Summary of different types of compound and their properties

SUBSTANCE	Nature of bonding	Physical properties
IONIC Eg NaCl	Attraction between oppositely charged ions. Infinite lattice of oppositely charged ions in three dimensions	High mpt, bpt Good conductors in liquid state Poor conductors in solid state Hard, strong, brittle
METALLIC Eg Mg	Attraction between cations and delocalised electrons. Infinite lattice of cations in three dimensions, with delocalized electrons in the spaces	High mpt, bpt Good conductors in solid state Good conductors in liquid state Strong, malleable
GIANT COVALENT Eg diamond	Infinite lattice of atoms linked by covalent bonds in three dimensions. Covalent bonds are pairs of electrons shared between two atoms	Very high mpt, bpt Poor conductors in solid state Poor conductors in liquid state Hard, strong, brittle
MOLECULAR Eg I2	Discrete molecules. Atoms in molecule linked by covalent bonds. (s or p, normal or dative) Weak intermolecular forces between molecules.	Low mpt, bpt Poor conductors in solid state Poor conductors in liquid state Soft, weak, powdery
GIANT COVALENT LAYERED Eg graphite	Infinite lattice of atoms linked by covalent bonds in two dimensions to form planes. Planes held together by intermolecular forces. Delocalised electrons in between layers	High mpt, bpt Good conductors parallel to planes Poor conductors perpendicular to planes Soft

 

Don’t forget to learn the structures of

 

• Sodium chloride

• Iodine

• Diamond

• Graphite

MOLECULAR SHAPES

When an atom forms a covalent bond with another atom, the electrons in the different bonds and the non-bonding electrons in the outer shell all behave as negatively charged clouds and repel each other. In order to minimise this repulsion, all the outer shell electrons spread out as far apart in space as possible.

 

Molecular shapes and the angles between bonds can be predicted by the VSEPR theory

VSEPR = valence shell electron pair repulsion

 

VSEPR theory consists of two basic rules:

 

i) All s-bonded electron pairs and all lone pairs arrange themselves as far apart in space as is possible. p-bonded electron pairs are excluded.

ii) Lone pairs repel more strongly than bonding pairs.

 

These two rules can be used to predict the shape of any covalent molecule or ion, and the angles between the bonds.

 

A) 2 electron pairs

 

If there are two electron pairs on the central atom, the angle between the bonds is 180^o.

 

 

Molecules which adopt this shape are said to be LINEAR.

E.g. BeCl₂, CO₂