Chemistry I Accelerated Study Guideline - Chapter Ten The Mole

Save this PDF as:
 WORD  PNG  TXT  JPG

Size: px
Start display at page:

Download "Chemistry I Accelerated Study Guideline - Chapter Ten The Mole"

Transcription

1 Chemistry I Accelerated Study Guideline - Chapter Ten The Mole By the end of this chapter the skills you should be able to demonstrate are: 1. Name the basic SI unit for measuring the amount of a substance. 2. Distinguish between the terms gram atomic mass, gram molecular mass, and gram formula mass. 3. Define the relationship between the gram formula mass and the molar mass of a substance. 4. Explain the centrality of the mole to chemical calculations. 5. Convert using the mole between mass, number of particles, molarity and volumes of gas at STP. 6. Calculate the percent composition of a substance from its chemical formula or experimental data. 7. Derive the empirical formula of a compound from experimental data. 8. Derive the molecular formula of a compound from experimental data. 9. Determine the formulas of hydrates. Suggested Problems: p #76, 77, 80, 81, 83, 87, 88, 89, 90, 92, 93

2 Video Worksheet: The Mole Please Answer the following questions while you watch the video 1. What is the most basic kind of matter? 2. What is the motto of the same number trucking company? 3. What type of substance behaves as if its particles do not touch? 4. What are conditions must exist in order so a container can hold the same number of gas particles? 5. What does the Law of Combining Volumes state? 6. What is Avogadro s hypothesis? 7. What did Avogadro say about gas particles? 8. What is Relative Molecular Mass? 9. For many years, what served as the standard for relative molecular mass? 10. What is the modern machine that can determine the relative atomic mass of elements? 11. What is an isotope of an atom? 12. What is the standard today for relative atomic mass? 13. What is the volume of a mole of gas particles at standard temperature and pressure? 14. What is Avogadro s number in scientific notation? page 2

3 Basic Mole Problems Calculate the number of moles in each of these X atoms of lithium 6.02 X atoms Li X 1 mole Li = 1.00 mole Li 6.02 X atoms Li X molecules of nitrogen X molecules N 2 X 1 mole N 2 = moles N X molecules N X molecules of hydrogen peroxide X 10 5 formula units of potassium chloride X molecules of beryllium oxide X molecules of aluminum phosphide X molecules of carbon dioxide X molecules of Lead(II) iodide X molecules of bromine molecules of methane Calculate the number of atoms in each of these mole of gold 1.00 mole Au X 6.02 X atoms Au = 6.02 X atoms Au 1 mole Au moles of lead page 3

4 moles of ethanol moles of sodium bromide moles of zinc chloride moles of potassium nitrate moles of sodium phosphate mole of Tin(IV) fluoride moles of oxygen moles of carbon dioxide Calculate the molar mass of each of these 1. Silver chloride 2. Sodium hydroxide 3. Propane 4. Octane 5. Benzene 6. Copper(II) sulfate 7. methylamine (CH 3 NH 2 ) 8. Ethandiol (C 2 H 6 O 2 ) 9. Chloroform (CHCl 3 ) 10. Tribromosilane (SiHBr 3 ) 11. Sulfurous Acid 12. Ammonium phosphide page 4

5 Calculate the number of grams in each of these mole of Boron 1.00 mole B X 10.8 g B = 10.8 g B 1 mole B moles of Copper 2.00 mole Cu X 63.5 g Cu = 127 g Cu 1 mole Cu moles of Neon moles of Sodium Fluoride mole of glucose moles of nitrogen moles of magnesium oxide moles of calcium chloride moles of aluminum sulfide moles of water Calculate the number of moles in each of these g of carbon 12.0 g C X 1 mole C = 1.00 mole C 12 g C g of lithium oxide g of magnesium sulfide 89.4 g Li 2 O X 1 mole Li 2 O = 3.00 moles Li 2 O 29.8 g Li 2 O page 5

6 g of potassium phosphide g of sulfur dioxide g of calcium fluoride g of copper(ii) bromide g of diboron trioxide g of aluminum flouride g of sodium chloride Convert each of these to moles x molecules of carbon dioxide x molecules of chlorine x molecules of water molecules of tetraphosphorus decoxide molecule of ammonia grams of ammonia grams of calcium carbonate grams of water 8. page 6

7 grams of sulfuric acid gram of sodium chloride grams of lead(ii) sulfate grams of pentane grams of C 4 H 8 O grams of potassium permanganate x formula units of barium nitrate x formula units of magnesium bromide x molecules of ethane 17. Convert each of these to mass in grams moles of ammonia moles of sodium chloride moles of hydrochloric acid moles of sodium sulfate x 10 4 moles of silver chloride moles of calcium chloride moles of hydrofluoric acid 24. page 7

8 moles of silicon dioxide moles of nitrogen 26. Convert each of these to numbers of atoms moles of sulfur moles of silver moles of carbon dioxide moles of phosphorous trichloride moles of ammonia moles of sulfur dioxide x 10 3 moles of carbon monoxide moles of selenium moles of oxygen moles of silver nitrate moles of sodium fluoride 37. One step volume problems 38. How many moles are in 893 L of air at STP? What is the volume of moles of nitrogen gas at STP? How many moles of oxygen gas are in 694 L at STP? 40. page 8

9 41. What is the volume of 13.8 moles of carbon monoxide gas at STP? How many moles of neon gas are in 3.68 L at STP? What is the volume of moles of hydrosulfuric acid gas at STP? How many moles of argon gas are in 101 L at STP? What is the volume of 138 moles of hydrobromic acid gas at STP? 45. Two step mole problems 46. How many formula units are in 3.5 grams of sodium hydroxide? How many grams are in 6.10 x molecules of ethane? How many formula units are in 5.1 grams of titanium(iv) oxide? What is the mass of 3.62 x molecules of methanol? How many formula units are in 1.47 grams of lead(ii) chloride? What is the mass of 2.94 x molecules of decane? 51. page 9

10 52. How many formula units are in 5.62 grams of hydrosulfuric acid? How many atoms are in a tank that has 5.00 mol of nitrogen dioxide gas? How many formula units are in 3.00 grams of sodium chloride? How many molecules are in 30.6 grams of butanol? How many atoms are in L of helium at STP? If 12.1 grams of dry ice (carbon dioxide) are converted into gas at STP, what volume would it fill? 57. Molarity 1. What mass of potassium phosphate is needed to prepare 4.00 liters of 1.50 M solution? What mass of 2-pentanol is needed to prepare 1.50 liters of 3.00 M solution? 2. page 10

11 3. What volume in µl of 1.40 M acetic acid solution can be prepared using moles of acetic acid? What is the molarity of a solution that contains 85.0 grams of sodium sulfate in 325 ml of solution? What is the molarity of a solution that contains 215 grams of aluminum sulfate in 2.75 cubic decimeters of solution? What volume in µl of M solution can be prepared using 18.5 grams of sodium hydroxide? What is the molarity of a solution that contains 125 grams of ethanol in cubic decimeters of solution? What volume of M solution can be prepared using 90.0 grams of ammonium chloride? What is the molarity of a solution that contains 145 grams of sodium chloride in 275 ml of solution? How many grams of potassium chloride are needed to prepare L of a 1.50 M solution? 10. page 11

12 11. What is the molarity of a solution that contains 85.6 grams of hydrochloric acid in dm 3 of solution? How many grams of sodium hydroxide are needed to prepare 3.00 dm 3 of a 1.90 M solution? What is the molarity of a solution that contains 8.77 grams of potassium iodide in 4.75 dm 3 of solution? How many grams of iron(iii) chloride are needed to prepare 2.00 L of a 3.00 M solution? What is the molarity of a solution that contains 14.1 grams of ammonia in dm 3 of solution? How many grams of potassium hydroxide are needed to prepare 10.5 L of a 2.50 M solution? 16. page 12

13 Percent composition 1. Find the percent composition of a compound that contains 1.94 g of carbon, g of hydrogen and 2.58 g of sulfur in a 5.00-g sample of the compound 2. A sample of an unknown compound with a mass of g has percent fluorine and percent iron. If the compound is decomposed, how much of each element will be recovered? 3. Find the percent composition of a compound that contains 2.63 g of carbon, g of hydrogen and g of oxygen. 4. A sample of an unknown compound with a mass of g has percent carbon, 6.71 percent hydrogen, 4.06 percent nitrogen and percent oxygen. What is the mass of each element in this compound? 5. Find the percent composition of a compound that contains g of chlorine, g of oxygen and g of phosphorus. 6. Find the percent composition of a compound that contains 1.51 g of chromium, 1.13 g of potassium and 1.62 g of oxygen. 7. A sample of a compound with a mass of g is analyzed. The sample is found to contain only fluorine and oxygen. If the compound contains g oxygen, calculate the percent composition of the compound. page 13

14 Empirical Formulas 1. Determine the empirical formula of a compound containing g of gold and g chlorine. 2. Determine the empirical formula of a compound containing g of gallium and g phosphorus. 3. Determine the empirical formula of a compound containing 47.9% zinc and 52.1% chlorine by mass. 4. Determine the empirical formula of a compound containing 1.75 g of carbon and g bromine. 5. Determine the empirical formula of a compound containing 20.23% aluminum and 79.77% chlorine by mass. page 14

15 6. Determine the empirical formula of a compound containing g of carbon and g oxygen. 7. Determine the empirical formula of a compound containing g of calcium and g chlorine. 8. Determine the empirical formula of a compound containing g of carbon, g of hydrogen and g oxygen. 9. Determine the empirical formula of a compound containing 24.74% potassium, 34.76% manganese and 40.50% oxygen by mass. 10. Determine the empirical formula of a compound containing 2.16 g of aluminum, 3.85 g of sulfur and 7.68 g oxygen. page 15

16 Molecular Formulas 1. Determine the molecular formula of a compound containing g of palladium and 0.80 g of hydrogen. The molar mass of the compound is g/mol. 2. Determine the molecular formula of a compound that is 30.45% nitrogen and 69.55% oxygen. The molar mass of the compound is 92 g/mol. 3. Determine the molecular formula of a compound containing 42.4 g of hydrogen and g of carbon. The molar mass of the compound is 30.0 g/mol. page 16

17 4. Determine the molecular formula of a compound containing only boron and iodine if in a g sample, the mass of the iodine is found to be g. The molar mass of the compound is g/mol. 5. Determine the molecular formula of a compound containing g of oxygen and g of phosphorus. The molar mass of the compound is g/mol. page 17

18 Hydrates 1. Find the empirical formula of the hydrate given that it is 27.76% manganese, 35.83% chlorine and 36.40% water. 2. Two hydrates of cobalt(ii) chloride exist. One is 21.68% water the other is 45.43% water. What are their empirical formulas? page 18

19 Challenge Problems The Mole 1. How many molecules are in a sample of water that requires 8.40 kcal of heat energy to raise the temperature by 34.0 C? 2. A compound of hydrogen and carbon has a molar mass 114 g/mol. If one mole of the compound contains g of hydrogen, what is the compound s molecular formula? 3. How many atoms of iron are in a cube of iron that is 1.00 x 10 5 µm on a side? Use a reference source to find the density of iron. page 19

20 4. A mixture of salt and pepper analyses to be 50% chlorine by mass. If pepper contains no chlorine, what percent of the mixture is pepper? 5. A solution is made that is 2.00 M for aluminum nitrate. What volume of this solution contains moles of nitrate ions? page 20

21 6. A solution of ammonium sulfate is made that is 2.25 M for ammonium ions. What volume of this solution can be produced using only 50.0 g of ammonium sulfate? 7. A sample of hydrated sodium salt gives off 2.02 x molec. of water when it is heated. When the dehydrated sample is analyzed it is found to contain g sodium, g phosphorus, L hydrogen gas and 1.25 L of oxygen gas at STP. Calculate the empirical formula of the hydrate. page 21

22 Mole Word Scramble Use the clues provided to help you unscramble the letter to form words related to the mole. The letters in the circle spell out, in order, the name of a famous chemist. CLUES 1. 1/12 of a Carbon-12 atom 2. Mass of one object compared to that of another object x of anything 4. Method for solving a problem 5. Found by adding the atomic masses of all the elements in the molecule 6. Means that there are two atoms in a molecule 7. Formula representing the smallest whole-number ratio of atoms in a compound 8. Number of moles of dissolved substance per liter of solution 1. S A N I O M S M T T U A C I 2. V E T S A M S I R E L A 3. L O E M 4. M A H L T G I O R 5. R A L S U C E S A M L O M 6. T A D I M O C I 7. I M P E C I L A R 8. R I L Y T A O M NAME: page 22

Unit 3 Notepack Chapter 7 Chemical Quantities Qualifier for Test

Unit 3 Notepack Chapter 7 Chemical Quantities Qualifier for Test Unit 3 Notepack Chapter 7 Chemical Quantities Qualifier for Test NAME Section 7.1 The Mole: A Measurement of Matter A. What is a mole? 1. Chemistry is a quantitative science. What does this term mean?

More information

MOLES AND MOLE CALCULATIONS

MOLES AND MOLE CALCULATIONS 35 MOLES ND MOLE CLCULTIONS INTRODUCTION The purpose of this section is to present some methods for calculating both how much of each reactant is used in a chemical reaction, and how much of each product

More information

Moles, Molecules, and Grams Worksheet Answer Key

Moles, Molecules, and Grams Worksheet Answer Key Moles, Molecules, and Grams Worksheet Answer Key 1) How many are there in 24 grams of FeF 3? 1.28 x 10 23 2) How many are there in 450 grams of Na 2 SO 4? 1.91 x 10 24 3) How many grams are there in 2.3

More information

Unit 9 Stoichiometry Notes (The Mole Continues)

Unit 9 Stoichiometry Notes (The Mole Continues) Unit 9 Stoichiometry Notes (The Mole Continues) is a big word for a process that chemist s use to calculate amounts in reactions. It makes use of the coefficient ratio set up by balanced reaction equations

More information

Programme in mole calculation

Programme in mole calculation Programme in mole calculation Step 1 Start at the very beginning Atoms are very small indeed! If we draw a line 1 metre long, 6,000,000,000 (6 billion) atoms could be lined end to end. So a scientist cannot

More information

Solution. Practice Exercise. Concept Exercise

Solution. Practice Exercise. Concept Exercise Example Exercise 9.1 Atomic Mass and Avogadro s Number Refer to the atomic masses in the periodic table inside the front cover of this textbook. State the mass of Avogadro s number of atoms for each of

More information

Study Guide For Chapter 7

Study Guide For Chapter 7 Name: Class: Date: ID: A Study Guide For Chapter 7 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. The number of atoms in a mole of any pure substance

More information

MOLECULAR MASS AND FORMULA MASS

MOLECULAR MASS AND FORMULA MASS 1 MOLECULAR MASS AND FORMULA MASS Molecular mass = sum of the atomic weights of all atoms in the molecule. Formula mass = sum of the atomic weights of all atoms in the formula unit. 2 MOLECULAR MASS AND

More information

Problem Solving. Mole Concept

Problem Solving. Mole Concept Skills Worksheet Problem Solving Mole Concept Suppose you want to carry out a reaction that requires combining one atom of iron with one atom of sulfur. How much iron should you use? How much sulfur? When

More information

Molar Mass Worksheet Answer Key

Molar Mass Worksheet Answer Key Molar Mass Worksheet Answer Key Calculate the molar masses of the following chemicals: 1) Cl 2 71 g/mol 2) KOH 56.1 g/mol 3) BeCl 2 80 g/mol 4) FeCl 3 162.3 g/mol 5) BF 3 67.8 g/mol 6) CCl 2 F 2 121 g/mol

More information

Practice questions for Chapter 8

Practice questions for Chapter 8 Practice questions for Chapter 8 2) How many atoms of nickel equal a mass of 58.69 g? (Refer to the Periodic Table.) A) 1 B) 28 C) 58.69 D) 59 E) 6.02 x 1023 Answer: E Section: 8.1 Avogadro's Number 6)

More information

SCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGraw-Hill Ryerson, 2001

SCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, Chemistry 11, McGraw-Hill Ryerson, 2001 SCH 4C1 Unit 2 Problem Set Questions taken from Frank Mustoe et all, "Chemistry 11", McGraw-Hill Ryerson, 2001 1. A small pin contains 0.0178 mol of iron. How many atoms of iron are in the pin? 2. A sample

More information

W1 WORKSHOP ON STOICHIOMETRY

W1 WORKSHOP ON STOICHIOMETRY INTRODUCTION W1 WORKSHOP ON STOICHIOMETRY These notes and exercises are designed to introduce you to the basic concepts required to understand a chemical formula or equation. Relative atomic masses of

More information

HOMEWORK 4A. Definitions. Oxidation-Reduction Reactions. Questions

HOMEWORK 4A. Definitions. Oxidation-Reduction Reactions. Questions HOMEWORK 4A Oxidation-Reduction Reactions 1. Indicate whether a reaction will occur or not in each of following. Wtiring a balcnced equation is not necessary. (a) Magnesium metal is added to hydrochloric

More information

Unit 10A Stoichiometry Notes

Unit 10A Stoichiometry Notes Unit 10A Stoichiometry Notes Stoichiometry is a big word for a process that chemist s use to calculate amounts in reactions. It makes use of the coefficient ratio set up by balanced reaction equations

More information

Chemical Composition Review Mole Calculations Percent Composition. Copyright Cengage Learning. All rights reserved. 8 1

Chemical Composition Review Mole Calculations Percent Composition. Copyright Cengage Learning. All rights reserved. 8 1 Chemical Composition Review Mole Calculations Percent Composition Copyright Cengage Learning. All rights reserved. 8 1 QUESTION Suppose you work in a hardware store and a customer wants to purchase 500

More information

Chapter 3. Stoichiometry: Ratios of Combination. Insert picture from First page of chapter. Copyright McGraw-Hill 2009 1

Chapter 3. Stoichiometry: Ratios of Combination. Insert picture from First page of chapter. Copyright McGraw-Hill 2009 1 Chapter 3 Insert picture from First page of chapter Stoichiometry: Ratios of Combination Copyright McGraw-Hill 2009 1 3.1 Molecular and Formula Masses Molecular mass - (molecular weight) The mass in amu

More information

Mole Notes.notebook. October 29, 2014

Mole Notes.notebook. October 29, 2014 1 2 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

More information

Diagnostic/Introductory Activity. Word Search

Diagnostic/Introductory Activity. Word Search Diagnostic/Introductory Activity Find any 10 of the first 20 elements. Word Search Q H Z S B N Q J B C N P K M A A M M O O A O E C H E H H U A T L R U X D R E V L G O N I D I O U E I Y I Z N O O S M L

More information

Mole Calculations Multiple Choice Review PSI Chemistry

Mole Calculations Multiple Choice Review PSI Chemistry Mole Calculations Multiple Choice Review PSI Chemistry Name The Mole and Avogadro's Number 1)What is the SI unit for measurement of number of particles in a substance? A) kilogram B) ampere C) candela

More information

Description of the Mole Concept:

Description of the Mole Concept: Description of the Mole Concept: Suppose you were sent into the store to buy 36 eggs. When you picked them up you would get 3 boxes, each containing 12 eggs. You just used a mathematical device, called

More information

IB Chemistry. DP Chemistry Review

IB Chemistry. DP Chemistry Review DP Chemistry Review Topic 1: Quantitative chemistry 1.1 The mole concept and Avogadro s constant Assessment statement Apply the mole concept to substances. Determine the number of particles and the amount

More information

The Mole. Chapter 2. Solutions for Practice Problems

The Mole. Chapter 2. Solutions for Practice Problems Chapter 2 The Mole Note to teacher: You will notice that there are two different formats for the Sample Problems in the student textbook. Where appropriate, the Sample Problem contains the full set of

More information

Formulae, stoichiometry and the mole concept

Formulae, stoichiometry and the mole concept 3 Formulae, stoichiometry and the mole concept Content 3.1 Symbols, Formulae and Chemical equations 3.2 Concept of Relative Mass 3.3 Mole Concept and Stoichiometry Learning Outcomes Candidates should be

More information

Formulae, Equations & Formula Mass

Formulae, Equations & Formula Mass St Peter the Apostle High School Chemistry Department Formulae, Equations & Formula Mass N4 & N5 Homework Questions Answer questions as directed by your teacher. National 4 level questions are first followed

More information

MOLE CONVERSION PROBLEMS. 2. How many moles are present in 34 grams of Cu(OH) 2? [0.35 moles]

MOLE CONVERSION PROBLEMS. 2. How many moles are present in 34 grams of Cu(OH) 2? [0.35 moles] MOLE CONVERSION PROBLEMS 1. What is the molar mass of MgO? [40.31 g/mol] 2. How many moles are present in 34 grams of Cu(OH) 2? [0.35 moles] 3. How many moles are present in 2.5 x 10 23 molecules of CH

More information

9. The molar mass of hydrazine is 32 g/mol and its empirical formula is NH 2. What is its molecular formula?

9. The molar mass of hydrazine is 32 g/mol and its empirical formula is NH 2. What is its molecular formula? Dr. Rogers Solutions Homework 1. Give the name for the following compounds and state whether they are ionic or not A. Ba(NO 3 ) 2 B. NaH C. PCl 5 D. CO E. NH 4 OH F. Ca(MnO 4 ) 2 G. N 2 O 4 H. NaHSO 4

More information

WRITE IN THE CORRECT FORMULA THEN BALANCE THE CHEMICAL EQUATIONS

WRITE IN THE CORRECT FORMULA THEN BALANCE THE CHEMICAL EQUATIONS WRITE IN THE CORRECT FORMULA THEN BALANCE THE CHEMICAL EQUATIONS 1. Hydrogen Oxygen Water METALLIC OXIDE WATER BASE 2. Sodium oxide Water Sodium hydroxide 3. Calcium oxide Water Calcium hydroxide 4. Potassium

More information

Chapter 1: Moles and equations. Learning outcomes. you should be able to:

Chapter 1: Moles and equations. Learning outcomes. you should be able to: Chapter 1: Moles and equations 1 Learning outcomes you should be able to: define and use the terms: relative atomic mass, isotopic mass and formula mass based on the 12 C scale perform calculations, including

More information

CHEMICAL REACTIONS AND REACTING MASSES AND VOLUMES

CHEMICAL REACTIONS AND REACTING MASSES AND VOLUMES CHEMICAL REACTIONS AND REACTING MASSES AND VOLUMES The meaning of stoichiometric coefficients: 2 H 2 (g) + O 2 (g) 2 H 2 O(l) number of reacting particles 2 molecules of hydrogen react with 1 molecule

More information

Unit 7A - The Mole. We Need to Count atoms. The Mole and Molar Mass

Unit 7A - The Mole. We Need to Count atoms. The Mole and Molar Mass Unit 7A - The Mole The Mole and Molar Mass We Need to Count atoms Airbags are inflated by a chemical reaction: electrical 2 NaN 3 (s) 3 N 2 (g) + 2 Na(s) decomposition Each airbag needs the right amount

More information

Chapter 3 Mass Relationships in Chemical Reactions

Chapter 3 Mass Relationships in Chemical Reactions Chapter 3 Mass Relationships in Chemical Reactions Student: 1. An atom of bromine has a mass about four times greater than that of an atom of neon. Which choice makes the correct comparison of the relative

More information

Problem Solving. Percentage Composition

Problem Solving. Percentage Composition Skills Worksheet Problem Solving Percentage Composition Suppose you are working in an industrial laboratory. Your supervisor gives you a bottle containing a white crystalline compound and asks you to determine

More information

602X10 21 602,000,000,000, 000,000,000,000 6.02X10 23. Pre- AP Chemistry Chemical Quan44es: The Mole. Diatomic Elements

602X10 21 602,000,000,000, 000,000,000,000 6.02X10 23. Pre- AP Chemistry Chemical Quan44es: The Mole. Diatomic Elements Pre- AP Chemistry Chemical Quan44es: The Mole Mole SI unit of measurement that measures the amount of substance. A substance exists as representa9ve par9cles. Representa9ve par9cles can be atoms, molecules,

More information

CHAPTER 3 COMPOUNDS AND MOLECULES

CHAPTER 3 COMPOUNDS AND MOLECULES Chapter 3 Compounds and Molecules Page 1 CHAPTER 3 COMPOUNDS AND MOLECULES 3-1. Octane, a component of gasoline, has eight carbon atoms and eighteen hydrogen atoms per molecule. Its formula is written

More information

10.3 Percent Composition and Chemical Formulas. Chapter 10 Chemical Quantities Percent Composition and Chemical Formulas

10.3 Percent Composition and Chemical Formulas. Chapter 10 Chemical Quantities Percent Composition and Chemical Formulas Chapter 10 Chemical Quantities 101 The Mole: A Measurement of Matter 102 Mole-Mass and Mole-Volume Relationships 103 Percent Composition and Chemical Formulas 1 CHEMISTRY & YOU What does the percent composition

More information

Ch. 10 The Mole I. Molar Conversions

Ch. 10 The Mole I. Molar Conversions Ch. 10 The Mole I. Molar Conversions I II III IV A. What is the Mole? A counting number (like a dozen) Avogadro s number (N A ) 1 mole = 6.022 10 23 representative particles B. Mole/Particle Conversions

More information

CHEMICAL NAMES AND FORMULAS

CHEMICAL NAMES AND FORMULAS 9 CHEMICAL NAMES AND FORMULAS SECTION 9.1 NAMING IONS (pages 253 258) This section explains the use of the periodic table to determine the charge of an ion. It also defines polyatomic ion and gives the

More information

Chemistry Post-Enrolment Worksheet

Chemistry Post-Enrolment Worksheet Name: Chemistry Post-Enrolment Worksheet The purpose of this worksheet is to get you to recap some of the fundamental concepts that you studied at GCSE and introduce some of the concepts that will be part

More information

0.786 mol carbon dioxide to grams g lithium carbonate to mol

0.786 mol carbon dioxide to grams g lithium carbonate to mol 1 2 Convert: 2.54 x 10 22 atoms of Cr to mol 4.32 mol NaCl to grams 0.786 mol carbon dioxide to grams 2.67 g lithium carbonate to mol 1.000 atom of C 12 to grams 3 Convert: 2.54 x 10 22 atoms of Cr to

More information

Other Stoich Calculations A. mole mass (mass mole) calculations. GIVEN mol A x CE mol B. PT g A CE mol A MOLE MASS :

Other Stoich Calculations A. mole mass (mass mole) calculations. GIVEN mol A x CE mol B. PT g A CE mol A MOLE MASS : Chem. I Notes Ch. 12, part 2 Using Moles NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. 1 MOLE = 6.02 x 10 23 representative particles (representative particles

More information

neutrons are present?

neutrons are present? AP Chem Summer Assignment Worksheet #1 Atomic Structure 1. a) For the ion 39 K +, state how many electrons, how many protons, and how many 19 neutrons are present? b) Which of these particles has the smallest

More information

How much does a single atom weigh? Different elements weigh different amounts related to what makes them unique.

How much does a single atom weigh? Different elements weigh different amounts related to what makes them unique. How much does a single atom weigh? Different elements weigh different amounts related to what makes them unique. What units do we use to define the weight of an atom? amu units of atomic weight. (atomic

More information

Name Date Class CHEMICAL QUANTITIES. SECTION 10.1 THE MOLE: A MEASUREMENT OF MATTER (pages 287 296)

Name Date Class CHEMICAL QUANTITIES. SECTION 10.1 THE MOLE: A MEASUREMENT OF MATTER (pages 287 296) Name Date Class 10 CHEMICAL QUANTITIES SECTION 10.1 THE MOLE: A MEASUREMENT OF MATTER (pages 287 296) This section defines the mole and explains how the mole is used to measure matter. It also teaches

More information

Summer Assignment Coversheet

Summer Assignment Coversheet Summer Assignment Coversheet Course: A.P. Chemistry Teachers Names: Mary Engels Assignment Title: Summer Assignment A Review Assignment Summary/Purpose: To review the Rules for Solubility, Oxidation Numbers,

More information

Test 3 Formula and math of formula review. 2. The oxide of metal X has the formula XO. Which group in the Periodic Table contains metal X?

Test 3 Formula and math of formula review. 2. The oxide of metal X has the formula XO. Which group in the Periodic Table contains metal X? Name: Sunday, November 04, 2007 Test 3 Formula and math of formula review 1. Which is an example of a binary compound? 1. acetic acid 3. potassium hydroxide 2. nitric acid 4. potassium oxide 2. The oxide

More information

Useful only for measuring the mass of very small objects atoms and molecules!

Useful only for measuring the mass of very small objects atoms and molecules! Chapter 9 Chemical Composition (Moles) Which weighs more, 1 atom of He or 1 atom of O? Units of mass: Pound Kilogram Atomic mass unit (AMU) There are others! 1 amu = 1.66 x 10-24 grams = mass of a proton

More information

TOPIC 7. CHEMICAL CALCULATIONS I - atomic and formula weights.

TOPIC 7. CHEMICAL CALCULATIONS I - atomic and formula weights. TOPIC 7. CHEMICAL CALCULATIONS I - atomic and formula weights. Atomic structure revisited. In Topic 2, atoms were described as ranging from the simplest atom, H, containing a single proton and usually

More information

IB Chemistry 1 Mole. One atom of C-12 has a mass of 12 amu. One mole of C-12 has a mass of 12 g. Grams we can use more easily.

IB Chemistry 1 Mole. One atom of C-12 has a mass of 12 amu. One mole of C-12 has a mass of 12 g. Grams we can use more easily. The Mole Atomic mass units and atoms are not convenient units to work with. The concept of the mole was invented. This was the number of atoms of carbon-12 that were needed to make 12 g of carbon. 1 mole

More information

Unit 2: Quantities in Chemistry

Unit 2: Quantities in Chemistry Mass, Moles, & Molar Mass Relative quantities of isotopes in a natural occurring element (%) E.g. Carbon has 2 isotopes C-12 and C-13. Of Carbon s two isotopes, there is 98.9% C-12 and 11.1% C-13. Find

More information

Chemical Calculations: The Mole Concept and Chemical Formulas. AW Atomic weight (mass of the atom of an element) was determined by relative weights.

Chemical Calculations: The Mole Concept and Chemical Formulas. AW Atomic weight (mass of the atom of an element) was determined by relative weights. 1 Introduction to Chemistry Atomic Weights (Definitions) Chemical Calculations: The Mole Concept and Chemical Formulas AW Atomic weight (mass of the atom of an element) was determined by relative weights.

More information

Exercise 3.5 - Naming Binary Covalent Compounds:

Exercise 3.5 - Naming Binary Covalent Compounds: Chapter Exercise Key 1 Chapter Exercise Key Exercise.1 Classifying Compounds: Classify each of the following substances as either a molecular compound or an ionic compound. a. formaldehyde, CH 2 O (used

More information

CHAPTER 8: CHEMICAL COMPOSITION

CHAPTER 8: CHEMICAL COMPOSITION CHAPTER 8: CHEMICAL COMPOSITION Active Learning: 1-4, 6-8, 12, 18-25; End-of-Chapter Problems: 3-4, 9-82, 84-85, 87-92, 94-104, 107-109, 111, 113, 119, 125-126 8.2 ATOMIC MASSES: COUNTING ATOMS BY WEIGHING

More information

Element of same atomic number, but different atomic mass o Example: Hydrogen

Element of same atomic number, but different atomic mass o Example: Hydrogen Atomic mass: p + = protons; e - = electrons; n 0 = neutrons p + + n 0 = atomic mass o For carbon-12, 6p + + 6n 0 = atomic mass of 12.0 o For chlorine-35, 17p + + 18n 0 = atomic mass of 35.0 atomic mass

More information

Chapter 8 How to Do Chemical Calculations

Chapter 8 How to Do Chemical Calculations Chapter 8 How to Do Chemical Calculations Chemistry is both a qualitative and a quantitative science. In the laboratory, it is important to be able to measure quantities of chemical substances and, as

More information

Balancing Chemical Equations Worksheet

Balancing Chemical Equations Worksheet Balancing Chemical Equations Worksheet Student Instructions 1. Identify the reactants and products and write a word equation. 2. Write the correct chemical formula for each of the reactants and the products.

More information

B) atomic number C) both the solid and the liquid phase D) Au C) Sn, Si, C A) metal C) O, S, Se C) In D) tin D) methane D) bismuth B) Group 2 metal

B) atomic number C) both the solid and the liquid phase D) Au C) Sn, Si, C A) metal C) O, S, Se C) In D) tin D) methane D) bismuth B) Group 2 metal 1. The elements on the Periodic Table are arranged in order of increasing A) atomic mass B) atomic number C) molar mass D) oxidation number 2. Which list of elements consists of a metal, a metalloid, and

More information

CHEMICAL EQUATIONS and REACTION TYPES

CHEMICAL EQUATIONS and REACTION TYPES 31 CHEMICAL EQUATIONS and REACTION TYPES The purpose of this laboratory exercise is to develop skills in writing and balancing chemical equations. The relevance of this exercise is illustrated by a series

More information

Nomenclature of Ionic Compounds

Nomenclature of Ionic Compounds Nomenclature of Ionic Compounds Ionic compounds are composed of ions. An ion is an atom or molecule with an electrical charge. Monatomic ions are formed from single atoms that have gained or lost electrons.

More information

10 The Mole. Section 10.1 Measuring Matter

10 The Mole. Section 10.1 Measuring Matter Name Date Class The Mole Section.1 Measuring Matter In your textbook, read about counting particles. In Column B, rank the quantities from Column A from smallest to largest. Column A Column B 0.5 mol 1.

More information

The Mole Concept and Atoms

The Mole Concept and Atoms Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Chapter 4 24 September 2013 Calculations and the Chemical Equation The Mole Concept and Atoms Atoms are exceedingly

More information

Multiple Choice Identify the letter of the choice that best completes the statement or answers the question.

Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. Introduction to Chemistry Exam 2 Practice Problems 1 Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1.Atoms consist principally of what three

More information

Chapter 1 The Atomic Nature of Matter

Chapter 1 The Atomic Nature of Matter Chapter 1 The Atomic Nature of Matter 6. Substances that cannot be decomposed into two or more simpler substances by chemical means are called a. pure substances. b. compounds. c. molecules. d. elements.

More information

Sample Exercise 2.1 Illustrating the Size of an Atom

Sample Exercise 2.1 Illustrating the Size of an Atom Sample Exercise 2.1 Illustrating the Size of an Atom The diameter of a US penny is 19 mm. The diameter of a silver atom, by comparison, is only 2.88 Å. How many silver atoms could be arranged side by side

More information

@ Oxford Fajar Sdn. Bhd. (008974-T) 2012. Matter. 1.1 Atoms and Molecules 1.2 Mole Concept 1.3 Stoichiometry

@ Oxford Fajar Sdn. Bhd. (008974-T) 2012. Matter. 1.1 Atoms and Molecules 1.2 Mole Concept 1.3 Stoichiometry 1 Matter 1.1 Atoms and Molecules 1.2 Mole Concept 1.3 Stoichiometry 2 Chemistry for Matriculation Semester 1 1.1 Atoms and Molecules LEARNING OUTCOMES Describe proton, electron and neutron in terms of

More information

Unit 6. Chapter 10: The MOLE! Date In Class Homework. % Composition & Calculating Empirical Formulas

Unit 6. Chapter 10: The MOLE! Date In Class Homework. % Composition & Calculating Empirical Formulas Date In Class Homework 10/22 Thur Counting By Mass Lab 10/23 Fri (mole day!!!) THE MOLE! in room 137 10/26 Mon (LSM) More on the Mole Watch empirical and molecular formula video. 10/27 Tue % Composition

More information

Name Date Class CHEMICAL QUANTITIES. SECTION 10.1 THE MOLE: A MEASUREMENT OF MATTER (pages 287 296)

Name Date Class CHEMICAL QUANTITIES. SECTION 10.1 THE MOLE: A MEASUREMENT OF MATTER (pages 287 296) 10 CHEMICAL QUANTITIES SECTION 10.1 THE MOLE: A MEASUREMENT OF MATTER (pages 287 296) This section defines the mole and explains how the mole is used to measure matter. It also teaches you how to calculate

More information

2. ATOMIC, MOLECULAR AND EQUIVALENT MASSES

2. ATOMIC, MOLECULAR AND EQUIVALENT MASSES 2. ATOMIC, MOLECULAR AND EQUIVALENT MASSES INTRODUCTION: EQUIVALENT WEIGHT Since hydrogen is the lightest of all elements, it was chosen as a standard for determination of equivalent weights. On this basis,

More information

Stoichiometry Review

Stoichiometry Review Stoichiometry Review There are 20 problems in this review set. Answers, including problem set-up, can be found in the second half of this document. 1. N 2 (g) + 3H 2 (g) --------> 2NH 3 (g) a. nitrogen

More information

CHAPTER 9. 9.1 Naming Ions. Chemical Names and Formulas. Naming Transition Metals. Ions of Transition Metals. Ions of Transition Metals

CHAPTER 9. 9.1 Naming Ions. Chemical Names and Formulas. Naming Transition Metals. Ions of Transition Metals. Ions of Transition Metals CHAPTER 9 Chemical Names and Formulas 9.1 Naming Ions Monatomic Ions: a single atom with a positive or negative charge Cation (rules): listed first Anion (rules): ide ending Transition Metals have a varying

More information

Stoichiometry. What is the atomic mass for carbon? For zinc?

Stoichiometry. What is the atomic mass for carbon? For zinc? Stoichiometry Atomic Mass (atomic weight) Atoms are so small, it is difficult to discuss how much they weigh in grams We use atomic mass units an atomic mass unit (AMU) is one twelfth the mass of the catbon-12

More information

Stoichiometry. 1. The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 0.1; (4) 0.2.

Stoichiometry. 1. The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 0.1; (4) 0.2. Stoichiometry 1 The total number of moles represented by 20 grams of calcium carbonate is (1) 1; (2) 2; (3) 01; (4) 02 2 A 44 gram sample of a hydrate was heated until the water of hydration was driven

More information

Chapter 5 - Molecules and Compounds

Chapter 5 - Molecules and Compounds Chapter 5 - Molecules and Compounds How do we represent molecules? In pictures In formula In name Ionic compounds Molecular compounds On the course website, you will find a list of ions that I would like

More information

Concept 1. The meaning and usefulness of the mole. The mole (or mol) represents a certain number of objects.

Concept 1. The meaning and usefulness of the mole. The mole (or mol) represents a certain number of objects. Chapter 3. Stoichiometry: Mole-Mass Relationships in Chemical Reactions Concept 1. The meaning and usefulness of the mole The mole (or mol) represents a certain number of objects. SI def.: the amount of

More information

Molecular Formula: Example

Molecular Formula: Example Molecular Formula: Example A compound is found to contain 85.63% C and 14.37% H by mass. In another experiment its molar mass is found to be 56.1 g/mol. What is its molecular formula? 1 CHAPTER 3 Chemical

More information

Chemistry: Chemical Equations

Chemistry: Chemical Equations Chemistry: Chemical Equations Write a balanced chemical equation for each word equation. Include the phase of each substance in the equation. Classify the reaction as synthesis, decomposition, single replacement,

More information

Calculation of Molar Masses. Molar Mass. Solutions. Solutions

Calculation of Molar Masses. Molar Mass. Solutions. Solutions Molar Mass Molar mass = Mass in grams of one mole of any element, numerically equal to its atomic weight Molar mass of molecules can be determined from the chemical formula and molar masses of elements

More information

Lecture Notes Chemistry E-1. Chapter 3

Lecture Notes Chemistry E-1. Chapter 3 Lecture Notes Chemistry E-1 Chapter 3 http://inserbia.info/news/wp-content/uploads/2013/05/tamiflu.jpg http://nutsforhealthcare.files.wordpress.com/2013/01/tamiflu-moa.jpg The Mole A mole is a certain

More information

Understanding Chemical Equations

Understanding Chemical Equations Connections Understanding Chemical Equations Have you ever... Seen the result of mixing baking soda and vinegar? Used friction to light a match? Seen a car eaten through by rust? Chemical equations model

More information

Calculating Molar Mass of a Compound

Calculating Molar Mass of a Compound Instructions for Conversion Problems For every conversion problem Write the number in the problem down with unit and a multiplication sign Decide which conversion factor you should use, Avagadro s or molar

More information

ATOMS. Multiple Choice Questions

ATOMS. Multiple Choice Questions Chapter 3 ATOMS AND MOLECULES Multiple Choice Questions 1. Which of the following correctly represents 360 g of water? (i) 2 moles of H 2 0 (ii) 20 moles of water (iii) 6.022 10 23 molecules of water (iv)

More information

Calculating Atoms, Ions, or Molecules Using Moles

Calculating Atoms, Ions, or Molecules Using Moles TEKS REVIEW 8B Calculating Atoms, Ions, or Molecules Using Moles TEKS 8B READINESS Use the mole concept to calculate the number of atoms, ions, or molecules in a sample TEKS_TXT of material. Vocabulary

More information

Chapter 4. Chemical Composition. Chapter 4 Topics H 2 S. 4.1 Mole Quantities. The Mole Scale. Molar Mass The Mass of 1 Mole

Chapter 4. Chemical Composition. Chapter 4 Topics H 2 S. 4.1 Mole Quantities. The Mole Scale. Molar Mass The Mass of 1 Mole Chapter 4 Chemical Composition Chapter 4 Topics 1. Mole Quantities 2. Moles, Masses, and Particles 3. Determining Empirical Formulas 4. Chemical Composition of Solutions Copyright The McGraw-Hill Companies,

More information

11-1 Stoichiometry. Represents

11-1 Stoichiometry. Represents 11-1 Stoichiometry What is stoichiometry? Calculations that relate the quantities of substances. It is the study of quantitative (measurable amounts) relationships in chemical reactions and equations.

More information

Balancing Chemical Equations

Balancing Chemical Equations Balancing Chemical Equations 1. sodium carbonate + calcium hydroxide sodium hydroxide + calcium carbonate Na 2 CO 3 + Ca(OH) 2 2 NaOH + CaCO 3 2. carbon dioxide + water carbonic acid CO 2 + H 2 O H 2 CO

More information

Chapter 10 Chemical Quantities

Chapter 10 Chemical Quantities Chapter 10 Chemical Quantities 101 The Mole: A Measurement 102 Mole-Mass and Mole-Volume Relationships 103 Percent Composition and Chemical Formulas 1 Copyright Pearson Education, Inc, or its affiliates

More information

Naming Compounds Handout Key

Naming Compounds Handout Key Naming Compounds Handout Key p. 2 Name each of the following monatomic cations: Li + = lithium ion Ag + = silver ion Cd +2 = cadmium ion Cu +2 = copper (II) ion Al +3 = aluminum ion Mg +2 = magnesium ion

More information

CHEMICAL NAMES AND FORMULAS

CHEMICAL NAMES AND FORMULAS 6 CEMICAL NAMES AND FORMULAS SECTION 6.1 INTRODUCTION TO CEMICAL BONDING (pages 133 137) This section explains how to distinguish between ionic and molecular compounds. It also defines cation and anion

More information

Period 3 elements

Period 3 elements 3.1.4.2 Period 3 elements 173 minutes 169 marks Page 1 of 17 Q1. (a) Explain why certain elements in the Periodic Table are classified as p-block elements. Illustrate your answer with an example of a p-block

More information

Problem Solving. Stoichiometry of Gases

Problem Solving. Stoichiometry of Gases Skills Worksheet Problem Solving Stoichiometry of Gases Now that you have worked with relationships among moles, mass, and volumes of gases, you can easily put these to work in stoichiometry calculations.

More information

CHEMISTRY MEMORIZATION: STEPS FOR SOLVING STOICHIOMETRY PROBLEMS: MEMORIZE THESE use these till they are in your dreams!!!

CHEMISTRY MEMORIZATION: STEPS FOR SOLVING STOICHIOMETRY PROBLEMS: MEMORIZE THESE use these till they are in your dreams!!! CHEMISTRY MEMORIZATION: STEPS FOR SOLVING STOICHIOMETRY PROBLEMS: MEMORIZE THESE use these till they are in your dreams!!! 1. Complete reaction, determine the compounds, check oxidation numbers of each

More information

Ch. 6 Chemical Composition and Stoichiometry

Ch. 6 Chemical Composition and Stoichiometry Ch. 6 Chemical Composition and Stoichiometry The Mole Concept [6.2, 6.3] Conversions between g mol atoms [6.3, 6.4, 6.5] Mass Percent [6.6, 6.7] Empirical and Molecular Formula [6.8, 6.9] Bring your calculators!

More information

Chem 1100 Chapter Three Study Guide Answers Outline I. Molar Mass and Moles A. Calculations of Molar Masses

Chem 1100 Chapter Three Study Guide Answers Outline I. Molar Mass and Moles A. Calculations of Molar Masses Chem 1100 Chapter Three Study Guide Answers Outline I. Molar Mass and Moles A. Calculations of Molar Masses B. Calculations of moles C. Calculations of number of atoms from moles/molar masses 1. Avagadro

More information

Chemistry Assessment Unit AS 1

Chemistry Assessment Unit AS 1 Centre Number 71 Candidate Number ADVANCED SUBSIDIARY (AS) General Certificate of Education January 2011 Chemistry Assessment Unit AS 1 assessing Basic Concepts in Physical and Inorganic Chemistry [AC111]

More information

Chemistry Unit 7 Objectives Stoichiometry I By the time we finish this unit, you should be able to these:

Chemistry Unit 7 Objectives Stoichiometry I By the time we finish this unit, you should be able to these: Chemistry Unit 7 Objectives Stoichiometry I By the time we finish this unit, you should be able to these: 1. Review Concepts: a) Determine the molar mass of a substance and use it to convert between the

More information

Counting Atoms and Molecules: The Mole

Counting Atoms and Molecules: The Mole Chapter 5 Practice Problems Counting Atoms and Molecules: The Mole Solutions for Practice Problems Student Textbook pages 167 168 1. Problem The two stable isotopes of boron exist in the following proportions:

More information

Number of moles of solute = Concentration (mol. L ) x Volume of solution (litres) or n = C x V

Number of moles of solute = Concentration (mol. L ) x Volume of solution (litres) or n = C x V 44 CALCULATIONS INVOLVING SOLUTIONS INTRODUCTION AND DEFINITIONS Many chemical reactions take place in aqueous (water) solution. Quantities of such solutions are measured as volumes, while the amounts

More information

Unit 6 The Mole Concept

Unit 6 The Mole Concept Chemistry Form 3 Page 62 Ms. R. Buttigieg Unit 6 The Mole Concept See Chemistry for You Chapter 28 pg. 352-363 See GCSE Chemistry Chapter 5 pg. 70-79 6.1 Relative atomic mass. The relative atomic mass

More information

Chapter 3. Molecules, Compounds, and Chemical Composition

Chapter 3. Molecules, Compounds, and Chemical Composition Chapter 3 Molecules, Compounds, and Chemical Composition Elements and Compounds Elements combine together to make an almost limitless number of compounds. The properties of the compound are totally different

More information

Periodic Table, Valency and Formula

Periodic Table, Valency and Formula Periodic Table, Valency and Formula Origins of the Periodic Table Mendelѐѐv in 1869 proposed that a relationship existed between the chemical properties of elements and their atomic masses. He noticed

More information