Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry Mock exam > Chemistry Mock exam Paper one > Flashcards

Chemistry Mock exam Paper one Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

In a periodic table where are metals and non- metals

A

Metals are on the left hand side and non- metals are on the right

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Compound

A

A substance that contains two or more atoms which have been bonded together in a chemical reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

An ion

A

A charged particle formed when an atom, or a group of atoms lose or gain their electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Reactants

A

Substances that react together in a chemical reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Products

A

They join the atoms back in a different way to form products

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Solid closeness of particles

A

Very close

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Liquid closeness of particles

A

Close

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Gas closeness of particles

A

Far away

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Solid arrangement of particles

A

Regular pattern

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Liquid arrangement of particles

A

Randomly arranged

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Gas arrangement of particles

A

Randomly arranged

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Solid movement of particles

A

Vibrate around a fixed position

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Liquid movement of particles

A

Move around eachother

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Gas movement of particles

A

Move quickly in all directions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Solid energy of particles

A

low energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

liquid energy of particles

A

Greater energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Gas energy of particles

A

Highest energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Evaporation

A

Particles leave a liquid from its surface only, They rise to the surface and escape to the surroundings, forming a gas.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Condensation

A

Condensation is the change of the physical state of matter from gas phase into liquid phase, and is the reverse of vapourisation. The word most often refers to the water cycle.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Atoms’ nucleus

A

Atoms contain a nucleus which contains protons and neutrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

The electrons

A

Move around the nucleus in electrons shells

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Electron’s charge

A

Electrons charge is negative and tiny but they cover up of space.,

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Element

A

A substance made up of atoms that all have the same number of protons in their nucleus

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

isotopes

A

Are different forms of the same element which have the same number of protons but different atomic mass and.a different number of neutrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

relative atomic mass calculation

A

Sum of (isotopes abundance or percentage x isotope mass number divided by sum of all the percentages of all the isotopes

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

Making bonds

A

Involves giving atoms away, taking or sharing electrons- only electrons are involved

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

Compound consisting of non-metal and metal atoms

A

Consists of ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

Ionic bonding

A

The opposite charges of the ion means that if they’re strongly attracted to eachother

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

Non metal compound

A

Consists of molecules

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

Covalent bonding

A

Each atom shares an electrons with another atom

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

Filtration

A

Can be used if your product is an insoluble solid that needs to be separated from a liquid reaction mixture- also be used for purification of water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

Crystallisation

A

Pour the solution into an evaporating dish and gently heat the solution. Some of the solvent will evaporate and the solution will get more concentrated

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

Distilisation

A

Distilisation is used to separate mixtures which contain liquids- simple and fractional

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

Simple distillation

A

Used to separate out a liquid from its solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

Fractional distillation

A

If youve got a mixture of liquids you can separate it

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

Plum pudding model Person

A

JJ Thompson concluded form his experiments that atoms weren’t solid spheres measurements of charge and mass showed that an atom must contain even smaller.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
37
Q

Plum Pudding model

A

Showed the atom as a ball of positive charge with electrons stuck in it

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
38
Q

Nucleus model

A

Tiny, positively charged nucleus at the centre where most of the mass is concentrated, cloud of negative electrons surround the nucleus- a lot of empty space

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
39
Q

electron shells

A

max number 2, 8, 8

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
40
Q

Mendeleev

A

Put the elements in the order of their atomic mass but didn’t switch that order. Gaps were left to make sure that elements with similar properties stayed in the same groups.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
41
Q

Periodic table arrangement

A

Non-metals are on the right, metals are on the left, order of their increasing atomic number (proton)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
42
Q

Metals

A

Elements which can form positive ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
43
Q

Non metals

A

Don’t generally form positive ions when they react

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
44
Q

Metals to the left electrons’

A

Don’t have many electrons to remove and metals towards the bottom have outer electrons which are a long way from the nucleus- weaker attraction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
45
Q

Non metals’ attraction

A

They have lots of electrons to remove to get a fuller outer Sheller towards the top- electrons are close to the nucleus meaning they have a stronger attraction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
46
Q

Metal’s properties

A

Strong, malleable, good at conducting heat and electricity and have high melting points

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
47
Q

Non-metal’s properties

A

Dull looking, more brittle, aren’t always solids, don’t generally conduct electricity

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
48
Q

transition metals

A

Centre of the periodic table, typical metals have the properties of a normal metal- very dense and shiny.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
49
Q

Transition metals special properties

A

They have more than one ion, often coloured, they also make good catalysts

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
50
Q

Group 1 elements

A

All have one outer electron in their outer shell, makes them very reactive- all soft and have low density

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
51
Q

Increasing reactivity- group 1 elements

A

Outer electron is easily lost as the attraction between the nucleus and electron decreases as the electron is further away from the nucleus

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
52
Q

Group 1 reacting with water

A

React vigourously to produce hydrogen gas, the more reactive down the group the more violent the reaction is

53
Q

Group 1 reacting with chlorine

A

React vigorusly with chlorine gas to from white metal chloride salts

54
Q

Group 1 reacting with oxygen

A

Form a metal oxide.

55
Q

Group 7 elements

A

The halogens, become less reactive, harder to gain an extra electron because the outer shell’s further away from the nucleus

56
Q

group 7 properties

A

Have higher melting points, having higher relative atomic masses

57
Q

Halogens form ionic bonds with metals

A

Form 1-ions called halides

58
Q

Displacement reaction

A

Can occur between a more reactive halogen and the salt of a less reactive one

59
Q

Group 0 elements

A

Called the noble gases, all have eight electrons in their outer energy level.

60
Q

Group 0 electron shell stable

A

Energetically stable don’t have to give up or gain electrons to become more stable- don’t react with a lot

61
Q

Boiling points of group 0

A

The boiling points increase as you go further down the group because of the number of electrons leading to greater intermolecular forces

62
Q

Ions

A

Charged particles they can be single atoms or groups of atoms

63
Q

Atoms with full outer shells

A

They are more stable

64
Q

Metals forming ions

A

They gain electrons and therefore become positive

65
Q

Non metals forming ions

A

They gain electors into their outer shell and become negative

66
Q

Group 1, 2, 6, 7

A

Most likely to form ions

67
Q

Group 1 and 2 elements

A

They are metals and they lose electrons to form positive ions

68
Q

Group 6 and 7 are non-metals

A

They gain electrons to form negative ions

69
Q

Ionic compounds

A

Have a structure called a giant lattice

70
Q

Giant ionic lattice

A

Form a closely packed negative lattice and there are very strong electrostatic forces of attraction between oppositely charged ions in all directions

71
Q

Ionic compound properties

A

Hight melting points, high boiling points due to many strong bonds between the ions- contain a lot of energy

72
Q

Simple molecular substances

A

Made up of molecules containing a few atoms joined together by covalent bonds

73
Q

Polymers

A

Long chains of repeating units

74
Q

Allotropes of carbon

A

Different structual forms of the same element in the same physical state

75
Q

Diamond is very hard

A

Giant covalent structure, each form 4 covalent bonds - doesn’t conduct electricity as it has no free electrons or ions

76
Q

Graphite contains sheets of hexagons

A

In each carbon atom only forms three covalent binds creating sheets of carbon atoms arranged in hexagons

77
Q

electrolysis

A

Electrolysis is the process by which ionic substances are decomposednto simpler substances when an electric current is passed through them. Electricity is the flow of electrons or ions.

78
Q

Accuracy

A

A measurement is considered accurate if it is judged to be close to the true value

79
Q

Precision

A

Precise measurements are ones in which there its very little spread

80
Q

Reactants and products in a chemical equation

A

Reactants go on the left, products go on the right

81
Q

The conservation of mass

A

Mass is near lost or gained, the total mass of products is always equal at the end of the reaction and at the beginning

82
Q

The empirical formula

A

The empirical formula of a compound is the simplest whole number ratio of atoms of each element in the compound.

83
Q

Reacting mass calculations

A

Example: When 12 g of carbon is burned in air, 44 g of carbon dioxide is produced. What mass of carbon is needed to produce 11 g of carbon dioxide?

12 divided by 44
11 x (12 divided by 44)
84
Q

Reacting mass calculations with balanced equations

A

Balance the equation,

unknown mass = known mass ÷ total Mr of known substance × total Mr of unknown substance

85
Q

The Ph scale

A

A meaner of how acidic or alkaline a solution is

86
Q

The lower the Ph is…

A

The more acidic it is

87
Q

The higher the Ph

A

The more alkaline it is

88
Q

A natural substance has

A

PH 7

89
Q

How can you measure the PH of a solution

A

By using an indicator which is a dye changing colour depending on whether its above or below a certain Ph

90
Q

A ph probe

A

Can be used the measure the ph electronically

91
Q

An acid

A

A substance that forms aqueous solutions with a ph of less than 7

92
Q

A base

A

A substance with a ph greater than 7

93
Q

An alkali

A

A base that dissolves in water to form a solution with a ph greater than 7

94
Q

PH 7

A

Neutral

95
Q

Neutralisation

A

The reaction between acids and bases

96
Q

Tiltrations

A

Allow you to find out exactly how much acid Is needed to neutralise a quantity of alkali

97
Q

Equipment used for tiltration

A

Pipette and pipette filller- add a set volume of alkali to the conical flask

98
Q

Strong acids

A

Ionise completely in water

99
Q

Weak acids

A

Do not fully ionise in solution

100
Q

Ionisation of a weak acids

A

Is a reversible reaction

101
Q

If the concentration of H + ions is higher

A

The rate of reaction is faster

102
Q

Strong acids will be more reactive than…

A

Weak acids with the same concentration

103
Q

What is Ph the measure of?

A

the concentration in hydrogen ions

104
Q

For every decrease of 1 on the ph scale

A

Means the concentration of h+ ions increases by a factor of 10

105
Q

Basic equation for the concentration changes

A

Factor. H+ ion concentration changes by = 10- (to the power of whatever concentration for example if ph falls from 7 to 4 the difference is -3– 10-(-3)

106
Q

The reactivity series

A

Lists metals in order of their reactivity towards other substances

107
Q

Metals reactivity

A

Depends by how easily they lose their electrons

108
Q

The higher up the reactivity series..

A

The more positive ions

109
Q

The speed of the reaction is indicated by?

A

By the rate at which the hydrogen bubbles are given off

110
Q

Oxides

A

Common metals react with oxygen

111
Q

reduction

A

The reaction that operates a metal from its oxides called a reduction reaction

112
Q

Oxidation

A

Gain of oxygen

113
Q

Metals can be extracted from their ores using…

A

reduction or carbon

114
Q

oxides and ores

A

Often the ores that the metals need to be extracted from

115
Q

Metals higher than carbon

A

need to be extracted by electrolysis

116
Q

Metals below carbon

A

Need to be extracted through reduction or carbon

117
Q

A loss of electrons

A

Oxidation

118
Q

Gain of electrons

A

Reduction

119
Q

Redox reactions

A

Are displacement reactions

120
Q

A more reactive metal…

A

Will displace a less reactive metal from its compound

121
Q

Metal ion in displacement reactions

A

Metal ions always gain electrons- they are reduced.

122
Q

Metal atom in displacement reactions

A

Always loses the electrons- they oxidise

123
Q

Exothermic

A

Transfers energy to the surroundings, usually by heating- rise in temperature

124
Q

Endothermic

A

One which takes in energy from the surroundings and falls in temperature

125
Q

Bond breaking

A

Endothermic

126
Q

Bond formation

A

exothermic

127
Q

An electrochemical cell

A

Basic system made up of two different electrodes in contact with an electrolyte

128
Q

Electrolyte

A

Is a liquid that contains ions which react with electrodes

129
Q

Fuel cell

A

An electrical cell thats supplied with a fuel and oxygen and uses energy from the reaction between them to produce electrical energy

Chemistry Mock exam (1 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions