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Chapter 6: Problem 30

Draw Lewis structures for the following molecules. Remember that hydrogen can form only a single bond. a. \(\mathrm{NF}_{3} \quad\) d. \(\mathrm{CCl}_{2} \mathrm{F}_{2}\) b. \(\mathrm{CH}_{3} \mathrm{OH} \quad\) e. \(\mathrm{HOCI}\) c. \(\mathrm{CIF}\)

Short Answer

Expert verified
The Lewis structures show how atoms are bonded in molecules, considering that Hydrogen can form only a single bond. The number of valence electrons and how atoms are arranged play a crucial role in building these structures.

Step by step solution

01

Draw Lewis Structures for NF3

The molecule NF3 (Nitrogen trifluoride) contains one nitrogen atom and three fluorine atoms. It's known that nitrogen has 5 valence electrons and fluorine has 7. Arrange the atoms: place Nitrogen in the center and the three Fluorine atoms surrounding it. Draw a single bond between Nitrogen and each Fluorine atom, and distribute the remaining electrons as lone pairs on the atoms. Nitrogen will have one lone pair. Each Fluorine atom will have three lone pairs.
02

Draw Lewis Structures for CCl2F2

The molecule CCl2F2 (Dichlorodifluoromethane) contains one carbon atom, two chlorine atoms, and two fluorine atoms. Carbon has 4 valence electrons, Chlorine has 7, and Fluorine has 7. Arrange the atoms: place Carbon in the center, Chlorine and Fluorine atoms surrounding it. Draw single bonds between the Carbon and each of the Chlorine and Fluorine atoms, and distribute the remaining electrons as lone pairs on the atoms. Each Fluorine and Chlorine atom will have three lone pairs.
03

Draw Lewis Structures for CH3OH

The molecule CH3OH (Methanol) contains one carbon atom, four hydrogen atoms, and one oxygen atom. Carbon has 4 valence electrons, Hydrogen has 1, and Oxygen has 6. Arrange the atoms: place Carbon in the center, the Oxygen atom and three Hydrogen atoms surrounding it, and one Hydrogen atom bonded to the Oxygen. Draw single bonds between these atoms, and distribute the remaining electrons as lone pairs on the Oxygen atom. The Oxygen atom will have two lone pairs.
04

Draw Lewis Structures for HOCl

The molecule HOCl (Hypochlorous acid) contains one hydrogen atom, one oxygen atom, and one chlorine atom. Hydrogen has 1 valence electron, Oxygen has 6, and Chlorine has 7. Arrange the atoms: place Oxygen in the center and Hydrogen and Chlorine atoms surrounding it. Draw single bonds between these atoms, and distribute the remaining electrons as lone pairs on the Oxygen and Chlorine atoms. Oxygen will have two lone pairs and Chlorine will have three lone pairs.
05

Draw Lewis Structures for ClF

The molecule ClF (Chlorine monofluoride) contains one chlorine atom and one fluorine atom. It's known that Chlorine has 7 valence electrons and Fluorine has 7. Arrange the atoms: Chlorine bonded with Fluorine, draw a single bond between them and distribute the remaining electrons as lone pairs on the atoms. Each Chlorine and Fluorine atom will have three pairs of electrons.

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Most popular questions from this chapter

Name the following covalent compounds. a. \(\mathrm{SF}_{4}\) b. \(\mathrm{XeF}_{4}\) c. \(\mathrm{PBr}_{5}\) d. \(\mathrm{N}_{2} \mathrm{O}_{5}\) e. \(\mathrm{Si}_{3} \mathrm{N}_{4}\)

How does a covalent bond differ from an ionic bond?

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

Explain why a halogen is unlikely to form a double bond with another element.

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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