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Edexcel GCSE Chemistry Higher > Topic 9 - Separate Chemistry 2 > Flashcards

Topic 9 - Separate Chemistry 2 Flashcards

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1
Q

Nano

A

1 billionth

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2
Q

1 nanometer

A

1 x 10^-9 meters (.000000001m)

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3
Q

size of a pinhead

A

1 million nanometers

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4
Q

Applications (Glass)

A

On GLASS: Titanium oxide nanoparticles trigger a chemical reaction that breaks down dirt when the sun shines on it and when it rains the water lands on the glass and washes off the broken down dirt.

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5
Q

Applications (Cosmetic Industry)

A

Nanoparticles absorb deeper into the skin.

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6
Q

Application (Cancer fighting drugs)

A

Gold Nanocages carry the drugs to the tumour. They are strong yet light.

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7
Q

Risks of nanoparticles

A

More and more Nanoparticles in the ATMOSPHERE.

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8
Q

What is a functional group?

A

A group of atoms in a molecule that determines how that molecule’s chemical properties

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9
Q

State the functional group of alkanes

A

(C-C)

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10
Q

State the fucntional group of alkenes

A

(C=C)

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11
Q

What is are isomers? (2)

A

Molecules with the same molecular formula but different arrangements of atoms

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12
Q

Draw Ethane, Ethene, Ethanoic acid, Ethanol, Ethyl Ethanoate and both the repeating unit and section of poly(ethene)

A

Check image

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13
Q

Why can’t but-3-ene exist?

A

but-3-ene is just but-1-ene with the functional group on the other end of the molecule (isomers are numbered starting from the end closest to the functional group)

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14
Q

What are the products of the complete combustion of hydrocarbons?

A

Carbon dioxide and water

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15
Q

What defines complete combustion?

A

The full oxidisation of every atom in the hydrocarbon

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16
Q

What products can also be produced in the incomplete combustion of hydrocarbons?

A

Carbon monoxide (toxic) and soot/carbon (orange flame test)

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17
Q

What does bromine water test for?

A

unsaturated molecules

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18
Q

What happens in the bromine water test?

A

the bromine water decolourises from orange-brown to clear as the bromine undergoes an addition reaction with the unsaturated molecule forming a colourless product and removing bromine from the solutin

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19
Q

What product is formed when ethene reacts with bromine?

A

1,2-dibromoethane (1,2 means that there are TWO bromine atoms are attached to ONE carbon atom EACH)

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20
Q

Define an addition reacyion

A

A reaction where reactants combine to form one larger product molecule and no other products

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21
Q

Describe the fermentation process to produce alcohol (5)

A

Crush plant material to form a sugar solution. Add sugar solution (eg glucose) to a jar with yeast. Place airlock on jar to create an anaerobic environment but allow carbon dioxide to escape. Keep jar at 35 degrees and control pH to maintain optimums for yeast. This produces alcohol with a concentration of up to 15%

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22
Q

Describe the fractional distillation of ethanol (4)

A

The ethanol solution is heated. The heated liquid evaporates and their vapours cool as they rise up a fractionating column. As ethanol has a lower boiling point than water (78 degrees), it remains a gas for longer, and so separates from the water. This separated solution then condenses and is collected

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23
Q

State the general formula of alchols

A

CnH2n+1OH

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24
Q

State the functional group of alcohols

A

OH

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25
Q

Describe the chemical properties of alcohols (3):

A

Produce carbon dioxide and water on complete combustion. Can be oxidised to from carboxylic acids in the presence of oxidising agents such as hot copper oxide. React with reactive metals such as sodium, forming hydrogen gas as one of the products

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26
Q

How does chain length affect alcohol reactivity with sodium?

A

The shorter the chain length, the more reactive

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27
Q

State 5 uses of alcohols:

A

Solvents, Cosmetics, Recreation, Varnishes, Bio-methanol and bio-ethanol are renewable fuels

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28
Q

State the functional group of carboxylic acids:

A

-COOH

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29
Q

State the general formula of carboxylic acids

A

CnH2n+1COOH (where n is number of carbons - 1) OR CnH2nO2

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30
Q

What is the relationship between carbon chain length and acidity in carboxylic acids?

A

The shorter the chain length, the more acidic

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31
Q

What is the pH range of carboxylic acid solutions?

A

3-6

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32
Q

Describe four carboxylic acid reactions:

A
  1. CA + metal —> salt + hydrogen. 2. CA + base —> salt + water. 3. CA + carbonates —> salt + water + carbon dioxide. 4. CA + oxide —> salt + water
33
Q

What happens to a carboxylic acid in solution?

A

The COOH group forms a H+ ion while the rest of the molecule forms the negative ion (salt). This is because hydrogen is less reactive than the metal.

34
Q

Naming salts

A

Metal + acid prefix + -anoate (eg, ethanoic acid + lithium —> lithium ethanoate + hydrogen)

35
Q

Carboxylic acids are weak acids. What does this mean?

A

Weak acids are acids which do not fully dissociate in solution to form the max number of H+ ions

36
Q

What is a polymer?

A

A large molecule made from lots of repeating monomers joined togetehr

37
Q

Why can’t polymers be given specific relative molecular masses?

A

They can be different lengths, and so contain differing numbers of atoms

38
Q

What determines a polymer’s properties?

A

The monomer it is made from

39
Q

State three polymers, their monomers and whether they are natural or not:

A
  1. Protein - amino acid - natural. 2. Plastics - it depends - synthetic. 3. DNA - nucleotides - natural
40
Q

Define addition polymerisation

A

A reaction in which monomers join together to form only one product: a polymer.

41
Q

Describe the addition polymerisation of ethene and how you would draw it (2)

A

One of the bonds in the double bond in ethene breaks open and another ethene molecule joins on. This process repeats with many monomers

42
Q

State the properties and uses of poly(ethene)

A

Flexible (cling film) cheap (plastic bags) good insulator (poly tunnels)

43
Q

State the properties and uses of poly(propene)

A

Flexible(ropes) can be spun into fibres(carpet) Shatterproof(buckets)

44
Q

State the properties and uses of poly(chloroethene)

A

Tough(windows) can be hard(gutters) good insulator(wiring insulation)

45
Q

State the properties and uses of poly(tetrafluoroethene)

A

slippery(non-stick utensils and pans), water resistant(coatings on clothes)

46
Q

State 5 problems with synthetic polymers:

A

Most are not biodegradable(cannot be broken down by microbes). Most cannot be recycled, so go to landfill. All produce carbon dioxide (greenhouse gas) and some produce toxic substances when burnt. Most are made from crude oil. Wildlife can get tangled in/ingest them

47
Q

State 2 advantages of synthetic polymers:

A

Not biodegradable, so last long. Some can be recycled

48
Q

Describe the steps to recycle a polymer (6)

A

Collect waste. Sort waste by hand into different types. Dispose of non-recyclables in landfill. Clean polymers and grind into chippings. Purify chippings. Melt chippings and process into new products

49
Q

What is condensation polymerisation?

A

A process in which monomers join together to form a polymer and eliminate a small molecule, such as water

50
Q

What are plastic bottles made from and why?

A

PET (a polyester) because it is strong, light, shatterproof and recyclable

51
Q

State the functional group of esters:

A

-COO-

52
Q

How are esters formed?

A

By a condensation reaction when a carboxylic acid reacts with an alcohol in the presence of a catalyst. Carboxylic acid + alcohol —> ester + water

53
Q

What molecules do you need to form polyesters?

A

Diols and dicarboxylic acids so an ester link can form on both sides of the ester

54
Q

Describe what happens in condensation polymerisation (2)

A

The oxygen and hydrogen from the carboxylic acid COOH group and hydrogen from the alcohol OH group join to make H2O. The remaining carbon and oxygen from the carboxylic acid COOH group and oxygen from the alcohol OH group join together to form an ester link, pulling the carboxylic acid and alcohol together to form an ester

55
Q

How do you name esters?

A

Start with the name of the alcohol, change the ending from -anol to -yl and add the name of the carboxylic acid with -anoate instead of -anoic Example: ethanol and ethanoic acid gives ethyl ethanoate

56
Q

Name two types of condensation polymer:

A

Polyesters and Polyamides

57
Q

State the balanced equation for the fermentation of glucose to produce ethanol

A

C6H12O6 —> 2C2H5OH + 2CO2

58
Q

what is feedstock?

A

A raw material used to provide reactants for an industrial reaction.

59
Q

Flame test process

A

Dip nichrome wire loop in HCl, then distilled water, then into the metal compound. Hold metal compound in flame and note the colour

60
Q

Lithium flame colour

A

Crimson/red

61
Q

Sodium flame colour

A

Yellow

62
Q

Potassium flame colour

A

Lilac

63
Q

Calcium flame colour

A

Orange-red

64
Q

Copper flame colour

A

Green-blue

65
Q

Metal hydroxide test

A

Add an excess of sodium hydroxide to each metal compound.

66
Q

Aluminium, metal hydroxide test

A

White precipitate formed, dissolves to colourless in excess NaOH

67
Q

Calcium, metal hydroxide test

A

White precipitate formed

68
Q

Copper, metal hydroxide test

A

Blue precipitate formed

69
Q

Iron (II), metal hydroxide test

A

Green precipitate formed

70
Q

Iron (III), metal hydroxide test

A

Brown precipitate formed

71
Q

Test for halide ions

A

Add dilute nitric acid followed by silver nitrate solution

72
Q

Chloride test result

A

White precipitate formed

73
Q

Bromide test result

A

Cream precipitate formed

74
Q

Iodide test result

A

Yellow precipitate formed

75
Q

Test for carbonates

A

Add dilute HCl, if a carbonate is present then there will be fizzing.

76
Q

Why does the carbonate test fizz if positive?

A

If a carbonate is present then it will react with the acid and produce CO2.

77
Q

Test for sulphate ions

A

add dilute hydrochloric acid followed by barium chloride solution

78
Q

Positive sulphate test result

A

White precipitate formed

Edexcel GCSE Chemistry Higher (12 decks)

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