As Chemistry

Electronegativity

A measure of the attraction of a bonded atom for the pair of electrons in a covalent bond

Covalent bond

A bond formed by a shared pair of electrons

A bond between non- metals

Double covalent bond

2 atoms share 2 pairs of electrons

Ionic bond

The electrostatic attraction between oppositely charged ions.

A bond between Metallic and non metalic

Metallic bond

The electrostatic attraction between positive metal ions and delocalised electrons

A bond between metallic and metallic

Noble gases

Group 8

Stable electon configuration

Giant ionic lattices

-will not conduct electricity when solid as there are no free ions.
- When molten they will conduct electricity as the ions are now free and able to carry a charge.

NO2+

Nitrate

C03 2+

Carbonate

SO4 2-

Sulphate

NH4+

Ammonium

Dative covalent bonding

A shared pair of electrons that has been provided by one atom.

Examples of compounds that do not obey the octet rule:

Sulfur hexaflouride, SF6

Lone pairs of electrons

repel more than bonded pairs

Intramolecular bonds
(i.e intranet)

Covalent
Ionic
Metallic

Intermolecular bonds
(i.e internet)

Hydrogen bonds
v.d.w forces
Permanent dipole- permanent dipole

Van de Waals forces

Very weak attractive forces between induced dipoles in neighbouring molecules

Hydrogen bonds

A strong dipole-dipole attraction between an electron defficient hydrogen atom on one molecule and a lone pair of electrons on a highly electronegative atom on a different molecule.

Hydrogen

is not electronegative. It can attach to lone pairs of electrons.

properties of water resulting in hydrogen bonding

- ice less dense than water because ice has an open lattice with the Hydrogen bonds holding the water molecules apart.

Covalent lattice

Diamond
Graphite

-

Linear

180 degrees

-

Non-linear

104.5 degrees

-

Trigonal planar

120 degrees

-

Triangular pyramidal

107 degrees

-

Tetrahedral

109.5

-

Trigonal bipyramidial

120 + 90 degrees

-

Octahedral

90 degrees