Arrangement of Electrons in Atoms
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1 CHAPTER 4 REVIEW Arrangement of Electrons in Atoms Teacher Notes and Answers Chapter 4 SECTION 1 SHORT ANSWER 1. In order for an electron to be ejected from a metal surface, the electron must be struck b a single photon with at least the minimum energ needed to knock the electron loose. 2. The ground state is the lowest energ state of the atom. When the atom absorbs energ, it can move to a higher energ state, or ecited state. 3. A photon is emitted when an atom moves from an ecited state to its ground state or to a lower-energ ecited state. 4. When an atom loses energ, it falls from a higher energ state to a lower energ state. The frequenc of the emitted light, observed in an element s line-emission spectrum, ma be measured. The energ of each transition is calculated using the equation E = hv, where v is the frequenc of each of the lines in the element s lineemission spectrum. From the analsis of these results, the energ levels of an atom atom of each element ma be determined. 5. Energ is proportional to frequenc, and ultraviolet radiation has a higher frequenc than infrared radiation. To produce ultraviolet radiation, electrons must drop to lower energ levels than the do to produce infrared radiation. 6. Wave B has the higher frequenc. Wavelength is inversel proportional to frequenc, so as the wavelength decreases, its frequenc increases. 7. Si different photons were emitted. Each time an ecited helium atom falls back from an ecited state to its ground state or to a lower energ state, it emits a photon of radiation that shows up as this specific line-emission spectrum. There are si lines in this helium spectrum H m SECTION 2 SHORT ANSWER 1. d 2. a 3. a 4. c 5. c 6. c 7. c 8. Scientists knew that an wave confined to a space could have onl certain frequencies. De Broglie suggested that electrons should be considered as waves confined to the space around an atomic nucleus; in this wa, electron waves could eist onl at specific frequencies. According to the relationship E = hv, these frequencies correspond to the specific quantied energies of the Bohr orbitals. 9. The principal quantum number refers to the main energ level. The angular momentum quantum number refers to the shape of the orbital. The magnetic quantum number refers to the orientation of an orbital around the nucleus. The spin quantum number indicates the spin state of an electron in an orbital. 10. The Heisenberg uncertaint principle states that it is impossible to determine simultaneousl both the position and velocit of an electron (or an other particle). Because measuring the position of an electron actuall changes its position, there is alwas a basic uncertaint in tring to locate an electron. Thus, the eact position of the electron cannot be found. An electron cloud or orbital represents the region that is the probable location of an electron. 11. Modern Chemistr 1 Arrangement of Electrons in Atoms
2 SECTION 3 SHORT ANSWER 1. The Pauli eclusion principle states that no two electrons in an atom ma have the same set of four quantum numbers. If both electrons in the same orbital had the same spin state, each electron would have the same four quantum numbers. If one electron has the opposite spin state, the fourth quantum number is different and the eclusion principle is obeed. 2. This orbital notation is possible if the helium atom is in an ecited state p 3s ; 2 p 2 p 2 p 3s p ; 2 p 2 p 2 p p 3s 3 p 4s ; 2 p 2 p 3s 3 p 3 p 3 p 4s 2 p p 3s ; 2 p 2 p 2 p 3s p 3s ; 2 p 2 p 2 p 3s p ; p 9. a. Pauli eclusion principle b. Hund s rule 2 p 2 p Modern Chemistr 2 Arrangement of Electrons In Atoms
3 CHAPTER 4 REVIEW Arrangement of Electrons in Atoms SECTION 1 SHORT ANSWER Answer the following questions in the space provided. 1. In what wa does the photoelectric effect support the particle theor of light? 2. What is the difference between the ground state and the ecited state of an atom? 3. Under what circumstances can an atom emit a photon? 4. How can the energ levels of the atom be determined b measuring the light emitted from an atom? 5. Wh does electromagnetic radiation in the ultraviolet region represent a larger energ transition than does radiation in the infrared region? Modern Chemistr 3 Arrangement of Electrons in Atoms
4 SECTION 1 continued 6. Which of the waves shown below has the higher frequenc? (The scale is the same for each drawing.) Eplain our answer. 7. How man different photons of radiation were emitted from ecited helium atoms to form the spectrum shown below? Eplain our answer. PROBLEMS Write the answer on the line to the left. Show all our work in the space provided. 8. What is the frequenc of light that has a wavelength of 310 nm? 9. What is the wavelength of electromagnetic radiation if its frequenc is H? Modern Chemistr 4 Arrangement of Electrons In Atoms
5 CHAPTER 4 REVIEW Arrangement of Electrons in Atoms SECTION 2 SHORT ANSWER Answer the following questions in the space provided. 1. How man quantum numbers are used to describe the properties of electrons in atomic orbitals? (a) 1 (c) 3 (b) 2 (d) 4 2. A spherical electron cloud surrounding an atomic nucleus would best represent (a) an s orbital. (c) a combination of two different p orbitals. (b) a p orbital. (d) a combination of an s and a p orbital. 3. How man electrons can an energ level of n = 4 hold? (a) 32 (c) 8 (b) 24 (d) 6 4. How man electrons can an energ level of n = 2 hold? (a) 32 (c) 8 (b) 24 (d) 6 5. Compared with an electron for which n = 2, an electron for which n = 4 has more (a) spin. (c) energ. (b) particle nature. (d) wave nature. 6. According to Bohr, which is the point in the figure below where electrons cannot reside? (a) point A (c) point C (b) point B (d) point D 7. According to the quantum theor, point D in the above figure represents (a) the fied position of an electron. (b) the farthest position from the nucleus that an electron can achieve. (c) a position where an electron probabl eists. (d) a position where an electron cannot eist. Modern Chemistr 5 Arrangement of Electrons in Atoms
6 SECTION 2 continued 8. How did de Broglie conclude that electrons have a wave nature? 9. Identif each of the four quantum numbers and the properties to which the refer. 10. How did the Heisenberg uncertaint principle contribute to the idea that electrons occup clouds, or orbitals? 11. Complete the following table: Principal quantum number, n Number of sublevels Tpes of orbitals 1 1 s 2 2 s, p 3 3 s,p,d 4 4 s,p,d,f Modern Chemistr 6 Arrangement of Electrons In Atoms
7 CHAPTER 4 REVIEW Arrangement of Electrons in Atoms SECTION 3 SHORT ANSWER Answer the following questions in the space provided. 1. State the Pauli eclusion principle, and use it to eplain wh electrons in the same orbital must have opposite spin states. 2. Eplain the conditions under which the following orbital notation for helium is possible: Write the ground-state electron configuration and orbital notation for each of the following atoms: 3. Phosphorus 4. Nitrogen 5. Potassium Modern Chemistr 7 Arrangement of Electrons in Atoms
8 SECTION 3 continued 6. Aluminum 7. Argon 8. Boron 9. Which guideline, Hund s rule or the Pauli eclusion principle, is violated in the following orbital diagrams? a. b. Modern Chemistr 8 Arrangement of Electrons In Atoms
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