Ionisation Energy

Question 1

What is the trend down the group in first ionisation energy?

Answer 1

-The atoms get bigger so there is a larger atomic radius and more shielding so there is a weaker attraction to the nucules from the outer shell.

Question 2

Why is there a decrease from magnesium to aluminium in first ionisation?

Answer 2

-The first electron removed in aluminium is in 3p as 3p is higher in energy so the electron is easier to remove.

Question 3

What is first ionisation energy?

Answer 3

The minimum amount of energy required to remove 1 mole of electrons from 1 mole of gaseous atoms to form 1 mole of gaseous ions under standard conditions.

Question 4

What is the equation for first ionisation energy?

Answer 4

M(g)——>M+ + e-

Question 5

Why is there a decrease from phosphorus to sulfur in first ionisation energy?

Answer 5

Sulfur has the first example of spin repulsion in 3p (electrons repelling)

Question 6

What is the atomic radius?

Answer 6

-Increases down a group
-Decreases across a period.

Question 7

What is the general trend of the first ionisation energy graph?

Answer 7

-It increases
-This is because the nucular charge increases but the atomic radius does not.

Question 8

What is shielding?

Answer 8

-When electrons near the nucules ‘block’ the force of attraction from other electrons so outer electrons will be taken away and are easier to take asway.