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IGCSE > Chemistry > Flashcards

Chemistry Flashcards

1
Q

What does the alloy brass consist mainly of?

A

30% Zinc and 70% Copper

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2
Q

MP & BP change in an impure substance

A

MP Decreases and BP increases

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3
Q

Are nitrate salts soluble or insoluble?

A

All of them are soluble

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4
Q

Are ethanoate salts soluble or insoluble?

A

They are all soluble

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5
Q

Are sodium, potassium and ammonium

salts soluble or insoluble?

A

They are all soluble

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6
Q

Are chloride salts soluble or insoluble?

A

Most are soluble except Silver and Lead(II).

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7
Q

Are Sulphate salts soluble or insoluble?

A

Most are soluble except Barium, Calcium and Lead (II)

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8
Q

Are carbonate salts soluble or insoluble?

A

Most are insoluble except Sodium, Potassium and Ammonium

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9
Q

Are Hydroxide salts soluble or insoluble?

A

Most are insoluble except Sodium, Potassium and Calcium (Slightly soluble)

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10
Q

Fractions(2)

A

Part of Petroleum with molecules of similar properties. BP and number of carbon chains.

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11
Q

What increases each fraction when Carbon Chain gets longer?

A

The boiling point and viscosity.

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12
Q

Refinery Gas- Uses, Carbon Atoms and BP

A

Heating and Cooking, 1-4 Carbon Atoms, Below 25 °C

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13
Q

Kerosene/Paraffin - Uses, Carbon Atoms and BP

A

For making jet fuel,12-16 atoms, 150-240°C

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14
Q

Gasoline/Petrol - Uses, Carbon Atoms and BP

A

Fuel for Cars, 4-12 atoms , 40-100°C

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15
Q

Naphta - Uses, Carbon Atoms and BP

A

Raw Product for producing chemicals, 7-14 atoms, 90-150°C

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16
Q

Diesel/Gas Oil - Uses, Carbon Atoms and BP

A

Fuel for Diesel Engines, 14-18 atoms, 220-300°C

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17
Q

Conditions for Substitution Reactions of Alkanes with Halogen

A

Ultraviolet Radiation

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18
Q

Fuel Oil- Uses, Carbon Atoms and BP

A

Fuel for ships and for home heating, 19-25 atoms, 250-320°C

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19
Q

Lubricating Oil - Uses, Carbon Atoms and BP

A

For Lubricants,Polishes, Waxes - 20 to 40 atoms, 300-350

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20
Q

Bitumen - Uses, Carbon Atoms and BP

A

For surfacing roads, more than 70 atoms, more than 350°C

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21
Q

When is the pipette used?

A

Most accurate way of measuring a fixed volume of liquid,usually 10cm3 and 25cm3.

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22
Q

When is the Burette used?

A

Most accurate way of measuring a variable volume of liquid between 0cm3 and 50cm3.

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23
Q

Retention Factor

A

Distance moved by compound ÷ Distance moved by Solvent

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24
Q

What force holds ionic compounds together?

A

The electrostatic force of attraction between positive and negative charges hold ionic compounds together. Often creating a lattice structure of regularly ordered alternating positive and negative ions.

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25
Q

Ionic Compound (4 Properties)

A

High MP & BP
NOT VOLATILE
POLAR COMPOUNDS and Water Soluble
Conducts electricity when in molten or aqueous state

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26
Q

Covalent Compounds (4 Properties)

A

Low MP and BP
Usually Volatile
Tends to be non-polar and insoluble in water however dissolves in organic solvents
Cannot conduct electricity

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27
Q

Diamond Structure

A

Each carbon atom bonds with 4 other carbon, forming a tetrahedron

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28
Q

Diamond Properties and Uses

A

High MP, Extremely Hard and Dense(3.51g/cm3)

Used in jewellery and as cutting tools and their tips.

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29
Q

Uses of Graphite

A

Used in pencils
As an industrial lubricant in engines and locks
Also used to make non reactive electrodes for electrolysis

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30
Q

Structure of Silicon Dioxide

A

A tetrahedron is formed with 1 silicon atom and four oxygen atoms.Each oxygen atom bonds with 2 silicon atoms

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31
Q

What is SiO2 found as and what are its uses?

A

Naturally occurs as sand and quartz.It is cheap and used to make sandpaper and to line the insides of furnaces

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32
Q

Malleable

A

Able to be hammered or pressed into shape without breaking or cracking

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33
Q

Ductile

A

Able to be drawn out into thin wire

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34
Q

What is Avogadro’s Constant

A

6.02×10^23

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35
Q

Test for Hydrogen

A

Gas burns with a pop when a sample is lit with a lighted splint.

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36
Q

Test for Oxygen

A

Relights a glowing splint

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37
Q

Colour of Bromine,Chlorine, Fluorine

A

Red-Brown,Yellow-Green,Pale Yellow

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38
Q

Products and Conditions of Catalytic Cracking

A

Smaller Hydrocarbons and Hydrogen,
Hydrogen and Alkenes products increase if higher pressures and >700°C is used
600-700°C,
Hot catalyst of Silica or Alumina,

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39
Q

Homologous Series (4)

A

Same General Formula
Same Functional Group
Similar Chemical Properties
Difference between each member’s Molecular formula is CH2

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40
Q

How to distinguish between Alkane and Alkene

A

Alkene turns bromine water colourless while alkane doesnt

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41
Q

Addition Polymerization

A

Smaller Unsaturated molecules or monomers react together usually in the presence of a catalyst to form addition polymer.

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42
Q

Hydrogenation (4)

A

The addition reaction between Hydrogen and Alkene to form an Alkane.
150 ° C, Nickel Catalyst
Vegetable Oils into Margarine

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43
Q

Hydration(4)

A

Addition reaction between steam and Alkenes to form Alcohol
Around 300-330°C
60-70 ATM
Concentrated phosphoric acid catalyst

44
Q

2 methods of manufacturing ethanol

A

Hydration of ethene with steam

Fermentation of glucose

45
Q

3 Conditions of Fermentation of Glucose

A

Yeast,
Absence of Oxygen
Between 15 to 35°C

46
Q

Carboxylic Acids

A

Colorless liquids that are weakly acidic acids with functional group -COOH
Forms ethanoate salts

47
Q

Effect of adding NaOH or Ammonia solution to Al3+ salt

A

NaOH-White precipitate, dissolves in excess to form colourless solution
Ammonia- White precipitate, insoluble in excess ammonia

48
Q

Effect of adding NaOH solution to Ammonium NH4 +1

A

Ammonia gas is produced when warmed

49
Q

Ca2+

A

White precipitate, insoluble in excess NaOH

Ammonia-Very faintly visible white precipitate

50
Q

Chromium 3+

A

NaOH- Green precipitate, forms a green solution in excess

Ammonia- Grey-Green Precipitate, insoluble in excess

51
Q

Copper (2+)

A

NaOH- Light blue precipitate, insoluble in excess

Ammonia- Light blue precipitate, soluble in excess to form Dark blue colour

52
Q

Iron 2+

A

NaOH and Ammonia- Green Precipitate, insoluble in excess

53
Q

Iron 3+

A

NaOH and Ammonia- Red brown precipitate, insoluble in excess

54
Q

Zn 2+

A

NaOH and Ammonia-

White precipitate, dissolves in excess to form colourless solution

55
Q

Flame test for Li+

A

Red colour

56
Q

Flame test for Ca2+

A

Orange Red

57
Q

Flame test for Cu 2+

A

Blue green

58
Q

Flame test for K+

A

Lilac

59
Q

Flame test for Na+

A

Yellow colour

60
Q

Order of Petroleum Fractional Distillation

A 
Refinery Gas-
Gasoline
Naphta
Kerosene or Paraffin
Diesel oil
Fuel oil
Lubricating oil
Bitumen
61
Q

Chemical Cell

A

More Reactive metal is cathode

Less reactive is anode

62
Q

Phenolphthalein

A

Neutral Colourless
Acid Colourless
Base Red

63
Q

Methy Orange

A

Neutral Orange
Acid Pink
Base Yellow

64
Q

Carbonate Test

A

Add Dilute Acid

CO2 produced which makes limewater cloudy

65
Q

Halides

A

Add nitric acid then silver nitrate.
Chloride- White ppt
Bromide- Cream ppt
Iodide- Yellow ppt

66
Q

Nitrate

A

Add aqueous Sodium Hydroxide then aluminium.

Ammonia is produced which turns red litmus paper blue

67
Q

Sulfate

A

Add nitric acid then add aqueous barium nitrate

White ppt is formed

68
Q

Sulfite

A

Add Dilute HCl, Warm gently.

SO2 produced which turns potassium manganate (VII) from purple to colourless

69
Q

Trend of Density, MP and BP and reactivity of water of Group 1 metals down the group

A

Density Increases
MP and BP decreases
Reactivity increases down the group

70
Q

Which metals react with cold water and form hydroxides

A

Group 1 Metals and calcium

71
Q

Decomposition of Group 1 Metal Nitrates

A

Sodium nitrite plus oxygen

72
Q

Thermal Decomposition of Calcium to Copper Nitrates

A

Metal Oxide plus Brown fumes of Nitrogen Dioxide plus Oxygen

73
Q

Thermal Decomposition of Carbonates

A

Difficult to decompose Group 1 metals
The less reactive the metal, the lower the temperature required.
Gold, Silver etc carbonates don’t exist

74
Q

Thermal Decomposition of Metal oxides

A

Usually very difficult to decompose these oxides.
Aluminium oxide requires thousands of degree
Silver oxide decomposition is possible

75
Q

Thermal Decomposition of Hydroxides

A

Group 1 metals don’t decompose
Calcium to Copper- Forms Oxide and Water
Metals below copper don’t form hydroxides

76
Q

Purification of Iron after Extraction

A

Oxygen and Powdered Calcium Oxide is added to the iron
Oxygen oxides the carbon, phosphorus,silicon and Sulfur to form oxides.
Silicon and Phosphorus oxides react with Powdered Calcium Oxide to form a slag. mainly Calcium silicate

77
Q

Recall Iron and Zinc Extraction

A

Chemistry 10 notes

78
Q

Uses and properties of Copper

A

Malleable, Good conductor of Electricity, Non-toxic and unreactive

Uses- Electrical Wires and Water Pipes

79
Q

Uses and properties of Aluminium

A

Strength and low density, resistance to corrosion

Uses - Food Containers, Manufacture of Aircraft

80
Q

Use of Mild steel

A

Car body panels and wires

81
Q

Stainless steel

A

Cutlery and sinks, chemical plants

82
Q

Uses of Zinc

A

Galvanising - Coating a metal like iron to protect it from corrosion
To make brass which is harder and corrosion resistant than copper

83
Q

Chlorination

A

Adding chlorine to the water supply to kill microorganisms

84
Q

Filtration

A

The process is used to remove large insoluble particles by passing the water through layers of sand and gravel filters that trap larger particles.

85
Q

Fractional Distillation of Oxygen and Nitrogen

A

-200C
Nitrogen collects at the top of the column (-190C)
Liquid O2 is then removed from the bottom of the column (-183)

86
Q

Rusting of Iron

A

Oxygen and Water must be present for rusting to occur.
Redox process that happens faster in salty water.
Iron+Water+Oxygen

87
Q

Manufacture of Ammonia

A 
Haber's Process
Hydrogen and Nitrogen to give Ammonia
Iron Beads as catalyst
450 degrees Celsius
200 atm
88
Q

Uses of Sulfur Dioxide

A

Bleach for paper and Food Preservative

89
Q

Manufacture of Sulfuric Acid

A

Recall and then check chemistry 12

90
Q

Oleum

A

H2S2O7

91
Q

Uses of Sulfuric Acid

A

Dilute- Catalyst and to clean metal surfaces

Concentrated- Car batteries, Acid Drain Cleaners, Phosphate fertilizers, soaps , detergents and paints dyes

92
Q

Properties of Sulfuric Acid

A

Powerful Dehydrating agent
Corrosive and Oxidising Agent
Strong dibasic acid

93
Q

Limestone Cycle

A 
Calcium Carbonate (Limestone) is heated to form Calcium Oxide (Quick Lime), which forms Calcium Hydroxide(Slaked Lime) when reacting with water then Calcium Hydroxide forms Limewater (Aqueous Calcium Hydroxide) when dissolved in water.
Finally Limewater becomes limestone when CO2 IS ADDED
94
Q

Uses of Limestone and it’s products

A

Used in the manufacture of iron and cement.
Used in blast furnace
Slaked Lime: Flue gas desulfurization
Used in treating acidic soils and acidic industrial waste

95
Q

Manufacture of Cement

A

Manufactured by heating a mixture of powdered limestone and clay in rotary,
then Calcium sulfate and water are added to produce cement
Forming a hardened interlocked structure of calcium aluminate and calcium silicate (which is cement)

96
Q

Formation of Ethanoic Acid

A

Oxidation:

1) by fermentation
2) with acidified potassium manganate

97
Q

Esterification

A

Carboxylic acid + Alcohol —> Ester + Water

Concentrated Sulfuric Acid Catalyst

98
Q

Nerve

A

A bundle of Neurones

99
Q

Adrenaline

A

Increases blood glucose concentration for increased respiration
Dilating pupils
Breathing rate increased.
Diverting blood flow towards muscles

100
Q

Homeostasis

A

Maintenance of a constant internal environment

101
Q

Type 1 diabetes

A

Condition where Insulin secreting cells in the pancreas are unable to produce Insulin

102
Q

Drug

A

any substance taken into the body that modifies or affects chemical reactions in the body

103
Q

Depressant drug

A

Slows down signals in the nerves and brain

Eg. ethanol and heroin

104
Q

Smoking Risks

A

Causes CHD, Chronic obstructive pulmonary disease and cancers such as lung cancer
Tar- Carcinogen
Nicotine- Addictive substance which narrows blood vessels
Carbon monoxide- reduces carrying capacity of Oxygen in blood

105
Q

Cu

A

Brown

106
Q

CuO

A

Black

107
Q

CuCO3

A

Green

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