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 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