1.3.4 - 1.3.5 Electron Configuration

Question 1

Electron Configuration

Answer 1

The arrangement of electrons in orbitals around a nucleus

Question 2

How are electrons arranged?

Answer 2

Electrons are arranged in energy levels –> energy levels are made up of sublevels –> sub-levels are made up of orbitals –> each orbital can hold up to 2 electrons with opposite spins

Question 3

What is the energy level represented by?

Answer 3

A number

Question 4

What is the sublevel represented by?

Answer 4

s, p, d, f

Question 5

Orbital

Answer 5

The region of space that electrons are most likely to be in.
- can hold up to 2 electrons with opposite spins
- electrons prefer to occupy orbitals of their own

Question 6

What is the orbital represented by?

Answer 6

A box

Question 7

Aufbau Principle

Answer 7

Electrons enter the lowest energy orbital available
- electrons fill 4s sublevel before the 3d sublevel

Question 8

What are the exceptions to the Aufbau Principle? Why does this occur?

Answer 8

Chromium (Cr) & Copper (Cu)

Electrons from 4s is used to fill 3d as d-sublevels are more stable either half filled or fully filled.

Question 9

Ionisation

Answer 9

The highest energy electrons are lost first when an ion is formed.
- 4s electrons are removed before 3d electrons