Chemistry 2 Chapter 13: Electrons in Atoms Please do not write on the test Use an answer sheet! 1 point/problem 45 points total

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1 Chemistry 2 Chapter 13: Electrons in Atoms Please do not write on the test Use an answer sheet! 1 point/problem 45 points total 1. Calculate the energy in joules of a photon of red light that has a frequency of 4.35 x s 1. a x x c x d x e x Write the electron configuration for the atom Rb, using the appropriate noble-gas for abbreviation. a. [Ne]5s 1 b. [Kr]5s 1 c. [Ar]5s 1 d. [Ne]4s 1 e. [Ar]4s 1 3. Is energy emitted or absorbed when the electronic transition from n = 3 to n = 6 occurs in hydrogen? a. emitted b. absorbed 4. How many electrons can occupy a 5f subshell? 0 b. 12 c. 14 d. 8 e How many electrons can occupy a 3p subshell? 0 b. 12 c. 14 d. 2 e What is the maximum number of electrons that can occupy a 3d subshell? d. 5 e What is the maximum number of electrons that can occupy a 3s subshell?

2 d. 5 e. 6 f Identify the element that corresponds to the following electron configuration: [Ar]4s 2 3d 10 4p 4. a. Se b. S c. Ge d. Cr e. Br 9. Which one of the following subshells contains only one orbital? a. 5d b. 6f c. 4s d. 3d 10. Calculate the wavelength in m of microwave radiation that corresponds to an energy of 2.63 J/mol photons. a b x x d x 10 7 e x Calculate the frequency in s 1 of ultraviolet radiation that has a wavelength of 248 nm. a c x d x e Identify the element that corresponds to the following electron configuration: [Kr]5s 2 4d 10 5p 1. a. Y b. In c. Sb d. Ga e. Al

3 13. Identify the element that corresponds to the following electron configuration: 1s 2 2s 2 2p 6 3s 2 3p 5. a. F b. Cl c. Br d. I 14. Of the following regions of the electromagnetic spectrum, which one has the shortest wavelength? a. X-rays b. radio waves c. microwaves d. gamma rays e. ultraviolet f. infrared 15. Calculate the frequency in hertz of a radar wave with a wavelength of 125 mm. a x x c x 10 6 d. 240 e How many orbitals are there in a 4p subshell? 17. An atom in the ground state a. has all electrons in the n = 1 orbital. b. is finely divided. c. will not absorb electromagnetic radiation of any wavelength. d. has all electrons in the lowest-energy orbits possible. 18. The energy from the right type of radiation can be used to make a molecule vibrate faster. Light of wavelength 3.34 x 10 6 m can excite vibrations in HCl. What is the energy of a photon with this wavelength? a x J b x J c x J d x J e x 10 4 J

4 19. Identify the element that corresponds to the following electron configuration: [Ne]3s 2 3p 1. a. B b. C c. Al d. Si e. Ga 21. The Heisenberg uncertainty principle states that it is impossible to precisely know both the position and the of an electron in an atom. a. mass b. color c. momentum d. shape 22. In the hydrogen atom, which of the following orbitals has the lowest energy? a. 5s b. 3p d d. 6d e. 4p 23. How many subshells are there in an energy level with n = 3? 24. What is the lowest-numbered principal shell in which d orbitals are found? 25. What is the lowest-numbered principal shell in which s orbitals are found? 26. What is the lowest-numbered principal shell in which p orbitals are found?

5 27. What is the lowest-numbered principal shell in which f orbitals are found? 28. Who discovered the electron and proposed the Plum-Pudding model? a. J. J. Thomson b. Niels Bohr c. E. Rutherford d. John Dalton e. Albert Einstein 29. How does the energy of an electron change as it moves away from the nucleus? a. decreases b. increases c. stays the same 30. What is the shape of the 3p atomic orbital? a. No clue, since Mr. Schmidt s pictures looked fuzzy. b. sphere c. dumbbell d. bar e. square 31. Who proposed the planetary model of the atom? a. J. J. Thomson b. Niels Bohr c. E. Rutherford d. John Dalton e. Albert Einstein 32. Who ushered in today s atomic model with his work on atoms? a. J. J. Thomson b. Niels Bohr c. E. Rutherford d. John Dalton e. Albert Einstein 33. Which of the following energy levels is the lowest? a. 3d

6 b. 4s c. 4p f 34. If three electrons are available to fill three empty 2p orbitals (oxygen), how will the electrons be distributed in the three orbitals? a. one electron in each orbital b. two electrons in each orbital c. three electrons in each d. oxygen is a gas, therefore has no electrons 35. If two electrons occupy the same orbital, what is the direction of their spins? a. electrons do not spin-ever! b. opposite spin c. always counterclockwise d. always clockwise 36. What is the next atomic orbital in the series: 1s, 2s, 2p, 3s, 3p? a. 2d f d d. 3f e. 4s 37. How many half-filled orbitals are there in a bromine atom (hint: drawing an arrow diagram will help!). 38. According to the Aufbau principle: a. an orbital may be occupied by only two electrons b. electrons in the same orbital must have opposite spins c. electrons enter orbitals of highest energy first d. electron enter orbitals of lowest energy first 39. How does the speed of light change as light moves from a distant star toward earth in the vacuum of space? a. Speed decreases b. Speed increases c. Remains constant 40. The amplitude of a wave is the measure of the. a. distance between crests

7 b. number of cycles per unit time c. height from origin to crest d. number of particles in a wave front 41. Which of the following electromagnetic waves have the highest frequencies? a. uv b. x-rays c. microwaves d. gamma waves e. infrared waves 42. The light given off by an electric charge through Ne vapor is. a. continuous spectrum b. a single wave c. an emission spectrum d. white light 43. The lowest energy state of an atom is called. a. excited state b. ground state c. confused chemistry state 44. Which of the following quantum leaps would be associated with the greatest energy of emitted light? a. n=5 to n=1 b. n=1 to n=5 c. n=2 to n=5 d. n=5 to n=2 e. n=5 to n=3 45. Which of the following terms describes your first weeks in Chemistry 2? a. treading water b. dog paddling c. record time in the freestyle d. stuck at the bottom of the pool.

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