1) What type of relationship (direct or indirect) exists between wavelength, frequency, and photon energy?

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1 Chapter 7 Study Guide Name: AP Chemistry 6 points DUE AT TEST (Mon., 11/20/17) Date: Topics/people to be covered on the test: wavelength frequency c=ëí ideas of Max Planck E=hí quanta photons relationship between E and ë spectra wave-particle duality of nature de Broglie equation Bohr model ground state relationship between E and energy level degenerate excited state Heisenberg Uncertainty Principle orbital shapes Erwin Schrödinger Pauli Exclusion Principle Hund s rule quantum numbers Dmitri Mendeleev orbital diagrams Aufbau principle first ionization energy atomic radius chemical families ionization energy valence e - Practice questions: 1) What type of relationship (direct or indirect) exists between wavelength, frequency, and photon energy? 2) Microwave radiation has a wavelength on the order of 1.0 cm. Calculate the frequency and energy of a single photon of this radiation. [í=3.0 x Hz, E = 2.0 x J] 3) A photon of ultraviolet light has enough energy to mutate a strand of human DNA. What is the frequency and energy of a single UV photon with a wavelength of 25 nm? [í=1.2 x Hz, E=8.0 x J]

2 4) One type of electromagnetic radiation has a frequency of x 10-6 hertz, another type has a wavelength of 2.12 x m, and a third type has photons with energy equal to 3.97 x J each. Identify each type of electromagnetic radiation and place them in increasing order of photon energy and frequency. 5) (a) What is the difference between an orbit (Bohr model) and an orbital (quantum mechanical model)? (b) Why does the Bohr model violate Heisenberg s Uncertainty Principle? 6) (a) Draw orbital diagrams (arrows) for the elements Na, Co, and Kr. (b) How many unpaired electrons are present in each element? 7) The elements Si, Ga, As, Ge, Al, Cd, S, and Se are all used in the manufacture of various semiconductor devices. Write the expected noble gas electron configuration for these atoms. ex> lithium is [He] 2s 1 8) Write the electron configuration for the following: (a) The third element in Group 15

3 (b) Element 116 (c) An element with three unpaired 5d electrons (d) The halogen with electrons in the 6p orbitals 9) In mercury, (a) How many electrons occupy atomic orbitals with n = 3? (b) How many electrons occupy d atomic orbitals? (c) How many electrons have spin up? 10) Which of the following represent(s) an excited state? Write the ground state configuration for any that are excited. Indicate how many unpaired electrons are present in each of the ground state configurations. (a) 1s 2 2s 2 3p 1 (b) 1s 2 2s 2 2p 6 (c) 1s 2 2s 2 2p 4 3s 1 (d) [Ar]4s 2 3d 5 4p 1 11) Arrange the following groups of atoms in order of increasing atomic radius (size): (a) Te, S, Se (b) K, Br, Ni (c) Ba, Si, F 12) Arrange the following groups of atoms in order of increasing first ionization energy. (a) Te, S, Se (b) K, Br, Ni (c) Ba, Si, F

4 13) In each of the following, indicate which would have a smaller radius: (a) H or He (b) Cl, In, or Se (c) Nb, Zn, or Si (d) Na -, Na, or Na + 14) Rank the elements Be, B, C, N, and O in order of increasing first ionization energy. Explain your reasoning. 15) Barium emits photons of light with energies of 3.59 x J. What color is that? [554 nm, yellow] 16) It takes 7.21 x J of energy to remove an electron from an iron atom. What is the maximum wavelength of light that can do this? 17) p. 333 #92 18) p. 335 #130

5 19) Answer the following multiple-choice questions from p. 338-A: 1) 6) 2) 9) 4) 20) (a) Write the complete electron configuration for the Na + ion in the ground state. (b) Using principles of atomic structure, explain why the Na + ion is larger than the Li + ion. (c) Below is a representation of a portion of a crystal of LiCl. Identify the ions in the representation by writing the appropriate formula (Li + or Cl - ) below: 21) Account for the following observations in terms of atomic theory and/or quantum theory: (a) Atomic size decreases from Na to Cl in the periodic table. (b) The first ionization of K is less than that of Na. 22) The only common oxide of zinc has the formula ZnO. (a) (b) Write the electron configuration for a Zn atom in the ground state. From which sublevel are electrons removed when a Zn atom in the ground state is oxidized (forms Zn 2+ )?