# Test number under student ID

```M-Exam 2
test # ……………
NAME……..…………….......................................................
BIG SCANTRON: 1-Write LAST NAME first, first name last 2-Test number under
student ID .
E = RH (1/nf2-1/ni2)
Solubility table
1) The total concentration of ions in a 0.250 M solution of HCl is __________.
A) essentially zero.
B) 0.125 M
C) 0.250 M
D) 0.500 M
E) 0.750 M
2) The net
ionic equation for the reaction between aqueous solutions of HF and KOH is
__________.
A) HF  KOH  H 2 O  K   F
B) HF  OH   H 2 O  F
C) HF  K   OH   H 2 O  KF
D) H   OH   H 2 O
E) H   F  K   OH   H 2 O  K   F
3) What is the concentration (M) of KCl in a solution made by mixing 25.0 mL of 0.100 M KCl
with 50.0 mL of 0.100 M KCl?
A) 0.100
B) 0.0500
C) 0.0333
D) 0.0250
E) 125
4) What is the concentration (M) of CH 3 OH in a solution prepared by dissolving 11.7 g of
CH 3 OH in sufficient water to give exactly 230 mL of solution?
A) 11.9
B) 1.59  10-3
C) 0.0841
D) 1.59
E) 11.9 10-3
5) There are __________ mol of bromide ions in 0.500 L of a 0.300 M solution of AlBr 3 .
A) 0.150
B) 0.0500
C) 0.450
D) 0.167
E) 0.500
6) Calculate the concentration (M) of sodium ions in a solution made by diluting 50.0 mL of a
0.874 M solution of sodium sulfide to a total volume of 250.0 mL.
A) 0.175
B) 4.37
C) 0.525
D) 0.350
E) 0.874
7) The wavelength of a photon that has an energy of 5.25  1019 J is __________ m.
A) 3.79 107
B) 2.64 106
C) 2.38 1023
D) 4.211024
E) 3.79 107
8) Calculate the energy (J) change associated with an electron transition from n = 2 to n = 5 in a
Bohr hydrogen atom.
A) 6.5  10 19
B) 5.5 1019
C) 8.7  10 20
D) 4.6  10 19
E) 5.8 1053
9) The lowest energy shell that contains f orbitals is the shell with n = __________.
A) 3
B) 2
C) 4
D) 1
E) 5
10) In a hydrogen atom, an electron in a __________ orbital can absorb a photon, but cannot
emit a photon.
A) 3s
B) 2s
C) 3p
D) 1s
E) 3f
11)
[Ar]4s2 3d10 4p3 is the electron configuration of a(n) __________ atom.
A) As
B) V
C) P
D) Sb
E) Sn
12) A 31.5 mL aliquot of H 2 SO 4 (aq) of unknown concentration was titrated with 0.0134 M
NaOH (aq). It took 23.9 mL of the base to reach the endpoint of the titration. The concentration
(M) of the acid was __________.
A) 0.0102
B) 0.00508
C) 0.0204
D) 0.102
E) 0.227
13) Which combination will produce a precipitate?
A) NH 4 OH (aq) and HCl (aq)
B) AgNO 3 (aq) and Ca(C 2H 3O 2) 2(aq)
C) NaOH (aq) and HCl (aq)
D) NaCl (aq) and HC 2 H 3 O 2 (aq)
E) NaOH (aq) and Fe(NO 3 ) 2 (aq)
14) The lowest orbital energy is reached when the number of electrons with the same spin is
maximized. This statement describes __________.
A) Pauli Exclusion Principle
B) Planck's constant
C) deBroglie hypothesis
D) Heisenberg Uncertainty Principle
E) Hund's rule
15) Which set of three quantum numbers (n, l, ml) corresponds to a 3d orbital?
A) 3, 2, 2
B) 3, 3, 2
C) 3, 2, 3
D) 2, 1, 0
E) 2, 3, 3
16) Which one of the following represents an impossible set of quantum numbers for an electron
in an atom? (arranged as n, l, ml, and ms)
A) 2, 1, -1, -1/2
B) 1, 0, 0, 1/2
C) 3, 3, 3, 1/2
D) 5, 4, - 3, 1/2
E) 5, 4, -3, -1/2
17) Which electron configuration represents a violation of the Pauli exclusion principle?
A)
B)
C)
D)
E)
18) The valence shell of the element X contains 2 electrons in a 5s subshell. Below that shell,
element X has a partially filled 4d subshell. What type of element is X?
A) main group element
B) chalcogen
C) halogen
D) transition metal
E) alkali metal
19)An electron in a(n) __________ subshell experiences the smallest effective nuclear
charge in a many-electron atom.
A) 3f
B) 3p
C) 3d
D) 3s
E) 4s
20)A tin atom has 50 electrons. Electrons in the __________ subshell experience the higest
effective nuclear charge.
A) 1s
B) 3p
C) 3d
D) 5s
E) 5p
21) The first ionization energies of the elements __________ as you go from right to left across a
period of the periodic table, and __________ as you go from the top to the bottom of a group in
the table.
A) increase, increase
B) increase, decrease
C) decrease, increase
D) decrease, decrease
E) are completely unpredictable
22) In
which set of elements would all members be expected to have very similar chemical
properties?
A) Ca, Sr, Ba
B) N, O, F
C) Na, Mg, K
D) S, Se, Si
E) Ne, Na, Mg
23) Of the hydrogen halides, only __________ is a weak acid.
A) HCl (aq)
B) HBr (aq)
C) HF (aq)
D) HI (aq)
E) They are all weak acids.
24)Atomic radius generally increases as we move __________.
A) down a group and from right to left across a period
B) up a group and from left to right across a period
C) down a group and from left to right across a period
D) up a group and from right to left across a period
E) down a group; the period position has no effect
25) Which of the following correctly lists the five atoms in order of increasing size (smallest to
largest)?
A) O &lt; F &lt; S &lt; Mg &lt; Ba
B) F &lt; O &lt; S
C) F &lt; O &lt; S
D) O &lt; F &lt; S
E) F &lt; S &lt; O
&lt;
&lt;
&lt;
&lt;
Mg &lt; Ba
Ba &lt; Mg
Ba &lt; Mg
Mg &lt; Ba
26) Of the choices below, which gives the order for first ionization energies?
A) Cl &gt; S &gt; Al &gt; Ar &gt; Si
B) Ar &gt; Cl &gt; S &gt; Si &gt; Al
C) Al &gt; Si &gt; S &gt; Cl &gt; Ar
D) Cl &gt; S &gt; Al &gt; Si &gt; Ar
E) S &gt; Si &gt; Cl &gt; Al &gt; Ar
27)Which of the following has the largest second ionization energy?
A) Si
B) Mg
C) Al
D) Na
E) P
28)
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