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Chemistry AS Level More Specific > Atomic Structure > Flashcards

Atomic Structure Flashcards

1
Q

In the nucleus, there is…

A

Neutrons and protons

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2
Q

Most of the mass in the atom is because?

A

Nucleus (protons and neutrons)

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3
Q

How do electrons move?

A

In orbitals

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4
Q

The orbitals in an atom take up?

A

Most of the volume

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5
Q

The diameter of the nucleus is what compared to the rest of the atom?

A

Very small

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6
Q

What is the relative mass and charge of protons?

A

1 and +1

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7
Q

What is the relative mass and relative charge of a neutron?

A

1 and 0

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8
Q

What is the relative mass and charge of an electron?

A

1/2000 and -1

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9
Q

What does the mass number tell you?

A

Total number of neutrons and protons

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10
Q

What does the atomic number tell you?

A

The number of protons

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11
Q

For neutrally charged atoms, what can we say about the number of protons and neutrons?

A

They are equal

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12
Q

If they atom is charged, what can we say about the number of protons and electrons?

A

They are unequal

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13
Q

In a positively charged ion, there are

A

More protons than electrons

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14
Q

In a negatively charged ions, there are

A

More electrons than protons

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15
Q

Define isotope

A

Atoms with the same number of protons and electrons but different number of neutrons

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16
Q

Do isotopes have the same chemical properties? Why?

A

Yes

The same number and arrangement of electrons i.e the same electron configuration

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17
Q

Do isotopes have the same physical properties? Why?

A

No, but only slightly

Depends on mass of an atom

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18
Q

Examples of how physical properties of an isotopes differ

A

Different densities, rates of diffusion

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19
Q

What was Dalton’s model of an atom like?

A

Solid spheres

Different spheres make up the different elements

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20
Q

What was Thompson’s model of the atom like?

A

Came up with the ‘plum pudding’ model
Discovered electrons
Electrons were surrounded by positively charged ‘pudding’

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21
Q

What was Rutherford’s model of an atom like?

A

Tiny positively charged nucleus surrounded by a ‘cloud’ of negative electrons. Most of the atom was empty space

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22
Q

How did Rutherford prove that Thompson’s plum pudding model was wrong?

A

Through the gold foil experiment

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23
Q

If Thompson’s model was right, what would the experiment shown? Explain why

A

That all of the alpha particles would be deflected

The positive alpha particle would be repelled by the positive atom

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24
Q

What actually happened during the gold foil experiment?

A

Most of the particles went straight through the foil with only a small number being deflected backwards

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25
Q

What was Rutherford’s model called?

A

Nuclear model of the atom

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26
Q

What was wrong with Rutherford’s model?

A

The cloud of electrons would collapse into the nucleus, causing the atom to dissipate

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27
Q

What did Bohr propose in his model?

A

That electrons are split into orbitals of fixed energy.

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28
Q

What happens when an electron moves across a shell?

A

Electromagnetic radiation is absorbed or emitted

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29
Q

When an electron is moving to a shell closer to the nucleus, then…

A

Electromagnetic radiation is emitted

30
Q

When an electron is moving to a shell that is further away from the nucleus, then…

A

Electromagnetic radiation is absorbed

31
Q

Atoms are made up of?

A

Protons, neutrons and electrons

32
Q

How do you work out whether electromagnetic radiation is emitted or absorbed during the movement of electrons?

A

The arrows go in opposite directions

33
Q

Why is Bohr’s original model wrong?

A

Not all electrons in a shell have the same energy level

34
Q

How has Bohr’s model been refined?

A

Now includes subshells.

35
Q

Despite Bohr’s model not being completely correct, why is it still used?

A

Simple and explains many experimental observations

36
Q

Define relative atomic mass

A

The average mass of an atom of an element, taking in consideration abundance and isotopes, in comparison 1/12th of a carbon-12 atom

37
Q

Define relative isotopic mass

A

The mass of an atom of an isotope of an element compared with 1/12th of a carbon-12 atom

38
Q

Define relative molecular mass

A

The average mass of a molecule, taking into consideration abundance and isotopes, compared with 1/12th of a carbon-12 atom

39
Q

Explain the first step of electrospray ionisation

A

The sample is dissolved in a polar solvent and pushed through a capillary needle at high pressure. A high voltage is applied to it, causing the particles to lose an electron. The ionised particles are separated from the solvent, leaving a gas of positive ions

40
Q

Explain the second step of time of flight

A

All the ions are accelerated by an electromagnetic field, giving each ion the same kinetic energy as the rest. This means that ions with a smaller mass/charge ratio are more accelerated as they are lighter

41
Q

What happens during the third stage of time of flight?

A

The ions leave the electromagnetic field at a constant speed and a constant kinetic energy and therefore continue through the drift region in the same state

42
Q

What happens in the forth region?

A

Ions with lower mass/charge will reach the detector first. The detector records the current created when the ion hits it and the amount of time the ion takes to travel through the spectrum, which is then used to create a mass spectrum

43
Q

Why must the time of flight have a vacuum?

A

So that the gas sample particles do not collide with other particles and distort the results

44
Q

What is the difference in time of flight method using electro bombardment?

A

They use an electro gun to remove an electron of the atom

45
Q

How is a current created in time of flight?

A

The electron is given back to the ion

46
Q

What are the two problems with electro bombardment?

A

Fragmentation

The removal of more than one electron

47
Q

What is electro spray used to analyse?

A

Large bio molecules

Polar organic molecules

48
Q

What polar solvents are used in electro spray?

A

Water, methanol, or both

49
Q

What is the current used in electro spray?

A

4000 volts

50
Q

What is the fancy word for ionised spray?

A

Nebulise

51
Q

How is the solvent evaporated?

A

Through the high voltage

52
Q

What is the fancy word for solvent evaporation?

A

Desolvation

53
Q

Why is the sample dissolved in a polar substance?

A

Provides the H+ ion

54
Q

Each shell is given what help use identify it?

A

Principal quantum number

55
Q

As the shell furthers from the nucleus, the principal quantum number _________ and the energy __________?

A

Increases and increases

56
Q

Each individual shell is divided into?

A

Subshells

57
Q

What are the types of subshells?

A

S, P, D, F

58
Q

How many orbitals does the S subshell have? And how many electrons can it hold?

A

1 and 2

59
Q

How many orbitals in the p subshell? And how many electrons can it hold?

A

3 and 6

60
Q

How many orbitals are there is the p subshell? And how many electrons can it hold

A

5 and 10

61
Q

How many orbitals are there in the f subshell? And how many electrons can it hold?

A

7 and 14

62
Q

How many electrons can each individual orbital hold?

A

2

63
Q

How do we write short hand electron configuration?

A

The last noble gas in square brackets and additional subshells listed after

64
Q

What are the two elements that do not form normal electron configuration? Why?

A

Chromium and copper

They donate one of their 4s electrons to the 3D orbital, because it is more stable with a full or half-full 3D orbital

65
Q

When transition metals become an ion they…

A

Lose their electron from the 4s orbital before their 3D orbital

66
Q

The S block elements lose their outer electrons

A

to form positive ions with an inert gas configuration

67
Q

Those in the p block gain electrons

A

To form negative ions with inert gas configuration

68
Q

Those in group 0 have…

A

A full outer shell so they are inert

69
Q

What are the three ways electron configuration can be shown

A

Subshell notation
Arrows in boxes
Energy level diagram

70
Q

What are the three rules to working out electron configuration

A

Electrons fill up the lowest energy subshell first
Electrons fill orbitals in a sub-shell singly before they start sharing
For ions, add or remove the electrons from the highest occupying sub-shell

Chemistry AS Level More Specific (1 decks)

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