Chapter 7

Compare the stability of a lithium atom with that of its ion, Li+

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

Apply Why are all of the elements in group 18 relatively unreactive, whereas those in group 17 are very reactive?

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 b. sulfur c. barium d. lithium

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

Relate lattice energy to ionic-bond strength.

Apply Use electron configurations, orbital notation, and electron-dot structures to represent the formation of an ionic compound from the metal strontium and the nonmetal chlorine.

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

\(\mathrm{CaCl}_{2}\)

\(\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}\)

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.

Design an experiment that could be used to distinguish between a metallic solid and an ionic solid. Include at least two different methods for comparing the solids. Explain your reasoning.

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. a. cesium b. rubidium c. gallium d. zinc e. strontium

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 b. fluorine 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.

Briefly discuss three physical properties of ionic solids that are linked to ionic bonds.

Describe an ionic crystal, and explain why ionic crystals for different compounds might vary in shape.

How does lattice energy change with a change in the size of an ion?

Determine the ratio of cations to anions in each. a. potassium chloride, a salt substitute b. calcium fluoride, used in the steel industry c. calcium oxide, used to remove sulfur dioxide from power-plant exhaust d. strontium chloride, used in fireworks

Discuss the formation of an ionic bond between zinc and oxygen

Using orbital notation, diagram the formation of an ionic bond between aluminum and fluorine.

Using electron configurations, diagram the formation of an ionic bond between barium and nitrogen.

Conductors Under certain conditions, ionic compounds conduct an electric current. Describe these conditions, and explain why ionic compounds are not always used as conductors

Which compounds are not likely to occur: \(\mathrm{CaKr}, \mathrm{Na}_{2} \mathrm{S}\) \(\mathrm{BaCl}_{3}, \mathrm{MgF} ?\) Explain your choices.

Which has the greater lattice energy, CsCl or KCl? \(\mathrm{K}_{2} \mathrm{O}\) or CaO? Explain your choices.

What information do you need to write a correct chemical formula to represent an ionic compound?