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AQA Physical Chemistry > Atomic Structure > Flashcards

Atomic Structure Flashcards

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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
Q

How many D orbitals are found together?

A

5

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26
Q

How many electrons do D orbitals hold altogether?

A

10

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27
Q

How many electrons can 1 D orbital hold?

A

2

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28
Q

In energy level 1 what are the orbitals?

A

One S

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29
Q

In energy level 1 how many electrons are found?

A

2

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30
Q

In energy level 1 What is the notation?

A

1s

31
Q

In energy level 2 what are the orbitals?

A

One S and three P

32
Q

In energy level 2 how many electrons are found?

A

8

33
Q

In energy level 2 what is the notation?

A

2s2p

34
Q

In energy level 3 what are the orbitals?

A

One S, three P and five D

35
Q

In energy level 3 how many electrons are found?

A

18

36
Q

In energy level 3 what is the notation?

A

3s3p3d

37
Q

In energy level 4 what are the orbitals?

A

One S, three P and five D

38
Q

In energy level 4 how many electrons are found?

A

18

39
Q

In energy level 4 what is the notation?

A

4s4p4d

40
Q

What do ‘electrons in boxes’ show?

A

Electron pairing and spin

41
Q

What is Hunds rule?

A

Electrons occupy empty orbitals before pairing to minimise repulsion

42
Q

Why does the notation change for ions?

A

To account for the loss/gain of electrons

43
Q

Which electrons are affected?

A

Outer electrons only

44
Q

What does isoelectronic mean?

A

Same electronic structure

45
Q

What is the rule for transition metals?

A

4s in before 3d and 4s out before 3d

46
Q

What is the 1st molar ionisation energy?

A

The energy required to remove 1 mole of electrons from 1 mole of gaseous atoms (kj.mol^-1)

47
Q

What is the 1st molar ionisation energy equation?

A

X(g) -> X^+ (g) + e^-

48
Q

What does the 1st molar ionisation energy depend on?

A
  • Nuclear Charge- Sheilding- Distance
49
Q

How does nuclear charge effect I.E.?

A

As nuclear charge increases so does I.E.

50
Q

How does sheilding effect I.E.?

A

As sheilding increases, I.E. decreases

51
Q

How does distance effect I.E.?

A

As distance increases, I.E. decreases

52
Q

How does molar I.E. change down a group?

A

Decreases

53
Q

How does nuclear charge change down a group?

A

Increases

54
Q

How does sheilding change down a group?

A

Increases

55
Q

How does distance of e^- to nucleus change going down a group?

A

Increases

56
Q

What effect do an increase in sheilding and distance have?

A

they lower the effective charge on the nucleus which decreases the attraction between the nucleus and the outer e^-

57
Q

How does I.E. change across a period?

A

Increases

58
Q

How does nuclear charge change across a period?

A

Increases

59
Q

How does distance change across a period?

A

No change

60
Q

How does sheilding change across a period?

A

No change

61
Q

How does attraction between outer electron and the nucleus change?

A

Increases

62
Q

How does energy needed change?

A

Increases

63
Q

Why is there an exception between groups 2 and 3?

A

3 is easier to remove than 2 because of sheilding from the full s orbital

64
Q

Why is there an exception between groups 5 and 6?

A

6 is easier to remove than 5 because of electron repulsion between paired electrons

65
Q

What is a successive I.E.?

A

The energy required to remove electrons one by one from the same atom

66
Q

Define the second ionisation energy?

A

The energy required to remove 1 mole of electrons from one mole of gaseous 1+ ions

67
Q

What is the second ionisation energy equation?

A

X+ (g) -> X^2+ (g) + e^-

68
Q

What is the general trend in successive I.E.s?

A

Increase in I.E. because of increasing effective charge on the nucleus because of decreased sheilding, decreased distance and therefore stronger nuclear attraction

69
Q

What are the large jumps caused by?

A

Moving from an outer energy shell inwards

70
Q

What does the notation detail?

A

The positions of the electrons in their respective energy levels and orbitals

71
Q

What does the big number represent?

A

The energy level

72
Q

What does the letter represent?

A

The orbital type

73
Q

What does the superscript represent?

A

Number of electrons in the orbital

AQA Physical Chemistry (12 decks)

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