Ionisation energies

0 of 10 answered, 0 correct

1. Question 1 of 10

   Which equation represents the first ionisation energy of magnesium?

   AA, Mg(s) → Mg⁺(g) + e⁻BB, Mg(g) → Mg⁺(g) + e⁻CC, Mg(g) + e⁻ → Mg⁻(g)DD, Mg⁺(g) → Mg²⁺(g) + e⁻

2. Question 2 of 10

   Which of these Period 3 elements has the highest first ionisation energy?

   AA, NaBB, AlCC, PDD, S

3. Question 3 of 10

   Why is the first ionisation energy of aluminium lower than that of magnesium?

   AA, Al's outer electron is in a 3p subshell, higher in energy than 3sBB, Al has one more proton than MgCC, Al's outer electron is paired in its orbitalDD, Al has an extra full shell of shielding

4. Question 4 of 10

   Why does first ionisation energy decrease down Group 2?

   AA, Nuclear charge decreases down the groupBB, The outer electron is further away and more shieldedCC, The outer electrons become paired down the groupDD, Atomic radius decreases down the group

5. Question 5 of 10

   The first five successive ionisation energies of element X are 578, 1817, 2745, 11 577 and 14 842 kJ mol⁻¹. Which group is X in?

   AA, Group 2BB, Group 3CC, Group 4DD, Group 5

6. Question 6 of 10

   Why is the second ionisation energy of an element always larger than the first?

   AA, The electron is removed from a positive ionBB, The electron always comes from a shell nearer the nucleusCC, The second electron is always pairedDD, The ion has gained a proton

7. Question 7 of 10

   Why does first ionisation energy generally increase across Period 3?

   AA, Nuclear charge increases with similar shieldingBB, The number of shells decreasesCC, Shielding increases across the periodDD, Atomic radius increases across the period

8. Question 8 of 10

   Which element has the highest first ionisation energy?

   AA, FBB, NeCC, NaDD, Ar

9. Question 9 of 10

   Which observation is evidence that electrons are arranged in shells?

   AA, The large drop in first ionisation energy from Ne to NaBB, The drop in first ionisation energy from Mg to AlCC, The drop in first ionisation energy from P to SDD, The gradual rise in first ionisation energy from Na to Ar

10. Question 10 of 10

    The first ionisation energy of magnesium is 738 kJ mol⁻¹ and the second is 1451 kJ mol⁻¹. How much energy is needed to turn 1 mol of Mg(g) into Mg²⁺(g)?

    AA, 713 kJ mol⁻¹BB, 1451 kJ mol⁻¹CC, 2189 kJ mol⁻¹DD, 738 kJ mol⁻¹