Oxygen family Questions in English

(C) The ozone $(O_3)$ molecule is angular in shape and is a resonance hybrid of two contributing structures. Due to resonance,the bond order in ozone is $1.5$,which is intermediate between a single bond $(1)$ and a double bond $(2)$. In molecular oxygen $(O_2)$,the bond order is $2$. Since bond length is inversely proportional to bond order,the $O-O$ bond length in $O_3$ is greater than the $O=O$ bond length in $O_2$. Therefore,statement $C$ is incorrect.

(C) $H_2S_2O_8$ (Peroxodisulphuric acid or Marshall's acid) contains a peroxide linkage ($-O-O-$ bond). The structure is as follows:
$HO-S(=O)_2-O-O-S(=O)_2-OH$

(D) $H_{2}SO_{4}$ saturated with $SO_{3}$ is called $Oleum$ or $Sulphan$.
The chemical reaction is: $H_{2}SO_{4} + SO_{3} \longrightarrow H_{2}S_{2}O_{7}$.

(C) At room temperature and pressure,$P_4O_{10}$ exists as a white solid.
$SO_2$ is a colourless gas.
$NO_2$ is a brown gas.
However,$SO_3$ exists as a colourless,crystalline transparent solid at room temperature,not a gas.
Therefore,the statement that $SO_3$ is a colourless gas is not true.

(B) The reaction of sodium sulfide with sulfur is given by: $Na_{2}S + nS \rightarrow Na_{2}S_{(n+1)}$,where $(X) = Na_{2}S_{(n+1)}$.
The reaction of sodium sulfite with sulfur is given by: $Na_{2}SO_{3} + S \rightarrow Na_{2}S_{2}O_{3}$,where $(Y) = Na_{2}S_{2}O_{3}$.

(D) Statement $I$ is false. While the oxidation state of oxygen in $OF_2$ is $+2$,in $SO_2$,oxygen is in a $-2$ oxidation state. However,the covalency of oxygen is restricted to two due to the absence of $d$-orbitals in its valence shell,meaning it cannot exceed a covalency of two.
Statement $II$ is true; the small size,high electronegativity,and absence of $d$-orbitals account for the anomalous properties of oxygen compared to other group $16$ elements.
Thus,Statement $I$ is false and Statement $II$ is true.