Chapter 1.4, Problem 16P

(a)

Interpretation Introduction

Interpretation: The appropriate formal charge of each atoms in given species should be given.

Concept introduction:

• Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).
• Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.
• Formal charge: It is the electrostatic charge that would reside on an atom in a molecule or polyatomic ion if all bonding electron are shared equally between pairs of atoms.
• Formal charge calculation: The formal charge for atom in a molecule or ion is calculated based on the Lewis structure of the molecule or ion by following the given equation below:
• Formal charge calculation of molecule or ion $\text{=NVE-{LPE+}\frac{\text{1}}{\text{2}}\left(\text{BE}\right)$

(b)

Interpretation Introduction

Interpretation: The appropriate formal charge of each atoms in given species should be given.

Concept introduction:

• Lone-pair electrons are valence electrons that are not used in bonding.
• A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.
• Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).
• Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.
• When the atom is neutral, C form 2 bonds, N forms 3 bonds O forms 2 bonds and H or a halogen forms 1 bond.
• A carbocation has a positively charge carbon, a carbon has a negatively charge carbon and a radical has an unpaired electron.

(c)

Interpretation Introduction

Interpretation: The appropriate formal charge of each atoms in given species should be given.

Concept introduction:

• Lone-pair electrons are valence electrons that are not used in bonding.
• A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.
• Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).
• Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.
• When the atom is neutral, C form 2 bonds, N forms 3 bonds O forms 2 bonds and H or a halogen forms 1 bond.
  • A carbocation has a positively charge carbon, a carbon has a negatively charge carbon and a radical has an unpaired electron

(d)

Interpretation Introduction

Interpretation: The appropriate formal charge of each atoms in given species should be given.

Concept introduction:

• Lone-pair electrons are valence electrons that are not used in bonding.
• A proton is positively charged hydrogen ion. A hybrid ion is a negatively charged hydrogen ion.
• Formal charge = the number of valence electron – the number of electrons the atom has to itself (the entire lone pair electron and one – half of the bonding electrons).
• Lewis structure indicates which atom is bonded together and show lone pairs and formal charge.
• When the atom is neutral, C form 2 bonds, N forms 3 bonds O forms 2 bonds and H or a halogen forms 1 bond.
• A carbocation has a positively charge carbon, a carbon has a negatively charge carbon and a radical has an unpaired electron.