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.

Question

Want to see the full answer?

Answer 1

Question

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.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Students have asked these similar questions

Name the molecules & Identify any chiral center CH3CH2CH2CHCH₂CH₂CH₂CH₂ OH CH₂CHCH2CH3 Br CH3 CH3CHCH2CHCH2CH3 CH3

Curved arrows are used to illustrate the flow of electrons. Using the provided starting and product structures, draw the curved electrons-pushing arrows for the following reaction or mechanistic step(s).

Answer 2

Question

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.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 3

Question

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.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 4

Question

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.

Expert Solution & Answer

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 5

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.

Answer 6

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.

Answer 7

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.

Answer 8

Expert Solution & Answer

Answer 9

Expert Solution & Answer

Answer 10

Want to see the full answer?

Check out a sample textbook solution

See solution

Answer 11

Ch. 4 - Prob. 1RQ Ch. 4 - Prob. 2RQ Ch. 4 - What are the structural differences among chlorine...Ch. 4 - Prob. 4RQ Ch. 4 - What are the charges on simple ions formed from...Ch. 4 - Prob. 6RQ Ch. 4 - In what group of the periodic table would elements...Ch. 4 - Prob. 8RQ Ch. 4 - Prob. 9RQ Ch. 4 - Prob. 10P

Concept explainers

Videos

Want to see the full answer?

Chapter 4 Solutions