation
b. Hydrolysis
c. Aerobic oxidation

d. Dehydration synthesis
9. The structural formula shown represents urea. This structural formula indicates that urea is: a. An
organic

Chelation Therapy Research Paper
Is Chelation Therapy Right For You
Scientists believe that our body often contains microscopic pieces of heavy metal such as mercury,
lead or even straightener. While generally disregarded by traditional medicine, these traces of
pollutants in our bodies could cause or irritate health conditions including heart disease and cancer.
Chelation therapy is any non–surgical treatment that is considered to purge these poisonous metals
from the physique. In this article, we'll inform you of that metal detoxification works and how it can
get a lean body. Chelation therapy is the supervision of chelating agents to get rid of heavy metals
from the entire body. This metal detoxing can be done intravenously, intramuscularly or by mouth.
Alternative ... Show more content on Helpwriting.net ...
This treatment is also widely used for your treatment of chronic degenerative ailments involving the
circulatory program. The chelation halts unhealthy effects and triggers the body's healing process,
usually reversing the damage. Numerous patients who could not walk due to muscle mass pain or
angina soreness have reported that they can walk without pain following this treatment. The
chemical EDTA is actually mixed with vitamins and minerals and it is administered by a great
intravenous drip over a period of three hours. EDTA binds with and removes, through the kidneys,
toxic metals such as direct, aluminum, cadmium, arsenic, tin, and also excess iron and also copper.
These heavy metals bring about the formation of free–radicals which are a major reason behind
degenerative illnesses including heart and blood vessel disease. The EDTA is eliminated from the
body, 95 per cent via the renal system and 5 % via the bile, along with the poisonous metals and free
ionic calcium which it provides locked onto, in its transit through the circulatory system. There have
been several side effects associated with chelation therapy. One of the most common problems of
this metal as well as

Metal-Only Lewis Pairs with Transition Metal Lewis Basas
Metal–Only Lewis Pairs with Transition Metal Lewis Basas
Introduction:
History of Metal–Metal Dative Bonding Concept In 1961, Vaska and Diluzio synthesized a lemon–
yellow compound known as the organometallic complex trans–[IrCl(CO)(PPh3)2]. This was
achieved by reducing iridium(III) to iridium(I) using just triphenylphosphine and an alcohol. This
was significant because they had prepared an iridium carbonyl complex without the use of carbon
monoxide. This complex has reversible dioxygen coordination, but more importantly, it is extremely
reactive with acids, halides, and dihydrogen yielding stable Ir(III) addition products. The discovery
of this Iridium complex meant that laboratories across the globe could now easily create, in one step
and several hours, an air–stable compound that could undergo oxidative addition reactions. Also, the
reaction could be monitored by watching the carbonyl C–O stretching band in the IR spectrum and
NMR spectroscopy later on. Because Vaska's complex was so stable, its reactivity was limited. The
complex serves as an excellent molecular platform for defining how oxidative addition reactions
make homo– and heterogeneous catalysis a reality. While the term "oxidative addition is a staple in
inorganic chemistry and catalysis, the step transition metal Lewis basicity is almost never seen.
There are numerous methods that a metal can cleave an element–element bond, from concerted,
side–on cleavage to backside attack. Most oxidative addition

Evaluation of the Gas Law Constant Essay
Vanessa Gale
Formal Lab:
Evaluation of the Gas Law Constant
Dr. Monzyk
Due 06/25/2012
Purpose:
The purpose of this lab is to evaluate the gas law constant. The ideal gas law is represented as
PV=nRT, where R represents the gas law constant. To determine R, we must find the other
parameters, P, V, n and T through the experiment.
Equipment and Materials:
Large beaker
Ring stand
Clamp
Copper wire
100 mL eudiometer tube
Magnesium (Mg) ribbon
M6 H2SO4 (Sulfuric Acid)
Wash bottle filled with distilled water
Procedure:
First I cut a piece of Mg ribbon and used steel wool to rub off the MgO (magnesium oxide). I then
used the scale to determine when I had approximately 0.0440g of Mg. I then wrapped the Mg with ...
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Water vapor and magnesium oxide on the surface of the magnesium ribbon can cause error in this
experiment. 2. A) R would increase if the liquid level in the tube is lower than the level in the beaker.
B) R would decrease if there was magnesium oxide on the magnesium ribbon because it would
generate less H2.
C) R would decrease if the H2 escapes the beaker because there

Identifying Covalent, Ionic And Hydrogen Bonds
After completing the lab, we will be able to identify covalent, ionic, and hydrogen bonds. Hydrogen
bonds are the weakest between all the three types of bonds we will be observing and it occurs
between hydrogen and oxygen atom or nitrogen atom; hydrogen bonds are a type of dipole–dipole
bond. A dipole–dipole interaction occurs because of polar molecules. We should know that the bond
between hydrogen and oxygen in a water molecule is covalent. Another example, of covalent bond is
the bond between all the atoms that compose ethane. Another objective that we will observe is
solubility, the lab mentions. An example, of an ionic bond is NaCl, this is an ionic bond because the
Na+ and Cl–, the sodium atom (cation) gives a pair of electrons to the ... Show more content on
Helpwriting.net ...
A water molecule is able to interact with up to four other water molecules to create a tetrahedral. The
second part of the lab, we will be observing cohesion and adhesion theories. Cohesion is when water
molecules stick to each other and adhesion is the occurrence of water molecules sticking to other
molecules. To observe adhesion and cohesion, we will pipette a drop of water on a piece of parafilm;
we will be looking for if they water will be stuck together or did it spread apart, we will be
explaining our observations. We will then, repeat the same experiment, however instead of parafilm
we will use a glass slide; we will try to compare cohesion between the water molecules and the
adhesion between the water and glass slide. After, we are done pipetting the water and observing, we
will then demonstrate what happened in the pipette part (both the parafilm and the glass slide) of the
experiment using the 12 water molecules and the non–magnetic tray. The third part of the experiment
consists of testing

Ionic Compounds And Molecular Compounds
Introduction: Ionic compounds and molecular compounds are very different. These differences can
be used to distinguish one from another by using the main properties for each compound. For
example, if a substance could not conduct electricity and had low melting points, it would be labeled
as a molecular compound since those properties correspond directly with the properties of a
molecular compound. If a substance was able to conduct electricity and had high melting points, it
would be labeled as a ionic compound because those properties correspond directly with the
properties of an ionic compound. The differences in whether a substance has the ability to conduct
electricity or not and whether it has high or low melting temperatures can be ... Show more content
on Helpwriting.net ...
Covalent compounds are the opposite. Instead, covalent bonds can melt very fast under heat. Also,
covalent compounds are not good conductors of electricity, whether in solid or liquid form. If you
have a substance, you can verify whether its an ionic compound or a covalent compound by seeing
whether it's a metal nonmetal relationship or nonmetal nonmetal relationship. The objective of the
experiment is to find out which of the known substances were ionic compounds and which were
molecular compounds based on their properties. We predict that the compounds with high melting
points and conduction of electricity would be ionic compounds because those are the specific
properties of an ionic compound. The compounds with low melting points and no conduction of
electricity would be covalent compounds because those are the specific properties of a covalent
compound. The solubility of the six compounds were checked when each compound was mixed in
water and the conductivity of electricity was tested with the electrodes. High and low melting points
were tested by putting different substances above a flame and seeing how long it took to melt. It was
found that three mystery compounds were ionic compounds while the other three mystery
compounds were molecular compounds. Materials and Methods : Before the experiment was
initiated, qualitative observations were taken for all six mystery compounds and recorded. Necessary
precautions like wearing safety

Lab 04
Student Name: Melissa Tatum
Student ID: 4593119
Date: 7 Dec 2014
Course and Section Number: SCIN131 A004 Fall 14
Lesson 4 Lab: Chromatography and Ionic versus Covalent Bonds
PART 1
Begin by viewing the following Thinkwell video
15.1.3 CIA Demonstration: Chromatography
After you watch the above video, answer the questions below in sufficient detail:
(a) (3 pts.) This video discusses 3 different types of chromatography. List each one mentioned, and
describe their differences in as much detail as possible (your points earned will be proportional to the
level of detail in your discussion). Which one was used in this lab demonstration?
Answer: Gas chromatography (GC) – utilized by scientists in order to be able to separate the volatile
... Show more content on Helpwriting.net ...
The stationary phase will absorb or slow down different components of the tested solution to
different degrees creating layers as the components of the solution are separated. Chromatography
was invented by the Russian botanist, Mikhail Tsvet. Chemists use this process to identify unknown
substances by separating them into the different molecules that make them up.
(c) Suppose I melted a grape (purple) popsicle and ran a chromatogram of the resulting substrate.
[i] (1 pts.) In the simplist case, what would I expect to see? Include as much detail as possible.
Answer: Once the chromatogram has been completed and is ready to be measured and calculated, on
the plate that was used to perform the chromatogram you should see where the red and blue have
completely separated. The red food coloring dye should be lower on the plate than the blue food
coloring dye.
<– example of results

[ii] (4 pts.) Suppose that the dot/area representing the longest wavelength of color in this situation
was located 21 mm from the baseline, and the dot/area representing the shortest wavelength of color
was located 36 mm from the baseline (see Figure 9.4 on page 288 for help). If the solvent traveled 57
mm from the baseline, what was the Rf for each of these two components of the sample? [SHOW
ALL WORK TO RECEIVE CREDIT]
Answer: Rf = distance sample moved from

Needy Nitrogen History
Here is a story about rules and standards set so high by elements these days. The hardest standard for
a compound to meet is the Octet rule. [6] Single atoms can only wish to live up to the rule. Only a
select few can meet this rule when created, The Noble Gases. The Noble Gases are born full of life
and beauty. The only Noble Gas that lives around this town is Natural Neon. Everyone around town
wishes they were him.[1] A new fellow around town is Needy Nitrogen. He was musician, so he
joined a community band. Some of his new friends includes: Happy Hydrogen, Lite Lithium, and
coping Carbon. All of the friends and Needy Nitrogen have fallen short of Octet rule. It can be show
by a quick description of each ones Electron dot notation. Each atom ... Show more content on
Helpwriting.net ...
Within each one of the songs, the solos or leads created a bond to bond. Each molecular formula was
different and causes different experience for the electrons. Some polar covalent, some nonpolar
covalent, and some ionic, but together they all competed for popularity with Natural Neon. They all
either shared or transfer to trump Natural neon. Each element had a quick thing to say. Natural neon
told us that he was not at all sad about being kicked off his Octet rule podium. He was glad to see
everyone becoming stable. Needy Nitrogen and Coping Carbon were very pleased to become
bonded. They could be held together by a couple of intermolecular forces, Dipole–Dipole, Hydrogen
bonding, or London dispersion. They were glad they were living a molecular compound life. Happy
Hydrogen and his backup guitar player, Lite Lithium was so excited about their song. On
Performance day, Lite Lithium lost his guitar pick, so Happy hydrogen transferred him his. But he
was still upset because it could not get its Lewis Dot Structure. This song was still great because it
was an ionic compound. Last, Lite lithium would like to show his heat of vaporization and Thermal
Conductivity. He was a one act show with the help of himself. The moral of the story is that just
because there are standard set that are unreachable by yourself, does not mean they are reachable
with the help of your friends and Chemical

Lab 12 Essay
1. What is an ionic bond? Typically an ionic bond occurs between one metal and one non–metal ion.
One atom borrows one or more electrons from another atom. An ionic bond is a type of chemical
bond that occurs when one atom loses an electron to form a positive ion and the other atom gains an
electron to form a negative ion, which then result in attraction. 2. What is a covalent bond? A
covalent bond is a bond that occurs when atoms in a molecule share a pair of electrons. For example,
"the atoms in sugar do not form ions; instead, they are held together because of shared electrons."
3. Do you think sugar or salt will melt at a higher temperature? Explain your answer. Since sugar is
composed of covalent bonds and salt ... Show more content on Helpwriting.net ...
Questions
1. Why is it important to use distilled water instead of tap water used in Part 1? Distilled water is
formed from condensed steam, which therefore makes it free from mineral and organic salts. Regular
water is physically purified and chemically treated to kill germs, but contains many salts in it.
Distilled water is free of salts, but regular tap water contains many salts. Therefore, if we are trying
to see what happens for sugar, it would not be purely sugar if we used tap water because tap water
contains salts. If we used tap water we would be mixing salt and sugar so we would not get accurate
results.
2. In Part 1, why did you not observe a stream of bubbles coming off the stainless steel screw in the
sugar solution? Since sugar is composed of covalent bonds and therefore as we saw in part 2, takes
much less time to melt, I think we didn't observe bubbles because there was not as much as a
reaction since it "melted" so much faster. Also, sugar does not change its composition when added to
water, but salt does. Therefore, perhaps the sugar does not cause the screw to bubble much.
3. Did any bubbles form off the screw in the sugar solution at all? Why might this happen despite
your answer to Question 2? I did see occasional bubbles, which could be due to the slight chemical
reaction of the two chemicals. However, it was obviously not as strong as with the salt since the salt
changed

What About Chemical Bonds?
What About Chemical Bonds ?
Many scientists worked on development of chemical bonds
Empodecols,Democritos, Aristo, Dalton and Avogadro ....
It was a big issue in ancient times
How compounds bonded together ?
Their hypothesis help to discover
Ionic and covalent bonds
The electrons quicken around the core
Diffuse object of negatively charged electrons carry the electrical load ,
Protons and Neutrons lie inside the core Same number of electrons that balances the load but which
are positively charged protons ,
Neutral particles carry electric charge neutrons.
The particle increases, additional electron it changes into anion
Presently it has a few charges
Which weakened my life drive hard.
Some more electrons needed in the valence shell
To ... Show more content on Helpwriting.net ...
I let the electron shopping
My name is ionic bondsI tend to not take Electron
Electrons are shopping them
Last orbits are completed 8
Ionic bond is formed between Na + and Cl–
Na gives +1 and Cl takes –1
Negative ions we called anions –1
Positive ions we called cations +1 Thus both reach each other
Such a nice ionic compound NaCl
Lewis structure is used to show chemical bonds
Inner shell electrons and valence with a symbol showing the core
It composed of dots showing the electrons
Make sure electrons are safe

The vitality broke the compound
As it conquer the power of higher sum
Presently there 's no more bond
Which changes my life again into grieve.
Again, it formed into recently ionic bond
Furthermore, has an in number, power of fascination
Presently I can manage a tasteful life which now change over me into suffice.
CRITIQUE
Since ancient times what the forces that hold atoms together was one of the issues facing the people
of science.Empedocles and Aristotle shared the same opinion. The universe of fire, water, earth and
air to occur, and they think that they could be united with each other. The mixture or compound itself
can not be separated without causing movement power.
According to Democritos,

Disadvantages Of 4 White Powders
From the table four appropriate simple tests can be conducted in order to determine the structure type
and identify the four white powders. This includes conducting tests of melting point, flame color,
solubility and the conductivity in water (H20). The melting point of a substance is the temperature at
which the material changes from a solid to a liquid state. The determination of melting points is a
form of identification and test method for organic substance. The melting point is an easy way
measure and classify substances. Testing the flame color is an appropriate test as metal ions change
the color of a flame when they are heated. Different metal ions give different colors to the flame. So
flame tests can be used to identify the presence of a particular metal in a sample. Solubility is
appropriate as a solvent a substance will dissolve in gives hints to its identity. Conductivity in water
(H20) identifies if a substance is ionic or molecular. If a solution of compound and water has high
conductivity level, the compound is ionic if not it is molecular.
– Flame test
– Melting POINT
– Solubility
– Conductivity in water
Materials:
– 8 test tubes
–Test Tube Rack
–Spatula
–Electrical conductor kit
– Four unknown substances (C,F, E, D)
– Peg
– Distilled water
Procedure: Flame color
1.

Ionic And Covalent Compounds Essay
Chris Naoum
Mr. Jeff Handley
Science A
1/27/2016
Ionic and Covalent Compounds
Introduction:
Methods:
–Water solubility
–melting point
– conductivity of electricity
properties of covalent bonds:
– Liquid or gaseous (its state at room temperature)
– It is formed when two non–metals have similar electro negativities
– Its melting point is low
Properties of ionic bonds:
– Solid (its state at room temperature)
– It is formed between a metal and a non–metal
– Its melting point is high
Two methods chosen: Method 1: Water solubility can be used to figure out if a compound is ionic or
covalent because once the compound is put into the Distilled H2O it would dissolve since its ionic
but if the powder is insoluble then its covalent meaning ... Show more content on Helpwriting.net ...
If the powder dissolves then to make sure it is ionic or a type of covalent pour the 150 ml of ethanol
into a beaker and pour 1.5 grams of the same powder into the chemical, if the powder dissolves it is
covalent but if it doesn't dissolve its ionic.
8. Record all observations on the reaction of the water and ethanol
9. Repeat steps 1–8 for other 5 powders
Melting Point procedure:

1. Take the aluminum dish and separate the middle using a pencil
2. Put 3 grams of two different powders in the separate panels
3. Put the retort stand over the Bunsen burner
4. Turn the Bunsen burner on and set a specific temperature(start low) place the aluminum dish on
the retort stand above the Bunsen burner
5. If the powder does not burn then raise the temperature to a very high temp.
6. If the powder melts at a high temperature (800 plus) then its ionic but if it melts at a low temp its
covalent
7. Make sure to use the infrared thermometer to check what temperature the powder started melting
at and record the reaction and what temperature the powder melted at
8. Repeat steps 1–7 for the other powders
Works cited:
BBC News. BBC, Web. 26 Jan. 2016.

Consequences Of Chemistry : Chemistry Of The Water Of Water
Analysis: By solvent Water as a solvent Water is one of the most common solvents used in the world.
We found that when mineral oil (decane) is added to water the two repel each other and separate,
leaving the oil on the surface of the water. Water is polar and decane is nonpolar and because
opposites do not attract the decade does not dissolve not the water. When isopropyl alcohol is added
to water it formed little sting like structures as it dissolved. Both the solvent and solute are polar
which is why the alcohol dissolved so nicely into the water. When copper (II) chloride was added to
the water it turned a bright blue–green colour, but did not dissolve. This is because copper (II)
chloride is an ionic compound and the forces of attraction holding it together are stronger than the
force of attraction between water and the positive and negative ions. The coconut oil did not dissolve
when added to the water because coconut oil is very nonpolar, so the water could not pull apart any
of the positive or negative sides. When the glucose was added to the water, it dissolved immediately.
The glucose is polar and so is water, so the water will pull the slightly positive and negative sides
decomposing the crystals. Decane as a solvent When water was added to decane the same thing
happened as when decane was added to water, this being that the two solutions stayed separated.
When isopropyl was added to decane it became a thicker substance and the alcohol bubbled back to
the top

Density Measurement Lab
Procedure In this lab, there was six specimens including three metals,steel, aluminum, brass, and
three polymers, PVC, Nylon and polyethylene. Each of these six specimens was going to be tested
its hardness and conductivity and measured its density.
Density Measurement
There was two methods to measure the density of materials. First method was to calculate the
volume of the specimens in mathematical way. First dividing the specimen into three parts as shown
in Figure 1.
Figure 1
Then using caliper to measure the length, width and height of those three rectangular parts. After
getting the measurement of the specimen, using mathematical equation V= LxWxH to calculate the
volume of each rectangles and then adding them up to get the final ... Show more content on
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However, the natures between the two are quite different. Covalent bonds are formed by nonmetal
and nonmetal. Electrons in the covalent bond are shared and no atom wants to leave the other
adjacent atom because they all want to be stable. Thus, the covalent bond between atoms is very
strong. However, there is van der Waals bond between two molecules. Van der Waals bond is the
basis of chemical bonding and is weaker than all the primary bonds. Van der Waals bond has weaken
a material such as polymers because the attraction force between molecules is not strong. However,
for metallic bonding, metal ions are bonded with metal ions. The bonding connection between the
two is always to be metallic bond. Hence, when comparing materials containing covalent and
metallic bonds generally, it is easier to find out that materials which are made of metal are relatively
stronger than materials made of polymers. Furthermore, due to the directionality of covalent bond, it
restricts electrons to travel freely, so molecules of covalent bond are not able to conduct electricity
like metallic bond which has a travelled electric current.
The major differences of these two chemical bonds are shown obviously in the lab. Metals has larger
density values, higher hardness than polymers and able to conduct electricity while polymers is not
able to. To understand the distinction in atomic bonding, one can utilize the knowledge in his

What Are The Advantages And Disadvantages Of Enzyme...
following side chains of the amino acids: lysine (ε–amino group), cysteine (thiol group), and aspartic
and glutamic acids (carboxylic group). The covalent reactions commonly employed give rise to
enzymes linked to the support through either amide, ether, thio–ether, or carbamate bonds. Therefore,
the enzyme is strongly bound to the matrix and, in many cases, it is also stabilized, however, because
of the covalent nature of the bond, the matrix has to be discarded together with the enzyme once the
enzymatic activity decays. For example glutaraldehyde used for enzyme immobilisation is classified
under the activation method, in this reaction the amine group reacts with the activated matrix. The
covalent binding is normally formed between the ... Show more content on Helpwriting.net ...
The interaction between the enzyme and the surface of the matrix through weak forces by salt
linkage, hydrogen bonds, hydrophobic bonds, ionic bonds and van der waals forces. The advantage
of enzyme adsorption is minimum activation step and as a result of minimum activation, no reagents

Intermolecular Forces Essay
Intermolecular forces are the attractive and/or repulsive forces among independent particles, such as
molecules, atoms, or ions, within a sample of matter. These forces differ from chemical bonds, or
intramolecular forces, because chemical bonds exist between the atoms of a single molecule. For
example, intermolecular forces could be described as the forces that attract many water molecules
together, while chemical bonds refer to the bonds between the hydrogen and oxygen atoms of a
single water molecule. Chemical bonds are also generally more permanent and stronger than
intermolecular forces.
There are various types of intermolecular forces, all which differ in strength. These forces include:
ion–ion forces, dipole–dipole forces, ion–dipole forces, ion–induced dipole, dipole–induced dipole,
and London dispersion forces. The amount of charge, how it is distributed, and how long a charge
distribution will last, all factor into how strong the intermolecular forces are. ... Show more content
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These forces attract ions rather strongly. In a pure ionic compound, we call these forces ionic bonds
and consider it to be an intramolecular force. In a mixture of substances, however, it is seen as an
intermolecular force since the ions are interacting without being bonded. Ion–ion forces are repulsive
if they are cation–cation or anion–anion, and are attractive if they are cation–anion. Charge and size
influence the strength of these forces. Small molecules with large charge magnitudes would have
stronger ion–ion forces acting between them because these factors would allow for closer approach
to their

Chemical Bonds Lab
Chemical Bonds Lab Paper Shawn Guillot & Kiara Wilson There are many types of chemical bonds
and forces that bind molecules together. The two most basic types of bonds are characterized as
either ionic or covalent. In the lab we separated Citric Acid, Calcium Chloride, Sucrose, Potassium
Iodine, Phenyl Salicylate ,and Sodium Chloride into two groups ionic and Covalent bonds .The
Chemical Difference between ionic bonding and covalent bonding is, a covalent bond is formed
between two nonmetals that have similar electronegativities. Metals are left half and center of the
Periodic Table and Nonmetals are upper right of the Periodic Table. The electrical attraction between
large numbers of cations and anions which is the transfer of the ... Show more content on
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In this lab we performed four test. Using these test we discovered how the chemicals compounds
Citric Acid, Calcium Chloride, Sucrose, Potassium Iodine, Phenyl Salicylate , and Sodium Chloride
reacted to heat and many solutions. We also noticed that Phenyl salicylate was the least reactive out
of all chemical compounds. Using the information discovered from the lab we were able to separate
the chemical compounds into two groups. In group one were the chemical compounds Calcium
chloride, Citric acid, Potassium iodide, Sodium chloride, and Sucrose these chemical compounds
reacted to three of the four test. Group two was just Phenyl salicylate which reacted to only one of
the four test. We also were able to state that group one was a covalent compound group and, group
two was an ionic compound

Chemistry Bonding Assignment

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