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Chemistry > Chemistry GCSE Paper 1 > Flashcards

Chemistry GCSE Paper 1 Flashcards

1
Q

How many different elements are in the periodic table?

A

100

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2
Q

What is a compound?

A

made from 2 or more elements which are combined chemically

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3
Q

What is a molecule?

A

formed when two atoms join together by chemical bonds

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4
Q

How can compounds be seperated into elements?

A

Chemical reactions

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5
Q

What is a mixture?

A

consists of two or more elements not chemically combined together

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6
Q

What is an atom?

A

The smallest particle

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7
Q

What is an Element?

A

made of only one type of atom

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8
Q

What are some examples of physical processes where mixtures can be separated?

A 
Filtration
crystallisation
simple distillation
fractional distillation
chromotography
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9
Q

What does chromatography separate?

A

mixtures which include inks, dyes and colouring agents in food

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10
Q

What does filtration separate?

A

Separates a solid that can dissolve from one that can’t

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11
Q

What does evaporation separate?

A

separates a liquid and solid by boiling off the liquid

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12
Q

What does distillation separate?

A

Separates liquids with different boiling points

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13
Q

What does the plum pudding model suggest?

A

The atom is a ball of positive charge with negative electrons embedded in it

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14
Q

What did the alpha particle scattering experiment lead to?

A

led to the conclusion that the mass of an atom was concentrated at the centre and that the nucleus was charged. This nuclear model replaced the plum pudding model

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15
Q

What did James Chadwick experimental work suggest?

A

provided the evidence to show the existence of neutrons within the nucleus. This was about 20 years after the nucleus became and accepted scientific idea

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16
Q

Who adapted the nuclear model and what did it suggest?

A

Niels Bohr suggests that electrons orbit the nucleus at specific distances

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17
Q

What did later experiments lead to?

A

led to the idea that the positive charge of any nucleus could be subdivided into a whole number of smaller particles, each particle having the same amount of positive charge. The name proton was given to these particles

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18
Q

What is the relative charge of a proton?

A

+1

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19
Q

What is the relative charge of the neutron?

A

0

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20
Q

What is the relative charge of the Electron?

A

-1

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21
Q

The number of electrons is equal to the number of what in the nucleus?

A

protons

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22
Q

What is the atomic number?

A

number of protons

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23
Q

What is the relative mass of protons?

A

1

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24
Q

What is the relative mass of neutrons?

A

1

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25
Q

What is the relative mass of electrons?

A

very small

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26
Q

What is the mass number?

A

sum of the protons and neutrons in an atom

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27
Q

What is an isotope?

A

element that has the same number of protons but a different number of neutrons

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28
Q

What are the elements in the periodic table ordered in?

A

ordered in atomic number

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29
Q

What are the columns in the periodic table known as?

A

Groups

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30
Q

Why is the table called the periodic table?

A

similar properties occur at regular intervals

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31
Q

Elements in the same group in the periodic table have the same number of what?

A

same number of electrons in their outer shell

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32
Q

How did people attempt to classify elements before the discovery of neutrons protons and electrons?

A

Arranging them in order of their atomic weight

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33
Q

What are the elements in Group 1 called?

A

Alkali metals

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34
Q

What does lithium do when it reacts with water?

A

floats, moves very quickly and fizzes

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35
Q

What does potassium do when it reacts with water?

A

floats, moves quickly, melts and fizzes gas may ignite with an orange flame

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36
Q

What does sodium do when it reacts with water?

A

floats, moves slowly and fizzes

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37
Q

Alkali metals generally become …………………. dense going down the group

A

less

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38
Q

What does caesium do when it reacts with water?

A

explodes almost instantly and breaks the glass container

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39
Q

How does lithium react when burnt?

A

orange flame
red flame
burnt fast
white solid left

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40
Q

How does sodium react when burnt?

A

orange flame
burnt slowly
melted
went silver

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41
Q

How does potassium react when burnt?

A

purple flame
burnt really fast
melted

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42
Q

Is the lithium oxide alkaline or acid?

A

Alkaline

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43
Q

Is the sodium oxide alkaline or acid?

A

Alkaline

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44
Q

Is the potassium oxide alkaline or acid?

A

Alkaline

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45
Q

Elements that react to form positive ions are …

A

metals

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46
Q

Elements that do not form positive ions are ….

A

non - metals

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47
Q

Majority of elements are …

A

metals

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48
Q

Where are metals found on the periodic table?

A

left and towards the bottom of the periodic table

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49
Q

Where are non metals found on the periodic table?

A

towards the right and top of the periodic table

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50
Q

What are the elements in group 0 called?

A

noble gases

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51
Q

Why are noble gases used for lights?

A

they don’t mix and are unreactive. They are also less dangerous then other gases

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52
Q

Why are noble gases unreactive?

A

have a dull outer shell of electrons

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53
Q

Do the atoms get smaller or bigger further down the group 0?

A

bigger

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54
Q

Does the boiling point increase or decrease the further down group 0?

A

Increases

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55
Q

Does the density of the atom decreases or increase as you go down group 0 and why?

A

increase because larger atoms take up more space so it makes it a stable element

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56
Q

What are the elements in Group 1 called?

A

Alkali metals

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57
Q

Does the reactivity of the elements in group 1 increase or decrease going down the group?

A

increase

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58
Q

What are the elements in Group 7 called?

A

halogens

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59
Q

What are halogens?

A

non metals and consist of molecules made of pair of atoms

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60
Q

When does ionic bonding occur?

A

Occurs in compounds formed from metals combined with non metals

61
Q

When does covalent bonding occur?

A

occurs in most non metallic elements and in compounds of non metals

62
Q

Where does metallic bonding occur?

A

occurs in metallic elements and alloys

63
Q

What happens during ionic bonding?

A

metal atoms lose electrons to become positively charges and non metals gain electrons

64
Q

What is an ionic compound?

A

Giant structure of ions

65
Q

How are ionic compounds held together?

A

strong electrostactic forces of attraction between oppositely charged ion

66
Q

What is covalent bonding?

A

when atoms share pairs of electrons

67
Q

The bonds between atoms are…..

A

strong

68
Q

What are diamond and silicon dioxide?

A

giant covalent structures

69
Q

What are polymers?

A

covalently bonded substances which have very large molecules

70
Q

What does metals consist of?

A

giant structures of atoms arranged in a regular pattern

71
Q

What are the electrons like in the outer shell of a metal atom?

A

delocalised and are free to move through the whole structure

72
Q

What does the sharing of delocalised electrons do?

A

gives rise to strong metallic bonds

73
Q

What is giant tetrohedral?

A

each carbon bonded to four others

74
Q

What is graphite?

A

giant hexagonal layer. each carbon makes only three bonds to other carbon

75
Q

Why does diamond have a high melting point?

A

have strong covalent bond

giant covalent bond

76
Q

Why does graphite conduct electricity?

A

it contain delocalised elctrons

carbon is only bonded to three other carbons

77
Q

Why can graphite be used in the leads of pencils?

A

layers slip easy

weak intomellecular forces

78
Q

How are gas particles arranged?

A

randomly placed and they move around freely

79
Q

How are liquid particles arranged?

A

The particles are place near each other but not that close that they touch

80
Q

How are solid particles arranged?

A

Placed in neat rows they vibrate against each other

81
Q

What are the structures like for ionic compounds and how does this affects the melting point and boiling point?

A

regular structures in which they have strong electrostatic forces of attractions. They have high melting point and high boiling points because of the large amount of energy needed to break the many strong bonds

82
Q

Which substances usually consist of small molecules?

A

gases

liquids

83
Q

Which ones weaker intermolecular forces or covalent bonds?

A

intermolecularr

84
Q

What are polymers like?

A

very large molecules. the atoms are linked to other atoms by strong covalent bonds. The intermollecular forces between molecules are relatively strong so are solid at room temperature

85
Q

What is the state of giant covalent structures and what is the melting point like?

A

solids

very high melting points

86
Q

What are the bonds like in giant covalent structures?

A

strong covalent bonds

87
Q

What are the bonds in metals?

A

ginat structures with strong metallic bonding

88
Q

How are the atoms arranged in pure metals?

A

arranged in layers which allows metals to be bent and shaped

89
Q

What are alloys?

A

pure metals mixed with other metals

90
Q

Why are metals good conductors of electricity?

A

declocalised electrons in the metal carry electrical charge through the metal

91
Q

Whys are metals good conductors of thermal energy?

A

energy is transferred by the delocalised electrons

92
Q

What is graphene?

A

a single layer of graphite

93
Q

What are fullerenes?

A

molecules of carbon atoms with hollow shapes

94
Q

What shape is the structures of fullerenes like?

A

hexagonal rings of carbon atoms

95
Q

What are carbon nanotubes?

A

cylindrical fullerenes with very high length to diameter ratio

96
Q

What does the proporties of carbon nanotubes make them useful for?

A

nanotechnology
electronics
materials

97
Q

What is the relative formula mass of a compound?

A

sum of the relative atomic masses of the atoms in the numbers shown in the formula

98
Q

What is the mass of one mole of a substance equal to?

A

relative formula mass

99
Q

Chemical reactions take place in what?

A

solutions

100
Q

What is the atom economy a measure of?

A

amount of starting materials that end up as useful products

101
Q

What is the equation for the percentage atom economy?

A

relative formula mass of desired products / sum of relative formula masses of all reactants x 100

102
Q

What can the concentration of solution be measured by?

A

mol/dm3

103
Q

What does metals react to to produce metal oxides?

A

oxygen

104
Q

What is oxidation?

A

when the metals gain oxygen

105
Q

What is reduction?

A

when the metals lose oxygen

106
Q

What is oxidation?

A

Loss of electrons

107
Q

What is reduction?

A

gain of electrons

108
Q

What can soluble salts be made from?

A

acids by reacting them with solid insoluble substances

109
Q

What does acid produce in aqueous solutions?

A

hydrogen ions

110
Q

What does aqueous solutions of alkalis contain?

A

hydroxide ions

111
Q

What is a solution of pH7?

A

neutral

112
Q

What are aqueous solutions of acids of less than 7?

A

alkalis

113
Q

What are aqueous solutions of acids of greater than 7?

A

Acid

114
Q

What happens to strong acids in aqueous solutions?

A

become completely ionised

115
Q

What happens toweak acids in aqueous solutions?

A

only partially ionised

116
Q

What does passing an electric current through eletrolytes do to the ions?

A

cause ions to move to the electrodes

117
Q

What type of ions go to the cathode?

A

posotive

118
Q

What type of ions go to the anode?

A

negative

119
Q

When do you use electrolysis to extract a metal from a molten compound?

A

when metal is too reactive o be extracted by reduction with carbon

120
Q

What is an endothermic reaction?

A

takes in energy from surrondings

121
Q

What is an exothermic reaction?

A

one that transfers energy to the surronding

122
Q

exothermic reaction?

A

energy released from forming new bonds is greater than the energy needed to break existing bonds

123
Q

endothermic reaction

A

energy needed to break existing bonds is greater than the energy release from forming new bonds

124
Q

What is the formula for hydrogen gas?

A

H2

125
Q

What is the formula for nitrogen gas?

A

N2

126
Q

What is the formula for ammonia?

A

NH3

127
Q

What is the formula for sulfuric acid?

A

H2SO4

128
Q

What is ionic bonding?

A

Transfer of electrons from a metal to a non metal

129
Q

What is the properties if a giant ionic lattice?

A

High melting point
High boiling point
Only conducts electricity when molten or dissolved

130
Q

What are the properties of a covalent bond?

A

Low melting point
Low boiling point
Do not conduct electricity

131
Q

What are some giant covalent compounds?

A

Graphite

Diamond

132
Q

What are some properties of giant covalent structure?

A

High melting and boiling point
Do not conduct electricity
Do not dissolve

133
Q

What is diamonds structure?

A

Giant covalent
Carbon
Each carbon makes 4 bonds

134
Q

What are the properties of diamond?

A

Hard

135
Q

What is graphite structure?

A

Giant covalent
Carbon
Each carbon 3 bonds

136
Q

What are some properties of graphite

A

Soft

Conducts electricity

137
Q

What are some similarities between graphite and diamond?

A

Pure carbon

138
Q

What are some differences between graphite and diamond?

A

Graphite 3 bonds and is soft

Diamond 4 bonds and hard

139
Q

How do u work out concentration?

A

Amount / volume

140
Q

What is a metal and acid going to give u?

A

Salt and hydrogen

141
Q

What do u do before calculating the mass?

A

Balance the equation

142
Q

What does a acid and metal oxide form?

A

Salt and water

143
Q

What does an acid and metal hydroxide form?

A

Salt and water

144
Q

What does an acid and metal base form?

A

Salt and water

145
Q

What does a acid and metal carbonate form?

A

Salt and water and carbon dioxide

146
Q

What is titration?

A

A technique used to find out how much of an acid is needed to neutralise and alkali or unknown concentration or vice versa

147
Q

What is an ore?

A

A rock containing a metal or a metal compound

148
Q

What is fractional distillation?

A

Where you separate crude oil into hydrocarbons with similar properties. The properties are called fractions

149
Q

What are alkanes?

A

Hydrocarbon molecules that are saturated

Chemistry (6 decks)

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