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I. Matter and Changes
1. Iron (III) Nitrate is completely dissolved in water to make a transparent (can see through)
blue solution. This solution may be classified as:
A) pure substance
C)
element
B) heterogeneous mixture D)
homogeneous mixture
2. Hydrochloric acid actively reacting with metals to create hydrogen gas is an example of a:
A)
chemical property
C)
physical property
B)
chemical change
D)
physical change
3. Which of the following is not an example of a physical change?
A)
water boiling
C)
lead melting
B)
sugar dissolving
D)
food souring
4. Which of these steps in the digestive process is a physical change?
A) Saliva changing carbohydrates to sugars
B) The hormone insulin metabolizing
C) Enzymes breading down proteins to amino acids
D) Liquids being absorbed in the large intestine
5. Bones are made up of many minerals, one of which is Calcium. What can calcium be classified
as?
A)
homogeneous mixture
C)
element
B)
compound
D)
heterogeneous mixture
6. Which state of matter is characterized by high density and low compressibility?
A)
gas
C)
liquid
B)
solid D)
all of the above
7. Ms. Bailey had a glass of water and tacos with lettuce, cheese, and chicken for lunch. Which
of the following correctly classifies what she ate?
A) Water: Compound
B) Water: Compound
Tacos: Heterogenous Mixture
Tacos: Homogenous Mixture
C) Water- Element
D) Water: Element
Tacos: Compound
Tacos: Heterogenous Mixture
8. Which of the following is an extensive property of a bubble of H2 gas?
A)
percent oxygen
C)
density
B)
radius
D)
temperature
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II. Atomic Structure, Matter and Nuclear Chemistry
9. Consider an element Ub that has two naturally occurring isotopes with the
following percent abundances: the isotope with a mass number of 11.0 is 42.0%
abundant; the isotope with a mass number of 18.0 is 58.0% abundant. What is the
average atomic mass for element Z? (Answer with 2 decimal places.)
a.
15.10 g
c.
15.35 g
b.
15.06 g
d.
15.92 g
10. Which model supports Rutherford’s discovery of the nucleus?
a.
The nucleus of made of neutrons only.
b.
The nucleus is made of protons, neutrons and electrons.
c.
The nucleus is positive and outside the nucleus is negative.
d.
The nucleus is made of electrons and protons.
11. In a fusion reaction, what is happening to the atom involved?
a.
Energy is absorbed.
c.The nucleus is combined with another nucleus.
b.
Energy does not change. d.The nucleus is split.
12. What particle is needed to complete this nuclear reaction?
Mn + H  ____ + 5
Co
a.
c.
51
26
Fe
b.
Fe
d.
Cr
13. Which of the following types of radiation is the most difficult to protect yourself
from?
a.
b.
Gamma
Beta
c.
d.
Alpha
All of the above
14. What particle is needed to complete this equation?
N
a.
+ ______ 
C + He
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1
2
Name_______________________
a.
n
Answers to Final Exam Study Guide
b
e
e
c.
d.
15. Nuclear fission ________.
a.
Produces hydrogen nuclei.
b.
The separation of one nucleus to form two nuclei of smaller mass
c.
Occurs when large nuclei fuse together.
d.
All of the above.
16. Which of the following types of radiation has negligible mass and does not
change the number of protons or neutrons in an atom’s nucleus?
a.
Alpha
c.
Beta
b.
Gamma
d.
None of the above
III. Data Analysis and Nuclear Chemistry
17. Round the following measurement to three significant figures: 0.50971 cm2.
A)
0.51 cm2
C)
0.509 cm2
2
B)
0.510 cm
D)
0.5097 cm2
18. How many significant figures are in the measurement 102.410 meters?
A)
five C)
four
B)
six
D)
three
19. Convert 28,500 waves/sec into scientific notation.
A)
2.85x104 waves/sec
C)
2.85 x103 waves/sec
-3
B)
2.85x10 waves/sec
D)
2.85x10-4 waves/sec
20. Perform this calculation: 4.6x10-5 divided by 2.5x10-3
A)
0.018 C)
0.152
B)
1.6
D)
6.58
21. Which nuclear particle has the least penetrating power and lowest mass?
This Question is mistaken. Alpha has the least penetrating power, and beta has the
lowest mass out of the options.
A)
a positron ( )
C)
a neutron ( )
B)
a beta particle (
22. Beta particles
A)
are helium nuclei
) D)
an alpha particle (
)
C)
can be stopped by lead
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B)
Answers to Final Exam Study Guide
consist of two protons and four neutrons
D)
all of the above
23. The equation below shows the radioactive decay of thorium (Th).
?
Which of the following particles is released in this reaction?
A)
proton
B)
beta
C)
neutron
D)
alpha
24. The element Hydrogen has 3 naturally occuring isotopes. The isotope with a
mass of 1.00 is 98.5% abundant; the isotope with a mass of 2.00 is 1.00%
abundant; and the isotope with a mass of 3.00 is 0.500% abundant. What is the
average atomic mass of Hydrogen?
None of the answer choices are correct for this problem. The answer is 1.02.
A)
1.008 amu
C)
1.155 amu
B)
1.21 amu
D)
1.342 amu
IV. Electromagnetic Spectrum and Electron Configuration
25. What is the electron configuration for this element?
2p


2s

1s

a.
b.
1s12s22p6
1s22s22p2
c.
d.
1s22s22p4
1s11p12p6
26. How many valence electrons are present in the element with an atomic number of 16?
a.
b.
1
6
c.
d.
5
7
27.
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Which label on the model represents the amplitude and wavelength respectively?
a.
b.
Q, S
R, T
c.
d.
S, Q
T, R
28. UV and IR light are invisible to the human eye. What makes IR light less dangerous than
UV light?
a. IR light has longer wavelenths, and higher energy
b. IR light has shorter wavelengths, and lower energy
c. IR light has shorter wavelengths, and lower energy
d. IR light has longer wavelengths, and lower energy
29. What is the frequency of a wave that has a wavelength of 5x10-7m?
a.
b.
3.33 x10-14 Hz
6.00 Hz
c.
d.
6 x1014 Hz
2.00x10-17 Hz
30. Which element is represented by the following electron configuration?
1s22s22p63s23p64s1
a.
b.
Sc
Ar
c.
d.
K
Ca
31. What block is represented by the number 2?
a.
b.
s
d
c.
d.
f
p
32. How many valence electrons are shown in this picture?
a.
b.
8
3
c.
d.
5
11
5
Name_______________________
Answers to Final Exam Study Guide
33. Name this element:
2p

2s

1s

a.
b.
C
N

c.
d.

O
F
34. What is the lowest energy state of an atom?
a. Ground State b. Hund’s Rule
c. Excited State d. Aufbau Principle
35. Which of the following states that an electron occupies the lowest available energy orbital?
a. Ground State b. Hund’s Rule
c. Excited State d. Aufbau Principle
V. Periodic Table and Trends
36. Of the following elements Ga, Ar, Xe, and I, which is a metal?
a.
b.
Xe
c.
Ar
I
d.
Ga
37. A mystery element Q can be cut with a knife easily, and will produce hydrogen (H 2) gas
when put into water. The reaction is very explosive. What group is this element most likely
found in?
a.
Group 18, Noble Gas
c.
Group 17, Halogens
b.
Group 2, Alkaline earth metals
d.
Group 1, Alkali metals
38. What underlining similarities explain how elements are arranged in rows and columns on
the periodic table?
a.
similarity in size
b.
similarity in melting point
c.
d.
similarity in symbol
similarity in properties
39. When moving across a period (from left to right), what happens to electronegativity, and
the atomic radius?
a.
Electronegativity decreases and Atomic Radius increases
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Name_______________________
b.
c.
d.
Answers to Final Exam Study Guide
Electronegativity increases and Atomic Radius decreases
Electronegativity increases, and Atomic Radius increases.
Electronegativity decreases, and Atomic Radius increases.
40. Based on the following elements which group correctly shows increasing ionization
energy?
a.
Be, Mg, Ca, Sr, Ba
b.
F, Cl, Br, I, At
c.
d.
Al, Si, P, O, F
F, O, B, C, N
41. Which model below appropriately identifies the Noble Gases?
a.
c.
b.
d.
42. What is electronegativity?
a.
one half the distance between nuclei of identical atoms
b.
c.
d.
the distance from the nucleus to the outer orbital of an ion
tendency of an atom to attract electrons in a chemical bond
energy required to remove an electron from an atom
VI. Bonding and Nomenclature
43. Which type of bond is found in sodium iodide?
a.
b.
covalent
ionic
c.
d.
hydrogen
metallic
44. In which of the following is the name and formula given correctly?
a.
b.
Sodium nitride, NaN
Aluminum Sulfate, Al2S3
c.
d.
cobaltous fluoride, CoF3
tin (IV) fluoride, SnF4
45. Given the ionic compound CuF, what is the name of this compound?
a.
b.
copper (I) fluoride
copper (II) fluoride
c.
d.
copper (I) fluorate
copper (II) fluorate
46. Which of these elements exist as a diatomic molecule?
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Name_______________________
a.
b.
Li
B
c.
d.
Answers to Final Exam Study Guide
Cl
C
47. What type of geometry does BCl3 have?
a.
b.
pyramidal
c.
trigonal planar d.
bent
tetrahedral
48. Hexane (C3H6) and Calcium Chloride (CaCl2) have very different boiling points. Hexane
boils at 68 °C, while Calcium Chloride melts at 1,935 °C. What is the best explaination for the
difference in boiling points?
a.
Hexane is polar and Calcium Choloride is an ionic compound.
c.
Hexane is a covalent compound and Calcium Chloride is an ionic compound.
b.
Hexane is an ionic compound and Calcium Chloride is a covalent compound.
d.
Both are ionic, the reason for the difference is unknown.
49. A mystery compound X is insoluble (does not dissolve) in water, and compound Y does.
Compound X and Y are most likely
a.
covalent, covalent
c. ionic, ionic
b.
covalent, ionic
d. ionic, covalent
50. What is the formula of trinitrogen pentafluoride?
a.
b.
N2F5
N3F5
c.
d.
NF3
N5F10
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