Brainscape's Knowledge GenomeTM

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


See full index

A Level Chemistry AQA > Atomic structure > Flashcards

Atomic structure Flashcards

Chap 1- physical

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

What is relative atomic mass?

A

Ratio of the average mass of one atom of an element to 1/12 of the mass of an atom of carbon-12

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

How many orbitals does each sub shell have?

A

Half the max electron number
Eg s has max 2 electrons so 1 orbital

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

Where does 4s and 5s go?

A

3p, 4s, 3d, 4p, 5s, 4d

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

What are 2 exceptions to the general configuration rule?

A

Chromium and copper

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

Configuration of chromium

A

[Ar] 4s1, 3d5

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

Configuration of copper

A

[Ar] 4s1, 3d10

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

What parts of the periodic table are s, p, d, f?

A

S: before transition metals
P: elements after transition metals
D: transition metals
F: under transition metals

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

Formula for number of electrons in each shell

A

2n squared

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

Size of an electron

A

0.0005

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

No. Of electrons in s subshell

A

2

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

No. Of electrons in p subshell

A

6

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

No. Of electrons in d subshell

A

10

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

No. Of electrons in f subshell

A

14

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

How can you tell if an element is a transition metal from its configuration?

A

Partially filled d orbitals
Eg [Ar] 4s2 3d8 is a transition metal but [Ar] 4s2 3d10 would not be as 3d10 is full

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

2 things ToF finds?
What 2 things does this help calculate?

A

•Mass and abundance of isotopes
•Ar & Mr

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

2 types of ionisation

A

Electron impact
Electronspray

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

Equation for electron impact

A

X (g) + e- —> X+ (g) + 2e-

18
Q

What is the electron impact process?

A

(Bang bang)
Fire electrons to knock off atom’s electron

19
Q

What is the electron spray process? (4 points)

A
  • Dissolve in volatile solvent
  • Apply high voltage
  • Inject thru hypodermic needle as spray into ionisation chamber
  • Gains proton and evaporates
20
Q

Electron impact/ Electron spray is used for what size molecules?

A

Impact: SMALL
Spray: BIG

21
Q

What molecular ions travel fastest?

A

Smallest/Lightest ones

22
Q

Electron spray equation

A

X (g) + H+ —> XH+ (g)

23
Q

Technique of Tof (broken into 6 parts)

A

•Inject sample
•Vaporise
•Ionise
•Accelerate (using electric field)
•Ion drift
•Detector (produces a current when hit with ions)

24
Q

How to convert g/mol (what periodic table is in) to kg for KE equation

A

Divide by (1000 x Avogadros constant)

25
Q

What is size of current proportional to?

A

Number of ions

26
Q

What mass unit are all elements in the PT in?

A

g/mol

27
Q

What does mass spectra show?

A

Abundance of isotopes/fragments in a sample and their ratios

28
Q

M/z

A

Mass/charge
So basically just mass as charge=1

29
Q

What are the smaller peaks on a mass spectra caused by? How do you calculate their m/z values?

A

Fragments
Sum of the involved isotopes’ masses

30
Q

What is 1st ionisation energy? (2 points)

A

• energy required to remove 1 e- from each atom in 1 mole of gaseous atoms
• and produce 1 mole of 1+ gaseous ions

31
Q

What effect does removing electrons have on ions? Why?

A

Atomic radius gets smaller
As there are more protons than electrons to pull in electrons

32
Q

What 3 factors affect ionisation energies?

A

Atomic radius
No. of protons
Shielding (no. of shells)

33
Q

When atomic radius increases, what happens to nuclear attraction?

A

decreases

34
Q

When number of protons increases, what happens to nuclear attraction?

A

increases

35
Q

When shielding (inner electrons repelling outer ones) increases, what happens to nuclear attraction?

A

decreases

36
Q

Down a group, ionisation energy…

A

decreases

37
Q

Across a period, ionisation energy…

A

increases

38
Q

Why are there dips in ionisation energy when going across a period? (3 reasons)

A

if there is 1 electron in an orbital, it’s easier to remove
increase in subshell shielding
if 2 electrons are paired up in an orbital, it’s easier to remove (they repel each other)

39
Q

True or false: group 1 has higher overall ionisation energies than group 0

A

False- group 0 have full outer shells, so requires more energy than group 1

40
Q

Why is there jumps in successive ionisation energies?

A

There is a jump every time electrons start to be removed from a new, lower shell

A Level Chemistry AQA (6 decks)

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