Complete Table 7.14 by placing the symbols, formulas, and

Compare the stability of a lithium atom with that of its ion, L i +.

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

Model Draw models to represent the formation of the positive calcium ion and the negative bromide ion

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

Challenge Explain how elements in the two groups shown on the periodic table at the right combine to form an ionic compound.

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

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

Challenge Write the general formula for the ionic compound formed by elements from the two groups shown on the periodic table at the right

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.

Name the following compounds.

Name the following compounds.

Name the following compounds.

Name the following compounds.

Challenge The ionic compound N H 4Cl O 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 Ion 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.

Model Draw a model to represent the physical property of metals known as ductility, or the ability to be drawn into a wire. Base your drawing on the electron sea model shown in Figure 7.11.

How do positive ions and negative ions form?

When do chemical bonds form?

Why are halogens and alkali metals likely to form ions? Explain your answer. C B A D G E F Figure 7.14

The periodic table shown in Figure 7.14 contains elements labeled AG. For each labeled element, state the number of valence electrons and identify the ion that will form

Discuss the importance of electron affinity and ionization energy in the formation of ions. 2s 1s 3s 2p 3p Figure 7.15

The orbital notation of sulfur is shown in Figure 7.15. Explain how sulfur forms its ion

Give the number of valence electrons in an atom of each element. a. cesium d. zinc b. rubidium e. strontium c. gallium

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

Discuss the formation of a 3+ scandium ion using its orbital notation, shown in Figure 7.16.

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?

In Figure 7.14, the element labeled B is barium, and the element labeled E is iodine. Explain why the compound formed between these elements will not be BaI.

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

Look at Figure 7.14; describe the ionic compound that form from the elements represented by C and D.

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: CaKr, N a 2 S, BaC l 3 , MgF? Explain your choices.

Use Table 7.6 to determine which ionic compound has the highest melting point: MgO, KI, or AgCl. Explain your answer

Which has the greater lattice energy, CsCl or KCl? K 2 O or CaO? Explain your choices.

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

When are subscripts used in formulas for ionic compounds?

Discuss how an ionic compound is named.

Using oxidation numbers, explain why the formula Na F 2 is incorrect.

Explain what the name scandium(III) oxide means in terms of electrons lost and gained, and identify the correct formula.

Give the formula for each ionic compound. a. calcium iodide b. silver(I) bromide c. copper(II) chloride d. potassium periodate e. silver(I) acetate

Name each of the following ionic compounds. a. K 2 O b. CaC l 2 c. M g 3 N 2 d. NaClO e. KN O 3

Complete Table 7.14 by placing the symbols, formulas, and names in the blanks. Table 7.14 Identifying Ionic Compounds Cation Anion Name Formula ammonium sulfate Pb F 2 lithium bromide N a 2 C O 3 M g 2+ P O 4 3-

Chrome Chromium, a transition metal used in chrome plating, forms both the C r 2+ and C r 3+ ions. Write the formulas for the ionic compounds formed when each of these ions react with fluorine and oxygen ions

Which are correct formulas for ionic compounds? For those that are not correct, give the correct formula and justify your answer. a. AlCl c. BaO H 2 b. N a 3 S O 4 d. F e 2 O

Write the formulas for all of the ionic compounds that can be formed by combining each of the cations with each of the anions listed in Table 7.15. Name each compound formed. Table 7.15 List of Cations and Anions Cations Anions K + S O 3 2- N H 4 + I - F e 3+ N O 3 -

Describe a metallic bond.

Briefly explain why metallic alloys are made.

Briefly describe how malleability and ductility of metals are explained by metallic bonding

Compare and contrast the two types of metal alloys.

Explain how a metallic bond is similar to an ionic bond.

Brass Copper and zinc are used to form brass, an alloy. Briefly explain why these two metals form a substitutional alloy and not an interstitial alloy

How is a metallic bond different from an ionic bond?

Silver Briefly explain why silver is a good conductor of electricity.

Steel Briefly explain why steel, an alloy of iron, is used to build the supporting structure of many buildings

The melting point of beryllium is 1287C, while that of lithium is 180C. Explain the large difference in values.

Titanium has a boiling point of 3287C, and copper has a boiling point of 2567C. Explain why there is a difference in the boiling points of these two metals.

Alloys Describe the difference between the metal alloy sterling silver and carbon steel in terms of the types of alloys involved.

Give the number of valence electrons for atoms of oxygen, sulfur, arsenic, phosphorus, and bromine.

Explain why calcium can form a C a 2+ ion but not a C a 3+ ion.

Which ionic compounds would have the greatest lattice energy: NaCl, KCl, or MgC l 2 ? Explain your answer

Give the formula for each ionic compound. a. sodium sulfide b. iron(III) chloride c. sodium sulfate d. calcium phosphate e. zinc nitrate

Cobalt, a transition metal, forms both the C o 2+ and C o 3+ ions. Write the correct formulas, and give the name for the oxides formed by the two different ions.

Complete Table 7.16. Table 7.16 Element, Electron, and Ion Data Element Valence Electrons Ion Formed Selenium Tin Iodine Argon

Gold Briefly explain why gold can be used both in jewelry and as a conductor in electronic devices

Discuss the formation of the nickel ion with a 2+ oxidation number.

Compare the oxyanions sulfate and sulfite.

Using electron-dot structures, diagram the formation of an ionic bond between potassium and iodine.

Magnesium forms both an oxide and a nitride when burned in air. Discuss the formation of magnesium oxide and magnesium nitride when magnesium atoms react with oxygen and nitrogen atoms.

An external force easily deforms sodium metal, while sodium chloride shatters when the same amount of force is applied. Why do these two solids behave so differently?

Name each ionic compound. a. CaO b. BaS c. AlP O 4 d. Ba(OH ) 2 e. Sr(N O 3 )

Design a concept map to explain the physical properties of both ionic compounds and metallic solids.

Predict which solid in each pair will have the higher melting point. Explain your answers. a. NaCl or CsCl b. Ag or Cu c. N a 2 O or MgO

Compare and contrast cations and anions

Observe and Infer Identify the mistakes in the incorrect formulas and formula names, and design a flowchart to prevent the mistakes. a. copper acetate d. disodium oxide b. M g 2 O 2 e. A l 2 S O 43 c. P b 2 O 5 S2- Al3+ N3- Ca2+ F- Na+ Figure 7.17

Apply Examine the ions in the beaker shown in Figure 7.17. Identify two compounds that could form using the available ions, and explain why this is possible.

Apply Praseodymium is a lanthanide element that reacts with hydrochloric acid, forming praseodymium(III) chloride. It also reacts with nitric acid, forming praseodymium(III) nitrate. Praseodymium has the electron configuration [Xe]4 f 3 6 s 2 . a. Examine the electron configuration, and explain how praseodymium forms a 3+ ion. b. Write the correct formulas for both compounds formed by praseodymium.

Hypothesize Look at the locations of potassium and calcium on the periodic table. Form a hypothesis to explain why the melting point of calcium is considerably higher than the melting point of potassium.

Assess Explain why the term delocalized is an appropriate term for the electrons involved in metallic bonding.

Apply All uncharged atoms have valence electrons. Explain why elements such as iodine and sulfur do not have metallic bonds.

Analyze Explain why lattice energy is a negative quantity

Ionic Compounds Chrysoberyl is a transparent or translucent mineral that is sometimes opalescent. It is composed of beryllium aluminum oxide, BeA l 2 O 4 . Identify the oxidation numbers of each of the ions found in this compound. Explain the formation of this ionic compound.

You are given a liquid of unknown density. The mass of a graduated cylinder containing 2.00 mL of the liquid is 34.68 g. The mass of the empty graduated cylinder is 30.00 g. Given this information, determine the density of the liquid. (Chapter 2)

In the laboratory, students used a balance and a graduated cylinder to collect the data shown in Table 7.17. Calculate the density of the sample. If the accepted value of this sample is 7.01 g/mL, calculate the percent error. (Chapter 2) Table 7.17 Volume and Mass Data Mass of sample 19.21 g Volume of water alone 39.0 mL Volume of water + sample 43.1 mL

A mercury atom drops in energy from 1.413 1 0 -18 J to 1.069 1 0 -18 J. (Chapter 5) a. What is the energy of the photon emitted by the mercury atom? b. What is the frequency of the photon emitted by the mercury atom? c. What is the wavelength of the photon emitted by the mercury atom?

Which element has the greater ionization energy, chlorine or carbon? (Chapter 6)

Compare and contrast the ways in which metals and nonmetals form ions, and explain why they are different. (Chapter 6)

What are transition elements? (Chapter 6)

Write the symbol and name of the element that fits each description. (Chapter 6) a. the second-lightest of the halogens b. the metalloid with the lowest period number c. the only group 16 element that is a gas at room temperature d. the heaviest of the noble gases e. the group 15 nonmetal that is a solid at room temperature

Free Radicals Many researchers believe that free radicals are responsible for the effects of aging and cancer. Research free radicals, and write about the cause and what can be done to prevent free radicals.

Growing Crystals Crystals of ionic compounds can be easily grown in the laboratory setting. Research the growth of crystals, and design an experiment to grow a crystal in the laboratory.

Identify the anions and cations listed in Table 7.18

Create a bar graph of each ions concentration. Explain why this is a difficult graph to draw.

Sodium chloride is not the only ionic compound that forms from sea water. Identify four other compounds that could be formed that contain the sodium ion. Write both the formula and the name for each compound.