AP CHEMISTRY. Ms. M. Morse
|
|
- Rose Cobb
- 7 years ago
- Views:
Transcription
1 AP CHEMISTRY Congratulations on your decision to take Advanced Placement Chemistry! This course will be challenging, but it may also be one of the most rewarding experiences of your high school years. I expect you to put forth your best efforts. If you do, you will succeed in this course and earn a 5 on the AP Exam (up to 8 college credits.) AP classes are taught as college courses not just collegelevel courses. I will do as much as I can to help you learn, but you are responsible for learning and understanding everything covered in class. Sometimes you will be required to watch assigned lectures online before coming to class. I will tell you when everything is due, but I won t chase after you. If you were absent and you need to turn in an assignment late, it is your responsibility to show it to me or it to me. If you re having trouble with something, you need to be proactive about learning it, either by coming in for help after school, consulting with your classmates, or by getting outside help. This expectation is effective immediately, and it applies to this summer assignment. The requirements for this course are comparable for any college course, except that this course is equivalent to two semesters of college chemistry. It will require much more time and effort than most of your other courses. Each textbook chapter has problem sets at the end and completing these problems will be an expected routine part of your homework. In addition, I will assign problems from other sources. The goals of this summer assignment are to make sure you haven t completely forgotten Chemistry I, to give you a warmup for AP Chemistry, and to make you aware of the level of work required for this course. If you are not willing or not able to take on this responsibility, please change your schedule immediately. Only dedicated students should take this demanding course. The nomenclature part of the assignment is due by July 16. You may mail it or bring it to school and have it placed in my mailbox. The textbook problems are due the first day of class. Procrastination and AP courses do not mix. Do not wait to start the problems. In order to do quality higher level work, you must allow yourself sufficient time to complete it. Last minute work is often incorrect or incomplete. You may work with your friends in the class, as long as you list the names of the people you worked with and each person turns in a separate copy. I am assuming that you are comfortable with the basics: stoichiometry, equation and formula writing, balancing, gas laws, etc. The first three chapters of the textbook for the course, General Chemistry 4 th ed. by Hill, Petrucci, McCreary, & Perry will be used for your summer assignment. There will be a quick review during the first two weeks of school and then a test. After that, we will move at a pace of approximately one chapter every two weeks. This course also includes laboratory experiments which require writing prelabs and some formal lab reports. The AP chemistry exam is scheduled first next year on May 4, 2015, and I expect everyone to take the exam. Additional time after school will also be required to prepare for the AP exam, but most students have found this worthwhile. If you have questions this summer, please or text me. I am looking forward to another exciting year. Ms. M. Morse mmmorse@vbschools.com
2 Sign up for the class website on Edmodo immediately! This will allow you to communicate with me and your classmates as you complete your summer assignment. The Edmodo class code is gutyga This assignment should be a good review of what you mastered in your first chemistry course. Part I: Complete Inorganic Nomenclature Worksheets 1 & 2 (below) Memorize the names and formulas of all the polyatomic ions on the sheet. There will be a quiz on this the first week back. Part I is due by July 16 to my KHS mailbox Part II: Read chapters 13 of the textbook and study the example problems in the chapters before attempting to solve the problems. Show all work!! Chapter One : problems # 19, 26, 28, 38, 40, 42, 50, 52, 54, 56, 64, 66, 68, 70, 81, 82, 84, 94, 95, 100 Chapter Two : problems # 22, 23, 30, 34, 38, 42, 44, 68, 70, 91, 93, 97, 108 Chapter Three: problems # 20, 22, 34, 40, 44, 48, 50, 56, 58, 64, 78, 80, 84, 88, 96, 102, 116 This summer assignment will be your first grade of the year and will be worth at least 50 points. Part II is due the first day of class. Part III: Memorize the solubility rules (attached.) This will make your first month in class much easier. Your work should be neat and organized. Show all work where applicable. Credit will be given only if work is shown. he answers to the Exercises and some problems are at the back of the book in Appendix E, so you may try those problems and check your answers. There will be a test on this material second week of school This summer assignment is posted on the Kempsville HS website. If you did not sign out a textbook with me, then you may get a book in the Guidance Office from Monday to Thursday this summer.
3 Inorganic Nomenclature WS 1 Write the formulas for the following compounds. 1. mercury(ii) fluoride 26. phosphoric acid 2. potassium chloride 27. lithium permanganate 3. potassium permanganate 28. iron(iii) hydrogen phosphate 4. potassium perchlorate 29. sodium carbonate 5. zinc oxide 30. magnesium hydrogen carbonate 6. barium hydroxide 31. tin(iv) phosphate 7. ammonium permanganate 32. nitric acid 8. calcium carbonate 33. zinc chloride 9. barium phosphate 34. sodium dihydrogen phosphate 10. iron(iii) oxide 35. mercury(i) chloride 11. cobalt(iii) fluoride 36. iron(ii) nitrite 12. carbonic acid 37. copper(ii) ammonium phosphate 13. potassium sulfate 38. sodium magnesium phosphate 14. sodium hydrogen sulfate 39. tin(iv) hydrogen carbonate 15. phosphorus pentafluoride 40. sodium permanganate 16. silver oxide 41. potassium fluoride 17. lead(ii) clorite 42. calcium sulfate 18. copper(i) chromate 43. hydrochloric acid 19. calcium perchlorate 44. antimony trichloride 20. acetic acid 45. tetrarsenic decoxide 21. lithium iodide 46. ammonium chloride 22. aluminum sulfate 47. ammonium nitrate 23. hydrobromic acid 48. iodine pentafluoride 24. mercury(i) hypochlorite 49. sodium hydrogen carbonate 25. chromium(iii) chloride 50. barium hydroxide
4 Inorganic Nomenclature Worksheet 2 Print the name of each of the following compounds on the line next to the formula. 1. FeCl 3 2. HF 3. PbSO 4 4. KrF 2 5. NaCl 6. P 2 O 5 7. AlBr 3 8. Ba(NO 3 ) 2 9. BrF P 4 O FePO Hg 2 SO KH 14. Co 2 (SO 3 ) N 2 O N 2 O 17. Fe(NO 2 ) Sn 3 (PO 4 ) H 2 O Be(OH) Sr(HCO 3 ) Sr(OH) P 4 S Hg 2 O Hg 2 (OH) 2
5 26. NH 4 F 27. XeF K 2 Cr 2 O NH 4 OH 30. (NH 4 ) 3 PO N 2 O SnCrO Al 2 O CuCO ClO CuS 37. MgI CoCl NaCN 40. Hg 3 N BrO SiF Sb 2 O LiH 45. SF SnI KOH 48. K 2 O 49. H 2 SO Li 2 O
6 Symbols and Charges for Polyatomic Ions Formula Name Formula Name NO 3 nitrate ClO 4 perchlorate NO 2 CrO 4 2 Cr 2 O 7 2 nitrite ClO 3 chromate ClO 2 chlorate chlorite dichromate ClO hypochlorite CN cyanide IO 4 CNO cyanate IO 3 SCN thiocyanate IO 2 periodate iodate iodite OH hydroxide IO hypoiodite O 2 2 NH 2 CO 3 2 SO 4 2 SO 3 2 C 2 O 4 2 PO 4 3 PO 3 3 S 2 O 3 2 AsO 3 3 AsO 4 3 SeO 4 2 peroxide BrO 3 bromate amide BrO hypobromite carbonate HCO 3 sulfate HSO 4 sulfite MnO 4 oxalate phosphate HPO 4 2 phosphite H 2 PO 4 hydrogen carbonate (bicarbonate) hydrogen sulfate (bisulfate) permanganate hydrogen phosphate dihydrogen phosphate thiosulfate HS hydrogen sulfide arsenite BO 3 3 arsenate SiO 3 2 selenate C 2 H 3 O 2 borate silicate acetate (alternate way to write acetate is CH 3 COO ) There is one positive polyatomic ion. It is NH 4 + and is called the ammonium ion. Writing just the plus sign or minus sign for ions with +1 or 1 charges is standard practice
7 Solubility Rules Follow these rules in numerical order. If rule #1 does not apply, go to rule #2. If rule # 2 does not apply, go to rule #3 and so on. 1. All compounds of alkali metals and NH 4 + are soluble. 2. All nitrates, chlorates, perchlorates, and acetates are soluble (AgC 2 H 3 O 2 is moderately soluble) 3. The chlorides, bromides, and iodides of most metals are soluble (exceptions: Pb +2, Ag +, Hg 2 +2 ). 4. All sulfates are soluble except for those of Sr +2, Ba +2, Pb +2, Hg 2 +2, and those of Ca +2 and Ag + are moderately soluble. 5. All carbonates, chromates, and phosphates are insoluble, except those of alkali metals and NH All hydroxides are insoluble except for those of alkali metals and NH 4 + ; those of Ca +2, Sr +2 and Ba +2 are moderately soluble. 7. All sulfides of metals are insoluble, except for those of alkali metals, alkaline, earth metals and NH All oxides are insoluble, except for those of alkali metals, Ca +2, Sr +2 and Ba +2
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 informationNomenclature 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 informationNomenclature 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 informationDecomposition. Composition
Decomposition 1. Solid ammonium carbonate is heated. 2. Solid calcium carbonate is heated. 3. Solid calcium sulfite is heated in a vacuum. Composition 1. Barium oxide is added to distilled water. 2. Phosphorus
More informationCHAPTER 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 informationPolyatomic Ions Worksheet. 2. Name or write the formula for the following Type I polyatomic ionic compounds
Polyatomic Ions Worksheet Polyatomic Practice 1. Name or write the formula for the following polyatomic ions sulfate - CO nitrite MnO perphosphate - SO hypoiodite BrO chlorite - CO phosphite - PO percarbonate
More informationWRITING 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 informationCHEMICAL NOMENCLATURE
CHEMICAL NOMENCLATURE Chemical nomenclature The process of giving unambiguous chemical formulas or chemical names to elements and compounds Introduction Chemistry is the study of matter (elements and compounds)
More informationMonatomic 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 informationTutorial 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 informationNaming 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 informationCHEMICAL 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 informationFORMULAS AND NOMENCLATURE OF IONIC AND COVALENT COMPOUNDS Adapted from McMurry/Fay, section 2.10, p. 56-63 and the 1411 Lab Manual, p. 27-31.
FORMULAS AND NOMENCLATURE OF IONIC AND COVALENT COMPOUNDS Adapted from McMurry/Fay, section 2.10, p. 56-63 and the 1411 Lab Manual, p. 27-31. TYPES OF COMPOUNDS Ionic compounds are compounds composed of
More informationNomenclature 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 informationAP Chemistry Reaction Questions
AP Chemistry Reaction Questions Directions: Give the formulas to show the reactants and the products for the following chemical reactions. Each of the reactions occurs in aqueous solution unless otherwise
More informationNaming 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 informationNAMING 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 informationDavid A. Katz Chemist, Educator, Science Communicator, and Consultant Department of Chemistry, Pima Community College
WRITING CHEMICAL EQUATIONS 2004, 2002, 1989 by David A. Katz. All rights reserved. Permission for classroom used provided original copyright is included. David A. Katz Chemist, Educator, Science Communicator,
More informationHOMEWORK 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 informationPolyatomic 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 informationCHEMISTRY B- FACTOR LABEL PACKET NAME: HR: PAGE 1. Chemistry B. Factor Label Packet
CHEMISTRY B- FACTOR LABEL PACKET NAME: HR: PAGE 1 Chemistry B Factor Label Packet CHEMISTRY B- FACTOR LABEL PACKET NAME: HR: PAGE 2 PERIODIC TABLE OF ELEMENTS WITH OXIDATION NUMBERS +1 0 H +2 +3-3 He Li
More informationSolution. 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 informationBalancing 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 informationSample 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 informationWriting 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 informationChemistry Themed. Types of Reactions
Chemistry Themed Types of Reactions 1 2 Chemistry in the Community-2015-2016 Types of Reactions Date In-Class Assignment Homework T 10/20 TEST on Reactivity of Metals and Redox None W 10/21 Late Start
More information6 Reactions in Aqueous Solutions
6 Reactions in Aqueous Solutions Water is by far the most common medium in which chemical reactions occur naturally. It is not hard to see this: 70% of our body mass is water and about 70% of the surface
More informationExperiment 5. Chemical Reactions A + X AX AX A + X A + BX AX + B AZ + BX AX + BZ
Experiment 5 Chemical Reactions OBJECTIVES 1. To observe the various criteria that are used to indicate that a chemical reaction has occurred. 2. To convert word equations into balanced inorganic chemical
More informationElements 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 informationOxidation 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 informationRules 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 informationChapter 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 informationMoles, 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 informationChapter 2 Compounds and Chemical Reactions. 6. The number of atoms in one formula unit of the substance, CO(NH 2 ) 2, is
Chapter 2 Compounds and Chemical Reactions Multiple Choice 1. Which one of the following elements exists as a diatomic molecule when it is in the free state? a. H b. He c. Li d. Be e. B 6. The number of
More informationPART 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 informationPeriodic 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 informationWRITING AP EQUATIONS
WRITING AP EQUATIONS AP equation sets are found in the free-response section of the AP test. This is a 15 point question and you can practice for it all year! You are given three equations and you must
More informationFORMULA WRITING AND NOMENCLATURE OF INORGANIC COMPOUNDS 2011, 2006, 2004, 2002, 1990 by David A. Katz. All rights reserved.
FORMULA WRITING AND NOMENCLATURE OF INORGANIC COMPOUNDS 2011, 2006, 2004, 2002, 1990 by David A. Katz. All rights reserved. I. OXIDATION NUMBERS When chemical elements combine in a chemical reaction to
More informationNumber of moles of solute = Concentration (mol. L ) x Volume of solution (litres) or n = C x V
44 CALCULATIONS INVOLVING SOLUTIONS INTRODUCTION AND DEFINITIONS Many chemical reactions take place in aqueous (water) solution. Quantities of such solutions are measured as volumes, while the amounts
More informationName: 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 informationExperiment 1 Chemical Reactions and Net Ionic Equations
Experiment 1 Chemical Reactions and Net Ionic Equations I. Objective: To predict the products of some displacement reactions and write net ionic equations. II. Chemical Principles: A. Reaction Types. Chemical
More informationMolarity of Ions in Solution
APPENDIX A Molarity of Ions in Solution ften it is necessary to calculate not only the concentration (in molarity) of a compound in aqueous solution but also the concentration of each ion in aqueous solution.
More informationChapter 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 information19.2 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 informationChapter 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 informationCalculating Molar Mass of a Compound
Instructions for Conversion Problems For every conversion problem Write the number in the problem down with unit and a multiplication sign Decide which conversion factor you should use, Avagadro s or molar
More informationTopic 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 informationName 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 informationUnit 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 informationUnit 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 informationCHAPTER 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 informationNaming Ionic Compounds Answer Key
Naming Ionic Compounds Answer Key Give the name of the following ionic compounds: Name 1) Na 2 CO 3 sodium carbonate 2) NaOH sodium hydroxide 3) MgBr 2 magnesium bromide 4) KCl potassium chloride 5) FeCl
More informationUnit 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 informationMolar 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 informationBASIC CONCEPTS of CHEMISTRY Please revise: names of element, Periodic Table (understanding the notation), acid, base and salt nomenclature
BASIC CONCEPTS of CHEMISTRY Please revise: names of element, Periodic Table (understanding the notation), acid, base and salt nomenclature 1. Definitions of acid and base There are several methods of defining
More informationneutrons 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 informationSCH 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 informationName: 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 informationW1 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 informationb. 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 informationSOLUBILITY PRODUCT CONSTANTS
SOLUBILITY PRODUCT CONSTANTS Compound Formula K sp (25 C) Aluminium hydroxide Al(OH) 3 3 10-34 Aluminium phosphate AlPO 4 9.84 10-21 Barium bromate Ba(BrO 3 ) 2 2.43 10-4 Barium carbonate BaCO 3 2.58 10-9
More informationChapter 16: Tests for ions and gases
The position of hydrogen in the reactivity series Hydrogen, although not a metal, is included in the reactivity series because it, like metals, can be displaced from aqueous solution, only this time the
More informationNames and Formulas in General Chemistry
Names and Formulas in General Chemistry Mastering names and formulas takes practice the more you do, the more you remember and the easier it gets! This is a skill that will help to open up the subject
More informationChemistry 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= 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 informationChapter 9 Practice Test - Naming and Writing Chemical Formulas
Chapter 9 Practice Test - Naming and Writing Chemical Formulas Matching Match each itme with the correct statement below. Match each item with the correct statement below. a. monatomic ion f. cation b.
More informationMolecules, 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 informationCHEMICAL NAMES AND FORMULAS
6 CEMICAL NAMES AND FORMULAS SECTION 6.1 INTRODUCTION TO CEMICAL BONDING (pages 133 137) This section explains how to distinguish between ionic and molecular compounds. It also defines cation and anion
More informationProblem 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 informationINORGANIC NOMENCLATURE ~ NAMING INORGANIC COMPOUNDS
INORGANIC NOMENCLATURE ~ NAMING INORGANIC COMPOUNDS Every compound has its own CHEMICAL FORMULA and its own NAME. The nomenclature (naming systems) for IONIC and MOLECULAR compounds are different. IONIC
More informationChemistry: Chemical Equations
Chemistry: Chemical Equations Write a balanced chemical equation for each word equation. Include the phase of each substance in the equation. Classify the reaction as synthesis, decomposition, single replacement,
More information1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436 #1, 7, 8, 11
SCH3U- R.H.KING ACADEMY SOLUTION & ACID/BASE WORKSHEET Name: The importance of water - MAKING CONNECTION READING 1. Read P. 368-375, P. 382-387 & P. 429-436; P. 375 # 1-11 & P. 389 # 1,7,9,12,15; P. 436
More informationCHEM 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 informationAqueous Ions and Reactions
Aqueous Ions and Reactions (ions, acids, and bases) Demo NaCl(aq) + AgNO 3 (aq) AgCl (s) Two clear and colorless solutions turn to a cloudy white when mixed Demo Special Light bulb in water can test for
More informationChemical Equations. Chemical Equations. Chemical reactions describe processes involving chemical change
Chemical Reactions Chemical Equations Chemical reactions describe processes involving chemical change The chemical change involves rearranging matter Converting one or more pure substances into new pure
More informationSolution a homogeneous mixture = A solvent + solute(s) Aqueous solution water is the solvent
Solution a homogeneous mixture = A solvent + solute(s) Aqueous solution water is the solvent Water a polar solvent: dissolves most ionic compounds as well as many molecular compounds Aqueous solution:
More informationChapter 7: Chemical Reactions
Chapter 7 Page 1 Chapter 7: Chemical Reactions A chemical reaction: a process in which at least one new substance is formed as the result of a chemical change. A + B C + D Reactants Products Evidence that
More informationSanta Monica College Chemistry 11
Types of Reactions Objectives The objectives of this laboratory are as follows: To perform and observe the results of a variety of chemical reactions. To become familiar with the observable signs of chemical
More informationChapter 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 informationModule Four Balancing Chemical Reactions. Chem 170. Stoichiometric Calculations. Module Four. Balancing Chemical Reactions
Chem 170 Stoichiometric Calculations Module Four Balancing Chemical Reactions DePauw University Department of Chemistry and Biochemistry Page 1 Introduction to Module Four When making a cheeseburger you
More informationChapter 4 Chemical Reactions
Chapter 4 Chemical Reactions I) Ions in Aqueous Solution many reactions take place in water form ions in solution aq solution = solute + solvent solute: substance being dissolved and present in lesser
More informationChapter 16 Acid-Base Equilibria
Chapter 16 Acid-Base Equilibria Learning goals and key skills: Understand the nature of the hydrated proton, represented as either H + (aq) or H 3 O + (aq) Define and identify Arrhenuis acids and bases.
More informationExercise 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 informationProblem 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 informationNomenclature and the Periodic Table To name compounds and to determine molecular formulae from names a knowledge of the periodic table is helpful.
Nomenclature and the Periodic Table To name compounds and to determine molecular formulae from names a knowledge of the periodic table is helpful. Atomic Number = number of protons Mass Number = number
More informationChapter 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 informationINCOMPATIBILITY OF COMMON LABORATORY CHEMICALS
INCOMPATIBILITY OF COMMON LABORATORY CHEMICALS When certain hazardous chemicals are stored or mixed together, violent reactions may occur because the chemicals are unsuitable for mixing, or are incompatible.
More informationExperiment 8 - Double Displacement Reactions
Experiment 8 - Double Displacement Reactions A double displacement reaction involves two ionic compounds that are dissolved in water. In a double displacement reaction, it appears as though the ions are
More informationGeneral Chemistry I topics
General Chemistry I topics Periodic table, ions and ionic compounds, stoichiometry, concentration, formula weights, interconverting masses and moles, thermochemistry, enthalpy, wave behavior of matter,
More informationMultiple 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 informationIB 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 informationStoichiometry 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 informationAqueous 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 informationCHEMICAL 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 informationTOPIC 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 informationMOLES 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 informationSEATTLE CENTRAL COMMUNITY COLLEGE DIVISION OF SCIENCE AND MATHEMATICS. Oxidation-Reduction
SEATTLE CENTRAL COMMUNITY COLLEGE DIVISION OF SCIENCE AND MATHEMATICS OxidationReduction Oxidation is loss of electrons. (Oxygen is EN enough to grab e away from most elements, so the term originally meant
More informationGeneral Chemistry Lab Experiment 6 Types of Chemical Reaction
General Chemistry Lab Experiment 6 Types of Chemical Reaction Introduction Most ordinary chemical reactions can be classified as one of five basic types. The first type of reaction occurs when two or more
More informationChemical Reactions. Section 9.1 Reactions and Equations pages 282 288 SOLUTIONS MANUAL. Practice Problems pages 284 287
CHAPTER 9 Chemical Reactions Section 9.1 Reactions and Equations pages 282 288 Practice Problems pages 284 287 Write skeleton equations for the following word equations. 1. Hydrogen and bromine gases react
More informationExperiments in General Chemistry I CHM 11. Department of Physical Sciences Kingsborough Community College The City University of New York
Experiments in General Chemistry I CHM 11 Department of Physical Sciences Kingsborough Community College The City University of New York Schedule of Laboratory Experiments Each week we will meet to perform
More information