Question

Iron exhibits $+ 2$ and $+ 3$ oxidation states. Which of the following statements about iron is incorrect?
A. Ferrous oxide is more basic in nature than the ferric oxide
B. Ferrous compounds are relatively more ionic than the corresponding ferric compounds
C. Ferrous compounds are less volatile than the corresponding ferric compounds
D. Ferrous compounds are more easily hydrolysed than the corresponding ferric compounds

Answer 1

The oxidation state of an element is related to the number of electrons that an atom loses, gains, or uses when joining with another atom in compounds. It also determines the ability of an atom to oxidize (to lose electrons) or to reduce (to gain electrons) other atoms or compounds. Most of the transition metals have multiple potential oxidation states. Iron exhibits $+ 2$ an oxidation state in ferrous oxide and $+ 3$ oxidation state in the ferric oxide.

Complete step by step answer:
Less is the oxidation state, more is the basic character of a compound which means ferrous oxide is more basic than ferric oxide. This statement (A) is correct.
Less is the oxidation state, more is the polarizing power hence more is the ionic character of a compound which means ferrous oxide is more ionic than ferric oxide. Thus statement B) is correct.
The lesser the charge and higher the ionic character, the less is the volatility of a compound. Thus statement (C) is correct
The higher the oxidation state and thus greater the covalent nature, the greater is the ease of hydrolysis of the compound. Ferric oxide will be more easily hydrolyzed than ferrous oxide. Thus statement (D) is false

So, the correct answer is Option (D).

Note: Iron chemical compounds, which include ferrous ( $F{e^{2 + }}$ ) and ferric ( $F{e^{3 + }}$ ) compounds, have multiple uses. Iron oxide mixed with aluminum powder may be ignited to create a thermite reaction used in welding and purifying ores. Iron can form binary compounds with the halogens and the chalcogens. Aside from the ferric and ferrous oxidation states, iron often occurs in higher oxidation states. An example of the same is the purple potassium ferrate ( ${K_2}Fe{O_4}$ ) which contains iron in its $+ 6$ oxidation state. There are also many mixed-valence compounds which contain both iron(II) and iron(III) centers, such as magnetite and Prussian blue $\left( {F{e_4}{{\left( {Fe{{\left( {CN} \right)}_6}} \right)}_3}} \right)$