Chapter 7

Compare the stability of a lithium atom with that of its ion, \(\text{Li}^+\).

Describe two different causes of the force of attraction in a chemical bond.

Summarize ionic bond formation by correctly pairing these terms: cation, anion, electron gain, and electron loss.

Apply Write out the electron configuration for each atom. Then, predict the change that must occur in each to achieve a noble-gas configuration. a. nitrogen \(\quad\) b. sulfur \(\quad\) c. barium \(\quad\) d. lithium

Explain how an ionic compound forms from these elements. sodium and nitrogen

Explain how an ionic compound forms from these elements. lithium and oxygen

Explain how an ionic compound forms from these elements. strontium and fluorine

Explain how an ionic compound forms from these elements. aluminum and sulfur

Explain how an ionic compound made up of charged particles can be electrically neutral.

Describe the energy change associated with ionic bond formation, and relate it to stability.

Identify three physical properties of ionic compounds that are associated with ionic bonds, and relate them to bond strength.

Explain how ions form bonds, and describe the structure of the resulting compound.

Design a concept map that shows the relationships among ionic bond strength, physical properties of ionic compounds, lattice energy, and stability.

Write formulas for the ionic compounds formed by the following ions. potassium and iodide

Write formulas for the ionic compounds formed by the following ions. magnesium and chloride

Write formulas for the ionic compounds formed by the following ions. aluminum and bromide

Write formulas for the ionic compounds formed by the following ions. cesium and nitride

Write formulas for ionic compounds composed of the following ions. sodium and nitrate

Write formulas for ionic compounds composed of the following ions. calcium and chlorate

Write formulas for ionic compounds composed of the following ions. aluminum and carbonate

Challenge Write the formula for an ionic compound formed by ions from a group 2 element and polyatomic ions composed of only carbon and oxygen.

Name the following compounds. NaBr

Name the following compounds. \(\mathrm{CaCl}_{2}\)

Name the following compounds. \(\mathrm{KOH}\)

Name the following compounds. \(\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}\)

Name the following compounds. \(\mathrm{Ag}_{2} \mathrm{CrO}_{4}\)

Challenge The ionic compound \(\mathrm{NH}_{4} \mathrm{ClO}_{4}\) is a key reactant used in solid rocket boosters, such as those that power the Space Shuttle into orbit. Name this compound.

State the order in which the ions associated with a compound composed of potassium and bromine would be written in the chemical formula and the compound name.

Describe the difference between a monatomic ion and a polyatomic ion, and give an example of each.

Apply lon \(X\) has a charge of \(2+,\) and ion \(Y\) has a charge of \(1-.\) Write the formula unit of the compound formed from the ions.

State the name and formula for the compound formed from Mg and Cl.

Write the name and formula for the compound formed from sodium ions and nitrite ions.

Analyze What subscripts would you most likely use if the following substances formed an ionic compound? a. an alkali metal and a halogen b. an alkali metal and a nonmetal from group 16 c. an alkaline earth metal and a halogen d. an alkaline earth metal and a nonmetal from group 16

Contrast the structures of ionic compounds and metals.

Explain how the conductivity of electricity and the high boiling points of metals are explained by metallic bonding.

Contrast the cause of the attraction in ionic bonds and metallic bonds.

Summarize alloy types by correctly pairing these terms and phrases: substitutional, interstitial, replaced, and filled in.

How do positive ions and negative ions form?

Why are halogens and alkali metals likely to form ions? Explain your answer.

Discuss the importance of electron affinity and ionization energy in the formation of ions.

Give the number of valence electrons in an atom of each element. \(\begin{array}{ll}{\text { a. cesium }} & {\text { d. zinc }} \\ {\text { b. rubidium }} & {\text { e. strontium }} \\ {\text { c. gallium }}\end{array}\)

Explain why noble gases are not likely to form chemical bonds.

Discuss the formation of the barium ion.

Explain how an anion of nitrogen forms.

The more reactive an atom, the higher its potential energy. Which atom has higher potential energy, neon or fluorine? Explain.

Explain how the iron atom can form both an iron \(2+\) ion and an iron \(3+\) ion.

Predict the reactivity of each atom based on its electron configuration. a. potassium \(\quad\) b. fluorine \(\quad\) c. neon

What does the term electrically neutral mean when discussing ionic compounds?

Discuss the formation of ionic bonds.

Explain why potassium does not bond with neon to form a compound.