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CHEMISTRY Module 5: Physical Chemistry And Transition Elements > 5.3.1 Transition Elements > Flashcards

5.3.1 Transition Elements Flashcards

1
Q

Chromium and copper electron configuration

A

4s sub-shell only fills singly

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2
Q

What is a transition element

A

D-block element that form at least one ion with a partially filled d-orbital

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3
Q

What d-block elements don’t classify as transition elements

A

Scandium and zinc
Sc3+ and Zn2+

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4
Q

Properties of transition elements

A

Form compounds in which transition element has different oxidation states
Form coloured compounds
Elements and their compounds can act as catalysts

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5
Q

Use of iron catalyst

A

Haber process, manufacture of ammonia from nitrogen and hydrogen
N2 (g) + 3H2 (g) -> 2NH3 (g)

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6
Q

Use of vanadium (V) oxide (V2O5) (s) catalyst

A

Contact process, production of sulphur trioxide from oxidation of sulphur dioxide
2SO2 (g) + O2 (g) -> 2SO3 (g)

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7
Q

Use of nickel catalyst

A

Hydrogenation of vegetable fats to form margarine

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8
Q

Use of manganese (IV) oxide (s) catalyst

A

Catalytic decomposition of hydrogen peroxide forming oxygen
2H2O2 (aq) -> 2H2O (l) + O2 (g)

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9
Q

Equation for iron as a catalyst

A

S2O82- (aq) + 2I- (aq) -> 2SO42- (aq) + I2 (aq)
Iron as a catalyst:
S2O82- (aq) + Fe2+ (aq) -> 2SO42- (aq) + Fe3+ (aq)
Fe3+ (aq) + 2I- (aq) -> I2 (aq) + Fe2+ (aq)

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10
Q

Equation for Cu2+ as a catalyst

A

Zn (s) + H2SO4 (aq) -> ZnSO4 (aq) + H2 (g)

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11
Q

What is a ligand

A

Molecule or ion that donates a pair of electrons to a central metal ion to form a coordinate bond

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12
Q

What is the coordination number

A

Number of coordinate bond attached to the central metal ion

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13
Q

What’s a monodentate ligand

A

Ligand that can donate one pair of electrons to a central metal ion

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14
Q

Examples of monodentate ligands

A

H2O
NH3
Cl-
CN-
OH-

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15
Q

What’s a bidentate ligand

A

Ligand that can donate two lone pairs of electrons to a central metal ion, forming 2 coordinate bonds

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16
Q

Examples of bidentate ligands

A

Ethandioate (C2O4 2-)
1,2-diaminoethane (NH2CH2CH2NH2)

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17
Q

What is a compound with a coordination number of 6

A

Octahedral (90º)

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18
Q

What is a compound with a coordination number of 4

A

Tetrahedral (109.5º)
Square planar (90º)

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19
Q

Examples of square planar complexes

A

Platinum, palladium, gold
E.g. [Pt(NH3)4]2+

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20
Q

Cis-trans isomerism in square planar complexes

A

Cis: 2 of the same groups are next to eachother (90º)
Trans: 2 of the same groups are opposite eachother (180º)

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21
Q

Cis-trans isomerism in octahedral complexes

A

Cis: two of the same groups are adjacent to eachother (90º)
Trans: two of the same groups opposite each other (180º)

22
Q

Optical isomerism definition

A

Optical isomers (enantiomers) are non-superimposable mirror images of eachother

23
Q

What octahedral complex can undergo optical isomerism

A

The cis isomer

24
Q

How is cis-platin used in medicine

A

Forms platinum complex inside of a cell, binds to DNA, prevents it replicating
[PtCl2(NH3)2]

25
What’s a ligand substitution reaction
One ligand in a complex ion is replaced by another
26
Aqueous copper (II) ions complex ion
Copper (II) sulfate dissolved in water [Cu(H2O)6]2+ Pale blue
27
Excess of aqueous ammonia added to aqueous copper (II) ions
Pale blue to dark blue [Cu(H2O)6]2+ (aq) + 4NH3 (aq) -> [Cu(NH3)4(H2O)2]2+ (aq) + 4H2O (l) Ligand substitution
28
Ammonia dropwise to aqueous copper (II) ions
Initially, pale blue precipitate of Cu(OH)2 formed Precipitate dissolves in excess ammonia to form dark blue solution, [Cu(NH3)4(H2O)2]2+ (aq)
29
Excess concentrated HCl added to aqueous copper (II) ions
Pale blue to yellow [Cu(H2O)6]2+ (aq) + 4Cl- (aq) <=> [CuCl4]2- (aq) + 6H2O (l) Octahedral to tetrahedral Intermediate green colour Adding water = paler blue solution
30
Aqueous chromium (III) ions complex ion
Chromium (III) potassium sulfate ( KCr(SO4)2.12H2O ) dissolved in water [Cr(H2O)6]3+ formed Pale purple If chromium (III) sulfate is dissolved, green solution formed, [Cr(H2O)5SO4]+
31
Addition of aqueous ammonia to aqueous chromium (III) ions
Dropwise: - Grey-green precipitate of Cr(OH)3 formed - Precipitate dissolves in excess ammonia to form [Cr(NH3)6]3+ [Cr(H2O)6]3+ (aq) + 6NH3 (aq) -> [Cr(NH3)6]3+ (aq) + 6H2O (l)
32
How is ligand substitution used in the body
Haemoglobin has 4 protein chains, each has haem molecule with a central metal ion of Fe2+ As blood goes through the lungs, oxygen binds to haemoglobin, oxyhaemoglobin forms which releases oxygen when needed Haemoglobin can bind to carbon dioxide which is carried back to the lungs, where it is released and exhaled Carbon monoxide can bind to Fe2+ ion, forms carboxyhaemoglobin, ligand substitution reaction between oxygen and carbon monoxide, CO binds more strongly than O2 (irreversible)
33
What is a precipitation reaction
Two aqueous solutions containing ions react to form an insoluble ionic solid (precipitate)
34
Cu2+ (aq) with NaOH (aq)
Blue solution reacts to form blue precipitate of copper (III) hydroxide Cu2+ (aq) + 2OH- (aq) -> Cu(OH)2 (s) Insoluble in excess NaOH
35
Fe2+ (aq) with NaOH (aq)
Pale green solution reacts to form green precipitate of iron (II) hydroxide Fe2+ (aq) + 2OH- (aq) -> Fe(OH)2 (s) Insoluble in excess but turns brown at surface in air, Fe2+ to Fe3+ Fe(OH)2 (s) -> Fe(OH)3 (s)
36
Fe3+ (aq) with NaOH (aq)
Pale yellow solution reacts to form orange-brown precipitate of iron (III) hydroxide Fe3+ (aq) + 3OH- (aq) -> Fe(OH)3 (s) Insoluble in excess
37
Mn2+ (aq) in NaOH (aq)
Pale pink solution reacts to form light brown precipitate of manganese (II) hydroxide, darkens in air Mn2+ (aq) + 2OH- (aq) -> Mn(OH)2 (s)
38
Cr3+ (aq) in NaOH (aq)
Violet solution reacts to form grey-green precipitate of chromium (III) hydroxide Cr3+ (aq) + 3OH- (aq) -> Cr(OH)3 (s) Soluble in excess to form dark green solution Cr(OH)3 (s) + 3OH- (aq) -> [Cr(OH)6]3- (aq)
39
Aqueous ammonia with Fe2+
Green precipitate of Iron (II) hydroxide formed, doesn’t dissolve or react further
40
Aqueous ammonia with Fe3+ (aq)
Orange-brown precipitate of Iron (III) hydroxide formed, doesn’t dissolve or react further
41
Mn2+ with aqueous ammonia
Light-brown precipitate of manganese (II) hydroxide formed, doesn’t dissolve or react further
42
Aqueous manganese (II) complex ion
Pale pink solution from manganese (II) sulfate ( MnSO4.4H2O (s) ) [Mn(H2O)6]2+
43
Aqueous iron (III) complex ion
Pale green solution from iron (II) sulfate ( FeSO4.7H2O (s) ) [Fe(H2O)6]2+
44
Aqueous iron (III) complex ion
Yellow solution from FeCl3.6H2O (s) [Fe(H2O)6]3+
45
Aqueous cobalt (III) complex ion with excess HCl
CoCl4 2- Blue solution
46
Redox titration of iron (II) and manganate (VII) ions
Purple (MnO4-) to colourless (Mn2+) MnO4- (aq) + 8H+ (aq) + 5Fe2+ (aq) -> Mn2+ (aq) + 5Fe3+ (aq) + 4H2O (l)
47
Redox titration of iron (III) and iodide ions
Orange-brown (Fe3+) to brown (I2) 2Fe3+ (aq) + 2I- (aq) -> 2Fe2+ (aq) + I2 (aq)
48
Reduction of aqueous dichromate (VI) ions
Orange (Cr2O72-) to green (Cr3+) Cr2O72- (aq) +14H+ (aq) + 3Zn (s) -> 2Cr3+ (aq) + 7H2O (l) + 3Zn2+ (aq)
49
Oxidation of chromium (III) ions
Green (Cr3+) to yellow (CrO42-) 3H2O2 + 2Cr3+ + 10OH- -> 2CrO42- + 8H2O
50
Redox reaction of copper (II) and iodide ions
Pale blue solution (Cu2+) to white precipitate (CuI) in brown solution (I2) 2Cu2+ (aq) + 4I- -> 2CuI (aq) + I2 (s)
51
Disproportionation of copper (I) ions
Forms brown precipitate (Cu) and blue solution (CuSO4) Cu2O (s) + H2SO4 (aq) -> Cu (s) + CuSO4 (aq) + H2O (l)

CHEMISTRY Module 5: Physical Chemistry And Transition Elements (8 decks)

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