04 - Ionisation

Question 1

Between which electron and the nucleus is the force of attraction the weakest

Answer 1

Sodium [the furthest one away]

Question 2

Ionisation

Answer 2

when an atom loses an electron from its outer shell

Question 3

First Ionisation energy

Answer 3

The energy required to remove 1 electron from each atom in one mole of gaseous atoms of an element to form one mole of gaseous 1+ ions

Question 4

Atomic Radias pattern on a periodic table

Answer 4

Increases down a group
decreases across a period

Question 5

First ionisation energy pattern

Answer 5

Increases across a period
decreases down a group

Question 6

Nuclear charge patterm
attraction of electrons to the nucleus pattern

Answer 6

The nuclear charge increases across a period - each successive element has one more proton than the last.
- Therefore, attraction of electrons to the nucleus increases.
- Atomic radius decreases [so electrons are closer to the nucleus].

Question 7

Ionisation energy increase

Answer 7

There is a large increase in ionisation energy when it removes an electron from the shell below. This is because these electrons are closer to the nucleus and there is less sheilding.

Question 8

How do ionisation energies vary across a period

Answer 8

They increase

Question 9

Reasons ionisation energy decreases down a group

Answer 9

• The atomic radius increases
• There is increased sheilding

Question 10

In which state, solid, liquid or gas are ionisation energies measured

Answer 10

Gas