Question: Name each of the following binary compounds,

> If an electric current is passed through aqueous solutions of sodium chloride, sodium bromide, and sodium iodide, the elemental halogens are produced at one electrode in each case, with hydrogen gas being evolved at the other electrode. If the liquid is

> When hydrogen sulfide, H2S, gas is bubbled through a solution of lead(II) nitrate, Pb(NO3)2, a black precipitate of lead(II) sulfide, PbS, forms, and nitric acid, HNO3, is produced. Write the unbalanced chemical equation for this reaction.

> If aqueous solutions of potassium chromate and barium chloride are mixed, a bright yellow solid (barium chromate) forms and settles out of the mixture, leaving potassium chloride in solution. Write a balanced chemical equation for this process.

> Consider a hypothetical element M, which is capable of forming stable simple cations that have charges of 1+, 2+, and 3+, respectively. Write the formulas of the compounds formed by the various M cations with each of the following anions. a. chromate b

> Consider a hypothetical simple ion M2+. Determine the formula of the compound this ion would form with each of the following anions. a. acetate b. permanganate c. oxide d. hydrogen phosphate e. hydroxide f. nitrite

> Most metallic elements form oxides, and often the oxide is the most common compound of the element that is found in the earth’s crust. Write the formulas for the oxides of the following metallic elements. a. potassium b. magnesium c. iron(II) d. iron

> A compound has the general formula X2O, with X representing an unknown element or ion and O representing oxygen. Which of the following could not be a name for this compound? a. sodium oxide b. iron(II) oxide c. copper(I) oxide

> Although we write the formula of sodium chloride as NaCl, we realize that NaCl is an ionic compound and contains no molecules. Explain.

> Name the following compounds. a. HClO3 b. CoCl3 c. B2O3 d. H2O e. HC2H3O2 f. Fe(NO3)3 g. CuSO4

> Name the following compounds. a. AuBr3 b. Co(CN)3 c. MgHPO4 d. B2H6 e. NH3 f. Ag2SO4 g. Be(OH)2

> Name the following compounds. a. Ca(C2H3O2) 2 b. PCl3 c. Cu(MnO4) 2 d. Fe2 (CO3) 3 e. LiHCO3 f. Cr2S3 g. Ca(CN) 2

> Complete the following list by filling in the missing oxyanion or oxyacid for each pair. CIO,- HIO3 CIO- BrO,- HCIO2

> Examine the following table of formulas and names. Which of the compounds is/are named correctly? Formula……………………………………..Name a. Al2S3………………………………………dialuminum trisulfate b. CuNO3……………………………………….…copper(III) nitrate c. Fe(ClO4) 2………………………………….……iron(III

> On some periodic tables, hydrogen is listed both as a member of Group 1 and as a member of Group 7. Write an equation showing the formation of H+ ion and an equation showing the formation of H- ion.

> Nitrogen and oxygen form numerous binary compounds, including NO, NO2, N2O4, N2O5, and N2O. Give the name of each of these oxides of nitrogen.

> Before an electrocardiogram (ECG) is recorded for a cardiac patient, the ECG leads are usually coated with a moist paste containing sodium chloride. What property of an ionic substance such as NaCl is being made use of here?

> Iron forms both 2+ and 3+ cations. Write formulas for the oxide, sulfide, and chloride compound of each iron cation, and give the name of each compound in both the nomenclature method that uses Roman numerals to specify the charge of the cation and the -

> Write the formula for each of the following substances. a. calcium hydrogen sulfate b. zinc phosphate c. iron(III) perchlorate d. cobaltic hydroxide e. potassium chromate f. aluminum dihydrogen phosphate g. lithium bicarbonate h. manganese(II) ac

> In a simple binary ionic compound, which ion (cation/anion) has the same name as its parent element?

> Write the formula for each of the following substances. a. sodium peroxide b. calcium chlorate c. rubidium hydroxide d. zinc nitrate e. ammonium dichromate f. hydrosulfuric acid g. calcium bromide h. hypochlorous acid i. potassium sulfate j. ni

> Write the formula for each of the following acids. a. hydrocyanic acid b. nitric acid c. sulfuric acid d. phosphoric acid e. hypochlorous acid f. hydrobromic acid g. bromous acid h. hydrofluoric acid

> Write the formula for each of the following acids. a. hydrosulfuric acid b. perbromic acid c. acetic acid d. hydrobromic acid e. chlorous acid f. hydroselenic acid g. sulfurous acid h. perchloric acid

> Write the formula for each of the following compounds that contain polyatomic ions. Be sure to enclose the polyatomic ion in parentheses if more than one such ion is needed to balance the oppositely charged ions. a. ammonium acetate b. ferrous hydroxid

> Write the formula for each of the following compounds that contain polyatomic ions. Be sure to enclose the polyatomic ion in parentheses if more than one such ion is needed to balance the oppositely charged ion(s). a. ammonium nitrate b. magnesium acet

> Write the formula for each of the following binary compounds of nonmetallic elements. a. diphosphorus monoxide b. sulfur dioxide c. diphosphorus pentoxide d. carbon tetrachloride e. nitrogen tribromide f. silicon tetrafluoride g. sulfur dichloride

> Write the formula for each of the following binary compounds of nonmetallic elements. a. carbon disulfide b. water c. dinitrogen trioxide d. dichlorine heptoxide e. carbon dioxide f. ammonia g. xenon tetrafluoride

> Write the formula for each of the following simple binary ionic compounds. a. magnesium fluoride b. ferric iodide c. mercuric sulfide d. barium nitride e. plumbous chloride f. stannic fluoride g. silver oxide h. potassium selenide

> Write the formula for each of the following simple binary ionic compounds. a. cobalt(II) chloride b. cobaltic chloride c. sodium phosphide d. iron(II) oxide e. calcium hydride f. manganese(IV) oxide g. magnesium iodide h. copper(I) sulfide

> Name each of the following acids. a. HOCl b. H2SO3 c. HBrO3 d. HOI e. HBrO4 f. H2S g. H2Se h. H3PO3

> In naming ionic compounds, we always name the second.

> Name each of the following acids. a. HCl b. H2SO4 c. HNO3 d. HI e. HNO2 f. HClO3 g. HBr h. HF i. HC2H3O2

> Many acids contain the element in addition to hydrogen.

> Give a simple definition of an acid.

> Name each of the following compounds, which contain polyatomic ions. a. NaMnO4 b. AlPO4 c. CrCO3 d. Ca(ClO)2 e. BaCO3 f. CaCrO4

> Name each of the following compounds, which contain polyatomic ions. a. NH4NO3 b. Ca(HCO3)2 c. MgSO4 d. Na2HPO4 e. KClO4 f. Ba(C2H3O2)2

> Give the name of each of the following polyatomic ions. a. NH4+ b. H2PO4- c. SO42- d. HSO3- e. ClO4- f. IO3-

> Give the name of each of the following polyatomic ions. a. HCO3- b. C2H3O2- c. CN- d. OH- e. NO2- f. HPO42-

> Carbon occurs in several common polyatomic anions. List the formulas of as many such anions as you can, along with the names of the anions.

> Write the formulas for the following compounds (refer to your answers to Problem 30). a. sodium cyanide b. calcium carbonate c. potassium hydrogen carbonate d. magnesium acetate

> Write the formula for each of the following carbon-containing ions, including the overall charge of the ion. a. cyanide b. carbonate c. hydrogen carbonate d. acetate

> Cations are ions, and anions are ions.

> Write the formula for each of the following phosphorus- containing ions, including the overall charge of the ion. a. phosphide b. phosphate c. phosphite d. hydrogen phosphate

> A series of oxyanions of iodine, comparable to the series for chlorine discussed in the text, also exists. Write the formulas and names for the oxyanions of iodine.

> Complete the following list by filling in the missing names or formulas of the oxyanions of chlorine. CIO,- hypochlorite CIO,- chlorite

> In naming oxyanions, when there are more than two members in the series for a given element, what prefixes are used to indicate the oxyanions in the series with the fewest and the most oxygen atoms?

> For the oxyanions of sulfur, the ending -ite is used for SO32- to indicate that it contains than does SO42-.

> A(n) is a polyatomic ion containing at least one oxygen atom and one or more atoms of at least one other element.

> What is a polyatomic ion? Give examples of five common polyatomic ions.

> Name each of the following binary compounds, using the periodic table to determine whether the compound is likely to be ionic (containing a metal or a nonmetal) or nonionic (containing only nonmetals). a. RaCl2 b. SeCl2 c. PCl3 d. Na3P e. MnF2 f. Z

> Many over-the-counter antacid tablets are now formulated using calcium carbonate as the active ingredient, which enables such tablets to also be used as dietary calcium supplements. As an antacid for gastric hyperacidity, calcium carbonate reacts by comb

> What is a binary chemical compound? What are the two major types of binary chemical compounds? Give three examples of each type of binary compound.

> Name each of the following binary compounds, using the periodic table to determine whether the compound is likely to be ionic (containing a metal and a nonmetal) or nonionic (containing only nonmetals). a. Fe3P2 b. CaBr2 c. N2O5 d. PbCl4 e. S2F10 f

> What is meant by a strong electrolyte? Give two examples of substances that behave in solution as strong electrolytes.

> When the ionic solute K3PO4 is dissolved in water, what can you say about the number of potassium ions (K+) present in the solution compared with the number of phosphate ions (PO43-) in the solution?

> Reactions involving the combustion of fuel substances make up a subclass of reactions.

> How do we define a combustion reaction? In addition to the chemical products, what other products do combustion reactions produce? Give two examples of balanced chemical equations for combustion reactions.

> Silver oxide may be decomposed by strong heating into silver metal and oxygen gas. Write the unbalanced chemical equation for this process.

> For the reaction 2Na(s) + O2(g) Na2O2(s), show how electrons are gained and lost by the atoms.

> For the reaction Mg(s) + Cl2(g) MgCl2(s), illustrate how electrons are gained and lost during the reaction.

> If oxygen molecules, O2, were to react with magnesium atoms, how many electrons would each magnesium atom lose? How many electrons would each oxygen atom gain? How many magnesium atoms would be needed to react with each oxygen molecule? What charges woul

> If atoms of the metal calcium were to react with molecules of the nonmetal fluorine, F2, how many electrons would each calcium atom lose? How many electrons would each fluorine atom gain? How many calcium atoms would be needed to react with one fluorine

> The thermite reaction produces so much energy (heat) that the iron is initially formed as a liquid. 2Al(s) + Fe2O3(s) 2Fe(s) + Al2O3(s) Describe the transfer of electrons for both the aluminum and iron.

> Give an example of a simple chemical reaction that involves the transfer of electrons from a metallic element to a nonmetallic element.

> What is an oxidation–reduction reaction? What is transferred during such a reaction?

> When writing the chemical equation for a reaction, how do you indicate that a given reactant is dissolved in water? How do you indicate that a precipitate has formed as a result of the reaction?

> Along with the three strong acids emphasized in the chapter (HCl, HNO3, and H2SO4), hydrobromic acid, HBr, and perchloric acid, HClO4, are also strong acids. Write equations for the dissociation of each of these additional strong acids in water.

> Write balanced equations showing how three of the common strong acids ionize to produce hydrogen ion.

> If electricity of sufficient voltage is passed into a solution of potassium iodide in water, a reaction takes place in which elemental hydrogen gas and elemental iodine are produced, leaving a solution of potassium hydroxide. Write the unbalanced equatio

> What is a salt? Give two balanced chemical equations showing how a salt is formed when an acid reacts with a base.

> If 1000 NaOH units were dissolved in a sample of water, the NaOH would produce Na1 ions and OH2 ions.

> Write the formulas and names of three common strong acids and strong bases.

> The same net ionic process takes place when any strong acid reacts with any strong base. Write the equation for that process.

> What is meant by a strong base? Are the strong bases also strong electrolytes? Explain.

> What is meant by a strong acid? Are the strong acids also strong electrolytes? Explain.

> Another step in the qualitative analysis of cations (see Exercise 28) involves precipitating some of the metal ions as the insoluble sulfides (followed by subsequent treatment of the mixed sulfide precipitate to separate the individual ions). Write balan

> A reaction in aqueous solution that results in the formation of a solid is called a reaction.

> Many plants are poisonous because their stems and leaves contain oxalic acid, H2C2O4, or sodium oxalate, Na2C2O4; when ingested, these substances cause swelling of the respiratory tract and suffocation. A standard analysis for determining the amount of o

> The procedures and principles of qualitative analysis are covered in many introductory chemistry laboratory courses. In qualitative analysis, students learn to analyze mixtures of the common positive and negative ions, separating and confirming the prese

> Liquid hydrazine, N2H4, has been used as a fuel for rockets. When the rocket is to be launched, a catalyst causes the liquid hydrazine to decompose quickly into elemental nitrogen and hydrogen gases. The rapid expansion of the product gases and the heat

> Many chromate (CrO42-) salts are insoluble, and most have brilliant colors that have led to their being used as pigments. Write balanced net ionic equations for the reactions of Cu2+, Co3+, Ba2+, and Fe3+ with chromate ion.

> Write the balanced molecular, complete ionic, and net ionic equations for the reaction between nickel(II) chloride and sodium sulfide.

> Which of the following most accurately describes a spectator ion? a. An ion that is used up in a chemical reaction; it is limiting. b. An ion that participates in a chemical reaction but is always present in excess c. An ion that becomes part of the p

> A solution of zinc nitrate is mixed with a solution of potassium hydroxide. A precipitate forms. Complete and balance the equation for this reaction, including the phases of each reactant and product.

> What is a “driving force”? What are some of the driving forces discussed in this section that tend to make reactions likely to occur? Can you think of any other possible driving forces?

> On the basis of the general solubility rules given in Table 7.1, for each of the following compounds, explain why the compound would not be expected to be appreciably soluble in water. Indicate which of the solubility rules covers each substance’s partic

> On the basis of the general solubility rules given in Table 7.1, for each of the following compounds, explain why the compound would be expected to be appreciably soluble in water. Indicate which of the solubility rules covers each substanceâ€

> Using the general solubility rules given in Table 7.1, which of the following ions will form a precipitate with SO42-? a. Ba2+ b. Na+ c. NH4+ d. At least two of the above ions will form a precipitate with SO42-. e. All of the above ions will form a

> In a chemical reaction, the total number of atoms present after the reaction is complete is (larger than/smaller than/the same as) the total number of atoms present before the reaction began.

> For the unbalanced chemical equation HCl(g) + O2(g) H2O(g) + Cl2(g) a. list the reactant(s). b. list the product(s).

> If a sample of pure hydrogen gas is ignited very carefully, the hydrogen burns gently, combining with the oxygen gas of the air to form water vapor. Write the unbalanced chemical equation for this reaction.

> Balance the following chemical equations. MnO2(s) + CO(g) Mn2O3(aq) + CO2(g) Al(s) + H2SO4(aq) Al2(SO4)3(aq) + H2(g) C4H10(g) + O2(g) CO2(g) + H2O(l) NH4I(aq) + Cl2(g)

> Using different shapes to distinguish between different elements, draw a balanced equation for the following reaction at the microscopic level. NH3(g) + O2(g) NO(g) + H2O(g)

> Balance the following chemical equation: CuSO4(aq) + KI(s) CuI(s) + I2(s) + K2SO4(aq)

> Which of the following statements about chemical reactions is false? a. When balancing a chemical equation, all subscripts must be conserved. b. When one coefficient is doubled, the rest of the coefficients in the balanced equation must also be doubled

> When lead(II) sulfide is heated to high temperatures in a stream of pure oxygen gas, solid lead(II) oxide forms with the release of gaseous sulfur dioxide. Write the unbalanced chemical equation for this reaction.

> When copper(II) oxide is boiled in an aqueous solution of sulfuric acid, a strikingly blue solution of copper(II) sulfate forms along with additional water. Write the unbalanced chemical equation for this reaction.

> What are the substances to the left of the arrow in a chemical equation called? To the right of the arrow? What does the arrow itself mean?

> When solid red phosphorus, P4, is burned in air, the phosphorus combines with oxygen, producing a choking cloud of tetraphosphorus decoxide. Write the unbalanced chemical equation for this reaction.

> Which of the following statements is false for the reaction of hydrogen gas with oxygen gas to produce water? (a, b, and c represent coefficients) a H2(g) + b O2(g) c H2O(g) a. The ratio of “ayc” must always equal one. b. The sum o

> When a strip of magnesium metal is heated in oxygen, it bursts into an intensely white flame and produces a finely powdered dust of magnesium oxide. Write the unbalanced chemical equation for this process.