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1. subatomic particles (p,n & e) 2. atomic mass/number & periodic table 3 ground v. excited states 4. valence e-/ dot diagrams 5. electron configuration - short 6. atomic model 7. creation of light -- bohr, wave mechanical, rutherford Name: ___________________________ a 1) ____ Which subatomic particle is negatively charged? a) b) c) d) electron neutron positron proton c What is the mass number of a carbon atom that contains six protons, eight neutrons, and six electrons? 2) ____ a) 6 b) 8 c) 14 d) 20 d An atom in the ground state has a stable valence electron configuration. This atom could be an atom of 3) ____ a) Al b) Cl 8 valence electron (noble c) Na gases, group 18) d) Ne b Which electron configuration represents an atom in an excited state? 4) ____ a) 2–7 b) 2–6–2 c) 2–8–1 d) 2–8–8–2 c What information is necessary to determine the atomic mass of the element chlorine? 5) ____ a) the atomic mass of each artificially produced isotope of chlorine, only b) the relative abundance of each naturally occurring isotope of chlorine, only c) the atomic mass and the relative abundance of each naturally occurring isotope of chlorine d) the atomic mass and the relative abundance of each naturally occurring and artificially produced isotope of chlorine Base your answers to questions 6 through 8 on the information to the right. 6) State, in terms of the number of subatomic particles, one similarity and one difference between the atoms of these isotopes of sulfur. They all contain 16 protons Similarity: ______________________________________ They have different # of neutrons Difference: _____________________________________ 7) In the space provided, draw a Lewis electron-dot diagram for an atom of sulfur-33. 8) atomic mass = (mass)(%) + (mass)(%)+ # of valence electrons 8) In the space provided, calculate the atomic mass of sulfur. = 30.249 + 0.243 + 1.457 32.06 u + a In an atom of argon-40, the number of protons 9) ____ a) equals the number of electrons b) equals the number of neutrons c) is less than the number of electrons d) is greater than the number of electrons = Regents Review - Atomic Structure Created: February 2010 1-3 0.00719 Name: ___________________________ a An electron in a sodium atom moves from the third shell to the fourth shell. This change is a result of the atom 10) ____ a) b) c) d) absorbing energy releasing energy gaining an electron losing an electron Base your answers to questions 11 and 12 on the information below. In 1897, J. J. Thomson demonstrated in an experiment that cathode rays were deflected by an electric field. This suggested that cathode rays were composed of negatively charged particles found in all atoms. Thomson concluded that the atom was a positively charged sphere of almost uniform density in which negatively charged particles were embedded. The total negative charge in the atom was balanced by the positive charge, making the atom electrically neutral. In the early 1900s, Ernest Rutherford bombarded a very thin sheet of gold foil with alpha particles. After interpreting the results of the gold foil experiment, Rutherford proposed a more sophisticated model of the atom. 11) State one conclusion from Rutherford’s experiment that contradicts one conclusion made by Thomson. Rutherford experiment determined that an atom is mostly empty space. 12) State one aspect of the modern model of the atom that agrees with a conclusion made by Thomson. The atom has a positive nucleus. b Which electron configuration represents an excited state for a potassium atom? 13) ____ a) 2-8-7-1 b) 2-8-7-2 c) 2-8-8-1 d) 2-8-8-2 Given the bright-line spectra of three elements and the spectrum of a mixture formed from at least two of these elements: a Which elements are 14) ____ present in this mixture? a) E and D, only b) E and G, only c) D and G, only d) D, E, and G 15) Describe the electrons in an atom of carbon in the ground state. Your response must include: • the charge of an electron • the location of electrons based on the wave-mechanical model • the total number of electrons in a carbon atom An electron has a negative charge, and is located in areas of probability outside the nucleus, there are 6 electrons in carbon b Which two particles have opposite charges? 16) ____ a) an electron and a neutron b) an electron and a proton c) a proton and a neutron d) a proton and a positron Regents Review - Atomic Structure 2-3 Created: February 2010 Name: ___________________________ a Which statement describes how an atom in the ground state becomes excited? 17) ____ a) b) c) d) The atom absorbs energy, and one or more electrons move to a higher electron shell. The atom absorbs energy, and one or more electrons move to a lower electron shell. The atom releases energy, and one or more electrons move to a higher electron shell. The atom releases energy, and one or more electrons move to a lower electron shell. d Which symbol represents an atom in the ground state with the most stable valence electron configuration? 18) ____ a) B b) O Noble gases have stable octet, 8 valence ec) Li d) Ne b Each diagram to the right represents the nucleus of a 19) ____ different atom. Which diagrams represent nuclei of the same element? same # of protons = same element a) D and E, only b) D, E, and Q different # of neutrons = isotope c) Q and R, only different # of electrons = ion d) Q, R, and E Base your answers to questions 20 through 23 on the information to the right. The atomic and ionic radii for sodium and chlorine are shown in the table below. 20) Write the ground state electron configuration for the ion that has a radius of 181 picometers. ion of Chlorine = 18e 2 2 6 2 6 or 2-8-8 1s 2s 2p 3s 3p ___________________________________ 21) Convert the radius of an Na+ ion to meters. _____________________ 102.x10-12 = 1.2 x 10-10 22) Explain, in terms of atomic structure, why the radius of an Na atom is larger than the radius of an Na+ion. Na has 3 energy level while Na+ has only 2 energy levels Base your answers to questions 23 and 23 on the information below. The nucleus of one boron atom has five protons and four neutrons. 5 23) Determine the total number of electrons in the boron atom. ___________________ + 5 24) Determine the total charge of the boron nucleus. ________________ number of protons neutrons don't have a charge Regents Review - Atomic Structure 3-3 Created: February 2010 1. Gram formula mass = mass of 1 mole = atomic mass in grams 2. mass = gfm 4. particles = 6.02x1023 6. conservation of mass Name: ______________________ 3. volume = 22.4L/mol 5. % composition 7. mass <--> mole d 1) ____ A 1.0-mole sample of krypton gas has a mass of a) b) c) d) 19 g 36 g 39 g 84 g 1 mole = 6.02x1023 atoms of Krypton = atomic mass in grams moles ratio Given the balanced equation representing a reaction: 28 moles 2) Determine the total number of moles of oxygen that react completely with 8.0 moles of C2H6.____________ 3) Determine the mass of 5.20 moles of C2H6 . Show your work. mass = moles x gfm = 5.20 moles x 30 g/mol = 156 g Base your answers to questions 4 through 8 on the information below. Arsenic is often obtained by heating the ore arsenopyrite, FeAsS. The decomposition of FeAsS is represented by the balanced equation below. 125 = 67.5 + X In the solid phase, arsenic occurs in two forms. One form, yellow arsenic, has a density of 1.97 g/cm3 at STP. The other form, gray arsenic, has a density of 5.78 g/cm3 at STP. When arsenic is heated rapidly in air, arsenic(III) oxide is formed. Although arsenic is toxic, it is needed by the human body in very small amounts. The body of a healthy human adult contains approximately 5 milligrams of arsenic. 0.005 g 4) Convert the mass of arsenic found in the body of a healthy human adult to grams. _________________ 1000 mg = 1 g 5) When heated, a 125.0-kilogram sample of arsenopyrite yields 67.5 kilograms of FeS. Determine the total mass of conservation of mass arsenic produced in this reaction. total mass of reactants = total mass of products 125.0 g = 67.5g + X X = 57.5 g As2O3 6) Write the formula for the compound produced when arsenic is heated rapidly in air. _____________________ (III) --> As+3 stock system 7) Explain, in terms of the arrangement of atoms, why the two forms of arsenic have different densities at STP. gray arsenic has particles that are more closely packed together creating a high density 8) Calculate the percent composition by mass of arsenic in arsenopyrite. Your response must include both a correct numerical setup and the calculated result. % comp by mass = mass of part x100 % comp = 74.9 g/mol x100 mass of whole 162.7 g/mol = 46% of FeAsS is As a The gram-formula mass of NO2 is defined as the mass of 9) ____ a) one mole of NO2 b) one molecule of NO2 c) two moles of NO d) two molecules of NO Regents Review – Moles 1-2 Created: February 2010 Name: ______________________ c The particles in which sample of LiCl(s) have the same average kinetic energy as the particles in a 2.0-mole 10) ____ sample of H2O(l) at 25°C? a) 1.0 mol at 75°C b) 2.0 mol at 50.°C c) 3.0 mol at 25°C d) 4.0 mol at 0°C temperature = average kinetic energy 11) Based on data collected during a laboratory investigation, a student determined an experimental value of 322 joules per gram for the heat of fusion of H2O. Calculate the student’s percent error. Your response must include a correct numerical setup and the calculated result. % error = dif. from accepted accepted x 100 = 12 J/g x 100 334 J/g = 3.59% don't forget about this equation Base your answers to questions 12 through 14 on the information below. A method used by ancient Egyptians to obtain copper metal from copper(I) sulfide ore was heating the ore in the presence of air. Later, copper was mixed with tin to produce a useful alloy called bronze. 12) Calculate the density of a 129.5-gram sample of bronze that has a volume of 14.8 cubic centimeters. Your response remember 1 mole = 22.4L must include a correct numerical setup and the calculated result. this is even easier Density = mass/volume = 129.5 g / 14.8 cm3 8.75 g/cm3 1084oC 13) Convert the melting point of the metal obtained from copper(I) sulfide ore to degrees Celsius. ______________ 0 K = -273oC 14) A 133.8-gram sample of bronze was 10.3% tin by mass. Determine the total mass of tin in the sample. Mass of part = % composition x total mass = 10.3 % x 133.8 g = 13.78 g of tin in the sample = 13.8 g b 15) ____ Which rigid cylinder contains the same number of gas molecules at STP as a 2.0-liter rigid cylinder containing H2(g) at STP? a) 1.0-L cylinder of O2(g) gases: same volume = same moles = same # of particles b) 2.0-L cylinder of CH4(g) c) 1.5-L cylinder of NH3(g) d) 4.0-L cylinder of He(g) 200g X + 88 = Given the balanced equation representing a reaction: c What is the total mass of CaO(s) that reacts completely with 88 grams of CO2(g) to produce 200. grams of 16) ____ CaCO3(s)? a) 56 g conservation of mass b) 88 g c) 112 g d) 288 g Regents Review – Moles 2-2 Created: February 2010 Name: _____________________________ b 1) ____ Which substance can be decomposed by chemical means? a) b) c) d) aluminum octane silicon xenon 2 Which equation represents an exothermic reaction at 298 K? 2) ____ d Changes in activation energy during a chemical reaction are represented by a 3) ____ a) cooling curve b) heating curve c) ionization energy diagram d) potential energy diagram Given the equation representing a reaction: b Which statement describes this reaction at equilibrium? 4) ____ a) The concentration of N2O4(g) must equal the concentration of NO2(g). b) The concentration of N2O4(g) and the concentration of NO2(g) must be constant. c) The rate of the forward reaction is greater than the rate of the reverse reaction. d) The rate of the reverse reaction is greater than the rate of the forward reaction. Given the balanced equation representing a reaction: d Which type of chemical reaction is represented by this equation? 5) ____ a) double replacement b) single replacement c) substitution d) synthesis Given the balanced equation representing a reaction: c Decreasing the concentration of Na2S2O3(aq) decreases the rate of reaction because the 6) ____ a) activation energy decreases b) activation energy increases c) frequency of effective collisions decreases d) frequency of effective collisions increases Given the equation representing a reaction at equilibrium: b Which change favors the reverse reaction? 7) ____ a) decreasing the concentration of HI(g) b) decreasing the temperature c) increasing the concentration of I2(g) d) increasing the pressure Regents Review – Reactions 1-4 Created: February 2010 Name: _____________________________ a 8) ____ Which reaction occurs spontaneously? a) b) c) d) Cl2(g) + 2NaBr(aq) ÆBr2(l) + 2NaCl(aq) Cl2(g) + 2NaF(aq) ÆF2(g) + 2NaCl(aq) I2(s) + 2NaBr(aq) ÆBr2(l) + 2NaI(aq) I2(s) + 2NaF(aq) ÆF2(g) + 2NaI(aq) b 9) ____ Which substance can not be decomposed by a chemical change? a) ammonia b) copper c) propanol d) water a 10) ____ The activation energy of a chemical reaction can be decreased by the addition of a) a catalyst b) an indicator c) electrical energy d) thermal energy c Why can an increase in temperature lead to more effective collisions between reactant particles and an 11) ____ increase in the rate of a chemical reaction? a) The activation energy of the reaction increases. b) The activation energy of the reaction decreases. c) The number of molecules with sufficient energy to react increases. d) The number of molecules with sufficient energy to react decreases. 1 12) ____ Which equation represents a decomposition reaction? Given the balanced particle-diagram equation: c Which statement describes the type of change and the 13) ____ chemical properties of the product and reactants? a) The equation represents a physical change, with the product and reactants having different chemical properties. b) The equation represents a physical change, with the product and reactants having identical chemical properties. c) The equation represents a chemical change, with the product and reactants having different chemical properties. d) The equation represents a chemical change, with the product and reactants having identical chemical properties. c What is the oxidation state of nitrogen in the compound NH4Br? 14) ____ a) –1 b) +2 c) –3 d) +4 15) Identify the element in Period 3 of the Periodic Table that reacts Na _____________ with oxygen to form an ionic compound represented by the formula X2O. ______ 16) On the potential energy diagram provided draw an arrow to represent the activation energy of the forward reaction. a In which type of reaction do two or more substances combine to 17) ____ produce a single substance? a) synthesis b) decomposition c) single replacement d) double replacement Regents Review – Reactions 2-4 Created: February 2010 Name: _____________________________ Base your answers to questions 18 through 20 on the information below. A 1.0-gram strip of zinc is reacted with hydrochloric acid in a test tube. The unbalanced equation below represents the reaction. 18) Balance the equation for the reaction of zinc and hydrochloric acid, using the smallest whole-number coefficients. 2 HCl(aq) Æ ____ H2(g) + ____ ZnCl2(aq) ____ Zn(s) + ____ 19) Explain, using information from Reference Table F, why the symbol (aq) is used to describe the product ZnCl2. ZnCl2 is soluble in water 20) Explain, in terms of collision theory, why using 1.0 gram of powdered zinc, instead of the 1.0-gram strip of zinc, would have increased the rate of the reaction. 1.0 gram of powder has more surface area for effective collisons d In which type of reaction do two lighter nuclei combine to form one heavier nucleus? 21) ____ a) combustion b) reduction c) nuclear fission d) nuclear fusion b For which compound is the process of dissolving in water exothermic? 22) ____ a) NaCl b) NaOH c) NH4Cl d) NH4NO3 b 23) ____ Which quantities must be equal for a chemical reaction at equilibrium? a) the activation energies of the forward and reverse reactions b) the rates of the forward and reverse reactions c) the concentrations of the reactants and products d) the potential energies of the reactants and products Given the balanced equation representing a reaction: c Which statement describes the energy changes in this reaction? 24) ____ a) Energy is absorbed as bonds are formed, only. b) Energy is released as bonds are broken, only. c) Energy is absorbed as bonds are broken, and energy is released as bonds are formed. d) Energy is absorbed as bonds are formed, and energy is released as bonds are broken. Given the balanced equation representing a phase change: b Which statement describes this change? 25) ____ a) It is endothermic, and entropy decreases. b) It is endothermic, and entropy increases. c) It is exothermic, and entropy decreases. d) It is exothermic, and entropy increases. Regents Review – Reactions 3-4 Created: February 2010 Name: _____________________________ a 26) ____ In a biochemical reaction, an enzyme acts as a catalyst, causing the a) b) c) d) activation energy of the reaction to decrease potential energy of the reactants to decrease kinetic energy of the reactants to increase heat of reaction to increase Base your answers to questions 27 through 30 on the information below. An experiment is performed to determine how concentration affects the rate of reaction. In each of four trials, equal volumes of solution A and solution B are mixed while temperature and pressure are held constant. The concentration of solution B is held constant, but the concentration of solution A is varied. The concentration of solution A and the time for the reaction to go to completion for each trial are recorded in the data table below. 27) Describe the relationship between the concentration of solution A and the time for the reaction to go to completion. As the concentration of solution A decreases, the reaction time increases 28) On the grid provided, mark an appropriate scale on the axis labeled “Reaction Time (s).” 29) On the same grid, plot the data from the data table. Circle and connect the points. 30) Identify one factor, other than the concentration of the solutions, that can affect the rate of this reaction. temperature, catalyst Regents Review – Reactions 4-4 Created: February 2010 1. phases of matter 6. heat transfer 2. vapor pressure 3. specific heat 4. STP 5. kinetic molecular theory 7. heat/cooling curve 8. heat of fusion & vaporization 9. combined gas law Name:_________________________________ a Standard pressure is equal to 1) ____ a) b) c) d) 1 atm 1 kPa 273 atm 273 kPa Ref. table cover c A large sample of solid calcium sulfate is crushed into smaller pieces for testing. Which two physical properties 2) ____ are the same for both the large sample and one of the smaller pieces? a) mass and density b) mass and volume c) solubility and density d) solubility and volume kinetic molecular theory c According to the kinetic molecular theory, the molecules of an ideal gas 3) ____ model of how gases behave a) have a strong attraction for each other assumptions about gases b) have significant volume c) move in random, constant, straight-line motion p. 24-26 from book d) are closely packed in a regular repeating pattern b At 65°C, which compound has a vapor pressure of 58 kilopascals? 4) ____ a) ethanoic acid reference table H b) ethanol c) propanone d) water b A person with a body temperature of 37°C holds an ice cube with a temperature of 0°C in a room where the air 5) ____ temperature is 20.°C. The direction of heat flow is heat travels from source a) from the person to the ice, only to sink (high to low) b) from the person to the ice and air, and from the air to the ice c) from the ice to the person, only d) from the ice to the person and air, and from the air to the person d At standard pressure, which element has a freezing point below standard temperature? 6) ____ a) In freezing point = melting point b) Ir c) Hf "liquid at 0oC " d) Hg The graph below represents the relationship between temperature and time as heat is added to a sample of H2O. c Which statement correctly describes the energy of the particles of the 7) ____ sample during interval BC? a) Potential energy decreases and average kinetic energy increases. b) Potential energy increases and average kinetic energy increases. c) Potential energy increases and average kinetic energy remains the same. d) Potential energy remains the same and average kinetic energy increases. 4 At STP, which 2.0-gram sample of matter uniformly fills a 340-milliliter closed container? 8) ____ (1) Br2(l) (2) Fe(NO3)2(s) uniformly filling a container, must be a gas (3) KCl(aq) (4) Xe(g) c Under which conditions of temperature and pressure would a real gas behave most like an ideal gas? 9) ____ a) 200. K and 50.0 kPa Kinetic molecular theory b) 200. K and 200.0 kPa act most ideal at high temp. and low pressure c) 600. K and 50.0 kPa act least ideal at low temp. and high pressure d) 600. K and 200.0 kPa Regents Review – Matter 1-5 Created: February 2010 Name:_________________________________ Base your answers to questions 10 through 12 on the information below. A sample of helium gas is in a closed system with a movable piston. The volume of the gas sample is changed when both the temperature and the pressure of the sample are increased. The table below shows the initial temperature, pressure, and volume of the gas sample, as well as the final temperature and pressure of the sample. 10) In the space provided, show a correct numerical setup for calculating the final volume of the helium gas sample. P1V1 T1 = P2V2 T2 (2.0)(500mL) 200 K = (7.0)(V2) 300 K ref table T V = 214 mL o 27 C 11) Convert the final temperature of the helium gas sample to degrees Celsius. _______________________ 12) Compare the total number of gas particles in the sample under the initial conditions to the total number of gas particles in the sample under the final conditions. they are the same closed container Base your answers to questions 13 through 16 on the information below. 13) On the grid provided, mark an appropriate scale on the axis labeled “Boiling Point (K).” 14) On the same grid, plot the data from the data table. Circle and connect the points. 15) Based on the data in the table, state the relationship between the boiling point at 1 atmosphere and molar mass for these four substances. As the molar mass increases, the boiling point increases. 16) State, in terms of intermolecular forces, why the boiling point of propane at 1 atmosphere is lower than the boiling point of butane at 1 atmosphere. Propane has weaker intermolecular attractions causing it to have a lower boiling point than butane. Regents Review – Matter 2-5 Created: February 2010 Name:_________________________________ Base your answers to questions 17 and 18 on the information below. At a pressure of 101.3 kilopascals and a temperature of 373 K, heat is removed from a sample of water vapor, causing the sample to change from the gaseous phase to the liquid phase. This phase change is represented by the equation below. entropy - randomness of particles 17) Explain, in terms of particle arrangement, why entropy decreases during this phase change. The entropy decrease because water has more organized particles than a gas. 18) Determine the total amount of heat released by 5.00 grams of water vapor during this phase change. q = mHv q = 5.00g x 2259 J/g q = 11295 J melting/freezing - heat of fusion vaporization/condensation - heat of vaporization Reference table cover Base your answers to questions 19 through 21 on the information below. A soft-drink bottling plant makes a colorless, slightly acidic carbonated beverage called soda water. During production of the beverage, CO2(g) is dissolved in water at a pressure greater than 1 atmosphere. The bottle containing the solution is capped to maintain that pressure above the solution. As soon as the bottle is opened, fizzing occurs due to CO2(g) being released from the solution. 19) Explain why CO2(g) is released when a bottle of soda water is opened. try to visualize the situation When the cap is released, the CO2 is released because the pressure is decreased. reference table K & L Carbonic acid 20) Write the chemical name of the acid in soda water. ________________________ 21) State the relationship between the solubility of CO2(g) in water and the temperature of the aqueous solution. As the temperature increases, the solubility will decrease. b Which type of matter is composed of two or more elements that are chemically combined in a fixed proportion? 22) ____ a) solution solids - increase temp = inc solubility b) compound gases - increase temp = dec. solubility c) homogeneous mixture d) heterogeneous mixture gas - dec. pressure = dec. solubility d Particles are arranged in a crystal structure in a sample of 23) ____ a) H2(g) b) Br2(l) c) Ar(g) d) Ag(s) b Matter is classified as a 24) ____ a) substance, only b) substance or as a mixture of substances c) homogenous mixture, only d) homogenous mixture or as a heterogeneous mixture Regents Review – Matter 3-5 Created: February 2010 Name:_________________________________ a A beaker contains both alcohol and water. These liquids can be separated by distillation because the liquids have different 25) ____ a) b) c) d) boiling points densities particle sizes solubilities forcing a liquid to change to a gas liquids of different boiling points can be separated by distillation c Which term is defined as a measure of the average kinetic energy of the particles in a sample of matter? 26) ____ a) activation energy b) potential energy c) temperature d) entropy c Under which conditions of temperature and pressure does a sample of neon behave most like an ideal gas? 27) ____ a) 100 K and 0.25 atm high temp. & low pressure b) 100 K and 25 atm creates the most space for particles c) 400 K and 0.25 atm d) 400 K and 25 atm b According to the kinetic molecular theory, which statement describes the particles in a sample of an ideal gas? 28) ____ a) The force of attraction between the gas particles is strong. b) The motion of the gas particles is random and straight-line. c) The collisions between the gas particles cannot result in a transfer of energy between the particles. d) The separation between the gas particles is smaller than the size of the gas particles themselves. c Which statement describes the transfer of heat energy that occurs when an ice cube is added to an insulated 29) ____ container with 100 milliliters of water at 25°C? source to sink a) Both the ice cube and the water lose heat energy. b) Both the ice cube and the water gain heat energy. c) The ice cube gains heat energy and the water loses heat energy. d) The ice cube loses heat energy and the water gains heat energy. c Which quantity of heat is equal to 200. joules? 30) ____ a) 20.0 kJ b) 2.00 kJ 1000 joules in a kilojoule c) 0.200 kJ d) 0.0200 kJ 4 Which graph represents the relationship between pressure and volume for a sample of an ideal gas at constant 31) ____ temperature? compressing a syringe c The entropy of a sample of H2O increases as the sample changes from a 32) ____ a) gas to a liquid solids - lowest entropy b) gas to a solid gases - highest entropy c) liquid to a gas d) liquid to a solid a Which statement describes the particles of an ideal gas based on the kinetic molecular theory? 33) ____ a) The gas particles are relatively far apart and have negligible volume. p. 24-26 in book b) The gas particles are in constant, nonlinear motion. c) The gas particles have attractive forces between them. d) The gas particles have collisions without transferring energy. Regents Review – Matter 4-5 Created: February 2010 Name:_________________________________ c Under which conditions of temperature and pressure would a 1-liter sample of a real gas behave most like an ideal gas? 34) ____ a) b) c) d) 100 K and 0.1 atm 100 K and 10 atm 500 K and 0.1 atm 500 K and 10 atm high temp - low pressure d Which type of energy is associated with the random motion of the particles in a sample of gas? 35) ____ a) chemical energy b) electromagnetic energy c) nuclear energy d) thermal energy = heat d At STP, a 7.49-gram sample of an element has a volume of 1.65 cubic centimeters. The sample is most likely 36) ____ a) Ta b) Tc = mass/ volume density c) Te 7.49/1.65 = 4.54 g/cm3 reference table S d) Ti b What occurs when a 35-gram aluminum cube at 100.°C is placed in 90. grams of water at 25°C in an insulated cup? 37) ____ a) Heat is transferred from the aluminum to the water, and the temperature of the water decreases. b) Heat is transferred from the aluminum to the water, and the temperature of the water increases. c) Heat is transferred from the water to the aluminum, and the temperature of the water decreases. d) Heat is transferred from the water to the aluminum, and the temperature of the water increases. a Which temperature is equal to 120. K? 38) ____ a) 153°C 0oC = 273K b) 120.°C c) 293°C X = 120K d) 393°C d A rigid cylinder contains a sample of gas at STP. What is the pressure of this gas after the sample is heated to 39) ____ 410 K? @ STP temp. = 273K a) 1.0 atm pressure = 1.0 atm b) 0.50 atm c) 0.67 atm d) 1.5 atm inc. heat = inc. pressure Base your answers to questions 40 through 42 on the information below. A phase change for carbon dioxide that occurs spontaneously at 20.°C and 1.0 atmosphere is represented by the balanced equation below. sublimation 40) Write the name of this phase change. _________________________ 41) Describe what happens to the potential energy of the CO2 molecules as this phase change occurs. the potential energy will increase 42) In the space provided, use the key to draw at least five molecules in the box to represent CO2 after this phase change is completed. mixture - two or more substances not combined - can be separated heterogeneous and homogeneous compound - two or more elements chemically combined in a definite ratio Regents Review – Matter 5-5 Created: February 2010 1. metals, nonmetals & metalloids 2. groups and periods 3. atomic radius Name: _______________________ d 1) ____ Which element has the greatest density at STP? 4. atoms v. ions 5. ionization energy a) barium Table S b) beryllium 6. electronegativity c) magnesium 7. Reference tables - periodic table & table S d) radium c Which element is a metalloid? 2) ____ a) Al B, Si, Ge, As, Sb, Te b) Ar c) As d) Au c An element that is malleable and a good conductor of heat and electricity could have an atomic number of 3) ____ a) 16 definition of a metal b) 18 c) 29 d) 35 a An atom of an element has a total of 12 electrons. An ion of the same element has a total of 10 electrons. 4) ____ Which statement describes the charge and radius of the ion? are you positive a) The ion is positively charged and its radius is smaller than the radius of the atom. b) The ion is positively charged and its radius is larger than the radius of the atom. you lost the c) The ion is negatively charged and its radius is smaller than the radius of the atom. smaller cat d) The ion is negatively charged and its radius is larger than the radius of the atom. d Magnesium and calcium have similar chemical properties because a magnesium atom and a calcium atom 5) ____ have the same a) atomic number groups have the same # of valence eb) mass number c) total number of electron shells d) total number of valence electrons c Which statement describes a chemical property of bromine? 6) ____ a) Bromine is soluble in water. b) Bromine has a reddish-brown color. c) Bromine combines with aluminum to produce AlBr3. d) Bromine changes from a liquid to a gas at 332 K and 1 atm. physical properties d An atom of aluminum in the ground state and an atom of gallium in the ground state have the same 7) ____ a) mass same group b) electronegativity c) total number of protons d) total number of valence electrons b Which element has the greatest density at STP? 8) ____ a) scandium b) selenium c) silicon d) sodium ESRT d A sample of an element is malleable and can conduct electricity. This element could be 9) ____ a) H b) He c) S d) Sn Regents Review_ Periodic Table 1-2 Created: February 2010 Name: _______________________ b Which general trend is demonstrated by the Group 17 elements as they are considered in order from top to 10) ____ bottom on the Periodic Table? ionization energy dec. a) a decrease in atomic radius down a electronegativiy dec. b) a decrease in electronegativity group c) an increase in first ionization energy atomic radius inc. d) an increase in nonmetallic behavior d Which element is a liquid at 758 K and standard pressure? 11) ____ a) gold 1338 if temp. is higher than b) silver 1235 melting point --> liquid 2045 c) platinum 577 d) thallium metallic character inc. across a period ionization energy inc. electronegativity inc. atomic radius dec. metallic character dec. a An element that has a low first ionization energy and good conductivity of heat and electricity is classified as a 12) ____ a) metal def of metal b) metalloid c) nonmetal d) noble gas c The chemical properties of calcium are most similar to the chemical properties of 13) ____ a) Ar b) K same group c) Mg d) Sc b Which element is a liquid at STP? 14) ____ a) argon b) bromine group 17 shows all three phases of matter c) chlorine d) sulfur b Which statement describes a chemical property of aluminum? 15) ____ a) Aluminum is malleable. physical properties b) Aluminum reacts with sulfuric acid. c) Aluminum conducts an electric current. d) Aluminum has a density of 2.698 g/cm3 at STP. a Which element has an atom in the ground state with a total of three valence electrons? 16) ____ a) aluminum b) lithium group 13 c) phosphorus d) scandium b As atomic number increases within Group 15 on the Periodic Table, atomic radius 17) ____ a) decreases, only b) increases, only down a group each element c) decreases, then increases d) increases, then decreases has additional energy levels making them larger Regents Review_ Periodic Table 2-2 Created: February 2010 1. bonds between atoms 2. Ionic v. covalent Name: ______________________ 3. polar v. nonpolar molecules a Which formula represents a nonpolar molecule? 1) ____ a) b) c) d) CH4 HCl H2O NH3 4. ions forming bonds 5. Molecular v. empirical formula 6. Diatomic molecules 7. intermolecular attractions 8. dot diagrams symmetrical = nonpolar asymmetrical = polar c The compound XCl is classified as ionic if X represents the element 2) ____ a) H b) I ionic bonds form neutral compounds c) Rb Which group has a +1 charge? X+?Cl-1 --> X+1Cl-1 d) Br c The chemical bonding in sodium phosphate, Na3PO4, is classified as 3) ____ a) ionic, only Metal + polyatomic ion b) metallic, only covalent ionic c) both covalent and ionic d) both covalent and metallic d Which element is composed of molecules that each contain a multiple covalent bond? 4) ____ a) chlorine N2 N N N N b) fluorine c) hydrogen d) nitrogen c What is the empirical formula for a compound with the molecular formula C6H12Cl2O2? 5) ____ a) CHClO b) CH2ClO empirical formula = simplest whole number ratio c) C3H6ClO d) C6H12Cl2O2 b Which two particle diagrams represent mixtures of 6) ____ diatomic elements? seven that make a seven a) A and B b) A and C plus hydrogen c) B and C N2, O2, F2, d) B and D Cl2, Br2, I2 & H2 c Which statement describes oxygen gas, O2(g), and ozone gas, O3(g)? 7) ____ a) They have different molecular structures, only. b) They have different properties, only. c) They have different molecular structures and different properties. d) They have the same molecular structure and the same properties. allotropes same element two different structures a Which type of substance can conduct electricity in the liquid phase but not in the solid phase? 8) ____ ionic has free moving ions in the a) ionic compound b) molecular compound liquid phase and when dissolved c) metallic element d) nonmetallic element 9) a Why is a molecule of CO2 nonpolar even though the bonds between the carbon atom and the oxygen atoms are polar? ____ a) b) c) d) The shape of the CO2 molecule is symmetrical. The shape of the CO2 molecule is asymmetrical. The CO2 molecule has a deficiency of electrons. The CO2 molecule has an excess of electrons. Regents Review _ Bonding 1-3 Created: February 2010 Name: ______________________ a Which formula represents a molecular compound? 10) ____ a) b) c) d) HI KI KCl LiCl molecular compounds are covalently bonded a The relatively high boiling point of water is due to water having 11) ____ a) hydrogen bonding stronger intermolecular attractions b) metallic bonding causes higher melting and boiling points c) nonpolar covalent bonding d) strong ionic bonding 2 A compound has the empirical formula CH2O and a gram-formula mass of 60. grams per mole. What is the 12) ____ molecular formula of this compound? empirical formula = 30 60/30 = 2 d Which formula represents strontium phosphate? 13) ____ a) SrPO4 PO4-3 Sr+2 b) Sr3PO8 +6 + -6 = 0 c) Sr2(PO4)3 d) Sr3(PO4) Sr (PO ) dot diagrams for ionic bonds have [] 4 Which Lewis electron-dot diagram represents calcium oxide? 14) ____ 3 4 2 15) ____ d Which formula represents a nonpolar molecule? a) HCl b) H2O c) NH3 d) CH4 b Which element has an atom with the greatest tendency to attract electrons in a chemical bond? 16) ____ a) carbon b) chlorine c) silicon electronegativity d) sulfur c The nitrogen atoms in a molecule of N2 share a total of 17) ____ a) one pair of electrons b) one pair of protons each bond shares a pair of electrons total 6ec) three pairs of electrons d) three pairs of protons a An ionic compound is formed when there is a reaction between the elements 18) ____ a) strontium and chlorine b) hydrogen and chlorine ionic bond --> metal + nonmetal c) nitrogen and oxygen d) sulfur and oxygen a Which compound has both ionic and covalent bonding? 19) ____ a) CaCO3 metal + polyatomic ion b) CH2Cl2 c) CH3OH d) C6H12O6 Regents Review _ Bonding 2-3 Created: February 2010 Name: ______________________ b The liquids hexane and water are placed in a test tube. The test tube is stoppered, shaken, and placed in a test tube rack. 20) ____ The liquids separate into two distinct layers because hexane and water have different a) formula masses b) molecular polarities "like dissolves like" -c) pH values d) specific heats 21) _c ___ Hydrogen bonding is a type of a) strong covalent bond b) weak ionic bond c) strong intermolecular force d) weak intermolecular force polar dissolve polar polar covalent bond -- unequal sharing nonpolar covalent bond -- diatomics, equally sharing electrons ** greater difference the bond will be more polar c Which formula represents copper(I) oxide? 22) ____ a) CuO b) CuO2 c) Cu2O d) Cu2O2 Cu+1 O-2 +2 + -2 = 0 Cu2O c Which element, represented by X, reacts with fluorine to produce the compound XF2? 23) ____ a) aluminum X+? F-1 b) argon +1 -1(2) +2 -2 = 0 c) magnesium d) sodium MgF +2 --> group 2 metal 2 Base your answers to questions 24 through 26 on the information below. At STP, iodine, I2, is a crystal, and fluorine, F2, is a gas. Iodine is soluble in ethanol, forming a tincture of iodine. A typical tincture of iodine is 2% iodine by mass. 24) Compare the strength of the intermolecular forces in a sample of I2 at STP to the strength of the intermolecular forces both nonpolar - Vanderwaals force increases with in a sample of F2 at STP. F2 has weaker intermolecular forces molecule size - I2 is larger than F2 25) In the space provided, draw a Lewis electron-dot diagram for a molecule of I2. 25) 26) Determine the total mass of I2 in 25 grams of this typical tincture of iodine. 26) mass = total mass x % = 25 g x 2% = 0.5 g Iodine is 2% of the total mass Base your answers to questions 27 through 29 on the information below. Carbon has three naturally occurring isotopes, C-12, C-13, and C-14. Diamond and graphite are familiar forms of solid carbon. Diamond is one of the hardest substances known, while graphite is a very soft substance. Diamond has a rigid network of bonded atoms. Graphite has atoms bonded in thin layers that are held together by weak forces. Recent experiments have produced new forms of solid carbon called fullerenes. One fullerene, C60, is a spherical, cagelike molecule of carbon. 27) Determine both the total number of protons and the total number of neutrons in an atom of the naturally occurring carbon isotope with the largest mass number. C-14 8 neutrons Neutrons: _______________ 6 protons Protons _______________ covalent 28) Identify the type of bonding in a fullerene molecule. ______________________ 29) State, in terms of the arrangement of atoms, the difference in hardness between diamond and graphite. Diamond has stronger forces of attraction between atoms. Regents Review _ Bonding 3-3 Created: February 2010 1. intermolecular attractions and boiling point 2. Polar and nonpolar solutions and miscibility 3. freezing and boiling points and conc. of solution 4. Molarity equation 5. concentration calc. (ppm) 6. solubility chart Table F 7. solubility curves Table G Name: ____________________________ b Compared to the freezing point and boiling point of water at 1 atmosphere, a solution of a salt and water at 1 1) ____ atmosphere has a a) lower freezing point and a lower boiling point b) lower freezing point and a higher boiling point c) higher freezing point and a lower boiling point d) higher freezing point and a higher boiling point inc. concentration causes the freezing point decreases, and boiling point increases d How do the boiling point and freezing point of a solution of water and calcium chloride at standard pressure 2) ____ compare to the boiling point and freezing point of water at standard pressure? a) Both the freezing point and boiling point of the solution are higher. b) Both the freezing point and boiling point of the solution are lower. c) The freezing point of the solution is higher and the boiling point of the solution is lower. d) The freezing point of the solution is lower and the boiling point of the solution is higher. c Which substance is an electrolyte? 3) ____ a) CCl4 b) C2H6 electrolyte - conducts electricity b/c it has c) HCl free moving ions - ionic d) H2O a What is the total mass of solute in 1000. grams of a solution having a concentration of 5 parts per million? 4) ____ a) 0.005 g b) 0.05 g reference table - back cover c) 0.5 g d) 5 g a Which compound is least soluble in water at 60.°C? 5) ____ a) KClO3 b) KNO3 reference table - G c) NaCl d) NH4Cl b 6) ____ Which sample of HCl(aq) contains the greatest number of moles of solute particles? a) 1.0 L of 2.0 M HCl(aq) largest volume with the b) 2.0 L of 2.0 M HCl(aq) c) 3.0 L of 0.50 M HCl(aq) greatest concentration d) 4.0 L of 0.50 M HCl(aq) d What is the mass of NH4Cl that must dissolve in 200. grams of water at 50.°C to make a saturated solution? 7) ____ a) 26 g b) 42 g c) 84 g reference table G d) 104 g c Which solution has the highest boiling point at standard pressure? 8) ____ 2 ions a) 0.10 M KCl(aq) b) 0.10 M K2SO4(aq) 3 ions greater number of impurities = higher boiling poit 4 ions c) 0.10 M K3PO4(aq) K3PO4 --> 3K+ + PO4-3 d) 0.10 M KNO3(aq) 2 ions a What is the molarity of 1.5 liters of an aqueous solution that contains 52 grams of lithium fluoride, LiF, (gram9) ____ formula mass = 26 grams/mole)? 2 step problem a) 1.3 M moles = 2 moles/1.5L b) 2.0 M molarity = moles/liter c) 3.0 M = 1.3 M d) 0.75 M Regents Review – Solutions moles = mass/gfm = 52 g / 26 g/mole 1-2 = 2 moles Created: February 2010 Name: ____________________________ Base your answers to questions 10 through 14 on the information to the below. Bond energy is the amount of energy required to break a chemical bond. The table below gives a formula and the carbon-nitrogen bond energy for selected nitrogen compounds. 10) Describe, in terms of electrons, the type of bonding between the carbon atom and the nitrogen atom in a molecule of methanamine. C-N bond 3 pair 2 pair Carbon and nitrogen share electrons creating a covalent bond 11) Identify the noble gas that has atoms in the ground state with the same electron configuration as the nitrogen in a molecule Ne - neon of isocyanic acid. _______________________ N - 7 electrons + 3e- 1 pair = 10 electrons neon 12) State the relationship between the number of electrons in a carbon-nitrogen bond and carbon-nitrogen bond energy. As the number of electrons in the carbon-nitrogen bond decreases, the bond energy decreases 13) Explain, in terms of charge distribution, why a molecule of hydrogen cyanide is polar. "Saturday Night Party" hydrogen cyanide has asymetrical charge distribution 14) A 3.2-gram sample of air contains 0.000 74 gram of hydrogen cyanide. Determine the concentration, in parts per reference back cover million, of the hydrogen cyanide in this sample. ppm = 0.00074 g of Hydrogen cyanide/3.2 g of air x 1,000,000 = 231 or 230 15) Based on Table G, determine the total mass of NH3 that must be dissolved in 200. grams of water to produce a 110 g saturated solution at 20.°C.______________________ Base your answers to questions16 and 17 on the information below. The dissolving of solid lithium bromide in water is represented by the balanced equation below. 16) Calculate the total mass of LiBr(s) required to make 500.0 grams of an aqueous solution of LiBr that has a concentration of 388 parts per million. Your response must include both a correct numerical setup and the calculated result. 388 ppm = x/500 x 1,000,000 0.194 g 17) Based on Table F, identify one ion that reacts with Br ions in an aqueous solution to form an insoluble compound. Ag+, Pb2+, Hg22+ _____________________________ a precipitate will form Regents Review – Solutions 2-2 Created: February 2010 1. LEO goes GER 2. oxidation states 3. half reactions 4. Electrochemical cells - voltaic and electrolytic 4. AN OX, RED CAT 5. table Name:_______________________________ Given the balanced equation representing a reaction: c During this reaction, the oxidation number of Fe changes from 1) ____ a) +2 to 0 as electrons are transferred b) +2 to 0 as protons are transferred c) +3 to 0 as electrons are transferred d) +3 to 0 as protons are transferred Base your answers to questions 2 through 4 on the information below. A voltaic cell with magnesium and copper electrodes is shown in the diagram below. The copper electrode has a mass of 15.0 grams. When the switch is closed, the reaction in the cell begins. The balanced ionic equation for the reaction in the cell is shown below the cell diagram. After several hours, the copper electrode is removed, rinsed with water, and dried. At this time, the mass of the copper electrode is greater than 15.0 grams. 2) State the direction of electron flow through the wire between the electrodes when the switch is closed. Mg is oxidized electrons will travel from Mg to Cu 3) State the purpose of the salt bridge in this cell. keep the solutions neutral 4) Explain, in terms of copper ions and copper atoms, why the mass of the copper electrode increases as the cell operates. Your response must include information about both copper ions and copper atoms. Copper electrode increases because copper ions are attracted to the electrode where they gain electrons and form copper atoms Base your answers to questions 6 through 8 on the information below. In a laboratory investigation, a student constructs a voltaic cell with iron and copper electrodes. Another student constructs a voltaic cell with zinc and iron electrodes. Testing the cells during operation enables the students to write the balanced ionic equations below. 5) State evidence from the balanced equation for the cell with iron and copper electrodes that indicates the reaction in the cell is an oxidation-reduction reaction. Cu gains electrons (reductions) and Fe loses electrons (oxidation) electrons 6) Identify the particles transferred between Fe2+ and Zn during the reaction in the cell with zinc and iron electrodes. ____________ 7) Write a balanced half-reaction equation for the reduction that takes place in the cell with zinc and iron electrodes. Fe+2 + 2e- --> Fe 8) State the relative activity of the three metals used in these two voltaic cells. Zn is the most active then Fe and Cu is the least active Regent Review – Redox Reaction 1-2 Created: February 2010 Name:_______________________________ d Which substance can be broken down by chemical means? 9) ____ a) b) c) d) magnesium manganese mercury methanol d The diagram below represents an operating electrochemical cell 10) ____ and the balanced ionic equation for the reaction occurring in the cell. Which statement identifies the part of the cell that conducts electrons and describes the direction of electron flow as the cell operates? a) Electrons flow through the salt bridge from the Ni(s) to the Zn(s). b) Electrons flow through the salt bridge from the Zn(s) to the Ni(s). c) Electrons flow through the wire from the Ni(s) to the Zn(s). d) Electrons flow through the wire from the Zn(s) to the Ni(s). Base your answers to questions 11 through 13 on the information below. In a laboratory investigation, magnesium reacts with hydrochloric acid to produce hydrogen gas and magnesium chloride. This reaction is represented by the unbalanced equation below. 11) State, in terms of the relative activity of elements, why this reaction is spontaneous. Mg is more reactive than H2 12) Balance the equation, using the smallest whole-number coefficients. 2 13) Write a balanced half-reaction equation for the oxidation that occurs. Mg0 --> Mg+2 + 2e- Base your answers to questions 14 through 16 on the information below. The diagram below shows a system in which water is being decomposed into oxygen gas and hydrogen gas. Litmus is used as an indicator in the water. The litmus turns red in test tube 1 and blue in test tube 2. The oxidation and reduction occurring in the test tubes are represented by the balanced equations below. 14) Identify the information in the diagram that indicates this system is an electrolytic cell. an electrical source is required to cause the reaction -2 --> 0 _______ 15) Determine the change in oxidation number of oxygen during the reaction in test tube 1. _______________ 16) Explain, in terms of the products formed in test tube 2, why litmus turns blue in test tube 2. OH- ions are produced in test tube 2 which is a base causing litmus to turn blue Regent Review – Redox Reaction 2-2 Created: February 2010 1. arrhenius definition of an acid and base 2. Bronsted-Lowry definition 3. neutralization equation 3. reactant/products of neutralization 4. indicators 5. pH scale and strength 6. naming acids & bases Name: _________________________________ a Which word equation represents a neutralization reaction? 1) ____ a) base + acid Æsalt + water definition b) base + salt Æwater + acid c) salt + acid Æbase + water d) salt + water Æacid + base d An aqueous solution of lithium hydroxide contains hydroxide ions as the only negative ion in the solution. Lithium 2) ____ hydroxide is classified as an a) aldehyde b) alcohol definition c) Arrhenius acid d) Arrhenius base a One alternate acid-base theory states that an acid is an 3) ____ + a) H donor b) H+ acceptor Bronsted-Lowry c) OH−donor − d) OH acceptor B A A D b Which substance is always a product when an Arrhenius acid in an aqueous solution reacts with an Arrhenius 4) ____ base in an aqueous solution? a) HBr neutralization reaction b) H2O water and salt are product c) KBr d) KOH d Which change in pH represents a hundredfold increase in the concentration of hydronium ions in a solution? 5) ____ a) pH 1 to pH 2 100X more acidic b) pH 1 to pH 3 c) pH 2 to pH 1 10X scale d) pH 3 to pH 1 b Which indicator would best distinguish between a solution with a pH of 3.5 and a solution with a pH of 5.5? 6) ____ a) bromthymol blue b) bromcresol green Reference table M c) litmus d) thymol blue Given the equation: b Which ion is represented by X? 7) ____ a) hydroxide b) hydronium c) hypochlorite d) perchlorate hydronium = H3O+ Base your answers to questions 8 and 9 on the information below. In performing a titration, a student adds three drops of phenolphthalein to a flask containing 25.00 milliliters of HCl(aq). Using a buret, the student slowly adds 0.150 M NaOH(aq) to the flask until one drop causes the indicator to turn light pink. The student determines that a total volume of 20.20 milliliters of NaOH(aq) was used in this titration. 3 8) The concentration of the NaOH(aq) used in the titration is expressed to what number of significant figures? ______ 9) Calculate the molarity of the HCl(aq) used in this titration. Your response must include both a correct numerical setup and the calculated result. Ma X Regents Review – Acids & Bases Ma X Va = Mb X 25.00mL = 0.150M X = 0.121 M 1-2 Vb X 20.20mL Created: February 2010 Name: _________________________________ b One acid-base theory defines a base as an 10) ____ a) H+donor b) H+ acceptor BAAD rule - Bronsted Lowry c) H+ donor + BAAD -Bases Accept Acid Donate d) H acceptor 11) A student completes a titration by adding 12.0 milliliters of NaOH(aq) of unknown concentration to 16.0 milliliters of 0.15 M HCl(aq). What is the molar concentration of the NaOH(aq)? 0.15M Ma X Va = Mb X X 16.00mL = Mb Mb = 0.20 M Vb X 12.0mL Base your answers to questions 12 through 14 on the information below. A student used blue litmus paper and phenolphthalein paper as indicators to test the pH of distilled water and five aqueous household solutions. Then the student used a pH meter to measure the pH of the distilled water and each solution. The results of the student’s work are recorded in the table below. 12) Identify the liquid tested that has the lowest hydronium ion concentration. household ammonia ____________________________ strongest base 13) Explain, in terms of the pH range for color change on Reference Table M, why litmus is not appropriate to differentiate the acidity levels of tomato juice and vinegar. both substances have pH values below that of the activation range of litmus 14) Based on the measured pH values, identify the liquid tested that is 10 times more acidic than vinegar. c The data collected from a laboratory titration are used to calculate the 15) ____ a) rate of a chemical reaction b) heat of a chemical reaction MaVa = MbVb c) concentration of a solution d) boiling point of a solution pH = 2.3 c When one compound dissolves in water, the only positive ion produced in the solution is H3O(aq). This 16) ____ compound is classified as a) a salt b) a hydrocarbon c) an Arrhenius acid d) an Arrhenius base d Which salt is produced when sulfuric acid and calcium hydroxide react completely? 17) ____ a) CaH2 H2SO4 b) CaO CaOH c) CaS d) CaSO4 CaSO + HO 4 Regents Review – Acids & Bases neutralization 2 2-2 Created: February 2010 1. Alkanes, Alkenes, Alkynes 2. bonding and molecular properties of hydrocarbons 3. sat. v. unsaturated 4. functional groups: alcohols, acids, halides, esters, ethers, ketones, amines, amides 5. isomers 6. organic - polymerization, saponification, halogenation, combustion, esterification, fermentation Name:reaction _____________________________ b 1) ____ Which compound is a saturated hydrocarbon? a) propanal saturated hydrocarbons have all single bonds - alkanes b) propane unsaturated have at least one double or triple bond c) propene d) propyne alkenes, alkynes b The isomers butane and methylpropane differ in their 2) ____ a) molecular formulas isomers - different structure same b) structural formulas c) total number of atoms per molecule molecular formula d) total number of bonds per molecule a Which particle has the greatest mass? 3) ____ a) an alpha particle not b) a beta particle organicc) a neutron d) a positron d A beta particle may be spontaneously emitted from 4) ____ a) a ground-state electron b) a stable nucleus c) an excited electron after the 2nd carbon d) an unstable nucleus double bond 4 Which formula represents 2-butene? 5) ____ Base your answers to questions 6 through 8 on the information below. During a bread-making process, glucose is converted to ethanol and carbon dioxide, causing the bread dough to rise. Zymase, an enzyme produced by yeast, is a catalyst needed for this reaction. 6) Balance the equation provided for the reaction that causes bread dough to rise, using the smallest whole-number coefficients. 2 2 7) In the space provided draw a structural formula for the alcohol formed in this reaction. 7) H H H - C - C -OH 8) State the effect of zymase on the activation energy for this reaction. zymase is a catalyst H H 8) Zymase lowers the activation energy. c A straight-chain hydrocarbon that has only one double bond in each molecule has the general formula 9) ____ a) CnH2n−6 b) CnH2n−2 alkene - general formulas c) CnH2n reference table Q d) CnH2n+2 Regents review – Organic Chemistry 1-1 Created: April 2008 polymerization - connecting small molecules saponification - fat and base make soap Name: _____________________________ esterification - acid and alcohol d Which reaction results in the production of soap? halogenation - hydrocarbon and halogen 10) ____ combustion - hydrocarbon and oxygen produce a) esterification b) fermentation carbon dioxide and energy c) polymerization fermentation - glucose and enzyme produce d) saponification CO2 and alcohol a Ethanol and dimethyl ether have different chemical and physical properties because they have different 11) ____ a) b) c) d) functional groups molecular masses numbers of covalent bonds percent compositions by mass one is an alcohol and the other is an ether isomers 1 Which formula represents an unsaturated hydrocarbon? 12) ____ Base your answers to questions 13 through 17 on the information below. Biodiesel is an alternative fuel for vehicles that use petroleum diesel. Biodiesel is produced by reacting vegetable oil with CH3OH. Methyl palmitate, C15H31COOCH3, a compound found in biodiesel, is made from soybean oil. One reaction of methyl palmitate with oxygen is represented by the balanced equation below. methanol 13) Write an IUPAC name for the compound that reacts with vegetable oil to produce biodiesel.___________________ 14) Explain, in terms of both atoms and molecular structure, why there is no isomer of CH3OH. The atoms can not be rearranged to created any different molecular structure. reference table R ester 15) Identify the class of organic compounds to which methyl palmitate belongs. .___________________ combustion reaction 16) Identify the type of organic reaction represented by the balanced equation. .___________________ 17) State evidence from the balanced equation that indicates the reaction is exothermic. energy is a product a What is the empirical formula of a compound that has a carbon-to-hydrogen ratio of 2 to 6? 18) ____ a) CH3 b) C2H6 c) C3H d) C6H2 C4H9COOH Given the formula for an organic compound: d This compound is classified as an 19) ____ a) aldehyde b) amine c) ester d) organic acid Regents review – Organic Chemistry 2-2 Created: April 2008 Name: _____________________________ a Butanal and butanone have different chemical and physical properties primarily because of differences in their 20) ____ a) b) c) d) functional groups molecular masses molecular formulas number of carbon atoms per molecule functional groups determine the properties of organic molecuels Base your answers to questions 21 through 23 on the information below. The formula below represents a hydrocarbon. alkane,alkene, alkyne alkane 21) Identify the homologous series to which this hydrocarbon belongs. ________________ 22) Explain, in terms of carbon-carbon bonds, why this hydrocarbon is saturated. all carbon atoms are bonded to another carbon atom with a single bond 23) In the space provided, draw a structural formula for one isomer of this hydrocarbon. Regents review – Organic Chemistry 3-3 Created: April 2008 1. transmutation 2. nuclear notation 3. emission particles 4. Fusion and Fission 5. Natural v. artificial transmutation 6. common uses of radioisotopes Name: __________________________ 4 Which particle has the least mass? 1) ____ mass number of protons d Which nuclide is used to investigate human thyroid gland disorders? 2) ____ a) carbon-14 b) potassium-37 c) cobalt-60 d) iodine-131 d 3) ____ A change in the nucleus of an atom that converts the atom from one element to another element is called a) combustion b) neutralization definition c) polymerization d) transmutation 2 4) ____ Which particle is emitted from a hydrogen-3 nucleus when it undergoes radioactive decay? reference table N Base your answers to questions 5 through 7 on the information below. Cobalt-60 is commonly used as a source of radiation for the prevention of food spoilage. Bombarding cobalt-59 nuclei with neutrons produces the nuclide cobalt-60. A food irradiation facility replaces the cobalt-60, a source of gamma rays, when the radioactivity level falls to of its initial level. The nuclide cesium-137 is also a source of radiation for the prevention of food spoilage. reference table N beta particle 5) Identify one emission spontaneously released by a cobalt-60 nucleus. ___________________ 6) Determine the total number of years that elapse before an original cobalt-60 source in an irradiation facility must be replaced. 1-1/2-1/4-1/8 (3-half lives) 3 x 5.26y = 15.78 y 7) Complete the nuclear equation provided for the decay of cesium-137. Your response must include the symbol, atomic number, and mass number of the missing particle. top numbers must equal 137 Ba 56 bottom numbers must equal b What is the half-life of a radioisotope if 25.0 grams of an original 200.-gram sample of the isotope remains 8) ____ unchanged after 11.46 days? 200 --> 100 --> 50 --> 25 a) 2.87 d b) 3.82 d 11.46/3 = 3.82 d c) 11.46 d d) 34.38 d Base your answers to questions 80 and 81 on the information below. Scientists are investigating the production of energy using hydrogen-2 nuclei (deuterons) and hydrogen-3 nuclei (tritons). The balanced equation below represents one nuclear reaction between two deuterons. 9) State, in terms of subatomic particles, how a deuteron differs from a triton. deuteron has 1 neutron and a mass of 2 triton has 2 neutrons and a mass of 3 fusion 10) Identify the type of nuclear reaction represented by the equation._______________________ Regents Review _ Nuclear Energy 1-2 Created: February 2010 light nuclei combining to form heavier nuclei Name: __________________________ 11) ____ Which nuclear emission has the greatest mass and the least penetrating power? a) b) c) d) an alpha particle a beta particle a neutron a positron 12) ____ Which radioisotope has an atom that emits a particle with a mass number of 0 and a charge of 1? a) 3H beta b) 16N beta c) 19Ne positron d) 239Pu alpha 13) ____ In which type of reaction do two lighter nuclei combine to form one heavier nucleus? a) combustion definition - fusion b) reduction c) nuclear fission d) nuclear fusion 14) ____ Which radioisotope is used to treat thyroid disorders? a) Co-60 b) I-131 c) C-14 d) U-238 15) Determine the total time that must elapse until only ¼ of an original sample of the radioisotope Rn-222 remains 7.74 days unchanged. ______________ 1 --> 1/2 --> 1/4 = 2 1/2 life periods 2 x 3.82 days = 7.74 days Base your answers to questions 16 through 18 on the information below. Hydrocarbons and fissionable nuclei are among the sources used for the production of energy in the United States. A chemical reaction produces much less energy than a nuclear reaction per mole of reactant. The balanced chemical equation below represents the reaction of one molecule of a hydrocarbon with two molecules of oxygen. The nuclear equation below represents one of the many possible reactions for one fissionable nucleus. In this equation, X represents a missing product. combustion 16) Identify the type of organic reaction represented by the chemical equation. ________________________ 17) On the labeled axes provided, draw a potential energy diagram for the reaction of the hydrocarbon with oxygen. exothermic 1 + 235 = 89 + X + 1 x= 146 0 X = 56 + 92 = 36 + X + 0 18) Write an isotopic notation for the missing product represented by X in the nuclear equation. Regents Review _ Nuclear Energy 2-2 146 Ba 56 Created: February 2010