(a)
Interpretation:
The kekule structure should be drawn for the given molecule
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.
- 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.
kekule structure:
Without lone pairs of electros in Lewis structures is known as kekule structure.
(b)
Interpretation:
The kekule structure should be drawn for the given molecule
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.
kekule structure:
Without lone pairs of electros in Lewis structures is known as kekule structure.
(c)
Interpretation:
The kekule structure should be drawn for the given molecule
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.
kekule structure:
Without lone pairs of electros in Lewis structures is known as kekule structure.
(d)
Interpretation:
The kekule structure should be drawn for the given molecule
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.
kekule structure:
Without lone pairs of electros in Lewis structures is known as kekule structure.
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