CL 24- transition metals Flashcards

1
Q

electron configuration of Cr

A

1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d⁵

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2
Q

electron configuration of Cu

A

1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d¹⁰

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3
Q

transition metal

definition

A
  • a d-block element that has an ion with an incomplete d-sub-shell
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4
Q

colours of Cu²⁺ and Mn²⁺

A

blue and pale pink

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5
Q

two examples of transition-metal elements that form compounds with more than one oxidation state

A
  • Fe²⁺ / Fe³⁺
  • Mn²⁺ / MnO₄⁻
  • Cu²⁺ / Cu⁺
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6
Q

ligand

definition

A
  • a species that can donate one or more lone pairs to form dative covalent bonds to a central metal ion forming a complex ion
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7
Q

monodentate ligand examples

A
  • only form one dative covalent bond
  • H₂O
  • NH₃
  • OH⁻
  • Cl⁻
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8
Q

bidentate ligand examples

A
  • forms two dative covalent bonds
  • ethane-1,2-diamine
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9
Q

complex ion

definition

A
  • a central transition metal bonded to one or more electron donating species (ligands) by dative covalent bonds, from the ligand to the metal
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10
Q

coordination number

definition

A
  • the no. of dative covalent bonds between the ligands and the central metal ion
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11
Q

octahedral complex ion

reasoning for shape, example of complex ion

A
  • element connected to central metal ion in period 2, so there is room for 6 dative covalent bonds
  • e.g. H₂O, NH₃
  • [Cr (H₂O) ₆] ³⁺
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12
Q

tetrahedral complex ion

reasoning for shape, example of complex ion

A
  • element connected to central metal ion in period 3, larger donor atoms so there is only room for 4 dative covalent bonds
  • Cl
  • [Cu (Cl) ₄] ²⁻
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13
Q

square planar complex ion

reasoning for shape, example of complex ion

A
  • an exception to the rule, only with Pt and Ni
  • 4 ligands attached
  • [Pt (Cl) ₂ (NH₃)₂ ]
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14
Q

linear complex ions

A
  • only Ag with 2 donor atoms
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15
Q

cis-trans isomerism (only) in complex ions

when does it occur

A
  • in an octahedral complex, monodentate ligands - 4 of one, and 2 another
  • square planar complex, monodentate ligands- 2 of each
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16
Q

optical isomerism (only) in complex ions

A
  • octahedral complex
  • 3 bidentate ligands
17
Q

optical and cis-trans isomerism in complex ions

A
  • octahedral complex
  • 2 bidentate ligands and 2 monodentate ligands
  • 3 different isomers- trans isomer doesn’t have optical isomerism
18
Q

cis-platin

idk if you need to know this

A
  • [Pt (Cl)₂ (NH₃) ₂ ]
  • attacks tumours, and in many cases it works to shrink the tumour, but it has many unpleasant side effects and can lead to kidney damage
19
Q

ligand substitution reactions for adding NH₃ to Cu²⁺ (in water)

first precipitation reaction, then ligand substitution with excess NH₃

A
  • [Cu (H₂O)₆ ] ₍ₐ₎+ 2NH₃ ₍ₐ₎ –> [Cu (OH)₂ (H₂O)₄ ] ₍ₛ₎ +2NH₄⁺₍ₐ₎
  • pale blue solution to pale blue precipitate (initially)
  • [Cu (H₂O)₆ ] ₍ₐ₎ + 4NH₃ ₍ₐ₎ –> [Cu (NH₃)₄ (H₂O)₂ ] ²⁺₍ₐ₎ + 4H₂O₍ₗ₎
  • pale blue solution to dark blue solution
20
Q

ligand substitution reactions for adding HCl to Cu²⁺ (in water)

A
  • [Cu (H₂O)₆ ] + 4Cl⁻ –> [CuCl₄]²⁻ + 6H₂O
  • pale blue solution to yellow solution
21
Q

ligand substitution reactions for adding with NH₃ with Cr³⁺

first precipitation reaction, then ligand substitution with excess NH₃

A
  • [Cr (H₂O)₆ ] ³⁺ + 3NH₃ –> [Cr (H₂O)₃ (OH)₃ ] + 3NH₄⁺
  • violet solution to grey precipitate
  • [Cr (H₂O)₆ ] ³⁺ + 6NH₃ –> [Cr (NH₃) ₆ ] ³⁺ + 6H₂O
  • violet solution to purple solution
22
Q

importance of iron in haemoglobin

A
  • Fe has 4 dative bonds with N atoms on haem, and 1 dative bond to the protein globin
  • this leaves 1 space for carrying O₂ or CO
  • O₂ reversibly binds to the Fe ion; however if O₂ levels are low, water is susbtituted instead
  • if CO is present, this will bind over to O₂ as it binds more strongly than oxygen, and binds irreversibly
  • if conc of carboxyhaemoglobin becomes too high, O₂ transport is prevented, leading to death
23
Q

precipitation reaction with NaOH/NH₃
Cu²⁺

A
  • Cu²⁺ + 2OH⁻ –> Cu (OH)₂
  • blue solution to blue precipitate
  • Cu also reacts with excess NH₃ (ligand substitution reaction)
24
Q

precipitation reaction with NaOH/NH₃
Fe²⁺

A
  • Fe²⁺ + 2OH⁻ –> Fe (OH) ₂
  • pale green solution to green precipitate
25
precipitation reaction with NaOH/NH₃ Fe³⁺
* Fe³⁺ + 3OH⁻ --> Fe (OH)₃ * yellow solution to orange precipitate
26
precipitation reaction with NaOH/NH₃ Mn²⁺
* Mn²⁺ + 2OH⁻ --> Mn (OH) ₂ * pale pink solution to pale brown solution
27
precipitation reaction with NaOH/NH₃ Cr³⁺
* Cr³⁺ + 3OH⁻ --> Cr (OH)₃ * violet solution to grey precipitate * Cr reacts with excess NH₃ in a ligan substitution reaction
28
oxidation of Fe²⁺/Fe³⁺ and reduction of MnO₄⁻/Mn²⁺ form overall equation and state colour changes
* 5Fe²⁺ + MnO₄⁻ + 8H⁺ --> Mn²⁺ + 5Fe³⁺ + 4H₂O * purple solution to colourless solution (Mn)
29
oxidation of I⁻/I₂ and reduction of Fe³⁺/Fe²⁺ form overall equation and state colour changes
* 2Fe³⁺ + 2I⁻ --> 2Fe²⁺ + I₂ * orange solution to pale green solution (Fe) and I₂ is brown
30
oxidation of Cr³⁺/CrO₄²⁻ and reduction of H₂O₂/OH⁻ form overall equation under alkaline conditions
* 3H₂O₂ + 2Cr³⁺ + 10OH⁻ --> 2CrO₄²⁻ + 8H₂O
31
oxidation of Zn/Zn²⁺ and reduction of Cr₂O₇²⁻/Cr³⁺ form overall equation and state colour changes explain what happens when excess Zn added
* 3Zn + Cr₂O₇²⁻ + 14H⁺ --> 3Zn²⁺ + 2Cr³⁺ + 7H₂O * orange solution to green solution (Cr) * when excess Zn is added, Cr³⁺ ions are reduced further to Cr²⁺ Zn + 2Cr³⁺ --> Zn²⁺ + 2Cr²⁺ green solution to blue solution (Cr)
32
write an equation for the reaction of Cu²⁺ with I⁻ state colour changes associated with this reaction
* 2Cu²⁺ + 4I⁻ --> 2CuI + I₂ * pale blue solution to white precipitate (Cu) and I₂ is brown