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

In the following electron dot structure,the correct calculation of the formal charge on the nitrogen atoms from left to right is $\overset{\centerdot \centerdot}{\mathop{N}}\text{=}\mathop{N}\text{=}\overset{\centerdot \centerdot}{\mathop{N}}$

The formal charge on the central oxygen atom in ozone $(O_3)$ is:

Which of the following is $INCORRECT$ regarding the molecule and the type of overlapping in the bridge bond?

Which of the following molecules is theoretically not possible?

In which of the following molecules,all atoms are coplanar?

Vedclass Test Series

Exam Paper Generator

Online Exam Module