Question

The acidic oxide among the following is:
(A) $C{{l}_{2}}{{O}_{5}}$
(B) $C{{l}_{2}}O$
(C) $C{{l}_{2}}{{O}_{3}}$
(D) $C{{l}_{2}}{{O}_{7}}$

Answer 1

Hint: The acidity of oxides is based on the nature and property of compounds. These oxides are binary compounds formed when other elements react with oxygen, which is highly reactive. Metals and non-metals also react with oxygen forms metal oxides which are basic.

Complete step by step answer:
The classification of oxides based on their acidic and basic characteristics
(a) Acidic oxides
(b) Basic oxides
(c) Amphoteric oxides
(d) Neutral oxides

Acidic oxides: An oxide is said to be acidic when combined with water to form acid. Most non-metals produce acidic oxides when dissolving in water.
For example, Silicon, phosphorus, sulfur, and chlorine oxides are acidic.
Non-metal reacts with oxygen to form acidic compounds of acidic acid which are bound together with covalent bonds. These compounds are also called acidic anhydride.
Chlorine forms oxides are acidic, which are $C{{l}_{2}}O,Cl{{O}_{2}},C{{l}_{2}}{{O}_{7}}$ . Out of all chlorine oxides, dichloro heptoxide $C{{l}_{2}}{{O}_{7}}$, Chlorine (VII) oxide is more acid than all chlorine oxide. Because it reacts with water, it gives the strongest acid perchloric acid.
$C{{l}_{2}}{{O}_{7}}+{{H}_{2}}O\to 2HCl{{O}_{4}}$

In Dichlorine heptoxide, chlorine is the highest oxidation state of chlorine is +7. It continues the trends of being strong acids along 3peiords of element oxides.
The pH of the hypocaloric acid around 0, like sulphuric acid.
So, the correct answer is “Option D”.

Note: Chlorine, bromine, and iodine form oxides with oxidation states ranging from +1 to +7. The stability order of oxides formed by halogens, I > Cl > Br. Chlorine oxides $C{{l}_{2}}O,Cl{{O}_{2}},C{{l}_{2}}{{O}_{7}}$ are highly reactive oxidizing agents and tend to explode.