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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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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Valence Electrons
Valence electrons are the outermost electrons in an atom and are crucial in determining an atom's ability to bond with other atoms. They dictate the chemical properties and reactivity of an element. Every atom strives to have a full set of valence electrons, typically eight, aligning with the octet rule for stability. This concept is pivotal in Lewis structures, which visualize these valence electrons as dots around elemental symbols.
  • Valence electrons are involved in forming bonds鈥攕ingle, double, or triple鈥攂etween atoms.
  • In Lewis structures, valence electrons can be shared between atoms to form covalent bonds or transferred to achieve stability.
Understanding valence electrons aids in predicting how different atoms will interact and bond within a molecule, forming the foundation for understanding molecular structure.
Molecular Geometry
Molecular geometry refers to the three-dimensional shape or arrangement of atoms within a molecule. This geometrical configuration is a consequence of the spatial arrangements of valence electron pairs around the central atom, often predicted using Lewis structures. For a molecule to be stable, these electron pairs, including bonding and nonbonding pairs, arrange themselves to minimize repulsions according to the VSEPR theory鈥擵alence Shell Electron Pair Repulsion theory.
  • VSEPR theory helps in predicting the geometry of a molecule based on the repulsion between electron pairs.
  • Common molecular shapes include linear, bent, tetrahedral, trigonal planar, and trigonal pyramidal.
The molecular geometry not only influences physical properties such as boiling and melting points but also chemical reactivity and interaction with other molecules.
Chemical Bonding
Chemical bonding is the process whereby atoms combine to form molecules. There are several types of bonds, including ionic, covalent, and metallic bonds, each forming through different interactions among valence electrons. Lewis structures are particularly useful in visualizing covalent bonding, where electrons are shared between atoms.
  • Covalent bonds arise when two atoms share one or more pairs of valence electrons to achieve stability.
  • Ionic bonds occur when electrons are transferred from one atom to another, forming charged ions.
  • Metallic bonds arise within metals, with electrons forming a "sea" that allows them to move freely.
By representing molecules with Lewis structures, one can quickly gain insights into potential bonding patterns, molecular shapes, and reactivity. Understanding chemical bonding through these visual models is essential for the study and application of chemistry.

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Most popular questions from this chapter

Without using Fig. \(8.3\), predict which bond in each of the following groups will be the most polar. a. \(\mathrm{C}-\mathrm{H}, \mathrm{Si}-\mathrm{H}, \mathrm{Sn}-\mathrm{H}\) b. \(\mathrm{Al}-\mathrm{Br}, \mathrm{Ga}-\mathrm{Br}, \mathrm{In}-\mathrm{Br}, \mathrm{Tl}-\mathrm{Br}\) c. \(\mathrm{C}-\mathrm{O}\) or \(\mathrm{Si}-\mathrm{O}\) d. \(\mathrm{O}-\mathrm{F}\) or \(\mathrm{O}-\mathrm{Cl}\)

In general, the higher the charge on the ions in an ionic compound, the more favorable the lattice energy. Why do some stable ionic compounds have \(+1\) charged ions even though \(+4,+5\), and \(+6\) charged ions would have a more favorable lattice energy?

Write electron configurations for the most stable ion formed by each of the elements Te, \(\mathrm{Cl}, \mathrm{Sr}\), and \(\mathrm{Li}\) (when in stable ionic compounds).

Consider the following: \(\operatorname{Li}(s)+\frac{1}{2} \mathrm{I}_{2}(g) \rightarrow \operatorname{LiI}(s) \Delta H=\) \(-292 \mathrm{~kJ} . \mathrm{LiI}(s)\) has a lattice energy of \(-753 \mathrm{~kJ} / \mathrm{mol}\). The ionization energy of \(\operatorname{Li}(g)\) is \(520 . \mathrm{kJ} / \mathrm{mol}\), the bond energy of \(\mathrm{I}_{2}(g)\) is \(151 \mathrm{~kJ} / \mathrm{mol}\), and the electron affinity of \(\mathrm{I}(g)\) is \(-295 \mathrm{~kJ} / \mathrm{mol}\). Use these data to determine the heat of sublimation of \(\operatorname{Li}(s)\).

Use the following data to estimate \(\Delta H_{\mathrm{f}}^{\circ}\) for barium bromide. $$ \mathrm{Ba}(s)+\mathrm{Br}_{2}(g) \longrightarrow \operatorname{BaBr}_{2}(s) $$ $$ \begin{array}{lr} \text { Lattice energy } & -1985 \mathrm{~kJ} / \mathrm{mol} \\ \text { First ionization energy of Ba } & 503 \mathrm{~kJ} / \mathrm{mol} \\ \text { Second ionization energy of Ba } & 965 \mathrm{~kJ} / \mathrm{mol} \\ \text { Electron affinity of } \mathrm{Br} & -325 \mathrm{~kJ} / \mathrm{mol} \\\ \text { Bond energy of } \mathrm{Br}_{2} & 193 \mathrm{~kJ} / \mathrm{mol} \\ \text { Enthalpy of sublimation of } \mathrm{Ba} & 178 \mathrm{~kJ} / \mathrm{mol} \end{array} $$
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