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Defns Flashcards

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1
Q

What does acid Arrhenius mean?

A

Produces h+ ion by disassociation in aqueous solution.

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2
Q

What does acid Bronsted Lowry mean?

A

Proton donor.

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3
Q

What does acidic oxide mean?

A

Oxide that lowers the ph in water.

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4
Q

Activation energy.

A

Minimum energy required for colliding particles fo react.

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5
Q

What is addition polymerisation?

A

Monomers combining to form a large molecule.

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6
Q

What’s it adsorption?

A

The method of attachement of gaseous or liquid molecules to a solid surface.

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7
Q

Atomic Absorption Spectroscopy

A

Instrumental method used to analyse water for heavy metals.

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8
Q

Atomic number

A

Number of protons in nucleus

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9
Q

atomic orbital

A

Region of space surrounding nucleus where electrons normally found.

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10
Q

Atomic radius

A

Half the dust and between the centres of singly bonded atoms of the same element

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11
Q

Atomic sub level

A

A division of a main energy level consisting of one or more orbitals of the same energy

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12
Q

Auto ignition

A

Premature ignition

Reduces power

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13
Q

Avogrados law

A

Equal volume of gases contain equal numbers of molecules under same conditions of temperature and pressure

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14
Q

Base Arrhenius

A

Produces OH- as only anion in aqueous solution

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15
Q

Base bronsted lowry

A

Proton acceptor

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16
Q

Biochemical oxygen demand

A

Amount of oxygen produced per ppm when a given sample is put in the dark at 20C for 5 days

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17
Q

Bond energy

A

Average amount of energy to break 1 mole of bonds into separate atoms in gaseous state

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18
Q

Boyles law

A

Pressure is inversely proportional to volume for definite mass of a gas at constant temp
PV=K

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19
Q

Catalyst

A

A substance that alters the rate of the reaction but is not used ip

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20
Q

Catalytic cracking

A

Splitting of long chain molecules

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21
Q

Catalytic poison

A

Substance that blocks the active site of the catalyst and stops it from working

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22
Q

Charles law

A

Volume varies directly with kelvin temperature at constant pressure

P/V =K

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23
Q

Chemical Equillibrium

A

Rate of forward reaction is equal to rate of backwards reaction

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24
Q

Chromatography

A

Separation of a mixture of components based on their relative attractions for a stationary phase while carried by a mobile phase

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25
Q

Condensation reaction

A

Production of a more complex molecule with formation of an unsaturated compound or double bond by the loss of a small molecule

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26
Q

Conjugate acid

A

Produced by a gain of h+ ion

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27
Q

Conjugate pair

A

Acid-base differing by h+ ion

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28
Q

Crystals

A

Regular solids made up of particles with faces inserting at fixed angles or particles in a lattice

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29
Q

Dobereniers triads

A

Elements of similar properties in groups of three

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30
Q

Dynamic

A

Reaction has not stopped

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31
Q

Effective collision

A

One that results in a reaction

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32
Q

Electrolysis

A

Chemical reaction caused by electric current passing through an electrolyte

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33
Q

Electronegatovity

A

Measure of relative attraction for a shared pair of electrons in a covalent bonf

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34
Q

Element

A

Cannot be broken down into anything simpler

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35
Q

Energy level

A

Shell in which electrons of equal energy occupy

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36
Q

Eutrophication

A

Excess plant growth caused by excess nutrients in watwr

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37
Q

Excited state

A

Higher energy level

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38
Q

Feedstock

A

Modified and purified raw mayerials

39
Q

First ionisation energy

A

Minimum energy required to remove the most loosely held electron from an isolated gaseous atom in its ground state

40
Q

Flocculation

A

Clumping of suspended solids

41
Q

Gay lussacs law

A

The volumes of reacting gases are in whole number ratios

42
Q

Greenhouse factor

A

Effect compared w CO2

43
Q

Greenhouse effect

A

Blocking the escape of radiation by the atmosphere

44
Q

Greenhouse gas

A

Atmospheric gas that prevents the escape of heat

45
Q

Ground state

A

Lowest energy level

46
Q

Half life

A

Time taken for have the nucleus of a given sample to decay

47
Q

Hard water

A

Water that doesn’t easily form a lather with soap

Forms a scum with soap

48
Q

Temporary hardness

A

Removed by boiling

Caused by calcium hydrogen carbonate

49
Q

Hardness

A

Not removed by boiling

Caused by magnesium chloride

50
Q

Heat of combustion

A

Heat change when one mole of a substance is burned completely in excess oxygen

51
Q

Heat of formation

A

Heat change when one mole of compound is formed from it elements in their standard states

52
Q

Heat of reaction

A

Heat change when the number of moles of the reactants in the balanced equation react completely

53
Q

Heisenburgs uncertainty principle

A

It is not possible to measure the exact position and velocity of electron at same tome

54
Q

Heterogeneous catalysis

A

Reactants and catalyst at different phases

55
Q

Homogeneous catalysis

A

Reactants and catalysts at same lhase

56
Q

Homologous series

A

Have same general formula
Same functional group
Each differ by CH2

57
Q

Hydrocarbon

A

Made of hydrogen and carbon only

58
Q

Ideal gas

A

A gas that obeys the gas laws at all values of temperature and pressure

59
Q

Immisicble liquids

A

Do not mix or do not dissolve in eachother

60
Q

Isomers

A

Same molecular formula different structural formula

61
Q

Isotopes

A

Atoms of same element with different mass numbers due to different numbers of neutrons

62
Q

Intermolecular

A

Forces between molecules

63
Q

Intra molecular

A

Forces between atoms in a molecule

64
Q

Kw

A

[H+][OH-] or [H3O+][OH-]

65
Q

Le chatelier pronciple

A

Reactions at equilibrium apposé applied stresses

66
Q

Limiting reacgant

A

Substance that is totally consumed when the chemical reaction is complete

67
Q

Mole

A

Contains. The avogrados number 6 x 10^23 particles.

Relative molecular mass in grams

68
Q

Mass number

A

Number of neutrons and number of protons

69
Q

Nitrogen fixation

A

Conversion of atmospheric nitrogen to compounds that can be used by plants

70
Q

Octane number

A

Measure of a fuels tendency to resist knocking

71
Q

Orbital

A

Region where electrons normally found

72
Q

Oxidation

A

Loss of electrons

Increase in oxidation number

73
Q

Ph

A

-log 10 h3O+

74
Q

PI bond

A

side on overlap of p orbitals

75
Q

Primary standard

A 
A solution of known concentration
Pure
Stable
Very soluble
Higher molecular mass
76
Q

Primary sewage treatment

A

Removal of solids by screening and sedimentayikn

77
Q

Radioactivity

A

Spontaneous breaking up of an unstable nucleus with the emission of one or more types of electrons

78
Q

Rate of chemical reaction

A

Concentration per unit tome

79
Q

Reduction

A

Gain of an electron

Loss in oxidation number

80
Q

Relative atomic mass

A

Average mass of atoms of element relative to 1/12 of the mass of a carbon 12 atom

81
Q

Reversible

A

Can go in both directions

82
Q

Scrubbing

A

Removal of pollutants from industrial chimney gases

83
Q

Secondary treatment

A

The removal of suspended solids by screening and sedimentation and then by
Biological oxidation of microorganisms

84
Q

Sigma bond

A

Head on overlap of orbitals

85
Q

Standardised

A

Concentration got by titration

86
Q

Sting acid

A

Good proton donor

87
Q

Strong acid Arrhenius

A

Dissociated fully in aqueous solution

88
Q

Structural isomer

A

Same molecular formula but different structural formula

89
Q

Sub level

A

Subdivision of a main energy level consisting of one or more orbitals of the same energy

90
Q

Tertiary treatment

A

Removal of phosphates and nitrates

91
Q

Unsaturated

A

Contains one or more double or triple carbon to carbon bond

92
Q

Volatile

A

Easily vapourised

93
Q

Weak acid

A

Poor proton donor

94
Q

Weak acid Arrhenius

A

Does not dissociate filly in aqueous solution

Chemistry (33 decks)

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