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Chemistry > transition metals > Flashcards

transition metals Flashcards

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1
Q

properties of d-block elements

A
  • high MP/BP
  • shiny
  • conduct electricity + heat
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2
Q

what elements have special cases in electron configuration

A
  • chromium and copper
  • 3d fills before 4s so they both have 1 e- in 4s
  • reason : stability
  • half filled 3d5 and full 3d10 gives additional stability to chromium and copper
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3
Q

define transition elements

A
  • d-block elements that form at least one ion with a partially filled d-orbital
  • scandium and zinc are d-block but no t-metals
  • Sc3+ forms empty d-orbital
  • Zn2+ forms full d-orbital
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4
Q

properties of transition metals

A
  • form compounds where the t-elements has a diff Ox. state
  • form coloured compounds
  • catalysts
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5
Q

transition metals as catalysts

A
  • Haber process - iron catalyst
  • contact process to form sulphur trioxide (SO3) from oxidation of sulphur dioxide - vanadium (V) oxide catalyst (V2O5).
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6
Q

Cu2+ with:

  • NaOH
  • excess NaOH
A
  • blue solution to blue precipitate of Cu(OH)2

- no change bc ppt = insoluble

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7
Q

Fe2+ with:

  • NaOH
  • excess NaOH
A
  • pale green solution to green ppt of Fe(OH)2 (brown when exposed to air Fe(OH)3)
  • no change , ppt = insoluble
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8
Q

Fe3+ with:

  • NaOH
  • excess NaOH
A
  • pale yellow sol to orange/brown ppt

- no change , ppt = insoluble

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9
Q

Mn2+ with :

  • NaOH
  • excess NaOH
A
  • pale pink sol to light brown ppt (darkens on standing)

- no change , ppt = insoluble

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10
Q

Cr3+ with:

  • NaOH
  • excess NaOH
A
  • green solution to grey/green precipitate

- in excess = dark green Cr(OH)6

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11
Q

Fe2+

  • NH3
  • excess NH3
A
  • no reaction bc don’t dissolve

- pale green to green

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12
Q

Fe3+

  • NH3
  • excess NH3
A
  • no reaction bc don’t dissolve

- pale yellow to orange/brown ppt

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13
Q

Mn2+

  • NH3
  • excess NH3
A
  • no reaction bc don’t dissolve

- same as NaOH : pale pink to light brown

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14
Q

Cu2+

  • NH3
  • excess NH3
A
  • blue to blue ppt

- ppt dissolves = deep blue solution of [Cu(NH3)4(H2O)2]2+

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15
Q

Cr3+

  • NH3
  • excess NH3
A
  • green to grey/green gel ppt

- dissolves in excess to form purple sol of [Cr(NH3)6]3+

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16
Q

Zn2+ ion colour

A
  • colourless
17
Q

Al3+ ion colour

A
  • colourless
18
Q

ligand

A
  • mol/ion
  • bonds to metal ion
  • forms coordinate bond
  • donates a lone pair of e- into a vacant d-orbital
  • H20 , :CN- , :NH3
19
Q

complex ion

A
  • central metal ion surrounded by ligands
20
Q

monodentate ligand

bidentate ligand

A
  • donates one pair of e- to central metal ion

- donates 2 lone pairs of e- to the central metal ion

21
Q

when is a square planar complex formed

A
  • t-metals with eight d-e- in d-sub shell
  • Platinum(II) , palladium (II) and gold (III)
  • bond angle 90
  • cis-platin drug
22
Q

stereoisomer

A
  • same structural formula but a different arrangement of atoms in space.
23
Q

what types of stereoisomerism can complex ions display

A
  • cis-trans

- optical

24
Q

structural formula for 1,2-diaminoethane

A

NH2CH2CH2NH2

25
Q

cis platin as an anti-cancer drug

A
  • during chemotherapy
  • an anti-cancer drug
  • colourless liquid
  • drip into vein
  • forms a platinum complex inside of cells
  • binds onto DNA of cancerous cells
  • prevents division
  • trans molecule is ineffective
26
Q

Cu2+ reaction with NH3

A
  • [Cu(H20)6]2+ + 4NH3 = [Cu(NH3)4(H20)2]2+ + 4H20
  • in ammonia = pale blue
  • excess ammonia = dark blue
  • 4 NH3 ligands replace 4H2O ligands
  • 2 H2O left over
27
Q

Cu2+ with HCL

A
  • [Cu(H20)6]2+
  • add conc HCl
  • 6 H2O replaced by 4 chloride ligands
  • pale blue to green intermediate to yellow
  • ## [Cu(H2O)6]2+ + 4Cl- = [CuCl4]2- + 6H20
28
Q

why do only 4 Cl- ligands bond with Cu

A
  • chloride ligands are larger than water ligands

- fewer chloride can fit around central Cu2+ ion

29
Q

Cr3+ with ammonia

A
  • [Cr(H2O)6]3+ undergoes ligand substitution with excess NH3
  • first, grey ppt of Cr(OH)3 formed
  • Cr(OH)3 ppt dissolves in excess NH3 to form purple [Cr(NH3)6]3+
  • [Cr(NH3)6]3+ = violet

Chemistry (21 decks)

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