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Chemistry Module 5 > Chapter 3 Transition metals > Flashcards

Chapter 3 Transition metals Flashcards

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1
Q

What are transition metals?

A

Metals that form at least 1 ion with a partially filled d subshell

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2
Q

Which block of the periodic table are transition metals most commonly a part of?

A

d block

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3
Q

Which metals are in the d block but are not transition metals?

A

Scandium and Zinc as they don’t form at least one ion with a partially filled d subshell

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4
Q

Which transition metals are exceptions to Hund’s rule?

A

Chromium (Cr) - 4s1, 3d5
Copper (Cu) - 4s1, 3d10

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5
Q

What are some chemical properties of transition metals?

A
  • variable oxidation states
  • form coloured solutions when dissolved in water (coloured ions)
  • can act as catalysts
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6
Q

What are some physical properties of transition metals?

A
  • high melting/ boiling point
  • high densities
  • conduct electricity
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7
Q

What is a disadvantage of using transition metals as catalysts?

A

Health hazard due to toxicity of transition metals

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8
Q

What are some examples of transition metals being used as industrial catalysts?

A
  • Iron catalyst in Haber process (N2 + 3H2 → 2NH3)
  • Nickel catalyst in hydrogenation of alkenes
  • Vanadium(V) oxide/ V2O5 catalyst in contact process (2SO2 + O2 →2SO3)
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9
Q

What is a ligand?

A

A molecule/ ion that can donate a pair of electrons to the central transition metal ion to form a coordinate bond.

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10
Q

What is a complex ion?

A

Transition metal ion bonded to one or more ligands by dative covalent bonds

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11
Q

What is a monodentate ligand?

A

Ligand that donates one lone pair to form one dative covalent bond with a transition metal.

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12
Q

What is a multidentate ligand?

A

Ligand that uses more than one lone pair to form more than one dative covalent bond with a transition metal.

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13
Q

What is a bidentate ligand?

A

Ligand that uses 2 lone pairs to form 2 dative covalent bonds with a transition metal.

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14
Q

What is the coordination number?

A

The number of dative covalent bonds formed between ligands and a central transition metal

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15
Q

What is the name of the shape of a molecule with 4 monodentate ligands in the same plane bonded to a central metal atom?

A

Square planar

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16
Q

Examples of monodentate ligands?

A
  • H2O
  • NH3
  • Cl-
  • CN-
  • SCN-
  • OH-
  • NO2-
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17
Q

Examples of bidentate ligands?

A
  • NH2
  • CH2CH2NH2 (ethane-1,2-diamine)
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18
Q

What colour is Cu2+?

A

blue

19
Q

What colour is Fe2+?

A

green

20
Q

What colour is Fe3+?

A

yellow

21
Q

What colour is Mn2+?

A

pink

22
Q

What colour is Cr3+?

A

violet (or green)

23
Q

What are the conditions for stereoisomerism in an octahedral complex?

A
  • 4 of one monodentate ligand and 2 of another
  • 3 of one monodentate ligand and 3 of another
  • 2 of one bidentate ligand and 2 monodentate
24
Q

What conditions for stereoisomerism in square planar molecules?

A

2 of one monodentate ligand and 2 of another

25
Q

What are conditions for optical isomerism in an octahedral complex?

A
  • 2 bidentate ligands and 2 monodentate ligands - cis isomer
  • 3 bidentate ligands
26
Q

What is the structure of cis platin?

A

[PtCl2(NH3)2]

27
Q

What is cis-platin used for and how does it work?

A

Used as a cancer treatment.
It works by dissociation of chloride ions and Pt(NH3)2 binding to DNA, stopping the DNA from separating and being able to duplicate during cell division, causing the cell to die.

28
Q

What can ligand substitution cause a change in?

A
  • colour
  • coordination number
  • coordination geometry (shape)
29
Q

What is meant by amphoteric?

A

Acts as a base and an acid

30
Q

How does ligand substitution occur in haemoglobin?

A

Each haemoglobin contains 4 Fe2+ ions and each Fe2+ ion is present as an octahedral complex ion. 4 of the lone pairs come from Nitrogen atoms, the 5th is from a nitrogen on the protein globin and the 6th is a weakly bonded water molecule. In the lungs O2 concentration is so high, the water ligand is substituted for an oxygen molecule, forming oxyhaemaglobin.

31
Q

What is the issue with breathing in CO in terms of haemaglobin?

A

The haemoglobin swaps its water ligand for a CO ligand forming carboxyhaemaglobin. CO is a strong ligand so doesn’t readily exchange with oxygen or water ligands so haemoglobin can’t transport oxygen.

32
Q

What is an example of a change in geometry as a result of substitution and why does this occur?

A
  • This occurs because the ligands are different sizes
  • [Cu(H2O)6]2+ + 4Cl- ⇌ [CuCl4]2- + 6H2O
  • octahedral & pale blue ⇌ tetrahedral & yellow
33
Q

What is an example of a ligand substitution with excess ammonia?

A

[Cr(H2O)6]3+ + 6NH3 ⇌ [Cr(NH3)6]3+ + 6H2O
octahedral & violet ⇌ octahedral & purple

34
Q

How does Cu2+ react with excess ammonia?

A
  • Partial substitution
    [Cu(H2O)6]2+ + 4NH3 ⇌ [Cu(NH3)4(H2O)2]2+ + 4H2O
    octahedral & pale blue ⇌ octahedral & deep blue
35
Q

What colour precipitate is formed when Cu2+ reacts with NaOH?

A

(pale blue solution to) deep blue precipitate

36
Q

What colour precipitate is formed when Fe2+ reacts with NaOH or aqueous ammonia?

A

(pale green solution to) green precipitate

37
Q

What colour precipitate is formed when Fe3+ reacts with NaOH or aqueous ammonia?

A

(yellow solution to) orange precipitate

38
Q

What colour precipitate is formed when Mn2+ reacts with NaOH or aqueous ammonia?

A

(pale pink solution to) brown precipitate

39
Q

What colour precipitate is formed when Cr3+ reacts with NaOH or aqueous ammonia?

A

(green solution to) grey-green precipitate

40
Q

What is the equation for the reduction of Fe3+ to Fe2+ using iodide, including colours?

A

2Fe3+ + 2I- → 2Fe2+ + I2
rust → brown

41
Q

What is the equation for the oxidation of Fe2+ to Fe3+ using manganate, including colours?

A

5Fe2+ + 8H+ + MnO4- → 5Fe3+ + Mn2+ + 4H2O
dark purple → pink

42
Q

What is the equation for the oxidation of Cu+ to Cu2+, including colours?

A

2Cu+ → Cu2+ + Cu
colourless → blue

43
Q

What is the equation for the reduction of Cu2+ to Cu+ using iodide, including colours?

A

2Cu2+ + 4I- → 2CuI + I2
Pale blue → Brown

Chemistry Module 5 (3 decks)

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