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OCR A Chemistry A Level > Module 2 > Flashcards

Module 2 Flashcards

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1
Q

What are isotopes?

A

atoms of the same element with different numbers of neutrons and different masses

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2
Q

What is relative isotopic mass?

A

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

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3
Q

What is relative atomic mass?

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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4
Q

What is the mass number?

A

the number of protons and neutrons in the nucleus; always the biggest number

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5
Q

What is the atomic number?

A

the number of protons

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6
Q

What are ions?

A

atoms that have lost or gained electrons

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7
Q

How do you calculate relative atomic mass?

A

(abundance A x m/z A) + (abundance B x m/z B) / total abundance OR 100 (if % abundance given)

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8
Q

What are some complex ions?

A

OH⁻ (hydroxide)
NO₃⁻ (nitrate)
NH₄⁺ (ammonium)
SO₄²- (sulphate)
CO₃²- (carbonate)
Ag+ (silver)
Zn²⁺ (zinc)

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9
Q

What are spectator ions?

A

ions which aren’t involved in the reaction; they are cancelled out in simplest ionic equations

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10
Q

How to work out moles in solids?

A

n = mass / Mr
mass in grams

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11
Q

How to work out moles in liquids?

A

n = v x c
volume in dm3
concentration in moldm-3

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12
Q

How do you convert from cm3 to dm3 to m3?

A

cm3 to dm3: divide by 1000
dm3 to m3: divide by 1000
cm3 to m3: divide by 1000000

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13
Q

How to work out moles in gases?

A

n = v / 24dm3

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14
Q

What is the ideal gas equation?

A

pV = nRT
pressure in Pa
volume in m3
R (gas constant) is 8.31 JK-1mol-1
temperature in K

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15
Q

What are the standard conditions?

A

`298K
100kPa

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16
Q

What is the empirical formula?

A

the simplest whole number ratio of elements in a compound

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17
Q

How to work out percentage yield?

A

(actual yield / theoretical yield) x 100

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18
Q

How to work out atom economy?

A

(Mr of desired product / Mr of all products) x 100
balance equation and use big numbers when calculating moles

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19
Q

What are acids?

A

proton donors; donate H+ ions which are just protons

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20
Q

What are bases?

A

proton acceptors

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21
Q

What is an alkali?

A

a soluble base; produce OH- ions

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22
Q

What is a weak acid?

A

acids which partially dissociate in solution

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23
Q

What is a strong acid?

A

acids which fully dissociate in solution

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24
Q

What are polyprotic acids?

A

acids which can donate more than 1 proton
e.g. H2SO4 (diprotic) and H3PO4 (triprotic)

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25
Q

What is the overall ionic equation for neutralisation?

A

H+ (aq) + OH- (aq) ⇌ H2O (l)

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26
Q

What is produced when a metal and acid react together?

A

a salt and hydrogen

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27
Q

What is produced when a metal oxide and acid react together?

A

a salt and water

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28
Q

What is produced when a metal hydroxide and acid react together?

A

a salt and water

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29
Q

What is produced when a metal carbonate and acid react together?

A

a salt, water and carbon dioxide

30
Q

What are concordant results?

A

results within 0.10 cm3 of each other

31
Q

How do you work out a titre?

A

titre = final volume - initial volume

32
Q

What colours does the indicator phenolphthalein produce in acids and alkalis?

A

acids = colourless
alkalis = pink

33
Q

What colours does the indicator methyl orange produce in acids and alkalis?

A

acids = red
alkalis = yellow

34
Q

What is oxidation?

A

loss of electrons

35
Q

What is reduction?

A

gain of electrons

36
Q

What is a redox reaction?

A

reactions which involve both reduction and oxidation

37
Q

What happens to reducing agents?

A

they lose electrons and so are oxidised themselves

38
Q

What happens to oxidising agents?

A

they gain electrons and so are reduced themselves

39
Q

What are the oxidation state rules?

A
  • uncombined elements are always 0
  • ions have the same charge as on the ion
  • group 1 is always +1
  • group 2 is always +2
  • aluminium is always +3
  • hydrogen is +1 except in hydrides where it is -1
  • chlorine is -1 except in compounds with F or O where it is +1
  • fluorine is always -1
  • oxygen is -2 except in peroxides where it is -1 and OF2 where it is +2
40
Q

What are the 4 subshells?

A

s-subshell
p-subshell
d-subshell
f-subshell

41
Q

How many orbitals and therefore how many electrons can each subshell hold?

A

s-subshell: 1 orbital; holds 2 electrons
p-subshell: 3 orbitals; holds 6 electrons
d-subshell: 5 orbitals; holds 10 electrons
f-subshell: 7 orbitals; holds 14 electrons

42
Q

How many electrons can be held in shell 1?

A

2 electrons (1s)

43
Q

How many electrons can be held in shell 2?

A

8 electrons (2s, 2p)

44
Q

How many electrons can be held in shell 3?

A

18 electrons (3s, 3p, 3d)

45
Q

How many electrons can be held in shell 4?

A

32 electrons (4s, 4p, 4d, 4f)

46
Q

What shape is the s-orbital?

A

spherical; the 2 electrons can move anywhere within the sphere

47
Q

What shape is the p-subshell?

A

3 orbitals in a dumbbell shape; each orbital holds 2 electrons that can move anywhere within the shape

48
Q

What is spin pairing?

A

when 2 electrons occupy 1 orbital and they spin in opposite directions

49
Q

What are the rules to electron configuration?

A
  • fill 4s before 3d
  • place electrons singularly first then pair up (due to electron repulsion)
50
Q

What are the 2 electron configuration anomalies?

A
  • copper: fully fills 3d before 4s
  • chromium: singularly fills 3d before 4s
51
Q

What is ionic bonding?

A

the electrostatic attraction between positive and negative ions

52
Q

What structure do ionic compounds have?

A

giant ionic lattice structure

53
Q

Do ionic compounds conduct electricity?

A

yes when molten or aqueous; the ions dissociate and so are free to move and carry a charge

54
Q

Do ionic compounds dissolve in water?

A

yes; most do as water molecules are polar and so they attract the positive and negative ions

55
Q

Do ionic compounds have high or low melting points?

A

high; there are many electrostatic forces between the oppositely charged ions so a lot of energy is required to overcome them

56
Q

What is covalent bonding?

A

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

57
Q

What is a dative covalent/coordinate bond?

A

where 1 atom donates both electrons in a shared pair of electrons

58
Q

What are the rules to the shape of molecules?

A
  • bond pairs repel equally
  • lone pairs repel more than bond pairs
  • 2 lone pairs repel even further
59
Q

What is the name and bond angle of molecules with 2 bond pairs?

A

linear; 180°
e.g. BeCl2

60
Q

What is the name and bond angle of molecules with 3 bond pairs?

A

trigonal planar; 120°
e.g. BF3

61
Q

What is the name and bond angle of molecules with 4 bond pairs?

A

tetrahedral; 109.5°
e.g. CH4

62
Q

What is the name and bond angle of molecules with 5 bond pairs?

A

trigonal bipyramidal; 90° and 120°
e.g. PCl5

63
Q

What is the name and bond angle of molecules with 6 bond pairs?

A

octahedral; 90°
e.g. SF6

64
Q

What is the name and bond angle of molecules with 3 bond pairs and 1 lone pair?

A

trigonal pyramidal; 107°
e.g. NH3

65
Q

What is the name and bond angle of molecules with 2 bond pairs and 2 lone pairs?

A

non-linear; 104.5°
e.g. H2O

66
Q

What is electronegativity?

A

the ability of an atom to attract electrons in a bonding pair to itself

67
Q

What is the most electronegative element?

A

fluorine; the closer to fluorine the more electronegative an element is

68
Q

What are induced dipole dipole forces also known as?

A

London forces

69
Q

What are induced dipole dipole forces?

A

when electrons in a molecule/atom form a dipole when they move near to another atom/molecule
the δ+ on 1 atom/molecule becomes attracted to a δ- on another atom/molecule creating a force of attraction; exist in all molecules/atoms regardless of polarity but only exist when 2 molecules/atoms are nearby

70
Q

What are permanent dipole dipole forces?

A

when the δ+ of one molecule is attracted to the δ- on another molecule; only exists in molecules with a polarity and these interactions are permanent

71
Q

What is hydrogen bonding?

A

occurs when hydrogen on 1 molecule forms a bond with the lone pair on nitrogen, oxygen or fluorine on another molecule

72
Q

Name the three intermolecular forces in increasing strength.

A

induced dipole dipole, permanent dipole dipole, hydrogen bonding

OCR A Chemistry A Level (1 decks)

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