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Chemistry > Inorganic > Flashcards

Inorganic Flashcards

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1
Q

Shapes of molecules and bond angle

A

Linear - 180, 2BP 0LP
Bent - 104.5, 2BP 2LP
Trigonal planar - 120, 3BP
Trigonal pyramidal - 107, 3BP 1LP
Tetrahedral - 109.5, 4BP
Trigonal bipyramidal - 90 & 120, 5BP 0LP
Octahedral - 90 & 180, 6BP

Electrons repel to point of max separation/minimum repulsion

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2
Q

Outline 3 types of IMF

A

PDPD < IDPDP < H Bonding
IDPDP - Temporary dipole in 1 molecule creates induced dipole in near molecules
PDPD - interactions between partial +ve /-ve charges between polar molecules
H bonding - when H is directly bonded to O/N/F

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3
Q

Simple molecular vs Giant covalent

A

Simple molecular:
- lots of molecules
- weak intermolecular forces between discrete molecules
- does not require a lot of energy to break
Giant covalent:
- lattice of atoms
- M,S, CB T R A L O E T B

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4
Q

Diamond / Graphite / Graphene

A

Diamond:
- M,S,CB T R A L O E T B
- each C atom covalently bonded to 4 other C atoms
Graphite:
- M,S,CB T R A L O E T B
- each C atom covalently bonded to 3 other C atoms
- delocalised electrons between layers
- able to conduct electricity
Graphene:
- M,S CB T R A L O E T B
- each C atom covalently bonded to 3 other C atom

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5
Q

Trend of atomic radius across period

A
  • Decreases
  • Increased nuclear charge with similar shielding
  • outer electrons more strongly attracted to nucleus
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6
Q

Trend of atomic radius down group

A
  • Increases
  • more quantum shells so more shielding
  • electrons further away from nucleus
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7
Q

Trend of IE across period

A
  • Increases
  • increasing nuclear charge
  • similar shielding
  • electrons more attracted to nucleus
  • more energy required to remove
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8
Q

Trend of IE down group

A
  • Decreases
  • increasing atomic/ionic radius
  • electrons less strongly attracted to nucleus
  • less energy required to remove electron
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9
Q

Trend of bond length down group

A
  • increases
  • increasing atomic radius across group
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10
Q

Why S IE less than O IE

A
  • electron removed is paired in p-orbital
  • electrons have opposite spins and repel each other
  • less energy required to remove electron
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11
Q

Differences between experimental and theoretical lattice energies

A

High difference:
- large difference due to covalent character
- state ion charge and high charge density
- large anion size
- anion electron cloud easily distorted

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12
Q

Group 7 boiling point trend

A
  • Increases
  • increasing electrons down group
  • stronger london forces
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13
Q

Group 2 thermal stability trend

A
  • increases
  • ions have lower charge density
  • less polarising power
  • distorts anion electron cloud less
  • less energy required to break bond
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14
Q

Group 2 hydroxide solubility trend

A
  • increases down the group
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15
Q

What does similar experimental and theoretical lattice energies mean

A
  • bonding is almost 100% ionic
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16
Q

Group 2 sulphate trend

A
  • increases down the group
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17
Q

Outline Flame Test Procedure

A
  1. dip Pt loop in concentrated HCl
  2. dip into sample
  3. hold under non-luminous flame
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18
Q

Why can you not double C-C bond enthalpy to get C=C bond enthalpy

A
  • C=C weaker than 2x C-C bonds
  • made up of pi & sigma bonds, 2x sigma
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19
Q

How flame colours are created

A
  1. heat excites e- to higher energy level
  2. electrons de-excited back to original level
  3. energy lost via photon of light
  4. photon of light is colour
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20
Q

Silver halide precipitates

A

White - Cl
Cream - Br
Yellow - I

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21
Q

Flame colours

A

Li - red
Na - yellow-orange
K - lilac
Rb - red
Cs - blue-violet
Ca - orange-red
Sr - crimson
Ba - pale green
Cu - blue green with white flashes
Pb - greyish white

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22
Q

Describe action of catalytic converter

A
  1. influx of harmful gases (CO, NO)
  2. rhodium catalyst converts gases to CO2 and N2
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23
Q

Outline changes to MB model

A

Temp increase: (Decrease is opposite)
- Shifts curve to the right and lower
- Greater proportion of particles have energy greater than Ea

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24
Q

Outline how catalysts function

A
  1. lowers activation energy
  2. providing an alternative pathway for the reaction with lower Ea
25
Q

Industrial comments on Haber process

A
  • expensive due to high pressure and temperature conditions
  • important for NH3 fertilisers/agriculture
  • 200atm ./ 450C compromise on ROR and yield
26
Q

Pros and cons of alternative fuels

A

Pros:
- sustainable
- less pollution than fossil fuels
Cons:
- slow process
- low percentage yield

27
Q

Features and conditions for dynamic equilibrium

A
  1. closed system
  2. concentrations of P and R = constant
  3. forward reaction rate = backwards rate
28
Q

Le Chatelier’s principle

A

Temperature:
increase temperature favours endothermic side &VV
Pressure:
increase pressure favours side w/ fewer moles of gas &VV
Concentration:
increase [reactants] favours reaction producing products &VV
Catalyst:
- no effect on POE
- increases ROR of fwd and bwd reaction

29
Q

Kp and Kc

A

Kp:
- curved brackets
- value only affected by change in temp
Kc:
- square brackets
- value only affected by change in temp

30
Q

Bronsted-Lowry acids & bases

A

Acid: proton donor
Base: proton acceptor
C.Acid - linked to base
C.Base - linked to acid

31
Q

Lewis acid & bases

A

Acid: electron pair acceptor
Base: electron pair donor

32
Q

Predict pH of water at temp > 298K (2019)

A
  1. neutral
  2. [H] and [OH-] are equal
33
Q

Explain why scandium isn’t a transition metal (2020)

A
  1. last electron added is in d subshell
  2. so is a d block element
  3. does not form a stable ion with a partially filled d subshell
  4. state ionic electronic configuration
  5. state full or empty subshell
34
Q

Assumptions of Ka = [H+]^2/[A]

A
  1. [HA] = [initial acid]
  2. No H+ come from water dissociation
35
Q

Entropy

A

Total entropy = entropy sys + entropy surr
Entropy sys = entropy Pr - entropy Re
Entropy surr = -AH/T
Feasible when entropy is positive

36
Q

Gibbs free energy

A

AG= AH - (TAS)
Feasible when AG less than 0
AG = -RTlnK

37
Q

Why are bond enthalpy values always positive

A

Energy input is needed in order to break bonds

38
Q

E cell calculation

A

OA - RC

39
Q

E cell representation
Zn (Ra) and Cu (Oa)

A

State symbols always included
Zn | Zn2+ || Cu2+ | Cu

40
Q

Why is a salt bridge used

A

Electrons can move without affecting the reactions

41
Q

Limitations of standard E cell calculations for feasibility

A
  1. non standard conditions
  2. kinetic factors
42
Q

Fuel cells

A

Pros:
- Produces electrical current without being recharged
- environmentally friendly
Cons:
- hydrogen is very flammable
- expensive to produce/make

43
Q

Naming ion complexes

A
  1. Number of ligands
  2. Molecule attached to ligand
  3. Metal ion centre
  4. charge in roman numerals
    E.g [hexaaquacopper(II)]2+ion
44
Q

Ion colours in limiting NH3

A

cr(III) - green ppte
Fe(II) - green ppte
Fe(III) - brown ppte
Co(II) = blue ppte
Cu(II) - blue ppte

45
Q

Ion colours in excess NH3

A

cr(III) - purple sltn
Fe(II) - no change
Fe(III) - no change
Co(II) = yellow solution
Cu(II) - dark blue solution

46
Q

Ion colours in limiting NaOH

A

cr(III) - green ppte
Fe(II) - green ppte
Fe(III) - brown ppte
Co(II) = blue ppte
Cu(II) - blue ppte

47
Q

Ion colours in excess NaOH

A

cr(III) - green sltn
Fe(II) - no change
Fe(III) - no change
Co(II) - no change
Cu(II) - no change

48
Q

Vanadium oxidation states & colours

A

You Better Get Vanadium

49
Q

Why is a chromium ion coloured

A
  1. Has a partially filled d-orbital
  2. so electrons can be promoted
50
Q

Outline heterogenous catalysts function

A
  1. adsorption onto catalyst active site on surface
  2. bonds are weakened
  3. products desorbed from catalyst surface
51
Q

Outline homogenous catalysts function

A
  1. combination with reactions to produce intermediate
  2. enthalpy change of formation of intermediate is low
  3. Ea reduced
52
Q

Autocatalysis & catalyst poisoning

A

Auto - when a product acts a catalyst
Poisoning - when impurities block active sites of heterogenous catalysts

53
Q

Outline TOF Mass spec process

A
  1. Ionisation - vaporisation and e- removed, making 1+ ions
  2. Acceleration towards -ve plate
  3. Deflection - deflected into curved path
  4. Detection - gain electron when hit the detection plate, producing flow
  5. Analysis
54
Q

Outline TLC

A

Procedure on layer of silica, not paper
Movement measured using UV

55
Q

Outline GLC

A
  • powdered substance used as stationary phase
  • High pressure gas used as mobile phase
  • useful for separating volatile liquids
56
Q

Outline column chromatography

A
  • Mobile and stationary phases in a column
  • retention times depend on sample’s affinity to stationary phase
57
Q

Outline 1H NMR spec

A

Integration trace - number of H in that environment
Singlet - No H on adjacent C
Doublet - 1 H on adjacent C
Continues

58
Q

Outline enantiomers & optical isomerism

A
  1. Chiral carbon centre makes trigonal planar carbocation intermediate
  2. Equal chance of nucleophile attack above and below carbocation
  3. Produces racemic mix of 2 enantiomers
  4. do not rotate plane polarised light

Chemistry (6 decks)

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