Group 2 Metals

Question 1

Describe reactivity as you go down group 2

Answer 1

• in group 2, reactivity increases down the group
• more shells, more shielding, more electrons
• weaker forces of attraction between positive nucleus and outer electrons
• therefore it is easier to lose an electron
• therefore reactivity increases

Question 2

Describe ionisation energy as you go down group 2

Answer 2

• atomic radius increases
• more electrons, more shells, more shielding
• weaker forces of attraction between outer electron and positive nucleus
• ionisation energy decreases as you go down the group

Question 3

Describe the melting point of group 2 down the group

Answer 3

• melting point decreases as you go down the group
• weaker metallic bonding as you go down the group
• metallic bonding gets weaker as the size of the atom (ion) gets bigger
• weaker forces of attraction between the outer electron and the nucleus
• therefore melting points decreases

Question 4

When group 2 metals react with water, what do they produce?

Answer 4

Metal hydroxide and hydrogen

Question 5

Describe the effect of steam on the reaction between magnesium and water

Answer 5

• Mg reacts very slowly with water
• reaction can be faster with steam
• as it provides extra energy
• when steam is used, Mg burns with a bright white flame to form hydrogen and magnesium oxide, a white powder

Question 6

Describe the solubility of hydroxides down group 2

Answer 6

• solubility of hydroxides increases down the group
• meaning magnesium hydroxide is the least soluble and barium hydroxide is the most soluble

Question 7

Describe the solubility of sulfates down group 2

Answer 7

• solubility of group 2 sulfates decreases down the group
• meaning magnesium sulfate is most soluble and barium sulfate is least soluble

Question 8

Describe the tests for cations in group 2

Give observations

Answer 8

Can be identified with a series of flame tests

Calcium - brick red
Strontium - red
Barium - pale green