Houston Community College System

Size: px
Start display at page:

Download "Houston Community College System"

Transcription

1 . Houston Community College System Chemistry 1311 EXAM # 1A The Periodic table of the Chemical Elements 1

2 CHEM 1311 Sample Exam #1A (1,2, and 3) Part I. Multiple choice questions. ( 4 points each) Direction- Please write your correct choice in space provide. 1. The distance between carbon atoms in ethylene is 134 picometers. Which of the following express the distance in meters? A. 1.34x10-13 m B. 1.34x10-10 m C. 1.34x10-7 m D. 1.34x10-6 m 2. Acetic acid boils at F. What is boiling point in degrees celsius? A C B C C C D C 3. Which of the following expressed measurement 52,030.2 m in correct scientific notation? A x10 4 m B x10 4 m C. 5.20x10 4 m D. 5.2x10 4 m 4. Select the answer with correct number of decimal places for the following sum g g g = A g B g C. 26 g D g 5. Which of the following is a non-metal? A. Li B. Be C. Os D. I 6. Bromine is the only non-metal that is liquid at room temperature. Consider the isotope bromine-81, Br. Select the combination which list the correct atomic number, neutron number, and mass number respectively. A. 35,46,81 B. 35,81,46 C. 81,46,35 D. 46,81,35 7. Which of the following name is correct for given chemical formula? A. I 2 O 5, iodine pentoxide B. LiNO 3, lithium nitrate C. PbO, lead(i) oxide D. H 2 SO4, hydrosulfuric acid 8. Which of the following chemical formula is not correct for given chemical name? A. ferric oxide, Fe 2 O 3 B. calcium hydroxide, Ca(OH) 2 C. tetrasulfur dinitride, S 4 N 2 D. potassium chlorite, KClO 3 9. What is the mass in grams of mole common antiacid, calcium carbonate? A. 4.00x10 2 g B g C. 4.00x10-2 g D. 2.50x10-3 g 2

3 10. Which one of the following reactions is not balanced? A. 2C 6 H 6(l) + 15O 2(g) 12CO 2(g) + 6H 2 O (g) B. B 2 O 3(s) + 6HF (l) 2BF 3(g) + 3H 2 O (l) C. UO 2(g) + 4HF (l) UF 4(s) + 4H 2 O (l) D. 2B 5 H 9(l) + 12O 2(g) 5B 2 O 3(s) + 9 H 2 O (g) 11. Which identification is INCORRECT for the element? A. Na, sodium B. S, sulfur C. P, potassium D. Zn, zinc 12. Which of the following is not a chemical change? A. burning coal B. making bread rise using baking soda C. boiling an egg D. boiling water 13. Which ion has a -1 charge? A. CO 3 B. HSO 3 C. NH 4 D. SO Which of the following is improperly labeled? A. Cu- transition metal B. Mg- alkaline earth metal C. Br- halogen D. U- noble gas 15. How many carbon atoms are in CH 3 -CH 2 -COO-CH 3 A. 1 B. 2 C. 3 D. 4 Part II. Show all your work for complete credit. 16. The density of mercury, the only metal to exist as liquid at room temperature, is 13.6 g/cm 3. What is the density in pounds per cubic inch (lb/in 3 )? ( 1 lb=454 g, 1 in =2.54 cm) ( 8 points) 17. The speed needed to scape the pull of earth, s gravity is 11.3 km/s. What is this speed in mi/hr? ( 1 mi= km) ( 6 points) 18. Lithium, is used in dry cells and storage batteries and in high temperature lubricants, it has two naturally occurring isotopes, 6 Li and 7 Li. Calculate the atomic mass of lithium. ( 8 points) isotopes isotopic mass(amu) abundance(%) 6 Li Li Terphthalic acid, used in the production of polyester fibers and films, is composed of carbon, hydrogen, and oxygen. when g of acid is subjected to combustion analysis 3

4 it produced g CO 2 and g H 2 O. What is its empirical and molecular formula if its molar mass is 172 g/mol. ( 8 points) 20. Aluminum reacts with oxygen to produce aluminum oxide which can be used as an absorbent, desiccant or catalyst for organic reactions. ( 10 points) 4 Al (s) + 3 O 2(g) 2 Al 2 O 3(s) A mixture of 82.4 g of aluminum (M=26.98 g/mol) and g of oxygen (M=32.00 g/mol) is allowed to react. a) Identify the limiting reactant. b) Calculate the mass of aluminum oxide formed. c) Determine the mass of the excess reactant present in the vessel when the reaction is complete. d) What is the percentage yield for the reaction if reaction mixture produce 120 g of aluminum oxide? Bonus question( 10 points)- show all your work. a) When 11.2 g CaCO 3 reacts with excess hydrochloric acid, as below, 4.61 g of CO 2 is produced. What is the percent yield of CO 2? Do not type the units with your answer. CaCO 3 (s) + 2 HCl(aq) CO 2 (g) + CaCl 2 (aq) + H 2 O(l) (not balanced) b) Calcium reacts with oxygen to make calcium oxide, CaO. What is the theoretical yield of CaO(s) that could be prepared from 7.63 g of Ca(s) and 2.56 g of O 2 (g)? 4

5 CHEM 1311 SAMPLE EXAM # 1A - KEY (1, 2, and 3) PART-I 1. B (pico = 10-12, 134 x m = 1.34 x m) 2. C C = 5/ 9(F-32) = 5/ 9( ) = 5/ 9(212.2) = o C 3. A 4. D sum = g, round off to the least number of decimal point (one), sum = 29.3 g 5. D 6. A 7. B LiNO 3 is Lithium nitrate 8. D potassium chlorate, KClO 3 9. B CaCO 3 = 1(40) + 1(12) + 3(16) = 100 g/ml 10. C 2H 2 O (l) 11. C P is the symbol for phosphorous 12. D boiling water is a phase change from liquid to vapor 13. B HSO 3 (bisulfite) 14. D Uranium is an inner transition metal 15. D four carbon atoms PART-II g 1 lb (2.54 cm) x x = lb/ in 3 cm g 1 in km 1 mi 3600 sec x x = 2.53 x 10 4 mi/hr sec km 1 hr 18. Ave. atomic wt. of Li = (7.50/100) ( ) + (92.50/100) ( ) = 6.95 a.m.u. 19. m c = (3/11) mco 2 = (3/11)(1.471) = g, m H = (1/9) mh 2 O = (1/9) (0.391) = g m O = m - (m c + m H ) = ( ) = g C = /12 = , / = 2.14 = 2 H = /1 = , / = 2.78 = 3 O = /16 = , / = 1 = 1 5

6 empirical formula is C 2 H 3 O = 2(12) + 3(1) + 1(16) = 43 X = ( 172/ 43) = 4, (C 2 H 3 O) 4 or C 8 H 12 O 4 20a) (4x27) g (3x32) g (2x102) g 4 Al + 3 O 2 2Al 2 O g g X g (82.4) (2) (102) Al 2 O 3 from Al = = g = 156 g 4 x 27 (117.65) (2) (102) Al 2 O 3 from O 2 = = g 3 x 32 So, Al produce smaller amount of Al 2 O 3. Al is the limiting reagent. b) 156 g Al 2 O 3 formed c) (4x27) g (3x32) g 4 Al + 3 O 2 2Al 2 O g X g (82.4) (3) (32) O 2 used up in the reaction = x 27 O 2 (excess) = g = 44.4 g = 73.2 g 120 d) % yield = x 100 = 77% 156 BONUS QUESTION: a) CaCO 3 (s) + 2 HCl(aq) CO 2 (g) + CaCl 2 (aq) + H 2 O(l) (11.2 g, CaCO 3 ) x ( 1 mole CaCO 3 / 100 g Mwt. ) ( 1mole CO 2 /1 mole CaCO 3 ) (44 g CO 2 / 1 mole CO 2 ) = g CO 2 % yield = ( g, actual value / g, theoretical value) x 100 = 93.5 % b) 2 Ca + O 2 2 CaO (7.63 g Ca) (1 mol Ca / 40 g) ( 1 molo 2 /2 mol Ca) ( 32 g O 2 / 1 mol O 2 ) = g O 2 6

7 3.052 g O 2 requried to react woth 7.63 g Ca. Since have only 2.56 g O 2 in the reaction, therefore O 2 is limiting reagent. (2.56 g, O 2 ) ( 1 mol / 32 g O 2 ) ( 2 mol CaO / 1 mol O 2 ) (56 g CaO / 1 mol CaO ) = 8.96 g CaO, theoretical value of CaO Houston Community College System Chemistry 1311 EXAM # 1B Comparison of Temperature Scales 7

8 CHEM 1311 Exam #1B (1,2, and 3) Directions- please answer the following multiple-choice questions next to each number. Please show all your work for bonus question and part (II) questions in the space provided. Part (I) - Multiple Choice - (3 points each) 1. Which number definitively distinguishes one element from another element? A. charge number B. number of neutrons C. number of protons D. number of electrons 2. A 239.5g sample of Benzene is found to occupy a volume of 274ml. What is its density? A B C D Convert 3.50 ft to cm. A. 107 cm B. 2.9 x 10 2 cm C cm D. 503 cm 4. How many electrons, protons, and neutrons are in an atom of 197 Au 3+? A. 77 electrons, 79 protons, 117 neutrons B. 80 electrons, 78 protons, 116 neutrons C. 76 electrons, 79 protons, 118 neutrons D. 80 electrons, 80 protons, 115 neutrons 5. Which name is incorrect? A. HBr hydrobromic acid B. AlCl 3, aluminum (III) chloride C. MgS, magnesium sulfide D. Mg 3 N 2, magnesium nitrite 6. Which one of the following is improperly labeled? A. He (noble gas) B. K (alkali metal) C. Ca (transition metal) D. Br (halogen) 7. Calculate the formula weight of aniline, C 6 H 7 N. A. 93.g B. 85g C. 62g D. 49g 8. Forty centimeters is equal to how many nanometers(nm)? 8

9 A x 10 8 nm B x nm C x nm D x nm 9. The state of matter with the highest measure of entropy or disorder is called state. A. solid B. gas C. liquid D. mixed 10. Octane burns according to the following equation: 2C 8 H O 2 16CO H 2 O How many grams of CO 2 are produced when 5.00 g of C 8 H 18 are burned? A g B g C g D g 11. The elements with the same atomic number but different atomic masses are called. A. reactants B. isotopes C. anions D. molecules 12. Which of these compounds is not ionic? A. Li 2 SO 4 B. NaF C. SO 3 D. all of these 13. What is the molar mass of cryolite (Na 3 AlF 6 )? A B C D How many Magnesium atoms are in 3.00 moles of Mg 3 (PO 4 ) 2? A x B x C x D x An oxide of iron has the formula Fe 3 O 4. What mass percent of oxygen does it contain? A. 0.72% B. 60% C. 27.6% D. 72.6% 16. Determine the empirical formula of a compound that has (by mass) 85.7% carbon, 14.28% hydrogen. A. CH B. CH 2 C. C 2 H D. C 3 H The empirical formula of styrene is CH, its molecular weight is What is the molecular formula of styrene? A.C 8 H 8 B. C 4 H 4 C. C 10 H 10 D. none of these 18. Give (in order) the correct coefficients to balance the following reaction: C 2 H 4 + O 2 CO 2 + H 2 O A. 1,2,2,4 B. 1,1,1,2 C. 2,2,2,2 D. 1,3,2,2 9

10 19. The melting point of Sulfur is C. What is this on the Fahrenheit scale? A F B F C F D F 20. When g of ethylene ( C 2 H 4 ) burns in oxygen to give carbon dioxide and water, how many grams of CO 2 are produced? A g B g C g D g Part (II) - Show all your work. (8 points each) 21. A hypothetical pure metallic cube has a side of 3.00 cm and a mass of 9.0 grams. What is the density of this cube in ounces per cubic inch (oz/in 3)? (Remember, 16oz equal 1 pound, 2.2lbs = 1kg) 22. A substance, N x O y, has the composition by mass 69.57% O. Calculate the molecular formula of this substance if its molecular mass is 92 grams. 23. A reaction that produces crude iron from iron ore is shown below: Fe 3 O 4 (s) + 4CO (g) 3 Fe (s) + 4CO 2 (g) in How many moles of iron could be produced from the reaction of 2.5 mol Fe 3 O 4 and 3.0 mol of CO? Identify limiting reactant and determine how many moles of unreacted substance remained the reaction. 24. A g sample of a compound known to contain C,H, and O was burned in oxygen to yield g of CO 2 and g of H 2 O. What is the molecular formula of the compound if the molar mass of compound is approximately 140 g. 25. Perform the following calculations and round off the answers to the proper significant figures. a) ml ml ml = b) ( g/ml)(9.00 ml) = 10

11 BONUS question-show all your work.(10 points) Naturally occurring element Y exists in two isotopic forms: Y-57 ( amu ), Y-58 ( amu) Calculate the percentage of each isotope if the average atomic weight of X is amu. CHEM 1311 SAMPLE EXAM # 1B - KEY (1, 2, and 3) Part (I) 1. C 6. C 11. B 16. B 2. A 7. A 12. C 17. A 3. A 8. A 13. B 18. D 4. C 9. B 14. A 19. D 5. D 10. C 15. C 20. B Part (II) 21. D = m/v = (9.0 g/27.00 cm 3 ) = 0.33 g/cm 3 (0.33 g/cm 3 ) ( 10-3 kg/ 1g) ( 2.2lb/ 1kg) ( 16 oz / 1lb) ((2.54cm) 3 /1in 3 )= 0.19oz/ in N = 30.43% O = 69.57% moles N = (92g/14g)(0.3043) = moles O = (92g /16g)(0.6957) = 4.00, So the molecular formula is = N 2 O 4 OR: N = 30.43/14 = /174/2.174 = 1 O =69.57/16 = /2.174 = 2; (empirical formula is NO 2 ) (NO 2 ) X ( )X = (46)X = 92; X = 2; (NO 2 ) 2 N 2 O mole 4.0 mole 3 mole 4 mole Stoichiometric Relations Fe 3 O 4 (s) + 4CO (g) 3 Fe (s) + 4CO 2 (g) 2.5 mole 3.0 mole X mole Stoichiometric molar ratio of reactants Fe 3 O 4 /4CO =1/4 =

12 Given 2.0 mole Fe 3 O 4 to 2.5 mole CO; molar ratio is 2.5/3.0 = Fe 3 O 4 is in excess and CO is limiting reagent. So use CO for stoichiometric relations to other reactant and products. X (from Fe 3 O 4 ) X (from CO) (2.5)(3.0) = = 7.5 moles Fe 1.0 (3.0)(3.0) = = 2.25 moles Fe (CO is limiting reagent) 4.0 mol CO used in the reaction = ( 3.0 mol CO)( 1 mol Fe 3 O 4 mol/ 4 mol CO) = 0.75 mol = 1.75 mol Fe remain in the reaction 24. mc = 3/11(1.729) = g, C mh = 1/9 (0.3535) = g, H mo = ( ) = g, O C (0.4715/0.9301)(140/12) = 5.9 = 6.0 H ( /0.9301)(140/1) = 5.9 = 6.0 O (0.4194/0.9301)(140/16) = 3.9 = 4.0, Therefore the molecular formula is C 6 H 6 O 4 OR C = ( /12) = ( / ) = 1.49 =1.5; 1.5 x 2 = 3 H = ( /1) = ( / ) = 1.49 = 1.5; 1.5 x 2 = 3 O = (0.4194/ 16)= ( / ) = 1.00 = 1.0; 1 x 2 = 2 The empirical formula is ; C 3 H 3 O 2 (C 3 H 3 O 2 ) n = 140, (71) n = 140, n = 140 /71, n = 2 the molecular formula is ; C 6 H 6 O a) 15.0 ml is the number with the least number of decimal places. Answer is 44.8 ml b) 9.00 ml is the number with the least number of significant figures(3 sig. Fig.) Answer is 386 g BONUS 12

13 Let fractional abundance of isotope X-57 be A; then = (Y/100) (100 Y/100) Y = 20.1% for isotope X-57. and % abundance of isotope X-58 is 79.9%. 13

1. The distance between carbon atoms in ethylene is 134 picometers. Which of the following express the distance in meters?

1. The distance between carbon atoms in ethylene is 134 picometers. Which of the following express the distance in meters? CHEM 1411 Exam #1 (1,2, and 3) Name: Score Part I. Multiple choice questions. ( 4 points each) Direction- Please write your correct choice in space provide. 1. The distance between carbon atoms in ethylene

More information

CHEM 1411 SAMPLE FINAL EXAM

CHEM 1411 SAMPLE FINAL EXAM PART I - Multiple Choice (2 points each) CHEM 1411 SAMPLE FINAL EXAM 1. The distance between carbon atoms in ethylene is 134 picometers. Which of the following expresses this distance in meters? A. 1.34

More information

UNIT 1 Chemical Reactions Part II Workbook. Name:

UNIT 1 Chemical Reactions Part II Workbook. Name: UNIT 1 Chemical Reactions Part II Workbook Name: 1 Molar Volume 1. How many moles of a gas will occupy 2.50 L at STP? 2. Calculate the volume that 0.881 mol of gas at STP will occupy. 3. Determine the

More information

Houston Community College System

Houston Community College System Houston Community College System Chemistry 1305/1405 FINAL EXAM REVIEW Vitamin A Helps form and maintain healthy teeth, skeletal and soft tissue, mucous membranes, and skin. CHEM 1305/1405 Final Exam PART

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

This packet contains review material from Pre-AP Chemistry. Be prepared to take a quiz over this material during the first week of school.

This packet contains review material from Pre-AP Chemistry. Be prepared to take a quiz over this material during the first week of school. This packet contains review material from Pre-AP Chemistry. Be prepared to take a quiz over this material during the first week of school. How many significant figures (digits) are represented by each

More information

Advanced Placement Chemistry ~ Summer Assignment Part 2. Name

Advanced 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 information

2. Relative molecular mass, M r - The relative molecular mass of a molecule is the average mass of the one molecule when compared with

2. Relative molecular mass, M r - The relative molecular mass of a molecule is the average mass of the one molecule when compared with Chapter 3: Chemical Formulae and Equations 1. Relative atomic mass, A r - The relative atomic mass of an element is the average mass of one atom of an element when compared with mass of an atom of carbon-12

More information

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

Counting by mass: The Mole. Unit 8: Quantification of Chemical Reactions. Calculating molar mass. Particles. moles and mass. moles and particles Unit 8: Quantification of Chemical Reactions Chapter 10: The mole Chapter 12: Stoichiometry Counting by mass: The Mole Chemists can t count individual atoms Use moles to determine amounts instead mole

More information

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

Unit Five- Chemical Quantities Chapter 9: Mole ratios, conversions between chemicals in a balanced reaction (mole, mass), limiting reactant, % yield

Unit 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 information

CH 221 Sample Exam Exam II Name: Lab Section:

CH 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 information

CHM 100 CHEMISTRY MAN & ENVIRONMENT Comprehensive SAMPLE MIDTERM EXAM

CHM 100 CHEMISTRY MAN & ENVIRONMENT Comprehensive SAMPLE MIDTERM EXAM CHM 100 CHEMISTRY MAN & ENVIRONMENT Comprehensive SAMPLE MIDTERM EXAM Multiple Choice: Identify the choice that best completes the statement or answers the question. 1. Determine the mass in grams of a

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

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

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

Unit 1 SOME BASIC CONCEPTS OF CHEMISTRY I. Multiple Choice Questions (Type-I) 1. Two students performed the same experiment separately and each one of them recorded two readings of mass which are given

More information

CHM 134 General Chemistry I Name SOLUTIONS Exam 1, Fall 2008 Dr. Steel

CHM 134 General Chemistry I Name SOLUTIONS Exam 1, Fall 2008 Dr. Steel CHM 14 General Chemistry I Name SOLUTIONS Exam 1, Fall 2008 Dr. Steel Section 1: Multiple Choice. Circle the choice that is the best answer to each question. Each question in this section is worth 2 points.

More information

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

(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

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

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

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

CHEM 121a Exam 1 Fall 1997

CHEM 121a Exam 1 Fall 1997 SSN CHEM 121a Exam 1 Fall 1997 This exam consists of 20 multiple choice questions (each worth 3 points), and 4 problems (each worth 10 points). There are a total of 100 possible points. Part I. Multiple

More information

Funsheet 3.0 [WRITING & BALANCING EQUATIONS] Gu/R. 2017

Funsheet 3.0 [WRITING & BALANCING EQUATIONS] Gu/R. 2017 Funsheet 3.0 [WRITING & BALANCING EQUATIONS] Gu/R. 2017 Balance the following chemical equations. Remember, it is not necessary to write "1" if the coefficient is one. 1. N 2 + H 2 NH 3 2. KClO 3 KCl +

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

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

CHM 1045 Qualifying Exam

CHM 1045 Qualifying Exam CHM 1045 Qualifying Exam 1. Which of the following is the basic unit of volume in the metric system? A) liter B) kilogram C) meter D) centimeter E) gram 2. Which of the following is the largest unit? A)

More information

AP Chemistry Summer Assignment

AP Chemistry Summer Assignment AP Chemistry Summer Assignment Due Date: Thursday, September 1 st, 2011 Directions: Show all of your work for full credit. Include units and labels. Record answers to the correct number of significant

More information

Name. Last 5 digits of Student Number: XXX X (may be the same as your social security number) Chem 103 Sample Examination #1

Name. Last 5 digits of Student Number: XXX X (may be the same as your social security number) Chem 103 Sample Examination #1 α page 1 of 8 KEY ame Last 5 digits of Student umber: XXX X (may be the same as your social security number) hem 103 Sample Examination #1 This exam consists of eight (8) pages, including this cover page.

More information

First Semester Final Exam Study Guide

First Semester Final Exam Study Guide First Semester Final Exam Study Guide Name: Chemistry 1 2 3 4 5 6 7 60 multiple choice questions Chapter 4 1. Explain the law of conservation of mass. 2. What mass of product is produced in the following

More information

First Semester Final Exam Study Guide

First Semester Final Exam Study Guide First Semester Final Exam Study Guide Name: Chemistry 1 2 3 4 5 6 7 60 multiple choice questions Chapter 1 1. Define matter and list five examples. Chapter 2 2. Define pure substance. 3. Define element.

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

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

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

Practice Problems: Set #3-Solutions

Practice Problems: Set #3-Solutions Practice Problems: Set #3-Solutions IIa) Balance the following equations:(10) 1) Zn (s) + H 3 PO 4 (aq) Zn 3 (PO 4 ) 2 (s) + H 2 (g) 3Zn (s) + 2H 3 PO 4 (aq) Zn 3 (PO 4 ) 2 (s) + 3H 2 (g) 2. Mg 3 N 2 (s)

More information

CHM 111 Final Fall 2012

CHM 111 Final Fall 2012 Name Part I. Multiple Choice 1. Consider the following specific heats of metals. Metal copper cobalt chromium gold silver CHM 111 Final Fall 2012 Specific Heat 0.385 J/(g C) 0.418 J/(g C) 0.447 J/(g C)

More information

Balancing Equations Notes

Balancing Equations Notes . Unit 9 Chemical Equations and Reactions What is a Chemical Equation? A is a written representation of the process that occurs in a chemical reaction. A chemical equation is written with the (starting

More information

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

!!! DO NOT OPEN THIS EXAM BOOK UNTIL TOLD TO DO SO BY THE INSTRUCTOR!!! CHEM 142 - 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

More information

1. Which of the following is describing a physical property of a substance?

1. Which of the following is describing a physical property of a substance? CHM 1045 Test #1 September 19, 2000 1. Which of the following is describing a physical property of a substance? a. It does not react with ammonia b. It dissolves in acid to give off hydrogen gas. c. It

More information

Review for Chemistry Final Exam [Chapters 1-9 & 12]

Review for Chemistry Final Exam [Chapters 1-9 & 12] Name: Block: Date: Chapter 1 Matter and Change Review for Chemistry Final Exam [Chapters 1-9 & 12] 1-1. Define the terms matter and atom. 1-2. Define the terms element and compound and list some examples

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

CP Chemistry Final Exam Review

CP 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 information

Stoichiometry CHAPTER 12

Stoichiometry CHAPTER 12 CHAPTER 12 Stoichiometry 12.1 Using Everyday Equations Stoichiometry is the calculation of quantities in chemical equations. * The balanced equation gives the ratios for the reactants and products. 3 eggs

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

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

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

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

More information

Unit 6: Stoichiometry. How do manufacturers know how to make enough of their desired product?

Unit 6: Stoichiometry. How do manufacturers know how to make enough of their desired product? Unit 6: Stoichiometry How do manufacturers know how to make enough of their desired product? Chocolate Chip Cookies Using the following recipe, complete the questions. Cookie Recipe 1.5 c sugar 1 c. butter

More information

Formulas and Models 1

Formulas 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 information

AP Chemistry Summer Review Assignment

AP Chemistry Summer Review Assignment Name: Period: Chem I Teacher/year: AP Chemistry Summer Review Assignment Due on the FIRST DAY OF SCHOOL! A. Chemical Foundations 1. The beakers shown below have different precisions. a. Label the amount

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

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

1071-1st Chem Exam (A)

1071-1st Chem Exam (A) 1071-1st Chem Exam-1071017(A) MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) The correct answer (reported to the proper number of significant

More information

9.) A chloride of rhenium contains 63.6% rhenium. What is the formula of this compound? (ReCl 3 )

9.) A chloride of rhenium contains 63.6% rhenium. What is the formula of this compound? (ReCl 3 ) Homework Stoichiometry 1.) An oxide of iron has the formula Fe 3 O 4. What mass percent of iron does it contain? (72.360%) 2.) Hydrocortisone valerate is an ingredient in hydrocortisone cream, prescribed

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

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

Chapter 8 Chemical Reactions

Chapter 8 Chemical Reactions Chemistry/ PEP Name: Date: Chapter 8 Chemical Reactions Chapter 8: 1 7, 9 18, 20, 21, 24 26, 29 31, 46, 55, 69 Practice Problems 1. Write a skeleton equation for each chemical reaction. Include the appropriate

More information

Due Friday, August 18 th, 2017 Mrs. Hockstok - AP Chemistry Class Olentangy Orange High School Summer Assignment

Due Friday, August 18 th, 2017 Mrs. Hockstok - AP Chemistry Class Olentangy Orange High School Summer Assignment Due Friday, August 18 th, 2017 Mrs. Hockstok - AP Chemistry Class Olentangy Orange High School Summer Assignment 2017-2018 You will have a quiz on the first day of school (August 16 th, 2017) on the polyatomic

More information

IGCSE (9-1) Edexcel - Chemistry

IGCSE (9-1) Edexcel - Chemistry IGCSE (9-1) Edexcel - Chemistry Principles of Chemistry Chemical Formulae, Equations and Calculations NOTES 1.25: Write word equations and balanced chemical equations (including state symbols): For reactions

More information

Honor s Chemistry: Fall Semester Final

Honor s Chemistry: Fall Semester Final Honor s Chemistry: Fall Semester Final Name 1. Explain what is wrong with the statement My friend burned a piece of paper (a hydrocarbon) that had the final exam on it and it disappeared. (Be sure to use

More information

HL First-Year Chemistry

HL First-Year Chemistry 1. Atomic Structure and Stoichiometry Solutions to further problems: 1. (a) 55 86 6 Fe (b) Rb (c) 1 1 7 81 Tl (d) Cr HL First-Year Chemistry. Introduction of the source, vaporization of the sample, ionization,

More information

CP Chemistry Final Exam Review

CP 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 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

Chapter 3 Stoichiometry: Calculations with Chemical Formulas and Equations. Stoichiometry

Chapter 3 Stoichiometry: Calculations with Chemical Formulas and Equations. Stoichiometry Chapter 3 : Calculations with Chemical Formulas and Equations Anatomy of a Chemical Equation CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2 H 2 O (g) Anatomy of a Chemical Equation CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2

More information

Stoichiometry. The quantitative study of reactants and products in a chemical reaction. Burlingame High School Chemistry

Stoichiometry. The quantitative study of reactants and products in a chemical reaction. Burlingame High School Chemistry Stoichiometry The quantitative study of reactants and products in a chemical reaction 1 Stoichiometry Whether the units given for reactants or products are moles, grams, liters (for gases), or some other

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

CH 221 Chapter Four Part II Concept Guide

CH 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 information

2. The accepted density for copper is 8.96 g/ml. Calculate the percent error for a measurement of 8.86 g/ml.

2. The accepted density for copper is 8.96 g/ml. Calculate the percent error for a measurement of 8.86 g/ml. Chem 250 2 nd Semester Exam Review Worksheet (answers and units are at the end of this worksheet, cross them off as you write down the answers to each question.) 1. Round to the correct number of significant

More information

CH141, Fall 2017 Exam 1 10/3/2017. Section (please circle): A(Rice) B(McKinney)

CH141, 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 information

SIC CONCEPTS TS OF CHEMISTRY. Unit. I. Multiple Choice Questions (Type-I)

SIC CONCEPTS TS OF CHEMISTRY. Unit. I. Multiple Choice Questions (Type-I) Unit 1 SOME BASIC B SIC CONCEPTS CONCEP TS OF CHEMISTRY CHEMIS I. Multiple Choice Questions (Type-I) 1. Two students performed the same experiment separately and each one of them recorded two readings

More information

Slide 1 / 90. Stoichiometry HW. Grade:«grade» Subject: Date:«date»

Slide 1 / 90. Stoichiometry HW. Grade:«grade» Subject: Date:«date» Slide 1 / 90 Stoichiometry HW Grade:«grade» Subject: Date:«date» Slide 2 / 90 1 The calculation of quantities in chemical equations is called. A B C D E accuracy and precision dimensional analysis percent

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

Name: Class: Date: ID: A. (g), what is the ratio of moles of oxygen used to moles of CO 2 produced? a. 1:1 b. 2:1 c. 1:2 d. 2:2

Name: Class: Date: ID: A. (g), what is the ratio of moles of oxygen used to moles of CO 2 produced? a. 1:1 b. 2:1 c. 1:2 d. 2:2 Name: Class: _ Date: _ Chpt 12 review Multiple Choice Identify the choice that best completes the statement or answers the question. 1. What is conserved in the reaction shown below? H 2 + Cl 2 2HCl a.

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

Semester 1 Exam Review

Semester 1 Exam Review Semester 1 Exam Review 1. Compare physical and chemical changes in matter. Physical changes involve changing a substance s shape, texture, or size, not its chemical composition. Chemical changes result

More information

REVIEW of Grade 11 Chemistry

REVIEW of Grade 11 Chemistry REVIEW of Grade 11 Chemistry SCH4U_08-09 NAME: Section A: Review of Rules for Significant Digits All measurements have a certain degree of associated with them. All the accurately known digits and the

More information

Spring Semester Final Exam Study Guide

Spring Semester Final Exam Study Guide Honors Chemistry Name Period AlCl3 Cu2S NaCN HI PCl3 CrBr3 Naming and Formula Writing 1. Write the name or formula for each of the following: HClO2 (NH4)2SO4 I4O10 H3N NiN H3PO4 Mercury (II) bromide Phosphorous

More information

Chemistry Midterm Exam Review Sheet Spring 2012

Chemistry 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 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

Chemistry 1-2E Semester I Study Guide

Chemistry 1-2E Semester I Study Guide Chemistry 1-2E Semester I Study Guide Name Hour Chapter 1 1. Define the following terms. Matter Mass Law of Conservation of Mass 2. Define and give 2 examples of the following: Pure substance Element Compound

More information

Stoichiometry CHAPTER 12

Stoichiometry CHAPTER 12 CHAPTER 12 Stoichiometry 12.1 Using Everyday Equations Stoichiometry is the calculation of quantities in chemical equations. Jan 16 7:57 AM May 24 10:03 AM * The balanced equation gives the ratios for

More information

Balancing Equations Notes

Balancing Equations Notes . Unit 6 Chemical Equations and Reactions What is a Chemical Equation? A Chemical Equation is a written representation of the process that occurs in a chemical reaction. A chemical equation is written

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

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) A 25 g sample of sugar is found to contain 51.4% oxygen by mass. Another 250 g sample

More information

Ch 8 Quant. in Chem RXNs/Stoichiometry STUDY GUIDE Accelerated Chemistry

Ch 8 Quant. in Chem RXNs/Stoichiometry STUDY GUIDE Accelerated Chemistry Ch 8 Quant. in Chem RXNs/Stoichiometry STUDY GUIDE Accelerated Chemistry Name /108 TRUE/FALSE. Write 'T' if the statement is true and 'F' if the statement is false. Correct the False statments by changing

More information

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

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

More information

General Chemistry First Semester Final Exam Study Guide 60 multiple choice questions

General Chemistry First Semester Final Exam Study Guide 60 multiple choice questions General Chemistry First Semester Final Exam Study Guide 60 multiple choice questions 1. Define product. 2. Define reactant. 3. Label the products and reactants in the following chemical reactions: H 2

More information

Chemistry Final Exam Sample Items

Chemistry Final Exam Sample Items Chemistry Final Exam Sample Items 1. Which best describes the current atomic theory? a. Atoms consist of electrons circling in definite orbits around a positive nucleus. b. Atoms are composed of electrons

More information

Mass Relationships in Chemical Reactions. Chapter 3 Chang & Goldsby Modified by Dr. Juliet Hahn

Mass Relationships in Chemical Reactions. Chapter 3 Chang & Goldsby Modified by Dr. Juliet Hahn Mass Relationships in Chemical Reactions Chapter 3 Chang & Goldsby Modified by Dr. Juliet Hahn Example 3.6 (3) We now write, 6.07 g CH 4 1 mol CH 4 16.04 g CH 4 = 0.378 mol CH 4 Thus, there is 0.378 mole

More information

Quantitative Chemistry. AQA Chemistry topic 3

Quantitative Chemistry. AQA Chemistry topic 3 Quantitative Chemistry AQA Chemistry topic 3 3.1 Conservation of Mass and Balanced Equations Chemical Reactions A chemical reaction is when atoms are basically rearranged into something different. For

More information

AP CHEMISTRY THINGS TO KNOW

AP 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 information

UNIT 3 IB MATERIAL BONDING, MOLES & STOICHIOMETRY

UNIT 3 IB MATERIAL BONDING, MOLES & STOICHIOMETRY UNIT 3 IB MATERIAL Name: BONDING, MOLES & STOICHIOMETRY ESSENTIALS: Know, Understand, and Be Able To Apply the mole concept to substances. Determine the number of particles and the amount of substance

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

The Atom, The Mole & Stoichiometry. Chapter 2 I. The Atomic Theory A. proposed the modern atomic model to explain the laws of chemical combination.

The Atom, The Mole & Stoichiometry. Chapter 2 I. The Atomic Theory A. proposed the modern atomic model to explain the laws of chemical combination. Unit 2: The Atom, The Mole & Stoichiometry Chapter 2 I. The Atomic Theory A. proposed the modern atomic model to explain the laws of chemical combination. Postulates of the atomic theory: 1. All matter

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

Chemistry 11 Course Review

Chemistry 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 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

2. The beakers shown below have different precisions.

2. The beakers shown below have different precisions. Name: Period: Chem I Teacher: AP Chemistry Summer Review Assignment Due on the FIRST DAY OF SCHOOL! A. Chemical Foundations 1. For each of the following pieces of glassware, provide a sample measurement

More information

Nomenclature (Naming Compounds) and Chemical Formulas

Nomenclature (Naming Compounds) and Chemical Formulas Nomenclature (Naming Compounds) and Chemical Formulas 1 Ions formed from a single atom Monatomic Ions Charges are determined by whether ion has lost electrons (+) or gained electrons (-) Symbols are written

More information

GENERAL CHEMISTRY I CHEM SYSTEM FINAL EXAM VERSION A Fall 2016

GENERAL CHEMISTRY I CHEM SYSTEM FINAL EXAM VERSION A Fall 2016 GENERAL CHEMISTRY I CHEM 1411 SYSTEM FINAL EXAM VERSION A Fall 2016 Departmental Final Exam General Chemistry I, CHEM 1411 Fall 2016 VERSION A Part I: 35 Multiple Choice (2 pts each). Directions: Select

More information