But
______ pts. out of 80 pts. = _________ % = Name:
Advanced Chemistry: Test #3 (Atomic Theory & Periodic Trends)
Multiple Choice: On the answer sheet darken the letter
corresponding to the best answer. (1 pt.
each)
1. According to the Aufbau order, which of
the following has a half-filled subshell?
a. Ca
b. Si
c. S
d. Sb
e. Fe
2. Which
of the following statements is true?
a. The frequency of green light is higher
than blue light, and the wavelength of green light is higher than blue
light.
b. The frequency of green light is higher than
blue light, and the wavelength of green light is lower than blue light.
c. The speed of green light is higher than
blue light, and the frequency of green light is lower than blue light.
d. The frequency of green light is lower than
blue light, and the wavelength of green light is lower than blue light.
e. The frequency of green light is lower than
blue light, and the wavelength of green light is higher than blue light.
3. As the wavelength of electromagnetic radiation
increases:
a. its energy increases
b. its frequency increases
c. its speed must increase
d. more than one of the above are
true
e. none of the above is true
4. An
orbital is a region around the nucleus:
a. where an electron is always found
b. that defines the exact path of an
electron
c. where there is a high probability of
finding an electron
d. that defines the average distance of
an electron from the nucleus
e. that can contain one or more subshells of electrons
5. In
comparing the radii of an antimony (Sb) atom and a
tellurium (Te) atom (atomic numbers 51 & 52):
a. Te has a larger radius because it has
more electrons.
b. Sb has a
larger radius because it has fewer protons, so the outer shell isn't pulled in
as tightly.
c. Sb has a
smaller radius because it is has a half-filled p subshell.
d. they both have about the same radius
because they are both metalloids.
e. they both have about the same radius
because of the shielding effect.
6. In
comparing the first ionization energy (IE1) of calcium (Ca) and
magnesium (Mg):
a. Ca has a higher IE1 because
its radius is smaller.
b. Mg has a higher IE1 because
its radius is smaller.
c. Ca has a higher IE1 because
its s subshell is full.
d. Mg has a higher IE1 because
its s subshell is full.
e. they both have about the same IE1
because they have the same number of electrons in their outer shells.
7. In
comparing the radii of a nitrogen (N) atom and phosphorus (P) atom:
a. Phosphorus has a larger radius because
it has more electrons.
b. Nitrogen has a larger radius because
it has fewer protons, so the outer shell isn't pulled in as tightly.
c. Phosphorus has a larger radius because
it needs an additional electron shell to accommodate its electrons.
d. Nitrogen has a larger radius because
it has a half-filled p subshell.
e. they both have about the same radius
because of the shielding effect.
8. In
comparing the first ionization energy (IE1) of beryllium (Be) and
boron (B):
a. Be has a higher IE1 because
its radius is smaller.
b. B has a higher IE1 because
its radius is smaller.
c. Be has a higher IE1 because
its s subshell is full.
d. B has a higher IE1 because
its s subshell is full.
e. They both have about the same IE1
because B only has one more electron than Be.
9. In
comparing the radii of a titanium (Ti) atom and a
chromium (Cr) atom:
a. Cr has a larger radius because it has
more electrons.
b. Ti has a larger radius because it has
fewer protons, so the outer shell isn't pulled in as tightly.
c. Cr has a larger radius because it
needs an additional electron shell to accommodate its electrons.
d. Ti has a larger radius because it has
an extra energy level in its electron configuration.
e. They both have about the same radius
because of the shielding effect.
10. Sodium
(Na) and potassium (K) are chemically very similar because:
a. they have about the same atomic
radius
b. they have about the same ionization
energy
c. they have about the same electron
affinity
d. they have the same number of electrons
in their outer shells
e. they are both solids at room
temperature
11. In
comparing the electron affinity (EA) of phosphorus (P) and nitrogen (N):
a. phosphorus has a higher EA because its
radius is smaller.
b. nitrogen has a higher EA because its
radius is smaller.
c. phosphorus has a higher EA because its
p subshell is half full.
d. nitrogen has a higher EA because its p
subshell is half full.
e. They both have about the same EA
because they have the same number of electrons in their outer shells.
12. In
comparing the radii of a chromium (Cr) atom and a Molybdenum (Mo) atom:
a. Mo has a larger radius because it has
more electrons.
b. Cr has a larger radius because it has
fewer protons, so the outer shell isn't pulled in as tightly.
c. Mo has a larger radius because it
needs an additional electron shell to accommodate its electrons.
d. Cr has a larger radius because it has
a half-filled d subshell.
e. They both have about the same radius
because of the shielding effect.
13. In
comparing the electron affinity (EA) of sulphur (S)
and phosphorus (P):
a. S has a higher EA because its radius
is smaller.
b. P has a higher EA because its radius
is smaller.
c. S has a higher EA because its p subshell is half full.
d. P has a higher EA because its p subshell is half full.
e. They both have about the same EA
because they are right next to each other in the periodic table.
14. In
comparing the nonmetallic activity of sulphur (S) and
selenium (Se):
a.
b. Selenium is more active because it has
a lower electron affinity.
c.
d. Selenium is more active because it has
a higher electron affinity.
e. They both have about the same
activity, because they both have the same number of valence electrons.
15. In
comparing the metallic activity of calcium (Ca) and strontium (Sr):
a. Ca is more active because it has a
higher ionization energy.
b. Sr is more
active because it has a higher ionization energy.
c. Ca is more active because it has a
lower ionization energy.
d. Sr is more
active because it has a lower ionization energy.
e. They both have about the same
activity, because they have the same number of valence electrons.
16. Nonmetals
can be described as follows:
a. brittle, good conductors of heat and electricity,
gain electrons easily
b. brittle, good conductors of heat and
electricity, lose electrons easily
c. brittle, poor conductors of heat and
electricity, lose electrons easily
d. brittle, good conductors of heat and
electricity, gain electrons easily
e.
brittle, poor conductors of
heat and electricity, gain electrons easily
17. Which of the following
statements is true regarding typical potassium ions when compared to potassium
atoms (K) and argon atoms (Ar)?
a. Potassium ions have a larger radius
than either K or Ar atoms.
b. Potassium ions have a larger radius
than K atoms, but a smaller radius than Ar
atoms.
c. Potassium ions have a smaller radius
than either K or Ar atoms.
d. Potassium ions have a smaller radius
than K atoms, but a larger radius than Ar atoms.
e. Potassium ions are about the same size
as K atoms, but are larger than Ar atoms.
18.
Which of the following
statements is true regarding sulphide ions when
compared to sulphur atoms (S) and argon atoms (Ar)?
a. Sulphide
ions have a larger radius than either S or Ar
atoms.
b. Sulphide
ions have a larger radius than S atoms, but a smaller radius than Ar.
c. Sulphide
ions have a smaller radius than either S or Ar atoms.
d. Sulphide
ions have a smaller radius than S atoms, but a larger radius than Ar.
e. Sulphide
ions have about the same radius as S atoms, but are larger than Ar atoms.
19. Which
of the following tend to have more than one oxidation number:
a. alkali metals
b. alkaline earth metals
c. noble gases
d. outer transition metals
e. none of the above; all of the above
have only one oxidation number
20. Which
of the following is not a typical property of metals?
a. good electrical conductivity
b. good conductor of heat
c. malleable (easily shaped)
d. gain electrons easily
e. all of the above are properties of
metals
21. What
type of neutral atom has seven electrons in its outer shell?
a. alkali metal
b. halogen
c. noble gas
d. rare earth element
e. alkaline earth element
22. What
type of neutral atom has two electrons in its outer shell?
a. alkali metal
b. halogen
c. noble gas
d. alkaline earth element
e. none of the above
23. What
type of neutral atom has eight electrons in its outer shell?
a. alkali metal
b. halogen
c. noble gas
d. rare earth element
e. alkaline earth element
24. What
type of neutral atom has one electron in its outer shell?
a. alkali metal
b. halogen
c. noble gas
d. rare earth element
e. alkaline earth element
25. What
type of neutral atom has eight electrons in an f subshell?
a. alkali metal
b. halogen
c. noble gas
d. rare earth element
e. alkaline earth element
26. The
way in which an atom reacts chemically is determined by:
a. the number of neutrons
b. the number of electrons in its outer
shell
c. the number of electrons in the lowest
energy level
d. the average atomic mass numbers of its
isotopes
e. the arrangement of its protons
For each of the following, write the
symbol for an element that has the electron configuration described:
27.
The outer shell of a neutral
atom consists of 2 electrons in an s subshell. The next shell in from the outer shell
consists of 2 electrons in an s subshell, 6 electrons
in a p subshell, and 8 electrons in a d subshell. This could
be an atom of: (1 pt.)
28.
The outer shell of a neutral
atom consists of 2 electrons in an s subshell. The next shell in from the outer shell
consists of 2 electrons in an s subshell and 6
electrons in a p subshell. This could be an atom of: (1 pt.)
29.
The outer shell of a neutral
atom consists of 2 electrons in an s subshell and 6
electrons in a p subshell. The next shell in from the outer shell
consists of 2 electrons in an s subshell, 6 electrons
in a p subshell, and 10 electrons in a d subshell. This could
be an atom of: (1 pt.)
Short Answer / Fill in the Blank:
(1 pt. each)
30. How
many valence electrons does tellurium (Te) have? ____
31. How
many valence electrons does vanadium (V) have?
____
32. How
many different sublevels are theoretically possible in the sixth energy
level? ____
33. The
5p sublevel may contain up to how many electrons? ____
34. The
number of electrons that can exist in the same orbital of the 4f sublevel
is: ____
35. The
number of orbitals theoretically possible in the
third energy level is: ____
36. How
many electrons are in the outer energy level of an atom of germanium (Ge)? ____
37. What
element has the following electron configuration? 1s22s22p63s23p5 ______
38. How
many electrons are represented by the following electron configuration? [Ar]4s23d8 ____
39. Write
the symbol for an element that has no known compounds. _____
40.
Write the symbol for any rare
earth element: _____
41.
Write the symbol for any
halogen: _____
42.
Write the symbol for any
alkaline earth element: _____
43.
Write the symbol for an
element that has three electrons in a d subshell:
_____
44.
Write the symbol for an
element that has one electron in a p subshell: _____
45.
Write the symbol for an
element that tends to form ions with a +4 charge: ____
46.
Write the symbol for an
element that has a half-filled s subshell: _____
47.
How many electrons in an atom
can have a principal quantum number of 3 and a secondary quantum number of
2? ____
48.
How many electrons in an atom
can have a principal quantum number of 4 and a magnetic quantum number of
2? ____
49.
How many electrons in an atom
can have a principal quantum number of 2 and a secondary quantum number of
2? ____
50.
How many electrons in an atom
can have a principal quantum number of 4 and a spin quantum number of +½ ? ____
51. Write
the symbols of the following elements in order of increasing nonmetallic
activity (lowest to highest):
S, Se, Cl, As (2 pts.)
52.
Write the symbols of the
following elements in order of increasing metallic activity (lowest to
highest):
Fe, Rb,
Ca, Cu (2 pts.)
53.
Draw a p orbital. (1 pt.)
Of the elements K, Ca, Rb, Sr, Se, Br, Te, and I:
(1 pt. each)