Lab Chem Practice Test 6                Name: ____________________________   Date: _________



1.
Draw the Lewis structures for the following compounds to assist you in answering this question.

CBr2H2        BH3        XeCl4        SF4        HCl

How many of the compounds are nonpolar?
A.
1
B.
2
C.
3
D.
4
E.
5


Draw the Lewis Structure for each of the following molecules. Use the following choices to describe the molecular structure of each of the following molecules or ions.
a. linear
b. trigonal planar
c. tetrahedral
d. pyramidal
e. V-shaped
Reference: Ref 11-3

2.
CH4

Answer:


Draw the Lewis Structure for each of the following molecules. Use the following choices to describe the molecular structure of each of the following molecules or ions.
a. linear
b. trigonal planar
c. tetrahedral
d. pyramidal
e. V-shaped
Reference: Ref 11-3

3.
SO2

Answer:


Draw the Lewis Structure for each of the following molecules. Use the following choices to describe the molecular structure of each of the following molecules or ions.
a. linear
b. trigonal planar
c. tetrahedral
d. pyramidal
e. V-shaped
Reference: Ref 11-3

4.
PF3

Answer:


Draw the Lewis Structure for each of the following molecules. Use the following choices to describe the molecular structure of each of the following molecules or ions.
a. linear
b. trigonal planar
c. tetrahedral
d. pyramidal
e. V-shaped
Reference: Ref 11-3

5.
OCl2

Answer:


6.
Draw the Lews Structure for each of the following compounds:

      NH3        CO2        CH4        H2

How many of the compounds above are nonpolar?
A.
1
B.
2
C.
3
D.
4
E.
5


7.
True or false? The frequency of the wave indicates how many wave peaks pass a certain point per given time period.
A. True
B. False


8.
Which color of visible light has the most energy per photon?
A.
violet
B.
blue
C.
green
D.
yellow
E.
red


9.
Which color of visible light has the least amount of energy per photon?
A.
violet
B.
blue
C.
green
D.
yellow
E.
red


10.
Which of the following is a reasonable criticism of the Bohr model of the atom?
A.
It makes no attempt to explain why the negative electron does not eventually fall into the positive nucleus.
B.
It does not adequately predict the line spectrum of hydrogen.
C.
It does not adequately predict the ionization energy of the valence electron(s) for elements other than hydrogen.
D.
It does not adequately predict the ionization energy of the first-energy-level electrons for one-electron species for elements other than hydrogen.
E.
It shows the electrons to exist outside the nucleus.


11.
As the principal energy level increases in an atom's orbitals, the average distance of an electron energy level from the nucleus ______________.
A.
increases
B.
decreases
C.
stays the same
D.
varies
E.
none of these


12.
Consider the following representation of a 2p orbital:



Which of the following statements best describes the movement of electrons in a p orbital?
A.
The electrons move along the outer surface of the p orbital, similar to a “figure 8” type of movement.
B.
The electrons move within the two lobes of the p orbital, but never beyond the outside surface of the orbital.
C.
The electrons are concentrated at the center (node) of the two lobes.
D.
The electrons are moving in only one lobe at any given time.
E.
The electron movement cannot be exactly determined.


13.
A given set of f orbitals consists of ______________ orbital(s).
A.
1
B.
3
C.
5
D.
7
E.
9


14.
The maximum number of electrons allowed in the p sublevel of the third principal level is
A.
1
B.
2
C.
3
D.
6
E.
8


15.
The number of unpaired electrons in a nitrogen atom is
A.
1
B.
2
C.
3
D.
4
E.
5


16.
Choose the correct electron configuration for oxygen in an excited state.
A.
1s22s22p4
B.
1s22s22p32d1
C.
1s22s22p44s1
D.
1s22s22p34s1
E.
1s22s22p34s14p1


17.
The number of electrons in the third sublevel of an iron atom is
A.
3
B.
6
C.
8
D.
26
E.
56


18.
All these atoms have seven electrons in their outermost energy levels except
A.
H
B.
F
C.
Cl
D.
Br
E.
I


19.
The maximum number of electrons in the second principal energy level of an atom is
A.
2
B.
6
C.
8
D.
18
E.
32


20.
When moving down a group (family) in the periodic table, the number of valence electrons
A.
remains constant
B.
increases by 2 then 8 then 18 then 32
C.
doubles with each move
D.
decreases regularly
E.
changes in an unpredictable manner


21.
The Group III elements through the Group VIII elements form an area of the periodic table where the electron sublevels being filled are
A.
p orbitals
B.
s and p orbitals
C.
d orbitals
D.
p and d orbitals
E.
f orbitals


22.
How many unpaired electrons does the element cobalt (Co) have in its lowest energy state?
A.
0
B.
1
C.
2
D.
3
E.
7


23.
How many of the following electron configurations for the species in their ground state are correct?
I. Ca: 1s22s22p63s23p64s2
II. Mg: 1s22s22p63s1
III. V: [Ar] 3s23d3
IV. As: [Ar] 4s23d104p3
V. P: 1s22s22p63p5
A.
1
B.
2
C.
3
D.
4
E.
5


24.
True or false? The 47th electron of silver, Ag, will be in a d orbital.
A. True
B. False


25.
Consider the following representation of the one orbital below. The points represent various electron locations.

Where could an electron be located in the representation above?
A.
Point A
B.
Point B
C.
Point C
D.
Point D
E.
An electron could be located at any of these points.


26.
What element has the electron configuration 1s22s22p63s23p64s23d104p5?
A.
Cl
B.
Se
C.
I
D.
Kr
E.
Br


27.
What element has the electron configuration 1s22s22p63s23p3?
A.
N
B.
P
C.
S
D.
Al
E.
Cl


28.
What element has the electron configuration 1s22s22p63s23p64s23d104p65s24d105p66s2?
A.
Ba
B.
Sn
C.
Pb
D.
Po
E.
none of these


29.
Write the electron configuration for Co.

Answer:


30.
Write the electron configuration for Ca.

Answer:


31.
Write the electron configuration for Cd.

Answer:


32.
Which of the following statements is true?
A.
The krypton 1s orbital is smaller than the helium 1s orbital because krypton’s p and d orbitals crowd the s orbitals.
B.
The krypton 1s orbital is larger than the helium 1s orbital because krypton contains more electrons.
C.
The krypton 1s orbital is smaller than the helium 1s orbital because krypton’s nuclear charge draws the electrons closer.
D.
The krypton 1s orbital and helium 1s orbital are the same size because both s orbitals can only have two electrons.
E.
The krypton 1s orbital is larger than the helium 1s orbital because krypton’s ionization energy is lower so it’s easier to remove electrons.


33.
Which of the following atoms has the smallest atomic radius?
A.
As
B.
Sb
C.
Bi
D.
P
E.
N


34.
True or false? Covalent bonding occurs when a metal reacts with a nonmetal.
A. True
B. False


Use the following choices to classify the bonds in each of the following molecules.
a. ionic
b. polar covalent
c. non polar covalent
Reference: Ref 11-1

35.
OCl2 ______________

Answer:


Use the following choices to classify the bonds in each of the following molecules.
a. ionic
b. polar covalent
c. non polar covalent
Reference: Ref 11-1

36.
K2O ______________

Answer:


Use the following choices to classify the bonds in each of the following molecules.
a. ionic
b. polar covalent
c. non polar covalent
Reference: Ref 11-1

37.
CoCl2 ______________

Answer:


Use the following choices to classify the bonds in each of the following molecules.
a. ionic
b. polar covalent
c. non polar covalent
Reference: Ref 11-1

38.
CF4 ______________

Answer:


39.
Which of the following compounds contains an ionic bond?
A.
HCl(g)
B.
NaCl
C.
CCl4
D.
SO2
E.
O2


40.
Which of the following compounds contains one or more covalent bonds?
A.
NaCl
B.
CaO
C.
CO2
D.
Cs2O
E.
BaBr2


41.
The least electronegative element of those listed is
A.
O
B.
Pb
C.
Ba
D.
Cu
E.
Se


42.
Arrange the following elements in order of increasing electronegativity (from the smallest to the largest): N, Be, F, C.
A.
N < C < Be < F
B.
C < F < Be < N
C.
F < N < C < Be
D.
Be < C < N < F
E.
C < N < F < Be


43.
One of the most important characteristics of the water molecule is its ______________, which allows it to surround and attract both positive and negative ions.
A.
polarity
B.
strength
C.
magnetism
D.
fluidity
E.
stability


44.
Which of the following has the smallest radius?
A.
S2-
B.
Cl-
C.
Ar
D.
K+
E.
Ca2+


45.
Which of the following ions has the same electron configuration as an argon atom?
A.
Br-
B.
S3-
C.
P3+
D.
K+
E.
Ca+


46.
The electron configuration for Ca2+ is identical to that of
A.
Ne
B.
Kr
C.
Ca
D.
Ar


47.
Which of the following is the product of the reaction Al + O2?
A.
AlO
B.
AlO2
C.
AlO3
D.
Al3O2
E.
Al2O3


48.
Which element listed below has the electron configuration 1s22s22p63s23p4?
A.
Se
B.
O
C.
P
D.
S
E.
none of these


49.
Write the electron configuration for Sr2+.

Answer:


50.
True or false? A packet of energy of electromagnetic radiation is called a neutron.
A. True
B. False


51.
A photon is produced when an electron
A.
moves to a higher energy level
B.
moves to a lower energy level
C.
absorbs energy
D.
is in an orbital


52.
Which of the following species are polar? (Check all that apply.)
 
A.
HBr
B.
NO3–
C.
H2O
D.
SF4
E.
KrCl4
F.
I3–

Answer:


53.
Which of the following atoms has the highest ionization energy?
A.
Al
B.
Si
C.
P
D.
As
E.
Sb


54.
Which of the following statements is correct and provides the best explanation for what happens when the first two electrons are removed from calcium?
A.
Energy is released when either electron comes off since calcium is a metal and not very electronegative.
B.
It takes less energy to remove the second electron from calcium as compared to the first because calcium wants to have eight electrons in its outer shell (and thus have a noble gas configuration).
C.
It takes less energy to remove the first electron as compared to the second because it is in a higher energy level than the second electron.
D.
It takes more energy to remove the second electron as compared to the first because the nucleus binds the electrons more tightly as each electron is removed.
E.
Electrons cannot be removed from calcium since it is a metal and only wants to gain electrons to become more stable.


55.
Order the elements S, Cl, and F in terms of increasing ionization energy.
A.
S, Cl, F
B.
Cl, F, S
C.
F, S, Cl
D.
F, Cl, S
E.
S, F, Cl


STOP This is the end of the test. When you have completed all the questions and reviewed your answers, press the button below to grade the test.