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Chapter 1: Problem 14

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

Short Answer

Expert verified
Redraw nitromethane as CH3−N−O−O with all single bonds, showing neutral atoms.

Step by step solution

01

Understand the given structure

Nitromethane (CH3NO2) typically has a structure with a nitrogen atom bonded to two oxygen atoms (one with a double bond and one with a single bond) and a carbon atom bonded to a nitrogen atom and three hydrogen atoms.
02

Identify atoms and their possible bonds

In this step, recognize that the carbon atom will form four bonds, nitrogen can make three bonds, and each hydrogen will form one bond. Each oxygen normally forms two bonds (considering one bond if it has a charge).
03

Redesign the structure with single bonds

Reorganize the structure so that all atoms have neutral charges by ensuring nitrogen forms three bonds and oxygen forms two bonds. Since all bonds should be single, explore different bonding scenarios.
04

Confirm the neutral charge

Verify that each atom has a neutral charge by making sure the number of bonds corresponds to the valency of each atom: Carbon (4 bonds), Nitrogen (3 bonds), Oxygen (2 bonds), Hydrogen (1 bond).
05

Draw the final structure

The correct structure will have the carbon atom bonded to three hydrogen atoms and one nitrogen atom. The nitrogen will then be bonded to two oxygen atoms using single bonds. Each oxygen atom will also have a lone pair to account for its valence electrons.

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Key Concepts

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

Chemical Bonding
Chemical bonding is the force that holds atoms together in a molecule. This happens because atoms want to achieve a full outer shell of electrons, which makes them more stable.
There are three main types of chemical bonds:
  • **Covalent Bonds**: Atoms share electron pairs.
  • **Ionic Bonds**: Atoms transfer electrons, creating charged ions.
  • **Metallic Bonds**: Electrons are shared over many atoms in a lattice (common in metals).
In nitromethane (CH3NO2), the bonding involves covalent bonds. Here, carbon covalently bonds with hydrogen (H), nitrogen (N), and oxygen (O) atoms. Understanding these bonding types is crucial in predicting molecule behavior and structure.
Lewis Structures
Lewis structures help visualize the bonding in a molecule. They show how atoms share or transfer electrons to achieve full outer shells. To draw a Lewis structure:
  • Determine the total number of valence electrons.
  • Arrange atoms with the least electronegative atom in the center (excluding H).
  • Draw single bonds between central and outer atoms.
  • Distribute remaining electrons to satisfy the octet rule (Hydrogen follows a duet rule).
In the case of nitromethane, carbon is usually central, bonded to three hydrogens, and one nitrogen. The nitrogen then bonds to two oxygens. Adjusting to ensure all atoms have neutral charges is crucial, as in the exercise.
Neutral Atoms
A neutral atom has no overall charge, meaning the number of protons equals the number of electrons. In molecular structures, this balance ensures stability. When drawing structures like nitromethane, it's important to ensure:
  • **Carbons** form 4 bonds (4 valence electrons).
  • **Hydrogens** form 1 bond (1 valence electron).
  • **Nitrogens** form 3 bonds (5 valence electrons).
  • **Oxygens** form 2 bonds (6 valence electrons), plus lone pairs as needed.
In the exercise, we adjust to make sure each element maintains its valence requirements, keeping all atoms neutral.
Valency
Valency is the atom's ability to bond with other atoms, based on the number of electrons it can share or transfer. It stems from the atom's need to fill its outer electron shell. Here’s a summary of valency for key elements:
  • **Carbon (C)**: Valency 4, forms 4 bonds.
  • **Hydrogen (H)**: Valency 1, forms 1 bond.
  • **Nitrogen (N)**: Valency 3, forms 3 bonds (sometimes 5 in certain compounds).
  • **Oxygen (O)**: Valency 2, forms 2 bonds, often with lone pairs.
For neutral nitromethane, ensure these elements follow their valency rules to create correct, stable structures. Verify each atom's bond count matches its valency for neutrality.

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Most popular questions from this chapter

Draw Lewis structures for the following charged species. In each case, the charge is shown closest to the charged atom. (a) \(-\mathrm{OH}\) (b) \(-\mathrm{BH}_{4}\) (c) \({ }^{+} \mathrm{NH}_{4}\) (d) \({ }^{-} \mathrm{Cl}\) (e) \({ }^{+} \mathrm{CH}_{3}\) (f) \({ }^{+} \mathrm{OH}_{3}\) (g) \({ }^{+} \mathrm{NO}_{2}\)

What is the simplest molecule? If \(\mathrm{H}_{2}\) is the second simplest molecule, the answer to this question must be "H \(_{2}\) minus something." What might the "something" be? The answer will appear farther along in the text, so think about this question for a while now.

Each of the following compounds has at least one multiple bond. Draw a Lewis structure for each molecule. Use lines to indicate electrons in bonds and dots to indicate nonbonding electrons. (a) \(\mathrm{F}_{2} \mathrm{CCF}_{2}\) *(b) \(\mathrm{H}_{3} \mathrm{CCN}\) (c) \(\mathrm{H}_{2} \mathrm{CO}\) (d) \(\mathrm{H}_{2} \mathrm{CCO}\) (e) \(\mathrm{H}_{2} \mathrm{CCHCHCH}_{2}\) (f) \(\mathrm{H}_{3} \mathrm{CNO}\) (g) \(\mathrm{H}_{3} \mathrm{COCOH}\)

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.

Write the electronic configurations for the atoms in the fourth row of the periodic table, \({ }_{19} \mathrm{~K}\) through \({ }_{36} \mathrm{Kr}\).
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