1. a. Calculate the wavelength of electromagnetic radiation that has a frequency of 5.56 MHz. b. Calculate the frequency of electromagnetic radiation that has a wavelength equal to 667 nm. 2. Electromagnetic radiation at the blue end of the visible spectrum has a wavelength of 400 nm. a. Calculate the frequency of the radiation. b. Calculate the energy of one photon of this radiation. c. Calculate the energy of one mole of photons of this radiation.
3. From the emission spectrum for hydrogen a. How many lines appear in the visible region (Balmer series)? b. Why so few? The Lyman series occurs in the UV region. c. How many lines would you expect in the Lyman series? 4. Calculate the frequency of the line in the hydrogen spectrum corresponding to the electron transition from n=9 to n=8. Whereabouts in the electromagnetic spectrum does this line occur? 5. Describe the electron density pattern for a a. 2s orbital b. 3p x orbital c. 3d xy orbital
6. Write the electron configurations of the following elements using the shorthand notation for the noble gas cores. a. phosphorus b. nickel c. osmium d. californium e. titanium 7. Which orbital is filled following these orbitals? a. 3d b. 4s c. 5p d. 5f
8. How many electrons can be accommodated in a. a d subshell b. a set of f orbitals c. the n = 4 shell d. the 7s orbital e. a p x orbital 9. What is wrong with the following ground state electron configurations?
10. How many unpaired electrons are there in a. a nitrogen atom b. an iodine atom c. a nickel (II) cation d. an oxide ion? 11. Arrange the elements S, Ge, P, and Si in order of increasing atomic size. 12. Arrange the ions Na +, K +, Cl, and Br in order of increasing size. 13. Arrange the elements Be, Ca, N, and P in order of increasing ionization energy.
14. Which one of each of the following pairs would you expect to have the higher electron affinity? a. Cl or Cl b. Na or K c. Br or I 15. Which elements fit the following descriptions: a. the smallest alkaline earth metal b. has a valence shell configuration 4f 14 5d 10 6s 1 c. the halogen with the lowest ionization energy d. has 13 more electrons than argon e. the smallest non metal
f. the Group 4A element with the largest ionization energy g. its 3+ ion has the electron configuration [Kr] 4d 10 16. Which electronic transition in the hydrogen atom results in the emission of visible light? A. n = 3 to n = 2 B. n = 3 to n = 1 C. n = 4 to n = 3 D. n = 2 to n = 4 E. n = 2 to n = 6 17. The maximum number of electrons in an atom that can have quantum numbers n = 5, l= 3 is A. 2 B. 6 C. 8 D. 10 E. 14 18. Which compound is expected to have the strongest ionic bond? A. NaF B. KF C. RbF D. KCl E. NaCl 19. What is the electron configuration of the Ti 3+ ion? A. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 2 4s 2 B. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 2 C. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 1 D. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 E. 1s 2 2s 2 2p 6 3s 2 3p 6
20. What is the total number of completely or partially filled p orbitals in a gaseous arsenic atom in the ground state? A. 3 B. 6 C. 8 D. 9 E 10 21. When placed in the highest to lowest order for ionization energy, what is the correct order for the species, Cl -, Ar, K +? A. Cl - > Ar > K + B. Ar > K + > Cl - C. K + > Cl > Ar, D. K + > Ar > Cl - E. Cl - = Ar = K + 22. Which element has the largest first ionization energy? A. Be B. B C. C D. N E. O 23. Which energy transition in the hydrogen atom will be the greatest? A. n=2 to n=1 B. n=3 to n=2 C. n=4 to n=3 D. n=5 to n=4 E. n=6 to n=5 24. The elements in which of the following have most nearly the same atomic radius? A. Be, B, C, N B. Ne, Ar, Kr, Xe C. Mg, Ca, Sr, Ba D. C, P, Se, I E. Cr, Mn, Fe, Co
25. Which of the following represents the ground state electron configuration for the Mn 3+ ion? (Atomic number Mn = 25) A. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 4 B. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 5 4s 2 C. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 2 4s 2 D. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 8 4s 2 E. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 3 4s 1 26. In the periodic table, as the atomic number increases from 11 to 17, what happens to the atomic radius? A. It remains constant. B. It increases only. C. It increases, then decreases. D. It decreases only. E. It decreases, then increases. Use these answers for questions 19-22. A. 1s 2 2s 2 2p 5 3s 2 3p 5 B. 1s 2 2s 2 2p 6 3s 2 3p 6 C. 1s 2 2s 2 2p 6 2d 10 3s 2 3p 6 D. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 5 E. 1s 2 2s 2 2p 6 3s 2 3p 6 3d 3 4s 2 27. An impossible electronic configuration 28. The ground-state configuration for the atoms of a transition element 29. The ground-state configuration of a negative ion of a halogen 30. The ground-state configuration of a common ion of an alkaline earth element
Use these answers for questions 31-33 A. Heisenberg uncertainty principle B. Pauli exclusion principle C. Hund's rule D. Shielding effect E. Wave nature of matter 31. Can be used to predict that a gaseous carbon atom in its ground state is paramagnetic 32. Indicates that an atomic orbital can hold no more than two electrons 33. Predicts that it is impossible to determine simultaneously the exact position and the exact velocity of an electron 34. All of the following statements concerning the characteristics of the halogens are true EXCEPT A. The first ionization energies (potentials) decrease as the atomic numbers of the halogens increase. B. Fluorine is the best oxidizing agent. C. Fluorine atoms have the smallest radii. D. Iodine liberates free bromine from a solution of bromide ion. E. Fluorine is the most electronegative of the halogens. Questions 35-36 Consider atoms of the following elements. Assume that the atoms are in the ground state. A. S B. Ca C. Ga D. Sb E. Br 35. The atom that contains exactly two unpaired electrons. 36. The atom that contains only one electron in the highest occupied energy sublevel.
37. The effective nuclear charge experienced by the outermost electron of Na is different than the effective nuclear charge experienced by the outermost electron of Ne. This difference best accounts for which of the following? A. Na has a greater density at standard conditions than Ne. B. Na has a lower first ionization energy than Ne C. Na has a higher melting point than Ne. D. Na has a higher neutron-to-proton ratio than Ne. E. Na has fewer naturally occurring isotopes than Ne. FREE RESPONSE 1. The emission spectrum of hydrogen consists of several series of sharp emission lines in the ultraviolet (Lyman series), the visible (Balmer series), and the infrared (Paschen series, Brackett series, Pfund series, etc,) regions of the spectrum. a. Why does the emission spectrum consist of discrete wavelengths rather than a continuum wavelength? b. What feature of Bohr's model (other than wavelength) distinguishes one series of lines from another? In other words what makes the Lyman series different from the Balmer, etc. c. Draw and label an electron energy level diagram for the hydrogen atom and indicate on it the transition corresponding to the line of lowest frequency in the Balmer series.
d. One of the wavelengths of light in the Balmer series is 410 nm. Calculate the frequency and energy of this wavelength. 2. Consider an atom of titanium. a. Write the complete electron configuration of titanium. b. Write the complete electron configuration of Ti 2+. c. Write the chemical formula for titanium (IV) oxide. Would you expect the titanium oxide to be colored? Explain your answer. d. Predict the relative values of the first ionization energy of calcium and titanium. Explain the basis of your prediction.
CDO AP Chemistry Unit 5 3. The values of the first ionization energies of the period 3 elements are given in units of KJ/mol Na = 495; Mg = 738; Al = Si = 786; P = 1012; S = 1000; Cl = 1251; Ar = 1521 a. State the general trend and explain the trend using the terms screening effect and effective nuclear charge. b. Explain why the first ionization energy of sulfur is lower than that of phosphorus. c. Explain why the first ionization energy of aluminum is lower than that of magnesium. d. Predict the relative values of the second ionization energies of sodium and magnesium. Explain your reasoning. e. Why is the first ionization energy of potassium lower than that of sodium? CDO AP Chemistry Fall 2015