CHEMICAL NAMES AND FORMULAS

CHEMICAL NAMES AND FORMULAS Practice Problems In your notebook, solve the following problems. SECTION 9.1 NAMING IONS What is the charge on the ion typically formed by each element? a. oxygen c. sodium e. nickel, 2 electrons lost b. iodine d. aluminum f. magnesium How many electrons does the neutral atom gain or lose when each ion forms? a. Cr 3+ c. Li + e. Cl b. P 3 d. Ca 2+ f. O 2 Name each ion. Identify each as a cation or an anion. a. Sn 2+ c. Br e. H b. Co 3+ d. K + f. Mn 2+ Write the formula (including charge) for each ion. Use Table 9.3 if necessary. a. carbonate ion c. sulfate ion e. chromate ion b. nitrite ion d. hydroxide ion f. ammonium ion Name the following ions. Identify each as a cation or an anion. a. CN c. PO 4 3 e. Ca 2+ b. HCO 3 d. Cl f. SO 3 2 SECTION 9.2 NAMING AND WRITING FORMULAS FOR IONIC COMPOUNDS Write the formulas for these binary ionic compounds. a. magnesium oxide c. potassium iodide e. sodium sulfide b. tin(ii) fluoride d. aluminum chloride f. ferric bromide Write the formulas for the compounds formed from these pairs of ions. a. Ba 2+, Cl c. Ca 2+, S 2 e. Al 3+, O 2 b. Ag +, I d. K +, Br f. Fe 2+, O 2 Name the following binary ionic compounds. a. MnO 2 c. CaCl 2 e. NiCl 2 g. CuCl 2 b. Li 3N d. SrBr 2 f. K 2S h. SnCl 4

NAMING AND WRITING FORMULAS FOR IONIC COMPOUNDS Apply the rules for naming and writing formulas for binary ionic compounds Apply the rules for naming and writing formulas for compounds with polyatomic ions binary compound Use this completion exercise to check your understanding of the concepts and terms that are introduced in this section. Each blank can be completed with a term, short phrase, or number. Binary ionic compounds are named by writing the name of the 1 followed by the name of the. 2 Names of binary compounds end in. 3 For example, NaI is. 4 When a cation has more than one ionic charge, a 5 is used in the name. Compounds with polyatomic ions whose names end in -ite or -ate contain a polyatomic 6 that includes. 7 In writing the formula of an ionic compound, the net ionic charge must be. 8 6. 7. 8. Part B True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. 9. The systematic name for baking soda (NaHCO 3) is sodium bicarbonate. 10. In writing a formula for an ionic compound, the net ionic charge of the formula must be zero.

NAMING AND WRITING FORMULAS FOR MOLECULAR COMPOUNDS Interpret the prefixes in the names of molecular compounds in terms of their chemical formulas Apply the rules for naming and writing formulas for binary molecular compounds Use this completion exercise to check your understanding of the concepts and terms that are introduced in this section. Each blank can be completed with a term, short phrase, or number. Binary molecular compounds are composed of two 1 elements. The name of this type of compound ends in. 2 Prefixes are used to show how many 3 of each element are present in a molecule of the compound. For example, the name of As 2S 5 is. 4 Part B True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. Binary molecular compounds contain carbon. 6. Charges must be balanced when writing formulas for molecular compounds. 7. CO 2 is named monocarbon dioxide.

NAMING AND WRITING FORMULAS FOR ACIDS AND BASES Apply three rules for naming acids Apply the rules in reverse to write formulas of acids Apply the rules for naming bases acid base Use this completion exercise to check your understanding of the concepts and terms that are introduced in this section. Each blank can be completed with a term, short phrase, or number. An acid is a compound that contains one or more 1 atoms and produces 2 when dissolved in water. There are rules for naming acids. For example, HBr is called 3 acid, whereas HNO 3 is called 4 acid. A base is a(n) 5 compound that produces 6 when dissolved in water. Ionic compounds that are bases are named in the same way as other 7 compounds, that is, the name of the 8 is followed by the name of the. 9 6. 7. 8. 9. Part B True-False Classify each of these statements as always true, AT; sometimes true, ST; or never true, NT. 10. A compound that contains hydrogen atoms will be an acid when dissolved in water.

THE LAWS GOVERNING FORMULAS AND NAMES Define the laws of definite proportions and multiple proportions Apply the rules for writing chemical formulas by using a flowchart Apply the rules for naming chemical compounds by using a flowchart law of definite proportions law of multiple proportions Use this completion exercise to check your understanding of the concepts and terms that are introduced in this section. Each blank can be completed with a term, short phrase, or number. [Use Figure 9.20 to complete this exercise.] The law of 1 states that in samples of any chemical compound, the masses of the elements are always in the same. 2 The law of 3 states that whenever the same two elements form more than one compound, the different masses of one element that combine with the same mass of the other element are in the ratio of 4 numbers. H 3PO 4 is a(n). 5 It is called. 6 CCl 4 is not a(n). 7 It contains two elements, so it is a 8 compound. It does not contain a metal, so it is a binary 9 compound. The compound is called. 10 Pb(C 2H 3O 2) 2 is not a(n). 11 It contains more than two. 12 C 2H 3O 2 is a polyatomic. 13 Pb is a Group 14 metal. The compound is called. 15 6. 7. 8. 9. 10. 1 1 1 1 1

CHEMICAL QUANTITIES Practice Problems In your notebook, solve the following problems. SECTION 10.1 THE MOLE: A MEASUREMENT OF MATTER What is the molar mass of sucrose (C 12H 22O 11)? What is the molar mass of each of the following compounds? a. phosphorus pentachloride (PCl 5) b. uranium hexafluoride (UF 6) Calculate the molar mass of each of the following ionic compounds: a. KMnO 4 b. Ca 3(PO 4) 2 How many moles is 52 10 24 molecules of water? How many atoms of zinc are in 0.60 mol of zinc? 6. What is the mass of 00 mol of oxygen (O 2)? SECTION 10.2 MOLE MASS AND MOLE VOLUME RELATIONSHIPS What is the molar mass of each of the following compounds? a. C 6H 12O 6 b. NaHCO 3 c. C 7H 12 d. KNH 4SO 4 Calculate the mass in grams of each of the following: a. 8.0 mol lead oxide (PbO) d. 50 10 2 mol molecular oxygen (O 2) b. 0.75 mol hydrogen sulfide (H 2S) e. 30 mol ethylene glycol (C 2H 6O 2) c. 0.00100 mol silicon tetrahydride (SiH 4) How many grams are in 73 mol of dinitrogen pentoxide (N 2O 5)? How many grams are in 0.658 mol of calcium phosphate [Ca 3(PO 4) 2]? Calculate the number of moles in each of the following: a. 0.50 g sodium bromide (NaBr) d. 0.00100 g monochloromethane (CH 3Cl) b. 15 g magnesium nitrate [Mg(NO 3) 2] e. 50 10 3 g propylene glycol [C 3H 6(OH) 2] c. 02 g magnesium chloride (MgCl 2) 6. A chemist plans to use 430 grams of ammonium nitrate (NH 4NO 3) in a reaction. How many moles of the compound is this? 7. A solution is to be prepared in a laboratory. The solution requires 0.0465 mol of quinine (C 20H 24N 2O 2). What mass, in grams, should the laboratory technician obtain in order to make the solution?

THE MOLE: A MEASUREMENT OF MATTER Relate Avogadro s number to a mole of a substance Calculate the mass of a mole of any substance Describe methods of measuring the amount of something Compare and contrast the atomic mass of an element and its molar mass mole (mol) Avogadro s number representative particle molar mass Key Equations moles = representative particles 6.02 10 representative particles 23 representative particles = moles 23 6.02 10 representative particles Use this completion exercise to check your knowledge of the terms and your understanding of the concepts introduced in this section. Each blank can be completed with a term, short phrase, or number. Chemists relate units of counting, of mass, and of volume to a single quantity called the. 1 The number of representative particles in a mole of a substance is. 2 To find the mass of a mole of a compound, scientists add together the 3 of the atoms making up the compound. When you substitute the unit grams for amu, you obtain the 4 of the compound. There are 5 representative particles in a mole of any substance.

MOLE-MASS AND MOLE-VOLUME RELATIONSHIPS Convert the mass of a substance to the number of moles of a substance, and the number of moles of a substance to mass Calculate the volume of a quantity of gas at STP Avogadro s hypothesis standard temperature and pressure (STP) molar volume Key Equations mass (grams) mass (grams) = number of moles moles = mass (grams) mass (grams) grams grams 24 L = mole L 24 L volume of gas = moles of gas Use this completion exercise to check your knowledge of the terms and your understanding of the concepts introduced in this section. Each blank can be completed with a term, short phrase, or number. At STP (0 C and 1 atmosphere pressure), one mole of any gas occupies a volume of 1 L. This quantity is known as the 2 of the gas. To determine the volume in liters of 00 mol of SO 2 gas at STP, you would use 3 as a conversion factor., 4 expressed in the units g/l, is used as a conversion factor when converting from volume to molar mass. When converting between numbers of representative particles, masses, and volumes, you must always convert to 5 as an intermediate step.

PERCENT COMPOSITION AND CHEMICAL FORMULAS Calculate the percent by mass of an element in a compound Interpret an empirical formula Compare and contrast empirical and molecular formulas percent composition empirical formula Key Equation mass of element % mass of element = 100% mass of compound Use this completion exercise to check your knowledge of the terms and your understanding of the concepts introduced in this section. Each blank can be completed with a term, short phrase, or number. The 1 of a compound is the percent by mass of each element in a compound. The percent by mass of an element in a compound is the number of grams of the element per 2 g of the compound, multiplied by 100%. To calculate the percent by mass of an element in a known compound, divide the mass of the element in one mole by the 3 and multiply by 100%. A(n) 4 formula represents the lowest 5 ratio of the elements in a compound. It can be calculated from a compound s percent composition. The 6 formula of a compound is either the same as its empirical formula, or it is some whole-number multiple of it. 6.