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Inorganic Flashcards

(58 cards)

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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

Study These Flashcards
A
  1. lowers activation energy
  2. providing an alternative pathway for the reaction with lower Ea
25
Industrial comments on Haber process
- expensive due to high pressure and temperature conditions - important for NH3 fertilisers/agriculture - 200atm ./ 450C compromise on ROR and yield
26
Pros and cons of alternative fuels
Pros: - sustainable - less pollution than fossil fuels Cons: - slow process - low percentage yield
27
Features and conditions for dynamic equilibrium
1. closed system 2. concentrations of P and R = constant 3. forward reaction rate = backwards rate
28
Le Chatelier's principle
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
Kp and Kc
Kp: - curved brackets - value only affected by change in temp Kc: - square brackets - value only affected by change in temp
30
Bronsted-Lowry acids & bases
Acid: proton donor Base: proton acceptor C.Acid - linked to base C.Base - linked to acid
31
Lewis acid & bases
Acid: electron pair acceptor Base: electron pair donor
32
Predict pH of water at temp > 298K (2019)
1. neutral 2. [H] and [OH-] are equal
33
Explain why scandium isn't a transition metal (2020)
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
Assumptions of Ka = [H+]^2/[A]
1. [HA] = [initial acid] 2. No H+ come from water dissociation
35
Entropy
Total entropy = entropy sys + entropy surr Entropy sys = entropy Pr - entropy Re Entropy surr = -AH/T Feasible when entropy is positive
36
Gibbs free energy
AG= AH - (TAS) Feasible when AG less than 0 AG = -RTlnK
37
Why are bond enthalpy values always positive
Energy input is needed in order to break bonds
38
E cell calculation
OA - RC
39
E cell representation Zn (Ra) and Cu (Oa)
State symbols always included Zn | Zn2+ || Cu2+ | Cu
40
Why is a salt bridge used
Electrons can move without affecting the reactions
41
Limitations of standard E cell calculations for feasibility
1. non standard conditions 2. kinetic factors
42
Fuel cells
Pros: - Produces electrical current without being recharged - environmentally friendly Cons: - hydrogen is very flammable - expensive to produce/make
43
Naming ion complexes
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
Ion colours in limiting NH3
cr(III) - green ppte Fe(II) - green ppte Fe(III) - brown ppte Co(II) = blue ppte Cu(II) - blue ppte
45
Ion colours in excess NH3
cr(III) - purple sltn Fe(II) - no change Fe(III) - no change Co(II) = yellow solution Cu(II) - dark blue solution
46
Ion colours in limiting NaOH
cr(III) - green ppte Fe(II) - green ppte Fe(III) - brown ppte Co(II) = blue ppte Cu(II) - blue ppte
47
Ion colours in excess NaOH
cr(III) - green sltn Fe(II) - no change Fe(III) - no change Co(II) - no change Cu(II) - no change
48
Vanadium oxidation states & colours
You Better Get Vanadium
49
Why is a chromium ion coloured
1. Has a partially filled d-orbital 2. so electrons can be promoted
50
Outline heterogenous catalysts function
1. adsorption onto catalyst active site on surface 2. bonds are weakened 3. products desorbed from catalyst surface
51
Outline homogenous catalysts function
1. combination with reactions to produce intermediate 2. enthalpy change of formation of intermediate is low 3. Ea reduced
52
Autocatalysis & catalyst poisoning
Auto - when a product acts a catalyst Poisoning - when impurities block active sites of heterogenous catalysts
53
Outline TOF Mass spec process
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
Outline TLC
Procedure on layer of silica, not paper Movement measured using UV
55
Outline GLC
- powdered substance used as stationary phase - High pressure gas used as mobile phase - useful for separating volatile liquids
56
Outline column chromatography
- Mobile and stationary phases in a column - retention times depend on sample's affinity to stationary phase
57
Outline 1H NMR spec
Integration trace - number of H in that environment Singlet - No H on adjacent C Doublet - 1 H on adjacent C Continues
58
Outline enantiomers & optical isomerism
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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