Topic 4.1.1 - Trends in group 2 elements

Question 1

What happens to reactivity as you descend group 2?

Answer 1

Increases

Question 2

Why does reactivity increase down group 2?

Answer 2

Atomic radii increases so decreases forces of attraction between positive nuclei and electrons. So easier to remove electrons.

Question 3

definition for first ionisation energy.

Answer 3

The energy required to remove an electron from each atom in one mole of atoms in the gaseous state.

Question 4

Definition for second ionisation energy.

Answer 4

The energy required to remove an electron from each singly charged ion in one mole of positive ions in the gaseous state.

Question 5

What force does ionisation energy need to overcome?

Answer 5

The electrostatic forces of attraction between the electron being removed and the protons in the nucleus.

Question 6

What happens to ionisation energy as you descend group 2 and why does this happen?

Answer 6

Decreases
Ionic radius increases and so there is less attraction between electron being removed and positive nuclei.

Question 7

Factors that effect ionisation energy.

Answer 7

Nuclear charge
Electron shielding
The orbital in which the electron exists.

Question 8

Describe electron shielding.

Answer 8

The repulsion between filled inner shells and the electron being removed.
As number of filled shells increases, the repulsion on the electron being removed increases.