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Ch.24 - The Chemistry of Life: Organic and Biological Chemistry
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
All textbooksBrown 14th EditionCh.24 - The Chemistry of Life: Organic and Biological ChemistryProblem 57a3
Chapter 24, Problem 57a3

(a) Draw Lewis structures for chloromethane 1CH3Cl2, chloroethene 1C2H3Cl2, and chloroethyne 1C2HCl2. Draw Lewis structures for chloroethyne 1C2HCl2.

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Identify the total number of valence electrons for each molecule. For chloromethane (CH3Cl), add the valence electrons of carbon (4), three hydrogens (1 each), and chlorine (7). For chloroethene (C2H3Cl), add the valence electrons of two carbons (4 each), three hydrogens (1 each), and chlorine (7). For chloroethyne (C2HCl), add the valence electrons of two carbons (4 each), one hydrogen (1), and chlorine (7).
Arrange the atoms in each molecule. In chloromethane, carbon is the central atom with three hydrogens and one chlorine attached. In chloroethene, the two carbons form a double bond, with two hydrogens attached to one carbon and one hydrogen and one chlorine attached to the other carbon. In chloroethyne, the two carbons are connected by a triple bond, with one hydrogen attached to one carbon and chlorine attached to the other carbon.
Complete the octets of the surrounding atoms using lone pairs. In chloromethane, ensure that chlorine has three lone pairs. In chloroethene, ensure that the chlorine has three lone pairs and the carbon with one hydrogen has no lone pairs. In chloroethyne, ensure that the chlorine has three lone pairs.
Check the formal charges to ensure the most stable structure. All atoms should ideally have a formal charge of zero, adjusting lone pairs if necessary.
Draw the Lewis structures based on the above steps, showing all valence electrons as either bonding pairs or lone pairs around each atom.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Lewis Structures

Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They use dots to represent electrons and lines to represent bonds between atoms. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting the reactivity of compounds.
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Valence Electrons

Valence electrons are the outermost electrons of an atom and are crucial in determining how atoms bond with each other. The number of valence electrons influences the type of bonds formed (single, double, or triple) and the overall structure of the molecule. Knowing how to count and distribute valence electrons is key to accurately drawing Lewis structures.
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Molecular Geometry

Molecular geometry refers to the three-dimensional arrangement of atoms within a molecule. It is influenced by the number of bonds and lone pairs around the central atom, which can affect the molecule's physical and chemical properties. Understanding molecular geometry helps in predicting the behavior of molecules in reactions and their interactions with other substances.
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Related Practice
Textbook Question
Section 2.9 introduced the idea of structural isomerism, with 1-propanol and 2-propanol as examples. Determine which of these properties would distinguish these two substances: (a) boiling point, (b) combustion analysis results, (c) molecular weight, (d) density at a given temperature and pressure. You can check on the properties of these two compounds in Wolfram Alpha (http://www.wolframalpha.com/) or the CRC Handbook of Chemistry and Physics.
Textbook Question
(c) Write a structural formula for 1-pentanol, the alcohol derived from pentane by making a substitution on one of the carbon atoms.
Textbook Question

Write a balanced chemical equation using condensed structural formulas for

b. the saponification (base hydrolysis) of methyl benzoate.

Textbook Question

(a) Draw Lewis structures for chloromethane 1CH3Cl2, chloroethene 1C2H3Cl2, and chloroethyne 1C2HCl2. Draw Lewis structures for chloroethene 1C2H3Cl2.

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Textbook Question

(a) Draw Lewis structures for chloromethane 1CH3Cl2, chloroethene 1C2H3Cl2, and chloroethyne 1C2HCl2. Draw Lewis structures for chloromethane 1CH3Cl2.