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Chapter 6: Problem 32

Draw Lewis structures for the following molecules. a. \(\mathrm{O}_{2}\) b. \(\mathrm{CS}_{2}\) c. \(\mathrm{N}_{2} \mathrm{O}\)

Short Answer

Expert verified
Lewis structures are visual representations of the bonding between atoms in a molecule, and the lone pairs of electrons in the molecule. The molecules \(\mathrm{O}_{2}\), \(\mathrm{CS}_{2}\), and \(\mathrm{N}_{2} \mathrm{O}\) in their Lewis structures have double and triple bonds which are crucial to fulfill the octet rule for all atoms in the molecule.

Step by step solution

01

Drawing Lewis Structure for \(\mathrm{O}_{2}\)

In \(\mathrm{O}_{2}\), each Oxygen atom has 6 valence electrons. The goal is to form a bond between the two Oxygen atoms and then complete the octets with unshared pairs. Thus, firstly, place an Oxygen atom at the center and another at the border. Draw a double bond between them. Then, add unshared pairs of electrons around each oxygen until each has 8 electrons associated with it, finally resulting in the Lewis structure of O2.
02

Drawing Lewis Structure for \(\mathrm{CS}_{2}\)

In \(\mathrm{CS}_{2}\), the central atom, Carbon, has 4 valence electrons, and the Sulphur atoms acting as side atoms have 6 valence electrons each. First, draw the carbon in the center with one sulfur at either side. Connect each Sulfur to the Carbon via a double bond. Drawing a double bond with each Sulfur completes the octet for Carbon and each Sulfur atom.
03

Drawing Lewis Structure for \(\mathrm{N}_{2} \mathrm{O}\)

In \(\mathrm{N}_{2} \mathrm{O}\), each Nitrogen atom has 5 valence electrons and the Oxygen atom has 6 valence electrons. Place a single Nitrogen atom in the center with one Nitrogen atom and an Oxygen atom on each side. Draw a triple bond between the two Nitrogen atoms and a double bond between the Nitrogen and the Oxygen atom. Complete remaining places around Oxygen atom with lone pairs to fulfill its octet.

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Most popular questions from this chapter

How are the inner-shell electrons represented in a Lewis structure?

According to VSEPR theory, what molecular shapes are associated with the following types of molecules? a. \(\mathrm{AB}\) b. \(\mathrm{AB}_{2}\) c. \(\mathrm{AB}_{3}\) d. \(\mathrm{AB}_{4}\)

How does a Lewis structure show a bond between two atoms that share four electrons?

Devise a set of criteria that will allow you to classify the following substances as covalent, ionic, or metallic: \(\mathrm{CaCO}_{3}, \mathrm{Cu}, \mathrm{H}_{2} \mathrm{O}, \mathrm{NaBr}\) and \(\mathrm{C}(\) graphite). Show your criteria to your teacher.

Draw Lewis structures for the following polyatomic ions. a. \(\mathrm{OH}^{-}\) b. \(\mathrm{O}_{2}^{2-}\) c. \(\mathrm{NO}^{2-}\) d. \(\mathrm{NO}^{2+}\) e. \(\mathrm{AsO}_{4}^{3-}\)
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