Semester 1 Review Chemistry

Size: px
Start display at page:

Download "Semester 1 Review Chemistry"

Transcription

1 Name Period Date Semester 1 Review Chemistry Units & Unit Conversions Ch. 3 (p ) PART A SI UNITS What type of measurement is indicated by each of the following units? Choices are in the last column. 1. g/ml 2. s 4. g 5. cm 3 7. mg 8. L density length mass 3. km 6. mm 9. g/cm 3 time volume PART B DENSITY 10. A small gold nugget has volume of 0.87 cm 3. What is its mass if the density of gold is 19.3 g/cm 3? 11. What volume is occupied by 35.2 g of carbon tetrachloride if its density is 1.60 g/ml? PART B UNIT CONVERSIONS Perform the following SI prefix conversions: kg = g ml = L mm = m cm = km Atomic Structure 4,5 ( ) STATES OF MATTER 1. Draw a diagram to represent 8 particles in each state of matter. (HINT: Recall that plasma is gaslike but with one major difference.) SOLID LIQUID GAS PLASMA PART A SUBATOMIC PARTICLES The table below contains information about several elements. In each case, enough information has been provided for you to fill in the blanks. Assume all atoms are neutral. Ch. 3 Uncertainty in Measurements CHEM

2 Isotope Name Nuclear Symbol Atomic Number Mass Number # of Protons # of Electrons # of Neutrons 1. calcium Au PART B AVERAGE ATOMIC MASS 8. Calculate the average atomic mass for neon if its abundance in nature is 90.5% neon-20, 0.3% neon-21, and 9.2% neon Calculate the average atomic mass of silver if 13 out of 25 atoms are silver-107 and 12 out of 25 atoms are silver Distinguish between mass number, relative atomic mass, and average atomic mass. Periodic Trends Ch. 6 (p ) 1. Put the following elements in order from smallest to largest atomic radius and explain why: C, O, Sn, Sr. 2. Put the following elements in order from lowest to highest first ionization energy and explain why: Al, Ar, Cs, Na. Ionic Compounds Ch. 2 & 13

3 3. Explain what happens to the radius of an atom as you move from left to right across a period. 4. Define Cation and Anion and describe what types of atoms form cations and anions. Ionic Compounds Ch. 7 (p ) PART A IONIC NAMES Name the following ionic compounds. Remember to consider polyatomic ions and Roman numerals. 1. ZnCl 2 PART B IONIC FORMULAS Write formulas for the following ionic compounds. Remember to consider polyatomic ions and Roman numerals. 9. potassium iodide 2. Cu 2 CO 3 3. Na 2 C 2 O 4 4. Fe 2 O 3 5. MgCO 3 6. NH 4 NO 3 7. LiF 8. SnBr iron(iii) sulfide 11. potassium phosphate 12. magnesium chloride 13. tin(iv) chloride 14. sodium hydroxide 15. mercury(ii) oxide 16. aluminum acetate Ionic Compounds Ch. 2 & 13

4 Use Lewis electron dot diagrams to show the formation of the following molecular substances. Include partial charges if a polar bond is formed. 16. Br PCl 3 PART C MOLECULAR NAMES Name the following compounds. 18. SiO S 4 N Cl 2 O 21. PF 3 PART D MOLECULAR FORMULAS Write formulas for the following compounds. 22. sulfur trioxide 23. carbon tetrachloride 24. diphosphorous pentoxide 25. sulfur hexafluoride Molar Conversions Ch. 10 (p ) ***FOR ALL CALCULATIONS, SHOW YOUR WORK AND INCLUDE UNITS & SIG FIGS*** PART A MOLAR MASS 1. Calculate the molar mass for each of the following compounds. Include units! calcium nitrate Formula: lead(ii) iodide Formula: Semester 1 Study Guide CHEM

5 PART B MOLAR CONVERSIONS (Show your work and include units!) 2. How many moles of ammonia are in molecules of ammonia? Formula: Answer: 3. You need 2.5 moles of aluminum for an experiment. How many atoms of aluminum is this? Formula: Answer: 4. There are atoms of copper in the outer shell of pennies. How many grams of copper is this? Formula: Answer: Balancing Equations CH. 11 ( ) Balance the following chemical equations. 1. N 2 + O 2 N 2 O 2. KI + Cl 2 KCl + I 2

6 3. C 2 H 6 + O 2 CO 2 + H 2 O 4. Mg(NO 3 ) 2 + K 3 PO 4 Mg 3 (PO 4 ) 2 + KNO 3 Stoichiometry Ch. 12 (p ) 1. How many liters of ammonia gas are formed in this reaction after 25L of Nitrogen React? N 2 + H 2 NH ml of 2.00M H 2 SO 4 react, how many grams of Na 2 SO 4 will be formed? H 2 SO 4 + NaOH Na 2 SO 4 + H 2 O 3. If 6.57 g of iron reacted and g of iron(iii) chloride are obtained. Calculate the theoretical yield and percent yield of FeCl 3. Fe + HCl H 2 + FeCl 3

7 4. How many grams of lithium sulfate will be formed when 25 grams of sulfuric acid react with an excess of lithium hydroxide in the following reaction? H2SO4 + LiOH Li2SO4 + H2O 5. How many grams of sodium acetate are required to react completely with 30 grams of iron (III) nitrate in the following reaction? NaC2H3O2 + Fe(NO3)3 NaNO3 + Fe(C2H3O2)3 6. How many grams of fluorine gas will it take to convert 100 grams of C2H4 to C2H4F2 using the following reaction? C2H4 + F2 C2H4F2 The Nature of Solutions Ch. 15,16 (p ) 5. What is the difference between a strong electrolyte and a weak electrolyte? 6. Define the following Terms; unsaturated, saturated and supersaturated. Use the solubility curve to answer questions How many grams of potassium nitrate can dissolve in 100 g of water at 50 C? 8. At 20 C, a solution contains 120 g of NaNO 3 in 100 g of water. Is this solution saturated, unsaturated, or supersaturated? 9. You need to make a solution containing 150 g of potassium chloride in 300 g of water. What temperature is required?

8 Molarity Solve the following molarity problems. Show all work and include correct units and sig figs! 10. Find the molarity of a solution in which 58 g of NaCl are dissolved in 2.5 L of solution. 11. How many grams of KMnO 4 should be used to prepare 2.00 L of a 0.500M solution? 12. What volume of 0.25M solution can be made from 5.0 g of KCl? 13. Find the molarity of a 450 ml solution containing 13.7 g of ZnSO How many grams of CuCl 2 are required to make 75 ml of a 0.20M solution?

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

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

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

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

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

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 104 Final Exam Content Evaluation and Preparation for General Chemistry I Material

Chemistry 104 Final Exam Content Evaluation and Preparation for General Chemistry I Material Chemistry 104 Final Exam Content Evaluation and Preparation for General Chemistry I Material What is 25 mph in mm s 1? Unit conversions What is 1025 K in o F? Which is larger 1 ft 3 or 0.1 m 3? What is

More information

Memorize: Understand: Know how to:

Memorize: Understand: Know how to: NAME: CLASS PERIOD: REVIEW FOR HONORS CHEMISTRY SEMESTER 1 EXAM Memorize: Understand: Know how to: 1 SI units for different measurements (length, volume, number, mass, temperature, density) Definition

More information

Silver nitrate solution is added to sodium dichromate solution

Silver nitrate solution is added to sodium dichromate solution Chem. 110 50 Points Final Exam Part 1 Practice Write the chemical names or formulas for the following a H 2 SO 4 b NiNO 2 c Aluminum thiosulfate d Plumbic acetate e Ag 2 C 2 O 4 f P 2 O 5 g Cyanic acid

More information

1. 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 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

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

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

Chemistry Review. a) all of the b) a&b c) a,b&c d) a,b&d above

Chemistry Review. a) all of the b) a&b c) a,b&c d) a,b&d above Chemistry Review 1. The elements whose symbols are P, C, and N are (a) potassium, cadmium, and nickel. (b) potassium, carbon, and nitrogen. (c) phosphorus, calcium, and neon. (d) phosphorus, carbon, and

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

Regents Chemistry Unit 3- Bonding, Moles & Stoichiometry Study Guide & Pre-Test KEY

Regents Chemistry Unit 3- Bonding, Moles & Stoichiometry Study Guide & Pre-Test KEY Name: Regents Chemistry Unit 3- Bonding, Moles & Stoichiometry Study Guide & Pre-Test KEY Focus Questions for the Unit: How are compounds different... from elements?... from mixtures? What role do valence

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

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

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 molecule of water contains hydrogen and oxygen in a 1:8 ratio by mass. This is a statement

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

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

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

Review Multiple Choice Questions

Review 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 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

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

Period: Chemistry Semester 1 Final Exam Review Packet. 1. What is the difference between a hypothesis and a theory?

Period: Chemistry Semester 1 Final Exam Review Packet. 1. What is the difference between a hypothesis and a theory? Chemistry Name: Period: Chemistry Semester 1 Final Exam Review Packet 1. What is the difference between a hypothesis and a theory? 2. Distinguish between quantitative and qualitative observations. States

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

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

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

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

Final Exam Study Guide Honors Chemistry Semester Multiple Choice Questions

Final Exam Study Guide Honors Chemistry Semester Multiple Choice Questions Final Exam Study Guide Honors Chemistry Semester 1 2017 60 Multiple Choice Questions Name: Students should be able to: Convert between metric units Convert between scientific notation and expanded (decimal)

More information

Regents Chemistry Practice Problems from Units 1-9 March 2018

Regents Chemistry Practice Problems from Units 1-9 March 2018 1. Which is a pure substance? A) table salt B) bronze C) air D) soil 2. A tentative explanation of certain facts that provides the basis for further experimentation is a(n) A) observation B) hypothesis

More information

2. Identify each of the following samples of matter as heterogeneous or homogeneous.

2. 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 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

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

Name: 1. Show all work on Math Problems!!! Significant Figures and Calculations (*all math problems will require the use of sig figs)

Name: 1. Show all work on Math Problems!!! Significant Figures and Calculations (*all math problems will require the use of sig figs) Name: 1 AP Chemistry Summer Assignment The goal of this assignment is to make sure that everyone has the fundamentals that they will need to be successful in Chemistry II & AP Chemistry. You should have

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

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. CHM 210 Chemistry Homework #3 Compounds and Their Bonds (Ch. 4) Due: MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question. 1) The octet rule indicates that

More information

Chemical Bonding. Chemical Bonds. Metals, Ions, or Molecules. All Matter Exists as Atoms,

Chemical Bonding. Chemical Bonds. Metals, Ions, or Molecules. All Matter Exists as Atoms, Chemical Bonding Valence electrons (the outer most electrons) are responsible for the interaction between atoms when forming chemical compounds. Another way to say that is that valence electrons are the

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

1. [7 points] How many significant figures should there be in the answer to the following problem?

1. [7 points] How many significant figures should there be in the answer to the following problem? 1 of 6 10/20/2009 3:54 AM Avogadro s Number = 6.022 10 23 1. [7 points] How many significant figures should there be in the answer to the following problem? (29.0025 + 0.2)/(6.1345 36.101) (a) 1 (b) 2

More information

26. 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

26. 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 information

CH 4 AP. Reactions in Aqueous Solutions

CH 4 AP. Reactions in Aqueous Solutions CH 4 AP Reactions in Aqueous Solutions Water Aqueous means dissolved in H 2 O Moderates the Earth s temperature because of high specific heat H-bonds cause strong cohesive and adhesive properties Polar,

More information

Reactions in Aqueous Solutions

Reactions in Aqueous Solutions Reactions in Aqueous Solutions 1 Chapter 4 General Properties of Aqueous Solutions (4.1) Precipitation Reactions (4.2) Acid-Base Reactions (4.3) Oxidation-Reduction Reactions (4.4) Concentration of Solutions

More information

2014 Chemistry 1 st Semester Exam Review Packet

2014 Chemistry 1 st Semester Exam Review Packet Name: Date: Hour: 2014 Chemistry 1 st Semester Exam Review Packet 1. What percentage of the water on Earth is salt water? (1 point) A. 97.2% B. 0.009% C. 2.11% D. 2.8 % 2. One similarity between all mixtures

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

Part A Answer all questions in this part.

Part A Answer all questions in this part. Part A Directions (1-24): For each statement or question, record on your separate answer sheet the number of the word or expression that, of those given, best completes the statement or answers the question.

More information

Chemistry 20 Lesson 36 The Whole Enchilada

Chemistry 20 Lesson 36 The Whole Enchilada Unit I: Science 10 Review Chemistry 20 Lesson 36 The Whole Enchilada 1. Classify the substances as ionic (i), molecular (m), or acid (a) and provide the IUPAC name and the state of matter at SATP where

More information

AP Chemistry Honors Unit Chemistry #4 2 Unit 3. Types of Chemical Reactions & Solution Stoichiometry

AP Chemistry Honors Unit Chemistry #4 2 Unit 3. Types of Chemical Reactions & Solution Stoichiometry HO AP Chemistry Honors Unit Chemistry #4 2 Unit 3 Chapter 4 Zumdahl & Zumdahl Types of Chemical Reactions & Solution Stoichiometry Students should be able to:! Predict to some extent whether a substance

More information

Funsheet 9.1 [VSEPR] Gu 2015

Funsheet 9.1 [VSEPR] Gu 2015 Funsheet 9.1 [VSEPR] Gu 2015 Molecule Lewis Structure # Atoms Bonded to Central Atom # Lone Pairs on Central Atom Name of Shape 3D Lewis Structure NI 3 CF 4 OCl 2 C 2 F 2 HOF Funsheet 9.1 [VSEPR] Gu 2015

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

Bonding, Moles & Unit 3. Stoichiometry

Bonding, Moles & Unit 3. Stoichiometry Bonding, Moles & Unit 3 Stoichiometry Warm-up! Chem Catalyst 1.What part of the atom participates in the reactivity of elements? 2.What does the octet rule have to do with reactivity? 3.Based on what you

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

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

Questions Booklet. UNIT 1: Principles & Applications of Science I CHEMISTRY SECTION. Level 3 Applied Science. Name:.. Teacher:..

Questions Booklet. UNIT 1: Principles & Applications of Science I CHEMISTRY SECTION. Level 3 Applied Science. Name:.. Teacher:.. Level 3 Applied Science UNIT 1: Principles & Applications of Science I CHEMISTRY SECTION Questions Booklet Name:.. Teacher:.. Level 3 Applied Science 2017-2018 Unit 1 (Chemistry) 1 1. State the relative

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

General Chemistry 1 CHM201 Unit 2 Practice Test

General 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 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

4) Tetrasulfur trioxide. 5) barium fluoride. 6) nitric acid. 7) ammonia

4) Tetrasulfur trioxide. 5) barium fluoride. 6) nitric acid. 7) ammonia Unit 9: The Mole- Funsheets Part A: Molar Mass Write the formula AND determine the molar mass for each of the following. Be sure to include units and round you answer to 2 decimal places. 1) calcium carbonate

More information

1 st Semester Final Review Sheet (Chapters 2-7)

1 st Semester Final Review Sheet (Chapters 2-7) CP Chemistry Name: Period: 1 st Semester Final Review Sheet (Chapters 2-7) Matter (Chapter 2) 1. What is the definition of an element? 2. What is the definition of a compound? 3. What is the definition

More 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

Honors Chemistry Semester 1 Final Review

Honors Chemistry Semester 1 Final Review Honors Chemistry Semester 1 Final Review Ch. 1 Introduction to Chemistry Chemistry: its branches, technology, scientific method, and problem solving. 1. Know the definition of matter. 2. Know the definition

More information

Name Date Period Ionic Bonding Puzzle Activity

Name Date Period Ionic Bonding Puzzle Activity Name Date Period Ionic Bonding Puzzle Activity Introduction When metals and non-metals chemically react, the atoms will tend to form ions or charged atoms. Ions form because electrons are either gained

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

UNIT 9 - STOICHIOMETRY

UNIT 9 - STOICHIOMETRY General Stoichiometry Notes STOICHIOMETRY: tells relative amts of reactants & products in a chemical reaction Given an amount of a substance involved in a chemical reaction, we can figure out the amount

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

insoluble partial very soluble (< 0.1 g/100ml) solubility (> 1 g/100ml) Factors Affecting Solubility in Water

insoluble partial very soluble (< 0.1 g/100ml) solubility (> 1 g/100ml) Factors Affecting Solubility in Water Aqueous Solutions Solubility is a relative term since all solutes will have some solubility in water. Insoluble substances simply have extremely low solubility. The solubility rules are a general set of

More information

Chapter 4 Compounds and Their Bonds. Octet Rule. Metals Form Positive Ions. Ionic and Covalent Bonds. Formation of a Sodium Ion, Na +

Chapter 4 Compounds and Their Bonds. Octet Rule. Metals Form Positive Ions. Ionic and Covalent Bonds. Formation of a Sodium Ion, Na + Chapter 4 Compounds and Their Bonds Octet Rule 4.1 Octet Rule and Ions An octet Is 8 valence electrons. Is associated with the stability of the noble gases. Helium (He) is stable with 2 valence electrons

More information

Unit 1 - Foundations of Chemistry

Unit 1 - Foundations of Chemistry Unit 1 - Foundations of Chemistry Chapter 2 - Chemical Reactions Unit 1 - Foundations of Chemistry 1 / 42 2.1 - Chemical Equations Physical and Chemical Changes Physical change: A substance changes its

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

Chemistry Study Guide

Chemistry Study Guide Chemistry Study Guide Marking Period 3 Exam Week of 3/21/17 Study Guide due - When studying for this test, use your do nows, notes, homework, class handouts, and your textbook. Vocabulary Chapter 7 Anion

More information

Part 01 - Notes: Reactions & Classification

Part 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 information

Practice Packet Unit 6: Moles & Stoichiometry

Practice Packet Unit 6: Moles & Stoichiometry Regents Chemistry: Mr. Palermo Practice Packet Unit 6: Moles & Stoichiometry 1 LESSON 1: Moles and Molar Mass 1. Put an M if the substance is molecular/covalent, an I if ionic under the formula listed.

More information

CHEMICAL 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 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 information

2. Which of the following salts form coloured solutions when dissolved in water? I. Atomic radius II. Melting point III.

2. Which of the following salts form coloured solutions when dissolved in water? I. Atomic radius II. Melting point III. 1. Which pair of elements reacts most readily? A. Li + Br 2 B. Li + Cl 2 C. K + Br 2 D. K + Cl 2 2. Which of the following salts form coloured solutions when dissolved in water? I. ScCl 3 II. FeCl 3 III.

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

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

Write the name or formula for:

Write the name or formula for: Do Now Date: Tuesday, November 2, 2015 Objective: Name and write formulas for ionic and molecular (covalent) compounds. Write the name or formula for: K 2 SO 4 NaNO 3 Calcium Hydroxide Tuesday, November

More information

Unit 9 Stoichiometry Notes

Unit 9 Stoichiometry Notes Unit 9 Stoichiometry Notes Stoichiometry is a big word for a process that chemist s use to calculate amounts in reactions. It makes use of the coefficient ratio set up by balanced reaction equations to

More information

Chapter 6: Ionic and Molecular Compounds

Chapter 6: Ionic and Molecular Compounds Chapter 6: Ionic and Molecular Compounds 1. Recall that the group number indicates the number of valence electrons for any element in that group. Each noble gas has eight valence electrons (except helium,

More information

Naming Simple Compounds

Naming Simple Compounds Naming Simple Compounds Ionic Compounds Ionic compounds consist of positive and negative ions. have attractions called ionic bonds between positively and negatively charged ions. have high melting and

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

Unit 1: INTRO TO CHEM

Unit 1: INTRO TO CHEM CHEMISTRY MIDTERM EXAM REVIEW: FALL SEMESTER MIDTERM WILL INCLUDE: 1. DISTRICT MIDTERM 50 MULTIPLE CHOICE QUESTIONS (50 POINTS) 2. DISTRICT CONSTRUCTED RESPONSES (2O POINTS) 3. TEACHER PORTION: 15 MULTIPLE

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

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

Name: Unit 1: Nature of Science

Name: 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 information

Questions 1 to 58 must be answered on the Scantron sheets.

Questions 1 to 58 must be answered on the Scantron sheets. Questions 1 to 58 must be answered on the Scantron sheets. Base your answers to questions 1 to 5 on the heating curve for a pure substance that is shown below. 1. The freezing point of the substance is

More information

ed. Brad Collins Aqueous Chemistry Chapter 5 Some images copyright The McGraw-Hill Companies, Inc. Sunday, August 18, 13

ed. Brad Collins Aqueous Chemistry Chapter 5 Some images copyright The McGraw-Hill Companies, Inc. Sunday, August 18, 13 ed. Brad Collins Aqueous Chemistry Chapter 5 Some images copyright The McGraw-Hill Companies, Inc. A solution is a homogenous mixture of 2 or more substances at the molecular level The solute(s) is(are)

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

Name Date. 9. Which substance shows the least change in solubility (grams of solute) from 0 C to 100 C?

Name Date. 9. Which substance shows the least change in solubility (grams of solute) from 0 C to 100 C? Solubility Curve Practice Problems Directions: Use the graph to answer the questions below. Assume you will be using 100g of water unless otherwise stated. 1. How many grams of potassium chloride (KCl)

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

Symbols. Table 1 A set of common elements, their symbols and physical state

Symbols. Table 1 A set of common elements, their symbols and physical state Symbols Symbols are a kind of shorthand system for writing down elements and compounds. Each element has a particular one or two letter symbol. The first letter of a symbol is always capital, and if there

More information

HONORS CHEMISTRY. Chapter 1 Introduction to Chemistry 1. What is chemistry?

HONORS CHEMISTRY. Chapter 1 Introduction to Chemistry 1. What is chemistry? HONORS CHEMISTRY FIRST SEMESTER EXAM REVIEW Chapter 1 Introduction to Chemistry 1. What is chemistry? 2. Identify the independent and dependent variables using the graph to the right. IV: DV: 3. Write

More information

Chemistry Semester Two Exam Review. The test will consist of 50 multiple choice questions over the following topics.

Chemistry Semester Two Exam Review. The test will consist of 50 multiple choice questions over the following topics. Chemistry Semester Two Exam Review Name The test will consist of 50 multiple choice questions over the following topics. 1) Measuring (1): Triple beam balance, graduated cylinder, thermometer, ruler 2)

More information

AP Chemistry Unit #4. Types of Chemical Reactions & Solution Stoichiometry

AP Chemistry Unit #4. Types of Chemical Reactions & Solution Stoichiometry AP Chemistry Unit #4 Chapter 4 Zumdahl & Zumdahl Types of Chemical Reactions & Solution Stoichiometry Students should be able to: Predict to some extent whether a substance will be a strong electrolyte,

More information

Advanced Chemistry Final Review

Advanced 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

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

Chapter 6. Types of Chemical Reactions and Solution Stoichiometry

Chapter 6. Types of Chemical Reactions and Solution Stoichiometry Chapter 6 Types of Chemical Reactions and Solution Stoichiometry Chapter 6 Table of Contents (6.1) (6.2) (6.3) (6.4) (6.5) (6.6) (6.7) (6.8) Water, the common solvent The nature of aqueous solutions: Strong

More 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

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