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definitions Flashcards

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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
Q

electronegativity

A

the relative tendency of an atom in a covalent bond in a molecule to attract electrons in a covalent bond to itself.

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26
Q

periodicity

A

a repeating pattern across different periods

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27
Q

first ionisation energy

A

the Energy needed to remove an electron from each atom in one mole of gaseous atoms

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28
Q

metallic bonding

A

the electrostatic force of attraction between the positive metal ions and the delocalised electrons

29
Q

second ionisation energy

A

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
Q

activation energy

A

the minimum
energy which particles need to collide to start a reaction

31
Q

standard conditions

A

100 kPa pressure
298 K (room temperature or 25oC)
Solutions at 1mol dm-3

32
Q

enthalpy change of reaction

A

the enthalpy change when the number of moles of reactants as specified in the balanced equation react together

33
Q

standard enthalpy change of formation

A

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
Q

standard enthalpy change of combustion

A

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
Q

enthalpy change of neutralisation

A

the enthalpy change when solutions of an acid and an alkali react together under standard conditions to produce 1 mole of water.

36
Q

mean bond enthalpy

A

the enthalpy change when
one mole of bonds of (gaseous covalent) bonds is broken (averaged over different molecules)

37
Q

catalyst

A
  • 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
Q

general formula

A

algebraic formula for a homologous series

39
Q

structural formula

A

shows the minimal detail that shows the arrangement of atoms in a
molecule,

40
Q

displayed formula

A

show all the covalent bonds present in a molecule

41
Q

aliphatic

A

a compound containing carbon and hydrogen joined together in straight chains, branched chains or
non-aromatic rings

42
Q

alicyclic

A

an aliphatic compound arranged in non-aromatic rings with or without side chains

43
Q

aromatic

A

a compound containing a benzene ring

44
Q

homologous series

A

families of organic compounds with the same functional group and same general formula.

45
Q

functional group

A

is an atom or group of atoms which when present in different molecules
causes them to have similar chemical properties

46
Q

structural isomer

A

same molecular formula different structural formula

47
Q

chain isomers

A

Compounds with the same molecular formula but different
structures of the carbon skeleton

48
Q

position isomer

A

Compounds with the same molecular formula but different structures
due to different positions of the same functional group on the same carbon skeleton

49
Q

functional group isomer

A

Compounds with the same molecular formula but
with atoms arranged to give different functional groups

50
Q

cracking

A

conversion of large hydrocarbons to smaller molecules of by breakage of C-C bonds

51
Q

alkenes

A

unsaturated hydrocarbons

52
Q

nucleophile

A

electron pair donator

53
Q

electrophile

A

electron pair acceptor

54
Q

rate of reaction

A

the change in concentration of a substance in unit time
Its usual unit is mol dm-3s
-1

55
Q

buffer solution

A

solution where the pH does not change
significantly if small amounts of acid or alkali are added to it.

56
Q

enthalpy of atomisation

A

the enthalpy
change when 1 mole of gaseous atoms is formed
from the element in its standard state

57
Q

first ionisation energy

A

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
Q

second ionisation energy

A

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
Q

first electron affinity

A

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
Q

lattice enthalpy

A

the standard enthalpy change when 1 mole of an ionic crystal lattice is formed from its constituent ions in gaseous form.

61
Q

enthalpy of hydration

A

Enthalpy change when one mole of gaseous ions
become aqueous ions .

62
Q

enthalpy of solution

A

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
Q

standard electrode potential

A

the emf of a half cell composed compared to a standard hydrogen half cell
- measured at 298k, 1moldm-3, 100Kpa

64
Q

fuel cell

A

uses energy from the reaction of a fuel with oxygen to create a voltage

65
Q

conjugate acid base pair

A

contains 2 species that can be inter converted by transfer of a proton

66
Q

weighted mean mass

A

(The mean/average mass) taking into account the
relative abundancies of the isotopes

67
Q

radical

A

species with an unpaired electron

68
Q

heterolytic fission

A

one atom recieve two electrons
breaking of covalent bond

chem (6 decks)

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