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Science > Chemistry paper 1 c1-7 > Flashcards

Chemistry paper 1 c1-7 Flashcards

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1
Q

Name the 3 subatomic particles

A

Protons, neutrons, electrons

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2
Q

Name the 2 subatomic particles in the nucleus

A

Protons and neutrons

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3
Q

Give the location of electrons in the atom

A

Orbiting the nucleus in shells

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4
Q

Give the maximum number of electrons in the first shell

A

Maximum of 2

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5
Q

Give the maximum number of electrons in the second and third shells

A

Maximum of 8

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6
Q

Give the charge of a proton

A

Positive (+1)

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7
Q

Give the charge of a neutron

A

Neutral (0)

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8
Q

Give the charge of an electron

A

Negative (-1)

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9
Q

Explain why the overall charge of an atom is zero

A

Same number of protons and electrons

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10
Q

Define an atom

A

Smallest particle that makes up all matter

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11
Q

Define an element

A

Substances made from only one type of atom

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12
Q

Define a compound

A

Substances made from two or more types of atoms bonded together

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13
Q

Define a mixture

A

Groups of atoms, elements and compounds that are mixed but not bonded

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14
Q

Define an ion

A

Charged particle formed when an atom has lost or gained electrons

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15
Q

Define an isotopes

A

Atoms of the same element (same number of protons) with a different number of neutrons

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16
Q

Name the process to separate two liquids

A

Distillation

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17
Q

Name the process to separate an insoluble solid from a liquid

A

Filtration

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18
Q

Name the process to separate a soluble solid from a liquid

A

Crystallisation

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19
Q

Name the four scientists involved in the development of the periodic table

A

John Dalton, John Newlands, Dimitri Mendeleev, Henry Moseley

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20
Q

Describe the contribution of Dalton to develop the periodic table

A

Ordered elements based on their atomic mass

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21
Q

Describe the contribution of Newlands to develop the periodic table

A

Kept atomic mass. Discovered a repeating pattern every 8th element

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22
Q

Describe the contribution of Mendeleev to develop the periodic table

A

Switched positions of elements that did not fit patterns. Left gaps for undiscovered elements

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23
Q

Describe the contribution of Moseley to develop the periodic table

A

Ordered elements based on the number of protons they had

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24
Q

Give the properties of alkali metals

A

Very reactive, low melting/boiling points, react vigorously with water and halogens

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25
Q

Give the properties of the halogens

A

Low melting/boiling points, poor conductors of heat/electricity, toxic, react with alkali metals

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26
Q

Give the properties of noble gases

A

Very unreactive, stable, full outer shell, exist as single atoms

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27
Q

Identify the pattern of reactivity in group 1 (Alkali metals)

A

The Alkali metals become more reactive as you go down the periodic table

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28
Q

Identify the pattern of reactivity in group 7 (Halogens)

A

The Halogens become less reactive as you go down the periodic table

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29
Q

Give the word equation for the reaction between an alkali metal and water

A

Alkali metal + water → Alkali metal hydroxide + hydrogen

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30
Q

Define a displacement reaction

A

When a more reactive element takes the place of a less reactive element in a compound

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31
Q

List the three types of bonding

A

Ionic, covalent, metallic

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32
Q

State the type of bonding that occurs between metals

A

Metallic

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33
Q

State the type of bonding that occurs between non-metals

A

Covalent

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34
Q

State the type of bonding that occurs between metals and non-metals

A

Ionic

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35
Q

Describe what happens in ionic bonding

A

Electrons are lost or gained

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36
Q

Describe what happens during covalent bonding

A

Electrons are shared

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37
Q

List the properties of solids

A

Fixed shape, fixed volume, cannot be compressed, particles arranged in rows, particles vibrate in fixed positions

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38
Q

List the properties of liquids

A

Can change shape, fixed volume, cannot be compressed, particles not arranged in rows, particles can slide past each other

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39
Q

List the properties of gases

A

Can change shape, can change volume, can be compressed, particles arranged randomly, particles move freely in all directions

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40
Q

Describe the properties of ionic compounds

A

High melting and boiling points, conducts electricity when molten/dissolved, brittle

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41
Q

Give the structure that ionic compounds form

A

Giant lattices

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42
Q

Explain why ionic compounds have high melting/boiling points

A

Strong electrostatic forces between oppositely charged ions, lots of energy needed to overcome them

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43
Q

Explain why simple covalent molecules have low melting/boiling points

A

Weak intermolecular forces between molecules, these are easily overcome

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44
Q

State the material that diamond, graphene and graphite are made from

A

Carbon atoms

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45
Q

List the properties of diamond

A

Hard, strong, cannot conduct electricity

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46
Q

Explain why diamond is hard and strong

A

Forms 4 covalent bonds per atom. This is the max number of bonds. Lots of energy required to break them

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47
Q

Describe the structure of Graphene

A

2D sheet of carbon atoms arranged in hexagons

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48
Q

Describe the structure of graphite

A

3D structure made from multiple graphene layers

49
Q

List the properties of graphite

A

Soft, brittle, can conduct electricity, 3D

50
Q

Explain why graphite is soft

A

Graphite has layers. There are weak forces between layers. These layers can slide over each other

51
Q

Explain why graphite can conduct electricity

A

Only forms 3 bonds per atom. This means there is 1 spare electron that can conduct electricity

52
Q

List the properties of metals

A

High melting/boiling points, conduct electricity, malleable

53
Q

Describe the structure of metals

A

Positive metal ions. A sea of delocalised electrons. Strong electrostatic forces between them

54
Q

Define atomic number

A

The number of protons in the nucleus of an atom

55
Q

Define mass number

A

The number of protons PLUS the number of neutrons

56
Q

Define isotope

A

Isotopes have the same number of protons but a different number of neutrons

57
Q

Define relative formula mass

A

The mass of a molecule

58
Q

Describe how to calculate relative formula mass

A

Add up all the relative atomic masses of each atom in the molecule

59
Q

State how to calculate % by mass

A

(Ar of the element / Mr of the compound) x 100

60
Q

State the equation for calculating concentration

A

Concentration = mass / volume

61
Q

State the units for concentration

A

g/dm3

62
Q

Describe how to convert from cm3 to dm3

A

Divide by 1000

63
Q

Describe how to convert from dm3 to cm3

A

Times by 1000

64
Q

Define the reactivity series

A

List of metals in order of reactivity

65
Q

Name the metals that can be extracted using carbon

A

Zinc, iron, tin, lead, copper, silver, gold, platinum

66
Q

Name the metals that can only be extracted using electrolysis

A

Potassium, sodium, calcium, magnesium, aluminium

67
Q

Define displacement reaction

A

When a more reactive metal takes the place of a less reactive metal

68
Q

Give the general word equation for the reaction between a metal and oxygen

A

Metal + Oxygen → Metal oxide

69
Q

Give the general word equation for the reaction between a metal and acid

A

Metal + acid → salt + hydrogen

70
Q

Give the general word equation for the reaction between a metal oxide and carbon

A

Metal oxide + carbon → Metal + carbon dioxide

71
Q

Give the general word equation for the reaction between an acid and a base

A

Acid + base → Salt + water

72
Q

Give the general word equation for the reaction between a metal carbonate and acid

A

Metal carbonate + acid → Salt + water + carbon dioxide

73
Q

Give the general word equation for the reaction between a metal and water

A

Metal + water → Metal hydroxide + hydrogen

74
Q

Name the salt produced by hydrochloric acid

A

Metal chloride

75
Q

Name the salt produced by sulphuric acid

A

Metal sulphate

76
Q

Name the salt produced by nitric acid

A

Metal nitrate

77
Q

Define an ore

A

A rock that contains enough metal atoms to make extracting them commercially viable

78
Q

Define oxidation

A

Gain of oxygen, loss of electrons

79
Q

Define reduction

A

Loss of oxygen, gain of electrons

80
Q

Define salt

A

An ionic compound with no overall charge

81
Q

Which ion makes a substance acidic?

A

H+

82
Q

Which ion makes a substance alkaline?

A

OH-

83
Q

Define a base

A

Chemicals capable of neutralising acids

84
Q

Give three examples of bases

A

Metal oxides, Metal hydroxides, Metal carbonates

85
Q

Define an alkali

A

Soluble base

86
Q

Define electrolysis

A

Splitting a compound using electricity

87
Q

State the states of matter required for electrolysis to take place

A

Molten (melted) or aqueous (dissolved in water)

88
Q

Explain why electrolysis works with molten/aqueous compounds

A

Ions are free to move towards the electrodes

89
Q

Explain why electrolysis won’t work if the compound is solid

A

Ions are arranged in rows and cannot move towards the electrodes

90
Q

State the type of compounds that can be split by electrolysis

A

Ionic compounds

91
Q

State the types of elements found in ionic compounds

A

Made from a metal and a nonmetal

92
Q

Define ion

A

Charged particle formed when atoms lose or gain electrons

93
Q

State the type of element that forms cations

A

Metals

94
Q

State the type of element that forms anions

A

Non-metals

95
Q

State the name of the positive electrode

A

Anode

96
Q

State the name of the negative electrode

A

Cathode

97
Q

Explain which ions are attracted to the anode

A

Anions, since they are negatively charged and attracted to the positively charged anode

98
Q

Explain which ions are attracted to the cathode

A

Cations, since they are positively charged and attracted to the negatively charged cathode

99
Q

Explain what happens to ions at the anode

A

Anions lose electrons to become atoms. They are oxidised

100
Q

Explain what happens to ions at the cathode

A

Cations gain electrons to become atoms. They are reduced

101
Q

Explain why cryolite is used in the electrolysis of aluminium oxide to make aluminium

A

Cryolite reduces the melting point of aluminium oxide so less energy is needed to melt it

102
Q

Explain why the anodes need constant replacing in the extraction of aluminium

A

The anodes are made of graphite. This reacts with the oxygen produced at the anode, forming carbon dioxide gas

103
Q

State which ions are contributed by water in solutions of ionic compounds

A

Hydrogen ion H+, Hydroxide ion OH-

104
Q

Explain how the product produced at the cathode during electrolysis of solutions is determined

A

If the metal ion from the ionic compound is more reactive than hydrogen, then hydrogen is formed. If it is less reactive, then the metal is formed

105
Q

Explain how the product produced at the anode during electrolysis of solutions is determined

A

If the anion is a halide ion (chloride, bromide, iodide), then the halogen (chlorine, bromine, iodine) is produced. If the anion is anything else (e.g. sulfate, nitrate) then oxygen is produced

106
Q

Explain how a third product of electrolysis of solutions can be made

A

The ions that are left behind in the solution following electrolysis form a third product

107
Q

Define an exothermic reaction

A

An exothermic reaction is one that transfers energy from the reacting chemicals to the surrounding area

108
Q

Define an endothermic reaction

A

An endothermic reaction is one that transfers energy from the surrounding area to the reacting chemicals

109
Q

Define activation energy

A

The minimum energy needed for a reaction to take place

110
Q

Define bond energy

A

The energy required to break a specific chemical bond

111
Q

Define a reaction profile

A

The relative difference in the energy of reactants and products

112
Q

Give the charge for an endothermic reaction in bond energy

A

positive

113
Q

Give the charge for an exothermic reaction in bond energy

A

Positive

114
Q

Give the reaction type when the energy of the products is lower than the energy of the reactants

A

Exothermic

115
Q

Give the reaction type when the energy of the products is higher than the energy of the reactants

A

Endothermic

116
Q

Give an example of an exothermic reaction

A

Fireworks, combustion, self heating cans, hand warmers

117
Q

Give an example of an endothermic reaction

A

Thermal decomposition, ice packs

118
Q

Identify if making bonds is exothermic or endothermic

A

Exothermic

119
Q

Identify if breaking bonds is exothermic or endothermic

A

Endothermic

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