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GCSE Combined Science > Chemistry Paper 1 > Flashcards

Chemistry Paper 1 Flashcards

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1
Q

What is an atom?

A

The smallest part of an element that can exist

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2
Q

What is an element?

A

A substance made of only one type of atom

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3
Q

What is a compound?

A

A substance made of two or more different atoms chemically bonded together

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4
Q

How are compounds formed?

A

From chemical reactions

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5
Q

What is involved in a chemical reaction?

A

The formation of one or more new substances and an energy change

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6
Q

What is a molecule?

A

A substance made of more than one atom chemically bonded together

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7
Q

What is a mixture?

A

A substance made of more than one thing not chemically bonded together

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8
Q

How can mixtures be separated?

A

Physical processes (filtration, crystallisation, simple distillation, fractional distillation and chromatography)

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9
Q

Name three subatomic particles

A

Protons, neutrons, electrons

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10
Q

State the relative masses and charges of the subatomic particles

A

Mass: Protons: 1, neutrons: 1, electrons: 0.
Charge: Protons: +1, neutrons: 0, electrons: -1

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11
Q

What is the plum pudding model of the atom?

A

A ball of positively charge with negative electrons stubbed into it

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12
Q

What did the gold foil experiment (alpha particle scattering) prove?

A

The atoms have a dense nucleus with a positive charge

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13
Q

What did Chadwich discover?

A

The neutron

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14
Q

What did Bohr’s experiments show?

A

That electrons are in specific shells

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15
Q

What is the atomic number of an atom?

A

The number of protons in an atom

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16
Q

What is the mass number of an atom?

A

The number of protons + the number of neutrons in an atom

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17
Q

In the electron shell model, how are the subatomic particles arranged in an atom?

A

Protons and neutrons in the nucleus, electron orbiting in shells

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18
Q

Why is the number of electrons in an atom equal to the number of protons?

A

As their charges cancel out

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19
Q

How many electrons can go in the first shell?

A

2

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20
Q

How many electrons can go in the second and third shell?

A

8

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21
Q

What are the groups in the periodic table?

A

The columns, numbered 1, 2, 3, 4, 5, 6, 7, 0

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22
Q

What can the group tell you about the electrons in an atom?

A

How many electrons in the outer shell. E.g. carbon is in group 4 so has 4 electrons in the outer shell

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23
Q

What are the periods in the periodic table?

A

The rows in the periodic table

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24
Q

What can the period tell you about the electrons in an atom?

A

How many shells an atom has. E.g. carbon is in the second period so has two shells

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25
Q

Why do atoms have no overall charge?

A

The number of electrons and protons are equal

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26
Q

Approximately how large are atoms?

A

Radius is about 0.1nm

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27
Q

How large is the nucleus compared to the whole atom?

A

About 1/10,000 the size

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28
Q

What are isotopes?

A

Atoms of the same element with a different number of neutrons

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29
Q

What is abundance?

A

The % of atoms in a sample with a particular mass

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30
Q

What is the relative atomic mass of an element?

A

An average value for the mass that takes account of the abundance of the isotopes of the element

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31
Q

In the modern periodic table, how are the atoms arranged?

A

By their atomic number and in groups according to chemical properties

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32
Q

Why do elements in the same group have similar chemical properties?

A

Because they have the same number of electrons in their outer shell

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33
Q

Before the discovery of protons, neutrons and electrons, how did scientists organise elements?

A

By their atomic weight

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34
Q

Why did Mendeleev leave gaps in his periodic table?

A

For elements that had not yet been discovered

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35
Q

Which discovery meant that organising elements by their atomic weight was not always correct?

A

Isotopes

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36
Q

Where are metals on the periodic table found?

A

To the left and bottom of the periodic table

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37
Q

What is an ion?

A

An atom which has lost or gained electrons

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38
Q

What kinds of ions do metals and non-metals form?

A

Metals form positive, non-metals form negative

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39
Q

What name is given to the group 0 elements?

A

Noble gases

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40
Q

Why are the group 0 elements unreactive?

A

They have full outer shells so do not need to lose or gain electrons

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41
Q

How does the boiling point of group 0 elements change down the group?

A

Increases down the group

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42
Q

Explain why the group 1 elements are called alkali metals?

A

They are metals that form alkalis when they react with water

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43
Q

What are the products of the alkali metals in a reaction with oxygen, water, halogen?

A

Oxygen: metal oxide
Water: metal hydroxide + hydrogen
Halogen: metal halide

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44
Q

Explain why the group 1 elements get more reactive down the group

A

More electrons, more shielding, weaker electrostatic attraction from the nucleus to the outer shell, easier to lose an electron

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45
Q

What is the name given to elements in group 7?

A

Halogens

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46
Q

How does the boiling point of group 7 elements change down the group?

A

Increases down the group

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47
Q

Explain why the group 7 elements get less reactive down the group

A

More electrons, more shielding, weaker electrostatic attraction from the nucleus to the outer shell, harder to gain an electron

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48
Q

What is a displacement reaction?

A

Where a more reactive element displaces a less reactive one from a compound

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49
Q

What are the three types of bond?

A

Covalent, ionic and metallic

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50
Q

What happens to the electrons in an ionic bond?

A

They are transferred

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51
Q

If an atom has gained electrons, what charge will it have as an ion?

A

Negative

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52
Q

If an atom has lost electrons, what charge will it have has an ion?

A

Positive

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53
Q

What type of elements will form ionic bonds?

A

Metal + non-metal

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54
Q

What is the charge on elements from group one and two?

A

Group 1: 1+, group 2: 2+

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55
Q

What is the charge on elements from group six and seven?

A

Group 6: 2-, group 7:1-

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56
Q

Describe the structure and bonding in an ionic compound

A

Giant ionic lattice held together by strong electrostatic force of attraction between positive and negative ions

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57
Q

State the melting and boiling points of ionic compounds

A

High

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58
Q

Explain the melting and boiling points of ionic compounds

A

High due to strong electrostatic forces of attraction which require a lot of energy to break

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59
Q

Explain why ionic compounds do not conduct electricity when solid

A

The ions are not free to move and carry charge

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60
Q

Explain why ionic compounds conduct electricity when molten or in solution

A

The ions are free to move and carry charge

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61
Q

What happens to the electrons in a covalent bond?

A

They are shared

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62
Q

What type of elements will form covalent bonds?

A

Non-metal + non-metal

63
Q

What two types of substance have covalent bonds?

A

Giant covalent substances and small molecules

64
Q

How many bonds does each carbon have in diamond?

A

4

65
Q

Explain why diamond and silicon dioxide have high melting points

A

Giant structures, strong covalent bonds between the atoms, requires a lot of energy to break

66
Q

Explain why most covalent substances do not conduct electricity

A

There are no electrons or ions that are free to move and carry charge

67
Q

Making full reference to structure and bonding in graphite, explain how it conducts electricity

A

Each carbon has 3 bonds, 1 electron is delocalised and therefore free to carry charge through the graphite

68
Q

Explain why graphite can act as a lubricant

A

Weak forces between layers which are free to slide over each other

69
Q

What type of substance are methane and water?

A

Small molecules

70
Q

Describe the structure of small molecules

A

Strong covalent bonds between atoms, weak intermolecular forces holding the molecules together

71
Q

Explain why small molecules have low melting points

A

It is a simple molecular substance with weak forces between the molecules (which are easy to break)

72
Q

What is a polymer?

A

Millions of small molecules joined together in a chain to form a large molecule

73
Q

Why do larger molecules have higher melting points than smaller ones?

A

Intermolecular force strengthens with increased molecule size

74
Q

What is graphene?

A

One layer of graphite

75
Q

What is graphene used for?

A

Electronics and composite materials

76
Q

What is fullerene?

A

Substance made of carbon atoms arranged in a cage

77
Q

What are nanotubes?

A

Cylindrical fullerenes

78
Q

What are nanotubes used for?

A

Electronics, nanotechnology and materials

79
Q

What is the conservation of mass?

A

That atoms cannot be created or destroyed

80
Q

When a metal forms a metal oxide, why does the mass increase?

A

Because oxygen atoms have been added

81
Q

When an acid reacts with a metal, why does the mass decrease?

A

Because a gas is produced and escapes

82
Q

What is relative formula mass?

A

The sum of the relative masses of each atom in a compound

83
Q

What are the four state symbols and what do they stand for?

A

(s) solid (l) liquid (g) gas (aq) aqueous

84
Q

What symbol do we use for relative formula mass?

A

Mr

85
Q

(HT) What is a mole?

A

A number of particles

86
Q

(HT) What is Avogadro’s number?

A

6.022x1023

87
Q

(HT) What formula relates moles, mass and Mr?

A

Mass = Mr x Moles

88
Q

(HT) What is a limiting reactant?

A

A reactant that does not have enough mass to react with all the product

89
Q

What is the unit for concentration?

A

g/dm3

90
Q

Which formula relates concentration, mass and volume?

A

concentration = mass/volume

91
Q

What is the reactivity series?

A

A list of elements ordered by their reactivity

92
Q

How can metals be placed in order of their reactivity?

A

Add the metals to water or acid and see which ones react the most vigorously

93
Q

What is the name for a reaction where oxygen is removed from a compound?

A

Reduction

94
Q

Why is gold found in the Earth’s crust as the metal itself?

A

It is unreactive

95
Q

What process is used to extract metals less reactive than carbon?

A

Reduction with carbon

96
Q

What process is used to extract metals more reactive than carbon?

A

Electrolysis

97
Q

What is an ore?

A

A material containing enough metal in it for it to be economically worthwhile to extract the metal.

98
Q

What is a displacement reaction?

A

A reaction in which a more reactive element takes the place of a less reactive element in one of its compounds or in solution

99
Q

Define oxidation in the context of loss and gain of electrons

A

Oxidation is the loss of electrons

100
Q

Define reduction in the context of loss and gain of electrons

A

Reduction is the gain of electrons

101
Q

Define acid in terms of pH

A

A substance with a pH of less than 7

102
Q

Define acids in terms of ions

A

A substance which releases H+ ions in solution

103
Q

State the three common acids and give their formulae

A

Hydrochloric acid, HCl(aq), Sulphuric acid, H2SO4 (aq), Nitric acid, HNO3;

104
Q

Which ions do the common acids form in solution?

A

HCI forms H+ and CI-, H2SO4 forms 2H+ and SO42-, HNO3, forms H+ and NO3-

105
Q

What is a neutral solution?

A

A solution with a pH of 7. Water is an example

106
Q

How do you measure pH?

A

With an indicator or pH probe

107
Q

What is a base?

A

A metal oxide, hydroxide or carbonate that will react with an acid. E.g. copper oxide

108
Q

What is an alkali?

A

A soluble base. E.g. sodium hydroxide

109
Q

Which ions are always present in a solution of an alkali?

A

OH-

110
Q

What is a salt?

A

A compound formed when some or all of the hydrogen from an acid is replaced by a metal

111
Q

What type of salts are formed by the three main acids?

A

Hydrochloric acid produces chlorides, sulphuric acid = sulphates, nitric acid = nitrates

112
Q

What is a neutralisation reaction?

A

A reaction involving an acid that results in a neutral solution

113
Q

Which ions always react together in a neutralization reactions between acids and alkalis?

A

H+ and OH-

114
Q

Write the equation showing the reaction between H+ and OH- ions

A

Н+ + OH- -> H2O

115
Q

Complete the equation:
metal + acid

A

-> salt + hydrogen gas

116
Q

Complete the equation:
metal hydroxide + acid

A

-> salt + water

117
Q

Complete the equation:
metal oxide + acid

A

-> salt + water

118
Q

Complete the equation:
metal carbonate + acid

A

-> salt + water + carbon dioxide

119
Q

How do you make a soluble salt from an acid?

A

React the acid with a base. E.g. to make copper sulphate react copper oxide with sulphuric acid

120
Q

If a salt is in solution, how do you extract it as a solid?

A

Allow the water to evaporate and it will leave the salt behind as a solid (crystallisation)

121
Q

What is a strong acid?

A

An acid which completely splits up into its ions in water. E.g. when HCl is in water all the HCI molecules split up into H* and CI-

122
Q

What is a weak acid?

A

An acid which will have some molecules which do not split up into their ions.
E.g. in ethanoic acid only some of the molecules will have split up into the ethanoate ion and H* ions.

123
Q

What is the relationship between the strength of an acid and its pH?

A

As an acid increases in strength the pH decreases.

124
Q

What is a concentrated acid?

A

An acid where there are lots of acid particles in the water.

125
Q

What is a dilute acid?

A

An acid where there are fewer acid particles in the water.

126
Q

How does pH depend on the concentration of H+ in a solution?

A

As the concentration of H* increases by a factor of ten, the pH decreases by one

127
Q

What is electrolysis?

A

Using electricity to produce elements from an ionic compound

128
Q

What is an electrolyte?

A

A liquid or aqueous ionic compound

129
Q

What is the name for the positive electrode?

A

The anode

130
Q

What is the name for the negative electrode?

A

The cathode

131
Q

Do positive ions move to the anode or the cathode?

A

Cathode

132
Q

Do negative ions move to the anode or the cathode?

A

Anode

133
Q

What are the two main disadvantages of using electrolysis to extract metals?

A

Requires a large amount of energy to melt the compounds and to produce the necessary electricity

134
Q

Why is aluminium oxide mixed with cryolite when extracting aluminium?

A

To lower the melting point

135
Q

What is produced at the anode and cathode in the electrolysis of aluminium oxide?

A

Aluminium at the cathode and oxygen at the anode

136
Q

Why does the anode need to be replaced in the electrolysis of aluminium oxide?

A

The oxygen reacts with the carbon electrode to produce carbon dioxide.

137
Q

For a simple ionic liquid, where is the metal produced?

A

Cathode

138
Q

For a simple ionic liquid, where is the non-metal produced?

A

Anode

139
Q

In the electrolysis of an ionic solution, when will hydrogen be produced?

A

If it is more reactive than hydrogen

140
Q

In the electrolysis of an ionic solution, when will oxygen be produced?

A

If the non-metal is not a halogen

141
Q

What can happen to water molecules in the electrolysis of solutions?

A

They break down into hydrogen and hydroxide ions

142
Q

What is a half equation?

A

An equation which shows electron transfer at one of the electrodes

143
Q

State the law of conservation of energy.

A

Energy cannot be created or destroyed, it can only transferred from one place to another.

144
Q

What is an exothermic reaction?

A

A reaction where energy is transferred to the surroundings.

145
Q

Give two examples of exothermic reactions.

A

Combustion, respiration

146
Q

What happens to the temperature of the surroundings during an exothermic reaction?

A

Increases

147
Q

What is an endothermic reaction?

A

A reaction where energy is transferred from the surroundings.

148
Q

Give two examples of endothermic reactions.

A

Thermal decomposition reactions, citric acid and sodium hydrogencarbonate.

149
Q

What happens to the temperature of the surroundings during an endothermic reaction?

A

Decreases

150
Q

State two uses of exothermic reactions

A

Self-heating cans, hand warmers

151
Q

State two uses of endothermic reactions

A

Some cooling sports injury packs

152
Q

What is a reaction profile?

A

A diagram which shows whether the reactants have more or less energy than the products.

153
Q

(HT) State which of bond breaking and bond making is endothermic and which is exothermic

A

Breaking: exothermic, making: endothermic

154
Q

(HT) How do we work out the overall energy change of a reaction?

A

Work out the difference between the energy needed to break all the bonds the reactants and the energy release to form all the bonds in the products.

GCSE Combined Science (6 decks)

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