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Ch.9 - Molecular Geometry and Bonding Theories
Brown - Chemistry: The Central Science 14th Edition
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Tutti i libri di testoBrown 14th EditionCh.9 - Molecular Geometry and Bonding TheoriesProblema 60e
Capitolo 9, Problema 60e

Ethyl acetate, C4H8O2, is a fragrant substance used both as a solvent and as an aroma enhancer. Its Lewis structure is
(e) How many valence electrons remain in nonbonding pairs in the molecule?

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1
Determine the total number of valence electrons in the molecule by adding the valence electrons of each atom: Carbon (C) has 4 valence electrons, Hydrogen (H) has 1, and Oxygen (O) has 6.
Calculate the total number of valence electrons for ethyl acetate, C_4H_8O_2, by multiplying the number of each type of atom by its valence electrons and summing them up.
Draw the Lewis structure of ethyl acetate, ensuring that each atom achieves a full valence shell, typically 8 electrons for C and O, and 2 for H.
Identify the bonding pairs of electrons (shared between atoms) and subtract these from the total number of valence electrons to find the number of nonbonding electrons.
Count the remaining electrons that are not involved in bonding (lone pairs) to determine how many valence electrons remain in nonbonding pairs in the molecule.

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Valence Electrons

Valence electrons are the outermost electrons of an atom and are crucial for chemical bonding. In the context of molecules, they determine how atoms interact and bond with each other. For ethyl acetate, understanding the total number of valence electrons helps in constructing its Lewis structure and analyzing its bonding and nonbonding electron pairs.
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Transition Metals Valence Electrons

Lewis Structure

A Lewis structure is a diagram that represents the bonding between atoms in a molecule and the lone pairs of electrons that may exist. It visually depicts how valence electrons are arranged among atoms, showing both bonding pairs (shared electrons) and nonbonding pairs (lone pairs). For ethyl acetate, drawing the Lewis structure is essential to identify the distribution of electrons and to count the nonbonding pairs.
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Lewis Dot Structures: Ions

Nonbonding Electron Pairs

Nonbonding electron pairs, also known as lone pairs, are pairs of valence electrons that are not involved in bonding with other atoms. These pairs can influence the molecular geometry and reactivity of a compound. In ethyl acetate, calculating the number of nonbonding pairs is important for understanding its molecular shape and properties, as they affect how the molecule interacts with other substances.
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