Give the molecular formula for each of the following acids: a. sulfurous acid b. chloric

a. What are monatomic ions? b. Give three examples of monatomic ions.

How does the chemical formula for the nitrite ion differ from the chemical formula for the nitrate ion?

Using only the periodic table, write the symbol of the ion most typically formed by each of the following elements: a.K d. Cl b. Ca e.Ba c.S f.Br

Write the formula for and indicate the charge on each of the following ions: a. sodium ion b. aluminum ion c. chloride ion d. nitride ion e. iron(II) ion f. iron(III) ion

Name each of the following monatomic ions: a. K d. Clb. Mg2 e. 02 c. AP L Ca

Write formulas for the binary ionic compounds formed between the following elements. (Hint: See Sample Problem A.) a. sodium and iodine b. calcium and sulfur c. zinc and chlorine d. barium and fluorine e. lithium and oxygen

Give the name of each of the following binary ionic compounds. (Hint: See Sample Problem B.) a. KC1 c. Li20 b. CaBr2 d. MgCl2

Write the formulas for and give the names of the compounds formed by the following ions: a. Cr2and F b. Ni2and 02 c. Fe3and 02

What determines the order in which the component elements of binary molecular compounds are written?

Name the following binary molecular compounds according to the prefix system. (Hint: See Sample Problem D.) a. CO2 d. SeF6 b. Cd 4 e. As205 C- PC15

Write formulas for each of the following binary molecular compounds. (Hint: See Sample Problem D.) a. carbon tetrabromide b. silicon dioxide c. tetraphosphorus decoxide d. diarsenic trisuffide

Distinguish between binary acids and oxyacids, and give two examples of each.

a. What is a salt? b. Give two examples of salts.

Name each of the following acids: a. BF d. H2SO4 b. HBr e. H3PO4 c. HNO3

Give the molecular formula for each of the following acids: a. sulfurous acid b. chloric acid c. hydrochloric acid d. hypochlorous acid e. perchloric acid f. carbonic acid g. acetic acid

Write formulas for each of the following compounds: a. sodium fluoride b. calcium oxide c. potassium sulfide d. magnesium chloride e. aluminum bromide L lithium nitride g. iron(II) oxide

Name each of the following ions: a. NH f. CO b. CIO- g. PO c. OH- h. CH3C00 d. SO i. HCO e. NO j. CrO

Write the formula and charge for each of the following ions: a. ammonium ion g. copper(II) ion b. acetate ion h. tin(II) ion c. hydroxide ion i. iron(III) ion d. carbonate ion j. copper(I) ion e. sulfate ion k. mercury(I) ion f. phosphate ion 1. mercury(II) ion

Name each of the following ions according to the Stock system: a. Fe2 d. Pb b. Fe3 e. Sn2 c. Pb2 f. Sn

Name each of the binary molecular compounds in item 11 by using the Stock system.

Write formulas for each of the following compounds: a. phosphorus(III) iodide b. sulfur(II) chloride c. carbon(IV) sulfide d. nitrogen(V) oxide

a. What are oxidation numbers? b. What useful functions do oxidation numbers serve?

Name each of the following ionic compounds by using the Stock system: a. NaCl b. KF c. CaS d. Co(NO3)2 e. FePO4 f. Hg2SO g. H93(PO4)2

Assign oxidation numbers to each atom in the following compounds. (Hint: See Sample Problem E.) a. HI b. PBr3 c. GeS2 d. KH e. As205 1. H3PO

Assign oxidation numbers to each atom in the following ions. (Hint: See Sample Problem E.) a. NO b. ClO C. PO d. Cr204 e. CO

a. Define formula mass. b. In what unit is formula mass expressed?

What is meant by the molar mass of a compound?

Determine the formula mass of each of the following compounds or ions. (Hint: See Sample Problem F.) a. glucose, C6111206 b. calcium acetate, Ca(CH3COO)2 c. the ammonium ion, NH41 d. the chlorate ion, ClO

Determine the number of moles of each type of monatomic or polyatomic ion in one mole of the following compounds. For each polyatomic ion, determine the number of moles of each atom present in one mole of the ion. a. KNO3 b. Na2SO4 c. Ca(OH)2 d. (NH4)2S03 e. Ca3(PO4)2 f. Al2(Cr04)3

Determine the molar mass of each compound MIXED i ,&vi i av listed in item 29. (Hint: See Sample Problem G.)

Determine the number of moles of compound in each of the following samples. (Hint: See Sample Problem I.) a. 4.50 g H20 b. 471.6 g Ba(OH)2 c. 129.68 g Fe3(PO4)2

Determine the percentage composition of each of the following compounds. (Hint: See Sample Problem J.) a. NaCl b. AgNO3 c. Mg(OH)2

Determine the percentage by mass of water in the hydrate CuSO45H20. (Hint: See Sample Problem K.)

What three types of information are used to find an empirical formula from percentage composition data?

What is the relationship between the empirical formula and the molecular formula of a compound?

Determine the empirical formula of a cornpound containing 63.50% silver, 8.25% nitrogen, and 28.25% oxygen. (Hint: See Sample Problem L.)

Determine the empirical formula of a coipound found to contain 52.11% carbon, 13.14% hydrogen, and 34.75% oxygen.

What is the molecular formula of the molecule that has an empirical formula of CH20 and a molar mass of 120.12 g/mol?

A compound with a formula mass of 42.08 amu is found to be 85.64% carbon and 14.36% hydrogen by mass. Find its molecular formula.

Chemical analysis shows that citric acid contains 37.51% C, 4.20% H, and 58.29% 0. What is the empirical formula for citric acid?

Name each of the following compounds by using the Stock system: a. LiBr b. Sn(NO3)2 c. FeC12 d. MgO e. KOH f. Fe03 g. AgNO3 h. Fe(OH)2 i. CrF

What is the mass in grams of each of the following samples? a. 1.000 mol NaCl b. 2.000 mol H20 c. 3.500 mol Ca(OH)2 d. 0.625 mol Ba(NO3)2

Determine the formula mass and molar mass of each of the following compounds: a. XeF b. C12H2406 c. Hg212 d.CuCN

Write the chemical formulas for the following compounds: a. aluminum fluoride b. magnesium oxide c. vanadium(V) oxide d. cobalt(II) sulfide e. strontium bromide f. sulfur trioxide

How many atoms of each element are contained in a single formula unit of iron(III) for mate, Fe(CH02)3 'H20? What percentage by mass of the compound is water?

Name each of the following acids, and assign oxidation numbers to the atoms in each: a. HNO2 b. H2S03 c. H2CO3 d. HI

Determine the percentage composition of the following compounds: a. NaC1O b. H2S03 c. C2H5COOH d. BeCl2

Name each of the following binary compounds: a. Mg12 e. SO2 b. NaF f. PBr3 C- CS2 g. CaCl2 d. N204 h. AgI

Assign oxidation numbers to each atom in the following molecules and ions: a. CO2 e. H202 b. NH f. P4010 c. Mn04 g. OF2 d. S2032-

A 175.0 g sample of a compound contains 56.15 g C, 9.43 g H, 74.81 g 0, 13.11 g N, and 21.49 g Na. What is the compound's empirical formula?

Analyzing Information Sulfur trioxide is produced in the atmosphere through a reaction of sulfur dioxide and oxygen. Sulfur dioxide is a primary air pollutant. Analyze the formula for sulfur trioxide. Then, list all of the chemical information from the analysis that you can.

Analyzing Data In the laboratory, a sample of pure nickel was placed in a clean, dry, weighed crucible. The crucible was heated so that the nickel would react with the oxygen in the air. After the reaction appeared complete, the crucible was allowed to cool and the mass was determined. The crucible was reheated and allowed to cool. Its mass was then determined again to be certain that the reaction was complete. The following data were collected: Mass of crucible = 30.02 g Mass of nickel and crucible = 31.07 g Mass of nickel oxide and crucible = 31.36 g Determine the following information based on the data given above: Mass of nickel = Mass of nickel oxide = Mass of oxygen = Based on your calculations, what is the empirical formula for the nickel oxide?

Review the common reactions of Group 1 metals in the Elements Handbook, and answer the following questions: a. Some of the Group 1 metals react with oxygen to form superoxides. Write the formulas for these compounds. b. What is the charge on each cation for the formulas that you wrote in (a)? c. How does the charge on the anion vary for oxides, peroxides, and superoxides?

Review the common reactions of Group 2 metals in the Elements Handbook, and answer the following questions: a. Some of the Group 2 metals react with oxygen to form oxides. Write the formulas for these compounds. b. Some of the Group 2 metals react with oxygen to form peroxides. Write the formulas for these compounds. c. Some of the Group 2 metals react with nitrogen to form nitrides. Write the formulas for these compounds. d. Most Group 2 elements form hydrides. What is hydrogen's oxidation state in these compounds?

Review the analytical tests for transition metals in the Elements Handbook, and answer the following questions: a. Determine the oxidation state of each metal in the precipitates shown for cadmium, zinc, and lead. b. Determine the oxidation state of each metal in the complex ions shown for iron, manganese, and cobalt. c. The copper compound shown is called a coordination compound. The ammonia shown in the formula exists as molecules that do not have a charge. Determine copper's oxidation state in this compound.

Review the common reactions of Group 15 elements in the Elements Handbook, and answer the following questions: 59. a. Write formulas for each of the oxides listed for the Group 15 elements. b. Determine nitrogen's oxidation state in the oxides listed in (a).

Nomenclature Biologists who name newly discovered organisms use a system that is structured very much like the one used by chemists in naming compounds. The system used by biologists is called the Linnaeus system, after its creator, Carolus Linnaeus. Research this system in a biology textbook, and then note similarities and differences between the Linnaeus system and chemical nomenclature.

Common Chemicals Find out the systematic chemical name and write the chemical formula for each of the following common compounds: a. baking soda d. limestone b. milk of magnesia e. lye c. Epsom salts f. wood alcohol

Performance Assessment Your teacher will supply you with a note card that has one of the following formulas on it: NaCH3COO31-120, MgC12.6H20, LiC21-1302'21120, or MgSO47H20. Design an experiment to determine the percentage of water by mass in the hydrated salt assigned to you. Be sure to explain what steps you will take to ensure that the salt is completely dry. If your teacher approves your design, obtain the salt and perform the experiment. What percentage of water does the salt contain?

Both ammonia, NH3, and ammonium nitrate, NH4NO3, are used in fertilizers as a source of nitrogen. Which compound has the higher percentage of nitrogen? Research the physical properties of both compounds, and find out how each compound is manufactured and used. Explain why each compound has its own particular application. (Consider factors such as the cost of raw ingredients, the ease of manufacture, and shipping costs.)