C4 - Group 1 elements
- Created by: Naomi
- Created on: 23-01-13 19:29
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- The group 1 elements
- Properties of alkali metals
- React vigorously with water and give off hydrogen gas
- The metal reacts with water to form an alkali - the hydroxide of the metal
- Reactivity of the alkali metals with water increases down group 1
- Potassium is more reactive than sodium
- Sodium is more reactive than lithium
- The group 1 metals are:
- Lithium
- Sodium
- Potassium
- Rubidium
- Caesium
- Francium
- Explaining reactivity patterns
- Atoms of group 1 have similar properties because they have one electron in their outer shell
- Atoms of alkali metals react, losing one electron and forming:
- A full outer shell, to create a stable electronic structure
- An ion, which has one more positive charge in its nucleus than negative electrons in the shells, so it becomes a positive ion
- The more shells the atom has the more weakly attracted the electrons are to the nucleus, so are easily lost
- That is why atoms in the lower periods are more reactive than the ones in the higher periods
- The easier it is for an atom to lose an electron the more reactive it is
- The easier it is for an atom to lose an electron the more reactive it is
- That is why atoms in the lower periods are more reactive than the ones in the higher periods
- If electrons are lost, the process is called reduction
- A flame test can be used to find out if lithium, sodium or potassium are present in a compound
- Lithium burns red
- Sodium burns yellow
- Potassium burns lilac
- Properties of alkali metals
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