Which of the following molecules has no lone | vedclass

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

Question

(B) The number of lone pairs on the central atom can be calculated using the formula: $	ext{Lone pairs} = \frac{1}{2} [V - B]$,where $V$ is the numbe

Vedclass · Accepted Answer

$SF_6$

Vedclass · Answer

(B) The number of lone pairs on the central atom can be calculated using the formula: $	ext{Lone pairs} = \frac{1}{2} [V - B]$,where $V$ is the number of valence electrons of the central atom and $B$ is the number of bonding electrons (or bonds formed). For $SF_6$: The central atom Sulfur $(S)$ has $6$ valence electrons and forms $6$ bonds with Fluorine atoms. $	ext{Lone pairs} = \frac{1}{2} [6 - 6] = 0$. For $SO_2$: Sulfur has $6$ valence electrons,forms $4$ bonds with Oxygen,leaving $1$ lone pair. For $NH_3$: Nitrogen has $5$ valence electrons,forms $3$ bonds with Hydrogen,leaving $1$ lone pair. For $SF_4$: Sulfur has $6$ valence electrons,forms $4$ bonds with Fluorine,leaving $1$ lone pair. Thus,$SF_6$ has no lone pair on the central atom.

Which of the following molecules has no lone pair of electrons on the central atom?

Similar Questions

The structure of $Cl_2O_7$ is:

The number of lone pairs of electrons on the central $I$ atom in $I_{3}^{-}$ is $.......$

In which of the following molecules are the bond lengths not equal?

The number of species below that have two lone pairs of electrons on their central atom is ..... . (Round off to the nearest integer)
$SF_{4}, BF_{4}^{-}, ClF_{3}, AsF_{3}, PCl_{5}, BrF_{5}, XeF_{4}, SF_{6}$

The molecular shapes of $SF_4$,$CF_4$,and $XeF_4$ are

Vedclass Test Series

Exam Paper Generator

Online Exam Module