Metallic Bonding GCSE Quiz

Do you know how metals bond?

Good Luck!


How do Metals Conduct Electricity?

Metals are able to conduct electricity because when they bond, each atom donates its spare electron’s from its outer shell to a delocalised pool. Since electrons have a charge of -1, electrons in the delocalised pool are able to move and carry a charge. This also explains why metals are good conductors of heat since electrons can also move thermal energy.

When a voltage (potential difference) is applied, the delocalised electrons move in the same direction and an electrical current flows.

Metallic bonding also explains the differences in electrical conductivity between different metals. Metals which are in groups 1, 2 and 3 of the periodic table all have different electrical conductivities because they have contrasting numbers of electrons in their outermost shell. The group number tells us the number of electrons in the outer shell of an element and since all of these electrons are donated to a delocalised pool, metals with a higher group number such as aluminium have a higher conductivity than metals with a lower group number such as sodium.

Metallic bonding GCSE

Why are Metals Malleable?

Metals are malleable because when they bond metallically, they form uniform layers with a delocalised pool of electrons holding the ions together. These layers are strongly attracted to the delocalised pool but not to each other, so it is possible for the layers to slide over each other, rather than crack or break.

The electrostatic bonds between metal ions are very strong and this contributes to their hardness and also their high melting and boiling points. In order to break apart the bonds between the metal ions, lots of energy is required and therefore high temperatures or pressures.

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