Exam 1 Study Guide and Practice Problems Key Student’s Learning Outcomes: As a result of these practice problems, students will be able to: Chapter 7 a. b. c. d. e. f. g. h. i. j. k. l. m. n. o. p. q. r. s. t. u. Define the wavelength and frequency of a wave. Relate the wavelength, frequency, and speed of light. Describe the different regions of the electromagnetic spectrum. State Planck’s quantization of vibrational energy. Define Planck’s constant and photon. Describe the photoelectric effect. Calculate the energy of a photon from its frequency or wavelength. State the postulates of Bohr’s theory of the hydrogen atom. Relate the energy of a photon to the associated energy levels of an atom. Determine the wavelength or frequency of a hydrogen atom transition. Describe the difference between emission and absorption of light by an atom. State the de Broglie relation. Calculate the wavelength of a moving particle. Define quantum mechanics. State Heisenberg’s uncertainty principle. Relate the wave function for an electron to the probability of finding the electron at a location in space. Define atomic orbital. Define each of the quantum numbers for an atomic orbital. State the rules for the allowed values for each quantum number. Apply the rules for quantum numbers. Describe the shapes of s, p, and d orbitals. Chapter 8 a. b. c. d. e. f. g. h. i. j. k. l. m. n. o. p. q. r. s. Define electron configuration and orbital diagram. State and apply the Pauli Exclusion Principle. Define building-up principle. Define noble-gas core and valence electron. Define main-group element, transition element, & inner-transition elements, and s-block, p-block, d-block and fblock. Determine the configuration of an atom using the building-up principle. Determine the configuration of an atom using the period and group number. Write electronic configurations for atoms and ions using the shorthand noble gas notation. State and apply Hund's rule. Define paramagnetic substance and diamagnetic substance. Write electronic configuration and orbital diagram for anions and cations. State the general periodic trends in size of atomic radii. Define effective nuclear charge. Determine relative atomic sizes from periodic trends. State the general periodic trends in ionization energy. Define first ionization energy. Define electron affinity. State the broad general trend in electron affinity across any period. Define basic oxide, acidic oxide, and amphoteric oxide. 1 t. State the main group corresponding to an alkali metal, an alkaline earth metal, a chalcogen, a halogen, and a noble gas. CHM 1040 Review a. b. c. d. Limiting Reactant Molarity Dilution Solution Stoichiometry 1. Lead(II) carbonate is prepared according to the following reaction: Pb(C2H3O2)2(aq) + H2O(l) + CO2(g) → PbCO3(s) + 2HC2H3O2(aq) What is the theoretical yield of acetic acid, HC2H3O2, when 5.95 g of lead(II) acetate are mixed with 1.25 g of carbon dioxide and excess water? 2. How many grams of solid NaOH must be added to 10.0 mL of 0.250 M AlCl 3 to exactly precipitate all of the aluminum? (Adding excess hydroxide causes the aluminum to dissolve again.) Write the balanced chemical equation before you start solving the problem. 3. What is the frequency and energy of a photon of green light with a wavelength of 525.1 nm? 4. An electron in a hydrogen atom undergoes a transition from n = 4 to n = 1. a. Is the photon absorbed or released? b. What is the energy of the photon involved? 2 c. What is the wavelength of the photon involved? 5. What is the wavelength of an electron moving at 4.05 x 106 m/s? The mass of an electron is 9.10939 x 10-31 kg. 6. Label each as Allowed (A) or Not Allowed (NA). Explain if it is not allowed. a. n = 2, l = 1, ml = 2, ms = +½ NA; for l = 1, ml can only be -1, 0, or +1 b. n = 2, l = 2, ml = -2, ms = -½ NA; for n = 2, l can only be 0, 1 c. n = 4, l = 2, ml = 2, ms = 0 NA; ms can only be +1/2 or -1/2 d. n = 2, l = 1, ml = 0, ms = -1/2 Allowed; no explanation required. 7. What is the name for Group IIA. → Alkaline Earth Metals/Elements Write the generic valence electron configuration. ns2 Its elements are diamagnetic or paramagnetic? Diamagnetic 8. Draw the valence shell orbital diagram of Mn. Be sure to label each subshell. Draw the electron configuration using the noble gas notation for Mn atom. [Ar]4s23d5 9. Write the following in order of increasing atomic radius: Be, Mg, Na Be < Mg < Na 10. Write the following in order of increasing ionic radius: Br-, Cl-, FF- < Cl- < Br3 11. Write the following in order of increasing first ionization energy: O, S, Se Se < S < O 12. Write the following in order of increasing first ionization energy: Al, Mg, Na Na < Al < Mg 13. Write the following in order of increasing electron affinity: Be, F, N Be < N < F 14. A proton is roughly 1800 times more massive than an electron. If a proton and an electron are traveling at the same speed, A) the wavelength of the photon will be about 1800 times longer than the wavelength of the electron. B) the wavelength of the photon will be about 1800 times longer than the wavelength of the electron. C) the wavelength of the photon will be roughly equal to the wavelength of the electron. D) the wavelength of the electron will be about 1800 times longer than the wavelength of the photon. E) the wavelength of the electron will be about 1800 times longer than the wavelength of the photon. Ans: E 15. Which one of the following sets of quantum numbers is not possible? A) A B) B Ans: B C) C D) D E) E 16. A possible set of quantum numbers to describe an electron in a 4s subshell is A) n = 4, l = 0, ml = 1 , ms = +1/2 D) n = 3, l = 1, ml = 1, ms = - 1/2 B) n = 4, l = 0, ml = 0, ms = - 1/2 E) n = 3, l = 0, ml = 0, ms = +1/2 C) n = 4, l = 1, ml = 1, ms = +1/2 Ans: B 17. Consider the element with the electron configuration [Kr]5s24d7. This element is A) a representative element. D) an actinide element. B) a transition metal. E) a noble gas. C) a nonmetal. Ans: B 18. Concerning the electron configuration of sulfur, 1s22s22p63s23p4, which of the following represents the core electrons only? A) 1s2 B) 1s22s2 C) 1s22s22p6 D) 1s22s22p63s2 E) 3s23p4 Ans: C 4 19. Since arsenic is a nonmetal, As2O3 is expected to be a/an _____ oxide. A) acidic B) ionic C) amphoteric D) neutral E) basic Ans: A Conversion Factors 1J=1 kg • m 2 (exact) s2 Physical Constants (Note: these are not exact numbers) Avogadro’s number ..................... NA = 6.0221367 x 1023 mol Electronic charge .......................... e = 1.60217733 x 10-19 C Electron rest mass ......................... me = 9.1093897 x 10-31 kg Molar gas constant ....................... R = 0.08205783 L • atm mol • K ........................ 8.314510 J mol • K ........................ 8.314510 cal mol • K Neutron rest mass ........................ mn = 1.6749286 x 10-27 kg Plank’s constant ............................ h = 6.6260755 x 10-34 J • s Proton rest mass ........................... mp = 1.6726231 x 10-27 kg Rydberg constant.......................... RH = 2.179 x 10-18 J Speed of light (in a vacuum)........ c = 2.99792458 x 108 m s 5
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