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Chemistry IGCSE > Paper 1: downfalls of my knowledge > Flashcards

Paper 1: downfalls of my knowledge Flashcards

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1
Q

4.8 how does fractional distillation work?

A

Oil is heated in a fractionating column until it evaporates, it then condenses at different temperatures which separates the oil into different fractions which contain molecules with a similar number of carbon atoms.

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2
Q

4.9 what is the order of the different levels of the fractionating column?

A 
Refinery gases.
Gasoline/ petrol.
Kerosene. 
Diesel.
Fuel oil.
Bitumen.
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3
Q

4.12 what are the products of complete combustion?

A

Water and carbon dioxide.

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4
Q

4.15 what impurities are found in most fuels?

A

Most fuels contain sulphur impurities.

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5
Q

4.17 what is catalytic cracking?

A

The breakdown of long chain carbon compounds into small chain carbon compounds.

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6
Q

4.22 what is the reaction between halogens and alkanes under the presence of UV light?

A

Halogen + alkane -UV-> halogenoalkane + hydrogen halide

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7
Q

4.31 how can ethanol be oxidised?

A

By burning it in air, leaving it to react with air, or heating it in sulphuric acid in the presence of potassium dichromate.

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8
Q

4.34 what is the functional group of carboxylic acids

A

> COOH

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9
Q

4.35 what is the displayed formula of ethanoic acid?

A

H-C-O-H
ll
O

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10
Q

4.36 describe the reaction of carboxylic acids and metal?

A

Carboxylic acid + metal -> salt + hydrogen

It’s a slow reaction with lots of fizzing to form a colourless solution.

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11
Q

4.36 describe the reaction of carboxylic acids and metal carbonate?

A

Carboxylic acid + metal carbonate -> salt + carbon dioxide + water
It’s a slow reaction, lots of fizzing, to form a colourless solution.

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12
Q

4.37 what is an example of something which contains ethanol?

A

Vinegar.

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13
Q

4.38 what is the functional group of an ester?

A

> COO

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14
Q

4.39 what reaction forms an ester?

A

Ethanol + carboxylic acid —acid catalyst—> ester + water

…-O-H + H-O-… —> H-O-H + …

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15
Q

4.42 describe a use of an ester?

A

Esters are volatile and have distinct smells so are used in food flavourings and perfumes.

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16
Q

1.8 what is an element?

A

A substance made of one type of atom.

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17
Q

1.10 what is simple distillation used for?

A

It’s used to separate a pure liquid from a mixture of liquids by a proses of heating, evaporation, cooling, and condensing the pure substance.

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18
Q

1.10 what is crystallisation used for?

A

To separate a soluble salt from a solution.

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19
Q

1.11 how does a chromatogram provide information about the composition of a mixture?

A

Paper chromatography separates mixtures into individual compounds. The compounds have unique Rf values (distance traveled by ink/ distance traveled by solvent) which can be used to identify them.

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20
Q

1.16 what is the relative atomic mass?

A

An average value which takes into account the abundance of different isotopes of each element.

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21
Q

1.20 how do you differentiate between a metal and a nonmetal?

A

If an element is electrically conductive and a basic oxide, it is a metal.
If an element is not electrically conductive and a acidic base, it is a nonmetal.

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22
Q

1.27 what is a mol in grams?

A

The relative formula mass.

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23
Q

1.28 equation linking moles, mass, and Mr

A

Mass (g)

Mr (g mol^-1) | moles (mol)

24
Q

1.30 how do you calculate the percentage yield?

A

Percentage yield = amount of product formed / maximum amount of product possible x 100

25
Q

1.36 experimentally find the formula of magnesium oxide.

A

Weigh the magnesium.
Heat it in a crucible to form magnesium oxide.
Weigh the magnesium oxide.
Mass of oxygen = mass of magnesium oxide - mass of magnesium
Moles of magnesium = mass / Mr
Calculate the ratio.
Use the ratio to find the empirical formula.

26
Q

1.41 how are ionic compounds electrostatically bonded together?

A

The positive and negative ions. This force works in all directions forming giant lattices.

27
Q

1.43 do ionic compounds carry electric charges?

A

Only when molten.

28
Q

1.44 what is covalent bonding?

A

When an electron is shared in a non-metal compounds.

29
Q

1.45 what is electrostatically bonded in covalent compounds?

A

The negative pairs of electrons and positive nuclei.

30
Q

1.48 what is the link between the relative molecular mass and melting and boiling points?

A

Positive correlation.

31
Q

1.49 why do covalent compounds have high melting and boiling points?

A

All the atoms in these structures are linked to the other atoms by strong covalent bonds and big intermolecular bonds both of which need a lot of energy to overcome.

32
Q

2.9 what is the composition of air?

A

78% nitrogen
21% oxygen
0.9% argon
0.004% carbon dioxide

33
Q

2.10 what are two reactions you can use to find the percentage of oxygen in air?

A

Iron rusting.

Phosphorous is lit so water will rise in a bell jar.

34
Q

2.11 how does magnesium fire?

A

Bright white flame + a white ash

35
Q

2.11 how does sulphur flame?

A

Blue

36
Q

2.17 reactivity order

A 
Potassium.
Sodium.
Lithium.
Calcium.
Magnesium.
Aluminium.
Carbon.
Zinc.
Iron.
Hydrogen.
Copper.
Silver.
Gold.
37
Q

2.18 phenolphthalein?

A

Pink in alkaline and colourless in acidic.

38
Q

2.28 methyl orange?

A

Yellow in alkaline, pink in acidic.

39
Q

2.31 alkaline and acids source which ions?

A

Acids: H+
Alkalies: OH-

40
Q

2.34 predict solubility?

A

Sodium, potassium, ammonium, and nitrates are all soluble.
Chlorides are soluble except those of lead and silver.
Sulphates are soluble except those those of barium, lead, and calcium.
Carbonates and hydroxides are insoluble except those of sodium, potassium, and ammonium.

41
Q

2.35 proton transfer?

A

Acids are proton donors. Bases accept protons.

42
Q

2.38 what are examples of bases?

A

Metal oxides, metal hydroxides, and ammonia.

43
Q

2.38 what are alkalies?

A

Bases which are soluble in water.

44
Q

2.42 describe a acid and alkali titration.

A

Copper oxide: base.
Sulphuric acid: acid.
Add excess base to acid, filter it, dab to dry.

45
Q

2.44 what is a chemical test for ammonia?

A

Damp red litmus paper turns blue, or add it to some hydrogen chloride and a white smoke of ammonium chloride should appear.

46
Q

2.46 what colour is copper in a flame test?

A

Blue-green.

47
Q

2.46 what colour is calcium in a flame test?

A

Orange-red.

48
Q

2.46 what is a chemical test for ammonium?

A

Ammonium + sodium hydroxide -> ammonia

49
Q

2.46 what is a chemical test for copper?

A

Add sodium hydroxide, a blue precipitate will appear.

50
Q

2.46 what is a chemical test for iron (II)?

A

Add sodium hydroxide, a green precipitate should form.

51
Q

2.46 what is a chemical test for iron (III)?

A

Add sodium hydroxide, a brown participate should form.

52
Q

2.48 what is a chemical test for chloride ions?

A

Add dilute nitric acid, a white precipitate should form.

53
Q

2.48 what is a chemical test for bromide ions?

A

Add nitric acid, a cream precipitate should form.

54
Q

2.48 what is a chemical test for iodine ions?

A

Add nitric acid, a yellow precipitate should form.

55
Q

2.48 what is a chemical test for sulphate ions?

A

Add hydrochloric acid and then barium chloride solution and a white precipitate should form.

56
Q

2.48 what is a chemical test for carbonates?

A

Add dilute acid and carbon dioxide gas should be given off.

Chemistry IGCSE (1 decks)

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