Test Review Unit 3_1_Amount of substance Mole, molar mass and Avogadro s number test
|
|
- Stephanie Summers
- 5 years ago
- Views:
Transcription
1 Test Review Unit 3_1_Amount of substance Mole, molar mass and Avogadro s number test (Information extracted from file FQ3eso_t3_1_Amount of substance ) The Mole Read and then answer the Multiple choice exercise: Just like a dozen means twelve things, a mole is a much larger number of things. These things can be atoms, or molecules, or eggs; however, in chemistry, we usually use the mole to refer to the amounts of atoms or molecules. A mole is defined as the number of things equal to the number of atoms in exactly 12 g of carbon-12; equals things. Experimental measurements have determined that this number is very large: 1 mol = things The numerical value of things in a mole is often called Avogadro s number (N A ), which is also known as the Avogadro constant, after Amadeo Avogadro, an Italian chemist who first proposed its importance. One mole of a compound contains the Avogadro's number (6.022 x 1023) of molecules (molecular compound) or formula units (ionic compound). The molar mass of a compound tells you the mass of 1 mole of that substance. In other words, it tells you the number of grams per mole of a compound. The units for molar mass are, therefore, grams/mole. Knowing the molar mass of a substance, we can calculate the number of moles in a certain mass of a substance and vice versa. The molar mass is used as the conversion factor. Mole, molar mass and Avogadro s number test Multiple Choice: Identify the letter of the choice that best completes the statement or answers the question x is called number. a. Avogadro s c. Aristotle s b. Newton s d. Planck s 2. There are x atoms in one of atoms. a. mole c. amu b. Newton d. kilogram 3. The mass in grams of one mole of any pure substance is called its mass
2 a. atomic c. molar b. formula d. molecular 4. If 24 g of carbon is measured on a balance, how many atoms have been indirectly counted? a. 2 c x b. 24 d x = x Which element has a molar mass of 31 g/mole? a. Potassium c. Gallium b. Phosphorus d. Palladium 6. Which is the mass of an atom of calcium? a. 20 amu c. 40 amu b. 20 g d. 40 g 7. The number of atoms in a mole of any pure substance is called a. its atomic number. c. its mass number. b. Avogadro s number. d. its gram-atomic number. 8. What can be said about 1 mol Ag and 1 mol Au? a. They are equal in mass. b. They contain the same number of atoms. c. Their molar masses are equal. d. They have the same atomic mass. 9. An Avogadro s number of any element is equivalent to a. the atomic number of that element. c particles. b. the mass number of that element. d. 12 g of that element The molar mass of an element is the mass of one a. atom of the element. c. gram of the element. b. liter of the element. d. mole of the element. To determine the molar mass of an element, one must know the element s a. Avogadro number. c. number of isotopes. b. atomic number. d. atomic mass. What SI unit is used to measure the number of representative particles in a substance? a. kilogram c. kelvin b. ampere d. mole Avogadro's number of representative particles is equal to one. a. kilogram c. kelvin b. gram d. mole 14. How many moles of tungsten (W) atoms are in atoms of tungsten? a moles c moles
3 b moles d moles How many atoms are in 3.5 moles of arsenic (As) atoms? a atoms c atoms b atoms d atoms The atomic masses of any two elements contain the same number of. a. atoms c. ions b. grams d. milliliters To determine the formula mass of a compound you should a. add up the atomic masses of all the atoms present. b. add up the atomic masses of all the atoms present and divide by the number of atoms present. c. add up the atomic numbers of all the atoms present. d. add up the atomic numbers of all the atoms present and divide by the number of atoms present 18. Which of the following elements exists as a diatomic molecule? a. Neon (Ne) c. Nitrogen (N 2 ) b. Lithium (Li) d. Sulfur (S 8 ) 19. What is true about the molar mass of chlorine gas (Cl 2 )? a. The molar mass is 35.5 g. b. The molar mass is 71.0 g. c. The molar mass is equal to the mass of one mole of chlorine atoms. d. none of the above 20. Avogadro s number of phosphorus (P) atoms would have a mass of a x g c g b x g d g 21. A mole of a chemical substance represents a. the molar mass of that substance expressed in atomic mass units. b. an Avogadro s number of grams of that substance c. 1.0 g of that substance d. None of the above The atomic masses of He and Be are 4.00 and 9.01 amu, respectively. Which of the following statements is true? a. A mole of Be contains more atoms than a mole of He. b. A mole of He is heavier than a mole of Be. c. A mole of Be contains the same number of atoms as a mole of He. d. none of the above Which of the following samples contains the greatest number of atoms? a x C atoms c g of N atoms
4 b. 2.0 g of He atoms d. 4 moles of O atoms Which of the following statements concerning Avogadro s number is correct? a. It has the value 6.02 x b. It denotes the number of molecules in one mole of any molecular substance. c. It is the mass, in grams, of one mole of any substance.. d. It denotes the number of atoms in one mole of any substance. Which of the following samples contains the greatest number of atoms? a. 1 mole of C. c. 3 moles of N b. 2 moles of He d. 4 moles of O Mole, molar mass and Avogadro s number test. Answers 1. a 11. d 21. d 2. a 12. d 22. c 3. c 13. d 23. d 4. d 14. b 24. d 5. b 15. c 25. b 6. c 16. a 7. b 17. a 8. b 18. c 9. c 19. b 10. d 20. d
5 Converting Moles to Number of Atoms or Number of molecules: Propane is a gas used for cooking and heating. How many molecules are there in 2.12 mol of propane (C3H8)? 1.- Analyze: - List the knowns and the unknown. The desired conversion is: moles molecules KNOWNS: number of moles = 2.12 mol C3 H8 1 mol C3 H8 = molecules C3 H8 UNKNOWN: number of molecules C3 H8 2.- Calculate Solve for the unknown. First write the conversion factor to convert from moles to molecules molecules C3H8 1 mol C3H8 (Remember to write the conversion factors so that the unit in the denominator cancels the unit in the numerator of the previous factor.) Multiply the moles of C3H8 by the conversion factors. = 1.28 x molecules C3H8 Do it yourself: - How many atoms are there in 2 moles carbon (C)? = 1.20 x atoms C
6 - How many molecules are present in 2.76 mol of H 2 O? - How many molecules are there in 4.00 moles of glucose, C6H12O6? Molecules= 4.00 moles x10 molecules 1 mole = 2.41 x molecules Converting Number of Atoms or Number of molecules to Moles: - How many moles of magnesium is 3.01 x atoms of magnesium? 1 mole n= 3.01 x atoms x10 atoms = 5 x 10-2 moles The molar mass The molar mass of a compound tells you the mass of 1 mole of that substance. In other words, it tells you the number of grams per mole of a compound. The units for molar mass are, therefore, grams/mole. To find the molar mass of a compound: 1.- Use the chemical formula to determine the number of each type of atom present in the compound. 2.- Multiply the atomic mass (from the periodic table) of each element by the number of atoms of that element present in the compound. 3.- Add it all together and put units of grams/mole after the number. Knowing the molar mass of a substance, we can calculate the number of moles in a certain mass of a substance and vice versa, as these examples illustrate. The molar mass is used as the conversion factor. Calculate the relative molecular mass of each of the following: (a) H 2 S (b) CH 4 (c) NH 3 (d) C 4 H 10 (e) C 6 H 12 O 6 (f) C 12 H 22 O 11 (g) C 2 H 5 OH. Answers: (a) M r (H 2 S) = 2 X M r (H) + M r (S) =2 X = = 34 amu
7 (b) M r (CH 4 ) = M r (C) + 4 X M r (H) = X 1 = = 16 amu (c) M r (NH 3 ) = M r (N) + 3 X M r (H) = X 1 = = 17 amu (d) M r (C 4 H 10 ) = 4 X M r (C) + 10 X M r (H) = 4 X X 1 = = 58 amu (e) M r (C 6 H 12 O 6 ) = 6 X M r (C) + 12 X M r (H) + 6 X M r (O) = 6 X X X 16 = = 180 amu (f) M r (C 12 H 22 O 11 ) = 12 X M r (C) + 22 X M r (H) + 11 X M r (O) = 12 X X X 16 = = 342 amu (g) M r (C 2 H 5 OH) = 2 X M r (C) + 5 X M r (H) + M r (O) + M r (H) = 2 X X = = 46 amu Mole-Mass Conversions 1. How many moles in 28 grams of CO2? Gram-formula-mass of CO g/mol 1 mole 28 g CO 2 = 0.64 moles CO g 2 2. What is the mass of 5 moles of Fe2O3? Gram-formula-mass Fe 2 O g/mol g 5 moles Fe 2 O 3 = 800 grams Fe 1 mole 2 O 3 What is the mass of 3.56 mol of HgCl 2? The molar mass of HgCl 2 is g/mol.
1/7/14. Measuring Matter. How can you convert among the count, mass, and volume of something? Apples can be measured in three different ways.
Chapter 10 Chemical Quantities 102 Mole-Mass and Mole-Volume Relationships 103 Percent Composition and Chemical Formulas 1 Measuring Matter Measuring Matter How can you convert among the count, mass, and
More informationAtoms, Molecules, and the Mole
The Mole Now that we know how to write and name chemical compounds, we need to understand how chemists use these formulas quantitatively. As chemists, we need to know how many atoms or molecules are reacting
More informationChapter 10 Chemical Quantities
Chapter 10 Chemical Quantities 10.1 The Mole: A Measurement of Matter OBJECTIVES: Describe methods of measuring the amount of something. Define Avogadro s number as it relates to a mole of a substance.
More informationAverage 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 informationChapter 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 CHEMISTRY & YOU How can you quantify the amount of
More informationTHE MOLE (a counting unit)
MOLE AND MATH THE MOLE (a counting unit) 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 mole eggs = 6.022 x 10 23 eggs 1 dozen
More informationUnit 6: Chemical Quantities. Understanding The Mole
Unit 6: Chemical Quantities Understanding The Mole 1 How do We Typically Measure Matter? You can measure mass, or volume, or you can count pieces. We measure mass in grams. We measure volume in liters.
More informationChapter 10 Chemical Quantities
101 The Mole: A Measurement 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,
More informationCHEMISTRY MOLES PACKET PAGE 1. Chemistry Moles Packet
CHEMISTRY MOLES PACKET PAGE 1 Chemistry Moles Packet CHEMISTRY MOLES PACKET PAGE 2 INTRODUCTION TO MOLES We are about to start on a unit of chemical calculations called stoichiometry. Stoichiometry is
More informationChapter 3. Mass Relationships in Chemical Reactions
Chapter 3 Mass Relationships in Chemical Reactions In this chapter, Chemical structure and formulas in studying the mass relationships of atoms and molecules. To explain the composition of compounds and
More informationWhat is a Representative Particle
Chapter 7 Moles What is a Representative Particle The smallest unit into which a substance can be broken down without changing the composition of the substance. Atoms, molecules, and formula units What
More informationNotes: 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 informationMolar Calculations - Lecture Notes for Chapter 6. Lecture Notes Chapter Introduction
Page 1 of 9 Page 2 of 9 Lecture Notes Chapter 6 1. Introduction a. The above equation describes the synthesis of water from hydrogen and oxygen. b. It is not balanced, however. c. Notice how the number
More informationLecture Notes Chapter 6
Lecture Notes Chapter 6 1. Introduction a. The above equation describes the synthesis of water from hydrogen and oxygen. b. It is not balanced, however. à c. Notice how the number of oxygen atoms on left
More information7.1 Describing Reactions. Burning is a chemical change. When a substance undergoes a chemical change, a chemical reaction is said to take place.
Burning is a chemical change. When a substance undergoes a chemical change, a chemical reaction is said to take place. Chemical Equations What is the law of conservation of mass? The law of conservation
More informationStoichiometry. Chapter 3
Stoichiometry Chapter 3 Chemical Stoichiometry Stoichiometry: The study of quantities of materials consumed and produced in chemical reactions. In macroworld, we can count objects by weighing assuming
More informationGeneral Chemistry. Chapter 3. Mass Relationships in Chemical Reactions CHEM 101 (3+1+0) Dr. Mohamed El-Newehy 10/12/2017
General Chemistry CHEM 101 (3+1+0) Dr. Mohamed El-Newehy http://fac.ksu.edu.sa/melnewehy Chapter 3 Mass Relationships in Chemical Reactions 1 In this chapter, Chemical structure and formulas in studying
More informationWhat Is a Mole? How is Avogadro s number related to a mole of any substance? The Mole: A Measurement of Matter. What is a Mole?
10.1 > What is a Mole? What Is a Mole? How is Avogadro s number related to a mole of any substance? 1 of 43 10.1 > What is a Mole? A mole of any substance contains Avogadro s number of representative particles,
More informationChapter 10. How you measure how much? Moles. Representative particles. Conversion factors. Chemical Quantities or
Chapter 10 Chemical Quantities or 1 2 How you measure how much? You can measure mass, or volume, or you can count pieces. We measure mass in grams. We measure volume in liters. We count pieces in MOLES.
More informationMass Relationships in Chemical Reactions
Mass Relationships in Chemical Reactions Chapter 3 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Micro World atoms & molecules Macro World grams Atomic mass
More information23 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 informationName Date Class. representative particle molar mass representative particles
10.1 THE MOLE: A MEASUREMENT OF MATTER Section Review Objectives Relate Avogadro s number to a mole of a substance Calculate the mass of a mole of any substance Describe methods of measuring the amount
More information1. 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 information4) 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 informationChemistry 101 Chapter 8 Chemical Composition
Chemistry 101 Chapter 8 Chemical Composition Atomic mass unit (amu): a unit of the scale relative masses of atoms (1 amu = 1.66 10-24 g). Atomic weight (Atomic mass): the atomic weight of an element given
More informationFinding Formulas. using mass information about a compound to find its formula
Finding Formulas using mass information about a compound to find its formula Molecular Formula Molecular formula is the actual formula of compounds which form molecules. For example, the molecular formula
More informationTopic 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 informationCHAPTER 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 informationThe Mole: A Measurement of Matter
The Mole: A Measurement of Matter Vocabulary mole, Avogadro's number, representative particle, molar mass Every year contestants from all over the world travel to Harrison Hot Springs in British Columbia,
More informationUnit 6 Chemical Analysis. Chapter 8
Unit 6 Chemical Analysis Chapter 8 Objectives 39 Perform calculations using the mole to calculate the molar mass 40 Perform calculations using the mole to convert between grams, number of particles, volume,
More informationThe 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 informationUnit III: Quantitative Composition of Compounds
Unit III: Quantitative Composition of Compounds A. Atoms and Isotopes B. Atomic Composition of Chemical Compounds C. Formula and Molecular Mass D. Calculations using Moles of Atoms E. Calculations using
More informationStoichiometry. Introduction. Rx between Hydrogen and Oxygen can be described as: Balanced equation: Or Avogadros Number: (number of Molecules)
Stoichiometry Introduction Rx between Hydrogen and Oxygen can be described as: Balanced equation: Or Or Avogadros Number: (number of Molecules) Or Moles (amount of a substance containing avogadros number
More informationWhat is a Mole? An Animal or What?
Unit 7: (Chapter 9) Chemical Quantities What is a Mole? An Animal or What? Section 9.1 The Mole: A Measurement of Matter Describe how Avogadro s number is related to a mole of any substance. Calculate
More informationThe Mole. One mole = x things Avogadro s number: N A = x 10 23
The Mole 1 atom or 1 molecule is a very small entity not convenient to operate with The masses we usually encounter in chemical experiments vary from milligrams to kilograms Just like one dozen = 12 things
More information6.02 x 1023 CHAPTER 10. Mole. Avogadro s Number. Chemical Quantities The Mole: A Measurement of Matter Matter is measured in one of three ways:
Chapter 10 Notes CHAPTER 10 10.1 The Mole: A Measurement of Matter Matter is measured in one of three ways: Chemical Quantities Mole SI unit that measures the amount of a substance A mole of a substance
More informationHow do you measure matter?
How do you measure matter? You may count how many you have. Determine a substances mass and weight. Determine a substances volume. But how can you relate these three types of measurements to one another?
More informationChemistry for Today General Organic and Biochemistry 9th Edition Seager
Chemistry for Today General Organic and Biochemistry 9th Edition Seager TEST BANK Full download at: https://testbankreal.com/download/chemistry-today-general-organic-biochemistry-9thedition-seager-test-bank/
More informationDo Now. Agenda Welcome back! The beginning of ALL THE MATH! Homework PBJ procedure Pages 1-3 of HW packet
Do Now Agenda Welcome back! The beginning of ALL THE MATH! Homework PBJ procedure Pages 1-3 of HW packet All the math Molar Mass the mass of one mole of any substance, reported in grams (gram atomic mass)
More informationMeasuring 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 informationChapter 2: Mass Relations in Formulas, Chemical Reactions, and Stoichiometry
Previous Chapter Table of Contents Next Chapter Chapter 2: Mass Relations in Formulas, Chemical Reactions, and Stoichiometry Section 2.1: The Atomic Mass The atomic mass is the mass of 1 atom. Atoms are
More informationWELCOME BACK FROM SPRING BREAK
7 MOLES & CHEMICAL COMPOSITION WELCOME BACK FROM SPRING BREAK BELL RINGER (1) WHAT WAS THE MOST IMPORTANT CHEMICAL STORY THAT YOU HEARD ABOUT OVER BREAK? Short paragraph name, date, period Part 2 Brainstorm
More informationChemistry Section Review 7.3
Chemistry Section Review 7.3 Multiple Choice Identify the choice that best completes the statement or answers the question. Put the LETTER of the correct answer in the blank. 1. The molar mass of an element
More informationTHE MOLE. Chapter 10 Who is that Little Guy with Squinty Eyes?
THE MOLE Chapter 10 Who is that Little Guy with Squinty Eyes? THE MOLE NO, Not this mole, this guy has nothing to do with Chemistry! THINGS YOU SHOULD KNOW Chapter 10 Section 1 and 2 Know what a mole is.
More informationب 3 18 قسم الكيمياء مصطفي عيد
memxtd@yahoo.com m.moustapha@sau.edu.sa 0115888078 ب 3 18 قسم الكيمياء مصطفي عيد The Atom Nucleus Electron Shell or Orbit The Atom. What are the 3 major parts of an atom? Proton Neutron Electron Stoichiometry
More informationMass Relationships in Chemical Reactions
Mass Relationships in Chemical Reactions Chapter 3 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Micro World atoms & molecules Macro World grams Atomic mass
More informationThe Mole. Chemistry 11
The Mole Chemistry 11 Atomic Masses The atoms of different elements have different masses: Since the mass of an atom is very small, we use a special unit to describe it Unified Atomic Mass Unit One unified
More informationAtoms Section 2 Section 2: The Structure of Atoms
Section 2: The Structure of Atoms Preview Key Ideas Bellringer What Is in an Atom? Atomic Number and Mass Number Isotopes Atomic Masses Math Skills Key Ideas What is the difference between protons, neutrons,
More informationPart 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 information1. 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 information6/28/11. Avogadro s Number and the Mole. The Mole. The Mole. The Mole (mol)
Avogadro s Number and the Mole Molecular weight: The sum of atomic weights of all atoms in a molecule. Formula weight: The sum of atomic weights of all atoms in one formula unit of any compound. Mole:
More informationUnit 5 COUNTING PARTICLES
Unit 5 COUNTING PARTICLES Counting By Weighing We can weigh a large number of the objects and find the average mass. Once we know the average mass we can equate that to any number of the objects. EXAMPLE:
More information1. 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. Mole Definition & Background The mole was developed
More informationStoichiometry Ratios of Combination
Chapter 3 Stoichiometry Ratios of Combination Dr. A. Al-Saadi 1 Preview Concepts of atomic mass, molecular mass, mole, molar mass, and percent compositions. Balancing chemical equations. Stoichiometric
More informationExamples: Al2(SO4)3 Al 2 x 27.0 = S 3 x 32.1 = O 12 x 16.0 = NiSO3 6H2O Ni 1 x 58.7 = S 1 x 32.1 = O 3 x 16.0 = H2O 6 x 18.0 =
Moles Conversion factor: a fraction, equal to one, used to change one unit into another. A conversion factor is formed from an equality! Example: 12 inches = 1 foot 12 in or 1 ft 1 ft 12 in Dimensional
More informationChemical Calculations: The Mole concept and Chemical Formula. Law of Definite Proportions (John Dalton) Chapter 9
Chapter 9 Chemical Calculations: The Mole concept and Chemical Formula This material is not included in Midterm 1 1 Law of Definite Proportions (John Dalton) Chapter 9 A given compound always contains
More informationChemical Reactions. Chapter 17
Chemical Reactions Chapter 17 Chemical Equations C+O 2 CO 2 C (s) +O 2 (g) CO 2 (g) Reactants on left, products on right Each are balanced because same number of atoms of reactants as products Some equations
More informationChemistry 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 informationChemistry 11 INTRODUCTION TO UNIT TWO THE MOLE
Chemistry 11 INTRODUCTION TO UNIT TWO THE MOLE What is a dozen? Consider: the mass of 12 donuts does not equal the mass of 12 timbits OR, consider: 150 g donuts vs. 150 g timbits. You will need a lot more
More informationDescription 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 informationChapter 8. Chemical Composition
Chapter 8 Chemical Composition Section 8.1 Counting by Weighing Objects do not need to have identical masses to be counted by weighing. All we need to know is the average mass of the objects. To count
More informationCHAPTER 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 informationChemistry Crunch #3.2: Name: KEY What Is a Mole? Why? Learning Goals: Prerequisites:
Chemistry Crunch #3.2: Name: KEY What Is a Mole? Why? 1) In the world around you, a variety of different measures are used to specify amounts. For example, at the store you might buy 10 apples or a 5 lb
More informationSlide 1. Slide 2 Mass in amus. Slide 3 MOLES! MOLES! MOLES! Joe s 2 nd Rule of Chemistry
Slide 1 MOLES! MOLES! MOLES! Joe s 2 nd Rule of Chemistry Slide 2 Mass in amus The weighted average isotope mass is what is present in the periodic table. We saw that it is better to view the units of
More informationChemists 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 informationChapter 3. Stoichiometry
Chapter 3 Stoichiometry Chapter 3 Chemical Stoichiometry Stoichiometry The study of quantities of materials consumed and produced in chemical reactions. Since atoms are so small, we must use the average
More informationCHAPTER 9 AVOGADRO S NUMBER
CHAPTER 9 AVOGADRO S NUMBER Just like we count in dozens, gross or ream, we count atoms in groups because of their minute sizes. Like in finding the number of atoms in12.01g of C, Experiments have shown
More informationSlide 2 / 158. Mole Calculations
Slide 1 / 158 Slide 2 / 158 Mole Calculations Slide 3 / 158 Table of Contents Click on the topic to go to that section Avogadro's Number Molar Mass Molar Volume Percent Composition Emperical Formula Slide
More information9/18/2013. Scientists represent atoms by using different colored circles, called a model.
Pre-Lab Notes Lab Title: Behavior of Gases: Molar Mass of a Vapor Purpose: To determine the molar mass of a gas from a knowledge of its mass, temperature, pressure, and volume. Each element is unique.
More information7 Quantitative Composition of Compounds. Chapter Outline. The Mole. Slide 1. Slide 2. Slide 3
1 7 Quantitative Composition of Compounds Black pearls are composed of calcium carbonate, CaCO 3. The pearls can be measured by either weighing or counting. Foundations of College Chemistry, 14 th Ed.
More informationGermanium 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 informationMass Relationships in Chemical Reactions
Mass Relationships in Chemical Reactions Chapter 3 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Micro World atoms & molecules Macro World grams Atomic mass
More informationChemistry Chapter 3. Stoichiometry. (three sections for this chapter)
Chemistry Chapter 3 Stoichiometry (three sections for this chapter) Chemistry Chapter 3 Stoichiometry Section 1 3.1-3.4 Average Atomic Mass The Mole Molar Mass Average Atomic Mass Average mass of objects
More informationName Date Class CHEMICAL QUANTITIES. SECTION 10.1 THE MOLE: A MEASUREMENT OF MATTER (pages )
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 informationUnit 1 review. Chapter 1, chapter , 2.4
Unit 1 review Chapter 1, chapter 2.1-2.2, 2.4 The Organization of Matter Matter Mixtures: a) Homogeneous (Solutions) b) Heterogeneous Pure Substances Elements Compounds Atoms Nucleus Protons Quarks Electrons
More informationChapter 3 Stoichiometry
Chapter 3 Sep 22 1:45 PM Average atomic mass: The weighted average of all isotopes of a specific element. Takes into consideration abundance of each isotope. (% x M 1 ) + (% x M 2 ) +... Sep 22 1:45 PM
More informationMolar Mass. The total of the atomic masses of all the atoms in a molecule:
Molar Mass The total of the atomic masses of all the atoms in a molecule: Ex: H 2 O H (1.0079) x 2 atoms = 2.0158 grams O (15.999) x 1 atom = 15.999 grams 18.0148 grams (18.0 grams) Ex: Cu(NO 3 ) 2 Cu
More informationMass Relationships of Atoms
Mass Relationships of Atoms The Mole - the fundamental SI measure of amount of substance - the amount of substance that contains as many elementary entities as there are atoms in exactly 12 g of carbon-12
More information1 P a g e C h a p t e r 7 C h e m i c a l Q u a n t i t i e s a n d t h e M o l e
1 P a g e C h a p t e r 7 C h e m i c a l Q u a n t i t i e s a n d t h e M o l e Chapter 7 The Mole: A measurement of matter Vocabulary: Mole (mol) Avogadro Number = 6.02 x 1023 Representative particle
More informationCHEMISTRY MOLES PACKET 2017 NAME: PER:
CHEMISTRY MOLES PACKET 2017 NAME: PER: We have learned that a mole can be a certain mass of a substance and a certain number of particles. A mole can also be a measure of volume when we are talking about
More informationOutcomes: Interpret a balanced chemical equation in terms of moles, mass and volume of gases. Solve stoichiometric problems involving: moles, mass,
Stoichiometry Outcomes: Interpret a balanced chemical equation in terms of moles, mass and volume of gases. Solve stoichiometric problems involving: moles, mass, volume, and heat of reaction. Stoichiometry
More informationUnit 3. Stoichiometry
Unit 3. Stoichiometry Upon successful completion of this unit, the students should be able to: 3.1 Define atomic mass and solve related problems. 1. Gallium has two naturally occurring isotopes, and gallium-70
More informationChem101 - Lecture 2. Atoms and Molecules
Chem101 - Lecture 2 Atoms and Molecules Elements Elements are pure substances containing only one kind of atom (homoatomic). There are at last count 114 elements. - 88 of them are naturally occurring.
More informationComposition and formulae. Of moles and men
Composition and formulae Of moles and men Learning objectives Count atoms in formula Define the mole Determine numbers of atoms or molecules in molar quantities Determine molar mass from chemical formula
More informationUnit III: Quantitative Composition of Compounds
Unit III: Quantitative Composition of Compounds A. Atoms and Isotopes B. Atomic Composition of Chemical Compounds C. Formula and Molecular Mass D. Calculations using Moles of Atoms E. Calculations using
More informationMOLECULAR FORMULA AND EMPIRICAL FORMULA
MOLECULAR FORMULA AND EMPIRICAL FORMULA Molecular Formula is a formula indicating the actual number of atoms of each element making up a molecule. The molecular formula must accurately state the exact
More informationDetermining Chemical Formulas
SECTION 7.4 Determining Chemical Formulas When scientists discover or produce a new compound, they analyze it to learn its composition. Often what they measure is the percentage composition of the substance.
More informationUnit 4: The MOLE & STOICHIOMETRY. Essential Question: What is a MOLE and why do we use it to measure chemical things PRECISELY?
Unit 4: The MOLE & STOICHIOMETRY Essential Question: What is a MOLE and why do we use it to measure chemical things PRECISELY? What makes a figure SIGNIFICANT? n Non-Zero DIGITS n 1.589 n 0.897 n 3600
More informationBonding, Moles & Unit 3. Stoichiometry
Bonding, Moles & Unit 3 Stoichiometry Warm-up! Chem Catalyst 1.What part of the atom participates in the reactivity of elements? 2.What does the octet rule have to do with reactivity? 3.Based on what you
More informationCHEMISTRY Matter and Change
CHEMISTRY Matter and Change Table Of Contents Section.1 Measuring Matter Section.2 Mass and the Mole Section.3 Moles of Compounds Chapter : Section.4 Empirical and Molecular Formulas Section.5 Formulas
More informationCH301 REVIEW: CHEMICAL FORMULAS, COMPOSITION STOICHIOMETRY
CH301 REVIEW: CHEMICAL FORMULAS, COMPOSITION STOICHIOMETRY Summary. Much of high school chemistry was devoted to introducing the concept of Dalton s ATOMIC THEORY which provides a foundation for a more
More information2.1. SYMBOLS AND FORMULAS A unique symbol is used to represent each element. Formulas are used to represent compounds.
2.1. SYMBOLS AND FORMULAS A unique symbol is used to represent each element. Formulas are used to represent compounds. Symbols of Elements Atoms and Molecules ELEMENTAL SYMBOLS A symbol is assigned to
More informationCHEMICAL QUANTITIES. Chapter Six
CHEMICAL QUANTITIES Chapter Six Introducing the Mole The dozen is a unit of quantity If I have a dozen atoms, I have 12 atoms by definition. The mole(mol) is a very important unit of quantity in chemistry.
More information9/14/ Chemistry Second Edition Julia Burdge. Stoichiometry: Ratios of Combination. Molecular and Formula Masses
9/14/1 Chemistry Second Edition Julia Burdge Stoichiometry: Ratios of Combination Copyright (c) The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 1 Stoichiometry: Ratios
More informationTHE 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 information9.1.1 CHEMICAL EQUATIONS AND STOICHIOMETRY
9.1.1 CHEMICAL EQUATIONS AND STOICHIOMETRY Work directly from Zumdahl (Chapter 3). Work through exercises as required, then summarise the essentials of the section when complete. A chemical equation is
More information6.02 X Lesson # 9.1: The Mole. Unit 9: Math of Chemistry Chemical Quantities Part I. Yes, you will need a calculator for this chapter!
Unit 9: Math of Chemistry Chemical Quantities Part I Lesson # 9.1: The Mole Yes, you will need a calculator for this chapter! The Mole 6.02 X 10 23 Lesson 9.1: The Mole: A Measurement of Matter OBJECTIVES:
More informationReacting Masses 1 of 24 Boardworks Ltd 2016
Reacting Masses 1 of 24 Boardworks Ltd 2016 Reacting Masses 2 of 24 Boardworks Ltd 2016 What is a mole? 3 of 24 Boardworks Ltd 2016 A mole is an SI unit that is used to denote the number of atoms or molecules
More informationI hope you aren't going to tear open the package and count the nails. We agree that. mass of nails = 1340 g g = g
The Mole Concept Counting by weighing The size of molecule is so small that it is physically difficult if not impossible to directly count out molecules. this problem is solved using a common trick. Atoms
More information