Properties of Metals

1. Why do metals have similar properties because of this structure?

The structure of positive ions and free electrons creates a 'sea' of delocalised electrons, causing them to be good conductors of electricity/insoluble/malleable.
The structure of positive ions and free electrons creates a 'sea' of delocalised ions, causing them to be bad conductors of electricity/soluble/malleable.
The structure of negative atoms and free electrons creates a 'sea' of delocalised atoms that bounce into each other and spread things, meaning the properties are the same as the atoms function the same in all metals.

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They have high melting points and form very colourful compounds.
They have low melting points and are all poisonous solids and liquids at room temperature.
They have very high melting and boiling points and form very reactive compounds.
They are very soft and can be cut with a knife and form colourless compounds.

Metals are found on the right and middle of the table as most elements are metals so they take up a lot of room.
Metals are on the left and right of the table, but most elements aren't metals so they don't take up much space.
Metals are on the left and middle of the table, as most elements are metal so they take up a lot of space.
Metals cover the whole of the table, as all of the elements are metals.

They consist of a regular arrangement of atoms held together with ionic bonds.
They consist of a regular lattice structure resulting in a giant structure of negative ions and trapped electrons.
They consist of a regular arrangement of atoms held together with metallic bonds.
They consist of an irregular arrangement of ions held together with metallic bonds.

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