MODERN CHEMISTRY. 8. What is the formula for aluminum sulfate? 9. What is the formula for barium hydroxide?

Size: px
Start display at page:

Download "MODERN CHEMISTRY. 8. What is the formula for aluminum sulfate? 9. What is the formula for barium hydroxide?"

Transcription

1 MODERN CHEMISTRY Date Name Period Multiple Choice - Identify the choice that best completes the statement or answers the question. Use answer-key worksheet (Page 6) to key in answers to questions. 1. A chemical formula includes the symbols of the elements in the compound and subscripts that indicate a) atomic mass of each element. b) number of atoms or ions of each element that are combined in the compound. c) formula mass. d) charges on the elements or ions. 2. A chemical formula for a molecular compound represents the composition of a) a molecule; b) an atom; c) the ions that make up the compound; or d) the crystal lattice. 3. How many atoms of fluorine are present in a molecule of carbon tetrafluoride, CF 4? a) 1; b) 2; c) 4 or d) 5 4. The formula for carbon dioxide, CO 2, can represent a) one molecule of carbon dioxide. b) 1 mol of carbon dioxide molecules. c) the combination of 1 atom of carbon and 2 atoms of oxygen. d) all of the above. 5. What is the formula for zinc fluoride? a) ZnF; b) ZnF 2; c) Zn 2F; or d) Zn 2F 3 6. What is the formula for the compound formed by calcium ions and chloride ions? a) CaCl; b) Ca 2Cl; c) CaCl 3; or d) CaCl 2 7. What is the formula for the compound formed by lead(ii) ions and chromate ions? a) PbCrO 4; b) Pb 2CrO 4; c) Pb 2(CrO 4) 3; or d) Pb(CrO 4) 2 8. What is the formula for aluminum sulfate? a) AlSO 4; b) Al 2SO 4; c) Al 2(SO 4) 3; or d) Al(SO 4) 3 9. What is the formula for barium hydroxide? a) BaOH; b) BaOH 2; c) Ba(OH) 2; or d) Ba(OH) 10. Name the compound Ni(ClO 3) 2. a) nickel(ii) chlorate; b) nickel(ii) chloride; c) nickel(ii) chlorite; or d) nickel(ii) peroxide 11. Name the compound Zn 3(PO 4) 2. a) zinc potassium oxide; b) trizinc polyoxide; c) zinc phosphate; or d) zinc phosphite 12. Name the compound KClO 3. a) potassium chloride; b) potassium trioxychlorite; c) potassium chlorate; or d) hypochlorite 13. Name the compound Fe(NO 3) 2. a) iron(ii) nitrate; b) iron(ii) nitrite; c) iron(iii) nitrate; or d) iron(iii) nitride 14. Name the compound Al 2S 3. a) aluminum sulfate; b) aluminum sulfur; c) aluminum(ii) sulfate; or d) aluminum sulfide 15. Name the compound CF 4. a) calcium fluoride; b) carbon fluoride: c) carbon tetrafluoride; or d) monocalcium quadrafluoride 16. Name the compound SiO 2. a) silver oxide b) silicon oxide; c) silicon dioxide; or d) monosilver dioxide 17. Name the compound SO 3. a) sulfur trioxide; b) silver trioxide; c) selenium trioxide; or d) sodium trioxide MODERN CHEMISTRY 1 0F 6 CHAPTER 7 QUIZ AND CHAPTER REVIEW

2 18. Name the compound N 2O 3. a) dinitrogen oxide; b) nitrogen trioxide; c) nitric oxide; or d) dinitrogen trioxide 19. What is the formula for silicon dioxide? a) SO 2; b) SiO 2; c) Si 2O; or d) S 2O 20. What is the formula for dinitrogen trioxide? a) Ni 2O 3; b) NO 3; c) N 2O 6; or d) N 2O What is the formula for sulfur dichloride? a) SCl; ). SCl 2; c) S 2Cl; or d) S 2Cl What is the formula for diphosphorus pentoxide? a) P 2PeO 5; b. PO 5 ; c. P 2O 4; or d. P 2O What is the formula for hydrochloric acid? a) HF b) HCl c) HClO d) H 2CO The oxidation number of fluorine is a) always 0; b) 1 in all compounds; c) +1 in all compounds; or d) equal to the negative charge of all the metal ions in a compound. 25. What is the oxidation number of oxygen in most compounds? a) 8; b) -2; c) 0; or d) What is the oxidation number of a pure element? a) 1; b) 0; c) +1; or d) In a compound, the algebraic sum of the oxidation numbers of all atoms equals a) 0; b) 1: c) 8; or d) the charge on the compound. 28. What is the oxidation number of hydrogen in compounds containing metals? a) 1; b) 0; c) +1; or d) the charge on the metal ion 29. In a polyatomic ion, the algebraic sum of the oxidation numbers of all atoms is equal to a) 0; b) the number of atoms in the ion; c) 10; or d) the charge of the ion. 30. What is the oxidation number of oxygen in H 2O 2? a) 2; b) -1; c) +2; or d) What is the oxidation number of hydrogen in KH? a) 1; b) 0; c) +1; or d) What is the oxidation number of hydrogen in H 2O? a) 0; b) +1; c) +2; or d) What is the oxidation number of sulfur in SO 2? a) 0; b) +1; c) +2; or d) What is the oxidation number of sulfur in H 2SO 4? a) 2; b) 0; c) +4; or d) What is the oxidation number of oxygen in CO 2? a) 4; b) -2; c) 0; or d) Name the compound N 2O 2 using the Stock system. a) dinitrogen monoxide; b) nitrogen dioxide; ); nitrogen(ii) oxide; d) nitrogen oxide(ii) 37. Name the compound SO 2 using the Stock system. a) sulfur(ii) oxide; b) sulfur(iv) oxide; c) sulfur dioxide; d) sulfur oxide 38. Name the compound CCl 4 using the Stock system. a) carbon(iv) chloride; b) carbon tetrachloride; c) carbon chloride; or d) carbon hypochlorite 39. Name the compound H 2O using the Stock system. a) water; b) hydrogen dioxide; c) hydrogen(i) oxide; or d) hydrogen(ii) oxide 40. Name the compound CO 2 using the Stock system. a) carbon(iv) oxide; b) carbon dioxide; c) monocarbon dioxide; or d) carbon oxide MODERN CHEMISTRY 2 0F 6 CHAPTER 7 QUIZ AND CHAPTER REVIEW

3 41. Name the compound PBr 5 using the Stock system. a) potassium hexabromide; b) phosphorus(v) pentabromide; c) phosphorus(v) bromide; or d) phosphoric acid 42. The molar mass of an element is the mass of one a) atom of the element; b. crystal of the element.; c) gram of the element; or d) mole of the element. 43. What is the sum of the atomic masses of all the atoms in a formula for a compound? a) molecular mass; b) formula mass; c) atomic mass; or d) actual mass 44. What is the formula mass of magnesium chloride, MgCl 2? a) 46 amu; b) amu; c) amu; or d) amu 45. What is the formula mass of ethyl alcohol, C 2H 5OH? a) amu; b) amu; c) amu; or d) amu 46. What is the formula mass of (NH 4) 2SO 4? a) amu; b) amu; c) amu; or d) amu 47. The molar mass of MgI 2 is a) the sum of the masses of 1 mol of Mg and 2 mol of I. b) the sum of the masses of 1 mol of Mg and 1 mol of I. c) the sum of the masses of 1 atom of Mg and 2 atoms of I. d) the sum of the masses of 1 atom of Mg and 1 atom of I. 48. The molar mass of NO 2 is g/mol. How many moles of NO 2 are present in g? a) mol; b) mol; c; mol; or d) mol 49. The molar mass of CCl 4 is g/mol. How many grams of CCl 4 are needed to have mol? a) 5 g; b) g; c) g; or d) g 50. The molar mass of H 2O is g/mol. How many grams of H 2O are present in 0.20 mol? a) 0.2 g; b) 3.6 g; c) 35.9 g; or d g 51. The molar mass of LiF is g/mol. How many moles of LiF are present in g? a) mol; b) mol; c) mol; or d mol 52. The molar mass of CS 2 is g/mol. How many grams of CS 2 are present in mol? a) 0.13 g; b) g; c) g; or d) g 53. The molar mass of NH 3 is g/mol. How many moles of NH 3 are present in g? a) mol; b) mol; c) mol; or d) mol 54. What is the mass of mol glucose, C 6H 12O 6? a) 24.0 g; b) 43.2 g; c) g; or d) 750. g 55. How many Cl - ions are present in 2.00 mol of KCl? a) 1.20 x ; b) 6.02 x ; c) 2.00; or d) How many OH - ions are present in 3.00 mol of Ca(OH) 2? a) 3.00; b) 6.00; c x ; or d) 2.06 x How many oxygen atoms are there in mol of CO 2? a) 6.02 x10 23 ; b) 3.01 x ; c) ; or d) How many Mg 2+ ions are found in 1.00 mol of MgO? a) 3.01 x ; b) 6.02 x ; c x ; or d) 6.02 x If mol of Na + combines with mol of Cl - to form NaCl, how many formula units of NaCl are present? a) 3.01 x ; b) 6.02 x ; c) 6.02 x ; or d) How many molecules are there in 5.0 g of methyl alcohol, CH 3OH? a) 9.4 x ; b) 3.0 x ; c) 3.6 x ; or d) 3.8 x10 24 MODERN CHEMISTRY 3 0F 6 CHAPTER 7 QUIZ AND CHAPTER REVIEW

4 61. What is the percentage composition of CF 4? a) 20% C, 80% F; b) 13.6% C, 86.4% F; c) 16.8% C, 83.2% F; or d) 81% C, 19% F 62. What is the percentage composition of CO? a) 50%; C, 50% O; b) 12% C, 88% O; c) 25% C, 75% O; or d. 43% C, 57% O 63. What is the percentage composition of CuCl 2? a) 33% Cu, 66% Cl; b) 50% Cu, 50% Cl; c) 65.50% Cu, 34.50% Cl; or d) 47.27% Cu, 52.73% Cl 64. The percentage composition of sulfur in SO 2 is about 50%. What is the percentage of oxygen in this compound? a) 25%; b) 50%; c) 75%; or d) 90% 65. What is the mass percentage of OH - in Ca(OH) 2? a) 45.9%; b) 66.6%; c) 75%; or d) 90.1% 66. What is the mass percentage of chlorine in NaCl? a) 35.45%; b) 50%; c) 60.7%; or d) 64.5% 67. A formula that shows the simplest whole-number ratio of the atoms in a compound is the a) molecular formula; b) ideal formula; c) experimental formula; or d) empirical formula. 68. The empirical formula is always the accepted formula for a(n) a) atom; b) molecule; c) molecular compound; or d) ionic compound. 69. The empirical formula for a compound shows the symbols of the elements with subscripts indicating the a) actual numbers of atoms in a molecule. b) number of moles of the compound in 100 g. c) smallest whole-number ratio of the atoms. d) atomic masses of each element. 70. The empirical formula may not represent the actual composition of a unit of a(n) a) ionic compound; b) molecular compound; c) salt; or d) crystal. 71. What is the empirical formula for a compound that is 31.9% potassium, 28.9% chlorine, and 39.2% oxygen? a) KClO 2; b) KClO 3; c) K 2Cl 2O 3; or d) K2Cl2O5 72. What is the empirical formula for a compound that is 43.6% phosphorus and 56.4% oxygen? a) P 2O 7; b) PO 3; c) P 2O 3; or d) P 2O What is the empirical formula for a compound that is 53.3% O and 46.7% Si? a) SiO; b) SiO 2; c) Si 2O; or d) Si 2O A compound contains g of F and 40.8 g of C. What is the empirical formula for this compound? a) CF 4; b) C 4F; c) CF; or d) CF A compound contains 64 g of O and 8 g of H. What is the empirical formula for this compound? a. H 2O; b) H 2O 2; c) HO 2; or d) HO 76. What is the empirical formula for a compound that is 36.1% Ca and 63.9% Cl? a) CaCl; b) Ca 2Cl; c) CaCl 2; or d. Ca 2Cl A compound contains 27.3 g of C and 72.7 g of O. What is the empirical formula for this compound? a) CO; b) CO 2; c) C 2O; or d) C 2O To find the molecular formula from the empirical formula, one must determine the compound's a) density; b) formula mass; c) structural formula; or d) crystal lattice. MODERN CHEMISTRY 4 0F 6 CHAPTER 7 QUIZ AND CHAPTER REVIEW

5 79. A molecular compound has the empirical formula XY 3. Which of the following is a possible molecular formula? a) X 2Y 3; b) XY 4; c) X 2Y 5; or d) X 2Y The molecular formula for vitamin C is C 6H 8O 6. What is the empirical formula? a) CHO; b) CH 2O; c) C 3H 4O 3; or d) C 2H 4O Of the following molecular formulas for hydrocarbons, which is an empirical formula? a) CH 4; b) C 2H 2; c) C 3H 6; or d) C 4H Which of the following molecular formulas does not have the corresponding empirical formula XY 2Z? a) X 2Y 4Z 2; b) XYZ; c) X 6Y 12Z 6; or d) X 3Y 6Z A compound's empirical formula is C 2H 5. If the formula mass is 58 amu, what is a) C 3H 6; b) C 4H 10; c) C 5H 8; or d) C 5H A compound's empirical formula is N 2O 5. If the formula mass is 108 amu, what is a) N 2O 5; b) N 40O 10; c) NO 3; or d) N 2O A compound's empirical formula is CH. If the formula mass is 26 amu, what is a) C 2H 2; b) CH 3; c) CH 4; or d) C 4H 86. A compound's empirical formula is NO 2. If the formula mass is 92 amu, what is a) NO b) N 2O 2; c) NO 4; or d) N 2O A compound's empirical formula is CH 3. If the formula mass is 30 amu, what is a) CH 3; b) CH 4; c) C 2H 6; or d) C 3H A compound's empirical formula is HO. If the formula mass is 34 amu, what is a) H 2O; b) H 2O 2; c) HO 3; or d) H 2O What is the molecular formula of a compound that has a formula mass of amu and an empirical formula of CH 3Cl? a) CHCl; b) CH 2Cl; c) CH 3Cl; or d) CH 2Cl The molar mass of aluminum is g/mol and the molar mass of fluorine is g/mol. The molar mass of aluminum trifluoride, AlF 3 is a) g/mol; b) g/mol; c) g/mol; or d) g/mol 92. The molar mass of copper is g/mol, the molar mass of sulfur is g/mol, and the molar mass of oxygen is g/mol. The molar mass of copper(ii) sulfate, CuSO 4 is a) g/mol; b) g/mol; c) g/mol; or d) g/mol 93. The molar mass of iron is g/mol, the molar mass of silicon is g/mol, and the molar mass of oxygen is g/mol. The molar mass of iron(ii) silicate, Fe 2SiO 4 is a) g/mol; b) g/mol; c) g/mol; or d) g/mol 94. The molar mass of aluminum is g/mol and the molar mass of oxygen is g/mol. The molar mass of Al 2O 3 is a) g/mol; b) g/mol; c) g/mol; or d) g/mol 95. The name for the CrO 4 ion is a) Chromite; b) Carbon reduced Oxygen (IV); c) Chromate; or d) Chromogenn 96. The name for the NO 3- ion is a) Nitrite; b) Nitrous; c) Nitrate; or d) Nitride MODERN CHEMISTRY 5 0F 6 CHAPTER 7 QUIZ AND CHAPTER REVIEW

6 Chapter 7 Worksheet Activity Answers Key Answers (1-32) (a, b, c, or d) Answers (33-64) (a, b, c, or d) Question Question Question Answers (65-96) (a, b, c, or d) MODERN CHEMISTRY 6 0F 6 CHAPTER 7 QUIZ AND CHAPTER REVIEW

Study Guide For Chapter 7

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

More information

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

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

More information

WRITING CHEMICAL FORMULA

WRITING CHEMICAL FORMULA WRITING CHEMICAL FORMULA For ionic compounds, the chemical formula must be worked out. You will no longer have the list of ions in the exam (like at GCSE). Instead you must learn some and work out others.

More information

Monatomic Ions. A. Monatomic Ions In order to determine the charge of monatomic ions, you can use the periodic table as a guide:

Monatomic Ions. A. Monatomic Ions In order to determine the charge of monatomic ions, you can use the periodic table as a guide: Monatomic Ions Ions are atoms that have either lost or gained electrons. While atoms are neutral, ions are charged particles. A loss of electrons results in a positive ion or cation (pronounced cat-eye-on

More information

Name: Block: Date: Test Review: Chapter 8 Ionic Bonding

Name: Block: Date: Test Review: Chapter 8 Ionic Bonding Name: Block: Date: Test Review: Chapter 8 Ionic Bonding Part 1: Fill-in-the-blank. Choose the word from the word bank below. Each word may be used only 1 time. electron dot structure metallic electronegativity

More information

Sample Exercise 2.1 Illustrating the Size of an Atom

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

More information

Nomenclature Packet. 1. Name the following ionic compounds: a. Al 2 O 3 Aluminum oxide. b. Cs 2 O Cesium oxide. c. Rb 3 N Rubidium nitride

Nomenclature Packet. 1. Name the following ionic compounds: a. Al 2 O 3 Aluminum oxide. b. Cs 2 O Cesium oxide. c. Rb 3 N Rubidium nitride Nomenclature Packet Worksheet I: Binary Ionic Compounds (representative metals) metals from groups 1A, 2A, and 3A (1, 2, and 13) have constant charges as ions and do NOT get Roman Numerals in their names

More information

Moles, Molecules, and Grams Worksheet Answer Key

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

More information

Molar Mass Worksheet Answer Key

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

More information

W1 WORKSHOP ON STOICHIOMETRY

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

More information

Stoichiometry Review

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

More information

MOLECULAR MASS AND FORMULA MASS

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

More information

Balancing Chemical Equations Worksheet

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

More information

Naming Compounds. There are three steps involved in naming ionic compounds- naming the cation, naming the anion, and naming the entire compound.

Naming Compounds. There are three steps involved in naming ionic compounds- naming the cation, naming the anion, and naming the entire compound. Naming Compounds Naming compounds is an important part of chemistry. Most compounds fall in to one of three categories ionic compounds, molecular compounds, or acids. Part One: Naming Ionic Compounds Identifying

More information

Moles. Moles. Moles. Moles. Balancing Eqns. Balancing. Balancing Eqns. Symbols Yields or Produces. Like a recipe:

Moles. Moles. Moles. Moles. Balancing Eqns. Balancing. Balancing Eqns. Symbols Yields or Produces. Like a recipe: Like a recipe: Balancing Eqns Reactants Products 2H 2 (g) + O 2 (g) 2H 2 O(l) coefficients subscripts Balancing Eqns Balancing Symbols (s) (l) (aq) (g) or Yields or Produces solid liquid (pure liquid)

More information

Chapter 4 Compounds and Their Bonds

Chapter 4 Compounds and Their Bonds Chapter 4 Compounds and Their Bonds 4.1 Octet Rule and Ions Octet Rule An octet is 8 valence electrons. is associated with the stability of the noble gases. He is stable with 2 valence electrons (duet).

More information

CHEMICAL NAMES AND FORMULAS

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

More information

Nomenclature of Ionic Compounds

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

More information

MOLES AND MOLE CALCULATIONS

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

More information

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

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

More information

Chapter 3 Mass Relationships in Chemical Reactions

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

More information

CHAPTER 5: MOLECULES AND COMPOUNDS

CHAPTER 5: MOLECULES AND COMPOUNDS CHAPTER 5: MOLECULES AND COMPOUNDS Problems: 1-6, 9-13, 16, 20, 31-40, 43-64, 65 (a,b,c,e), 66(a-d,f), 69(a-d,f), 70(a-e), 71-78, 81-82, 87-96 A compound will display the same properties (e.g. melting

More information

Oxidation States of Nitrogen

Oxidation States of Nitrogen Oxidation States of Nitrogen HNO 3 NH 3 HNO 2 NO N 2 O N 2 HN 3 N 2 H 5 + +3 +2 +1 0-1/3-2 Oxidation +5-3 Reduction Oxidation States of Chlorine HClO 4 HClO 3 ClO 2 HClO 2 HClO Cl 2 HCl +5 +4 +3 +1 0 Oxidation

More information

Exercise 3.5 - Naming Binary Covalent Compounds:

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

More information

Moles. Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations

Moles. Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations Moles Balanced chemical equations Molar ratios Mass Composition Empirical and Molecular Mass Predicting Quantities Equations Micro World atoms & molecules Macro World grams Atomic mass is the mass of an

More information

Chapter 3. Molecules, Compounds and Chemical Equations

Chapter 3. Molecules, Compounds and Chemical Equations 3. Molecules, Compounds and Chemical Equations Stoichiometry Mole concept and Avogadro s Number Determining Chemical Formulas Name Compound Balancing Chemical Reactions Yields Solutions and Stoichiometry

More information

19.2 Chemical Formulas

19.2 Chemical Formulas In the previous section, you learned how and why atoms form chemical bonds with one another. You also know that atoms combine in certain ratios with other atoms. These ratios determine the chemical formula

More information

PART I: MULTIPLE CHOICE (30 multiple choice questions. Each multiple choice question is worth 2 points)

PART I: MULTIPLE CHOICE (30 multiple choice questions. Each multiple choice question is worth 2 points) CHEMISTRY 123-07 Midterm #1 Answer key October 14, 2010 Statistics: Average: 74 p (74%); Highest: 97 p (95%); Lowest: 33 p (33%) Number of students performing at or above average: 67 (57%) Number of students

More information

Chemistry Post-Enrolment Worksheet

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

More information

Chapter 5. Chapter 5. Naming Ionic Compounds. Objectives. Chapter 5. Chapter 5

Chapter 5. Chapter 5. Naming Ionic Compounds. Objectives. Chapter 5. Chapter 5 Objectives Name cations, anions, and ionic compounds. Write chemical formulas for ionic compounds such that an overall neutral charge is maintained. Explain how polyatomic ions and their salts are named

More information

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

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

More information

Chapter 8 How to Do Chemical Calculations

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

More information

Unit 9 Stoichiometry Notes (The Mole Continues)

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

More information

Naming Compounds Handout Key

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

More information

Unit 10A Stoichiometry Notes

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

More information

Ch. 10 The Mole I. Molar Conversions

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

More information

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

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

More information

NAMING QUIZ 3 - Part A Name: 1. Zinc (II) Nitrate. 5. Silver (I) carbonate. 6. Aluminum acetate. 8. Iron (III) hydroxide

NAMING QUIZ 3 - Part A Name: 1. Zinc (II) Nitrate. 5. Silver (I) carbonate. 6. Aluminum acetate. 8. Iron (III) hydroxide NAMING QUIZ 3 - Part A Name: Write the formulas for the following compounds: 1. Zinc (II) Nitrate 2. Manganese (IV) sulfide 3. Barium permanganate 4. Sulfuric acid 5. Silver (I) carbonate 6. Aluminum acetate

More information

Elements and Compounds. Chemical Bonds compounds are made of atoms held together by chemical bonds bonds are forces of attraction between atoms

Elements and Compounds. Chemical Bonds compounds are made of atoms held together by chemical bonds bonds are forces of attraction between atoms Elements and Compounds elements combine together to make an almost limitless number of compounds the properties of the compound are totally different from the constituent elements Tro, Chemistry: A Molecular

More information

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

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

More information

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

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

More information

Mole Notes.notebook. October 29, 2014

Mole Notes.notebook. October 29, 2014 1 2 How do chemists count atoms/formula units/molecules? How do we go from the atomic scale to the scale of everyday measurements (macroscopic scale)? The gateway is the mole! But before we get to the

More information

Calculation of Molar Masses. Molar Mass. Solutions. Solutions

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

More information

CHAPTER 3 Calculations with Chemical Formulas and Equations. atoms in a FORMULA UNIT

CHAPTER 3 Calculations with Chemical Formulas and Equations. atoms in a FORMULA UNIT CHAPTER 3 Calculations with Chemical Formulas and Equations MOLECULAR WEIGHT (M. W.) Sum of the Atomic Weights of all atoms in a MOLECULE of a substance. FORMULA WEIGHT (F. W.) Sum of the atomic Weights

More information

Naming Ionic Compounds

Naming Ionic Compounds Naming Ionic Compounds I. Naming Ions A. Cations (+ions) 1. Element name followed by "ion" (when in Group IA, IIA, Al 3+, Ga 3+, Zn 2+, Cd 2+, Ag +, Ni 2+ ). Na + sodium ion, K + potassium ion, Al 3+ aluminum

More information

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

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

More information

Unit 4 Conservation of Mass and Stoichiometry

Unit 4 Conservation of Mass and Stoichiometry 9.1 Naming Ions I. Monatomic Ions A. Monatomic ions 1. Ions formed from a single atom Unit 4 Conservation of Mass and Stoichiometry B. Naming Monatomic Ions 1. Monatomic cations are a. Identified by the

More information

Periodic Table, Valency and Formula

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

More information

Topic 4 National Chemistry Summary Notes. Formulae, Equations, Balancing Equations and The Mole

Topic 4 National Chemistry Summary Notes. Formulae, Equations, Balancing Equations and The Mole Topic 4 National Chemistry Summary Notes Formulae, Equations, Balancing Equations and The Mole LI 1 The chemical formula of a covalent molecular compound tells us the number of atoms of each element present

More information

CHEMICAL FORMULAS AND FORMULA WEIGHT CALCULATIONS

CHEMICAL FORMULAS AND FORMULA WEIGHT CALCULATIONS CHEMICAL FORMULAS AND FORMULA WEIGHT CALCULATIONS 1. THE MEANING OF A CHEMICAL FORMULA A chemical formula is a shorthand method of representing the elements in a compound. The formula shows the formulas

More information

Chemistry Final Study Guide

Chemistry Final Study Guide Name: Class: Date: Chemistry Final Study Guide Multiple Choice Identify the choice that best completes the statement or answers the question. 1. The electrons involved in the formation of a covalent bond

More information

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

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

More information

CHEM 1411 General Chemistry I Practice Problems, Chapters 1 3

CHEM 1411 General Chemistry I Practice Problems, Chapters 1 3 CHEM 1411 General Chemistry I Practice Problems, Chapters 1 3 Chapter 1 Chemistry: The Study of Change 1. Element, compound, homogeneous mixture (solution), or heterogeneous mixture: a) orange juice b)

More information

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

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

More information

= 11.0 g (assuming 100 washers is exact).

= 11.0 g (assuming 100 washers is exact). CHAPTER 8 1. 100 washers 0.110 g 1 washer 100. g 1 washer 0.110 g = 11.0 g (assuming 100 washers is exact). = 909 washers 2. The empirical formula is CFH from the structure given. The empirical formula

More information

ATOMS. Multiple Choice Questions

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

More information

7) How many electrons are in the second energy level for an atom of N? A) 5 B) 6 C) 4 D) 8

7) How many electrons are in the second energy level for an atom of N? A) 5 B) 6 C) 4 D) 8 HOMEWORK CHEM 107 Chapter 3 Compounds Putting Particles Together 3.1 Multiple-Choice 1) How many electrons are in the highest energy level of sulfur? A) 2 B) 4 C) 6 D) 8 2) An atom of phosphorous has how

More information

Chapter 3 Stoichiometry

Chapter 3 Stoichiometry Chapter 3 Stoichiometry 3-1 Chapter 3 Stoichiometry In This Chapter As you have learned in previous chapters, much of chemistry involves using macroscopic measurements to deduce what happens between atoms

More information

Chemical Calculations: Formula Masses, Moles, and Chemical Equations

Chemical Calculations: Formula Masses, Moles, and Chemical Equations Chemical Calculations: Formula Masses, Moles, and Chemical Equations Atomic Mass & Formula Mass Recall from Chapter Three that the average mass of an atom of a given element can be found on the periodic

More information

Nomenclature and Formulas of Ionic Compounds. Section I: Writing the Name from the Formula

Nomenclature and Formulas of Ionic Compounds. Section I: Writing the Name from the Formula Purpose: Theory: Nomenclature and Formulas of Ionic Compounds 1. To become familiar with the rules of chemical nomenclature, based on the classification of compounds. 2. To write the proper name of the

More information

Solution. Practice Exercise. Concept Exercise

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

More information

Chapter 1 The Atomic Nature of Matter

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

More information

Rules for Naming and Writing Compounds

Rules for Naming and Writing Compounds Rules for Naming and Writing Compounds I. Ionic Bonds bonding between a metal and nonmetal or the bond between a positive ion and a negative ion forming a binary compound. end in the suffix "ide" Or bonding

More information

Name period Unit 3 worksheet

Name period Unit 3 worksheet Name period Unit 3 worksheet Read chapter 8, 2.52.7 1. Explain the difference between metallic, ionic, and covalent bonding Metallic cations share a sea of electrons Ionic atoms give and take electrons

More information

neutrons are present?

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

More information

b. N 2 H 4 c. aluminum oxalate d. acetic acid e. arsenic PART 2: MOLAR MASS 2. Determine the molar mass for each of the following. a. ZnI 2 b.

b. N 2 H 4 c. aluminum oxalate d. acetic acid e. arsenic PART 2: MOLAR MASS 2. Determine the molar mass for each of the following. a. ZnI 2 b. CHEMISTRY DISCOVER UNIT 5 LOTS OF PRACTICE ON USING THE MOLE!!! PART 1: ATOMIC MASS, FORMULA MASS, OR MOLECULAR MASS 1. Determine the atomic mass, formula mass, or molecular mass for each of the following

More information

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

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

More information

CHEMICAL REACTIONS. Chemistry 51 Chapter 6

CHEMICAL REACTIONS. Chemistry 51 Chapter 6 CHEMICAL REACTIONS A chemical reaction is a rearrangement of atoms in which some of the original bonds are broken and new bonds are formed to give different chemical structures. In a chemical reaction,

More information

The Mole. Chapter 2. Solutions for Practice Problems

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

More information

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

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

More information

Chapter 4: Nonionic Compounds and Their Nomenclature

Chapter 4: Nonionic Compounds and Their Nomenclature 50 Chapter 4: Nonionic Compounds and Their Nomenclature A nonionic compound is a substance composed of atoms held together by chemical bonding forces, called covalent bonds. Covalent bonds are formed by

More information

Tutorial 2 FORMULAS, PERCENTAGE COMPOSITION, AND THE MOLE

Tutorial 2 FORMULAS, PERCENTAGE COMPOSITION, AND THE MOLE T-6 Tutorial 2 FORMULAS, PERCENTAGE COMPOSITION, AND THE MOLE FORMULAS: A chemical formula shows the elemental composition of a substance: the chemical symbols show what elements are present and the numerical

More information

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

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

More information

Solution. Practice Exercise. Concept Exercise

Solution. Practice Exercise. Concept Exercise Example Exercise 8.1 Evidence for a Reaction Which of the following is experimental evidence for a chemical reaction? (a) Pouring vinegar on baking soda gives foamy bubbles. (b) Mixing two solutions produces

More information

Name Class Date. Section: Calculating Quantities in Reactions. Complete each statement below by writing the correct term or phrase.

Name Class Date. Section: Calculating Quantities in Reactions. Complete each statement below by writing the correct term or phrase. Skills Worksheet Concept Review Section: Calculating Quantities in Reactions Complete each statement below by writing the correct term or phrase. 1. All stoichiometric calculations involving equations

More information

IB Chemistry. DP Chemistry Review

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

More information

Problem Solving. Percentage Composition

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

More information

1. What is the molecular formula of a compound with the empirical formula PO and a gram-molecular mass of 284 grams?

1. What is the molecular formula of a compound with the empirical formula PO and a gram-molecular mass of 284 grams? Name: Tuesday, May 20, 2008 1. What is the molecular formula of a compound with the empirical formula PO and a gram-molecular mass of 284 grams? 2 5 1. P2O 5 3. P10O4 2. P5O 2 4. P4O10 2. Which substance

More information

Molecules, Compounds, and Chemical Equations (Chapter 3)

Molecules, Compounds, and Chemical Equations (Chapter 3) Molecules, Compounds, and Chemical Equations (Chapter 3) Chemical Compounds 1. Classification of Elements and Compounds Types of Pure Substances (Figure 3.4) Elements -- made up of only one type of atom

More information

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

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

More information

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

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

More information

Polyatomic ions can form ionic compounds just as monatomic ions.

Polyatomic ions can form ionic compounds just as monatomic ions. 1 POLYATOMIC IONS We have seen that atoms can lose or gain electrons to become ions. Groups of atoms can also become ions. These groups of atoms are called polyatomic ions. Examples: O hydroxide ion NO

More information

Chapter 3 Chemical Compounds

Chapter 3 Chemical Compounds Chapter 3 Chemical Compounds 3.1 (a) formula unit; (b) strong electrolyte; (c) molecular compound; (d) acid; (e) nonelectrolyte; (f) oxoanion 3.2 (a) molecular formula; (b) weak electrolyte; (c) ionic

More information

Name: Class: Date: 2 4 (aq)

Name: Class: Date: 2 4 (aq) Name: Class: Date: Unit 4 Practice Test Multiple Choice Identify the choice that best completes the statement or answers the question. 1) The balanced molecular equation for complete neutralization of

More information

(b) Formation of calcium chloride:

(b) Formation of calcium chloride: Chapter 2: Chemical Compounds and Bonding Section 2.1: Ionic Compounds, pages 22 23 1. An ionic compound combines a metal and a non-metal joined together by an ionic bond. 2. An electrostatic force holds

More information

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

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

More information

Calculating Atoms, Ions, or Molecules Using Moles

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

More information

Formulae, stoichiometry and the mole concept

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

More information

Aqueous Solutions. Water is the dissolving medium, or solvent. Some Properties of Water. A Solute. Types of Chemical Reactions.

Aqueous Solutions. Water is the dissolving medium, or solvent. Some Properties of Water. A Solute. Types of Chemical Reactions. Aqueous Solutions and Solution Stoichiometry Water is the dissolving medium, or solvent. Some Properties of Water Water is bent or V-shaped. The O-H bonds are covalent. Water is a polar molecule. Hydration

More information

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

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

More information

Chemistry 65 Chapter 6 THE MOLE CONCEPT

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

More information

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

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

More information

1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) 3 (s) + H 2 (g)

1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) 3 (s) + H 2 (g) 1. When the following equation is balanced, the coefficient of Al is. Al (s) + H 2 O (l)? Al(OH) (s) + H 2 (g) A) 1 B) 2 C) 4 D) 5 E) Al (s) + H 2 O (l)? Al(OH) (s) + H 2 (g) Al (s) + H 2 O (l)? Al(OH)

More information

Unit 9 Compounds Molecules

Unit 9 Compounds Molecules Unit 9 Compounds Molecules INTRODUCTION Compounds are the results of combinations of elements. These new substances have unique properties compared to the elements that make them up. Compounds are by far

More information

Problem Solving. Mole Concept

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

More information

Stoichiometry. Unit Outline

Stoichiometry. Unit Outline 3 Stoichiometry Unit Outline 3.1 The Mole and Molar Mass 3.2 Stoichiometry and Compound Formulas 3.3 Stoichiometry and Chemical Reactions 3.4 Stoichiometry and Limiting Reactants 3.5 Chemical Analysis

More information

Unit 6 The Mole Concept

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

More information

Chapter 12: Oxidation and Reduction.

Chapter 12: Oxidation and Reduction. 207 Oxidation- reduction (redox) reactions Chapter 12: Oxidation and Reduction. At different times, oxidation and reduction (redox) have had different, but complimentary, definitions. Compare the following

More information

Writing and Balancing Chemical Equations

Writing and Balancing Chemical Equations Name Writing and Balancing Chemical Equations Period When a substance undergoes a chemical reaction, chemical bonds are broken and new bonds are formed. This results in one or more new substances, often

More information

Chapter 3: Stoichiometry

Chapter 3: Stoichiometry Chapter 3: Stoichiometry Key Skills: Balance chemical equations Predict the products of simple combination, decomposition, and combustion reactions. Calculate formula weights Convert grams to moles and

More information