Brainscape's Knowledge GenomeTM

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


See full index

Chemistry A-Level > 3.1.1 > Flashcards

3.1.1 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 are energy levels divided into?

A

sub-shells

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

How many electrons can an orbital hold?

A

2

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

What is a sub-shell

A

an orbital or combination of orbitals

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

How do electrons in orbitals reduce repulsions?

A

by spinning in opposite directions

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

How many types of orbitals are there and what are their names?

A

four, s, p, d, f

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

How many s orbitals are there at each level?

A

1

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

How many p orbitals are there at each level?

A

3

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

How many d orbitals are there at each level?

A

5

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

How is one electron in 1s subshell written?

A

1s^1

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

What order are the orbitals filled?

A

1s, 2s, 2p, 3s, 3p, 4s, 3d, 5s, 4d, 5p

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

When metal atoms lose electrons lose electrons where do they lose them from, and with the exception of which orbital?

A

The outermost level, with the exception of d block elements, which lose their 4s electrons first then their 4d ones.

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

What does isoelectronic mean?

A

Particles that have the same electron configuration

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

Name the sub-levels

A

S, P, D, F

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

How many electrons does an orbital hold?

A

2 of opposite spin

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

How many electrons can the sub-level S have?

A

2

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

How many electrons can the sub-level P have?

A

6

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

How many electrons can the sub-level D have?

A

10

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

How many electrons can the sub-level F have?

A

14

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Why must the electrons inside orbital be of opposite spin?

A

To reduce repulsion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

An atom fills up sub-shells in order of increasing energy, in what order are the sub-shells filled?

A

1S, 2S, 2P, 3S, 3P, 4S, 3D, 4P, 5S, 4D, 5P

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

How do electrons prefer to occupy orbitals?

A

On their own

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

What is the electronic structure of fluorine?

A

1S^2, 2S^2, 2P^5

23
Q

How do you write the electronic configuration in shorthand?

A

Start with the previous noble gas and put it in square brackets (eg. [Ne]) then follow it with the additional electrons and their sub-levels

24
Q

Which elements fill their orbitals and sub levels irregularly?

A

Chromium and Copper

25
Q

What’s the electron configuration of chromium?

A

[Ar]4S^1 3D^5

26
Q

What’s ever electron configuration of copper?

A

[Ar]4S^1 3D^10

27
Q

Define an s block element.

A

One whose outer electron is in an s sub-level?

28
Q

Define a p block element.

A

One whose outer electron is in a p sub-level?

29
Q

Define a d block element.

A

One whose outer electron is in a d sub-level?

30
Q

Define an f block element

A

One whose outer electron is in an f sub-level?

31
Q

Which set of elements are s block?

A

Group 1&2 plus H&He

32
Q

Which set of elements are d block?

A

The transition metals

33
Q

Which set of elements are d block?

A

The rest of the metals and most non metals

34
Q

What is 1st ionisation energy?

A

The energy required to remove one electron from each atom in a mole of gaseous atoms producing one mole of 1+ gaseous ions

35
Q

What is 2nd ionisation energy?

A

The energy required to remove the second electron (not both electrons)

36
Q

What is the equation for the first ionisation of sodium?

A

Na(g) —> Na+(g) + e-

37
Q

What is the equation for the 2nd ionisation of sodium?

A

Na+(g) –> Na2+(g) + e-

38
Q

What happens to the ionisation energy as you descend a group?

A

It decreases, because the atomic radius increases, more shielding, and there’s weaker attraction between the nucleus and the electron

39
Q

What happens to the ionisation energy as you go across a period and why?

A

Increases, because the atomic radius decreases (outer electron is still in the same shell but the larger positive charge from the nucleus causing the atom to shrink, more protons, stronger attraction between nucleus and outermost electron

40
Q

A graph depicts the ionisation energy across period three. Why does the graph dip from group 2 to group 3 (Mg to Al)?

A

Change from sub-level s to sub-level p, p orbital is higher energy than s

41
Q

A graph depicts the ionisation energy across period three. Why does the graph dip from group 5 to group 6 (P to S)

A

P e- from orbital with one e- (3P). S e- from orbital 3p with two e- therefore there’s more e- e- repulsion

42
Q

What’s a repeating pattern across a period called?

A

Periodicity

43
Q

Why are successive ionisation (2nd, 3rd, etc) energies always larger?

A

When the first electron is removed a positive ion is formed meaning the attraction between the nucleus and the remaining electrons is greater so more energy is required to remove the next electron

44
Q

How are ionisation energies linked to electronic structure?

A

There’s a large increase in ionisation when moving to the next sub-level due to there being lots shielding and the shell being clear so the nucleus is more attracted to the outermost electron

45
Q

The ionisation energy for an element are 1. 590, 2. 1150, 3. 4940 4. 6480, 5. 8120. Which group is this element in?

A

Group 2.

(Reason:
There’s a large increase in ionisation energy between three 2nd and 3rd ionisation meaning the element must be in group 2 as there are two electrons before it changes sub-level

46
Q

Which electrons do d block elements lose first?

A

4s electrons

47
Q

Define a transition metal.

A

An element that has a partially filled d level in its atomic or ionic form

48
Q

What has a higher ionisation energy, Na or Mg?

A

Mg, has more protons and a smaller atomic radius

49
Q

What has a higher ionisation energy, P or S?

A

P, in S electron is lost from orbital with two electrons but in P is lost from orbital with one electron, there’s more e- e- repulsion in S

50
Q

What has a higher ionisation energy, Ne or Ar?

A

Ne, it has a smaller atomic radius and more shielding

51
Q

What has a higher ionisation energy, Be or B?

A

Be, electron lost is from S orbital but in B is lost from p orbital, p orbital has higher energy than s orbital

52
Q

What has a higher ionisation energy, Ar or K?

A

Ar, electron in Ar is from shell 3 in K is from shell 4. Ar has a smaller atomic radius and less shielding

53
Q
A

Chemistry A-Level (3 decks)

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