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CHEMISTRY 207 SAMPLE TEST QUESTIONS KEY 1. Circle the correct answer. a. Which one of the following does not have resonance structures? b, Which one of the following has a square pyramid shape? c. Which one of the following molecules has a net dipole moment. The shape of the molecule is given below in parentheses. CF4 CH4 BH3 SO2 (tetrahedral) (tetrahedral) (bent) (trigonal planar) d. Which of the following is probably NOT a stable compound PH3 MgO MgF3 e. Which of the following molecules has the biggest dipole moment? H2 BrCl HF Li2O IBr f. Which one of the following molecules does NOT have a net dipole moment. The shape of the molecule is given below in parentheses. SF4 BF2Br NF3 CO2 (see-saw) (trigonal planar) linear (trigonal pyramid) g. Which one of the following has sp3 hybridization on the central atom? h. Which of the following ions is most likely to be stable. (Hint: consider the Lewis structures) NH NH2 NH3 NH4 i. Which of the following molecules has a Lewis structure similar to that of N2? H2 O2 CO Cl2 j. What is the formal charge on the sulfur atom in the figure on the right? +1 -1 0 -2 k. Which of the following bonds is least polar? HF ClBr CF 1 OF CHEMISTRY 207 SAMPLE TEST QUESTIONS KEY l. Including the one shown on the right, how many resonance forms can be drawn for PO43- O O P O O 2 m. n. o. 3 4 5 How many orbitals are there a set sp hybrid orbitals? 3 4 2 5 Which one of the following is linear? Which of the following molecules has a net dipole moment BF3 FCCF CCl4 trigonal planar linear tetrahedral ICl3 T shaped p. Select the molecule in which the central atom violates the octet rule NH3 CO2 BF3 PH3 q. Which of the following is a planar molecule CH4 BH3 PCl5 NH3 r. A molecule with sp3d hybridization on the central atom always has a trigonal bipyramid geometry always has five pairs of electrons or bonded atoms around the central atom always has five bonds on the central atom always is a non planar molecule s. The angle between the H-N-H bonds in NH3 is closest to 90 o 120 o 109.5 o 180 o t. Which of the following is the balanced net ionic equation for the precipitation of calcium phosphate when aqueous solutions of sodium phosphate and calcium chloride are mixed . 2Na3PO4(aq) + 3 CaCl2(aq) 6 NaCl(aq) + Ca3(PO4)2(s) 2 PO4(aq) + 3 Ca(aq) Ca3(PO4)2(s) PO4(aq) + Ca(aq) CaPO4(s) 6 Na(aq) + 2PO4(aq) + 3Ca(aq) +6 Cl(aq) 6 Na(aq) + 6 Cl(aq) + Ca3(PO4)2(s) u. Which one of the following is an acid base reaction? 2 HCl + Mg H2 + MgCl2 HCl + KOH H2O + KCl C(s) + O2(g) CO2(g) S8(s) + 4 Cl2 (g) 4 S2Cl2(l) v. Which of the following salts is insoluble in water? FeCl3 Na2CO3 2 Pb(NO3)2 Mn3(PO4)2 CHEMISTRY 207 SAMPLE TEST QUESTIONS KEY w. In which of the following molecules does Mn have an oxidation number of +6. MnS KMnO4 MnO2 K2MnO4 x. Which of the following reactions is NOT a redox reaction? Cu(s) + F2(g) CuF2(s) K2SO4(aq) + BaCl2(aq) BaSO4(s) + 2KCl(aq) 2HCl + Mg(s) H2(g) + MgCl2(aq) C(s) + O2(g) CO2(g) y. Which of the following is a fusion reaction? 7 4 3 2 n 73 Li 0 1 He 11H 42 He 01 222 86 1 0 Be Rn 235 92 U 218 84 Po 42 He Te 137 52 97 40 Zr 201 n z. The reactions in nuclear reactors can be best characterized as Fusion Alpha decay Fission aa. In the reaction alpha particle 27 13 Al ? Gamma decay Na 42 He , the missing particle must be a(an) 24 11 beta particle neutron positron bb. 232Th undergoes alpha decay. The decay product undergoes a beta decay. What is the product of the second decay? 228 232 228 228 Rn Ac Th Ac cc Which of the following types of materials is most dangerous if ingested Beta emitters Gamma emitters Alpha emitters x-ray emitters dd What is the missing product for the fission reaction shown below 236 142 91 + + ? 56 Ba 92 U 36 Kr three protons An alpha particle three neutrons A beta particle ee. The half-life for decay of 3H is 11 yr. How many years must pass to reduce a 16.0 gram sample to 2.0 g. 11 yrs 22 yrs 44 yrs 33 yrs ff. If an isotope is above the belt of stability in the plot of number of neutrons vs. number of protons then the isotope will most likely decay by electron capture positron emission alpha emission beta emission gg. Which one of the following is a ( antibonding) orbital? 3 CHEMISTRY 207 hh. SAMPLE TEST QUESTIONS KEY Which one of the following statements is TRUE? Bond length tends to decrease as bond strength increases Bond length tends to increase as bond strength increases Single bonds tend to be shorter than double bonds Triple bonds tend to be longer than double bonds __________________________________________________________________________ A a. b c. d e. f. B C D Which of the diagrams above corresponds to a molecule with a triple bond? __D____ Which of the diagrams above corresponds molecule with no net bonds? ___C_____ Which of the diagrams above could correspond to a N2 molecule? ____D____ Which of the diagrams above corresponds to a paramagnetic molecule? ____B____ Which of the diagrams above corresponds to a molecule with a double bond? __B____ Which of the diagrams above corresponds to a molecule with a single bond? __A____ 2. Fill in the blank a. How many grams of Na are in 10g of NaOH? molNaOH molNa 22.99gNa 5.75g 10gNaOH 40 g mol mol NaOH NaOH Na b. How many moles of NaCl are in 100 mL of 2 M NaCl (0.100L)(2 mol L-1) = 0.2 mol c. The molecule HCN contains _2 bonds and 2_ bonds. d. How many moles of hydrogen atoms are in ten moles of Ca(OH)2 ___10x2 = 20 e. How many S atoms are in two moles of S2Cl2 __2x2x6.02x1023__________ f. Give the approximate values of the angles shown in the figure on the right _109.5___, __120___ 4 CHEMISTRY 207 SAMPLE TEST QUESTIONS KEY h. 10 mL of a 2.5 M NaCl solution contains __0.025________ moles of NaCl i. For CrO4 the oxidation numbers are _+6_ for Cr and __-2___ for O What is the missing isotope in the following reaction 236 92 U + 141 56 Ba ? + 92 36 Kr 3 01n Balance the following equations C6H14(l) + 19/2 O2(g) 6 CO2(g) + 7 H2O(l) 2 CH3NH2 (l) + 9/2 O2(g) 2 CO2(g) + 5 H2O(l) + N2(g) _______________________________________________________________________________ Consider the reaction S8(s) + 4 Cl2 (g) 4 S2Cl2(l) If 10.00 g of S8 reacts as completely as possible with 8.00 g of Cl2, how many grams of S2Cl2(l) will be formed. Show all calculations and report the answer to the correct number of significant figures. 4 molS2Cl2 135.03 gS2Cl2 21.06 gS Cl S8 2 2 mol mol S8 S8 S2Cl2 molCl2 4 molS2Cl2 135.03 gS2Cl2 15.2 gS Cl 8.00 gCl2 2 2 70.90 gCl 4 molCl molS Cl 2 2 2 2 mol 10.00 g 256.5 g S8 15.2 g will be formed _______________________________________________________________________________ A compound 69.58% Ba, 6.090% C and 24.32% O. What is its empirical formula? 69.58 gBa molBa 0.507 molBa 1 37.34 g Ba 6.090 gC molC 0.507 molC 1 2.01 g C 24.32 gO molO 1.52 molO 16.00 gO 5 CHEMISTRY 207 Ba O C SAMPLE TEST QUESTIONS KEY 0.507 1.0 0.507 1.52 3.0 0.507 0.507 1.0 0.507 BaCO3 ___________________________________________________________________________ How many grams of C are in 50.0 g. of Na2CO3 FW Na2CO3 = 2x22.99 + 12.01 + 3x16.00 = 105.99 g/mol molC 12.01 gC 5.67 gC mol Na2CO3 Na2CO3 mol C _______________________________________________________________________________ 50.0 g Na2CO3 mol 105.99 g Na2CO3 What is the molarity of Na2CO3 solution that is made by dissolving 2.0 g of Na2CO3 in 250.00 mL of water. 2.0 g Na2CO3 0.0189 molNa CO 2 3 mol 105.99 g Na2CO3 Na2CO3 0.0189 molNa2CO3 1000 mL 2 7.55 10 M 250 mL L _______________________________________________________________________________ What is the molarity of the solution made by diluting 25.0 mL of 2.0 M hydrochloric acid to a final volume of 1.500 L. M1V1 = M2V2 V L 25.0 mL M2 M1 1 2.0 M 0.033 M V2 1.500 L 1000 mL _______________________________________________________________________________ Write balanced net ionic equations for the following reactions. K2CO3(aq) and CuCl2(aq) Cu2+ + CO32 CuCO3(s) BaCl2(aq) + AgNO3(aq) Ag+ + Cl AgCl(s) Write a balanced nuclear equation for each of the following positron emission by 11C 11 6 C 01 115B 6 CHEMISTRY 207 SAMPLE TEST QUESTIONS KEY alpha decay of 218Pb 218 82 Pb 42 214 80 Hg Draw Lewis structures for the following compounds. Show formal charges and resonance structures if appropriate. CH3F ClO3 HCN O O Cl O + two other resonance structures ELECTRONEGATIVITIES H Li Na K Rb Cs 2.1 1.0 0.9 0.8 0.8 0.7 Be Mg Ca Sr Ba 1.5 1.2 1.0 0.9 0.9 B Al Ga In Tl 2.0 1.5 1.8 1.7 1.8 C Si Ge Sn Pb 2.5 1.8 1.8 1.8 1.9 N P As Sb Bi 7 3.0 2.1 2.0 1.9 1.9 O S Se Te Po 3.5 2.5 2.4 2.1 2.0 F Cl Br I At 4.0 3.0 2.8 2.5 2.2