Chemistry 110Name_______________________Practice Exam 1BSection _______________________Midterm 1Signature ______________________IMPORTANT: On the scantron (answer sheet) you MUST clearly fill your name yourstudent number section number and test form (white cover = test form A; yellow cover= test form B). Use a #2 pencil.There are 28 questions on this exam. Check that you have done all of the problems andfilled in the first 28 bubbles on the scantron. The maximum score on this exam is 28points. Your score will be reported in percents (max 100%).Exam policyThis cover sheet must be signed and handed in with your answer sheet for yourexam to count.Calculators with text-programmable memory are not allowed.Relevant data and formulas including the periodic table are attached at the end ofthis exam.Your grade will be based only on what is on the scantron form.The answer key will be posted on the web after the exam (under “ExamSchedule”).HintsAs you read the question underline or circle key words to highlight them foryourself. Avoid errors from “mis-reading” the question.Pay attention to units and magnitudes (decimal places) of numbers obtained fromcalculations.There is no penalty for guessing. CHEMISTRY 110 PRACTICE EXAM 1B——————————————————————————–1. What is the mass of a piece of calcium that contains 8.075 × 1012Ca atoms?A. 1.341 × 10-11 gB. 3.353 × 1013 gC. 5.376 × 10-10 gD. 1.860 × 109 gE. 3.234 × 1014 g——————————————————————————–2. How many protons neutrons and electrons does 108Ag have?pneA.476162B.1084748C.624661D.476146E.None of the answers listed here are correct——————————————————————————————– ——————————————————————————————-3. For the following arrangement what is the internal energy changefor System A if q1 = 10 kJ q2 = 5 kJ w1 = 8 kJ and w2 = 10 kJ?A. 2 kJB. 7 kJC. 33 kJD. 10 kJE. 3 kJ——————————————————————————————-4. Of the following which element is the most electronegative?A. CaB. AtC. OD. AlE. Li——————————————————————————————-5. Which of the following sets is an incorrect set of quantum numbersfor an atom?A. n = 3 = 2 m =0 ms = 1/2B. n = 4 = 3 m = 2 ms = 1/2C. n = 2 = 2 m =2 ms = 1/2D. n = 1 = 0 m =0 ms = 1/2E. n = 3 = 1 m = 1 ms = 1/2——————————————————————————————– ——————————————————————————————-6. What is the percent sodium in sodium carbonate?A. 43.4%B. 11.3%C. 45.3%D. 27.7%E. 23.0%——————————————————————————————-7. Which of these choices is the electron configuration for thealuminum ion in its most common oxidation state?A. 1s22s22p63s2B. 1s22s22p63s23p2C. 1s22s22p63s23p1D. 1s22s22p6E. 1s22s22p63s23p4——————————————————————————————-8. Which of the elements listed below has the largest atomic radius?A. BB. AlC. SD. PE. Si——————————————————————————————– ——————————————————————————————-9. Which orbital has an unpaired electron in the ground state ofbromine?E. None of these: there are no unpaired electrons in theground state of bromine.——————————————————————————————-10. Which of the following is not true about enthalpy?A. It is an extensive property.B. It is a state function.C. It is measured under constant pressure.D. The enthalpies of a given process and its reverse have thesame magnitudes but opposite sign.E. It does not depend on the state of matter.——————————————————————————————-11. A compound is 53.3% C 11.2 % H and 35.5 % O by mass. Whatis the molecular formula of the compound if the molar mass is90 g/mol?A. CH2OB. C2H5OC. C4H10O2D. C3H6O3E. C5H14O——————————————————————————————– ——————————————————————————————-12. Which one of these ions has the smallest radius?A. K B. Cl-C. Na D. S2-E. O2——————————————————————————————–13. Which one of these has the greatest number of moles of atoms?A. 5.00 g of H2B. 25.00 g of CC. 82.00 g of PbD. 127.00 g of CuE. 384.00 g of Au——————————————————————————————-14. What is the wavelength of a photon emitted by a hydrogen atomwhen its electron drops from n=4 to n=2?A. None of the answers listed here.B. 364 µmC. 486 µmD. 486 nmE. 364 nm——————————————————————————————-15. Which of the following set of quantum numbers has the greatestnumber of degenerate orbitals?A. n = 3 = 2B. n = 4 = 3C. n = 2 = 1D. n = 6 = 0E. n = 1 = 0 ——————————————————————————————-16. How many unpaired electrons are in the ground state of Co3 ?A. 2B. 3C. 4D. 5E. 6——————————————————————————————-17. Which one of the following orbital diagrams is an excited stateelectron configuration of nitrogen?1s2s2p3sABCDE——————————————————————————————-18. Which of the following compounds is an ionic compound?A. KFB. CCl4C. CS2D. CO2E. ICl ——————————————————————————————-19. The first four ionization energies (I) for an atom are given below.What is the identity of this atom?I1 = 738 kJ/molI2 = 1451 kJ/molI3 = 7733 kJ/molI4 =10 542 kJ/mol.A. NaB. AlC. ClD. SiE. Mg——————————————————————————————-20. Select the compound with the highest lattice energy.A. CaSB. BaSC. NaID. MgOE. LiBr——————————————————————————————-21. Boron has two naturally occurring isotopes 10B and 11B. Theaverage atomic mass of boron is 10.811. What is the percentabundance of these isotopes?A. 20% 10B80 BB. 80% 10B20 BC. 50% 10B50 BD. 60% 10B40 BE. 40% 10B60 B——————————————————————————————– ——————————————————————————————-22. Rank the following electrostatic interactions in order of increasingelectrostatic potential energy.0.5 d0.5 d-1 11-14d 22-2 23A. 1 < 2 < 3B. 1 < 3 < 2C. 3 < 2 < 1D. 2 < 3 < 1E. 2 < 1 < 3-------------------------------------------------------------------------------------------23. In an experiment 90.1 g of FeCl3 x H2O is heated to drive off allof the water of hydration. The mass of the remaining salt is 54.1g. What is the value of x in the formula for the hydrate?A. 2B. 3C. 4D. 5E. 6-------------------------------------------------------------------------------------------- -------------------------------------------------------------------------------------------24. Assuming the pictures below schematically represent visible microwave and X-ray radiation what is the correct assignment?107 nm21000 nm1ABCDE1visiblemicrowaveX-rayX-rayvisible2X-rayvisiblemicrowavevisiblemicrowave0.1 nm33microwaveX-rayvisiblemicrowaveX-ray-------------------------------------------------------------------------------------------25. How many moles of ultra-violet photons with a wavelength of 400nm does it take to equal the energy in 1.0 mole of infraredradiation of 1000 nm?A. 0.080 molesB. 2.5 molesC. 0.40 molesD. 1.0 molesE. None of the answers listed here are correct--------------------------------------------------------------------------------------------------------------------------------------------------------------------------------------END of EXAM
