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Chapter 8: Problem 14

Does a Lewis structure tell which electrons come from which atoms? Explain.

Short Answer

Expert verified
A Lewis structure does not indicate which electrons come from which atoms. It is a representation of a molecule or ion that shows the arrangement of atoms and the distribution of valence electrons around each atom, mainly focusing on the distribution of valence electrons and the overall arrangement of atoms to predict the shape and help understand the bonding of a molecule.

Step by step solution

01

Introduction to Lewis Structure

A Lewis structure is a representation of a molecule or ion that shows the arrangement of atoms and the distribution of valence electrons around each atom. Its main purpose is to help predict the shape and to understand the bonding of a molecule.
02

Representing Atoms and Electrons

In a Lewis structure, atoms are represented by their chemical symbols, with single, double, or triple lines between them to indicate bonds. Valence electrons are shown as dots placed around the atoms.
03

Source of Electrons

A Lewis structure does not indicate which electrons come from which atoms. Electrons are shared between bonded atoms to achieve a stable octet (or duet for hydrogen), but the structure does not show the original source of these electrons.
04

Importance of Lewis Structure

Even though a Lewis structure does not show which electrons belong to which atoms, it remains a helpful tool for understanding the chemical bonding and molecular geometry of a molecule or ion. The main focus is on the distribution of valence electrons and the overall arrangement of atoms.

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Most popular questions from this chapter

Use the following data to estimate \(\Delta H_{\mathrm{f}}^{\circ}\) for magnesium fluoride. Lattice energy $$ \begin{aligned} \mathrm{Mg}(s)+\mathrm{F}_{2}(g) \longrightarrow & \mathrm{MgF}_{2}(s) \\ &-2913 \mathrm{~kJ} / \mathrm{mol} \end{aligned} $$ First ionization energy of \(\mathrm{Mg} \quad 735 \mathrm{~kJ} / \mathrm{mol}\) Second ionization energy of \(\mathrm{Mg} \quad 1445 \mathrm{~kJ} / \mathrm{mol}\) \(\begin{array}{ll}\text { Electron affinity of } \mathrm{F} & -328 \mathrm{~kJ} / \mathrm{mol}\end{array}\) Bond energy of \(\mathrm{F}_{2}\) \(154 \mathrm{~kJ} / \mathrm{mol}\) Enthalpy of sublimation for \(\mathrm{Mg}\) 150. \(\mathrm{kJ} / \mathrm{mol}\)

Use the formal charge arguments to rationalize why \(\mathrm{BF}_{3}\) would not follow the octet rule.

Benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right)\) consists of a six- membered ring of carbon atoms with one hydrogen bonded to each carbon. Write Lewis structures for benzene, including resonance structures.

Oxidation of the cyanide ion produces the stable cyanate ion, \(\mathrm{OCN}^{-}\). The fulminate ion, \(\mathrm{CNO}^{-}\), on the other hand, is very unstable. Fulminate salts explode when struck; \(\mathrm{Hg}(\mathrm{CNO})_{2}\) is used in blasting caps. Write the Lewis structures and assign formal charges for the cyanate and fulminate ions. Why is the fulminate ion so unstable? (C is the central atom in \(\mathrm{OCN}^{-}\) and \(\mathrm{N}\) is the central atom in \(\mathrm{CNO}^{-} .\) )

Predict the molecular structure (including bond angles) for each of the following. (See Exercises 111 and \(112 .\) ) a. \(\mathrm{XeCl}_{2}\) b. \(\mathrm{ICl}_{3}\) c. \(\mathrm{TeF}_{4}\) d. \(\mathrm{PCl}_{5}\)
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