Explain why sulfur dioxide and acetic acid have dipole moments- Use an.docx
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Explain why sulfur dioxide and acetic acid have dipole moments. Use an electronegativity argument. Solution * Sulphur dioxide has bent shape with one lone pair on Sulphur and two oxygen atoms are more electronegative than Sulphur. Hence the bond pair of electrons are strongly attracted by oxygen atoms where as lone pair move in opposite direction and net there exists some unequal distribution of electrons around central sulphur. Thus sulphur dioxide exhibits dipole moment. ** In Acetic acid the central C is attached to one - CH 3 group, one O with double bond and one - OH gorup. Around this Carbon, the shape is trigonal plananr. Since the electronegativity of O is greater than C, the bond pair of electrons spends more time nearer the O and hence there exists unequal distribution of electrons around central C. Thus the molecules has a net dipole moment. .
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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.
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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
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bonding between the carbons. If all the carbon-carbon bonds are single, the compound
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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.
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octane - unbranched (straight-chain)
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In chemistry, hybridisation (or hybridization) is the concept of mixing atomic
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1) Organic chemistry is the study of carbon-containing compounds. Early theories proposed that organic compounds contained a "vital force" not found in inorganic compounds, but experiments in the early 1800s showed that organic substances could be synthesized in the lab.
2) Carbon atoms can form up to four strong covalent bonds due to their electronic structure, allowing them to link together in chains and rings. The shapes and orientations of atomic orbitals help explain chemical bonding and reactivity.
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1. Atoms Atoms are structured by 3 main components. Protons, ne.pdf
1. Atoms:
Atoms are structured by 3 main components. Protons, neutrons and electrons. The core of the
atom consists of protons and neutrons. Protons are positively charged, and neutrons are neutral.
Electrons circle the core of the atom, and form a \"cloud\" of electrons. Electrons are negatively
charged.
2. Bonds:
You have different elements such as Na, Cl, H, O etc. Several COMPOUNDS that you may
have heard of include, NaCl and H2O. In order for these elements to form these compounds,
bonds need to form between them. When bonds are made energy is released.
3. Periodic Table:
The number of electrons that an atom of an element has is usually equal to it\'s atomic number.
More importantly there is a trend that you can determine what the number of valence (outer
most) electrons are. Group 1 has 1 valence electron, Group 2 has 2, Group 3 has 3, Group 8 has
0, Group 7 has 7, Group 6 has 6 (O, S, Se, Te), Group 5 has 5( N, P, As) and Group 4 has 4
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4. Electronegativity:
This means how reactive a certain element is. If an element has lots of valence electrons it will
have a high electronegativity because it wants that 1 electron, to fill its 8 compartments in its
shell. The trend for electronegativity is that electronegativity increases as you go across the
periodic table towards the right ->. As you go towards the right, you have more and more
valence electrons, therefore more \"want\" for electrons to fill up the compartments.
When you go (^) up the periodic table electronegativity also increases due to the distance the
electrons are away from the nucleus (core) of the atom.
5. Polarity:
Polarity just means you have 2 poles. Think of it like a magnet, you usually have a north pole
and a south pole OR a positive pole and a negative pole.
Different atoms have different charges. For example, H2O, consists of 2 hydrogens and 1
oxygen. Hydrogen is positively charged and oxygen is negatively charged. This is why water is
said to be polar. It consists of both a positive and a negative.
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Hope this helps! :)
Solution
1. Atoms:
Atoms are structured by 3 main components. Protons, neutrons and electrons. The core of the
atom consists of protons and neutrons. Protons are positively charged, and neutrons are neutral.
Electrons circle the core of the atom, and form a \"cloud\" of electrons. Electrons are negatively
charged.
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You have different elements such as Na, Cl, H, O etc. Several COMPOUNDS that you may
have heard of include, NaCl and H2O. In order for these elements to form these compounds,
bonds need to form between them. When bonds are made energy is released.
3. Perio.
The electrons which are involved in bond formatio.pdf
The electrons which are involved in bond formation between atoms are found in the
outermost shell (sometimes in the next to the outer-most shell) of the neutral atom; these are
called VALENCE ELECTRONS. The atoms of elements which have only one or two electrons
in their outermost shells (active shells) may lose electrons when they combine with atoms of
other elements. An atom which has lost one or more valence electrons possesses a positive
charge, and is called a POSITIVE ION. The sodium atom loses its one valence electron and
acquires a +1 charge when it enters into chemical combination with an atom of an element such
as chlorine. The magnesium atom may lose its two valence electrons and assume a +2 charge.
Na Na+ + e- The Na symbol to the left of the arrow represents a stable sodium atom while the
Na+ symbol to the right of the arrow represents an unstable sodium ion which has had a single
electron removed. Mg Mg++ + 2e- The Mg symbol to the left of the arrow represents a stable
magnesium atom while the Mg++ symbol to the right of the arrow represents an unstable
magnesium ion which has had two electrons removed. The smaller the number of valence
electrons in the atom, the greater the tendency of the element to lose electrons and thus form
positive ions during chemical combination with atoms of other elements. The energy required to
remove an electron from a neutral atom to form a positive ion is called the IONIZATION
POTENTIAL of the atom. Some metals have small ionization potentials and readily form
positive ions. The nonmetals, which have more electrons in their outer shells than the metals,
have large ionization potentials and show little tendency toward the formation of positive ions.
Atoms which lack one or two electrons of having an outermost shell of eight electrons readily
gain sufficient electrons from certain other atoms, such as sodium and magnesium, to make a full
compliment of eight electrons in the outside shell. Neutral atoms become NEGATIVE IONS by
gaining electrons. The nonmetals, such as Fluorine (F), Chlorine (Cl), Bromine (Br), Iodine (I),
Oxygen (O), Nitrogen (N) and Sulfur (S), readily form negative ions. Cl + e- Cl- Chlorine,
when in its stable form, possesses seven valence electrons and therefore has the ability to gain
one electron (as represented to the left of the arrow) giving it a negative charge of one when in
its unstable ionic form (as represented to the right of the arrow above). S + 2e- S-2 Sulfur, when
in its stable form, possesses six valence electrons and therefore has the ability to gain two
electrons giving it a negative charge of two when in its unstable ionic form. The attraction of a
neutral atom for electrons is known as its ELECTRON AFFINITY. The nonmetals have high
electron affinities and the metals have very low electron affinities. Thus, mainly the nonmetals
tend to form negative ions during chemical combination. When a positive ion and a negative ion
are brought close together, strong electr.
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Hybridization:
Developed by Linus Pauling, the concept of hybrid orbitals was a theory created to explain the structures of molecules in space. The theory consists of combining atomic orbitals (ex: s,p,d,f) into new hybrid orbitals (ex: sp, sp2, sp3).
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Organic Chemistry deals with carbon compounds and their structures and reactions. It originally focused on living substances but now includes synthetic compounds. Carbon forms the backbone of organic molecules due to its ability to form chains and complex structures through covalent bonding, including single, double and triple bonds. The hybridization of atomic orbitals, such as sp3 hybridization, allows carbon to form four bonds to other atoms and explains the shapes of organic molecules like methane. Understanding bonding concepts such as ionic and covalent bonds is essential to organic chemistry.
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First Year in Dentistry First Semester
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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.
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Atoms form bonds to attain a lower potential energy state. They do this through ionic bonds, where oppositely charged ions attract, or covalent bonds, where atoms share valence electrons. Whether a bond is ionic or covalent depends on the electronegativity difference between the atoms. Ionic bonds form between metals and nonmetals, while covalent bonds form between two nonmetals. Lewis structures use dots to represent valence electrons and show how atoms share electrons to achieve stable configurations like noble gases. Valence shell electron pair repulsion theory explains molecular shapes based on electron pair positioning.
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Answer: The Liabilities Topic includes the following Subtopics:
The definition of liability can help decide the accounting treatment of the situation. Under the Conceptual Framework a liability is a present obligation of the entity arising from past events, the settlement of which is expected to result in an outflow from the entity of resources embodying economic benefits. In this case, the past event is the fall and injury to the pedestrian.
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orbitals for molecules. It is an integral part of valence bond theory. Although sometimes taught
together with the valence shell electron-pair repulsion (VSEPR) theory, valence bond and
hybridization are in fact not related to the VSEPR model.[1] Contents [hide] 1 Historical
development 2 Types of hybridisation 2.1 sp3 hybrids 2.2 sp2 hybrids 2.3 sp hybrids 3
Hybridisation and molecule shape 3.1 Explanation of the shape of water 3.2 Controversy
regarding d-orbital participation 4 Hybridisation theory vs. MO theory 5 See also 6 External
links 7 References [edit]Historical development Chemist Linus Pauling first developed the
hybridisation theory in order to explain the structure of molecules such as methane (CH4).[2]
This concept was developed for such simple chemical systems, but the approach was later
applied more widely, and today it is considered an effective heuristic for rationalizing the
structures of organic compounds. For quantitative calculations of electronic structure and
molecular properties, hybridisation theory is not as practical as molecular orbital theory.
Problems with hybridisation are especially notable when the d orbitals are involved in bonding,
as in coordination chemistry and organometallic chemistry. Although hybridisation schemes in
transition metal chemistry can be used, they are not generally as accurate. Orbitals are a model
representation of the behaviour of electrons within molecules. In the case of simple
hybridisation, this approximation is based on atomic orbitals, similar to those obtained for the
hydrogen atom, the only atom for which an exact analytic solution to its Schrödinger equation is
known. In heavier atoms, like carbon, nitrogen, and oxygen, the atomic orbitals used are the 2s
and 2p orbitals, similar to excited state orbitals for hydrogen. Hybridised orbitals are assumed to
be mixtures of these atomic orbitals, superimposed on each other in various proportions. The
theory of hybridisation is most applicable under these assumptions. It gives a simple orbital
picture equivalent to Lewis structures. Hybridisation is not required to describe molecules, but
for molecules made up from carbon, nitrogen and oxygen (and to a lesser extent, sulfur and
phosphorus) the hybridisation theory/model makes the description much easier. The
hybridisation theory finds its use mainly in organic chemistry. Its explanation starts with the way
bonding is organized in methane. [edit]Types of hybridisation [edit]sp3 hybrids Hybridisation
describes the bonding atoms from an atom\'s point of view. That is, for a tetrahedrally
coordinated carbon (e.g., methane, CH4), the carbon should have 4 orbitals with the correct
symmetry to bond to the 4 hydrogen atoms. The .
Chap1
This document discusses different types of chemical bonds including ionic, covalent, and metallic bonds. It describes the formation of ionic bonds between metals and nonmetals and how ionization energy, electron affinity, and lattice energy contribute to the energetics of ionic bonding. Covalent bonding is explained as the sharing of electrons between nonmetals. Factors that determine bond polarity like electronegativity are also covered. The document provides details on writing Lewis structures, accounting for valence electrons and formal charges. Exceptions to the octet rule for molecules with odd numbers of electrons, incomplete octets, and expanded octets are explained.
Chemical bonding
The document summarizes different types of chemical bonds including ionic bonds, covalent bonds, metallic bonds, hydrogen bonds, and Van der Waals interactions. It describes how each type of bond forms and provides examples. Ionic bonds form through electrostatic attraction between oppositely charged ions. Covalent bonds form when atoms share one or more pairs of electrons. Metallic bonds result from delocalized electrons within metal structures. Hydrogen bonds are electrostatic attractions between hydrogen and electronegative atoms. Van der Waals interactions arise from correlations in polarizations between particles.
Chapter 1 Structure and Bonding.pptx
This document provides an overview of key concepts in organic chemistry structure and bonding. It discusses atomic structure, including electrons occupying atomic orbitals. Covalent bonding is described using valence bond theory and molecular orbital theory. Hybridization of atomic orbitals allows carbon to form single, double, and triple bonds with different geometries using sp, sp2, and sp3 hybrid orbitals. Examples like methane, ethylene, and acetylene are used to illustrate hybrid orbital bonding structures. Molecular representations like Lewis structures and condensed structural formulas are also introduced.
Organic Chemistry I
1) Organic chemistry is the study of carbon-containing compounds. Early theories proposed that organic compounds contained a "vital force" not found in inorganic compounds, but experiments in the early 1800s showed that organic substances could be synthesized in the lab.
2) Carbon atoms can form up to four strong covalent bonds due to their electronic structure, allowing them to link together in chains and rings. The shapes and orientations of atomic orbitals help explain chemical bonding and reactivity.
3) Atoms bond together, forming molecules, because the bonded state is lower in energy than separated atoms. Covalent bonds form when atoms share electrons to achieve stable noble gas electron configurations, as seen in the Lewis structure of methane
1. Atoms Atoms are structured by 3 main components. Protons, ne.pdf
1. Atoms:
Atoms are structured by 3 main components. Protons, neutrons and electrons. The core of the
atom consists of protons and neutrons. Protons are positively charged, and neutrons are neutral.
Electrons circle the core of the atom, and form a \"cloud\" of electrons. Electrons are negatively
charged.
2. Bonds:
You have different elements such as Na, Cl, H, O etc. Several COMPOUNDS that you may
have heard of include, NaCl and H2O. In order for these elements to form these compounds,
bonds need to form between them. When bonds are made energy is released.
3. Periodic Table:
The number of electrons that an atom of an element has is usually equal to it\'s atomic number.
More importantly there is a trend that you can determine what the number of valence (outer
most) electrons are. Group 1 has 1 valence electron, Group 2 has 2, Group 3 has 3, Group 8 has
0, Group 7 has 7, Group 6 has 6 (O, S, Se, Te), Group 5 has 5( N, P, As) and Group 4 has 4
(C,Si).
4. Electronegativity:
This means how reactive a certain element is. If an element has lots of valence electrons it will
have a high electronegativity because it wants that 1 electron, to fill its 8 compartments in its
shell. The trend for electronegativity is that electronegativity increases as you go across the
periodic table towards the right ->. As you go towards the right, you have more and more
valence electrons, therefore more \"want\" for electrons to fill up the compartments.
When you go (^) up the periodic table electronegativity also increases due to the distance the
electrons are away from the nucleus (core) of the atom.
5. Polarity:
Polarity just means you have 2 poles. Think of it like a magnet, you usually have a north pole
and a south pole OR a positive pole and a negative pole.
Different atoms have different charges. For example, H2O, consists of 2 hydrogens and 1
oxygen. Hydrogen is positively charged and oxygen is negatively charged. This is why water is
said to be polar. It consists of both a positive and a negative.
Water is also an example of hydrogen bonding, because Hydrogen is bonding with a large
molecule, oxygen.
Non-polar bonds are where there are no positives or negatives. An example would be a diatomic
molecule, such as oxygen gas: O2. Methane: CH4 is also considered to be non-polar because its
carbon atom covalently bonds with hydrogen atoms sharing almost completely equally.
Hope this helps! :)
Solution
1. Atoms:
Atoms are structured by 3 main components. Protons, neutrons and electrons. The core of the
atom consists of protons and neutrons. Protons are positively charged, and neutrons are neutral.
Electrons circle the core of the atom, and form a \"cloud\" of electrons. Electrons are negatively
charged.
2. Bonds:
You have different elements such as Na, Cl, H, O etc. Several COMPOUNDS that you may
have heard of include, NaCl and H2O. In order for these elements to form these compounds,
bonds need to form between them. When bonds are made energy is released.
3. Perio.
The electrons which are involved in bond formatio.pdf
The electrons which are involved in bond formation between atoms are found in the
outermost shell (sometimes in the next to the outer-most shell) of the neutral atom; these are
called VALENCE ELECTRONS. The atoms of elements which have only one or two electrons
in their outermost shells (active shells) may lose electrons when they combine with atoms of
other elements. An atom which has lost one or more valence electrons possesses a positive
charge, and is called a POSITIVE ION. The sodium atom loses its one valence electron and
acquires a +1 charge when it enters into chemical combination with an atom of an element such
as chlorine. The magnesium atom may lose its two valence electrons and assume a +2 charge.
Na Na+ + e- The Na symbol to the left of the arrow represents a stable sodium atom while the
Na+ symbol to the right of the arrow represents an unstable sodium ion which has had a single
electron removed. Mg Mg++ + 2e- The Mg symbol to the left of the arrow represents a stable
magnesium atom while the Mg++ symbol to the right of the arrow represents an unstable
magnesium ion which has had two electrons removed. The smaller the number of valence
electrons in the atom, the greater the tendency of the element to lose electrons and thus form
positive ions during chemical combination with atoms of other elements. The energy required to
remove an electron from a neutral atom to form a positive ion is called the IONIZATION
POTENTIAL of the atom. Some metals have small ionization potentials and readily form
positive ions. The nonmetals, which have more electrons in their outer shells than the metals,
have large ionization potentials and show little tendency toward the formation of positive ions.
Atoms which lack one or two electrons of having an outermost shell of eight electrons readily
gain sufficient electrons from certain other atoms, such as sodium and magnesium, to make a full
compliment of eight electrons in the outside shell. Neutral atoms become NEGATIVE IONS by
gaining electrons. The nonmetals, such as Fluorine (F), Chlorine (Cl), Bromine (Br), Iodine (I),
Oxygen (O), Nitrogen (N) and Sulfur (S), readily form negative ions. Cl + e- Cl- Chlorine,
when in its stable form, possesses seven valence electrons and therefore has the ability to gain
one electron (as represented to the left of the arrow) giving it a negative charge of one when in
its unstable ionic form (as represented to the right of the arrow above). S + 2e- S-2 Sulfur, when
in its stable form, possesses six valence electrons and therefore has the ability to gain two
electrons giving it a negative charge of two when in its unstable ionic form. The attraction of a
neutral atom for electrons is known as its ELECTRON AFFINITY. The nonmetals have high
electron affinities and the metals have very low electron affinities. Thus, mainly the nonmetals
tend to form negative ions during chemical combination. When a positive ion and a negative ion
are brought close together, strong electr.
Covalent Bonding PPT
This is Usefull pdf for the B.Sc II student In Sant Gadge Baba Amravati University Amravati and tis affiliated colleges admited students
Hybridization
INTRODUCTION:
Hybrid Orbitals
Developed by Linus Pauling, the concept of hybrid orbitals was a theory created to explain the structures of molecules in space. The theory consists of combining atomic orbitals (ex: s,p,d,f) into new hybrid orbitals (ex: sp, sp2, sp3).
Hybridization
Hybridization:
Developed by Linus Pauling, the concept of hybrid orbitals was a theory created to explain the structures of molecules in space. The theory consists of combining atomic orbitals (ex: s,p,d,f) into new hybrid orbitals (ex: sp, sp2, sp3).
Unit-8-Lesson-15-THE-CHEMICAL-BONDING.pptx
1. The document discusses different types of chemical formulas including molecular, empirical, and structural formulas. It provides examples of each type like H2O for water and C6H12 for hexene.
2. It also discusses ionic and covalent bonding. Ionic bonding involves the complete transfer of electrons from one atom to another, like from sodium to chlorine in NaCl. Covalent bonding involves the sharing of electron pairs between atoms.
3. The document describes electronegativity and how it relates to the polarity of covalent bonds. Polar covalent bonds form between atoms with an electronegativity difference of 0.5-1.6, while ionic bonds form between atoms with a difference above
Carbon and it's compounds - part 1
Carbon has an atomic number of 6 and electronic configuration of 2,4. It requires 4 electrons to achieve the inert gas configuration but cannot form stable ions. Instead, carbon overcomes this issue by forming covalent bonds where it shares its valence electrons with other carbon atoms or other elements. There are three main types of covalent bonds: single, double, and triple bonds which are formed by sharing one, two, or three pairs of electrons respectively. Carbon's ability to form long chains through catenation is due to its property of self-linkage through covalent bonds between identical carbon atoms.
Module 1.pdf
This document provides an overview of organic chemistry concepts including:
- The electronic structure of atoms and how this relates to bonding
- Different types of bonds (ionic, covalent, polar, nonpolar) and how they form
- Lewis structures and resonance forms
- Molecular shapes determined by hybridization of orbitals
- Isomerism including constitutional and geometric isomers
The document covers fundamental topics that provide context for understanding organic molecular structures and reactions.
Chapter 8 Covalent Bonds
1. Covalent bonds form when two atoms share one or more pairs of valence electrons in order to achieve a stable octet of electrons.
2. Molecules are formed when atoms are bonded together by covalent bonds, and molecular compounds are composed of molecules.
3. Molecular compounds tend to have lower melting and boiling points than ionic compounds and many are gases or liquids at room temperature.
Organic Chemistry 1.pdf
Organic Chemistry deals with carbon compounds and their structures and reactions. It originally focused on living substances but now includes synthetic compounds. Carbon forms the backbone of organic molecules due to its ability to form chains and complex structures through covalent bonding, including single, double and triple bonds. The hybridization of atomic orbitals, such as sp3 hybridization, allows carbon to form four bonds to other atoms and explains the shapes of organic molecules like methane. Understanding bonding concepts such as ionic and covalent bonds is essential to organic chemistry.
Chapter 9
First Year in Dentistry First Semester
Al-Azhar University - Gaza
Lama El Banna
general chemistry
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.
chemical bonding
Atoms form bonds to attain a lower potential energy state. They do this through ionic bonds, where oppositely charged ions attract, or covalent bonds, where atoms share valence electrons. Whether a bond is ionic or covalent depends on the electronegativity difference between the atoms. Ionic bonds form between metals and nonmetals, while covalent bonds form between two nonmetals. Lewis structures use dots to represent valence electrons and show how atoms share electrons to achieve stable configurations like noble gases. Valence shell electron pair repulsion theory explains molecular shapes based on electron pair positioning.
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In chemistry, hybridisation (or hybridization) is.pdf
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1. Atoms Atoms are structured by 3 main components. Protons, ne.pdf
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The electrons which are involved in bond formatio.pdf
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Solution
Answer: The Liabilities Topic includes the following Subtopics:
The definition of liability can help decide the accounting treatment of the situation. Under the Conceptual Framework a liability is a present obligation of the entity arising from past events, the settlement of which is expected to result in an outflow from the entity of resources embodying economic benefits. In this case, the past event is the fall and injury to the pedestrian.
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Solution
Answer: The Liabilities Topic includes the following Subtopics:
The definition of liability can help decide the accounting treatment of the situation. Under the Conceptual Framework a liability is a present obligation of the entity arising from past events, the settlement of which is expected to result in an outflow from the entity of resources embodying economic benefits. In this case, the past event is the fall and injury to the pedestrian.
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Your hard drive can have various partitions which usually contains only one file system, such as one file system housing the / file system or another containing the /home file system.
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Special Files
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When an auditor of financial statements does not confirm material accounts receivable, but is satisfied by the application of alternative auditing procedures, she normally should:
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Solution
Provisional Entries - Provisional Entries are made every month/Year to ensure few of those accounting entries which might not get recorded in time and should be recorded to ensure correct accounting . A provision can be a liability of uncertain timing or amount.
Provision entries are entries that are made to account for expenses that have not been accounted in the period for which it relates. Hence the provision is created by debiting the expenses and crediting the party account or liability account. Provision means liabilities It means payable account. It helps to control payable accounts like telephone charges, Gratuity , Providend Fund accounts.
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Solution
Contiguous File Allocation
+ fast sequential access
+ fast random access
+ low disk space overhead
- external fragmentation
- hard to grow file
Linked File Allocation
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+ easy to grow file
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Indexed File Allocation
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+ Pros
- Cons
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Solution
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Explain the purpose of a data member.
Solution
Answer
Data Member
It is nothing but an object may contain values which are stored internally and are unique to that object.
A data member may be any type. Including Classes already defined, references of object any type.
We need to declare a data member in the classs.
that is like in C++ we can write like in private , public blocks
private :
int sum;
------
------
public :
int a;
float value;
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In java we can write as
int a,b,c;
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Header files purpose:
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Solution
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Explain how goverment deficit lead to increases in the money supply?
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Interest Groups
Functions of interest groups
Activities
Structures
Legitimacy
Problems of analysis and research
BIBLIOGRAPHY
Interaction between the polity and organized interests has taken place in all periods of history. Estates, guilds, trading companies, and the like are the more immediate antecedents of the modern interest group, which may be defined as a voluntary association of individuals who band together for the defense of an
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Solution
Answer-
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Hope this helped you!
Thank You So Much! Please Rate this answer as you wish.(\"Thumbs Up\")
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Event Link:- https://meetups.mulesoft.com/events/details/mulesoft-mysore-presents-mule-event-processing-models/
Agenda
● What is event processing in MuleSoft?
● Types of event processing models in Mule 4
● Distinction between the reactive, parallel, blocking & non-blocking processing
For Upcoming Meetups Join Mysore Meetup Group - https://meetups.mulesoft.com/mysore/YouTube:- youtube.com/@mulesoftmysore
Mysore WhatsApp group:- https://chat.whatsapp.com/EhqtHtCC75vCAX7gaO842N
Speaker:-
Shivani Yasaswi - https://www.linkedin.com/in/shivaniyasaswi/
Organizers:-
Shubham Chaurasia - https://www.linkedin.com/in/shubhamchaurasia1/
Giridhar Meka - https://www.linkedin.com/in/giridharmeka
Priya Shaw - https://www.linkedin.com/in/priya-shaw
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Syllabus
Chapter-1
Introduction to objective, scope and outcome the subject
Chapter 2
Introduction: Scope and Specialization of Civil Engineering, Role of civil Engineer in Society, Impact of infrastructural development on economy of country.
Chapter 3
Surveying: Object Principles & Types of Surveying; Site Plans, Plans & Maps; Scales & Unit of different Measurements.
Linear Measurements: Instruments used. Linear Measurement by Tape, Ranging out Survey Lines and overcoming Obstructions; Measurements on sloping ground; Tape corrections, conventional symbols. Angular Measurements: Instruments used; Introduction to Compass Surveying, Bearings and Longitude & Latitude of a Line, Introduction to total station.
Levelling: Instrument used Object of levelling, Methods of levelling in brief, and Contour maps.
Chapter 4
Buildings: Selection of site for Buildings, Layout of Building Plan, Types of buildings, Plinth area, carpet area, floor space index, Introduction to building byelaws, concept of sun light & ventilation. Components of Buildings & their functions, Basic concept of R.C.C., Introduction to types of foundation
Chapter 5
Transportation: Introduction to Transportation Engineering; Traffic and Road Safety: Types and Characteristics of Various Modes of Transportation; Various Road Traffic Signs, Causes of Accidents and Road Safety Measures.
Chapter 6
Environmental Engineering: Environmental Pollution, Environmental Acts and Regulations, Functional Concepts of Ecology, Basics of Species, Biodiversity, Ecosystem, Hydrological Cycle; Chemical Cycles: Carbon, Nitrogen & Phosphorus; Energy Flow in Ecosystems.
Water Pollution: Water Quality standards, Introduction to Treatment & Disposal of Waste Water. Reuse and Saving of Water, Rain Water Harvesting. Solid Waste Management: Classification of Solid Waste, Collection, Transportation and Disposal of Solid. Recycling of Solid Waste: Energy Recovery, Sanitary Landfill, On-Site Sanitation. Air & Noise Pollution: Primary and Secondary air pollutants, Harmful effects of Air Pollution, Control of Air Pollution. . Noise Pollution Harmful Effects of noise pollution, control of noise pollution, Global warming & Climate Change, Ozone depletion, Greenhouse effect
Text Books:
1. Palancharmy, Basic Civil Engineering, McGraw Hill publishers.
2. Satheesh Gopi, Basic Civil Engineering, Pearson Publishers.
3. Ketki Rangwala Dalal, Essentials of Civil Engineering, Charotar Publishing House.
4. BCP, Surveying volume 1
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