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Chapter 1: Problem 11

Add electrons to complete the following Lewis structures. In each case, the charge is placed as close as possible to the charged atom. (a) \({ }^{+} \mathrm{CH}_{2}\) (b) \(-\mathrm{CH}_{2} \mathrm{CH}_{3}\) (c) \(\mathrm{HC}=\mathrm{CH}_{2}\) (d) \({ }^{+} \mathrm{OH}_{3}\) (e) \({ }^{-} \mathrm{OH}\) (f) \({ }^{+} \mathrm{NH}_{2}\) (g) \(-\mathrm{NH}_{2}\) (h) \(\mathrm{CH}_{3}-\mathrm{C} \equiv \mathrm{N}-\mathrm{H}\)

Short Answer

Expert verified
For Bundle aligned to each case scenario adding classified electron pair matching directions+ charge role placing as outlined

Step by step solution

01

- Draw the skeletal structure

Draw the basic structure of each molecule without showing electrons. Depict the atoms connected according to the molecular formula.
02

- Identify valence electrons

Identify the number of valence electrons for each atom. Carbon has 4 valence electrons, Hydrogen has 1, Oxygen has 6, and Nitrogen has 5.
03

- Place electrons around atoms

Distribute the valence electrons around the atoms to complete the octets (or duets for Hydrogen) adhering to the Lewis structure rules.
04

- Adjust for charges

If the molecule has a charge, add or remove electrons accordingly to the charged atom to reflect the overall molecular charge.
05

- Detailed solutions for each part

(a) For \textsuperscript{+}\text{CH}_2: \[ C{\textsuperscript{+}}(1e\textsuperscript{-})-H(2e\textsuperscript{-}) \]
06

Part by Part Explanation

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Skeletal Structure
In organic chemistry, the skeletal structure is a simplified representation of a molecule. It shows the arrangement of atoms and the bonds between them without explicitly depicting the hydrogen atoms bonded to carbons or the lone pairs of electrons. The skeletal structure is the backbone upon which we add further details, such as electron pairs and atomic charges.
To draw a skeletal structure:
  • Identify the main atoms, typically carbon and hydrogen.
  • Connect them based on the molecular formula.
  • Use lines to represent bonds: single lines for single bonds, double lines for double bonds, and triple lines for triple bonds.
  • Do not show hydrogen atoms bonded to carbons explicitly.
  • Only show hydrogen atoms bonded to other atoms like nitrogen or oxygen.
This simplified approach helps visualize complex organic molecules more easily, making it an essential step in constructing Lewis structures.
Valence Electrons
Valence electrons are the outermost electrons of an atom and are crucial in forming chemical bonds. Knowing the number of valence electrons helps in the distribution of electrons in the Lewis structure.
Here's a quick guide:
  • Carbon (C) has 4 valence electrons.
  • Hydrogen (H) has 1 valence electron.
  • Oxygen (O) has 6 valence electrons.
  • Nitrogen (N) has 5 valence electrons.
By identifying the valence electrons of each atom, you can correctly distribute the electrons to ensure stable molecule formation. For example, in a formaldehyde molecule (CH₂O), carbon has 4 valence electrons, hydrogen has 1 each, and oxygen has 6. Counting the total valence electrons guides the correct placement in the structure.
Octet Rule
The octet rule is a principle in chemistry that states atoms tend to form bonds until they have a complete set of eight valence electrons. This rule is essential to understanding how electrons are distributed in a molecule.
To apply the octet rule:
  • Ensure that each atom (except hydrogen, which is satisfied with 2 electrons) is surrounded by 8 electrons.
  • Distribute the valence electrons to complete the octets for each atom.
  • If extra electrons remain after satisfying octets, place them on more electronegative atoms like oxygen or nitrogen.
For example, in water (H₂O), oxygen needs 8 electrons surrounding it but has 6 valence electrons. Each hydrogen contributes 1 electron, allowing oxygen to complete its octet with shared pairs of electrons (forming bonds) and lone pairs.
Molecular Charge
Molecular charge refers to the overall charge of a molecule. For Lewis structures, it's important to adjust the number of electrons based on this charge.
To incorporate molecular charge:
  • If the molecule has a positive charge (cation), remove electrons to decrease the total count.
  • If the molecule has a negative charge (anion), add electrons to increase the total count.
  • Ensure that the charge is represented near the most logical atom, usually the more electronegative one.
For example, in a hydroxide ion (OH⁻), oxygen has 6 valence electrons and hydrogen has 1. Since there's an extra negative charge, add one more electron to oxygen, giving it a total of 8 and satisfying the octet rule while reflecting the overall negative charge.

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Most popular questions from this chapter

Write Lewis dot structures for the neutral diatomic molecules \(\mathrm{F}_{2}\) and \(\mathrm{N}_{2}\). In \(\mathrm{F}_{2}\), there is a single bond between the two atoms, but in \(\mathrm{N}_{2}\) there is a triple bond between the two atoms.

Explain why the two electrons in the \(2 p_{x}\) orbital of carbon \(\left({ }_{6} \mathrm{C}=1 s^{2} 2 s^{2} 2 p_{x}{ }^{2}\right)\) must have paired spins \((+1 / 2\) and \(-1 / 2)\).

Draw another structure for nitromethane in which every atom is neutral. Hint: There are only single bonds in this structure.

Write electronic configurations for the valence electrons of \({ }_{14} \mathrm{Si},{ }_{15} \mathrm{P}\), and \({ }_{16} \mathrm{~S}\). Indicate the spins of the electrons in the \(3 p\) orbitals with a small up or down arrow.

Show the direction of the dipole, if there is one, in the indicated bonds of the following molecules: $$ \mathrm{H}-\mathrm{Cl}, \mathrm{H}-\mathrm{F}, \mathrm{Li}-\mathrm{CH}_{3}, \mathrm{H}_{3} \mathrm{C}-\mathrm{Cl}, \mathrm{HO}-\mathrm{NH}_{2}, \mathrm{H}_{3} \mathrm{C}-\mathrm{CH}_{3} $$
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