Bonding

2BP 0LP

linear

3BP 0LP

trigonal planar

4BP 0LP

tetrahedral

5BP 0LP

trigonal bipyramidal

6BP 0LP

octahedral

3BP 1LP

pyramidal

4BP 1LP

see saw

5BP 1LP

square pyramidal

2BP 2LP

bent

3BP 2LP

T shaped

4BP 2LP

square planar

square planar bond angle

90

T shaped bond angle

90

Tetrahedral bond angle

109.5

V shaped bond angle

104.5

trigonal planar bond angle

120

trigonal pyramidal bond angle

107

square based pyramidal bond angle

88, 89

structure and bonding in graphite

layers of carbons where each carbon is bonded to 3 other carbons, weak VDW between the layers, many strong covalent bonds have to be broken

H bond drawing criteria

180 degrees between H and other molecule, drawn from one lone pair to another, partial charges drawn, H bond is drawn towards a lone pair on FON

explanation of shape

has xBP and xLP, LP repel more than BP, LP repel as much as possible. BP repel as much as possible. BP repel evenly. State shape name and bond angle

H bond definition

There is a large difference in electronegativity between H and FON, leading to H becoming delta positive and FON delta negative. The H bond is the interaction between the delta positive H and the electron rich lone pair on the FON atom.

Electronegativity Definition

the ability of an atom to pull a pair of electrons towards itself in a covalent bond

lone pairs repel extra __

2.5 degrees

why are metals malleable?

they have a regular lattice shape, where all the atoms are the same size, thus layers easily slide over each other.

metals bonding description?

regular lattice of positive metal cations surrounded by a delocalised sea of electrons

Van de Waals forces explanation (3)

1. electron random movement created a temporary dipole in a molecule

2. this induces a dipole in neighbouring molecules

3. the delta positive/negative molecules attract

why is something not polar?

molecule is symmetrical, dipoles cancel out