Unit 1 A2 Production and uses of substances in relation to properties

Question 1

How is the periodic table layout related to s, p, and d notation?

Answer 1

The periodic table is arranged into blocks (s, p, d) corresponding to the highest energy sublevel that is being filled in the elements’ electronic configuration.

Question 2

How do you represent the electronic arrangement of elements using s, p, d notation?

Answer 2

Elements are represented by their electron configuration in terms of orbitals: 1s², 2s² 2p⁶, 3s² 3p⁶, etc., where s, p, and d denote types of orbitals.

Question 3

What is first ionisation energy?

Answer 3

The first ionisation energy is the energy required to remove one mole of electrons from one mole of atoms in the gaseous state to form positive ions.

Question 4

Why does ionisation energy increase across Period 2 to 4?

Answer 4

Ionisation energy increases across a period because the atomic radius decreases and the nuclear charge increases, making it harder to remove electrons.

Question 5

Why does ionisation energy decrease down groups?

Answer 5

Ionisation energy decreases down a group because the atomic radius increases and the outer electrons are further from the nucleus, so they are more easily removed.

Question 6

What is electron affinity?

Answer 6

Electron affinity is the energy change when an electron is added to a neutral atom in the gaseous state, forming a negative ion.

Question 7

How does atomic radius change across periods and down groups?

Answer 7

Atomic radius decreases across a period due to increased nuclear charge, and it increases down a group due to additional electron shells.

Question 8

How does the radius of an ion change in contrast to the radius of the original atom?

Answer 8

Ionic radius is smaller for cations (positive ions) and larger for anions (negative ions) than their corresponding atomic radii.