J. D. Lee Solutions for Chapter: An Introduction to the Transition Elements, Exercise 1: Exercise 1

Write notes on the following:
The ligands which stabilise the low oxidation states.

Write notes on the following:

Back bonding in metal carbonyls

Describe the method by which extremely pure samples of the metals may be prepared:

Which of the ${\mathrm{M}}^{2+}$ and ${\mathrm{M}}^{3+}$ ions of the first-row transition elements are stable in aqueous solution, which are oxidizing and which are reducing?

Explain why certain ligands such as ${\mathrm{F}}^{-}$ tend to bring out the maximum oxidation state of an element, whilst others such as $\mathrm{CO}$ and dipyridyl bring out the lowest oxidation states.

Give reasons why carbonyl and cyanide complexes of the later transition elements $\mathrm{Cr}, \mathrm{Mn}, \mathrm{Fe}, \mathrm{Co}, \mathrm{Ni}$ are more stable, more common, and more likely to exist than similar compounds of the $\mathrm{s}-$block or early transition elements.

Why do the second and third rows of transition elements resemble each other much more closely than they resemble the first row?

What do you understand by the terms paramagnetism and diamagnetism? Predict the magnetic moment for octahedral complexes of ${\mathrm{Fe}}^{2+}$with strong field ligands and with weak field ligands.