Chapter 9

Write formulas for the following substances and designate their physical states. a. nitrogen dioxide gas b. liquid gallium c. barium chloride dissolved in water d. solid ammonium carbonate

Identify the reactants in the following reaction: When potassium is dropped into aqueous zinc nitrate, zinc and aqueous potassium nitrate form.

Balance the reaction of hydrogen sulfide with atmospheric oxygen gas. $$\mathrm{H}_{2} \mathrm{S}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g}) \rightarrow \mathrm{SO}_{2}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g})$$

Write word equations for the following skeleton equations. a. \(\mathrm{Cu}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{g}) \rightarrow \mathrm{CuO}(\mathrm{s})\) b. \(\mathrm{K}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(1) \rightarrow \mathrm{KOH}(\mathrm{aq})+\mathrm{H}_{2}(\mathrm{g})\) c. \(\mathrm{CaCl}_{2}(\mathrm{aq})+\mathrm{Na}_{2} \mathrm{SO}_{4}(\mathrm{aq}) \rightarrow \mathrm{CaSO}_{4}(\mathrm{s})+\mathrm{NaCl}(\mathrm{aq})\)

Balance the following reactions. a. \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}(\mathrm{s}) \rightarrow \mathrm{Cr}_{2} \mathrm{O}_{3}(\mathrm{s})+\mathrm{N}_{2}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(\mathrm{g})\) b. \(\mathrm{CO}_{2}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(1) \rightarrow \mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{6}(\mathrm{s})+\mathrm{O}_{2}(\mathrm{g})\)

Hydrogen iodide gas breaks down into hydrogen gas and iodine gas during a decomposition reaction. Write a skeleton equation for this reaction.

Write skeleton equations for these reactions. a. sodium carbonate(s) \(\rightarrow\) sodium oxide(s) \(+\) carbon dioxide \((\mathrm{g})\) b. aluminum(s) \(+\) iodine(s) \(\rightarrow\) aluminum iodide(s) c. iron(II) oxide(s) \(+\) oxygen \((\mathrm{g}) \rightarrow\) iron (III) oxide(s)

Write skeleton equations for these reactions. a. butane \(\left(\mathrm{C}_{4} \mathrm{H}_{10}\right)(1)+\) oxygen \((\mathrm{g}) \rightarrow\) carbon dioxide \((\mathrm{g})+\) water \((1)\) b. aluminum carbonate(s) \(\rightarrow\) aluminum oxide(s) \(+\) carbon dioxide \((\mathrm{g})\) c. silver nitrate (aq) \(+\) sodium sulfide (aq) \(\rightarrow\) silver sulfide(s) \(+\) sodium nitrate(aq)

Write a skeleton equation for the reaction between lithium(s) and chlorine gas to produce lithium chloride(s).

Write skeleton equations for these reactions. a. iron(s) \(+\) fluorine(g) \(\rightarrow\) iron (III) fluoride \((s)\) b. sulfur trioxide(g) \(+\) water \((1) \rightarrow\) sulfuric acid(aq) c. sodium(s) + magnesium iodide(aq) \(\rightarrow\) sodium iodide(aq) + magnesium(s) d. vanadium(s) \(+\) oxygen \((\mathrm{g}) \rightarrow\) vanadium \((\mathrm{V})\) oxide(s)

Write skeleton equations for these reactions. a. lithium \((s)+\operatorname{gold}(\text { III ) chloride }(a q) \rightarrow\) lithium chloride \((a q)+\operatorname{gold}(s)\) b. iron(s) \(+\operatorname{tin}(\mathrm{IV})\) nitrate ( aq) \(\rightarrow\) iron (III) nitrate \((a q)+\operatorname{tin}(s)\) c. nickel(II) chloride(s) \(+\) oxygen \((\mathrm{g}) \rightarrow\) nickel(II) oxide(s) + dichlorine pentoxide(g) d. lithium chromate(aq) \(+\) barium chloride \((a q) \rightarrow\) lithium chloride (aq) + barium chromate(s)

Write chemical equations for these reactions. a. When solid naphthalene \(\left(\mathrm{C}_{10} \mathrm{H}_{8}\right)\) burns in air, the reaction yields gaseous carbon dioxide and liquid water. b. Bubbling hydrogen sulfide gas through manganese(II) chloride dissolved in water results in the formation of the precipitate manganese(II) sulfide and hydrochloric acid. c. Solid magnesium reacts with nitrogen gas to produce solid magnesium nitride. d. Heating oxygen difluoride gas yields oxygen gas and fluorine gas.

List each of the four types of chemical reactions and give an example for each type.

How would you classify a chemical reaction between two reactants that produces one product?

Under what conditions does a precipitate form in a chemical reaction?

Will a metal always replace another metal in a compound dissolved in water? Explain.

In each of the following pairs, which element will replace the other in a reaction? a. tin and sodium \(\quad \) c. lead and silver b. fluorine and iodine \(\quad \) d. copper and nickel

Write a balanced chemical equation for the combustion of liquid methanol \(\left(\mathrm{CH}_{3} \mathrm{OH}\right)\).

Write chemical equations for each of the following synthesis reactions. a. boron + fluorine \(\rightarrow\) b. germanium \(+\) sulfur \(\rightarrow\) c. zirconium \(+\) nitrogen \(\rightarrow\) d. tetraphosphorus decoxide \(+\) water \(\rightarrow\) phosphoric acid

Combustion Write a chemical equation for the combustion of each of the following substances. If a compound contains carbon and hydrogen, assume that carbon dioxide gas and liquid water are produced. a. solid barium b. solid boron c. liquid acetone \(\left(\mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}\right)\) d. liquid octane \(\left(\mathrm{C}_{8} \mathrm{H}_{18}\right)\)

Write chemical equations for each of the following decomposition reactions. One or more products might be identified. a. magnesium bromide \(\rightarrow\) b. cobalt (II) oxide \(\rightarrow\) c. titanium (IV) hydroxide \(\rightarrow\) titanium (IV) oxide + water d. barium carbonate \(\rightarrow\) barium oxide \(+\) carbon dioxide

Write chemical equations for the following single-replacement reactions that might occur in water. If no reaction occurs, write \(NR\) in place of the products. a. nickel + magnesium chloride \(\rightarrow\) b. calcium \(+\) copper \((11)\) bromide \(\rightarrow\) c. potassium \(+\) aluminum nitrate \(\rightarrow\) d. magnesium \(+\) silver nitrate \(\rightarrow\)

Complete the following word equation. Solute \(+\) Solvent \(\rightarrow\)

Define each of the following terms: solution, solvent, and solute.

When reactions occur in aqueous solutions, what common types of products are produced?

Compare and contrast chemical equations and ionic equations.

What is a net ionic equation? How does it differ from a complete ionic equation?

Define spectator ion.

Write the net ionic equation for a chemical reaction that occurs in an aqueous solution and produces water.

Complete the following chemical equations a. \(\mathrm{Na}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(1) \rightarrow\) b. \(\mathrm{K}(\mathrm{s})+\mathrm{H}_{2} \mathrm{O}(1) \rightarrow\)

Complete the following chemical equation. $$\mathrm{CuCl}_{2}(\mathrm{s})+\mathrm{Na}_{2} \mathrm{SO}_{4}(\mathrm{aq}) \rightarrow$$

Write complete ionic and net ionic equations for each of the following reactions. a. \(\mathrm{K}_{2} \mathrm{S}(\mathrm{aq})+\mathrm{CoCl}_{2}(\mathrm{aq}) \rightarrow 2 \mathrm{KCl}(\mathrm{aq})+\mathrm{CoS}(\mathrm{s})\) b. \(\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq})+\mathrm{CaCO}_{3}(\mathrm{s}) \rightarrow\) \(\mathrm{H}_{2} \mathrm{O}(1)+\mathrm{CO}_{2}(\mathrm{g})+\mathrm{CaSO}_{4}(\mathrm{s})\) c. \(2 \mathrm{HClO}(\mathrm{aq})+\mathrm{Ca}(\mathrm{OH})_{2}(\mathrm{aq}) \rightarrow_{2 \mathrm{H}_{2} \mathrm{O}(1)+\mathrm{Ca}(\mathrm{ClO})_{2}(\mathrm{aq})}\)

A reaction occurs when hydrosulfuric acid \(\left(\mathrm{H}_{2} \mathrm{S}\right)\) is mixed with an aqueous solution of iron(III) bromide. The reaction produces solid iron(III) sulfide and aqueous hydrogen bromide. Write the chemical and net ionic equations for the reaction.

Paper A reaction occurs when sulfurous acid \(\left(\mathrm{H}_{2} \mathrm{SO}_{3}\right)\) is mixed with an aqueous solution of sodium hydroxide. The reaction produces aqueous sodium sulfite, a chemical used in manufacturing paper. Write the chemical and net ionic equations for the reaction.

Photosynthesis Identify the products in the following reaction that occurs in plants: Carbon dioxide and water react to produce glucose and oxygen

How will aqueous solutions of sucrose and hydrogen chloride differ?

Write the word equation for each of these skeleton equations. \(\mathrm{C}_{6} \mathrm{H}_{6}\) is the formula for benzene. a. \(C_{6} \mathrm{H}_{6}(1)+\mathrm{O}_{2}(\mathrm{g}) \rightarrow \mathrm{CO}_{2}(\mathrm{g})+\mathrm{H}_{2} \mathrm{O}(1)\) b. \(\mathrm{CO}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g}) \rightarrow \mathrm{CO}_{2}(\mathrm{g})\) c. \(\mathrm{Cl}_{2}(\mathrm{g})+\mathrm{NaBr}(\mathrm{s}) \rightarrow \mathrm{NaCl}(\mathrm{s})+\mathrm{Br}_{2}(\mathrm{g})\) d. \(\mathrm{CaCO}_{3}(\mathrm{s}) \rightarrow \mathrm{CaO}(\mathrm{s})+\mathrm{CO}_{2}(\mathrm{g})\)

Write skeleton equations for the following reactions. a. ammonium phosphate(aq) \(+\) chromium(III) bromide(aq) \(\rightarrow\) ammonium bromide (aq) \(+\) chromium (III) phosphate(s) b. chromium(VI) hydroxide(s) \(\rightarrow\) chromium (VI) oxide(s) \(+\) water ( \((1)\) c. aluminum(s) \(+\) copper \((1)\) chloride (aq) \(\rightarrow\) aluminum chloride(aq) \(+\) copper \((s)\) d. potassium iodide(aq) \(+\) mercury (I) nitrate(aq) \(\rightarrow\) potassium nitrate(aq) \(+\) mercury (I) iodide(s)

Predict whether each of the following reactions will occur in aqueous solutions. If you predict that a reaction will not occur, explain your reasoning. Note: Barium sulfate and silver bromide precipitate in aqueous solutions. a. sodium hydroxide + ammonium sulfate \(\rightarrow\) b. niobium(V) sulfate \(+\) barium nitrate \(\rightarrow\) c. strontium bromide \(+\) silver nitrate \(\rightarrow\)

Precipitate Formation The addition of hydrochloric acid to beakers containing solutions of either sodium chloride (NaCl) or silver nitrate \((KNO _{3} )\) causes a white precipitate in one of the beakers. a. Which beaker contains a precipitate? b. What is the precipitate? c. Write a chemical equation showing the reaction. d. Classify the reaction.

Write the skeleton equation and the balanced chemical equation for the reaction between iron and chlorine.

Write a chemical equation representing the decomposition of water into two gaseous products. What are the products?

Distinguish between an ionic compound and a molecular compound dissolved in water. Do all molecular compounds ionize when dissolved in water? Explain.

Classify the type of reactions that occur in aqueous solutions, and give an example to support your answer

Explain how an equation can be balanced even if the number of reactant particles differs from the number of product particles.

Apply Describe the reaction of aqueous solutions of sodium sulfide and copper(II) sulfate, producing the precipitate copper(II) sulfide.

Predict A piece of aluminum metal is placed in aqueous \(\mathrm{KCl}\) . Another piece of aluminum is placed in an aqueous \(\mathrm{AgNO}_{3}\) solution. Explain why a chemical reaction does or does not occur in each instance.

Design an Experiment You suspect the water in a lake close to your school might contain lead in the form of \(\mathrm{Pb}^{2+}(\mathrm{aq})\) ions. Formulate your suspicion as a hypothesis and design an experiment to test your theory. Write the net ionic equations for the reactions of your experiment. \(\left(\text { Hint: In aqueous solution, } P b^{2+} \text { forms com- }\right.\) pounds that are solids with \(C l^{-}, B r^{-}, I^{-},\) and \(S O_{4}^{2-}\) ions.)

Apply Write the chemical equations and net ionic equations for each of the following reactions that might occur in aqueous solutions. If a reaction does not occur, write \(NR\) in place of the products. Magnesium phosphate precipitates in an aqueous solution. a. KNO \(_{3}+\mathrm{CsCl} \rightarrow\) b. \(\mathrm{Ca}(\mathrm{OH})_{2}+\mathrm{KCN} \rightarrow\) c. \(\mathrm{Li}_{3} \mathrm{PO}_{4}+\mathrm{MgSO}_{4} \rightarrow\) d. \(\mathrm{HBrO}+\mathrm{NaOH} \rightarrow\)

Analyze Explain why a nail exposed to air forms rust, whereas the same nail exposed to a pure nitrogen environment does not form rust.