Determine whether each acid is a binary acid or an oxyacid and name each acid. If the

Do the properties of an element change when it combines with another element to form a compound? Explain.

How might the world be different if elements did not combine to form compounds?

What is the law of constant composition? Who discovered it?

What is a chemical formula? List some examples.

In a chemical formula, which element is listed first?

In a chemical formula, how do you calculate the number of atoms of an element within parentheses? Provide an example.

Explain the difference between a molecular formula and an empirical formula.

What is a structural formula? What is the difference between a structural formula and a molecular model?

What is the difference between a molecular element and an atomic element? List the elements that occur as diatomic molecules.

What is the difference between an ionic compound and a molecular compound?

What is the difference between a common name for a compound and a systematic name?

List the metals that form only one type of ion (that is, metals whose charge is invariant from one compound to another). What are the group numbers of these metals?

Identify the block in the periodic table of metals that tend to form more than one type of ion.

What is the basic form for the names of ionic compounds containing a metal that forms only one type of ion?

What is the basic form for the names of ionic compounds containing a metal that forms more than one type of ion?

How are compounds containing a polyatomic ion named?

Why are roman numerals needed in the names of ionic compounds containing a metal that forms more than one type of ion?

Which polyatomic ions have a 2- charge? Which polyatomic ions have a 3- charge?

What is the basic form for the names of molecular compounds?

How many atoms does each prefix specify? mono-, di-, tri-, tetra-, penta-, hexa-.

What is the basic form for the names of binary acids?

What is the basic form for the name of oxyacids whose oxyanions end with -ate?

What is the basic form for the name of oxyacids whose oxyanions end with -ite?

What is the formula mass of a compound?

Two samples of sodium chloride are decomposed into their constituent elements. One sample produces 4.65 g of sodium and 7.16 g of chlorine, and the other sample produces 7.45 g of sodium and 11.5 g of chlorine. Are these results consistent with the law of constant composition? Explain your answer.

Two samples of carbon tetrachloride are decomposed into their constituent elements. One sample produces 32.4 g of carbon and 373 g of chlorine, and the other sample produces 12.3 g of carbon and 112 g of chlorine. Are these results consistent with the law of constant composition? Explain your answer.

Upon decomposition, one sample of magnesium fluoride produced 1.65 kg of magnesium and 2.57 kg of fluorine. A second sample produced 1.32 kg of magnesium. How much fluorine (in grams) did the second sample produce?

Use the law of constant composition to complete the table summarizing the amounts of nitrogen and oxygen produced upon the decomposition of several samples of dinitrogen monoxide.

The mass ratio of sodium to fluorine in sodium fluoride is 1.21:1. A sample of sodium fluoride produces 34.5 g of sodium upon decomposition. How much fluorine (in grams) forms?

Use the law of constant composition to complete the table summarizing the amounts of iron and chlorine produced upon the decomposition of several samples of iron(III) chloride.

Write a chemical formula for the compound containing one nitrogen atom for every three iodine atoms.

Write a chemical formula for the compound containing one carbon atom for every four bromine atoms.

Write chemical formulas for compounds containing: (a) three iron atoms for every four oxygen atoms (b) one phosphorus atom for every three chlorine atoms (c) one phosphorus atom for every five chlorine atoms (d) two silver atoms for every oxygen atom

Write chemical formulas for compounds containing: (a) one calcium atom for every two iodine atoms (b) two nitrogen atoms for every four oxygen atoms (c) one silicon atom for every two oxygen atoms (d) one zinc atom for every two chlorine atoms

How many hydrogen atoms are in each of the formulas in Question 35?

How many oxygen atoms are in each chemical formula? (a) \(\mathrm{H}_{3} \mathrm{PO}_{4}\) (b) \(\mathrm{Na}_{2} \mathrm{HP}_{4}\) (c) \(\mathrm{Ca}\left(\mathrm{HCO}_{3}\right)_{2}\) (d) \(B a\left(C_{2} H_{3} O_{2}\right)_{2}\) Equation Transcription: Text Transcription: H_3PO_4 Na_2HP_4 Ca(HCO_3)_2 Ba(C_2H_3O_2)_2

Determine the number of each type of atom in each formula. (a) \(\mathrm{MgCI}_{2}\) (b) \(\mathrm{NaNO}_{3}\) (c) \(\mathrm{Ca}\left(\mathrm{NO}_{2}\right)_{2}\) (d) \(\mathrm{Sr}(\mathrm{OH})_{2}\) Equation Transcription: Text Transcription: MgCI_2 NaNO_3 Ca(NO_2)_2 Sr(OH)_2

Determine the number of each type of atom in each formula. (a) \(\mathrm{NH}_{4} \mathrm{CI}\) (b) \(M g_{3}\left(P O_{4}\right)_{2}\) (c) NaCN (d) \(\left.B a(H C)_{3}\right)_{2}\) Equation Transcription: Text Transcription: NH_4CI Mg_3(PO_4)_2 Ba(HC)_3)_2

Complete the table.

Complete the table.

Give the empirical formula that corresponds to each molecular formula. (a) \(\mathrm{C}_{2} \mathrm{H}_{6}\) (b) \(\mathrm{~N}_{2} \mathrm{O}_{4}\) (c) \(\mathrm{C}_{4} \mathrm{H}_{6} \mathrm{O}_{2}\) (d) \(\mathrm{NH}_{3}\) Equation Transcription: Text Transcription: C_2 H_6 N_2 O_4 C_4 H_6 O_2 NH_3

Give the empirical formula that corresponds to each molecular formula. (a) \(\mathrm{C}_{2} \mathrm{H}_{2}\) (b) \(\mathrm{CO}_{2}\) (c) \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\) (d) \(\mathrm{~B}_{2} \mathrm{H}_{6}\) Equation Transcription: Text Transcription: C_2 H_2 CO_2 C_6 H_12 O_6 B_2 H_6

Classify each element as atomic or molecular. (a) chlorine (b) argon (c) cobalt (d) hydrogen

Which elements have molecules as their basic units? (a) helium (b) oxygen (c) iron (d) bromine

Classify each compound as ionic or molecular. (a) \(\mathrm{CS}_{2}\) (b) CuO (c) KI (d) \(\mathrm{PCI}_{3}\) Equation Transcription: Text Transcription: CS_2 PCI_3

Classify each compound as ionic or molecular. (a) \(\mathrm{PtO}_{2}\) (b) \(\mathrm{CF}_{2} \mathrm{Cl}_{2}\) (c) CO (d) \(\mathrm{SO}_{3}\) Equation Transcription: Text Transcription: PtO_2 CF_2 CI_2 SO_3

Match the substances on the left with the basic units that compose them on the right. helium molecules \(\mathrm{CCI}_{4}\) formula units \(\mathrm{~K}_{2} \mathrm{SO}_{4}\) diatomic molecules bromine single atoms Equation Transcription: Text Transcription: CCI_4 K_2 SO_4

Match the substances on the left with the basic units that compose them on the right. \(\mathrm{NI}_{3}\) molecules copper metal single atoms \(\mathrm{SrCl}_{2}\) diatomic molecules nitrogen formula units Equation Transcription: Text Transcription: NI_3 SrCl_2

What are the basic units—single atoms, molecules, or formula units—that compose each substance? (a) \(B a B r_{2}\) (b) Ne (c) \(I_{2}\) (d) CO Equation Transcription: Text Transcription: BaBr_2 I_2

What are the basic units—single atoms, molecules, or formula units—that compose each substance? (a) \(\mathrm{Rb}_{2} \mathrm{O}\) (b) \(\mathrm{N}_{2}\) (c) \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{2}\) (d) \(\mathrm{~N}_{2} \mathrm{~F}_{4}\) Equation Transcription: Text Transcription: Rb_2 O N_2 Fe(NO_3)_2 N_2 F_4

Classify each compound as ionic or molecular. If it is ionic, determine whether the metal forms only one type of ion or more than one type of ion. (a) KCl (b) \(\mathrm{CBr}_{4}\) (c) \(\mathrm{NO}_{2}\) (d) \(\mathrm{Sn}\left(\mathrm{SO}_{4}\right)_{2}\) Equation Transcription: Text Transcription: CBr_4 NO_2 Sn(SO_4)_2

Classify each compound as ionic or molecular. If it is ionic, determine whether the metal forms only one type of ion or more than one type of ion. (a) \(\mathrm{CoCl}_{2}\) (b) \(\mathrm{CF}_{4}\) (c) \(\mathrm{BaSO}_{4}\) (d) NO Equation Transcription: Text Transcription: CoCl_2 CF_4 BaSO_4

Write a formula for the ionic compound that forms from each pair of elements. (a) sodium and sulfur (b) strontium and oxygen (c) aluminum and sulfur (d) magnesium and chlorine

Write a formula for the ionic compound that forms from each pair of elements. (a) aluminum and oxygen (b) beryllium and iodine (c) calcium and sulfur (d) calcium and iodine

Write a formula for the compound that forms from potassium and (a) acetate (b) chromate (c) phosphate (d) cyanide

Write a formula for the compound that forms from calcium and (a) hydroxide (b) carbonate (c) phosphate (d) hydrogen phosphate

Write formulas for the compounds formed from the element on the left and each of the elements on the right. (a) Li N, O, F b) Ba N, O, F (c) Al N, O, F

Name each ionic compound. In each of these compounds, the metal forms only one type of ion. (a) CsCl (b) \(\mathrm{SrBr}_{2}\) (c) \(\mathrm{~K}_{2} \mathrm{O}\) (d) LiF Equation Transcription: Text Transcription: SrBr_2 K_2 O

Write formulas for the compounds formed from the element on the left and each polyatomic ion on the right. (a) Rb NO3 -, SO4 2-, PO4 3- (b) Sr NO3 -, SO4 2-, PO4 3- (c) In NO3 -, SO4 2-, PO4 3- (Assume In charge is 3+.) Equation Transcription: Text Transcription: NO_3 ^- , SO_4 ^2- , PO_4 ^3-

Name each ionic compound. In each of these compounds, the metal forms only one type of ion. (a) LiI (b) MgS (c) \(B a F_{2}\) (d) NaF Equation Transcription: Text Transcription: BaF_2

Name each ionic compound. In each of these compounds, the metal forms more than one type of ion. (a) \(\mathrm{CrCl}_{2}\) (b) \(\mathrm{CrCl}_{3}\) (c) \(\mathrm{SnO}_{2}\) (d) \(\mathrm{PbI}_{2}\) Equation Transcription: Text Transcription: CrCl_2 CrCl_3 SnO_2 PbI_2

Name each ionic compound. In each of these compounds, the metal forms more than one type of ion. (a) \(\mathrm{HgBr}_{2}\) (b) \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) (c) \(\mathrm{Cu}_{2}\) (d) \(\mathrm{SnCl}_{4}\) Equation Transcription: Text Transcription: HgBr_2 Fe_2 O_3 CuI_2 SnCl_4

Determine whether the metal in each ionic compound forms only one type of ion or more than one type of ion and name the compound accordingly. (a) \(\mathrm{Cr}_{2} \mathrm{O}_{3}\) (b) NaI (c) \(\mathrm{CaBr}_{2}\) (d) SnO Equation Transcription: Text Transcription: Cr_2 O_3 CaBr_2

Determine whether the metal in each ionic compound forms only one type of ion or more than one type of ion and name the compound accordingly. (a) \(\mathrm{FeI}_{3}\) (b) \(\mathrm{PbCl}_{4}\) (c) \(\mathrm{SrI}_{2}\) (d) BaO Equation Transcription: Text Transcription: FeI_3 PbCl_4 SrI_2

Name each ionic compound containing a polyatomic ion. (a) \(\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}\) (b) \(\mathrm{~Pb}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2}\) (c) \(\mathrm{NH}_{4} \mathrm{I}\) (d) \(\mathrm{KClO}_{3}\) (e) \(\mathrm{CoSO}_{4}\) (f) \(\mathrm{NaClO}_{4}\) Equation Transcription: Text Transcription: Ba(NO_3)_2 Pb(C_2 H_3 O_2)_2 NH_4 I KClO_3 CoSO_4 NaClO_4

Name each ionic compound containing a polyatomic ion. (a) \(\mathrm{Ba}(\mathrm{OH})_{2}\) (b) \(\mathrm{Fe}(\mathrm{OH})_{3}\) (c) \(\mathrm{Cu}\left(\mathrm{NO}_{2}\right)_{2}\) (d) \(\mathrm{PbSO}_{4}\) (e) KClO (f) \(\mathrm{Mg}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2}\) Equation Transcription: Text Transcription: Ba(OH)_2 Fe(OH)_3 Cu(NO_2)_2 PbSO_4 Mg(C_2 H_3 O_2)_2

Name each polyatomic ion. (a) BrO- (b) \(\mathrm{BrO}_{2}\) - (c) \(\mathrm{BrO}_{3}\) - (d) \(\mathrm{BrO}_{4}\) - Equation Transcription: Text Transcription: BrO_2 BrO_3 BrO_4

Name each polyatomic ion. (a) IO- (b) \(\mathrm{IO}_{2}\) - (c) \(\mathrm{IO}_{3}\) - (d) \(\mathrm{IO}_{4}\) - Equation Transcription: Text Transcription: IO_2 IO_3 IO_4

Problem 69P Write a formula for each ionic compound. (a) copper(II) bromide (b) silver nitrate (c) potassium hydroxide (d) sodium sulfate (e) potassium hydrogen sulfate (f) sodium hydrogen carbonate

Write a formula for each ionic compound. (a) copper(I) chlorate (b) potassium permanganate (c) lead(II) chromate (d) calcium fluoride (e) iron(II) phosphate (f) lithium hydrogen sulfite

Name each molecular compound. (a) \(\mathrm{SO}_{2}\) (b) \(\mathrm{NI}_{3}\) (c) \(\mathrm{BrF}_{5}\) (d) NO (e) \(\mathrm{~N}_{4} \mathrm{Se}_{4}\) Equation Transcription: Text Transcription: SO_2 NI_3 BrF_5 N_4 Se_4

Name each molecular compound. (a) \(\mathrm{XeF}_{4}\) (b) \(\mathrm{PI}_{3}\) (c) \(\mathrm{SO}_{3}\) (d) \(\mathrm{SiCl}_{4}\) (e) \(\mathrm{I}_{2} \mathrm{O}_{5}\) Equation Transcription: Text Transcription: XeF_4 PI_3 SO_3 SiCl_4 I_2 O_5

Write a formula for each molecular compound. (a) carbon monoxide (b) disulfur tetrafluoride (c) dichlorine monoxide (d) phosphorus pentafluoride (e) boron tribromide (f) diphosphorus pentasulfide

Write a formula for each molecular compound. (a) chlorine monoxide (b) xenon tetroxide (c) xenon hexafluoride (d) carbon tetrabromide (e) diboron tetrachloride (f) tetraphosphorus triselenide

Determine whether the name shown for each molecular compound is correct. If not, provide the compound’s correct name. (a) \(\mathrm{NCl}_{3}\) nitrogen chloride (b) \(\mathrm{CI}_{4}\) carbon(IV) iodide (c) CO carbon oxide (d) \(\mathrm{SCl}_{4}\) sulfur tetrachloride Equation Transcription: Text Transcription: NCl_3 CI_4 SCl_4

Determine whether each acid is a binary acid or an oxyacid and name each acid. If the acid is an oxyacid, provide the name of the oxyanion. (a) \(\mathrm{HNO}_{2}\) (aq) (b) HI(aq) (c) \(\mathrm{H}_{2} \mathrm{SO}_{4}\) (aq) (d) \(\mathrm{HNO}_{3}\) (aq) Equation Transcription: Text Transcription: HNO_2 H_2 SO_4 HNO_3

Determine whether each acid is a binary acid or an oxyacid and name each acid. If the acid is an oxyacid, provide the name of the oxyanion. (a) \(\mathrm{H}_{2} \mathrm{CO}_{3}\) (aq) (b) \(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) (aq) (c) \(\mathrm{H}_{3} \mathrm{PO}_{4}\) (aq) (d) HCl(aq) Equation Transcription: Text Transcription: H_2 CO_3 HC_2 H_3 O_2 H_3 PO_4

Name each acid. (a) HClO (b) \(\mathrm{HClO}_{2}\) (c) \(\mathrm{HClO}_{3}\) (d) \(\mathrm{HClO}_{4}\) Equation Transcription: Text Transcription: HClO_2 HClO_3 HClO_4

Name each acid. (Hint: The names of the oxyanions are analogous to the names of the oxyanions of chlorine.) (a) \(\mathrm{HBrO}_{3}\) (b) \(\mathrm{HIO}_{3}\) Equation Transcription: Text Transcription: HBrO_3 HIO_3

Write a formula for each acid. (a) phosphoric acid (b) hydrobromic acid (c) sulfurous acid

Calculate the formula mass for each compound. (a) \(\mathrm{HNO}_{3}\) (b) \(\mathrm{CaBr}_{2}\) (c) \(\mathrm{CCl}_{4}\) (d) \(\mathrm{Sr}\left(\mathrm{NO}_{3}\right)_{2}\) Equation Transcription: Text Transcription: HNO_3 CaBr_2 CCl_4 Sr(NO_3)_2

Write a formula for each acid. (a) hydrofluoric acid (b) hydrocyanic acid (c) chlorous acid

Calculate the formula mass for each compound. (a) \(\mathrm{CS}_{2}\) (b) \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}\) (c) \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}\) (d) \(\mathrm{C}_{7} \mathrm{H}_{16}\) Equation Transcription: Text Transcription: CS_2 C_6 H_12 O_6 Fe(NO_3)_3 C_7 H_16

Arrange the compounds in order of decreasing formula mass. \(\mathrm{Ag}_{2} \mathrm{O}\), \(\mathrm{PtO}_{2}\), \(\mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}\), \(\mathrm{PBr}_{3}\) Equation Transcription: Text Transcription: Ag_2 O PtO_2 Al(NO_3)_3 PBr_3

Arrange the compounds in order of decreasing formula mass. \(\mathrm{WO}_{2}\), \(\mathrm{Rb}_{2} \mathrm{SO}_{4}\), \(\mathrm{~Pb}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2}\), RbI Equation Transcription: Text Transcription: WO_2 Rb_2 SO_4 Pb(C_2 H_3 O_2)_2

Write a molecular formula for each molecular model. (White = hydrogen; red = oxygen; black = carbon; blue = nitrogen; yellow = sulfur)

Write a molecular formula for each molecular model. (White = hydrogen; red = oxygen; black = carbon; blue = nitrogen; yellow = sulfur)

How many oxygen atoms are in each set? (a) four dinitrogen monoxide molecules (b) two calcium carbonate formula units (c) three sulfur dioxide molecules (d) five perchlorate ions

How many chlorine atoms are in each set? (a) three carbon tetrachloride molecules (b) two calcium chloride formula units (c) four phosphorus trichloride molecules (d) seven sodium chloride formula units

Specify the number of oxygen atoms (red) represented in each set of molecular models:

Complete the table:

Complete the table:

Is each name correct for the given formula? If not, provide the correct name. (a) \(\mathrm{Ca}\left(\mathrm{NO}_{2}\right)_{2}\) calcium nitrate (b) \(\mathrm{~K}_{2} \mathrm{O}\) dipotassium monoxide (c) \(\mathrm{PCl}_{3}\) phosphorus chloride (d) \(\mathrm{PbCO}_{3}\) lead (II) carbonate (e) \(\mathrm{KIO}_{2}\) potassium hypoiodite Equation Transcription: Text Transcription: Ca(NO_2)_2 K_2 O PCl_3 PbCO_3 KIO_2

Is each name correct for the given formula? If not, provide the correct name. (a) \(\mathrm{HNO}_{3}\) (aq) hydrogen nitrate (b) NaClO sodium hypochlorite (c) \(\mathrm{CaI}_{2}\) calcium diiodide (d) \(\mathrm{SnCrO}_{4}\) tin chromate (e) \(\mathrm{NaBrO}_{3}\) sodium bromite Equation Transcription: Text Transcription: HNO_3 CaI_2 SnCrO_4 NaBrO_3

For each compound, list the correct formula and calculate the formula mass. (a) barium bromide (b) dinitrogen trioxide (c) copper(I) sulfate (d) hydrobromic acid

For each compound, list the correct formula and calculate the formula mass. (a) tin(IV) sulfate (b) nitrous acid (c) sodium bicarbonate (d) phosphorus pentafluoride

Name each compound and calculate its formula mass. (a) \(\mathrm{PtO}_{2}\) (b) \(\mathrm{~N}_{2} \mathrm{O}_{5}\) (c) \(\mathrm{Al}\left(\mathrm{ClO}_{3}\right)_{3}\) (d) \(\mathrm{PBr}_{5}\) Equation Transcription: Text Transcription: PtO_2 N_2 O_5 Al(ClO_3)_3 PBr_5

A compound contains only carbon and hydrogen and has a formula mass of 28.06 amu. What is its molecular formula?

A compound contains only nitrogen and oxygen and has a formula mass of 44.02 amu. What is its molecular formula?

Name each compound and calculate its formula mass. (a) \(\mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}\) (b) \(\mathrm{P}_{2} \mathrm{O}_{3}\) (c) HClO(aq) (d) \(\mathrm{Cr}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{3}\) Equation Transcription: Text Transcription: Al_2(SO_4)_3 P_2 O_3 Cr(C_2 H_3 O_2)_3

Carbon has two naturally occurring isotopes: carbon-12 (mass = 12.00 amu) and carbon-13 (mass = 13.00 amu). Chlorine also has two naturally occurring isotopes: chlorine-35 (mass = 34.97 amu) and chlorine-37 (mass = 36.97 amu). How many \(\mathrm{CCl}_{4}\) molecules of different masses can exist? Determine the mass (in amu) of each of them. Equation Transcription: Text Transcription: CCl_4

Nitrogen has two naturally occurring isotopes: nitrogen-14 (mass = 14.00 amu) and nitrogen-15 (mass = 15.00 amu). Bromine also has two naturally occurring isotopes: bromine-79 (mass = 78.92 amu) and bromine-81 (mass = 80.92 amu). How many types of \(\mathrm{NBr}_{3}\) molecules of different masses can exist? Determine the mass (in amu) of each of them. Equation Transcription: Text Transcription: NBr_3

Examine each consumer product label. Write chemical formulas for as many of the compounds as possible based on what you have learned in this chapter.

Examine each substance and the corresponding molecular view and classify it as an atomic element, a molecular element, a molecular compound, or an ionic compound.

Molecules can be as small as two atoms or as large as thousands of atoms. In 1962, Max F. Perutz and John C. Kendrew were awarded the Nobel Prize for their discovery of the structure of hemoglobin, a very large molecule that transports oxygen from the lungs to cells through the bloodstream. The chemical formula of hemoglobin is \(\mathrm{C}_{2852} \mathrm{H}_{4864} \mathrm{O}_{832} \mathrm{~N}_{812} \mathrm{~S}_{8} \mathrm{Fe}_{4}\). Calculate the formula mass of hemoglobin. Equation Transcription: C2952H4664O832N812S8Fe4. Text Transcription: C_2952H_4664O_832N_812S8F_e4.

Specify the number of hydrogen atoms (white) represented in each set of molecular models: