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# Practice7ans - Practice Questions(with answers Quiz#7...

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Unformatted text preview: Practice Questions (with answers) Quiz #7 material 1. In a photoelectron experiment, light of wavelength 1.250 nm is incident on a sample of Neon. The light has sufficient energy to photoeject electrons from any orbital of Neon. The kinetic energy of the photoejected electrons is measured, and electrons of just three kinetic energies are found: 134.7 eV, 941.5 eV, and 970.0 eV. What is the energy of the 2s orbital of Neon? a. –21.8 eV b. –50.3 eV c. –857.1 eV d. –941.5 eV e. –970.0 eV 2. The energy of the 1s orbital in Zinc is –9,796 eV. What is Z eff for this 1s orbital? a. 98.9 b. 30.0 c. 26.8 d. 13.4 e. 8.94 3. Arrange the following orbitals from lowest energy to highest energy: 4d, 4f, 5s, 5p, 6s lowest energy → highest energy a. 5s 4d 5p 6s 4f b. 5s 5p 4d 4f 6s c. 4f 4d 5p 5s 6s d. 4f 6s 5p 4d 5s e. 6s 5s 5p 4d 4f 4. The orbital configuration 1s 2 2s 2 2p 5 3s is: a. the ground state of Na b. the ground state of Ne c. an excited state of F d. an excited state of Ne e. an excited state of Mg + 5. Which of the following orbital configurations does not satisfy Hund's Rule? a. 2p x 2 2p y 2 b. 3p x 2 3p y 2 3p z 1 c. 4p x 1 4p y 1 d. 2p x 1 2p y 1 2p z 1 e. all of them satisfy Hund's Rule 6. In going across the periodic table from Li to Ne the radius of the 1s orbital a. increases b decreases c. doesn't change d. increases from Li to B then decreases e. decreases from Li to B then increases 7. Which of the following are isoelectronic: S 2- , Cl − , Ar 2+ , K + a. S 2 − and Ar 2+ b. Cl − , Ar + , K + c. S 2 − , Cl − , K + d. Cl − , Ar 2+ , K + e. all of them 8. In the Be 2+ ion the electronic potential energy function is given by which of the following: a. − 2e 2 r 1 − 2e 2 r 2 b. − 4e 2 r 1 − 4e 2 r 2 c. − 2e 2 r 1 − 2e 2 r 2 + e 2 r 12 d. − 4e 2 r 1 − 4e 2 r 2 + e 2 r 12 ⇐ e. − 4e 2 r 1 − 4e 2 r 2 + 4e 2 r 12 9. In a many-electron atom which of the following are be true: a. The number of electrons with m s = +1/2 must be the same as the number of electrons with m s = − 1/2. b. Electrons in orbitals with different values of m l have different energies. c. The energy of orbitals increase as n + l increases. d. Any two orbitals of the same value of n have the same energy. e. All of these might be true, but they do not have to be true. 10. What makes it difficult to solve the Schrödinger Equation difficult for many-electron atoms is: a. The nuclear charge, Z, is greater than 1. b. The interaction of different electrons with the nuclear charge, Z, is different. c. The electrons must be in different orbitals....
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Practice7ans - Practice Questions(with answers Quiz#7...

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