1.1 Atomic Structure (part 2)

Question 1

What are the 4 sub shells

Answer 1

S, p, d, f

Question 2

How many electrons can the s she’ll hold

Answer 2

2

Question 3

How many electrons can the p she’ll hold

Answer 3

8

Question 4

How many electrons can the d she’ll hold

Answer 4

18

Question 5

How many electrons can the f she’ll hold

Answer 5

32

Question 6

What does each sub-she’ll consist of

Answer 6

Orbitals

Question 7

What is an orbital

Answer 7

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

Question 8

How many orbitals in the s sub shell

Answer 8

1 (holds a max of 2 electrons)

Question 9

How many orbitals does a p shell have

Answer 9

3 (holds a max of 6 electrons)

Question 10

How many orbitals in a d subshell

Answer 10

5 (holds a max of 10 electrons)

Question 11

How many orbitals in an f subshell

Answer 11

7 (holds a max of 14 electrons)

Question 12

What symbol is an unpaired electron represented by

Answer 12

An up arrow

Question 13

What symbol are paired electrons represented by

Answer 13

An up arrow to the left of a down arrow

Question 14

Why do sub shells have different energies

Answer 14

Shielding from the nucleus

Question 15

In what order do the energy levels fill with electrons

Answer 15

1s 2s 2p 3s 3p 4s 3d 4p

Question 16

How does each sub shell fill up

Answer 16

So that electrons remain unpaired if possible

Question 17

What happens when the subshell is half full

Answer 17

The electrons pair up

Question 18

Why does the 1s subshell have the lowest energy

Answer 18

It’s closest to the nucleons

Question 19

What is the electron configuration of nitrogen

Answer 19

1s2 2s2 2p3

Question 20

What is the electron configuration of potassium

Answer 20

1s2 2s2 2p6 3s2 3p6 4s1

Question 21

When are chromium and copper more stable

Answer 21

With half full + full 3D shells (3D fills before 4s)

Question 22

How can electron arrangements be abbreviated

Answer 22

By using the symbol of the previous noble gas

Question 23

Which electrons are removed first in transition metals

Answer 23

4s

Question 24

First ionisation energy

Answer 24

Energy needed to remove one electron from each atom in one mole of gaseous atoms

Question 25

3 factors which influence ionisation energies

Answer 25

1. Atomic radius- distance from nucleus to outer electron 2. Nuclear charge (no of protons) 3. Shells- more shells leads to more shielding

Question 26

What is the patterns between ionisation energy and ease of removing outer electron

Answer 26

The smaller the ionisation energy, the easier it is to remove outer electron

Question 27

What is the trend in 1st ionisation energy down a group

Answer 27

It decreases down a group

Question 28

Why does 1st ionisation energy decrease down a group

Answer 28

* shells increase so shielding increases * atomic radius increases to outweigh increase in nuclear charge * nuclear attraction on outer electron decreases so 1st ionisation energy decreases

Question 29

What is the trend in 1st ionisation energy across a period

Answer 29

Increase in 1st ionisation energy across a period

Question 30

Why is there an increase in 1st ionisation energy across a period

Answer 30

* shells + shielding remain same * nuclear charge increases * atomic radius decreases * nuclear attraction on outer electron increases so first ionisation energy increases

Question 31

Why is there a small dip in 1st ionisation energy between group 2 and 3 elements E.g. Be>B

Answer 31

* borons outer electron in 2p sub shell- further away from nucleus * easier to remove

Question 32

Why is there a small dip in 1st ionisation energy between nitrogen and oxygen (Applies to all group 5>6 elements)

Answer 32

*easier to remove as electrons are now paired- inter-orbital repulsion

Question 33

Why is there a big drop in 1st ionisation energy between the end of one period and start of the next

Answer 33

* more shells - more shielding * nuclear attraction decreases * ionisation energy lower

Question 34

What happens tomipnisation energy once one electron has been removed

Answer 34

Electrons become harder to remove

Question 35

First 4 ionisation energy equations of magnesium

Answer 35

1: mg(g) > mg+(g) + e- 2: mg+(g)> mg2+(g) + e- 3: mg2+(g) > mg3+(g) + e- 4: mg3+(g) > mg4+(g) + e- Altogether: mg4+(g) + 4e-

Question 36

Why does successive ionisation energy increase

Answer 36

As electrons are removed, fewer electrons are being attracted by the same number of protons. Therefore, attraction sequentially increases as successive ionisation energies increase

Question 37

What does the pattern of ionisation energy values tell us

Answer 37

The number of electrons in each energy level, and provides evidence for the existence of energy levels

Question 38

What does it mean if the ionisation energies are increasing in roughly equal steps?

Answer 38

The electrons are being removed from the same shell

Question 39

What does it mean if there is a big difference in two successive ionisation energies?

Answer 39

The electrons are being removed from different shells

Question 40

Why is the first ionisation energy of magnesium higher than that of sodium

Answer 40

Magnesium has more protons | Attraction between nucleus and outer electron is higher

Question 41

Why is the first ionisation energy of neon higher than that of sodium

Answer 41

Neons outer electron is closer to the nucleus than sodiums | Less shielding and stronger attraction between nucleus and outer electron

Question 42

Why is borons first ionisation energy lower than expected

Answer 42

Electron is being removed from 2p sub shell which is further from nucleus than 2s