ADVANCED CHEMISTRY TEST #1

1.  The elements of Period 2 have the same
        (A) atomic mass                (B) number of occupied energy levels
        (C) atomic number             (D) number of occupied sublevels

2.  Which electron configuration contains three half-filled orbitals?
        (A) 1s2 2s2 2p6                (B) 1s2 2s2 2p5
        (C) 1s2 2s2 2p3                (D) 1s2 2s2 2p4

3.  The total number of completely filled orbitals in an atom of nitrogen in the ground state is
        (A) 0            (B) 2            (C) 3            (D) 5

4.  Which of the following periods contains the greatest number of metals?
        (A) 1            (B) 2            (C) 3            (D) 4

5.  In an atom, the "s" sublevel has
        (A) 1 orbital            (B) 3 orbitals            (C) 5 orbitals            (D) 7 orbitals

6.  What is the maximum number of sublevels in the 3rd energy level?
        (A) 3            (B) 5            (C) 18            (D) 32

7.  Which sublevel is being filled with electrons in elements with atomic numbers 21 through 29?
        (A) 3s            (B) 4p            (C) 3d            (D) 4d

8.  The electron configuration of an atom in the ground state is 1s2 2s2 2p2.  The total number of occupied energy
     levels in this atom is
        (A) 1           (B) 2            (C) 3            (D) 4

9.  Which atom in the ground state contains only one completely filled "p" orbital?
        (A) N            (B) O            (C) He            (D) Be

10.  Energy is released when an electron changes from a sublevel of
        (A) 1s to 2p            (B) 2s to 3s            (C) 3s to 2s            (D) 3p to 5s

11.  Which electron transition results in the emission of energy?
        (A) 2s to 2p            (B) 2p to 3s            (C) 3d to 2p            (D) 3p to 4d

12.  Which atom in the ground state contains only one orbital that is partially occupied?
        (A) Si            (B) Ne            (C) Ca            (D) Na

13.  The possible values of an electron's spin quantum number (s) are
        (A) -1, 0, or 1            (B) + 1/2 or - 1/2            (C) +1 or -1            (D) 0 or 1

14.  How does the ground state electron configuration of the hydrogen atom differ from that of a ground state
       helium atom?
        (A) Hydrogen has one electron in a higher energy level.
        (B) Hydrogen has two electrons in a higher energy level.
        (C) Hydrogen contains a half-filled orbital.
        (D) Hydrogen contains a completely filled orbital.

15.  The characteristic bright-line spectrum of sodium is produced when its electrons
        (A) return to lower energy levels            (B) jump to higher energy levels
        (C) are lost by neutral atoms                  (D) are gained by neutral atoms

16.  The total number of orbitals that can exist at the 2nd main energy level is
        (A) 2            (B) 4            (C) 3            (D) 8

17.  The set of orbitals that are dumbbell-shaped and directed along the x, y, and z axes are called
        (A) d orbitals            (B) p orbitals            (C) f orbitals            (D) s orbitals

18.  The electron configuration for aluminum (atomic number 13) is
        (A) 1s2 2s2 2p3 3s2 3p3 3d1                (B) 1s2 2s2 2p6 3s2 2d1
        (C) 1s2 2s2 2p6 3s2 3p1                      (D) 1s2 2s2 2p9

19.  In the electron configuration for scandium (atomic number 21), what is the notation for the three highest
      energy electrons?
        (A) 4s2 3d1            (B) 3d3            (C) 4s3            (D) 4s2 4p1

20.  An orbital that could never exist according to the quantum description of the atom is
        (A) 3d            (B) 6d            (C) 8s            (D) 3f

21.  What values can the angular momentum quantum number (l) have when n = 2?
        (A) + 1/2 or - 1/2            (B) - 1/2, -1, or -2       ;     (C) 0, 1, or 2            (D) 0 or 1

22.  The atomic sublevel with the next highest energy level after 4p is
        (A) 4d            (B) 5p            (C) 4f            (D) 5s

23.  How many quantum numbers are needed to describe the energy state (and location) of an electron in an atom?
        (A) 1            (B) 3            (C) 2            (D) 4

24.  An atom in the ground state has a total of 12 electrons.  How many of these electrons are in "p" sublevels?
        (A) 12            (B) 4            (C) 8            (D) 6

25.  An atom of an element has the electron configuration 1s2 2s2 2p2.  What is the total number of electrons in its
       outermost energy level?
        (A) 6            (B) 2            (C) 5            (D) 4

26.  An atom has 8 electrons in a "d" sublevel.  How many "d" orbitals in this sublevel are half-filled?
        (A) 1           (B) 2            (C) 3            (D) 4

27.  Which represents the correct electron configuration of the outermost energy level of a group VIII A (8A or 18)
       element in the ground state?
        (A) s2 p2            (B) s2 p4            (C) s2 p6            (D) s2 p8

28.  The pair of elements with the most similar chemical properties are
        (A) Mg and S            (B) Ca and Br            (C) Mg and Ca            (D) S and Ar

29.  An element has an atomic number of 18.  What is the principal quantum number (n) of its outermost electrons?
        (A) 1            (B) 2            (C) 3            (D) 4

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