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Y10 Recall quiz questions Flashcards

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1
Q

Give every day use of endothermic reaction

A

sports injury packs

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2
Q

what sub-atomic particle was discovered first?

A

the electron

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3
Q

Before electrons were discovered, what were atoms thought to be?

A

indivisible

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4
Q

Before electrons were discovered, atoms were thought to be what

A

tiny spheres

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5
Q

What model did the discovery of the electron lead to?

A

the plum pudding model

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6
Q

What was the plum pudding model?

A

that the atom was a ball of positive charge with negative electrons embedded in it

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7
Q

What is the energy of the products compared to reactants in an exothermic reaction

A

less

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8
Q

What is the energy of the products compared to reactants in an endothermic reaction

A

more

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9
Q

What is activation energy

A

Minimum energy that particles must have for a reaction to occur

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10
Q

What is an exothermic reaction?

A

energy is transferred to the surroundings

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11
Q

What happens to the temperature of an exothermic reaction?

A

temperature increases

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12
Q

What is an endothermic reaction?

A

energy is taken in from the surroundings

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13
Q

What happens to the temperature of an endothermic reaction?

A

temperature decreases

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14
Q

How can you tell what a reaction profile represents

A

if reactants is above products it is exothermic and if it is below then it is endothermic

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15
Q

How does filtration work?

A

Pass through filter paper, liquid passes through, insoluble particles get caught by the filter paper

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16
Q

Where are the reactants found in an equation?

A

Left-hand side

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17
Q

Where are the products found in an equation?

A

Right-hand side

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18
Q

What is chromatography?

A

a method used to separate the coloured compounds in a mixture

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19
Q

How long have the proportions of the gases in the atmosphere been like today?

A

200 million years

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20
Q

What type of bond is formed between a metal and non-metals?

A

ionic

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21
Q

What type of bond involves gain or loss of electrons?

A

ionic

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22
Q

What happens when a metal and a non-metal form an ionic bond?

A

electrons are transferred (lost/gained)

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23
Q

What is the group number if an element forms a -2 ion?

A

6

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24
Q

If an atom loses two electrons to form an ion what charge will the ion have?

A

+2

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25
Q

Why do metals and non-metals form ionic bonds?

A

to achieve a full outer shell and be stable

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26
Q

What are the gases found in today’s atmosphere? cownn

A

nitrogen, oxygen, carbon dioxide, water vapour , noble gases

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27
Q

What are the percentages of the gases in today’s atmosphere?

A

80% nitrogen,20% oxygen, less than 1% other gases

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28
Q

What planets is the earth’s early atmosphere suggested to be like?

A

Mars and Venus, consisting mainly of carbon dioxide and little or no oxygen

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29
Q

What other gases were released by volcanoes?

A

Nitrogen, Methane, Ammonia

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30
Q

Which one is NOT one of the ways carbon dioxide levels were reduced?

A

Plants carry out respiration

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31
Q

Why did the percentage of oxygen increase in the early atmosphere?

A

Algae and plants released it during photosynthesis

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32
Q

What is the correct word equation for photosynthesis?

A

Carbon dioxide + water –> glucose + oxygen

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33
Q

When did algae first appear?

A

2.7 billion years ago

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34
Q

What did the increase in oxygen from algae and plants lead to?

A

Enabled animals to evolve

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35
Q

What do particulates contribute to?

A

global dimming (smog)

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36
Q

What are the particles like in an ionic bond?

A

Oppositely charged ions (positive and negative ions)

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37
Q

What is a carbon footprint?

A

The total amount of carbon dioxide and other greenhouse gases emitted over the full life cycle of a product, service or event

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38
Q

How can a carbon footprint be reduced?

A

By reducing emissions of carbon dioxide and methane by reducing use of cars (cycle/ walk instead), eat less meat, recycle

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39
Q

What type of bonding is likely to occur between group 1&2 metals with group 6&7 non-metals?

A

ionic

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40
Q

How are oxides of nitrogen produced when burning a fuel?

A

High temperature in car engines cause oxygen and nitrogen in the air to react

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41
Q

How is sulfur dioxide produced when burning a fuel?

A

Fuels contain sulfur as an impurity, when the fuel is burnt the sulphur reacts with Oxygen to form sulphur

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42
Q

what do oxides of nitrogen and sulfur dioxide lead to?

A

respiratory problems and acid rain

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43
Q

What does carbon dioxide contribute to?

A

global warming

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44
Q

What are the issues with the production of carbon monoxide?

A

poisonous

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45
Q

Why is it hard to detect if carbon monoxide is formed?

A

it is odourless and colourless so it can’t be seen

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46
Q

What is a pure substance?

A

A substance made up of single element or compound, not mixed with any other substances

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47
Q

What are the boiling and melting points like for pure substances?

A

At a fixed (specific) temperature

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48
Q

What are the boiling and melting points like for an impure (mixture) substances?

A

over a range

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49
Q

What is a formulation?

A

A mixture that has been designed as a useful product

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50
Q

Which method is used to separate dyes?

A

Chromatography

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51
Q

What type of force exists between oppositely charged ions?

A

Electrostatic force

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52
Q

What type of structure is found in ionic compounds?

A

Giant lattice

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53
Q

What formula would the following ions have: Mg2+ and O2?

A

MgO

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54
Q

Why do ionic compounds conduct when melted or dissolved in water? (walk,backpack)

A

Ions can move and carry a charge

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55
Q

What do atoms do in a covalent bond to get a full outer shell?

A

Share pairs of electrons

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56
Q

What gases can be released into the atmosphere when a fuel is burnt?

A

Carbon monoxide, sulphur dioxide, oxides of nitrogen

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56
Q

What type of bonding is formed between just non-metals?

A

Covalent

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57
Q

How are covalent bonds shared?

A

Electrons are shared

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57
Q

How many electrons does each atom donate in a single covalent bond?

A

1

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58
Q

What is the strength of a covalent bond?

A

Strong

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59
Q

What experiment led to idea that mass of the atom was concentrated in the centre?

A

Alpha Scattering Experiment

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60
Q

What would happen with the alpha particle experiment if the plum pudding model was correct?

A

Particles to pass straight through or slightly deflected

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61
Q

Why did most of the alpha particles go straight through?

A

Atom is mostly empty space

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62
Q

Why did some alpha particles deflect more than expected?

A

Alpha particles hit a positively charged centre and repelled

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63
Q

Why did very few alpha particles deflect backwards?

A

Alpha particles hit a concentrated mass

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64
Q

Why do atoms have no overall electrical charge?

A

An atom has the same number of positive protons as negative electrons

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65
Q

What is an isotope?

A

The same element but with the same number of protons but different numbers of neutrons

66
Q

Why is the relative atomic mass of chlorine not a whole number

A

Has more than one isotope

67
Q

How can we reduce the emissions of carbon dioxide and methane?

A

Reduce use of cars (cycle/ walk instead), Eat less meat, Recycle

68
Q

What is a major source of atmospheric pollutants? (COF)

A

Combustion of Fuels

69
Q

What do most fuels contain?(c,h,ss)

A

carbon, hydrogen and some contain sulphur

70
Q

What are the melting point of giant covalent structures?

A

High

71
Q

Why can diamond not conduct electricity?

A

No ions or delocalised electrons

72
Q

Why can graphite conduct electricity?

A

Contains delocalised electrons that are able to move and carry a charge through structure

73
Q

What is graphene?

A

One layer of graphite

74
Q

What are carbon nanotubes?

A

A cylinder tube of graphite

75
Q

What are fullerenes?

A

A hollow ball with hexagons of carbon atoms

76
Q

What human activities are increasing the level of carbon dioxide and methane

A

Farming cattle,landfill sites,deforestation

77
Q

Why don’t simple covalent molecules conduct electricity?

A

No ions or delocalised electrons

78
Q

What is the difference between graphene and graphite?

A

graphite has layers

79
Q

Why can graphite conduct electricity?

A

Contains delocalised electrons able to move and carry a charge through structure

80
Q

What do scientists believe human activity will do to the temperature of the earth?

A

Increase it, leading to climate change

81
Q

Why is it difficult to predict global warming?

A

speculation of the future and opinion presented in media

82
Q

What is the issue with climate change presented in the media?

A

Based on opinion, only parts of evidence is reported and can be biased

83
Q

What is climate change?

A

Increase in average global temperature

84
Q

What are the main four potential effects of global climate change?

A

glacier and polar ice melting, sea levels rising, patterns in rainfall changing leading to floods or droughts, habitats changing

85
Q

How are the atoms linked in a polymer?

A

Strong bonds between the atoms

86
Q

What happens to the boiling point of simple covalent molecules with increasing size?

A

Increases because there are more of the weak intermolecular forces present

87
Q

What was the first fullerene discovered?

A

Buckministerfullerene

88
Q

Why can metals conduct electricity?

A

Contains delocalised electrons able to move and carry a charge through structure

89
Q

Why are metals malleable?

A

When a force applied the layers of atoms can slide over each other

90
Q

Why are pure metals not suitable for many uses?

A

Too soft

91
Q

What is an alloy?

A

A mixture of metals

92
Q

Why are alloys harder than the pure metal?

A

Different sized atoms disrupt the layers

93
Q

What is the state symbol for a solid?

A

(s)

94
Q

What is the state symbol for a liquid?

A

(l)

95
Q

What is the state symbol for aqueous?

A

(aq)

96
Q

What is the state symbol for gas?

A

(g)

97
Q

What happens to the bonds/ forces when melting?

A

weakened

98
Q

What happens to the bonds/ forces when boiling?

A

broken

99
Q

What is gained during melting/ boiling?

A

energy

100
Q

What is the process called for: liquid –> gas?

A

evaporation

101
Q

What is the process called for: gas –> liquid?

A

condensation

102
Q

What is the process called for: liquid –> solid?

A

freezing

103
Q

What is the process called for: solid –> liquid?

A

melting

104
Q

How can you tell how many elements are present in a product?

A

count the number of capital letters

105
Q

How can you tell how many atoms are present in a product?

A

add the number (including the element without numbers which have 1 atom)

106
Q

What is the atomic mass (Ar)?

A

Top number on the periodic table

107
Q

What is the relative formula mass (Mr)?

A

Sum of the relative atomic masses of the atoms in the formula

108
Q

What is the law of conservation of mass

A

No atoms are lost or made during a chemical reaction so the mass of the products equals the mass as the reactants

109
Q

How do the relative formula masses of the reactants compare to the products?

A

they are equal

110
Q

What sub atomic particle is involved in bonding (chemical reactions)?

A

Electrons

110
Q

How many electrons are in each shell?

A

2,8,8

110
Q

What holds atoms of elements together in compounds?

A

chemical bonds

111
Q

How were early periodic tables arranged (Newland and Mendeleev)?

A

Atomic mass

111
Q

How is the modern periodic table ordered?

A

in order of atomic number

112
Q

What are elements with similar properties placed in?

A

groups

113
Q

What do all elements in the same group have in common?

A

the same number of electrons in the outer shell

114
Q

Where are the metals found in the periodic table?

A

left hand side

115
Q

Where are the non-metals found in the periodic table?

A

right hand side

116
Q

What is an ion?

A

a charged particle

117
Q

What types of ions do metals form?

A

Positive, as they lose electrons to get a full outer shell

118
Q

What types of ions do non-metals form?

A

Negative, as they gain electrons to get a full outer shell

119
Q

What elements are founds in the block of the periodic table between groups 2&3?

A

Transition metals

120
Q

What are the elements in group 0 called?

A

Noble gases

121
Q

Why are Noble gases unreactive/inert

A

As they have a full outer shell

122
Q

What happens to the boiling point of the Noble gases as you go down the group (increase in relative atomic mass)?

A

Increases

123
Q

What are the elements in group 1 called?

A

alkali metals

124
Q

How many electrons do all group 1 elements have in their outer shell?

A

1

125
Q

What are the elements in group 7 called?

A

Halogens

126
Q

How many electrons do all group 7 elements have in their outer shell?

A

7

127
Q

What state is chlorine at room temperature and its colour?

A

yellow/green gas

128
Q

What is the charge on a halide ion?

A

-1

129
Q

What sort of compounds do halogens form with other non metals?

A

covalent

130
Q

How many elements are present in H2S04?

A

3

131
Q

Describe how magnesium and oxygen form an ionic bond

A

Magnesium loses 2 electrons and Oxygen gains 2 electrons

132
Q

What are the properties of diamond?

A

Cannot conduct electricity and has high melting points/ high boiling points

133
Q

Why does diamond have a high melting point?

A

Require lots of energy to overcome strong covalent bonds between the atoms

134
Q

Why can diamond not conduct electricity?

A

No ions or delocalised electrons

135
Q

Describe the structure and bonding in diamond

A

Giant lattice structure and strong covalent bonds between atoms

136
Q

What are the properties of graphite?

A

Can conduct electricity, soft & slippery and high melting points/ high boiling points

137
Q

Why does graphite have a high melting point?

A

Strong covalent bonds between the atoms and require lots of energy to overcome

138
Q

Why can graphite conduct electricity?

A

Contains delocalised electrons able to move and carry a charge through structure

139
Q

How many atoms are present in H2SO4?

A

7

140
Q

What is the atomic mass (Ar)?

A

Top number on the periodic table

141
Q

What is the relative formula mass (Mr)?

A

Sum of the relative atomic masses of the atoms in the formula

142
Q

What is the law of conservation of mass

A

No atoms are lost or made during a chemical reaction so the mass of the products equals the mass as the reactants

143
Q

How do the relative formula masses of the reactants compare to the products?

A

they are equal

144
Q

Why could the mass of products be less than the mass of the reactants?

A

A gas is made which can escape

145
Q

Why could the mass of products be more than the mass of the reactants?

A

When a gas is added to a reactant

146
Q

What is concentration measured in?

A

Grams per decimetre cubed (g/dm3)

147
Q

How do you calculate concentration?

A

concentration = mass ÷ volume

148
Q

What units does mass have to be in when calculating concentration?

A

grams (g)

149
Q

What units does volume have to be in when calculating concentration?

A

decimetre cubed, dm3

150
Q

How do you convert cm3 to dm3?

A

÷ by 1000

151
Q

What is the balanced equation for photosynthesis?

A

6CO2 + 6H2O –> C6H12O6 + 6O2

152
Q

What useful substances have been formed as carbon dioxide decreased? (l,c,n)

A

Limestone, crude oil, natural gas

153
Q

What type of gas maintains the temperature on earth to be high enough to support life?

A

Greenhouse gases

154
Q

What greenhouse gases are increased due to human activity?

A

Carbon dioxide and methane

155
Q

What human activities are increasing the level of carbon dioxide and methane?

A

Farming cattle, rice paddy fields, landfill sites

156
Q

What do scientists believe human activity will do to the temperature of the earth?

A

Increase it, leading to climate change

157
Q

What does uncertainty mean?

A

the interval within which the true value of a quantity can be expected to lie

158
Q

What is crystallisation?

A

A way to separate a dissolved solid from a solution by evaporation to leave crystals of the solid

159
Q

A method used to separate two or more liquids?

A

fractional distillation

160
Q

What theory is given for the earth’s early atmosphere

A

First billion years gave rise to volcanic activity and released gases and water vapour condensed to form oceans

161
Q

What planets is the earth’s early atmosphere suggested to be like

A

Mars and Venus, consisting mainly of carbon dioxide and little or no oxygen

Chemistry (6 decks)

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