1.1 Atomic Structure Part 2

Question 1

What does each sub-shell consist of?

Answer 1

Orbitals

Question 2

What is an orbital?

Answer 2

A region which can hold a maximum of two electrons with opposite spins

Question 3

What is the complete electronic configuration of oxygen?

Answer 3

1S2, 2S2, 2P4

Question 4

What is the complete electronic configuration of silicon?

Answer 4

1S2, 2S2, 2P6, 3S2, 3P2

Question 5

Give the complete electronic configuration of potassium

Answer 5

1S2, 2S2, 2P6, 3S2, 3P6, 4S1

Question 6

What is the complete electronic structure of titanium?

Answer 6

1S2, 2S2, 2P6, 3S2, 3P6, 3d2, 4s2

Question 7

What is the electronic configuration of chromium?

Answer 7

1s2, 2s2, 2p6, 3s2, 3p6, 3d5, 4s1

Question 8

What is the complete electron configuration of copper?

Answer 8

1s2, 2s2, 2p6, 3s2, 3p6, 3d10, 4s1

Question 9

What are the two elements that don’t follow the complete electronic structure pattern?

Answer 9

Copper and chromium (Cu and Cr)

Question 10

What is the complete electronic configuration of an Na+ ion?

Answer 10

1s2, 2s2, 2p6

Question 11

What is the complete electronic configuration of an Mg 2+ ion?

Answer 11

1s2, 2s2, 2p6,

Question 12

What is the complete electronic configuration of a Cl- ion?

Answer 12

1s2, 2s2, 2p6, 3s2, 3p6

Question 13

What is the complete electronic configuration for a S 2- ion?

Answer 13

1s2, 2s2, 2p6, 3s2, 3p6

Question 14

What is first ionisation energy?

Answer 14

The energy needed to remove one mole of electrons from one mole of atoms in the gaseous state

Question 15

The first ionisation energy of sodium is the energy required for the following process:

Answer 15

Na(g) -> Na+(g) + e-

Question 16

What are the units for ionisation energy?

Answer 16

kJmol-1

Question 17

What are the factors, in order, that influence first ionisation energies?

Answer 17

• shielding
• distance
• nuclear charge

Question 18

Why does shielding influence first ionisation energies?

Answer 18

Increased shielding lowers the attraction of the outer electron ( more inner e- the lower the ionisation energy)

Question 19

Why does distance influence first ionisation energies?

Answer 19

The further away from the nucleus the e- is, the lower the attraction (1st ionisation energy decreases with increased distance)

Question 20

Why does nuclear charge influence the 1st ionisation energies?

Answer 20

The higher the nuclear charge the more attraction to the e- ions (more protons, higher 1st ionisation energy)

Question 21

What happens to the 1st ionisation energy as you go down a group?

Answer 21

It decreases

Question 22

Why does 1st ionisation energy decrease as you go down a group?

Answer 22

Shielding: increases, lower attraction
Distance: increases, lower attraction
Nuclear Charge: increases
Summary: 1st ionisation energy decreases as shielding and distance outweigh nuclear charge

Question 23

What happens to the 1st ionisation energy as you go across a period?

Answer 23

Increases

Question 24

Why does 1st ionisation energy increase across a period?

Answer 24

Shielding: Similar
Distance: DECREASES, attraction increases
Nuclear charge: Increases, attraction increases
Summary: attraction increases so 1st ionisation energy increases

Question 25

What is the clue to use the A-level structure stuff when answering questions on the trends in first ionisation energies?

Answer 25

It says there is a SMALL dip or increase

Question 26

What happens to the first ionisation energy between group 2 and 3 elements?

Answer 26

There is a small dip

Question 27

Why is there a small dip in first ionisation energies between group 2 and 3 elements? E.g Be -> B

Answer 27

The outer electron in boron is the first in the 2p subshell. So it is slightly further from the nucleus, so attraction decreases slightly

Question 28

Why is there a small dip in 1st ionisation energy between nitrogen and oxygen and again at phosphorous and sulfur?

Answer 28

Oxygen is the first element to have a pair of electrons in the 2p subshell. This creates some repulsion so the 1st ionisation energy decreases slightly

Question 29

Why is there a big drop in ionisation energy between the end of one period and the start of the next?

Answer 29

Shielding: Increases, lower attraction Distance: Increases, lower attraction Nuclear charge: small increase Summary: The large increases in shielding and distance outweigh the small increase in nuclear charge. Lower attraction, lower 1st ionisation energy

Question 30

What is the first ionisation energy of mg?

Answer 30

Mg(g) -> Mg+(g) + e- | STATE SYMBOLS ARE IMPORTANT

Question 31

What is the second ionisation of Mg?

Answer 31

Mg+(g) -> Mg2+(g) + e-

Question 32

Write an equation for the second ionisation energy of neon and explain whether this value will be higher or lower than the first ionisation energy of neon

Answer 32

Ne+(g) -> Ne2+(g) + e- The distance is slightly smaller so it is harder to remove the electron