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GROUP QUIZ UNIT 04 NAMES ________________________________ ________________________________ ________________________________ _______________________________ I. Fill in the charts (1 point per blank). Energy level (4 lowest) # sublevels Sublevel # orbitals # orbitals 1. _____ 15. ______ 29. ______ 2. _____ 16. ______ 30. ______ 3. _____ 17. ______ 31. 4. _____ 18. ______ 5. _____ 19. ______ 6. _____ 20. ______ 7. _____ 21. ______ 8. _____ 22. ______ 9. _____ 23. ______ 10. _____ 24. ______ 11. ______ 25. ______ 12. ______ 26. ______ 13. ______ 27. ______ 14. ______ 28. ______ 32. 33. Maximum # e-s # electrons NAME: __________________________________ Group Quiz Unit 4 I. Fill in the charts (1 point per blank). Energy level (4 lowest) # sublevels Sublevel Maximum # e-s # orbitals # orbitals # electrons II. Choose the best answer to each question (2 points each). ____1. If the third main energy level contains 15 electrons, how many more could it possible hold? a. 0 b. 1 c. 3 d. 17 ____2. At n = 1, the total number of electrons that could be found is a. 1. b. 2. c. 18. 6. d. ____3. If the four principal quantum numbers for the last electron of an element is n=4, l=2, m=-1, and ms= -1/2, what is the element? a. Zr b. Co c. Rh d. Se ____4. A three-dimensional region around a nucleus in which a particular electron may be found is called a(n) a. spectral line. b. electron path. c. orbital. d. orbit. ____5. An orbital that would never exist according to the quantum description of the atom is a. 3d. b. 8s. c. 6d. ____6. a. b. c. d. d. 3f. An orbital may be defined as the most stable state of an atom. the circular path followed by an electron around the nucleus. the positively charged central part of an atom. a highly probable location of an electron within the atom. ____7. The letter designations for the first four sublevels with the number of electrons available for each sublevel are a. s:1, p:3, d:10, and f:14. b. s:1, p:3, d:5, and f:7. c. s:2, p:6, d:10, and f:14. d. s:1, p:6, d:10, f:4. ____8. How many half-filled orbitals are there in a bromine atom? a. 1 b. 2 c. 3 d. 4 ____9. What is the electron configuration for neon? a. 1s22s22p43s2 b. 1s21p62s2 1s22s22p6 d. 1s22p63s2 5p d. 5s c. ____10. The atomic sublevel with the next highest energy after 4p is a. 4d b. 4f c. ____11. The Lewis-dot configurations of all noble gases beginning with neon would show how many dots around element’s symbol? a. 1 b. 2 c. 8 d. 10 ____12. The element with the electron configuration 1s22s22p63s23p2 is a. Mg b. C c. S d. the Si ____13. The Lewis-dot notation for an element in the third period is represented by a symbol surrounded by three dots. The electron configuration for this element is a. 1s22s22p63s23p1. b. 1s22s22p63s13p2. c. 1s22s22p53s23p2. d. 1s22s22p63s2. ____14. The Lewis-dot notation for fluorine would show a. 9 dots around the symbol. b. 1 dot around the symbol. c. 7 dots around the symbol. d. 8 dots around the symbol. ____15 How many electrons are needed to fill the third main energy level if it already contains 8 electrons. a. 0 b. 8 c. 10 d. 22 ____16. Complete the electron-configuration notation for bromine: 1s22s22p6 a. 3s23p64s24p5 b. 3s23p64s24p54d10 c. 2d103s23p64s24p5 d. 3s23p64s23d104p5 ____17. The major difference between a 1s orbital and a 2s orbital is that a. the 2s orbital can hold more electrons. b. the 2s orbital has a slightly different shape. c. the 2s orbital is at a higher energy level. d. the 1s orbital can have only one electron. ____18. The maximum number of electrons that can occupy any single orbital at any energy level is a. two, if they have opposite spins. b. two, if they have the same spin. c. one. d. no more than eight. ____19. The electron configuration for the element with atomic number 11 is a. 1s22s22p63s1. b. 2s22p23p6. c. 1s22s22p43s3. d. 1s22s22p22p62d1. ____20. The total number of orbitals that can exist at the second main energy level is a. 2. b. 3. c. 4. d. 8. d. 4 ____21. In the correct Lewis dot notation for sulfur, the symbol S is surrounded by a. three pairs of dots. b. two pairs of dots and two single dots. c. four single dots. d. two pairs of dots. ____22. How many sublevels are there in the second principal energy level? a. 1 b. 2 c. 3 ____23. What shapes of orbitals are in the third principal energy level? a. s only b. s and p only c. s, p, and d only d. s, p, d and f ____24. What is the maximum number of d orbitals in one energy level? a. 1 b. 3 c. 5 d. 7 ____25. What is the maximum number of electrons in the second principle energy level? a. 2 b. 8 c. 18 d. 32 d. 4f ____26. a. b. c. d. The formula 2n2 represents ___. the number of orbitals in a sublevel the maximum number of electrons that can occupy an energy level the number of sublevels in any energy level. None of the above. ____27. Which of the following sublevels has the lowest energy? a. 3d b. 4s c. 4p ____28. a. b. c. d. If three electrons are available to fill three empty 2p atomic orbitals, how will the electrons be distributed in the three orbitals? one electron in each orbital two electrons in one orbital, one in another, none in the third three in one orbital, one in the other two cannot be predicted, determined by random chance ____29. How many unpaired electrons are there in a sulfur atom? a. 0 b. 1 c. 2 ____30. What is the number of electrons in the outermost energy level of an oxygen atom? a. 2 b. 4 c. 6 d. 3 d. 8 III. Problems: Write the electron configurations using shorthand notation (2 points) and draw orbital spin diagrams for the following elements (2 points): 31. arsenic e- config: Spin diagram: 32. barium e- config: Spin diagram: Give the four quantum numbers for the following boxed electron. (1 point for each quantum number) 33. 1s 2s 2p