{"id":2399,"date":"2018-04-11T23:52:48","date_gmt":"2018-04-12T03:52:48","guid":{"rendered":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/chapter\/end-of-chapter-material-7\/"},"modified":"2019-05-14T16:45:41","modified_gmt":"2019-05-14T20:45:41","slug":"end-of-chapter-material-7","status":"publish","type":"chapter","link":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/chapter\/end-of-chapter-material-7\/","title":{"raw":"8.6 End of Chapter Problems","rendered":"8.6 End of Chapter Problems"},"content":{"raw":"
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1. Calculate the frequency and wavelength of light that is emitted contains 3.45 x 10-18<\/sup>J of energy. \u00a0What type of light is this?<\/p>\r\n

2. Convert the following light wavelengths into frequencies (Hz). (The speed of light c=2.998 x 108<\/sup>m\/s)<\/p>\r\n

a)\u00a0 <\/span>4.33 nm\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>b)\u00a0<\/span>2.35 x 10-10<\/sup>m\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0<\/span>c)\u00a0 <\/span>735 nm\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>d) 4.57 m<\/span>m<\/p>\r\n

3. Convert the following light frequencies into wavelengths (expressing the result in the indicated units), assuming the light is moving at the speed of light (c=2.998 x 108<\/sup>m\/s)<\/p>\r\n

a)\u00a0 <\/span>4.77 GHz (m)\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>b)\u00a0<\/span>2.89 kHz (cm)\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span><\/span><\/p>\r\n

c)\u00a0 <\/span>50. Hz (mm)\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>d) 2.88 MHz (<\/span>m<\/span>m)<\/span><\/p>\r\n

4. How does the energy possessed by an emitted photon compare to the difference in energy levels that gave rise to the emission of the photon?<\/p>\r\n

5. Explain the difference between continuous and discrete spectra.<\/p>\r\n

6. Describe one aspect of Bohr\u2019s model of the atom that \u201cworked\u201d. Describe one aspect of Bohr\u2019s model of the atom that did not \u201cwork\u201d.<\/p>\r\n

7. Draw an electron shell model of the following<\/p>\r\n

a)\u00a0 <\/span>chloride ion, Cl1-<\/sup>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>b)\u00a0<\/span>calcium ion, Ca2+<\/sup><\/p>\r\n

8. In what way are outer electron shells of oxygen and selenium similar? In what way are they different?<\/p>\r\n

9. Why is the view of an electron being a particle<\/i>in a fixed orbit<\/i>unacceptable?<\/p>\r\n

10. Explain the difference between an orbit and an orbital. Briefly describe the model that each refers to.<\/p>\r\n

11. Which law(s) (e.g.: Aufbau principle, Pauli exclusion principle or Hund\u2019s rule) is (are) violated in each of these ground state electron configurations. Write the correct configuration as well.<\/p>\r\n

a)\u00a0 <\/span>B = 1s1<\/sup>2s1<\/sup>2px<\/sub>1<\/sup>2py<\/sub>1<\/sup>2pz<\/sub>1\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span><\/sup><\/p>\r\n

b)\u00a0 <\/span>Sc = [Ne] 3s2<\/sup>3p6<\/sup>3d3<\/sup><\/p>\r\n

c)\u00a0 <\/span>Na = 1s2<\/sup>1p7<\/sup>2s2<\/sup>3s1\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span><\/sup><\/p>\r\n

d)\u00a0 <\/span>C = 1s2<\/sup>2s2<\/sup>2px<\/sub>2<\/sup><\/p>\r\n

12. Write the electron configurations and show the orbital box diagram for each of the following. Show only the valence\u00a0<\/i>electrons with the box notation.\r\na) Se\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>b) Cu\u00a0\u00a0\u00a0\u00a0 <\/span>c) Fe\u00a0\u00a0\u00a0\u00a0<\/span>d) Si<\/p>\r\n

13. Write the electron configuration, using core notation (condensed electron configuration), for the following.\r\na) Pt\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>b) Zr\u00a0\u00a0\u00a0\u00a0 <\/span>\u00a0<\/span>c) W<\/p>\r\n

14. How many orbitals in an atom can have the designation: 5p, 4d, n=5, n=4?<\/p>\r\n

15. The elements Si, Ga, As, Ge, Al, Cd, S and Se are all used in the manufacturing of various semiconductor devices. Write the expected electron configuration for each of these atoms<\/p>\r\n

16. Write the expected ground-state electron configuration for the following:<\/p>\r\n

a) The element(s) with one unpaired 5p electron.<\/p>\r\n

b) The, as yet undiscovered alkaline earth metal after (i.e. below in the periodic table) radium.<\/p>\r\n

c) The noble gas with electrons occupying 4f orbitals.<\/p>\r\n

d) The first-row transition metal with the most UNPAIRED electrons (i.e. electrons singly in orbitals).<\/p>\r\n

17. Which of the following electron configurations correspond to an excited state (i.e., is not a ground-state\/lowest energy electron configuration)?\u00a0 <\/span>Identify the atoms and write the ground-state electron configurations where appropriate.<\/p>\r\n

a)\u00a0 <\/span>1s2<\/sup>2s2<\/sup>3p1\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span><\/sup>b)\u00a0 <\/span>1s2<\/sup>2s2<\/sup>2p6<\/sup>\r\nc)\u00a0 <\/span>1s2<\/sup>2s2<\/sup>2p4<\/sup>3s1\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span><\/sup>d) [Ar]4s2<\/sup>3d5<\/sup>4p1<\/sup><\/p>\r\n

18. Arrange the following in order of increasing atomic size:\u00a0 <\/span>N, O, S<\/p>\r\n

19. Arrange the following in order of increasing ionization energy:\u00a0 <\/span>S, P, F<\/p>\r\n

20. How many valence electrons do the following atoms have?<\/p>\r\n

a)\u00a0 <\/span>Li\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>b)\u00a0<\/span>Al\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>c)\u00a0 <\/span>P<\/p>\r\n

21. Arrange the following groups of atoms in order of increasing size:<\/p>\r\n

a)\u00a0 <\/span>Be, Mg, Ca\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>b)\u00a0 <\/span>Te, I, Xe\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>c)\u00a0 <\/span>Ga, Ge, In<\/p>\r\n

22. Arrange the atoms in the previous exercise in order of increasing first ionization energy.<\/p>\r\n

23. In each of the following sets, which atom or ion has the smallest radius?<\/p>\r\n

a)\u00a0 <\/span>Li, Na, K\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>b)\u00a0<\/span>P, As\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>c)\u00a0 <\/span>O+<\/sup>, O, O-<\/sup>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>d)\u00a0<\/span>S, Cl, Kr\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>e)\u00a0 <\/span>Pd, Ni, Cu<\/span><\/p>\r\n

24. The first ionization energies of As and Se are 0.947 and 0.941 MJ\/mol respectively. \u00a0Rationalize these values in terms of electron configurations.<\/p>\r\n

25. For each of the pairs of elements\u00a0 <\/span>(O and F)\u00a0<\/span>and\u00a0 <\/span>(Ar and Br), pick the atom with:<\/p>\r\n

a)\u00a0 <\/span>higher (more negative) electron affinity\r\nb)\u00a0 <\/span>higher ionization energy\r\nc)\u00a0 <\/span>larger size<\/p>\r\n

26. What is the frequency of light if its wavelength is 1.00 m?<\/p>\r\n

27. What is the energy of a photon if its wavelength is 1.00 meter?<\/p>\r\n28. \u00a0a) \u00a0Predict the electron configurations of Sc through Zn.\r\n

\r\n\r\nb) \u00a0From a source of actual electron configurations, determine how many exceptions there are from your predictions in part a.\r\n\r\n<\/div>\r\n29. \u00a0Recently, Russian chemists reported experimental evidence of element 117. Use the periodic table to predict its valence shell electron configuration.\r\n\r\n30. \u00a0Which atom has a higher ionization energy (IE), O or P?\r\n\r\n31. \u00a0Which atom has a smaller radius, As or Cl?\r\n\r\n32. \u00a0How many IEs does an H atom have? Write the chemical reactions for the successive ionizations.\r\n\r\n33. \u00a0Based on what you know of electrical charges, do you expect Na+<\/sup> to be larger or smaller than Na?\r\n\r\n \r\n

Answers<\/h2>\r\n

1.\u00a0\u00a0 <\/span>5.21 x 1015<\/sup>s-1<\/sup>; \u00a0 5.76 x 10-8<\/sup>m; \u00a0 UV<\/span><\/p>\r\n

2.\u00a0\u00a0 <\/span>a) 6.92 x 1016<\/sup>Hz \u00a0 \u00a0 \u00a0\u00a0b) 1.28 x 1018<\/sup>Hz \u00a0 \u00a0 \u00a0c) 4.08 x 1014<\/sup>Hz \u00a0 \u00a0 \u00a0d) 6.56 x 1013<\/sup>Hz<\/span><\/p>\r\n

3.\u00a0\u00a0 <\/span>a) 0.0629 m \u00a0 \u00a0 \u00a0b) 1.04 x 107<\/sup>cm \u00a0 \u00a0 \u00a0c) 6.0 x 109<\/sup>mm \u00a0 \u00a0 \u00a0d) 1.04 x 108<\/sup>um<\/span><\/p>\r\n

4.\u00a0\u00a0 <\/span>equal<\/p>\r\n

5.\u00a0\u00a0 <\/span>continuous spectra contain all frequencies while discrete spectra only contain limited number of frequencies.<\/p>\r\n

6.\u00a0\u00a0 <\/span>The concept that the energy of the electron is quantized is true. The concept that the electron travels on a fixed path or \u201corbit\u201d is not the case.<\/span><\/p>\r\n

7.\u00a0\u00a0 <\/span>a)\u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/span>b)<\/span><\/p>\r\n

\"\"\u00a0<\/span><\/p>\r\n

8.\u00a0\u00a0 <\/span>They are similar in that they both need 2 more electrons to have a full outer shell. They are different in that they have a different number of electrons in the outer shell. O has 6 but Se has16.<\/span><\/p>\r\n

9.\u00a0\u00a0 <\/span>Viewing the electron as a particle does not recognize that it has wave-like properties. <\/span>Having a fixed orbit violates the Uncertainty Principle.<\/p>\r\n

10.\u00a0 <\/span>orbit: 2-D circular path in which an electron can be found. Orbital: 3-D region of space in which there\u2019s a high probability of finding the electron.<\/p>\r\n

11.\u00a0 <\/span>a) Aufbau. 1s2<\/sup>2s2<\/sup>2p1 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0<\/sup>b) Aufbau. [Ar]4s2<\/sup>3d1<\/sup>\r\nc) Aufbau & Pauli exclusion. <\/span>1s2<\/sup>2s2<\/sup>2p6<\/sup>3s1 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>d) Hund\u2019s rule. 1s2<\/sup>2s2<\/sup>2p2<\/sup><\/p>\r\n

12. Note: only the valence box diagram is shown in the following answers<\/p>\r\n

a)\u00a0 <\/span>1s2<\/sup>2s2<\/sup>2p6<\/sup>3s2<\/sup>3p6<\/sup>4s2<\/sup>3d10<\/sup>4p4<\/sup>\u00a0\u00a0<\/span>\r\n\"\"<\/span>\r\n<\/span><\/p>\r\n \r\n

b)\u00a0 <\/span>1s<\/span>2<\/sup>2s<\/span>2<\/sup>2p<\/span>6<\/sup>3s<\/span>2<\/sup>3p<\/span>6<\/sup>4s1<\/sup>3d10<\/sup><\/span><\/span>\"\"<\/span><\/p>\r\n \r\n

c)\u00a0 <\/span><\/span>1s2<\/sup>2s2<\/sup>2p6<\/sup>3s2<\/sup>3p6<\/sup>4s2<\/sup>3d6<\/sup><\/span>\"\"<\/span><\/p>\r\n

d)\u00a0 <\/span><\/span>1s2<\/sup>2s2<\/sup>2p6<\/sup>3s2<\/sup>3p2<\/sup><\/span>\"\"<\/span><\/p>\r\n

13.\u00a0 <\/span>a)\u00a0<\/span>[Xe]6s1<\/sup>4f14<\/sup>5d9<\/sup>\r\nb)\u00a0 <\/span>[Kr]5s2<\/sup>4d2<\/sup>\r\nc)\u00a0 <\/span>[Xe]6s2<\/sup>4f14<\/sup>5d4<\/sup><\/span><\/p>\r\n

14.\u00a0 <\/span>3;\u00a0<\/span>5;\u00a0 <\/span>25;\u00a0 <\/span>16<\/span><\/p>\r\n

15.\u00a0 <\/span>Si: 1s2<\/sup>2s2<\/sup>2p6<\/sup>3s2<\/sup>3p2<\/sup>\u00a0\u00a0\u00a0 <\/span>\r\nGa: 1s2<\/sup>2s2<\/sup>2p6<\/sup>3s2<\/sup>3p6<\/sup>4s2<\/sup>3d10<\/sup>4p1<\/sup>\u00a0\u00a0 <\/span>\r\nAs: 1s2<\/sup>2s2<\/sup>2p6<\/sup>3s2<\/sup>3p6<\/sup>4s2<\/sup>3d10<\/sup>4p3<\/sup>\u00a0\u00a0\u00a0 <\/span>\r\nGe: 1s2<\/sup>2s2<\/sup>2p6<\/sup>3s2<\/sup>3p6<\/sup>4s2<\/sup>3d10<\/sup>4p2<\/sup>\u00a0\u00a0\u00a0 <\/span>\r\nAl: 1s2<\/sup>2s2<\/sup>2p6<\/sup>3s2<\/sup>3p1<\/sup>\u00a0\u00a0\u00a0 <\/span>\r\nCd: 1s2<\/sup>2s2<\/sup>2p6<\/sup>3s2<\/sup>3p6<\/sup>4s2<\/sup>3d10<\/sup>4p6<\/sup>5s2<\/sup>4d10<\/sup>\u00a0\u00a0 <\/span>\r\nS: 1s2<\/sup>2s2<\/sup>2p6<\/sup>3s2<\/sup>3p4<\/sup>\u00a0\u00a0\u00a0 <\/span>\r\nSe: 1s2<\/sup>2s2<\/sup>2p6<\/sup>3s2<\/sup>3p6<\/sup>4s2<\/sup>3d10<\/sup>4p4<\/sup>\u00a0\u00a0\u00a0 <\/span><\/span><\/p>\r\n

16.\u00a0 <\/span><\/span>a) In: [Kr]5s2<\/sup>4d10<\/sup>5p1<\/sup>or I: [Kr]5s2<\/sup>4d10<\/sup>5p5<\/sup>\r\nb) Z = 120: [Rn]7s2<\/sup>5f14<\/sup>6d10<\/sup>7p6<\/sup>8s2<\/sup>\r\nc) Rn: [Xe]<\/span>6s2<\/sup>4f14<\/sup>5d10<\/sup>6p6<\/sup>\r\n<\/span>d) Cr: [Ar]4s1<\/sup>3d5<\/sup><\/p>\r\n

17.\u00a0 <\/span>a) excited state of B; 1s2<\/sup>2s2<\/sup>2p1<\/sup>\r\nb) ground state of Ne\r\nc) excited state of F: 1s2<\/sup>2s2<\/sup>2p5<\/sup>\r\nd) excited state of Fe: [Ar]4s2<\/sup>3d6<\/sup><\/p>\r\n

18.\u00a0 <\/span>O < N < S<\/span><\/p>\r\n

19.\u00a0 <\/span>P < S < F<\/span><\/p>\r\n

20.\u00a0 <\/span><\/span>a) 1;\u00a0\u00a0\u00a0 <\/span>b) 3;\u00a0\u00a0\u00a0 <\/span>c) 5<\/span><\/p>\r\n

21.\u00a0 <\/span>a) Be < Mg < Ca\r\nb) Xe < I < Te\r\nc) Ge < Ga < In<\/span><\/p>\r\n

22.\u00a0 <\/span>a) Ca < Mg < Be\r\nb) Te < I < Xe\r\nc) In < Ga < Ge<\/p>\r\n

23.\u00a0 <\/span>a) Li;\u00a0\u00a0<\/span>b) P;\u00a0\u00a0 <\/span>c) O+<\/sup>;\u00a0\u00a0 <\/span>d) Cl;\u00a0\u00a0<\/span>e) Cu<\/span><\/p>\r\n

24.\u00a0 <\/span>As: [Ar]4s2<\/sup>3d10<\/sup>4p3<\/sup>and Se: [Ar]4s2<\/sup>3d10<\/sup>4p4<\/sup>. <\/span>As has a half-filled 4p orbital which is more stable; Se has 2e in one of its 4p orbitals which gives rise to a larger electron-electron repulsion, making it easier for Se to lose an electron to reach a more stable half-filled 4p configuration, therefore Se has a smaller IE1<\/sub>.<\/p>\r\n

25.\u00a0 <\/span>a)\u00a0 <\/span>F, Br;\u00a0\u00a0\u00a0 <\/span>b) F, Ar;\u00a0\u00a0\u00a0 <\/span>c) O, Br<\/span><\/p>\r\n26. 3.00 \u00d7 108<\/sup> s\u22121<\/sup>\r\n\r\n27. 1.99 \u00d7 10\u221222<\/sup> J\r\n\r\n28. a) \u00a0The electron configurations are predicted to end in 3d<\/em>1<\/sup>, 3d<\/em>2<\/sup>, 3d<\/em>3<\/sup>, 3d<\/em>4<\/sup>, 3d<\/em>5<\/sup>, 3d<\/em>6<\/sup>, 3d<\/em>7<\/sup>, 3d<\/em>8<\/sup>, 3d<\/em>9<\/sup>, and 3d<\/em>10<\/sup>.\r\n\r\nb) \u00a0Cr and Cu are exceptions.\r\n\r\n29. Element 117\u2019s valence shell electron configuration should be 7s<\/em>2<\/sup>7p<\/em>5<\/sup>.\r\n\r\n30. O\r\n\r\n31. Cl\r\n\r\n32. H has only one IE: H \u2192\u00a0H+<\/sup> +\u00a0e\u2212<\/sup>\r\n\r\n33. smaller\r\n\r\n<\/div>\r\n<\/div>","rendered":"

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1. Calculate the frequency and wavelength of light that is emitted contains 3.45 x 10-18<\/sup>J of energy. \u00a0What type of light is this?<\/p>\n

2. Convert the following light wavelengths into frequencies (Hz). (The speed of light c=2.998 x 108<\/sup>m\/s)<\/p>\n

a)\u00a0 <\/span>4.33 nm\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>b)\u00a0<\/span>2.35 x 10-10<\/sup>m\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0<\/span>c)\u00a0 <\/span>735 nm\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>d) 4.57 m<\/span>m<\/p>\n

3. Convert the following light frequencies into wavelengths (expressing the result in the indicated units), assuming the light is moving at the speed of light (c=2.998 x 108<\/sup>m\/s)<\/p>\n

a)\u00a0 <\/span>4.77 GHz (m)\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>b)\u00a0<\/span>2.89 kHz (cm)\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span><\/span><\/p>\n

c)\u00a0 <\/span>50. Hz (mm)\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>d) 2.88 MHz (<\/span>m<\/span>m)<\/span><\/p>\n

4. How does the energy possessed by an emitted photon compare to the difference in energy levels that gave rise to the emission of the photon?<\/p>\n

5. Explain the difference between continuous and discrete spectra.<\/p>\n

6. Describe one aspect of Bohr\u2019s model of the atom that \u201cworked\u201d. Describe one aspect of Bohr\u2019s model of the atom that did not \u201cwork\u201d.<\/p>\n

7. Draw an electron shell model of the following<\/p>\n

a)\u00a0 <\/span>chloride ion, Cl1-<\/sup>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>b)\u00a0<\/span>calcium ion, Ca2+<\/sup><\/p>\n

8. In what way are outer electron shells of oxygen and selenium similar? In what way are they different?<\/p>\n

9. Why is the view of an electron being a particle<\/i>in a fixed orbit<\/i>unacceptable?<\/p>\n

10. Explain the difference between an orbit and an orbital. Briefly describe the model that each refers to.<\/p>\n

11. Which law(s) (e.g.: Aufbau principle, Pauli exclusion principle or Hund\u2019s rule) is (are) violated in each of these ground state electron configurations. Write the correct configuration as well.<\/p>\n

a)\u00a0 <\/span>B = 1s1<\/sup>2s1<\/sup>2px<\/sub>1<\/sup>2py<\/sub>1<\/sup>2pz<\/sub>1\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span><\/sup><\/p>\n

b)\u00a0 <\/span>Sc = [Ne] 3s2<\/sup>3p6<\/sup>3d3<\/sup><\/p>\n

c)\u00a0 <\/span>Na = 1s2<\/sup>1p7<\/sup>2s2<\/sup>3s1\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span><\/sup><\/p>\n

d)\u00a0 <\/span>C = 1s2<\/sup>2s2<\/sup>2px<\/sub>2<\/sup><\/p>\n

12. Write the electron configurations and show the orbital box diagram for each of the following. Show only the valence\u00a0<\/i>electrons with the box notation.
\na) Se\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>b) Cu\u00a0\u00a0\u00a0\u00a0 <\/span>c) Fe\u00a0\u00a0\u00a0\u00a0<\/span>d) Si<\/p>\n

13. Write the electron configuration, using core notation (condensed electron configuration), for the following.
\na) Pt\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>b) Zr\u00a0\u00a0\u00a0\u00a0 <\/span>\u00a0<\/span>c) W<\/p>\n

14. How many orbitals in an atom can have the designation: 5p, 4d, n=5, n=4?<\/p>\n

15. The elements Si, Ga, As, Ge, Al, Cd, S and Se are all used in the manufacturing of various semiconductor devices. Write the expected electron configuration for each of these atoms<\/p>\n

16. Write the expected ground-state electron configuration for the following:<\/p>\n

a) The element(s) with one unpaired 5p electron.<\/p>\n

b) The, as yet undiscovered alkaline earth metal after (i.e. below in the periodic table) radium.<\/p>\n

c) The noble gas with electrons occupying 4f orbitals.<\/p>\n

d) The first-row transition metal with the most UNPAIRED electrons (i.e. electrons singly in orbitals).<\/p>\n

17. Which of the following electron configurations correspond to an excited state (i.e., is not a ground-state\/lowest energy electron configuration)?\u00a0 <\/span>Identify the atoms and write the ground-state electron configurations where appropriate.<\/p>\n

a)\u00a0 <\/span>1s2<\/sup>2s2<\/sup>3p1\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span><\/sup>b)\u00a0 <\/span>1s2<\/sup>2s2<\/sup>2p6<\/sup>
\nc)\u00a0 <\/span>1s2<\/sup>2s2<\/sup>2p4<\/sup>3s1\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span><\/sup>d) [Ar]4s2<\/sup>3d5<\/sup>4p1<\/sup><\/p>\n

18. Arrange the following in order of increasing atomic size:\u00a0 <\/span>N, O, S<\/p>\n

19. Arrange the following in order of increasing ionization energy:\u00a0 <\/span>S, P, F<\/p>\n

20. How many valence electrons do the following atoms have?<\/p>\n

a)\u00a0 <\/span>Li\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>b)\u00a0<\/span>Al\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>c)\u00a0 <\/span>P<\/p>\n

21. Arrange the following groups of atoms in order of increasing size:<\/p>\n

a)\u00a0 <\/span>Be, Mg, Ca\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>b)\u00a0 <\/span>Te, I, Xe\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>c)\u00a0 <\/span>Ga, Ge, In<\/p>\n

22. Arrange the atoms in the previous exercise in order of increasing first ionization energy.<\/p>\n

23. In each of the following sets, which atom or ion has the smallest radius?<\/p>\n

a)\u00a0 <\/span>Li, Na, K\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>b)\u00a0<\/span>P, As\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>c)\u00a0 <\/span>O+<\/sup>, O, O–<\/sup>\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>d)\u00a0<\/span>S, Cl, Kr\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0\u00a0 <\/span>e)\u00a0 <\/span>Pd, Ni, Cu<\/span><\/p>\n

24. The first ionization energies of As and Se are 0.947 and 0.941 MJ\/mol respectively. \u00a0Rationalize these values in terms of electron configurations.<\/p>\n

25. For each of the pairs of elements\u00a0 <\/span>(O and F)\u00a0<\/span>and\u00a0 <\/span>(Ar and Br), pick the atom with:<\/p>\n

a)\u00a0 <\/span>higher (more negative) electron affinity
\nb)\u00a0 <\/span>higher ionization energy
\nc)\u00a0 <\/span>larger size<\/p>\n

26. What is the frequency of light if its wavelength is 1.00 m?<\/p>\n

27. What is the energy of a photon if its wavelength is 1.00 meter?<\/p>\n

28. \u00a0a) \u00a0Predict the electron configurations of Sc through Zn.<\/p>\n

\n

b) \u00a0From a source of actual electron configurations, determine how many exceptions there are from your predictions in part a.<\/p>\n<\/div>\n

29. \u00a0Recently, Russian chemists reported experimental evidence of element 117. Use the periodic table to predict its valence shell electron configuration.<\/p>\n

30. \u00a0Which atom has a higher ionization energy (IE), O or P?<\/p>\n

31. \u00a0Which atom has a smaller radius, As or Cl?<\/p>\n

32. \u00a0How many IEs does an H atom have? Write the chemical reactions for the successive ionizations.<\/p>\n

33. \u00a0Based on what you know of electrical charges, do you expect Na+<\/sup> to be larger or smaller than Na?<\/p>\n

 <\/p>\n

Answers<\/h2>\n

1.\u00a0\u00a0 <\/span>5.21 x 1015<\/sup>s-1<\/sup>; \u00a0 5.76 x 10-8<\/sup>m; \u00a0 UV<\/span><\/p>\n

2.\u00a0\u00a0 <\/span>a) 6.92 x 1016<\/sup>Hz \u00a0 \u00a0 \u00a0\u00a0b) 1.28 x 1018<\/sup>Hz \u00a0 \u00a0 \u00a0c) 4.08 x 1014<\/sup>Hz \u00a0 \u00a0 \u00a0d) 6.56 x 1013<\/sup>Hz<\/span><\/p>\n

3.\u00a0\u00a0 <\/span>a) 0.0629 m \u00a0 \u00a0 \u00a0b) 1.04 x 107<\/sup>cm \u00a0 \u00a0 \u00a0c) 6.0 x 109<\/sup>mm \u00a0 \u00a0 \u00a0d) 1.04 x 108<\/sup>um<\/span><\/p>\n

4.\u00a0\u00a0 <\/span>equal<\/p>\n

5.\u00a0\u00a0 <\/span>continuous spectra contain all frequencies while discrete spectra only contain limited number of frequencies.<\/p>\n

6.\u00a0\u00a0 <\/span>The concept that the energy of the electron is quantized is true. The concept that the electron travels on a fixed path or \u201corbit\u201d is not the case.<\/span><\/p>\n

7.\u00a0\u00a0 <\/span>a)\u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/span>b)<\/span><\/p>\n

\"\"\u00a0<\/span><\/p>\n

8.\u00a0\u00a0 <\/span>They are similar in that they both need 2 more electrons to have a full outer shell. They are different in that they have a different number of electrons in the outer shell. O has 6 but Se has16.<\/span><\/p>\n

9.\u00a0\u00a0 <\/span>Viewing the electron as a particle does not recognize that it has wave-like properties. <\/span>Having a fixed orbit violates the Uncertainty Principle.<\/p>\n

10.\u00a0 <\/span>orbit: 2-D circular path in which an electron can be found. Orbital: 3-D region of space in which there\u2019s a high probability of finding the electron.<\/p>\n

11.\u00a0 <\/span>a) Aufbau. 1s2<\/sup>2s2<\/sup>2p1 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0 \u00a0<\/sup>b) Aufbau. [Ar]4s2<\/sup>3d1<\/sup>
\nc) Aufbau & Pauli exclusion. <\/span>1s2<\/sup>2s2<\/sup>2p6<\/sup>3s1 \u00a0 \u00a0 \u00a0 \u00a0\u00a0<\/sup>d) Hund\u2019s rule. 1s2<\/sup>2s2<\/sup>2p2<\/sup><\/p>\n

12. Note: only the valence box diagram is shown in the following answers<\/p>\n

a)\u00a0 <\/span>1s2<\/sup>2s2<\/sup>2p6<\/sup>3s2<\/sup>3p6<\/sup>4s2<\/sup>3d10<\/sup>4p4<\/sup>\u00a0\u00a0<\/span>
\n\"\"<\/span>
\n<\/span><\/p>\n

 <\/p>\n

b)\u00a0 <\/span>1s<\/span>2<\/sup>2s<\/span>2<\/sup>2p<\/span>6<\/sup>3s<\/span>2<\/sup>3p<\/span>6<\/sup>4s1<\/sup>3d10<\/sup><\/span><\/span>\"\"<\/span><\/p>\n

 <\/p>\n

c)\u00a0 <\/span><\/span>1s2<\/sup>2s2<\/sup>2p6<\/sup>3s2<\/sup>3p6<\/sup>4s2<\/sup>3d6<\/sup><\/span>\"\"<\/span><\/p>\n

d)\u00a0 <\/span><\/span>1s2<\/sup>2s2<\/sup>2p6<\/sup>3s2<\/sup>3p2<\/sup><\/span>\"\"<\/span><\/p>\n

13.\u00a0 <\/span>a)\u00a0<\/span>[Xe]6s1<\/sup>4f14<\/sup>5d9<\/sup>
\nb)\u00a0 <\/span>[Kr]5s2<\/sup>4d2<\/sup>
\nc)\u00a0 <\/span>[Xe]6s2<\/sup>4f14<\/sup>5d4<\/sup><\/span><\/p>\n

14.\u00a0 <\/span>3;\u00a0<\/span>5;\u00a0 <\/span>25;\u00a0 <\/span>16<\/span><\/p>\n

15.\u00a0 <\/span>Si: 1s2<\/sup>2s2<\/sup>2p6<\/sup>3s2<\/sup>3p2<\/sup>\u00a0\u00a0\u00a0 <\/span>
\nGa: 1s2<\/sup>2s2<\/sup>2p6<\/sup>3s2<\/sup>3p6<\/sup>4s2<\/sup>3d10<\/sup>4p1<\/sup>\u00a0\u00a0 <\/span>
\nAs: 1s2<\/sup>2s2<\/sup>2p6<\/sup>3s2<\/sup>3p6<\/sup>4s2<\/sup>3d10<\/sup>4p3<\/sup>\u00a0\u00a0\u00a0 <\/span>
\nGe: 1s2<\/sup>2s2<\/sup>2p6<\/sup>3s2<\/sup>3p6<\/sup>4s2<\/sup>3d10<\/sup>4p2<\/sup>\u00a0\u00a0\u00a0 <\/span>
\nAl: 1s2<\/sup>2s2<\/sup>2p6<\/sup>3s2<\/sup>3p1<\/sup>\u00a0\u00a0\u00a0 <\/span>
\nCd: 1s2<\/sup>2s2<\/sup>2p6<\/sup>3s2<\/sup>3p6<\/sup>4s2<\/sup>3d10<\/sup>4p6<\/sup>5s2<\/sup>4d10<\/sup>\u00a0\u00a0 <\/span>
\nS: 1s2<\/sup>2s2<\/sup>2p6<\/sup>3s2<\/sup>3p4<\/sup>\u00a0\u00a0\u00a0 <\/span>
\nSe: 1s2<\/sup>2s2<\/sup>2p6<\/sup>3s2<\/sup>3p6<\/sup>4s2<\/sup>3d10<\/sup>4p4<\/sup>\u00a0\u00a0\u00a0 <\/span><\/span><\/p>\n

16.\u00a0 <\/span><\/span>a) In: [Kr]5s2<\/sup>4d10<\/sup>5p1<\/sup>or I: [Kr]5s2<\/sup>4d10<\/sup>5p5<\/sup>
\nb) Z = 120: [Rn]7s2<\/sup>5f14<\/sup>6d10<\/sup>7p6<\/sup>8s2<\/sup>
\nc) Rn: [Xe]<\/span>6s2<\/sup>4f14<\/sup>5d10<\/sup>6p6<\/sup>
\n<\/span>d) Cr: [Ar]4s1<\/sup>3d5<\/sup><\/p>\n

17.\u00a0 <\/span>a) excited state of B; 1s2<\/sup>2s2<\/sup>2p1<\/sup>
\nb) ground state of Ne
\nc) excited state of F: 1s2<\/sup>2s2<\/sup>2p5<\/sup>
\nd) excited state of Fe: [Ar]4s2<\/sup>3d6<\/sup><\/p>\n

18.\u00a0 <\/span>O < N < S<\/span><\/p>\n

19.\u00a0 <\/span>P < S < F<\/span><\/p>\n

20.\u00a0 <\/span><\/span>a) 1;\u00a0\u00a0\u00a0 <\/span>b) 3;\u00a0\u00a0\u00a0 <\/span>c) 5<\/span><\/p>\n

21.\u00a0 <\/span>a) Be < Mg < Ca
\nb) Xe < I < Te
\nc) Ge < Ga < In<\/span><\/p>\n

22.\u00a0 <\/span>a) Ca < Mg < Be
\nb) Te < I < Xe
\nc) In < Ga < Ge<\/p>\n

23.\u00a0 <\/span>a) Li;\u00a0\u00a0<\/span>b) P;\u00a0\u00a0 <\/span>c) O+<\/sup>;\u00a0\u00a0 <\/span>d) Cl;\u00a0\u00a0<\/span>e) Cu<\/span><\/p>\n

24.\u00a0 <\/span>As: [Ar]4s2<\/sup>3d10<\/sup>4p3<\/sup>and Se: [Ar]4s2<\/sup>3d10<\/sup>4p4<\/sup>. <\/span>As has a half-filled 4p orbital which is more stable; Se has 2e in one of its 4p orbitals which gives rise to a larger electron-electron repulsion, making it easier for Se to lose an electron to reach a more stable half-filled 4p configuration, therefore Se has a smaller IE1<\/sub>.<\/p>\n

25.\u00a0 <\/span>a)\u00a0 <\/span>F, Br;\u00a0\u00a0\u00a0 <\/span>b) F, Ar;\u00a0\u00a0\u00a0 <\/span>c) O, Br<\/span><\/p>\n

26. 3.00 \u00d7 108<\/sup> s\u22121<\/sup><\/p>\n

27. 1.99 \u00d7 10\u221222<\/sup> J<\/p>\n

28. a) \u00a0The electron configurations are predicted to end in 3d<\/em>1<\/sup>, 3d<\/em>2<\/sup>, 3d<\/em>3<\/sup>, 3d<\/em>4<\/sup>, 3d<\/em>5<\/sup>, 3d<\/em>6<\/sup>, 3d<\/em>7<\/sup>, 3d<\/em>8<\/sup>, 3d<\/em>9<\/sup>, and 3d<\/em>10<\/sup>.<\/p>\n

b) \u00a0Cr and Cu are exceptions.<\/p>\n

29. Element 117\u2019s valence shell electron configuration should be 7s<\/em>2<\/sup>7p<\/em>5<\/sup>.<\/p>\n

30. O<\/p>\n

31. Cl<\/p>\n

32. H has only one IE: H \u2192\u00a0H+<\/sup> +\u00a0e\u2212<\/sup><\/p>\n

33. smaller<\/p>\n<\/div>\n<\/div>\n","protected":false},"author":330,"menu_order":7,"template":"","meta":{"pb_show_title":"on","pb_short_title":"8.6 End of Chapter Problems","pb_subtitle":"","pb_authors":[],"pb_section_license":"cc-by-nc-sa"},"chapter-type":[],"contributor":[],"license":[54],"class_list":["post-2399","chapter","type-chapter","status-publish","hentry","license-cc-by-nc-sa"],"part":2362,"_links":{"self":[{"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/pressbooks\/v2\/chapters\/2399","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/pressbooks\/v2\/chapters"}],"about":[{"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/wp\/v2\/types\/chapter"}],"author":[{"embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/wp\/v2\/users\/330"}],"version-history":[{"count":17,"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/pressbooks\/v2\/chapters\/2399\/revisions"}],"predecessor-version":[{"id":3727,"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/pressbooks\/v2\/chapters\/2399\/revisions\/3727"}],"part":[{"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/pressbooks\/v2\/parts\/2362"}],"metadata":[{"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/pressbooks\/v2\/chapters\/2399\/metadata\/"}],"wp:attachment":[{"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/wp\/v2\/media?parent=2399"}],"wp:term":[{"taxonomy":"chapter-type","embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/pressbooks\/v2\/chapter-type?post=2399"},{"taxonomy":"contributor","embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/wp\/v2\/contributor?post=2399"},{"taxonomy":"license","embeddable":true,"href":"https:\/\/pressbooks.bccampus.ca\/chem1114langaracollege\/wp-json\/wp\/v2\/license?post=2399"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}