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GCSE Combined Science > Chemistry paper 1 > Flashcards

Chemistry paper 1 Flashcards

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1
Q 
Atomic structure (keywords) -
Atom
A

The smallest part of an element that can still be recognised as that element.

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2
Q 
Atomic structure (keywords) -
Atomic number
A

The number of protons (which equals the number of electrons) in an atom. It is sometimes called the proton number.

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3
Q 
Atomic structure (keywords) -
Electron
A

A tiny particle with a negative charge. Electrons orbit the nucleus of atoms or ions in shells.

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4
Q 
Atomic structure (keywords) -
Isotope
A

Atoms that have the same number of protons but different number of neutrons.

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5
Q 
Atomic structure (keywords) -
Mass number
A

Mass number the number of protons plus neutrons in the nucleus of an atom.

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6
Q 
Atomic structure (keywords) -
Proton
A

A tiny positive particle found inside the nucleus of an atom.

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7
Q 
Atomic structure (keywords) -
Nucleus (of an atom)
A

The very small and dense central part of an atom that contains protons and neutrons.

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8
Q 
Atomic structure (keywords) -
Product
A

A substance made as a result of a chemical reaction.

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9
Q 
Atomic structure (keywords) -
Reactant
A

A substance we start with before a chemical reaction takes place.

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10
Q 
Atomic structure (keywords) -
Law of conservation of mass
A

The total mass of the products formed in a reaction is equal to the total mass of the reactants.

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11
Q

Key parts for periodic table -

Group 1

A

Alkali metal
Reactive metals
Always forms +1 ions

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12
Q

Key parts for periodic table -

Group 2

A

Alkali earth metals
Less reactive
Always form +2 ions

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13
Q

Key parts for periodic table -

Transition metals

A

Typical metals

Shiny, malleable & high melting points

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14
Q

Key parts for periodic table -

Group 7

A

Halogens
Reactive gases
Always form -1 ions

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15
Q

Key parts for periodic table -

Group 0

A

Noble gases
Unreactive
Full outer shells

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16
Q

Shells -

First shell maximum number of electrons

A

2

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17
Q

Shells -

Second shell maximum number of electrons

A

8

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18
Q

Shells -

Third shell maximum number of electrons

A

8

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19
Q

Periodic table electronic structure -

Period (row)

A

Number of rings

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20
Q

Periodic table electronic structure -

Group (column)

A

Electrons in outer shell

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21
Q

Periodic table electronic structure -

Atomic number

A

Total number of electrons

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22
Q

History of the atom -

Dalton

A

All atoms look the same

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23
Q

History of the atom -

Thomson

A

Plum pudding model

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24
Q

History of the atom -

Rutherford

A

Nuclear model

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25
Q

History of the atom -

Bohr

A

Electron shells

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26
Q

Subatomic particle -

Protons

A 
Charge = +1
Mass = 1
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27
Q

Subatomic particle -

Electrons

A 
Charge = -1
Mass = 1/1800
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28
Q

Subatomic particle -

Neutrons

A 
Charge = 0
Mass = 1
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29
Q

Chromatography -

Purpose

A

Separate substrate from mixtures in solution.

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30
Q

Chromatography -

Key points

A 
Use a pencil to draw the line
Solvent soaks up the paper
Mixtures separate based on solubility
The number of dots is the number of substances in the mixture
The distance they travel can be compared
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31
Q

Separating substances key words -

Compound

A

Two or more elements chemically combined

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32
Q

Separating substances key words -

Mixture

A

Two or more elements or compounds mixed but not reacted

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33
Q

Separating substances key words -

Pure

A

Only one type of substance (molecules or atoms)

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34
Q

Separating substances key words -

Distilation

A

Separation of a liquid from a mixture (evaporate -> condense)

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35
Q

Separating substances key words -

Filtration

A

Separation of an insoluble solid from a solution

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36
Q

Separating substances key words -

Crystallisation

A

Used to obtain pure salt from a solution by evaporation

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37
Q

Law of conservation of mass

A

Reactant = products

The total mass of the reactants formed in a reaction equal to the total mass of the products

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38
Q

Periodic table -

Lavousier

A

The earliest attempt. Grouped elements based on their properties into gases, non-metals and earths.

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39
Q

Periodic table -

Dobereiner

A

Recognised traids of elements with chemically similar properties. Only a few worked.

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40
Q

Periodic table -

Newlands

A

Law of Octaves. Similarities between every 8 elements. Only worked up to Ca.

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41
Q

Periodic table -

Mendeleev

A

Left gaps, arranged elements by atomic weight and chemical properties.

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42
Q

Periodic table -

Group 1

A

Name - alkali metals
Features - metal, reactive
Typical changes - +1

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43
Q

Periodic table -

Group 7

A

Name - halogens
Features - non-metal, reactive
Typical changes - -1

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44
Q

Periodic table -

Group 0 or 8

A

Name - noble gases
Features - gases/non-metal, reactive
Typical changes - 0

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45
Q

Periodic table -

Lithium with oxygen

A
  • burns red flame

- white ash of lithium oxide

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46
Q

Periodic table -

Lithium with chlorine

A
  • burns red flame

- white ash of lithium chloride

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47
Q

Periodic table -

Lithium with water

A
  • floats, fizzes producing hydrogen gas

- produces colourless lithium hydroxide solution (alkali)

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48
Q

Periodic table -

Sodium with oxygen

A
  • burns more vigorously with yellow flame

- white ash of sodium oxide

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49
Q

Periodic table -

Sodium with chlorine

A
  • burns more vigorously with yellow flame

- white ash of sodium chloride

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50
Q

Periodic table -

Sodium with water

A
  • floats and melts, fizzes producing hydrogen gas

- produces colourless sodium hydroxide solution

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51
Q

Periodic table -

Potassium with oxygen

A
  • burns violently with lilac flame

- white ash of potassium oxide

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52
Q

Periodic table -

Potassium with chlorine

A
  • burns violently with lilac flame

- white ash of potassium chloride

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53
Q

Periodic table -

Potassium with water

A
  • floats, hydrogen gas sets on fire with lilac flame

- produces colourless potassium hydroxide solution

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54
Q

Periodic table -

Period definition

A

number of rings

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55
Q

Periodic table -

Group definintion

A

electrons in the outer shell

56
Q

Periodic table -

Structure definition

A

number of electrons in each shell

57
Q

chlorine + potassium bromide

A

2KCL + Br (small2)

58
Q

chlorine + potassium iodine

A

2KCl + I (small2)

59
Q

bromine + potassium chloride

A

no reaction

60
Q

bromine + potassium iodine

A

2KBr + I (small2)

61
Q

iodine + potassium chloride

A

no reaction

62
Q

iodine + potassium bromide

A

no reaction

63
Q

Size of atom

A

Larger atoms lose electrons more easily

Smaller atoms gain electrons more easily

64
Q

Nuclear charge

A

The higher the atomic number the greater the charge

65
Q

Electronic shielding

A

Complete shell block the positive charge from the nucleus, the more complete shells, the more the charge is blocked.

66
Q

Displacement reactions

A

A reactive element can displace a less reactive ion from a compound. So the reactive element kicks out the ion, forming a new compound, and turning the ion into and element. If the element it less reactive than the ion, then it can’t displace the ion and there will be no reaction.

67
Q

Transition metals

A
  • metals in the ‘d block’ of the periodic table
  • typical metals, high m.p/b.p, shiny, good conductors, malleable, ductile.
  • form colourful compounds
  • ions have multiple charges
  • make useful catalysts
68
Q

Structures & bonding -

Alloy

A

A mixture of two or more elements, at least one of which is a metal. (brass)

69
Q

Structure & bonding -

Covalent bond

A

The bond between two atoms that shares one or more pairs of electrons.

70
Q

Structure & bonding -

Delocalised electron

A

A bonding electron that is no longer associated with any one particular atom.

71
Q

Structure & bonding -

Gases

A

Substances that have no fixed shape or volume and can be compressed easily.

72
Q

Structure & bonding -

Giant covalent structure

A

A huge 3D network of covalently bonded atoms

73
Q

Structure & bonding -

Giant lattice

A

A huge 3D network of atoms or ions

74
Q

Structure & bonding -

Intermolecular forces

A

The attraction between the individual molecules in a covalently bonded substance.

75
Q

Structure & bonding -

Ionic bond

A

Bonds formed by the transfer of electrons and held together by the electrostatic force of attraction between positively and negatively charged ions.

76
Q

Structure & bonding -

Liquids

A

Substances that have a fixed volume, but they can flow and change their shape.

77
Q

Structure & bonding -

Polymer

A

Substance made from very large molecules made up of many repeating units (monomers).

78
Q

Structure & bonding -

Solids

A

Substances that have a fixed shape and a volume that cannot be compressed.

79
Q

Structure & bonding -

States of matter

A

The form in which matter can exist. A substance can be solid, liquid or gas.

80
Q

Ionic bonding -

Ionic solid

A
  • ions are in fixed positions in a giant lattice
  • they vibrate but cannot move around
  • it does not conduct electricity
81
Q

Ionic bonding -

Molten ionic compound

A
  • high temperature provides enough energy to overcome the many strong attractive forces between ions
  • ions are free to move around within the molten compound
  • it does conduct electricity
82
Q

Ionic bonding -

Ionic compound in solution

A
  • water molecules separate ions from the lattice
  • ions are free to move around within the solution
  • it does conduct electricity
83
Q

Giant covalent molecules -

Graphite

A
  • contains covalently bonded carbon atoms arranged in layers
  • no covalent bonds
  • between the layers there are weak intermolecular forces
  • layers can slide over eachother
  • soft and slippery
  • delocalised electrons allows it to conduct electricity
84
Q

Giant covalent molecules -

Diamond

A
  • carbon atoms have a rigid giant covalent structure

- hard/solid

85
Q

Simple covalent molecules

A
  • Have a weak intermolecular force
  • low melting and boiling points
  • no overall charge
  • no electrical charge
  • cannot conduct electricity
86
Q

Fullerenes

A
  • used for drug delivery, lubricants and catalysts due to large surface area
  • graphene is a single layer of graphite and so one atom thick
  • good electrical conductivity
87
Q

Metallic bonding

A
  • atoms in metals are closely packed together in regular layers
  • the positively charged metal ions are held together held by a ‘sea’ of electrons from the outer shell of each metal atom
  • good conductors of electricity and thermal energy
  • delocalised electron
  • layers of metal ions can slide over eachother
88
Q

Alloys

A
  • a mixture of 2 or more elements
  • at least one is a metal
  • usually harder than pure metals because the regular layers in pure metal are dissorted by the atoms of different sizes in an alloy
  • no layers can slide over one another
89
Q

Relative mass & moles -

Mass number

A

Number of protons and neutrons

90
Q

Relative mass & moles -

Isotopes

A

Same number of protons, different number of neutrons

91
Q

Relative mass & moles -

Relative atomic mass

A

Mass of atom (Ar) compared to (12) C. So sodium (Na) = 23

92
Q

Relative mass & moles -

Relative formula mass

A

The total of the relative atomic masses, added up in the ratio shown in the chemical formula, of a substance

93
Q

Relative mass & moles -

Moles

A

The amount of substance in the relative atomic or formula mass of a substance in grams

94
Q

Relative mass & moles -

Concentration

A

The amount of a substance dissolved in a given volume of liquid

95
Q

Metal oxide

A

Metals react with oxide to produce metal oxides. This is an oxidation reaction

96
Q

Displacement reaction

A

A more reactive metal can displace a less reactive metal from a compound

97
Q

Oxidation

A

Two definitions

  • chemicals are oxidised if they gain oxygen in a reaction
  • chemicals are oxidised if they lose electrons in a reaction
98
Q

Reduction

A

Two definitions

  • chemicals are oxidised if they lose oxygen in a reaction
  • chemicals are oxidised if they gain electrons in a reaction
99
Q

Acid

A

A chemical that dissolves in water to produce H+ ions

100
Q

Base

A

A chemical that reacts with acids and neutralise them

101
Q

Alkali

A

A base that dissolves in water

produces OH- ions in a solution

102
Q

Neurtralisation

A

When a neutral solution is formed from reacting and acid and an alkali.

103
Q

pH

A

A scale to measure acidity/alkalinity

104
Q

Strong acid (HT)

A

A strong acid is completely ionised in solution (e.g. hydrochloric, nitric and sulfuric acids

105
Q

Weak acid (HT)

A

A weak acid is only partially ionised in solution (e.g. ethanoic, citric and carbonic acids

106
Q

Potassium reaction

A

When potassium is added to water, the metal melts and floats. It moves around very quickly. The metal is also set on fire, with sparks and a lilac flame

107
Q

Sodium reaction

A

When sodium is added to water, it melts to form a ball that moves around on the surface. It fizzes rapidly

108
Q

Lithium reaction

A

When lithium is added to water, it floats. It fizzes steadily and becomes smaller

109
Q

Calcium reaction

A

fizzes quickly with dilute acid

110
Q

Magnesium reaction

A

fizzes quickly with dilute acid

111
Q

Zinc reaction

A

bubbles slowly with dilute acid

112
Q

Iron reaction

A

very slow reaction with dilute acid

113
Q

Copper reaction

A

no reaction with dilute acid

114
Q

Extracting metals -

very unreactive metals

A

found naturally in the ground

don’t need extracting

115
Q

Extracting metals -

metals less reactive than carbon

A

extracted by reduction with carbon

116
Q

Extracting metals -

metals more reactive than carbon

A

extracted by electrolysis

117
Q

Making a soluble salt

A
  • add solid metal, metal carbonate, metal oxide or metal hydroxide to an acid
  • add solid until no more reacts
  • filter off excess solid
  • evaporate to remove some of the water
  • leave to crystallise
  • remove all water in a desiccator / oven
118
Q

Electrolysis definition

A

The process of splitting an ionic compound by passing electricity through it

119
Q

Electrolyte definition

A

An ionic compound that is molten or dissolved in water. The ions are free to move

120
Q

Electrode definition

A

An electrical conductor that is placed in the electrolyte and connected to the power supply

121
Q

Cathode definition

A

The electrode attached to the negative terminal of the power supply

122
Q

Anode definition

A

The electrode attached to the positive terminal of the power supply

123
Q

Cathode descripition

A
  • metal
  • the metal if the metal is less reactive than hydrogen
  • hydrogen is produced if the metal is more reactive than hydrogen
124
Q

Anode description

A
  • non-metal
  • oxygen is produced unless the solution contains halide ions (chloride, bromide and iodide) when the halogen (chlorine, bromine and iodine) is being produced
125
Q

Aluminium electrolysis -

Cryolite

A

Aluminium oxide is dissolved in cryolite to lower it’s melting point. This saves money on energy costs.

126
Q

Aluminium electrolysis -

Cathode

A

Positive Al (small3+) ions move to the cathode. Aluminium is produced Al (small 3+) + 3e = Al

127
Q

Aluminium electrolysis -

Anode

A

Negative 0 (small2-) ions move to anode. Oxygen is made. 2O (small2) = O (small2) + 4e

128
Q

Conservation of energy

A

Energy is not created or destroyed, only transferred from one store to another

129
Q

Exothermic

A

A reaction that transfers energy to the surroundings so the temperature of the surroundings increases, e.g. combustion and neutralisation reactions. Used in self-heating cans and hand warmers

130
Q

Endothermic

A

A reaction that takes energy in from the surroundings so the temperature of the surroundings decreases, e.g. thermal decomposition. Used in sports injury packs

131
Q

Activation energy

A

The energy needed for particles to successfully react

132
Q

Breaking bonds

A

Energy is needed to break bonds

133
Q

Forming bonds

A

Energy is released when bonds are formed

134
Q

Exothermic energy profile

A

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

135
Q

Endothermic energy profile

A

Energy release from forming bonds is less than the energy needed to break bonds

GCSE Combined Science (4 decks)

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