Chemical Bonding I: Basic Concepts

1
Chemical Bonding IBasic Concepts

• Chapter 9

2
Valence electrons are the outer shell electrons
of an atom. The valence electrons are the
electrons that particpate in chemical bonding.
9.1
3
9.1
4
The Ionic Bond
He
Ne
1s22s1
1s22s22p5
1s2
1s22s22p6
9.2
5
Electrostatic (Lattice) Energy
Lattice energy (E) is the energy required to
completely separate one mole of a solid ionic
compound into gaseous ions.
Q is the charge on the cation
Q- is the charge on the anion
r is the distance between the ions
Lattice energy (E) increases as Q increases
and/or as r decreases.
r F lt r Cl
9.3
6
Born-Haber Cycle for Determining Lattice Energy
9.3
7
A covalent bond is a chemical bond in which two
or more electrons are shared by two atoms.
Lewis structure of F2
9.4
8
Lewis structure of water


Double bond two atoms share two pairs of
electrons
or
Triple bond two atoms share three pairs of
electrons
or
9.4
9
Lengths of Covalent Bonds
Bond Lengths Triple bond lt Double Bond lt Single
Bond
9.4
10
Comparison of Ionic and Covalent Compounds
9.4
11
Polar covalent bond or polar bond is a covalent
bond with greater electron density around one of
the two atoms
electron rich region
electron poor region
e- rich
e- poor
d
d-
9.5
12
Electronegativity is the ability of an atom to
attract electrons toward itself in a chemical
bond.
Electron Affinity - measurable, Cl is highest
Electronegativity - relative, F is highest
9.5
13
9.5
14
Classification of bonds by difference in
electronegativity
Difference
Bond Type
0
Covalent
? 2
Ionic
0 lt and lt2
Polar Covalent
9.5
15
Cs 0.7
Cl 3.0
3.0 0.7 2.3
Ionic
H 2.1
S 2.5
2.5 2.1 0.4
Polar Covalent
N 3.0
N 3.0
3.0 3.0 0
Covalent
9.5
16
Writing Lewis Structures

• Draw skeletal structure of compound showing what
  atoms are bonded to each other. Put least
  electronegative element in the center.
• Count total number of valence e-. Add 1 for each
  negative charge. Subtract 1 for each positive
  charge.
• Complete an octet for all atoms except hydrogen
• If structure contains too many electrons, form
  double and triple bonds on central atom as needed.

9.6
17
Step 1 N is less electronegative than F, put N
in center
Step 2 Count valence electrons N - 5 (2s22p3)
and F - 7 (2s22p5)
5 (3 x 7) 26 valence electrons
Step 3 Draw single bonds between N and F atoms
and complete octet on N and F
atoms.
Step 4 - Check, are of e- in structure equal
to number of valence e- ?
3 single bonds (3x2) 10 lone pairs (10x2) 26
valence electrons
9.6
18
Step 1 C is less electronegative than O, put C
in center
Step 2 Count valence electrons C - 4 (2s22p2)
and O - 6 (2s22p4) -2 charge 2e-
4 (3 x 6) 2 24 valence electrons
Step 3 Draw single bonds between C and O atoms
and complete octet on C and O
atoms.
Step 4 - Check, are of e- in structure equal
to number of valence e- ?
3 single bonds (3x2) 10 lone pairs (10x2) 26
valence electrons
Step 5 - Too many electrons, form double bond
and re-check of e-
9.6
19
Two possible skeletal structures of formaldehyde
(CH2O)
An atoms formal charge is the difference between
the valence electrons in an isolated atom and the
number of electrons assigned to that atom in a
Lewis structure.
The sum of the formal charges of the atoms in a
molecule or ion must equal the charge on the
molecule or ion.
9.7
20
-1
1
formal charge on C
4 -
2 -
½ x 6 -1
formal charge on O
6 -
2 -
½ x 6 1
9.7
21
0
0
formal charge on C
4 -
0 -
½ x 8 0
formal charge on O
6 -
4 -
½ x 4 0
9.7
22
Formal Charge and Lewis Structures

• For neutral molecules, a Lewis structure in which
  there are no formal charges is preferable to one
  in which formal charges are present.
• Lewis structures with large formal charges are
  less plausible than those with small formal
  charges.
• Among Lewis structures having similar
  distributions of formal charges, the most
  plausible structure is the one in which negative
  formal charges are placed on the more
  electronegative atoms.

9.7
23
A resonance structure is one of two or more Lewis
structures for a single molecule that cannot be
represented accurately by only one Lewis
structure.
9.8
24
Exceptions to the Octet Rule
The Incomplete Octet
BeH2
BF3
9.9
25
Exceptions to the Octet Rule
Odd-Electron Molecules
NO
The Expanded Octet (central atom with principal
quantum number n gt 2)
SF6
9.9
26
The enthalpy change required to break a
particular bond in one mole of gaseous molecules
is the bond energy.
Bond Energy
9.10
27
Average bond energy in polyatomic molecules
9.10
28
Bond Energies (BE) and Enthalpy changes in
reactions
Imagine reaction proceeding by breaking all bonds
in the reactants and then using the gaseous atoms
to form all the bonds in the products.
DH0 total energy input total energy released
SBE(reactants) SBE(products)
9.10
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DH0 SBE(reactants) SBE(products)
DH0 436.4 156.9 2 x 568.2 -543.1 kJ
9.10