3.6 Determining the Formula of a Compound
|
|
|
- Meredith Walsh
- 6 years ago
- Views:
Transcription
1 3.6 Determining the Formula of a Compound
2 Molecular compounds Copyright Houghton Mifflin Company. All rights reserved. 3 2
3 Formulas molecular formula = (empirical formula) n [n = integer] Ex. (CH 5 N) n or (CH 2 O) n To be able to specify the exact formula of the molecule involved, the molecular formula, we must know the molar mass. molecular formula = C 6 H 6 = (CH) 6 empirical formula = CH Copyright Houghton Mifflin Company. All rights reserved. 3 3
4 Molecular Formula Determination Method 1 Obtain the empirical formula Compute the mass corresponding to the empirical formula. Calculate the ratio Molar Mass/Empirical formula mass The integer from the previous step represents the number of empirical formula in one molecule. When the empirical formula subscripts are multiplied by this integer, the molecular formula results. Copyright Houghton Mifflin Company. All rights reserved. 3 4
5 Molecular Formula Determination Method 2 Using the mass percentages and the molar mass, determine the mass of each element present in one mole of compound. Determine the number of moles of each element present in one mole of compound. The integers from the previous step represent the subscripts in the molecular formula. Copyright Houghton Mifflin Company. All rights reserved. 3 5
6 EXAMPLE using Method 1 Determining the Empirical and Molecular Formulas of a Compound from Its Mass Percent Composition Dibutyl succinate is an insect repellent used against household ants and roaches. Its composition is 62.58% C, 9.63% H and 27.79% O. Its experimentally determined molecular mass (molar mass) is 230 amu. What are the empirical and molecular formulas of dibutyl succinate? Step 1: Determine the mass of each element in a 100g sample. C g H 9.63 g O g Copyright Houghton Mifflin Company. All rights reserved. 3 6
7 EXAMPLE continue Step 2: Convert masses to amounts in moles. n n C n O H = = 9.63 = g C g H g O 1mol C g C 1mol H g H 1mol O g O = mol C = 9.55 mol H = mol O Step 3: Write a tentative formula. Step 4: Convert to small whole numbers. C 5.21 H 9.55 O 1.74 C 2.99 H 5.49 O C = 5.21/1.74 = 2.99; H = 9.55/1.74 = 5.49; O = 1.74/1.74 = 1 Copyright Houghton Mifflin Company. All rights reserved. 3 7
8 EXAMPLE continue Step 5: Convert to a small whole number ratio since H Multiply 2 to get C 5.98 H O 2 Step 6: Determine the molecular formula. The empirical formula is C 6 H 11 O 2 (6 mol C x amu C/mol C + 11 mol H x amu H/mol + 2 mol O x amu) = amu Calc ratio = Molar Mass/ Empirical Formula Mass Molecular formula mass exp determined is 230 amu. Empirical formula mass is 115 amu. = 2 (C 6 H 11 O 2 ) n=2 The molecular formula is C 12 H 22 O 4 Copyright Houghton Mifflin Company. All rights reserved. 3 8
9 Learning Check A white power is analyzed and found to contain 43.64% phosphorus and 56.36% oxygen by mass. The compound has a molar mass of g/mol. What are the compounds empirical and molecular formulas? Copyright Houghton Mifflin Company. All rights reserved. 3 9
10 QUESTION The dye indigo is a compound with tremendous economic importance (blue jeans wouldn t be blue without it.) Indigo s percent composition is: 73.27% C; 3.84% H; 10.68%N and 12.21% O. What is the empirical formula of indigo? 1. C 6 H 4 NO 2. C 8 H 3 NO 3. C 8 H 5 NO 4. I know this should be whole numbers for each atom, but I do not know how to accomplish that. Copyright Houghton Mifflin Company. All rights reserved. 3 10
11 ANSWER Choice 3 is the smallest whole number ratio of the atoms that make up a molecule of indigo. The percentage must be converted to a mass, then the mass is converted to moles of the atoms and finally, the smallest is divided into the others to obtain the proper ratio. Copyright Houghton Mifflin Company. All rights reserved. 3 11
12 QUESTION Without further information, which of the following is more likely to be both a molecular formula and an empirical formula for a compound? Briefly explain why. H 2 O 2 ; C 6 H 6 ; C 2 H 6 O 1. H 2 O 2. The whole numbers for each atom are reduced as far as possible and still retain the identity of the molecule. 2. C 6 H 6. The whole number of atoms are equal for each element. 3. C 2 H 6 O. One element shows only one atom so the formula ratio could not be further reduced, but the molecular formula could just have one atom. 4. None of these, it is not possible for a formula to be both empirical and molecular. Copyright Houghton Mifflin Company. All rights reserved. 3 12
13 ANSWER Choice 3 shows the correct choice and proper justification. The whole numbers are reduced to their lowest value so C 2 H 6 O could be the empirical formula. The other choices could still be reduced to smaller whole numbers and maintain the same ratio. Section 3.6: Determining the Formula of a Compound Copyright Houghton Mifflin Company. All rights reserved. 3 13
Introductory Chemistry: A Foundation, 6 th Ed. Introductory Chemistry, 6 th Ed. Basic Chemistry, 6 th Ed.
Introductory Chemistry: A Foundation, 6 th Ed. Introductory Chemistry, 6 th Ed. Basic Chemistry, 6 th Ed. by Steven S. Zumdahl & Donald J. DeCoste University of Illinois Chapter 8 Chemical Composition
Introductory Chemistry: A Foundation, 6 th Ed. Introductory Chemistry, 6 th Ed. Basic Chemistry, 6 th Ed.
Introductory Chemistry: A Foundation, 6 th Ed. Introductory Chemistry, 6 th Ed. Basic Chemistry, 6 th Ed. by Steven S. Zumdahl & Donald J. DeCoste University of Illinois Chapter 9 Chemical Quantities Information
Announcement. Quiz # 1 and 2 on Friday, 28 November. Please bring a blue book!
Announcement Quiz # 1 and 2 on Friday, 28 November. Please bring a blue book! 1 Borax is the common name of an industrial cleaner, sodium tetraborate, Na 2 B 4 O 7. Suppose you have 20.0 g of borax. Calculate
Chemistry 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
NOTES: 10.3 Empirical and Molecular Formulas
NOTES: 10.3 Empirical and Molecular Formulas What Could It Be? Empirical Formulas Indicate the lowest whole number ratio of the atoms in a compound: 1) Determine moles of each element present in the compound
90.14 g/mol x g/mol. Molecular formula: molecular formula 2 empirical formula 2 C OH C O H
Whole-number multiple: M x M actual compound C2OH5 90.14 g/mol x 45.07 g/mol 90.14 g/mol x 45.07 g/mol 2 Molecular formula: molecular formula 2 empirical formula 2 C OH 2 5 C O H 4 2 10 Check Your Solution
Atoms, 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
Chapter 6 Empirical and Molecular Formulas
Chapter 6 Empirical and Molecular Formulas EMPIRICAL FORMULA A chemical formula that indicates the relative proportions of the elements in a molecule rather than the actual number of atoms of the elements.
Determining 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.
Chapter 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
Finding 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
Calculations with Chemical Formulas and Equations
Calculations with Chemical Formulas and Equations Mass and Moles of a Substance Chemistry requires a method for determining the numbers of molecules in a given mass of a substance. This allows the chemist
THE 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
Composition 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
3.9 Stoichiometric Calcs: Amounts of Reactants and Products
3.9 Stoichiometric Calcs: Amounts of Reactants and Products Law of Conservation of Mass The Law of Conservation of Mass indicates that in an ordinary chemical reaction, Matter cannot be created nor destroyed.
CHEMICAL FORMULA COEFFICIENTS AND SUBSCRIPTS 3O 2 2O 3. ! Formula that gives the TOTAL number of elements in a molecule or formula unit.
CHEMICAL FORMULA! Formula that gives the TOTAL number of elements in a molecule or formula unit. No Score from Exam 1? Go to 210 Whitmore and speak with Mike Joyce to get it straightened out. Which Skill
Mass 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
Chapter 3. Mass Relationships, Stoichiometry and Chemical Formulas. Announcements. Learning Objectives MOLE
Announcements HOUR EXAM 1 --Critical To Understand Chapter 3 July 18 6-7:30PM --Skip Combustion Analysis & Isomers (p.82-83 in Principles of Chemistry Text) See me if you donʼt understand! Chapter 3 Relationships,
Chapter 3 C 2 H 4 O2. Mass Relationships, Stoichiometry and Chemical Formulas. Announcements. Learning Objectives. C x H y Oz
Announcements HOUR EXAM 1 --Want me to do recitation again? July 18 6-7:30PM --Skip Combustion Analysis & Isomers (p.82-83 in Principles of Chemistry Text) See me if you donʼt understand! Chapter 3 Relationships,
Chemistry I Notes Unit 7: Stoichiometry Notes
Chemistry I Notes Unit 7: Stoichiometry Notes Stoichiometry Relating Mass to Numbers of Atoms The Mole The mole is the SI unit for amount of substance. A mole (abbreviated mol) is the amount of a substance
Using the Mole to Calculate % Composition, Empirical Formulas and Molecular Formulas
Using the Mole to Calculate % Composition, Empirical Formulas and Molecular Formulas Law of Definite Proportions Compounds have constant composition This means that the ratios by mass of the elements chemically
9/14/ 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
Atoms, Ions and Molecules Calculations
Atoms, Ions and Molecules Calculations 1. How do you calculate the atomic mass of an element? Atomic Mass = (% abundance of isotope 1)(mass of isotope 1) + (% abundance of isotope2)(mass of isotope 2)
Chapter 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
6 atomic # C symbol Carbon name of element atomic mass. o Examples: # 1 mol C = g # 1 mol O = g # 1 mol H = 1.
7.1 AVOGADRO S NUMBER AND MOLAR CONVERSIONS CHEMISTRY NOTES Identify the mole as the unit used to count particles, whether atoms, ions, or molecules. Use Avogadro s number to convert between amount in
Stoichiometry Dr. M. E. Bridge
Preliminary Chemistry Course Stoichiometry Dr. M. E. Bridge What is stoichiometry? The meaning of the word: The word stoichiometry comes from two Greek words: stoichon(meaning element ) and metron(meaning
Unit 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,
Mass 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
Chemistry Stoichiometry: Mole Ratios
a place of mind F A C U L T Y O F E D U C A T I O N Department of Curriculum and Pedagogy Chemistry Stoichiometry: Mole Ratios Science and Mathematics Education Research Group Supported by UBC Teaching
3/22/2017. Chapter 8. Chemical Composition. Counting by Weighing. Section 8.1
Chapter 8 Chemical Composition Section 8.1 Counting by Weighing 2 1 Section 8.1 Counting by Weighing A pile of marbles weigh 394.80 g. 10 marbles weigh 37.60 g. How many marbles are in the pile? 37.60
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
Lecture 11 - Stoichiometry. Lecture 11 - Introduction. Lecture 11 - The Mole. Lecture 11 - The Mole. Lecture 11 - The Mole
Chem 103, Section F0F Unit IV - Stoichiometry of Formulas and Equations Lecture 11 The concept of a mole, which is a very large group of atoms or molecules Determining the formulas for a compound Stoichiometry
What 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
General 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
Mass 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
MOLECULAR 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
Unit 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.
Chapter 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.
You should be reading Chapter 3 and practicing nomenclature from Chapter 2 (lots to know).
Announcements You should be reading Chapter 3 and practicing nomenclature from Chapter 2 (lots to know). Chapter 2: Please expect 1 or perhaps 2 to be collected as a Quiz grade on Tuesday. 1,2,4,13,14,16,18,20,24,27,34,38,40,42,45,50,53,54,
Unit 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
Ch 3. Chemical Reactions and Reaction Stoichiometry
Ch 3 Chemical Reactions and Reaction Stoichiometry { { Chemical Reactions involve the rearrangement of atoms. CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2 H 2 O (g) Reactant Products s Law of Conservation of Mass
Practice questions for Ch. 3
Name: Class: Date: ID: A Practice questions for Ch. 3 1. A hypothetical element consists of two isotopes of masses 69.95 amu and 71.95 amu with abundances of 25.7% and 74.3%, respectively. What is the
Chapter 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
Molar Conversions & Calculations
Molar Conversions & Calculations Ch. 11 The Mole 1 A. What is the Mole? A counting number (like a dozen) Avogadro s number (n) 1 mol = 6.02 x 10 23 items A VERY large amount!!!! 2 A. What is the Mole?
A TAKAMUL INTERNATIONAL SCHOOL CH.10 THE MOLE PREPARED BY MR. FAHAD AL-JARAH
A TAKAMUL INTERNATIONAL SCHOOL CH.10 THE MOLE PREPARED BY MR. FAHAD AL-JARAH Chapter Outline Section 10.1 Measuring Matter Key Concepts The mole is a unit used to count particles of matter indirectly.
Counting by mass: The Mole. Unit 8: Quantification of Chemical Reactions. Calculating molar mass. Particles. moles and mass. moles and particles
Unit 8: Quantification of Chemical Reactions Chapter 10: The mole Chapter 12: Stoichiometry Counting by mass: The Mole Chemists can t count individual atoms Use moles to determine amounts instead mole
Chemistry 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
Formula Mass. not all compounds are molecular formula mass calculated exactly the same way as molecular mass. Solid structure of NaCl
Molecular Mass Molecular Mass synonymous with molar mass and molecular weight is the sum of the atomic masses of all the atoms in a molecule the mass in grams of one mole of a compound Formula Mass not
Get out a sheet of paper to take some notes on.
Bellwork: Get out your old textbook and your ID. Get out a sheet of paper to take some notes on. Solve the following problem. Methyl alcohol, CH 3 OH, is a clean-burning, easily handled fuel. It can be
Topics in composition stoichiometry include the calculation of: Molar mass Percent Composition Molecular formula Empirical formulas
Composition Stoichiometry Composition Stoichiometry NOTES 1 So far, we ve studied the products of a chemical reaction in terms of their identity. Stoichiometry is a branch of chemistry dealing with quantities.
The quantities in formulas and in chemical reactions can be counted singly or in groups, such as the mole.
CHEM110 Week 4 Notes Mass relationships in Chemical Formulas Page 1 of 5 Recall the Law of Definite Proportions. All samples of a compound have the same atomic composition (or) all samples have the same
CHEMICAL 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.
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
Chapter 3 Calculations with Chemical Formulas and Equations
Chapter 3 Calculations with Chemical Formulas and Equations Contents and Concepts Mass and Moles of Substances Here we will establish a critical relationship between the mass of a chemical substance and
Chapter 3. Stoichiometry: Calculations with Chemical Formulas and Equations
Chapter 3. Stoichiometry: Calculations with Chemical Formulas and Equations Lecture Outline 3.1 Chemical Equations The quantitative nature of chemical formulas and reactions is called stoichiometry. Lavoisier
Chemical Equations. Chemical Equations
Page III-4a-1 / Chapter Four Part I Lecture Notes Chemical Reactions Chapter 4 Part 1 Chemistry as Cooking! - the Chemical Reaction "Recipe" and technique leads to successful creations Must know amounts
Examples: 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
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
1.3: Empirical and Molecular Formulas. Ms. Kiely Coral Gables Senior High IB Chemistry SL
1.3: Empirical and Molecular Formulas Ms. Kiely Coral Gables Senior High IB Chemistry SL Practice How heavy are 1.20 x 10²⁵ atoms of potassium? ANSWER How many grams in 1.20 x 10²⁵ atoms of potassium?
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
Mass 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
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
CHEMISTRY 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
1.2: Mole, Conversion Factors, Empirical & Molecular Formulas. Ms. Kiely Coral Gables Senior High IB Chemistry SL
1.2: Mole, Conversion Factors, Empirical & Molecular Formulas Ms. Kiely Coral Gables Senior High IB Chemistry SL TURN IN the Signed Syllabus and Topic 1 Exercises Bell-Ringer #2 What amount in grams is
The 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
9.1.1 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
7 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.
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
Chapter 3 Molecules, Compounds, and Chemical Equations
Chapter 3 Molecules, Compounds, and Chemical Equations 3.7 Formula Mass versus Molar mass Formula mass The average mass of a molecule or formula unit in amu also known as molecular mass or molecular weight
Topic 02 Atomic Structure 2.2: The Mass Spectrometer. IB Chemistry T02D02
Topic 02 Atomic Structure 2.2: The Mass Spectrometer IB Chemistry T02D02 2.1 The Mass Spectrometer - 1 hour 2.2.1 Describe and explain the operation of a mass spectrometer. (3) 2.2.2 Describe how the mass
Do 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)
Chapter 9. Chemical Calculations and Chemical Formulas
Chapter 9 Chemical Calculations and Chemical Formulas Chapter Map Making Phosphoric Acid Furnace Process for making H 3 PO 4 to be used to make fertilizers, detergents, and pharmaceuticals. React phosphate
Hydrates, Percent Composition, and Empirical and Molecular Formulas
Hydrates, Percent Composition, and Empirical and Molecular Formulas Hydrates Hydrates are ionic cmpds (salts) that have water molecules bound to their ions. Examples: CuSO 4 5H 2 O Fe(NO 3 ) 3 9H 2 O CoCl
Mole. The SI base unit used to measure the amount of a substance.
Stoichiometry Stoichiometry The study of quantitative relationships between the amounts of reactants used and products formed by a chemical reactions; it is based on the law of conservation of mass. Mole
Stoichiometry. 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
Mole Concept. Conversion Factors:
Today s focus. Mole Concept Avogadro s Number is 6.02x10 23 The mole unit is used to express: 1. A mass quantity 2. A counting quantity 1 water molecule 1 mole of water molecules Conversion Factors: 6.02x10
Chemistry 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
Honors Chemistry Unit 6 Moles and Stoichiometry Notes. Intro to the mole 1. What is the chemical mole? 2. What is Avogadro s number?
Honors Chemistry Unit 6 Moles and Stoichiometry Notes Intro to the mole 1. What is the chemical mole? 2. What is Avogadro s number? 3. What does it mean? 4. How is a mole like a dozen doughnuts? Formula
PowerPoint to accompany. Chapter 2. Stoichiometry: Calculations with Chemical Formulae and Equations. Dr V Paideya
PowerPoint to accompany Chapter 2 Stoichiometry: Calculations with Chemical Formulae and Equations Dr V Paideya Chemical Equations CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2 H 2 O (g) Figure 2.4 Chemical Equations
Chapter 3. Stoichiometry
1 hapter 3 Stoichiometry 2 Atomic Mass Avogadro s Number and Molar Mass 3 Atomic Mass: Mass of 1 atom in atomic mass units 1 amu = 1/12 of the mass of 1-12 atom = 1.661X10-24 g Naturally occurring carbon
Unit 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
Chapter 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.
Chemical Equations. Law of Conservation of Mass. Anatomy of a Chemical Equation CH4(g) + 2O2(g) Chapter 3
Chemical Equations Chemical equations are concise representations of chemical reactions. Chapter 3 : Calculations with Chemical Formulas and Equations Law of Conservation of Mass Anatomy of a Chemical
CHEMISTRY Matter and Change. Chapter 10: The Mole
CHEMISTRY Matter and Change Chapter 10: The Mole CHAPTER 10 Table Of Contents Section 10.1 Measuring Matter Section 10.2 Mass and the Mole Section 10.3 Moles of Compounds Section 10.4 Empirical and Molecular
Unit 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:
3 Stoichiometry: Calculations with Chemical Formulas and Equations
3 Stoichiometry: Calculations with Chemical Formulas and Equations 3.1 Chemical Equations Balance chemical equations. 3. Simple Patterns of Reactivity Predict products of a chemical reaction in a combination
If you're given a mass percent, you can use it as a conversion factor between the element and the compound
Announcements Wednesday, September 23, 2009 MasteringChemistry due dates (all at 11:59 pm): Ch 3: Fri, Sep 25 Exam 1: next Mon, Sep 28. 20-25 multiple choice questions Short answer (naming, chemical equations)
Molecular vs. Empirical Formula Chemistry H 2 O H 2 O 2. NaCl
Molecular vs Empirical Formula Chemistry Name Block Read the information below and then answer the questions that follow Definitions: Molecular formula the total number of atoms of each element in a compound
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
Molar 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
Chapter 3. Stoichiometry: Calculations with Chemical Formulas and Equations. Lecture Presentation
Lecture Presentation Chapter 3 : Calculations with Chemical Formulas and Equations John D. Bookstaver St. Charles Community College Cottleville, MO Law of Conservation of Mass We may lay it down as an
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.
Announcements. 1 point for every question attempted; 0.2 extra credit points for every correct answer
Announcements Print worksheet #3 prior to your Tuesday discussion section Solutions to worksheets #1 and #2 are posted online now A full schedule of readings and suggested problems is posted on the course
Ch. 3 The Mole: Relating the Microscopic World of Atoms to Laboratory Measurements. Brady & Senese, 5th Ed.
Ch. 3 The Mole: Relating the Microscopic World of Atoms to Laboratory Measurements Brady & Senese, 5th Ed. Index 3.1 The mole conveniently links mass to number of atoms or molecules 3.2 Chemical formulas
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
SL Chemistry. Friday August 28th Monday, August 31, 15
SL Chemistry Friday August 28th 2015 Agenda Warm Up: NONE Empirical and Molecular Formula Notes E & M handout (HW) Internal Assessment - Project Guides HOMEWORK Topic 1.1 Introduction to Particulate Nature
ب 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
Stoichiometry. Please take out your notebooks
Stoichiometry Please take out your notebooks Stoichiometry stochio = Greek for element metry = measurement Stoichiometry is about measuring the amounts of elements and compounds involved in a reaction.
Chapter 3: Molecules, Compounds and Chemical Equations: (continue and finish chapter 3: 8-11)
C h e m i s t r y 1 A : C h a p t e r 3 P a r t B P a g e 1 Chapter 3: Molecules, Compounds and Chemical Equations: (continue and finish chapter 3: 8-11) Homework: Read Chapters 3. Work out sample/practice
Chapter 3 Stoichiometry. Ratios of combination
Chapter 3 Stoichiometry Ratios of combination Topics Molecular and formula masses Percent composition of compounds Chemical equations Mole and molar mass Combustion analysis (Determining the formula of