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General Chemistry

by: Austen Pollich

General Chemistry CHM 11200

Marketplace > Purdue University > Chemistry > CHM 11200 > General Chemistry
Austen Pollich
GPA 3.75


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This 14 page Study Guide was uploaded by Austen Pollich on Saturday September 19, 2015. The Study Guide belongs to CHM 11200 at Purdue University taught by Staff in Fall. Since its upload, it has received 85 views. For similar materials see /class/207974/chm-11200-purdue-university in Chemistry at Purdue University.


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Date Created: 09/19/15
PURDUE UNIVERSITY Chemistry 112 Study Guide This study guide lists the topics or terms that should be mastered before you attempt the examination for credit in Chemistry 112 The material can be found in a number of books on the market A list of possible textbooks is given below Attached is a sample Chemistry 112 nal exam along with the answers Important 1 Read this material thoroughly if you expect to try for advanced placement and extra credit which counts towards graduation 2 Study the topics listed in the attached outline 3 Work many practice problems listed at the end of the corresponding chapters in textbooks 4 Come to the examination rested No one can do well on an exam when excessively fatigued You should therefore try to rest before taking the exam for credit If your trip to campus requires travel into the late hours of the night or a very early departure form your home you might be advised to allow for one nights rest in the Lafayette area before taking the examination Many students who are unsuccessful with the examination tell us that failure to take this advice contributed to their inability to complete the examination successfully Please consult your advanced credit schedule or your academic advisor for both the time and place of the examination Suggested Texts for study Fundamentals of Chemistry by Ralph Burns 2nd edition Prentice Hall F J 39 of General Organic and Rinln ical Chemistry by John Holum Wiley Chemist The Central Science by Brown Lemay Bursten Prentice Hall Chemist Principles and Practice by Reger Goode Mercer Saunders Other Resources Throughout the year Chemistry 112 final exams only are on file at the Stewart Copy Center STEW G 66 During the Fall and Spring semester old Chemistry 112 hourly exams are available in the Chemistry Resource Room WTHR 117 m Atmosphere Kinetic Molecular Theory Kinetic Energy Atmospheric Pressure de nition and units Boyles39 Law Charles39s law GayLussac s Law Combined Gas Law Standard Temperature and Pressure STP Molar Volume and Gas Density Ideal Gas Law universal gas constant Real Gases Dalton s Law of partial Pressures Vapor Pressure Gas Stoichiometry Diffusion Liquids and solids Intramolecular forces bonding types Intermolecular forces attractions of molecules one for another as a group called van der Waals hydrogen bonding Dispersion forces London forces Dipole forces Vaporization and condensation Boiling point Heat of Vaporization Heat of fusion specific heat Heating and cooling curves Amorphous solids crystalline solids ionic molecular covalent network metallic Solutions Homogeneous heterogeneous Solute solvent Miscible immiscible soluble insoluble concentrated dilute hydration solvation Effects of temperature and pressure on solubility Saturated and unsaturated Solubility of gases in liquids Solution Concentration Expressions Molarity percent by volume percent by mass parts per million ppm parts per billion ppb molality Colligative Properties of Solutions Colloids Osmosis Reaction Rates and Chemical Equilibrium Reaction Rates Collision Frequency Orientation Activation Energy Potential Energy Reaction pathway Endothermic Exothermic Factors that Effect Reaction Rates temperature concentration catalyst surface area Equilibrium Le Chatelier s Principle how changes in concentration temperature pressure affect equilibrium The Equilibrium Constant Expression Acids and Bases Arrhenius Theory BronstedLowry De nition conjugate acidbase pairs Hydrogen Hydronium ions Monoprotic Diprotic Triprotic acids Strong and Weak Acids de nitions and examples Use and Preparation of important industrial acids Reactions of Acids with Bases neutralization Reactions of Acids with Active metals with Metal Oxides with Carbonates and Bicarbonates with Metal Sul des Acid rain Reaction of Bases with salts of transition metals with amphoteric metals Reactions of amphoteric hydroxides with Acids and Bases Lewis De nitions of Acids and Bases Selfionization of water pH de nition and scale how to calculate pH and pOH Hydrolysis of salts in water Buffers AcidBase Titrations Oxidation and Reduction Oxidation numbers De nition of oxidation and reduction Oxidizing and Reducing agents Balancing oxidation reduction reactions Electrolytic and Voltaic Cells Anode and cathode reactions Nuclear Chemistry Alpha and beta particles gamma rays Symbols Half life and calculations Radiation units Radioactive decay Electron capture Deuterium tritium Radioisotope dating Fission Fusion Organic Chemistry IUPAC names and structures of alkanes alkenes alkynes Properties of alkanes alkenes alkynes Saturated and unsaturated hydrocarbons Cistrans isomerism Optical isomers Aromatic hydrocarbons names and substitutions Names and structures of Alcohols phenols ethers aldehydes ketones carboxylic acids esters amines amides Biochemistry Carbohydrates lipids amino acids proteins nucleic acids Vitamins hormones Monosaccharides Disaccharides Polysaccharides Fatty acids saturated and unsaturated fats Peptide bonds Enzymes DNA RNA Nucleotide Double Helix Transcription Replication 6 The air in a jar of homecanned beans is heated to the boiling point of water 100 C and the jar is sealed at that temperature Assume the pressure is 100 atm when the jar is sealed What will be the air pressure in the jar when it is cooled to room temperature 20 C a 020 atm b 500 atm c 079 atm d 127 atm e none of these Old questions are best Figure out the volume that 1 mole of laughing gas N20 occupies at 150 atm and 275 C a 15 L b 20 L c 30 L d 59 L e 75 L In the kinetic theory which of the following is not a property of an M gas a Gases consist of tiny particles in random motion b Collisions between gas molecules are perfectly elastic c There are attractive intermolecular forces d The average molecular kinetic energy is proportional to the Kelvin temperature e The volume occupied by gas molecules is negligible Which of the following phase changes is endothermic AH a freezing of water b liquefaction of air c condensation of butane gas to liquid d solidification of magnesium metal from its molten state e sublimation of solid dry ice to CO2 gas In which of the following compounds will there be hydrogen bonding 3 CH4 b H20 0 H2 d HI 9 BH3 Water dissolves many ionic salts because a H20 is a linear molecule b H20 is a very small molecule c H20 has a large vapor pressure d H20 is a polar molecule e H20 is a very volatile liquid A particular solid crystal has a structure consisting of cations at the lattice positions bound together by a sea ofmobile electrons This solid can e a copper b aluminum chloride c solid C02 d ice e diamond 144 g of ethanol CZHSOH and 960 g of water are mixed giving 2694 mL ofa solution with density of 0891 mL The water is considered to be the solvent What is the molarity M of ethanol in this solution a 116 b 313 c 150 d 8 4 a 3 1 b 1 50 c 11 d 32 6 e none of these As a chemical reaction proceeds the reaction rate generally decreases The main reason for this is a the temperature decreases as reaction proceeds b the catalyst is used up c the unreacted molecules have insuf cient energy d the concentrations of the reactants are decreasing e the energy of activation increases steadily In a chemical reaction between a solid substance and a gas the speed of reaction is proportional to a the surface area between solid and gas phases b the volume of gas plus the volume of solid c the solubility of the gas in the solid d the electronegativities of the reactants e the intermolecular attractions between gas and solid molecules 8 The equilibrium constant Ke for the following reaction at a certain temperature is found to e 62 When the equilibrium concentrations of H2g and 12g are 020 M and 025 M respectively at this temperature what is the equilibrium concentration of HIg H2g t 12 2 H1 a 176 M b 044 M c 310 M d 124 M e none of these Consider the following five reactions at equilibrium For one of these equilibrium systems increasing the pressure by decreasing the volume of the container will not disturb the equilibrium and will result in no changes in reactant concentrations Which one a H2g 3 H2 2 NH3g b 2 C0 02 2 C02 0 2N02 N204g d 2 N0 02 2 N02 6 H2g12g 2 H1 Which of the following statements is false a More than one hydrogen isotope eXists b Intense short range forces act between nucleons c decay is often accompanied by yray emission d Most neutronrich radioisotopes decay by neutron emission e Different isotopes of a single element are chemically similar ZgiPu decays by ocparticle emission to form the product X The identity of X is a 23in b ZSSU c 232C111 d 2ggTh e 271Pa 20 In pure water at 25 C a H30 1 10H 1 b H3Ol 10x 10 7 c H3Ol x OH 10 x 10 14 moles2liters2 d pH pOH e all of the above What is the pH ofa solution with H 00417 M CH3 CH CHZ ZH CHz CH3 CH3 EH2 CH3 a 183 b 318 c 138 d 813 e 83 a 1 b 3 E33 4 e 5 What is the proper IUPAC name of the following compound a 4ethyl2methylhexane b 3ethyl5methylhexane c 2methyl4ethylhexane d 4ethyl2methylnonane e none of the above The following is an example of an CH2 CH2 H2 a CchH3 a addition reaction b isomerization reaction c oxidationreduction reaction d polymerization reaction e a and c 21 22 23 24 25 26 How many dibromonitrobenzene isomers are there 2 E33 2 E33 8 e 10 The oxidation of a secondary alcohol can produce an a aldehyde b ketone c carboxylic acid d primary alcohol e tertiary alcohol An unsaturated fat a is always a synthetic product b can be safely digested in unlimited quantities c is not considered a lipid d will react with Brz e all of the above Which functional groups are not commonly found in disaccharides a carboxylates b amines c amides d alkynes e all ofthese Enzymes are polymers made of what type of monomer a fatty acids b proteins c nucleotides d hexoses e amino acids Enzymes a catalyze biochemical reactions b do not change the equilibrium state of a reaction c are oligosaccharides d a and b e a and c 27 28 The acetic acid acetate buffer solution maintains a pH near a 7476 b 0 c 476 d 925 e 7720 A coalbuming power plant releases 800 tons of sulfur dioxide 02 per day If all ofthis came back to us as acid rain in the form of H2804 how many tons of HZSO4 would fall a 1000 b 1080 c 1160 d 1225 e You cannot get H2804 from 02 The following reactions illustrate the process of corrosion to be used to answer questions 2930 29 30 31 I 2 Fe 02 2 H20 A 2 FeOH2 II 4 FeOH2 02 2 H20 A 4 FeOH3 III 2 FeOH3 A Fe203H20 H20 Which reactions are oxidationreduction reactions a 1 11 111 b 1 11 c 1 111 d 11 111 e 1 b I c 1 111 d 11 111 e 111 What are the three major components of the nucleotide a zwitterion amide Rgroup b base sugar phosphate c guanine adenine cytoseine d DNA RNA base e blood sweat tears 32 33 34 35 36 37 An amide is synthesized from a an alcohol and an alkane b a phosphate and an amine c a carboxylic acid and an amine d an amine and an alkane e a sugar and a carboxylic acid Benzene is aromatic because a it smells good b it is carcinogenic c it has delocalized TE electrons d it has 4 TE electrons e none of the above The basic structural principles of organic chemistry were developed around a 1650 b 1750 c 1850 d 1950 e 2050 What molecular units are used to make up nylon a naphthalene b H2N CH26 NHz c HOOCe CH247 COOH d a and b e b and c Te on is composed of what two elements a C H b C 0 c C N d C F e N 0 Which is chiral a horse shoe b baseball c a ship s propeller d benzene e coffee mug 38 39 40 Benzene is most soluble in a hexane b water c H3PO4 d CaO e NaOH BF3 NH3 is an example of a the reaction of a Bronsted acid and Bronsted base b the reaction of a Lewis acid and a Lewis base c the reaction of a Lewis acid and Bronsted base d the reaction of Lewis base and Bronsted acid Cistrans isomers have a different connectivities b the same geometry c different physical properties d are chiral e none of the above 14 Answers to the sample exam deEEdcdbEbcccEdcabc L234i61890L23456890 22222222233333333334 ccchdaaddaaEdbEccaE 0L234567oo90 12345678911111111112


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