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ISEB chemistry for IZZY > Chemical changes > Flashcards

Chemical changes Flashcards

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1
Q

Thermal decomposition of metal carbonates gives you what products?

A

Metal oxide plus carbon dioxide

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2
Q

State the word equation for the thermal decomposition of copper carbonate.

A

Copper carbonate ——-> copper oxide plus carbon dioxide

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3
Q

State the word equation for the thermal decomposition of potassium permanganate

A

potassium permanganate ————> potassium mangnate + manganese oxide + oxygen

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4
Q

What happens to the atoms during a chemical reaction?

A

Chemical bonds are broken and the atoms rearrange themselves.

Atoms are not created or destroyed

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5
Q

What is an exothermic chemical reaction?

A

One which gives out energy - usually heat

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6
Q

What is an endothermic chemical reaction?

A

One which takes in energy - usually heat

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7
Q

What changes could you see during a chemical reaction which show that changes have happened?

A
  1. There may be a colour change eg blue hydrated copper sulphate becomes white anhydrous copper sulphate
  2. You could get a gas given off - bubbles or even smelly fumes
  3. You could get a solid made
  4. Some things would even explode!
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8
Q

What is oxidation?

A

It is the gain of oxygen
A chemical reaction between a substance and oxygen where the oxygen combines with the substance
A good example is the oxidation of iron
Iron + oxygen —-> iron oxide (rust)

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9
Q

What is combustion?

A

It is an oxidation reaction which happens when a substance is burned in oxygen (air)

eg magnesium ribbon which is a shiny metal burns to give a white powder - magnesium oxide

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10
Q

State the three things needed for combustion to occur

A
  1. Fuel
  2. Oxygen
  3. Heat
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11
Q

Carbon will burn in oxygen, identify the product and describe the flame

A
  1. Carbon dioxide
  2. Orange flame
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12
Q

Sulfur will burn in oxygen, identify the product and describe the flame

A
  1. sulfur dioxide
  2. pale blue flame
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13
Q

Iron will burn in oxygen, identify the product and describe the flame

A
  1. Iron oxide
  2. orange flame
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14
Q

Magnesium will burn in oxygen, identify the product and describe the flame

A
  1. Magnesium oxide
  2. bright white flame
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15
Q

What is a hydrocarbon?

A

It is a fuel consisting of atoms of carbon and hydrogen
Examples are, methane, butane and propane, coal, petrol and oil
They are used to provide energy when burned
eg
Methane + Oxygen ——-> carbon dioxide + water (+ energy)
the energy isn’t a product with atoms so it is in brackets!

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16
Q

Describe the test for oxygen

A

If oxygen is collected in a test tube it will relight a glowing splint

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17
Q

Describe the test for carbon dioxide

A

carbon dioxide will turn limewater milky/cloudy

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18
Q

Explain the term thermal decomposition

A

When a substance is heated the heat breaks down the chemical bonds and two or more new substances are formed

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19
Q

State the word equation for the thermal decomposition of copper (II) carbonate
Describe the colour change

A

Copper (II) carbonate —-> copper (II) oxide + carbon dioxide
The green carbonate becomes black oxide

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20
Q

State the word equation for the thermal decomposition of hydrated cobalt chloride
Describe the colour change

A

hydrated cobalt chloride —–> anhydrous cobalt chloride + water
Pink hydrated becomes blue anhydrous

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21
Q

What is reduction

A

the opposite of oxidation it is removal of oxygen from a compound
eg iron oxide + carbon ——-> iron + carbon dioxide

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22
Q

Explain how a metal can be extracted from it’s ore

A

An ore is a rock containing metal compounds often oxides. Carbon can be used to extract some metals from their ore using a reduction reaction
eg iron oxide + carbon ——-> iron + carbon dioxide

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23
Q

Explain the pH scale

A

Numbers from 0 to 14 which describe how alkaline or acidic a substance is.
0 being the strongest acid down to 6 the weakest. 7 is neutral so not acid or alkali
the weakest alkali is 8 and the strongest 14

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24
Q

What is an indicator?

A

Something which can show how acid or alkaline a substance is by changing colour

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25
Q

Describe how you would use universal indicator to test the pH of an unknown solution

A
  1. A solution is a liquid so put a few drops on to a white dimple tile
  2. Add a few drops of universal indicator solution
  3. Check the colour of the mixture against a colour chart.
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26
Q

Identify some indicators and their uses

A
  1. Litmus paper- acids turn red and alkalis blue
  2. Red cabbage water - acid red, neutral purple, alkali turquoise or yellow
  3. Universal indicator acid red to yellow depending on strength, neutral green, alkali blue to purple
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27
Q

Explain the term base in chemistry

A

A base is any substance that will react with an acid to form a salt plus water.
The reaction is called neutralisation because the products are no longer acid or alkali and have a neutral pH of 7.
eg hydrochloric acid + sodium hydroxide —–> sodium chloride + water

28
Q

How are metal carbonates different from other bases in their reaction with acids?

A

Carbonates will give salt plus water like other bases but also carbon dioxide
eg hydrochloric acid + calcium carbonate ——> calcium chloride + water + carbon dioxide

29
Q

Identify the salt produced when hydrochloric acid is added to a base

A

chloride salt

30
Q

Identify the salt produced when sulfuric acid is added to a base

A

sulfate salt

31
Q

Identify the salt produced when nitric acid is added to a base

A

nitrate salt

32
Q

Explain how indigestion can be neutralised

A
  1. The stomach uses hydrochloric acid to digest food.
  2. Too much (excess) stomach acid can cause pain called indigestion
  3. A base such as magnesium oxide can be taken which will neutralise the excess acid and stop the pain
  4. The magnesium oxide reacts with the hydrochloric acid to form magnesium chloride and water which are both pH neutral.
  5. Indigestion tablets are made from medium strength bases as strong bases would send the pH too high which could damage the stomach and stop the digestive enzymes from working
33
Q

Explain how acid soil could reduce plant growth

A

Soil can be acidic, alkali or neutral depending on the minerals it was formed from
Some plants such as camillas prefer acid soil
Other plants prefer alkali or neutral soil.
Some hydrangea flowers change colour depending on the type of soil!
Calcium hydroxide (lime) can be added to soil to make it less acidic
Having the wrong pH in soil can stunt plant growth or even kill a plant

eg sulfuric acid + calcium hydroxide —–> calcium sulfate + water

34
Q

Ammonia is neutralised by nitric acid when making fertiliser. How is this reaction different from most other neutralisation reactions?

A

Nitric acid + ammonia ——-> ammonium nitrate
It is different because no water is produced.

35
Q

Explain how the product of nitric acid and ammonia is used by farmers and gardeners

A

Nitric acid + ammonia ——-> ammonium nitrate
Ammonium nitrate is added to soil as a source of nitrogen
Plants need nitrogen to produce proteins
Adding ammonium nitrate to the soil increases crop yields

36
Q

What is the mnemonic for the reactivity series of metals

A

PSC MAZIL CSG
Please send Charlie’s monkeys and zebras in lead cages safely guarded

37
Q

List the metals in order of reactivity greatest first

A

Potassium
Sodium
Calcium
Magnesium
Aluminium
Zinc
Iron
Lead
Copper
Silver
Gold

38
Q

Wherabouts does carbon sit in the reactivity series of metals?

A

between aluminium and zinc

39
Q

Wherabouts does hydrogen sit in the reactivity series of metals

A

between lead and copper

40
Q

Which metals can be extracted from their ore using carbon in a reduction reaction

A

Only those below carbon in the reactivity series so
Zinc
Iron lead
Copper
Siver
Gold

41
Q

How does the reactivity of metal affect our use of it?

A
  1. Very unreactive metals such as gold and silver don’t oxidise or corrode so are used for jewellery and electrical contacts
  2. Lead and copper also dont corrode and are used on roofs and pipes
  3. if iron is used in construction it usually has a barrier such as paint or oil to keep te air and water from it to prevent oxidation. This is because it is more reactive.
42
Q

How do metals react with dilute acid

A

Metal + acid ——-> salt + hydrogen

43
Q

Identify the salt produced when hydrochloric acid is added to a metal

A

chloride salt

44
Q

Identify the salt produced when sulfuric acid is added to a metal

A

sulphate salt

45
Q

Identify the salt produced when nitric acid is added to a metal

A

nitrate salt

46
Q

Which metals react violently with dilute acids?

A

PCS
potassium
calcium
sodium

47
Q

Which metals react fairly well with dilute acids?

A

MAZIL
magnesium
aluminium
zinc
iron
lead

48
Q

Which metals do not react with dilute acids?

A

CSG
copper
silver
gold

49
Q

If magnesium ribbon is put into a beaker of dilute sulfuric acid what will the products be?

A

Magnesium sulfate and hydrogen

50
Q

Which metals will react with water?

A

The ones above hydrogen in the reactivity table so
PSC will react with cold water
MAZIL will react with steam
CSG are below hydrogen so do not react

51
Q

Which metals will burn in oxygen?

A

All of them except gold and silver.
PSCM burn with a bright flame
AZILC react slowly when heated

52
Q

What is a displacement reaction?

A

When a more reactive metal kicks out a less reactive metal from its compound in a salt solution

53
Q

Identify the type of reaction and describe what happens when magnesium ribbon is placed into a test tube containing copper sulfate solution

A

A displacement reaction
take blue copper sulfate solution put in a strip of a more reactive metal such as magnesium.
The magnesium kicks the copper out of the sulphate solution forming magnesium sulfate solution which is colourless
The copper coats the metal ribbon turning it from silver colour to copper colour

Magnesium + Copper sulfate —> Magnesium sulfate plus copper

54
Q

Which metals could displace aluminum and which would not

A

PSCM could
ZILCSG could not
potassium sodium calcium magnesium yes
zinc iron lead copper silver gold no

55
Q

Identify the 3 different flames on a bunsen burner

A
  1. Yellow safety flame- air hole closed- not used for heating as causes soot but can be seen hence safety!
  2. Medium Blue flame - air hole half open - for gentle heating, hotter than a yellow flame
  3. Roaring Blue Flame - air hole fully open - vigorous heating it is the hottest flame
56
Q

When decomposition of copper carbonate is complete the colour changes from green to what?

A

white

57
Q

What colour is copper carbonate?

A

Green

58
Q

What colour is copper oxide?

A

White

59
Q

What does copper carbonate turn into when it is heated

A

Copper oxide

60
Q

How can we tell that a chemical reaction has taken place when we heat copper carbonate?

A

The colour changes from green to white

61
Q

What can you see when potassium permanganate is heated

A

Purple potassium permanganate becomes green potassium manganate

62
Q

What colour is potassium permanganate?

A

Purple

63
Q

What colour is potassium manganate?

A

Green

64
Q

What are the names of the elements or compounds on either side of an equation

A

The elements or compounds which are at the start are called the reactants, what is left are called the products.

65
Q

Describe the reactivity of group one metals in water

A

Group 1 metals all react violently in water to produce the metal hydroxide plus hydrogen

66
Q

Describe the reactivity of group 2 metals in water

A

The smaller group 2 metals will react with steam to produce a metal hydroxide plus hydrogen
As you move down the group the metals become more reactive and will react with cold water.
This is because the bonds are weaker as the last two electrons are further away from the nucleus

ISEB chemistry for IZZY (5 decks)

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