Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry AS level > 1.1 Atomic Structure Part 2 > Flashcards

1.1 Atomic Structure Part 2 Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

What does each sub-shell consist of?

A

Orbitals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What is an orbital?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What is the complete electronic configuration of oxygen?

A

1S2, 2S2, 2P4

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What is the complete electronic configuration of silicon?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Give the complete electronic configuration of potassium

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What is the complete electronic structure of titanium?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What is the electronic configuration of chromium?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What is the complete electron configuration of copper?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

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

A

Copper and chromium (Cu and Cr)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

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

A

1s2, 2s2, 2p6

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

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

A

1s2, 2s2, 2p6,

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

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

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

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

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What is first ionisation energy?

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

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

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What are the units for ionisation energy?

A

kJmol-1

17
Q

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

A
  • shielding
  • distance
  • nuclear charge
18
Q

Why does shielding influence first ionisation energies?

A

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

19
Q

Why does distance influence first ionisation energies?

A

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

20
Q

Why does nuclear charge influence the 1st ionisation energies?

A

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

21
Q

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

A

It decreases

22
Q

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

A

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

23
Q

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

A

Increases

24
Q

Why does 1st ionisation energy increase across a period?

A

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

25
Q

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

A

It says there is a SMALL dip or increase

26
Q

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

A

There is a small dip

27
Q

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

A

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

28
Q

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

A

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

29
Q

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

A

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

30
Q

What is the first ionisation energy of mg?

A

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

STATE SYMBOLS ARE IMPORTANT

31
Q

What is the second ionisation of Mg?

A

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

32
Q

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

A

Ne+(g) -> Ne2+(g) + e-

The distance is slightly smaller so it is harder to remove the electron

Chemistry AS level (8 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions