Practice Final # Jim and Tim s Excellent Adventure s in Final Exam Preparation. Practice Final

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1 Jim and Tim s Excellent Adventure s in Final Exam Preparation Practice Final What element has the electron configuration 1s 2 2s 2 2p 6 3s 2 3p 1? A. Na B. B C. C D. Co E. Al 2. Which of the following atoms has the most unpaired electrons in its ground state? A. Zn B. Bi C. Rn D. Po 3. In the photoelectric effect, brighter light of a given wavelength produces A. decreased attraction of the electrons to the metal. B. more photoelectrons. C. no effect. D. higher energy photoelectrons. E. higher frequency light. 4. According to the Bohr model of the hydrogen atom, which of the following gives light emission with the highest energy? A. from n = 4 to n = 2 B. from n = 6 to n = 5 C. from n = 1 to n = 5 D. from n = 5 to n = 6 E. from n = 3 to n = 1 Page 1

2 5. In the photoelectric effect, brighter light of a given wavelength produces A. decreased attraction of the electrons to the metal. B. more photoelectrons. C. no effect. D. higher energy photoelectrons. E. higher frequency light. 6. If an electron is in an orbital with 3 radial nodes and 3 angular nodes, what type of orbital is the electron occupying? A. 5s B. 2p C. 4d D. 6s E. 7f 7. Which is not a valid set of quantum numbers for an electron? A. n = 6, l = 2, ml = 0, ms = 1/2 B. n = 3, l = 2, ml = -2, ms = 1/2 C. n = 7, l = 0, ml = 0, ms = 1/2 D. n = 17, l = 16, ml = 16, ms = -1/2 E. n = 4, l = -2, ml = 2, ms = -1/2 8. Which statement(s) is (are) FALSE in comparing the electronic transition from n i = 5 to n f = 2 in H with that of electronic transition from n i = 2 to n f = 5 in Be 3+ A. A photon of the same frequency is involved in both transitions, but is emitted the H electronic transition and absorbed in the Be 3+ electronic transition. B. Two of the other four statements are FALSE C. The photon involved in the H transition lies in the visible spectrum while that involved in the Be 3+ transition lies in the UV region of the spectrum. D. The transition in H is a Balmer emission series line E. The wavelength of the photon emitted by H is 16 times the wavelength of the photon absorbed by Be What can be correctly calculated or determined using the Bohr model of the hydrogen atom? A. We can determine the wavelengths of line spectra for all atoms. B. We can determine the location of all electrons in all atoms. C. We can find the frequencies for the line spectrum of hydrogen. D. We can determine the location of the electron in the hydrogen atom. E. We can calculate the wavelength maximum for black body radiation. Page 2

3 10. Arrange the following atoms in the probable increasing order [smallest (1) to largest (4)] of their second ionization energies: Rb, Ca, Kr, I. A. (1) Ca, (2) I, (3) Kr, (4) Rb B. (1) I, (2) Kr, (3) Ca, (4) Rb C. (1) Rb, (2) Ca, (3) Kr, (4) I D. (1) Kr, (2) I, (3) Ca, (4) Rb 11. Why is it that isoelectronic ions with the same electron configuration do not have the same ionic radii? A. Different energy levels are occupied. B. Even though they have the same number of electrons, they have different effective nuclear charges. C. Nuclei are different sizes. D. There is more electron repulsion in the negative ions because extra electrons have been added. E. Isotopes have different masses and sizes. 12. What species has the largest radius? A. K B. S C. Ca 2+ D. Mg Which of the following shows the correct order for ionization energy? A. Cl > Si < Na B. Cl < Si < Na C. Cl < Si > Na D. Cl > Si > Na E. Na < Si = Cl 14. Give the orbital diagram for the electrons beyond the noble gas core in Hf. A. B. C. D. E. Page 3

4 15. Which of the following shows the correct order for ionization energy? A. Cl > Si < Na B. Cl < Si < Na C. Cl < Si > Na D. Cl > Si > Na E. Na < Si = Cl 16. Which principle(s) or rule(s), if any, does this configuration violate? A. rules for acceptable quantum numbers and atomic orbitals B. the Aufbau principle C. Hund's rule D. the Aufbau principle and Hund's rule E. none F. Pauli exclusion principle 17. What is the central atom in SO 2Cl 2? A. O B. both Cl C. both O D. S E. Cl 18. Which of the following species is not paired correctly with its ionic geometry? A. ClO 3- ; trigonal planar B. CO 3 2- ; trigonal planar C. I 3- ; linear D. SO 4 2- ; tetrahedral 19. Which of the following molecules is nonpolar? A. XeO 3 B. ClF 3 C. AsF 3 D. BF Which of the following molecules have the same geometries? A. SF 4 and CH 4 B. CO 2 and H 2O C. CO 2 and BeH 2 D. N 2O (NNO) and NO 2 Page 4

5 21. Which of the following is the correct Lewis structure of IF4 +? A. B. C. D. 22. The sulfur atom, with a formal charge of zero in the resonance structure of SO 3-2, has around it: A. three single bonds and one lone pair B. two double bonds, one single bond and a lone pair C. three double bonds and a lone pair D. one triple bond and a double bond E. two single bonds, one double bond and a lone pair 23. Which of the following should NOT have a dipole moment? A. O 3 B. PF 5 C. IBr D. IF 5 E. PH What is the formal charge on B in BF 4-? A. 1 B. -1 C. 2 D. 0 E. -2 Page 5

6 25. Predict the geometry and polarity of the CS 2 molecule. A. linear, polar B. linear, nonpolar C. tetrahedral, nonpolar D. bent, nonpolar E. bent, polar 26. Choose the correct statement about the compound SO 2 A. The two S-O bonds have different lengths and angles, since one is a single bond and the other a double bond. B. The S-O bonds are ionic in character. C. The molecule has a linear structure. D. The S atom has an unshared electron pair. 27. Although VSEPR usually is used to predict bond angles, it can be used to predict relative bond distances (or bond lengths). In the molecule PCl 5, the five P-Cl bond lengths are not the same. Which one(s) would you expect to be longer, which one(s) shorter, and why? A. One of the axial Cl's and two of the equatorial Cl's are longer. B. Axial Cl's are longer than equatorial Cl's. C. All five P-Cl bond lengths are the same. The question is false. D. Axial Cl's are shorter than equatorial Cl's. 28. Determine which of the following statements about the heteronuclear OF - ion is incorrect. A. OF is diamagnetic. B. The bond order is intermediate between O 2 and F 2. C. OF - has eight antibonding electrons. D. OF - has 10 bonding electrons. 29. Which of the following is not correctly matched with the hybridization about the central Xe atom? A. XeF 2; sp 3 d B. XeOF 4; sp 3 d 2 C. XeF 4; sp 3 D. XeO 3; sp The glow of C 2 can be seen at the edge of candle flames. What is the molecular orbital diagram of C 2? A. B. C. D. Page 6

7 31. What is the hybridization of nitrogen in the NH 4 + ion? A. 4sp B. s 2 p 2 C. sp 3 d D. sp 3 E. None of the above 32. What is a characteristic of an antibonding orbital? A. a high probability of finding electrons away from the region between bonded atoms B. has more than 2 electrons C. has no electrons D. a high probability of finding electrons parallel to the region between bonded atoms E. a high probability of finding electrons in the region between bonded atoms 33. Which of the following has the highest bond order according to the MO Theory? A. B 2 B. C 2 C. N 2 D. O 2 E. F The hybridization that agrees with the molecular geometry around the central atom in IF 5 is: A. sp B. sp 2 C. sp 3 D. sp 3 d E. sp 3 d Which of the following has a see-saw structure? A. BF 4 - B. BrF 4 - C. SeF 4 D. SiF 4 E. XeF Predict which of the following is not probable. A. a tetrahedral GeCl 4 molecule B. a trigonal planar BCl 3 C. a bent HCN molecule D. a T-shaped BrF 3 molecule E. a trigonal bipyramidal PCl 5 molecule Page 7

8 37. What hybrid orbitals are on the C atom in CH 3Cl A. sp 2 B. sp 3 d 2 C. sp 2 d D. sp 3 d E. sp Why doesn't the NO 2F molecule have a dipole moment of zero? A. The NO bonds are different lengths. B. Unshared electrons cause an asymmetrical charge distribution. C. There are more unshared electrons on one oxygen atom than the other. D. While the bonds are symmetrically arranged, they are unequal in the magnitude of their polarities. E. The bonds are not symmetrically arranged. 39. Which of the following leads to strong dispersion forces? a) small electronegative atoms b) polar bonds c) elongated molecules d) polarizability A. b, c, and d B. b and c C. c and d D. c E. a and b 40. Which of these molecules can form hydrogen bonds? A. N(CH 3) 3 B. PH 3 C. BH 3 D. HOCH 3 E. CH 3F 41. Arrange the following substances in the expected order of increasing melting point: CsCl, MgCl2, NaCl A. NaCl < MgCl 2 < CsCl B. Because these are all ionic compounds, their melting points are the same. C. MgCl 2 < CsCl < NaCl D. CsCl < NaCl < MgCl 2 E. MgCl 2 < NaCl < CsCl Page 8

9 42. Which of the following exhibits the largest dipole-dipole forces? A. CO 2 B. HCl C. N 2 D. CH 4 E. IBr 43. Which of the following can experience intermolecular forces other than London dispersion forces? A. carbon monoxide gas B. fluorine gas C. liquid carbon dioxide D. oxygen gas E. white phosphorus 44. In a glass of water, the molecules of water are kept in the glass and held to one another by: A. covalent bonds B. intermolecular forces C. ionic bonds D. shared electrons E. intramolecular forces 45. Which of the following is true concerning the distribution of alkali metals in the earth's crust? A. All have low abundances. B. The abundance for Fr is just 15 g/ton. C. Cs is the least abundant. D. Na and K have above-average abundances. E. All are abundant except Fr. 46. Which 2A element is present in the body in the greatest amount? A. Ba B. Be C. Sr D. Ca E. Mg 47. Why do group 2A elements have higher densities than group 1A? A. The 2A elements have more electrons. B. The masses of 2A elements are larger and the sizes are smaller. C. The masses of 2A elements are smaller and the sizes are smaller. D. The masses of 2A elements are larger and the sizes are larger. E. The masses of 2A elements are smaller and the sizes are larger. Page 9

10 48. What are some ways that Be and its compounds differ from the other elements in Group 2A? a. Be is much harder than the other Group 2A elements. b. Be has lower electrical conductivity than the other Group 2A elements. c. BeO reacts with water. d. BeCl2 is not an ionic compound. A. a B. a and d C. a and b D. b and c E. b 49. Write the formula of a tetraaquadichlorochromium(iii) ion. A. [CrCl 2 4H 2O] + B. [Cr(H 2O)4] 3+ Cl 2 C. [CrCl 2(H 2O)4] + D. [(H2O) 4Cl 2Cr 3] + E. [Cr(H2O) 4Cl 2] What is the name of the coordination compound that has the formula NH 4[Cr(NCS) 4(NH3) 2]? A. ammonium tetrathiocyanato-n diamminechromate(iii) B. ammonium diamminetetrathiocyanato-o chromate(iii) C. ammonium diamminetetrathiocyanato-n chromato(iii) D. ammonium diamminetetrathiocyanato-n chromate(iii) E. ammonia diamminetetrathiocyanato-n chromate(iii) 51. Which of the following statements associated with ligands or complex ions is incorrect? A. In a nitrito ligand, a nitrogen atom is the donor of the shared electron pair. B. An "ate" ending indicates a complex anion. C. The prefix "tris" is used for three neutral ligands when the name of the molecule has "di" in it. D. The prefix "bis" is used for two neutral ligands when the name of the molecule has "di" in it. E. The prefix "tetrakis" is used for four neutral ligands when the name of the molecule has "di" in it. 52. How many unpaired electrons are in the complex ion [Co(NO 2) 6] 4-? A. four B. one C. three D. five E. two Page 10

11 53. Which of the following complex ions are paramagnetic? a.[zn(h 2O)4] 2+ b.[cocl 4] - c.[cr(cn) 6] 4- A. c only B. a only C. b only D. b and c E. none of the above 54. Which of the following statements associated with isomers is incorrect? A. Structural isomers differ in the way the ligands are attached on the donor atoms. B. Isomers of any type have the same empirical formula. C. Enantiomers have superimposable mirror images. D. Cis isomers have two ligands adjacent along an edge, while trans isomers have ligands opposite. E. A compound that is a structural isomer of one compound can be a geometric isomer of a third compound. 55. A curie, Ci, is a common unit for measuring radiation. A curie is the amount of a radionuclide that has the same activity as one gram sample of radium-226: x 1010 disintegrations s -1. A smoke detector has 1.00 µci of 241 Am, which has a half-life of years. How many grams of 241 Am does the detector contain? A x 10-7 g B x g C x g D x g E g 56. When we bombard thorium-230 with a proton, we form an isotope that is naturally radioactive. Two alpha particles are byproducts of the reaction. What is the isotope? A. Ac B. Fr C. Fr D. Np E. Dy Page 11

12 57. The half-life of 197 Hg, which is used in kidney scans, is 1.08 x 10-2 hr. Determine the activity in Ci of a 3.00 ng sample of this isotope A x atoms s -1 B x atoms s -1 C x atoms s -1 D x atoms s -1 E x atoms s The mass of a strontium-95 atom is u. What is the binding energy of an atom of strontium-95? Necessary masses are: e = u; p = u; n = u A MeV B MeV C MeV D MeV E x 10 4 MeV 59. In the case of radioactive element X, which decays by electron emission with a half-life of four days to a stable nuclide of element Z. A. Two grams of element X is required to produce 1.5 grams of element Z after eight days. B. Element Z will weigh more than element X when decay is complete, since Z has the higher atomic number. C. After eight days the sample will consist of one-fourth element Z and three-fourths elements X. D. Element Z will weigh considerably less than element X after decay is complete because of the loss of electrons. 60. Which one of the following nuclear changes does not represent alpha particle emission? A Cm --> Pu B Ra --> Rn C U --> Ac D U --> Ac Page 12

Bonding/Lewis Dots Lecture Page 1 of 12 Date. Bonding. What is Coulomb's Law? Energy Profile: Covalent Bonds. Electronegativity and Linus Pauling

Bonding/Lewis Dots Lecture Page 1 of 12 Date Bonding What is Coulomb's Law? Energy Profile: Covalent Bonds Electronegativity and Linus Pauling 2.1 H 1.0 Li 0.9 Na 0.8 K 0.8 Rb 0.7 Cs 0.7 Fr 1.5 Be 1.2