Download AP Chem II Instructor: Mr. Malasky Name Period ______ Due Date

AP Chem II
Instructor: Mr. Malasky
Name _______________________________________ Period ________ Due Date __________
Ch. 7A.2 Atomic Structure.
Multiple Choice. Select the letter for the correct response.
____ 1. The Heisenberg uncertainty principle states that
a. electrons have no momentum
b. the position of an electron is impossible to determine
c. the faster an electron moves, the more unreliable is its energy
d. the momentum and the position of an electron cannot be precisely defined
simultaneously
e. Einstein’s theory of relativity is still unproved
____ 2. The four quantum numbers (n, l, ml, and ms) that describe the valence electron in the
cesium atom are
a. 6, 0, -1, +½
b. 6, 1, 1, +½
c. 6, 0, 0, +½
d. 6, 1, 0, +½
e. 6, 0, 1, -½
____ 3. Which of the following rules states that no two electrons in an atom can have the same
set of quantum numbers?
a. Hund’s rule
b. The Heisenberg Uncertainty principle
c. The Pauli Exclusion principle
d. The deBroglie hypothesis
e. The Bohr model
____ 4. If the angular momentum quantum number l equals 3, the total number of allowed
orbitals in just that subenergy level is
a. 1
b. 3
c. 5
d. 7
e. 8
____ 5. The element with the ground state electron configuration of [Ar]4s23d7 is
a. Mg
b. K
c. Ar
d. Co
e. Ni
____ 6. The electron configuration for the element antimony, Sb, is
a. [Na]3s22d103p3
b. [Ar]4s23d104p5
c. [Ar]4s23d104p3
d. [Kr]5s24d105p3
e. [Kr]5s24d105p5
over-------
____ 7. The number of unpaired electrons in the silicon atom is
a. 1
b. 2
c. 4
d. 5
e. 6
_____ 8. The differentiating electrons for transition elements are
a. d electrons
b. s electrons
c. p electrons
d. f electrons
e. valence electrons
____ 9. Which of the following sets of quantum numbers is unacceptable (n, l, ml, ms)
a. 4, 3, -2, +1/2
b. 3, 0, 1, -1/2
c. 3, 0, 0, -1/2
d. 3, 1, 1, +1/2
e. 2, 0, 0, -1/2
____ 10. The valence electrons are
a. all electrons in an atom beyond the preceding noble gas
b. all outermost electrons in a sublevel
c. s and p electrons in the highest energy level or shell
d. electrons in the last unfilled sublevel
e. any electrons that can ionize