3.1 - The periodic table

Question 1

Define “first Ionisation Energy (1st I.E.)” of an element.

Answer 1

The energy required to remove ONE ELECTRON from ONE MOLE OF ATOMS in a GASEOUS STATE.

Question 2

What are the 3 factors affecting ionisation energy

Answer 2

1. Atomic Radius
2. Nuclear Charge
3. Electron shielding

Question 3

Describe the trend of Atomic Radius.

Answer 3

The LARGER the atomic radius, the SMALLER the nuclear attraction experienced by the outer electrons.

Question 4

EXPLAIN the trend of Atomic Radius.

Answer 4

The positive charge of the nucleus is essentially further away from the outermost electron.

Question 5

Describe the trend of the Nuclear charge.

Answer 5

The HIGHER the nuclear charge, the LARGER the attractive force on the outer electrons.

Question 6

Describe Electron Shielding.

Answer 6

Inner shells of electrons repel the outer-shell electrons because they are all negative.

Question 7

Describe the trend of Electron Shielding.

Answer 7

The more inner shells there are, the larger the shielding effect and the smaller the nuclear attraction experienced by the outer electrons.

Question 8

Why is each successive ionisation energy higher than th one before?

Answer 8

As each electron is removed, there is less repulsion between the remaining electrons and each shell will be drawn in slightly closer to the nucleus.