Name: 
 

Chemistry Review Test 2007


Multiple Choice
Identify the choice that best completes the statement or answers the question.
 

 1. 
Fluorine 19 has a atomic mass number of 19 and an atomic number of 9.  How many protons does it have?
a.
6
b.
9
c.
10
d.
19
e.
28
 

 2. 
When Fluorine 19 is in a neutral state (no charge), how many electrons does it have?
a.
6
b.
9
c.
10
d.
19
e.
28
 

 3. 
How many neutrons does Fluorine 19 have?
a.
6
b.
9
c.
10
d.
19
e.
28
 

 4. 
The atomic number of an element is equivalent to the number of _____.
a.
protons.
b.
neutrons.
c.
protons plus electrons.
d.
protons plus neutrons.
e.
valence shells.
 

 5. 
The atomic mass of an element is approximately equivalent to the number of _____.
a.
protons.     
b.
neutrons.
c.
protons plus electrons.     
d.
protons plus neutrons.     
e.
valence shells.
 

 6. 
In its neutral state, the atom with which of the following atomic numbers would be most stable?
a.
1
b.
3
c.
7
d.
12
e.
18
 

 7. 
Forms of an element with different number of neutrons are _____.
a.
compounds
b.
molecules
c.
ions
d.
polar
e.
isotopes
 

 8. 
Glucose has the chemical formula C6H12O6.  How many atoms of oxygen does glucose contain?
a.
1
b.
6
c.
12
d.
16
e.
24
 

 9. 
Glucose has the chemical formula C6H12O6.  In 12 molecules of glucose, how many atoms of oxygen are there?
a.
6
b.
24
c.
48
d.
56
e.
72
 

 10. 
Consider a single glucose molecule, C6H12O6, and six molecules of carbon dioxide, CO2.  Which of the following statements is true?
a.
The two have identical numbers of carbon atoms.
b.
Six molecules of carbon dioxide have twice as many carbon atoms as a single glucose.
c.
The number of carbons atoms in six molecules of carbon dioxide will differ depending on its temperature.
d.
Glucose is made of a total of 12 atoms.
e.
None of the above statements are true.
 

 11. 
Magnesium has an atomic mass of 24.  Sulfur has an atomic mass of 32.  Oxygen has an atomic mass of 16.  Which is the best approximation of the molecular mass of MgSO4? 
a.
24
b.
72
c.
96
d.
120
e.
184
 

 12. 
A carbon atom has 4 electrons in its valence shell.  As a result, it generally forms _____ bonds with other atoms.
a.
2
b.
3
c.
4
d.
6
e.
8
 

 13. 
Look at the four molecules drawn below.  Consider the number of covalent bonds normally formed by hydrogen, oxygen, and carbon.  Look carefully at the following structures and determine which molecule is drawn correctly.
mc013-1.jpg
a.
a
b.
b
c.
c
d.
d
e.
none
 

 14. 
Which statement best describes why ions form?
a.
losing electrons always makes an atom more stable.
b.
ions need to form before atoms can form covalent bonds.
c.
ions form when atoms lose or gain electrons to fill its valence shell.
d.
ions are always more stable than the neutral form of the atom.
e.
none of the above.
 

 15. 
Consider a sodium ion.  When written in the form Na+, you can assume the atom has _____.
a.
gained one electron
b.
gained two electrons
c.
gained a proton
d.
lost one electron
e.
lost two electrons
 

 16. 
An ion forms by gaining or losing a(n) _____.
a.
proton
b.
neutron
c.
electron
d.
molecule
e.
nucleus
 

 17. 
Which of the following is an example of a stable ion?
a.
Ca5+
b.
Na2+
c.
O2
d.
H2O
e.
Cl-
 

 18. 
Which of the following statements does not describe an ionic interaction?
a.
atoms share electrons to form the bond.
b.
this type of bond is holds table salt together.
c.
it is a relatively weak interaction in solution and can be broken easily.
d.
they are weaker than covalent bonds.
e.
it is the interaction of oppositely charged ions.
 

 19. 
You have a solution with a pH of 4.  Which of the following statements is true?
a.
It must have a higher concentration of hydrogen ions compared to a solution with pH 2.
b.
The solution is basic.
c.
The solution has a concentration of hydrogen ions 100 times that of a solution with pH 6.
d.
It must have a lower concentration of hydrogen ions compared to a solution with pH 10.
e.
All of the statements are true.
 

 20. 
A chemically buffered solution _____.
a.
resists fluctuations in pH.
b.
is important in our bodies because living cells usually have a narrow range of pH in which they can function.
c.
is able to maintain a specific pH range; in other words, different buffers can maintain different pH’s.
d.
contain both molecules that can give off additional hydrogen ions and molecules that can bond with excess hydrogen ions to maintain a specific concentration of hydrogen ions in the solution.
e.
all of the above.
 

 21. 
Water is able to form hydrogen bonds because _____.
a.
the hydrogen atoms in a water molecule are weakly positive.
b.
the oxygen atom in a water molecule are weakly positive.
c.
one water molecule covalently bonds to other water molecules.
d.
electrons in the covalent bond between the oxygen atom and hydrogen atom in the same water molecule are shared equally.
e.
all of the above.
 

 22. 
Consider a single water molecule.  Which of the following statements describes the covalent bonds holding the molecule together?
a.
There are four electrons being shared in each covalent bond.
b.
This bond is polar; electrons shared between the oxygen and hydrogen are not distributed equally.
c.
They are weak bonds that are easily broken.
d.
This bond is broken when water evaporates.
e.
All of the statements describe covalent bonds found in water.
 

 23. 
The temperature of evaporation (liquid into gas) is much higher for water than for another liquid (call it X for this question).  Without knowing more about the chemistry of X, which of the following is the most logical chemical explanation for this observation?
a.
Covalent bonds form between molecules of X.  Since these are weak bonds, it takes less energy for liquid X to vaporize than it does for water.
b.
Liquid X must have higher surface tension than water.
c.
Water must form more hydrogen bonds between its molecules, requiring a relatively significant amount of energy to break individual water molecules away from each other.
d.
Both (a) and (c) must be true.
e.
Both (b) and (c) must be true.
 
 
The following four diagrams show different orientations of five water molecules.  Note that the diagrams vary in water molecule orientation and partial charges on the atoms.  Study the diagrams carefully and answer the following questions.

nar001-1.jpgnar001-2.jpg
nar001-3.jpgnar001-4.jpg
 

 24. 
Which of the above four diagrams show the correct orientation of water molecules interacting as a liquid?
a.
1.
b.
2.
c.
3.
d.
4.
e.
Both (1) and (4) are possible orientations.
 

 25. 
The interaction between individual water molecules:
a.
are weak interactions between opposite partial charges.
b.
break when temperature is increased.
c.
are covalent bonds.
d.
both (a) and (b) above.
e.
all answers are correct.
 



 
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