WKS 9.1 Calculating Molar Mass (1 page)

Size: px
Start display at page:

Download "WKS 9.1 Calculating Molar Mass (1 page)"

Transcription

1 WKS 9.1 Calculating Molar Mass (1 page) Find the molar mass (AKA the molecular or formula mass) for each of the following substances. Name of compound Formula of compound Work Molar Mass (g/mol) dichlorine heptaoxide cesium sulfite tin (IV) hydroxide acetic acid lead (IV) carbonate magnesium nitrite octahydrate potassium phosphide mercury (II) chloride barium bicarbonate ammonium bromide tetrahydrate oxygen gas strontium cyanide silver perchlorate iron (II) phosphate nitric acid copper (I) nitrate cadmium sulfate decahydrate zinc nitride diphosphorus pentaoxide copper (II) bromide iron (III) acetate tin (IV) phosphate chlorine gas ammonium permanganate 90% of a worksheet must be completed to earn credit for that worksheet! Page 1 of 10

2 WKS 9.2 Calculating with Molar Mass (1 page) PART A: MASS TO MOLES USING MOLAR MASS! (Remember: Molar Mass is the general term we use for atomic mass, formula mass, and molecular mass - all in g/mol.) YOU MUST SHOW YOUR WORK USING DIMENSIONAL ANALYSIS TO EARN CREDIT!!! 1. How many moles of nickel are are in 25 g of nickel? (0.43 mol) 2. What is the mass in grams of 1.25 moles of sulfur trioxide? (100. g) 3. How many moles of CaCO 3 are present in a 350 g sample of CaCO 3? (3.5 mol) 4. How many moles are there in 768 grams of iron (III) sulfate? (1.92 mol) 5. You have 13.2 moles of lead (II) nitrate. How many grams is this? (4.37 x 10 3 g) PART B: CALCULATING MOLAR MASS! Use the formula for molar mass for your calculation. (MM = mass / moles) YOU MUST SHOW YOUR WORK TO EARN CREDIT! 6. You have pounds of an unknown compound. It is known that this represents 4.5 moles of the compound. What is the molecular mass of the compound? Hint: There are 454 grams in 1 pound. (51.56 g/mol) 7. What is the molecular mass of a compound if it is known that 658 grams of this compound represent 6.89 moles? (95.5 g/mol) 8. What is the molecular mass of a compound if 54.4 moles weighs Kilograms? (62.7 g/mol) 9. If it is known that 41.6 grams of a pure, monatomic element represent 1.3 moles of the element, what is its atomic mass? a. What element do you think it is? b. If this were known to be a diatomic element instead, what would you predict it to be? 90% of a worksheet must be completed to earn credit for that worksheet! Page 2 of 10

3 WKS 9.3 Calculating with Avogadro s Number (1 page) YOU MUST SHOW YOUR WORK USING DIMENSIONAL ANALYSIS TO EARN CREDIT FOR THESE PROBLEMS! 1. How many moles are represented by 8.27 x molecules of sodium chloride? (1.37 moles) 2. Aspirin, C 9 H 8 O 4, is a commonly used pain killer. An average dose of aspirin in an aspirin tablet contains x 10-3 moles of aspirin. How many molecules does this represent? (1.671 x mlcl) 3. Magnesium sulfate is a salt commonly known as Epsom salts. Epsom salts are commonly used as soaking salts. How many formula units are in 9.6 moles of Epsom salts? (5.8 x f.u.) 4. How many atoms are in 28 g of sodium? (7.3 x atoms Na) 5. How many molecules of chlorine gas are in a 150 g sample? (1.3 X mlcl Cl 2 ) 6. Dioxin, C 12 H 4 Cl 4 O 2 is a powerful poison. How many moles of dioxin are there in g of dioxin? (2.174 mol) 7. One type of antibiotic, penicillin F, has the formula C 14 H 20 N 2 SO 4. How many molecules of penicillin are there in a 250 mg dose of penicillin? (4.8 x mlcl) 8. How many formula units would there be in a 54.3 gram sample of sodium nitrate? (3.85 x f.u.) 9. How much would 3.42 x formula units of mercury (II) oxide weigh in grams? (123g) 10. How many molecules are present in grams of carbon dioxide? (1.57 x molecules) 90% of a worksheet must be completed to earn credit for that worksheet! Page 3 of 10

4 WKS 9.4 Atoms Within Compounds (1 page) These calculations use Avogadro s number, but you are trying to calculate to the count of atoms within a compound. YOU MUST SHOW YOUR WORK USING DIMENSIONAL ANALYSIS TO EARN CREDIT FOR THESE PROBLEMS! 1. How many oxygen atoms are in 163 g. of Al 2 (SO 4 ) 3? (3.44 x atoms O) 2. How many oxygen atoms are in a 235 g sample of oxygen gas? (8.84 x atoms O) 3. How many atoms of chlorine are in 0.20 mole of phosphorus trichloride? (3.6 x atoms Cl) 4. How many DIATOMIC MOLECULES of chlorine would there be in 28.0 grams of chlorine gas? (2.37 x molecules) a. How many ATOMS of chlorine would be present in this same amount? (4.75 x atoms) 5. How many carbon atoms would there be in 200 grams of aluminum carbonate? (1.54 x atoms) 6. How many oxygen atoms are there in 170 grams of cesium phosphate? (8.29 x atoms) 7. If there are known to be 1.06 x oxygen atoms in a sample of barium permanganate, what is the mass of the entire sample of barium permanganate in grams? (82.5 g) 90% of a worksheet must be completed to earn credit for that worksheet! Page 4 of 10

5 WKS 9.5 All Kinds of Compound Stoichiometry!!! (1 page) These questions are combinations of all of the previous types. YOU MUST SHOW YOUR WORK USING DIMENSIONAL ANALYSIS TO EARN CREDIT FOR THESE PROBLEMS! 1. If the molar mass of a substance is 203 g/mol, how many moles are there in 4567 milligrams of this substance? (2.25 x 10-2 mol) 2. How many moles are there in 78 grams of nitrogen gas? (2.8 mol) 3. How many atoms of copper are there in 1.00 kg of pure copper? (9.48 x atoms) 4. How many pounds would 5.75 moles of magnesium hydroxide weigh? There are 454 grams in 1 pound. (0.739 lb) 5. What is the molar mass of a compound if it is known that 8.00 X 10 8 micrograms of it represents 2.55 moles? (314 g/mol) 6. How many atoms of zinc are required to weigh 5.40 nanograms? (5.00 x atoms) 7. I have 3.45 x molecules of water. a. How many moles are there in this amount of water? (5.73 moles) b. How much would this weigh in pounds? (0.227 lbs) 8. If there are known to be 7.93 x atoms of oxygen present in a sample of magnesium sulfate, how much does the sample of magnesium sulfate weigh in pounds? There are 454 grams in 1 pound. (.870 lbs) 9. How many oxygen atoms are there in 2.4 pounds of calcium acetate? There are 454 grams in 1 pound. (1.7 x atoms) 90% of a worksheet must be completed to earn credit for that worksheet! Page 5 of 10

6 WKS 9.6 Percent Composition Problems (2 pages) There are two types of percent composition problems (1) Ones where you are calculating the mass percent of elements, and (2) Ones where you are using the mass percent as a conversion factor within dimensional analysis. YOU MUST SHOW YOUR WORK TO EARN CREDIT FOR THESE PROBLEMS! 1. Calculate the % mass of each element in ammonium nitrate. (N 35.0 %, H 5.0%, %) 2. Calculate the percent of each element in hydrogen phosphate. (H-3.1%, P-31.6%, O-65.3%) 3. Calculate the percent of each element in iron (III) oxide. (Fe = 70.0%, O = 30.0%) 4. Calculate the percent of each element in barium phosphate. (Ba = 68.4%, P = 10.3%, O= 21.3%) 5. For the hydrate sodium sulfate decahydrate, calculate the following: a. The percent of sodium (by mass) in the hydrate (14.3%) b. The percent of oxygen (by mass) in the hydrated compound. (Don t forget about the water!) (69.6%) c. The percent of water (by mass) in the hydrate (55.9%) 6. Calculate the number of grams of magnesium in 50.0 g of magnesium sulfide. (21.6 g) 90% of a worksheet must be completed to earn credit for that worksheet! Page 6 of 10

7 WKS 9.6 Percent Composition Problems (continued) 7. Calculate the number of grams of iron in 80.0 kg of iron (II) carbonate. (3.86 x 10 4 g) 8. Calculate the mass of aluminum (in kg) in 200. Kg of aluminum oxide. (0.106 Kg) 9. What mass of LEAD could be obtained from 50.0 grams of lead (II) oxide ore which is only 30.0% pure lead (II) oxide? (13.9 g) 10. What mass of iron could be obtained from 40.0 grams of iron (III) oxide ore which is only 75.00% pure iron (III) oxide? (21.0 g) 11. A sample of brass contains (by mass) 28.0% zinc and 72.0% copper. If you are a brass manufacturer and only have 68.0 kg of copper and an unlimited supply of zinc, how many kg of brass could you produce? (94.4 kg) 90% of a worksheet must be completed to earn credit for that worksheet! Page 7 of 10

8 WKS 9.7 Empirical Formulas (1 page) Find the empirical formula for each of the following problems. Remember your helpful saying percent to mass, mass to mole, divide by the smallest, multiply until whole!. YOU MUST SHOW YOUR WORK TO EARN CREDIT FOR THESE PROBLEMS! 1. What is the empirical formula for a compound which contains g of iron, g of sulfur and g of oxygen? (FeSO 3 ) 2. Find the empirical formula for a compound which contains 32.8% chromium and 67.2% chlorine. (CrCl 3 ) 3. What is the empirical formula for a compound which contains 67.1% zinc and the rest is oxygen? (ZnO 2 ) 4. Barry Um has a sample of a compound which weighs 200 grams and contains only carbon, hydrogen, oxygen and nitrogen. By analysis, he finds that it contains grams of carbon, g of hydrogen, grams of oxygen and grams of nitrogen. Find its empirical formula. (C 5 H 3 O 2 N 2 ) 5. The characteristic odor of pineapple is due to ethyl butyrate, an organic compound which contains only carbon, hydrogen, and oxygen. If a sample of ethyl butyrate is known to contain g of carbon, g of hydrogen and g of oxygen, what is the empirical formula for ethyl butyrate? (C 3 H 6 O) grams of an organic sample which contains only carbon, hydrogen and oxygen is analyzed and found to contain grams of carbon, grams of hydrogen, and the rest is oxygen. What is the empirical formula for the compound? (C 3 H 6 O 2 ) 90% of a worksheet must be completed to earn credit for that worksheet! Page 8 of 10

9 WKS 9.8 Molecular Formulas and Hydrate Formulas (2 pages) Find the formulas for each of the following problems. YOU MUST SHOW YOUR WORK TO EARN CREDIT FOR THESE PROBLEMS! 1. What is the molecular formula of dichloroacetic acid if the empirical formula is CHOCl and the molecular mass is 128 g/mole? (C 2 H 2 O 2 Cl 2 ) 2. What is the molecular formula of cyanuric chloride if the empirical formula is CClN and the molecular mass is known to be g/mole? (C 3 Cl 3 N 3 ) 3. Find the molecular formula of a compound containing three elements if it is known that 26.7% of the compound is phosphorus, 12.1% is nitrogen and the rest is chlorine. The molecular mass is 695 g/mole. (P 6 N 6 Cl 12 ) 4. The ratio of carbon atoms to hydrogen atoms of oxygen atoms in a molecule of THC (the active ingredient in marijuana) is 11:15:1. The molecular mass of THC is 326 g/mole. What is the molecular formula for tetrahydrocannabinol, THC? (C 22 H 30 O 2 ) 5. A chemist has a sample of hydrated Li 2 SiF 6 and it weighs grams. He heats it strongly to drive off the water of hydration, and after heating, he found that the anhydrous compound has a mass of grams. Find the formula of the hydrate. (Li 2 SiF 6 2H 2 O) 6. A chemist has a sample of hydrated magnesium sulfite which weighs 1.50 grams. After heating it strongly, he finds that grams of water have been driven off. Find the correct formula of the hydrate. (MgSO 3 6H 2 O) 90% of a worksheet must be completed to earn credit for that worksheet! Page 9 of 10

10 WKS 9.8 Molecular Formulas and Hydrate Formulas (continued) 7. A chemist finds by experimentation that a certain compound contains 76.9% dry calcium sulfite and 23.1% water by weight in its crystal. What is the formula of the hydrate? (CaSO 3 2H 2 O) 8. A chemist heats a sample of hydrated lithium nitrate which weighs 170 grams and finds, after heating that it weighs 95.3 grams. Find the correct formula of the hydrate.(lino 3 3H 2 O) 9. A chemist heats a sample of barium bromide and finds that it gave off 10.8 grams of water. The compound which is left in the crucible after heating weighs 89.2 grams. What is the formula of the hydrate?(babr 2 2H 2 O) 90% of a worksheet must be completed to earn credit for that worksheet! Page 10 of 10

Unit 6: Mole Assignment Packet Period:

Unit 6: Mole Assignment Packet Period: Unit 6: Mole Assignment Packet Name: Period: A1: Mole Conversions 1. Identify the representative particle in each of the following: (atom, molecule, formula unit) a. CuSO 4 b. H 2 O c. NaCl d. Zn e. Cu

More information

WRITING FORMULAS: MOLAR MASS, %COMPOSITION, EMPIRICAL AND MOLECULAR FORMULAS

WRITING FORMULAS: MOLAR MASS, %COMPOSITION, EMPIRICAL AND MOLECULAR FORMULAS WRITING FORMULAS: MOLAR MASS, %COMPOSITION, EMPIRICAL AND MOLECULAR FORMULAS REVIEW: Polyatomic ions, writing names from formulas, oxidation number rules I. WRITING FORMULAS FROM NAMES: A. Rules: 1. Know

More information

HW 3 15 Hydrates Notes IC Hydrates HW 4 Water in a Hydrate IC/HW Unit 8 Test Review HW 5 X Unit 8 Test In class on 2/13 and 2/14

HW 3 15 Hydrates Notes IC Hydrates HW 4 Water in a Hydrate IC/HW Unit 8 Test Review HW 5 X Unit 8 Test In class on 2/13 and 2/14 Name: Unit 8- The Mole Day Page # Description IC/HW Due Date Completed All 2 Warm-up IC 1 3 4 Notes on the Mole IC 1 5 7 The Mole IC 1 8 9 Chemical Quantities HW 2 10 Percent Composition Notes IC X 2 Gum

More information

THE MOLE (a counting unit).again!

THE MOLE (a counting unit).again! Name: Period: Date: THE MOLE (a counting unit).again! A mole represents a, much in the same way that a dozen represents a set of twelve. 1 dozen eggs = 12 eggs; 1 mol eggs = 6.022 10 23 eggs 1 dozen carbon

More information

Note Taking Guide: Episode 701. Lab results: 1 doz grains of rice = g (Use this fact as a conversion factor.) Avogadro s Number - the = the number

Note Taking Guide: Episode 701. Lab results: 1 doz grains of rice = g (Use this fact as a conversion factor.) Avogadro s Number - the = the number Note Taking Guide: Episode 701 Name Lab results: 1 doz grains of rice = g (Use this fact as a conversion factor.)? grains of rice = 1.94 g Avogadro s Number - the = the number Molar Mass the of one of

More information

Chapter 8 Chemical Quantities

Chapter 8 Chemical Quantities Chapter 8 Chemical Quantities Molecular Weight and Moles Find the molecular mass or formula massof each of the following 1. HNO 3 2. Ammonium nitrate 3. Fe 2 O 3 4. Rubidium Sulfite 5. H 3 PO 4 6. Lithium

More information

Notes: Molar Mass, Percent Composition, Mole Calculations, and Empirical/Molecular Formulas

Notes: Molar Mass, Percent Composition, Mole Calculations, and Empirical/Molecular Formulas Notes: Molar Mass, Percent Composition, Mole Calculations, and Empirical/Molecular Formulas In Chemistry, a Mole is: the unit that measures the amount of a substance - equals 6.022 x 10 23 particles of

More information

Percent Composition, Empirical Formula, Molecular Formula, Hydrates

Percent Composition, Empirical Formula, Molecular Formula, Hydrates Name: Percent Composition, Empirical Formula, Molecular Formula, Hydrates Essential Questions How can one explain the structure, properties, and interactions of matter? How do substances combine or react

More information

Unit Two Worksheet WS DC U2

Unit Two Worksheet WS DC U2 Unit Two Worksheet WS DC U2 Name Period Short Answer [Writing]. Write skeleton equations representing the following reactions and then balance them. Then identify the reaction type. Include all needed

More information

Stoichiometry Chapter 9 Practice Assessment B

Stoichiometry Chapter 9 Practice Assessment B NAME Hour Date Stoichiometry Chapter 9 Practice Assessment B Objective 1: Interpret balanced chemical equations in terms of interacting moles, representative particles, masses, and gas volume at STP. Directions:

More information

Chapter 3 - Molecules, Compounds and Chemical Equations

Chapter 3 - Molecules, Compounds and Chemical Equations Chapter 3 - Molecules, Compounds and Chemical Equations Section 3.2 two general types of bonding between atoms found in compounds, ionic and covalent ionic bonds result when electrons have been transferred

More information

Exam 1 Worksheet Chemistry 102

Exam 1 Worksheet Chemistry 102 Exam 1 Worksheet Chemistry 102 Chapter 1 Introduction 1. Convert: a. 650 nm to inches b. 650 km to miles c. 345 mg to lb d. 145 lb to μg e. 4.50 10 10 km to μm f. 8.09 10 8 mg to Mg g. 9.00 10 5 ml to

More information

23 carbon atoms The number is known as Avogadro s d Number.

23 carbon atoms The number is known as Avogadro s d Number. THE MOLE (a counting unit).again! i A mole represents a set or group, much in the same way that a dozen represents a set of twelve. 1 dozen eggs = 12 eggs; 1 mol eggs = 6.022 10 23 eggs 1 dozen carbon

More information

AP Chemistry - Summer Assignment

AP Chemistry - Summer Assignment AP Chemistry - Summer Assignment NOTE: a. MUST SHOW ALL WORK FOR CREDIT!! b. Where work is required, do on a separate sheet of paper c. These are the foundational things you should be able to do when you

More information

CHAPTER 6 CHEMICAL COMPOSITION

CHAPTER 6 CHEMICAL COMPOSITION Chemistry Name Hour Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 6 CHEMICAL COMPOSITION Day Plans for the day Assignment(s) for the day 1 Begin Chapter

More information

Germanium 32. Nickel Uranium 92. Sulfur THE MOLE Worksheets

Germanium 32. Nickel Uranium 92. Sulfur THE MOLE Worksheets Germanium 32 Ge 72.61 Nickel 28 Ni 8.693 Uranium 92 U 238.029 Sulfur 16 S 32.066 THE MOLE Worksheets Measuring Matter Counting particles We always use the appropriate units for the number of objects. For

More information

Chapter 8 Nomenclature

Chapter 8 Nomenclature 8.1 Names of Atoms Chapter 8 Nomenclature Simple neutral atoms with no charge are named as is: Na is sodium atom, Ne is neon atom Know the names and symbols for elements #1-20 and Ba, Co, I, Cu, Fe, Pb,

More information

Notes: The Mole. What is the ratio of calcium ions to chloride ions in calcium chloride? Ca 2+ : Cl -

Notes: The Mole. What is the ratio of calcium ions to chloride ions in calcium chloride? Ca 2+ : Cl - Name I. Essential Terminology Notes: The Mole Period Chemistry Pre-AP The smallest particle of an element is the atom. Diatomic elements (like O 2 ) are the main exception to this. We say that diatomic

More information

If Sally has 4.56 x atoms of oxygen in a sample of aluminum oxide, how many kilograms of aluminum does she have?

If Sally has 4.56 x atoms of oxygen in a sample of aluminum oxide, how many kilograms of aluminum does she have? If Sally has 4.56 x 10 34 atoms of oxygen in a sample of aluminum oxide, how many kilograms of aluminum does she have? Bertha has.025 milligrams of sodium that she got from a sample of Sodium phosphate,

More information

Nomenclature (Naming Compounds) and Chemical Formulas

Nomenclature (Naming Compounds) and Chemical Formulas Nomenclature (Naming Compounds) and Chemical Formulas 1 Ions formed from a single atom Monatomic Ions Charges are determined by whether ion has lost electrons (+) or gained electrons (-) Symbols are written

More information

Polyatomic ions You should know the symbols, names, and charges for these common polyatomic ions. Polyatomic Ions to Know + ClO 3. ClO 4 NO

Polyatomic ions You should know the symbols, names, and charges for these common polyatomic ions. Polyatomic Ions to Know + ClO 3. ClO 4 NO AP Chemistry Summer Review Packet 2018 Section 1: Names and Formulas of ionic compounds. Name: Polyatomic ions You should know the symbols, names, and charges for these common polyatomic ions. Polyatomic

More information

This packet contains review material from Pre-AP Chemistry. Be prepared to take a quiz over this material during the first week of school.

This packet contains review material from Pre-AP Chemistry. Be prepared to take a quiz over this material during the first week of school. This packet contains review material from Pre-AP Chemistry. Be prepared to take a quiz over this material during the first week of school. How many significant figures (digits) are represented by each

More information

c formula units of potassium iodide a moles of beryllium b moles of calcium c mole of sulfur a. 6.

c formula units of potassium iodide a moles of beryllium b moles of calcium c mole of sulfur a. 6. Chapter 11 1. Identify and calculate the number of representative particles in each of the following quantities. a. 2.15 moles of gold 2.15 mol Au 1.29 10 24 atoms Au b. 0.151 mole of nitrogen oxide 0.15O

More information

UNIT 7 CHEMICAL FORMULAS WRITING FORMULAS NOTES. EXAMPLES: 1. carbon tetrachloride 2. calcium oxide. 3. iron (III) bromide 4.

UNIT 7 CHEMICAL FORMULAS WRITING FORMULAS NOTES. EXAMPLES: 1. carbon tetrachloride 2. calcium oxide. 3. iron (III) bromide 4. WRITING FORMULAS NOTES EXAMPLES: 1. carbon tetrachloride 2. calcium oxide 3. iron (III) bromide 4. lead (II) nitrate 5. aluminum hydroxide 6. ammonium chromate Notes- HONORS 1 NAMING COMPOUNDS NOTES EXAMPLES:

More information

Summer Assignment Part 2

Summer Assignment Part 2 Summer Assignment Part 2 Name: 1. Metric Conversions. Remember 1 cm 3 = 1 ml 1 L = 1 dm 3 ITEM GIVEN METRIC UNIT DESIRED METRIC UNIT A 8.43 cm mm B 2.41 x 10 2 cm m C 294.5 nm cm D 1.445 x 10 4 m km E

More information

Part 01 - Notes: The Mole and Its Calculations

Part 01 - Notes: The Mole and Its Calculations Part 01 - Notes: The Mole and Its Calculations Objectives: Identify, define, and explain: mole, Avogadro s number, representative particle, gram atomic mass, gram molecular mass, gram formula mass, molar

More information

Lesson 13: Ionic Equations & Intro to the Mole with Conversions

Lesson 13: Ionic Equations & Intro to the Mole with Conversions NOTES Name: Date: Class: Lesson 13: Ionic Equations & Intro to the Mole with Conversions Box 1: Balance: 1. Mg + O2 MgO 2. KClO3 KCl + O2 3. C2H6 + O2 CO2 + H2O Write and balance the equation that represents

More information

Unit 5. Chemical Composition

Unit 5. Chemical Composition Unit 5 Chemical Composition Counting by Mass Individually mass a few Calculate the average mass of one Can count large numbers of by mass Atomic Mass Unit (amu) 1 amu = 1.66 x 10-24 g Subatomic particles

More information

How to Use This Presentation

How to Use This Presentation How to Use This Presentation To View the presentation as a slideshow with effects select View on the menu bar and click on Slide Show. To advance through the presentation, click the right-arrow key or

More information

Duncan UNIT 7 - CHEMICAL FORMULAS WRITING FORMULAS NOTES. Does the second word end with -ide?

Duncan UNIT 7 - CHEMICAL FORMULAS WRITING FORMULAS NOTES. Does the second word end with -ide? WRITING FORMULAS NOTES Does the second word end with -ide? yes no / \ Is the second word "hydroxide"? \ no yes \ \ \ Is the first word "ammonium"? \ no yes ---------------------------------------------->

More information

Nomenclature for ionic compounds

Nomenclature for ionic compounds Name: Nomenclature for ionic compounds Nomenclature is a system of naming. This worksheet presents a widely used system of nomenclature for ionic compounds. There are two types of metal cations with different

More information

EIT Review S2007 Dr. J.A. Mack.

EIT Review S2007 Dr. J.A. Mack. EIT Review S2007 Dr. J.A. Mack www.csus.edu/indiv/m/mackj/ Part 1 Atom: The smallest divisible unit of an element Compound: A substance made of two or more atoms Ion: A charged atom or molecule Cation:

More information

Worksheet 1: REPRESENTATIVE PARTICLES

Worksheet 1: REPRESENTATIVE PARTICLES Worksheet 1: REPRESENTATIVE PARTICLES Directions: For each substance below, state the representative particle. If the RP is a molecule, state the number of atoms that make up the molecule. If the RP is

More information

Show your work for all questions; answer all parts of all questions. No work = no credit.

Show your work for all questions; answer all parts of all questions. No work = no credit. Quiz: Ch 3 & 4 Name: Version M (32 pts) September 16, 2005 AP Chem Period: 1 2 3 4 Show your work for all questions; answer all parts of all questions. No work = no credit. 1. (10 pts) A compound contains

More information

1. Hydrochloric acid is mixed with aqueous sodium bicarbonate Molecular Equation

1. Hydrochloric acid is mixed with aqueous sodium bicarbonate Molecular Equation NAME Hr Chapter 4 Aqueous Reactions and Solution Chemistry Practice A (Part 1 = Obj. 1-3) (Part 2 = Obj. 4-6) Objective 1: Electrolytes, Acids, and Bases a. Indicate whether each of the following is strong,

More information

Description Mole Activity. Late Lab Stamp (this stamp means you are not qualified to do lab and test corrections)

Description Mole Activity. Late Lab Stamp (this stamp means you are not qualified to do lab and test corrections) Unit 5 Notepack: Chapters 10 Chemical Quantities NAME Unit 5 Chemical Names, and Formulas & Moles Unit Goals- As you work through this unit, you should be able to: 1. Distinguish between ionic and molecular

More information

This exam will be given over 2 days. Part 1: Objectives 1-13 Part 2: Objectives 14-24

This exam will be given over 2 days. Part 1: Objectives 1-13 Part 2: Objectives 14-24 Name Hour January Exam Practice A This exam will be given over 2 days. Part 1: Objectives 1-13 Part 2: Objectives 14-24 This practice exam will be graded in the exam portion of the grade book. Objectives

More information

Chapter Six Chemical Names and Formulas WS C U1C6

Chapter Six Chemical Names and Formulas WS C U1C6 Chapter Six Chemical Names and Formulas WS C U1C6 Name Period Section 6.1 Part I: Matching. Match the definition with the term that best correlates to it. No definition will be used more than once. 1.

More information

H 2 O. Chapter 9 Chemical Names and Formulas

H 2 O. Chapter 9 Chemical Names and Formulas H 2 O Chapter 9 Chemical Names and Formulas Section 9.1 Naming Ions OBJECTIVES: Identify the charges on monatomic ions by using the periodic table, and name the ions. Section 9.1 Naming Ions OBJECTIVES:

More information

1.21. Formulae, equations and amounts of substance

1.21. Formulae, equations and amounts of substance 1.21. Formulae, equations and amounts of substance The mole is the key concept for chemical calculations DEFINITION: The mole is the amount of substance in grams that has the same number of particles as

More information

U N I T T E S T P R A C T I C E

U N I T T E S T P R A C T I C E South Pasadena Honors Chemistry Name 6 Compounds Period Date U N I T T E S T P R A C T I C E Section 1: Multiple Choice. Select the best answer choice for each question. (1 point each) 1. Bonds between

More information

CHAPTER 11. The Mole. Mole. One mole of = 6.02 x 10 = 6.02 x 10 CaCl = 6.02 x x 10. Representative Particle. molecules, or formula units

CHAPTER 11. The Mole. Mole. One mole of = 6.02 x 10 = 6.02 x 10 CaCl = 6.02 x x 10. Representative Particle. molecules, or formula units CHAPTER 11 The Mole 11.1 The Mole: Measurement of Matter Matter is measured in one of three ways: (How many?) Mole SI unit that measures the amount of a substance 6.02 x 10 particles of that substance.

More information

4) Tetrasulfur trioxide. 5) barium fluoride. 6) nitric acid. 7) ammonia

4) Tetrasulfur trioxide. 5) barium fluoride. 6) nitric acid. 7) ammonia Unit 9: The Mole- Funsheets Part A: Molar Mass Write the formula AND determine the molar mass for each of the following. Be sure to include units and round you answer to 2 decimal places. 1) calcium carbonate

More information

6.02 X Memorize this Number

6.02 X Memorize this Number Honors Chemistry - Unit 6 Chapters 3 & 7 The Mole Math with Chemical Formulas Voc. Assignment Due: Quiz Date(s): TBA Problem Set (UT Quest) Due: Test Date: Unit 6 Packet - Page 1 of 14 **VOCABULARY Assignment**

More information

Chem RG Chapter Packet 7 Mole & Chemical Composition. Assign Section # Name Ch 07 Test Review (turn in separately for graded points

Chem RG Chapter Packet 7 Mole & Chemical Composition. Assign Section # Name Ch 07 Test Review (turn in separately for graded points Name Period. Chem RG Chapter Packet 7 Mole & Chemical Composition Assign Section # Name 10 5 1. Assignment Sheet printed 2. Notes 7.1 3. Notes 7.2 4. Notes 7.3 5. 7.1 Chapter 7 WS #1 6. 7.2 Chapter 7 WS

More information

1.21. Formulae, equations and amounts of substance

1.21. Formulae, equations and amounts of substance 1.21. Formulae, equations and amounts of substance The mole is the key concept for chemical calculations DEFINITION: The mole is the amount of substance in grams that has the same number of particles as

More information

6. (a) NF 3 is nitrogen trifluoride. (b) HI is hydrogen iodide. (c) BBr 3 is boron tribromide.

6. (a) NF 3 is nitrogen trifluoride. (b) HI is hydrogen iodide. (c) BBr 3 is boron tribromide. 6. (a) NF 3 is nitrogen trifluoride. (b) HI is hydrogen iodide. (c) BBr 3 is boron tribromide. (d) C 6 H 14 is hexane. 7. (a) C 8 H 18 is octane. (b) P 2 S 3 is diphosphorus trisulfide. (c) OF 2 is oxygen

More information

Background: Understanding the Mole

Background: Understanding the Mole Background: Understanding the Mole 1. Why was it important for scientists to know the number of atoms in a sample of matter? 2. What was chosen to use as the standard on which to base the atomic masses

More information

Practice Packet Unit 3: Moles & Stoichiometry

Practice Packet Unit 3: Moles & Stoichiometry PRACTICE PACKET: Unit 3 Moles & Stoichiometry Regents Chemistry: Mr. Palermo Practice Packet Unit 3: Moles & Stoichiometry Vocabulary: Lesson 1: Lesson 2: Lesson 3: Lesson 4: Lesson 5: Lesson 6: Lesson

More information

Ionic and Metallic Bonding

Ionic and Metallic Bonding Unit 5: Ionic and Metallic Bonding H 2 O Valence Electrons are? The electrons responsible for the chemical properties of atoms, and are those in the outer energy level. Valence electrons - The s and p

More information

Part 01 - Notes: Reactions & Classification

Part 01 - Notes: Reactions & Classification Objectives: Identify, define, and explain: combination reaction, synthesis reaction, decomposition reaction, single replacement reaction, double replacement reaction, combustion reaction, rapid oxidation,

More information

NAMING IONIC COMPOUNDS

NAMING IONIC COMPOUNDS NAMING IONIC COMPOUNDS 1 WHAT ARE IONIC COMPOUNDS Ionic compounds are formed between elements that are in ionic form. A simpler way of determining whether a compound is ionic is to see if there are any

More information

PERCENTAGE COMPOSITION

PERCENTAGE COMPOSITION PERCENTAGE COMPOSITION Just like any percentage problems you are comparing the part to the whole. In chemistry, percentage composition is based on mass, not on numbers of atoms present. For Example, if

More information

Naming and Formula Writing

Naming and Formula Writing + Naming and Formula Writing + Chemical Formulas Shows the kind and number of atoms in the smallest piece of a substance Use subscripts to show the number of atoms per element Molecular formula- number

More information

You Try: Give the correct number of significant digits for the following: a cm b. 170 g c sec

You Try: Give the correct number of significant digits for the following: a cm b. 170 g c sec Mid-term Review- Chemistry Name January 2012 Kids Have Dropped Over Dead Converting Metrics Metric Conversions: Example: Convert 50.0 grams to kg You Try: If a building has a height of 20 600.5 mm, what

More information

Unit 2. Chapter 4-Atoms and Elements, continued

Unit 2. Chapter 4-Atoms and Elements, continued CHEMISTRY 110 LECTURE Unit 2 Chapter 4-Atoms and Elements, continued I Ions II ISOTOPES-Tools A. Tools 1. Atomic number, Z,, equals the number of protons 2. Mass number, A, equals the sum of protons and

More information

Section 1 Chemical Names and Formulas. Lesson Starter

Section 1 Chemical Names and Formulas. Lesson Starter Preview Lesson Starter Objectives Significance of a Chemical Formula Monatomic Ions Binary Ionic Compounds Writing the Formula of an Ionic Compound Naming Binary Ionic Compounds Naming Binary Molecular

More information

Chemistry 65 Chapter 6 THE MOLE CONCEPT

Chemistry 65 Chapter 6 THE MOLE CONCEPT THE MOLE CONCEPT Chemists find it more convenient to use mass relationships in the laboratory, while chemical reactions depend on the number of atoms present. In order to relate the mass and number of

More information

Mass Relationships in Chemical Reactions. Chapter 3 Chang & Goldsby Modified by Dr. Juliet Hahn

Mass Relationships in Chemical Reactions. Chapter 3 Chang & Goldsby Modified by Dr. Juliet Hahn Mass Relationships in Chemical Reactions Chapter 3 Chang & Goldsby Modified by Dr. Juliet Hahn Example 3.6 (3) We now write, 6.07 g CH 4 1 mol CH 4 16.04 g CH 4 = 0.378 mol CH 4 Thus, there is 0.378 mole

More information

The ions/polyatomic ions, solubility rules, and activity series will need to be memorized.

The ions/polyatomic ions, solubility rules, and activity series will need to be memorized. AP Chemistry Summer Assignment 2012 The summer assignment is designed to help you practice: - writing chemical formulas, names, and chemical equations - reaction types - predicting reaction products -

More information

1. Based on the information in Model 1 a. Identify three elements in the table that form only one type of cation.

1. Based on the information in Model 1 a. Identify three elements in the table that form only one type of cation. Honors Chemistry Ms. Ye Name Date Block Nomenclature Independent Unit Part 1 Definitions (some old, some new): Ion=an atom that has an unequal number of protons and electrons. o Cations are positively

More information

The chemical formulas of most of the elements are simply their elemental symbol:

The chemical formulas of most of the elements are simply their elemental symbol: Chemical Formulas A chemical formula gives the numbers and types of atoms that are found in a substance. When the substance is a discrete molecule, then the chemical formula is also its molecular formula.

More information

3) What is the correct value for Avogadro's number? 3) A) x 1033 B) x 1023 C) x D) x 1022

3) What is the correct value for Avogadro's number? 3) A) x 1033 B) x 1023 C) x D) x 1022 CHM1025 Exam 3 Chapters 6, 7, & 8 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) How many hydrogen atoms are in 35.0 grams of hydrogen gas? 1)

More information

Unit 6: Stoichiometry. How do manufacturers know how to make enough of their desired product?

Unit 6: Stoichiometry. How do manufacturers know how to make enough of their desired product? Unit 6: Stoichiometry How do manufacturers know how to make enough of their desired product? Chocolate Chip Cookies Using the following recipe, complete the questions. Cookie Recipe 1.5 c sugar 1 c. butter

More information

3. Most laboratory experiments are performed at room temperature at 65 C. Express this temperature in: a. F b. Kelvin

3. Most laboratory experiments are performed at room temperature at 65 C. Express this temperature in: a. F b. Kelvin Do all work on a separate sheet of paper so that you can show your work. Section A: Measurement and Math 1. Convert the following and show your work: a. 200 meters = miles. b. 650 in = meters c. 4 years=

More information

2. Relative molecular mass, M r - The relative molecular mass of a molecule is the average mass of the one molecule when compared with

2. Relative molecular mass, M r - The relative molecular mass of a molecule is the average mass of the one molecule when compared with Chapter 3: Chemical Formulae and Equations 1. Relative atomic mass, A r - The relative atomic mass of an element is the average mass of one atom of an element when compared with mass of an atom of carbon-12

More information

January Semester Exam Practice B This exam will be given over 2 days. Part 1: Objectives 1-13 Part 2: Objectives 14-24

January Semester Exam Practice B This exam will be given over 2 days. Part 1: Objectives 1-13 Part 2: Objectives 14-24 Name Hour January Semester Exam Practice B This exam will be given over 2 days. Part 1: Objectives 1-13 Part 2: Objectives 14-24 This practice exam will be graded in the exam portion of the grade book

More information

Name: Period: Score: Everything About Chemical Formulas

Name: Period: Score: Everything About Chemical Formulas Name: Period: Score: Everything About Formulas Compounds have unique names that identify them for us when we study chemical properties and changes. Chemists have devised a shorthand way of representing

More information

Unit 3 Chemical Quantities THE MOLE

Unit 3 Chemical Quantities THE MOLE Chemistry NAME Date Hour Unit 3 Chemical Quantities THE MOLE Practice Test Form C Second Half of Chapter 7 Objective 7 Use the mole to convert among measurements of mass, volume, and number of particles.

More information

Composion Stoichiometry

Composion Stoichiometry Composition Stoichiometry blank 3.3.13.notebook Due: Ch 10 RG Hummmm... How do you "measure" bananas? > How many? Count 1 dozen naners or 12 naners Composion Stoichiometry 3 new conversion factors > Avogadro's

More information

Average Atomic Mass. A new unit called the atomic mass unit (amu) was developed to deal with the very small units of mass for particles like the atom.

Average Atomic Mass. A new unit called the atomic mass unit (amu) was developed to deal with the very small units of mass for particles like the atom. Average Atomic Mass Since atoms are so small and the mass of individual atoms is also very small, it is not useful to use the units of grams or kilogram. A new unit called the atomic mass unit (amu) was

More information

3.1 Percent Composition

3.1 Percent Composition 3.1 Percent Composition The percentage composition of a compound refers to the relative mass of each element in a compound. The Law of Definite Proportions states that the elements in a given chemical

More information

The Mole Concept. It is easily converted to grams, no of particles or in the case of gas volume.

The Mole Concept. It is easily converted to grams, no of particles or in the case of gas volume. The Mole Concept The mole is a convenient unit A mole is the number of atoms present in exactly 12 g of the isotope carbon-12. In 12 g of carbon-12 there are 6.022 x 10 23 carbon atoms It is easily converted

More information

Chemists need a convenient method for counting accurately the number of atoms, molecules, or formula units in a sample of a substance.

Chemists need a convenient method for counting accurately the number of atoms, molecules, or formula units in a sample of a substance. I. Measuring Matter Chemists need a convenient method for counting accurately the number of atoms, molecules, or formula units in a sample of a substance. As you know, atoms and molecules are extremely

More information

Topic 7: The Mole Concept Relating Mass to Numbers of Atoms

Topic 7: The Mole Concept Relating Mass to Numbers of Atoms Topic 7: The Mole Concept Relating Mass to Numbers of Atoms (Chapter 3 in Modern Chemistry beginning on p.82) In order to understand the quantitative parts of chemistry, there are three very important

More information

1. Mole Definition & Background

1. Mole Definition & Background Unit 5: THE MOLE 1. Mole Definition & Background 2. Molar Mass 3. Mole Calculations 4. Percent Composition 5. Empirical Formulas 6. Molecular Formulas 1 1. Mole Definition & Background The mole was developed

More information

Warm-up. If aluminum cans weigh 20.g each, how many cans are in a 150 kg truckload of cans? (solve using conversion factors)

Warm-up. If aluminum cans weigh 20.g each, how many cans are in a 150 kg truckload of cans? (solve using conversion factors) Warm-up If aluminum cans weigh 20.g each, how many cans are in a 150 kg truckload of cans? (solve using conversion factors) 1 THE MOLE 2 Measuring Matter How do chemists determine amounts of chemicals

More information

AP Chemistry Unit 1 Review Guide: IUPAC Naming, Stoichiometry, Solution Chemistry

AP Chemistry Unit 1 Review Guide: IUPAC Naming, Stoichiometry, Solution Chemistry I. IUPAC Naming AP Chemistry Unit 1 Review Guide: IUPAC Naming, Stoichiometry, Solution Chemistry For Ionic Compounds: Formula to Name: 1. Identify the cation (positive ion) by name, then identify the

More information

Unit 9 The Mole Chapter 10 of your textbook

Unit 9 The Mole Chapter 10 of your textbook Unit 9 The Mole Chapter 10 of your textbook Learning Targets for Unit 9 Early Booklet E.C.: + 2 Unit 9.A Hwk. Pts.: / 36 Unit 9.A Lab Pts.: / 32 Late, Incomplete, No Work, No Units Fees? Y / N 1.1 I can

More information

Question 8 Chemical properties of metals and nonmetals. 1) magnesium 2) sulfur trioxide 3) iron (II) hydroxide 4) sodium nitrate

Question 8 Chemical properties of metals and nonmetals. 1) magnesium 2) sulfur trioxide 3) iron (II) hydroxide 4) sodium nitrate Question 8 Chemical properties of metals and nonmetals 1. Calcium oxide doesn t react with 1) NaNO 3 2) HCl 3) CO 2 4) H 2 O 2. Calcium oxide reacts with both of the following 1) SO 2 and O 2 2) H 2 O

More information

Nomenclature. Common Names. Common Names COMPOUNDS FORMED FROM IONS. Binary Ionic Compounds

Nomenclature. Common Names. Common Names COMPOUNDS FORMED FROM IONS. Binary Ionic Compounds PO 4 3- phosphate ion C 2 H 3 O 2 - acetate ion World of Chemistry: Chapter 4 Nomenclature HC 2 H 3 O 2 Acetic Acid Common Names Common Names A lot of chemicals have common lot of chemicals have common

More information

CRHS Academic Chemistry Unit 7 - Chemical Quantities. Notes. Key Dates

CRHS Academic Chemistry Unit 7 - Chemical Quantities. Notes. Key Dates Name Period CRHS Academic Chemistry Unit 7 - Chemical Quantities Notes Key Dates Quiz Date Exam Date Lab Dates Notes, Homework, Exam Reviews and Their KEYS located on CRHS Academic Chemistry Website: https://cincochem.pbworks.com

More information

Circle your lab section

Circle your lab section Homework 3 Circle your lab section Name TTh 8:00 MW 11:15 MW 2:30 Directions: Work out all problems on separate sheet(s) of paper and attach this page. To receive full credit you must show all work and

More information

1. How many moles of hydrogen are needed to completely react with 2.00 moles of nitrogen?

1. How many moles of hydrogen are needed to completely react with 2.00 moles of nitrogen? Stoichiometry Mole-to-Mole 1. How many moles of hydrogen are needed to completely react with 2.00 moles of nitrogen? N 2 + H 2 NH 3 2. If 5.50 moles of calcium carbide (CaC 2 ) reacts with an excess of

More information

Chemical reactions: Chemical reactions change substances into other substances.

Chemical reactions: Chemical reactions change substances into other substances. Chemical reactions: Chemical reactions change substances into other substances. A chemical equation is used to represent a reaction. This has the form: reactants à products Word equations use the names

More information

Measuring matter 11.1

Measuring matter 11.1 The Mole Ch 11 Measuring matter 11.1 Review 11.1 Vocabulary o molecule: two or more atoms that covalently bond together to form a unit New mole Avogadro s number Main Idea - Chemists use the mole to count

More information

THE MOLE. Avogadro s Number 1 mole = x items **items = atoms/molecules/particles etc The abbreviation for the unit mole is.

THE MOLE. Avogadro s Number 1 mole = x items **items = atoms/molecules/particles etc The abbreviation for the unit mole is. Chemistry 11 Mole III Name: Date: Block: 1. Relative Atomic Mass 2. The Mole 3. Molar Mass Relative Atomic Mass Mass: The amount of in an object. Atomic Mass: The mass of a particular atom. The atomic

More information

NOTES PACKET COLLIER CHEMISTRY PRE-AP

NOTES PACKET COLLIER CHEMISTRY PRE-AP SECOND NINE WEEKS NOTES PACKET COLLIER CHEMISTRY PRE-AP 1 2 UNIT 5 CHEMICAL NAMING & BALANCING Chapter 6, 15.1, 16.1 3 NOMENCLATURE: Atoms of elements combine to form that are represented by. All compounds

More information

SCH4U Chemistry Review: Fundamentals

SCH4U Chemistry Review: Fundamentals SCH4U Chemistry Review: Fundamentals Particle Theory of Matter Matter is anything that has mass and takes up space. Anything around us and in the entire universe can be classified as either matter or energy.

More information

INSTRUCTIONS ON EVERY AP EXAM:

INSTRUCTIONS ON EVERY AP EXAM: Most Common Reaction Types: 1. Acid-base neutralization (both weak & strong) 2. Nonmetal and metal oxides with water 3. Active metals with water 4. Single replacement redox 5. Double replacement precipitation

More information

This is a guide for your test #1.

This is a guide for your test #1. This is a guide for your test #1. 1) Lead melts at 601.0 C. What temperature is this in F? A. 302 F B. 365 F C. 1,050 F D. 1,082 F E. 1,114 F 2) Ammonia boils at -33.4 C. What temperature is this in F?

More information

MIDTERM REVIEW. UNIT 1: Mass/Measurement

MIDTERM REVIEW. UNIT 1: Mass/Measurement MIDTERM REVIEW UNIT 1: Mass/Measurement Practice Problems 1. Circle the word/phrase that best fits the statement: A. [ PHYSICAL OR CHEMICAL] changes are changes in which the identity of the substance does

More information

a) AlN or CaO AlN The ions involved are 3+/3-, while those involved in CaO are 2+/2-.

a) AlN or CaO AlN The ions involved are 3+/3-, while those involved in CaO are 2+/2-. SOLUTIONS - CHAPTER 5 Problems 1) Write Lewis dot symbols for the following atoms: a) Ca b) Se c) B d) Cl e) He 2) Write Lewis dot symbols for the following ions: a) Li + b) Cl - c) S 2- d) Sr 2+ e) N

More information

Notes on Mole 12.notebook. October 25, CaS. Ca + S. Oct 14 6:22 PM. Oct 14 6:23 PM. Oct 14 6:24 PM. Oct 14 6:23 PM MOLE.

Notes on Mole 12.notebook. October 25, CaS. Ca + S. Oct 14 6:22 PM. Oct 14 6:23 PM. Oct 14 6:24 PM. Oct 14 6:23 PM MOLE. How do chemists count atoms/formula units/molecules? How do we go from the atomic scale to the scale of everyday measurements (macroscopic scale)? The gateway is the mole! But before we get to the mole,

More information

1. Mole Definition & Background

1. Mole Definition & Background Unit 5: THE MOLE 1. Mole Definition & Background 2. Molar Mass 3. Mole Calculations 4. Percent Composition 5. Empirical Formulas 6. Molecular Formulas 1 1. Mole Definition & Background The mole was developed

More information

It s just like finding out your test score!!!

It s just like finding out your test score!!! It s just like finding out your test score!!! 97 correct out of 100 questions = 97 x 100 = 97% 100 Total of something x 100 = % TOTAL The chemical composition can be expressed as the mass percent of each

More information

9/19/07. Chemistry 6A Fall 2007 Dr. J. A. Mack. Molar Masses. Avagagro s s Number. Avogadro s Number and the Mole

9/19/07. Chemistry 6A Fall 2007 Dr. J. A. Mack. Molar Masses. Avagagro s s Number. Avogadro s Number and the Mole Chemistry 6A Fall 007 Dr. J. A. Mack Avogadro s Number and the Mole The concept of a mole is defined so that we may equate the amount of matter (mass) to the number of particles (mole). The Standard is

More information

Chem Chapter 2.notebook October 17, 2012

Chem Chapter 2.notebook October 17, 2012 Unit 1: Stoichiometry 1 Chapter 2: The Mole Atomic number the number of protons in an atom or ion Mass number the sum of the protons and neutrons in an atom 2 Isotope atoms which have the same number of

More information

CHAPTER 2 CHEMICAL FORMULAS & COMPOSITION STOICHIOMETRY

CHAPTER 2 CHEMICAL FORMULAS & COMPOSITION STOICHIOMETRY CHAPTER 2 CHEMICAL FORMULAS & COMPOSITION STOICHIOMETRY 1 One drop of water is about 0.05g or 0.05 ml One drop of water contains about 1.67 x 10 21 H 2 O molecules 167,000,000,000,000,000,000 H 2 O molecules

More information