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Final Chemistry Edexcel IGCSE - Hard Content > Hard Content > Flashcards

Hard Content Flashcards

1
Q

What is an exothermic reaction?

A

One that gives off heat energy into the surrounding

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2
Q

What is an endothermic reaction?

A

One that takes in heat energy from the surroundings

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3
Q

What is the enthalpy change?

A

the overall energy change in a reaction?

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4
Q

What is the enthalpy change in an exothermic reaction?

A

negative because energy is given out

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5
Q

What is the enthalpy change in an endothermic reaction?

A

positive because energy is taken in

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6
Q

How can you calculate heat energy transferred?

A

mass of liquid being heated x shc x change in temp

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7
Q

how do you calculate molar enthalpy change?

A

molar enthalpy change = -energy transferred / moles

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8
Q

Why is bond breaking endothermic?

A

the energy used to break the bonds is greater that the energy released forming them

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9
Q

Why is making bonds exothermic?

A

the energy released making the bonds is greater than the energy used to make them

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10
Q

how can you calculate bond energies?

A

total energy absorbed to break bonds - total energy released to make bonds

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11
Q

what are two examples of reversible reactions?

A

copper sulfate + water -> hydrated copper sulfate

ammonia + hydrogen chloride -> ammonium chloride

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12
Q

what is equilibrium

A

the state of a chemical reaction in which the forward and reverse reactions are occurring at the same rate, but the concentrations of the reactants and products remain the same

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13
Q

If the equilibrium lies to the left?

A

mainly reactants, little products

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14
Q

if the equilibrium lies to the right?

A

mainly products, little reactants

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15
Q

reactant concentration is increased:

A

reaction forming products is favoured and equilibrium shifts

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16
Q

product concentration is favoured:

A

reaction forming reactants favoured and equilibrium shifts

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17
Q

temperature of reaction is increased (equilibrium):

A

endothermic reaction will be favoured

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18
Q

temperature of reaction is decreased (equilibrium):

A

exothermic reaction will be favoured

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19
Q

pressure of reaction is increased (equilibrium):

A

side of reaction with fewer gas moles favoured

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20
Q

pressure of reaction is decreased (equilibrium):

A

side of reaction with more gas moles faovured

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21
Q

what is ionic bonding?

A

the strong electrostatic attraction between positive an negative ions (metal and non metal)

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22
Q

When an ionic compound is formed….

A

electrons are transferred from a metal to the non metal to form positive and negative ions

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23
Q

carbonate:

A

Co3 2-

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24
Q

nitrate:

A

NO3 -

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25
Q

ammonium:

A

NH4 +

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26
Q

hydroxide:

A

OH-

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27
Q

sulphate:

A

SO4 2-

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28
Q

what is the boiling and melting point of ionic compounds and why?

A

high, giant ionic lattice, strong ionic bonding, lots of energy to overcome

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29
Q

do ionic compounds conduct electricity?

A

Yes molten or dissolved as there are mobile delocalised electrons, no as a solid.

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30
Q

why are ionic compounds brittle

A

when a lattice layer is hit, a layer of ions is shifted so that ions with the same charge are lined up together and they then repel eachother

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31
Q

what are covalent bonds?

A

the strong electrostatic connection between nuclei and a shared pair of electrons

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32
Q

what is the boiling point of simple covalent molecules?

A

low because they have strong covalent bonds but weak IMF which require little energy to overcome

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33
Q

do simple covalent structures conduct electricity?

A

no because the molecules are neutral and carry no charge

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34
Q

what is the boiling point of giant covalent substances?

A

high, giant covalent lattice, strong covalent bonds, lots of energy to break

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35
Q

what is the conductivity of graphite?

A

can conduct as it has mobile delocalised electrons

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36
Q

how can you calculate percentage yield?

A

(actual/calculated) x 100

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37
Q

what are three possible reasons for percentage yield being less than 100%

A
  1. reaction may be reversible
  2. side reactions may have occured
  3. products may be lost (i.e., time taken putting on bung)
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38
Q

what equation links gas moles, moles and volume?

A

moles = volume/24 dm3

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39
Q

what equation links moles, volume and concentration?

A

moles = conc x vol

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40
Q

electrode:

A

terminal at which electricity enters of leaves the electrode

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41
Q

anion:

A

a negatively charged particle

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42
Q

cation:

A

positively charged particle

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43
Q

cathode:

A

the negative electrode

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44
Q

anode:

A

positively charged electrode

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45
Q

electrolysis:

A

the splitting up of an ionic compound to form two new products using electricity

46
Q

what occurs at the cathode?

A

attracts cations, reduction occurs, metal is formed

47
Q

what occurs at the anode?

A

attracts negative anions, oxidation occurs, a non metal covalent molecule is formed

48
Q

what three substances can beat H+ at the cathode?

A

copper, silver, gold

49
Q

what three substances can beat OH- at the anode?

A

bromine, iodine, chlorine

50
Q

list the reactivity series

A

potassium, sodium, lithium, calcium, magnesium, aluminium, carbon, zinc, iron, hydrogen, copper, silver, gold

51
Q

how are metals above carbon extracted from their ore?

A

electrolysis

52
Q

how are metals below carbon extracted from their ore?

A

displacement with carbon

53
Q

4 uses of copper:

A

unreactive - piped, conducts electricity - wires, heat conductor - pans, antibacterial - hospital surfaces

54
Q

2 uses of aluminium:

A

low density - aircrafts, aluminium oxide layer makes it unreactive - pans

55
Q

one use of low carbon steel:

A

strong and malleable - bridges (can rust)

56
Q

one use of high carbon steel:

A

very strong - cutting tools

57
Q

one use of stainless steel:

A

corrosion resistant - cutlery and kitchen sinks

58
Q

colour change of methyl orange:

A

acid - red, base - yellow

59
Q

colour change of phenolphthalein:

A

acid - colourless, base - pink

60
Q

colour change of red litmus

A

acid - red, base - blue

61
Q

colour change of blue litmus

A

acid - red, base - blue

62
Q

acid + metal ->

A

salt + hydrogen

63
Q

acid + metal oxide ->

A

salt + water

64
Q

acid + metal carbonate ->

A

salt + water + carbon dioxide

65
Q

what is the SNAP rule?

A

sodium, nitrate, aluminium and potassium salts are soluble

66
Q

what is the INCH rule?

A

insoluble carbonates and hydroxides except for snap salts

67
Q

What is the ClasPbAg rule?

A

Chlorides are soluble except lead and silver

68
Q

what is the SoSuBaCa rule?

A

soluble sulphates except for barium and calcium

69
Q

What does a precipitation reaction make?

A

sol + sol -> insol + sol

70
Q

What are the 6 steps to making a soluble salt from solid metal/excess base method?

A
  1. combine excess metal with acid
  2. add until bubbling stops/excess remains
  3. filter out metal
  4. boil off half to make saturated solution
  5. allow rest to evaporate
  6. filter excess liquid, dab crystals, leave on windowsill
71
Q

What are the five steps to making an insoluble salt?

A
  1. dissolve soluble salts in water
  2. combine two salt solutions
  3. filter, keep precipitate and discard solution
  4. wash precipitate
  5. allow to dry on windowsill
72
Q

lithium flame test:

A

red

73
Q

sodium flame test:

A

yellow

74
Q

potassium flame test:

A

lilac

75
Q

calcium flame test:

A

orange/red

76
Q

copper(II):

A

blue/green

77
Q

what is the test for cations?

A

add sodium hydroxide

78
Q

copper test for cations:

A

light blue precipitate

79
Q

iron (II) test for cations:

A

dark green precipitate

80
Q

iron (III) test for cations:

A

dark orange precipitate

81
Q

test for ammonium gas:

A

damp red litmus -> blue

82
Q

testing for carbonates:

A

add dilute HCl and it will produce Co2

83
Q

testing for sulphates:

A

add HCl then Barium Chloride (white precipitate)

84
Q

testing for halides

A

nitric acid, then silver nitrate - Cl=white Br=cream I=yellow

85
Q

test for chlorine

A

bleaches damp litmus

86
Q

general formula for alkanes:

A

CnH2n+2

87
Q

full name of alkane with two carbons:

A

ethane

88
Q

root of names of hydrocarbons (1-6)

A

eth, meth, prop, but, pent, hex

89
Q

structural isomers:

A

same molecular formula but different displayed formula

90
Q

alkane + bromine ->

A

bromo(alkane) + hydrogen bromide

91
Q

what is required for a bromine and alkane to react?

A

UV light

92
Q

describe the production of crude oil:

A

remains of marine plants and animals sink t bottom of ocean millions of years ago. they became buried preventing them from rotting. gradually became sedimentary rock, heat and pressure then built up causing them to become crude oil and natural gas

93
Q

from bottom to top, what are the fractions of fractional distillation?

A

bitumen, fuel oil, diesel, kerosene, gasoline, refinery gas

94
Q

what are the 3 steps to crude oil fractional distillation?

A
  1. crude oil is heated and vapourised
  2. vapour is pumped into column
  3. fractions condense at height where temp in column is lower than BP
95
Q

general formula of alkenes:

A

CnH2n

96
Q

are alkenes saturated or unsaturated

A

unsaturated

97
Q

what is the name of the alkene with 3 carbon atoms?

A

propene

98
Q

what is the colour change of alkenes + bromine?

A

orange -> colourless

99
Q

what is the reaction between alkenes and bromine called?

A

addition

100
Q

ethene + bromine ->

A

dibromomethane

101
Q

what is cracking?

A

the breaking down of long chain alkanes that are in surplus to high demand smaller chain alkanes

102
Q

what are two requirements for cracking?

A

600-700 degrees and aluminium oxide catalyst

103
Q

what is the general formula of alcohols?

A

CnH2n+1OH

104
Q

what does the oxidation reaction of ethanol require and produce?

A

acebacters, ethanoic acid

105
Q

what is the general formula of carboxylic acids?

A

CnH2nO2

106
Q

What is the functional group fo carboxylic acids?

A

C = O
\
O - H

107
Q

Carboxylic Acid + metal ->

A

salt + hydrogen

108
Q

Carboxylic Acid + metal carbonate ->

A

salt + water + carbon dioxide

109
Q

Carboxylic Acid + alcohol ->

A

ester + water

110
Q

how do you name an ester?

A

alcohol becomes first part (-yl), the Carboxylic Acid becomes the second bit (-anoate)

111
Q

How do you prepare a sample of an ester?

A

sulphuric acid + ethanol + ethnic acid in hot water bath with tube covered in cling film, leave for ten minutes. pour contents into sodium carbonate, ester will be visible as oily droplets

Final Chemistry Edexcel IGCSE - Hard Content (1 decks)

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