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1st Semester Final Review
* DO THESE PROBLEMS WITHOUT A CALCULATOR! *
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Name _________________________ KEY
Per ____ Date _______
Chemistry 1st Semester Final Review
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Bring a pencil and eraser for the exam. There will be no calculators allowed.
You will be given: PT (know names of #1-36, Au, Ag, Sn, Pb, Hg), activity series, solubility chart.
There will be 80 M/C questions worth 2.5 points each for a total of 200 points
% breakdown:
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6 questions each on Units 1 (ch 1 & 3), 2 (ch 2), 3 (ch 4 and 25), 4 (ch 5 & 6)
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about 14 questions each on Units 5 (ch 7,8,9), 6 (ch 10), 7 (ch 11), part of 8 (ch 12.1-12.2 (up to mole-mole)
Your lowest unit test score will be replaced if you score higher (in %) on the final [NOT the midterm]
o
Example:
Final
Exam
Unit 1
Unit 2
Midterm
Unit 5
Unit 6
previous
%
80
74
60
97
70
83
adjusted
%
80
74
60
97
83
83
o
Note: if your final score is not higher than any past unit exams, your scores will remain as is.
To review for Units 1-4, refer back to the 1st quarter midterm review WS
Final Schedule:
Tues 2, 3, wed, 5 and 6, thurs is 1 and 4
1st Quarter – a few questions to review (for the rest refer back to the 1st Quarter Midterm Review WS)
1. Complete the table:
Species
Name
Atomic Mass (amu)
# of Protons
# of Electrons
# of Neutrons
Al3+
Aluminum ion
27
13
13
14
S2-
Sulfide ion
32
16
16
16
2. Which pair of the following is correct to compare the size of radius?
A) F >F- , Na >Na+
B) F >F- , Na <Na+
C) F <F- , Na >Na+
D) F <F- , Na <Na+
UNIT 5 (Chapters 7, 8, 9) REVIEW – Ionic & Covalent Compounds
… Ionic Compounds
3. On the periodic table, label the charge with elements for groups 1, 2, and 13 – 18 when/if they form ions.
Label the charge of silver _+1, cadmium_+2, zinc +2, aluminum +3, and gallium +3 when they form ions.
1+
2+
3+
3-
2-
0
1-
4. Which of the followings correctly explained?
A) Metals lose electrons to form anions and nonmetals gain electrons to form cations.
B) Metals lose electrons to form cations and nonmetals gain electrons to form anions.
C) Metals gain electrons to form anions and nonmetals lose electrons to form cations.
D) Metals gain electrons to form cations and nonmetals lose electrons to form anions.
5. What types of elements compose an ionic compound?
A) all nonmetals
B) metals and nonmetals
C) all metals
D) none of the above
6. What are the characteristics/properties of an ionic compound (circle all that apply)?
A) dull
B) lustrous
C) malleable
D) ductile
E) hard
F) soft
G) usually solids at room temperature
H) are all soluble in water
I) conducts electricity as a solid
J) conducts electricity when dissolved in water
7. Which of the followings is correctly written in chemical formula if iron (III) ion and oxide ion.
A) FeO
B) Fe2O
C) FeO2
D) Fe2O3
E) Fe3O2
8. Write the corresponding name or formula.
1st Semester Final Review
Compound
Formula
Na2S
p. 2 of 6
Compound Name
Compound Name
Compound Formula
Sodium sulfide
Ammonium Sulfate
(NH4)2SO4
ZnCO3
Zinc carbonate
Iron (III) Bromide
FeBr3
Mg3N2
Magnesium nitride
Copper (II) Chloride
CuCl2
Ni(OH)2
Nickel(II) hydroxide
Silver Acetate
AgC2H3O2
AlCl3
Aluminum chloride
Potassium Oxide
K2O
Ca3(PO4)2
Calcium phosphate
Lithium Fluoride
LiF
… Covalent Compounds
9. Indicate the number represented by the prefixes:
mono-, di-, tri-, tetra-, penta-, hexa-, hepta-, octa-, nona-, deca. 1-10, respectively
10. Complete the following chart
bonds between (M+NM, NM)
Transfer or shares electrons?
IONIC
M+ NM
Transfer
COVALENT
NM
Share
Use charges to determine formula? (yes/no)
Yes
No
Switch charges to balance out formula? (yes/no)
Yes
No
Use prefixes? (yes/no)
Simplify to lowest whole # ratio? (yes/no)
Acids or ammonium compounds
Conducts electricity
High melting and boiling point
No
Yes
Yes
Yes
In aqueous form, yes
Yes
magnesium phosphide
Mg3P2
No
No
No
No (have lower)
disulfur monobromide
S2Br
Provide formula
11. What is the correct chemical name for NH3?
a. nitrogen hydroxide b. nitrogen (III) hydride c. nitrogen (III) hydroxide
12. What is the correct name for P4O10?
a. potassium oxide
d. decphosphoroush tetraphosphide
d. nitrogen trihydride
b. potassium decoxide
c. phosphorous decoxide
e. tetraphosphorous decoxide
13. Write the corresponding formula and indicate if the substance is ionic or covalent.
Name
I/C
Formula
Name
I/C
Formula
Sulfur hexafluoride
C
SF6
triphosphorus dioxide
C
P3O2
Nitrogen trihydride
C
NH3
tetracarbon monofluoride
C
C4F
Pentaphosphorus monoxide
C
P5O
lead (III) phosphide
I
PbP
iron (II) hydroxide
I
Fe(OH)2
zinc nitrate
I
Zn(NO3)2
ammonium sulfide
I
(NH4)2S
Aluminum carbonate
I
Al2(CO3)3
14. Describe the difference between an intramolecular bond and an intermolecular force. Use water as your
example.
Intramolecular – within a molecule (ex: for H-O-H, it is the bond between H-O and O-H).
Intermolecular – between molecules (ex: for H2O, the attraction between many H2O molecules).
15. Rank the following forces in increasing intermolecular attraction: dipole-dipole, hydrogen-bond, electrostatic,
dispersion force.
Dispersion, dipole-dipole, hydrogen-bond, electrostatic attraction
16. What type of intermolecular forces does water, sodium chloride, oxygen, and carbon monoxide have?
Hydrogen bonding, electrostatic attraction, dispersion, and dipole-dipole, respectively.
17. Which is stronger:
intermolecular forces or ionic bonds?
Ionic bonds or covalent bonds?
1st Semester Final Review
p. 3 of 6
hydrogen bonds or covalent bonds?
dipole-dipole or covalent bonds?
18. Explain the octet rule. In forming compounds, atoms tend to achieve the electron configuration of a
noble gas such as ns2np6. An octet is a set of eight.
19. Complete the following table. A reference chart is provided at the bottom.
# valence
Formula
Lewis dot structure
3-D Lewis Dot
electrons
SO3
6 + 3(6) = 24
CSe2
4 + 2(6) = 16
NCl3
5 + 3(7) = 26
: Se = C = Se :
..
..
Geometry/
Shape
Trigonal planar
(3 bonds, 0 lone)
Linear
(2 bonds, 0 lone)
: Se = C = Se :
..
..
Trigonal
pyramidal
(3 bonds, 1 lone)
Reference chart:
Geometry
# atoms
around central atom
# lone pairs
around central atom
Linear
2
0
Trigonal planar
3
0
Bent
2
1
Tetrahedral
4
0
Trigonal pyramidal
3
1
Bent
2
2
4
20. Given the following Lewis Dot structure, how many electrons are shared between AX?
21. Given the following Lewis Dot structures, how many lone pairs are around the central atom?
A.
2
0
B.
22. Which of the following structures is the correct VSEPR shape for carbon dioxide?
A.
B.
C.
23. Which of the following is the correct Lewis Dot Representation for phosphorous trihydride?
a.
b.
c.
d.
e. none of these
24. Which of the following is the correct Lewis Dot Representation for boron trifluoride
a.
b.
c.
d.
e. none of these
(should look like this:
25. Which of the following is an example of a non-polar covalent bond?
a. water
b. hydrofluoric acid
c. sodium bromide
d. chlorine (Cl – Cl)
UNIT 6 (Chapter 10) REVIEW – The Mole
26. Avogadro's number of representative particles is equal to one ____.
A) gram
B) mole
C) kilogram
D) atom
E) two of the above are true
)
1st Semester Final Review
p. 4 of 6
27. All of the following are equal to Avogadro's number EXCEPT ____.
A) the number of atoms of bromine in 1 mol Br2 (there are 2 (6.022x1023) atoms in Br2)
B) the number of atoms of gold in 1 mol Au
C) the number of molecules of nitrogen in 1 mol N2
D) the number of molecules of carbon monoxide in 1 mol CO
E) the number of formula units of magnesium chloride in 1 mol MgCl2
28. How many hydrogen atoms are in 5 molecules of isopropyl alcohol, C3H7O?
A) 5 x (6.02 x 1023)
B) 35 x (6.02 x 1023)
C) 35
D) 5
5 molecules C3H 7 O 
E) 7
7 atoms H
 35 atoms H
1 molecule C3H 7 O
29. How many moles of gold atoms are in 2.0 x 1023 atoms of gold?
A) 6.022 x 1023
B) 1.0
C) 0.50
D) 0.33
2.0 x1023 atoms Au 
1 mol Au
 0.33 mol Au
6.022 x1023 atoms Au
30. How many formula units are in 0.50 mol of sodium chloride?
A) 6.022 x 1023
B) 3.0 x 1023 C) 1.20 x 1024
0.50 mol NaCl 
E) 0.50 / 6.022x 1023
D) 3.0
6.022 x1023 formula units NaCl
 3.0 x1023 mol Au
1 mol NaCl
31. The mass of a mole of NaCl is the ____
A) atomic mass
B) molecular mass
C) molar mass
32. How many carbon atoms are found in 2.0 mol of C6H12O6?
A) 6.0
B) 12
C) 12 x (6.022 x 1023)
2.0 mol C6 H12O6 
E) 2 (6.022 x 1023)
D) average mass
D) 1.2 x 1024
E) 12 / (6.022 x 1023)
6.022 x1023 molecules C6 H12O6
6 atoms C

 12(6.022 x1023 ) atoms C
1 mol C6 H12O6
1 molec. C6 H12 O6
33. What is the molar mass of carbon dioxide?
A) 28.01 g/mol
B) 40.02 g/mol
C) 44.01 g/mol
CO2 = 1 (12.01) + 2 (16.00) = 44.01 g/mol
D) 76.01 g/mol
34. What is the molar mass of calcium hydroxide?
A) 41 g/mol
B) 57 g/mol
C) 58 g/mol
Ca(OH)2 = 1 (40) + 2 (16) + 2 (1.01) = 74.02 g/mol
D) 74 g/mol
35. What is the number of moles of argon atoms in 120 g of argon?
A) 0.50 mol
B) 2.0 mol
C) 3.0 mol
D) 120 x (6.022 x 1023) mol
120 g Ar 
E) 6.022 x 1023 mol
1 mol Ar
 3.0 mol Ar
40 g Ar
36. Pencil lead is composed of graphite, which is made of carbon. How many atoms of carbon can be found in 6.0
g of pencil lead?
A) 1.0
B) 3.01 x 1023
C) 6.022 x 1023
D) 6 x 12 (6.022 x 1023)
E) 6.0
6.0 g C 
1 mol C 6.022 x1023 atoms C

 3.01x1023 atoms C
12.01 g C
1 mol C
37. The lowest whole-number ratio of the elements in a compound is called the ____.
A) empirical formula B) molecular formula C) mole ratio D) lowest common denominator formula
38. Which of the following is NOT an empirical formula?
1st Semester Final Review
A) C2N2H7
p. 5 of 6
B) C3H9O6
C) Na2SO4
D) Sb2S3
E) at least two of the above
39. Which of the following is NOT true about empirical and molecular formulas?
A) The molecular formula of a compound can be the same as its empirical formula.
B) The molecular formula of a compound can be some whole-number multiple of its empirical formula.
C) Several compounds can have the same empirical formula, but have different molecular formulas.
D) The empirical formula of a compound can be triple its molecular formula.
E) at least two of the above are not true
40. If the molar mass of a compound is 266.7 g/mol and its empirical formula is B2H5, determine the molecular
formula.
A) 23
B) 10
C) B4H10
D) B6H15
E) B20H50
n
MM MF
266.7
266.7


 10  MF  10( EF )  10(B2 H 5 )= B20 H 50
MM EF 2(11)  5(1)
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UNIT 7 (Chapter 11) REVIEW – Balancing Equations, Reaction Types
41. When performing an experiment evidence of a chemical change includes
A) a color change
B) release of a gas
C) release of energy in form of heat or light
D) all of the above
42. The choice with the correct shorthand and meaning is:
A) (s) = solid, (aq) = gas
B) (g) = gas, (l) = liquid
C) (aq) = aqueous, (l) = lethal
D) all of these
43. Which of the following is true about this reaction: NaCl (aq) + AgNO3 (aq)  NaNO3(aq) + AgCl (s)
A) This is a single replacement reaction.
B) The cations of both reactants will switch places.
C) A white solid will form from two solutions.
D) Two of the above are true (choices B and C are true)
Balance each reaction and choose the answer that lists the correct coefficients
44. _____ (NH4)2Cr2O7

_____ N2
+ _____ H2O
a) 2, 4, 1, 2
b) 1, 1, 4, 1
c) 1, 1, 4, 2
d) 2, 2, 4,1
45. _____ C8H18
+ _____ O2

_____ CO2

___ Ag + ___ Cu(NO3)2
+ ____ Cr2O3
+ _____ H2O
a) 2, 4, 16, 18
b) 1, 1, 4,1
c) 1, 1, 4, 2
d) 2, 25, 16, 18
46. _____ Cu + ____ AgNO3
a) 2, 4, 1, 2
b) 1, 1, 4, 1
c) 1, 2, 2, 1
d) 2, 2, 4, 1
47. Use the activity series to circle the more reactive element.
A) Br2 or I2
B) Na or Mg
C) H2 or Na
D) Li or Cu
E) F2 or Cl2
1st Semester Final Review
48. Circle the reaction that will take place:
A) Cu + NaCl  (Cu is less reactive than Na)
C) I2 + KBr  (I2 is less reactive than Br2)
p. 6 of 6
B) Ca + HCl  (Ca is more reactive than H2)
D) they all take place
49. Circle all the following soluble salts. Refer to the solubility chart.
A) PbI2
B) Fe(OH)3
C) AgCl
D) (NH4)2SO4 E) PbNO3
H) (NH4)2SO4 I) Cu(C2H3O2)2 J) PbI2
K) Ca3(PO4)2 L) NaCl
F) Fe(OH)3
M) CuCO3
G) AgNO3
N) (NH4)2SO4
50. Determine which combination will result in a precipitate. Give the formula of the precipitate.
A) PbNO3 and AgNO3 solutions are mixed
N/R
B) AgNO3 and CuBr solutions are mixed
AgNO3 (aq) + CuBr (aq) AgBr (s) + CuNO3 (aq)
C) NaCl and (NH4)2SO4 solutions are mixed
N/R
D) Cu(C2H3O2)2 and NaCl solutions are mixed N/R
51. Determine the type of reaction (combination/synthesis (S), decomposition (D), combustion ( C ), single
displacement (SR), and double displacement (DR) ). Give the lowest whole number coefficients (include a "1")
that will balance the equation.
__ DR ___
a) ___3__ CaCl2 + ___2__ Na3PO4 
__ D ___
b) ___1__ (NH4 )2Cr2O7 
__1___ N2
__ C ___
c) ___2__ C8H18 + __25___ O2
___16__ CO2 + ___18__ H2 O
__ S ___
d) ___2__ Na

__ SR ___
e) ___1__ Cu + __2__ AgNO3
a.
+ ___1__ Cl2
__6___ NaCl + ___1__ Ca3(PO4)2
+ __4___ H2O
___2__ NaCl
 __2_ Ag + __1_ Cu(NO3)2
+ __1__ Cr2O3