Atomic Structure: First Ionisation Energy across a period

Question 1

What happens to the ionisation energy as we move across the period?

Answer 1

= increases
= number of protons increases
= same sheilding however
= size of atom decreases

Question 2

Why are elements in group 3 lesser than expected compared to group 2?

Answer 2

= g3 outerelectron is in the p sub shell
= g2 outer electron is in the s subshell
= the electron in the p sub shell is further away from the positive nucleus than the s sub shell
= more sheilding by s sub shell.

Question 3

Why are elements in group 6 lower than expected?

Answer 3

= outer electron in group 6 end in p4
= pair of electrons in one of the p orbitals- pair mutually repel so that they are further away from the nucleus

Question 4

What would the graph of a 2nd ionisation energy look like?

Answer 4

= moves to the left.