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A-Level Edexcel Chemistry > Chapter 1 - Steven > Flashcards

Chapter 1 - Steven Flashcards

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1
Q

What is the symbol of the proton?

A

P

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2
Q

What is the symbol of a neutron?

A

n

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3
Q

What is the symbol of an electron?

A

e-

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4
Q

What is the relative mass of a proton?

A

1

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5
Q

What is the relative mass of a neutron?

A

1

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6
Q

What is the relative mass of an electron?

A

1 / 1840

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7
Q

What is the relative charge of a proton?

A

+1

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8
Q

What is the relative charge of a neutron?

A

0

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9
Q

What is the relative charge of an electron?

A

-1

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10
Q

Where are protons located in the atom?

A

In the nucleus of the atom

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11
Q

Where are neutrons located in the atom?

A

In the nucleus of the atom

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12
Q

Where are electrons located in the atom?

A

In energy levels surrounding the nucleus

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13
Q

What does the nucleus contain?

A

Protons and neutrons

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14
Q

What is the atomic number?

A

The number of protons and electrons

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15
Q

What is the mass number?

A

The number of protons + number of neutrons

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16
Q

What are isotopes?

A

Different forms of the same element with different masses

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17
Q

What do all isotopes contain?

A

The same number of protons

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18
Q

What is the relative isotopic mass?

A

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

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19
Q

Why is the mass number and relative isotopic not always the same?

A

Because the isotopic mass number is not always a whole number as it is relative to the mass of carbon-12.

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20
Q

What is the relative atomic mass?

A

The weighted mean mass of an atom of an element compared to 1/12 of the mass of an atom of carbon-12.

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21
Q

What is the difference between the atomic mass and the isotopic mass?

A

The isotopic mass is from 1 isotope, whereas the atomic mass is taken from all the isotopes

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22
Q

What does a mass spectrometer measure?

A

The masses of atoms and molecules

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23
Q

What is the molecular ion peak?

A

The peak with the highest mass:intensity ratio on the spectrum

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24
Q

What are quantam shells?

A

Well-defined energy levels that

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25
Q

Where is the 1st quantam shell located?

A

In the region closest to the nucleus

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26
Q

What is the relative molecular mass?

A

The average mass of a molecule or formula, compared to 1/12 the mass of carbon-12

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27
Q

How do you work out the relative atomic mass of an element from its isotopic abundances?

A

1) Multiply each relative isotopic mass by its % abundance and add up the results
2) Divide by 100

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28
Q

What is a mass spectra produced by?

A

Mass spectrometers

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29
Q

List 2 things that mass spectrometers can tell us:

A
  • The relative isotopic mass

- The abundances of different elements

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30
Q

What does ‘m/z’ stand for?

A

The mass/charge ratio

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31
Q

What do electrons move round the nucleus in?

A

Quantum shells

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32
Q

Which have higher energy levels, shells near or far from the nucleus?

A

Shells far from the nucleus

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33
Q

What do subshells contain?

A

Different numbers of orbitals, which can hold up to 2 electrons

34
Q

How many orbitals does an s sub shell contain?

A

1

35
Q

How many orbitals does a p sub shell contain?

A

3

36
Q

How many orbitals does a d sub shell contain?

A

5

37
Q

How many orbitals does an f sub shell contain?

A

7

38
Q

How many electrons are in shell 1?

A

2

39
Q

How many electrons are in shell 2?

A

8

40
Q

How many electrons are in shell 3?

A

18

41
Q

How many electrons are in shell 4?

A

32

42
Q

What is an orbital?

A

The bit of space that an electron moves in

43
Q

What is spin-pairing?

A

When the electrons in each orbital have to spin in opposite directions

44
Q

What shape are s-orbitals?

A

Spherical

45
Q

What shape are p-orbitals?

A

Dumbell

46
Q

What angles are the 3 p-orbitals at to each other?

A

At right angles

47
Q

Do electrons fill orbitals singly or pair up?

A

They fill orbitals singly first

48
Q

What do electrons fill up first?

A

The lowest energy subshells

49
Q

What fills up first, the 4s subshell or the 3d subshell?

A

The 4s subshell

50
Q

What is the s-block of the periodic table?

A

Groups 1 + 2

51
Q

What is the d-block of the periodic table?

A

The transition metals

52
Q

What is the p-block of the periodic table?

A

Groups 3 to 7

53
Q

What is electromagnetic radiation?

A

Energy that’s transmitted as waves

54
Q

As you go along the EM radiation, what does the radiation increase in?

A

Frequency

55
Q

If an atoms’s electrons take in energy from the surroundings, what happens?

A

They can move to higher energy levels further from the nucleus

56
Q

How do electrons release energy?

A

By dropping from higher energy levels to a lower one

57
Q

What does an emission spectrum show you?

A

The frequencies of light emitted when electrons drop down energy levels

58
Q

As the number of energy levels increases, what decreases?

A

The distance between the set of lines on the emission spectra

59
Q

What are the 4 basic principles about electron shells?

A
  • Electrons Only exist in fixed orbits of shells
  • Each shell has a fixed energy
  • Radiation has a fixed frequency
  • When an electron moves between shells, EM radiation is emitted or absorbed
60
Q

Are energy levels discrete or continuous?

A

Discrete

61
Q

What does ‘discrete’ mean?

A

There is no in-between stage

62
Q

What is the 1st ionisation energy?

A

The energy needed to remove 1 electron from each ato in 1 mole of gaseous atoms to form 1 mole of gaseous 1+ atoms

63
Q

What are the 3 factors that affect ionisation energy?

A
  • Nuclear charge
  • Electron shell
  • Shielding
64
Q

How does nuclear charge affect ionisation energy?

A

The more protons there are in the nucleus, the stronger the atrraction to the electrons

65
Q

How does the elctron shell affect ionisation energy?

A

Attraction falls off rapidly with distance

66
Q

How does shielding affect ionisation energy?

A

As the number of electrons between the outer electrons and nucleus increases, the outer electrons feel less attraction to the nucleus.

67
Q

What does a high ionisation energy mean?

A

There is a strong attraction between the electronq and the nucleus, so more energy is needed to overcome the attraction and remove the nucleus

68
Q

As you go down a group in the periodic table, what happens to the ionisation energies?

A

They fall

69
Q

What is the 2nd ionsiation energy?

A

The energy needed to remove 1 electron from each ion in 1 mole of gaseous 1+ ions to form 1 moles of gaseous 2+ ions

70
Q

What is the equation for the nth ionsiation energy?

A

X^n+1 —> X^n+ +e-

71
Q

What happens to the atomic radius as you go across a period?

A

It decreases

72
Q

Does the ionisation energy increase or decrease as you go across a period?

A

It increases

73
Q

What is the drop in ionsiation energy between groups 5 and 6 due to?

A

-The electron repulsion

74
Q

As you go across a period, what happens to the type of bond formed between the atoms of the element?

A

The type of bond changes

75
Q

As the type of bond changes as you go across a period, what does this affect?

A

The melting and boiling point trend

76
Q

For metals, what happens to the melting and boiling point as you go across a period?

A

They increase

77
Q

What happens to the metallic bonds in metals as you go across a period?`

A

They get stronger

78
Q

Why do the metallic bonds in metals get stronger as you go across a period?

A

The metal ions have an increasing number of delocalised electrons and decreasing radius, so there is a stronger attraction between the metal ions and the electrons

79
Q

Why do carbon and silicon have high melting and boiling points?

A

Giant covalent lattice, meaning they have strong covalent bonds.

80
Q

Why do the elements with simple molecular structures have low melting and boiling points?

A

London forces are easily overcome as they are weak

81
Q

Why do the noble gases have low melting and boiling points?

A

They exist as individual atoms, resulting in weak London forces

A-Level Edexcel Chemistry (24 decks)

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