Periodicity- Ionisation Energies 3.7.2

Question 1

first ionisation energy definition

Answer 1

The energy required to remove one electron from each atom in one mole of gaseous atoms
Na (g) -> Na+ (g) + e-

Question 2

What factors affect ionisation energy?

Answer 2

Nuclear charge, Atomic radius and Shielding

Question 3

What happens if there’s pairs in a sub level?

Answer 3

The paired electrons repel/push other electrons away making it easier to remove, decreasing the ionisation energy.

Question 4

What happens to ionisation energy as you go up a group?

Answer 4

The IE increases - closer to nucleus, less shielding

Question 5

What happens to ionisation energy across a period?

Answer 5

The nuclear charge increases as you across north the group and the atomic radius decreases, there is a greater attraction between the nucleus and outer electrons so IE would increase.

Question 6

What is outweighed with first ionisation energies down a group?

Answer 6

Although nuclear charge increases its effect is outweighed by the increased radius and to a lesser extent, the increased shielding.