Chapter 10, Problem 10.78P

Interpretation Introduction

Interpretation:

From the given mass percentage composition of carbon, hydrogen, and chlorine Lewis structure of the unknown gaseous compound is to be determined.

Concept introduction:

An empirical formula gives the simplest whole number ratio of atoms of each element present in a molecule. The molecular formula tells the exact number of atoms of each element present in a molecule.

To draw the Lewis structure of the molecule there are following steps:

Step 1: Find the central atom and place the other atoms around it. The atom in a compound which has the lowest group number or lowest electronegativity considered as the central atom.

Step 2: Calculate the total number of valence electrons.

Step 3: Connect the other atoms around the central atoms to the central atom with a single bond and lower the value of valence electrons by 2 of every single bond.

Step 4: Allocate the remaining electrons in pairs so that each atom can get 8 electrons.

Step 5: Convert the lone pair into bond pair.

The formula for calculation of the density is as follows:

  $\text{d}=\frac{\text{PM}}{\text{RT}}$        (1)

Here,

$\text{d}$ is density.

$\text{P}$ is pressure.

$\text{M}$ is molar mass.

$\text{R}$ is universal gas constant.

$\text{T}$ is temperature.