The Lewis structure for O_3 molecule is given | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(A) The formal charge is calculated using the formula: $	ext{Formal charge} = 	ext{Total valence electrons} - 	ext{Total non-bonding electrons} - \

Vedclass · Accepted Answer

$-1, 0, +1$

Vedclass · Answer

(A) The formal charge is calculated using the formula: $	ext{Formal charge} = 	ext{Total valence electrons} - 	ext{Total non-bonding electrons} - \frac{1}{2} 	imes 	ext{Total bonding electrons}$.For oxygen atom $1$ (single bonded,$6$ lone pair electrons): $	ext{F.C.} = 6 - 6 - \frac{1}{2}(2) = -1$.For oxygen atom $2$ (double bonded,$4$ lone pair electrons): $	ext{F.C.} = 6 - 4 - \frac{1}{2}(4) = 0$.For oxygen atom $3$ (central atom,$2$ lone pair electrons,$6$ bonding electrons): $	ext{F.C.} = 6 - 2 - \frac{1}{2}(6) = +1$.Thus,the formal charges on oxygen atoms $1, 2, 3$ are $-1, 0, +1$ respectively.

The Lewis structure for $O_3$ molecule is given below. The correct formal charges on oxygen atoms labelled $1$,$2$,$3$ are respectively.

Similar Questions

Which of the following are isoelectronic species?
$I. CH_{3}^{+}$,$II. H_{3}O^{+}$,$III. NH_{3}$,$IV. CH_{3}^{-}$

The correct order of $O-O$ bond length in $O_{2}$, $H_{2}O_{2}$ and $O_{3}$ is

The bond energies of $F_2, Cl_2, Br_2$ and $I_2$ are $155.4, 243.6, 193.2$ and $151.2 \, kJ \, mol^{-1}$ respectively. The strongest bond is......

What is the number of sigma $(\sigma)$ bonds in $P_4O_{10}$?

The number of sigma $(\sigma)$ and pi $(\pi)$ bonds in peroxodisulphuric acid are, respectively:

Vedclass Test Series

Exam Paper Generator

Online Exam Module