Final Exam Version A CHEM1411 Fall 2006 Name
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1 Final Exam Version A CHEM1411 Fall 2006 Name Part I: Multiple Choice Please enter your name and the Version number on your scantron. Choose the ONE best answer for each question and enter your answer on the scantron. Each answer is worth 2 points. Part II: Esaay and show your work Please enter your name at the top of Part II. Carefully read the instructions for Part II. Each answer is worth 5 points. A periodic table, a page of constants and equations, as well as scratch paper are furnished. Turn in all papers, including scratch paper, with your exam and scantron. 1. What is the maximum number of electrons in an atom that has the quantum numbers as n=4, l= 2? A. 2 B. 4 C. 6 D. 8 E What will be the hybridization of the central atom in CO 2? A. sp B. sp 2 C. sp 3 D. sp 3 d E. sp 3 d 2 3. Which of the following pairs is a correct match? A. Ca 3 (PO 4 ) 2, calcium (II) phosphate B. (NH 4 ) 2 SO 4, ammonium sulfate C. Mg 2 O 2, magnesium oxide D. Cu(NO 3 ) 2, copper dinitrate E. H 2 CO 3, carbon acid 4. In the reaction of Al(OH) 3 with H 2 SO 4, how many moles of Al 2 (SO 4 ) 3 can be produced if the reaction is begun with 1.50 mole of Al(OH) 3? 2Al(OH) 3 + 3H 2 SO 4 --> Al 2 (SO 4 ) 3 + 3H 2 O A B C D E How many protons, electrons, and neutrons are there in 130 Ba 2+ A. 56p, 56e, 130n B. 56p, 54e, 130n C. 56p, 58e, 74n D. 56p, 54e, 74n E. 54p, 56e, 74n Page 1
2 6. Sulfur crystals melt at 113 C to form a yellow liquid that does not conduct electricity. What is the crystal type for crystalline sulfur? A. ionic B. molecular C. covalent network D. metallic E. impossible to know 7. How many atoms are in a body centered unit cell? A. 1 B. 2 C. 3 D. 4 E Which of the following electron configurations represent similar chemical properties of their atoms? (i) 1s 2 2s 2 2p 6 3s 2 (ii) 1s 2 2s 2 2p 4 (iii) 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 7 (iv) 1s 2 2s 2 (v) 1s 2 2s 2 2p 6 (vi) 1s 2 2s 2 2p 6 3s 2 3p 5 A. (i), (iv) B. (ii), (vi) C. (iii), (v) D. (i), (v) E. (ii), (iii) 9. What is the!h (kj/mol) for the following reaction? The bond enthalpies for H-H, I-I and H-I are 436.4, and kj/mol, respectively. 2HI(g)! H 2 (g) + I 2 (g) A B C D E What is the molecular shape of BF 3 and NH 3 respectively? A. bent, trigonal planar B. trigonal planar, trigonal pyramidal C. trigonal planar, tetrahedran D. trigonal pyramidal, trigonal planar E. tetrahedral, trigonal planar 11. Which of the following will have a net ionic equation describing a reaction that occurs? A. Cu(s) + Co 2+ (aq) B. Co(s) + Cu 2+ (aq) C. Cu(s) + H + (aq) D. H 2 (aq) + Cu 2+ (aq) E. Cu(s) + Na + (aq) How many significant figures are appropriate to show in the result after carrying out the operation below? ( ) =? A. 1 B. 2 C. 3 D. 4 E. 5 Page 2
3 13. Which of the following has the greatest first Ionization energy? A. He B. H C. P D. F E. Na 14. When the volume of a sample of gas is halved, what will happen to the pressure if the temperature does not change? A. the pressure will double B. the pressure will not change C. the pressure will be halved D. the pressure will triple E. the pressure will ob 1/4 of the original pressure g of methanol (CH 3 OH) is burned in a bonb calorimeter with a heat capacity of 10.4 kj/ C. How much heat is given off in kj/g if the temperature increases 4.19 C? A kj/g B kj/g C kj/g D kj/g E kj/g 16. In which of the following will Mn have an oxidation state of +5? A. Mn B. MnO 2 C. MnO3 - D. MnO 4 - E. MnCl How much heat is needed to raise the temperature of 102 g of water from 25.2 C to 89.3 C? A kj B kj C J D kj E J 18. Which of the following sets of quantum numbers in an atom is unacceptable? A. (1, 0, +1, +1/2) B. (3, 2, -2, -1/2) C. (3, 2, 0, -1/2) D. (4, 3, +2, +1/2) E. (3, 1, +1, +1/2) 19. Which of the following is a weak acid? A. sulfuric acid B. hydrochloric acid C. nitric acid D. citric acid E. hydrobromic acid 20. A gas sample at a pressure of 750 torr in a volume of 3.45 L is heated from 24.0 C to 56.0 C. What is the final pressure of the gas if the new volume is 4.46 L? A. 524 torr B. 760 torr C torr D. 643 torr E torr 21. How many liters of H 2 are needed to react with 2.00 L of O 2 in the following reaction if the temperature and the pressure do not change? 2 H 2 (g) + O 2 (g) --> 2 H 2 O (g) A L B L C L D L E L Page 3
4 22. What is the ion with +3 charge that has the same electron configuration as [Ar]? A. Sc 3+ B. Cr3 + C. Co 3+ D. Rh 3+ E. Ir What will be the final volume if 10.2 ml of 4.28 M HCl is diluted to produce M HCl? A B C D E How many hydrogen atoms are there in 8.0 g of CH 4? A. 1.20x10 23 B. 3.01x10 23 C. 6.02x10 23 D. 1.20x10 24 E. 2.40x Which of the following will have hydrogen bonding? A. CH 4 B. C 2 H 6 C. HF D. SnH 4 E. H 2 S 26. What is the equivalent temperature for 105 Fahrenheit in Kelvin? A. 41 B. 314 C. 378 D. 457 E A sample of carbon tetrachloride has a mass of g and a volume of 25.0 ml. What is its density (g/ml)? A B C D E Which will have the highest boiling point? A. CH 4 B. O 2 C. N 2 D. H 2 E. NH What are the coefficients respectively when the equation below is balanced? K 3 PO 4 + BaCl 2 ---> Ba 3 (PO 4 ) 2 + KCl is balanced? A. 2, 2, 1, 3 B. 2, 3, 1, 6 C. 6, 3, 1, 2 D. 3, 1, 2, 2 E. 1, 1, 3, Which of the following is a polar covalent bond? A. The OO bond in O 2 B. The CC bond in H 3 CCH 3 C. The MgCl bond in MgCl 2 D. The HO bond in H 2 O E. The NN bond in H 2 NNH 2 Page 4
5 31. Which of the following has 2 non-bonding domains around the central atom in the Lewis Structure? A. BrF 3 B. SO 2 C. NF 3 D. PCl 5 E. BeCl Which of the following is not a ground-state electron configuration? A. P: 1s 2 2s 2 2p 4 3s 2 3p 5 B. B: 1s 2 2s 2 2p 1 C. F: 1s 2 2s 2 2p 5 D. Cu: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 3d 10 E. Cr: 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 3d What is the mass percent (%) for K in K 2 CrO 4? A B C D E Which of the following is the empirical formula? A. C 2 H 4 B. CH 3 COOH C. ) P 4 O 10 D. NH 4 NO 2 E. Ag 2 CO3 35. Which of the following will be in the net ionic equation for the reaction of aqueous solutions of calcium chloride (CaCl 2 ) and lead(ii) nitrate [Pb(NO 3 ) 2 ]? A. PbCl 2 (s) B. CaCl 2 (aq) C.. 2 NO 3 - (aq) D. Ca(NO 3 ) 2 (aq) Page 5
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