1
Q
VSEPR Model
A
Valence shell electron pair repulsion.
Atom with 2 bonds=linear, sp hybridised, 180
3 bonds =trigonal planar, sp2 hybridised, 120
4 bonds= tetrahedral, sp3 hybridised, 109.5
2
Q
2n2
A
No of e- that can occupy a shell
3
Q
Sub-shells s,p,d,f
A
2,6,10,14 e-
4
Q
Orbitals
A
Negative charge clouds within sub-shells
5
Q
Ionic bond
A
Gain-lose relationship. Usually between non-metal+metal
6
Q
Covalent bonding
A
Non-metal e- sharing
7
Q
Metallic bonding
A
Obvious
8
Q
Dipole moment
A
More electronegative=partially negative charge and vice-versa
9
Q
Pi bonds
A
P orbital overlap=above and below the nuclei. Occur in double and triple bonds
10
Q
Sigma bonds
A
Overlap between 2 bonding nuclei. Single bonds only. Less reactive than pi bonds
