1 - Electron configuration

Question 1

Electron shells are split into __ _____

Answer 1

4 subshells

Question 2

What are the 4 types of subshell?

Answer 2

s, p, d and f

Question 3

How many orbitals does the s subshell contain?

Answer 3

1 orbital

Question 4

How many electrons can the s orbital hold?

Answer 4

2 electrons

Question 5

How many orbitals does the p subshell contain?

Answer 5

3 orbitals

Question 6

How many electrons can the p orbital hold?

Answer 6

6 electrons

Question 7

How many orbitals does the d subshell contain?

Answer 7

5 orbitals

Question 8

How many electrons can the d orbital hold?

Answer 8

10 electrons

Question 9

How many orbitals does the f subshell contain?

Answer 9

7 orbitals

Question 10

How many electrons can the f orbital hold?

Answer 10

14 electrons

Question 11

For transition metals Cr and Cu the 3d subshell must be…

Answer 11

half full (5 electrons) or full (10 electrons)

Question 12

Define ‘ionisation energy’

Answer 12

Ionisation energy is the minimum amount of energy required to remove 1 mole of electrons from 1 mole of atoms in the gaseous state

Question 13

Define ‘first ionisation energy’

Answer 13

The enthalpy change when 1 mole of gaseous atoms forms 1 mole of gaseous ions with a single positive charge

Question 14

Define ‘second ionisation energy’

Answer 14

The enthalpy change when one mole of gaseous ions with a single positive charge forms one mole of gaseous ions with a double positive charge

Question 15

What is the 1st IE equation?

Answer 15

H_(g) → H⁺_(g) + e^-

Question 16

What is the general trend of 1st ionisation energy along a period?

Answer 16

1st IE increases along a period

Question 17

Why does 1st IE increase along a period?

Answer 17

• Nuclear charge increases
• Outer electrons fill same shell so same amount of shielding
• Greater force of attraction between outer electron and nucleus

Question 18

What are the exceptions for increasing ionisation energy across a period?

Answer 18

In period 3, aluminium and sulfur show a decrease in ionisation energy

Question 19

What is the general trend of 1st ionisation energy down a group?

Answer 19

1st IE decreases down a group

Question 20

Why does 1st IE decrease down a group?

Answer 20

• Shielding increases
• Increase in distance of outer electron
• Less attraction between outer electron and nucleus

Question 21

How does shielding affect ionisation energy?

Answer 21

Shielding is when there are more electron shells between the nucleus and the outer electron
- more shielding: decreases IE as there is less attraction between nucleus and electron
- less shielding: more attraction between nucleus and electron

Question 22

How does atomic size / radius affect ionisation energy?

Answer 22

The bigger the atom the further away the outer electrons are from the nucleus
- bigger atom: less attraction between nucleus and outer electron
- smaller atom: more attraction between nucleus and outer electron

Question 23

How does nuclear charge affect ionisation energy?

Answer 23

The more protons in the nucleus the bigger the attraction between the nucleus and outer electrons
- greater nuclear charge: more attraction, larger IE
- smaller nuclear charge: less attraction, smaller IE