Which of the following compounds do not exist | vedclass

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(D) $1$. $SH_6$: Sulfur has a valence shell configuration of $3s^2 3p^4$. While it can expand its octet to form $SF_6$ due to the high electronegativi

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All of the above

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(D) $1$. $SH_6$: Sulfur has a valence shell configuration of $3s^2 3p^4$. While it can expand its octet to form $SF_6$ due to the high electronegativity of fluorine,hydrogen is not electronegative enough to stabilize the high oxidation state of sulfur in $SH_6$. Thus,$SH_6$ does not exist.$2$. $HFO_4$: Fluorine is the most electronegative element and cannot exhibit positive oxidation states in oxoacids like $HFO_4$. The structure is chemically unstable and does not exist.$3$. $FeI_3$: Iron$(III)$ iodide $(FeI_3)$ is unstable because the $Fe^{3+}$ ion is a strong oxidizing agent and the $I^-$ ion is a strong reducing agent. They undergo a redox reaction to form $FeI_2$ and $I_2$. Therefore,$FeI_3$ does not exist in a stable form.$4$. Since all the given compounds do not exist,the correct option is $D$.

List-$I$ (Molecule / Species)	List-$II$
$(P)$ $NO_2$ (Unpaired electron in)	$(1)$ Vacant $p$-orbital involved in hybridization
$(Q)$ $B_2H_6$	$(2)$ $sp^2$-orbital
$(R)$ $ClO_3$ (Unpaired electron in)	$(3)$ $sp^3$-orbital
$(S)$ $CH_3^+$	$(4)$ $120^\circ$ Bond angle

Which of the following compounds do not exist?

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