Title: Chapter 1. ATOMIC STRUCTURE AND THE PERIODIC TABLE
1Chapter 5 CHEMICAL BONDS AND MOLECULAR
STRUCTURE
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4Electronegativity
- Pauling Scale
- relative attraction of an atom for electrons, its
own and those of other atoms - same trends as ionization energy, increases from
lower left corner to the upper right corner - fluorine E.N. 4.0
5Electronegativities of the Elements
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7Chemical Bond Properties
- Non-polar bonds diff. EN 0
- Polar bonds diff. EN gt 0
- Ionic bonds diff. EN gt 1.5
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17Ionic Compounds
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29Covalent Bonding
- Sharing of electrons
- HH
- H-H
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31 Compare O-O and OO. Is OO expected to be
stronger, weaker, or the same strength?
32- Is OO expected to be
- longer, shorter, or the same length?
33Shell Model of the Atom
- G.N.Lewis
- 1875-1946
- American Chemist
- Lewis Symbol
- valence shell electrons Group A
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35Lewis Electron Dot Symbols
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38Lewis Structures
- Octet Rule
- In compound formation an atom gains or loses
electrons, or shares pairs of electrons, until
its valence shell has eight electrons.
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49Lewis Structures
CH4 methane
C2H6 ethane
50Multiple Covalent Bonds
- Double bond 2 pairs shared
- Triple bond 3 pairs shared
- Normally occurs between
- C atoms N atoms O atoms
- a C atom and a N, O or S atom
- a N atom and a O or S atom
- a S atom and an O atom
51Multiple Covalent Bonds
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78Shape PCl3
- Lewis Electron Dot Structure
.. .. .. Cl P Cl .. .. ..
Cl ..
3 bond pairs
1 lone pair gt AB3E
trigonal pyramidal shape
79Shape IF5
- Lewis Electron Dot Structure
- .. ..
- F F
- .. .. ..
- I F
- ..
- .. ..
- F F
- .. ..
5 bonds pairs
1 lone pair gt AB5E
Square pyramidal shaped
80Shape IF4-1
- Lewis Electron Dot Structure
- .. .. -1
- F F
- .. .. ..
- I F
- ..
- .. ..
- F
- ..
4 bond pairs 2 lone pairs gt AB4E2 square planar
shape
81Shape SO3
- Lewis Electron Dot Structure
- ..
- O S O
- .. .. ..
- O
- ..
- 3 bond pairs
- 0 lone pairs gt AB3
- trigonal planar shape
82- What would be expected to be the shape of
chloroform, CHCl3? - see-saw
- square planar
- tetrahedral
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95- Carbon monoxide, CO and carbon dioxide, CO2, are
linear molecules. Which one is the polar
molecule - CO
- CO2
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98Potential Energy Curve for H2
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116- What would be the name of the hybrid orbitals
created by joining 1s type, 3 p type and 2 d type
orbitals? - spd
- sp3d2
- s3p2d
117Sigma Bond s
- Bond with the greatest electron density on a
line connecting the atomic nuclei - s-s type p-p type s-p type
- s-sp3 type s-sp2 type s-sp type
- p-sp3 type p-sp2 type p-sp type
- sp3 - sp3 type sp2-sp2 type sp - sp type
- etc., including all combinations of s, p, d, and
hybrid orbitals
118Pi Bond p
- Bond with the greatest electron density above
and below a line connecting the atomic nuclei - p-p type
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120Bonding in Ethylene
121Bonding in Acetylene
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127Molecular Orbital Diagram
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132Molecular Orbital Diagram
133Molecular Orbital Diagram
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146Dipole-Dipole Forces
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148London (Dispersion) Forces
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151Hydrogen Bonds
152Hydrogen Bonds
153Bonding in Water
154- Water, H2O, and methane, CH4, have very similar
molar masses yet the boiling point for water is
approximately 200oC higher than that for methane.
The higher boiling point is due to - hydrogen bonding in water
- polarity of water molecules
- both of the above
- none of the above
155Structure of Ice