Chapter 7 Review Problems

CHAPTER 7 REVIEW PROBLEMS

(95 points)

(3 points) 1. The yellow light given off by a sodium vapor lamp used for public lighting has a wavelength of 589.0 nm. Determine the frequency of this radiation.

(3 points) 2. A laser used in eye surgery to fuse detached retinas produces radiation with a frequency of

4.688 x 1014 s-1. Determine the wavelength of this radiation.

(6 points) 3. It takes 208.4 kJ of energy to remove 1.00 mole of electrons from an atom on the surface of rubidium metal. Determine the amount of energy required to remove a single electron from an atom on the surface of rubidium metal. What is the maximum wavelength of light capable of doing this?

(4 points) 4. The ionization energy of gold is 890.1 kJ/mol. Is light with a wavelength of 225 nm capable of ionizing a gold atom (removing an electron) in the gas phase?

(3 points) 5. (a) A laser emits light with a frequency of 4.69 x 1014 s-1. Determine the energy of one photon of the radiation form this laser.

(3 points) (b) If the laser emits a pulse of energycontaining 5.00 x 1017 photons, determine the total energy of the pulse.

(3 points) (c) If the laser emits 1.30 x 10-2 J of energy during a pulse, determine the number of photons emitted during the pulse.

(3 points) 6. Determine the wavelength of an electron moving at a velocity of 5.97 x 106 m/s. The mass of an electron is 9.11 x 10-31 kg.

(3 points) 7. Determine the velocity of a neutron whose de Broglie wavelength is 500.0 pm. The mass of a neutron is 1.67 x 10-27 kg.

(4 points) 8. Determine the wavelength of light emitted when an electron transitions form the n = 4 energy level to the n = 3 energy level.

(4 points) 9. Determine the wavelength of light emitted when an electron transitions from the n = 5 energy level to the n = 3 energy level.

(4 points) 10. An excited hydrogen atom emits light with a frequency of 1.141 x 1014 s-1 to reach the energy level for which n = 4. In which principal quantum number did the electron begin?

(1 point) 11. Which of the following orbital designations are incorrect: 1s, 1p, 7d, 9s, 3f, 4f, 2d?

(1 point) 12. When n = 4, what are the possible values of l?

(1 point) 13. When l = 2, what are the possible values of ml?

(2 points) 14. Give the values of n, l, and mlfor each orbital in (a) the 2p subshell and (b) the 5d subshell.

(4 points) 15. Determine which of the following are permissible sets of quantum numbers for an electron in a hydrogen atom:

(a) n = 2, l = 1, ml = 1

(b) n = 1, l = 0, ml = -1

(d) n = 3, l = 3, ml = 0

(4 points) 16. How many orbitals in an atom can have the designation:

(a) 5p

(b) 3dz2

(d) n = 5

(e) n = 4

(5 points) 17. Give the maximum number of electrons in an atom that can have these quantum numbers:

(a) n = 4

(b) n = 5, ml = +1

(d) n = 3, l = 2

(e) n = 2, l = 1

(8 points) 18. Write the complete electron configuration for:

(a) Cl

(b) Sr

(d) Au

(4 points) 19. Write a noble gas electron configuration for:

(a) Fe

(b) Sb

(4 points) 20. Draw an orbital diagram for:

(a) Se

(b) Mg

(2 points) 21. A certain oxygen atom has the electron configuration: 1s22s22px22py2.

(a) How many unpaired electrons are present?

(b) In going from this state to the ground state would energy be energy be released or absorbed?

(3 points) 22. Arrange the following groups in order of increasing atomic size:

a. Rb, Na, Be

b. Sr, Ne, Se

c. Fe, P, O

(3 points)23. Arrange the following groups in order of increasing first ionization energy:

a. Rb, Na, Be

b. Sr, Ne, Se

c. Fe, P, O

(3 points) 24. In each of the following sets, which atom or ion has the smallest radius?

(a) Li, Na, K

(b) O+, O, O-

(4 points) 25. The first ionization energies of As and Se are 0.947 and 0.941 MJ/mol, respectively. Rationalize these values in terms of electron configurations.

(3 points) 26. For each of the following pairs of elements

(C and N)(Ar and Br)

pick the one with

(a) more favorable (exothermic) electron affinity

(b) higher ionization energy