ionic bonding

Question 1

Why are metals such good conductors of heat and electricity?

Answer 1

In solid metal, the metal atoms lose their outer electrons. These electrons become delocalised (i.e. they can move around freely within the metal) and the metal atoms become positively charged ions.

Question 2

What is the regular 3D pattern that is used to describe the shape of themetal ions

Answer 2

lattice

Question 3

How is a metal held together?

Answer 3

by the strongelectrostatic attractionbetween the positive metal ions and the negative electrons. This attraction can be referred to as metallic bonding.

Question 4

Strong

Answer 4

metals cannot easily be broken due to the strong metallic bonds (i.e. the electrostatic attraction between the positive metal ions and the delocalised electrons).

Question 5

High melting and boiling points

Answer 5

a lot of heat energy is required to break the strong metallic bonds (i.e. the electrostatic attraction between the positive metal ions and the delocalised electrons).

Question 6

Good electrical and thermal conductivity

Answer 6

the delocalised electrons can carry heat and electrical energy from one part of the metal to another as they are free to move.

Question 7

Malleable

Answer 7

metals can be bent or hammered into different permanent shapes because the electrons move when the metal ions move. The metallic bonding remains intact as the ion layers slide over each other.

Question 8

Ductile

Answer 8

metals can be stretched out into wires because the electrons move when the metal ions move. This keeps the metallic bonding intact as the layers of metal ions slide over each other.

Question 9

Insoluble in water

Answer 9

metals do not dissolve in water as the metallic bonding is very strong and so cannot be broken apart by water.

Question 10

Shiny

Answer 10

unreacted metals have a shiny surface and so can be used in jewellery. However, some metals can appear dull as they react with oxygen from the air forming a dull metal oxide layer.