Transition metals

Definition of transition metals

Can form IONS with incomplete d orbital

properties of transtion metals

Act as catalyst

Form complexes

Form coloured compounds

Variable oxidation states

Explain why transition metals form variable oxidative staes and hence coloured ions

The energy levels of adjacent s orbital and d orbital are close in energy so multiple electrons can be removed from d orbital

severel ions can be formed whilst still being stable

Whats the bonds are always present in complex ions

Dative bond between lone pair on ligand and metal ions

Definition of complex ion

Metal ion surrounded by coordinately bonded ligand

Define ligand

Ion/molecule which donates lone pair of electron to metal ion

Types of ligands and define them

Monodentate- donates 1 lone pair to central metal ion forming 1 coordiante bond

Bidentate-each donates 2 lone pairs to central metal ion to form coordination bonds of 2

Multidentate- each donates multiple lone pairs of electrons to form more than 2 coordianation bonds

Define Co ordination number

Number of coordinate bomds to the central metal ion

Example of monodentates

NH3

H2O

Cl-

Why cant electron pair repulsion theory be used to predict shape of complex ions

too many electrons in d orbital

Factors affecting shape of complex metal ion

Size of ligand

Coordination number

What ligands do octahedral complexes generally have and why?

NH3/H2O

smalll molecules so can fit around central metal ion easily

Properties of octahedral complexes

Coordination number of 6

Bond angle: 90

Can tetrahedral complexes contain Cl-

Yes they can , as Cl- is lare so only 4 can fit

Tetrahedral complex properties

Coordination number of 4

Bond angle - 109.5

What are the only 2 metals that can form square planar complexes

Pt2+ and Ni2+

What metal forms linear complex

Ag+