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Gcse What You Got Wrong Flashcards

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1
Q

Why are compounds always pure

A

Because they are always within a fixed ratio of atoms

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2
Q

What is an element

A

A substance that consists of only one type of atom
That can not be broken down any simpler by chemical means

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3
Q

Describe the arrangement of gases

A

A= random and widely spread out
M= move randomly in all directions and freely
P= rarely in contract with each other

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4
Q

As the temperature increases, what happens to the solubility of a gas

A

It decreases

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5
Q

In, the experiment for measuring solubility, state the word equation for the calculation at the end

A

Mass of crystals dissolved= (mass of crystals + basin) - (mass of basin)

Mass of water that evaporated (that the solvent was orignal dissolved in )= (mass of basin + solution )- (mass of basin + crystals)

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6
Q

Explain how the diffusion of potassium permanganate (iv) happens in water

A

Particles move from a high concentration to a low concentration
This is because there are gaps in the liquid and particles in a liquid are able to Slide Over each other
Therefore they can easily mix together

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7
Q

Explain why as temperature increases, solubility of a solid also increase

A

Because the solvent molecules have more kinetic energy
This means that they can more efficiently break apart solute molecules held together by intermolecular forces of attraction

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8
Q

Describe the structure of ionic substances, giant covalent substances, and metallic substances

A

Ionic:
-giant ionic lattice
-ions are regularly arranged
-and positive and negative ions repeat in a pattern

Giant covalent:
-giant lattice structure
-number of atoms is invariable
- so repeats on in 3D

Metallic
-giant metallic lattice
- held together by electrostatic attraction between positive ions and sea of delocalized

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9
Q

In the electrolysis of aluminum oxide, what deposits at the bottom

A

Molten aluminum

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10
Q

Why is diamond hard

A

Because of the rigid tetrahedral structure

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11
Q

How can you measure the initial volume of air, when measuring percentage of oxygen in the air using iron

A

Fill the connecting tube and the flask with water and then measure this out in a measuring cylinder

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12
Q

Explain how the phosphorus experiment works when measuring the percentage of oxygen in the air

A

-phosphorus is placed on an evaporating dish, on top of a trough of water in a bell jar
- it reacts with the oxygen in the air to form phosphorous oxide, a white smoke, which dissolves in the water
-this makes the water levels rise, and so you can measure the water levels before, and then the water levels after

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13
Q

What is the word equation for the thermal decomposition of metal carbonates

A

Metal carbonate—-) metal oxide + carbon dioxide

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14
Q

Give 5 word equationexamples of how carbon dioxide can be produced

A

Copper carbonate —-) copper oxide + carbon dioxide (thermal decomposition)
Calcium carbonate —-) calcium oxide + carbon dioxide (thermal decomposition)
Calcium carbonate + hydrochloric acid ——) calcium chloride + carbon dioxide + water
Carbon + oxygen —-) carbon dioxide
Petrol + oxygen —-) carbon dioxide + water

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15
Q

Give the balanced symbol equation for the reaction between calcium carbonate and hydrochloric acid

A

CaCO3(s) + HCL(aq) -—-) CaCl2 (aq) + CO2(g) + H2O(l)

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16
Q

Give the balanced symbol equation, using petrol to make carbon dioxide

A

2CH8H18 + 2O2 ——) 16CO2 + 18H2O

(This is the complete combustion of fuels, which always make carbon dioxide and water)

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17
Q

Describe an experiment to measur oxygen in the air, using iron WOOL

A

Soak iron wool on acetic acid to catalyse the reaction
Push into a measuring cylinder and then invert inside trough of water
Measure initial volume of air
As iron reacts with oxygen, the water level will rise to replace the space taken up by oxygen
Measure the final volume of oxygen

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18
Q

Give the equation to test that carbon dioxide has been given off

A

Bubbled in lime water to produce a white précipite of calcium carbonate
Ca(OH)2 + CO2 ——-) CaCO3 + H2O

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19
Q

When you keep bubbling carbon dioxide in a solution of calcium carbonate and water, give the balanced symbol equation of what happens and the colour change

A

CaCO3 + H2O + CO2 ——) Ca(HCO3)2(aq)
Colourless

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20
Q

State three substances that can be used to show combustion reactions, and give the flame colours produced aswell

A

Magnesium —-) white flame
Sulfur —-) dark blue flame
Hydrogen—-) pale blue flame

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21
Q

State the balanced symbol equation when magnesium oxide reacts with water, and when sulfur dioxide reacts with water

A

MgO+ H2O —-) Mg(OH)
SO2 + H2O —-) H2SO3 (SULFUROUS ACID)

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22
Q

Metal oxides are… in water
Non metal oxides are…. In water

A

Insoluble
Soluble

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23
Q

Describe the reaction between calcium and water

A

Slow reaction
Bubble form
White insoluble calcium hydroxide forms
In a colorless solution

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24
Q

Describe the reaction with magnesium with water and or steam

A

Does not react with water, because insoluble magnesium hydroxide layer is formed
Reacts with steam, to form magnesium oxide, which burns with a bright white flame. Also produces hydrogen

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25
Q

General word equation for metal and steam

A

Metal + steam —) metal oxide + hydrogen

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26
Q

Describe what happens to zinc in steam, and then iron in steam, with the colours

A

Zinc oxide formed, which is yellow upon heating but white upon cooling
Iron tetroxide formed, which is a darker grey

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27
Q

Describe the reaction between aluminum and hot and cold acid

A

Cold acid:
Reacts slowly and then vigorously,
Forms a layer of aluminum oxide, so the reaction stops

Hot acid: aluminum oxide layer is formed so reacts more vigorously

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28
Q

Describe the reactions of magnesium, zinc, and iron in hydrochloric acid

A

Magnesium:
- vigorous reaction
- rapid fizzing
-becomes hot
-colourless solution

Zinc:
-steady reaction
-steady fizzing
-becomes warm
- colourless solution

Iron:
-slow reaction
- fizzing
-slightly warm
- pale green solution

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29
Q

When iron reacts with hydrochloric acid, what colour is formed

A

Green pale solution

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30
Q

What two types of displacement reactions can you use to determine the reactivity of metals,
And then for each type state what will happen to the more reactive metal and then the less reactive metal.

A

-Metals with metal oxides, upon heating
-Metals with aqueous solutions of metal salt.

With metal oxides, more reactive metal is oxidized (as it binds more strongly to oxygen,
and less reactive metal is reduced

With aqueous solutions of metal salts, more reactive metal dissolves as it forms a solution
Less reactive metal coats the surface of the more reactive metal

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31
Q

Oxidizing agent defintion

A

Substance that oxidizes something else
So is reduced

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32
Q

What does the reactivity of metals depend upon

A

Their ability to from positive ions and lose electrons

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33
Q

Give the symbol way of writing hydrated iron (iii) oxide

A

Fe2O3.xH2O

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34
Q

Balanced symbol equation for the process of rust

A

4Fe + 3O2 + H2O —-) 2Fe2O3.XH2O

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35
Q

Galvanizing utilisés which two methods

A

Sacrificial protection
And the barrier method

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36
Q

percentage of argon in the air

A

0.9%

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37
Q

give the colours of the flames produced with the combustion reactions of sulphur, magnesium, hydrogen

A

sulfur, blue
magnesium, bright white
hydrogen, pale blue

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38
Q

give the thermal decomposition word equation reaction for a metal carbonate

A

metal oxide + carbon dioxide

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39
Q

give the word equation for the reaction between metal carbonate and acid

A

salt + carbon dioxide + water

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40
Q

give three ways that carbon dioxide can be produced

A

thermal decomposition of metal carbonates.
metal carbonate and acid, (react to form co2, salt, water)
combustion of fossil fuels

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41
Q

thermal decomposition of calcium carbonate has occurred. it is bubbled through lime water. what colour will it turn and what is produced

A

white precipitate,
because the decomposition results in the formation of carbon dioxide, when this bubbles in calcium hydroxide, it forms calcium carbonate and water

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42
Q

state the word equation for carbon dioxide is continuously bubbled through calcium hydroxide for a long time

A

calcium carbonate + carbon dioxide + water—— calcium hydrogen carbonate

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43
Q

reaction between,
metal + water
metal oxide + water
metal + steam

A

metal hydroxide + hydrogen
metal hydroxide
metal oxide + hydrogen

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44
Q

give descriptions of the reaction between,
magnesium +hcl
zinc + hcl
iron +hcl

A

vigorous,hot test tube, colourless
rapid reaction, warm test tube, colourless
slow reaction,slightyl warm, pale blue

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45
Q

what are two types of displacement reactions that can occur

A

combustion of metal oxide
reaction of metals with aqueous metal salt solutions

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46
Q

what is an ore

A

a rock that contains enough of the metal to extract it

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47
Q

what is a mineral

A

element or compound that occurs naturally

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48
Q

what is the relationship between steel and iron

A

steels are alloys of iron, mixed with different amounts of carbon

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49
Q

properties and uses of copper

A

unreactive
conducts electricity
malleable

pots and pans
electrical wires
water pipes

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50
Q

properties and uses of aluminium

A

resists corrosion
conducts electricity
low density

pots and pans
electric wires
car bodies

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51
Q

properties and uses of mild carbon steel

A

corrodes easily,
malleable
nails
carbodies

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52
Q

properties and uses of high carbon steel

A

brittle and hard,
cutting tools,
bridges

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53
Q

properties and uses of stainless steel

A

resists corrosion
strong
cutlery
sinks

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54
Q

stainless steel is an alloy of what

A

carbon and nickel

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55
Q

what is an alloy. then explain why alloys are harder than pure metals

A

alloys are mixtures of a metal with one or more other elements.
hard because has different sized atoms
which disrupts the regular lattice structure
so harder for the layers of ions to slide over each other

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56
Q

what colour does phenolphthalein and methyl orange turn in acid, and alkali solutions

A

phenolpthalein;
acid-colourless
alkali-pink
methyl;
acid-red
alkali; yellow

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57
Q

give 5 things to do in a titration to ensure accuracy
and give the value for results to be concordant

A

-use a white tile underneath
-swirl the solution to mix
-use water to rinse the flask at the end
-use a pipette with a pipette filler for an accurate reading
-always measure burette reading from bottom of the meniscus

concordant results are 0.2 + or_

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58
Q

an acid base reaction occurs and effervescence occurs. explain what type the base used was

A

base was a metal carbonate
bc when metal carbonate reacts with acids, co2 is given off which produces effervescence

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59
Q

Give four example of bases

A

Metal Carbonates
Metal oxides
Metal Hydroxides
Ammonia in solution

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60
Q

An acid is a proton..A bass is a proton…

A

Donor
Acceptor

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61
Q

Why must a titration be used to make a soluble salt of potassium sodium or ammonium

A

Because they are soluble in water, so it would not be known when the reaction is finished, and so exactly how much acid to add

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62
Q

What is the flame test colour for calcium

A

Orange

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63
Q

Describe how to carry out a precipation reaction for cations, and then give the observations made for each cation

A

Dissolve the salt in distilled water to form a solution (needs to be a solution for it to occur)
Add dilute sodium hydroxide
Observe the precipitate
Copper 2+—) blue
Ammonium ions, in cold—-) a smell. Ammonia in hot—-) red litmus turns blue
Iron 2+——) green
Iron 3+—-) brown

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64
Q

Describe what will happen to the colour of the precipitate if left out for a while, in the precipitation reaction of iron 2+

A

The iron (ii)hydroxide formed from the reaction will react with oxygen in the air to form iron (iii) hydroxide

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65
Q

Give the test for chlorine gas

A

1)take DAMP blue litmus paper and place in solution
2)will first turn red as chlorine dissolves in water to form an acidic soltuion
3)but will then turn it white because it beaches the paper

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66
Q

Give the test for carbonates

A

-add hydrochloric acid to the salt solution
-if fizzing is given off, this means a gas is produced
-and so test that the gas is carbon dioxide by bubbling it through limewater, to turn milky

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67
Q

Give the test for sulfates

A

-add hydrochloric acid to a solution of barium chloride (added to get rid of any carbonate or sulfite ions which could also form a précipitate)
-add this solution to the salt solution which is dissolved in distilled water
-a white precipitate of barium sulfate will form

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68
Q

Give the test for halides and the different observations

A

-add nitric acid to a solution of silver nitrate (the acid is added to get rid of any traces of other anions such as carbonates of sulfates
-add this solution to the solution of the halide dissolved in distilled water
-for chlorides, a white precipitate will form
-for bromides, a cream precipitate will form
-for iodides, a yellow precipitate will for,

69
Q

Give the formula for hydrated copper sulfate

A

CuSO4.5H2O

70
Q

Give the test for ammonium ions

A

Add sodium hydroxide to the solution
A pungent gas of ammonia will be given off
Test the GAS with DAMP red litmus, should turn blue

71
Q

Volatility…. As chain length increases (for hydrocarbons) and explain why
Melting + boiling….. as chain length increases (for hydrocarbons) explain why

A

Decreases, because longer chain length means greater atomic mass, and so stronger attraction between other molecules, so less able to evaporate

Increases, because longer chain length so greater atomic mass, so greater intermolecular forces of attraction, so more energy required to break apart

72
Q

When nitrogen oxide reacts with rain water what forms
When nitrogen oxide react with rain water and more oxygen what forms
Give the chemical formula for each

A

Nitric acid (HNO3)and nitrous acid(HNO2)
Nitric acid (HNO3)

73
Q

Give the word equation for the hydration of ethene

A

Ethene + steam —-) ethanol

74
Q

Give three word equations that involve the oxidation of ethanol

A

Combustion : ethanol + oxygen —-) carbon dioxide + water
Aerobic oxidation: ethanol + oxygen. —-) ethanoic acid. + water
Oxidizing agent: ethanol + potassium dichromate (IV) in dilute sulfuric acid. —-) ethanoic acid. + water

75
Q

Give two advantages and two advantages of using fermentation over hydration of ethene to produce ethanol

A

Adv: renewable, uses less energy
Dis: slower process, less efficient bc batch process

76
Q

Why is fermentation to produce ethanol done in an absence of air

A

Because of air got in it would oxidize the ethanol and produce ethanoic acid

77
Q

What is vinegar

A

An aqeous solution of ethanoic acid

78
Q

Write the formula for ethyl ethanoate

A

CH3COOCH2CH3

79
Q

When preparing an ester using distillation, why does the ester evaporate the quickest

A

Because it is volatile, so has a low boiling point

80
Q

Give the word equation to make an ester and then explain a basic method to do so

A

Alcohol + carboxylic acid —-) ester + water
1) add alcohol and Carboxylic acid to a beaker, with sulfuric acid
2)heat in a water bath
3) add sodium carbonate to remove acidic impurities
4)add calcium chloride to remove alcoholic impurities
5)the alcohol and acid will dissolve and the ester will float on top and you’ll be able to waft the smell

81
Q

Draw the monomer for poly(tetrafluroethene)

A

Two carbon atoms in the centre joined by a double bond, each attached to a single fluorine

82
Q

What is a polymer

A

A large molecule made by joining many smaller molecules together (monomers)

83
Q

Describe three conditions to occur for addition polymérisation to occur

A

-must be an alkene
-must use heat and Hugh pressures
-must use an initiator, not a catalyst

84
Q

Give two advantages and three disadvantges of landfill
Give two advantges and two disadvantges of incineration
(In terms of disposing of addition polymers)

A

Adv land; cheap, doesn’t produce green houe gases
Disad landfill: smells, unpleasant appearance, takes up space
Adv inciner:fuel can be used to heat home, dosent take up space
Disad inciner: produces green house gases, ashes still need to be disposed of

85
Q

Why are addition polymers non biodegradable

A

Because they have c-c bonds which makes them unreactive, and so they can not be broken down by other substances

86
Q

What is a polyester.
How is an ester link formed

A

Polyester is a type of condensation polymer formed when many ester links join together.
An ester link forms when the dicarboxylic acid functional group reacts the diol functional group, and a water molecule is lost in the process

87
Q

Give two conditions for condensation polymerization to occur

A

-two different functional groups must be present
-each monomer must have atleast two functional groups attached to it

88
Q

Give the word equation for condensation polymérisation

A

Dicarboxylic acid + diol monomer —-) poly (ester) + 2 water molecules

89
Q

Explain whether bond breaking is Exothermic or endothermic

A

Bond breaking is Endothermic,
Because amount of energy needed to break bonds,
Is greater than amount of energy released when bonds are formed

90
Q

Explain whether bond making is endo or Exothermic

A

Bond making is Exothermic,
Because amount of energy released to make bonds,
Is greater than amount of energy needed when bonds are broken

91
Q

Is displacement endo or Exothermic reaction

A

Can be both

92
Q

Explain the effect of increasing temperture on rate of reaction

A

Increasing temp, increases rate of reaction
Because particles have more kinetic energy
So are able to move more quickly
Therefore more frequent successful collisions per second
AND ALSO bc each collision has more energy,
There is a greater number of particles which have more energy than the activation energy require,
Therefore there are more succeful collisons

93
Q

Explain why the presence of a catalyst increases the rate of reaction

A

Because it decreases the activation energy required
By providing an alternative pathway with a lower activation energy
Therefore more particles have the minium amount of energy required for the reaction to occur

94
Q

Describe the reversible reaction of the dehydration of hydrated copper (ii) sulfate

A

When hydrated (ii) copper sulfate is heated, the blue crystals turn into a white powder anyhdrous copper sulfate and water.
This is the forward reaction,an endothermic reaction because energy is absorbed by the surroundings.
When water is added to anhydrous copper ii sulfate, it becomes blue copper sulfate crystals again.
This is an Exothermic reaction because heat is given out.

95
Q

Describe the reversible reaction of the decomposition of ammonium chloride

A

Ammonium chloride is a white solid. Upon heating, it breaks down into ammonia gas and hydrogen chloride. This is the forwards reaction whcih is endothermic, because energy is taken in.
If left to cool,the ammonia gas and hydrogen chloride reform to make the solid. This is the backwards reaction which is exothermic, because energy is released into surroundings

96
Q

What are the two conditions for dynamic equilibrium to occur:

A

-must be a reversible reaction
-must be in a closed container

97
Q

What happens at dynamic equilibrium

A

-The concentration of products and reacts remain constant, but not necessarily equal,
-because the forwards and backwards reactions happen at the same rate

98
Q

In the haber process, so when nitrogen and hydrogen combine to make ammonia, which direction is endothermic and which direction is exothermic

A

Forwards reaction is exothermic
Backwards reaction is endothermic

99
Q

Why does a catalyst not affect the position of equilibrium in a reversible reaction

A

Because a catalyst increases the overall rate of reaction.
So therefore, the rate of the the forward reaction increases at an equal rate as the backwards reaction does.
It only speeds p the reaction, and so does not have an effect on the position of equilibrium.

100
Q

What does the position of equilibrium mean

A

The side of the reaction which contains more particles

101
Q

What is the effect of temperture n the position of equilibrium

A

All reactions are endothermic in one direction and exothermic in the other direction.
If you increases the temperture, then the endothermic reaction will occur inorder to use more heat.
If you decrease the temperture, then the exothermic reaction will occur inorder to release more heat

102
Q

What is the effect of pressure on equilibrium

A

In all reactions, one side of the equation has more moles than the other.
If pressure increases, then the reaction om the side with thr least amount of moles will be encouraged, and fewer moles will be produced.
If you decreases the pressure, then the reaction on the side with the greater amount of moles will be encouraged and so more moles will be produced.

103
Q

Metal carbonate + acid =

A

Metal salt + co2 + water

104
Q

Two ways to make sure that all the acid is reacted, when mixing aluminum hydroxide and sulfuric acid to make a salt

A

Use excess aluminium hydroxide; [1 mark]
Stir (thoroughly); [1 mark]

105
Q

In an experiment to measure the value of x, in a water of crystallization, the value obtained is lower than what was expected. Explain why and how they could overcome this

A

The crystals were not heated for long enough so not all of the water was able to evaporate.
Can improve by reheating until your achieve a constant mass

106
Q

What is a solute

A

The solid that dissolves in a solvent

107
Q

What is a saturated solution

A

A solution in which the maximum amount of solute has dissolved as possible
AT A SPECFIC TEMPERATURE

108
Q

How does dilution occur

A

Because of diffusion, because particles of colour move from a high conc to low conc
And so can mix with the water molecules

109
Q

If comparing two setups of chromatography, what two things should be the same

A

Same solvent
Same chromatography paper

110
Q

What is atomic number

A

The number of protons in the nucleus of an atom

111
Q

Give six properties of metals

A

Good conductors pf electricity
Good conductors of heat
High density
High melting point
Malleable
Ductile

112
Q

Metal oxides are…
Non métal oxides are…

A

Basic
Acidic

113
Q

Why do ionic compounds have high melting points

A

Strong electrostatic forces of attraction
Between oppositely charged ions
So therefore large amounts of thermal energy needed to overcome these forces of attraction

114
Q

Why covalent substances low boiling + melting

A

Because weak intermolecular forces of attraction
Between the molecules
Therefore small amount of thermal energy required to overcome this attraction

115
Q

How many double bonds do alkenes have

A

Only one

116
Q

What is thermal decomposition

A

The breaking down of a COMPOUND
using heat

117
Q

How to calculate the solubility of a substance using experiment. Aka what formula could u use

A

Mass of solute/ mass of water removed
X100

118
Q

Give example of weak acid and string acid
Give example of weak alakali and strong alkali

A

Ethanoic acid, hydrochloric acid
Ammonia, sodium hydroxide

119
Q

Explain an experiment on how you can measure effect if catalyst on rate of reaction

A

Add certain volume of hydrogen peroxide to a conical flask
Measure certain mass of catalyst
Put a bung on
Measure time taken for certain volume of gas to be produced
Repeat with diff catalysts but with same mass, and same volume of hydrogène peroxide

120
Q

How do catalysts reduce the rate of reaction

A

They lower the activation energy required for a reaction
By providing an alternative reaction pathway with a lower activation energy
Therefore more particles have at least the minimum amount of energy required for reaction to occur

121
Q

What is the measurement that u take when measuring the effect of surface area on the rate of reaction

A

In a fixed amount of time, you are measuring the volume of gas produced
So every ten seconds, measure the amount of gas produced

122
Q

What is the first step of the flame test

A

Dip a loop of unreactive wire such as (platinum or Nichrome) dip in HYDROHCLORIC ACID

123
Q

In the flame test, what colour shows for the presence of sodium cations, and then for calcium cations

A

Sodium = yellow
Calcium =orange

124
Q

Apart from the flame test, describe another test you can carry out to identity cations

A

Adding sodium hydroxide to see if a precipitate will form.

1)so dissolve the salt in distilled water
2)then add sodium hydroxide
3)observe color of precipitate

125
Q

Why is sodium hydroxide specifically used to test for cations in the precipitate test

A

Because it is the only hydroxide that is soluble
Therefore when it reacts with a metal it forms a metal hydroxide
But metal hydroxides are all insoluble, so will form a precipate

126
Q

Apart from iron2+ and iron 3+, what are two other cations you can test for in the cation precipitate test

A

Ammonia
Copper 2+

127
Q

What is the chemical equation for the reaction between carbon dioxide and limewater

A

CO2 + CaOH2 ——-) CaCO3 + H2O

128
Q

Give the solubility rules of carbonates hydroxides and sulfates in order of what you’ve memorized

A

Sulfates: barium, lead, calcium
Carbonates: sodium, potassium, ammonium (all others insoluble)
Hydroxides: sodium, potassium, calcium (all others insoluble)

129
Q

Give the word equation to make a soluble salt.
Give the word equation to make an insoluble salt.

A

Insoluble base + acid—-) soluble salt + water
Soluble salt + soluble salt ——) insoluble salt + soluble salt

130
Q

Give the steps to make an insoluble salt

A

1)add soluble salt to soluble salt
2)filter off the précipitate
3)add to distilled water
4)observe the precipitate formed

131
Q

Give three examples of insoluble salts and the colour of the precipitates that they form

A

Lead sulfate
Barium sulfate (white precipitate)
Silver chloride (white precipitate)

132
Q

An insoluble salt is made, how do U identify the two substances that it was made from

A

The metal part usually comes from a nitrate
The non metal part usually comes from sodium, potassium or ammonium

133
Q

Give step one of making a soluble salt

A

Heat the acid under a Bunsen burner so that rate of reaction will also be sped up

134
Q

When making a soluble salt, give the next few steps after filtering off the excess base so that you’re left with salt solution and water

A

Heat to evaporate SOME of the water to form concentrated solution
Keep heating until saturated solution is formed
Leave soltuion to cool and to crystallize
Filter off the soltuion so that left with crystals as residue

135
Q

Why do you not evaporate off all the water when making a soluble salt

A

Because the water needs to be present for water of crystallization
And also to prevent it from decomposing

136
Q

Which one of the metals in the reactivity series does not react with water

A

Aluminum

137
Q

What happens when aluminum reacts with acid in the reactivity series

A

Slow to start, but eventually becomes more vigourous
(Aluminum oxide layer on top prevents reaction)

138
Q

State the colour changes of the three metals when they react with hydrochloric acid

A

Magnesium —) colourless
Zinc——) colourless
Iron——) green

139
Q

What are two types of displacement reaction that can occur, and what happens in them

A

Redox, with a metal and metal oxide (more reactive binds with oxygen)
An aqeous soltuion of a metal salt(more reactive displaces less reactive, less reactive coats the surface)

140
Q

Apart from magnesium, what two other substances can be used in a combustion reaction and give the colour of the flames that they produce

A

Sulfur, which forms a dark blue flame
Hydrogen, forms a pale blue flame

141
Q

What is an ore. What is a mineral. What is a native substance

A

Ore is a substance that contains enough of a wanted mineral in it
Mineral is a substance that occurs naturally
Native is s substance that occurs without any other minerals in it

142
Q

Describe the structure of ionic compounds

A

A giant lattice structure
Closely packed and regular arrangement
Of a repeating pattern of positive and negative ions
Held together by strong electrostatic forces of attraction between the oppsitely charged ions

143
Q

Graphite melting and boiling point

A

High melting and boiling point,
Bc although weak intermolecular forces of attraction holding the layers together
The individual atoms are held together by strong covalent bonds.
Require large amounts of heat energy to overcome

144
Q

Can graphite conduct electricty and explain

A

Yes
Because
Each carbon atom forms three bonds with three other carbon atoms
Therefore each carbon atom has one delocalized electron
Which is free to move and conduct a charge

145
Q

Describe a Metallic structure

A

Giant metallic lattice structure
Held together by positive ions
Surrounded by sea of delocalized electrons

146
Q

Anode rule
Cathode rule

A

Anode rule. If halide is parents it will be discharged.otherwise OH- will be discharged
Cathode rule. Least reactive will be discharged (relative to hydrogen)

147
Q

If OH- ions discharged at the anode, what produces will be produced

A

Oxygen and hydrogen
(Rmeber in the equation u also have to add 4e aswell tho)

148
Q

Give the general word equation for an alkene + bromine,

A

Alkene + bromine —-) alkane(1,2 dibromoalkane)

149
Q

General word equation for substitution

A

Alkane + halogen —) halogens alkane + hydrogen halide

150
Q

Give the general word equation for when ethanol is oxidized using a reducing agent

A

Ethanol + 2(o) —) ethanoic acid + water

151
Q

Give the general word equation when ethanol is oxidized used aerobic respiration

A

Ethanol + oxygen —-) ethanoic acid + water

152
Q

Give the eternal word equation for hydration of ethene

A

Ethene + steam —-) ethanol

153
Q

Give the general word equation for fermentation

A

Glucose —(yeast)—-)ethanol +co2

154
Q

Give the structural formula of methanoic acid
And then of ethanoic acid

A

HCOOH
CH3COOH

155
Q

Do carboxylic acids have a double bond or not

A

Yes

156
Q

Give three conditions required for addition polymerization

A

-Hugh temperatures and pressures
-must be unsaturated
-an initiator required

157
Q

Give the steps to make an ester

A

-Mix Carboxylic acid and alcohol together, and then add concentrated sulfuric acid as the catalyst
-add calcium carbonate to remove alcoholic impurities
-add sodium carbonate to remove acidic impurities
Ester will float on top

158
Q

Give the general word equation for condensation polymerization

A

Dicarboxylic acid + diol monomer —) poly(ester) + water

159
Q

When hydroxide ions are deposited at the anode, give the half equation

A

4OH~ ——) 2H2O + O2 + 4e~

160
Q

Concordant results differ by..

A

O.2cm3 or less

161
Q

How does a catalyst increase rate of reaction

A

Provides an alternative pathway
With a lower activation energy
Therefore more particles have more energy than the activation energy

162
Q

Reaction of ammonia and sulfuric acid word equation
Reaction of ammonium and sulfuric acid

A

Ammonia + sulfuric acid —-) ammonium sulfate
Ammonium + sulfuric acid —-) ammonium sulfate + water

163
Q

Metal oxide + water

A

Metal hydroxide

164
Q

Metal + steam

A

Metal oxide + hydrogen

165
Q

Metal + water

A

Metal hydroxide + hydrogen

166
Q

Metal + oxygen

A

Metal oxide

167
Q

Metal oxides are… (soluble/ insoluble)

A

Usually insoluble.
Except can form metal hydroxides sometimes

168
Q

Non metal oxides are ..soluble/ insoluble

A

Soluble

chemistry (18 decks)

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