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1
Q

atomic number

A

no of protons in the nucleus

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2
Q

mass number

A

number of protons and neutrons in the nucleus

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3
Q

isotope

A

atoms of the same element with the same number of protons, but different numbers of neutrons.

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4
Q

relative isotopic mass

A

the mass of one isotope compared to one twelfth of the mass of one atom of carbon-12

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5
Q

relative atomic mass

A

the weighted mean mass of one atom compared to one twelfth of the mass of one atom of carbon-12

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6
Q

relative molecular mass

A

the average mass of a molecule compared to one twelfth of the mass of one atom of carbon-12

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7
Q

the mole

A

the amount of substance in grams that has the same number of particles as there are atoms in 12 grams of carbon-12.

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8
Q

molar mass

A

the mass in grams of 1 mole of a substance and is given the unit of g mol-1

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9
Q

molar gas volume

A

the volume of 1 mole of a gas at a given temperature and pressure.

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10
Q

avogadro’s constant

A

There are 6.02 x 1023 atoms in 12 grams of carbon-12.

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11
Q

empirical formula

A

the simplest ratio of atoms of each element in the compound

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12
Q

molecular formula

A

the actual number of atoms of each element in the compound.

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13
Q

acid

A

releases H+ ions in aqueous solution

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14
Q

Bronsted- Lowry base

A

a proton (H+) acceptor

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15
Q

Bronsted- Lowry acid

A

a proton donor

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16
Q

alkali

A

soluble base that releases OH- ions in aqueous solution

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17
Q

strong acids

A

completely dissociate when dissolved in water

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18
Q

weak acid

A

slightly dissociate when dissolved in water, giving an equilibrium mixture

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19
Q

salt

A

formed when the H+ ion of an acid is replaced by a metal ion or an ammonium ion

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20
Q

oxidation

A

process of electron loss
results in an increase in oxidation number

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21
Q

reduction

A

process of electron gain
involved a decrease in oxidation number

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22
Q

ionic bonding

A

the electrostatic force of attraction between oppositely charged ions formed by electron transfer.

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23
Q

covalent bonding

A

the strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms

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24
Q

dative covalent bond

A

when the shared pair of electrons in the covalent bond come from only one of the bonding atoms.

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25
electronegativity
the relative tendency of an atom in a covalent bond in a molecule to attract electrons in a covalent bond to itself.
26
periodicity
a repeating pattern across different periods
27
first ionisation energy
the Energy needed to remove an electron from each atom in one mole of gaseous atoms
28
metallic bonding
the electrostatic force of attraction between the positive metal ions and the delocalised electrons
29
second ionisation energy
is the enthalpy change when one mole of gaseous ions with a single positive charge forms one mole of gaseous ions with a double positive charge
30
activation energy
the minimum energy which particles need to collide to start a reaction
31
standard conditions
100 kPa pressure 298 K (room temperature or 25oC) Solutions at 1mol dm-3
32
enthalpy change of reaction
the enthalpy change when the number of moles of reactants as specified in the balanced equation react together
33
standard enthalpy change of formation
the enthalpy change when 1 mole of the compound is formed from its elements under standard conditions (298K and 100kpa), all reactants and products being in their standard states
34
standard enthalpy change of combustion
the enthalpy change that occurs when one mole of a substance is combusted completely in oxygen under standard conditions. (298K and 100kPa), all reactants and products being in their standard states
35
enthalpy change of neutralisation
the enthalpy change when solutions of an acid and an alkali react together under standard conditions to produce 1 mole of water.
36
mean bond enthalpy
the enthalpy change when one mole of bonds of (gaseous covalent) bonds is broken (averaged over different molecules)
37
catalyst
- increase reaction rates without getting used up - They do this by providing an alternative route or mechanism with a lower activation energy so more molecules have energy above activation energy.
38
general formula
algebraic formula for a homologous series
39
structural formula
shows the minimal detail that shows the arrangement of atoms in a molecule,
40
displayed formula
show all the covalent bonds present in a molecule
41
aliphatic
a compound containing carbon and hydrogen joined together in straight chains, branched chains or non-aromatic rings
42
alicyclic
an aliphatic compound arranged in non-aromatic rings with or without side chains
43
aromatic
a compound containing a benzene ring
44
homologous series
families of organic compounds with the same functional group and same general formula.
45
functional group
is an atom or group of atoms which when present in different molecules causes them to have similar chemical properties
46
structural isomer
same molecular formula different structural formula
47
chain isomers
Compounds with the same molecular formula but different structures of the carbon skeleton
48
position isomer
Compounds with the same molecular formula but different structures due to different positions of the same functional group on the same carbon skeleton
49
functional group isomer
Compounds with the same molecular formula but with atoms arranged to give different functional groups
50
cracking
conversion of large hydrocarbons to smaller molecules of by breakage of C-C bonds
51
alkenes
unsaturated hydrocarbons
52
nucleophile
electron pair donator
53
electrophile
electron pair acceptor
54
rate of reaction
the change in concentration of a substance in unit time Its usual unit is mol dm-3s -1
55
buffer solution
solution where the pH does not change significantly if small amounts of acid or alkali are added to it.
56
enthalpy of atomisation
the enthalpy change when 1 mole of gaseous atoms is formed from the element in its standard state
57
first ionisation energy
the enthalpy change required to remove 1 mole of electrons from 1 mole of gaseous atoms to form 1 mole of gaseous ions with a +1 charge
58
second ionisation energy
the enthalpy change to remove 1 mole of electrons from one mole of gaseous 1+ ions to produces one mole of gaseous 2+ ions
59
first electron affinity
the enthalpy change that occurs when 1 mole of gaseous atoms gain 1 mole of electrons to form 1 mole of gaseous ions with a –1 charge
60
lattice enthalpy
the standard enthalpy change when 1 mole of an ionic crystal lattice is formed from its constituent ions in gaseous form.
61
enthalpy of hydration
Enthalpy change when one mole of gaseous ions become aqueous ions .
62
enthalpy of solution
the standard enthalpy change when one mole of an ionic solid dissolves in a large enough amount of water to ensure that the dissolved ions are well separated and do not interact with one another
63
standard electrode potential
the emf of a half cell composed compared to a standard hydrogen half cell - measured at 298k, 1moldm-3, 100Kpa
64
fuel cell
uses energy from the reaction of a fuel with oxygen to create a voltage
65
conjugate acid base pair
contains 2 species that can be inter converted by transfer of a proton
66
weighted mean mass
(The mean/average mass) taking into account the relative abundancies of the isotopes
67
radical
species with an unpaired electron
68
heterolytic fission
one atom recieve two electrons breaking of covalent bond

chem (6 decks)

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