Choose the best answer to each of the following questions.

1. Given a particle of mass m and velocity v, deBroglie’s hypothesis allows you to predict:

   2. Heisenbergs uncertainty principle pointed out that it is impossible to
       know the exact _________
       A. wavelength and charge of the electron.
       B. momentum and wavelength of the electron
       C. mass and charge of the electron
       D. position and momentum of the electron.

   3. By treating the electron as a wave function, Schrodinger was able to
       calculate
       A. the time it takes an electron to orbit the nucleus.
       B. the probability of locating the electron.
       C. the wavelength of the electron.
       D. the exact location of the electron.

   4. Which of the following orbitals is spherical?
       A. 5f
       B. 3p
       C. 2s
       D. 4d

   5.The principal quantum number best describe what characteristic of the
      electron?
      A. the spin.
      B. the shape of the charge cloud.
      C. the size of the charge cloud
      D. the color of the spectral line


   6. In the quantum mechanical view of the electron structure of the
       atom, the pathway or position of the electron is best represented by
       as _________
       A. an elliptical orbit
       B. a series of most probable positions represented by a cloud
       C. a circular orbit
       D. a straight line that radiate out from the nucleus

   7. What is the maximum number of electrons that can occupy the fourth
       Energy level?
       A. 4
       B. 16
       C. 8
       D. 32

   9. According to the Pauli exclusion principle, no two electrons in the
       same orbital can have the same
       A. set of quantum numbers
       B. orbital location
       C. average distance from the nucleus
       D. set of spectral lines

  10. The importance of the deBroglie equation to the development of our
        present theory or atomic structure was the _______
        A. calculation of the specific energy of an electron
        B. application of wave particle duality to a particle
        C. calculation of the energies of sublevels
        D. application of the uncertainty principle

  11. Which of the following is a possible ending to the electron
        configuration for an atom with a Lewis dot diagram of X
        A. 3s²3p⁶
        B. 5s²4d³
        C. 4s²3d¹⁰4p¹
        D. 2s¹2p²


  12. How many d-orbitals must be occupied by single electrons before the
       electrons can be paired?
       A. 5
       B. 1
       C. 7
       D. 3

  13. The two electrons in the outermost level of strontium are designated
       as 5s². How many quantum numbers do these two electrons have in
       common?
       A. 2
       B. 1
       C. 4
       D. 3

  14. How many dots would appear in the Lewis dot diagram of an element
       that had an electron configuration of 4s²3d¹⁰4p³?
       A. 5
       B. 2
       C. 3
       D. 15

  15. The 3s orbital differs from the 2s orbital in that it is
        A. smaller
        B. larger
        C. a different shape
        D. more crowded

 

1. Draw the atomic orbital energy diagram for the sodium atom.

 

2. Write out the electron configuration for vanadium (Z = 23)

 

3. A neutral atom has an electron configuration ending in 4s²3d⁸.

  4. Explain the concept of the wave-particle duality of nature. Why do
      NASA scientist not have to worry about this concept when working
      with the space shuttle?

  5. List the four quantum numbers, their names, symbols and what they
      represent.

6. Write the electron configurations and draw the Lewis dot diagrams for
    each of the following elements:
    a. Helium (He)
    b. Beryllium (Be)
    c. Carbon (C)
    d. Phosphorus (P)
    e. Chromium (Cr)
    f. Zirconium (Zr)

  7. Determine the number of valance electrons in each of the elements
      listed in question number 6.

  8. Complete the chart below.

Sublevel                      Number of Orbitals       Number of Electrons