Introductory Chemistry

Nivaldo J. Tro

Chapter 5

Molecules and Compounds - all with Video Answers

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Chapter Questions

Problem 1

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

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Problem 2

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

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Problem 3

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

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Problem 4

What is a chemical formula? List some examples.

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Problem 5

In a chemical formula, which element is listed first?

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Problem 6

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

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Problem 7

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

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Problem 8

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

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Problem 9

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

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Problem 10

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

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Problem 11

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

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Problem 12

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?

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Problem 13

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

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Problem 14

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

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Problem 15

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

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Problem 16

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

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Problem 17

How are compounds containing a polyatomic ion named?

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Problem 18

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

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Problem 19

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

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Problem 20

How many atoms does each prefix specify? mono-, $d i-$, $tritetra$-, $penta$-, $hexa-.$

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Problem 21

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

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Problem 22

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

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Problem 23

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

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Problem 24

What is the formula mass of a compound?

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Problem 25

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

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Problem 26

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

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Problem 27

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

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Problem 28

The mass ratio of sodium to fluorine in sodium fluoride is 1.21:1. A sample of sodium fluoride produces $34.5 \mathrm{g}$ of $\mathrm{so}^{-}$ dium upon decomposition. How much fluorine (in grams) forms?

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Problem 29

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.

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Problem 30

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.

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Problem 31

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

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Problem 32

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

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Problem 33

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

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Problem 34

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

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Problem 35

How many oxygen atoms are in each chemical formula?
(a) $\mathrm{H}_{3} \mathrm{PO}_{4}$
(b) $\mathrm{Na}_{2} \mathrm{HPO}_{4}$
(c) $\mathrm{Ca}\left(\mathrm{HCO}_{3}\right)_{2}$
(d) $\mathrm{Ba}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2}$

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Problem 36

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

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Problem 37

Determine the number of each type of atom in each formula.
(a) $\mathrm{MgCl}_{2}$
(b) $\mathrm{NaNO}_{3}$
(c) $\mathrm{Ca}\left(\mathrm{NO}_{2}\right)_{2}$
(d) $\operatorname{Sr}(\mathrm{OH})_{2}$

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Problem 38

Determine the number of each type of atom in each formula.
(a) $\mathrm{NH}_{4} \mathrm{Cl}$
(b) $\mathrm{Mg}_{3}\left(\mathrm{PO}_{4}\right)_{2}$
(c) NaCN
(d) $\mathrm{Ba}\left(\mathrm{HCO}_{3}\right)_{2}$

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Problem 39

Complete the table.

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Problem 40

Complete the table.

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Problem 41

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) $\mathrm{NH}_{3}$

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Problem 42

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) $\quad \mathrm{B}_{2} \mathrm{H}_{6}$

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Problem 43

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

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Problem 44

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

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Problem 45

Classify each compound as ionic or molecular.
(a) $\mathrm{CS}_{2}$
(b) $\mathrm{CuO}$
(c) $\mathrm{KI}$
(d) $\mathrm{PCl}_{3}$

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Problem 46

Classify each compound as ionic or molecular.
(a) $\mathrm{PtO}_{2}$
(b) $\mathrm{CF}_{2} \mathrm{Cl}_{2}$
(c) $\mathrm{CO}$
(d) $\mathrm{SO}_{3}$

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Problem 47

Match the substances on the left with the basic units that compose them on the right.
helium - molecules
$\mathrm{CCl}_{4} \quad$ formula units
$\mathrm{K}_{2} \mathrm{SO}_{4}$ - diatomic molecules
bromine $\quad$ single atoms

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Problem 48

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

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Problem 49

What are the basic units-single atoms, molecules, or formula units - that compose each substance?
(a) $\mathrm{BaBr}_{2}$
(b) $\mathrm{Ne}$
(c) $\mathrm{I}_{2}$
(d) $\mathrm{CO}$

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Problem 50

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) $\operatorname{Fe}\left(\mathrm{NO}_{3}\right)_{2}$
(d) $\mathrm{N}_{2} \mathrm{F}_{4}$

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Problem 51

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) $\operatorname{Sn}\left(S O_{4}\right)_{2}$

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Problem 52

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

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Problem 53

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

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Problem 54

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

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Problem 55

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

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Problem 56

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

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Problem 57

Write formulas for the compounds formed from the element on the left and each of the elements on the right.
$\begin{array}{llll}\text { (a) } & \mathrm{Li} & \mathrm{N}, \mathrm{O}, \mathrm{F}\end{array}$
(b) Ba $\quad \mathrm{N}, \mathrm{O}, \mathrm{F}$
$\begin{array}{lll}\text { (c) } & \text { Al } & \text { N, O, } \mathrm{F}\end{array}$

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Problem 58

Write formulas for the compounds formed from the element on the left and each polyatomic ion on the right.
(a) $\mathrm{Rb}$ $\mathrm{NO}_{3}^{-}, \mathrm{SO}_{4}^{2^{-}}, \mathrm{PO}_{4}^{3-}$
(b) Sr $\mathrm{NO}_{3}^{-}, \mathrm{SO}_{4}^{2-}, \mathrm{PO}_{4}^{3-}$
(c) In $\mathrm{NO}_{3}^{-}, \mathrm{SO}_{4}^{2-}, \mathrm{PO}_{4}^{3-}$
(Assume In charge is $3+.$ )

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Problem 59

Name each ionic compound. In each of these compounds, the metal forms only one type of ion.
(a) $\mathrm{CsCl}$
(b) $\operatorname{SrBr}_{2}$
(c) $\overline{K_{2} O}$
(d)$\mathrm{LiF}$

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Problem 60

Name each ionic compound. In each of these compounds, the metal forms only one type of ion.
(a) $\mathrm{LiI}$
(b) $\mathrm{MgS}$
(c) $\operatorname{BaF}_{2}$
(d) $\mathrm{NaF}$

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Problem 61

Name each ionic compound. In each of these compounds, the metal forms more than one type of ion.
(a) $\mathrm{Cr} \mathrm{Cl}_{2}$
(b) $\mathrm{CrCl}_{3}$
(c) $\mathrm{SnO}_{2}$
(d) $\mathrm{PbI}_{2}$

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Problem 62

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) $\mathrm{CuI}_{2}$
(d) $\operatorname{sn} C 1_{4}$

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Problem 63

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) $\operatorname{sn} \mathrm{O}$

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Problem 64

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) $\mathrm{Fel}_{3}$
(b) $\mathrm{PbCl}_{4}$
(c) $\operatorname{Sr} \mathrm{I}_{2}$
(d) BaO

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Problem 65

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) $\cos \mathrm{O}_{4}$
(f) $\mathrm{NaClO}_{4}$

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Problem 66

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) $\operatorname{Mg}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2}$

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Problem 67

Name each polyatomic ion.
(a) $\mathrm{BrO}^{-}$
(b) $\mathrm{BrO}_{2}^{-}$
(c) $\mathrm{BrO}_{3}^{-}$
(d) $\mathrm{BrO}_{4}$

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Problem 68

Name each polyatomic ion.
(a) $\mathrm{IO}^{-}$
(b) $\mathrm{IO}_{2}^{-}$
(c) $\mathrm{IO}_{3}^{-}$
(d) IO $_{4}$

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Problem 69

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

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Problem 70

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

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Problem 71

Name each molecular compound.
(a) $\mathrm{SO}_{2}$
(b) $\mathrm{NI}_{3}$
(c) $\mathrm{BrF}_{5}$
(d) NO
(e) $\mathrm{N}_{4} \mathrm{Se}_{4}$

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Problem 72

Name each molecular compound.
(a) $\mathrm{XeF}_{4}$
(b) $\mathrm{PI}_{3}$
(c) $\mathrm{SO}_{3}$
(d) $\mathrm{SiCl}_{4}$
(e) $\mathrm{I}_{2} \mathrm{O}_{5}$

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Problem 73

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

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Problem 74

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

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Problem 75

Determine whether the name shown for each molecular compound is correct. If not, provide the compound's correct name.
(a) $\mathrm{PBr}_{5} \quad$ phosphorus(V) pentabromide
(b) $\mathrm{P}_{2} \mathrm{O}_{3} \quad$ phosphorus trioxide
(c) $\mathrm{SF}_{4} \quad$ monosulfur hexafluoride
(d) $\mathrm{NF}_{4} \quad$ nitrogen trifluoride

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Problem 76

Determine whether the name shown for each molecular compound is correct. If not, provide the compound's correct name.
(a) $\mathrm{NCl}_{3} \quad$ nitrogen chloride a)
(b) $\mathrm{CI}_{4} \quad$ carbon(IV) iodide
(c) CO carbon oxide
(d) $\mathrm{SCl}_{4} \quad$ sulfur tetrachloride

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Problem 77

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) $\mathrm{HNO}_{2}(a q)$
(b) $\mathrm{HI}(a q)$
(c) $\mathrm{H}_{2} \mathrm{SO}_{4}(a q)$
(d) $\mathrm{HNO}_{3}(a q)$

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Problem 78

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) $\mathrm{H}_{2} \mathrm{CO}_{3}(a q)$
(b) $\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}(a q)$
(c) $\mathrm{H}_{3} \mathrm{PO}_{4}(a q)$
(d) $\mathrm{HCl}(a q)$

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Problem 79

Name each acid.
(a) HCIO
(b) $\mathrm{HClO}_{2}$
(c) $\mathrm{HClO}_{3}$
(d) $\mathrm{HClO}_{4}$

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Problem 80

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

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Problem 81

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

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Problem 82

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

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Problem 83

Calculate the formula mass for each compound.
(a) $\mathrm{HNO}_{3}$
(b) $\mathrm{CaBr}_{2}$
(c) $\mathrm{CCl}_{4}$
(d) $\operatorname{Sr}\left(\mathrm{NO}_{3}\right)_{2}$

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Problem 84

Calculate the formula mass for each compound.
(a) $\mathrm{CS}_{2}$
(b) $\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}$
(c) $\operatorname{Fe}\left(\mathrm{NO}_{3}\right)_{3}$
(d) $\mathrm{C}_{7} \mathrm{H}_{16}$

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Problem 85

Arrange the compounds in order of decreasing formula mass.
$\mathrm{Ag}_{2} \mathrm{O}, \mathrm{PtO}_{2}, \mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}, \mathrm{PBr}_{3}$

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Problem 86

Arrange the compounds in order of decreasing formula mass.
$\mathrm{WO}_{2}, \mathrm{Rb}_{2} \mathrm{SO}_{4}, \mathrm{Pb}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{2}, \mathrm{RbI}$

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Problem 87

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

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Problem 88

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

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Problem 89

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

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Problem 90

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

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Problem 91

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

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Problem 92

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

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Problem 93

Complete the table:

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Problem 94

Complete the table:

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Problem 95

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
$\begin{array}{lll}\text { (c) } \mathrm{PCl}_{3} & \text { phosphorus chloride }\end{array}$
(d) $\mathrm{PbCO}_{3} \quad$ lead(II) carbonate
(e) $\mathrm{KIO}_{2} \quad$ potassium hypoiodite

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Problem 96

Is each name correct for the given formula? If not, provide the correct name.
(a) $\mathrm{HNO}_{3}(a q)$ hydrogen nitrate
(b) $\mathrm{NaClO}$ sodium hypochlorite
(c) $\mathrm{CaI}_{2}$ calcium diadide
(d) $\operatorname{sn} C r O_{4}$ tin chromate
(e) $\mathrm{NaBrO}_{3}$ sodium bromite

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Problem 97

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

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Problem 98

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

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Problem 99

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) $\mathrm{PBr}_{5}$

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Problem 100

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) $\mathrm{HClO}(a q)$
(d) $\operatorname{Cr}\left(\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)_{3}$

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Problem 101

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

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Problem 102

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

Jennifer Hudspeth

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Problem 103

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.

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Problem 104

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.

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Problem 105

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.

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Problem 106

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 $\mathrm{C}_{2952} \mathrm{H}_{4664} \mathrm{O}_{832} \mathrm{N}_{812} \mathrm{S}_{8} \mathrm{Fe}_{4} .$ Calculate the formula mass of hemoglobin.

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Problem 107

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.

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Problem 108

Write the correct formula for each species: carbon monoxide, carbon dioxide, the carbonate ion. List as many similarities and differences between these three species as you can. Try to get at least one contribution from each group member.

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Problem 109

What questions do you need to ask about a substance in order to determine whether it is (1) an atomic element,
(2) a molecular element, (3) a molecular compound, or (4) an ionic compound? Write a detailed set of instructions describing how to determine the classification of a substance based on the answers to your questions.

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Problem 110

Name each compound: $\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}, \mathrm{N}_{2} \mathrm{O}, \mathrm{NaS}, \mathrm{CrCl}_{3}$
For each compound, include a detailed step-by-step description of the process you used to determine the name. (Tip: Each group member could name one compound and present it to the whole group.)

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Problem 111

Calculate the formula mass for each compound in Group Work Question 110 .

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