Chemical formulas allow chemists to calculate characteristic values for a compound.

Size: px
Start display at page:

Download "Chemical formulas allow chemists to calculate characteristic values for a compound."

Transcription

1 Chemical Formulas Using Analytical Data to Calculate Chemical Formulas Chemical formulas allow chemists to calculate characteristic values for a compound. Calculation Types You Must be Able to Complete X Molar Mass (Formula Mass) X Percentage Composition by Mass X Using Percentage Composition Data to Calculate Empirical Formulas New: Using Data to Calculate Molecular Formulas For Ionic Compounds There is only 1 type of chemical formula: The Empirical Formula The Empirical Formula Gives the simplest whole number ratio of ions that produces a neutral arrangement Gives the simplest whole number ratio of moles Molecular Compounds are Different Molecular Formula C 6 H 12 O 6 For each element this is the: Actual number of atoms Actual number of moles This is the blueprint for drawing the Lewis Structure This is the formula written from the name Additional examples: Molecular Formula H 2 O H 2 O 2 Empirical Formula C H 2 O This is the simplest whole number ratio For each element this is the reduced : number of atoms number of moles This is the backbone Not used to write a name Empirical Formula H 2 O HO N 2 O 4 NO 2 ICl 3 ICl 3 In general, for molecular compounds, the molecular formula will be the same as the empirical formula or the molecular formula will be larger.

2 Answer the Following Sample Concept Questions 1) The molecular formula for vitamin C is C 6 H 8 O 6. What is the empirical formula? a. CHO c. C 3 H 4 O 3 b. CH 2 O d. C 2 H 4 O 2 2) Which of the following could be an empirical formula? a. N 2 O 4 b. b. N 2 H 6 c. c. N 2 O 5 d. d. More than one could be an empirical formula. e. None of these are empirical formulas. 3) If the empirical formula of a compound is CH 2 what is a possible molecular formula for the compound? a. CH 2 b. C 2 H 6 c. C 4 H 8 d. More than one could be a molecular formula for CH 2. e. None of these could be a molecular formula for CH 2. In summary, sometimes the Molecular Formula = Empirical Formula Other times the Molecular Formula > Empirical Formula It is larger by X where X is a whole number Never is the Molecular formula smaller than the empirical formula Not sure what the difference is between Molecular and Empirical Formulas for Covalent Compounds? Watch this video: All set then move on to molecular formula calculations notes, videos and problems

3 How to Calculate Molecular Formula Problem Types Given % composition data or the empirical formula and The molecular formula mass To solve problems Use the relationships given in these two formulas you must memorize 1st Formula 2nd Formula X (Empirical Formula) = Molecular Formula Where X is a whole-number multiple found by X = Molecular Formula Mass What will vary, problem to problem, is the information you are given and what you have to do to find X.

4 Problem Type 1 Given: Empirical Formula and Molar Mass of the Molecular Formula Video: Watch and take notes

5 Problem Type Given: Empirical Formula and Molecular Formula Mass Step 1 Calculate the Step 2 Solve for X X = Molecular Formula Mass Step 3 Apply X X (Empirical Formula) = Molecular Formula Step 4 Write the Molecular Formula After watching the video solve the following problem on a separate sheet of paper. You must show all work A compound was analyzed. The empirical formula of the compound is C4H4O and the molar mass of the molecule is 136 g/1mole.

6 Problem Type #2 Given percentage composition data and the molecular formula mass Video: Watch and take notes.

7 Problem Type 2 Given: % Composition and Molecular Formula Mass Step 1 Calculate the Empirical Formula % to mass Grams to Moles etc. Step 2 Calculate the Step 3 Solve for X X = Molecular Formula Mass Step 4 Apply X X (Empirical Formula) = Molecular Formula Step 5 Write the Molecular Formula After watching the video solve the following problem on a separate sheet of paper. You must show all work A compound was analyzed and found to have 65.5% carbon, 5.5% hydrogen and 29.0% oxygen? If the molar mass of this molecule is 110.g/mole, what is the molecular formula?

Finding Formulas. using mass information about a compound to find its formula

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

More information

Chemistry 101 Chapter 8 Chemical Composition

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

More information

Using the Mole to Calculate % Composition, Empirical Formulas and Molecular Formulas

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

More information

MOLECULAR FORMULA AND EMPIRICAL FORMULA

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

More information

CHEMISTRY Matter and Change

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

More information

Covalent bonding, gives rise to the possibility to create big molecules; unlike ionic bonding form individual ions which are attracted to each other.

Covalent bonding, gives rise to the possibility to create big molecules; unlike ionic bonding form individual ions which are attracted to each other. Covalent bonding, gives rise to the possibility to create big molecules; unlike ionic bonding form individual ions which are attracted to each other. This is why, ionic compounds are always reduced to

More information

!"##$%&'()$*+,%'-./'

!##$%&'()$*+,%'-./' !"##$%&()$*+,%-./ 0,1,%$234%5$1673896:2:567$2(),#6;+%& 6!#6+)! CHAPTER 3-4: Concepts to Know! The difference between ionic and covalent bonds! Define cations and anions! Predict cation/anion

More information

90.14 g/mol x g/mol. Molecular formula: molecular formula 2 empirical formula 2 C OH C O H

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

More information

Percent yield Combustion analysis. General Chemistry I Dr. Stone Chapter 3 clicker 5

Percent yield Combustion analysis. General Chemistry I Dr. Stone Chapter 3 clicker 5 Percent yield Combustion analysis General Chemistry I Dr. Stone Chapter 3 clicker 5 % Yield = Actual x 100% Theoretical Actual= what is made Theoretical = the amount that could be made from the limiting

More information

CHEMISTRY Matter and Change. Chapter 10: The Mole

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

More information

Chapter No. 1 BASIC CONCEPTS MCQs Q.1 Smallest particle of an element which may or may not have independent existence (a) a molecule (b) an atom (c) an ion (d) an electron Q.2 Swedish chemist J. Berzelius

More information

CHEM UNIT 9: Chemical Reactions and Stoichiometry

CHEM UNIT 9: Chemical Reactions and Stoichiometry CHEM UNIT 9: Chemical Reactions and Stoichiometry http://teachersites.schoolworld.com/webpages/rcummings/ This is a good website that has videos of Mr. Cummings (our Chem. Dept. Head) lecturing on topics.

More information

Many common quantities have names that are used to describe them: Six of something are a half-dozen, and twelve are a dozen.

Many common quantities have names that are used to describe them: Six of something are a half-dozen, and twelve are a dozen. THE MOLE THE MOLE Many common quantities have names that are used to describe them: Two of something are called a pair. Three of something are called a trio. Six of something are a half-dozen, and twelve

More information

Hydrates, Percent Composition, and Empirical and Molecular Formulas

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

More information

THE MOLE (a counting unit)

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

More information

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 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.

More information

Mole Concept. Conversion Factors:

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

More information

Lecture 11 - Stoichiometry. Lecture 11 - Introduction. Lecture 11 - The Mole. Lecture 11 - The Mole. Lecture 11 - The Mole

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

More information

CHAPTER 9 AVOGADRO S NUMBER

CHAPTER 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 information

Chemistry Section Review 7.3

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

More information

ب 3 18 قسم الكيمياء مصطفي عيد

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

More information

Lewis Structures. Difference in electronegativity is greater then 1.7.

Lewis Structures. Difference in electronegativity is greater then 1.7. Lewis Structures Lewis structures can be drawn for:!! Ionic Compounds! Molecular Compounds! Polyatomic Compounds Ionic Compounds Contains metallic and non-metallic ions. Difference in electronegativity

More information

Elements and Compounds

Elements and Compounds Molecules, Compounds, and Chemical Equations Elements and Compounds elements combine to give almost limitless number of compounds C n H n + approx. 10 18 alkane hydrocarbons Chemical Bonds compounds are

More information

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 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

More information

Chemical Reactions. Chapter 17

Chemical 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 information

WELCOME BACK FROM SPRING BREAK

WELCOME 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 information

Summer Review for AP Biology

Summer Review for AP Biology Summer Review for AP Biology These questions are to help you review the knowledge from your previous science classes that you should already know. AP science classes refer to this as previous knowledge

More information

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 =

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

More information

SL Chemistry. Friday August 28th Monday, August 31, 15

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

More information

Chapter 3. Stoichiometry:

Chapter 3. Stoichiometry: Chapter 3. Stoichiometry: Watch Bozeman Videos & other videos on my website for additional help: Big Idea 1: Chemical Analysis Conservation of Atoms Balancing Equations Symbolic Representation Mole Big

More information

Chapter 6 Chemical Bonding

Chapter 6 Chemical Bonding Chapter 6 Chemical Bonding Section 6-1 Introduction to Chemical Bonding Chemical Bonds Valence electrons are attracted to other atoms, and that determines the kind of chemical bonding that occurs between

More information

Stoichiometry. Please take out your notebooks

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.

More information

For a quick and enjoyable introduction to Covalent vs Ionic Bonding watch this video:

For a quick and enjoyable introduction to Covalent vs Ionic Bonding watch this video: Covalent Bonding Covalent Bonding is the result of sharing of electron pairs between 2 nonmetal atoms Caution: sharing can be complicated Recall the Octet Rule: Atoms tend to gain, lose or share valence

More information

UNIT 4: THE MOLE & AVOGADRO

UNIT 4: THE MOLE & AVOGADRO UNIT 4: THE MOLE & AVOGADRO SC.912.P.8.9 Apply the mole concept & Law of Conservation of Mass to calculate the quantities of chemicals SC.912.P.8.7 Interpret formula representations of molecules & compounds

More information

Formula Mass. not all compounds are molecular formula mass calculated exactly the same way as molecular mass. Solid structure of NaCl

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

More information

15.0 g Fe O 2 mol Fe 55.8 g mol Fe = g

15.0 g Fe O 2 mol Fe 55.8 g mol Fe = g CHAPTER Practice Questions.1 1 Mg, O, H and Cl (on each side).. BaCl (aq) + Al (SO ) (aq) BaSO (s) + AlCl (aq).5 0.15 mol 106 g mol 1 = 1. g 15.0 g Fe O mol Fe 55.8 g mol Fe = 10.9 g 1 159.7 g mol FeO

More information

Unit III: Quantitative Composition of Compounds

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

More information

Solutions to the Extra Problems for Chapter 8

Solutions to the Extra Problems for Chapter 8 Solutions to the Extra Problems for Chapter 8. The answer is 83.4%. To figure out percent yield, you first have to determine what stoichiometry says should be made: Mass of MgCl 4.3 amu + 35.45 amu 95.

More information

Topics in composition stoichiometry include the calculation of: Molar mass Percent Composition Molecular formula Empirical formulas

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.

More information

Chemistry. Chapter 17

Chemistry. Chapter 17 Chemistry 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 Balancing Chemical

More information

Chapter 6 Empirical and Molecular Formulas

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.

More information

Lesson 01: Atomic Masses and Avogadro s Hypothesis. 01 Counting Atoms and Molecules

Lesson 01: Atomic Masses and Avogadro s Hypothesis. 01 Counting Atoms and Molecules Chemistry 11, Mole Concept, Unit 04 1 Lesson 01: Atomic Masses and Avogadro s Hypothesis 01 Counting Atoms and Molecules The chemical changes we observe always involve a certain number of atoms that rearrange

More information

9/14/ Chemistry Second Edition Julia Burdge. Stoichiometry: Ratios of Combination. Molecular and Formula Masses

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

More information

- Converting Moles (mol.) to grams (g):

- Converting Moles (mol.) to grams (g): Study Guide: Avogadro's # 1mol = 6.02x10^23 particles/atoms/ions/elephants use this as a conversion factor to calculate atoms in compound 1mol C / 6.02 x 10^23 atoms C Percent composition: [Mass of Element

More information

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

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

More information

7.1 Describing Reactions. Burning is a chemical change. When a substance undergoes a chemical change, a chemical reaction is said to take place.

7.1 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 information

Atoms, Molecules, and the Mole

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

More information

Percent Composition and Empirical Formulas

Percent Composition and Empirical Formulas Percent Composition and Empirical Formulas Content Objectives SWBAT calculate the percent composition by mass of each element in a compound. SWBAT calculate the empirical formula of a compound based on

More information

Table of Contents. 1. FTFs 2. Bingo Chip Activity 3. Moles Worksheet 4. HW Ch 10.1 & Worksheet 10.1 and

Table of Contents. 1. FTFs 2. Bingo Chip Activity 3. Moles Worksheet 4. HW Ch 10.1 & Worksheet 10.1 and Chapter 10: Moles Table of Contents 1. FTFs 2. Bingo Chip Activity 3. Moles Worksheet 4. HW Ch 10.1 & 10.2 5. Worksheet 10.1 and 10.2 6. Bubblegum Lab FTF Day 1 (yes, we are starting a new folder.) Feb.

More information

WJEC England GCSE Chemistry. Topic 3: Chemical formulae, equations and amount of substance. Notes. (Content in bold is for Higher Tier only)

WJEC England GCSE Chemistry. Topic 3: Chemical formulae, equations and amount of substance. Notes. (Content in bold is for Higher Tier only) WJEC England GCSE Chemistry Topic 3: Chemical formulae, equations and amount of substance Notes (Content in bold is for Higher Tier only) charges on ions an ion is formed when an atom loses or gains electrons

More information

L = 6.02 x mol Determine the number of particles and the amount of substance (in moles)

L = 6.02 x mol Determine the number of particles and the amount of substance (in moles) 1.1 The Mole 1.1.1 - Apply the mole concept to substances A mole is the name given to a certain quantity. It represents 6.02 x 10 23 particles. This number is also known as Avogadro's constant, symbolised

More information

Ch 3.3 Counting (p78) One dozen = 12 things We use a dozen to make it easier to count the amount of substances.

Ch 3.3 Counting (p78) One dozen = 12 things We use a dozen to make it easier to count the amount of substances. Ch 3.3 Counting (p78) One dozen = 12 things We use a dozen to make it easier to count the amount of substances. Moles the SI base unit that describes the amount of particles in a substance. Mole is abbreviated

More information

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

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

More information

Composition and formulae. Of moles and men

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

More information

Chapter 3. Stoichiometry: Calculations with Chemical Formulas and Equations

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

More information

1st Semester Review Worth 10% of Exam Score

1st Semester Review Worth 10% of Exam Score 1st Semester Review 2014-2015 Worth 10% of Exam Score Name: P: 1. Which of the following is the correct electron configuration for a neutral atom of oxygen in the ground state? A) 1s 2 2p 4 B) 1s 2 2s

More information

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

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

More information

Unit III: Quantitative Composition of Compounds

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

More information

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. 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

More information

6 atomic # C symbol Carbon name of element atomic mass. o Examples: # 1 mol C = g # 1 mol O = g # 1 mol H = 1.

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

More information

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 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?

More information

Forming Chemical Bonds

Forming Chemical Bonds Forming Chemical Bonds Why do atoms form chemical bonds? so that the system can achieve the lowest possible potential energy Example covalent bonding in H 2 H H Potential energy 0 Distance of separation

More information

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

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

More information

Measuring matter 11.1

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

More information

Unit 5 Percent Composition, Empirical Formulas, and Reactions

Unit 5 Percent Composition, Empirical Formulas, and Reactions Chemistry 1 West Linn High School Unit 5 Packet and Goals Name: Period: Unit 5 Percent Composition, Empirical Formulas, and Reactions Unit Goals: As you work through this unit, you should be able to: 1.

More information

Chapter 3: Water and the Fitness of the

Chapter 3: Water and the Fitness of the Chapter 3: Water and the Fitness of the Environment Concept 3.1 The polarity of water molecules results in hydrogen bonding 1. Study the water molecules at the right. On the central molecule, label oxygen

More information

Moles Homework Unit 6

Moles Homework Unit 6 VOCABULARY For each word, provide a short but specific definition from YOUR OWN BRAIN! No boring textbook definitions. Write something to help you remember the word. Explain the word as if you were explaining

More information

7. How many moles of hydrogen sulfide are contained in a 35.0-g sample of this gas? [A] 2.16 mol [B] 7.43 mol [C] 6.97 mol [D] 10.4 mol [E] 1.

7. How many moles of hydrogen sulfide are contained in a 35.0-g sample of this gas? [A] 2.16 mol [B] 7.43 mol [C] 6.97 mol [D] 10.4 mol [E] 1. 1. Bromine exists naturally as a mixture of bromine-79 and bromine-81 isotopes. An atom of bromine-79 contains [A] 35 protons, 44 neutrons, 35 electrons. [B] 79 protons, 79 electrons, and 35 neutrons.

More information

Counting by mass: The Mole. Unit 8: Quantification of Chemical Reactions. Calculating molar mass. Particles. moles and mass. moles and particles

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

More information

Chapter 9. Chemical Calculations and Chemical Formulas

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

More information

Covalent Molecules and Lewis Structures Time required: two 50-minute periods

Covalent Molecules and Lewis Structures Time required: two 50-minute periods Mega Molecules, LLC!!!!! Name: Hands-On Science with Molecular Models!! Date:!!!!!!!! Hour: Introduction Covalent Molecules and Lewis Structures Time required: two 50-minute periods To study covalent molecules,

More information

Two Types of Reactions. Chemistry Review. Hydronium Ion. Acid-Base Reactions. Acid-Base reactions Oxidation-Reduction reactions

Two Types of Reactions. Chemistry Review. Hydronium Ion. Acid-Base Reactions. Acid-Base reactions Oxidation-Reduction reactions Two Types of Reactions Chemistry Review Acid-Base reactions Oxidation-Reduction reactions Chapter 18 Review Questions Will be EXTRA CREDIT Acid-Base Reactions Hydronium Ion Transfer of hydrogen ions protons

More information

Part 01 - Notes: The Mole and Its Calculations

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

More information

Chapter 3: Molecules, Compounds and Chemical Equations: (continue and finish chapter 3: 8-11)

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

More information

Chemical Calculations: The Mole concept and Chemical Formula. Law of Definite Proportions (John Dalton) Chapter 9

Chemical 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 information

Week 7 & 8: Covalent Compounds. Part 1: Lewis Structures Part 2: Skeleton Structures

Week 7 & 8: Covalent Compounds. Part 1: Lewis Structures Part 2: Skeleton Structures Week 7 & 8: Covalent Compounds Part 1: Lewis Structures Part 2: Skeleton Structures Section 1: Lewis Structures Section 1: Lewis Structures / Objectives After this lesson I can define covalent bonding.

More information

Unit 6 Part 2. Mole Related Calculations

Unit 6 Part 2. Mole Related Calculations Unit 6 Part 2 Mole Related Calculations Several mole related calculations % composition Find the % of each element in a compound Empirical Formula Determine the simplest formula from mass or % composition

More information

6.02 X Memorize this Number

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

More information

Chapter 3. Mass Relationships in Chemical Reactions

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

More information

CHEMICAL QUANTITIES. Chapter Six

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.

More information

GPISD Pre-AP Chemistry 1 st Semester Final Summative Assessment Blueprint

GPISD Pre-AP Chemistry 1 st Semester Final Summative Assessment Blueprint GPISD 201-2016 Pre-AP Chemistry 1 st Semester Final Summative Assessment Blueprint SE Description Number of Questions C.4A C.4D C.B C.C C.6D C.6E C.7A C.7B C.7C C.7E C.8A C.8B C.8C C.8D TOTAL: C.4(A) Differentiate

More information

Name. Final empirical ratio. Multiply until whole. Element Mass Molar mass moles Mole ratio 12.01g/mol

Name. Final empirical ratio. Multiply until whole. Element Mass Molar mass moles Mole ratio 12.01g/mol EMPIRIAL FRMULA WRKSEET Problems that involve percentages, mass or moles of elements: Follow the poem. Show your work. Fill in the chart. Sometimes, the multiplier is 1. After awhile, you will not need

More information

Calculations with Chemical Formulas and Equations

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

More information

Chemistry 217 Problem Set 1

Chemistry 217 Problem Set 1 hemistry 217 Problem Set 1 Recommended Problems from the Book (1 st ed. in parentheses): 1.1, 1.3-1.9, 1.36-1.42, 1.57-1.62 (1.1-1.8, 1.34-1.40, 1.54-1.58) Supplemental Problems: Lewis structures: Weeks,

More information

What determines whether a substance will be a solid, liquid, or gas? Thursday, April 24, 14

What determines whether a substance will be a solid, liquid, or gas? Thursday, April 24, 14 What determines whether a substance will be a solid, liquid, or gas? Answer: The attractive forces that exists between its particles. Answer: The attractive forces that exists between its particles. For

More information

Metallic Bonds MOLECULES AND REACTIONS. Metallic Properties. Metallic Alloys. Mobility of electrons results in many properties of metals.

Metallic Bonds MOLECULES AND REACTIONS. Metallic Properties. Metallic Alloys. Mobility of electrons results in many properties of metals. Metallic Bonds MOLECULES AND REACTIONS Nucleus of metal atoms only weakly hold outer Weak attraction allows the to move from one atom to another quite freely Chapter 15, 17 Metallic Properties Mobility

More information

Molar Calculations - Lecture Notes for Chapter 6. Lecture Notes Chapter Introduction

Molar 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 information

Honors Chemistry Semester 1 Final Review

Honors Chemistry Semester 1 Final Review Honors Chemistry Semester 1 Final Review Ch. 1 Introduction to Chemistry Chemistry: its branches, technology, scientific method, and problem solving. 1. Know the definition of matter. 2. Know the definition

More information

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

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

More information

NCSD HIGH SCHOOL CHEMISTRY SCOPE AND SEQUENCE

NCSD HIGH SCHOOL CHEMISTRY SCOPE AND SEQUENCE UNIT Atomic Structure & Properties Periodic Table Bonding Chemical Reactions Moles / Stoichiometry Acids and Bases 15 Days 11 Days 16 Days 16 Days 26 Days 9 Days S T A N D A R D S H.1P.1 Explain how atomic

More information

Memorize: Understand: Know how to:

Memorize: Understand: Know how to: NAME: CLASS PERIOD: REVIEW FOR HONORS CHEMISTRY SEMESTER 1 EXAM Memorize: Understand: Know how to: 1 SI units for different measurements (length, volume, number, mass, temperature, density) Definition

More information

The Next Generation Science Standards (NGSS)

The Next Generation Science Standards (NGSS) The Next Generation Science Standards (NGSS) CHAPTER 4, LESSON 1: PROTONS, NEUTRONS, AND ELECTRONS HS-PS1-1. Use the periodic table as a model to predict the relative properties of elements based on the

More information

Lecture Notes Chapter 6

Lecture 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 information

A Getting-It-On Review and Self-Test Formulas and Equations

A Getting-It-On Review and Self-Test Formulas and Equations A Getting-It-On Review and Self-Test Formulas and Equations The mole is defined as a (1) of things. To three significant figures, this number has the value (2). Atomic weights are based on a mole of (3).

More information

HONORS CHEMISTRY Putting It All Together II

HONORS CHEMISTRY Putting It All Together II NAME: SECTION: HONORS CHEMISTRY Putting It All Together II Calculations in Chemistry It s time to pull out your calculators! In the first review sheet, you were able to write formulas of compounds when

More information

Molecular Structure and Bonding. Assis.Prof.Dr.Mohammed Hassan Lecture 2

Molecular Structure and Bonding. Assis.Prof.Dr.Mohammed Hassan Lecture 2 Molecular Structure and Bonding Assis.Prof.Dr.Mohammed Hassan Lecture 2 Lewis structures: Lewis Theory The octet rule All elements except hydrogen ( hydrogen have a duet of electrons) have octet of electrons

More information

Review of Chemistry 11

Review of Chemistry 11 Review of Chemistry 11 HCl C 3 H 8 SO 2 NH 4 Cl KOH H 2 SO 4 H 2 O AgNO 3 PbSO 4 H 3 PO 4 Ca(OH) 2 Al(OH) 3 P 2 O 5 Ba(OH) 2 CH 3 COOH 1. Classify the above as ionic or covalent by making two lists. Describe

More information

Molecular vs. Empirical Formula Chemistry H 2 O H 2 O 2. NaCl

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

More information

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: 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 information

Proportions to find moles Correctly organized Example. Problem

Proportions to find moles Correctly organized Example. Problem Reactions continued And chemical review!! Steps to find grams in chemical Balance the equation to get molar ratios Find molar mass of the substances in question Find moles of the one given in grams Set

More information