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OCR AS/A Level Chemistry A > DEFINITIONS SO FAR > Flashcards

DEFINITIONS SO FAR Flashcards

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1
Q

Atomic number

A

The number of protons in the nucleus of the atom

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2
Q

Mass (nucleon) number

A

The number of particles (protons and neutrons) in the nucleus

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3
Q

Isotopes

A

Atoms of the same element with the same number of neutrons but a different number of neutrons

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4
Q

Ions

A

An electrically charged particle formed by the loss or gain of one or more electrons from an atom or group of atoms

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5
Q

Relative isotopic mass

A

The mass of an atom of an isotope compared to 1/12th the mass of carbon 12

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6
Q

Relative atomic mass Ar

A

The weighted mean mass of an atom of an element compared to 1/12th the mass of carbon 12

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7
Q

Relative molecular mass Mr

A

The weighted mean mass of a molecule compared with 1/12th of the mass of an atom of carbon 12 (ONLY applies to simple covalent molecules e.g. O2 or CO2)

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8
Q

Relative formula mass

A

The weighted mean mass of a formula unit compared to 1/12th of the mass of an atom of carbon 12 (Can apply to ionic substances as they occur as giant lattices)

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9
Q

Molar gas volume

A

Volume per mole of gas.
Units= dm^3 mol^-1
At RTP= 24.0dm^3 mol^-1 approx.

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10
Q

Concentration (of a solution)

A

The amount of solute, in mol, dissolved per 1dm^3 (1000cm^3) of solution

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11
Q

Dilution

A

The process of decreasing the concentration of a solute in solution. Adding more solvent without adding more solute will reduce the concentration.

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12
Q

Compound

A

Atoms chemically joined

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13
Q

Molecule

A

2 or more atoms bonded with covalent bonds

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14
Q

Bond enthalpy

A

Average energy required to break one mole of that type of bond

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15
Q

Covalent bond

A

A shared pair of electrons

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16
Q

Ionic bond

A

Attraction (electrostatic) between oppositely charged ions

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17
Q

Element

A

Substance which contains only 1 type of atom

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18
Q

Orbital

A

A region that can be occupied by up to 2 electrons with opposite spins

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19
Q

Dative bond

A

Both of the shared electrons originate from the same species

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20
Q

Electronegativity

A

The ability of an atom to attract the bonding electrons in a covalent bond

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21
Q

Accuracy

A

How close to the true value a measurement is

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22
Q

Activation energy

A

Minimum energy required to start a reaction by breaking bonds in the reactants

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23
Q

Aim

A

The purpose of the investigation

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24
Q

Amount of substance

A

The quantity whose unit is mole. Amount of substance=counting atoms

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25
Q

Anhydrous

A

A substance containing no water molecules

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26
Q

Anion

A

Negatively charged ion

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27
Q

Anomalies

A

Data points that don’t fit the overall trend in the data

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28
Q

Anomalous

A

Results that don’t follow the general pattern of the data

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29
Q

Aqueous

A

A solution in which the solvent is water

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30
Q

Atom

A

Smallest object that retains properties of an element

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31
Q

Atomic structure

A
  • Positively charged nucleus
  • Negatively charged electrons in orbit
  • Atom has 0 overall charge (equal no of protons and electrons)
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32
Q

Avogadro constant Na

A

Number of atoms per mole of the carbon 12 isotope (6.02*10^23)

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33
Q

Bond angle

A

Angle formed between two adjacent bonds on the same atom

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34
Q

Bonded pair

A

Pair of electrons that have been shared between two chemically bonded atoms

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35
Q

Bonding region

A

Space where an electron can be found in a bond

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36
Q

Catalyst

A

Substance which increases rate of reaction without being used up during the reaction

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37
Q

Cation

A

Positively charged ion😺

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38
Q

Chemical energy

A

Special form of potential energy stored in chemical bonds

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39
Q

Continuous variable

A

A measured value which could be any number

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40
Q

Control variable

A

A factor YOU MUST keep constant in experiments

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41
Q

D-orbital

A

A region (within an atom) which can hold up to 2 electrons with opposite spins

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42
Q

Dehydration

A

Chemical reaction where a water molecule is eliminated from an organic compound

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43
Q

Delocalised electrons

A

Electrons that are shared between more than 2 atoms

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44
Q

Delta

A

“A little bit”

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45
Q

Dependant variable

A

Factor you observe in the experiment

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46
Q

Diatomic molecules

A

Molecules composed ONLY of 2 atoms (can be the same or different elements)

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47
Q

Displacement reaction

A

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

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48
Q

Distillation

A

Technique used to separate miscible liquids or solutions

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49
Q

Dot and cross diagrams

A

Model the electrons in chemical bonding

50
Q

Dot formulae

A

Ration between no. of compound molecules and the no. of water molecules within the crystalline structure

51
Q

Electron

A

Smallest particle that makes up an atom, carry negative charge

52
Q

Electron configuration

A

Arrangement of electrons in an atom or ion

53
Q

Electron shielding

A

Repulsion between electrons in different inner shells. Shielding reduces the attraction between the positive nucleus and negatively charged outer shell electrons.

54
Q

Empirical formula

A

Simplest whole no. ratio of atoms of each element in a compound

55
Q

Giant covalent lattice

A

3D Structure of atoms, all bonded together by strong covalent bonds

56
Q

Giant ionic lattice

A

3D Structure of oppositely charged ions, held together by strong electrostatic attraction between the oppositely charged ions

57
Q

Giant metallic lattice

A

3D Structure of positive ions and delocalised electrons, bonded with strong metallic bonds

58
Q

Group

A

Vertical column on periodic table
= No. of outer shell electrons
Same group=similar chemical properties

59
Q

Hydrated

A

Crystalline compound containing water molecules

60
Q

Hydration

A

Reaction where water is a reactant

61
Q

Hydrocarbons

A

Compound containing ONLY hydrogen and carbon atoms

62
Q

Hydrogen bond

A

Strong permanent dipole-dipole attraction between an electron deficient hydrogen atom on one molecule and a lone pair of electrons on a highly electronegative atom on a different molecule.

63
Q

Hypothesis

A

Prediction + explanation of the chemistry behind the prediction

64
Q

Incomplete combustion

A

Oxidising a fuel in a limited amount of air

65
Q

Independent variable

A

The factor you change

66
Q

Intermolecular force

A

Attractive force between neighbouring molecules or atoms

67
Q

Ionisation

A

Process of an atom becoming an ion

68
Q

Line of best fit

A

Shows trend of plotted points - could be a straight line, curve or S shape

69
Q

London dispersion forces

A

Attractive forces between induced dipoles in neighbouring molecules

70
Q

Lone pair

A

Outer shell pair of electrons not involved in chemical bonding

71
Q

Margin of error

A

Shows the range which the value lies within

72
Q

Metallic bonding

A

Electrostatic attraction between cations and delocalised electrons

73
Q

Method

A

Step by step detailed explanation of how to complete an experiment

74
Q

Molar mass M

A

Mass per mole of a substance

Units=g mol^-1

75
Q

Molar volume

A

Volume per mole of gas
Units= dm^3 mol^-1
At RTP= 24.0 dm^3 mol^-1

76
Q

Mole

A

Amount of substance containing as many particles as there are carbon atoms in exactly 12g of the carbon 12 isotope

77
Q

Molecular formula

A

Shows no. and type of the atoms of each element in the compound

78
Q

Neutron

A

Located in the nucleus of the atom
Mass=1
Charge=0

79
Q

Nucleons

A

Protons and neutrons

80
Q

P orbital

A

Region within the atom that can hold up to 2 electrons with opposite spins

81
Q

Particle model

A

Simplified model of matter, used to explain observations and make predictions

82
Q

Percentage yield

A

Actual amount, in mol, of product divided by theoretical amount, in mol, of product then times the answer by 100

83
Q

Period

A

Horizontal rows of the periodic table

Elements show trends in properties across a period

84
Q

Periodic table

A

Arrangement of chemical elements, organised by atomic number, electron configuration and recurring chemical properties

85
Q

Periodicity

A

Regular periodic variation of properties of elements with atomic no. and position in the periodic table

86
Q

Permanent dipole

A

Small charge difference across a bond due to differing electronegativities of the bonded atoms

87
Q

Permanent dipole-dipole interaction

A

Weak attractive force between permanent dipoles and permanent dipoles or induced dipoles in neighbouring polar molecules

88
Q

Polar covalent bond

A

Covalent bond which has a permanent dipole

89
Q

Precipitation reaction

A

Formation of a solid during a reaction (often formed when 2 aqueous solutions are mixed together)

90
Q

Precision

A

Degree to which repeated values (collected under the same conditions in the experiment) show the same result

91
Q

Product

A

Substances made/formed in a chemical reaction

92
Q

Proton

A

Found in nucleus

Has positive charge

93
Q

Qualitative data

A

Description of what is being observed

94
Q

Quantative data

A

Quantity (number) of what is being observed

95
Q

Rate of reaction

A

Change in concentration of a reactant or product in a given time

96
Q

Reactants

A

Substance that undergoes change in a reaction

97
Q

Reliable

A

Results that are similar once repeated

98
Q

S orbital

A

Spherical region, can hold up to 2 electrons with opposite spins

99
Q

Scatter graphs

A

Method of expressing quantative data
Independent variable must be continuous and on x axis
Dependent variable must be continuous and on ten y axis

100
Q

Separating funnel

A

Equipment used to separate immiscible liquids

101
Q

Shell

A

Group of atomic orbitals with the same principal quantum number, n

102
Q

Significant figures

A

Numbers used to represent a quantity that have a meaning

Degree of accuracy of answer

103
Q

Single covalent bonds

A

Atoms bonded by one shared pair of electrons between nuclei

104
Q

Simple molecular lattice

A

3D Structure of molecules held together by weak intermolecular forces

105
Q

Species

A

Any type of particle that takes place in a chemical reaction

106
Q

Standard form

A

Way of writing v small or v large numbers
A*10^n
A=value between 1 and 10
N=no of places and direction that the decimal point has been moved

107
Q

Stock solution

A

The solution has a know concentration. Used commonly in titrations to work out unknown info about another substance

108
Q

Sub shell

A 
Group of the same type of atomic orbitals (s,p,d or f) within a shell. 
S= max 2
P= max 6
D= max 10
F= max 14
109
Q

Valid experiment

A

Provides info to test the aim of the experiment

110
Q

Variables

A

Factors that can affect the outcome of the experiment

111
Q

Volume

A

Quantity of 3D space occupied by a solid, liquid or gas

112
Q

Water of crystallisation

A

Water molecules that form an essential part of the crust structure of a compound

113
Q

Yield

A

Amount of product obtained in a chemical reaction

114
Q

Hydrocarbon

A

A compound containing only carbon and hydrogen

115
Q

Saturated hydrocarbon

A

A hydrocarbon that only has single bonds

116
Q

Unsaturated hydrocarbon

A

A hydrocarbon that has double or triple covalent bonds between adjacent carbon atoms. It must contain at least one carbon-to-carbon double bond

117
Q

Aliphatic hydrocarbons

A

A hydrocarbon where carbon atoms are joined together in straight or branched chains

118
Q

Alicyclic hydrocarbons

A

Hydrocarbons where carbon atoms are joined together in a ring structure

119
Q

Functional group

A

A group of atoms that is responsible for the characteristic chemical reactions of a compound

120
Q

Homologous series

A

A series of organic compounds that have the same functional group with successive members differing by CH2

OCR AS/A Level Chemistry A (7 decks)

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