Structures

Front 1

Explain an ionic lattice

Back 1

Ionic compounds have a structure described as an ionic lattice.

It is a 3D network of positive and negative ions held together by ionic bonds (electrostatic forces) between the oppositely charged ions.

Front 2

Properties of ionic bonds

Back 2

Crystalline solids, high melting and boiling points, conducts electricity only when molten or dissolved in water, most dissolve in water, don't dissolve in organic substances.

Front 3

Properties of simple covalent substances

Back 3

Low melting and boiling points, don't conduct electricity because there are no charged electrons, mostly insoluble or have low solubility in water.

Front 4

What are the weak forces of attraction between molecules called?

Back 4

'Van der Waal's forces of attraction'.

Front 5

Properties of giant covalent structures

Back 5

No charged ions, all atoms bonded to each other by strong covalent bonds, very high melting and boiling points, don't conduct electricity even when molten (except graphite), usually insoluble in water.

Front 6

What are allotropes?

Back 6

Elements that can exist in two or more different physical form are said to exhibit allotropy, eg. diamond and graphite are allotropes

Front 7

Explain the structure of diamond

Back 7

Each carbon atom forms 4 covalent bonds in a very rigid structure.

Front 8

Properties of diamond

Back 8

Very hard solid because breaking diamond requires breaking many strong bonds, high melting and boiling points because lots of energy needed to break such strong bonds, insoluble in water, doesn't conduct electricity beacause there are no delocalised electrons.

Front 9

Explain the structure of graphite

Back 9

Each carbon atom only forms 3 covalent bonds leaving electrons to wander freely.

Front 10

Properties of graphite

Back 10

Soft slippery solid because the 3 bonds form layers which sre free to slide over each other, feels greasy and can be used to write with on paper, high melting and boiling points because of the 3 strong bonds, insoluble in water, conducts electricity because some delocalised electrons are not used in bonds and are free to wander and carry charge.

Front 11

Properties of metallic bonds

Back 11

Malleable and ductile as the layers can slide over each other without disrupting the bond, high melting and boiling points, good conductor of electricity even when molten because of free electrons that can carry charge about (when a potential difference if applied, they will move together allowing the current to flow).

Front 12

Define alloy

Back 12

A mixture of 2 or more elements, at least one of which is a metal, it has metallic properties.

Front 13

Uses of aluminium

Back 13

Overhead electrical wiring (good conductor of electricity) and alloys for aircrafts (strong and hard).

Front 14

Uses of copper

Back 14

Electrical wiring (good conductor of electricity) plumbing, brass and coinage (doesn't rust)

Front 15

Uses of iron

Back 15

Bridges and structures (strong and hard)

Front 16

Uses of magnesium

Back 16

Flares (burns with a bright white light) and alloys for aircrafts (strong and hard)