Module 2.2 | Electrons, Bonding and Structure

Question 1

2.2.1 a) Know the number of electrons that can fill the first four shells.

Answer 1

The maximum number of electrons that can fill the first four shells are 2, 8, 18 and 32.

Question 2

2.2.1 b) Define ‘atomic orbitals’.

Answer 2

A region around the nucleus that can hold up to two electrons, with opposite spins.

Question 3

2.2.1 b) Recall the shape of s- orbitals.

Answer 3

Spherical.

Question 4

2.2.1 b) Recall the shape of p- orbitals.

Answer 4

Dumbbell.

Question 5

2.2.1 b) Recall the number of orbitals that make up s- sub shells, and the number of electrons that can fill these sub-shells.

Answer 5

An s- sub shell contains only one orbital, and can hold up to two electrons.

Question 6

2.2.1 b) Recall the number of orbitals that make up p- sub shells, and the number of electrons that can fill these sub-shells.

Answer 6

A p- sub shell contains three orbitals, and can hold up to six electrons.

Question 7

2.2.1 b) Recall the number of orbitals that make up d- sub shells, and the number of electrons that can fill these sub-shells.

Answer 7

A d- sub shell contains five orbitals, and can hold up to ten electrons.

Question 8

2.2.1 c) Understand how orbitals are filled for the first three shells and the 4s and 4p shells.

Answer 8

In order of increasing energy.

Question 9

2.1.1 c) Understand how orbitals are filled for orbitals with the same energy.

Answer 9

Electrons occupy orbitals singly with the same spin before pairing begins.