(c) Transition metals

what block in the periodic table are transition metals found

d-block

what elements are the exceptions to the filling of the d orbitals following the aufbau principle

chromium and copper atoms

why are chromium and copper exceptions to the regular arrangement of electrons

It is easier for them to remove a 4s electron and bring it into the 3d subshell, which will give them a half filled or completely filled subshell, creating more stability

What is the Latin name for Tin

Stannate

What is the Latin name for silver

Argentate

What is the Latin name for lead

Plumbate

what is lost first when atoms from the first row of the transition elements form ions

the 4s electrons that are lost first rather than the 3d electrons

what is the oxidation number of uncombined elements

0

what is the oxidation number of ions containing single atoms

the charge on the ion

what must the sum of all the oxidation numbers of all the atoms in a neutral compound add up to

0

what must the sum of all the oxidation numbers of all the atoms in a polyatomic ion equal to

the charge on the ion

what are the properties of transition metals

have atoms or ions with an incompleted d subshell

have variable oxidation states

show catalytic ability

form coloured ions

what is a complex

a metal ion surrounded by ligands

what can ligands be classified as

monodentate, bidentate, quadridentate, hexadentate

What may ligands be

Negative ions or molecules with non-bonding pairs of electrons that they donate to the central atom or ion, forming dative covalent bonds

What is the coordination number

The total number of bonds from the ligands to the central transition metal

What must complexes contain to be able to write names and formulae according to IUPAC rules

Central metals that obey the normal IUPAC rules

copper (cuprate) and iron (ferrate)

ligands, including water, ammonia, halogens, cyanide, hydroxide, and oxalate

what are the d orbitals in a complex of a transition metal

No longer degenerate

When does splitting of d orbitals to higher and lower energies occur

When the electrons present in approaching ligands cause the electrons in the orbitals lying along the axes to be repelled

What are strong field ligands

Ligands that cause a large difference in energy between subsets of d orbitals

What are weak field ligands

Ligands that cause a small difference in energy between subsets of d orbitals

What is the spectrochemical series

Ligands being placed in order of their ability to split d orbitals

How can colours of many transition metal complexes be explained in terms of

d-d interactions

What is absorbed when electrons in a lower energy d orbital are promoted to a d orbital of higher energy

Light

When light of one colour is absorbed, what will be observed

The complementary coloir

When do electrons transition to higher energy levels

When energy corresponding to the ultraviolet or visible regions of the electromagnetic spectrum is absorbed

What do transition metals and their compounds act as

Catalysts

What state are heterogeneous catalysts in compared to the reactants

Different

What state are homogeneous catalysts in compared to the reactants

Same

How can heterogenous tests be explained in terms of

The formation of activated complexes and the absorption of reactive molecules onto active sites

How can homogenous catalysts be explained in terms of

changing oxidation states with the formation of intermediate complexes

state how transition metals can act as catalysts

unpaired d electrons, variable oxidation states, donating and accepting electrons, incomplete d orbitals

state what causes d orbital splitting

repulsion from electrons in the ligand, lone pairs in the ligand