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8/8/2019 Chap 5 Matter and Chemical Bonding
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FOUNDATION INFOUNDATION IN SCIENCESCIENCEFOUNDATION INFOUNDATION IN SCIENCESCIENCE
NIRWANA ACADEMY GROUP OF COLLEGESNIRWANA ACADEMY GROUP OF COLLEGES
CHEMISTRY ACHEMISTRY A
CHAPTER 3CHAPTER 3
MATTER AND CHEMICALMATTER AND CHEMICAL
BONDINGBONDING
CHAPTER 3CHAPTER 3
MATTER AND CHEMICALMATTER AND CHEMICAL
BONDINGBONDING
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CHM1001 CHEMSTRYACHAPTER 5: Matter and Chemical Bonding
LEARNING OUTCOMESLEARNING OUTCOMES
At the end of the lessons, student would beable to
understand the meaning of matter
distinguish between solid, liquid, gas andplasma
understand the physical changes of matter
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NATURE OF MATTERNATURE OF MATTER
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Three main matter: solid, liquid, gas
Another matter: plasma
Very depends on temperature; cause the
atoms, molecules or ions to move more activestate
Substance or compound still remain the same
When a substance exist as solid, liquid and gasat the same time (combination of all states),
the substance was to be in equilibrium state
NATURE OF MATTERNATURE OF MATTER
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CHM1001 CHEMSTRYACHAPTER 5: Matter and Chemical Bonding
NATURE OF MATTERNATURE OF MATTER
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Closely packed with fixed position
Less vibration
Have certain shape and arrange in the
form of crystal
High melting point due to strong attraction
SOLIDSOLID
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Quite close, do not have an absolute shapebut follows the shape of container with
fixed volume
Moving around randomly and collisionoccur
Weaker attraction than solid but have
higher energyStronger force have higher boiling point
LIQUIDLIQUID
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Far apart and also do not have an absoluteshape; filled up the space of the container
Freely and randomly move anywhere with
high velocities; random motionLess collision between particle and
container
Very low force of attraction
GASGAS
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Partially ionized gas; free proportion ofelectrons
Charge of ions move independently;
electrically conductive where it can respondstrongly to electromagnetic field
Has unique properties
PLASMAPLASMA
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Happens when reaches at a certain point
Melting point, boiling point, freezing point
Other factor which can influence: pressure
Physical changes and chemical changes
Physical changes: changes from one state toanother state
Chemical changes: changes of substance;involves certain process
CHANGES OF STATECHANGES OF STATE
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CHM1001 CHEMSTRYACHAPTER 5: Matter and Chemical Bonding
PHYSICAL CHANGESPHYSICAL CHANGES
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CHM1001 CHEMSTRYACHAPTER 5: Matter and Chemical Bonding
Gas was said to be a final state of matterSome substances exist as gas in room
temperature while other solid or liquid
substances would always converted to gasjust by heating at certain temperature
Ionic compounds only exist as solid andhardly to convert to gas unless when apply
an extremely high temperatureIt able to convert to liquid/molten state
but also with a high temperature
PROPERTIES OF GASPROPERTIES OF GAS
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CHM1001 CHEMSTRYACHAPTER 5: Matter and Chemical Bonding
Thus most of the covalent substance moreeasily to convert to gas at low temperaturethan the ionic compound because of thestrength of the bonds formed
All gases would have the followingcharacteristics:The volume and shape are depend on the
container Easily to mix evenly and completely when
confined to the same container
Have the lowest density than the other state
PROPERTIES OF GASPROPERTIES OF GAS
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A theory which introduced to define theproperties of gas
Some assumptions need to take note in order
to proceed to calculation Gas composed of molecules that are separated
from distances far to each other
Gas molecules are in constant motion in random
direction and collide to each other frequently. As aresult to this collision, energy can be transferred
from one molecule to another by maintaining the
total energy of the system
KINETIC MOLECULAR THEORYKINETIC MOLECULAR THEORY
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CHM1001 CHEMSTRYACHAPTER 5: Matter and Chemical Bonding
Gas molecules exert neither attractive norrepulsive forces with one another
The movement of the gas molecules are fairly
depends on T, V of the container, P in the
container
The collisions between gas molecules and the
walls of their container produce gas pressure
The gas molecules will be more energeticwhen a higher T is apply
KINETIC MOLECULAR THEORYKINETIC MOLECULAR THEORY
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CHM1001 CHEMSTRYACHAPTER 5: Matter and Chemical Bonding
Important units in calculation Pressure torr = 1mmHg; 1atm = 760mmHg/torr
1atm = 101,325 Pa / 1.01325105 Pa; Pa = pascals
= 1.0132510
2
kPa Temperature 0K = -273.15oC : absolute zero
0oC = 273.15K : Freezing point of water
100 oC = 373.15K : Boiling point of water
X oC = (X+273.15) K; sometime 273K was used
Volume Either liter, L or milliliter, mL
IDEAL GAS EQUATIONIDEAL GAS EQUATION
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Boyles Law: V at constant n and T
Charles Law: V T at constant n and P
Avogadros Law: V n at constant P and T
Since all involve the relationship of V, theexpression can be combine as
V V=R
PV=nRT
where R is the gas constant. Thus STP, R would have the value of0.0821 L atm K-1 mol -1. If the unit ofP is change to Pa or torr thevalue would be 8.3145103 L Pa K-1 mol-1 and 62.3637 L torr K-1 mol-1
respectively.
IDEAL GAS EQUATIONIDEAL GAS EQUATION
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formed between atoms due to the interactionof electrons
Tends to reach stability by fulfilling the
electrons in the valance shell with maximumnumbers of electrons; valance electrons
Have the ability to donate/lose electron,
receive electrons, share electron to form a
certain chemical bond
Form diatomic or polyatomic chemical
compound
CHEMICAL BONDINGCHEMICAL BONDING
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Can classified as strong bonds and weakbond
Strong bond involve sharing or transfer ofelectrons
Weak bond involve forces of attraction
Two main type of strong chemicalbonding: ionic bonding, covalent bonding
Hydrogen bonds and Van der Waals bondare example of weak chemical bond
CHEMICAL BONDINGCHEMICAL BONDING
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interaction between metal and non-metalto form a compound; electron transfer
Electron transfer forms ion; metal loses
electron form cation; non-metal gainelectron form anion
Attracted each other by electrostatic force
Non-metal with higher electronegativitytends to receive electron more rapidly to
form anion
IONIC BONDINGIONIC BONDING
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The larger the difference in electronegativitybetween two atoms, the stronger the ionic
bond
shows the properties below: The name of the metal also comes first followed
by the non-metal when naming the compound
Easily dissolve in water and in polar solvents; can
conduct electricity tend to form crystalline solids with high melting
temperatures and high boiling temperatures
IONIC BONDINGIONIC BONDING
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IONIC BONDINGIONIC BONDING
` Cation smaller than the parent atom; anion larger
than the parent atom
` Due to donation of electron valance of the metal
atom
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IONIC BONDINGIONIC BONDING
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CHM1001 CHEMSTRYACHAPTER 5: Matter and Chemical Bonding
Ionic compound are solid
Arrangement of repeatingunits of ions in a regularand orderly cubic patternin three dimensions with
the same orientation;crystal lattice
The interaction betweenions cause the structure tobe arrange in alternating
pattern
IONIC BONDINGIONIC BONDING
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CHM1001 CHEMSTRYACHAPTER 5: Matter and Chemical Bonding
IONIC BONDINGIONIC BONDING
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CHM1001 CHEMSTRYACHAPTER 5: Matter and Chemical Bonding
sharing of pairs of electrons between twoor more atoms
involve non-metal elements with same
elements or various elements whichdepends on electronegativity
Similar electronegativities promote greater
bonding; have similar electron density;non-polar
Usually no charged ions are form
COVALENT BONDINGCOVALENT BONDING
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COVALENT BONDINGCOVALENT BONDING
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not strongly attract to each other
have the following properties
tends to exist as liquid or gas or sometimes
solid with a very low MP and BPDo not conduct electricity because they are
neutral
Generally insoluble in water
They are volatile
NONNON--POLAR COVALENTPOLAR COVALENT
BONDINGBONDING
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NONNON--POLAR COVALENTPOLAR COVALENT
BONDINGBONDING
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NONNON--POLAR COVALENTPOLAR COVALENT
BONDINGBONDING
Double bonds
Triple bonds
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Have difference of electronegativity value;polar covalent bond
The electron density of the more
electronegative element is higherForm a partial negative charge and partial
positive charge
POLAR COVALENT BONDINGPOLAR COVALENT BONDING
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due to the unequal sharing of electronswhere the more electronegative atom will
attract electrons more stronger
To identify the polarity of the compound,it can be determine by calculating the
differences of the electronegativities values
POLAR COVALENT BONDINGPOLAR COVALENT BONDING
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Sometimes the atom with unbondedelectrons (lone pairs) tend to share with
other element or ion which have a room
to occupy the empty space or those withan incomplete outer shell
Also known as coordinate bond with the
symbol
DATIVE COVALENT BONDDATIVE COVALENT BOND
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DATIVE COVALENT BONDDATIVE COVALENT BOND
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Intramolecular attractions: attraction whichhold an individual atom together; ionic
bond, covalent bond
A molecule tends to attract to each otherwith the neighboring molecules; known as
intermolecular attractions
Van der Waals dipole-dipole attractions and
dispersion forces, hydrogen bond
BONDBOND ATTACTIONATTACTION
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Categorized under Van der Waals forceexist between polar covalent molecule
which due to the unequally distribution of
the electrons; polarizedwas said to have a permanent dipole
where each element are partial charge
=0.9
DIPOLEDIPOLE--DIPOLE ATTRACTIONDIPOLE ATTRACTION
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Due to the existence of dipole, a
molecule tends to attract each otherwith the neighboring molecule butrepel each other with same charge
DIPOLEDIPOLE--DIPOLE ATTRACTIONDIPOLE ATTRACTION
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Non-polar molecule have equally distributed electron but it
will be induced when a polar molecule interacts in the
system
DIPOLEDIPOLE--INDUCED ATTRACTIONINDUCED ATTRACTION
Cl Cl
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At some point, the electrons in the non-polar molecule tends tomove towards one end of the molecule to form a temporary partialcharge since the electrons are mobile; instantaneous dipole
DISPERSION FORCESDISPERSION FORCES
Cl Cl
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DISPERSION FORCESDISPERSION FORCES
When interacts with the other same non-polar molecule, the distribution of
electrons will be distort and the molecule
was said to be induced; temporarydipole/instantaneous induced attraction
Also known as a London force
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Happens in mono-atom Element with a large number of electrons will have larger
instantaneous dipole because the protons in nucleus less
hold up the large numbers of electrons in the outer shell,
so it is freely moved and easily to be polarized
Explains the increase in boiling point of noble gas group
DISPERSION FORCESDISPERSION FORCES
Xe Xe Xe Xe
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a special case of dipole forces whichinvolve molecule with large difference of
electronegativity value
attachment of hydrogen atom with thehighly electronegative atom: oxygen,
nitrogen, or fluorine, which has a partial
negative charge whereas hydrogen has the
partial positive charge
H-F: =1.9; HOH: =1.4; H2NH: =0.9
HYDROGEN BONDHYDROGEN BOND
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HYDROGEN BONDHYDROGEN BOND
The hydrogen on one molecule attached toF, O or N that is attracted to an F, O or N
of a different molecule
The strongest intermolecular attractionhowever, water has higher boiling point
then the others because it can form four
hydrogen bond
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In the case of ammonia, the amount ofhydrogen bonding is limited by the fact thateach nitrogen only has one lone pair wherethere aren't enough lone pairs to go aroundto satisfy all the hydrogens
Whereas in hydrogen fluoride, it has only onehydrogen attach to fluorine causing a shortageof hydrogens which will form only twohydrogen bonds
In water, there are exactly the right number ofeach. Water could be considered as the"perfect" hydrogen bonded system.
HYDROGEN BONDHYDROGEN BOND
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HYDROGEN BONDHYDROGEN BOND
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Properties of hydrogen bond
hold the two strands of the DNAdouble helix together
hold polypeptides together in such
secondary structures as the alpha helixand the beta conformation
help enzymes bind to their substrate;antibodies bind to their antigen
help transcription factors bind to eachother
help transcription factors bind toDNA
HYDROGEN BONDHYDROGEN BOND
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Water is the best example of hydrogen bond withseveral unique properties
Has the capability in dissolving many ioniccompounds Oxygen attaches to positive ions by co-ordinate (dative
covalent) bonds whereas hydrogen bonds to negative ionsusing hydrogen bonds
Known as hydration; the compound was said to behydrated
Heavy water: contain a higher proportionthan normal of the isotope deuterium
Hard water: contain high concentrations ofminerals such as Mg2+, Ca2+
HYDROGEN BONDHYDROGEN BOND
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HYDROGEN BONDHYDROGEN BOND
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HYDROGEN BONDHYDROGEN BOND
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Overlapping of atomic orbitals occursbetween atoms/polyatomic molecules
during formation of covalent bond(s)
Each atomic orbitals in an atom need to beoccupy at least one electron which will be
ready to overlap with another one
electron to form a single covalent bond
Two types of covalent bond: sigma bond
() and pi bond ()
HYBRIDIZATION OF ATOMIC
ORBITALS
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Sigma bond (): formation of covalent bondwhen two atomic orbitals on adjacent atomsoverlaps
Overlapping of one end of an atomic orbital
from one atom to another one end of anatomic orbital from another atom
Can be form by the overlapping of two sorbitals, one s orbital with one p orbital and
two p orbitalsThe electron density at the overlapping area
would be the greatest.
SIGMA BONDSIGMA BOND
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s s s-s overlappingExample: H2
s p s-p overlappingExample: HCl
p p p-p overlappingExample: Cl2
SIGMA BONDSIGMA BOND
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The other two p orbitals in one atom willform covalent bond by overlapping sideby side which known as pi bond giving thesymbol of
Pi bond (): formation of covalent bondwhen two p atomic orbitals areoverlapping sideways
Formation of pi bond are weaker thansigma bond as the bond is loosely held bythe atom nuclei
PI BONDPI BOND
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p p sideways one bond
overlappingExample: ethene
PI BOND
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