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Chemistry > transition metals > Flashcards

transition metals Flashcards

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1
Q

define transition elements

A

a metal that can form one or more stable ions with a partially filled d-subshell

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2
Q

what d-block elements arent transition metals and why

A

scandium and zinc do not form stable ion with partially filled d-subshell

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3
Q

what is the electron configuration of chromium

A

[Ar] 4s1 3d5

this is due to both 4s and 3d being half full gives chromium more stability than a full 4s and partially full 3d

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4
Q

whats the electron configuraton of copper and why

A

[Ar] 4s0 3d10

more stable with full 3d-subshell and half full 4s

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5
Q

how does energy levels change once the 3d subshell gains its first electron

and what does this result in

A
  • 4s become higher energy level than 3d
  • as 4s becomes higher energy level than 3d this means that electrons are lost from the 4s subshell before 3d
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6
Q

why are transition metals and their compounds good catalysts

A

they can change oxidation states by gaining or losing electrons within their d-orbitals

this means they can transfer electrons to speed up reactions.

theyre also good at adsorbing substances onto their surfaces to lower activation energy of reactions

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7
Q

name 3 industry uses of transition metals as catalysts

A

1) haber process, Fe
2) MnO2 is used in the decomposition of hydroge peroxide
3) production of hydrogen from zinc and acids, CuSO4 used as catalyst

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8
Q

name 4 chemical proeprties of transition metals

A
  • form complex ions
  • form coloured ions
  • good catalysts
  • exist in variable oxidation states
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9
Q

define complex ion

A

a metal ion surrounded by coordinately bonded ligands

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10
Q

define ligand

A

an atom, ion or molecule that donates a pair of electrons to a central metal ion in a complex ion

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11
Q

define coorinate bond

(dative covalent bond)

A

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

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12
Q

define monodentate ligand

A

a ligand that can only form one coordinate bond

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13
Q

define bidentate ligand

A

a ligand that can form 2 coordinate bonds

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14
Q

define multidentate ligand

A

a ligand that can form 3 or more coordinate bonds

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15
Q

define coordination number

A

number of coordinate bonds that are formed with the central metal ion in a complex ion

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16
Q

what shape and angles do complex ions have with a coordination number of 6

A

octahedral

90°

17
Q

whats a hexaaqua complex

A

6 water ligands around a central ion

18
Q

what shape and angles do complex ions have with a coordination number of 4

A
  • mostly tetrahedral with 109.5° angles e.g. [CuCl4]2-, [CoCl4]2-
  • some are square planar with 90° angles e.g. cisplatin [Pt(NH3)2(Cl2)]
19
Q

what is concidered a large ligand and what effect does this have

A

Cl-

only 4 can fit around the central metal ion

20
Q

draw the general shape of a tetrahedral complex ion

draw [CuCl4]2-

A
21
Q

draw 3d structure of cisplatin [Pt(NH3)2Cl2]

A
22
Q

draw the 2 optical isomers of [Ni(H2NCH2CH2NH2)3]2+

A
23
Q

Cis-trans isomerism can occur on what type of complex ions

A
  • square planar complex ions that have 2 pairs of ligands
  • octahedral complex ions with 4 ligands of 1 type and 2 of another
24
Q

define ligand substitutuion

A

a reation where 1 or more ligands are changed for one or more other ligands in a complex ion

25
Q

wirte the balanced equation for

[Cr(H2O)6]3+(aq) + NH3 ⇌

A

[Cr(H2O)6]3+(aq) + 6NH3(aq) ⇌ [Cr(NH3)6]3+(aq) + 6H2O(l)

26
Q

write the full balanced equations for the precipitatoin reactions of Iron(II) with 2OH- and 2NH3

A

[Fe(H2O)6]2+(aq) + 2OH-(aq) -> [Fe(OH)2(H2O)4]2+(s) + 2H2O(l)

[Fe(H2O)6]2+(aq) + 2NH3(aq) -> [Fe(OH)2(H2O)4]2+(s) + 2NH4+(aq)

27
Q

write full precipitate reaction for Copper(II) with 2OH- and 2NH3

state the colour change

A

Cu(H2O)6]2+(aq) + 2OH-(aq) -> Cu(OH)2(H2O)4](s) + 2H2O(l)

Cu(H2O)6]2+(aq) + 2NH3(aq) -> Cu(OH)2(H2O)4](s) + 2NH4+(aq)

pale blue -> blue prcpt

28
Q

write full precipitate reaction for Chromium(III) with 2OH- and 2NH3

state the colour change

A

[Cr(H2O)6]3+(aq) + 3OH-(aq) -> Cr(OH)3(H2O)3(s) + 3H2O(l)

[Cr(H2O)6]3+(aq) + 3NH3(aq) -> [Cr(OH)3(H2O)3](s) + 3NH4+(aq)

green -> grey-green prcpt

29
Q

write full precipitate reaction for Iron(III) with 2OH- and 2NH3

state the colour change

A

[Fe(H2O)6]3+(aq) + 3OH-(aq) -> Fe(OH)3(H2O)3(s) + 3H2O(l)

[Fe(H2O)6]3+(aq) + 3NH3(aq) -> [Fe(OH)3(H2O)3](s) + 3NH4+(aq)

yellow -> orange prcpt

30
Q

write full precipitate reaction for Manganese(II) with 2OH- and 2NH3

state the colour change

A

[Mn(H2O)6]2+(aq) + 2OH-(aq) -> [Mn(OH)2(H2O)4](s) + 2H2O(l)

[Mn(H2O)6]2+(aq) + 2NH3(aq) -> [Mn(OH)2(H2O)4](s) + 2NH4+(aq)

pale pink -> pink/buff prcpt

31
Q

whats used as an oxidising agent for oxidising Fe2+

what ion is present and whats its oxidation state

what is it reduced to

A

Acidified potassium manganate(VII) solution, KMnO4(aq)

MnO4- ions

manganese has an oxidation state of +7

manganese reduced to Mn2+

32
Q

WHAT reducing agent os used for Fe3+

whats it oxidised to

A

I-

I2

33
Q

whats used as an oxidising agent for Cr3+ -> Cr2O72-

A

H2O2(aq)

reduced to OH-

34
Q

WHATS THE REDUCING AGENT USED FOR Cr2O7 TO Cr3+

A

acidifed zinc

Zn oxidised to Zn+2

Chemistry (14 decks)

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