CH3.4 Chemistry of the d-block transition metals Flashcards
d block elements
Is the elements whose outer electrons are found in the d-orbitals,
transition element
is a metal that possesses a partially filled d sub-shell in its atom or stable ions.
which metals in the d block are not transition metals
zinc- full sub shell in both atoms and ions
electron configuration beyound argon
the 3d orbitals are filled before the 4s orbitals
exception to the rule of fill the 3d before the 4s
chronium and copper
how chronium fills its orbitals
fills up to and including the 3p orbital, one in the 4s , and one in each of the 3d orbitals.
how copper fills its orbitlas
fills as normal and then one in the 4s and then completely fills the 3d orbital/.
describe a transition metal complex
- size
- charge
- bonding and orbials
small
large positive charge
lots of available orbitals for bonding
form co-ordinate bonds
ligand
a small molecule with a lone pair that can form a bond to a transition metal
most common amount o fligans that would be found around one metal ion and name
6 octahedral
complex that has four ligans
tetrahedral
complex that has 6 ligands
octahedral
colour of
(Fe(H2O)6)3+
pale green
colour of (Fe(H2O)6)3+
Yellow
colour of (Cu(H2O)6)2+
blue
colour of (Cr(H2O)6)3+
dark green
colour of (Co(H2O)6)2+
pink
colour of (CuCl)2-
yellow or green
colour of (CoCl)2-
blue
Trans iosomers
when two water molecules are opposite each other.
which is most common trans or sist isomers
trans
what happens when the d-orbital split
gives two sets of orbitals close together in energy, electrons can move from the lower to higher orbital
how do electrons move within split d-orbitals
They gain the energy through the absorbtion of of energy through light.
how does the energy that is absorbed by the electron to move up a orbital relate
The energy it absorbes is one frequency of light which corresponds to the energy gap between the orbitals.
realtionship between energy absorbed and frequency
E=hf
how do complexes get there colours
The light that remains after a electron has moved within the split d-orbital by the equation E=hf gives the complex its colour.
iron used as a catalys
int he harbour process, to produce ammonita from nitrogen and hydrogen
nickel as a catalyst
The hydration of vegetable oils to from margarine
platinum as a catalyst
The oxidation of ammonia to form nitric acid
Vanadium oxide as a catalyst
The contact procces for the production of sulfuric acid
manganses dioxide
The caralytic decomposition of hydrogen peroxide
why are transition metals good as catalysts
because of there partially filled d-orbitals which have enough empty orbitals to combine with other molecules. molecules with lone pairs can form co-ordinate bonds to the metal atom to form complexesm and this can increases the reactivity of the species bonded to the metal, or bring two reacting molecules closer together.
how does oxidations and catalysts use of transition metals relate
The different ocidation states allows them to act as catalyst in redox reactions. They can act as oxidising or redusing agents for one of the reactants
typical heterogenous catalyts
Typically a solid that provides a surface for molecules to be absorbed and come together in a advantageous arrangement
typical homogenous catalyst
typically use their variable oxidation states to oxidis/reduxe a reactant which makes it much more reactive
catalyst
are substances which increases the rate of a chemical reaction by providing an alternating pathway with a lower acitvation energy.
homogenous catalyst
catalyst that are in the same physical state as the reaction that they catalyse
heterogenous catalyst
Are catalysts that are in different physical state from the reactino that they catalyse.
reaction of (Cr(H2O)6)3+ with hydroxide ions
grey-green precipitate of (Cr(H2O)3(OH)3)
excess OH- ions;
precipitate dissolves giving deep green solutionof (Cr(OH)6)3-
reaction of (Fe(H2O)6)2+ with OH- ions
Dark green precipitate of (Fe(H2O)4(OH)3)
excess OH- ions;
no further reaction for the bulk, (some red-brown colour seen at the surface due to oxidation by the air)
reaction of (Fe(H2O)6)3+ with OH- ions
Red-brown precipitate of (Fe(H2O)3(OH)3)
excess OH- ions ;
No further reaction
reaction of (Cu(H2O)6)2+ with OH- ions
pale blue precipitate of (Cu(H2O)4(OH)2)
excess OH- ions;
no further reaction
