Group 1 And 2

Question 1

Why does reactivity in group 2 increase as you go down the group?

Answer 1

The lower their first and second ionisation energies, the more likely they are to lose their electrons, so the more reactive they are.

Question 2

Metal+water➡️?

Answer 2

Metal hydroxide and hydrogen

M+2h2O➡️ M(OH)2 + H2

Question 3

Metal+oxides➡️? (burn in oxygen)

Answer 3

White solid oxides

2M+O2➡️ 2MO

Question 4

Metal+chlorine➡️?

Answer 4

White solid chlorides

M + Cl2➡️ MCl2

Question 5

Why do the oxides in group 2 form stringer alkaline solutions as they go down the group?

Answer 5

The hydroxides formed get more soluable.

Question 6

Why will both oxides and hydroxides of group 2 neutralise dilute acids? What will they form?

Answer 6

They’re bases. They will form solutions of corresponding salts.

Question 7

What are the trends for singly charged negative ions in solubility in group 2?

Answer 7

Solubility increases down the group. (ie. OH-)

Question 8

What are the trends in double charged negative ions in solubility in group 2?

Answer 8

Decrease down the group. (ie. SO4 2-)

Question 9

Why does the ionisation energy of group 2 decrease as go down the group?

Answer 9

More shielding so less a attraction to positive nucleus, electrons further away which reduces the electrostatic attraction between nucleus and outer electrons, easier it is to remove.