Transition Metals Flashcards
A coordinate bond is formed when a transition metal ion reacts with a ligand. Explain how this coordinate bond is formed
An electron pair on the ligand is donated from the ligand to the central metal ion.
In terms of bonding, explain the meaning of the term complex.
atom or ion or transition metal bonded to / surrounded by
one or more ligands
by co–ordinate bonding
describe what bidentate is
Two atoms or two points of attachment (1)
Each donating a lone electron pair
The complex ion formed in aqueous solution between cobalt(II) ions and chloride
ions is a different colour from the [Co(H2O)6]
2+ ion.
Explain why these complex ions have different colours
In different complexes the d orbital splitting will be different
Light energy is absorbed causing an electron to be excited
Different wavelength light will be absorbed or transmitted
Suggest why it is important that the container for each sample has the same
dimensions.
in a colorimeter
Absorption depends on (proportional to) path length / distance travelled through solution
Suggest one reason why a colorimetric method might be chosen in preference
to titration.
Quicker to analyse extracted samples than by titration / uses smaller
volumes of solution
Give the equation that relates the energy change ΔE to the Planck constant h and
the frequency of the visible light v.
ΔE = hv
Explain why this electron transition causes a solution containing the transition metal
ion to be coloured.
light is absorbed (to excite the electron)
The remaining colour / frequency / wavelength / energy is transmitted (through
the solution)
The energy change shown in the diagram represents the energy of red light and
leads to a solution that appears blue.
Blue light has a higher frequency than red light.
Suggest whether the energy change ΔE will be bigger, smaller or the same for a
transition metal ion that forms a red solution. Explain your answer.
Energy change …………………………………………………………………………………
Explanation ..
higher frequency of blue light absorbed, this means v is more, leads toa higher delta e
State 5 different features of transition metal complexes that cause a change in
the value of ΔE, the energy change between the ground state and the excited state
(Identity of the) metal
• Charge (on the metal) / oxidation state / charge on complex
• (Identity of the) ligands
• Co-ordination number / number of ligands
• Shape
When an aqueous solution containing [Cr(H2O)6]
3+ ions is warmed in the presence of
Cl– ions, [Cr(H2O)5Cl]2+ ions are formed and the colour of the solution changes.
Name this type of reaction.
Suggest, in terms of electrons, why the colours of the complex ions are different.
(ligand) substitution / replacement / exchange
Allow nucleophilic substitution
The energy levels/gaps of the d electrons are different
A different wavelength/frequency/colour/energy of light is absorbed (when d electrons are excited)
if fe3+ is purple why may it look brown
[Fe(H2O)6]3+(aq)
purple solution
may look yellow brown due to some
[Fe(H2O)5
(OH)]2+(aq)
due to rust
so fe3+ = yellow brown or purple
when something is warmed in the prescence of cl- ions another complex is formed and the colour of the solution changes, name this reac and suggest in terms of electrons why the colours of the complex ions differ
ligand subs
the energy gap of electrons are diff so a diff wavelength of light will be absorbed and a diff wavelength of light will be reflcted or transmitted
why may well water be more beneficial than pure water
contains iron, needed for haemoglobin for red blood cells to carry oxygen around the body
give the meaning of the term autocatalysed
the catalyst is a reaction product
example of a bidentate ligand
write them out like molecular so
c2o4- or h2nch2ch2nh2
By considering the properties of the reactants and products, state why it is possible
to use a spectrometer to measure the concentration of the manganate(VII) ions in
this reaction mixture.
As manganate VII ions are coloured (purple)
By reference to aqueous copper(II) ions, state the meaning of each of the
three terms in the equation ΔE = hv.
ΔE is the energy gained by the (excited) electrons (of Cu2+)
allow:
1
h (Planck’s) constant
1
v frequency of light (absorbed by Cu2+(aq)
Calcium fluoride crystals absorb ultra-violet light. Some of the energy gained is
given out as visible light. The name of this process, fluorescence, comes from the
name of the mineral, fluorite.
Use your knowledge of the equation ΔE = hν to suggest what happens to the
electrons in fluorite when ultra-violet light is absorbed and when visible light is given
out.
u. v. absorbed: electrons/they move to higher energy
(levels) /electrons excited
visible light given out: electrons/they fall back down/move to lower energy (levels)
Explain the meaning of the term complex ion.
ligands linked by covalent bonds
how is the light absorbed anyway
absorbed due to the electrons becoming excited. thats why, its bc they move to higher en levels
With reference to haemoglobin, explain why carbon monoxide is toxic.
Because it bonds to the iron/haemoglobin Allow blocks site /CO has greater affinity for haemoglobin /carboxyhaemoglobin more stable than oxyhaemoglobin 1 Displaces oxygen Or prevents transport of oxygen
why is something colourless
Ti(III) has a d electron that can be excited to a higher level
Allow idea that d electrons can be excited to another level (or
move between levels)
1
Absorbs one colour of light from white light
Allow idea that light is absorbed
1
Ti(IV) has no d electron so no electron transition with
energy equal to that of visible light
Give two reasons why the use of a spectrometer is the most appropriate
method for measuring the concentration of the coloured ions in this
experiment.
Rapid determination of concentration Or easy to get many readings 1 Does not use up any of the reagent/does not interfere with the reaction
