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zChemistry > Paper 2-SC17,18,19 > Flashcards

Paper 2-SC17,18,19 Flashcards

1
Q

What is group 1?

A

The alkali metals.

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2
Q

What are some of the physical properties of the group 1 metals?

A

They are malleable and conduct electricity. All have relatively low melting points, are soft and easily cut.

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3
Q

What are some of the chemical properties of the alkali metals?

A

They are very reactive and readily form compounds with non-metals. They are easily oxidised and burn brightly in air.

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4
Q

How does the reactivity of the alkali metals change as you go down the group?

A

It increases.

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5
Q

What does lithium+water do?

A

Bubbles fiercely on the surface.

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6
Q

What does sodium+water do?

A

Melts into a ball and fizzes about the surface.

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7
Q

What does potassium+water do?

A

Bursts into flames and flie about the surface.

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8
Q

Why does this trend of reactivity happen?

A

As you go down the group the atoms get larger, the force of attraction between the nucleus and outer shell electron decreases so the electron can be removed easier.

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9
Q

What are group 7?

A

Halogens.

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10
Q

What are all halogens?

A

Diatomic.

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11
Q

What are some of the physical properties of the halogens?

A

They are poor conductors of heat and electricity. Care has to be taken when handling halogens as they are all toxic and corrosive.

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12
Q

What happens to the melting point, boiling point and density as you go down the group 7?

A

Increase.

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13
Q

What is chlorine?

A

Green gas.

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14
Q

What is bromine?

A

Brown liquid.

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15
Q

What is iodine?

A

Purple/black solid.

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16
Q

How do halogens react?

A

react with metals and non-metals in a similar way. React with metals to form salts which contain halide ions.

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17
Q

What are some of the uses of the halogen salts?

A

Table salt. toothpaste, disinfectant in swimming pools.

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18
Q

What can all halogens be used as?

A

Disinfectants and bleaches as they can kill microorganisms and remove the colour from materials.

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19
Q

What do halogens react with hydrogen to form?

A

Halides which dissolve in water to form acidic solutions.

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20
Q

What happens to the reactivity of the halogens as you go down the group?

A

It decreases.

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21
Q

What does fluorine an iron wool cause?

A

Bursts into flames.

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22
Q

What does chlorine and iron wool cause?

A

Glows brightly.

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23
Q

What does bromine and iron wool cause?

A

Glows dull red.

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24
Q

What does iodine and iron wool cause?

A

Changes colour.

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25
Q

How can you work out the order of reactivity of halogens?

A

Displacement reactions.

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26
Q

How can the halogen trend of reactivity be explained?

A

As you go down the group the distance between the outermost shell and nucleus increases so the force of reaction between incoming electron and nucleus is less so ions do not form as easily.

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27
Q

What are group 0?

A

Noble gasses.

28
Q

What are the physical properties of the noble gasses?

A

Colourless, very low melting and boiling points and are poor conductors of heat and electricity.

29
Q

What are the chemical properties of the noble gases?

A

They are inert which means they do not react easily with anything which is why they exist as single atoms.

30
Q

When was the noble gas group discovered?

A

The end of the 19th century.

31
Q

Why were the noble gases difficult to detect?

A

Because they did not react with anything. and there are only small amounts of noble gases in our atmpsphere.

32
Q

What is Krypton uses for?

A

Photography lighting as it produces a brilliant white light whenb electricity is passed through it.

33
Q

What is argon used for?

A

Argon is denser than air and is added to the space above wine in the wine barrels to stop oxygen in the air reacting with the wine.

34
Q

What is helium used for?

A

Helium has a very low density and is non-flammable so it is used in weather balloons and airships.

35
Q

What is neon used for?

A

Neon produces a distinctive red-orange light when electricity is passed through it, this property makes it useful for making long lasting illuminated signs.

36
Q

Why are noble gasses unreactive?

A

Because they are stable.

37
Q

What is the rate of reaction?

A

The speed at which reactants are turned into products.

38
Q

How can we control rates of reactions?

A

Through altering variables such as concentration of solutions, and the size of pieces of solid reactant.

39
Q

Why are reactions normally faster at the start?

A

That is when the concentration of the reactants is the greatest.

40
Q

What must happen for chemical reactions to occur?

A

Particles must collide with enough energy to react.

41
Q

What happens during successful collisions?

A

The energy helps to break bonds so that the atoms can be rearranged to make new substances.

42
Q

What is the activation energy?

A

The energy needed for a reaction to occur.

43
Q

Why can reactions that need an activation energy continue?

A

They release energy.

44
Q

What are reactions that release energy?

A

Exothermic.

45
Q

What are reactions that take in energy?

A

Endothermic.

46
Q

Which reactions will not keep going unless energy is supplied continuously?

A

Endothermic.

47
Q

Surface area and rate of reaction?

A

Higher surface area so smaller chunks have higher rate of reaction as more surface area for colisions.

48
Q

What also affects reaction rate?

A

Pressure of gases, temp, surface area and concentration.

49
Q

What are catalysts?

A

Substances that speed up chemical reactions without being permanently changed and without altering the products.

50
Q

What is an example of a catalyst?

A

Platinum is used as a catalyst in the manufacturing of nitric acid from ammonia.

51
Q

What are the things called that show the rate of reaction?

A

Reaction profiles.

52
Q

What do catalysts require less of?

A

Activation energy.

53
Q

What does the graph of a catalysed reaction look like compared to a normal reaction?

A
54
Q

What are enzymes?

A

Large complex protein molecules that act as catalysts in biological reactions.

55
Q

What are enzymes essential in?

A

Living things and many industries as alcoholic drinks need an enzyme in yeast.

56
Q

What is an exothermic reaction?

A

Energy is transferred from stores of energy in chemical bonds to the surroundings.

57
Q

What are endothermic reactions?

A

Energy is transferred from the surroundings to stores of energy in chemical bonds.

58
Q

How do exo and endo reaction profiles differ?

A
59
Q

What does a precipitate form from?

A

Two solutions.

60
Q

NeutralisatioN?

A

Reaction between acid and a base.

61
Q

Displacement reaction?

A

The reaction between a metal and a compound of a less reactive metal or between a halogen and a compoind of a less reactive halogen.

62
Q

When salts are formed, is it exo or endo?

A

Depends.

63
Q

What reactions have low activation energy’s?

A

Precipitation and neutralisation reactions and start straight away.

64
Q

What reactions have high activation energy’s?

A

Combustion reactions.

65
Q

Is breaking bonds exo or endo?

A

Energy is transferred to the reactants to break their bonds so breaking bonds is endothermic.

66
Q

Is making bonds exo or endo?

A

Energy is transferred to the surroundings as bonds form so making bonds is exothermic.

67
Q

Can you do bond energy calculations?

A

Watch a video on it if you cant you stupid mongoloid.

zChemistry (8 decks)

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