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transition metal chemistry

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Total cards: 12•Content version: v4•Public deck•Updated: 8/1/2026

Card preview (12)

#1
Front (Question)

why do the typical characteristics of transition metals arise

Back (Answer)

they have incomplete d subshells (therefore Ti to Cu are considered to be transition metals)

#2
Front (Question)

what 2 elements in period 4 are not called transition metals and why

Back (Answer)

Sc (no 3d electrons) Zn (full 3d subshell) do not have the characteristic of incomplete d subshell so are not transition metals

#3
Front (Question)

give the 4 common properties of transition metals

Back (Answer)

• form complexes • form coloured ions • have variable oxidation states • act as catalyst

#4
Front (Question)

define ligand

Back (Answer)

molecule or ion that forms a co ordinate bond with a transition metal by donating a pair of electrons

#5
Front (Question)

define complex

Back (Answer)

central metal atom or ion surrounded by ligands

#6
Front (Question)

define co ordination number

Back (Answer)

number of coordinate bonds to the central metal atom or ion

#7
Front (Question)

define monodentate ligands and give 3 examples

Back (Answer)

forms only 1 dative covalent bond H20 , NH3 , Cl- Cl- is much larger than H2O or NH3

#8
Front (Question)

define bidentate ligands and give 2 examples

Back (Answer)

form 2 coordinate bonds per ligand 1,2- diaminoethane H2NCH2CH2NH2 C2O42- ethanedioate

#9
Front (Question)

give the formula for 1,2- diaminoethane

Back (Answer)

H2NCH2CH2NH2

#10
Front (Question)

give the formula for ethanedioate

Back (Answer)

C2O4 2-

#11
Front (Question)

define multidentate ligand and give an example

Back (Answer)

forms multiple coordinate bonds per ligand EDTA4- forms 6 coordinate bonds

#12
Front (Question)

how many coordinate bonds does EDTA4- form

Back (Answer)

6 coordinate bonds per ligand