Unit 5 Notepack: Chapters 10 NAME Chemical Quantities .
Unit 5 Notepack:Chemical QuantitiesChapters 10NAMEPeriod:Unit 5 – Chemical Names, and Formulas & MolesUnit Goals- As you work through this unit, you should be able to:1. Distinguish between ionic and molecular compounds.2. Relate cations and anions to metals and nonmetals.READ:3. Distinguish between chemical formulas, molecular formulas, and formula units.Chapter 9 & 104. Know the charges of the formulas for monatomic ions using the periodic table.5. Be familiar with the charges and the formulas for polyatomic ions.6. Apply the rules for naming and writing formulas for binary and ternary ionic compounds.7. Apply the rules for naming and writing formulas for binary molecular compounds.8. Describe how Avogadro’s number is related to a mole of any substance and the number of different particlesthat are a part of the substance.9. Calculate the mass of a mole of any substance.10. Calculate the volume of a mole of any gaseous substance at STP.11. Use moles to convert among measurements of mass, number of particles, and volume.12. Calculate the percent composition of a substance from its chemical formula or experimental data.13. Derive the empirical formula and molecular formula of a compound from experimental data.Assignments:DescriptionA5Chemical Names andFormulas WS(Goals 1-3)A6Ionic Compounds WS(Goals 4-6)A7A1A2Activities, Labs & Test540Mole ActivityMole Chalk ActivityHydrated Crystals PercentComposition LabEmperical Formula LabUnit 5 Test &Naming Master TestMolecular CompoundsWS(Goal 7)Mole Conversions WS(Goals 8 - 9)More Mole ConversionsWS(Goals 9-11)A3Percent CompositionWS(Goal 12)A4Emperical andMolecular Formulas WS(Goal 13)Late Lab Stamp(this stamp means you arenot qualified to do lab andtest corrections)Key Terms: mole, Avogadro’s number, molar mass, molar volume, STP, percent composition, molecularformula, empirical formula,Demo’s: Ethanol Spark Plug, Glass samples of moles, 1 mole of CO 2 in balloon, Making Water
Chapter 10.1: MoleWhat is a mole?How do we measure quantities ofmatter?What are examples of countingunits?What can we count in chemistry?How much is a mole?What is molar mass?What are the four representativeparticles that we can calculate themolar masses of? Give examples.10.1 Sample Calculations: We must show our work using dimensional analysis.1. How many moles of magnesium is 1.25 x 1023 atoms of magnesium?2. How many moles is 2.80 x 1024 atoms of silicon?
3. How many molecules is 0.360 mole of water?4. How many moles are equal to 2.41 x 1024 formula units of sodium chloride (NaCl)?5. How many atoms are in 2.12 moles of propane (C3H8)?6. How many atoms are there in 1.14 mole of sulfur trioxide?7. How many moles are there in 4.65 x 1024 molecules of nitrogen dioxide?8. How many atoms of Carbon are in 2.0 moles of C12H22O11, sucrose sugar?9. What is the molar mass of carbon?10. What is the molar mass of hydrogen gas?11. What is the molar mass of sulfur?12. What is the molar mass of sulfur trioxide?13. What is the molar mass of hydrogen?14. What is the molar mass of carbon dioxide?15. What is the molar mass of sodium chloride?
16. What is the molar mass of ammonium carbonate?17. What is the molar mass of potassium oxide?Review Problems:1. Find the gram formula mass of each compound:a. lithium sulfideb. iron (III) chloridec. calcium hydroxide2. How many oxygen atoms are in a representative particle of each substance?a. ammonium nitrateb. acetylsalicylic acid (C9H8O4), the chemical name of aspirinc. ozone (O3), a disinfectant and natural molecule found in the atmosphere3. How many moles in each of the following:a. 1.50 x 1023 molecules of ammonia, NH3?b. 1 billion (1 x 109) molecules of oxygen, O2?
c. 4.81 x 1024 atoms of lithium, Li?Chapter 10.2: Mole mass and Mole Volume Relationships.How are moles and mass related?What is STP?Why is STP important whenquantifying gases?What is the volume of a Mole ofGas at STP?
Mole MapOne step examples:1. Find the mass of 2.7 moles ofC6H12O6.2. How many moles are in 6.72gof Silver Nitrate?3. Determine the volume, in liters,of 0.60 moles of sulfur dioxidegas at STP.4. Determine the number ofmoles of oxygen gas in 11.5 L atSTP.Multi-step examples:5. What is the mass of 27 liters ofnitrogen dioxide at STP?
6. If you have 9.64 x 1024 mlc’s ofcarbon dioxide, what would bethe volume of that gas at STP?7. If you weight 301 grams ofAluminum Oxide, how manyformula units will you have?Sample Calculations:1. Find the mass, in grams of each.a. 3.32 mole of potassium atoms, K.b. 4.52 x 1021 molecules of C6H12O6c. 0.0112 liters of carbon dioxide2. Calculate the number of moles in 75 grams of each substance.a. dinitrogen trioxideb. sodium oxide3. How many grams are in 9.45 liters of dinitrogen trioxide?4. Find the number of moles in 92.2 grams of iron (III) oxide
5. What is the volume at STP of these gases?a. 3.20 x 10-3 mol carbon dioxideb. 0.960 grams of methane, CH4c. 3.70 x 10 24 molecules nitrogen gas6. Assuming STP, how many moles are in these volumes?a. 67.2 liters of sulfur dioxide gasb. 0.880 liters of helium gasc. 1,000 liters of neon gasChapter 10.3: Percent Composition and chemical formulasWhat is percent composition of acompound?How do we find the percent ofanything?
What is percent composition usedfor and how do we show our work?How do you calculate the percentcomposition of a compound?Example: Calculate the percent composition of potassium dichromate.Sample Calculations:1. 9.30 grams of magnesium combine completely with 3.48 grams of nitrogen gas to form a compound.What is the percent composition of this compound?2. 29.0 grams of silver combine completely with 4.30 grams of sulfur to form a compound. What is thepercent composition of this compound?3. Calculate the percent composition of these compounds:a. sodium bicarbonateb. ammonium chloridec. sulfur trioxide
A. Using Percent as a Conversion Factor1. You can use percent composition to calculate the number of of an element contained in aamount of a compound. To do this, you multiply the mass of the compound by aconversion factor that is based on the percent composition.Example: Calculate the mass of carbon in 82 grams of propane (C3H8).Sample Calculations:Calculate the grams of nitrogen in 125 grams of each fertilizer.a. CO(NH2)2b. NH3c. NH4NO3B. Calculating Empirical Formulas1. Determining the percent composition of a compound has an important application – calculating theempirical formula:2. Define empirical formula:3. Define molecular formula:4. The empirical formula may or may not be the same as the molecular formula5. Practice: These are all molecular formulas, in other words, true formulas. Write their empiricalformulas:H20H2O2CO2N2O46. We can use the percent composition of a compound to determine its empirical formula.Example: What is the empirical formula of a compound that is 25.9% nitrogen and 74.1% oxygen?
Sample Calculations:1. Calculate the empirical formula of each compound.a. 94.1% O, 5.9% Hb. 79.8% C, 20.2% Hc. 67.6% Hg, 10.8% S, 21.6% Od. 27.59% C, 1.15% H, 16.09% N, 55.17% OC. Molecular Formula Calculations1. The molecular formula is either the as the empirical formula or it is a simplenumber multiple of an empirical formula. For example, the empirical formula ofglucose is . The molecular formula is six times larger equaling. Notice that the molar mass of the molecule is times largerthan the empirical formula2. Calculate the molecular formula of a compound whose molar mass is 60.0 g/mol and the empiricalformula is CH4N.3. Find the molecular formula of ethylene glycol, which is used as antifreeze. The molar mass is 62 g/moland the empirical formula is CH3O
Distinguish between chemical formulas, molecular formulas, and formula units. 4. Know the charges of the formulas for monatomic ions using the periodic table. Chapter 9 & 10 5. Be familiar with the charges and the formulas for polyatomic ions. 6. Apply the rules for naming and writing formulas for binary and ternary ionic compounds. 7.
Trigonometry Unit 4 Unit 4 WB Unit 4 Unit 4 5 Free Particle Interactions: Weight and Friction Unit 5 Unit 5 ZA-Chapter 3 pp. 39-57 pp. 103-106 WB Unit 5 Unit 5 6 Constant Force Particle: Acceleration Unit 6 Unit 6 and ZA-Chapter 3 pp. 57-72 WB Unit 6 Parts C&B 6 Constant Force Particle: Acceleration Unit 6 Unit 6 and WB Unit 6 Unit 6
THIS IS A PREVIEW. The full product includes 5 comprehension questions for using text evidence for each of the following chapter sets: Chapters 1-5 Chapters 6-10 Chapters 11-15 Chapters 16-20 Chapters 21-25 Chapters 26-30 Also included are complete answer keys with page numbers for your reference or to provide to
Additional Questions for the Love Does Study Guide A Six-Week Study Program: Week 1 - read the Forward, Introduction, and chapters 1-4 Week 2 - read chapters 5-9 Week 3 - read chapters 10-14 Week 4 - read chapters 15-20 Week 5 - read chapters 21-26 Week 6 - read chapters 27-31 and the epilogue Advice to hosts
LESSONS TOPICS Lesson 1: Basics of Geography. Chapters 1-4 Lesson 2: The United States and Canada. Chapters 5-6 Lesson 3: Latin America. Chapters 7-9 Lesson 4: Northern, Western and Southern Europe. Chapters 10-12 Lesson 5: Eastern Europe and Russia. Chapters 13-14 Lesson 6: Australia, New Zealand and Oceania. Chapter 32-33
questions per chapter. However, if the textbook includes more or less than twenty chapters the default scheme can be adapted to include: A sub-set of available chapters if the textbook is composed of more than twenty chapters. A sub-set of available chapters with repetition of a number of chapters selected randomly (Ex.
International Financial Markets (Chapters 2-5) Exchange Rate Behavior (Chapters 6-8) Long-Term Investment and Financing Decisions (Chapters 13-18) Short-Term Investment and Financing Decisions (Chapters 19-21) Exchange Rate Risk Management (Chapters 9-12) Risk and Return of MNC Value and Stock Price of MNC 1.30
Carlo Rovelli Invitational A –chapters 1-2 Invitational B –chapters 1-2-3 District –chapters 3-4 Regional –chapters 4-5-6 State –chapters 5-6-7 Directed Study Questions. Each Test Increases in Di
System as the Army’s personnel accountability automation system with the electronic Military Personnel Office (throughout). o Deletes Personnel Transaction Register (AAC-P01) (throughout). Headquarters Department of the Army Washington, DC 1 April 2015 Personnel-General Personnel Accounting and Strength Reporting *Army Regulation 600–8–6 Effective 1 May 2015 H i s t o r y . T h i s p u b .
