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F325 Chemistry > Transition Metals > Flashcards

Transition Metals Flashcards

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1
Q

A transition elements is a d block element that:

A

Forms at least one ion with a partly filled d sub shell.

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2
Q

Transition elements…

A

Cu, Ti, V, Cr, Mn, Fe, Co

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3
Q

D block elements that are not transition elements…

A

Sc and Zn

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4
Q

Why are Sc and Zn not transition elements even though they’re in the D block?

A

Sc3+ is an ion with no d electrons.

Zn2+ has a completely filled d orbital.

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5
Q

Why is 4s electron sub shell filled before 3d?

A

4s orbitals have a lower energy than the 3d, and so is filled first.

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6
Q

What is the electronic configuration of chromium (Z = 24)?

A

1s2 2s2 2p6 3s2 3p6 4s1 3d5

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7
Q

What is the electronic configuration of copper (Z = 29)?

A

1s2 2s2 2p6 3s2 3p6 4s2 3d10

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8
Q

What is the electronic configuration of Cu2+ ion (copper = 29)?

A

1s2 2s2 2p6 3s2 3p6 4s0 3d9

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9
Q

Give 4 properties of transition elements?

A
  1. They form coloured compounds.
  2. They form complex with ligands.
  3. They are good catalysts.
  4. They can show several different oxidation states in their compounds.
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10
Q

Why are transition elements effective catalysts?

A

They can change oxidation state easily.

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11
Q

What is the equation for the Haber process?

A

N2 (g) + 3H2 (g) -> 2NH3 (g)

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12
Q

What is the catalyst in the Haber process?

A

Fe

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13
Q

What is the process that manufactures H2SO4 called?

A

The contact process.

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14
Q

What is the equation for the contact process?

A

2SO2 (g) + O2 (g) -> 2SO3 (g)

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15
Q

What is the catalyst in the hydrogenation of alkenes?

A

Nickel

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16
Q

What is the equation for the decomposition of hydrogen peroxide?

A

2H2O2 (aq) -> 2H2O (l) + O2 (g)

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17
Q

What is the catalyst for the decomposition of hydrogen peroxide?

A

MnO2.

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18
Q

Definition of a ligand.

A

A molecule or ion that can donate a pair of electrons to a transition metal ion.

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19
Q

Definition of coordination number.

A

The total number of coordinate bonds formed between the central metal ion and any ligands.

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20
Q

What is a complex ion?

A

A transition metal ion bonded to one or more ligands by coordinate bonds.

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21
Q

Why does the platin complex ion not have an overall charge?

A

The 2+ charge on platin is cancelled out by the 2Cl-

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22
Q

What is a monodentate ligand?

A

Ligand donates one pair of electrons to central metal ion (forms one coordinate bond).

23
Q

What is a bidentate ligand?

A

Ligand donates 2 pairs of electrons to central metal ion (forms two coordinate bonds).

24
Q

What is the observation of Cu2+ with OH-?

A

Pale blue solution forms pale blue precipitate.

25
Q

What is the observation of Co2+ with OH-?

A

Pink solution forms blue precipitate- turns beige in air.

26
Q

What is the observation of Fe2+ with OH-?

A

Pale green solution forms dark green precipitate- turns brown in air.

27
Q

What is the observation of Fe3+ with OH-?

A

Pale yellow solutions form red/brown precipitate.

28
Q

What is the equation of Cu2+ with OH-?

A

Cu2+ (aq) + 2OH-(aq) -> Cu(OH)2(s)

29
Q

What is the equation of Co2+ with OH-?

A

Co2+ (aq) + 2OH-(aq) -> Co(OH)2(s)

30
Q

What is the equation of Fe2+ with OH-?

A

Fe2+ (aq) + 2OH-(aq) -> Fe(OH)2(s)

31
Q

What is the equation of Fe3+ with OH-?

A

Fe3+ (aq) + 3OH-(aq) -> Fe(OH)3(s)

32
Q

Define ligand substitution.

A

A reaction in which one ligand in a complex ion is replaced by another ligand.

33
Q

What is the observation of Cu2+ with ammonia?

A

Pale blue solution forms light blue precipitate which redissolves to form dark blue solution.

34
Q

What is the equation of Cu2+ with ammonia?

A

[Cu(H2O)6]2+ + 4NH3 -> [Cu(NH3)4(H2O)2]2+ + 4H2O

35
Q

What is the observation of Cu2+ with conc HCl?

A

Pale blue solution changes to a yellow solution and finally a green solution.

36
Q

What is the equation of Cu2+ with conc HCl?

A

[Cu(H2O)6]2+ + 4Cl- -> [Cu(Cl)4]2- + 6H2O

37
Q

What is the observation of Co2+ with conc HCl?

A

Pale pink solution changes to a blue solution.

38
Q

What is the equation of Co2+ with conc HCl?

A

[Co(H2O)6]2+ + 4Cl- -> [CoCl4]2- + 6H2O

39
Q

Define stability constant.

A

The equilibrium constant for the formation of the complex ion from its constituent ions in solution.

40
Q

With reference to oxidation states and colours of compounds, explain why iron is a typical transition metal and aluminium is not.

A

Iron can exist in two different oxidation states- aluminium only one.
Iron can form coloured compounds/solutions- aluminium forms only colourless.

41
Q

What is a coordinate bond?

A

A covalent bond in which both electrons in the shared pair come from the same atom.

42
Q

What shape are 6 coordinate bonds?

A

Octahedral

43
Q

What shape are 4 coordinate bonds?

A

Tetrahedral (sometimes square planar)

44
Q

What is optical isomerism?

A

A type of stereoisomerism- it happens when an ion can exist in two non superimposable mirror images.

45
Q

Why is cis platin so important?

A

It can prevent DNA of cancerous cells reproducing by division.

46
Q

Give an example of 6 coordinate bonds (octahedral shape)

A

[Cu(H2O)6]2+

[Co(NH3)6]2+

47
Q

Give an example of 4 coordinate bonds (tetrahedral shape)

A

[CuCl4]2-

48
Q

Give an example of 4 coordinate bonds (square planar shape)

A

[NiCl2(NH3)2]

49
Q

Cu2+ Reactions…

  • With NaOH
  • With HCl
  • With NH3
A

NaOH
Precipitaiton reaction
Blue to Blue ppt
Cu2+(aq) + 2OH- (aq) -> Cu(OH)2 (s)

HCl
Blue to Green
[Cu(H2O)6]2+ + 4Cl- -> [Cu(Cl)4]2- + 6H2O

NH3 (conc/ excess dilute)
Blue to dark blue
[Cu(H2O)6]2+ + 4NH3 -> [Cu(H2O)2(NH3)4]2+

50
Q

What is cis-platin?

A

A complex of platinum (II) with two chloride ions and two ammonia molecules in a square planar shape.

51
Q

How does cis platin work?

A

The two Cl ligands are easily displaced, so cis platin loses them.
It then bonds to two N atoms on the DNA molecule of the cancerous cell instead.
This block will prevent cancerous reproduction.

52
Q

Give two examples of oxidising agents.

A

KMnO4

K2Cr2O7

53
Q

How do you carry out a redox titration with manganate (VIII) ions as the oxidising agent?

A

Measure out a quantity of reducing agent, eg Fe2+ ions.
Add dilute H2SO4 and
Using a burette, add MnO4- (aq), swirling
Stop when end point is reached
Repeat

54
Q

Write a half equation to show manganate (VII) ions acting as an oxidising agent.

A

MnO4- + 8H+ + 5e- -> Mn2+ + 4H2O
5Fe2+ -> 5Fe3+ + 5e-
MnO4- + 8H+ + 5Fe2+ -> Mn2+ + 4H2O + 5Fe3+

F325 Chemistry (10 decks)

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