The possible Lewis formulas for each of the following molecules should be drawn and explained. . Concept Introduction: Lewis dot structures also called as Lewis structures, Lewis dot structures, Lewis dot formulas, or Lewis electron dot structures (LEDS) or electron dot structures, are structures which demonstration the bonding amid atoms of a molecule and the lone pairs of electrons of the molecule. Below are the general rules of Lewis do structure: - Step 1− In the first step, first count the total number of valence electrons. While counting for ions charges should also be considered. Step 2 − In the second step, calculate the total number of electrons which would be required for every atom to complete the octet. Step 3 − In the third step, find the total number of bonding or shared electron by subtracting the results of step 1 from step 2. Step 4 − In the fourth step, each bond should be assigned the two-bonding electron. Step 5 − In the fifthstep, assign the remaining bonding electrons in pairs to form some of the bonds, the double bond and triple bond. Step 6 − In the sixth step, assign the outstanding electrons as lone pairs, so that all the atoms are provided to the octets Step 7 − In the last step, formal charges should be determined and place them subsequently to the suitable atoms.

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Chapter 4, Problem 86AP

Interpretation Introduction

Interpretation:

The possible Lewis formulas for each of the following molecules should be drawn and explained.

.

Concept Introduction:

Lewis dot structures also called as Lewis structures, Lewis dot structures, Lewis dot formulas, or Lewis electron dot structures (LEDS) or electron dot structures, are structures which demonstration the bonding amid atoms of a molecule and the lone pairs of electrons of the molecule.

Below are the general rules of Lewis do structure: -

Step 1− In the first step, first count the total number of valence electrons. While counting for ions charges should also be considered.

Step 2 − In the second step, calculate the total number of electrons which would be required for every atom to complete the octet.

Step 3 − In the third step, find the total number of bonding or shared electron by subtracting the results of step 1 from step 2.

Step 4 − In the fourth step, each bond should be assigned the two-bonding electron.

Step 5 − In the fifthstep, assign the remaining bonding electrons in pairs to form some of the bonds, the double bond and triple bond.

Step 6 − In the sixth step, assign the outstanding electrons as lone pairs, so that all the atoms are provided to the octets

Step 7 − In the last step, formal charges should be determined and place them subsequently to the suitable atoms.

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