Topic 1- Atomic Structure And Periodic Table

Question 1

Define first ionisation energy

Answer 1

The energy required to remove one mole of electrons from one mole of gaseous atoms to form one mole of positive gaseous ions.

Question 2

explain why Mg has a higher ionisation energy than Na?

Make reference to nuclear charge, shielding and attraction.

Answer 2

• Mg has more protons than Na so it has a greater nuclear charge.
• The electrons of Mg and Na are in the same subshell hence similar shielding.
• so the forces of attraction between nucleus and valent electrons are greater in Mg than Na .

Question 3

Why does Oxygen have a lower ionisation energy than nitrogen?

Answer 3

• In nitrogen, all the electrons are unpaired within the p-subshell.
• In oxygen, there is a pair within the p-subshell, which repel each other and this electron repulsion overcomes the nuclear so less energy required to remove electron from oxygen.

Question 4

what is the name of the s and p orbital shapes?

Answer 4

Shperical and dumbbell

Question 5

State how thermochemical data can be used to show a compound has polarised bonds.

Answer 5

-The experimental and theroetical values for the Born Haber cycle should be different, which shows that it has some covalent character.

Question 6

What is meant by an orbital

Answer 6

a region within an atom that can hold up to 2 electrons