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Chemistry Topic 1 > Lots Of Stuff > Flashcards

Lots Of Stuff Flashcards

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1
Q

Copper + sulphuric acid –>

A

There is no reaction because copper has a lower reactivity than hydrogen

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2
Q

Calcium + water

A

Calcium hydroxide + hydrogen

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3
Q

Zinc + steam –>

A

Zinc oxide + hydrogen

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4
Q

Aluminium + Sulfuric acid –>

A

Aluminium sulfate + hydrogen

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5
Q

Magnesium + nitric acid –>

A

Magnesium nitrate + hydrogen

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6
Q

How would you show that a test tube contained hydrogen gas?

A

You would hold a lit splint over/into the test tube and if it makes a popping sound hydrogen is present

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7
Q

Zinc + steam –>

A

Zinc oxide + hydrogen

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8
Q

Copper oxide can be reduced to copper metal by heating it in a steam of hydrogen gas. Why was the hydrogen passed through for 15 seconds before the gas was lit?

A

To avoid a small explosion between hydrogen and oxygen.

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9
Q

What does it mean if there is no further change in mass?

A

The experiment was performed until it was finished and the final mass was achieved.

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10
Q

Name two materials that would react together to give hydrogen and which would be suitable for the safe preparation of hydrogen in the lab

A

Zinc and hydrochloric acid

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11
Q

Name two materials that would react together to give hydrogen but which would not be suitable for making hydrogen in the lab

A

Potassium and water because the reaction is too explosive

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12
Q

Zinc + hydrochloric acid ->

A

Zinc chloride + hydrogen

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13
Q

Does potassium react with hydrogen?

A

No, because it is more reaction than hydrogen

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14
Q

An excess if magnesium powder was shaken with copper sulphate solution. The solution became colourless and a red brown powder was seen. Name the red power.

A

Copper

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15
Q

An excess if magnesium powder was shaken with copper sulphate solution. The solution became colourless and a red brown powder was seen. Name the colourless solution

A

Magnesium sulphate

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16
Q

Sodium oxide is heated with copper power. Will there be a reaction?

A

No, because sodium is higher than copper in the reactivity series.

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17
Q

What does a fractionating column do?

A

Separate liquids with different boiling points

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18
Q

Why is it better to dissolve solid in water in a polystyrene cup rather than a beaker?

A

Less heat escapes from the polystyrene

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19
Q

How to prevent a polystyrene cup from being knocked over

A

Place it inside a beaker

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20
Q

How can a student check the reliability of the result?

A

They could repeat the test and make sure the results are the same

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21
Q

Give a safety precaution a student should take when doing experiments

A

Do not touch a hot (basin) as it could burn you

Wear safety glasses

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22
Q

What happens during rusting?

A

The metal reacts with oxygen from the air to form an oxide

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23
Q

Write a chemical equation for the decomposition of hydrogen peroxide

A

2H2O2 —> 2H2O + O2

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24
Q

What is the test for oxygen

A

Put a glowing splint near the gas and if it relights the gas is oxygen

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25
Q

What name is used for the process in which steam turns into water

A

Condensation

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26
Q

What can be used to test for the presence of wh

water?

A

Anhydrous copper sulphate - it should turn from white to blue

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27
Q

Noble gases are very reactive/unreactive

A

Unreactive

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28
Q

Carbon dioxide + water –>

A

Carbonic acid

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29
Q

Give the acid rain equation

A

SO2 + H2O –> H2SO3

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30
Q

Give two pollutant gases that forms acid rain

A

Sulphur dioxide and nitrogen dioxide

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31
Q

State three problems caused by acid rain

A

Acid rain can affect lakes by poisoning the fish and plants
It also attacks structures made of iron and steel
It attacks buildings maybe of limestone and marble

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32
Q

State two observations that can be made when magnesium burns in oxygen

A

The magnesium glows bright white

At the end the magnesium oxide is a white solid

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33
Q

Give the chemical equation for the burning of magnesium, in oxygen

A

2Mg + O2 –> 2MgO

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34
Q

When universal indicator is added to magnesium oxide dissolved in water, the indicator turns blue when added to the solution. What does this tell us?

A

Magnesium oxide is an alkali

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35
Q

Describe an experiment to determine the percentage of oxygen in the air

A

Iron wool is placed at the end of a test tube and the test tube is placed in a beaker of water (upside down.) leave the iron wool until the water stops rising. Oxygen has been used up making iron (111) oxide. Then calculate the percentage of oxygen using this : volume of oxygen divided by total volume in measuring cylinder x 100

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36
Q

Give the chemical equation for the reaction of hydrochloric acid with sodium oxide

A

2Hcl + Na2O –> 2NaCl + H2O

37
Q

Metal + water —>

A

Metal oxide + hydrogen

Or

Metal hydroxide + hydrogen (if it is potassium, sodium, lithium, calcium - they are high in the reactivity series and soluble in water)

38
Q

Observations of sodium and cold water

A

It floats
It moves around the surface
It fizzes
It melts into a silvery ball because the reaction is exothermic

39
Q

Is sodium + water a useful method for preparing hydrogen?

A

No, the metal is too reactive

40
Q

Observations of potassium with cold water

A 
It floats
It fizzed
It moves around the surface
It melts into a silvery ball
It burns with a lilac flame
41
Q

It potassium and water a useful method for preparing hydrogen?

A

No, it is too hard to collect the hydrogen and dangerous of extract the metal

42
Q

Observations of calcium with cold water

A

It bobs up and down
It fizzes
Not all of the calcium dissolves so it gives us a slightly cloudy/milky solution : Ca(OH)2 is only slightly soluble

43
Q

Does magnesium react with cold water

A

VERY slowly

44
Q

Observations of magnesium reacting with steam

A

The magnesium glows bright white
White solid remains
A colourless gas is collected

45
Q

Metal + acid –>

A

Salt + hydrogen

46
Q

Salt:

A

An acid in which the hydrogen has been replaced by a metal

47
Q

Sulfuric acid:

A

H2SO4

48
Q

Hydrochloric acid

A

HCl

49
Q

Nitric acid

A

HNO3

50
Q

Sulfuric acid + metal –>

A

____ sulfate

51
Q

Hydrochloric acid + metal —>

A

_____ chloride

52
Q

Nitric acid + metal —>

A

______ Nitrate

53
Q

What is a catalyst

A

A substance that speeds up a reaction but remains chemically unchanged

54
Q

Add chromium powder to 50% hydrochloric acid

A

The solution should fizz and turn green

It produces hydrogen

55
Q

What is the purpose of anhydrous calcium chloride?

A

It acts as a drying agent

56
Q

Burning hydrogen produces what?

A

Water

57
Q

How to tell if water is pure?

A

Boil the liquid - measure boiling point and if it is at exactly 100 degrees Celsius the water is pure

58
Q

Hydrogen is able to remove ______ from certain metal oxides

A

Oxygen

59
Q

The removal of oxygen by hydrogen is called

A

Reduction

60
Q

Hydrogen + lead (11) oxide —>

A

Water + lead

61
Q

Which metal oxides would you expect hydrogen to be able to reduce?

A

Copper oxide, silver oxide, gold oxide, oxide of any metal below hydrogen

62
Q

Why do you think it is important that the splint id placed in the mouth of a test tube while testing for hydrogen

A

Oxygen from the air is needed

63
Q

Symbol equation of the reaction of hydrogen and nitrogen to make ammonia

A

3H2 + N2 –> 2NH3

64
Q

Ammonium:

A

NH4

65
Q

Ammonia

A

NH3

66
Q

What is hydrogen used for?

A

To turn unsaturated days such as vegetable lol into saturated fats such as margarine

Oxy-hydrogen flame for welding and cutting

Rocket fuel

67
Q

What happens in the decomposition of hydrogen peroxide

A

When dilute hydrogen peroxide is decomposed, either by heating it of by the use of a catalyst such as manganese oxide, MnO2, oxygen is produced and water it left behind

68
Q

What is the word equation for the decomposition of hydrogen peroxide

A

Hydrogen peroxide —> water + oxygen

69
Q

Clean a piece of magnesium using sandpaper. Why?

A

To remove the magnesium oxide coating

70
Q

Does magnesium oxide dissolve in water? State the pH of the resulting solution and give an equation

A

Slightly soluble
MgO + H2O –> Mg(OH)2
Forms magnesium hydroxide which is a weak alkali
Ph 9-11

71
Q

Does carbon dioxide dissolve in water?

A

Yes - slightly

PH - 6 (weak acid)

72
Q

Two possible equations for the reaction with carbon and oxygen

A

2C + O2 –> 2CO

C + O2 –> CO2

73
Q

Does sulphur dioxide dissolve in water?

A

Yes.

Ph-1 (strong acid)

74
Q

Properties of soluble basic (alkaline) oxides

A

They oxides dissolve in water to form hydroxides
They react with acids to form salts
They do not react with other alkalis
Oxides of this metal are at the top of the reactivity series in group 1 and some group 2

Eg potassium oxide, sodium oxide, calcium oxide

75
Q

Properties of insoluble basic oxides

A

These oxides do not dissolve in water
They react with acids to form salts but do not react with alkalis
Oxides of metals low in the reactivity series are of this type

Eg copper oxide, iron (111) oxide, silver oxide

76
Q

Is iron soluble in water?

A

No

77
Q

Properties of acidic oxides

A

These oxides usually dissolve in water to form acids
They react with alkalis to form salts but do not react with other acids
Non metal oxides are usually of this type

Eg, carbon dioxide, sulphur dioxide

78
Q

Neutral oxides properties

A

These oxides usually do not dissolve in water
They do not react with alkalis to form salts and neither do they react with acids
Non metal oxides are usually of this type
If a non metal forms two oxides the one with the more oxygen will be more acidic and the one with less more neutral

Eg carbon monoxide

79
Q

Percentages of oxygen in air?

A

Nitrogen 78%
Oxygen 21%
Argon 0.96%
Carbon dioxide 0.03%

80
Q

What is sulphur dioxide produced by

A

Fossil fuels such as coal

81
Q

Sulphur dioxide can affect people with…

A

Athsma

82
Q

CaCO3 + H2SO4 –>

A

CaSO4 + H2O + CO2

83
Q

Nitrogen dioxide can cause

A

acidic rain

84
Q

The extremely high temperature of a spark caused the nitrogen in the air to

A

Combine with oxygen

85
Q

Which balancing processes affect the concentration of oxygen?

A

Respiration (oxygen in)

Photosynthesis (oxygen out)

86
Q

What makes the percentage if carbon dioxide rise?

A

Deforestation
Increasing population
Burning fossil fuels

87
Q

What effects could an increase in carbon dioxide have?

A 
Co2 is a green house gas
This causes global warming
Sea level rises
Climate change
Desertification
88
Q

What could we do to reduce the concentration of sulphur dioxide and nitrogen oxide

A

Sulphur dioxide;
Use a flue gas
Desulfurisation

Nitrogen oxides;
Cars have catalytic converters which change harmful no2 into co and n2 and co2
Use less motorised transport

Chemistry Topic 1 (1 decks)

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