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Inorganic Chemistry
1. Answer ALL parts a) — c).
a) Explain briefly why ligand exchange reactions of Cr(III) are typically very slow.
b) Which of the two manganese complexes shown below will have the greatest value of Ao Give an explanation for your conclusion.
[Mn(H2O )6]2“, [Mn(CN)6]
C) Draw d-orbital splitting diagrams of each electronic configuration for which both high- and low-spin possibilities exist for octahedral transition metal complexes. In such cases, which factors determine whether an
octahedral metal complex adopts a high- or a low-spin d-electron configuration?
a) Explain briefly why ligand exchange reactions of Cr(III) are typically very slow.
b) Which of the two manganese complexes shown below will have the greatest value of Ao Give an explanation for your conclusion.
[Mn(H2O )6]2“, [Mn(CN)6]
C) Draw d-orbital splitting diagrams of each electronic configuration for which both high- and low-spin possibilities exist for octahedral transition metal complexes. In such cases, which factors determine whether an
octahedral metal complex adopts a high- or a low-spin d-electron configuration?
Inorganic Chemistry
Answer ALL parts a) — d).
a) Give the FULL electronic configuration of potassium.
b) Draw the radial distribution functions (RDFs) for the 4s and 3d orbitals, and use them to explain your answer to part a).
c) Explain briefly why many homoleptic transition metal complexes of carbon monoxide, CO, tend to obey the eighteen-electron rule.
d) For the ligands listed below, identify those that are n-acids and/or n- bases.
Br-, CO, H2O, PMe3
a) Give the FULL electronic configuration of potassium.
b) Draw the radial distribution functions (RDFs) for the 4s and 3d orbitals, and use them to explain your answer to part a).
c) Explain briefly why many homoleptic transition metal complexes of carbon monoxide, CO, tend to obey the eighteen-electron rule.
d) For the ligands listed below, identify those that are n-acids and/or n- bases.
Br-, CO, H2O, PMe3
Inorganic Chemistry
1 . Answer ALL parts a) — c).
a) Use the principles of Valence Shell Electron Pair Repulsion (VSEPR) to predict the structures of the following species.
XeF2; [XeF3]+; XeF4
b) Some of the halogens form oxo-acids in which their oxidation state is +7. Comment briefly on the observations that:
i) fluorine does not form a compound of this type;
ii) the compounds of iodine (H5IO6) and chlOrine (HCIO4) have different structures.
2 。Draw the structure of the following coordination compounds and determine the oxidation state, da nt electronic configuration, ( t2 gm eg” Or emt2" configuration and the spin only magnetic moment of the metal atom.
i) [CO(H2O )6]2+
ii) [Fe(ox)s]3-, ox = oxalate dianion, C2O42-
iii) [Ni(en)3]2+ , en = 1,2-diaminoethane
a) Use the principles of Valence Shell Electron Pair Repulsion (VSEPR) to predict the structures of the following species.
XeF2; [XeF3]+; XeF4
b) Some of the halogens form oxo-acids in which their oxidation state is +7. Comment briefly on the observations that:
i) fluorine does not form a compound of this type;
ii) the compounds of iodine (H5IO6) and chlOrine (HCIO4) have different structures.
2 。Draw the structure of the following coordination compounds and determine the oxidation state, da nt electronic configuration, ( t2 gm eg” Or emt2" configuration and the spin only magnetic moment of the metal atom.
i) [CO(H2O )6]2+
ii) [Fe(ox)s]3-, ox = oxalate dianion, C2O42-
iii) [Ni(en)3]2+ , en = 1,2-diaminoethane
Inorganic Chemistry
6. Answer ALL parts a) — c).
a) Draw the structure of the following coordination compounds and determine the oxidation state, dn electronic configuration,t2gm egn or emt2n configuration and the spin only magnetic moment (Us.o.) of the metal ion.
i. [Co(NH3)6]2+
ii. [Cu(en)3]2+, en = 1,2-diaminoethane
iii. [NiCl4]2-
B)Use the Bohr model of the hydrogen atom to explain atomic emission spectra. Your answer should include appropriate diagrams.
a) Draw the structure of the following coordination compounds and determine the oxidation state, dn electronic configuration,t2gm egn or emt2n configuration and the spin only magnetic moment (Us.o.) of the metal ion.
i. [Co(NH3)6]2+
ii. [Cu(en)3]2+, en = 1,2-diaminoethane
iii. [NiCl4]2-
B)Use the Bohr model of the hydrogen atom to explain atomic emission spectra. Your answer should include appropriate diagrams.
Inorganic Chemistry
1. Answer ALL parts a) — d).
a) The rate constant of for the exchange of a single water molecule in the complex [Cu(H2O)s] 2+ is one of the fastest known for a metal complex. Explain why it is so fast.
b) Determine the magnitude of the crystal field stabilisation energy in terms of for the following complexes:
[Cr(H2O)6) 3 +, [Mn(CO)6]+
c) Describe briefly what is meant by the terms n-donating and rr-accepting,
and provide one example of each. sj
d) Select the combinations of metal ion and ligand from the following list that will form the most stable complexes, and explain your choice.
Metal ions: Ag+, r3+
Ligands: EtS—, NH3
2. Answer ALL parts a) — c).
Draw a fully labelled energy level diagram for the atomic and molecular orbitals in F2-.[10]
b) Calculate the bond order of F2—, and state whether or not it is diamagnetic. [2]
Draw diagrams to illustrate the formation of molecular orbitals from atomic orbitals in F2-.
a) The rate constant of for the exchange of a single water molecule in the complex [Cu(H2O)s] 2+ is one of the fastest known for a metal complex. Explain why it is so fast.
b) Determine the magnitude of the crystal field stabilisation energy in terms of for the following complexes:
[Cr(H2O)6) 3 +, [Mn(CO)6]+
c) Describe briefly what is meant by the terms n-donating and rr-accepting,
and provide one example of each. sj
d) Select the combinations of metal ion and ligand from the following list that will form the most stable complexes, and explain your choice.
Metal ions: Ag+, r3+
Ligands: EtS—, NH3
2. Answer ALL parts a) — c).
Draw a fully labelled energy level diagram for the atomic and molecular orbitals in F2-.[10]
b) Calculate the bond order of F2—, and state whether or not it is diamagnetic. [2]
Draw diagrams to illustrate the formation of molecular orbitals from atomic orbitals in F2-.
Inorganic Chemistry
1.Rank the lead halide salts in order of their solubility in water?
2.Which is more soluble in water, NaIO3 or CSIO3?
3. Rank the group 2 Carbonates in order of thermal stability ?
2.Which is more soluble in water, NaIO3 or CSIO3?
3. Rank the group 2 Carbonates in order of thermal stability ?
Inorganic Chemistry
Which of the following molecules exhibit rotational and or vibrational spectra
H2, HF, CO, NO
H2, HF, CO, NO
Inorganic Chemistry
b) Explain the structures of XeO2F2 and XeOF2 on the basis of VSEPR theory.
Inorganic Chemistry
5. a) Name the factors that affect the thermal stability of alkali metal salts. Explain the
stability trend observed in case of nitrates of these metals.
b) Why is the monomeric beryllium hydride unstable? Describe the structure of
polymeric beryllium hydride.
stability trend observed in case of nitrates of these metals.
b) Why is the monomeric beryllium hydride unstable? Describe the structure of
polymeric beryllium hydride.
Inorganic Chemistry
3. a) Give the names of any two alloys of aluminium which have some amount of copper or
magnesium. How are these more advantageous than pure aluminium?
b) Why boric acid is a very weak monobasic acid (pH = 9.25)? Explain with suitable
equation.
c) Why iron, cobalt and nickel do not form typical interstitial carbides? Write the type of
carbides they form.
magnesium. How are these more advantageous than pure aluminium?
b) Why boric acid is a very weak monobasic acid (pH = 9.25)? Explain with suitable
equation.
c) Why iron, cobalt and nickel do not form typical interstitial carbides? Write the type of
carbides they form.
