Resource for Worksheets CHEMCP1Workbookv411_12.doc Rsource for Worksheets-2

Name: Date: Per: _ College Preparatory Chemistry Level Worksheet Book 2011-2012 Science Department Framingham High School 4th Edition Name: Date: Per: _ Table of Contents Table of Contents Scientific Method Matter Tree Element Symbols Physical vs Chemical Properties Physical vs Chemical Changes Metrics and Measurement 10 Metric System Worksheet 11 Using the Correct Units 12 Scientific Notation 13 Significant Figures Worksheet 14 Significant Figures Worksheet 15 Significant Figures Worksheet 16 Density 17 Accuracy vs Precision 18 Temperature & its Measurement 19 Percentage Error 20 Atomic Structure 21 Atomic Structure 22 Isotopes & Average Atomic Mass 23 Wave Worksheet 24 Electron Configuration Worksheet #1 25 Electron Configuration Worksheet #2 26 Writing Chemical Equations 27 Types of Reactions Worksheet 29 REDOX Worksheet 31 REDOX Worksheet 32 Balancing Equations Worksheet #1 33 Balancing Equations Worksheet #2 35 Name: Date: Per: _ Balancing Worksheet #3 37 Dimensional Analysis – or – Unit Analysis – or – Factor-Label Method #1 39 Dimensional Analysis – or – Unit Analysis – or – Factor-Label Method #2 40 Mole Worksheet 41 Mole Worksheet 42 Mole Worksheet 43 Molarity 44 Percent Composition Worksheet 45 Empirical and Molecular Formulas Worksheet 46 Stoichiometry Worksheet #1 47 Stoichiometry Worksheet #2 48 Stoichiometry #3 49 Stoichiometry Worksheet #4 50 Stoichiometry Worksheet #5 51 Limiting Reagent Worksheet 52 Freezing and Boiling Point Graph 54 Heat Calculations 55 Heat and Phase Changes 56 Heat and its Measurement 57 Thermochemistry Worksheet 58 Thermochemistry Worksheet 59 Nuclear Chemistry Worksheet 60 Boyles Law Worksheet 62 Charles’ Law 64 Temperature-Pressure Law 66 Gas Laws Worksheet #1 67 Gas Laws Worksheet #2 68 Gas Laws Worksheet #3 70 Gas Laws Worksheet #4 71 Gas Law Practice 73 Name: Date: Per: _ Bonding/Solutions Worksheet #1 74 Bonding/Solutions Worksheet #2 75 Bonding/Solutions Worksheet #3 76 Molarity Worksheet 77 Molarity Worksheet 78 Dilutions Worksheet 79 Rate Worksheet #1 80 Rate Worksheet #2 81 Rate Worksheet #3 82 Equilibrium Worksheet 83 Molarity, [H+], [OH-], pH, and pOH Relationships .85 Acid Base Worksheet #1 87 Acid Base Worksheet #2 88 Acid Base Worksheet #3 89 Acid Base Worksheet #4 90 Acids, Bases, Conjugate Acids and Conjugate Bases 91 Worksheet on pH and Strong Acid Base Reactions 92 Review Worksheet 93 Review Worksheet 94 Review Worksheet 95 Review Worksheet 96 Name: Date: Per: _ Scientific Method Put the following steps of the scientific method in the proper order _ Research the problem _ Observe and record _ Make a hypothesis _ Identify the problem _ Arrive at a conclusion _ Test the hypothesis Match the following terms with the correct definition: a) organized process used to test a hypothesis hypothesis b) an educated guess about a solution to control a problem variable c) observations and measurements recorded during an experiment experiment d) a judgement based on the results of an experiment conclusion theory e) a logical explanation for events that occur in nature data f) used to show that the result of an experiment is really due to the condition being tested g) factor that changes in an experiment Matter Tree All matter can be classified as either a substance (element or compound) or a mixture (homogeneous or heterogeneous) Pure substances are homogeneous and you can write their chemical formula There are two types of pure substances, elements and compounds Elements are one type of atom while compounds are two or more different atoms chemically bonded together Mixtures can have variable ratios There are two types of mixtures, homogeneous and heterogeneous A homogeneous mixture have the same composition all the way through A heterogeneous mixture does not have the same composition all the way through Classify the following as a substance or a mixture If it is a substance choose either element or compound If it is a mixture choose either heterogeneous or homogeneous Choose of the following: Substance Mixture Type of Matter Element Compound Homogeneou Heterogeneou s s Chlorine Water Soil Sugar Water Oxygen Carbon Dioxide Mint Chocolate chip Ice Cream Rubbing Alcohol Pure Air 10 Iron Element Symbols Elements are given names and symbols When writing the formulas of compounds, symbols are much easier to use than the names We need to be familiar with the names and symbols of common elements The symbol of an element is usually taken from the first one or two letters of the name of the element However, sometimes the symbol comes from the Latin name of the element! Write the symbol for the following elements: oxygen 11 plutonium hydrogen 12 americium chlorine 13 radium mercury 14 germanium fluorine 15 zinc barium 16 arsenic 17 lead helium uranium 18 iron radon 19 calcium 20 cobalt 10 sulfur Write the name of the element that corresponds to each of the following symbols: 21 Kr 26 _ 22 K _ 27 _ 23 C Ne 28 Si _ Pt _ 29 _ 25 Sn _ _ 24 Zr Na _ 30 Al _ 31 Cu _ 32 Ag _ 33 P _ 34 Mn _ 35 I _ 36 Au _ 37 Mg _ 38 Ni _ 39 Br _ 40 Hg _ Physical vs Chemical Properties A physical properties is observed with the senses and can be determined without destroying the object For example, color, shape, mass, length and odor are all examples of physical properties A chemical property indicates how a substance reacts with something else The original substance is fundamentally changed in observing a chemical property For example, the ability of iron to rust is a chemical property The iron has reacted with oxygen, and the original iron metal is changed It now exists as iron oxide, a different substance Classify the following properties as either chemical or physical by putting a check in the appropriate column Physical Property Blue Color Density Flammability Solubility Reacts with acid to form H2 Supports combustion Sour Taste Melting Point Reacts with water to form a gas 10 Reacts with a base to form water 11 Hardness 12 Boiling Point 13 Can neutralize a base 14 Luster 15 Odor Chemical Property Physical vs Chemical Changes In a physical change, the original substance still exists, it has only changed form In a chemical change, a new substance is produced Energy changes always accompany chemical changes Classify the following as being a physical or chemical change Sodium hydroxide dissolves in water Hydrochloric acid reacts with potassium hydroxide to produce a salt, water and heat A pellet of sodium is sliced in two Water is heated and changed to steam Potassium chlorate decomposes to potassium chloride & oxygen gas Iron rusts When placed in H2O, a sodium pellet catches on fire as hydrogen gas is liberated and sodium hydroxide forms Evaporation Ice melting 10 Milk sours 11 Sugar dissolves in water 12 Wood rotting 13 Pancakes cooking on a griddle 14 Grass growing in a lawn 15 A tire is inflated with air 16 Food is digested in the stomach 17 Water is absorbed by a paper towel 52.7 kJ 10 + Stress add H2 add I2 add HI remove H2 remove I2 remove HI increase temp decrease temp increase pressure decrease pressure H2 (g) + Equilibrium Shift Right At 462C, consider this reaction at equilibrium: NOCl (g)  NO (g) I2 (g) [H2] -  2HI (g) [I2] [HI] decrease increase - Keq same - + Cl2 (g) H = 20.5 kcal Answer TRUE or FALSE to each statement concerning the reaction Consider each as a separate case _ A If you initially started with only NOCl, the reaction would be exothermic _ B Increasing the concentration of NO causes an increase in the concentration of Cl _ C Decreasing the volume of the container favors the formation of NOCl _ D Decreasing the amount of chlorine gas causes the equilibrium to shift to the left _ E Increasing the temperature favors the formation of NO and chlorine gas _ F Adding argon gas, at constant pressure, will cause an increase in the products _ G Adding a catalyst generally decreases the amount of time required for the reaction to reach equilibrium _ H Adding more NOCl changes the value of the equilibrium constant _ I Increasing the temperature causes the equilibrium constant to change _ J Add a catalyst causes the equilibrium constant to change _ K Adding a catalyst increases the rate of the forward reaction _ L Increasing the temperature increases the rate of the forward reaction _ M Cooling the system causes the equilibrium to shift toward the right _ N At a given temperature, only one set of product and reactant concentrations satisfies the equilibrium constant Using the following equation: I2 (g)  2I (g) A If the equilibrium concentrations are as follows: [I2] = 1.2 M, [I] = 0.640 M write the Keq expression for the reaction B Calculate the value of Keq Equilibrium Worksheet Answer the following multiple-choice questions The equilibrium PCl5 (g)  PCl3 (g) + Cl2 (g) will be shifted to the right by: a Addition of a catalyst b Removal of Cl2 c Addition of an inert gas at constant volume d Removal of PCl5 (g) Complete the following table: NH4Cl (s) Stress add NH4Cl (s) Add NaCl (add Cl-) Remove NH4Cl (s) increase temp decrease temp increase pressure decrease pressure + heat  Equilibrium Shift NH4+ (aq) Amt NaOH (s) - + Cl- (aq) [Na+] [OH-] Keq - Consider the reversible system at equilibrium 2CO + O  2CO2 + heat When CO is removed: a The CO2 concentration will be increased b The CO2 concentration will be decreased c The amount of each substance will be unchanged d The amount of each substance will increased e The result can not be predicted from the information given What is the proper description of chemical equilibrium? a The frequencies of reactant and product collisions are identical b The concentrations of reactants and products are identical c The velocities of products and reactant molecules are identical d Reactant molecules are forming products as fast as product molecules are reacting to form reactants e The number of moles of reactants and products are equal (Next Page for More!) Calculate Keq in terms of molar concentrations for the reaction: N2 (g) + 3H2 (g)  2NH3 (g) + heat when the concentrations are N2 = 0.02M H2 = 0.01M , NH3 = 0.10M Write a Keq expression for the following reactions: a C2H6 (g) + O2 (g)  CO2 (g) + H2O(g) b PH3 (g)  P4 (g) + H2O(g) c HCl(g) + O2 (g)  Cl2 (g) + H2O(g) For the following equilibria, explain how the given stress affects the equilibrium point: a CaCO3(s)  CaO(s) + CO2(g) Removal of CO2 b N2(g) + O2 (g)  NO(g) Increase in pressure c SO3 (g) + Heat  SO2 (g) + O2 (g) Increase in Temperature Find the Keq for the reaction if [H2S] = 0.015 M, [H2] = 0.010 M, and the [S2] = 0.051 M H2S(g)  H2 (g) + S2 (g) Molarity, [H+], [OH-], pH, and pOH Relationships Molarity is a unit of concentration Recall, it stands for the moles of solute per liter of solution moles of solute liters of solution We use [] to symbolize molar concentration (molarity) [H+] is read “the concentration of hydrogen ions” Once we know one value (molarity of acid/base, [H +], [OH-], pH or pOH), we can find the others values These relationships will be useful for conversions: Molarity and concentration can depend on how many protons or hydroxide ions are in a compound Mono HCl Molarity of acid = [H+] [H+] = Molarity of acid KOH Molarity of base = [OH-] [OH-] = Molarity of base Poly H2SO4 x Molarity of acid = [H+] [H+] / = Molarity of acid [H+] x [OH-] = 1.0 x 10-14 pH + pOH = 14 [H+] = 10-pH [OH-] = 10-pOH pH = - log[H+] pOH = - log[OH-] Al(OH)3 x Molarity of base = [OH-] [OH-] / = Molarity of base pH + pOH [H ] - [OH ] Acid Base Worksheet #1 Define the following: a Arrhenius acid b Arrhenius base c Bronsted-Lowry acid d Bronsted-Lowry base Write the neutralization reactions for the following: a Sulfuric acid and potassium hydroxide b Phosphoric acid and calcium hydroxide c Nitric acid and magnesium hydroxide d Hydrofluoric acid and aluminum hydroxide Write the Ka or Kb expressions for the following (all acids/bases are aqueous): a HNO3 b HCl c NaOH d LiOH What is the difference between a solution with a pH of and a solution with a pH of 10? What are some properties of acids and bases? Using the equation for the auto-ionization of water and a K w = 1.0 x 10-14, calculate the pH and pOH of water Acid Base Worksheet #2 Find the pH of the following solutions: A 0.001 M solution of HCl (hydrochloric acid) A 0.09 M solution of HBr (hydrobromic acid) A 1.34 x 10-4 M solution of hydrochloric acid A 7.98 x 10-2 M solution of HNO3 (nitric acid) 12 L of a solution containing mole of hydrochloric acid 735 L of a solution containing 0.34 moles of nitric acid 120 mL of a solution containing 0.005 grams of hydrochloric acid 100 mL of a solution containing 1.00 grams of nitric acid 1.5 L of a solution containing 5.6 grams of hydroiodic acid 10 1.2 L of a solution containing 5.0 x 10-4 grams of hydrobromic acid Acid Base Worksheet #3 Using your knowledge of the Brønsted-Lowry theory of acids and bases, write equations for the following acid-base reactions and indicate each conjugate acidbase pair: a) HNO3 + OH-  b) NH3 + H2O  c) OH- + HPO4-2  Write the names for the following acids and bases: a) KOH b) H2SO4 c) C2H3O2H d) Fe(OH)2 e) HNO3 f) HCl g) NaOH h) H3PO4 If 0.001 moles of KOH are added to 0.1 L of solution, what is the: a pH b pOH When a student performs a titration in lab, he finds that it takes 23.2 mL of 34M HCl to neutralize 14.1 mL of NaOH What is the concentration of the NaOH? Acid Base Worksheet #4 What volume of 0.500 M HCl is required to neutralize 54.6 mL of 1.2 M KOH? What is the molarity of a solution of NaOH if it takes 45.7 mL of a 750 M solution of HNO to neutralize 43.9 mL? What is the molarity of an LiOH solution if it takes 48.0 mL to neutralize 35.0 mL of a 0.144 M solution of H2SO4? What is the pH and pOH of a solution made by adding water to 15 grams of hydroiodic acid (HI) until the volume of the solution is 2500 mL? What is an acid/base indicator used for? In a few steps, describe how you would titrate a base of unknown concentration with an acid with concentration M If 0.0025 moles of H2SO4 are added to 1.0 L of solution, what is the: c pH d pOH Determine the Bronsted-Lowry acid-base pairs for the following reactions: a HSO3+ H 2O  SO32+ H3O+ b HNO3 + H 2O  NO3- c HC4H7O2 + H 2O  C4H7O2- d HSO3- + H 2O  H2SO3 + OH- e NH3 + H 2O  NH4+ + OH- + H3O+ + H3O+ Acids, Bases, Conjugate Acids and Conjugate Bases HNO3 +  H2O Acid Base H3O+ NO3- + Conjugate Acid Conjugate Base Bronsted-Lowry Definition of Acids and Bases An acid is a proton (hydrogen ion) donor A base is a proton (hydrogen ion) acceptor Acids donate protons Bases accept protons Conjugate acids donate protons in the reverse reaction Conjugate bases accept protons in the reverse reaction Try these: Identify the acid, base, conjugate acid and conjugate bases in the following examples: a H2S + H2O  HS+ H3O+ b HClO2 + H2O  ClO2- + H3O+ c H2O + NH3  NH4+ + OH- d CO22- + H2O  HCO3- + OH- e H2PO4- + H2O  H3PO4 f H2PO4- + H2O  HPO42- + OH+ What are the conjugate bases of the following Bronsted-Lowry acids? a HF b HPO4-2 What are the conjugate acids of the following Bronsted-Lowry bases? a NO2b CN- H3O+ Worksheet on pH and Strong Acid Base Reactions Find the pH of the following: a 0.0001 M HNO3 e 0.000001 M LiOH b 0.001 M KOH f 0.0025 M HCl c 0.00001 M HCl g 0.0005 M NaOH d 0.1 M HCl h 0.0045 M LiOH Find the [OH-] of the following: a 0.0001 M HNO3 c 0.1 M HCl b 0.00001 M HCl d 0.0025 M HCl If 0.001 moles of KOH are added to 0.1 L of solution, what is the: a pH b pOH If 0.0025 moles of H2SO4 are added to 1.0 L of solution, what is the: a pH b pOH Review Worksheet 1 Write and balance the equation for the decomposition of Iron (II) oxide into its elements How many grams of FeO are needed to produce 140 grams of Fe? What volume of oxygen can be produced at STP from 25 g of Iron (II) oxide? What mass of iron is produced when 45 grams of oxygen are produced? Write and balance the equation for the combustion of pentane (C5H12) What mass of carbon dioxide is produced when 100.g of pentane is burned? What volume of water vapor at STP is produced when 250.g of pentane is burned? How many oxygen atoms are required to completely burn 50.g of pentane? Review Worksheet What’s the difference between a chemical and a physical property? Give two examples of each and explain how they are different Give four properties that are generally present in metals Thousand Island dressing and mayonnaise are mixed to make “secret sauce” for hamburgers  Chemical or physical change?  Your reason: Old ham goes bad in the refrigerator  Chemical or physical change?  Your reason: Fill in the following table: Element Number of Protons Number of Neutrons lithium carbon uranium Atomic Number Mass Number Isotope Notation \s\up 5( 6)Li 35 62 208 lead calcium Atomic Mass chlorine silver Number of Electrons 21 238 Review Worksheet If four moles of a gas at a pressure of 5.4 atmospheres have a volume of 120 liters, what is the temperature? If I initially have a gas with a pressure of 84 kPa and a temperature of 35 C and I heat it an additional 230 degrees, what will the new pressure be? Assume the volume of the container is constant My car has an internal volume of 2600 liters If the sun heats my car from a temperature of 200 C to a temperature of 550 C, what will the pressure inside my car be? Assume the pressure was initially 760 mm Hg How many moles of gas are in my car in problem #3? Write the complete ground state electron configurations for the following: 1) lithium 2) oxygen 3) calcium 4) titanium 5) rubidium Write the abbreviated (short-cut method) ground state electron configurations for the following: 6) nitrogen 7) chlorine 8) iron 9) zinc _ 10) tellurium Review Worksheet 1) What is the difference between an ionic and a covalent bond? 2) Draw the structural formulas and electron dot formulas for the following compounds Then determine the shapes of the molecules, the bond types and the molecule polarities a Water b Carbon dioxide c Sulfur difluoride d Arsenic trichloride 3) A 65 gram sample of water is heated from 25C to 85C How much heat did the water absorb? 4) Sketch a graph depicting the heating of water from -25C to 125C Be sure to include all of the necessary information 5) If you have two substances with different specific heats that absorb the same amount of energy, how will each substance react? ... When we say forms, produces, or becomes, we put a forms arrow A chemical reaction occurs between solid Zinc (Zn) and Hydrochloric Acid solution (HCl) forming Zn(s) + HCl(aq)  After forms, becomes,... Zn(NO3)2 + Ag _ (Next page for More!) Write and balance the equations for the following reactions Be sure to include the state of matter for example (s) for solid a aqueous sodium chloride... business transactions She traded all the goats for sheep at an exchange rate of goats for sheep Next, she exchanged all the sheep for hogs at a rate of sheep for hogs weighing 250 lbs each She sold