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GCSE Combined Chemistry (Edexcel) > Topic 5 & 6 - Groups in the Periodic Table and Rates of Reaction and Energy Changes COMPLETE PK > Flashcards

Topic 5 & 6 - Groups in the Periodic Table and Rates of Reaction and Energy Changes COMPLETE PK Flashcards

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1
Q

1 What do atoms of the same element have in common?

A

their atomic number/number of protons

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2
Q

2 Roughly how many elements are found naturally?

A

90 to 100

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3
Q

3 In what order are elements arranged in the periodic table?

A

in order of increasing atomic number

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4
Q

4 What do you call the columns in the periodic table?

A

groups

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5
Q

5 What is special about the elements that are in the same group of the periodic table?

A

similar properties

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6
Q

6 What is similar about the electronic configuration of elements in the same group?

A

same number of outer electrons

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7
Q

7 What is formed when a group 1 element reacts with water?

A

an alkali/metal hydroxide + hydrogen

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8
Q

8 What is the charge on the ions of elements in group 1?

A

1+

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9
Q

9 The first two elements in group 1 are lithium and sodium. What is the third element?

A

potassium

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10
Q

10 What name is given to group 1 elements?

A

the alkali metals

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11
Q

11 What happens to the reactivity of the group 1 elements as you go down the group?

A

it increases

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12
Q

12 What is produced when lithium reacts with water?

A

lithium hydroxide and hydrogen

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13
Q

13 Why do alkali metals get more reactive as you go down the group?

A

the outermost electron is further and further away, and so more easily removed

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14
Q

14 What name is given to group 7 elements?

A

the halogens

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15
Q

15 State an example of a group 7 element.

A

one of: fluorine, chlorine, bromine, iodine or astatine

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16
Q

16 What is the state of a substance at room temperature, if it has a melting point of 7 °C and a boiling point of 59 °C?

A

liquid

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17
Q

17 What ion is in all acid solutions?

A

H+

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18
Q

18 Do metals usually form ionic compounds with other metals, non-metals, neither or both?

A

non-metals

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19
Q

19 State the formula of the compound formed when calcium reacts with bromine.

A

CaBr2

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20
Q

20 What is the name and colour of the only liquid halogen?

A

bromine, brown

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21
Q

21 What does chlorine look like?

A

pale green gas

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22
Q

22 How is the appearance of iodine different from that of the three halogens above it in group 7?

A

solid and darker/black in colour

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23
Q

23 Name the compound formed when hydrogen reacts with chlorine.

A

hydrogen chloride

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24
Q

24 What kind of solution is formed when hydrogen fluoride dissolves in water – acidic, neutral or alkaline?

A

acidic

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25
Q

25 Complete the equation: Ca(s) + Cl2(g) →

A

CaCl2(s)

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26
Q

26 What ions are present in potassium fluoride?

A

K+ and FI-

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27
Q

27 State one similarity in the electronic configurations of fluorine and chlorine.

A

same number of outer electrons

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28
Q

28 Describe the trend in reactivity of group 7 elements.

A

decreasing down the group

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29
Q

29 What type of reaction occurs between chlorine and potassium bromide?

A

displacement and redox

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30
Q

30 What is formed when chlorine water is added to sodium bromide solution?

A

sodium chloride + bromine

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31
Q

31 What type of reaction is the reaction between chlorine water and sodium bromide solution an example of?

A

displacement, redox

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32
Q

32 Fluorine atoms are more reactive than chlorine atoms. What does fluorine have fewer of that explains this?

A

electron shells

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33
Q

33 H Describe reduction in terms of electron transfer.

A

gain of electrons

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34
Q

34 Where is group 0 found in the periodic table?

A

last column on right-hand side

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35
Q

35 What name is given to group 0 elements?

A

the noble gases

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36
Q

36 Name a group 0 element.

A

one of: helium, neon, argon, krypton, xenon or radon

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37
Q

37 What is similar about the electronic configuration of all group 0 elements?

A

full outer shell

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38
Q

38 How are noble gases similar in terms of chemical properties?

A

all unreactive

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39
Q

39 Describe the trend in the boiling points of the elements, down group 0.

A

increasing

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40
Q

40 What happens to the reactants during a chemical reaction?

A

They are changed into new substances/products/used up.

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41
Q

41 What happens to the rate of most reactions as the reaction proceeds?

A

It slows down.

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42
Q

42 In reactions involving solutions, what happens to the rate if the concentrations at the start are decreased?

A

They become slower.

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43
Q

43 What size of solid lumps reacts fastest in chemical reactions: small, medium or large?

A

small

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44
Q

44 Apart from concentration and surface area, name one other variable that can change the speed of a chemical reaction.

A

temperature or pressure or catalyst

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45
Q

45 What happens in a precipitation reaction?

A

A solid forms.

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46
Q

46 What does it mean if effervescence is seen during a reaction?

A

A gas is being produced.

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47
Q

47 What happens to the concentration of reactants as a reaction proceeds?

A

It decreases.

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48
Q

48 What happens to the concentration of products as a reaction proceeds?

A

It increases.

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49
Q

49 Why is there a loss in mass during the reaction between calcium carbonate and hydrochloric acid?

A

A gas is given off/lost.

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50
Q

50 What usually happens to the rate of a reaction as the reaction proceeds?

A

It slows down.

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51
Q

51 What happens to the concentration of reactants as a reaction proceeds?

A

It decreases.

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52
Q

52 In a graph of concentration of products against time, how do you know when the reaction is finished?

A

The graph levels off.

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53
Q

53 A reaction is followed by measuring the volume of gas produced. What other measurement could be used?

A

measuring mass lost

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54
Q

54 What usually happens to the speed of a reaction as the temperature is decreased?

A

It gets slower.

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55
Q

55 How does increasing the concentration of a solution affect the rate of reaction?

A

It increases the rate.

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56
Q

56 What is the link between the size of the solid lumps and the surface area of a fixed mass of solid?

A

The smaller the lumps, the larger the surface area.

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57
Q

57 What type of solid lumps will react fastest?

A

the smallest lumps or powders

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58
Q

58 In reactions involving gases, how does gas pressure affect the reaction rate?

A

Increased pressure increases the rate.

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59
Q

59 What must the reacting molecules do for a reaction to occur?

A

They must collide with enough energy.

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60
Q

60 What has to happen before a reaction takes place?

A

Reacting molecules must collide with enough energy.

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61
Q

61 Describe two ways of measuring reaction rates in a reaction that produces a gas.

A

measuring volume of gas formed and mass lost by reactants

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62
Q

62 Explain how increasing concentrations increases the rate of a reaction.

A

More collisions occur.

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63
Q

63 What change in condition increases the speed of the reacting molecules?

A

increasing temperature

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64
Q

64 How can you increase the surface area of a solid?

A

Divide the solid into smaller pieces.

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65
Q

65 Explain how increasing the surface area of a solid increases the rate of reaction.

A

More collisions can occur.

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66
Q

66 Which change in condition only affects reactions involving gases?

A

pressure

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67
Q

67 What is the activation energy in a reaction?

A

minimum energy needed by reactants for them to react

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68
Q

68 What does a catalyst do?

A

speeds up a chemical reaction

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69
Q

69 What do you call a biological catalyst?

A

an enzyme

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70
Q

70 What do we call any substance that dissolves in a solvent to form a solution?

A

solute

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71
Q

71 What products form when an acid is neutralised by an alkali?

A

a salt and water

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72
Q

72 What do we call an insoluble substance that can form when two solutions are mixed?

A

precipitate

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73
Q

73 Which substance, polystyrene or copper, is the better heat insulator?

A

polystyrene

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74
Q

74 Energy is transferred by heating in three ways: convection, radiation and what else?

A

conduction

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75
Q

75 Zinc reacts with copper sulfate solution. What solid product forms?

A

copper

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76
Q

76 What gas is needed for fuels to burn?

A

oxygen

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77
Q

77 Fuels may ignite if a spark hits them. What else can make a fuel ignite?

A

a flame/heating strongly

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78
Q

78 Is energy transferred to or from the electrolyte during electrolysis?

A

to

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79
Q

79 Give two ways by which energy is transferred to the surroundings in an explosion.

A

two from: by heating, by sound, by light, by a force

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80
Q

80 What type of reaction takes in energy from the surroundings?

A

endothermic

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81
Q

81 What happens to the temperature of an acid when an alkali is added to it?

A

It goes up/increases.

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82
Q

82 What simple piece of apparatus is used to measure temperature?

A

thermometer

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83
Q

83 What unit is used for energy?

A

J/joule/kJ/kilojoule

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84
Q

84 What type of bond (ionic, covalent or metallic) exists between non-metals

A

covalent

85
Q

85 In combustion reactions, is energy taken in from the surroundings or given out?

A

given out

86
Q

86 How is energy transferred between reactants and surroundings during dissolving?

A

by heating

87
Q

87 Which of these reactions, displacement or precipitation, always heats up the surroundings?

A

displacement

88
Q

88 The temperature goes down when ammonium nitrate dissolves in water. Is this an exothermic process or an endothermic process?

A

endothermic

89
Q

89 Energy is taken in so that bonds can be broken. Is this an exothermic or an endothermic process?

A

endothermic

90
Q
  1. Burning methane - endothermic or exothermic?
A

exothermic

91
Q

What are group number 1 elements of the periodic table also known as?

A

Alkali metals

92
Q

What are group number 7 elements of the periodic table also known as?

A

Halogens

93
Q

What are group number 8 elements of the periodic table also known as?

A

Noble gases

94
Q

What are the metals in the middle of the periodic table known as?

A

The transition metals

95
Q

Group 8 can also be called group _

A

0

96
Q

Noble gases have a ____ outer shell

A

full

97
Q

Noble gases are extremely reactive/unreactive

A

Unreactive

98
Q

Give 2 uses of noble gases

A

Balloons and neon lights

99
Q

Halogens are metals/non-metals

A

Non-metals

100
Q

Halogens are ________ molecules

A

diatomic

101
Q

What does being a diatomic molecule mean?

A

They are going to go around together in pairs

102
Q

Give the formula for a diatomic molecule

A

Any of the following: Cl2, F2​, Br2​, etc

103
Q

How can fluorine easily gain an electron?

A

By sharing it with another fluorine

104
Q

Diatomic molecules want to gain _ electron

A

1

105
Q

How can diatomic molecules gain an electron?

A

By sharing an electron with something that is the same

106
Q

Halogens are highly reactice/unreactive

A

reactive

107
Q

The most reactive halogens are at the bottom/top of the periodic table

A

Top

108
Q

The boiling point increases as we move up/down group 7

A

Down

109
Q

Elements at the top of group 7 have a low/high boiling point

A

Low

110
Q

Elements at the bottom of group 7 have a low/high boiling point

A

High

111
Q

When halogens react they loose/gain an electron

A

gain

112
Q

Do halogens form +1 or -1 ions?

A

-1

113
Q

Gaining an electron is reduction/oxidation

A

Reduction

114
Q

How can you remember whether losing an electron is oxidation or reduction?

A

OIL RIG

Oxidation is Loss, Reduction is Gain

115
Q

Halogens react rapidly and violently with group _ metals

A

1

116
Q

Why do halogens react rapidly and violently with group 1 metals?

A

Because group 1 metals want to loose 1 electron

117
Q

A more reactive element will displace a…

A

Less reactive element

118
Q

Reactions when a more reactive element displaces a less reactive element are called…

A

displacement reactions

119
Q

What are halogens mostly used for?

A

Sterilising things, such as chlorine in a swimming pool

120
Q

Why are the most reactive halogens at the top?

A

That is where there is the least shielding between the electron they want to gain and the nucleus

121
Q

Alkali metals react very violently with…

A

water

122
Q

What happens when alkali metals react with water?

A

Different coloured flames are produced

123
Q

Group _ metals are what are used to make the different colours in fireworks

A

1

124
Q

The lilac flame from potassium is commonly used to make

A

fireworks

125
Q

Alkali metals are s___ g___ metals

A

soft grey

126
Q

Alkali metals are hard to cut/easy to cut

A

easy to cut

127
Q

True/False: Alkali metals need to be kept in sand

A

False, they need to be kept in oil

128
Q

Why do alkali metals need to be kept in oil?

A

So they don’t react with oxygen or the water in the air because it is a very violent reaction

129
Q

When a metal reacts with oxygen it produces a…

A

metal oxide

130
Q

When a metal reacts with water it produces a…

A

metal hydroxide

131
Q

The dullness after an alkali metal has been cut is the metal oxide/hydroxide

A

Oxide

132
Q

Metal hydroxide is acidic/alkaline

A

Alkaline

133
Q

How can you see if something is an acid or alkali?

A

Use an indicator

134
Q

Alkali metal + water -> metal hydroxide is a very endothermic/exothermic reaction

A

exothermic

135
Q

Alkali metal + water releases a lot of heat and also releases…

A

hydrogen gas - this is what the fizzing is

136
Q

The most reactive alkali metals are at the top/bottom of the periodic table

A

bottom

137
Q

The least reactive alkali metals are at the top/bottom of the periodic table

A

top

138
Q

Alkali metals at the bottom of the periodic table have high/low melting and boiling points

A

low

139
Q

Alkali metals at the top of the periodic table have high/low melting points and boiling points

A

High

140
Q

Alkali metals want to loose/gain an electron

A

Loose

141
Q

Why are the alkali metals at the bottom of the periodic table the most reactive?

A

Because there is more shielding between the electron that they want to use and the positive nucleus in the middle

142
Q

Give a way of following a reaction

A

Either loss of mass or production of gas

143
Q

When is looking for a loss of mass a good way to follow a reaction?

A

When you have added something solid like marble chips into a liquid and you know that a gas is going to be produced

144
Q

Why is looking for a loss of mass good when adding something solid to a liquid, knowing that a gas is going to be produced?

A

The gas will just go through the cotton wool at the top of the tube and out, and the mass will go down

145
Q

Apart from measuring a loss of mass, what is a good way of following a solid + liquid -> gas reaction?

A

Collecting the gas in a measuring syringe or an inverted measuring cylinder

146
Q

When measuring the rate of reaction, it is important to look carefully at the u____ used

A

units

147
Q

There is a graph showing rate of reaction, with volume of CO2 produced (cm3) on the y axis and time in minutes on the x. What is this graph measuring?

A

cm3/minute

148
Q

There is a graph showing rate of reaction, with mass in grams on the y axis and time in seconds on the x. What is this graph measuring?

A

g/s

149
Q

What do you need to draw on a graph to find the rate of reaction at a particular point?

A

A tangent

150
Q

Once you have drawn the tangent on a graph that you want to find the rate of reaction at a particular point of, what do you need to do?

A

Find the gradient of the tangent

151
Q

When calculating rate of reaction at a certain point of a graph, what units do you need to use?

A

The ones on the graph

152
Q

How do you find the gradient of a line?

A

Change in y / change in x

153
Q

There will be the same/different rates of reaction at different points on a graph

A

Different

154
Q

Sodium thiosulfate + hydrochloric acid

We can follow rate of reaction by looking at…

A

colour change taking place or how it changes from clear/colourless to opaque

155
Q

Why do you need to constantly wash things out when doing sodium thiosulfate + hydrochloric acid?

A

So you’re not contaminating things

156
Q

Why do you need to be careful not to go above 60 degrees when doing sodium thiosulfate + hydrochloric acid?

A

Nasty gases will start to come off at the end

157
Q

Why is it important not to get anything on your hands when doing sodium thiosulfate + hydrochloric acid?

A

It will start to irritate your hands

158
Q

Why is it important the same person measures rate of reaction (sodium thiosulfate + hydrochloric acid)?

A

So differences in people’s eyes don’t effect the results

159
Q

One way that we can collect ___ is by using an inverted measuring cylinder and putting a d_______ t___ through there

A

Gas, delivery tube

160
Q

When collecting gas using an inverted measuring cylinder and a delivery tube, one thing that we need to be careful about is the ___ that is aready in the measuring cylinder before/after you start the experiment

A

gas, before

161
Q

When collecting gas using an inverted measuring cylinder and a delivery tube, the gas will move from the connical flask, through the delivery tube and in to the _________ ________

A

measuring cylinder

162
Q

When collecting gas using an inverted measuring cylinder and a delivery tube, why do we collect the gas in the measuring cylinder?

A

So we can measure it

163
Q

When collecting gas using an inverted measuring cylinder and a delivery tube, what is a common cause of errors?

A

The gas that is already in the cylinder before you start / gas is lost before you manage to get the bung on

164
Q

When collecting gas using an inverted measuring cylinder and a delivery tube, when adding large marble chips, what starts to collect in the measuring cylinder?

A

Bubbles

165
Q

When collecting gas using an inverted measuring cylinder and a delivery tube, why is gas sometimes lost?

A

Some can escape before you manage to get the bung on

166
Q

When collecting gas using an inverted measuring cylinder and a delivery tube, what happens when you add powdered calcium carbonate?

A

It increases, bubbles are produced much faster and the measuring cylider fills up very quickly

167
Q

When we have particles moving around at a low temperature, they are moving ______ with little/lots of energy

A

slowly litte

168
Q

True/False: When particles at a low temperature collide, there is always a reaction

A

False, there is not always a reaction

169
Q

When particles with high temperature, they move at ____ speed with lots of/little energy

A

high, lots of

170
Q

True/False: When partices at high temperature collide, there is no reaction

A

False: There are a lot of reactions taking place

171
Q

True/False: Temperature can effect rate of reaction

A

True

172
Q

Sugar cubes in hot water will dissolve much faster/slower than sugar cubes in cold water

A

Faster

173
Q

The higher the temperature, the faster/slower the rate of reaction will be

A

faster

174
Q

Why does temperature increase rate of reaction?

A

Particles have more energy, so they can move around faster, which leads to more frequent and successful collisions

175
Q

Temperature increases rate of reaction because particles have more ______, so they can move around ______, which leads to more ________ and successful collisions

A

energy, faster, frequent

176
Q

When we have a lump of something, there is less/more surface area, so there is less/more space to react

A

less

177
Q

When we have a powder of something, there is less/more surface area, so there is less/more space to react

A

more

178
Q

The larger the surface area, the faster/slowe the rate of reaction

A

faster

179
Q

Why does large surface area increase rate of reaction?

A

Because there are more particles available to react, leading to more successful collisions

180
Q

The larger the surface area, the ______ the rate of reaction, this is because there are ____ particles availble to react, leading to more __________ collisions

A

faster, more, successful

181
Q

When there are things at a high pressure / at a high concentration, they’re much more/less likely to bump in to each other and react

A

more

182
Q

When there are things at a low concentration, they’re much more/less likely to bump in to each other and react

A

less

183
Q

The higher the concentration/pressure, the ______ the rate of reaction

A

faster

184
Q

Why is the rate of reaction faster when concentration/pressure is higher?

A

Here are more particles in a fixed volume, so there is a higher chance of successful collisions

185
Q

What does a catalyst do?

A

Makes a reaction easier to happen, speeds up the reaction and lowers activation energy

186
Q

True/False: An example of something a catalyst does is fixes reactants in place so it is easier for the other reactant to find it

A

True

187
Q

True/False: Whenever there is a reaction, there is an activation energy

A

True

188
Q

What does the hump on this graph represent?

A

The activation energy

189
Q

Which side of the graph is the activation energy measured from? (Before the hump or after the hump)

A

After the hump

190
Q

Catalysts increase/decrease activation energy

A

Decrease

191
Q

What is the effect of activation energy being lowered by a catalyst?

A

It is easier for a reaction to take place

192
Q

The blue line on this graph shows activation energy. The green line shows it after it has been _________, so it is easier for the reaction to take place.

A

catalysed

193
Q

An endothermic reaction feels like it gets colder/hotter

A

colder

194
Q

An exothermic reaction feels like it gets colder/hotter

A

Hotter

195
Q

Endothermic reactions take energy in/give energy out

A

Take energy in

196
Q

Exothermic reactions take energy in/give energy out

A

Give energy out

197
Q

In an endothermic reaction, the energy of the products is ______ than the energy of the reactants

A

higher

198
Q

Does this graph represent an endothermic or an exothermic reaction?

A

Endothermic

199
Q

In an exothermic reaction, the products have _____ energy than the reactants

A

lower

200
Q

Does this graph represent an endothermic or an exothermic reaction?

A

Exothermic

201
Q

True/False: Electrolysis is an endothermic reaction

A

True

202
Q

True/False: Burning is an endothermic reaction

A

False, it is an exothermic reaction

203
Q

True/False: Neutralisation is an exothermic reaction

A

True

204
Q

Bond breaking takes energy in/gives energy out

A

Takes energy in

205
Q

Bond making takes energy in/gives energy out

A

Gives energy out

206
Q

Burning hydrogen in water will give water.

What is the balanced equation for this reaction?

A

2H2 + O2 -> 2H2O

207
Q

Burning hydrogen in oxygen will give water, calculate the energy change for this reaction

Bond energies:

H-H = 436kj/mol

O=O = 498 kj/mol

O-H = 464 kj/mol

A

-486kj/mol

208
Q

If the calculated energy change for a reaction is negative, you know that the reaction is endothermic/exothermic

A

Exothermic

209
Q
A

GCSE Combined Chemistry (Edexcel) (5 decks)

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