Question

Assertion:
Water is an oxide of hydrogen represented by the formula ${{{H}}_2}{{O}}$. However, oxide of fluorine is represented by the formula ${{O}}{{{F}}_2}$ and not ${{F}}{{{O}}_2}$.
Reason:
Formulas of any compound are contained in such a way that more electropositive element comes first and less electropositive element later.
A.Both assertion and reason are correct and reason is the correct explanation of the assertion
B.Both assertion and reason are correct but reason is not the correct explanation of the assertion
C.Assertion is correct but reason is incorrect
D.Both assertion and reason are incorrect

Answer 1

Some elements can form oxides with oxygen. Generally, oxides are of four types-acidic, basic, neutral and amphoteric oxides. These oxides are formed based on electronegativity. Oxygen can form stable chemical bonds with these elements.

Complete step by step answer:
The assertion says water is an oxide of hydrogen represented by the formula ${{{H}}_2}{{O}}$. However, oxide of fluorine is represented by the formula ${{O}}{{{F}}_2}$ and not ${{F}}{{{O}}_2}$.
So the statement is completely true as the formula of water and oxide of fluorine is correct.
So the assertion is correct.
Now we will check the reason.
The reason says formulas of any compounds are contained in such a way that more electropositive element comes first and less electropositive element later.
The rule for naming a compound is as follows.
In nomenclature of simple molecular compounds, the more electropositive atom is written first and the more electronegative element is written last with an -ide suffix.
So the reason is also correct.
Also the reason explains the assertion.

So, the correct answer is Option A.

Additional information:
Oxygen fluorides are strong oxidizing agents with high energy and can release their energy either instantaneously or at a controlled rate. Thus, these compounds attracted much attention as potential fuels in jet propulsion systems. As the name suggests oxygen fluoride is a fluoride of oxygen.
Electropositivity can be defined as the tendency of an atom to donate electrons and form positively charged cations. This property is primarily exhibited by metallic elements, especially the alkali metals and the alkaline earth metals. It is important to note that electropositivity is the opposite of electronegativity, which is a measure of the tendency of an atom to gain electrons and form negatively charged anions.

Note: The electropositivity of an element is dependent on several factors such as the metallic character of the element, the distance between the nucleus and the valence shell, the effective nuclear charge acting on the valence electrons, and the ionization energy of the element.