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1 AP#Chemistry#Summer#Work# Mr.#Herring# # The#work#in#this#summer#packet#reflects#the#knowledge#and#skills#you#need#to#possess#when#you#enter# this#class.##if#you#fail#to#do#the#work,#and#don t#know#this#information#hands#down,#you#place#yourself#in#a# position#where#you#are#likely#to#struggle#and#suffer#setbacks#the#entire#year.# # Please#do#not#hesitate#to# #me#with#any#questions#you#may#have.##I#check#my# #regularly.# # Know%the%following:% Metric%System% Significant%Figures%(sig%figs)% Stoichiometry% The%following%rules:% Rules%for%Naming%Acids% Solubility%Rules% Rules%for%assigning%oxidation%umber% Common%Polyatomic%ions% Atomic%trends:% Atomic%Radii% Charges%and%Ions%(cations%and%anions)% Ionization%Energy% Electron%Affinity% Electronegativity% Some%Thermochemistry% % % Complete%the%tasks%and%problems%with%each%of%the%following%links%to%web%pages:% % ; % Balancing equations practice web links # Complete#all#of#the#accompanying#worksheets#in#this#packet.##Where#required,#calculated#answers#must# contain#correct#units,#and#be#written#to#the#correct#number#of#sig#figs#using#the#rules#for#writing#sig#figs.## Failure%to%write%the%correct%units,%and/or%report%answers%to%the%correct%number%of%sig%figs%MAKES% YOUR%ANSWER%INCORRECT!!% % # % %

2 SCIENTIFIC NOTATION WORKSHEET #1 NAME EXPRESS EACH OF THE FOLLOWING NUMBERS IN PROPER SCIENTIFIC NOTATION: = 2. 50,000. = = ,000 = = ,000,000,000 = = = EXPRESS EACH OF THE FOLLOWING AS COMMON NUMBERS: x 10 5 = x 10-4 = x 10 5 = x 10-3 = x = x = PERFORM EACH OF THE FOLLOWING OPERATIONS USING SCIENTIFIC NOTATION. YOUR ANSWERS SHOULD BE ROUNDED TO THE TENTHS COLUMN IN EACH ANSWER. 15. (2.3 x 10 3 )(4.0 x 10 5 ) = 16. (9.6 x 10-1 )(5.2 x 10 2 ) = 17. (4.56 x 10-6 )(3.1 x 10-3 ) = 18. (5.7 x 10 8 )(2.3 x 10-4 ) = x 10 2 = 1.3 x x 10 5 = x (1.3 x 10 5 )(8.2 x 10-2 ) = 7.4 x x x 10 3

3 #2 PHYSICAL AND CHEMICAL PROPERTIES AND CHANGES Name PHYSICAL PROPERTY CHEMICAL PROPERTY 1. observed with senses 1. indicates how a substance 2. determined without destroying matter reacts with something else 2. matter will be changed into a new substance after the reaction Identify the following as a chemical (C) or physical property (P): 1. blue color 2. density 3. flammability (burns) 4. solubility (dissolves) 5. reacts with acid 6. supports combustion 7. sour taste 8. melting point 9. reacts with water 10. hardness 11. boiling point 12. luster 13. odor 14. reacts with air PHYSICAL CHANGE CHEMICAL CHANGE 1. a change in size, shape, or state 1. a change in the physical and 2. no new substance is formed chemical properties 2. a new substance is formed Identify the following as physical (P) or chemical (C) changes. 1. NaCl (Table Salt) dissolves in water. 9. Milk sours. 2. Ag (Silver) tarnishes. 10. Sugar dissolves in water. 3. An apple is cut. 11. Wood rots. 4. Heat changes H 2 O to steam. 12. Pancakes cook. 5. Baking soda reacts to vinger. 13. Grass grows. 6. Fe (Iron) rusts. 14. A tire is inflated. 7. Alcohol evaporates. 15. Food is digested. 8. Ice melts. 16. Paper towel absorbs water. Physical and Chemical Changes Part A Can you recognize the chemical and physical changes that happen all around us? If you change the way something looks, but haven t made a new substance, a physical change (P) has occurred. If the substance has been changes into another substance, a chemical change (C) has occurred. 1. An ice cube is placed in the sun. Later there is a puddle of water. Later still the puddle is gone. 2. Two chemical are mixed together and a gas is produce. 3. A bicycle changes color as it rusts. 4. A solid is crushed to a powder. 5. Two substances are mixed and light is produced. 6. A piece of ice melts and reacts with sodium. 7. Mixing salt and pepper. 8. Chocolate syrup is dissolved in milk. 9. A marshmallow is toasted over a campfire. 10. A marshmallow is cut in half.

4 Part B Read each scenario. Decide whether a physical or chemical change has occurred and give evidence for your decision. The first one has been done for you to use as an example. Scenario Physical or Chemical Change? Evidence 1. Umm! A student removes a loaf of bread hot from the oven. The student cuts a slice off the loaf and spreads butter on it. Physical No change in substances. No unexpected color change, temperature change or gas given off. 2. Your friend decides to toast a piece of bread, but leaves it in the toaster too long. The bread is black and the kitchen if full of smoke. 3. You forgot to dry the bread knife when you washed it and reddish brown spots appeared on it. 4. You blow dry your wet hair In baking biscuits and other quick breads, the baking powder reacts to release carbon dioxide bubbles. The carbon dioxide bubbles cause the dough to rise. You take out your best silver spoons and notice that they are very dull and have some black spots. A straight piece of wire is coiled to form a spring Food color is dropped into water to give it color. Chewing food to break it down into smaller particles represents a change, but the changing of starch into sugars by enzymes in the digestive system represents a change. In a fireworks show, the fireworks explode giving off heat and light. Part C: True (T) or False (F) 1. Changing the size and shapes of pieces of wood would be a chemical change. 2. In a physical change, the makeup of matter is changed. 3. Evaporation occurs when liquid water changes into a gas. 4. Evaporation is a physical change. 5. Burning wood is a physical change. 6. Combining hydrogen and oxygen to make water is a physical change. 7. Breaking up concrete is a physical change. 8. Sand being washed out to sea from the beach is a chemical change. 9. When ice cream melts, a chemical change occurs. 10. Acid rain damaging a marble statue is a physical change.

5 ATOMIC STRUCTURE WORKSHEET NAME Atoms are composed of three sub-atomic particles: the proton, the neutron, and the electron. The proton and the neutron are found in the nucleus. Electrons are found in a cloud surrounding the nucleus. The atomic number of an element is equal to the number of protons in that element. If the atom is neutral, the number of electrons (-) is equal to the number of protons (+). If the atom carries a charge, it is referred to as an ion. The charge on an ion indicates an imbalance between protons and electrons. If the ion has a positive charge, there are more protons than electrons. To find the number of electrons, you must subtract the charge from the atomic number. If the ion has a negative charge, there are more electrons than protons. To find the number of electrons, you must add the charge to the atomic number. The mass number is a whole number equal to the number of protons plus neutrons. This is because we say that protons and neutrons each have a mass of 1 amu (standardized from Carbon-12). This number is not on the periodic table. The atomic mass is the weighted average atomic mass of all the naturally occurring isotopes of an element. This number is located on the periodic table and is usually a decimal. (Remember, an isotope is an atom of the same element with a different number of neutrons; an ion is an atom of the same element with a different number of electrons.) X= element Mass number Charge A= mass number (# of protons + # of neutrons) Z= atomic number (# of protons) A - Z = # of neutrons Isotopic symbol is in this form: Atomic number Element symbol A Z Complete the chart. X Or, you might see: X A Example: Aluminum - 26 Element/Ion 1 1 H 1 1 H N Ca Ag Ag1+ Atomic Number Atomic Mass Mass Number Protons Neutrons Electrons

6 Define the following: Atomic Number Mass Number Atomic Mass Isotope Ion Isotope Name Isotope Symbol Number of Protons Neutrons Electrons Atomic Number Mass Number Argon-40 Argon-38 Bismuth Fe Pb Aluminum-27 Manganese SUMMARIZE: How do you find the number of protons for any atom? How do you find the number of neutrons for any atom? How do you find the number of electrons for any atom?

7 #4 Periodic Trends Worksheet 1) Rank the following elements by increasing atomic radius: carbon, aluminum, oxygen, potassium. 2) Rank the following elements by increasing electronegativity: sulfur, oxygen, neon, aluminum. 3) What is the difference between electron affinity and ionization energy? 4) Why does fluorine have a higher ionization energy than iodine? 5) Why do elements in the same family generally have similar properties? For chemistry help, visit Cavalcade Publishing All Rights Reserved

8 #5 Naming Ionic Compounds Give the name and molar mass of the following ionic compounds: Name Molar Mass 1) Na 2 CO 3 2) NaOH 3) MgBr 2 4) KCl 5) FeCl 2 6) FeCl 3 7) Zn(OH) 2 8) Be 2 SO 4 9) CrF 2 10) Al 2 S 3 11) PbO 12) Li 3 PO 4 13) TiI 4 14) Co 3 N 2 15) Mg 3 P 2 16) Ga(NO 2 ) 3 17) Ag 2 SO 3 18) NH 4 OH 19) Al(CN) 3 20) Be(CH 3 COO) 2 WKS001x Cavalcade Publishing ( All Rights Reserved

9 For the following compounds, give the formulas and the molar masses: Formula Molar Mass 22) sodium phosphide 23) magnesium nitrate 24) lead (II) sulfite 25) calcium phosphate 26) ammonium sulfate 27) silver cyanide 28) aluminum sulfide 29) beryllium chloride 30) copper (I) arsenide 31) iron (III) oxide 32) gallium nitride 33) iron (II) bromide 34) vanadium (V) phosphate 35) calcium oxide 36) magnesium acetate 37) aluminum sulfate 38) copper (I) carbonate 39) barium oxide 40) ammonium sulfite 41) silver bromide 42) lead (IV) nitrite WKS001x Cavalcade Publishing ( All Rights Reserved

10 #6 Ionic Compound Formula Writing Worksheet Write chemical formulas for the compounds in each box. The names are found by finding the intersection between the cations and anions. Example: The first box is the intersection between the zinc cation and the chloride anion, so you should write ZnCl 2, as shown. chloride ZnCl 2 acetate nitrate Oxide nitride sulfate zinc iron (II) iron (III) gallium silver lead (IV) Write the formulas for the following compounds: 1) copper (II) chloride 2) lithium acetate 3) vanadium (III) selenide 4) manganese (IV) nitride 5) beryllium oxide 6) sodium sulfate 7) aluminum arsenide 8) potassium permanganate 9) chromium (VI) cyanide 10) tin (II) sulfite 11) vanadium (V) fluoride 12) ammonium nitrate Ionic Compound Naming Chilton Honors Chemistry

11 #6b Names & Formulas for Ionic Compounds Give the name or formula of the following ionic compounds: Name 1) Na 2 CO 3 2) NaOH 3) MgBr 2 4) KCl 5) FeCl 2 6) FeCl 3 7) Zn(OH) 2 8) Be 2 SO 4 9) CrF 2 10) Al 2 S 3 11) PbO 12) Li 3 PO 4 13) TiI 4 14) Co 3 N 2 15) Mg 3 P 2 16) Ga(NO 2 ) 3 17) Ag 2 SO 3 18) NH 4 OH 19) Al(CN) 3 20) Be(CH 3 COO) 2 Formula 21) sodium phosphide 22) magnesium nitrate 23) lead (II) sulfite 24) calcium phosphate 25) ammonium sulfate 26) silver cyanide 27) aluminum sulfide 28) beryllium chloride 29) copper (I) arsenide 30) iron (III) oxide 31) gallium nitride 32) iron (II) bromide 33) vanadium (V) phosphate 34) calcium oxide 35) magnesium acetate 36) aluminum sulfate 37) copper (I) carbonate 38) barium oxide 39) ammonium sulfite 40) silver bromide Ionic Compound Naming Chilton Honors Chemistry

12 #7 Balance the equations below: Balancing Chemical Equations 1) N 2 + H 2 NH 3 2) KClO 3 KCl + O 2 3) NaCl + F 2 NaF + Cl 2 4) H 2 + O 2 H 2 O 5) Pb(OH) 2 + HCl H 2 O + PbCl 2 6) AlBr 3 + K 2 SO 4 KBr + Al 2 (SO 4 ) 3 7) CH 4 + O 2 CO 2 + H 2 O 8) C 3 H 8 + O 2 CO 2 + H 2 O 9) C 8 H 18 + O 2 CO 2 + H 2 O 10) FeCl 3 + NaOH Fe(OH) 3 + NaCl 11) P + O 2 P 2 O 5 12) Na + H 2 O NaOH + H 2 13) Ag 2 O Ag + O 2 14) S 8 + O 2 SO 3 15) CO 2 + H 2 O C 6 H 12 O 6 + O 2 16) K + MgBr KBr + Mg 17) HCl + CaCO 3 CaCl 2 + H 2 O + CO 2 18) HNO 3 + NaHCO 3 NaNO 3 + H 2 O + CO 2 19) H 2 O + O 2 H 2 O 2 20) NaBr + CaF 2 NaF + CaBr 2 21) H 2 SO 4 + NaNO 2 HNO 2 + Na 2 SO 4 WKS001x Cavalcade Publishing ( All Rights Reserved

13 #8 Writing'Chemical'Equations' ' Part%A' 'Translate)all)the)formulaic)equations)to)word)equations.))' ' 1. Na2O'+'H2O' 'NaOH' 2. 2HgO(s)' '2Hg(l)'+'O2(g)' 3. BaCl2(aq)'+'Na2CrO4(aq)' 'BaCrO4(s)'+'2NaCl(aq)' 4. CS2(l)'+'3O2(g)' 'CO2(g)'+'2SO2(g)' 5. NaCl(aq)'+'AgNO3(aq)' 'NaNO3(aq)'+'AgCl(s)' 6. H2(g)'+'Cl2(g)' '2HCl(g)' 7. 2H2O(l)' '2H2(g)'+'O2(g)' 8. Zn(s)'+'HCl(aq)' 'ZnCl2(aq)'+'H2(g)' 9. Al4C3(s)'+'H2O(l)' 'CH4(g)'+'Al(OH)3(s)' 10. Al2(SO4)3'+'Ca(OH)2' 'Al(OH)3'+'CaSO4' 11. 2K(s)'+'2H2O(l)' '2KOH(aq)'+'H2(g)' 12. H2SO4(aq)' 'SO3(g)'+'H2O(l)' 13. 2KClO3(s)' '2KCl(s)'+'3O2(g)' 14. CH3OH(g)'+'O2(g)' 'CO2(g)'+'H2O(g)' ' Part%B' 'Translate)all)the)word)equations)to)formulaic)equations)and)then)balance)them.' ' 1. Sodium'combines'with'chlorine'to'produce'sodium'chloride.' 2. When'solid'copper'reacts'with'aqueous'silver'nitrate,'the'products'are'aqueous'copper'II' nitrate'and'silver'metal.' 3. Solid'iron'III'oxide'and'carbon'monoxide'gas'produce'iron'metal'and'carbon'dioxide'gas.' 4. Sulfuric'acid'and'sodium'hydroxide'react'to'form'sodium'sulfate'and'water.' 5. Vanadium'II'oxide'with'iron'III'oxide'results'in'the'formation'of'vanadium'V'oxide'and'iron'II' oxide.' 6. Aluminum'reacts'with'oxygen'to'produce'aluminum'oxide.' 7. Mercury'II'oxide'decomposes'to'produce'mercury'and'oxygen' 8. Sodium'carbonate'decomposes'to'produce'sodium'oxide'and'carbon'dioxide' 9. Carbon'dioxide'gas'reacts'with'solid'lithium'hydroxide'to'produce'solid'lithium'carbonate'and' water.' 10. Ammonia'gas'reacts'with'oxygen'gas'to'produce'nitrogen'monoxide'gas'and'steam.' 11. Solid'ammonium'nitrate'decomposes'to'produce'dinitrogen'monoxide'gas'and'water.' 12. Carbon'monoxide'reacts'with'hydrogen'to'produce'methanol.' 13. Liquid'carbon'disulfide'reacts'with'oxygen'gas'to'produce'carbon'dioxide'gas'and'sulfur' dioxide'gas.' 14. Aluminum'metal'reacts'with'aqueous'copper'II'chloride'to'produce'aqueous'aluminum' chloride'and'solid'copper.' 15. Solid'ammonium'chloride'decomposes'to'produce'ammonia'gas'and'gaseous'hydrochloric' acid.' '

14 #9 Predicting Reaction Products Balance the equations and predict the products for the following reactions: 1) Na + FeBr 3 2) NaOH + H 2 SO 4 3) C 2 H 4 O 2 + O 2 4) NH 3 + H 2 O 5) PbSO 4 + AgNO 3 6) PBr 3 7) HBr + Fe 8) KMnO 4 + ZnCl 2 9) MnO 2 + Sn(OH) 4 10) O 2 + C 5 H 12 O 2 11) H 2 O 2 12) PtCl 4 + Cl 2 WKS001x Cavalcade Publishing ( All Rights Reserved

15 #10 StoichiometryWorksheet 1.Na 2SIO 3(s)+8HF(aq) H 2SiF 6(aq)+2NaF(aq)+3H 2O(l) a.howmanymolesofhfareneededtoreactwith0.300molofna 2SiO 3? b.howmanygramsofnafformwhen0.500molofhfreactswithexcessna 2SiO 3? c.howmanygramsofna 2SiO 3canreactwith0.800gofHF? 2.C 6H 12O 6(aq) 2C 2H 5OH(aq)+2CO 2(g) a.howmanymolesofco 2areproducedwhen0.400molofC 6H 12O 6reactsinthis fashion? b.howmanygramsofc 6H 12O 6areneededtoform7.50gofC 2H 5OH? c.howmanygramsofco 2formwhen7.50gofC 2H 5OHareproduced? 3.Fe 2O 3(s)+CO(g) Fe(s)+CO 2(g)(unbalanced!) a.calculatethenumberofgramsofcothatcanreactwith0.150kgoffe 2O 3

16 b.calculatethenumberofgramsoffeandthenumberofgramsofco 2formed when0.150kgoffe 2O 3reacts 4.2NaOH(s)+CO 2(g) Na 2CO 3(s)+H 2O(l) a.whichreagentisthelimitingreactantwhen1.85molnaohand1.00molco 2are allowedtoreact? b.howmanymolesofna 2CO 3canbeproduced? 5.C 6H 6+Br 2 C 6H 5Br+HBr a.whatisthetheoreticalyieldofc 6H 5Brinthisreactionwhen30.0gofC 6H 6reacts with65.0gorbr 2? b.iftheactualyieldofc 6H 5Brwas56.7g,whatisthepercentyield?

17 #11 Stoichiometry: Mass-Mass Problems 1. 2KClO 3 2KCl + 3O 2 How many grams of potassium chloride, KCl, are produced if 25.0g of potassium chlorate, KClO 3, decompose? 2. N 2 + 3H 2 2NH 3 How many grams of hydrogen, H 2, are necessary to react completely with 50.0 g of nitrogen, N 2? 3. How many grams of ammonia, NH 3, are produced in the reaction with 50.0 g of N 2, nitrogen, in Problem 2? 4. 2AgNO 3 + BaCl 2 2AgCl + Ba(NO 3 ) 2 How many grams of AgCl, silver chloride, are produced from 5.0 g of AgNO 3, silver nitrate? 5. How many grams of BaCl 2, barium chloride, is necessary to react with the 7.5 g AgNO 3, silver nitrate, in Problem 4?

18 #12 Percent, Actual, and Theoretical Yield 1) LiOH + KCl LiCl + KOH a) I began this reaction with 20 grams of lithium hydroxide. What is my theoretical yield of lithium chloride? b) I actually produced 6 grams of lithium chloride. What is my percent yield? 2) C 3 H O 2 3 CO H 2 O a) If I start with 5 grams of C 3 H 8, what is my theoretical yield of water? b) I got a percent yield of 75% How many grams of water did I make? 3) Be + 2 HCl BeCl 2 + H 2 My theoretical yield of beryllium chloride was 10.7 grams. If my actual yield was 4.5 grams, what was my percent yield? 4) 2 NaCl + CaO CaCl 2 + Na 2 O What is my theoretical yield of sodium oxide if I start with 20 grams of calcium oxide? For chemistry help, visit Cavalcade Publishing All Rights Reserved

19 5) FeBr KCl FeCl KBr a) What is my theoretical yield of iron (II) chloride if I start with 34 grams of iron (II) bromide? b) What is my percent yield of iron (II) chloride if my actual yield is 4 grams? 6) TiS + H 2 O H 2 S + TiO What is my percent yield of titanium (II) oxide if I start with 20 grams of titanium (II) sulfide and my actual yield of titanium (II) oxide is 22 grams? 7) U + 3 Br 2 UBr 6 What is my actual yield of uranium hexabromide if I start with 100 grams of uranium and get a percent yield of 83%? 8) H 2 SO 4 H 2 O + SO 3 If I start with 89 grams of sulfuric acid and produce 7.1 grams of water, what is my percent yield? For chemistry help, visit Cavalcade Publishing All Rights Reserved

20 #13 Name: Per: Date: Row Thermochemistry Review Worksheet 1.Definitions: -Endothermic: -Exothermic: -Enthalpy: -Law of Conservation of Energy -Heat of Reaction: -Heat of Fusion -Specific Heat 2. Explain why water is used in a calorimeter? What unique properties does water have? Calculations: 1. How many Joules of heat energy would be required to raise the temperature of 16.0g of lead from 25 C to its melting point of 327 C for a length of time long enough to completely melt the lead. Given: The specific heat capacity of lead is 0.159J/gK and the molar enthalpy of fusion is 24.7J/g. Specific heat is in Kelvin. Must convert C to Kelvin. Q=mcΔT Q=1460J 2. How much energy is absorbed by 300g of methanol, CH 3 OH, as it evaporates? Given: The molar heat of vaporization is 35.3kJ/mol. 300 * (1/45.02) * (35.3/1) = 200 J (1 sigfig) 3. If 540g of water condenses on a car during a cool night, calculate the amount of energy released to the air during this condensation. Given: The molar heat of vaporization of water is 40.79kJ/mol. 540 * (1/18.02) * (40.79/1) = 1200kj 2 sig figs

21 4. Calculate the amount of energy that is needed to change 125g of ice at -25 C to water at 75 C. Be sure to sketch a Phase Diagram of this process before beginning the work. Given: Molar enthalpy of fusion is 6.009kJ/mol, molar enthalpy of vaporization is 40.79kJ/mol, the specific heat of solid H 2 O is 2.1J/gK, the specific heat of liquid H 2 O is 4.186J/gK, and the specific heat of gas H 2 O is 1.7J/gK. 125 * 2.1 * 100 = 26000kj 5. What is the molar enthalpy of the formation of 1mol H 2 SO 4(l) given the following information? 2H 2(g) + O 2(g)! 2H 2 O (g) ΔH rxn = -484kJ 2S (s) + 3O 2(g)! 2SO 3(g) ΔH rxn = -890kJ H 2(g) + 2O 2(g) + S (s)! H 2 SO 4(l) ΔH rxn = -814kJ H 2 O (g) + SO 3(g)! H 2 SO 4(l) ΔH rxn = xkj 115KJ 6. What is the molar enthalpy of the formation of 1mol C 2 H 6 gas given the following information? C 2 H 4(g) + 3O 2(g)! 2CO 2(g) + 2H 2 O (l) ΔH rxn = -1401kJ 2C 2 H 6(g) + 7O 2(g)! 4CO 2(g) + 6H 2 O (l) ΔH rxn = -3100kJ 2H 2(g) + O 2(g)! 2H 2 O (l) ΔH rxn = -572kJ C 2 H 4(g) + H 2(g)! C 2 H 6(g) ΔH rxn = xkj -137KJ 7. The reaction for the fermentation of glucose is C 6 H 12 O 6 (aq)! 2CO 2(g) + 2C 2 H 5 OH (aq) ΔH rxn = -67kJ a. Is this reaction endothermic or exothermic? b. Calculate the energy released when 250g of glucose C 6 H 12 O 6 (aq) ferments. 250 * (1/180.07) * (-67/1) = -93KJ

PHYSICAL AND CHEMICAL PROPERTIES AND CHANGES

PHYSICAL AND CHEMICAL PROPERTIES AND CHANGES Name Key PHYSICAL PROPERTY CHEMICAL PROPERTY 1. observed with senses 1. indicates how a substance 2. determined without destroying matter reacts with something