Chp1 Ochem
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1
Ionic bonding
transfer of electrons between metal and non-metal
2
Covalent bonding
relative equal sharing of electrons between two atoms
3
Lewis Structure Basic Rules
1. Determine total valance e-
2. Place atoms and make bonds
3. subtract bond # from total e-
4. Place remaining valence e-
2. Place atoms and make bonds
3. subtract bond # from total e-
4. Place remaining valence e-
4
How many bonds does carbon want to make
4
5
3 classes of bonding
ionic
polar covalent
nonpolar covalent
polar covalent
nonpolar covalent
6
What what electronegativity difference do polar covalent bonds arise at
0.5 - 2
Ionic > 2
Covalent < 0.5
Ionic > 2
Covalent < 0.5
7
inductive effect (polarity of a bond)
shifting of electrons in a bond toward the more electronegative atom
8
Dipole moment aka
The polarity of a molecule
The vector sum of all bond polarities inside a molecule
The vector sum of all bond polarities inside a molecule
9
Common atoms that create inductive effects when bonded to carbon
O, N, F, Cl, Br (towards these atoms)
10
Sp3
4 groups around the atom
Group (atom or lone PAIR)
Group (atom or lone PAIR)
11
Sp2
3 groups around the atom
12
Sp
1 group around the atom
13
Tetrahedral bond angle
109.5 degrees
14
Formal charge hack
difference between wanted valence electrons and (bond + number of existing valence electrons in molecule)
15
Relative importance of Resonance Structure
1. Identical Resonance (in benzenes)
2. Minimize charges
3. Complete Octets
4. Negative charge on more electronegative atom
2. Minimize charges
3. Complete Octets
4. Negative charge on more electronegative atom
16
what does strength of acid increase respective of
electronegativity and size of bonded atom (to hydrogen)
17
What polar effects effect acid strength
Resonance
Inductive Effects
Hybridization
Inductive Effects
Hybridization
18
Sp2 trigonal planar rule
if lone pair on an atom is one space away from a pi bond, it does not contribute to hybridization
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