Name:     ID: 
 
Email: 

Honors Chemistry Final Exam

 1. 
What causes NH3 to have it’s shape, according to VSEPR theory?
a.
repulsive forces between unshared pairs of electrons and bonds
b.
the unusual location of the free electrons
c.
interaction between the fixed orbitals of the unshared pairs of hydrogen
d.
ionic attraction and repulsion
 

 2. 
How many moles of CH4 are contained in 96.0 grams of  CH4?
a.
3.00 moles
c.
6.00 moles
b.
12.0 moles
d.
16.0 moles
 

 3. 
Which type of bond is formed by the transfer of electrons from one atom to another?
a.
a covalent bond
c.
a coordinate covalent bond
b.
an ionic bond
d.
a hydrogen bond
 

 4. 
What is the name of the compound whose formula is H2SO4?
a.
sulfuric acid
c.
hydrosulfurous acid
b.
sulfurous acid
d.
hydrosulfuric acid
 

 5. 
Which statement describes a chemical property of iron?
a.
Iron combines with oxygen to form rust.
b.
Iron conducts electricity and heat.
c.
Iron can be drawn into a wire.
d.
Iron can be flattened into sheets.
 

 6. 
Which of the following is an example of a physical change?
a.
breaking glass
c.
burning gasoline
b.
rusting of iron
d.
lighting a match
 

 7. 
What is the total number of electrons present in an atom of mc007-1.jpg?
a.
86
b.
27
c.
59
d.
32
 

 8. 
The gram molecular mass of Ca3(PO4)2 is
a.
279 g
b.
342 g
c.
246 g
d.
310 g
 

 9. 
Which group contains elements with a total of four electrons in the outermost energy level (valence shell)?
a.
Group 1A
b.
Group 2A
c.
Group 6A
d.
Group 4A
 

 10. 
Given the unbalanced equation:
mc010-1.jpg
What is the coefficient in front of the CaSO4 when the equation is completely balanced with the smallest whole-number coefficients?
a.
2
b.
4
c.
1
d.
3
 

 11. 
Which of the following factors contributes to the increase in atomic size within a group in the periodic table as the atomic number increases?
a.
an increase in number of protons
b.
an increase in size of the nucleus
c.
fewer electrons in the highest occupied energy level
d.
more shielding of the electrons in the highest occupied energy level
 

 12. 
A person attemps to fill their car tires with 9.03x1023 molecules of nitrogen gas (N2).  How many moles did the person attempt to put in the tires?
a.
1.50 moles
c.
0.667 moles
b.
42.0 moles
d.
33.6 moles
 

 13. 
Which of the following is a correct Lewis dot structure for potassium chloride?
a.
mc013-1.jpg
c.
mc013-3.jpg
b.
mc013-2.jpg
d.
mc013-4.jpg
 

 14. 

4K(s) + O2(g) mc014-1.jpg  2K2O(s)
Under certain conditions potassium can react with oxygen in air to form potassium oxide according to the above equation.  Which image best represents the amount of potassium required to completely react with all of the oxygen shown in the flask below?
mc014-2.jpgmc014-3.jpg
a.
mc014-4.jpg
c.
mc014-6.jpg
b.
mc014-5.jpg
d.
mc014-7.jpg
 

 15. 
A red light is measured to have a wavelength of 6.71 x 10-7 m. Given the speed of light (3.00 x 108 m/s) and Planck’s constant (6.63 x 10-34 Js), calculate the energy of one photon of this light.
a.
4.42 x 10-3 J
c.
2.96 x 10-19 J
b.
1.33 x 10-18 J
d.
1.48 x 10-18 J
 

 16. 
Which of the following elements has the smallest atomic radius?
a.
O
b.
K
c.
S
d.
Li
 

 17. 
Given the balanced equation:
AgNO3 + NaCl mc017-1.jpg NaNO3 + AgCl
Which compound would precipitate out of the reaction?
a.
NaNO3
c.
NaCl
b.
AgCl
d.
AgNO3
 

 18. 
A solution containing a large concentration of dissolved ions can be classified as a(n) ________.
a.
weak solution
c.
suspension
b.
Strong electrolyte
d.
Solvent
 

 19. 
The solid block shown here has a mass of 146 grams.  What is the block’s density?
mc019-1.jpg
a.
8.1 g/cm3
c.
54 g/cm3
b.
2.7 g/cm3
d.
0.37 g/cm3
 

 20. 
When 20 mL of 1.0 M HCl is diluted to a total volume of 60 mL, the concentration of the resulting solution is
a.
0.50 M
b.
1.0 M
c.
0.25 M
d.
0.33 M
 

 21. 
According to the Brønsted-Lowry definition, an acid is any species that can
a.
accept an electron
c.
accept a proton
b.
donate a proton
d.
donate an electron
 

 22. 
Which orbital notation shows the lowest energy arrangement of valence electrons for 1s22s22p3?
a.
mc022-1.jpg
b.
mc022-2.jpg
c.
mc022-3.jpg
d.
mc022-4.jpg
 

 23. 
Which of the following atoms has six valence electrons?
a.
argon (Ar)
c.
sulfur (S)
b.
magnesium (Mg)
d.
silicon (Si)
 

 24. 
A monochromatic beam of light has a frequency of 7.69 x 1014 Hz (hertz).  What is the energy of a photon of this light?
a.
3.90 x 10-7 J
c.
2.59 x 10-40 J
b.
5.10 x 10-19 J
d.
6.92 x 10-31 J
 

 25. 
An atom of lithium-7 has an equal number of
a.
electrons and neutrons
c.
positrons and neutrons
b.
electrons and protons
d.
positrons and protons
 

 26. 
If 75.0 % of the isotope of an element have a mass of 35.0 amu and 25.0 % of the isotopes have a mass of 37.0 amu, what is the average atomic mass of the element?
a.
37.0 amu
b.
35.5 amu
c.
36.0 amu
d.
35.0 amu
 

 27. 
What is the molarity of a KF (aq) solution containing 116 g of KF in 1.00 L of solution?
a.
3.00 M
b.
4.00 M
c.
2.00 M
d.
1.00 M
 

 28. 
What is the pH of a 0.01 M solution of KOH?
a.
1
b.
13
c.
2
d.
12
 

 29. 
Sulfur dioxide is the cause of acid rain and is common pollutant caused by volcanic eruptions, the burning of fossil fuels, and the exhaust from industrial facilities.  What is the mass in gram of 0.75 mole of SO2? (MM: 64.07 g/mol)
a.
32 g
c.
48 g
b.
16 g
d.
24 g
 

 30. 
What is the mass number of an ion that has 83 protons, 80 electrons, and 126 neutrons?
a.
206
b.
83
c.
209
d.
289
 

 31. 
In a solution, litmus paper turned blue.  The pH of this solution could be
a.
10
b.
2
c.
3
d.
4
 

 32. 
Which of the following elements has an electron configuration of 1s22s22p63s23p1?
a.
aluminum
c.
lithium
b.
phosphorous
d.
calcium
 

 33. 
Logan is studying a substance.  Which property of the substance is chemical?
a.
its density
c.
its melting point
b.
its flammability
d.
its temperature
 

 34. 
When the reaction
mc034-1.jpg
is completely balanced using smallest whole numbers, the coefficient of H2O will be
a.
2
b.
1
c.
3
d.
4
 

 35. 
Chemical equations must be balanced to satisfy
a.
the law of definite proportions.
b.
the law of multiple proportions.
c.
Avogadro’s principle.
d.
the law of conservation of mass.
 

 36. 
What is the percent mass oxygen in acetone (C3H6O)? 
a.
27.6 %
b.
1.00 %
c.
10.3 %
d.
62.0 %
 

 37. 
Sodium, mercury, argon and neon are used in the production of lamps. There are fewer safety guidelines regarding the handling of neon and argon than for mercury and sodium. Which of the following best describes the properties of elements in the same family as neon and argon?
a.
Solid at room temperature and mostly unreactive with strong acids
c.
Solid at room temperature
b.
Mostly unreactive
d.
Gaseous at room temperature and highly reactive
 

 38. 
The H3O+ ion concentration of a solution is 1 x 10-4 M.  This solution is
a.
acidic and has a pH of 4
c.
basic and has a pH of 4
b.
acidic and has a pH of 10
d.
basic and has a pH of 10
 

 39. 
Which set of procedures and observations indicates a chemical change
a.
Ethanol is added to an empty beaker and the ethanol eventually disappears.
b.
A solid is gently heated in a crucible and the solid slowly turns to liquid.
c.
Large crystals are crushed with a mortar and pestle and become powder.
d.
A cool, shiny metal is added to water in a beaker and rapid bubbling occurs.
 

 40. 
Metallic bonds occur between atoms of
a.
neon
b.
copper
c.
fluorine
d.
sulfur
 

 41. 
According to the Arrhenius definition, a substance that is classified as an acid will always produce _______ in solution
a.
I-(aq)
b.
K+(aq)
c.
H+(aq)
d.
F-(aq)
 

 42. 
Which graph shows the pressure-temperature realationship expected for an ideal gas?
a.
mc042-1.jpg
c.
mc042-3.jpg
b.
mc042-2.jpg
d.
mc042-4.jpg
 

 43. 
1s22s22p63s23p64s1 is the electron configuration for which element?
a.
calcium (Ca)
c.
argon (Ar)
b.
potassium (K)
d.
aluminum (Al)
 

 44. 
Which equation represents a neutralization reaction?
a.
CaO(s) + H2O(l) mc044-1.jpg Ca(OH)2(aq)
b.
H2SO4(aq) + CaCO3(aq) mc044-2.jpg CaSO4(aq) + H2O(l) +CO2(g)
c.
HNO3(aq) + KOH(aq) mc044-3.jpg KNO3(aq) + H2O(l)
d.
2 HCl(aq) + Zn(s) mc044-4.jpg ZnCl2(aq) + H2(g)
 

 45. 
As wavelength increases, what happens to Frequency and Energy?
a.
Frequency decreases, Energy increases
c.
Both Increase
b.
Both Decrease
d.
Frequency increases, Energy decreases
 

 46. 
Given a pH of 3.8, which of the following is true?
a.
can be neutralized by a strong acid
c.
contains more H+ ions than OH-
b.
has a slightly basic pH
d.
Contains more OH- ions than H+ ions
 

 47. 
Which of the following quantum leaps of an electron would be associated with the greatest energy of emitted light?
a.
Energy Level=  6 to  5
b.
Energy Level = 4 to  5
c.
Energy Level  = 5 to  2
d.
Energy Level = 5 to  1
 

 48. 
An atom is electrically neutral because the
a.
number of protons equals the nubmer of electrons.
b.
ratio of the number of neutrons to the number of electrons is 1:1.
c.
ratio of the number of neutrons to the number of protons is 2:1.
d.
number of protons equals the number of neutrons.
 

 49. 
What is the Lewis dot structure for nitogen trifluoride (NF3)
a.
mc049-1.jpg
c.
mc049-3.jpg
b.
mc049-2.jpg
d.
mc049-4.jpg
 

 50. 
What is the total number of molecules in 1.0 mole of Cl2 (g)?
a.
35
c.
70
b.
6.02 x 1023
d.
12 x 1024
 

 51. 
Which is the correct name of the compound with the formula NH4NO2?
a.
ammonia nitrite
c.
ammonium nitrite
b.
ammonia nitrate
d.
ammonium nitrate
 

 52. 
The bonds present in nitrogen dioxide (NO2) are
a.
ionic
c.
metallic
b.
covalent
d.
van der Waals
 

 53. 
Carbon reacts with chlorine to form CCl4.  What is the name of this compound?
a.
carbon 4-chloride
c.
carbon tetrachloride
b.
tetracarbon chloride
d.
1-carbon 4-chloride
 

 54. 
In the reaction
mc054-1.jpg
an acid-base conjugate pair is
a.
mc054-2.jpg and mc054-3.jpg
c.
mc054-6.jpg and mc054-7.jpg
b.
mc054-4.jpg and mc054-5.jpg
d.
mc054-8.jpg and mc054-9.jpg
 

 55. 
Given the reaction:
mc055-1.jpg
How many moles of CO2 are produced when 11.2 liters of C8H16 gas, measured at STP, reacts completely?
a.
4.00 mole
b.
8.00 moles
c.
30.0 mole
d.
10.0 moles
 

 56. 
Which kind of bond is formed when two atoms share electrons to form a molecule?
a.
metallic
b.
covalent
c.
ionic
d.
electovalent
 

 57. 
Which temperature is the same as -13 °C?
a.
773 K
b.
286 K
c.
747 K
d.
260 K
 

 58. 
Orange light has a frequency of 5.0 x 1014 Hz (hertz) in a vaccuum.  What is the wavelength of this light?
a.
1.5 x 1023 m
c.
1.7 x 106 m
b.
2.0 x 10-15 m
d.
 6.0 x 10- 7 m
 

 59. 
Which of the following models best represents the shape of a compound with trigonal planar geometry?
a.
mc059-1.jpg
c.
mc059-3.jpg
b.
mc059-2.jpg
d.
mc059-4.jpg
 

 60. 
One of the wavelengths emitted by hydrogen atoms is
6.56 x 10-7 m. Calculate the frequency if the speed of light is 3.00 x 108 m/s..
a.
4.57 x 10-6 Hz
c.
1.97 x 1014 Hz
b.
4.57 x 10-7 Hz
d.
4.57 x 1014 Hz
 

 61. 
Which pair of elements form an ionic bond with each other?
a.
ICl
b.
CCl
c.
KCl
d.
PCl
 

 62. 
What is the maximum number of orbitals in the p sublevel?
a.
4
b.
3
c.
5
d.
2
 

 63. 
Ethanol (C2H5OH) is used in hand sanatizer.  If 115 grams of C2H5OH is used to to make a batch of hand sanatizer, then how many moles are present in the batch? (MM: 46.08 g/mol)
a.
1.00 mol
c.
2.50 mol
b.
3.00 mol
d.
1.50 mol
 

 64. 
Given the reaction:
mc064-1.jpg
How many moles of C6H12O6 (s) are needed to produce 24 moles of carbon dioxide?
a.
4.0 moles
b.
12 moles
c.
1.0 mole
d.
24 moles
 

 65. 
What formula represents lead (II) phosphate?
a.
Pb3(PO4)2
c.
Pb2(PO4)3
b.
Pb4PO4
d.
PbPO4
 

 66. 
Which of the following atoms have the largest atomic radius?
a.
magnesium (Mg)
c.
chlorine (Cl)
b.
iodine (I)
d.
barium (Ba)
 

 67. 
The reaction for the decomposition of PCl5 to chlorine and PCl3 is shown below.
PCl5(g) mc067-1.jpg PCl3(g) + Cl2(g)

If the equilibrium concentrations are [PCl5] = 1.0 M, [PCl3] = 0.10 M, [Cl2] = 0.10 M, what is the value of the equilibrium constant? 
a.
1.0 x 10-4
c.
1.0 x 102
b.
2.0 x 10-2
d.
1.0 x 10-2
 

 68. 
Which sample of matter is a pure substance?
a.
ammonia gas (NH3)
c.
air (O2, N2, CO2)
b.
salt water (NaCl + H2O)
d.
hydrochloric acid solution (HCl + H2O)
 

 69. 
Beryllium is classified as
a.
a transition metal
c.
an alkali metal
b.
a noble gas
d.
an alkaline earth metal
 

 70. 
What is the name for the compound FeS
a.
iron (II) sulfide
c.
iron (II) sulfate
b.
iron (III) sulfide
d.
iron (III) sulfate
 

 71. 
What trend can be seen as the atomic number increases in period 3?
a.
increasing electronegativity
c.
decreasing atomic mass
b.
decreasing first ionization energy
d.
increasing atomic radius
 

 72. 
Which of the following atoms has a smallest  atomic radius?
a.
Be
b.
F
c.
C
d.
Li
 

 73. 
A neon sign is being made with 80 grams of neon.  How many atoms are contained the neon sign?
a.
2.40 x 1024 atoms
c.
4.80 x 1024 atoms
b.
1.20 x 1024 atoms
d.
6.02 x 1023 atoms
 

 74. 
In theory, how many grams of H2O can be produced if an experiment used 12.75 grams of sulfur dioxide and 3.96 grams of hydrosulfuric acid? (MM H2S = 34.082 g/mol ; MM SO2 = 64.064 g/mol; MM H2O = 18.015 g/mol )
2 H2S (g) + SO2 (g) mc074-1.jpg 3 S (g) + 2 H2O (g)





a.
1.50 grams
c.
1.98 grams
b.
7.17 grams
d.
3.96 grams
 

 75. 
Co(H2O)62+(aq) + 4 Cl-(aq) mc075-1.jpg CoCl42-(aq) + 6 H2O(l)

Write the Keq expression of the reaction above
a.
Keq = mc075-2.jpg
c.
Keq = mc075-4.jpg
b.
Keq = mc075-3.jpg
d.
Keq = mc075-5.jpg
 

 76. 
The covalent bonds in water are polar because
a.
O is more electronegative than H.
c.
O and H are equally electronegative.
b.
H is more electronegative than O.
d.
water molecules are cohesive.
 

 77. 
Which element within any given period of the Periodic Table would always have the lowest first ionization energy?
a.
a halogen
c.
an alkali metal
b.
a noble gas
d.
an alkaline earth metal
 

 78. 
What is the formula mass of calcium nitrate, Ca(NO3)2?
a.
150 g
c.
102 g
b.
70.0 g
d.
164 g
 

 79. 
Which subatomic particles are located in the nucleus of a neon atom?
a.
electrons and protons
c.
electrons and neutrons
b.
protons and electrons
d.
protons and neutrons
 

 80. 
The correct formula for sodium oxide is
a.
Na2O
b.
S2O
c.
NaO2
d.
SO2
 

 81. 
Which atom contains exactly 15 protons?
a.
nitrogen-15
c.
oxygen-15
b.
phosphorous-32
d.
sulfur-32
 



 
         Start Over