Chemistry

Paul Flower, Klaus Theopold, Richard Langley

Chapter 18

Representative Metals, Metalloids, and Nonmetals - all with Video Answers

Educators

Chapter Questions

Problem 1

How do alkali metals differ from alkaline earth metals in atomic structure and general properties?

Aadit S.

Aadit S.

Numerade Educator

Problem 2

Why does the reactivity of the alkali metals decrease from cesium to lithium?

Sisi G.

Numerade Educator

Problem 3

Predict the formulas for the nine compounds that may form when each species in column 1 of Table 18.3 reacts with each species in column $2 .$
$$\begin{array}{|c|c|}
\hline 1 & 2 \\\hline \mathrm{Na} & 1 \\
\hline \mathrm{Sr} & \mathrm{Se} \\
\hline \mathrm{Al} & 0 \\
\hline\end{array}$$

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Problem 4

Predict the best choice in each of the following. You may wish to review the chapter on electronic structure for relevant examples.
(a) the most metallic of the elements $\mathrm{Al}$, Be, and $\mathrm{Ba}$
(b) the most covalent of the compounds $\mathrm{NaCl}, \mathrm{CaCl}_{2},$ and $\mathrm{BeCl}_{2}$
(c) the lowest first ionization energy among the elements $\mathrm{Rb}, \mathrm{K},$ and $\mathrm{Li}$
(d) the smallest among $\mathrm{Al}, \mathrm{Al}^{+}$, and $\mathrm{Al}^{3+}$
(e) the largest among $\mathrm{Cs}^{+}, \mathrm{Ba}^{2+},$ and $\mathrm{Xe}$

Sisi G.

Numerade Educator

Problem 5

Sodium chloride and strontium chloride are both white solids. How could you distinguish one from the other?

Aadit S.

Numerade Educator

Problem 6

The reaction of quicklime, $\mathrm{CaO},$ with water produces slaked lime, $\mathrm{Ca}(\mathrm{OH})_{2},$ which is widely used in the construction industry to make mortar and plaster. The reaction of quicklime and water is highly exothermic:
$\mathrm{CaO}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{Ca}(\mathrm{OH})_{2}(s) \quad \Delta H=-350 \mathrm{~kJ} \mathrm{~mol}^{-1}$
(a) What is the enthalpy of reaction per gram of quicklime that reacts?
(b) How much heat, in kilojoules, is associated with the production of 1 ton of slaked lime?

Shahina -.

Numerade Educator

Problem 7

Write a balanced equation for the reaction of elemental strontium with each of the following:
(a) oxygen
(b) hydrogen bromide
(c) hydrogen
(d) phosphorus
(e) water

Aadit S.

Numerade Educator

Problem 8

How many moles of ionic species are present in $1.0 \mathrm{~L}$ of a solution marked $1.0 \mathrm{M}$ mercury(I) nitrate?

Nadia L.

Numerade Educator

Problem 9

What is the mass of fish, in kilograms, that one would have to consume to obtain a fatal dose of mercury, if the fish contains 30 parts per million of mercury by weight? (Assume that all the mercury from the fish ends up as mercury(II) chloride in the body and that a fatal dose is $0.20 \mathrm{~g}$ of $\mathrm{HgCl}_{2}$.) How many pounds of fish is this?

Aadit S.

Numerade Educator

Problem 10

The elements sodium, aluminum, and chlorine are in the same period.
(a) Which has the greatest electronegativity?
(b) Which of the atoms is smallest?
(c) Write the Lewis structure for the simplest covalent compound that can form between aluminum and chlorine.
(d) Will the oxide of each element be acidic, basic, or amphoteric?

Sisi G.

Numerade Educator

Problem 11

Does metallic tin react with HCl?

Aadit S.

Numerade Educator

Problem 12

What is tin pest, also known as tin disease?

Sisi G.

Numerade Educator

Problem 13

Compare the nature of the bonds in $\mathrm{PbCl}_{2}$ to that of the bonds in $\mathrm{PbCl}_{4}$.

Aadit S.

Numerade Educator

Problem 14

Is the reaction of rubidium with water more or less vigorous than that of sodium? How does the rate of reaction of magnesium compare?

Sisi G.

Numerade Educator

Problem 15

Write an equation for the reduction of cesium chloride by elemental calcium at high temperature.

Aadit S.

Numerade Educator

Problem 16

Why is it necessary to keep the chlorine and sodium, resulting from the electrolysis of sodium chloride, separate during the production of sodium metal?

Sisi G.

Numerade Educator

Problem 17

Give balanced equations for the overall reaction in the electrolysis of molten lithium chloride and for the reactions occurring at the electrodes. You may wish to review the chapter on electrochemistry for relevant examples.

Aadit S.

Numerade Educator

Problem 18

The electrolysis of molten sodium chloride or of aqueous sodium chloride produces chlorine.
Calculate the mass of chlorine produced from $3.00 \mathrm{~kg}$ sodium chloride in each case. You may wish to review the chapter on electrochemistry for relevant examples.

Nadia L.

Numerade Educator

Problem 19

What mass, in grams, of hydrogen gas forms during the complete reaction of $10.01 \mathrm{~g}$ of calcium with water?

Aadit S.

Numerade Educator

Problem 20

How many grams of oxygen gas are necessary to react completely with $3.01 \times 10^{21}$ atoms of magnesium to yield magnesium oxide?

Sisi G.

Numerade Educator

Problem 21

How many grams of oxygen gas are necessary to react completely with $3.01 \times 10^{21}$ atoms of magnesium to yield magnesium oxide?

Sisi G.

Numerade Educator

Problem 21

Magnesium is an active metal; it burns in the form of powder, ribbons, and filaments to provide flashes of brilliant light. Why is it possible to use magnesium in construction?

Aadit S.

Numerade Educator

Problem 22

Why is it possible for an active metal like aluminum to be useful as a structural metal?

Sisi G.

Numerade Educator

Problem 23

Describe the production of metallic aluminum by electrolytic reduction.

Aadit S.

Numerade Educator

Problem 24

What is the common ore of tin and how is tin separated from it?

Sisi G.

Numerade Educator

Problem 25

A chemist dissolves a 1.497-g sample of a type of metal (an alloy of $\mathrm{Sn}, \mathrm{Pb}, \mathrm{Sb},$ and $\mathrm{Cu}$ ) in nitric acid, and metastannic acid, $\mathrm{H}_{2} \mathrm{SnO}_{3}$, is precipitated. She heats the precipitate to drive off the water, which leaves $0.4909 \mathrm{~g}$ of tin(IV) oxide. What was the percentage of tin in the original sample?

Aadit S.

Numerade Educator

Problem 26

Consider the production of $100 \mathrm{~kg}$ of sodium metal using a current of 50,000 A, assuming a $100 \%$ yield.
(a) How long will it take to produce the $100 \mathrm{~kg}$ of sodium metal?
(b) What volume of chlorine at $25^{\circ} \mathrm{C}$ and 1.00 atm forms?

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Problem 27

What mass of magnesium forms when $100,000 \mathrm{~A}$ is passed through a $\mathrm{MgCl}_{2}$ melt for $1.00 \mathrm{~h}$ if the yield of magnesium is $85 \%$ of the theoretical yield?

Aadit S.

Numerade Educator

Problem 28

Give the hybridization of the metalloid and the molecular geometry for each of the following compounds or ions. You may wish to review the chapters on chemical bonding and advanced covalent bonding for relevant examples.
(a) $\mathrm{GeH}_{4}$
(b) $\mathrm{SbF}_{3}$
(c) $\mathrm{Te}(\mathrm{OH})_{6}$
(d) $\mathrm{H}_{2} \mathrm{Te}$
(e) $\mathrm{GeF}_{2}$
(f) $\mathrm{TeCl}_{4}$
(g) $\mathrm{SiF}_{6}^{2-}$
(h) $\mathrm{SbCl}_{5}$
(i) $\mathrm{TeF}_{6}$

Sisi G.

Numerade Educator

Problem 29

Write a Lewis structure for each of the following molecules or ions. You may wish to review the chapter on chemical bonding.
(a) $\mathrm{H}_{3} \mathrm{BPH}_{3}$
(b) $\mathrm{BF}_{4}^{-}$
(c) $\mathrm{BBr}_{3}$
(d) $\mathrm{B}\left(\mathrm{CH}_{3}\right)_{3}$
(e) $\mathrm{B}(\mathrm{OH})_{3}$

Shahina -.

Numerade Educator

Problem 30

Describe the hybridization of boron and the molecular structure about the boron in each of the following:
(a) $\mathrm{H}_{3} \mathrm{BPH}_{3}$
(b) $\mathrm{BF}_{4}^{-}$
(c) $\mathrm{BBr}_{3}$
(d) $\mathrm{B}\left(\mathrm{C} \mathrm{H}_{3}\right)_{3}$
(e) $\mathrm{B}(\mathrm{OH})_{3}$

Shahina -.

Numerade Educator

Problem 31

Using only the periodic table, write the complete electron configuration for silicon, including any empty orbitals in the valence shell. You may wish to review the chapter on electronic structure.

Aadit S.

Numerade Educator

Problem 32

Write a Lewis structure for each of the following molecules and ions:
(a) $\left(\mathrm{CH}_{3}\right)_{3} \mathrm{SiH}$
(b) $\mathrm{SiO}_{4}^{4-}$
(c) $\mathrm{Si}_{2} \mathrm{H}_{6}$
(d) $\mathrm{Si}(\mathrm{OH})_{4}$
(e) $\mathrm{SiF}_{6}{ }^{2-}$

Nadia L.

Numerade Educator

Problem 33

Describe the hybridization of silicon and the molecular structure of the following molecules and ions:
(a) $\left(\mathrm{CH}_{3}\right)_{3} \mathrm{SiH}$
(b) $\mathrm{SiO}_{4}^{4-}$
(c) $\mathrm{Si}_{2} \mathrm{H}_{6}$
(d) $\mathrm{Si}(\mathrm{OH})_{4}$
(e) $\mathrm{SiF}_{6}^{2-}$

Aadit S.

Numerade Educator

Problem 34

Describe the hybridization and the bonding of a silicon atom in elemental silicon.

Nadia L.

Numerade Educator

Problem 35

Classify each of the following molecules as polar or nonpolar. You may wish to review the chapter on chemical bonding.
(a) $\mathrm{SiH}_{4}$
(b) $\mathrm{Si}_{2} \mathrm{H}_{6}$
(c) $\mathrm{SiCl}_{3} \mathrm{H}$
(d) $\mathrm{SiF}_{4}$
(e) $\mathrm{SiCl}_{2} \mathrm{~F}_{2}$

Shahina -.

Numerade Educator

Problem 36

Silicon reacts with sulfur at elevated temperatures. If 0.0923 g of silicon reacts with sulfur to give $0.3030 \mathrm{~g}$ of silicon sulfide, determine the empirical formula of silicon sulfide.

Nadia L.

Numerade Educator

Problem 37

Name each of the following compounds:
(a) $\mathrm{TeO}_{2}$
(b) $\mathrm{Sb}_{2} \mathrm{~S}_{3}$
(c) $\mathrm{GeF}_{4}$
(d) $\mathrm{SiH}_{4}$
(e) $\mathrm{GeH}_{4}$

Aadit S.

Numerade Educator

Problem 38

Write a balanced equation for the reaction of elemental boron with each of the following (most of these reactions require high temperature):
(a) $\mathrm{F}_{2}$
(b) $\mathrm{O}_{2}$
(c) $S$
(d) Se
(e) $\mathrm{Br}_{2}$

Nadia L.

Numerade Educator

Problem 39

Why is boron limited to a maximum coordination number of four in its compounds?

Aadit S.

Numerade Educator

Problem 40

Write a formula for each of the following compounds:
(a) silicon dioxide
(b) silicon tetraiodide
(c) silane
(d) silicon carbide
(e) magnesium silicide

Nadia L.

Numerade Educator

Problem 41

From the data given in Appendix 1 , determine the standard enthalpy change and the standard free energy change for each of the following reactions:
(a) $\mathrm{BF}_{3}(g)+3 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{B}(\mathrm{OH})_{3}(s)+3 \mathrm{HF}(g)$
(b) $\mathrm{BCl}_{3}(g)+3 \mathrm{H}_{2} \mathrm{O}(I) \longrightarrow \mathrm{B}(\mathrm{OH})_{3}(s)+3 \mathrm{HCl}(g)$
(c) $\mathrm{B}_{2} \mathrm{H}_{6}(g)+6 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow 2 \mathrm{~B}(\mathrm{OH})_{3}(s)+6 \mathrm{H}_{2}(g)$

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Problem 42

A hydride of silicon prepared by the reaction of $\mathrm{Mg}_{2}$ Si with acid exerted a pressure of 306 torr at $26^{\circ} \mathrm{C}$ in a bulb with a volume of $57.0 \mathrm{~mL}$. If the mass of the hydride was $0.0861 \mathrm{~g}$, what is its molecular mass? What is the molecular formula for the hydride?

David C.

Numerade Educator

Problem 43

Suppose you discovered a diamond completely encased in a silicate rock. How would you chemically free the diamond without harming it?

Aadit S.

Numerade Educator

Problem 44

Carbon forms a number of allotropes, two of which are graphite and diamond. Silicon has a diamond structure. Why is there no allotrope of silicon with a graphite structure?

Nadia L.

Numerade Educator

Problem 45

Nitrogen in the atmosphere exists as very stable diatomic molecules. Why does phosphorus form less stable $\mathrm{P}_{4}$ molecules instead of $\mathrm{P}_{2}$ molecules?

Aadit S.

Numerade Educator

Problem 46

Write balanced chemical equations for the reaction of the following acid anhydrides with water:
(a) $\mathrm{SO}_{3}$
(b) $\mathrm{N}_{2} \mathrm{O}_{3}$
(c) $\mathrm{Cl}_{2} \mathrm{O}_{7}$
(d) $\mathrm{P}_{4} \mathrm{O}_{10}$
(e) $\mathrm{NO}_{2}$

Nadia L.

Numerade Educator

Problem 47

Determine the oxidation number of each element in each of the following compounds:
(a) $\mathrm{HCN}$
(b) $\mathrm{OF}_{2}$
(c) $\mathrm{AsCl}_{3}$

Aadit S.

Numerade Educator

Problem 48

Determine the oxidation state of sulfur in each of the following:
(a) $\mathrm{SO}_{3}$
(b) $\mathrm{SO}_{2}$
(c) $\mathrm{SO}_{3}^{2-}$

Nadia L.

Numerade Educator

Problem 49

Arrange the following in order of increasing electronegativity: $\mathrm{F} ; \mathrm{Cl} ; \mathrm{O} ;$ and $\mathrm{S}$.

Aadit S.

Numerade Educator

Problem 50

Why does white phosphorus consist of tetrahedral $\mathrm{P}_{4}$ molecules while nitrogen consists of diatomic $\mathrm{N}_{2}$ molecules?

Nadia L.

Numerade Educator

Problem 50

Why does white phosphorus consist of tetrahedral $\mathrm{P}_{4}$ molecules while nitrogen consists of diatomic $\mathrm{N}_{2}$ molecules?

Nadia L.

Numerade Educator

Problem 51

Why does hydrogen not exhibit an oxidation state of 1 - when bonded to nonmetals?

Aadit S.

Numerade Educator

Problem 52

The reaction of calcium hydride, $\mathrm{CaH}_{2}$, with water can be characterized as a Lewis acid-base reaction:
$\mathrm{CaH}_{2}(s)+2 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{Ca}(\mathrm{OH})_{2}(a q)+2 \mathrm{H}_{2}(g)$
Identify the Lewis acid and the Lewis base among the reactants. The reaction is also an oxidation-reduction reaction. Identify the oxidizing agent, the reducing agent, and the changes in oxidation number that occur in the reaction.

Nadia L.

Numerade Educator

Problem 53

In drawing Lewis structures, we learn that a hydrogen atom forms only one bond in a covalent compound. Why?

Aadit S.

Numerade Educator

Problem 54

What mass of $\mathrm{CaH}_{2}$ is necessary to react with water to provide enough hydrogen gas to fill a balloon at $20^{\circ} \mathrm{C}$ and 0.8 atm pressure with a volume of $4.5 \mathrm{~L} ?$ The balanced equation is:
$\mathrm{CaH}_{2}(s)+2 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{Ca}(\mathrm{OH})_{2}(a q)+2 \mathrm{H}_{2}(g)$

Nadia L.

Numerade Educator

Problem 55

What mass of hydrogen gas results from the reaction of 8.5 g of $\mathrm{KH}$ with water? $\mathrm{KH}+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{KOH}+\mathrm{H}_{2}$

Aadit S.

Numerade Educator

Problem 56

Carbon forms the $\mathrm{CO}_{3}^{2-}$ ion, yet silicon does not form an analogous $\mathrm{SiO}_{3}{ }^{2-}$ ion. Why?

Nadia L.

Numerade Educator

Problem 57

Complete and balance the following chemical equations:
(a) hardening of plaster containing slaked lime $\mathrm{Ca}(\mathrm{OH})_{2}+\mathrm{CO}_{2} \longrightarrow$
(b) removal of sulfur dioxide from the flue gas of power plants $\mathrm{CaO}+\mathrm{SO}_{2} \longrightarrow$
(c) the reaction of baking powder that produces carbon dioxide gas and causes bread to rise $\mathrm{NaHCO}_{3}+\mathrm{NaH}_{2} \mathrm{PO}_{4} \longrightarrow$

Aadit S.

Numerade Educator

Problem 58

Heating a sample of $\mathrm{Na}_{2} \mathrm{CO}_{3} \cdot \mathrm{xH}_{2} \mathrm{O}$ weighing $4.640 \mathrm{~g}$ until the removal of the water of hydration leaves $1.720 \mathrm{~g}$ of anhydrous $\mathrm{Na}_{2} \mathrm{CO}_{3}$. What is the formula of the hydrated compound?

Nadia L.

Numerade Educator

Problem 59

Write the Lewis structures for each of the following:
(a) $\mathrm{NH}^{2-}$
(b) $\mathrm{N}_{2} \mathrm{~F}_{4}$
(c) $\mathrm{NH}_{2}^{-}$
(d) $\mathrm{NF}_{3}$
(e) $\mathrm{N}_{3}^{-}$

Aadit S.

Numerade Educator

Problem 60

For each of the following, indicate the hybridization of the nitrogen atom (for $\mathrm{N}_{3}-$, the central nitrogen).
(a) $\mathrm{N}_{2} \mathrm{~F}_{4}$
(b) $\mathrm{NH}_{2}^{-}$
(c) $\mathrm{NF}_{3}$
(d) $\mathrm{N}_{3}-$

Nadia L.

Numerade Educator

Problem 61

Explain how ammonia can function both as a Brønsted base and as a Lewis base.

Aadit S.

Numerade Educator

Problem 62

Determine the oxidation state of nitrogen in each of the following. You may wish to review the chapter on chemical bonding for relevant examples.
(a) $\mathrm{NCl}_{3}$
(b) CINO
(c) $\mathrm{N}_{2} \mathrm{O}_{5}$
(d) $\mathrm{N}_{2} \mathrm{O}_{3}$
(e) $\mathrm{NO}_{2}^{-}$
(f) $\mathrm{N}_{2} \mathrm{O}_{4}$
(g) $\mathrm{N}_{2} \mathrm{O}$
(h) $\mathrm{NO}_{3}^{-}$
(i) $\mathrm{HNO}_{2}$
(j) $\mathrm{HNO}_{3}$

Shahina -.

Numerade Educator

Problem 63

For each of the following, draw the Lewis structure, predict the ONO bond angle, and give the hybridization of the nitrogen. You may wish to review the chapters on chemical bonding and advanced theories of covalent bonding for relevant examples.
(a) $\mathrm{NO}_{2}$
(b) $\mathrm{NO}_{2}^{-}$
(c) $\mathrm{NO}_{2}^{+}$

Aadit S.

Numerade Educator

Problem 64

How many grams of gaseous ammonia will the reaction of 3.0 g hydrogen gas and 3.0 g of nitrogen gas produce?

Nadia L.

Numerade Educator

Problem 65

Although $\mathrm{PF}_{5}$ and $\mathrm{AsF}_{5}$ are stable, nitrogen does not form $\mathrm{NF}_{5}$ molecules. Explain this difference among members of the same group.

Aadit S.

Numerade Educator

Problem 66

The equivalence point for the titration of a $25.00-\mathrm{mL}$ sample of $\mathrm{CsOH}$ solution with $0.1062 \mathrm{M} \mathrm{HNO}_{3}$ is at $35.27 \mathrm{~mL}$. What is the concentration of the $\mathrm{CsOH}$ solution?

David C.

Numerade Educator

Problem 67

Write the Lewis structure for each of the following. You may wish to review the chapter on chemical bonding and molecular geometry.
(a) $\mathrm{PH}_{3}$
(b) $\mathrm{PH}_{4}^{+}$
(c) $\mathrm{P}_{2} \mathrm{H}_{4}$
(d) $\mathrm{PO}_{4}^{3-}$
(e) $\mathrm{PF}_{5}$

Aadit S.

Numerade Educator

Problem 68

Describe the molecular structure of each of the following molecules or ions listed. You may wish to review the chapter on chemical bonding and molecular geometry.
(a) $\mathrm{PH}_{3}$
(b) $\mathrm{PH}_{4}^{+}$
(c) $\mathrm{P}_{2} \mathrm{H}_{4}$
(d) $\mathrm{PO}_{4}^{3-}$

Nadia L.

Numerade Educator

Problem 69

Complete and balance each of the following chemical equations. (In some cases, there may be more than one correct answer.)
(a) $\mathrm{P}_{4}+\mathrm{Al} \longrightarrow$
(b) $\mathrm{P}_{4}+\mathrm{Na} \longrightarrow$
(c) $\mathrm{P}_{4}+\mathrm{F}_{2} \longrightarrow$
(d) $\mathrm{P}_{4}+\mathrm{Cl}_{2} \longrightarrow$
(e) $\mathrm{P}_{4}+\mathrm{O}_{2} \longrightarrow$
(f) $\mathrm{P}_{4} \mathrm{O}_{6}+\mathrm{O}_{2} \longrightarrow$

Aadit S.

Numerade Educator

Problem 70

Describe the hybridization of phosphorus in each of the following compounds: $\mathrm{P}_{4} \mathrm{O}_{10}, \mathrm{P}_{4} \mathrm{O}_{6}, \mathrm{PH}_{4} \mathrm{I}$ (an ionic compound), $\mathrm{PBr}_{3}, \mathrm{H}_{3} \mathrm{PO}_{4}, \mathrm{H}_{3} \mathrm{PO}_{3}, \mathrm{PH}_{3},$ and $\mathrm{P}_{2} \mathrm{H}_{4}$. You may wish to review the chapter on advanced theories of covalent bonding.

Nadia L.

Numerade Educator

Problem 71

What volume of $0.200 \mathrm{M} \mathrm{NaOH}$ is necessary to neutralize the solution produced by dissolving $2.00 \mathrm{~g}$ of $\mathrm{PCl}_{3}$ is an excess of water? Note that when $\mathrm{H}_{3} \mathrm{PO}_{3}$ is titrated under these conditions, only one proton of the acid molecule reacts.

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Problem 72

How much $\mathrm{POCl}_{3}$ can form from $25.0 \mathrm{~g}$ of $\mathrm{PCl}_{5}$ and the appropriate amount of $\mathrm{H}_{2} \mathrm{O} ?$

Nadia L.

Numerade Educator

Problem 73

How many tons of $\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}$ are necessary to prepare 5.0 tons of phosphorus if the yield is $90 \% ?$

Aadit S.

Numerade Educator

Problem 74

Write equations showing the stepwise ionization of phosphorous acid.

Nadia L.

Numerade Educator

Problem 75

Draw the Lewis structures and describe the geometry for the following:
(a) $\mathrm{PF}_{4}^{+}$
(b) $\mathrm{PF}_{5}$
(c) $\mathrm{PF}_{6}^{-}$
(d) $\mathrm{POF}_{3}$

Aadit S.

Numerade Educator

Problem 76

Why does phosphorous acid form only two series of salts, even though the molecule contains three hydrogen atoms?

Nadia L.

Numerade Educator

Problem 77

Assign an oxidation state to phosphorus in each of the following:
(a) $\mathrm{NaH}_{2} \mathrm{PO}_{3}$
(b) $\mathrm{PF}_{5}$
(c) $\mathrm{P}_{4} \mathrm{O}_{6}$
(d) $\mathrm{K}_{3} \mathrm{PO}_{4}$
(e) $\mathrm{Na}_{3} \mathrm{P}$
(f) $\mathrm{Na}_{4} \mathrm{P}_{2} \mathrm{O}_{7}$

Aadit S.

Numerade Educator

Problem 78

Phosphoric acid, one of the acids used in some cola drinks, is produced by the reaction of phosphorus(V) oxide, an acidic oxide, with water. Phosphorus(V) oxide is prepared by the combustion of phosphorus.
(a) Write the empirical formula of phosphorus(V) oxide.
(b) What is the molecular formula of phosphorus(V) oxide if the molar mass is about 280 .
(c) Write balanced equations for the production of phosphorus(V) oxide and phosphoric acid.
(d) Determine the mass of phosphorus required to make $1.00 \times 10^{4} \mathrm{~kg}$ of phosphoric acid, assuming a yield of $98.85 \%$

Nadia L.

Numerade Educator

Problem 79

Predict the product of burning francium in air.

Aadit S.

Numerade Educator

Problem 80

Using equations, describe the reaction of water with potassium and with potassium oxide.

Nadia L.

Numerade Educator

Problem 81

Write balanced chemical equations for the following reactions:
(a) zinc metal heated in a stream of oxygen gas
(b) zinc carbonate heated until loss of mass stops
(c) zinc carbonate added to a solution of acetic acid, $\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}$
(d) zinc added to a solution of hydrobromic acid

Aadit S.

Numerade Educator

Problem 82

Write balanced chemical equations for the following reactions:
(a) cadmium burned in air
(b) elemental cadmium added to a solution of hydrochloric acid
(c) cadmium hydroxide added to a solution of acetic acid, $\mathrm{CH}_{3} \mathrm{CO}_{2} \mathrm{H}$

Nadia L.

Numerade Educator

Problem 83

Illustrate the amphoteric nature of aluminum hydroxide by citing suitable equations.

Aadit S.

Numerade Educator

Problem 84

Write balanced chemical equations for the following reactions:
(a) metallic aluminum burned in air
(b) elemental aluminum heated in an atmosphere of chlorine
(c) aluminum heated in hydrogen bromide gas
(d) aluminum hydroxide added to a solution of nitric acid

Nadia L.

Numerade Educator

Problem 85

Write balanced chemical equations for the following reactions:
(a) sodium oxide added to water
(b) cesium carbonate added to an excess of an aqueous solution of HF
(c) aluminum oxide added to an aqueous solution of $\mathrm{HClO}_{4}$
(d) a solution of sodium carbonate added to solution of barium nitrate
(e) titanium metal produced from the reaction of titanium tetrachloride with elemental sodium

Aadit S.

Numerade Educator

Problem 86

What volume of $0.250 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}$ solution is required to neutralize a solution that contains $5.00 \mathrm{~g}$ of $\mathrm{CaCO}_{3} ?$

Nadia L.

Numerade Educator

Problem 87

Which is the stronger acid, $\mathrm{HClO}_{4}$ or $\mathrm{HBrO}_{4}$ ? Why?

Aadit S.

Numerade Educator

Problem 88

Write a balanced chemical equation for the reaction of an excess of oxygen with each of the following. Remember that oxygen is a strong oxidizing agent and tends to oxidize an element to its maximum oxidation state.
(a) $\mathrm{Mg}$
(b) $\mathrm{Rb}$
(c) Ga
(d) $\mathrm{C}_{2} \mathrm{H}_{2}$
(e) CO

David C.

Numerade Educator

Problem 89

Which is the stronger acid, $\mathrm{H}_{2} \mathrm{SO}_{4}$ or $\mathrm{H}_{2} \mathrm{SeO}_{4}$ ? Why? You may wish to review the chapter on acid-base equilibria.

Aadit S.

Numerade Educator

Problem 90

Explain why hydrogen sulfide is a gas at room temperature, whereas water, which has a lower molecular mass, is a liquid.

Nadia L.

Numerade Educator

Problem 91

Give the hybridization and oxidation state for sulfur in $\mathrm{SO}_{2}$, in $\mathrm{SO}_{3}$, and in $\mathrm{H}_{2} \mathrm{SO}_{4}$.

Aadit S.

Numerade Educator

Problem 92

Which is the stronger acid, $\mathrm{NaHSO}_{3}$ or $\mathrm{NaHSO}_{4}$ ?

David C.

Numerade Educator

Problem 93

Determine the oxidation state of sulfur in $\mathrm{SF}_{6}, \mathrm{SO}_{2} \mathrm{~F}_{2}$, and KHS.

Aadit S.

Numerade Educator

Problem 94

Which is a stronger acid, sulfurous acid or sulfuric acid? Why?

David C.

Numerade Educator

Problem 95

Oxygen forms double bonds in $\mathrm{O}_{2}$, but sulfur forms single bonds in $\mathrm{S}_{8}$. Why?

Aadit S.

Numerade Educator

Problem 96

Give the Lewis structure of each of the following:
(a) $\mathrm{SF}_{4}$
(b) $\mathrm{K}_{2} \mathrm{SO}_{4}$
(c) $\mathrm{SO}_{2} \mathrm{Cl}_{2}$
(d) $\mathrm{H}_{2} \mathrm{SO}_{3}$
(e) $\mathrm{SO}_{3}$

Nadia L.

Numerade Educator

Problem 97

Write two balanced chemical equations in which sulfuric acid acts as an oxidizing agent.

Aadit S.

Numerade Educator

Problem 98

Explain why sulfuric acid, $\mathrm{H}_{2} \mathrm{SO}_{4}$, which is a covalent molecule, dissolves in water and produces a solution that contains ions.

Nadia L.

Numerade Educator

Problem 99

How many grams of Epsom salts $\left(\mathrm{MgSO}_{4} \cdot 7 \mathrm{H}_{2} \mathrm{O}\right)$ will form from $5.0 \mathrm{~kg}$ of magnesium?

Aadit S.

Numerade Educator

Problem 100

What does it mean to say that mercury(II) halides are weak electrolytes?

Nadia L.

Numerade Educator

Problem 101

Why is $\mathrm{SnCl}_{4}$ not classified as a salt?

Aadit S.

Numerade Educator

Problem 102

The following reactions are all similar to those of the industrial chemicals. Complete and balance the equations for these reactions:
(a) reaction of a weak base and a strong acid $\mathrm{NH}_{3}+\mathrm{HClO}_{4} \longrightarrow$
(b) preparation of a soluble silver salt for silver plating $\mathrm{Ag}_{2} \mathrm{CO}_{3}+\mathrm{HNO}_{3} \longrightarrow$
(c) preparation of strontium hydroxide by electrolysis of a solution of strontium chloride $\mathrm{SrCl}_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \stackrel{\text { electrolysis }}{\longrightarrow}$

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Problem 103

Which is the stronger acid, $\mathrm{HClO}_{3}$ or $\mathrm{HBrO}_{3}$ ? Why?

Aadit S.

Numerade Educator

Problem 104

What is the hybridization of iodine in $\mathrm{IF}_{3}$ and $\mathrm{IF}_{5} ?$

Nadia L.

Numerade Educator

Problem 105

Predict the molecular geometries and draw Lewis structures for each of the following. You may wish to review the chapter on chemical bonding and molecular geometry.
(a) $\mathrm{IF}_{5}$
(b) $\mathrm{I}_{3}^{-}$
(c) $\mathrm{PCl}_{5}$
(d) $\mathrm{SeF}_{4}$
(e) $\mathrm{ClF}_{3}$

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Problem 106

Which halogen has the highest ionization energy? Is this what you would predict based on what you have learned about periodic properties?

Nadia L.

Numerade Educator

Problem 107

Name each of the following compounds:
(a) $\mathrm{BrF}_{3}$
(b) $\mathrm{NaBrO}_{3}$
(c) $\mathrm{PBr}_{5}$
(d) $\mathrm{NaClO}_{4}$
(e) $\mathrm{KClO}$

Aadit S.

Numerade Educator

Problem 108

Explain why, at room temperature, fluorine and chlorine are gases, bromine is a liquid, and iodine is a solid.

David C.

Numerade Educator

Problem 109

What is the oxidation state of the halogen in each of the following?
(a) $\mathrm{H}_{5} \mathrm{IO}_{6}$
(b) $\mathrm{IO}_{4}^{-}$
(c) $\mathrm{ClO}_{2}$
(d) $\mathrm{ICl}_{3}$
(e) $\mathrm{F}_{2}$

Shahina -.

Numerade Educator

Problem 110

Physiological saline concentration- that is, the sodium chloride concentration in our bodies -is approximately $0.16 \mathrm{M}$. A saline solution for contact lenses is prepared to match the physiological concentration. If you purchase $25 \mathrm{~mL}$ of contact lens saline solution, how many grams of sodium chloride have you bought?

MP

Mihir P.

Numerade Educator

Problem 111

Give the hybridization of xenon in each of the following. You may wish to review the chapter on the advanced theories of covalent bonding.
(a) $\mathrm{XeF}_{2}$
(b) $\mathrm{XeF}_{4}$
(c) $\mathrm{XeO}_{3}$
(d) $\mathrm{XeO}_{4}$
(e) $\mathrm{XeOF}_{4}$

Aadit S.

Numerade Educator

Problem 112

What is the molecular structure of each of the following molecules? You may wish to review the chapter on chemical bonding and molecular geometry.
(a) $\mathrm{XeF}_{2}$
(b) $\mathrm{XeF}_{4}$
(c) $\mathrm{XeO}_{3}$
(d) $\mathrm{XeO}_{4}$
(e) $\mathrm{XeOF}_{4}$

Nadia L.

Numerade Educator

Problem 113

Indicate whether each of the following molecules is polar or nonpolar. You may wish to review the chapter on chemical bonding and molecular geometry.
(a) $\mathrm{XeF}_{2}$
(b) $\mathrm{XeF}_{4}$
(c) $\mathrm{XeO}_{3}$
(d) $\mathrm{XeO}_{4}$
(e) $\mathrm{XeOF}_{4}$

Aadit S.

Numerade Educator

Problem 114

What is the oxidation state of the noble gas in each of the following? You may wish to review the chapter on chemical bonding and molecular geometry.
(a) $\mathrm{XeO}_{2} \mathrm{~F}_{2}$
(b) $\mathrm{KrF}_{2}$
(c) $\mathrm{XeF}_{3}^{+}$
(d) $\mathrm{XeO}_{6}^{4-}$
(e) $\mathrm{XeO}_{3}$

Nadia L.

Numerade Educator

Problem 115

A mixture of xenon and fluorine was heated. A sample of the white solid that formed reacted with hydrogen to yield 81 mL of xenon (at STP) and hydrogen fluoride, which was collected in water, giving a solution of hydrofluoric acid. The hydrofluoric acid solution was titrated, and $68.43 \mathrm{~mL}$ of $0.3172 \mathrm{M}$ sodium hydroxide was required to reach the equivalence point. Determine the empirical formula for the white solid and write balanced chemical equations for the reactions involving xenon.

Aadit S.

Numerade Educator

Problem 116

Basic solutions of $\mathrm{Na}_{4} \mathrm{XeO}_{6}$ are powerful oxidants. What mass of $\mathrm{Mn}\left(\mathrm{NO}_{3}\right)_{2} \cdot 6 \mathrm{H}_{2} \mathrm{O}$ reacts with $125.0 \mathrm{~mL}$ of a $0.1717 M$ basic solution of $\mathrm{Na}_{4} \mathrm{XeO}_{6}$ that contains an excess of sodium hydroxide if the products include Xe and solution of sodium permanganate?

David C.

Numerade Educator