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AQA Physical Chemistry > Atomic Structure > Flashcards

Atomic Structure Flashcards

1
Q

What does TOF mass spectrometry detect?

A

The mass and relative abundances of isotopes in 3 stages

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2
Q

What are the 3 stages of TOF mass spectrometry?

A

1 - Ionisation2- Acceleration3- Detection

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3
Q

How is ionisation carried out in TOF mass spectrometry?

A
  • By electron Impact- Sample is vaporised- Electrons are fired with an electron gun at the vaporised sample- An electron is knocked off to give 2 e-‘s and a positively charged ion
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4
Q

How is acceleration carried out in TOF mass spectrometry?

A
  • Positively charged ions approach two charged plates that have an electrical field- Ions are accelerated forward with the same kinetic energy - Ions will have different velocities depending on their mass- Ion drift
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5
Q

How is detection carried out in TOF mass spectrometry?

A
  • Negatively charged detector- As ions hit the detector they gain an e- causing an electrical current- current is detected, monitored and analysed to give a spectra
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6
Q

What does mass spectra show?

A

The relative abundances of different isotopes present and their masses

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7
Q

What is m/z?

A

The mass to charge ratio

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8
Q

What are the units of kinetic energy?

A

Joules

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9
Q

What are the units of mass?

A

Kg

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10
Q

What are the units of velocity?

A

Metres per second

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11
Q

What are the units of distance?

A

Metres

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12
Q

What are the units of time?

A

Seconds

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13
Q

How do you work out the mass of one ion?

A

Divide the Ar by Avogadros constant

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14
Q

How do you work out kinetic energy?

A

Half the mass times the velocity squared

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15
Q

How do you calculate velocity?

A

The square root of 2 x kinetic energy divided by mass

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16
Q

What shape are S orbitals?

A

Spherical

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17
Q

How many S orbitals are found together?

A

1

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18
Q

How many electrons do S orbitals hold altogether?

A

2

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19
Q

How many electrons can 1 S orbital hold?

A

2

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20
Q

What shape are P orbitals?

A

Figure of 8

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21
Q

How many P orbitals are found together?

A

3

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22
Q

How many electrons do P orbitals hold altogether?

A

6

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23
Q

How many electrons can 1 P orbital hold?

A

2

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24
Q

What shape are D orbitals?

A

Various

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25
How many D orbitals are found together?
5
26
How many electrons do D orbitals hold altogether?
10
27
How many electrons can 1 D orbital hold?
2
28
In energy level 1 what are the orbitals?
One S
29
In energy level 1 how many electrons are found?
2
30
In energy level 1 What is the notation?
1s
31
In energy level 2 what are the orbitals?
One S and three P
32
In energy level 2 how many electrons are found?
8
33
In energy level 2 what is the notation?
2s2p
34
In energy level 3 what are the orbitals?
One S, three P and five D
35
In energy level 3 how many electrons are found?
18
36
In energy level 3 what is the notation?
3s3p3d
37
In energy level 4 what are the orbitals?
One S, three P and five D
38
In energy level 4 how many electrons are found?
18
39
In energy level 4 what is the notation?
4s4p4d
40
What do 'electrons in boxes' show?
Electron pairing and spin
41
What is Hunds rule?
Electrons occupy empty orbitals before pairing to minimise repulsion
42
Why does the notation change for ions?
To account for the loss/gain of electrons
43
Which electrons are affected?
Outer electrons only
44
What does isoelectronic mean?
Same electronic structure
45
What is the rule for transition metals?
4s in before 3d and 4s out before 3d
46
What is the 1st molar ionisation energy?
The energy required to remove 1 mole of electrons from 1 mole of gaseous atoms (kj.mol^-1)
47
What is the 1st molar ionisation energy equation?
X(g) -> X^+ (g) + e^-
48
What does the 1st molar ionisation energy depend on?
- Nuclear Charge- Sheilding- Distance
49
How does nuclear charge effect I.E.?
As nuclear charge increases so does I.E.
50
How does sheilding effect I.E.?
As sheilding increases, I.E. decreases
51
How does distance effect I.E.?
As distance increases, I.E. decreases
52
How does molar I.E. change down a group?
Decreases
53
How does nuclear charge change down a group?
Increases
54
How does sheilding change down a group?
Increases
55
How does distance of e^- to nucleus change going down a group?
Increases
56
What effect do an increase in sheilding and distance have?
they lower the effective charge on the nucleus which decreases the attraction between the nucleus and the outer e^-
57
How does I.E. change across a period?
Increases
58
How does nuclear charge change across a period?
Increases
59
How does distance change across a period?
No change
60
How does sheilding change across a period?
No change
61
How does attraction between outer electron and the nucleus change?
Increases
62
How does energy needed change?
Increases
63
Why is there an exception between groups 2 and 3?
3 is easier to remove than 2 because of sheilding from the full s orbital
64
Why is there an exception between groups 5 and 6?
6 is easier to remove than 5 because of electron repulsion between paired electrons
65
What is a successive I.E.?
The energy required to remove electrons one by one from the same atom
66
Define the second ionisation energy?
The energy required to remove 1 mole of electrons from one mole of gaseous 1+ ions
67
What is the second ionisation energy equation?
X+ (g) -> X^2+ (g) + e^-
68
What is the general trend in successive I.E.s?
Increase in I.E. because of increasing effective charge on the nucleus because of decreased sheilding, decreased distance and therefore stronger nuclear attraction
69
What are the large jumps caused by?
Moving from an outer energy shell inwards
70
What does the notation detail?
The positions of the electrons in their respective energy levels and orbitals
71
What does the big number represent?
The energy level
72
What does the letter represent?
The orbital type
73
What does the superscript represent?
Number of electrons in the orbital

AQA Physical Chemistry (12 decks)

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