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Physical Chemistry > Atomic Structure > Flashcards

Atomic Structure Flashcards

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1
Q

What are the 3 subatomic particles in an atom?

A

Proton
Neutron
Electron

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2
Q

Relative mass and Relative charge of a Proton?

A

Mass - 1
Charge - +1

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3
Q

Relative mass and Relative charge of a Neutron?

A

Mass - 1
Charge - 0

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4
Q

Relative mass and Relative charge of an Electron?

A

Mass - 1/1840
Charge - -1

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5
Q

What is the atomic radius?

A

The distance from the nucleus to the outermost shell.

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6
Q

What are ions?

A

Charged particles.

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7
Q

What is the ion for Na? (Use Periodic Table)

A

Na^+

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8
Q

What is the ion for Ca? (Use Periodic Table)

A

Ca^2+

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9
Q

What is the ion for Al? (Use Periodic Table)

A

Al^3+

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10
Q

What is the ion for N? (Use Periodic Table)

A

N^3-

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11
Q

What is the ion for O? (Use Periodic Table)

A

O^2-

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12
Q

What is the ion for Cl? (Use Periodic Table)

A

Cl^-

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13
Q

What are isotopes?

A

Isotopes are elements with the same number of protons but a different number of neutrons.

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14
Q

What are the 4 letters of electron configuration?

A

S
P
D
F

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15
Q

What letter is not important for A Level Chemistry?

A

F

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16
Q

How many electrons can S hold?

A

2

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17
Q

How many electrons can P hold?

A

6

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18
Q

How many electrons can D hold?

A

10

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19
Q

Electron Configuration order?

A

1s
2s
2p
3s
3p
4s
3d
4p
4d
4f

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20
Q

What is the electron configuration for C? (Use the Periodic Table)

A

1s^2
2s^2
2p^2

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21
Q

What is the electron configuration for Fe? (Use the Periodic Table)

A

1s^2
2s^2
2p^6
3s^2
3p^6
4s^2
3d^6

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22
Q

What is the electron configuration for Se (Use the Periodic Table)

A

[Ar]
4s^2
3d^10
4p^4

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23
Q

What is the electron configuration for Cr? (Use the Periodic Table)

A

[Ar]
4s^1
3d^5

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24
Q

What is the electron configuration for Cu? (Use the Periodic Table)

A

[Ar]
4s^1
3d^10

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25
Q

What is the electron configuration for Fe^3+? (Use the Periodic Table)

A

[Ar]
3d^5

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26
Q

What happens in electron configuration when elements are ionised?

A

Electrons are lost from 4s first.

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27
Q

Describe the S orbital.

A

It is spherical in shape.
It can hold 2 electrons.

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28
Q

What does the orbital show us?

A

Where the path of an electron would be.

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29
Q

What are the sub orbitals of the P orbital?

A

Px
Py
Pz

30
Q

How many electrons can Px hold?

A

2

31
Q

How many electrons can Py hold?

A

2

32
Q

How many electrons can Pz hold?

A

2

33
Q

How many electrons can the full P orbital hold?

A

6

34
Q

How many D sub orbitals are there?

A

5

35
Q

Why do we draw electron pairs as one going up and one going down?

A

Hunt’s theory was that if electrons are pairing up, they must spin in opposite directions.

36
Q

What is Aufbau’s principle?

A

Electrons must fill up from the lowest energy orbital upwards.

37
Q

What is ionisation energy?

A

The amount of energy needed to remove 1 mole of electrons from 1 mole of atoms in the gaseous state.

38
Q

Show the first ionisation energy for Na.

A

Na(g) –> Na(g)^+ + e-

39
Q

What is the second ionisation energy?

A

The amount of energy needed to remove 1 mole of electrons from 1 mole of ions in the gaseous state.

40
Q

Show the second ionisation energy for Ca.

A

Ca(g)^+ –> Ca(g)^2+ + e-

41
Q

What happens to ionisation energy as we go down a group?

A

Ionisation energy decreases.

42
Q

What happens to ionisation energy as we go across a group?

A

Ionisation energy increases.

43
Q

What are the 3 things that can affect ionisation enegry?

A

Number of protons
Atomic Radius
Shielding

44
Q

How does the number of protons affect IE?

A

As we go across a period, the number of protons increases thus IE increases aswell.

45
Q

How does the atomic radius affect IE?

A

The further away the outermost electron is from the nucleus, the easier it is to remove the electron from the atom. As you go down the group the atoms get significantly bigger meaning the amount of energy required to remove the electron from the atom decreases. Thus IE decreases as you go down a group.

46
Q

How does shielding affect IE?

A

The greater the shielding the less energy required to remove the outer electron. Thus IE decreases as we go down the group and the amount of shielding increases.

47
Q

What is shielding?

A

The lessening of the pull of the nucleus by the inner shells of electrons.

48
Q

What is the plum pudding model?

A

Atoms consisted of a sphere of positive charge with small negative charges distributed evenly within it.

49
Q

What is the electron shell model?

A

The atom consists of a small, dense central nucleus surrounded by orbiting electrons in electron shells.

50
Q

Who discovered the electron shell model?

A

Rutherford in the scattering experiment in 1911.

51
Q

What is relative atomic mass?

A

The mean mass of an atom of an element divided by one twelfth of the mean mass of an atom of the carbon-12 isotope.

52
Q

Mr equation?

A

Mean mass of an atom of an element / 1/12 x mean mass of c-12 isotope.

53
Q

What happens when there’s an isotope?

A

Neutral atoms of isotopes will react chemically in the same way because their proton number and electron configuration is the same. However, the different mass number means they have different physical properties.

54
Q

What is mass spectrometry?

A

An analytical technique used to identify different isotopes and find the overall relative atomic mass of an element.

55
Q

What is Time of Flight mass spectrometry?

A

It records the time it takes for ions of each isotope to reach a detector.

56
Q

What can be produced from TOF mass spectrometry?

A

Spectra can be produced showing each isotope present.

57
Q

What 5 main events occur when a sample enters a TOF spectrometer?

A

1)Ionisation
2)Acceleration
3)Ion Drift
4)Detection
5)Analysis

58
Q

What is acceleration?

A

The positively charged ions are then accelerated towards a negatively charged detection plate.

59
Q

What is ion drift?

A

The ions are then deflected by a magnetic field into a curved path. The radius of their path is dependent on the charge and mass of the ion.

60
Q

What is detection?

A

When the positive ions hit the negatively charged detection plate, they gain an electron producing a flow of charge. The greater the abundance, the greater the current produced.

61
Q

What happens during analysis?

A

The current values are used in combination with the flight times to produce a spectra print out with the relative abundance of each isotope displayed.

62
Q

What may happen during the ionisation process?

A

A 2+ charged ion is produced.
Thus it’ll be more affected by the magnetic field.
It’ll produce a curved path of a smaller radius.
As a result, its mass to charge ratio (m/z) is halved.
This can be seen on the spectra as a trace at half the expected m/z value.

63
Q

How to calculate Ar using spectra?

A

m/z x abundance/total abundance

64
Q

What is the order for electron configuration?

A

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

65
Q

When do successive ionisation energies occur?

A

When further electrons are removed which usually requires more energy.

66
Q

Why does ionisation energy required more energy?

A

As electrons are removed, the electrostatic force of attraction between the positive nucleus and the negative outer electron increases. Thus more energy is needed to overcome this attraction so ionisation energy increases.

67
Q

What is an orbital?

A

A region around the nucleus that can hold up to two electrons.

68
Q

What are the two types of ionisation for a mass spectrometer?

A

Electron impact
Electrospray ionisation

69
Q

What is electron impact?

A

An electron gun knocks off one electron from each particle to form 1+ molecular ions.

70
Q

What is electrospray ionisation?

A

Sample is dissolved in a volatile solvent and injected through a fine hypodermic needle to give an aerosol. The needle is attached to a positive terminal of a high voltage power supply and particles gain a proton from the solvent as they leave the needle producing XH+ ions.

71
Q

When would you use electrospray ionisation?

A

For substances with higher molecular mass including biological molecules.

72
Q

When is electron impact used?

A

For organic or inorganic molecules with a low formula mass.

Physical Chemistry (4 decks)

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