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QUESTION 1 1. Draw a correct Lewis structure for BrF4- (Br in middle, surrounded by F's ) that puts a -1 formal charge on bromine, zero formal charge on all F's. How many lone pairs (unshared pairs) are on the central atom? 2. 1 2 3 4 5 6 7 0 2. 1 2 3 4 5 6 7 0 2. 1 2 3 4 5 6 7 0 QUESTION 2 8 points 1. In the correct Lewis Structure for N2H2, skeleton H N N H, how many lone pairs (unshared pairs) are in the entire molecule? Put a zero formal charge on all atoms. QUESTION 3 8 points 1. In the correct Lewis Structure for C2H2, skeleton H C C H, how many lone pairs (unshared pairs) are in the entire molecule? QUESTION 4 8 points 1. Use the bond enthalpy table to estimate the enthalpy change, ΔHrxn , of the following. Bond Enthalpy Table Bond enthalpy kJ/mole Bond enthalpy kJ/mole C-H 413 O-O 204 C-O 358 C=C 620 H-H 436 C-C 347 2C≡O + 4H-H->C2H4 C2H4 has this skeleton: HH CC HH O=O 498 C≡O 1046 H-O 460 C≡C 812 + 2H-O-H 2. -813 kJ/molrxn 510 kJ/molrxn -276 kJ/molrxn -8210 kJ/molrxn -2840 kJ/molrxn 96.9 kJ/molrxn 2070 kJ/molrxn - 74.3 kJ/molrxn 2. 1 2 3 4 5 6 7 0 2. 1 2 3 4 5 6 7 QUESTION 5 1. Draw a correct Lewis structure for SF5 (S in middle, surrounded by F's ) that puts a zero formal charge on all atoms. How many lone pairs are on the central atom? 8 points QUESTION 6 8 points 1. Draw a correct Lewis structure for NF2- (N in middle, surrounded by F's ) that puts a -1 formal charge on N. How many lone pairs (unshared pairs) are on the central atom? 0 2. 1 2 3 4 5 6 7 0 2. 1 2 3 4 5 6 7 0 2. 1 2 3 4 5 6 7 0 QUESTION 7 8 points 1. Draw a correct Lewis structure for KrF4 (Kr in middle, surrounded by F's ) that puts a 0 formal charge on all atoms. How many lone pairs(unshared pairs) are on the central atom? QUESTION 8 1. Draw a Lewis structure for BrO2- (Br is in the middle) that puts a negative one formal charge on one O, and that has zero formal charge for the other O's and that has zero formal charge on Br. How many lone pairs (unshared pairs) are in the entire ion? 8 points QUESTION 9 1. In the correct Lewis Structure for HOCN (skeleton [HOCN]) that puts zero formal charge on all atoms, how many lone pairs (unshared pairs) are in the entire molecule? 8 points 8 points QUESTION 10 1. Draw a correct Lewis structure for CO32- (C in middle, surrounded by O's ) that puts a 0 formal charge on carbon. How many lone pairs (unshared pairs) are on the central atom? 2. 1 2 3 4 5 6 7 0 QUESTION 11 Carbon is an example of a(n): homogeneous mixture heterogeneous mixture element compound QUESTION 12 1. 2. 1. 2. 5 points A material has density of 6.62 g/cm3 . How many cm3 are in 70.0 g of the material? 60.7 cm3 8.54 cm3 10.6 cm3 32.9 cm3 1.58 cm3 92.7 cm3 8.73 cm3 2.55 cm3 QUESTION 13 How many sig figs in this number? 1 2 3 4 5 6 7 8 5 points 1. 2. 9.01 x 104 1. A large brick made of nickel metal has length 26.0 inches and width 8.00 inches. It has mass 125.0 kg. How high is the brick? Density of nickel is 8.90 g/cm3 2. 7.39 inches 5.60 inches 11.4 inches 1.40 inches 4.12 inches 2.66 inches 8.01 inches 3.15 inches QUESTION 15 1. Express 1.47 miles in inches 2. 9.31 x 104 in 20900 in 9.78 x 108 in 32.0 in 3.51 x 1012 in 2.77 x 108 in 346 in 3.05 x 106 in QUESTION 16 5 points 5 points QUESTION 14 2. 1 2 3 4 5 6 7 8 QUESTION 17 5 points 5 points 1. When you perform the following operation, how many significant figures should your answer have? (1.8613 x 10-2 + 2.567 x 10-3) x (7.54311 x 103) 1. When you perform the following operations, how many significant figures should your answer have? Assume these are measured quantities. (44.00 + 0.10) x 19.6000 = 2. 1 2 3 4 5 6 7 8 QUESTION 18 1. How many electrons in Na+? 2. 7 13 5 10 8 3 11 QUESTION 19 1. What is mass number of a Si atom that has 16 neutrons? 2. 32 9 21 14 35 33 30 10 QUESTION 20 5 points 5 points 2. Iron (III) bromide lithium phosphide perchlorous acid copper (I) hydroxide Copper (II) chloride Iron (II) nitrate 5 points 1. Which of the following is NOT a correct name? (five are correct names for any compound, but one is NOT correct for any compound) 5 points QUESTION 21 1. Which of the following is NOT a correct formula? (five are correct formulas but one is not correct for any compound) 2. NaI Ca(NO3)3 NaNO3 Na2O K3PO4 KOH QUESTION 22 1. How many grams of carbon tetrachloride in 1.60 mol? 2. 79.0 g 56.3 g 542 g 85.0 g 246 g 21.8 g 8.44 g 76.5 g QUESTION 23 1. How many H atoms are in 4.29 x 10-10 g Ca(OH)2? 2. 6.97 x 1012 atoms 8.31 x 10-9 atoms 5.44 x 10-11 atoms 6.97 x 1032 atoms 5.44 x 1014 atoms 1.53 x 1019 atoms 8.31 x 104 atoms 1.53 x 1024 atoms QUESTION 24 5 points 5 points 5 points 1. If a chemist places 50.0 grams of NaCl in a 4.00 L flask, and fills the flask to the 4.00-liter mark with water, the resultant solution is of what molarity? 2. 2.55 M 2.00 M 3.51 M 0.0431 M 1.16 M 1.95 M 0.355 M 0.214 M QUESTION 25 5 points 1. Calculate the volume of 18.0 M H2SO4 required to prepare 1.00 liter of 0.900 M H2SO4 . 2. 219 mL 322 mL 34.9 mL 20.1 mL 50.0 mL 4.93 mL 406 mL 18.0 mL QUESTION 26 1. What is reducing agent in the following reaction? CuO + H2 --> Cu+H2O 2. OinCuO H2 Cu H in H2O O in H2O 2. sp sp2 sp3 sp3d sp3d2 2. sp sp2 sp3 sp3d 5 points QUESTION 27 1. What is the hybridization of S in H2S ? (S in middle) QUESTION 28 1. What is the hybridization of C in H2CO? (C in middle of H's and O) 7 points sp3d2 2. sp sp2 sp3 sp3d sp3d2 2. sp sp2 sp3 sp3d sp3d2 2. sp sp2 sp3 sp3d sp3d2 2. CspandNsp Csp2 and C2p Csp2 and Csp3 Csp and N2p Csp3 and Csp C2p and C2p Csp2 and Csp Nsp and Csp2 QUESTION 29 1. What is the hybridization of Xe in XeF4? (Xe in middle) 7 points QUESTION 30 7 points 1. For HNO2, what is the hybridization of N? skeleton is H O N O QUESTION 31 7 points 1. For PO43-, what is the hybridization of P? QUESTION 32 7 points 1. Consider the following molecule: CH3C≡N Which atomic orbitals overlap to form the carbon-carbon sigma bond of this molecule? QUESTION 33 7 points 1. What is the electron domain arrangement of PF4-? (P in middle, surrounded by F’s) (i.e., what is the electron pair arrangement, arrangement of areas of high electron density.) 2. linear octahedral t-shaped see-saw bent square pyramidal trigonal planar trigonal pyramidal trigonal bipyramidal tetrahedral square planar 2. linear octahedral t-shaped see-saw bent square pyramidal trigonal planar trigonal pyramidal trigonal bipyramidal tetrahedral square planar 2. linear octahedral t-shaped see-saw bent planar square pyramidal trigonal planar QUESTION 34 1. What is the molecular geometry of NF4+ ? (N in middle, surrounded by F’s) 7 points QUESTION 35 7 points 1. What is the molecular geometry of PF3 ? (P in middle, surrounded by F’s) trigonal pyramidal trigonal bipyramidal tetrahedral square planar bent 2. linear trigonal planar tetrahedral bent trigonal bipyramidal octahedral 2. linear octahedral t-shaped see-saw bent square pyramidal trigonal planar trigonal pyramidal trigonal bipyramidal tetrahedral square planar 2. linear trigonal planar tetrahedral bent QUESTION 36 7 points 1. What is the electronic geometry (arrangement of electron pairs) around central atom in XeF4? (Xe in middle) QUESTION 37 1. What is the electron pair arrangement (arrangement of areas of high electron density) of IO3- ? (I in middle, surrounded by O’s) 7 points QUESTION 38 7 points 1. What is the electronic geometry (arrangement of electron pairs) around central atom in IO2- ? (I in middle) trigonal bipyramidal octahedral 1. Consider these molecules. Which is polar? 2. SF6 CO2 PCl5 BeCl2 CH2Cl2 CH4 2. BF3 CO2 BH3 BeF2 CI4 CH3Cl 2. H2CO HF NCl3 H2O C6H12 2. CF4 CH2OH PF5 BeBr2 CO2 SF6 QUESTION 1 QUESTION 2 3 points 1. Consider these molecules. Which is polar? QUESTION 3 3 points 1. Which is a nonpolar molecule? QUESTION 4 1. Which is polar? 3 points 1. Which of the following molecules should have the lowest boiling point? 2. a nonpolar molecule of 64 grams per mole A polar molecule of 142 g/mole a nonpolar molecule of 234 g/mole an ionic compound 2. PCl5 CH3F PF5 BeF2 SiF4 2. viscosity swimming lessons surface tension ionic forces 2. Br2 CS2 PCl5 CF4 CI4 CH3Cl QUESTION 2 3 points 1. Which is a polar molecule among the following? QUESTION 3 3 points 1. A needle can float on the surface of water because of QUESTION 4 3 points 1. Consider these molecules. Which are polar? QUESTION 5 3 points 1. Which is polar? 2. CF4 CH2OH PF5 BeBr2 CO2 SF6 2. HBr KCl CO2 CH3Br HF CH2O (C is in middle) 2. MgCO3 HF NaCl H2O C6H12 2. 186g 8.62 g 577 g 131 g 90.1 g 424 g 2740 g QUESTION 6 3 points 1. Which of these species is capable of hydrogen-bonding among itself? QUESTION 7 3 points 1. For which of the following species are the intermolecular interactions entirely due to dispersion forces? QUESTION 1 1. Refer to the following equation. How many grams of grams of NaN3 are required to produce 75.0 liter of N2 gas at 25 oC and 748 mm Hg, assuming 100 percent yield? 6NaN3(s) + Fe2O3 (s) → 3Na2O(s) + 2Fe (s) + 9N2(g) 318 g 2. 4.88 g 18.9 g 0.351g 32.9 g 0.288 g 1.80 g 0.897 2. Flask B has a higher mass of gas If the temperature of flask B changes to 210 °C, the pressure of flask B will increase The flasks have molecules with the same average speed If the temperature of flask B changes to 5 °C, the pressure of flask B will decrease 2. There are no forces between gas particles. Gas molecules move slower at higher temperatures. Gas particles occupy a tiny volume compared with the volume of their container Gas particles are in constant, random motion Gas particles cause pressure when they collide with the walls of the container. QUESTION 2 5 points 1. How many grams of CO are present in a 600 mL container if the temperature is 22.0 oC and the pressure is 2.60 atm? QUESTION 3 5 points 1. In two flasks of having equal volume, sample A contains H2 gas at 55°C and 2.00 atm and sample B contains O2gas at 55°C and 2.00 atm. Which statement is FALSE? QUESTION 4 5 points 1. Which of the following statements conflicts with the kinetic molecular theory of gases? QUESTION 5 5 points 1. 1.30 grams of C7H6O2 is combusted in a bomb calorimeter. The water's temperature rose from 20.00 oC to 21.58 oC . The heat capacity of the calorimeter is 10.90 kJ/oC. What is the enthalpy change (ΔH) for this reaction? The thermochemical equation is: 2C7H6O2 + 15O2 ->14CO2 + 6H2O ΔHrxn = ? (molar mass C7H6O2 is 122.13 g/mol) 2. – 8010 kJ/mol – 3230 kJ/mol – 705.0 kJ/mol – 2910 kJ/mol – 901.0 kJ/mol – 652.0 kJ/mol – 2730 kJ/mol – 13400 kJ/mol 2. 6.375 kJ/mol rxn -657.2 kJ/mol rxn 14.80 kJ/mol rxn -3120 kJ/mol rxn -658.0 kJ/mol rxn -42.96 kJ/mol rxn 569.0 kJ/mol rxn -2451 kJ/mol rxn QUESTION 6 5 points 1. Reaction of 6.300 grams of C2H6(g) according to the reaction below released 327.6 kJ of heat. What is the ΔH of the reaction? 2 C2H6(g) + 7 O2(g) ---> 4 CO2(g) + 6 H2O(l) ΔHrxn = ? QUESTION 7 1. 85.00 mL of 0.3500 M CuSO4 solution is mixed with 85.00 mL of 0.7000 M NaOH solution in a coffee cup calorimeter. The two solutions are both initially at 21.00 degree centigrade. Predict the final temperature of the solution after the reaction. Assume that the aqueous solutions have the same specific heat as water (4.184 J/ g oC ) and the same density of water (1.00 g/mL) . CuSO4 + 2NaOH --> Na2SO4+ Cu(OH)2 ∆Hrxn = -99.30 kJ/molrxn 5 points 2. 12.80 oC 32.85 oC 19.11 oC 30.65 oC 23.06 oC 25.15 oC 21.74 oC 35.26 oC negative, and the process is endothermic. positive, and the process is exothermic. positive, and the process is endothermic. negative, and the process is exothermic. QUESTION 8 5 points 1. The sign of ∆H for the process Heat + 2HgO --> 2Hg + O2 is 5 points QUESTION 9 1. Which of the following would be exothermic? 2. the burning of gasoline the melting of gold the boiling of water The changing of solid ice to liquid water 2. 2.32 x 10-8 m 1.91 x 10-7 m 2.17 x 10-6 m 6.02 x 107 m 1.73 x 10-8 m 7.12 x 10-7 m 1.99 x 108 m 1.98 m 2. 4.50 x 1017 J 7.84 x 10-12 J 2.83 x 10-17 J 6.21 x 10-20 J 5.06 x 10-19 J -6.44 x 1014 J 1.64 x 10-18 J 3.80 x 10-18 J QUESTION 10 5 points 1. Calculate the wavelength of a photon absorbed by a hydrogen atom when an electron is promotedfromthen=4tothen=7 state. QUESTION 11 1. When an electron falls from a higher to a lower energy level in an atom, the photon released has a wavelength of 121.6 nm. What is the energy difference between the two energy levels, in J? 5 points

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