structure and bonding

what atoms does ionic bonding concern

One positive metal ion(cation) and one negative ion(anion)

Define ionic bonding

the electrostatic attraction between oppositely charged ions.

Describe ionic bonding

When one or more electrons are transferred from a metal atom to a non-metal atom to give them both full shells. Metal atom loses electrons(oxidation). The non-metal atom gains electrons(reduction).

What type of attraction is ionic bonding

Strong electrostatic attraction between positive and negative ions.

Give the properties of ionic compounds

• High melting and boiling point

Usually solid at room temp. Lots of energy required to break the forces between the ions

• Soluble in water

The positive ions can be pulled away from the structure by the negative end of the water molecule and vice versa, breaking the structure.

• Conduct electricity when molten or in solution

When molten, the ions move freely therefore can carry a charge and create a current. When solid, the ions are locked in a lattice

• Ionic crystal shatter easily

Layers can slip over one another when a force is applied to the structure. When they slip, similar charges may be next to each other, which results in repulsion, shattering the structure.

What type of structure do ionic compounds form

giant ionic lattice

What is a covalent bond

A shared pair of electrons between two atoms

what is the equations for number of covalent bonds

number of bonds = 8 - number of outer shell electrons

give properties of simple covalent molecules

• simple structure

• usually liquid or gas at room temp

• Atoms held together by strong bonds

• molecules held together by weak intermolecular forces

• low solubility in water, don’t contains ions.

• don’t conduct electricity when molten. Don’t contain ions

describe the structure of giant covalent molecules

Contain strong covalent bonds between many atoms. 3D structure know as a giant covalent lattice.

properties of giant covalent structures

• high melting and boiling points

• atoms held together by very strong covalent bonds

• low solubility

• don’t conduct electricity when molten

Describe metallic bonding

The outer electronic become free to move around the structure. They become delocalised. Thus keacea a structure of metal ions surrounded by a sea of delocalised electrons. It is the strong electrostatic attraction between positive metal ions and a seas of delocalised electrons

Properties of metallic structures

High melting andboiling points

Good conductors of electricity and heat- electrons can move through the structure

Metals are malleable and ductile -layers can slide over one another

Can be made into alloys

Why are alloys less maleablethan metal structures

The larger atoms in an alloy disrupt the structure, meaning th layers don’t slide over each other

What is graphene

A single layer of graphite(one atom thick)

What is fullerene

Layers of graphene in a hollow 3d shape

Uses of nanotubes

Drug delivery into body

Good catalysts

Used in circuits

What is the size range of nanoparticles

1-100nm

Size range of fine particles

100-2500nm

Size range of coarse particles

2500-10000nm

Magnesium ion symbol

Mg²+

Sulphate ion symbol

SO4²-

Chlorine ion symbol

Cl-

Carbonate ion symbol

Co3²-

Ammonium ion symbol

NH4+

Copper ion symbol

Cu²+

Aluminium ion symbol

Al³+