Name: _____________________________________
AP Chemistry: Unit 7 Test
Questions 1 – 3
(A)
Cs
(B)
Ag
(C)
Pb
(D)
Br
(E)
Se
1.
Has the highest electronegativity
2.
Has the lowest first ionization energy
3.
Has the largest atomic radius.
4.
Which of the following statements about atoms is NOT correct?
(A)
Atoms are electrically neutral because they have the same number of protons and electrons.
(B)
All atoms of a given element must have the same number of protons, neutrons, and electrons.
(C)
Most of the volume of an atom contains only electrons.
(D)
The nucleus is positively charged.
(E)
Almost all of the mass of an atom is in the nucleus.
5.
(A)
(B)
(C)
(D)
(E)
Which of the following best helps to account for the fact that the F- ion is smaller than the O2- ion?
F- has a larger nuclear mass than O2- has
F- has a larger nuclear charge than O2- has
F- has more electrons than O2- has
F- is more electronegative than O2- is
F- is more polarizable than O2- is
6.
Which of the following shows the correct number of protons, neutrons, and electrons in a neutral
cesium-134 atom?
Proton
Neutrons
Electrons
55
55
55
55
79
55
55
79
79
79
55
79
`
134
55
134
(A)
(B)
(C)
(D)
(E)
Consider atoms of the following elements for questions 7 and 8 below. Assume that the atoms are in the ground
state.
(A)
(B)
(C)
(D)
(E)
S
Ca
Ga
Sb
Br
7.
The atom that contains exactly two unpaired electrons
8.
The atom that contains only one electron in the highest occupied energy level orbital.
9.
In which of the following groups are the three species isoelectronic; i.e., have the same number of
electrons?
(A)
(B)
(C)
(D)
(E)
S2-, K+, Ca2+
Sc, Ti, V2+
O2-, S2-, ClMg2+, Ca2+, Sr2+
Cs, Ba2+, La3+
10.
The atomic mass of copper is 63.55. Given that there are only two naturally occurring isotopes of
copper, 63Cu and 65Cu, the natural abundance of the 65Cu isotope must be approximately:
(A)
(B)
(C)
(D)
(E)
90 %
70 %
50 %
25 %
10 %
11.
Which of the following properties generally decreases across the periodic table from sodium to chlorine?
(A)
(B)
(C)
(D)
(E)
First ionization energy
Atomic mass
Electronegativity
Maximum value of the oxidation number
Atomic radius
12.
The effective nuclear charge experienced by the outermost electron of Na is different than the effective
nuclear charge experienced by the outermost electron of Ne. This difference best accounts for which of
the following?
Na has a greater density at standard conditions than Ne.
Na has a lower first ionization energy than Ne.
Na has a higher melting point than Ne.
Na has a higher neutron-to-proton ratio than Ne.
(A)
(B)
(C)
(D)
Question 13-16 refer to atoms for which the occupied atomic orbitals shown below.
13. Represents an atom that is chemically unreactive
14. Represents an atom in an excited state
15. Represents an atom that has four valence electrons.
16. Represents an atom of a transition metal.
17.
In the Born–Haber cycle for
energy of Na?
, which of the following processes corresponds to the first ionization
A)
B)
C)
D)
E)
18. Which of the following is a correct interpretation of the results of Rutherford's experiments in which gold
atoms were bombarded with alpha particles?
(A) Atoms have equal numbers of positive and negative charges.
(B) Electrons in atoms are arranged in shells.
(C) Neutrons are at the center of an atom.
(D) Neutrons and protons in atoms have nearly equal mass.
(E) The positive charge of an atom is concentrated in a small region.
Questions 20-23
(A) Heisenberg uncertainty principle
(B) Pauli exclusion principle
(C) Hund's rule (principle of maximum multiplicity)
(D) Shielding effect
(E) Wave nature of matter
19. Indicates that an atomic orbital can hold no more than two electrons
20. Predicts that it is impossible to determine simultaneously the exact position and the exact velocity of an
electron
Short Answer Problems:
1) Account for each of the following in terms of principles of atomic structure, including the number,
properties, and arrangements of subatomic particles.
(a) The second ionization energy of sodium is about three time greater than the second ionization energy of
magnesium.
(b) The difference between the atomic radii of Na and K is relatively large compared to the difference between
the atomic radii of Rb and Cs.
(c) The radius of the Ca atom is 0.197 nanometer; the radius of the Ca2+ ion is 0.099 nanometer. Account for
this difference.
2. Calculate the energy of a photon of electromagnetic radiation for blue light (480 nm).
3. Write the complete electron configuration for the following particles:
a)!
22Ti
b)!
14Si
c)!
31Ga
d)!
17Cl
e)!
27Co
3+
1-
2+