topic 15: transition metals

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Total cards: 24•Content version: v4•Public deck•Updated: 8/1/2026

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Front (Question)

what is the electronic configuration of Sc

Back (Answer)

1s2 2s2 2p6 3s2 3p6 4s2 3d1

Front (Question)

what is the electronic configuration of Ti

Back (Answer)

1s2 2s2 2p6 3s2 3p6 4s2 3d2

Front (Question)

what is the electronic configuration of V

Back (Answer)

1s2 2s2 2p6 3s2 3p6 4s2 3d3

Front (Question)

what is the electronic configuration of Cr

Back (Answer)

1s2 2s2 2p6 3s2 3p6 4s1 3d5

Front (Question)

what is the electronic configuration of Mn

Back (Answer)

1s2 2s2 2p6 3s2 3p6 4s2 3d5

Front (Question)

what is the electronic configuration of Fe

Back (Answer)

1s2 2s2 2p6 3s2 3p6 4s2 3d6

Front (Question)

what is the electronic configuration of Co

Back (Answer)

1s2 2s2 2p6 3s2 3p6 4s2 3d7

Front (Question)

what is the electronic configuration of Ni

Back (Answer)

1s2 2s2 2p6 3s2 3p6 4s2 3d8

Front (Question)

what is the electronic configuration of Cu

Back (Answer)

1s2 2s2 2p6 3s2 3p6 4s1 3d10

#10

Front (Question)

what is the electronic configuration of Zn

Back (Answer)

1s2 2s2 2p6 3s2 3p6 4s2 3d10

#11

Front (Question)

what is a transition metal

Back (Answer)

d-block elements that form one or more stable ions with incompletely-filled d-orbital

#12

Front (Question)

what are the characteristics of transition metals

Back (Answer)

• complex formation * formation of coloured ions • variable oxidation state • catalytic activity

#13

Front (Question)

why is Zn not a transition metal

Back (Answer)

Zn can only form a +2 ion. in this ion the Zn2+ has a complete d orbital and so does not meet the criteria of having an incomplete d orbital in one of its compounds

#14

Front (Question)

why is Sc not a transition metal

Back (Answer)

Sc can only form a +3 ion. In this ion the Sc3+ has an empty d orbital and so does not meet the criteria of having an incomplete d orbital in one of its ions

#15

Front (Question)

what is a complex

Back (Answer)

s a central metal ion surrounded by ligands

#16

Front (Question)

what is a ligand

Back (Answer)

an atom, ion or molecule which can donate a lone electron pair

#17

Front (Question)

coordinate bonding

Back (Answer)

co-ordinate bonding is involved in complex formation. co-ordinate bonding is when the shared pair of electrons in the covalent bond come from only one of the bonding atoms. co-ordination number: the number of co-ordinate bonds formed to a central metal ion

#18

Front (Question)

ligands can be monodentate, bidentate or multidentate. what do these words mean

Back (Answer)

can form one coordinate bond per ligand which have two atoms with lone pairs and can form two coordinate bonds per ligand

#19

Front (Question)

describe the structure of EDTA4- anion

Back (Answer)

6 donor sites (4O and 2N) and forms a 1:1 complex with metal(II) ions

#20

Front (Question)

colour changes arise from changes in what 3 things

Back (Answer)

oxidation state co-ordination number ligand

#21

Front (Question)

[Co(NH3)6]2+ (aq)  [Co(NH3)6]3+ (aq) +e- yellow —> brown what causes the colour change in the equation

Back (Answer)

in this equation only oxidation state is changing

#22

Front (Question)

Cu(H2O)62+ + 4Cl-  [CuCl4]2- + 6H2O blue —> green what causes the colour change in this equation

Back (Answer)

In this equation both ligand and co- ordination number are changing

#23

Front (Question)

Co(H2O)62+ + 6 NH3  Co(NH3)62+ + 6H2O pink —> yellow brown

Back (Answer)

in this equation only the ligand is changing

#24

Front (Question)

how do colour arises

Back (Answer)

colour arises from electronic transitions from the ground state to excited states: between different d orbitals a portion of visible light is absorbed to promote d electrons to higher energy levels. the light that is not absorbed is transmitted to give the substance colour