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A level chemistry > Module 2.1 Atoms and reactions > Flashcards

Module 2.1 Atoms and reactions Flashcards

1
Q

Electron relative mass and relative charge:

A

mass: 1/2000 (basically 0) charge: -1

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2
Q

Proton relative mass and relative charge

A

mass: 1 charge: +1

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3
Q

neutron relative mass and relative charge:

A

mass: 1 charge: 0

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4
Q

Mass number tells you?

A

the total no. of protons and neutrons

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5
Q

Atomic number tells you

A

no of protons in the nucleus it identifies element as all atoms of the same element have same number of protons.

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6
Q

define Isotope

A

are atoms with the same number of protons but different number of neutrons.

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7
Q

rutherford nuclear model of atom

A

tiny positively charged nucleus. mass concentrated there
the nucleus is surrounded by a cloud of -ve electrons
most of the atom is empty space

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8
Q

Bohr improved nuclear model 4 principles

A
  • electrons can only exist in fixed orbitals / shells
  • each shell has a fixed energy
  • when electron moves between shells electromagnetic radiation is emitted or absorbed
  • because the energy of shells is fixed, the radiation will have a fixed frequency.
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9
Q

relative atomic mass Ar

A

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

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10
Q

relative isotopic mass

A

the mass of an atom of an isotope, compared with 1/12th of the mass of an atom of carbon 12.

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11
Q

relative molecular / formula mass Mr

A

the average mass of a molecule or formula unit compared to 1/12th of the mass of an atom of carbon 12.

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12
Q

Ar can be worked out from isotopic abundances by

A
  1. multiple each relative isotopic mass by its % relative isotopic abundances and add up results
  2. divide by 100
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13
Q

avogrado constant Na

A

6.02 x 10(23)

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14
Q

number of moles:

A

no. of particles / avogrado constant

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15
Q

Molar mass is

A

the mass of one mole of something
the same as Mr
units: g mol-1

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16
Q

room temperature and pressure r.t.p

A

298k (25c) 101.3 KPa

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17
Q

molar gas volume at r.t.p

A

24 dm3 mol-1

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18
Q

ideal gas equation

A 
pV= nRT
p = pressure (Pa)
V= volume (m3)
n = no. of moles 
R = 8.314 J K-1 mol-1
T = temperature (K)
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19
Q

empirical formula

A

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

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20
Q

molecular formula

A

actual no. of atoms of each type of element in a compound

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21
Q

formula of nitrate ion

A

NO(3)-

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22
Q

formula of carbonate ion

A

CO(3) 2-

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23
Q

formula of sulfate ion

A

SO(4) 2-

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24
Q

formula of hydroxide ion

A

OH-

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25
Q

formula of ammonium ion

A

NH(4) +

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26
Q

formula of zinc ion

A

Zn2+

27
Q

formula of silver ion

A

Ag+

28
Q

acid + base –>

A

salt + water

29
Q

water of crystallisation

A

solid salt that is hydrated water molecules are incorporated into the lattice.
one mol of hydrated salt always has the same no of mols of water of crystalisation.
when they are heated they loose the water becoming anhydrous.

30
Q

Acids

A

proton donors.

when mixed with water release H+

31
Q

Bases

A

proton acceptor

release OH-

32
Q

hydrochloric acid

A

HCl

33
Q

sulfuric acid

A

H2SO4

34
Q

nitric acid

A

HNO3

35
Q

ethanoic acid

A

CH3COOH

36
Q

sodium hydroxide

A

NaOH

37
Q

potassium hydroxide

A

KOH

38
Q

ammonia

A

NH3

39
Q

metal + acid –>

A

metal salt + hydrogen

40
Q

metal oxide + acid –>

A

salt + water

41
Q

Metal hydroxide + acid –>

A

salt + water

42
Q

Metal carbonate + acid –>

A

metal salt + CO2 + water

43
Q

amonia + acid –>

A

amonium salt (NH4something)

44
Q

meniscus

A

the bottom of the curve of water in burrete

45
Q

methyl red indicator

A

turns yellow to red when adding acid to alkali

46
Q

phenolphthalein indicator

A

turns pink to colourless when adding acid to alkali

47
Q

percentage yeild =

A

actual yield/ theoretical yield x 100

48
Q

% atom economy =

A

molecular mass of desired product /
sum of Mr of all product
x 100

49
Q

oxidation number tells you:

A

how many electrons an atom has donated or accepted to form an ion or to form part of a compound.

50
Q

4 rules of oxidation numbers:

A
  1. all uncombined elements have an oxidation no. of 0
    as they haven’t accepted or donated any electrons.
  2. oxidation no. of simple, monotonic ion (consisting of
    one atom) is the same as its charge
  3. for molecular ions the sum of oxidation no. is same as
    overall charge of the ion
  4. for neutral compound the overall oxidation number is 0
    if made up of more than one element each element
    will have own oxidation no.
51
Q

oxidation numbers of oxygen

A 
-2 
except peroxides (O(2) 2-) where it is -1 
and O(2) where it is 0
52
Q

oxidation numbers of hydrogen

A

+1
except metal hydrides MH(x) (M = metal) where its -1
and molecular hydrogen (H2) where its 0

53
Q

roman numerals in name means

A

the oxidation number of the element before it e.g
iron(II) sulfate meaning iron has oxidation no. of +2 formula= FeSO(4)
iron (III) sulfate iron= +3 formula Fe2 (SO4)2

54
Q

oxidation

A

loss of electrons

55
Q

reduction

A

gain of electrons

56
Q

redox reaction

A

where both reduction and oxidation occur simultaneously

57
Q

oxidising agent

A

accepts electrons and gets reduced

58
Q

reducing agent

A

donates electrons and gets oxidised

59
Q

when electrons or lost or gained what happens to oxidation no.

A

oxidation no of an atom will increase by 1 for each electron lost.
oxidation no of an atom will decrease by 1 for each electron gained

60
Q

if oxidation number increases

A

then the element has lost electrons and been oxidised

61
Q

if oxidation number decreases

A

then the element has gained electrons and been reduced

62
Q

metals usually form

A

positive ions by donating electrons

they usually have +ve oxidation no.

63
Q

non metals usually

A

gain electrons

meaning they have -ve oxidation no.

64
Q

metal + acid is a redox reaction because

A

metal atoms are oxidised, losing e- to form +ve metal ions (in salts)
hydrogen ions are reduced, gaining electrons and forming hydrogen molecules
e.g Mg + 2HCl –> MgCl(2) + H(2)
H oxidation no. decreases from +1 to 0
Mg oxidation no. increased from 0 to +2

A level chemistry (5 decks)

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