!!! DO NOT OPEN THIS EXAM BOOK UNTIL TOLD TO DO SO BY THE INSTRUCTOR!!!

Size: px
Start display at page:

Download "!!! DO NOT OPEN THIS EXAM BOOK UNTIL TOLD TO DO SO BY THE INSTRUCTOR!!!"

Transcription

1 CHEM Exam 1 Version B!!! DO NOT OPEN THIS EXAM BOOK UNTIL TOLD TO DO SO BY THE INSTRUCTOR!!! Instructor: Dr. Kari Pederson NO GRAPHING CALCULATORS ALLOWED Date: Friday, July 15 ONLY CALCULATORS MAY BE USED AS CALCULATORS (you may not use your cellular phone as a calculator) Time: 9:40-10:40am NO HEADPHONES ALLOWED (EARPLUGS ARE OK) Location: BAG 154 NO HATS WITH BRIMS ALLOWED!!! PLEASE READ THIS!!! Indicate all of the following on your scantron form or five points will be deducted from your exam score: First Name, Last Name, Student Number, Section, Exam Version YOUR FULL NAME: first name last name YOUR SECTION/SEAT: discussion section seat number EXAM 1 VERSION B Page 1 of 10

2 Question Points Possible Score Scantron Info? -5 TOTAL 100 EXAM 1 VERSION B Page 2 of 10

3 MULTIPLE CHOICE: CONCEPTS. 3 pts each 24 POINTS TOTAL Please mark the one correct answer for each of the following questions on your scantron. 1. Which of the following is a physical property of the element chlorine? A) Chlorine is a gas that is poisonous if inhaled. B) Chlorine will react with sodium to make salt. C) Chlorine is a gas that will become a liquid at 34.4 ºC. D) Chlorine is used in water treatment as a disinfectant. E) Chlorine exists as a diatomic molecule. 2. Which metric prefix symbol means 1 x 10-3? A) p B) m C) M D) k E) n 3. As chemists and other scientists seek to understand the principles that govern nature they employ what is called the scientific method. The first step in this method is. A) the proposal of a hypothesis B) the testing of a scientific law C) the making of observations D) the application for a research grant E) the testing of a hypothesis 4. Reaction of 10.0 grams of calcium with of sulfur gave 22.0 grams of calcium sulfide. All the calcium was used, but there were 20.0 grams of sulfur left over. A) 12.0 grams B) 22.0 grams C) 32.0 grams D) 42.0 grams Conservation of Mass: total mass reactants = total mass products mass sulfur = ( 22.0g calcium sulfide g excess sulfur)! 10.0g calcium = 32.0g 5. Of the following, only would not be classified as a pure substance. A) sucrose B) acetic acid C) oxygen D) a granite rock E) water EXAM 1 VERSION B Page 3 of 10

4 6. Which statement best describes isotopes? A) atoms in the same vertical group B) atoms with the same number of neutrons and different numbers of protons C) atoms with the same number of protons and different numbers of neutrons D) atoms with the same numbers of protons and neutrons E) atoms in the same horizontal period 7. The element is classified as a metal whereas is classified as a metalloid. A) Sr, Ge B) Ni, Ba C) As, Sb D) Br, Si E) Rb, I 8. In an atom of Zn. A) the number of protons equals the number of neutrons B) 30 electrons are found outside the nucleus C) 35 protons are found in the nucleus D) the total number of electrons and protons equals 65 E) 30 neutrons are found in the nucleus EXAM 1 VERSION B Page 4 of 10

5 MULTIPLE CHOICE: SHORT CALCULATIONS. 5 pts each 40 TOTAL POINTS Please mark the one correct answer for each of the following questions on your scantron. 9. The volume of a ball bearing is 1.37 mm 3. What is its volume in cubic centimeters (cm 3 )? A) 1.37 x 10 3 cm 3 B) 1.37 x 10 1 cm 3 C) 1.37 x 10-1 cm 3 D) 1.37 x 10-3 cm 3 3 1cm 1.37mm 3 " %! # $ 10mm & ' = 1.37! 10 (3 cm A sugar contains 42.14% C, 6.48% H and 51.46% O. What is the molecular formula of the sugar if its molar mass is approximately 330 g/mol? A) C 11 H 22 O 11 B) C 13 H 2 O 16 C) C 20 H 20 O 17 D) CH 2 O 42.14g C! 1mol C g C = 3.511mol C 6.48g H! 1mol H 1.008g H = 6.43mol H 1mol O 51.46g C! g O = 3.216mol O empirical formula: CH 2 O empirical mass = 1! amu C empirical mass molecular mass = 30.0amu 330.1amu = 11 molecular formula: C 11 H 22 O 11 ( ) + ( 2! 1.008amu H ) + ( 1! amu O) = 30.0amu 11. Calculate the moles of calcium ions present in a milliliter of M calcium sulfate. A) 2.65 x 10-1 moles B) 5.30 x 10-1 moles C) 2.65 x 10-4 moles D) 5.30 x 10-4 moles Formula: CaSO 4 1L 1mL! 1000mL! 0.265mol CaSO 4 1mol Ca2+! = 2.65! 10 "4 mol Ca 2+ 1L 1mol CaSO 4 EXAM 1 VERSION B Page 5 of 10

6 12. A stock solution of potassium dichromate, K 2 CrO 4, is made by dissolving 76.2 g of the compound in 1.00 L of solution. How many milliliters of this solution are required to prepare 1.00 L of M K 2 CrO 4? A) 392 ml B) 255 ml C) 76.2 ml D) 39.2 ml M 1 V 1 = M 2 V g mol K 2 CrO 4 = 2! g mol K = ( ) + ( g mol Cr) + ( 4! g mol O) 76.2g g mol = 0.392mol K 2CrO 4 M 1 = 0.392mol K 2CrO 4 = 0.392M K 2 CrO L 1.00L! mol L V 1 = = 0.255L! 1000mL mol L 1L = 255mL 13. Calculate the number of lithium ions in 21.4 mg of lithium nitride. A) 3.70 x ions B) 4.62 x ions C) 6.15 x ions D) 3.70 x ions Formula: Li 3 N 1g 21.4mg Li 3 N! 1000mg! 1mol Li N 3 3mol Li+ 6.02! Li + ions! = 1.1! Li + ions 34.83g Li 3 N 1mol Li 3 N 1mol Li What is the mass % of H in ammonium hydrogen sulfate (NH 4 HSO 4 )? A) 0.9% B) 3.5% C) 4.4% D) 12% ( ( )) g mol H g mol S + ( 4! g molo) molar mass = g mol N + 4! g mol H = g mol NH 4 HSO 4 5! g mol H mass%h =! 100% = 4.4% g mol NH 4 HSO 4 EXAM 1 VERSION B Page 6 of 10

7 15. Naturally occurring copper ( amu) is composed of two isotopes, copper-63 ( amu) and copper-65 ( amu). From this, one can conclude that naturally occurring copper is composed of. A) approximately 20% copper-63 and 80% copper-65 B) approximately 80% copper-63 and 20% copper-65 C) approximately 30% copper-63 and 70% copper-65 D) approximately 70% copper-63 and 30% copper amu = ( x)62.916amu + ( 1! x)64.955amu x = What is the correct name of Pb(ClO 4 ) 2? A) lead(ii) perchlorate B) lead(iv) perchlorate C) lead(ii) chlorate D) lead(iv) chlorate E) lead(ii) chlorite EXAM 1 VERSION B Page 7 of 10

8 MATCHING. 2 pts each 16 POINTS TOTAL Please indicate the letter of the one correct answer for each of the following questions in the blank. 17. The conversion of CO (g) into CO 2 (g) is an example of a(n) C change/reaction. 18. Give the chemical symbol/name (whichever is missing) for each of the following elements: A) S O B) Boron J C) Na M D) Ni Q E) Iron L 19. Reaction of 5.80 grams of aluminum with 4.80 grams of oxygen gives grams of aluminum oxide with 0.40 grams of aluminum left over. This illustrates the Law of Z. 20. The number of I is equal to the number of electrons in a neutral atom. A) Physical B) K C) Chemical D) Os E) Calcium F) Electrons G) Nitrogen H) I I) Protons J) B K) Decomposition L) Fe M) Sodium N) Ir O) Sulfur P) In Q) Nickel R) P S) Carbon T) O U) Neutrons V) Lead W) Br X) Multiple Proportions Y) Definite Proportions Z) Conservation of Mass EXAM 1 VERSION B Page 8 of 10

9 LONG ANSWER. 20 POINTS TOTAL 21. In lab, a student mixes 8.0 ml aqueous solutions of sodium sulfide (4.0 M) and copper(iii) chloride (2.5 M) are mixed together. A) What is the net ionic equation for this reaction? (3 pts) 2Cu 3+ (aq) + 3S 2 (aq) Cu 2 S 3 (s) If you are unable to write the balanced net ionic equation or no precipitate would form in this reaction (i.e., no reaction would occur), use the following information for the remainder of the problem: 60. ml of 0.50 M iron(iii) chloride solution and 40.0 ml of 7.5 M ammonium sulfide solution are mixed in order to precipitate iron(iii) sulfide according to the following balanced net ionic equation: 2Fe 3+ (aq) + 3S 2- (aq) Fe 2 S 3 (s) B) Assuming the reaction goes to completion, what mass of precipitate will form? (6 pts) 0.008L solution! 4.0mol Na 2 S 1L solution 0.008L solution! 2.5mol CuCl 3 1L solution 1mol S2"! = 0.032mol S2" 1mol Na 2 S! 1mol Cu 3+ 1mol CuCl 3 = 0.020mol Cu 3+ Need 3 S 2- ions for every 2 Cu 2+ ions, so Cu 2+ is limiting reactant mol Cu 3+! 1mol Cu 2 S 3 2mol Cu 3+! g Cu 2 S 3 1mol Cu 2 S 3 = 2.2g Cu 2 S 3 Alternate problem: 0.50mol FeCl 3 L solution! 0.060L solution = 0.030mol FeCl 3! 7.5mol Na 2 S L solution! L solution = 0.30mol ( NH 4 ) 2 S! 1mol Fe3+ 1mol FeCl 3 = 0.030mol Fe 3+ 1mol S 2" ( ) 2 S 1mol NH 4 2:3 Fe 3+ :S 2- mole ratio in balanced net ionic equation, so equivalents Fe 3+ and 0.10 equivalents S 2-. Fe 3+ is limiting reagent mol S 2! " 1mol Fe 2 S 3 2mol Fe 3+ = 0.015mol Fe 2 S 3 " g Fe 2 S 3 1mol Fe 2 S 3 = 3.1g Fe 2 S 3 = 0.30mol S2" EXAM 1 VERSION B Page 9 of 10

10 What mass of each excess ion will remain? (9 pts) 0.032mol S 2! " 2mol Na+ 1mol S 2! 0.064mol Na +! = 0.064mol Na+ initially! 0mol Na + used = 0.064mol Na + excess g Na+ 1mol Na + = 1.5g Na + excess " 3mol Cl 0.020mol Cu 3+! 1mol Cu = 0.060mol Cl " initially " 0mol Cl " used = 0.060mol Cl " excess 3+! g Cl 0.060mol Cl! " = 2.1g Cl! excess 1mol Cl! # 3mol 0.032mol S 2! initially! 0.020mol Cu 3+ S2! & " $ % 2mol Cu 3+ ' ( used = 0.002mol S2! excess 0.002mol S 2! " g S2! 1mol S 2! = 0.064g S 2! excess Alternate Problem: 0.30mol S 2! " 2mol NH + 4 = 0.60mol NH + 1mol S 2! 4 initially! 0mol NH + 4 used = 0.60mol NH + 4 excess 0.60mol NH + 4! g NH 4 = 11g NH excess 1mol NH 4 " 3mol Cl 0.030mol Fe 3+! 1mol Fe = 0.090mol Cl " initially " 0mol Cl " used = 0.090mol Cl " excess 3+! g Cl 0.090mol Cl! " = 3.2g Cl! excess 1mol Cl! # 3mol 0.30mol S 2! initially! 0.030mol Fe 3+ S2! & " $ % 2mol Fe 3+ ' ( used = 0.255mol S2! excess mol S 2! " g S2! 1mol S 2! = 8.2g S 2! excess D) If the student recovers 2.00 g of precipitate, what is the percent yield? (If you did not calculate a theoretical yield in part B, use 3.53 g here) (2 pts) 2.00g PbCl 2 2.2g PbCl 2! 100% = 91% yield Alt. 2.00g Fe 2 S 3 3.1g Fe 2 S 3! 100% = 65% yield EXAM 1 VERSION B Page 10 of 10

CHEM 60 Spring 2016 Exam 2 Ch 5-8, 100 points total.

CHEM 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 information

Lab Chemistry - Final Exam Review 1. Express in scientific notation. A) D) B) E) C)

Lab 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 information

AP Chemistry - Summer Assignment

AP Chemistry - Summer Assignment AP Chemistry - Summer Assignment NOTE: a. MUST SHOW ALL WORK FOR CREDIT!! b. Where work is required, do on a separate sheet of paper c. These are the foundational things you should be able to do when you

More information

Unit Two Worksheet WS DC U2

Unit 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 information

Form A. Exam 1, Ch 1-4 September 23, Points

Form 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 information

This exam will be given over 2 days. Part 1: Objectives 1-13 Part 2: Objectives 14-24

This exam will be given over 2 days. Part 1: Objectives 1-13 Part 2: Objectives 14-24 Name Hour January Exam Practice A This exam will be given over 2 days. Part 1: Objectives 1-13 Part 2: Objectives 14-24 This practice exam will be graded in the exam portion of the grade book. Objectives

More information

1) What is the volume of a tank that can hold Kg of methanol whose density is 0.788g/cm 3?

1) 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 information

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

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

More information

Semester 1 Review Chemistry

Semester 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 information

SCI-CH Chem Test II fall 2018 Exam not valid for Paper Pencil Test Sessions

SCI-CH Chem Test II fall 2018 Exam not valid for Paper Pencil Test Sessions SCI-CH Chem Test II fall 2018 Exam not valid for Paper Pencil Test Sessions [Exam ID:25FPCV 1 When a strontium atom loses its valence electrons, it has the same electron configuration as which element?

More information

CHEM 171 EXAMINATION 1. October 9, Dr. Kimberly M. Broekemeier. NAME: Key

CHEM 171 EXAMINATION 1. October 9, Dr. Kimberly M. Broekemeier. NAME: Key CHEM 171 EXAMINATION 1 October 9, 008 Dr. Kimberly M. Broekemeier NAME: Key I A II A III B IV B V B VI B VII B VIII I B II B III A IV A V A VI A VII A inert gase s 1 H 1.008 Li.941 11 Na.98 19 K 9.10 7

More information

Solid Gas Liquid Plasma

Solid Gas Liquid Plasma Unit 1: MATTER 1. Define CHEMISTRY: 2. Define MATTER: Use one of the states of matter to complete each statement. (Words will be used more than once.) Solid Gas Liquid Plasma 3. A has definite volume and

More information

TYPES OF CHEMICAL REACTIONS

TYPES 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 information

5. [7 points] What is the mass of gallons (a fifth) of pure ethanol (density = g/cm 3 )? [1 gallon = Liters]

5. [7 points] What is the mass of gallons (a fifth) of pure ethanol (density = g/cm 3 )? [1 gallon = Liters] 1 of 6 10/20/2009 3:55 AM Avogadro s Number, N A = 6.022 10 23 1. [7 points] Given the following mathematical expression: (15.11115.0)/(2.154 10 3 ) How many significant figures should the answer contain?

More information

1. Hydrochloric acid is mixed with aqueous sodium bicarbonate Molecular Equation

1. Hydrochloric acid is mixed with aqueous sodium bicarbonate Molecular Equation NAME Hr Chapter 4 Aqueous Reactions and Solution Chemistry Practice A (Part 1 = Obj. 1-3) (Part 2 = Obj. 4-6) Objective 1: Electrolytes, Acids, and Bases a. Indicate whether each of the following is strong,

More information

2H 2 (g) + O 2 (g) 2H 2 O (g)

2H 2 (g) + O 2 (g) 2H 2 O (g) Mass A AP Chemistry Stoichiometry Review Pages Mass to Mass Stoichiometry Problem (Review) Moles A Moles B Mass B Mass of given Amount of given Amount of unknown Mass of unknown in grams in Moles in moles

More information

JOHN BURKE HIGH SCHOOL

JOHN BURKE HIGH SCHOOL JOHN BURKE HIGH SCHOOL Chemistry 2202 Midterm Examination January, 2013 Instructions: Part I: Multiple Choice: Choose the best answer to each item. Place all answers on the Answer Sheet provided. 40 marks

More information

Unit 1 Atomic Structure

Unit 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 information

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

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 information

ACP Chemistry (821) - Mid-Year Review

ACP 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 information

Chem 1A Dr. White Fall Handout 4

Chem 1A Dr. White Fall Handout 4 Chem 1A Dr. White Fall 2014 1 Handout 4 4.4 Types of Chemical Reactions (Overview) A. Non-Redox Rxns B. Oxidation-Reduction (Redox) reactions 4.6. Describing Chemical Reactions in Solution A. Molecular

More information

During photosynthesis, plants convert carbon dioxide and water into glucose (C 6 H 12 O 6 ) according to the reaction:

During 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 information

Fill in the blanks with the appropriate word, phrase, number, or unit.

Fill in the blanks with the appropriate word, phrase, number, or unit. Name (PRINT CLEARLY) Seat Number Exam 1 (100 points) Chemistry 1303.002 September 20, 2017 On my honor, I have neither given nor received unauthorized aid on this exam. Signed Date Fill in the blanks with

More information

4. Magnesium has three natural isotopes with the following masses and natural abundances:

4. Magnesium has three natural isotopes with the following masses and natural abundances: Exercise #1. Determination of Weighted Average Mass 1. The average mass of pennies minted after 1982 is 2.50 g and the average mass of pennies minted before 1982 is 3.00 g. Suppose that a bag of pennies

More information

CHAPTER 6 CHEMICAL COMPOSITION

CHAPTER 6 CHEMICAL COMPOSITION Chemistry Name Hour Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 6 CHEMICAL COMPOSITION Day Plans for the day Assignment(s) for the day 1 Begin Chapter

More information

Final 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 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 information

Physical and Chemical Changes and Properties

Physical and Chemical Changes and Properties Physical and Chemical Changes and Properties Practice 1.1 pg. 11 Determine whether each change is physical or chemical. What kind of property (chemical or physical) is demonstrated in each case? a. A copper

More information

4 CO O 2. , how many moles of KCl will be produced? Use the unbalanced equation below: PbCl 2. PbSO 4

4 CO O 2. , how many moles of KCl will be produced? Use the unbalanced equation below: PbCl 2. PbSO 4 Honors Chemistry Practice Final 2017 KEY 1. Acetylene gas, C 2, is used in welding because it generates an extremely hot flame when combusted with oxygen. How many moles of oxygen are required to react

More information

Name Student ID Number Lab TA Name and Time

Name Student ID Number Lab TA Name and Time Name Student ID Number Lab TA Name and Time CHEMISTRY 2A Exam I Fall 2012 - Enderle Instructions: CLOSED BOOK EXAM! No books, notes, or additional scrap paper are permitted. All information required is

More information

Unit (2) Quantitative Chemistry

Unit (2) Quantitative Chemistry Unit (2) Quantitative Chemistry Chapter (1) :The mole & chemical equation Lesson (1) Mole and chemical equation Chemical equation: The chemical symbols and formulas of the reactants and products which

More information

This is a guide for your test #1.

This is a guide for your test #1. This is a guide for your test #1. 1) Lead melts at 601.0 C. What temperature is this in F? A. 302 F B. 365 F C. 1,050 F D. 1,082 F E. 1,114 F 2) Ammonia boils at -33.4 C. What temperature is this in F?

More information

Test Booklet. Subject: SC, Grade: HS 2008 Grade High School Chemistry. Student name:

Test Booklet. Subject: SC, Grade: HS 2008 Grade High School Chemistry. Student name: Test Booklet Subject: SC, Grade: HS 2008 Grade High School Chemistry Student name: Author: North Carolina District: North Carolina Released Tests Printed: Tuesday July 17, 2012 1 How many protons and electrons

More information

4. Draw a concept map showing the classifications of matter. Give an example of each.

4. 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 information

Chapter 4. Aqueous Reactions and Solution Stoichiometry

Chapter 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 information

Chapter 3 - Molecules, Compounds and Chemical Equations

Chapter 3 - Molecules, Compounds and Chemical Equations Chapter 3 - Molecules, Compounds and Chemical Equations Section 3.2 two general types of bonding between atoms found in compounds, ionic and covalent ionic bonds result when electrons have been transferred

More information

c. K 2 CO 3 d. (NH 4 ) 2 SO 4 Answer c

c. K 2 CO 3 d. (NH 4 ) 2 SO 4 Answer c Chem 130 Name Exam 2, Ch 4-6 July 7, 2016 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 and

More information

Half Yearly Exam 2015

Half Yearly Exam 2015 GOZO COLLEGE Secondary School KULLEĠĠ TA GĦAWDEX Skola Sekondarja Half Yearly Exam 015 Year 9 Track 3 CHEMISTRY Time: 1½ hours Name: Class: Useful Data: Atomic numbers and relative atomic masses are given

More information

How many hydrogen atoms are there in the empirical formula of propene, C 3 H 6? How many neutrons are there in one atom of 24 Mg?

How many hydrogen atoms are there in the empirical formula of propene, C 3 H 6? How many neutrons are there in one atom of 24 Mg? 1 A 2 B 3 C The atomic number of Na is 11. How many electrons are there in a sodium ion, Na +? How many hydrogen atoms are there in the empirical formula of propene, C 3 H 6? What is the mass in grams

More information

(DO NOT WRITE ON THIS TEST)

(DO NOT WRITE ON THIS TEST) Final Prep Chap 8&9 (DO NOT WRITE ON THIS TEST) Multiple Choice Identify the choice that best completes the statement or answers the question. 1. After the correct formula for a reactant in an equation

More information

ACCELERATED CHEMISTRY SEMESTER 1 PROBLEM SHEET

ACCELERATED CHEMISTRY SEMESTER 1 PROBLEM SHEET ACCELERATED CHEMISTRY SEMESTER 1 PROBLEM SHEET 100. Determine the number of significant figures in the following numbers: a. 100 b. 0.000123 c. 1.00300 d. 1.2300 e. 1.20 x 10 16 f..00010100 Write the following

More information

Exam 1 Worksheet Chemistry 102

Exam 1 Worksheet Chemistry 102 Exam 1 Worksheet Chemistry 102 Chapter 1 Introduction 1. Convert: a. 650 nm to inches b. 650 km to miles c. 345 mg to lb d. 145 lb to μg e. 4.50 10 10 km to μm f. 8.09 10 8 mg to Mg g. 9.00 10 5 ml to

More information

AP WORKSHEET 4s: Calculations Summary

AP WORKSHEET 4s: Calculations Summary AP WORKSHEET 4s: Calculations Summary TYPE 1: Those involving Avogadro s number (the mole concept). Question 1 A sample of Ge is found to contain 9.7 x 10 23 atoms of Ge. How many moles of Ge atoms are

More information

DEPARTMENT OF CHEMISTRY AND CHEMICAL TECHNOLOGY GENERAL CHEMISTRY 202-NYA-05 21, 22 TEST 1 24-SEPT-2012 INSTRUCTOR: I. DIONNE.

DEPARTMENT OF CHEMISTRY AND CHEMICAL TECHNOLOGY GENERAL CHEMISTRY 202-NYA-05 21, 22 TEST 1 24-SEPT-2012 INSTRUCTOR: I. DIONNE. DEPARTMENT OF CHEMISTRY AND CHEMICAL TECHNOLOGY GENERAL CHEMISTRY 202-NYA-05 21, 22 TEST 1 24-SEPT-2012 INSTRUCTOR: I. DIONNE Print your name: Answers INSTRUCTIONS: Answer all questions in the space provided.

More information

Name (printed): Signature:

Name (printed): Signature: CHEM Lab Section Number: Name (printed): Signature: This exam consists of 36 questions all of equal value for a total of 225 points. Make sure that your test has all of the pages. Please read each problem

More information

Chemical Formulas and Chemical Nomenclature. Mr. Matthew Totaro Legacy High School Honors Chemistry

Chemical Formulas and Chemical Nomenclature. Mr. Matthew Totaro Legacy High School Honors Chemistry Chemical Formulas and Chemical Nomenclature Mr. Matthew Totaro Legacy High School Honors Chemistry 1 Molecular View of Elements and Compounds 2 Atomic Elements Atomic Elements = elements whose smallest

More information

IONIC CHARGES. Chemistry 51 Review

IONIC CHARGES. Chemistry 51 Review IONIC CHARGES The ionic charge of an ion is dependent on the number of electrons lost or gained to attain a noble gas configuration. For most main group elements, the ionic charges can be determined from

More information

The chemical formulas of most of the elements are simply their elemental symbol:

The chemical formulas of most of the elements are simply their elemental symbol: Chemical Formulas A chemical formula gives the numbers and types of atoms that are found in a substance. When the substance is a discrete molecule, then the chemical formula is also its molecular formula.

More information

Chem 101 Review. Fall 2012

Chem 101 Review. Fall 2012 Chem 101 Review Fall 2012 Elements, Atoms, Ions Elements in nature symbols Constant composition chemical formula Dalton s atomic theory Atomic structure what makes up the atom ions isotopes Periodic table

More information

AP 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

AP 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 information

Day 2 & Day 3 Online Video Reviews: Video Lesson # 1: Ionic Formulas; Using Criss-Cross Method

Day 2 & Day 3 Online Video Reviews: Video Lesson # 1: Ionic Formulas; Using Criss-Cross Method Name: Period: Final Exam Fall 2017 Video Review +5 points will be added to the final exam score if the entire packet is complete. The packet is due the class period of the final exam NO EXCEPTIONS! The

More information

Exam 1, Ch September 21, Points

Exam 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 information

3. Most laboratory experiments are performed at room temperature at 65 C. Express this temperature in: a. F b. Kelvin

3. Most laboratory experiments are performed at room temperature at 65 C. Express this temperature in: a. F b. Kelvin Do all work on a separate sheet of paper so that you can show your work. Section A: Measurement and Math 1. Convert the following and show your work: a. 200 meters = miles. b. 650 in = meters c. 4 years=

More information

Chapter 4: Types of Chemical reactions and Solution Stoichiometry

Chapter 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 information

Sophomore AP Chem Practice Problems

Sophomore AP Chem Practice Problems Due on 8/17/18 Sophomore AP Chem Practice Problems Scientific notation and significant figures Determine the number of Significant Figures in the following numbers: 00034 2431. 8900 0.0094 Convert the

More information

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

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

More information

b. Na. d. So. 1 A basketball has more mass than a golf ball because:

b. 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 information

Chapter 3. Mass Relationships in Chemical Reactions

Chapter 3. Mass Relationships in Chemical Reactions Chapter 3 Mass Relationships in Chemical Reactions In this chapter, Chemical structure and formulas in studying the mass relationships of atoms and molecules. To explain the composition of compounds and

More information

Honors text: Ch 10 & 12 Unit 06 Notes: Balancing Chemical Equations

Honors text: Ch 10 & 12 Unit 06 Notes: Balancing Chemical Equations Notes: Balancing Chemical Equations Effects of chemical reactions: Chemical reactions rearrange atoms in the reactants to form new products. The identities and properties of the products are completely

More information

Houston Community College System

Houston Community College System . Houston Community College System Chemistry 1311 EXAM # 1A The Periodic table of the Chemical Elements 1 CHEM 1311 Sample Exam #1A (1,2, and 3) Part I. Multiple choice questions. ( 4 points each) Direction-

More information

January Semester Exam Practice B This exam will be given over 2 days. Part 1: Objectives 1-13 Part 2: Objectives 14-24

January Semester Exam Practice B This exam will be given over 2 days. Part 1: Objectives 1-13 Part 2: Objectives 14-24 Name Hour January Semester Exam Practice B This exam will be given over 2 days. Part 1: Objectives 1-13 Part 2: Objectives 14-24 This practice exam will be graded in the exam portion of the grade book

More information

Chapter 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 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 information

Practice Multiple Choice

Practice Multiple Choice Practice Multiple Choice 1. A theory differs from a hypothesis in that a theory A. cannot be disproved C. always leads to the formation of a law B. represents an educated guess D. has been subjected to

More information

Chemistry Final Review 2017

Chemistry Final Review 2017 Chemistry Final Review 2017 Atomic/Molecular Structure and Periodic Trends 1. What is the atomic number trend on the periodic table? 2. On the following periodic table label metals, nonmetals, Alkali metals,

More information

AP Chemistry Unit 1 Review Guide: IUPAC Naming, Stoichiometry, Solution Chemistry

AP Chemistry Unit 1 Review Guide: IUPAC Naming, Stoichiometry, Solution Chemistry I. IUPAC Naming AP Chemistry Unit 1 Review Guide: IUPAC Naming, Stoichiometry, Solution Chemistry For Ionic Compounds: Formula to Name: 1. Identify the cation (positive ion) by name, then identify the

More information

Introductory 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 information

4. What is the law of constant composition (also known as the law of definite proportion)?

4. What is the law of constant composition (also known as the law of definite proportion)? Name: Exercises #1: 1. What is the law of conservation of mass? 2. Show that the results of the following experiments illustrate the law of conservation of mass. Experiment #1: a 5.00-g sample of pure

More information

Chem 42 Final Review Sheet Mr. J. Fassler Spring 2018

Chem 42 Final Review Sheet Mr. J. Fassler Spring 2018 Chem 42 Final Review Sheet Mr. J. Fassler Spring 2018 These problems are given to help you review concepts you may have forgotten. Old tests, quizzes and review sheets are also important in studying. Chapter

More information

Unit 4. Multiple Choice Identify the choice that best completes the statement or answers the question.

Unit 4. Multiple Choice Identify the choice that best completes the statement or answers the question. Unit 4 Multiple Choice Identify the choice that best completes the statement or answers the question. 39. Changing a subscript in a correctly written chemical formula a. changes the number of moles represented

More information

Polyatomic ions You should know the symbols, names, and charges for these common polyatomic ions. Polyatomic Ions to Know + ClO 3. ClO 4 NO

Polyatomic ions You should know the symbols, names, and charges for these common polyatomic ions. Polyatomic Ions to Know + ClO 3. ClO 4 NO AP Chemistry Summer Review Packet 2018 Section 1: Names and Formulas of ionic compounds. Name: Polyatomic ions You should know the symbols, names, and charges for these common polyatomic ions. Polyatomic

More information

Chem Exam 1. September 26, Dr. Susan E. Bates. Name 9:00 OR 10:00

Chem Exam 1. September 26, Dr. Susan E. Bates. Name 9:00 OR 10:00 Chem 1711 Exam 1 September 26, 2013 Dr. Susan E. Bates Name 9:00 OR 10:00 N A = 6.022 x 10 23 mol 1 I A II A III B IV B V B VI B VII B VIII I B II B III A IV A V A VI A VII A inert gases 1 H 1.008 3 Li

More information

Chem!stry. Assignment on Redox

Chem!stry. Assignment on Redox Chem!stry Name: ( ) Class: Date: / / Assignment on Redox Question 1: Which one of the following elements is the most powerful reducing agent? A Aluminium B Copper C Lead D Potassium Question 2: Which of

More information

**continued on next page**

**continued on next page** Chapter 9 Stoichiometry Section 9.1 Introduction to Stoichiometry Standard.e.: Students know how to calculate the masses of reactant and products in a chemical reaction from the mass of one of the reactants

More information

Which of the following answers is correct and has the correct number of significant figures?

Which of the following answers is correct and has the correct number of significant figures? Avogadro s Number, N A = 6.022 10 23 1. [7 points] Carry out the following mathematical operation: 6.06 10 3 + 1.1 10 2 Which of the following answers is correct and has the correct number of significant

More information

CHEMISTRY 202 Hour Exam I. Dr. D. DeCoste T.A.

CHEMISTRY 202 Hour Exam I. Dr. D. DeCoste T.A. CHEMISTRY 0 Hour Exam I September, 016 Dr. D. DeCoste Name Signature T.A. This exam contains 3 questions on 11 numbered pages. Check now to make sure you have a complete exam. You have two hours to complete

More information

What type of solution that contains all of the

What type of solution that contains all of the What type of solution that contains all of the solute it can hold at a given temperature? Saturated Solution What type of solution that contains less solute than it is able to hold at a given temperature?

More information

REVIEW OF BASIC CHEMISTRY ANSWER KEY

REVIEW OF BASIC CHEMISTRY ANSWER KEY REVIEW OF BASIC CHEMISTRY ANSWER KEY 1. Name the following elements. Spelling counts: 2. Write the symbols for the following elements. H hydrogen sodium Na S sulphur phosphorus P Cl chlorine fluorine F

More information

Name: Period: CHEMISTRY I HONORS SEMESTER 1 EXAM REVIEW

Name: Period: CHEMISTRY I HONORS SEMESTER 1 EXAM REVIEW Name: Period: CHEMISTRY I HONORS SEMESTER 1 EXAM REVIEW Unit 1: Nature of Science What rules must be obeyed to safely conduct an experiment? What are the components of a good scientific experiment? What

More information

Name Period CH 180 Practice Test: Chapters 3 and 4

Name Period CH 180 Practice Test: Chapters 3 and 4 Name Period CH 180 Practice Test: Chapters 3 and 4 Multiple Choice: 1. 11. 2. 12. 3. 13. 4. 14. 5. 15. 6. 16. 7. 17. 8. 18. 9. 19. 10. 20. 21. 22. 23. 24. 25. 26. 27. 1 Directions: Answer all questions.

More information

Dr. Rick Fletcher. Clearly print your name in the name section of the Scantron answer sheet.

Dr. Rick Fletcher. Clearly print your name in the name section of the Scantron answer sheet. Dr. Rick Fletcher Homework 2 Chemistry 101 March 6, 2009 There is one most correct response to each of the multiple choice questions. Choose the best answer. Each of the twenty-five questions is worth

More information

Name. Academic Chemistry Stoichiometry Notes. Unit #10 Test Date: cincochem.pbworks.com

Name. Academic Chemistry Stoichiometry Notes. Unit #10 Test Date: cincochem.pbworks.com Name Academic Chemistry Stoichiometry Notes Unit #10 Test Date: cincochem.pbworks.com Resources Unit 10 Common Polyatomic Ions List 20 Name Common Polyatomic Ion Ions Name Ion acetate C 2 H 3 O 2 or CH3

More information

Chem 205: GENERAL CHEMISTRY I MIDTERM EXAMINATION

Chem 205: GENERAL CHEMISTRY I MIDTERM EXAMINATION Concordia University CHEM 205 Winter 2007 -- MIDTERM EXAM Student ID #: Chem 205: GENERAL CHEMISTRY I MIDTERM EXAMINATION PLEASE READ THIS WHILE WAITING TO START INSTRUCTIONS: This test paper includes

More information

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

MULTIPLE 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) When the following equation is balanced, the coefficients are. 1) NH3 (g) + O2 (g) NO2

More information

Unit 10: Stoichiometry. Stoichiometry= the process of using a to determine the relative amounts of reactants and products involved in a reaction.

Unit 10: Stoichiometry. Stoichiometry= the process of using a to determine the relative amounts of reactants and products involved in a reaction. Unit 10: Stoichiometry Stoichiometry= the process of using a to determine the relative amounts of reactants and products involved in a reaction. Info given by a chemical equation: Chemical changes involve

More information

4) Please indicate whether each of the following units are intensive or extensive. a) Density Intensive Extensive. b) Temperature Intensive Extensive

4) 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 information

941_1 st Exam_ ) Which of the following is not an example of matter? A) wood B) water C) air D) light E) atoms Answer: D

941_1 st Exam_ ) Which of the following is not an example of matter? A) wood B) water C) air D) light E) atoms Answer: D 941_1 st Exam_941020 1) Which of the following does not represent a physical property? A) boiling point B) odor C) density D) reaction with oxygen E) solubility in water 2) Which of the following is not

More information

1st Semester Review Worth 10% of Exam Score

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

More information

CHEMISTRY 1A SPRING 2011 EXAM 1 KEY CHAPTERS 1-4

CHEMISTRY 1A SPRING 2011 EXAM 1 KEY CHAPTERS 1-4 You might find the following useful. Electronegativities H 2.2 CHEMISTRY 1A SPRING 2011 EXAM 1 KEY CHAPTERS 1- Li Be B C N O F 0.98 1.57 2.0 2.55.0..98 Na Mg Al Si P S Cl 0.9 1.1 1.61 1.9 2.19 2.58.16

More information

PRACTICE COMPREHENSIVE EXAM #1 7 th GRADE CHEMISTRY

PRACTICE 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 information

EIT Review S2007 Dr. J.A. Mack.

EIT Review S2007 Dr. J.A. Mack. EIT Review S2007 Dr. J.A. Mack www.csus.edu/indiv/m/mackj/ Part 1 Atom: The smallest divisible unit of an element Compound: A substance made of two or more atoms Ion: A charged atom or molecule Cation:

More information

Experiment #3: When 2.0 g of sodium hydroxide reacts with 2.2 g carbon dioxide, 4.2 g of baking soda (sodium bicarbonate) is produced.

Experiment #3: When 2.0 g of sodium hydroxide reacts with 2.2 g carbon dioxide, 4.2 g of baking soda (sodium bicarbonate) is produced. Name: Dalton s Atomic Theory: (1) Matter is composed of very small units called atoms. Atom is the smallest unit that possesses the chemical property of an element. (2) An element contains only one type

More information

Name AP Chemistry September 30, 2013

Name 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 information

1. How many protons, electrons, and neutrons are in one atom of the following isotopes (6 points)?

1. How many protons, electrons, and neutrons are in one atom of the following isotopes (6 points)? Chemistry 11 Department of Physical Sciences Kingsborough Community College City University of New York NAME Exam 1: Chapters 1-3 50 points 1. How many protons, electrons, and neutrons are in one atom

More information

2) How many oxygen atoms are there in 1.55 ng of Ca3(PO4)2? a) 3.01 x b) 1.20 x c) 3.01 x d) 1.21 x e) 2.

2) How many oxygen atoms are there in 1.55 ng of Ca3(PO4)2? a) 3.01 x b) 1.20 x c) 3.01 x d) 1.21 x e) 2. Name: Directions: Answer the following questions based on your review of Chapters 1-4 in your text along with your education in Chemistry Level I. You must defend your answers in order to receive credit.

More information

Composion Stoichiometry

Composion Stoichiometry Composition Stoichiometry blank 3.3.13.notebook Due: Ch 10 RG Hummmm... How do you "measure" bananas? > How many? Count 1 dozen naners or 12 naners Composion Stoichiometry 3 new conversion factors > Avogadro's

More information

MIDTERM REVIEW. UNIT 1: Mass/Measurement

MIDTERM REVIEW. UNIT 1: Mass/Measurement MIDTERM REVIEW UNIT 1: Mass/Measurement Practice Problems 1. Circle the word/phrase that best fits the statement: A. [ PHYSICAL OR CHEMICAL] changes are changes in which the identity of the substance does

More information

SCH4U Chemistry Review: Fundamentals

SCH4U Chemistry Review: Fundamentals SCH4U Chemistry Review: Fundamentals Particle Theory of Matter Matter is anything that has mass and takes up space. Anything around us and in the entire universe can be classified as either matter or energy.

More information

Chem 101 Practice Exam 3 Fall 2012 You will have a Solubility Table and Periodic Table

Chem 101 Practice Exam 3 Fall 2012 You will have a Solubility Table and Periodic Table Chem 101 Practice Exam Fall 01 You will have a Solubility Table and Periodic Table 1. A 1.6-mol sample of KClO was decomposed according to the equation KClO (s) KCl(s) O (g) How many moles of O are formed

More information

AP Chemistry Summer Assignment

AP Chemistry Summer Assignment Name AP Chemistry Summer Assignment Welcome to AP chemistry! This summer assignment is intended to help you review the basic topics you learned in pre-ap chemistry that are crucial for your success in

More information

CHEM 1413 Chapter 4 Homework Questions TEXTBOOK HOMEWORK

CHEM 1413 Chapter 4 Homework Questions TEXTBOOK HOMEWORK CHEM 1413 Chapter 4 Homework Questions TEXTBOOK HOMEWORK Chapter 3 3.68 Calculate each of the following quantities: (a) Mass (g) of solute in 185.8 ml of 0.267 M calcium acetate (b) Molarity of 500. ml

More information

Unit 2. Chemical Foundations: Elements, Atoms, and Ions

Unit 2. Chemical Foundations: Elements, Atoms, and Ions Unit 2 Chemical Foundations: Elements, Atoms, and Ions Memorize the list of elements You will have a quiz on this list. All of the elements will be on the quiz! Elements in the Earth System (% mass in

More information