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LGS GCSE OCR Chemistry A > C4 > Flashcards

C4 Flashcards

1
Q

What are the group 1 elements also known as?

A

Alkali metals

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2
Q

What is the general trend in density down group 1?

A

Increasing

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3
Q

What is the general trend in melting point down group 1?

A

Decreasing

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4
Q

What is the general trend in reactivity down group 1?

A

Increasing

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5
Q

Explain the trend in reactivity down group 1.

A

Reactivity increases as you go down the group;
because the outer shell electron gets further from the nucleus;
so there is a weaker force of attraction between the outer shell electron and the nucleus;
so the outer shell electron is lost more readily

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6
Q

Which group 1 element reacting with water does this best describe?
Fizzes steadily and slowly dissapears

A

lithium

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7
Q

Which group 1 element reacting with water does this best describe?
melts to form a silver ball, fizzes vigourously and quickly disappears

A

sodium

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8
Q

Which group 1 element reacting with water does this best describe?
immediately ignites, burns with a lilac flame and very quickly disappears

A

potassium

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9
Q

What two products are formed when group 1 metals react with water?

A

hydrogen and a metal hydroxide

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10
Q

Would you expect the solution formed from the reaction of a group 1 metal with water to be acidic or alkaline?

A

alkaline

due to the formation of a metal hydroxide

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11
Q

What name are the group 17 (old group 7) elements known by?

A

The halogens

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12
Q

What name is given to a compound containing a group 17 (old group 7) element?

A

Halide

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13
Q

What is the general trend in reactivity of the halogens going down the group?

A

Decreasing

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14
Q

What is the general trend in melting and boiling points of the halogens going down the group?

A

Increasing

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15
Q

What is the general trend of the colours of the halogens going down the group?

A

Tend to get darker

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16
Q

What is the general trend in the density of the halogens going down the group?

A

Increasing

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17
Q

Explain the trend in reactivity of the halogens going down the group.

A

Reactivity decreases as you go down the group;
because the outer shell gets further from the nucleus;
so there is a weaker force of attraction between the outer shell electrons and the nucleus;
so electrons are gained less readily

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18
Q

Which halogens can displace other halogens from their halide compounds?

A

More reactive halogens can displace less reactive halogens from their halide compounds

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19
Q

Which halogens can displace iodine from NaI?

A

fluorine, chlorine and bromine

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21
Q

Which halogens can displace bromine from KBr

A

fluorine and chlorine

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21
Q

Which halogens can displace chlorine from KCl

A

fluorine

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22
Q

What are the products of this displacement reaction?

Cl2 + 2KBr –>

A

Cl2 + 2KBr –> 2KCl + Br2

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23
Q

What are the products of this displacement reaction?

F2 + 2NaI –>

A

F2 + 2NaI –> 2NaF + I2

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24
Q

What observations would you expect to make when adding aqueous chlorine solution to a solution of potassium bromide?

A

Colourless potassium bromide solution turns orange/brown

due to the formation of bromine

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25
Q

What name are the group 0 elements commonly known as?

A

The noble gases

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26
Q

What is the general trend in the density of the group 0 elements going down the group?

A

Increasing

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27
Q

What is the general trend in boiling points of the group 0 elements going down the group?

A

Increasing

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28
Q

Explain the lack of reactivity of the group 0 elements?

A

All group 0 elements have a full outer shell of electrons;
so they have no tendency to either gain or lose electrons;
so they don’t readily form ions or covalent bonds

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29
Q

```

~~~

What are some general properties of all metals

A

Shiny when freshly cut;
good conductors of electricity;
malleable

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30
Q

In what ways do the properties of the transition metals differ from the group 1 metals?

A

Transition metals are stronger and harder;
have higher densities;
have higher melting points

except mercury which is a liquid at room temperature

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31
Q

Why do the compounds of transition metals sometimes include roman numerals in their formulae?

A

Transition metal elements often form several ions with different charges.

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32
Q

What name is given to the elements in groups 3 to 12 of the periodic table?

A

Transition metals

33
Q

What test is used for carbon dioxide?

A

When carbon dioxide is bubbled through limewater, the limewater turns cloudy due to the formation of a white precipitate

34
Q

What test is used for chlorine?

A

Chlorine turns damp blue litmus red, then bleaches it white.

35
Q

What test is used for hydrogen?

A

When a lit splint is held to the mouth of a container filled with hydrogen, the hydrogen ignites with a squeaky pop

36
Q

What test is used for oxygen?

A

A glowing splint will reignite when held in a container of oxygen

37
Q

What flame test colour indicates lithium ions?

38
Q

What flame test colour indicates sodium ions?

39
Q

What flame test colour inidcates potassium ions?

40
Q

What flame test colour indicates calcium ions?

A

Orange-red

41
Q

What flame test colour indicates copper ions?

A

Green-blue

42
Q

A red flame is indicative of which ion?

43
Q

A yellow flame is indicative of which ion?

44
Q

A lilac flame is indicative of which ion?

45
Q

An orange-red flame is indicative of which ion?

46
Q

A green-blue flame is indicative of which ion?

47
Q

A green precipitate during a hydroxide precipitate test indicates the presence of which ion?

48
Q

An orange-brown precipitate during a hydroxide precipitate test indicates the presence of which ion?

49
Q

An blue precipitate during a hydroxide precipitate test indicates the presence of which ion?

50
Q

A white precipitate that does not redissolve in excess sodium hydroxide during a hydroxide precipitate test indicates the presence of which ion?

51
Q

A white precipitate that redissolves in excess sodium hydroxide during a hydroxide precipitate test indicates the presence of which ion?

52
Q

What colour precipitate is formed when sodium hydroxide is added to a solution containing iron(II) ions?

53
Q

What colour precipitate is formed when sodium hydroxide is added to a solution containing iron(III) ions?

A

orange-brown

54
Q

What colour precipitate is formed when sodium hydroxide is added to a solution containing copper(II) ions?

55
Q

What colour precipitate is formed when sodium hydroxide is added to a solution containing calcium ions?

56
Q

What colour precipitate is formed when sodium hydroxide is added to a solution containing zinc ions?

57
Q

How can a zinc hydroxide precipitate be distinguished from a calcium hydroxide precipitate?

A

The zinc hydroxide precipitate will redissolve in excess sodium hydroxide, whislt the calcium hydroxide precipitate will not redissolve

58
Q

What test is used for sulfate ions?

A

A white precipitate will form when barium chloride solution is added to a solution containing sulfate ions

the precipitate is insoluble barium sulfate

59
Q

What test is used for carbonate ions?

A

A solution containing carbonate ions will effervesce when dilute acid is added

Due to the formation of carbon dioxide gas - test also works on solids

effervescence = bubbling

60
Q

What test is used for chloride ions?

A

A white precipitate forms when silver nitrate solution is added to a solution containing chloride ions.

the precipitate is insoluble silver chloride

61
Q

What test is used for bromide ions?

A

A cream precipitate forms when silver nitrate solution is added to a solution containing bromide ions.

the precipitate is insoluble silver bromide

62
Q

What test is used for iodide ions?

A

A yellow precipitate forms when silver nitrate solution is added to a solution containing iodide ions.

the precipitate is insoluble silver iodide

63
Q

An white precipitate during a silver nitrate test indicates the presence of which ion?

64
Q

An cream precipitate during a silver nitrate test indicates the presence of which ion?

65
Q

An yellow precipitate during a silver nitrate test indicates the presence of which ion?

66
Q

Effervescene when dilute acid is added to a solution indicates the presence of which ion?

67
Q

A white precipitate when barium chloride is added to a solution indicates the presence of which ion?

68
Q

Why might you acidify a solution with hydrochloric acid before carrying out the barium chloride test?

A

To make sure any carbonate ions have reacted to form carbon dioxide first

otherwise a precipitate of barium carbonate could give a false positive

69
Q

State three advantages instrumenta methods of analysis have over chemical methods of analysis.

A

greater sensitivity;
greater accuracy;
greater speed

70
Q

In a gas chromatogram, what is represented by each peak

A

a substance present in the mixture

71
Q

How many peaks would a gas chromatogram of a pure substance have?

72
Q

How many peaks would a gas chromatogram of a mixture of three compounds have?

73
Q

What feature of a gas chromatogram represents the relative amount of a substance?

A

The area under the peak

74
Q

What is the time taken for a substance to travel through a gas chromatography column known as?

A

retention time

75
Q

What are the three main uses of mass spectrometry?

A

measuring the mass of atoms and molecules;
determining the relative amounts of different isotopes of an atom;
determining the stucture of molecules

76
Q

In a mass spectrum, what does the peak to the far right represent?

A

the molecular ion

77
Q

In a mass spectrum, what do the peaks to the left of the right-most peak represent?

A

different fragments of the molecular ion

78
Q

What quantity is measured on the horizontal axis of a mass spectrum

A

the mass to charge ratio
(m/z)

where m is mass and z is charge

79
Q

What is the m/z ratio of the molecular ion equal to?

A

the relative formula mass (Mr) of the molecule

assuming at GCSE that the molecular ion has a +1 charge

LGS GCSE OCR Chemistry A (7 decks)

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