Textbook Question
(d) Can two s orbitals combine to form a p bond? Explain.
Ch.9 - Molecular Geometry and Bonding Theories
Chapter 9, Problem 57a
(a) Draw Lewis structures for chloromethane (CH3Cl), chloroethene (C2H3Cl), and chloroethyne (C2HCl).
Verified step by step guidance1
Start by identifying the total number of valence electrons for each molecule. For chloromethane (CH3Cl), carbon has 4 valence electrons, each hydrogen has 1, and chlorine has 7, totaling 14 valence electrons.
For chloromethane (CH3Cl), place carbon in the center as it is the least electronegative. Connect the carbon atom to three hydrogen atoms and one chlorine atom using single bonds. Distribute the remaining electrons to satisfy the octet rule, ensuring chlorine has 8 electrons around it.
For chloroethene (C2H3Cl), calculate the total valence electrons: each carbon has 4, each hydrogen has 1, and chlorine has 7, totaling 18 valence electrons. Place the two carbon atoms in the center, connect them with a double bond, and attach three hydrogen atoms and one chlorine atom using single bonds.
Distribute the remaining electrons in chloroethene (C2H3Cl) to satisfy the octet rule, ensuring each carbon has 8 electrons around it and chlorine also has 8 electrons.
For chloroethyne (C2HCl), calculate the total valence electrons: each carbon has 4, hydrogen has 1, and chlorine has 7, totaling 14 valence electrons. Place the two carbon atoms in the center, connect them with a triple bond, and attach one hydrogen atom and one chlorine atom using single bonds. Distribute the remaining electrons to satisfy the octet rule, ensuring chlorine has 8 electrons around it.
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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 valence electrons and lines to indicate bonds between atoms. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting reactivity.
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Lewis Dot Structures: Ions
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 molecule's structure and stability. For example, carbon has four valence electrons, which allows it to form four bonds, while chlorine has seven, leading to its tendency to form one bond.
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Hybridization
Hybridization is the concept of mixing atomic orbitals to form new hybrid orbitals that can accommodate bonding. It helps explain the geometry of molecules based on the types of bonds formed. For instance, in chloroethene, the carbon atoms undergo sp2 hybridization, resulting in a planar structure with a double bond, which is important for understanding the molecule's reactivity and properties.
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Related Practice
Textbook Question
(b) Imagine that you could hold two atoms that are bonded together, twist them, and not change the bond length. Would it be easier to twist (rotate) around a single s bond or around a double 1s plus p2 bond, or would they be the same?
Textbook Question
(b) What is the hybridization of the carbon atoms in each molecule?
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Textbook Question
Propylene, C3H6, is a gas that is used to form the important polymer called polypropylene. Its Lewis structure is (a) What is the total number of valence electrons in the propylene molecule?