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Chemistry (JW) > Off by heart list > Flashcards

Off by heart list Flashcards

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1
Q

ion

A

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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2
Q

isotopes

A

atoms of the same element with the same number of protons and different numbers of neutrons, therefore with different masses

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3
Q

relative isotopic mass

A

the mass of an isotope relative to 1/12th of the mass of an atom of carbon-12

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4
Q

relative atomic mass

A

weighted mean mass compared with 1/12th of the mass of carbon-12

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5
Q

electronegativity

A

the tendency of an atom in a covalent bond to attract (the bonded pair of electrons) electron density

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6
Q

covalent bond

A

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

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7
Q

dative covalent bond

A

covalent bond in which both electrons come from the same atom

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8
Q

ionic bond

A

electrostatic attraction between positive and negative ions

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9
Q

Avogadro’s constant (definition and formula using it)

A

The number of atoms in one mole of atoms of any element.

no. moles = no.particles/6.02 x 10^23

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10
Q

The ideal gas equation (including units)

A 
pV = nRT
p= Pa
V= m^3
n= mol
R= 8.314 Jmol-1K-1
T= K
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11
Q

Acid

A

a proton donor

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12
Q

Base

A

a proton acceptor/ substance which readily accepts H+ ions from an acid

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13
Q

A Salt is formed when…

A

an acid has one or more hydrogen ions replaced by either a metal ion or an ammonium ion

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14
Q

Weak acid

A

partially dissociates

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15
Q

Strong acid

A

fully dissociates

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16
Q

Alkali

A

a soluble base that releases OH- in aqueous solution

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17
Q

ionisation energy

A

energy required to remove electrons one by one from an atom / energy required to become an ion

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18
Q

reducing agent

A

chemical that is oxidised

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19
Q

oxidising agent

A

chemical that is reduced

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20
Q

disproportionation

A

oxidation and reduction of the same element in a redox reaction

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21
Q

gas volumes equation

A

no. moles = volume (dm3) / 24

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22
Q

solution concentration equation

A

moles (mol) = concentration(moldm-3) x volume (dm3)

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23
Q

homologous series

A

a series of organic compounds having the same functional group and similar chemical properties but with each successive member differing by CH2

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24
Q

structural isomers

A

molecules with the same molecular formula but with different structural formula

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25
Q

Reasons for varying boiling points of organic compounds (2)

A
  • increasing chain length increases surface contact and London forces
  • more branches, less surface contact, less London forces between molecules
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26
Q

Oxidation number : elements in natural state

A

0

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27
Q

Oxidation number : the sum of the atoms of any molecule

A

0

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28
Q

Oxidation number : the sum of the components of any ion

A

The charge on that ion

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29
Q

Oxidation numbers - rules for order of assigning oxidation numbers to specific elements

A
  • Groups 1,2,3 always equal to charge (+1,+2,+3)
  • Fluorine always -1
  • Hydrogen usually +1
  • Oxygen usually -2
  • Chlorine usually -1
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30
Q

Products of complete combustion

A

CO2 and H20

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31
Q

Products of incomplete combustion

A

CO, C and H20

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32
Q

Valency

A

Number of electrons an atom loses or gains (ionic) or the number of bonds it can form (covalent)

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33
Q

Difference between relative molecular mass and relative formula mass

A

Molecular- for simple molecules

Formula- for giant structures

34
Q

What does a binary compound contain and how do you name them?

A

Contains two elements only.

Use name of first element but change the end of the second to -ide (in ionic, metal ion always comes first)

35
Q

Molar mass

A

Mass per mole of a substance (gmol-1)

36
Q

Empirical formula

A

Simplest whole number ratio of atoms of each element present in a compound

37
Q

Molecular formula

A

The actual number and type of atoms of each element in a molecule

38
Q

Hydrated Salt

A

Water molecules are part of the compounds crystalline structure (water of crystallisation)

39
Q

First ionisation energy

A

The energy needed to remove 1 mole of electrons from 1 mole of gaseous atoms (to form 1 mole of gaseous 1+ ions)

40
Q

Free radical

A

A radical is a species with an unpaired electron

41
Q

Stereoisomers

A

Have the same structural formula but different arrangements in space

42
Q

Electrophiles

A

Species with a whole of partial positive charge. They are electron loving.
ELECTRON PAIR ACCEPTORS

43
Q

Explaining why Markovnikoffs (ov’s) Rule is followed

A

The secondary (or tertiary) carbocation formed in the reaction is more energetically stable than the primary (or secondary) one which would be formed if the addition was the other way round, and so less activation energy is needed.

44
Q

Homolytic fission

A

Covalent bond breaks with each bonded atom taking an electron from the shared pair of electrons from the bond.

45
Q

Periodicity

A

Regular repeating pattern of variations of properties with Ar and Position on the periodic table

46
Q

Bond enthalpy

A

Energy needed to break one mole of bonds in the substance in the gaseous state.

47
Q

Reflux

A

Continuous process of evaporation followed by condensation

48
Q

What are the standard conditions ?

A

298K and 100kPa

49
Q

Standard enthalpy of formation

A

Energy required to make one mole of compound from its constituent elements in their standard states

50
Q

First electron affinity

A

Energy change when one mole if singly negative ions is made from one mole of gaseous atoms

51
Q

Mean bond enthalpy

A

Average energy change when one mole of a particular bond is broken in one mole of gaseous molecules

52
Q

What does Hess’ Law state?

A

That the energy change of a reaction is independent of the route, providing the conditions are constant

53
Q

Activation energy

A

Minimum amount of energy needed for a reaction to take place

54
Q

Standard enthalpy change,

A

The heat energy change at constant pressure under standard conditions (pressure 100
kPa ; temperature 298 K ).

55
Q

Standard molar enthalpy change of formation,

A

The enthalpy change when one mole of a compound is formed from its constituent
elements under standard conditions, with all reactants and products in their standard states.

56
Q

Standard molar enthalpy change of combustion

A

The enthalpy change when one mole of a compound is completely burned in excess
oxygen under standard conditions, all reactants and products in their standard states.

57
Q

Mean bond energy

A

The enthalpy change when 1 mole of a particular type of bond is broken or made (all
species in the gas phase) averaged over many different molecules

58
Q

Lattice enthalpy

A

Energy released when one mole of a crystal is formed from its constituent ions in their gaseous state , standard conditions

59
Q

Standard conditions?

A

298K , 100/101 kPa

60
Q

Enthalpy of atomisation

A

Enthalpy change when one mole of gaseous atoms is formed from the element in its standard state

61
Q

Electron affinity

A

Enthalpy change accompanying the gain of 1 mole of electrons by 1 mole of atoms in the gaseous phase

62
Q

Enthalpy of formation

A

Enthalpy change when 1 mole of a compound is formed from its constituent elements in their standard states

63
Q

Transition Metal

A

Element which forms one or more stable ions which have incompletely filled d orbitals

64
Q

Complex ion

A

Metal ion surrounded by coordinately bonded ligands

65
Q

What do all ligands have in common?

A

Active lone pairs of electrons in the outer energy level. They are used to form coordinate bonds with the metal ion

66
Q

Coordination number

A

Number of coordinate bonds that are formed with the central metal or ion

67
Q

Standard electrode potential

A

Potential difference/ voltage of half call compared with standard hydrogen electrode

Standard conditions: 298K, 1moldm-3, 1atm

68
Q

Half life

A

Time for concentration to reduce by half

69
Q

Charge on anode/cathode in cells

A

anode= negative

cathode=positive

70
Q

More positive electrode potential=

A

better oxidising agent (gives up electrons more readily)

71
Q

calculate overall cell potential

A

more positive - more negative

72
Q

rate =

A

concentration/time

73
Q

zero order

A

concentration has no effect on rate

74
Q

first order

A

change in concentration gives same change to the rate

75
Q

second order

A

any change in concentration changes the rate by the square of the concentration change

76
Q

What is rate constant specific to?

A

Temperature

77
Q

Bigger value of k =

A

faster reaction

78
Q

half life equation=

A

ln 2 / k

79
Q

gradient of a rate-concentration graph =

A

k

80
Q

rate determining step

A

the slowest step of the reaction mechanism

reactants in this step are in the rate equation

81
Q

fuel cells

A

produce electrical power using the energy from the chemical reaction of a fuel with oxygen

82
Q

pH

A

-log10[H+]

Chemistry (JW) (3 decks)

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