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Ch.9 - Molecular Geometry and Bonding Theories
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Brown 14th EditionCh.9 - Molecular Geometry and Bonding Theories문제 57a
9장, 문제 57a

(a) Draw Lewis structures for chloromethane (CH3Cl), chloroethene (C2H3Cl), and chloroethyne (C2HCl).

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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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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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가이드 코스
04:28
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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가이드 코스
02:12
Transition Metals Valence Electrons

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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가이드 코스
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Hybridization
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