Download - POLARITY
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POLARITY
POLAR BONDS Bonds between atoms
POLAR MOLECULES Polarity between molecules Occurs when polar bonds create a dipole moment
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Bond Polarity
HCl is POLAR because it has a positive end and a negative end.
Cl has a greater share in bonding electrons than does H.
Cl has slight negative charge (-d) and H has slight positive charge (+ d)
H Cl••
••
+d -d••
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Bond PolarityWhich bond is more polar (or DIPOLAR)? O—H O—F 3.5 - 2.1 3.5 - 4.0 1.4 0.5 OH is more polar than OF
and polarity is “reversed.”
O H+d-d
O F+d -d
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Molecular PolarityMolecules—such as HCl and H2O— can be POLAR
(or dipolar). They have a DIPOLE MOMENT. The polar HCl
molecule will turn to align with an electric field.
Figure 9.15
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Molecular PolarityMolecules will be polar ifa)bonds are polar ANDb)the molecule is NOT “symmetric”
All above are NOT polar
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Polar or Nonpolar?Compare CO2 and H2O. Which one is polar?
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Polar or Nonpolar?• Consider AB3 molecules: BF3, Cl2CO, and NH3.
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Molecular Polarity, BF3 F
F FB
B atom is positive and F atoms are negative.
B—F bonds in BF3 are polar.
But molecule is symmetrical and NOT polar
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Molecular Polarity, HBF2B atom is positive but H & F atoms are negative.
H
F FB
B—F and B—H bonds in HBF2 are polar. But molecule is NOT symmetrical and is polar.
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Is Methane, CH4, Polar?
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Is CH3F Polar?
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BONDING/FORCES• INTRAMOLECULAR FORCES
– Ionic– Covalent– Metallic
• INTERMOLECULAR FORCES– Van der Waal’s Forces
• London dispersion• Dipole-Dipole• Hydrogen Bonding
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Bonding, Intermolecular Forces (IMF)
IMF < intramolecular forces (covalent, metallic, ionic bonds)
IMF strength: solids > liquids > gases Boiling points and melting points are good
indicators of relative IMF strength.
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Summary of IMF
Van der Waals forces
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Types of Crystalline Solids
Type Particles Forces Notable properties
Examples
Atomic Atoms London dispersion
Poor conductors
Very low MP
Ar (s),Kr (s)
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Type Particles Forces Notable
propertiesExample
s
Molecular
Molecules
(polar or non-
polar)
London dispersion, dipole-
dipole, H-bonds
Poor conductors
Low to moderate MP
CO2 (s),C12H22O11,H2O (s)
SucroseCarbon dioxide (dry ice)Ice
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Type Particles Forces Notable
properties Examples
Ionic
Anions and
CationsElectrostatic attractions
Hard & brittle
High MPPoor conductors
Some solubility in H2O
NaCl,Ca(NO3)2
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Type Particles Forces Notable
properties Examples
Covalent (a.k.a.
covalent network)
Atoms bonded
in a covalent network
Covalent bonds
Very hardVery high MP
Generally insoluble
Variable conductivity
C (diamond
& graphite)
SiO2 (quartz)
Ge, Si, SiC, BN
DiamondGraphite
SiO2
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Type Particles Forces Notable properties
Examples
Metallic
Metal cations in a diffuse, delocalized e- cloud /
sea of e-
Metallic bonds
Excellent conductors
MalleableDuctileHigh but wide range of MP
Cu, Al, Fe
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