Question: Name each of the following binary compounds.

> Kyle Sanders was auditing the financial statements of World Wholesale Industries when she was presented with a curious situation. A member of World’s top management team approached her with an anonymous note that had been retrieved from the company’s sug

> Chacon University is a Midwest university with 16,000 students, using various legacy systems for student records, financial systems, human resources, and financial aid. The president of Chacon heard a presentation about ERP systems at a seminar for unive

> Michael Michner Industries (MMI) is a manufacturer of warehouse and inventory tracking systems. MMI has four U.S. plants and three warehouses. The company employs 3,500 workers at these facilities and the corporate headquarters. MMI is using legacy syste

> In the early days of computers, Chris Schuler was a very enterprising young man who, while attending UCLA, was also conducting a major fraud against Continental Telephone and Telegraph Company (CT&T). At the height of his fraud in 2015, he was collecting

> Gleason, Inc., is a manufacturer of plastic knobs for lawn and garden tractors and lawn mowers. The company has always used traditional paper based systems to conduct transactions with its customers. For example, when a customer ordered knobs, Gleason pe

> The EnviroPlan Company, a small business with 100 employees, sells environmental consulting services to large companies around the United States. It employs 40 consultants who travel the United States, assisting clients with environmental compliance. To

> Cody Chambers agreed to help his fraternity obtain sponsors for its annual charitable event to be held during Homecoming week. He accepted this responsibility at the recommendation of last year’s fundraiser, who told Cody that the task would require appr

> Lynn Roberts frequently makes purchases from mail order catalogs. Recently, she ordered a dress she intended to wear to her cousin’s wedding. Unfortunately, she did not receive the package on time, and on the evening before the wedding, Lynn went shoppin

> Why is it sometimes necessary to change business processes when IT systems are applied to business processes?

> The CEO of Missouri Motor Company, Jason Bell, resigned on November 1, 2014. His resignation had been negotiated with the Board of Directors of Missouri Motor after it was revealed that Mr. Bell violated the company’s corporate ethics policy by having an

> Cooper’s Cues Company is a small manufacturing operation that makes and sells pool cues for sporting goods stores and billiard halls in Baltimore, Maryland, and the surrounding local area. Rob Cooper and his wife, Stacy are the owners and only employees

> Consider any recent purchase you made at a department store such as Target, Walmart, or Kmart. A business process that occurred was the sale of a product to you. However, to make that sale, the department store had to engage in many other processes that

> The fast food industry has been dramatically altered through IT enablement. However, IT enablement has not completely eliminated manual processes in fast food franchise restaurants such as McDonald’s, Wendy’s, and Burger King. Required: Using your expe

> Explain the importance of user authentication and network break-in controls in extranets.

> Describe the differences between B2C and B2B.

> Describe the activities that take place in the supply chain of a manufacturing firm.

> Describe the benefits to the consumer of B2C sales.

> How does the use of HTML, URLs, domain names, and SSL contribute to an Internet that can be used worldwide?

> Categorize each of the following as one‐to-one, one‐to‐many, or many‐to‐many: • Subsidiary ledgers and general ledgers • Transactions and special journal • General ledgers and trial balances

> How do you think a company may be able to influence a supplier to meet its business processing requirements?

> Suppose that a large company uses batch processing for recording its inventory purchases. Other than its slow response time, what would be the most significant problem with using a batch processing system for recording inventory purchases?

> Think of a database that would be needed at a professional service firm to maintain the contact list of clients/patients at the office of a CPA, attorney, or medical doctor. Identify the fields likely to be used in this database. If you were constructing

> Describe why there may be two authorizations related to revenue, expenditures, and conversion processes before they are posted to the general ledger.

> Describe the steps in a manual accounting cycle.

> Explain the internal control environment of source of capital and investment processes.

> Describe the steps in investment processes and explain how top management is involved.

> Describe the steps in source of capital processes and explain how top management is involved.

> Using the table below, match the IT systems on the left with their definitions on the right: CAD a. A network including production equipment, computer terminals, and accounting systems CAM b. Electronic workstation including advanced graphics and 3D

> When taking a physical inventory count at a typical manufacturing facility, which category of inventory (raw materials, work‐in‐process, or finished goods) is likely to be the most time consuming to count and determine the relevant costs for? Why?

> Describe how a cost accountant would cancel a production order upon completion of the related product. Why is this important?

> How is integration across business processes different between legacy systems and modern, integrated systems?

> How might the sales and cash collection processes at a Wal‐Mart store differ from the sales and cash collection processes at McDonald’s?

> Elemental boron is produced in one industrial process by heating diboron trioxide with magnesium metal, also producing magnesium oxide as a by-product. Write the unbalanced chemical equation for this process.

> Which of the following statements is(are) correct? a. The symbols for the elements magnesium, aluminum, and xenon are Mn, Al, and Xe, respectively. b. The elements P, As, and Bi are in the same family on the periodic table. c. All of the following ele

> Provide the name of the acid that corresponds to the formula given in the following table. Formula Acid Name H,SO, HC,H;O2 HCIO, HOCI HCN

> What are the names of the compounds that correspond to the formulas given in the following table? Formula Compound Name Co(NO2)2 AsFs LICN K;SO3 Li,N PbCrO4

> What are the formulas of the compounds that correspond to the names given in the following table? Compound Name Formula Carbon tetrabromide Cobalt(II) phosphate Magnesium chloride Nickel(II) acetate Calcium nitrate

> Complete the following table to predict whether the given atom will gain or lose electrons in forming the ion most likely to form when in ionic compounds. Gain (G) or Lose (L) Electrons lon Formed Atom K Cs Br Se

> Write the formula for each of the following compounds, which 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. silver(I) perchlorate (usually ca

> Write the formula of each of the following ionic substances. a. sodium dihydrogen phosphate b. lithium perchlorate c. copper(II) hydrogen carbonate d. potassium acetate e. barium peroxide f. cesium sulfite

> Write the formula for each of the following binary compounds of nonmetallic elements. a. sulfur dioxide b. dinitrogen monoxide c. xenon tetrafluoride d. tetraphosphorus decoxide e. phosphorus pentachloride f. sulfur hexafluoride g. nitrogen dioxid

> The notation “(l)” after a substance’s formula indicates it exists in the state.

> Give the name of each of the following simple binary ionic compounds. a. NaBr b. MgCl2 c. AlP d. SrBr2 e. AgI f. K2S

> Name each of the following compounds, which contain polyatomic ions. a. LiH2PO4 b. Cu(CN)2 c. Pb(NO3)2 d. Na2HPO4 e. NaClO2 f. Co2(SO4)3

> Give the name of each of the following polyatomic anions. a. CO32- b. ClO3- c. SO42- d. PO43- e. ClO4- f. MnO4-

> Write the formula for each of the following chromium-containing ions, including the overall charge of the ion. a. chromous b. chromate c. chromic d. dichromate

> Examine the following table of formulas and names. Which of the compounds is/are named incorrectly? Formula……………………………………….Name a. Al2S3……………………dialuminum trisulfide b. KClO3……………………….potassium chlorate c. Rb2O….…………………………..rubidium oxide d. CrPO4……………c

> Which oxyanion of nitrogen contains a larger number of oxygen atoms, the nitrate ion or the nitrite ion?

> Name each of the following compounds. a. Fe(C2H3O2)3 b. BrF c. K2O2 d. SiBr4 e. Cu(MnO4)2 f. CaCrO4

> Write the name of each of the following ionic substances, using -ous or -ic endings to indicate the charge of the cation. a. SnCl2 b. FeO c. SnO2 d. PbS e. Co2S3 f. CrCl2

> Why are the physical states of the reactants and products often indicated when writing a chemical equation?

> In which of the following pairs is the name incorrect? Give the correct name for the formulas indicated. a. Ag2O, disilver monoxide b. N2O, dinitrogen monoxide c. Fe2O3, iron(II) oxide d. PbO2, plumbous oxide e. Cr2(SO4)3, chromium(III) sulfate

> We indicate the charge of a metallic element that forms more than one cation by adding a(n) after the name of the cation.

> Give the name of each of the following simple binary ionic compounds. a. BeO b. MgI2 c. Na2S d. Al2O3 e. HCl f. LiF g. Ag2S h. CaH2

> Balance the following chemical equations. Fe(s) + O2(g) Fe2O3(s) PbO2(s) PbO(s) + O2(g) H2O2(l) O2(g) + H2O(l)

> What does “balancing” an equation accomplish?

> For each of the following processes that show the formation of ions, complete the process by indicating the number of electrons that must be gained or lost to form the ion. Indicate the total number of electrons in the ion, and in the atom from which it

> For each of the negative ions listed in column 1, use the periodic table to find in column 2 the total number of electrons the ion contains. A given answer may be used more than once. Column 1………………….Column 2 [ 1] Se2-………………………….[a] 18 [ 2] S2-………………………

> An ion with two more electrons than it has protons has a charge.

> An atom that has lost three electrons will have a charge of .

> An ion with one less electron than it has protons has a charge.

> When an atom gains two electrons, the ion formed has a charge of .

> Under what physical state at room temperature do each of the halogen elements exist?

> For a metallic element that forms two stable cations, the ending is used to indicate the cation of lower charge and the ending is used to indicate the cation of higher charge.

> The elements of Group 7 (fluorine, chlorine, bromine, and iodine) consist of molecules containing atom(s) .

> The formula for ammonium phosphate is .

> The noble metals gold, silver, and platinum are often used in fashioning jewelry because they are relatively .

> 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.