CHAPTER 8 PRACTICE TEST QUESTIONS (END OF CHAPTER 7 TOO)

CHAPTER 8 PRACTICE TEST QUESTIONS (END OF CHAPTER 7 TOO) Information that most likely will be on the front cover of your exam: h i Z 2 ΔE = @ 2.18 x 10 @ 18 f Z 2 f J j @ k n f 2 n i 2 1. Which of the following sets of quantum numbers is allowed? n l m l m s a. 1 0 1 + ½ b. 1 1 0 ½ c. 2 1 2 + ½ d. 3 2 3 ½ e. 4 3 3 + ½ 2. Determine the set of quantum numbers that describe the last electron added to As (Z = 33). a. n = 3, l = 2, m l = 0, m s = + ½ b. n = 3, l = 2, m l = 1, m s = ½ c. n = 4, l = 1, m l = +1, m s = + ½ d. n = 3, l = 1, m l = +1, m s = ½ e. n = 4, l = 1, m l = 0, m s = ½ 3. Determine the set of four quantum numbers that describe the last electron added to Ne (the outermost electron). n l m l m s a. 2 1 +1 ½ b. 2 2 +1 ½ c. 3 0 0 + ½ d. 2 1 0 + ½ e. 3 2 +2 + ½ 4. Determine the four quantum numbers that describe the last electron added to the Se atom. a. n = 4, l = 0, m l = 0, m s = ½ b. n = 4, l = 2, m l = 1, m s = ½ c. n = 4, l = 1, m l = 1, m s = + ½ d. n = 4, l = 2, m l = 0, m s = + ½ e. n = 4, l = 1, m l = 1, m s = ½ 5. Determine the set of quantum numbers that describe the electron added to a Br atom as it forms an ion (last electron in the Br ion). a. n = 4, l = 1, m l = 0, m s = + ½ b. n = 5, l = 4, m l = 3, m s = + ½ c. n = 3, l = 0, m l = 0, m s = ½ d. n = 4, l = 1, m l = 1, m s = ½ e. n = 4, l = 2, m l = 2, m s = ½

6. Determine the set of 4 quantum numbers that describe the last electron added to an atom of B. a. n = 2, l = 0, m l = 0, m s = +½ b. n = 3, l = 2, m l = 3, m s = +½ c. n = 2, l = 1, m l = 2, m s = +3/2 d. n = 3, l = 1, m l = 0, m s = ½ e. n = 2, l = 1, m l = 1, m s = +½ 7. How many electrons in a given atom can have the following quantum numbers? n = 3 l = 2 a. 2 b. 8 c. 10 d. 18 e. 32 8. How many orbitals in a given atom can be described by the following quantum numbers? a. 3 b. 4 c. 5 d. 6 e. 10 n = 4, l = 2 9. Which of the following combinations of quantum numbers are NOT allowed? a. n = 4, l = 4, m l = 0 b. n = 3, l = 2, m l = 2 c. n = 8, l = 4, m l = 3 d. n = 1, l = 0, m l = 0 e. None of the above are allowed combinations of quantum numbers. 10. Determine the ground state electron configuration of Ba 2+. a. [Xe]6s 2 b. [Kr]5s 2 4d 10 5p 6 c. [Xe]6s 2 5d 2 d. [Kr] 5s 2 4d 10 5p 4 e. [Xe]6s 2 4f 2 11. Determine the ground state electron configuration for Te 2. a. [Kr]5s 2 4d 10 5p 6 b. [Kr]5s 2 4d 10 5p 4 c. [Kr]5s 2 4d 10 5p 2 d. [Kr]5s 2 4d 10 5p 6 6s 2 e. [Kr]4d 10 5p 6

12. Determine the ground state electron configuration for I. a. [Kr]5s 2 4d 10 5p 5 b. [Kr]5s 2 4d 10 5p 4 c. [Xe]6s 1 d. [Kr]4d 10 5p 5 e. [Kr]5s 2 4d 10 5p 6 13. What species is represented by the following ground state electron configuration if its nucleus contains 35 p + and 44 n? a. Kr b. Sr 2+ c. Ru 2+ d. Br e. Au + [Ar]4s 2 3d 10 4p 6 14. Determine the ground state electron configuration for the Sr ion. a. [Kr]5s 2 b. [Kr]5s 2 4d 2 c. [Ar]4s 2 3d 10 4p 6 d. [Ca]3d 10 4p 6 5s 2 e. [Ar]4s 2 4p 6 4d 10 15. According to the Bohr model, which of the following one electron species requires the most energy to ionize? a. N 6+ b. H c. O 7+ d. Li 2+ e. He + 16. Which of the following reactions represents ionization energy? a. Na(s) Na + (aq) + e b. Na(s) + e Na (aq) c. Cl(g) + e Cl (aq) d. Cl(g) Cl + (g) + e e. None of the above represent ionization energy. 17. Determine ΔE for the n = 1 to n = 5 transition in the O 7+ ion. a. 2.09 x 10 18 J b. 1.34 x 10 16 J c. 6.74 x 10 8 J d. 1.39 x 10 17 J e. 1.74 x 10 18 J

18. Which of the following sets of quantum numbers appropriately describes ONE orbital in the 3d subshell? a. n = 3, l = 3, m l = 0 b. n = 4, l = 3, m l = 3 c. n = 2, l = 1, m l = 1 d. n = 5, l = 2, m l = 2 e. n = 3, l = 2, m l = 1 19. How many electrons in a single atom can have the n = 3, l = 1 designation? a. 1 b. 2 c. 4 d. 6 e. 10 20. Using the Bohr equation, calculate the amount of energy needed to remove the electron from 1.8 moles of He + ions. a. +8.72 x 10 18 J b. +1.97 x 10 7 J c. +5.25 x 10 6 J d. +9.45 x 10 6 J e. +4.66 x 10 18 J

MORE CHAPTER 8 PRACTICE TEST QUESTIONS Information that most likely will be on the front cover of your exam: J = kgm 2 /s 2 c = 3.00 x 10 8 m/s E=hν E=hc/λ h = 6.626 x 10 34 J s c = λν λ = h/mu 2 1/λ = R(1/n 1 1/n 2 2 ) ΔE = 2.18 x 10 18 J(z 2 2 /n f z 2 /n 2 i ) Rydberg constant = 1.096776 x 10 7 m 1 1. Which of the following transitions in a hydrogen atom will emit a photon with the longest wavelength of light? a. n = 3 to n = 4 b. n = 5 to n = 4 c. n = 2 to n = 1 d. n = 2 to n = 5 e. n = 3 to n = 2 2. Which of the following objects would you estimate to have the shortest debroglie wavelength if they are all traveling at the same speed? a. baseball b. marble c. bowling ball d. electron e. pebble 3. Which of the following statements is TRUE? a. If we determine the location of an electron, we can also determine it s path. b. Electrons can behave as waves or as particles, depending on the situation. c. Emission of light by an atom is an endothermic process. d. The Bohr model (or equation) works well to predict the atomic spectra of most atoms. e. None of the above are true. 4. How many orbitals in an atom can have the n = 4, l = 3 designation? a. 3 b. 5 c. 7 d. 10 e. 14

5. Determine the ground state electron configuration for Se + ion. a. [Ar]4s 2 3d 10 4p 5 b. [Ar]4s 2 3d 10 4p 4 c. [Ar]4s 2 3d 10 4p 6 d. [Ar]4s 2 3d 10 4p 3 e. [Ar]4s 1 3d 10 4p 4 6. Determine the set of quantum numbers that describe the last electron added to a Zn atom. (Zinc is element #30) n l m l m s a. 4 0 0 ½ b. 3 2 +2 ½ c. 4 2 1 + ½ d. 3 1 0 + ½ e. 2 1 +1 + ½ 7. Use the Bohr equation to calculate the amount of energy required to remove the electrons from 0.33 moles of Li 2+ ions. a. 1.18 x 10 7 J b. 1.96 x 10 17 J c. 2.87 x 10 7 J d. 3.90 x 10 6 J e. 1.73 x 10 6 J 8. Which of the following bonds has the least ionic character? a. Na Cl b. N O c. B F d. I F e. B N 9. Place the following in order of increasing atomic radius. a. Li < N < As < Cl b. N < Li < Cl < As c. As < Cl < N < Li d. Cl < As < Li < N e. Li < N < Cl < As Li N As Cl

10. Place the following bonds in order of increasing ionic character. a. N O < As O < As F b. As F < As O < N O c. As F < N O < As O d. N O < As F < As O e. As O < As F < N O As O As F N O 11. Which of the following is the longest bond? a. Si O b. Si S c. P I d. O Cl e. S Br 12. Place the following in order of decreasing lattice energy. a. KBr > RbI > MgS b. KBr > MgS > RbI c. RbI > KBr > MgS d. MgS > RbI > KBr e. MgS > KBr > RbI KBr RbI MgS 13. Which of the following reactions represents electron affinity? a. O (g) + e O (g) b. Mg (g) Mg + (g) + e c. O 2 (g) 2O (g) d. Ca + (g) Ca 2+ (g) + e e. None of the above represent electron affinity. 14. Which of the following is paramagnetic? a. Nb 3+ b. Ti 4+ c. Sr d. Zn e. None of the above.

15. Place the following in order of decreasing atomic size. a. O > Se > Ca > Rb b. Rb > Se > Ca > O c. Rb > Ca > Se > O d. O > Ca > Se > Rb e. Ca > Rb > O > Se Se O Ca Rb 16. Place the following in order of decreasing ionic size. a. Sr 2+ > Rb + > Se 2 > Br b. Sr 2+ > Rb + > Br > Se 2 c. Br > Se 2 > Sr 2+ > Rb + d. Rb + > Br > Se 2 > Sr2 + e. Se 2 > Br > Rb + > Sr 2+ Sr 2+ Se 2 Br Rb + 17. Determine the identity of the Period 2 element that possesses the following ionization energies (in MJ/mol). IE 1 = 1.09 IE 2 = 2.35 IE 3 =4.62 IE 4 =6.22 IE 5 = 37.83 IE 6 = 47.28 a. O b. N c. C d. B e. Be 18. Which of the following species are paramagnetic? a. Ca b. S 2 c. Zn 2+ d. Sr 2+ e. None of the above are paramagnetic. 19. Which of the following has the highest IE 3? a. P b. Mg c. Al d. O e. N

20. Consider the ionization energies (IE 1 ) for the following elements. Choose the statement below that best explains these observed values. P = 1012 kj/mol S = 999 kj/mol Cl = 1256 kj/mol a. Ionization energy always increases as atomic size decreases. b. Chlorine has an unusually high IE 1 because it has a very high electron affinity. c. Phosphorus has an unusually high IE 1 because it doesn t typically form ionic compounds. d. Sulfur has a lower IE 1 than would be predicted because the loss of one electron leaves sulfur with a stable, half filled p subshell. e. None of these statements explains the observed IE 1 values for these elements. 21. Which of the following statements is TRUE concerning the following table of ionization energies? kj/mol IE 1 IE 2 IE 3 IE 4 IE 5 IE 6 IE 7 IE 8 X 580 1815 2740 11,600 14,821 18,354 23,294 27,428 Y 785 1575 3227 4350 16,068 19,797 23,751 29,247 Z 1010 1905 2910 4957 6265 21,238 25,390 29,831 A 998 2248 3352 4550 6995 8484 27,070 31,676 D 1250 2295 3817 5152 6533 9349 11,000 33,557 a. Element X contains 4 valence electrons. b. Element D could be Cl. c. Element Z may be Si. d. Element Y is most likely P. e. None of the above statements are true. 22. Which of the following will be MOST attracted to a magnetic field (most paramagnetic)? a. Mn b. Co c. Zn 2+ d. Sc e. Ar 23. How many of the following species are paramagnetic? a. 0 b. 1 c. 2 d. 3 e. 4 Cd 2+ Se Ti 2+ Br