Chapter 10, Problem 10.86P

Interpretation Introduction

Interpretation:

Lewis structure of ${\text{H}}_2{\text{C}}_2{\text{O}}_4$, ${\text{HC}}_2{\text{O}}_4^{-}$, and ${\text{C}}_2{\text{O}}_4^{2-}$ is to be drawn and also the relative $\text{C}-\text{O}$ bond length and bond strength in these molecules are to be compared.

Concept introduction:

The steps to draw the Lewis structure of the molecule are as follows:

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.

Bond order is directly proportional to the bond strength and inversely proportional to the bond length.

A single bond is weaker and longer than a double bond and a triple bond is strongest and shortest.