14 MC pts problem pts. = 24 pts. total possible
|
|
- Beryl Sheena Ray
- 5 years ago
- Views:
Transcription
1 CHE 211 Answers in BOLD RED EXAM 1, 2014 KEY On this mastery- based exam, you must score at least 70% to complete the exam. If your score is less than 70% you will have to do a retake of one or two chapters material (normally those on which you did worst). Any new points beyond what you score this time on those chapters will then be added to your score up to a maximum of 75%. Multiple Choice (2% each) and Problems (10% each, partial credit possible) grouped by chapter Please select the BEST answer to each multiple choice question and mark it clearly on the answer sheet. Problems should be answered in the space immediately after each. SHOW ALL WORK! Thank you. CHAPTER 1 (BASICS) 14 MC pts problem pts. = 24 pts. total possible 1. Which of the following molecular scenes depicts a mixture of three substances, 2 of which are compounds? D 2. What physical state would be the best match for all four of the molecular scene drawings above? A. liquid B. gas C. solid D. aqueous 3. The energy of chemical bonds is from the relative position of atoms in relation to others; this is thus a form of A. kinetic energy B. potential energy 4. How many milliliters (ml) are there in a liter (L)? A. 1,000,000 B. 100 C. 1,000 D. 10, A liquid substance in a sealed container disappears when heated and returns upon cooling. This is probably a A. physical change B. chemical change C. neither has occurred D. both have occurred 6. A piece of iron ore with a volume of 733 ml has a mass of 3775 g. What is its density in g/ml? A (sig fig) B C D The temperature of a lab is stated to be 303 Kelvin. What would that be in F? (see data sheet for conversions) A. 79 B. 92 C. 84 D. 86 Answer as requested. If calculations are required, then please show those also. Two students are competing for a summer lab job. The lab supervisor tests their competence by having them weigh the same object on ten different balances, all supposedly accurate to ±0.001 g. Bob comes up with an average weight of g with a standard deviation of g, while Gloria gets g on average, with a standard deviation of g. The actual object weight was g according to the supervisor. Using the terms precision and accuracy, compare the quality of the work each person did (i.e., which was most precise and which was most accurate [could be the same person] and what do you mean by each of those terms?). Precision is how consistent a set of measurements is; based upon this, Gloria has more precision (is more precise) because her standard deviations are smaller, indicating her measurements were closer Accuracy is a measure of how close a set of measurements is to the true value; on that basis, Bob is more accurate, since his average value is closer to the true value of the weight, even thought his standard deviation is worse. This could occur is Bob had poor technique, while Gloria may have had some systematic error in her measurements.
2 CHE 211 Exam 1 Key Page 2 CHAPTER 2 (MATTER) 14 MC pts problem pts. = 24 pts. total possible 1. Which statement is correct? A. a pure substance can be an element or a compound B. impure substances must be homogeneous mixtures C. molecules must contain 2 or more elements D. only heterogeneous substances are true mixtures 2. J.J. Thomson was able to discover some of the properties of the electron, but he could only determine its A. mass/charge ratio B. mass C. charge D. magnetic field 3. Thomson created the plum pudding atomic model. Who disproved that model by his experiments? A. Millikan B. Einstein C. Rutherford D. Geiger 4. Two atoms are isotopes of one another. This means their count is the same but not their count. A. electron ; proton B. neutron ; electron C. proton ; neutron D. proton ; electron 5. Which of these is a metalloid? A. Se B. Ba C. C D. Ar 6. Which chemical species is covalently bonded but is itself an ion? A. cations B. anions C. monoatomic ions D. polyatomic ions 7. What is the proper name (not a common name) for Se 2Br 4? A. diselenium tetrabromide B. selenium (II) bromide C. selenium (II) bromide (IV) D. selenic bromide John Dalton s Atomic Theory had four postulates. State them, then explain the current scientific viewpoint on each (Is it still considered true? Why or why not? What is the current atomic theory s new statement? Dalton s Postulate Still considered true? Why? New Statement (now) All matter consists of atoms, which are indivisible and unchanging In part; we now know atoms are divisible All stable matter consists of atoms; they maybe divided but are then not stable. Atoms cannot be converted to other elements atoms No. Elements may undergo nuclear transmutations. Atoms can be converted to those of other elements by nuclear reactions All atoms of one element have a unique mass and set of properties No; all atoms of one element have the same proton count Every element s atoms have a unique proton count; their neutron count and thus mass may vary Atoms of elements combine to form compounds Yes Unchanged Extra credit (5 points maximum) for each of the following, fill in the empty boxes as listed Formula Ionic or covalent? Proper chemical name KNO 3 Ionic Potassium nitrate IF 5 Covalent Iodine pentafluoride CF 4 Covalent Carbon tetrafluoride CoSO 4 Ionic Cobalt (II) sulfate P 2Se 5 Covalent Diphosphorus pentaselenide
3 CHE 211 Exam 1 Key Page 3 CHAPTER 3 (STOICHIOMETRY) 16 MC pts problem pts. = 26 pts. total possible 1. What is the molar mass of niacin, C 6H 5NO 2? A. 142 g B. 123 g C g D. 114 g 2. Niacin (see above question) has a density of g/cm 3. What volume should 3 moles of it have? A. 289 cm 3 B. 175 cm 3 C. 205 cm 3 D cm 3 3. If we have moles of niacin, how many ATOMS would we have all together? A x B x C x D x Two different substances have the same molecular formula. That means that they also have the same: A. structures B. properties C. bonds between atoms D. empirical formula 5. When a mole of the fuel undecane, C 11H 24, is fully combusted to CO 2 and H 2O, it requires moles of O 2. A. 23 B. 17 C. 20 D Wood alcohol is the older name for methanol, CH 3OH, which used to be made by heating wood in a closed chamber. It is now made by two reactions: C(s) + H 2O(l) à CO(g) + H 2(g) and CO(g) + 2 H 2(g) à CH 3OH(l). What, then, is the equation for the combined reactions used to produce methanol commercially? A. C(s) + H 2O(l) + H 2(g) à CH 3OH(l) B. 2 C(s) + 4 H 2(g) + O 2(g) à 2 CH 3OH(l) C. C(s) + H 2O(l) + H 2(g)à CO(g) + CH 3OH(l) D. CO(g) + H 2(g) + H 2O(l) à CH 3OH(l) + ½ O 2(g) 7. Formaldehyde is made by doing 2 CH 3OH(g) + O 2(g) à 2 CH 2O(g) + 2 H 2O(g) at 300 C. If you start with 64 g of CH 3OH and 64 g of O 2, how many grams of formaldehyde (CH 2O) should be produced, at most? A g B. 30. g C. 60. g D g 8. If you run the reaction described in question 7 and get 52 g of formaldehyde, what was the percent yield? A. 87% B. 43% C. 170% D. 41% SHOW WORK, either directly by doing the calculations below, or as setups for calculator use. An alcohol (an organic compound which contains only C, H, and O) is burned and its combustion products analyzed. This combustion analysis showed that the alcohol was 65.71%C and 12.41% H by weight (the remainder being O). What is the empirical formula of this alcohol? 100% - (65.71% %) = 21.88% O by weight So, 100 g of the alcohol = g C g H g O. Need to find the molar ratios: g C / ( g C/mol) = 5.47 mol C 5.47/1.37 = g H/ (1.008 g/mol) = 12.3 mol H 12.3/1.37 = g O/ ( g/mol) = 1.37 mol O 1.37/1.37 = 1 This, the empirical formula = C 4H 9O If the estimated molecular weight of this alcohol is about 150 g/mole, what would its molecular formula be? Molar mass of C 4H 9O = = /73 2, so molecular formula is twice the empirical (it will always be a whole number multiple) Thus, molecular formula is C 8H 18O 2
4 CHE 211 Exam 1 Key Page 4 CHAPTER 4 (REACTION TYPES) 16 MC pts problem pts. = 26 pts. total possible 1. The compound sodium phosphate (Na 3PO 4) is dissolved to make a 1.0 M solution. What is the concentration of all the ions in total in this solution? A. 1.0 M B. 4.0 M C. 2.0 M D M ml of 2.33 M NaNO 3 is measured out carefully by a student. How many moles of NaNO 3 did he pour out? A B C D Which of these ionic substances is most likely to NOT be water soluble? A. KNO 3 B. LiCl C. (NH 4) 2SO 4 D. Ca 3(PO 4) 2 4. Strong acids are generally: A. covalent substances that ionize 100% in water B. ionic substances that are very soluble in water C. covalent substances that ionize 1% in water D. ionic substances that contain very stable oxyanions 5. Ba(OH) 2 and HClO 3 react: Ba(OH) HClO 3 à Ba(ClO 3) H 2O. If ml of unknown concentration Ba(OH) 2 is titrated with M HClO 3, ml of the acid is needed. What is the Ba(OH) 2 molarity? A B C. 0. D In the unbalanced reaction S 2O I 2 + H 2O à I + SO H +, gets oxidized and gets reduced. A. S ; I B. O ; S C. H ; O D. I ; H 7. When the redox equation in question 6 gets balanced, what are the respective coefficients of S 2O 3 2, I 2, & H 2O? A. 2 ; 6 ; 7 B. 2 ; 5 ; 8 C. 1 ; 4 ; 5 D. 1 ; 3 ; 4 8. What is the oxidation number of the S in thiosulfate ion, S 2O 3 2? A. +4 B. +2 C. +3 D. +6 Balance the following two reactions and then write a NET IONIC EQUATION for each of them, with all states. Sr(NO 3) 2(aq) + Na 2SO 4(aq) à SrSO 4(s) + NaNO 3(aq) Balancing is simple in this case: Sr(NO 3) 2(aq) + Na 2SO 4(aq) à SrSO 4(s) + 2 NaNO 3(aq) Sr 2+ (aq) + 2 NO 3 (aq) + 2 Na + (aq) + SO 4 2 (aq) à SrSO 4(s) +2 NO 3 (aq) + 2 Na + (aq) Which will simplify to a net ionic equation of: Sr 2+ (aq) + SO 4 2 (aq) à SrSO 4(s) HNO 3(aq) + Fe(s) à Fe(NO 3) 3(aq) + H 2O(l) + NO(g) This is a redox reaction: Fe à Fe e and N e à N 2+ Electrons already balance so the Fe and NO should both be 1; other species must be balanced to acknowledge those facts: 4 HNO 3(aq) + Fe(s) à Fe(NO 3) 3(aq) + 2 H 2O(l) + NO(g) The net ionic equation will ignore the unchanged nitrate ions: [can use H + or H 3O + ] 4 H + [or 3 H 3O + ] + NO 3 (aq) + Fe (s) à Fe 3+ (aq) + NO(g) + 2 H 2O(l) [or 3 H 2O]
5 CHE 211 Exam 1 Key Page 5
1. My answers for this Chemistry 102 exam should be graded with the answer sheet associated with: a) Form A b) Form B c) Form C d) Form D e) Form E
Hour Exam I Page 1 1. My answers for this Chemistry 102 exam should be graded with the answer sheet associated with: a) Form A b) Form B c) Form C d) Form D e) Form E 2. Consider the measurements 9.74
More informationCH 221 Sample Exam Exam II Name: Lab Section:
Exam II Name: Lab Section: Part I: Multiple Choice Questions (100 Points) Use a scantron sheet for Part I. There is only one best answer for each question. 1. When methanol undergoes complete combustion,
More information1 st Semester Final Review Sheet (Chapters 2-7)
CP Chemistry Name: Period: 1 st Semester Final Review Sheet (Chapters 2-7) Matter (Chapter 2) 1. What is the definition of an element? 2. What is the definition of a compound? 3. What is the definition
More informationChemistry 11 Course Review
Introduction to Chemistry 1. 0.0006 mm =? µm Chemistry 11 Course Review 6. A 0.0460 L piece of copper has a mass of 410.32 g. Calculate the density of copper in g/ml. 2. 0.054 ml =? nl 3. 3.5 µg/l =? mg/ml
More informationSummary Chapter One 1. Scientific Method (know definitions). 2. Quantitative versus Qualitative measurements. 3. Accuracy versus Precision.
Summary Chapter One 1. Scientific Method (know definitions). 2. Quantitative versus Qualitative measurements. 3. Accuracy versus Precision. 4. Systematic versus Random errors. 5. Significant Figures. 6.
More informationReactions in Aqueous Solutions
Reactions in Aqueous Solutions 1 Chapter 4 General Properties of Aqueous Solutions (4.1) Precipitation Reactions (4.2) Acid-Base Reactions (4.3) Oxidation-Reduction Reactions (4.4) Concentration of Solutions
More information4. Draw a concept map showing the classifications of matter. Give an example of each.
Name Bring calculator, pencils, and this completed worksheet to the midterm exam. For problems involving an equation, carry out the following steps: 1. Write the equation. 2. Substitute numbers and units.
More informationDuring photosynthesis, plants convert carbon dioxide and water into glucose (C 6 H 12 O 6 ) according to the reaction:
Example 4.1 Stoichiometry During photosynthesis, plants convert carbon dioxide and water into glucose (C 6 H 12 O 6 ) according to the reaction: Suppose that a particular plant consumes 37.8 g of CO 2
More informationName: Chemistry 400: General Chemistry Miller Exam I September 20, 2017 Approximately 150 points
Name: Chemistry 400: General Chemistry Miller Exam I September 20, 2017 Approximately 150 points Please answer each of the following questions to the best of your ability. If you wish to receive partial
More information5. Measured quantities, such as length, mass, or time, can best be described as:
1. How many significant figures are there in the number 0.0006042? a. 7 b. 3 c. 8 d. 4 e. 0 2. The agreement of a particular value with the true value is called a. accuracy. b. error. c. precision. d.
More informationChapter 4: Stoichiometry of Chemical Reactions. 4.1 Writing and Balancing Chemical Equations
Chapter 4: Stoichiometry of Chemical Reactions 4.1 Writing and Balancing Chemical Equations A chemical equation represents or symbolizes a chemical reaction. o Substances are represents by their chemical
More informationCHEMISTRY 102A/E Hour Exam I. T. Hummel SECTION
CHEMISTRY 10A/E September 3, 010 T. Hummel NAME SIGNATURE SECTION SAMPLE This exam is made up of an answer sheet, two cover sheets and 7 numbered pages. Below are instructions for coding the answer sheet.
More informationCHE 105 ALTERNATE EXAMINATION I February 9, 2012
CHE 105 ALTERNATE EXAMINATION I February 9, 2012 University of Kentucky Department of Chemistry PLEASE READ THESE DIRECTIONS CAREFULLY BEFORE STARTING THE EXAMINATION! It is extremely important that you
More informationAP Chemistry. 9. Which of the following species CANNOT function as an oxidizing agent? (A) Cr 2 O 72 (B) MnO 4 (C) NO 3 (D) S (E) I
Name AP Chemistry AP Chemistry Exam Part I: 40 Questions, 40 minutes, Multiple Choice, No Calculator Allowed Bubble the correct answer on your scantron for each of the following. Use the following answers
More informationb. Na. d. So. 1 A basketball has more mass than a golf ball because:
Chem I Semester Review All of the following are general characteristics of a substance in the liquid state except a. definite volume. c. not easily compressed. b. able to flow. d. definite shape. In the
More informationSemester 1 Review Chemistry
Name Period Date Semester 1 Review Chemistry Units & Unit Conversions Ch. 3 (p. 73-94) PART A SI UNITS What type of measurement is indicated by each of the following units? Choices are in the last column.
More informationChapter 6. Types of Chemical Reactions and Solution Stoichiometry
Chapter 6 Types of Chemical Reactions and Solution Stoichiometry Chapter 6 Table of Contents (6.1) (6.2) (6.3) (6.4) (6.5) (6.6) (6.7) (6.8) Water, the common solvent The nature of aqueous solutions: Strong
More informationVolume of water g g? 50.0 ml ?
MID-TERM EXAM REVIEW! KEY! Unit 1 Convert the following: 1.) 2.02 x 10 15 mg = g 2.02 x 10 15 mg 1 g = 2.02 x 10 12 g 1000 mg 2.) 1.29 x 10-7 m = cm 1.29 x 10-7 m 100 cm = 1.29 x 10-5 cm 1 m 3.) 13.5 dm
More informationSection EXAM III Total Points = 150. November 15, Each student is responsible for following directions. Read this page carefully.
Name Chemistry 11100 Test 66 Section EXAM III Total Points = 150 TA Thursday, 8:00 PM November 15, 2012 Directions: 1. Each student is responsible for following directions. Read this page carefully. 2.
More informationName AP Chemistry September 30, 2013
Name AP Chemistry September 30, 2013 AP Chemistry Exam Part I: 40 Questions, 40 minutes, Multiple Choice, No Calculator Allowed Bubble the correct answer on the blue side of your scantron for each of the
More informationIntroductory Chemistry I Chemistry 1111 September 17, 2009 Hour Examination I Name There is a Periodic Table and a summary of solubility rules attached to the end of this examination. You may use a non-programmed
More information2) Isotopes are atoms of the same element, which have the same number of but a different number.
AP Chemistry Semester 1 Exam Review Alternate Atomic Structure 1) Fill in the table: Name Per Isotope Symbol Atomic Mass Mass # Atomic # # of protons # of neutrons # of electrons Hydrogen-1 16 16 18 35.45
More informationChemistry Midterm Exam Review Sheet Spring 2012
Chemistry Midterm Exam Review Sheet Spring 2012 1. Know your safety rules 2. A shopping mall wanted to determine whether the more expensive Tough Stuff floor wax was better than the cheaper Steel Seal
More informationPart A Answer all questions in this part.
Part A Directions (1-24): For each statement or question, record on your separate answer sheet the number of the word or expression that, of those given, best completes the statement or answers the question.
More informationCP Chemistry Final Exam Review
I. Matter and Measurement 1) Chemical or physical property? CP Chemistry Final Exam Review Diamond is a very hard substance. The density of aluminum is 2.7 g/cm 3. Zinc reacts with acid. Copper melts at
More informationQuick Review. - Chemical equations - Types of chemical reactions - Balancing chemical equations - Stoichiometry - Limiting reactant/reagent
Quick Review - Chemical equations - Types of chemical reactions - Balancing chemical equations - Stoichiometry - Limiting reactant/reagent Water H 2 O Is water an ionic or a covalent compound? Covalent,
More informationChemistry 11 Course Review
Chemistry 11 Course Review Unit 2 Introduction to Chemistry Pages in Student Workbook Class Assignments 9-40 Hand-In #1 Unit Conversions Hand-In #2 Significant Digits Experiment 3-A - Determining the Mass/Volume
More informationMULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
Exam Name MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) A 25 g sample of sugar is found to contain 51.4% oxygen by mass. Another 250 g sample
More informationChapter Four: Reactions in Aqueous Solution
Chapter Four: Reactions in Aqueous Solution Learning Outcomes: Identify compounds as acids or bases, and as strong, weak, or nonelectrolytes Recognize reactions by type and be able to predict the products
More informationMemorize: 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 informationCH141, Fall 2017 Exam 1 10/3/2017. Section (please circle): A(Rice) B(McKinney)
C141, Fall 2017 Exam 1 10/3/2017 Name: Section (please circle): A(Rice) B(McKinney) Part I. Short Answer: Answer 8 of the following 9 questions. Clearly indicate which question you do NOT want counted,
More informationChapter 4. Chemical Quantities and Aqueous Reactions
Lecture Presentation Chapter 4 Chemical Quantities and Aqueous Reactions Reaction Stoichiometry: How Much Carbon Dioxide? The balanced chemical equations for fossilfuel combustion reactions provide the
More informationLab Chemistry - Final Exam Review 1. Express in scientific notation. A) D) B) E) C)
Lab Chemistry - Final Exam Review 1. Express 30554000 in scientific notation. A) 3 10 7 D) 30554 10 3 B) 3.0554 10 7 E) 305540 10 7 C) 306 10 7 2. What is the result of the following multiplication expressed
More informationChem 127, Final Exam December 10, 2003
I. (55 points) This part of the final corresponds to Exam I. It covers the material in Chapters 1, 2 and 3. A. (10 points) Answer the following questions by writing your answers on the blanks provided.
More informationChapter How many grams of a 23.4% by mass NaF solution is needed if you want to have 1.33 moles of NaF?
Chapter 13 1. Which of the following compounds is a strong electrolyte? a. NH 4Cl b. NaCl c. NaC 2H 3O 2 d. HCl e. All of the above 2. A solution that is 13.58% by mass of sugar contains 13.75 grams of
More informationChapter 9 Practice Worksheet: Reactions in Aqueous Solutions
Chapter 9 Practice Worksheet: Reactions in Aqueous Solutions 1. The compound H 2 S is classified as a weak electrolyte. Describe/draw how it reacts when placed in water. Completely dissociates in water.
More informationName. Student ID # CHEMISTRY 121 [Tyvoll] EXAM I. September 30, Possibly Useful Information:
Name Student ID # CHEMISTRY 121 [Tyvoll] EXAM I September 30, 2004 1 2 3 4 5 Possibly Useful Information: 1) ( ) ( ) ( ) ( ) ( ) 1 in = 2.540 cm 1 kg = 2.205 lb 2) ( ) ( ) ( ) ( ) ( ) R = 8.314 J K -1
More informationCP Chemistry Final Exam Review
I. Matter and Measurement 1) Chemical or physical property? CP Chemistry Final Exam Review Diamond is a very hard substance. The density of aluminum is 2.7 g/cm 3. Zinc reacts with acid. Copper melts at
More informationChapter 4 - Types of Chemical Reactions and Solution Chemistry
Chapter 4 - Types of Chemical Reactions and Solution Chemistry 4.1 Water, the Common Solvent - the water molecule is bent with and H-O-H angles of approx. 105 º - O-H bonds are covalent - O is slightly
More informationNote: there are 5 points of extra credit built in to this exam. 1. (4 points) For each of the following element categories, give three examples.
Exam 1 Chem 1A, Fall 2016 Fossum Name: Note: there are 5 points of extra credit built in to this exam. 1. (4 points) For each of the following element categories, give three examples. a. noble gases b.
More informationGeneral Chemistry Study Guide
General Chemistry 1311 Study Guide Name : Louise K number: Date: Oct 02006 Instructor: Jingbo Louise Liu kfjll00@tamuk.edu 1 Chapter 04 & 05 (10 questions required and 5 questions for extra credit) Credited
More information4) Please indicate whether each of the following units are intensive or extensive. a) Density Intensive Extensive. b) Temperature Intensive Extensive
EXAM ONE Nomenclature Balancing Reactions Protons, Neutrons, Electrons Natural Abundance Solubility Rules Net Ionic Reactions Atom, Mole, Gram Conversions Empirical Formulas Solution Chemistry / Molarity
More informationLaw of Definite Proportion** (Proust): A given compound always contains exactly the same proportion of elements by mass.
# 10 Notes Unit 2: Laws, Properties & Mols Ch. Atoms, Molecules, Ions 5 Chemical Laws: I. Law of Conservation of Mass** (Lavoisier): Mass cannot be created or destroyed. II. III. IV. Law of Definite Proportion**
More informationAP CHEMISTRY THINGS TO KNOW
AP CHEMISTRY THINGS TO KNOW Diatomic Molecules H2-hydrogen gas (do not write H) N2-nitrogen gas (do no write N) O2-oxygen gas (do not write O) F2-fluorine gas (do not write F) Cl2-chlorine gas (do not
More informationForm A. Exam 1, Ch 1-4 September 23, Points
Chem 130 Name Exam 1, Ch 1-4 September 23, 2011 100 Points Please follow the instructions for each section of the exam. Show your work on all mathematical problems. Provide answers with the correct units
More informationAdvanced Placement Chemistry ~ Summer Assignment Part 2. Name
Advanced Placement Chemistry ~ Summer Assignment Part 2 Name Topic 1: Measurements and Dimensional Analysis Appropriately read and report a measurement correctly with one uncertain digit. State the number
More informationCHEMISTRY 15 EXAM II-Version A (White)
CHEMISTRY 15 EXAM II-Version A (White) Dr. M. Richards-Babb June 8, 2001 An optical scoring machine will grade this examination. The machine is not programmed to accept the correct one of two sensed answers
More informationChapter 4 Types of Chemical Reaction and Solution Stoichiometry
Chapter 4 Types of Chemical Reaction and Solution Stoichiometry Water, the Common Solvent One of the most important substances on Earth. Can dissolve many different substances. A polar molecule because
More informationCH 221 Chapter Four Part II Concept Guide
CH 221 Chapter Four Part II Concept Guide 1. Solubility Why are some compounds soluble and others insoluble? In solid potassium permanganate, KMnO 4, the potassium ions, which have a charge of +1, are
More informationFormulas and Models 1
Formulas and Models 1 A molecular formula shows the exact number of atoms of each element in the smallest unit of a substance An empirical formula shows the simplest whole-number ratio of the atoms in
More informationUnit Two Worksheet WS DC U2
Unit Two Worksheet WS DC U2 Name Period Short Answer [Writing]. Write skeleton equations representing the following reactions and then balance them. Then identify the reaction type. Include all needed
More informationFINAL EXAM REVIEW QUESTIONS
FINAL EXAM REVIEW QUESTIONS Matter and Chemical Bonding 1) Classify each of the following as either a element, compound, a solution or a heterogeneous mixture: a) vinegar b) mercury c) brass d) potassium
More informationName: Name: Worksheet 23 Chem 101 Review 1.) What is the best answer to report for?
Name: Name: Name: Name: Worksheet 23 Chem 101 Review 1.) What is the best answer to report for? 2.) Ethylene glycol freezes at 11.5 o C. What is this temperature in o F? 3.) Three people measure a length
More informationACP Chemistry (821) - Mid-Year Review
ACP Chemistry (821) - Mid-Year Review *Be sure you understand the concepts involved in each question. Do not simply memorize facts!* 1. What is chemistry? Chapter 1: Chemistry 2. What is the difference
More informationFinal Exam Review Questions You will be given a Periodic Table, Activity Series, and a Common Ions Chart CP CHEMISTRY
Final Exam Review Questions You will be given a Periodic Table, Activity Series, and a Common Ions Chart CP CHEMISTRY Part A True-False State whether each statement is true or false. If false, correct
More informationGeneral Chemistry 1 CHM201 Unit 2 Practice Test
General Chemistry 1 CHM201 Unit 2 Practice Test 1. Which statement about the combustion of propane (C 3H 8) is not correct? C 3H 8 5O 2 3CO 2 4H 2O a. For every propane molecule consumed, three molecules
More informationResearch tells us fourteen out of any ten individuals like chocolate. Happy Halloween!
CHEMISTRY 101 Hour Exam II October 31, 2006 Adams/Le Name KEY Signature T.A./Section Research tells us fourteen out of any ten individuals like chocolate. Happy Halloween! This exam contains 17 questions
More informationinsoluble partial very soluble (< 0.1 g/100ml) solubility (> 1 g/100ml) Factors Affecting Solubility in Water
Aqueous Solutions Solubility is a relative term since all solutes will have some solubility in water. Insoluble substances simply have extremely low solubility. The solubility rules are a general set of
More informationChemistry Mid-Term Exam Review Spring 2017
Unit 1 Measurement & Math Accuracy & Precision (recognizing given lab data) Density calculations Number of SFs in a measurement, Round answers to correct number of SFs Percent Error Unit conversions in
More informationChapter 4: Types of Chemical reactions and Solution Stoichiometry
Chapter 4: Types of Chemical reactions and Solution Stoichiometry 4.1 Water, The Common Solvent State why water acts as a common solvent. Draw the structure of water, including partial charge. Write equations
More informationChemistry 150/151 Review Worksheet
Chemistry 150/151 Review Worksheet This worksheet serves to review concepts and calculations from first semester General Chemistry (CHM 150/151). Brief descriptions of concepts are included here. If you
More informationAP Chapter 4: Reactions in Aqueous Solution Name
AP Chapter 4: Reactions in Aqueous Solution Name WarmUps (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. AP Chapter 4: Reactions in Aqueous Solution 2 WarmUps
More informationChapter 4. Reactions in Aqueous Solution
Chapter 4. Reactions in Aqueous Solution 4.1 General Properties of Aqueous Solutions A solution is a homogeneous mixture of two or more substances. A solution is made when one substance (the solute) is
More informationTYPES OF CHEMICAL REACTIONS
TYPES OF CHEMICAL REACTIONS Precipitation Reactions Compounds Soluble Ionic Compounds 1. Group 1A cations and NH 4 + 2. Nitrates (NO 3 ) Acetates (CH 3 COO ) Chlorates (ClO 3 ) Perchlorates (ClO 4 ) Solubility
More informationUnit 4a: Solution Stoichiometry Last revised: October 19, 2011 If you are not part of the solution you are the precipitate.
1 Unit 4a: Solution Stoichiometry Last revised: October 19, 2011 If you are not part of the solution you are the precipitate. You should be able to: Vocabulary of water solubility Differentiate between
More information4) Convert: a) 10 m = km b) 500 g = mg c) 250 ml = L
Data Analysis 1) Define: a) Accuracy b) Precision 2) The actual density of water is 1.00 g/ml Fred Wilma Barney Trial 1 1.12 g/ml 0.88 g/ml 1.00 g/ml Trial 2 1.13 g/ml 1.07 g/ml 1.01 g/ml Trial 3 1.11
More information6. Place the following elements in order of increasing atomic radii: Mg, Na, Rb, Cl.
CH141 Practice Problems/Practice Final Exam Page 1 of 12 Name: 1. What is the SO 4 2- concentration of a solution prepared by dissolving 3.00 g of Na 2 SO 4 in 1.00 L of water? 2. What is the hybridization
More informationCHEM 60 Spring 2016 Exam 2 Ch 5-8, 100 points total.
Name Exam No. F CHEM 60 Spring 2016 Exam 2 Ch 5-8, 100 points total. Multiple Choice. (20 questions, 3 points each = 60 points total) Mark the letter on the scantron form corresponding to the one best
More informationSolubility Rules See also Table 4.1 in text and Appendix G in Lab Manual
Ch 4 Chemical Reactions Ionic Theory of Solutions - Ionic substances produce freely moving ions when dissolved in water, and the ions carry electric current. (S. Arrhenius, 1884) - An electrolyte is a
More informationCHM152LL Solution Chemistry Worksheet
Name: Section: CHM152LL Solution Chemistry Worksheet Many chemical reactions occur in solution. Solids are often dissolved in a solvent and mixed to produce a chemical reaction that would not occur if
More informationCHE 105 SU17 Exam 1. Which statement describes a chemical change? Question #: 1. Question #: 2. Question #: 3
CHE 105 SU17 Exam 1 Your Name: Your ID: Question #: 1 The state of matter in which atoms or molecules do not have a fixed volume or shape and are free to move relative to each other is a 1 [solid, liquid,
More information1. Which type of bond involves the transfer of electrons from one atom to another? A. Hydrogen bond C. Metallic bond B. Ionic bond D.
1. Which type of bond involves the transfer of electrons from one atom to another? A. Hydrogen bond C. Metallic bond B. Ionic bond D. Covalent bond 2. Ethene (C 2 H 4 ) and cyclohexane (C 6 H 12 ) have
More informationExam 1, Ch September 21, Points
Chem 130 Name Exam 1, Ch 1-4.2 September 21, 2018 100 Points Please follow the instructions for each section of the exam. Show your work on all mathematical problems. Provide answers with the correct units
More informationUnit Five- Chemical Quantities Chapter 9: Mole ratios, conversions between chemicals in a balanced reaction (mole, mass), limiting reactant, % yield
Chemistry Midterm Review Exam date: Wednesday, 2/15 during class The midterm exam must be completed before February vacation if you are absent The midterm exam is worth 6% of your year grade and it contains
More informationCHEMISTRY 102 A/E Fall 2008 HOUR EXAM I NAME Dr. Christine Yerkes. A. DO NOT open the exam until you are instructed to do so.
CHEMISTRY 102 A/E Fall 2008 HOUR EXAM I NAME Dr. Christine Yerkes October 1, 2008 SIGNATURE Test Form A QUIZ TA A. DO NOT open the exam until you are instructed to do so. B. The exam has 6 pages. After
More informationUnit 1 Atomic Structure
Unit 1 Atomic Structure Unit 1 Text Questions 1.1 Atoms/Ions/Isotopes Problems Ch 5 Prob: 9,23,24,38 1.2 Average Atomic Mass Problems Ch 5 Prob: 15,17 1.3 Atomic Theory Development Problems Ch 5 Prob:
More information1) What is the volume of a tank that can hold Kg of methanol whose density is 0.788g/cm 3?
1) Convert the following 1) 125 g to Kg 6) 26.9 dm 3 to cm 3 11) 1.8µL to cm 3 16) 4.8 lb to Kg 21) 23 F to K 2) 21.3 Km to cm 7) 18.2 ml to cm 3 12) 2.45 L to µm 3 17) 1.2 m to inches 22) 180 ºC to K
More informationUnit 3: Solubility Equilibrium
Unit 3: Chem 11 Review Preparation for Chem 11 Review Preparation for It is expected that the student understands the concept of: 1. Strong electrolytes, 2. Weak electrolytes and 3. Nonelectrolytes. CHEM
More informationCHEMISTRY 102A Spring 2012 Hour Exam II. 1. My answers for this Chemistry 102 exam should be graded with the answer sheet associated with:
. My answers for this Chemistry 0 exam should be graded with the answer sheet associated with: a) Form A b) Form B c) Form C d) Form D e) Form E. A sample of LSD (D-lysergic acid diethylamide, C 4 H 30
More information1011_1st Exam_
1011_1st Exam_1011017 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) Which of the following functional groups gives acidic properties to organic
More informationChem 205: GENERAL CHEMISTRY I MIDTERM EXAMINATION
Concordia University CHEM 205 Fall 2006 -- MIDTERM EXAM Student ID #: Chem 205: GENERAL CHEMISTRY I MIDTERM EXAMINATION PLEASE READ THIS WHILE WAITING TO START INSTRUCTIONS: This test paper includes 8
More informationName Date Class STUDY GUIDE FOR CONTENT MASTERY
Stoichiometry Section 12.1 What is stoichiometry? In your textbook, read about stoichiometry and the balanced equation. For each statement below, write true or false. 1. The study of the quantitative relationships
More informationNanoscale pictures: Figs. 5.1, 5.4, and 5.5
Solutions and concentration Solution: a homogeneous mixture of two or more substances. Example: water, sugar, flavor mixture (Coke). The substances are physically combined, not chemically combined or bonded
More informationChapter 4. Types of Chemical Reactions and Solution Stoichiometry
Chapter 4 Types of Chemical Reactions and Solution Stoichiometry Chapter 4 Table of Contents 4.1 Water, the Common Solvent 4.2 The Nature of Aqueous Solutions: Strong and Weak Electrolytes 4.3 The Composition
More information1. [7 points] How many significant figures should there be in the answer to the following problem?
1 of 6 10/20/2009 3:54 AM Avogadro s Number = 6.022 10 23 1. [7 points] How many significant figures should there be in the answer to the following problem? (29.0025 + 0.2)/(6.1345 36.101) (a) 1 (b) 2
More informationPRACTICE COMPREHENSIVE EXAM #1 7 th GRADE CHEMISTRY
Name: Date: Class: PRACTICE COMPREHENSIVE EXAM #1 7 th GRADE CHEMISTRY BUBBLE SHEETS AND PERIODIC TABLES ARE ATTACHED. PLEASE DETACH. YOU MAY WRITE ON THE PERIODIC TABLE. PART ONE: Multiple choice. Choose
More informationCP Chemistry Midterm Topic List
CP Chemistry Midterm Topic List Converting SI Units (Kilo, Hecto, Deca, Base Unit, Deci, Centi, Milli) Scientific Notation Precision versus Accuracy Properties of Matter Classification of Matter (Element/Compound/Mixture)
More information1. What is the mass percent of sulfur in Al 2 (SO 4 ) 3? A % C % B % D %
1. What is the mass percent of sulfur in Al 2 (SO 4 ) 3? A. 9.372 % C. 28.12 % B. 21.38 % D. 42.73 % 2. How many grams of phosphorus are in 35.70 g of P 2 O 5? A. 6.359 g C. 15.58 g B. 23.37 g D. 31.16
More information2 A ruler is marked in.1 cm intervals. What is the uncertainty associated with the ruler? a) 1 cm b) 0.1 cm c) 0.01 cm d) cm
Practice Final (Print) Name last First Signature Introduction to General Chemistry, Ch152 Practice Final Exam 1 Who was first responsible for presenting the planetary model of the atom? a) Dalton b) Millikan
More information(50 pts.) 26. (24 pts.) 27. (8 pts.) 28. (18 pts.) TOTAL (100 points)
Moorpark College Chemistry 11 Spring 2011 Instructor: Professor Torres Examination #2: Section Two March 12, 2011 Name: (print) Name: (sign) Directions: Make sure your examination contains ELEVEN total
More informationLab Day and Time: Instructions. 1. Do not open the exam until you are told to start. Page # Points possible Points awarded
Name: Lab Day and Time: Instructions 1. Do not open the exam until you are told to start. 2. This exam is closed note and closed book. You are not allowed to use any outside material while taking this
More informationChapter 4. Aqueous Reactions and Solution Stoichiometry
Sample Exercise 4.1 (p. 127) The diagram below represents an aqueous solution of one of the following compounds: MgCl 2, KCl, or K 2 SO 4. Which solution does it best represent? Practice Exercise 1 (4.1)
More informationChem. 1A Final. Name. Student Number
Chem. 1A Final Name Student Number All work must be shown on the exam for partial credit. Points will be taken off for incorrect or no units. Calculators are allowed. Cell phones may not be used for calculators.
More informationThe June 2018 Chemistry Regents Exam
The June 2018 Chemistry Regents Exam 1 Which statement describes the charge and location of an electron in an atom? (1) An electron has a positive charge and is located outside the nucleus. (2) An electron
More information2. What is the charge of the nucleus in an atom of oxygen-17? (1) 0 (2) 2 (3) +8 (4) +17
60 Most Missed Chemistry Regents Exams Questions 1. In the wave-mechanical model, an orbital is a region of space in an atom where there is (1) a high probability of finding an electron (2) a high probability
More informationName. Practice Test 2 Chemistry 111
Name Practice Test 2 Chemistry 111 1) In the aqueous reaction of K 2 SO 4 (aq) + Ba(NO 3 ) 2 (aq) BaSO 4 (s) + 2KNO 3 (aq), which ions are the spectator ions? A) Ba 2+ 2- and SO 4 B) Ba 2+ and K + C) Ba
More informationAP Chemistry Semester 1 Practice Problems
AP Chemistry Semester 1 Practice Problems 1. Adipic Acid contains 49.32% C, 43.84% O, and 6.85% H by mass. What is the empirical formula? a) C 3 H 5 O 2 b) C 3 H 3 O 4 c) C 2 HO 3 d) C 2 H 5 O 4 e) C 3
More informationIB CHEMISTRY SL. SUMMER REVIEW Mrs. Coronado IB Chemistry SL
IB CHEMISTRY SL SUMMER REVIEW Mrs. Coronado Name: IB Chemistry SL 20182019 Prior to beginning the year of IB Chemistry you must complete the following exercises in review from your past experiences in
More informationCHEM 200/202. Professor Jing Gu Office: EIS-210. All s are to be sent to:
CHEM 200/202 Professor Jing Gu Office: EIS-210 All emails are to be sent to: chem200@mail.sdsu.edu My office hours will be held in GMCS-212 on Monday from 9 am to 11 am or by appointment. ANNOUNCEMENTS
More informationChem GENERAL CHEMISTRY I MIDTERM EXAMINATION
Concordia University CHEM 205 Fall 2009, B LAST NAME: FIRST NAME: STUDENT ID: Chem 205 - GENERAL CHEMISTRY I MIDTERM EXAMINATION PLEASE READ THIS BOX WHILE WAITING TO START INSTRUCTIONS: Calculators are
More information