Fall 2024 CHEM 1021 Optional Practice Lecture Midterm II (Chapters 3 & 4) PDF

Dr. Jim Bloxton CHEM 1021 Fall 2024 Optional Practice Lecture Midterm II (Chapters 3 and 4 from 12 th Edition) Note: This is optional practice material for chapters 3 and 4 from 12th Edition. These are sample questions that may or may not be used on a quiz, midterm or final exam. This practice mi...

Dr. Jim Bloxton CHEM 1021 Fall 2024 Optional Practice Lecture Midterm II (Chapters 3 and 4 from 12 th Edition) Note: This is optional practice material for chapters 3 and 4 from 12th Edition. These are sample questions that may or may not be used on a quiz, midterm or final exam. This practice midterm is not an exhaustive list of questions that could appear on quizzes or exams. Other questions that are not found in this practice material will be on the actual quiz, midterm and final exam. Learn the basic principles and then be prepared to apply the principles to problems that you have not seen before. It is important to do all of the homework problems that are in your Chem 1021 lecture text in addition to the questions in this optional practice lecture midterm II; optional practice lecture quizzes for chapters 3 and 4 from 12th Edition. Make sure that you do all of the Chemical Connections homework questions that have assigned as well as the homework problems and Chemical Connection problems at the end of Chapters 3 and 4. Note: The number of questions and distribution of questions on an actual exam may be different that the number of questions and distribution of questions on this practice exam. Note: It is very important to remember that Chemistry is a cumulative topic and that the material that was covered in previous chapters needs to be reviewed as this material will continue to reappear in concepts that are needed to solve new problems. 1. What is the formula of the iodate ion? A. IO4 B. IO2- C. I- D. IO3- E. None of these. 2. What is the name of (NH4)2HPO3? A. Diammonium hydrogenphosphate B. Ammonia hydrogenphosphate C. Ammonium hydrogenphosphite D. Ammonium hydrogenphosphate 3. What is a medical use of AgNO3? A. Treatment of bipolar disorder B. Antibiotic C. To strengthen teeth (external) D. Diuretic E. None of these. 4. What is the formula of bromous acid? A. HBr B. HBrO4 C. HBrO D. HBrO2 5. Write the ground state electron configuration of the most stable ion that Rb forms. A. 1s22s22p63s23p64s23d104p65s1 B. 1s22s22p63s23p64s23d104p65s2 C. 1s22s22p63s23p64s23d104p6 D. [Ar]4s24d104p6 E. Both C and D. 6. Write the ground state electron configuration of the most stable ion that I forms. A. 1s22s22p63s23p64s23d104p65s24d105p5 B. 1s22s22p63s23p64s23d104p65s24d105p4 C. 1s22s22p63s23p64s23d104p65s24d105p6 D. [Kr]5s24d105p6 E. Both C and D. 7. How many protons, electrons and neutrons are there in the most stable ion that barium-138 forms? A. 56 p, 56 e, 82 n B. 56 p, 58 e, 82 n C. 56 p, 54 e, 82 n D. 54 p, 56 e, 82 n 8. How many protons, electrons and neutrons are there in the most stable ion that phosphorus-31 forms? A. 15 p, 15 e, 16 n B. 15 p, 18 e, 16 n C. 15 p, 12 e, 16 n D. 15 p, 15 e, 19 n 9. Which of the following represents hydrogen fluoride? A. HF(g) B. HFO C. HF(aq) D. HFO2 10. What is the name of O2F2? A. Oxygen fluoride B. Dioxygen difluorine C. Dioxide difluoride D. Dioxygen difluoride 11. What is the formula of chromium(VI) carbonate? A. Cr2CO3 B. Cr(CO3)6 C. Cr(CO3)3 D. CrCO3 E. None of these. 12. Which of the following is true about the CH2O molecule? A. The central bond angle is approximately 120.0○. B. The actual shape of the molecule around the central atom is trigonal planar. C. This molecule does not contain a polar bond(s). D. Both A and B. E. Choices A, B and C. 13. Write the formula for an ionic compound from lead and sulfur. A. Pb2S3 B. PbS C. PbS2 D. Both A and B E. Both B and C. 14. Which of the following is true about the correct Lewis structure for CH3Cl? A. The C atom has three single bonds to it and one double bond to it. B. There are no polar bond(s) in the molecule. C. This is a polar molecule. D. The actual shape of the molecule is tetrahedral and the HCH bond angle is approximately 109.5◦. E. Both C and D. 15. Which of the following is a nonpolar molecule that has polar bond(s)? A. H2O B. CH3F C. C2F4 D. HF E. Both A and C. 16. Calculate the formula weight of Cr2(SO3)3. A. 344.21 amu B. 184.06 amu C. 392.21 amu D. 280.06 amu 17. How many grams of Cr2(SO3)3 are found in 0.315 mol of Cr2(SO3)3? A. 124. B. 0.803 C. 108. D. 1.09 x 10 3 18. How many g of sulfur are found in 7.02 x 1022 formula units of Cr2(SO3)3? A. 11.2 g B. 3.75 g C. 33.7 g D. 37.1 g 19. Balance the following equation: C7H14 + O2 → CO2 + H2O A. C7H14 + O2 → 7CO2 + 7H2O B. C7H14 + 21O2 → 7CO2 + 7H2O C. 2C7H14 + 21O2 → 14CO2 + 14H2O D. 2C5H10 + 15O2 → 10CO2 + 10H2O 20. Which of the following is true concerning the following reaction? Cu2+(aq) + Zn(s) → Cu(s) + Zn2+(g) A. Zn(s) is oxidized and is the reducing agent and Cu(s) is reduced and is the oxidizing agent. B. Cu2+(aq) is reduced and is the oxidizing agent and Zn(s) is oxidized and is the reducing agent. C. Zn2+(aq) is reduced and is the oxidizing agent and Cu2+(aq) is oxidized and is the reducing agent. D. Zn(s) is reduced and is the oxidizing agent and Cu2+(aq) is oxidized and is the reducing agent. The following information may be helpful for questions 21 - 23. MM of H2 = 2.02 g/mol MM of NO = 30.01 g/mol MM of N2 = 28.02 g/mol MM of H2O = 18.02 g/mol Consider the following reaction for questions 21 - 23. 2 H2(g) + 2 NO(g)  N2(g) + 2 H2O(g) 21. If 31.8 g of H2(g) is combined with 127.1 g of NO(g) to produce 22.8 g of N2(g) what is the limiting reactant? A) H2 B) NO C) N2 D) H2O 22. If 31.8 g of H2(g) is combined with 127.1 g of NO(g) to produce 22.8 g of N2(g) what is the percent yield? A) 61.6% B) 38.4% C) 17.9% D) 71.7% 23. What mass of H2(g) in grams is needed to form 220.6 g of N2(g)? A) 15.9 B) 31.8 C) 221. D) 7.95 24. Which of the following is true about the production of 156.0 g of iron according to the following thermochemical equation? Fe2O3(s) + 196.5 kcal → 2 Fe(s) + 3/2 O2(g) A. 274.4 kcal of energy is consumed and this is an endothermic reaction. B. 548.9 kcal of energy is consumed and this is an endothermic reaction. C. 548.9 kcal of energy is produced and this is an exothermic reaction. D. 638.6 kcal of energy is consumed and this is an endothermic reaction. 25. How does fluoride ion protect the enamel against tooth decay? A. Fluoride ions replace hydroxide ions in hydroxyapatite and this results in the formation of the more acid soluble fluoroapatite. B. Fluoride ions replace hydrogen ions in hydroxyapatite and this results in the formation of the less acid soluble fluoroapatite. C. Fluoride ions replace hydroxide ions in hydroxyapatite and this results in the formation of the less acid soluble fluoroapatite. D. Fluoride ions replace calcium ions in hydroxyapatite and this results in the formation of the less acid soluble fluoroapatite. 26. A substance has a specific heat of 0.420 cal/g.oC. What is the mass of the substance if 1.15 kcal of heat raises its temperature from 25.0oC to 39.0oC? A. 0.196 g B. 5.10 g C. 19600. cg D. 196. g E. Both C and D. 27. Which of the following is a balanced net ionic equation for the reaction of a solution of Na2CO3(aq) with a solution of SrCl2(aq)? A. Na2CO3(aq) + SrCl2(aq) → SrCO3(s) + 2NaCl(aq) B. 2Na+(aq) + CO32-(aq) + Sr2+(aq) + 2Cl-(aq) → SrCO3(s) + 2Na+(aq) + 2Cl-(aq) C. CO32-(aq) + Sr2+(aq) → SrCO3(s) D. 2Na+(aq) + 2Cl-(aq) → 2Na+(aq) + 2Cl-(aq) 28. What are the names and formulas of the spectator ions in question 27? A. Sodium ion Na+ and chloride Cl- B. Strontium ion Sr2+ and carbonate ion CO32- C. Sodium ion Na+ and carbonate ion CO32- D. Strontium ion Sr2+ and chloride ion Cl- 29. Which of the following is true? A. In a reduction half reaction electrons are products. B. In an oxidation half reaction electrons are products. C. In an oxidation half reaction electrons are reactants. D. In a REDOX reaction electrons are products. 30. Which of the following is true? A. In an endothermic reaction heat flows from the system into the surroundings. B. In an exothermic reaction heat flows from the system into the surroundings. C. In an endothermic reaction heat ∆T is positive. D. In an exothermic reaction heat ∆T is negative.