Question

Determine the number of bonding electrons and the number of nonbonding electrons in the structure of cs2.

Answer 1

Carbon disulfide ( S=C=S)  is made up of one carbon atom and two sulfur atom. 
Carbon has 4 valence electrons while sulfur has 6 electrons. 
During bonding all the four carbon valence electrons are used in bonding while each sulfur atom contributes two electrons two the bond formation.
Therefore; 4 + 2(2) = 8 electrons are used for bonding, while 8 electrons ( four from each sulfur atom) are not used for bond formation. 

Answer 2

The number of bonding and non-bonding electrons in ${\text{C}}{{\text{S}}_2}$ are $\boxed8$ and $\boxed8$ respectively.

Further explanation:

In order to determine the number of bonding and non-bonding electrons first, we need to draw the correct Lewis structure of ${\text{C}}{{\text{S}}_2}$ the molecule.

The Lewis structure is the chemical representation of an element along with the nonbonding pairs. For covalent molecules, the number of electrons involved in bonding and the remaining nonbonding pairs can be represented while writing the Lewis structures. Lewis structures help predict the geometry, polarity, and reactivity of the molecules.

The central atom is usually the least electronegative atom other than hydrogen. Hence out of carbon and sulphur, the former will act as the central metal atom. So arrange the two sulphur atoms around the carbon. Next, determine the number of valence electrons.

The total number of valence electrons of ${\text{C}}{{\text{S}}_2}$ is calculated as,

${\text{Total valence electrons}} = \left[ {\left( {\text{1}} \right)\left( {{\text{Valence electrons of Carbon}}} \right){t{ + }}\left( 2 \right)\left( {{\text{Valence electrons of sulphur}}} \right)} \right]$  

Since carbon carries 4 valence electron and sulphur carries 6 valence electrons. So,

$\begin{aligned}{\text{Total valence electrons}}\left( {{\text{TVE}}} \right) &= \left[ {\left( 1 \right)\left( 4 \right)+\left( 2\right)\left( 6 \right)}\right]\\&= 16\\\end{aligned}$  

Lewis structure of ${\mathbf{C}}{{\mathbf{S}}_{\mathbf{2}}}$ and its linear shape along with the bonding and non-bonding electron pairs is apparent in the attached image.

Out of 16 electrons, eight electrons are involved in the formation of four bonds between the carbon and two sulfur atom. Carbon forms one sigma and one pi bond with each sulfur atom respectively. So now we are left with 8 electrons. These will constitute the non-bonding (lone pairs). 2 lone are present on each sulfur atom.

Learn more:

1. Coordination number for lithium sulfide crystals: https://brainly.com/question/75586212

2. Scientific notation: https://brainly.com/question/4935921

Answer details:  

Grade: High School

Subject: Chemistry

Chapter: Molecular structure and chemical bonding.

Keywords: Lewis structure, valence electrons, CS2, a single bond, bonding electrons, non-bonding electrons, and total valence electrons.