Principles of Transition Metal Chemistry - exam practice

1s² 2s² 2p⁶ 3s² 3p⁶ 3d³

1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹ 4s²

1s² 2s² 2p⁶ 3s² 3p⁶ 3d³ 4s²

1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁵ 4s²

two 3d electrons

two 4s electrons

one 4s electron and one 3d electron

two 4p electrons

[Cr(NH₃)₄Cl₂]⁺ and [Mn(H₂O)₆]²⁺

CrO₄^2- and TiCl₃

Cr₂O₃ and [Fe(CN)₆]^3-

Cr₂O₇^2- and MnO₄^-

+1

+5

+6

+7

CH₃NH₂

CN^-

NH₃

NH₄⁺

vanadium

chromium

manganese

iron

[Co(NH₃)₆]³⁺

[Co(NH₃)₅(H₂O)]³⁺

[Co(NH₃)₅(Cl)]²⁺

[Co(NH₃)₄(Cl)₂]⁺

it is in the d block of the periodic table

it forms stable ions in which it has different oxidation numbers

it has incompletely filled d orbitals

it forms stable ions which have incompletely filled d orbitals

excited electrons emit light in the blue region of the spectrum as they drop back to the ground state

excited electrons emit light in the red region of the spectrum as they drop back to the ground state

electrons absorb light in the red region of the spectrum and the residual frequencies are observed

electrons absorb light in the blue region of the spectrum and the residual frequencies are observed

the bonding in both complexes is dative covalent

the bonding in both complexes is ionic

the bonding in Pt(NH₃)₂Cl₂ is dative covalent and in CrCl₄^- is ionic

the bonding in Pt(NH₃)₂Cl₂ is ionic and in CrCl₄^- is dative covalent

is square-planar

is tetrahedral

contains a double bond

is octahedral

transition metals form coloured ions and complexes

transition metals display variable oxidation states

a ligand accepts a pair of electrons from a transition metal

a complex is a central metal atom or ion surrounded by ligands

Cr₂O₇^2-_(aq)

Fe²⁺_(aq)

Fe³⁺_(aq)

Cu²⁺_(aq)

oxidation state of the metal

number of ligands in the complex

identity of the ligands in the complex

isotope of the metal

identity of the ligand

temperature of the solution

identity of the metal

oxidation number of the metal

[Ne]3s²3p⁶4s¹

[Ar]3d⁹

1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p²

[Ar]4s¹3d⁵

the different colours are due to the different charges on the complex

the different ligands cause different splitting in the 3d orbitals

the oxidation state of cobalt is different in each complex

[CoCl₆]^3- absorbs orange light

as electrons are promoted to higher energy levels, light of a certain colour is absorbed, and the complementary colour is observed

as electrons return to lower energy levels, light of a certain colour is emitted, and the complementary colour is observed

as electrons are promoted to higher energy levels, light of a certain colour is absorbed, so the complex appears to have the same colour

as electrons return to lower energy levels, light of a certain colour is emitted, so the complex appears to have the same colour

0

1+

2+

3+

0

1+

2+

3+

coordination number: 2; m = 0

coordination number: 2; m = 4$-$

coordination number: 6; m = 0

coordination number: 6; m = 4$-$