Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory

McMurry8th EditionChemistryISBN: 9781292336145Not the one you use?Change textbook

McMurry 8th Edition

Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory

Problem 22

Chapter 6, Problem 22

Which of the following spheres is likely to represent a metal atom and which a nonmetal atom? Which sphere in the products represents a cation and which an anion?

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Identify the characteristics of metal and nonmetal atoms. Metals typically lose electrons to form cations and are usually larger in their atomic form. Nonmetals typically gain electrons to form anions and are usually smaller in their atomic form.

Examine the spheres in the image. The larger spheres are likely to represent metal atoms, and the smaller spheres are likely to represent nonmetal atoms.

Determine which spheres represent cations and anions in the products. Cations are positively charged and are smaller than their neutral atoms, while anions are negatively charged and are larger than their neutral atoms.

Compare the sizes of the spheres in the reactants and products. The smaller green sphere in the products likely represents a cation, and the larger red sphere in the products likely represents an anion.

Conclude that the larger green sphere in the reactants represents a metal atom, the larger red sphere in the reactants represents a nonmetal atom, the smaller green sphere in the products represents a cation, and the larger red sphere in the products represents an anion.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Metal and Nonmetal Properties

Metals are typically characterized by their ability to conduct electricity and heat, malleability, ductility, and a shiny appearance. They tend to lose electrons during chemical reactions, forming cations. Nonmetals, on the other hand, are generally poor conductors, brittle in solid form, and can gain or share electrons, forming anions. Understanding these properties helps in identifying which spheres represent metals and nonmetals.

Ionic Compounds and Charge

Ionic compounds are formed when metals react with nonmetals, resulting in the transfer of electrons. Metals lose electrons to become positively charged cations, while nonmetals gain electrons to become negatively charged anions. This charge distinction is crucial for determining the identity of the spheres in the products, as cations and anions will have different colors or sizes based on their electron configurations.

Visual Representation of Atoms

In the provided image, different colored spheres represent various atoms, with size and color often indicating their type and charge. Typically, larger spheres may represent metals (cations) due to their lower electronegativity and tendency to lose electrons, while smaller spheres may represent nonmetals (anions) that gain electrons. Analyzing these visual cues is essential for correctly identifying the nature of each atom in the context of the question.

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Related Practice

Textbook Question

Given the following values for steps in the formation of CaO(s) from its elements, draw a Born–Haber cycle similar to that shown in Figure 6.7. Eea1 for O1g2 = -141 kJ/mol Eea2 for O1g2 = 745.1 kJ/mol Heat of sublimation for Ca1s2 = 178 kJ/mol Ei1 for Ca1g2 = 590 kJ/mol Ei1 for Ca1g2 = 1145 kJ/mol Bond dissociation energy for O21g2 = 498 kJ/mol Lattice energy for CaO1s2 = 3401 kJ/mol

Textbook Question

What is the difference between a molecule and an ion?

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Textbook Question

Given the following information, construct a Born–Haber cycle to calculate the lattice energy of CaCl₂(s). (LO 6.13)

Net energy change for the formation of CaCl₂(s) form Ca(s) and Cl₂(g) = -795.4 kJ/mol

Heat of sublimation for Ca(s) = +178 kJ/mol

E_i1 for Ca(s) = +590 kJ/mol

E_i2 for Ca(g) = +1145 kJ/mol

Bond dissociation energy for Cl₂(g) = +243 kJ/mol

E_ea1 for Cl(g) = -348.6 kJ/mol

(a) 2603 kJ/mol (b) 2254 kJ/mol (c) 2481 kJ/mo (d) 1663 kJ/mol

Textbook Question

Three binary compounds are represented on the following drawing: red with red, blue with blue, and green with green. Give a likely formula for each compound.

Textbook Question

Which element has the largest atomic radius? (LO 5.20) (a) Rb (b) Co(c) Mgd) As

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Textbook Question

For a multielectron atom, a 3s orbital lies lower in energy than a 3p orbital because (LO 5.16)(a) a 3p orbital has more nodal surfaces than a 3s orbital. (b) an electron in a 3p orbital has a higher probability of being closer to the nucleus than an electron in a 3s orbital.(c) inner electrons shield electrons in a 3p orbital more effec-tively than electrons in a 3s orbital. (d) the energy of the electron can be spread between three 3p orbitals instead of only one 3s orbital.

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