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Chemistry > C1-5 Revision > Flashcards

C1-5 Revision Flashcards

1
Q

Aquaeous solution

A

Mixture made by adding a soluble substance to water

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2
Q

Atom

A

the smallest part of an element that can still be recognised as that element

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3
Q

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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4
Q

Balanced symbol equation

A

a symbol equation in which there are equal numbers of each type of atom on either side of the equation

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5
Q

Biofuel

A

Fuel made from animal or plant products

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6
Q

Chromatography

A

the process whereby small amounts of dissolved substances are separated by running a solvent
along a material such as absorbent paper

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7
Q

Compound

A

substance made when two or more elements are chemically bonded together

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8
Q

Electron

A

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

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9
Q

Electronic structure

A

set of numbers to show the arrangement of electrons in their shells (or energy levels)

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10
Q

Element

A

substance made up of only one type of atom. An element cannot be broken down chemically into any
simpler substance

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11
Q

Group

A

All the elements in the columns (labelled 1 to 7 and 0) in the periodic table

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12
Q

Ion

A

a charged particle produced by the loss or gain of electrons

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13
Q

Isotope

A

atoms that have the same number of protons but different number of neutrons, i.e., they have the same atomic
number but different mass numbers

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14
Q

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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15
Q

Mass number

A

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

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16
Q

Neutron

A

A dense particle found in the nucleus of an atom. It is electrically neutral, carrying no charge

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17
Q

Noble gases

A

the very unreactive gases found in Group 0 of the periodic table. Their atoms have very stable electronic structures

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18
Q

Nucleus (of an atom)

A

the very unreactive gases found in Group 0 of the periodic table. Their atoms have very stable electronic structures, radius of nucleus 1/10,000 that of an atom

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19
Q

Periodic table

A

an arrangement of elements in the order of their atomic numbers, forming groups and periods

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20
Q

Product

A

A substance made as a result of a chemical reaction

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21
Q

Proton

A

A tiny positive particle found inside the nucleus of an atom

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22
Q

Reactant

A

a substance we start with before a chemical reaction takes place

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23
Q

Shell

A

an area in an atom, around its nucleus, where electrons are found

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24
Q

State symbol

A

the abbreviations used in balanced symbol equations to show if reactants and products are solid (s), liquid (l), gas
(g) or dissolved in water (aq)

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25
Q

Symbol equation

A

an equation that helps you see how much of each substance is involved in a chemical reaction by showing the
chemical symbols and formulae of all the reactants and products involved

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26
Q

Word equation

A

way of describing what happens in a chemical reaction by showing the names of all reactants and the products
they form

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27
Q

Alkali metal

A

elements in Group 1 of the periodic table

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28
Q

Halogens

A

The elements found in Group 7 of the periodic table

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29
Q

Universal indicator

A

mixture of indicators that can change through a range of colours to show how strongly acidic or alkaline liquids
and solutions are

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30
Q

Alloy

A

a mixture of two or more elements, at least one of which is a metal

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31
Q

Covalent bond

A

the bond between two atoms that share one or more pairs of electrons

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32
Q

Covalent bonding

A

the attraction between two atoms that share one or more pairs of electrons (non-metals)

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33
Q

Delocalised electron

A

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

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34
Q

Dot and cross diagram

A

a drawing to show only the arrangement of outer shell electrons of the atoms or ions in a substance

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35
Q

Fullerene

A

form of the element carbon that can exist as large cage-like structures, based on hexagonal rings of carbon atoms

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36
Q

Gases

A

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

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37
Q

Giant covalent structure

A

A huge 3D network of covalently bonded atoms

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38
Q

Giant lattice

A

a huge 3D network of atoms or ions

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39
Q

Giant structure

A

A huge 3D network of atoms or ions

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40
Q

Intermolecular force

A

the attraction between the individual molecules in a covalently bonded substance

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41
Q

Ionic bond

A

the electrostatic force of attraction between positively and negatively charged ions

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42
Q

Liquids

A

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

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43
Q

Particle theory

A

a theory that explains the properties of solids, liquids and gases based on the fact that all matter is made from tiny
particles. It describes the movement of particles and the distance between them

44
Q

Polymer

A

A substance made from very large molecules made up of many repeating units

45
Q

Solids

A

substances that have a fixed shape and volume that cannot be compressed

46
Q

States of matter

A

the forms in which matter can exist. A substance can be solid, liquid or gas

47
Q

Avogadro constant

A

the number of atoms, molecules, or ions in a mole of any substance (i.e., 6.02 × 10
-23
per mol)

48
Q

Concentration

A

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

49
Q

Limiting reactant

A

the reactant in a chemical reaction that when used up causes the reaction to stop

50
Q

Mole

A

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

51
Q

relative atomic mass Ar

A

the average mass of the atoms of an element compared with carbon-12 (which is given a mass of exactly 12). The
average mass must take into account the proportions of the naturally occurring isotopes of the element

52
Q

Relative formula mass Mr

A

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

53
Q

Acid

A

when dissolved in water, its solution has a pH value less than 7. Acids are proton (H
+
ion) donors

54
Q

Alkali

A

its solution has a pH value more than 7

55
Q

Base

A

the oxide, hydroxide, or carbonate of a metal that will react with an acid, forming a salt as one of the products. (If a
base dissolves in water it is called an alkali). Bases are proton (H+ ion) acceptors
Accepts hydrogen ions when dissolved in water
Bases:
Metal oxide
Metal carbonate
Metal hyroxide=alkalis-dissolve in water
All alkalis are bases but not all bases are alkalis

Ammonia=alkalis-dissolve in water

56
Q

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

57
Q

Electrolysis

A

the breakdown of a substance containing ions by electricity

58
Q

Equilibrium

A

the point in a reversible reaction at which the forward and backward rates of reaction are the same. Therefore, the
amounts of substances present in the reacting mixture remain constant

59
Q

Half equation

A

an equation that describes reduction (gain of electrons) or oxidation (loss of electrons)

60
Q

Ionic equation

A

an equation that shows only those ions or atoms that change in a chemical reaction

61
Q

Metal ore

A

a rock that contains enough of a metal or metal compound that it is worth extracting the metal

62
Q

Neutral

A

a solution with a pH value of 7 which is neither acidic nor alkaline. Alternatively, something that carries no overall
electrical charge

63
Q

Neutralisation

A

the chemical reaction of an acid with a base in which a salt and water are formed. If the base is a carbonate or
hydrogen carbonate, carbon dioxide is also produced in the reaction

64
Q

Ore

A

rock which contains enough metal to make it economically worthwhile to extract the metal

65
Q

Oxidation/oxidised

A

a reaction where oxygen is added to a substance / or when electrons are lost from a substance

66
Q

pH/pH scale

A

a number which shows how strongly acidic or alkaline a solution is

67
Q

Reactivity series

A

a list of elements in order of their reactivity

68
Q

Reduction/redused

A

A reaction in which oxygen is removed or electrons are gained

69
Q

Salt

A

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

70
Q

Strong acids

A

these acids completely ionise in aqueous solutions

71
Q

Weak acids

A

acids that do not ionise completely in aqueous solutions

72
Q

Molecules

A

Small groups of atoms that are covalently bonded

73
Q

Noble gases=unreactive coz

A

Do not easily form molecules coz atoms stable arrangements of electrons

74
Q

Polyatomic elements

A

Consisting multiple atoms chemically bonded e.g. sulphur and phosphorus

75
Q

Diatomic elements

A

Consisting of 2 atoms chemically bonded

76
Q

Monoatomic elements

A

Noble gases (single atoms)

77
Q

Ionic bonding

A

Electrostatic attraction between oppositely charged ions (metal+non-metal)

78
Q

Current

A

Flow of charges

79
Q

Charges

A

Ions or electrons

80
Q

Do ionic solids conduct electricity

A

No because ions are not free to flow and are held in rigid lattice only in water or when melted

81
Q

Can metals conduct electricity

A

Yes because delocalised electrons are free to flow in metal

82
Q

Dative covalent bond

A

Only one of the atom contributes all of the electrons

83
Q

Metallic bond

A

Electrostatic attraction between delocalised electrons and positive nucleus within a pure metal

84
Q

Molecular formula

A

Show actual amount of atoms in a molecule

85
Q

Empirical formula

A

Shows the simplest ratio of atoms which make up a molecule

86
Q

Moles

A

Mass/relative formula mass AND concentration (mol/dm3)*volume(cm3/ml/dm3)

87
Q

Concentration(g/dm3)

A

Mass(g)/volume(dm3) AND amount of solute(g)/volume of solution(dm3)

88
Q

Idm3

A

1000cm3 and 1000ml

89
Q

Percentage yield

A

Real yield
———— *100
Theoretical

90
Q

Ionic properties

A

High melting and boiling point, doesn’t conduct as a solid, conducts in a liquid, solution doesn’t conduct

91
Q

Simple molecular properties

A

Low melting and boiling point, doesn’t conduct electricity and solution insoluble

92
Q

Giant covalent bond properties

A

Very high melting and boiling point, doesn’t conduct and isn’t soluble

93
Q

Metallic properties

A

High melting and boiling point, conducts in a states and insolubsle

94
Q

Concentrated=

A

Large amount of dissolved, high concentration hydrogen ions

95
Q

Dilute acids=

A

Small amount dissolved, low concentration hydrogen ions

96
Q

Weak acids=

A

Only partially ionise/dissociate

97
Q

Strong acids

A

Fully ionise/dissociate

98
Q

Difference between bases and alkalis

A

All alkalis are bases but not all bases are alkalis
Alkalis:metal hydroxide, ammonia NH3
Bases:metal carbonate, metal oxide

99
Q

Why percentage yield is not 100%

A

Errors or spills
Incomplete reaction
Un desirable side effects

100
Q

Metal+acid->

A

Salt+hydrogen

101
Q

Metal oxide+acid->

A

Salt+water

102
Q

Metal hydroxide+acid->

A

Salt+water

103
Q

Metal carbonate+acid

A

Salt+water+carbon dioxide

104
Q

Acid+base->

A

Water+salt (apart from ammonia which just =a salt)

105
Q 
Common acids
HCI(aq)->
H2SO4(aq)->
HNO3(aq)->
H3PO4(aq)->
CH3COOH(aq)->
A 
Dissociate (split up)
[H]+[Cl]-          chloride
2[H]+[SO4]2-        Sulphate
[H]+[NO3]-           Nitrate
3[H]+[PO]3-          Phosphate
[H]+[CH3COO]-         Ethanoate
Acids release hydrogen ions (proton) when dissolved
The 'ate' is in the acid with oxygen
106
Q

Electrons:OILRIG

A

Oxidation Is Loss Reduction Is Gain

Chemistry (7 decks)

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