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AP CHEMISTRY FALL SEMESTER EXAM REVIEW 90 minute MC Section + 20 minute FRQUnit 2: Reactions and Aqueous SolutionsComplete combustion of a sample of a hydrocarbon in excess oxygen produces equimolar quantities of carbon dioxide and water. What could be the molecular formula of the compound?If the mass percent of an element in a pure sample is given, be able to determine why another given sample is at a lower mass percent of the element. If you have two beakers of the same volume with different compounds and you combine them into one beaker, be able to predict what concentrations of each compound would give a precipitate. When given different compounds, be able to identify which one would be an isomer, dissolves in acidic/basic solutions, and solubility in water.Calculate molarity of one ion if another ion’s concentration is given when dissolved in water.Know weak/strong acids/bases Identify oxidizing and reducing agents. Be able to calculate the amount of moles produced from combing two molecules.Write a net ionic equationSolubility rulesCalculate mole fractionCalculate empirical formulaWhat do you rinse a buret with before you do a titration?Know how to calculate the amount of water needed to make a dilution.Calculate percent yield.Predict solubility of salts in water.What piece of laboratory glassware is needed for preparing a certain volume of an aqueous solution from a solid.Unit 3: Gas LawsDraw a particulate showing the formation of water vapor from hydrogen gas and oxygen gas in a rigid container.If given the molar mass, temperature and pressure of a gas, be able to:Calculate the average kinetic energy of a gas moleculeCalculate the density of a gasIf the pressure of each gas is increased at constant temperature until condensation occurs, which gaswill condense at the lowest pressure? Highest pressure?If different containers of different gases have the same volume and temperature, be able to find the total pressure once they are all combined if the ratio of atoms is given.If a reaction were to go to completion, know how to calculate the total pressure in the container.Based on temperature and pressure of different molecules, be able to determine which one behaves most like an ideal gas and lowest/highest root mean square.Gas Law calculations (Boyles, Charles, Gay-Lussac, Ideal) Calculate number of moles produced in a gas collection tube.Gas Lab: what measurements were needed to be able to calculate the molar mass of the gas?Be able to calculate vapor pressure of a substance when given the mole fraction and vapor pressure of water.Unit 4: Atomic Structure and PeriodicityWhen given ionic radius, be able to predict relative strength of the ion’s attraction to water and why.If there is a mixture of two elements with similar average atomic masses, be able to know what would happen if you ran them through a mass spectrometer. How would you determine if a different sample was purely one element?What would explain why one molecule can absorb UV but not visible light and another molecule could absorb both?When comparing two different element’s PES, be able to explain why one peak comes before another.Based on periodic trends, be able to predict the atomic radius and first ionization of an element when given the same information for other elements.Know periodic trends for electronegativity, first-ionization energy, atomic radius.Unit 5: BondingLewis electron-dot diagrams, molecular geometry, bond angle and polarity Predict the hybridization of a compound.Unit 6: States of Matter, IMF, SolutionsBe able to rank liquids based on IMF when given vapor pressureBe able to identify hydrogen bonding in water.Explain why two molecules of different elements would have different boiling points (ie. type of solid, type of bond, polarity, IMFs, electronegativity)The dissolution of an ionic solute in a polar solvent can be imagined as occurring in three steps. In step 1, the separation between ions in the solute is greatly increased, just as will occur when the solute dissolves in the polar solvent. In step 2, the polar solvent is expanded to make spaces that the ions will occupy. In the last step, the ions are inserted into the spaces in the polar solvent. Be able to describe the enthalpy change, ?H, for each step.Be able to relate IMF, frequency of collisions, number of molecules and speed to the pressure of a container before and after equilibrium.What are the covalent network solids and why would conductivity increase if another element is placed within the network?Know properties of solids: covalent network, molecular, ionicWhy would one element be stronger when alloyed with one element than a different element?Be able to explain why different compounds would have different boiling points based on IMF, bonding, ionic radius, or energy. Know what phases exist where on a phase diagram.Be able to explain why one substance is a liquid whereas another is a gas at the same temperature and pressure.PRACTICE PROBLEMSWhat is the mass of H2SO4 (molecular weight 98.1) in 50.0 milliliters of a 6.00-molar solution? 29.4 gramsHow many milliliters of 11.6-molar HCl must be diluted to obtain 1.0 liter of 3.0-molar HCl? 250 mLA 40.0 mL sample of 0.25 M KOH is added to 60.0 mL of 0.15 M Ba(OH)2. What is the molar concentration of OH?(aq)in the resulting solution? (Assume that the volumes are additive) 0.28 MThe volume of distilled water that should be added to 10.0 mL of 6.00 M HCl(aq) in order to prepare a 0.500 M HCl(aq) solution is approximately ___?110. mLWhat is the final concentration of barium ions, [Ba2+], in solution when 100. mL of 0.10 M BaCl2(aq) is mixed with 100. mL of 0.050 M H2SO4(aq)? 0.025 M What number of moles of O2 is needed to produce 142 grams of P4O10 from P? (Molecular weight P4O10 = 284) 2.50 moleThe alkenes are compounds of carbon and hydrogen with the general formula CnH2n. If 3.50 gram of any alkene is burned in excess oxygen, what number of moles of H2O is formed? 0.250 mole3 Ag(s) + 4 HNO3 → 3 AgNO3 + NO(g) + 2 H2OThe reaction of silver metal and dilute nitric acid proceeds according to the equation above. If 0.10 mole of powdered silver is added to 10. milliliters of 6.0-molar nitric acid, what is the number of moles of NO gas that can be formed? 0.015 moleWhen 70. milliliter of 3.0-molar Na2CO3 is added to 30. milliliters of 1.0-molar NaHCO3, what is the resulting concentration of Na+ ? 4.5 M A 20.0-milliliter sample of 0.200-molar K2CO3 solution is added to 30.0 milliliters of 0.400-molar Ba(NO3)2 solution. Barium carbonate precipitates. What is the concentration of barium ion, Ba2+, in solution after the reaction? 0.160 MA 27.0-gram sample of an unknown hydrocarbon was burned in excess oxygen to form 88.0 grams of carbon dioxide and 27.0 grams of water. What is a possible molecular formula of the hydrocarbon? C4H6How many grams of calcium nitrate, Ca(NO3)2, contains 24 grams of oxygen atoms? 41 grams The mass of element Q found in 1.00 mole of each of four different compounds is 38.0 grams, 57.0 grams, 76.0 grams, and 114 grams, respectively. A possible atomic weight of Q is 19.019. The simplest formula for an oxide of element X (MM = 76.0) that is 24.0 percent oxygen by weight is___. X2O3 BrO3? + 5 Br? + 6 H+ 3 Br2 + 3 H2OIf 25.0 milliliters of 0.200-molar BrO3? is mixed with 30.0 milliliters of 0.450-molar Br? solution that contains a large excess of H+, what is the amount of Br2 formed, according to the equation above? 8.10 x 10-3 moleHow many moles of solid Ba(NO3)2 should be added to 300. milliliters of 0.20-molar Fe(NO3)3 to increase the concentration of the NO3? ion to 1.0-molar? (Assume that the volume of the solution remains constant.) 0.060 moleSamples of F2 gas and Xe gas are mixed in a container of fixed volume. The initial partial pressure of the F2 gas is 8.0 atmospheres and that of the Xe gas is 1.7 atmospheres. When all of the Xe gas reacted, forming a solid compound, the pressure of the unreacted F2 gas was 4.6 atmospheres. The temperature remained constant. What is the formula of the compound? XeF4It is suggested that SO2 (molar mass 64 grams), which contributes to acid rain, could be removed from a stream of waste gases by bubbling the gases through 0.25-molar KOH, thereby producing K2SO3. What is the maximum mass of SO2 that could be removed by 1,000. liters of the KOH solution? 8.0 kgWhen a 1.25-gram sample of limestone was dissolved in acid, 0.44 gram of CO2 was generated. If the rock contained no carbonate other than CaCO3, what was the percent of CaCO3 by mass in the limestone? 80%... Fe(OH)2 + ... O2 + ... H2O ... Fe(OH)3If 1 mole of O2 oxidizes Fe(OH)2 according to the reaction represented above, how many moles of Fe(OH)3 can be formed?4What mass of Au is produced when 0.0500 mol of Au2S3 is reduced completely with excess H2? 19.7 gA 1.0 L sample of an aqueous solution contains 0.10 mol of NaCl and 0.10 mol of CaCl2. What is the minimum number of moles of AgNO3 that must be added to the solution in order to precipitate all of the Cl? as AgCl(s) ? (Assume that AgCl is insoluble.) 0.30 molWhen hafnium metal is heated in an atmosphere of chlorine gas, the product of the reaction is found to contain 62.2 percent Hf by mass and 37.4 percent Cl by mass. What is the empirical formula for this compound? HfCl3In the periodic table, as the atomic number increases from 11 to 17, what happens to the atomic radius? It decreases only.What is the ground state electron configuration for the Mn3+ ion? 1s2 2s22p6 3s23p63d4 Ca, V, Co, Zn, As: Gaseous atoms of which of the elements above are paramagnetic? V, Co, and AsTwo flexible containers for gases are at the same temperature and pressure. One holds 0.50 gram of hydrogen and the other holds 8.0 grams of oxygen. Which of the following statements regarding these gas samples is FALSE?The volume of the hydrogen container is the same as the volume of the oxygen container.The number of molecules in the hydrogen container is the same as the number of molecules in the oxygen container.The density of the hydrogen sample is less than that of the oxygen sample.The average kinetic energy of the hydrogen molecules is the same as the average kinetic energy of the oxygen molecules.The average speed of the hydrogen molecules is the same as the average speed of the oxygen molecules. Which of the following aqueous solutions has the highest boiling point?0.10 M potassium sulfate, K2SO4(B) 0.10 M hydrochloric acid, HCl(C) 0.10 M ammonium nitrate, NH4NO3(D) 0.10 M magnesium sulfate, MgSO4(E) 0.20 M sucrose, C12H22O11 Which of the following does NOT behave as an electrolyte when it is dissolved in water?CH3OHK2CO3NH4BrHISodium acetate, CH3COONa Which of the following has the lowest conductivity?0.1 M CuS040.1 M KOH0.1 M BaCl20.1 M HF0.1 M HNO3 The elements in which of the following have most nearly the same atomic radius?Be, B, C, NNe, Ar, Kr, XeMg, Ca, Sr, BaC, P, Se, ICr, Mn, Fe, Co All of the following statements concerning the characteristics of the halogens are true EXCEPT:The first ionization energies (potentials) decrease as the atomic numbers of the halogens increase.Fluorine is the best oxidizing agent.Fluorine atoms have the smallest radii.Iodine liberates free bromine from a solution of bromide ion.Fluorine is the most electronegative of the halogens. Next 2 questionsLithiumNickelBromineUranium Fluorine Is a gas in its standard state at 298 K EReacts with water to form a strong base AIonization Energies for element X (kJ mol?1) First Second Third Fourth Five 580 1815 2740 11600 14800 The ionization energies for element X are listed in the table above. On the basis of the data, element X is most likely to be NaMgAlSiP Which of the following represents a pair of isotopes? AtomicNumber MassNumber (A) I.II. 67 1414 (B) I.II. 614 714 (C) I.II. 614 1428 (D) I.II. 77 1314 (E) I.II. 816 1620 Next 3 questions1s2 2s22p5 3s23p51s2 2s22p6 3s23p61s2 2s22p62d10 3s23p61s2 2s22p6 3s23p63d51s2 2s22p6 3s23p63d3 4s2 The ground-state configuration for the atoms of a transition element EAn impossible electronic configurationC The ground-state configuration of a common ion of an alkaline earth element BNext 4 questionsHeisenberg uncertainty principlePauli exclusion principleHund's rule (principle of maximum multiplicity)Shielding effectWave nature of matterCan be used to predict that a gaseous carbon atom in its ground state is paramagnetic CExplains the experimental phenomenon of electron diffraction EIndicates that an atomic orbital can hold no more than two electrons BPredicts that it is impossible to determine simultaneously the exact position and the exact velocity of an electron ANext 4 questions. Represents an atom that is chemically unreactive DRepresents an atom in an excited state ARepresents an atom that has four valence electrons. CRepresents an atom of a transition metal. ENext 3 questionsFSMgArMn Forms monatomic ions with 2? charge in solutions BForms a compound having the formula KXO4 EForms oxides that are common air pollutants and that yield acidic solution in water BNext 3 questionsOLaRbMgN What is the most electronegative element of the above? AWhich element exhibits the greatest number of different oxidation states? EWhich of the elements above has the smallest ionic radius for its most commonly found ion? DGiven that a solution is 5 percent sucrose by mass, what additional information is necessary to calculate the molarity of the solution? II and IIIThe density of waterThe density of the solutionThe molar mass of sucroseGiven that a solution is 5 percent sucrose by mass, what additional information is necessary to calculate the molarity of the solution? II and IIIThe density of waterThe density of the solutionThe molar mass of sucrose ................
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