Basics

Question 1

What reduces the effect of electron pair repulsion?

Answer 1

In order for electrons to exist in the same orbital, they must have opposite spins.

Question 2

What is the structure of a S orbital described as?

Answer 2

Spherical

Question 3

What is the structure of a P orbital described as?

Answer 3

Dumbell shaped lobes

Question 4

What is the order of electron filling?

Answer 4

1s,2s,2p,3s,3p,4s,3d,4p

Question 5

What can be used to represent the electron configuration up to 4s,3d in relation to the boxes?

Answer 5

[Ar]

Question 6

Why does an electron move from the 4s orbital to the 3d orbital (copper + chromium)

Answer 6

To create a more stable half full or full 3d sub-shell respectively.

Question 7

What increases as you go down the group, and what is the result relating to ionisation energy?

Answer 7

Atomic radius, outer electrons further away from the nucleus, resulting in a weaker attraction

Shielding, more shells between the nucleus and outer shell, weaker attraction

Due to the weaker attraction between the outer electrons and nucleus it has a lower ionisation energy.

Question 8

Why is there a decrease in first IE between magnesium and aluminium?

Answer 8

The outer electron in aluminium sits in a higher energy sub-shell (3p) which is slightly further away from the nucleus, making the attraction weaker.

Question 9

Why is first IE lower in sulfur between phosphorus, when it should follow the general increasing trend.

Answer 9

Removing an electron from sulfur involves taking it from an orbital with 2 electrons in, since electrons repel it takes less energy to remove it

Question 10

How can the process for first ionisation energy of an element be summarised in an equation?

Answer 10

X(g)—> X+(g) + e-

Question 11

What is another word for a positive ion?

Answer 11

Cation

Question 12

What is another word for a negative ion?

Answer 12

Anion