Name Date Hour Honors Chemistry Final Exam Study Guide. For problems 1-4, express each number in scientific notation
|
|
- Martin Lucas
- 5 years ago
- Views:
Transcription
1 Name Date Hour Honors Chemistry Final Exam Study Guide For problems 1-4, express each number in scientific notation 1.) m 2.) mi 3.) m 4.) m ) Convert 3.55 kg to grams 6.) Convert 8944 mm to meters 7.) Convert 4598 mg to kilograms 8.) Convert L to milliliters 9.) Convert 22.5 in. To centimeters 10.) 126 ft to meters 11.) 825 yd to kilometers 12.) 2.4 in. To millimeters ) A gangsta needs to chase after the dirty thief who snitched his wallet. The thief is super fast but will get tired of running after running 10.0 km and the gangsta has a running pace of 7.5 mi/h. How many minutes will the gangsta be running before the thief gets tired? (Hint: 7.5 mi/h as a conversion factor between distance and time) 14.) A gangsta got in a fight and knocked out a guys tooth crown which is supposedly real gold. After testing it to determine its density he finds out that it displaces 10.7 ml of water and has a mass of 206 g. Could the gangsta have really scored himself some legit gold? 15.) An automobile gasoline tank holds 42 kg of gasoline. When the gasoline burns, 168 kg of oxygen are consumed and carbon dioxide and water are produced. What is the total combined mass of carbon dioxide and water that is produced?
2 16.) A common type of handwarmer contains iron powder that reacts with oxygen to form an oxide of iron. As soon as the handwarmer is exposed to air, the reaction begins and heat is emitted. Is the reaction between the iron and oxygen exothermic or endothermic? Draw an energy diagram showing the relative energies of the reactants and the products in the reaction ) Which statements about protons are true? A.) Protons have twice the mass of neutrons B.) Protons have the same magnitude of charge as elections but are opposite in sign C.) Most atoms have more protons than elections D.) Protons have a charge of ) List the symbol and atomic number corresponding to each element A.) Carbon B.) Nitrogen C.) Sodium D.) Potassium E.) Copper 19.) Classify each element as a metal, nonmetal or metalloid A.) Sr B.) Mg C.) F D.) N E.) As 20.) Which elements would you expect to lose elections in chemical changes? A.) Potassium B.) Sulfur C.) Fluorine D.) Barium E.) Copper 21.) Classify each element as halogen, a noble gas, or neither A.) Cl B.) Kr C.) F D.) Ga E.) He 22.) Which pair of elements do you expect to be most similar? Why? A.) Si and P B.) Cl and F C.) Na and Mg D.) Mo and Sn E.) N and Ni
3 23.) Complete each ionization equation. A.) B.) C.) D.) 24.) Predict the ion formed by each element A.) Rb B.) K C.) Al D.) O 25.) Write the symbol for each isotope in the form A.) Cobalt-60 B.) Neon-22 C.) Iodine-131 D.) Plutonium ) Determine the number of protons and neutrons in each isotope: A.) B.) C.) D.) 27.) Use the law of constant composition to complete the table summarizing the amounts of nitrogen and oxygen produced upon the decomposition of several samples of dinitrogen monoxide. 28.) How many oxygen atoms are in each chemical formula? A.) H 3 PO 4 B.) Na 2 HPO 4 C.) Ca(HCO 3 ) 2 D.) Ba(C 2 H 3 O 2 ) 2 29.) Classify each compound as ionic or molecular A.) CS 2 B.) CuO C.) KI D.) PCl 3
4 30.) What are the basic units--single atoms, molecules, or formula units--that compose each substance? A.) BaBr 2 B.) Ne C.) I 2 D.) CO 31.) Name each ionic compound. In each of these compounds, the metal forms more than one type of ion. A.) CrCl 2 B.) CrCl 3 C.) SnO 2 D.) PbI 2 32.) Name each ionic compound containing a polyatmoic ion A.) Ba(NO 3 ) 2 B.) Pb(C 2 H 3 O 2 ) 2 C.) NH 4 I D.) KClO 3 E.) CoSO 4 F.) NaClO 4 33.) Write a formula for each ionic compound. A.) Copper (II) Bromide B.) Silver Nitrate C.) Potassium Hydroxide D.) Sodium Sulfate E.) Potassium Hydrogen Sulfate F.) Sodium Hydrogen Carbonate 34.) Name each molecular compound. A.) SO 2 B.) NI 3 C.) BrF 5 D.) NO E.) N 4 Se 4 35.) How many moles of atoms are in each elemental sample? A.) 1.34 g Zn B.) 24.9 g Ar C.) 72.5 g Ta D.) g Li 36.) How many atoms are in each elemental sample? A.) 16.9 g Sr B.) 26.1 g Fe C.) 8.55 g Bi D.) 38.2 g of P
5 37.) Complete the table: 38.) Determine the number of moles of molecules (or formula units) in each sample. A.) 38.2 g sodium chloride B.) 36.5 g nitrogen monoxide C.) 4.25 kg carbon dioxide D.) 2.71 mg carbon tetrachloride 39.) Complete the table: 40.) Calculate the mass percent composition of nitrogen in each compound. A.) N 2 O B.) NO C.) NO 2 D.) N 2 O 5 41.) Iron ores have different amounts of iron per kilogram of ore. Calculate the mass percent composition of iron for each iron ore: Fe 2 O 3 (hematite), Fe 3 O 4 (magnetite), FeCO 3 (siderite). Which ore has a the highest iron content? 42.) The rotten smell of decaying animal carcass is partially due to a nitrogen-containing compound called putrescine. Elemental analysis of putrescine shows that it consists of 54.50% C, 13.73% H, and 31.77% N. Calculate the empirical formula of putrescine. 43.) The molar masses and empirical formulas of several compounds containing carbon and chlorine are as follows. Find the molecular formula of each compound. A.) g/ mol, CCl B.) g/mol, C 2 HCl 3 C.) g/mol, C 2 HCl
6 44.) Butanedione, a component of butter and body odor, has a cheesy smell. Elemental analysis of butanedione gave the mass percent composition: C, 55.80%; H, 7.03%; O, 37.17%. The molar mass of butanedione is g/mol. Determine the molecular formula of butanedione. 45.) Write a balanced chemical equation for each chemical reaction. A.) Solid lead (II) sulfide reacts with aqueous hydrochloric acid to form solid lead (II) chloride and dihydrogen sulfide gas. B.) Gaseous carbon monoxide reacts with hydrogen gas to form gaseous methane (CH 4 ) and liquid water C.) Solid iron (III) oxide reacts with hydrogen gas to form solid iron and liquid water D.) Gaseous ammonia (NH 3 ) reacts with gaseous oxygen to form gaseous nitrogen monoxide and gaseous water E.) Solid magnesium reacts with aqueous copper (I) nitrate to form aqueous magnesium nitrate and solid copper F.) Gaseous dinitrogen pentoxide decomposes to form nitrogen dioxide and oxygen gas G.) Solid calcium reacts with aqueous nitric acid to form aqueous calcium nitrate and hydrogen gas H.) Liquid methanol (CH 3 OH) reacts with oxygen gas to form gaseous carbon dioxide and gaseous water I.) Solid Vanadium (V) Oxide with hydrogen gas to form solid vanadium (III) oxide and liquid water J.) BaO 2 (s) + H 2 SO 4 (aq) --> BaSO 4 (s) + H 2 O 2 (aq) K.) Co(NO 3 ) 3 (aq) + (NH 4 ) 2 S(aq) --> Co 2 S 3 (s) + NH 4 NO 3 (aq) L.) Li 2 O(s) + H 2 O(l) --> LiOH(aq) M.) Hg 2 (C 2 H 3 O 2 ) 2 (aq) + KCl(aq) --> Hg 2 Cl 2 (s) + KC 2 H 3 O 2 (aq) 46.) Determine whether each compound is soluble or in-soluble. For the soluble compounds, identify the ions present in solution. A.) NaC 2 H 3 O 2 B.) Sn(NO 3 ) 2 C.) AgI D.) Na 3 (PO 4 )
7 47.) Determine whether each equation for a precipitation reaction is correct. Correct any incorrect equations. If no reaction occurs, write NO REACTION. A.) Ba(NO 3 ) 2 (aq) + (NH 4 ) 2 SO 4 (aq) --> BaSO 4 (s) + 2 NH 4 NO 3 (aq) B.) BaS(aq) + 2 KCl(aq) --> BaCl 2 (s) + K 2 S(aq) C.) 2 KI(aq) + Pb(NO 3 ) 2 (aq) --> PbI 2 (s) + 2 KNO 3 (aq) D.) Pb(NO 3 ) 2 (aq) + 2 LiCl(aq) --> 2 LiNO 3 (s) + PbCl 2 (aq) 48.) A solution contains an unknown amount of dissolved calcium. Addition of mol of K 3 PO 4 causes complete precipitation of all the calcium. How many moles of calcium were dissolved in the solution? What mass of calcium was dissolved in the solution?
3) What is the correct value for Avogadro's number? 3) A) x 1033 B) x 1023 C) x D) x 1022
CHM1025 Exam 3 Chapters 6, 7, & 8 MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) How many hydrogen atoms are in 35.0 grams of hydrogen gas? 1)
More informationUnit Two Worksheet WS DC U2
Unit Two Worksheet WS DC U2 Name Period Short Answer [Writing]. Write skeleton equations representing the following reactions and then balance them. Then identify the reaction type. Include all needed
More informationChapter 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 informationChemical Reactions CHAPTER Reactions and Equations
CHAPTER 9 Chemical Reactions 9.1 Reactions and Equations The process by which atoms of one or more substances are rearranged to form different substances is called a chemical reaction. There are a number
More informationBalancing Equations Notes
. Unit 9 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 informationCHM 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 informationUnit 4: Reactions and Stoichiometry
Unit 4: Reactions and Stoichiometry Reactions Chemical equation Expression representing a chemical reaction Formulas of reactants on the left side Formulas of products on the right side Arrow(s) connect(s)
More informationIdentify the reaction type, predict the products, and balance the equations. If it is a special decomposition or synthesis, identify which kind.
Identify the reaction type, predict the products, and balance the equations. If it is a special decomposition or synthesis, identify which kind. 1. calcium + oxygen 2. cupric carbonate 3. aluminum + hydrochloric
More informationUnit IV: Chemical Equations & Stoichiometry
Unit IV: Chemical Equations & Stoichiometry A. The chemical equation B. Types of chemical reactions A. Activity series of metals B. Solubility rules C. Rules for writing and balancing equations D. Calculations
More informationBalancing 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 informationGeneral Chemistry 1 CHM201 Unit 2 Practice Test
General Chemistry 1 CHM201 Unit 2 Practice Test 1. Which statement about the combustion of propane (C 3H 8) is not correct? C 3H 8 5O 2 3CO 2 4H 2O a. For every propane molecule consumed, three molecules
More informationCh 7 Chemical Reactions Study Guide Accelerated Chemistry SCANTRON
Ch 7 Chemical Reactions Study Guide Accelerated Chemistry SCANTRON Name /80 TRUE/FALSE. Write 'T' if the statement is true and 'F' if the statement is false. Correct the False statments by changing the
More informationChemical Equations and Chemical Reactions
Chemical Equations Chemical Equations and Chemical Reactions Chemical equations are concise representations of chemical reactions. Chemical Equations Symbols Used in Chemical Equations The formulas of
More informationBalancing 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 informationChemical Reactions. Ch. 11 Chemical Reactions. Chemical Reactions. Chemical Reactions
Chemical Reactions Ch. 11 Chemical Reactions when a substance changes identity Reactants - original Products - resulting law of conservation of mass total mass of reactants = total mass of products In
More informationIntroductory Chemistry I Chemistry 1111 September 17, 2009 Hour Examination I Name There is a Periodic Table and a summary of solubility rules attached to the end of this examination. You may use a non-programmed
More information5. [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 informationACP Chemistry (821) - Mid-Year Review
ACP Chemistry (821) - Mid-Year Review *Be sure you understand the concepts involved in each question. Do not simply memorize facts!* 1. What is chemistry? Chapter 1: Chemistry 2. What is the difference
More informationCHAPTER 9 CHEMICAL QUANTITIES
Chemistry Name Hour Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 9 CHEMICAL QUANTITIES Day Plans for the day Assignment(s) for the day 1 Begin Chapter
More informationCHM 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 information2. Identify each of the following samples of matter as heterogeneous or homogeneous.
EOC REVIEW #1 1. List the following in order from smallest to largest. (A) 1 dm 3 (B) 1 ml (C) 1 cl (D) 1 L (E) 1 dl 2. Convert the following. Express your answer in standard scientific notation. (A) 36
More informationThis 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 informationAqueous Reactions. The products are just the cation-anion pairs reversed, or the outies (A and Y joined) and the innies (B and X joined).
Aqueous Reactions Defining Aqueous Reactions Aqueous reactions are reactions that take place in water. To understand them, it is important to understand how compounds behave in water. Some compounds are
More information1) What is the volume of a tank that can hold Kg of methanol whose density is 0.788g/cm 3?
1) Convert the following 1) 125 g to Kg 6) 26.9 dm 3 to cm 3 11) 1.8µL to cm 3 16) 4.8 lb to Kg 21) 23 F to K 2) 21.3 Km to cm 7) 18.2 ml to cm 3 12) 2.45 L to µm 3 17) 1.2 m to inches 22) 180 ºC to K
More informationPractice 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 informationFinal Exam Review Questions You will be given a Periodic Table, Activity Series, and a Common Ions Chart CP CHEMISTRY
Final Exam Review Questions You will be given a Periodic Table, Activity Series, and a Common Ions Chart CP CHEMISTRY Part A True-False State whether each statement is true or false. If false, correct
More informationThe photograph in the textbook provides evidence that an exothermic chemical reaction is occurring.
Preview Lesson Starter Objectives Indications of a Chemical Reaction Characteristics of Chemical Equations Significance of a Chemical Equation Balancing Chemical Equations Section 1 Describing Chemical
More informationChapter 01 Quiz Chang General Chemistry
Chapter 01 Quiz Chang General Chemistry 1. A bathroom-type scale is calibrated (marked off) in tenths of a kilogram from 1 to 200 kg and you can estimate to the nearest two-hundredths of a kilogram. How
More informationSemester 1 Review Chemistry
Name Period Date Semester 1 Review Chemistry Units & Unit Conversions Ch. 3 (p. 73-94) PART A SI UNITS What type of measurement is indicated by each of the following units? Choices are in the last column.
More informationSolid 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 informationChem A Ch. 9 Practice Test
Name: Class: Date: Chem A Ch. 9 Practice Test Matching Match each item with the correct statement below. a. product d. balanced equation b. reactant e. skeleton equation c. chemical equation 1. a new substance
More informationCP Chemistry Final Exam Review
I. Matter and Measurement 1) Chemical or physical property? CP Chemistry Final Exam Review Diamond is a very hard substance. The density of aluminum is 2.7 g/cm 3. Zinc reacts with acid. Copper melts at
More informationFormulas and Models 1
Formulas and Models 1 A molecular formula shows the exact number of atoms of each element in the smallest unit of a substance An empirical formula shows the simplest whole-number ratio of the atoms in
More informationDuring photosynthesis, plants convert carbon dioxide and water into glucose (C 6 H 12 O 6 ) according to the reaction:
Example 4.1 Stoichiometry During photosynthesis, plants convert carbon dioxide and water into glucose (C 6 H 12 O 6 ) according to the reaction: Suppose that a particular plant consumes 37.8 g of CO 2
More informationCHAPTER 8 CHEMICAL REACTIONS AND EQUATIONS
CHAPTER 8 CHEMICAL REACTIONS AND EQUATIONS CHEMICAL REACTIONS Occurs when matter combines or breaks apart to produce new kinds of matter with different properties with a change in energy. EVIDENCE FOR
More informationStoichiometry. Homework EC. cincochem.pbworks.com. Academic Chemistry DATE ASSIGNMENT
Unit 10 Resournces Name Academic Chemistry Stoichiometry Homework On-Time LATE DATE ASSIGNMENT 100 70 10.1 10.2 10.3 10.4 10.5 10.6 EC 16 cincochem.pbworks.com Stoichiometry Live in the now. Garth Algar
More information11.2 Types of Chemical Reactions> Chapter 11 Chemical Reactions Types of Chemical Reactions Describing Chemical Reactions
Chapter 11 Chemical 11.1 Describing Chemical 11.2 Types of Chemical 11.3 in Aqueous Solution 1 CHEMISTRY & YOU What happens to the wax when you burn a candle? When you burn a candle, a chemical reaction
More informationPRACTICE EXAMINATION QUESTIONS FOR 1.2 AMOUNT OF SUBSTANCE
PRACTICE EXAMINATION QUESTIONS FOR 1.2 AMOUNT OF SUBSTANCE 1. Nitroglycerine, C 3 H 5 N 3 O 9, is an explosive which, on detonation, decomposes rapidly to form a large number of gaseous molecules. The
More information5. The mass of oxygen required to completely convert 4.0 grams of hydrogen to water is 1) 8.0 grams; 2) 2.0 grams; 3) 32 grams; 4) 16 grams.
CHEMISTRY TEST NAME: MASS AND VOLUME DATE: EQUATION RELATIONSHIPS Directions: For each of the following questions, choose the number that best answers the question and place it on your answer sheet. Directions:
More information8 Chemical Equations. Flames and sparks result when aluminum foil is dropped into liquid bromine.
8 Chemical Equations Flames and sparks result when aluminum foil is dropped into liquid bromine. Chapter Outline 8.1 The Chemical Equation 8.2 Writing and Balancing Chemical Equations 8.3 Types of Chemical
More informationChemistry 11 Course Review
Introduction to Chemistry 1. 0.0006 mm =? µm Chemistry 11 Course Review 6. A 0.0460 L piece of copper has a mass of 410.32 g. Calculate the density of copper in g/ml. 2. 0.054 ml =? nl 3. 3.5 µg/l =? mg/ml
More informationQuestion 8 Chemical properties of metals and nonmetals. 1) magnesium 2) sulfur trioxide 3) iron (II) hydroxide 4) sodium nitrate
Question 8 Chemical properties of metals and nonmetals 1. Calcium oxide doesn t react with 1) NaNO 3 2) HCl 3) CO 2 4) H 2 O 2. Calcium oxide reacts with both of the following 1) SO 2 and O 2 2) H 2 O
More informationHow 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 informationForm A. Exam 1, Ch 1-4 September 23, Points
Chem 130 Name Exam 1, Ch 1-4 September 23, 2011 100 Points Please follow the instructions for each section of the exam. Show your work on all mathematical problems. Provide answers with the correct units
More informationExam 3. Objectives: Nomenclature
Exam 3 Objectives: o Nomenclature m-nm, m(vos)-nm, nm-nm o Evidence for Chemical Reactions o Writing Chemical Equations o Balancing Chemical Equations o Classifying Chemical Reactions o Combination Reactions
More information2. 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 informationBalancing Equations Notes
. Unit 7 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 informationChemical Reactions. Chemical changes are occurring around us all the time
Chemical changes are occurring around us all the time Food cooking Fuel being burned in a car s engine Oxygen being used in the human body The starting materials are called reactants The ending materials
More informationUnit 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 information1. Dimensional Analysis: convert the following values a. 47,340 cm to m Unit 1: Chemistry Matters b. 40.64 km to m c. 58,700 ml to L 2. Calculate the number of significant figures a. 0.0210 b. 3.6056 c.
More informationVOCABULARY Define. 1. reactants. 2. products. 3. chemical equation. 4. precipitate. 5. word equation
CHAPTER 8 HOMEWORK 8-1 (pp. 241 245) Define. 1. reactants 2. products 3. chemical equation 4. precipitate 5. word equation GRAPHIC ORGANIZER Complete the chart by listing three signs that suggest that
More informationAnswer Sheet for Sample Problems for Chemistry Level 1 Final Exam 2016 Study Guide
Answer Sheet for Sample Problems for Chemistry Level 1 Final Exam 2016 Study Guide Electrons in Atoms Chapter 5 1. What is the frequency of green light, which has a wavelength of 4.90 x 10-7 m? 8 c 3.00x10
More information1. 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 information2 nd Semester Study Guide 2016
Chemistry 2 nd Semester Study Guide 2016 Name: Unit 6: Chemical Reactions and Balancing 1. Draw the remaining product 2. Write a balanced equation for the following reaction: The reaction between sodium
More informationCHEMICAL REACTIONS. Introduction. Chemical Equations
CHEMICAL REACTIONS Chemistry I Chapter 7 1 Chemical Equations Their Job: Depict the kind of reactants and products and their relative amounts in a reaction. 4 Al (s) + 3 O 2 (g) ---> 2 Al 2 O 3 (s) The
More informationChem 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 informationPart 01 - Notes: Reactions & Classification
Objectives: Identify, define, and explain: combination reaction, synthesis reaction, decomposition reaction, single replacement reaction, double replacement reaction, combustion reaction, rapid oxidation,
More informationSpring 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 informationName: Unit 1: Nature of Science
Name: Unit 1: Nature of Science 1. Using the picture above, list lab safety rules that are being ignored. 2. What are the steps to the scientific method? 3. Convert the following into scientific notation:
More informationChemical Bonds In elements and compounds, the atoms are held together by chemical bonds.
Chemical Bonds In elements and compounds, the atoms are held together by chemical bonds. Forming a bond makes an atom more stable, so atoms form as many bonds are they are able to. Bonds are made using
More information1. 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 informationAP CHEMISTRY THINGS TO KNOW
AP CHEMISTRY THINGS TO KNOW Diatomic Molecules H2-hydrogen gas (do not write H) N2-nitrogen gas (do no write N) O2-oxygen gas (do not write O) F2-fluorine gas (do not write F) Cl2-chlorine gas (do not
More informationCHEMICAL REACTIONS. The process by which one or more substances are changed into one or more different substances
CHEMICAL REACTIONS The process by which one or more substances are changed into one or more different substances Equations Reactions are represented by a chemical equation Reactants Products Must have
More informationJanuary 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 informationReview Multiple Choice Questions
Chapter 2 Matter and Changes Review Multiple Choice Questions 1. The random molecular motion of a substance is greatest when the substance is a. condensed b. a liquid c. frozen d. a gas 2. After elements
More informationExam III Material Chapter 7-CHEMICAL REACTIONS, continued
Exam III Material Chapter 7-CHEMICAL REACTIONS, continued A chemical reaction occurs when there is a change in chemical composition. I. Double Replacement/Double Exchange/Metathesis Reactions In an double
More informationUNIT 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 informationMoles, Mass, and Limiting Reactants
Moles, Mass, and Limiting Reactants Interpreting a Chemical Equation 1. How many moles of chlorine gas react with 1 mol of hydrogen gas according to the balanced chemical equation? (a) 1 mol (b) 2 mol
More informationPhysical Science Study Guide
Name: Class: Date: Physical Science Study Guide Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Mendeleev arranged the known chemical elements in a table
More informationLesson (1) Mole and chemical equation
Lesson (1) Mole and chemical equation 1 When oxygen gas reacts with magnesium, magnesium oxide is formed. Such Reactions are described by balanced equations known as "chemical equations" Δ 2Mg(s) + O2(g)
More informationb. Na. d. So. 1 A basketball has more mass than a golf ball because:
Chem I Semester Review All of the following are general characteristics of a substance in the liquid state except a. definite volume. c. not easily compressed. b. able to flow. d. definite shape. In the
More informationChemical Equation Calculations
Mole Relationships Chemical Equation Calculations 1. How many moles of chlorine gas react with 1 mol of hydrogen gas according to the balanced chemical equation? (a) 1 mol (b) 2 mol (c) 3 mol (d) 4 mol
More informationStudy Guide: Stoichiometry
Name: Study Guide: Stoichiometry Period: **YOUR ANSWERS MUST INCLUDE THE PROPER NUMBER OF SIG FIGS AND COMPLETE UNITS IN ORDER TO RECEIVE CREDIT FOR THE PROBLEM.** BALANCE THE FOLLOWING EQUATIONS TO USE
More informationName: Unit 1: Nature of Science
Name: Unit 1: Nature of Science 1. Using the picture above, list lab safety rules that are being ignored. 2. What are the steps to the scientific method? 3. Convert the following into scientific notation:
More informationUnit Five- Chemical Quantities Chapter 9: Mole ratios, conversions between chemicals in a balanced reaction (mole, mass), limiting reactant, % yield
Chemistry Midterm Review Exam date: Wednesday, 2/15 during class The midterm exam must be completed before February vacation if you are absent The midterm exam is worth 6% of your year grade and it contains
More informationChapter 7. Chemical Equations and Reactions
Chemical Equations and Reactions Chemical and Physical Changes In a physical change, the chemical composition of the substance remains constant. Examples of physical changes are the melting of ice or the
More information2) Isotopes are atoms of the same element, which have the same number of but a different number.
AP Chemistry Semester 1 Exam Review Alternate Atomic Structure 1) Fill in the table: Name Per Isotope Symbol Atomic Mass Mass # Atomic # # of protons # of neutrons # of electrons Hydrogen-1 16 16 18 35.45
More informationAP 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 informationCHEMICAL REACTIONS. Types of Reactions. Steps to Writing Reactions
Types of Reactions CHEMICAL REACTIONS There are five types of chemical reactions we will talk about: 1. Synthesis reactions 2. reactions 3. Single displacement reactions 4. reactions 5. Combustion reactions
More information26. N 2 + H 2 NH N 2 + O 2 N 2 O 28. CO 2 + H 2 O C 6 H 12 O 6 + O SiCl 4 + H 2 O H 4 SiO 4 + HCl 30. H 3 PO 4 H 4 P 2 O 7 + H 2 O
Balance the following chemical equations: (Some may already be balanced.) 1. H 2 + O 2 H 2 O 2. S 8 + O 2 SO 3 3. HgO Hg + O 2 4. Zn + HCl ZnCl 2 + H 2 5. Na + H 2 O NaOH + H 2 6. C 10 H 16 + Cl 2 C +
More information1. How many significant digits are there in each of the following measurements? (½ mark each) a) ha b) s. c) d) 0.
SCH 4U_07-08 SCH3U: REVIEW NAME: (TOTAL SCORE = 80) 1. How many significant digits are there in each of the following measurements? (½ mark each) a) 204.45 ha b) 18.23 s c) 380 000 d) 0.00560 g 2. Name
More informationReview Material for Exam #2
Review Material for Exam #2 1. a. Calculate the molarity of a solution made with 184.6 mg sample of potassium dichromate dissolved in enough water to give 500.0 ml of solution. b. What is the molarity
More informationUnit 6 Assignment Packet Name Period A1 Worksheet: Writing and Balancing Chemical Equations
Unit 6 Assignment Packet Name Period A1 Worksheet: Writing and Balancing Chemical Equations 1. Describe the following word equation with a statement or sentence: Iron + Oxygen iron (III) oxide 2. In a
More information4) Please indicate whether each of the following units are intensive or extensive. a) Density Intensive Extensive. b) Temperature Intensive Extensive
EXAM ONE Nomenclature Balancing Reactions Protons, Neutrons, Electrons Natural Abundance Solubility Rules Net Ionic Reactions Atom, Mole, Gram Conversions Empirical Formulas Solution Chemistry / Molarity
More informationWhat 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 informationNOTE: This practice exam contains more than questions than the real final.
NOTE: This practice exam contains more than questions than the real final. 1. The wavelength of light emitted from a green laser pointer is 5.32 10 2 nm. What is the wavelength in meters? 2. What is the
More informationChemistry 400: General Chemistry Sacramento City College HW#1: Review to Begin Chemistry 400. Review of Chapter 1
Chemistry 400: General Chemistry Sacramento City College HW#1: Review to Begin Chemistry 400 Review of Chapter 1 1) Identify a liquid. A) definite volume and definite shape B) definite volume and no definite
More informationC hapter ATOMS. (c) (ii) and (iii) (d) (ii) and (iv)
C hapter 3 ATOMS AND MOLECULES 1. Which of the following correctly represents 360 g of water? (i) 2 moles of H 2 0 (ii) 20 moles of water (iii) 6.022 10 23 molecules of water (iv) 1.2044 10 25 molecules
More informationCH 221 Sample Exam Exam II Name: Lab Section:
Exam II Name: Lab Section: Part I: Multiple Choice Questions (100 Points) Use a scantron sheet for Part I. There is only one best answer for each question. 1. When methanol undergoes complete combustion,
More information11.3 Reactions in Aqueous Essential Understanding Reactions that occur in aqueous solutions are double-replacement
13. Is the following sentence true or false? Hydrocarbons, compounds of hydrogen and carbon, are often the reactants in combustion reactions. 14. Circle the letter of each compound that can be produced
More information!!! 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 informationCHM1045 Exam 2 Chapters 3, 4, & 10
1. Upon analysis, a compound is found to contain 22.8% sodium, 21.8% boron, and 55.4% oxygen. What is its empirical formula? a. NaBO b. NaB 2 O 5 c. Na 2 B 4 O 7 d. Na 3 BO 4 e. None of the above. 2. The
More information4 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 informationChemical Reactions Unit
Name: Hour: Teacher: ROZEMA / Chemistry Chemical Reactions Unit 1 P a g e 2 P a g e 3 P a g e 4 P a g e 5 P a g e 6 P a g e Chemistry Balancing Equations Balance the following equations by inserting the
More informationChem 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 informationUnit 2. Chapter 4-Atoms and Elements, continued
CHEMISTRY 110 LECTURE Unit 2 Chapter 4-Atoms and Elements, continued I Ions II ISOTOPES-Tools A. Tools 1. Atomic number, Z,, equals the number of protons 2. Mass number, A, equals the sum of protons and
More informationPolyatomic 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 informationQuantitative chemistry Atomic structure Periodicity
IB chemistry Units 1-3 review Quantitative chemistry Significant figures The mole- be able to convert to number of particles and mass Finding empirical and molecular formulas from mass percentage States
More informationAtoms, Molecules, and Ions (Chapter 2) 1. a. Give the name and symbol for one alkaline earth metal.
Atoms, Molecules, and Ions (Chapter 2) 1. a. Give the name and symbol for one alkaline earth metal. b. Give the name and symbol for one transition metal. c. Give the name and symbol for one noble gas.
More informationAdvanced Chemistry Final Review
Advanced Chemistry Final Review 1. What are the products of complete combustion of hydrocarbons? Hydrocarbons are compounds made of carbon and oxygen. When they burn (combine with oxygen) they form carbon
More information