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AQA Physical Chemistry > Fundamental Chemistry > Flashcards

Fundamental Chemistry Flashcards

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1
Q

What is an atom made up of?

A

A nucleus and energy levels (shells)

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2
Q

What does the nucleus contain?

A

Proton and neutrons

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3
Q

What do energy levels contain?

A

Electrons

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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

negligible

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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

What is the overall charge of an atom

A

0

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11
Q

Why is the overall charge of atom 0?

A

There are equal numbers of protons and electrons therefore the charges cancel out

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12
Q

What does the number of energy levels =?

A

Period number of the element

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13
Q

What does the number of electrons in the outer energy level =?

A

Group number of the element

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14
Q

What is the mass number?

A

Sum of protons and neutrons

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15
Q

What is the proton number?

A

Number of protons in an electron

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16
Q

What is the number of electrons equal to?

A

Number of protons

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17
Q

How do you calculate the number of neutrons?

A

Mass number - proton number

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18
Q

What are isotopes?

A

Atoms with the same number of protons, but a different number of neutrons

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19
Q

What is different about isotopes?

A

Mass number because the number of neutrons changes so they have different masses and therefore a slight variance in physical properties

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20
Q

What is the mass number of an isotope referred to as?

A

Relative isotopic mass

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21
Q

What is the same about isotopes?

A

Their chemical properties because their electron configuration doesn’t change

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22
Q

What shows the existence of isotopes?

A

Mass spectroscopy

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23
Q

What does Mass Spectroscopy calculate?

A

Ar - relative atomic mass

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24
Q

What does Ar take into account?

A

The relative isotopic masses and their relative abundances

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25
Q

What is an ion?

A

An atom or molecule with a net electronic charge due to a loss or gain of electrons

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26
Q

Why do ions form?

A

They form as the loss/gain of electrons provides electronic stability by creating a ‘full’ outer energy level

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27
Q

What do metals tend to form?

A

positive ions

28
Q

What are positive ions?

A

cations

29
Q

Why do metals form cations?

A

Because they tend to have few electrons in their outer energy level, it is therefore easier for them to lose electrons

30
Q

What do non-metals tend to form?

A

negative ions

31
Q

What are negative ions?

A

anions

32
Q

Why do non-metals form anions?

A

Because they tend to have many electrons in their outer energy level, it is therefore easier for them to gain electrons. There are exceptions e.g. H^+

33
Q

What ionic charge do group 1 metals form?

A

1+

34
Q

What ionic charge do group 2 metals form?

A

2+

35
Q

What are some cation examples?

A

Al^3+, Ag^+, Zn^2+, Pb^2+, Cu^+, Cu^2+, Fe^2+, Fe^3+, K^+, Mg^2+

36
Q

What ionic charge do group 7 non-metals form?

A

1-

37
Q

What ionic charge do group 6 non-metals form?

A

2-

38
Q

What ionic charge do group 5 non-metals form?

A

3-

39
Q

Give anion examples

A

Cl^-, O^2-, N^3-

40
Q

What do transition metals have?

A

Variable oxidation states

41
Q

What is an ammonium ion?

A

NH4^+

42
Q

What is the charge on an ammonium ion?

A

+

43
Q

What is a hydronium ion?

A

H3O^+

44
Q

What is the charge on a hydronium ion?

A

+

45
Q

What is a hydroxide ion?

A

OH^-

46
Q

What is the charge on a hydroxide ion?

A

-

47
Q

What is a nitrate ion?

A

NO3^-

48
Q

What is the charge on a nitrate ion?

A

-

49
Q

What is a cyanide ion?

A

CN^-

50
Q

What is the charge on a cyanide ion?

A

-

51
Q

What is a carbonate ion?

A

CO3^2-

52
Q

What is the charge on a carbonate ion?

A

2-

53
Q

What is a sulphate ion?

A

SO4^2-

54
Q

What is the charge on a sulphate ion?

A

2-

55
Q

What is a phosphate ion?

A

PO4^3-

56
Q

What is the charge on a phosphate ion?

A

3-

57
Q

What is a molecular ion?

A

A covalent non-metal compound with an overall charge

58
Q

What doesn’t change when ions forms?

A

The number of protons or neutrons

59
Q

What are the 3 steps for writing a formulae?

A
  • Write doen all ions- Balance the charges by adding ions- Remove charges and write the formula
60
Q

What sound all charges add up to in a formula?

A

0

61
Q

What do you change when balancing?

A

The big numbers

62
Q

What do you not change when balancing?

A

The small numbers

63
Q

What is the method for balancing equations?

A
  • Check the formulae- Balance the metals first- Give it a go- Practise
64
Q

What does stoichiometry give?

A

The relative quantitative relationships between substances in a chemical equation

65
Q

What does stoichiometry allow you to work out?

A

The amount of substance if only one is known

AQA Physical Chemistry (12 decks)

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