Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

A-Levels > Chemistry Inorganic > Flashcards

Chemistry Inorganic Flashcards

1
Q

Tetrahedral bond shape

A

109.5, 4 bonding, 0 lone

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Pyramidal bond shape

A

107, 3 bonding, 1 lone

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Non-linear bond shape

A

104.5, 2 bonding, 2 lone

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Pauling electronegativity on Periodic Table

A

increases up and to the right (as highest nuclear charge, lowest atomic radius)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Pauling electronegativity range for polar covalent

A

0 to 1.8

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Why water is less dense as ice

A

each water molecule can form 4 hydrogen bonds
- H bonds extend outwards, holding water slightly apart and forming an open tetrahedral lattice full of holes
- holes decrease density

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Ionisation energies down a group

A

decrease, as radius increases, shielding increases, so nuclear attraction decreases, so force of electrostatic attraction lower

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Ionisation energies across a period

A

increase, as shielding same, nuclear charge increases, radius decreases, so electrostatic attraction stronger

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Giant covalent structures

A

Boron, Carbon, Silicon

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Simple molecular structures

A

P4, S8, F2, N2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Group 2 reactivity down group

A

increases (stronger reducing agents), ionisation energies decrease down group as more shielding and lower nuclear charge

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Group 2 hydroxide solubility and pH down group

A

higher solubility and pH, as more reactive i guess

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Halogen reactivity down group

A

decreases, radius increases, more shielding, so less nuclear attraction to capture electrons from another species, weaker oxidising agents

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Halogen colours in water

A

chlorine - pale green
bromine - orange
iodine - brown

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Halogen colours in cyclohexane

A

chlorine - pale green
bromine - orange
iodine - violet

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Order of tests

A

carbonate, sulfate, halide

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

NH4+ test

A

add NaOH, warm, gas will turn red moist pH paper blue

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Enthalpy formation

A

enthalpy change of 1 mol of compound is formed from elements with everything in standard states

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Enthalpy combustion

A

1 mol of substance reacts completely with oxygen

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Enthalpy neutralisation

A

energy change of acid and base reacting to form 1 mol of water, always -57

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Enthalpy bond breaking

A

positive, endothermic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

adsorption

A

weakly bonding to surface of catalyst

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

Concentration-time graphs

A

zero - straight line -m
first+ - concave down (first has constant half-life)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Rate-concentration graphs

A

zero - horizontal straight
first - straight line +m
second - concave up

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

Iodine clock reaction

A

turns blue-black at end-point, no more sodium thiosulfate so iodine no longer used up as it forms, so turns starch indicator blue-black

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

water specific heat capacity (JK-1g-1)

A

4.18 NOT 4.2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

Bronsted-Lowry acid

A

proton donor

28
Q

Bronsted-Lowry base

A

proton acceptor

29
Q

hydronium ion

A

H3O+

30
Q

Ka, pKa, and acid strength

A

higher Ka, lower pKa, stronger acid

31
Q

Weak acid approximations

A

H+ eqm = A- eqm
HA eqm = HA start

32
Q

Weak acid buffer

A

weak acid and conjugate base

33
Q

How to select indicator

A

pH range should be entirely within equivalence point (vertical line on graph)

34
Q

Methyl orange

A

pH range 4-2, yellow at 4, red at 2

35
Q

Phenolphthalein

A

pH range of 10-8, pink/purple at 10, white at 8

36
Q

Type of titration where no indicator suitable

A

Weak acid, weak base
this is because no vertical section

37
Q

Lattice enthalpy

A

enthalpy change of formation of 1 mol of an ionic compound from gaseous ions under standard conditions

38
Q

Atomisation enthalpy

A

enthalpy of 1 mol of gaseous atoms formed the element in its standard state [always endothermic]

39
Q

2nd electron affinities are…

A

endothermic, as energy is required to force another electron onto the negative ion

40
Q

Solution enthalpy

A

enthalpy change when 1 mol of a solute dissolves in a solvent

41
Q

Hydration enthalpy

A

enthalpy of 1 mol of aqueous ions formed from 1 mol of gaseous ions
- down halogens becomes less exothermic (more positive) as ion size greater so attraction to water weaker

42
Q

Ionic size and lattice enthalpy

A

as ionic radius increases, attraction between ions decreases, lattice energy less negative, m.p. decreases

43
Q

Ionic charge and lattice enthalpy

A

ionic charge increases, attraction between ions increases, lattice energy more negative, m.p. increases

44
Q

Ionic size and hydration enthalpy

A

ionic radius increases, attraction between ion and water molecules decreases, hydration energy less negative

45
Q

Ionic charge and hydration enthalpy

A

ionic charge increases, attraction with water molecules increases, hydration energy becomes more negative

46
Q

predicting solubility

A

if sum of hydration enthalpies is larger than magnitude of lattice enthalpy, overall enthalpy change of solution will be exothermic and compound should dissolve

47
Q

d-block elements with 1 4s electron, rest have 2

A

chromium and copper

48
Q

d-block, not transition

A

zinc and scandium

49
Q

transition metal catalysts

A

iron in Haber process, V2O5 (vanadium(V) oxide) in Contact process [sulfur trioxide from sulfur dioxide and oxygen]

50
Q

chromium oxidation state colours

A

Cr(III) - green, Cr(VI) - yellow/orange

51
Q

Cu2+ and NaOH

A

blue solution reacts to form blue precip. of copper(II) hydroxide, insoluble in excess NaOH

52
Q

Fe2+ and NaOH

A

pale green solution reacts to form green precip. of iron(II) hydroxide, insoluble in excess NaOH
HOWEVER turns brown at surface as iron oxidised to iron(III)

53
Q

Fe3+ and NaOH

A

pale yellow solution reacts to form orange-brown precip of iron(III) hydroxide, insoluble in excess NaOH

54
Q

Mn2+ and NaOH

A

pale pink solution reacts to form light brown precip. of manganese(II) hydroxide which darkens in air, insoluble in excess NaOH

55
Q

Cr3+ and NaOH

A

violet solution reacts to form grey-green precip. of chromium(III) hydroxide, precipitate is SOLUBLE in excess NaOH and forms dark green solution (hexa-hydroxide chromium complex)

56
Q

Cu2+ and ammonia

A

copper(II) hydroxide (blue precip.) dissolves in excess ammonia to form deep blue solution with 4 ammonia ligands and 2 water ligands

57
Q

Cr3+ and ammonia

A

green precip. Cr(OH)3 dissolves in excess ammonia to form hexa-ammonia complex which is a purple solution

58
Q

Fe2+, Fe3+, Mn2+ with ammonia

A

same as NaOH, form hydroxide precipitates and do not dissolve in excess ammonia

59
Q

CuI

A

white solid

60
Q

pH buffer if volume changed

A

same

61
Q

acidic buffer

A

excess WEAK acid, strong alkali

62
Q

conjugate acid base pair for blood

A

carbonic acid, HCO3-

63
Q

salt bridge

A

completes circuit, allows ions to flow BUT doesn’t allow solutions to mix

64
Q

weak acid/base titrations

A

no indicator as no sharp pH change, colour changes too gradual

65
Q

average bond enthalpy

A

average amount of energy needed to break 1 mole of bonds in gaseous state

66
Q

Kp

A

does not change with pressure, does with temperature

67
Q
A

A-Levels (4 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions