Periodicity

Question 1

What factors affect ionisation energy?

Answer 1

Nuclear charge, atomic radii and electron shielding

Question 2

How does atomic radius affect ionisation energy?

Answer 2

The greater the distance between the nucleus and the outer electron the less the nuclear attraction

Question 3

How does nuclear charge affect the ionisation energy?

Answer 3

The more protons there are in the nucleus of an atom, the greater the attraction between the nucleus and the outer electron

Question 4

How does electron shielding affect the ionisation energy?

Answer 4

Electrons are negatively charged so inner shell electrons repel the outer electrons (shielding effect), so the attraction between the nucleus and outer electrons is reduced

Question 5

Why does ionisation energy decrease down the noble gases?

Answer 5

Atomic radius increases, shielding increases and nuclear attraction on outer electrons decreases

Question 6

Why is there an increase in ionisation energy across period 2?

Answer 6

Nuclear charge increases, same shell so similar shielding, nuclear attraction increases and atomic radii decreases

Question 7

What elements can form giant covalent lattices?

Answer 7

Carbon, silicon and boron

Question 8

What is the trend in solubility of group 2 hydroxides moving down the group?

Answer 8

Increases down the group, so the resulting solution contains more OH- ions and becomes more alkaline

Question 9

What’s an example of group 2 compounds use in agriculture?

Answer 9

Calcium hydroxide is used to increase pH of acidic soils

Question 10

What’s an example of group 2 compounds in medicine?

Answer 10

Magnesium hydroxide and calcium carbonate can be sued to neutralise stomach acid