CHM 1030 Examination 2A February 20, 2002

Transcription

1 CHM 1030 Examination 2A February 20, 2002 SOME GENERAL INFORMATION 1 in = 2.54 cm 1 mile = 5280 ft 16 oz = 1 lb = g 32 liq oz = 1 qt = 0.25 gal = L speed of light (c) = m/s 1 cal = J 1 u = x g INSTRUCTIONS (Read carefully): This examination has 2 pages of problems, 1 double-sided answer sheet (same color as examination), and 1 blank sheet for scratch work. Read each question carefully. Be sure that you can read one of the periodic tables in the front of the lecture hall; if you cannot, move to a seat where you can. For all problems, provide answers that have the correct number of significant figures. Show your work so that you may receive credit and partial credit for your answers. Put your answers in the space provided on the answer sheet. Show your work! Only the answer sheets will be collected for grading. On both sides of the answer sheet, be sure to print your name, sign your name, and give your student number. Good luck! REGRADE POLICY: If you have a question about the number of points that you earned on your graded exam answer sheet, do not make changes or additions to your returned, graded answer sheet. Write on a separate sheet of paper what items you believe that you were not given sufficient credit and the reasons why you think so. Attach it to your answer sheet and give it to Dr. Hilinski after a lecture or during an office hour, preferably within 2 weeks after it is returned. Part I. [34 pts] Problems [4 pts] (a) Specifically which subatomic particle is present in different numbers in nitrogen-14 and nitrogen- 15? (b) Are nitrogen-14 and nitrogen-15 called (i) different elements, (ii) isotopes, (iii) allotropes, or (iv) isomers? (choose one) 2. [10 pts] Consider the symbol Ca 2+ (a) How many protons are there in this ion? (b) How many neutrons are there in this ion? (c) How many electrons are there in this ion? (d) What is the mass number of this ion? (e) Is this ion (i) a cation or (ii) an anion? 3. [10 pts] (a) Give the group number and the chemical family name to which iodine belongs. (b) Is iodine (i) a metal or (ii) a nonmetal? (choose one) (c) Give the formula for the form in which iodine exists as an element. (d) At room temperature and one atmosphere pressure, does iodine exist as a (i) solid, (ii) liquid, or (iii) gas? (choose one) 4. [6 pts] (a) Give the group number and the chemical family name to which magnesium belongs. (b) Is magnesium a (i) a metal or (ii) a nonmetal? (choose one) 5. [2 pts] Give the symbol of a transition element. 6. [2 pts] Give the symbol of an inner transition element.

2 CHM 1030 Examination 2A February 20, 2002 Page 2 Part II. [34 pts] Problems [4 pts] (a) What is the maximum number of electrons that can be contained in the 4d subshell? (b) How many different orbitals are there in the 4d subshell? 8. [4 pts] Draw the shape of a 2p x orbital. Clearly identify where the nucleus is. 9. [6 pts] Give the ground-state electron configuration in orbitals for the nitrogen atom using arrows for electrons. 10. [4 pts] A monatomic ion that has a charge of 2+ has the following ground-state electron configuration: 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6. (a) Give the Lewis structure for this monatomic ion. (b) How many valence electrons does this ion have? 11. [8 pts] Give the symbol or formula for each of the following ions. (a) iron(ii) ion (b) aluminum ion (c) nitrite ion (d) permanganate ion 12. [8 pts] Give the correctly spelled names for each of the following. (a) Cl 2 (b) OH (c) Ag + (d) HCO 3 Part III. [32 pts] Problems [4 pts] (a) Which is larger (i) a potassium atom or (ii) a potassium ion? (choose one) (b) Which is larger (i) a chloride ion or (ii) a bromide ion? (choose one) 14. [6 pts] Give a Lewis structure for each of the following. (a) a carbon atom (b) a potassium ion (c) an oxide ion 15. [4 pts] Give a Lewis structure for the cyanide ion whose formula is CN. Be sure to show nonzero all formal charges. 16. [8 pts] Give the formal charge for each of the indicated atoms. If it is zero, write a b c d O H. O. S O O O O H B H H 17. [4 pts] Give the name of each of the following compounds. (a) NH 4 NO 3 (b) Mg(OH) [4 pts] Give the formula for each of the following compounds. (a) copper(ii) chloride (b) sodium monohydrogen phosphate 19. [2 pts] Give the symbol or formula of the reducing agent in the following balanced chemical equation. Mg + S MgS

3 CHM 1030 February 20, 2002 PRINTED NAME: EXAMINATION 2A LAST 4 DIGITS SOC. SEC. NO.: ROW SEAT SIGNED NAME: I. [34] II. [34] III. [32] TOTAL[100] 1a 1b 2a 2b 2c 2d 2e 3a 3b 3c 3d 4a 4b 5 6 7a 7b a 10b 11a 11b 11c 11d 12a 12b 12c 12d

4 CHM 1030 February 20, 2002 EXAMINATION 2A PRINTED NAME: SIGNED NAME: 13a 13b 14a 14b 14c 15 16a 16b 16c 16d 17a 17b 18a 18b 19

5 CHM 1030 Examination 2B February 20, 2002 SOME GENERAL INFORMATION 1 in = 2.54 cm 1 mile = 5280 ft 16 oz = 1 lb = g 32 liq oz = 1 qt = 0.25 gal = L speed of light (c) = m/s 1 cal = J 1 u = x g INSTRUCTIONS (Read carefully): This examination has 2 pages of problems, 1 double-sided answer sheet (same color as examination), and 1 blank sheet for scratch work. Read each question carefully. Be sure that you can read one of the periodic tables in the front of the lecture hall; if you cannot, move to a seat where you can. For all problems, provide answers that have the correct number of significant figures. Show your work so that you may receive credit and partial credit for your answers. Put your answers in the space provided on the answer sheet. Show your work! Only the answer sheets will be collected for grading. On both sides of the answer sheet, be sure to print your name, sign your name, and give your student number. Good luck! REGRADE POLICY: If you have a question about the number of points that you earned on your graded exam answer sheet, do not make changes or additions to your returned, graded answer sheet. Write on a separate sheet of paper what items you believe that you were not given sufficient credit and the reasons why you think so. Attach it to your answer sheet and give it to Dr. Hilinski after a lecture or during an office hour, preferably within 2 weeks after it is returned. Part I. [34 pts] Problems [4 pts] (a) Specifically which subatomic particle is present in different numbers in nitrogen-14 and nitrogen- 15? (b) Are nitrogen-14 and nitrogen-15 called (i) different elements, (ii) allotropes, (iii) isotopes, or (iv) isomers? (choose one) 2. [10 pts] Consider the symbol Ca 2+ (a) How many neutrons are there in this ion? (b) How many protons are there in this ion? (c) How many electrons are there in this ion? (d) What is the mass number of this ion? (e) Is this ion (i) an anion or (ii) a cation? 3. [10 pts] (a) Give the group number and the chemical family name to which iodine belongs. (b) Is iodine (i) a metal or (ii) a nonmetal? (choose one) (c) Give the formula for the form in which iodine exists as an element. (d) At room temperature and one atmosphere pressure, does iodine exist as a (i) solid, (ii) liquid, or (iii) gas? (choose one) 4. [6 pts] (a) Give the group number and the chemical family name to which magnesium belongs. (b) Is magnesium a (i) a metal or (ii) a nonmetal? (choose one) 5. [2 pts] Give the symbol of an inner transition element. 6. [2 pts] Give the symbol of a transition element.

6 CHM 1030 Examination 2B February 20, 2002 Page 2 Part II. [34 pts] Problems [4 pts] (a) What is the maximum number of electrons that can be contained in the 5d subshell? (b) How many different orbitals are there in the 5d subshell? 8. [4 pts] Draw the shape of a 2p x orbital. Clearly identify where the nucleus is. 9. [6 pts] Give the ground-state electron configuration in orbitals for the nitrogen atom using arrows for electrons. 10. [4 pts] A monatomic ion that has a charge of 2+ has the following ground-state electron configuration: 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6. (a) Give the Lewis structure for this monatomic ion. (b) How many valence electrons does this ion have? 11. [8 pts] Give the symbol or formula for each of the following ions. (a) aluminum ion (b) iron(ii) ion (c) permanganate ion (d) nitrite ion 12. [8 pts] Give the correctly spelled names for each of the following. (a) Cl 2 (b) OH (c) Ag + (d) HCO 3 Part III. [32 pts] Problems [4 pts] (a) Which is smaller (i) a potassium atom or (ii) a potassium ion? (choose one) (b) Which is smaller (i) a chloride ion or (ii) a bromide ion? (choose one) 14. [6 pts] Give a Lewis structure for each of the following. (a) a carbon atom (b) a sodium ion (c) an oxide ion 15. [4 pts] Give a Lewis structure for the cyanide ion whose formula is CN. Be sure to show nonzero all formal charges. 16. [8 pts] Give the formal charge for each of the indicated atoms. If it is zero, write a b c d O H. O. S O O O O H B H H 17. [4 pts] Give the name of each of the following compounds. (a) Mg(OH) 2 (b) NH 4 NO [4 pts] Give the formula for each of the following compounds. (a) copper(i) chloride (b) potassium monohydrogen phosphate 19. [2 pts] Give the symbol or formula of the reducing agent in the following balanced chemical equation. Mg + S MgS

7 CHM 1030 February 20, 2002 PRINTED NAME: EXAMINATION 2B LAST 4 DIGITS SOC. SEC. NO.: ROW SEAT SIGNED NAME: I. [34] II. [34] III. [32] TOTAL[100] 1a 1b 2a 2b 2c 2d 2e 3a 3b 3c 3d 4a 4b 5 6 7a 7b a 10b 11a 11b 11c 11d 12a 12b 12c 12d

8 CHM 1030 February 20, 2002 EXAMINATION 2B PRINTED NAME: SIGNED NAME: 13a 13b 14a 14b 14c 15 16a 16b 16c 16d 17a 17b 18a 18b 19