Name: _____Key_____________________
Block: ______ Date: _________________
Honors Chemistry
Fall Final Review
This is your review for your fall final. These questions are meant to prepare you for the type of questions
and topics you will see on your final. Use your notes, assignments, and textbook (chapters 2-8) in helping
answer these questions and prepare for your final. Good luck! And remember to sleep and eat well; a
tired and hungry brain is not a smart brain. 
Unit 1
1. Which kind of graph would be best to use with these data?
Amount of Salt
0g
2g
5g
10 g
15 g
Added
Boiling
99.7
101.2
102.4
106.9
108.3
temperature, ºC
a. Line graph
c. Bar graph
b. Circle graph
d. None of the above
2. Look at the table of density data for an unknown substance. Based on the table, the mass of 11
mL of this substance would be 32.4 g.
Density Data
Volume (mL)
Mass (g)
2.0
5.4
4.0
10.8
6.0
16.2
8.0
21.6
10.0
27.0
3. A metal cube has a mass of 54 g and a volume of 20.0 cm3. Is this metal composed of pure
aluminum? Explain. (density of aluminum is 2.7 g/cm3)
54
= 2.7 g/cm3
Yes, this is pure aluminum because they density is the same.
20.0
4. A car covers a distance of 112.6 km in 1.8 hours. Calculate its speed in meters per second.
112.6 km
1000 m
1 hr
1 min
= 17.38 m/sec
1.8 hr
1 km
60 min
60 sec
5. How long would it take (in hours) an airplane traveling at the speed of sound (740 miles per hour;
“mach 1”) to travel around the earth, at the equator? The circumference of the earth is 25,000
miles.
25,000 mi
1 hr
= 33.78 hours
740 mi
6. A common unit of power is the watt: 1 watt = 1 amp⋅volt. Ordinary house current is 120 volts.
How many amps of current are drawn by a 60 watt light bulb?
60 watt
1 amp·volt
= 0.5 amps
1 watt
120 volt
Unit 2
7. Rocky Road ice cream is a heterogeneous mixture.
8. Which is a chemical property of copper?
a. Has a boiling point of 2567ºC
b. Reacts in air to form a green layer
c. Has the symbol Cu
d. Is a solid at room temperature
9. The accepted value is 29.35. Which correctly describes this student’s experimental data?
Trial
Measurement
1
29.48
2
28.97
3
29.27
a. Accurate but not precise
c. Both accurate and precise
b. Precise but not accurate
d. Neither accurate nor precise
10. The accepted value is 1.43. Which correctly describes this student’s experimental data?
Trial
Measurement
1
1.29
2
1.93
3
0.88
a. Accurate but not precise
c. Both accurate and precise
b. Precise but not accurate
d. Neither accurate nor precise
11. The accepted value for a quantity is 5.67 g. If the measure value is 5.89 g, what is the percent
error?
a. 1.04%
c. 3.74% (I got 3.88% on my calculator)
b. 96.3%
d. -3.74% (can’t have a negative % error)
12. Samples of gases containing nitrogen and oxygen were decomposed by electricity and the volume
of each gas produced was measured. Based on these results, which is the correct chemical formula
for Sample 4?
Gas Samples
Sample
Volume of Nitrogen (L) Volume of Oxygen (L)
1
2.00
3.02
2
1.01
1.99
3
1.98
4.99
4
1.98
1.02
a. N2O2
c. NO2
b. NO
d. N2O
13. Which is a compound?
a. Sodium
b. Sea water
c. carbon dioxide
d. brass
14. According to the Law of Conservation of Mass, in any chemical change
a. The mass of reactants is greater than the mass of products
b. The mass of reactants is less than the mass of products
c. The mass of reactants is equal to the mass of products
d. The masses of products and reactants have no predictable relationship
15. A chemical composition of two or more different elements joined together in fixed proportions is
known as a(n) ____.
a. Compound
c. Homogeneous mixture
b. Element
d. Heterogeneous mixture
16. Which scientist described a positively charged core (“nucleus”) in the middle of a lot of empty
space?
a. Chadwick
c. Rutherford
b. Thomson
d. Bohr
17. Which scientist developed the model of the atom shown?
a. Chadwick
c. Rutherford
b. Thomson
d. Bohr
18. Which two have the same mass?
Atom
1
2
3
4
a. Atoms 1 & 2
b. Atoms 2 & 4
Atoms
Proton Neutron Electron
8
10
8
10
9
10
9
9
9
8
11
8
c. Atoms 1 & 4
d. Atoms 2 & 3
19. Atoms with the same number of protons but different number of neutrons are called isotopes.
20. An alpha particle is positively charged. (a helium nucleus, 2 protons and 2 neutrons)
21. If 19.9 grams of copper are burned in air to produce 25.0 grams of copper oxide, what is the mass
of oxygen from the air that is needed?
25.0 – 19.9 = 5.1 g of oxygen
22. What is the average atomic mass of the element?
Isotope
Mass (amu)
Phosphorus-29
29
Phosphorus-31
31
Phosphorus-32
32
�
5
100
× 29� + �
71
100
× 31� + �
24
100
Percent Abundance
5%
71%
24%
× 32� = 31.14 amu
23. What is the percentage by mass of A if 4.07 g of it reacts with 10.63 g of X to form a compound of
mass 14.70 g? Also, calculate the percentage by mass of X in the compound.
A: 4.07 ÷ 14.70 = .2769 × 100 = 27.69%
X: 10.63 ÷ 14.70 = .7231 × 100 = 72.31%
24. Two different compounds are formed by the elements nitrogen and oxygen. The first compound,
compound P1, contains 64.17% by mass nitrogen and 35.73% by mass oxygen. The second
compound, compound P2, contains 47.21% by mass nitrogen and 52.79% by mass oxygen. What
is the ratio of nitrogen to a fixed mass of oxygen for the two compounds?
(There were typos in the question, those have been corrected above…sorry)
64.17
47.21
1.7959
= 1.7959…
= .8942…
= 2.00 2:1 ratio nitrogen to oxygen
35.73
52.79
.8942
25. An element X has three naturally occurring isotopes: X-24, X-25, and X-26. The atomic mass of
X-25 is 24.986 amu and the relative abundance is 10.00%. The atomic mass of X-26 is 25.982
amu and the relative abundance is 11.01%. Given that the weighted atomic mass of the element X
is 24.305, calculate the mass contribution due to the isotope X-24 and identify the element.
100 – 10 – 11.01 = 78.99% abundance X-24
10
11.01
78.99
�
× 24.986� + �
× 25.982� + �
× 𝑋𝑋� = 24.305 amu
100
100
100
2.4986 + 2.8606 + .7899X = 24.305
5.3592 + .7899X = 24.305
.7899X = 18.946
X = 23.985 amu mass of X-24
26. What were the results of Rutherford’s gold foil experiment? What did these results disprove?
From doing the gold foil experiment, Rutherford concluded that atoms are composed of a small,
positively charge nucleus with negatively charged particles surrounding it.
His results disproved Thompson’s plum-pudding model that stated the atom was a large positively
charged area with negative particles distributed throughout.
27. A researcher’s experiment yields a result that is 4.7% to high. Her result was 47.2 g for the mass.
𝐸𝐸𝐸𝐸𝐸𝐸𝐸𝐸𝐸𝐸𝐸𝐸𝐸𝐸𝐸𝐸𝐸𝐸𝐸𝐸𝐸𝐸𝐸𝐸 −𝐴𝐴𝐴𝐴𝐴𝐴𝐴𝐴𝐴𝐴𝐴𝐴
Calculate the actual mass. (
× 100)
𝐴𝐴𝐴𝐴𝐴𝐴𝐴𝐴𝐴𝐴𝐴𝐴
47.2−𝐴𝐴
�
𝐴𝐴
× 100� = 4.7%
47.2−𝐴𝐴
= 0.047
47.2 – A = 0.047A
47.2 = 1.047A
A = 45.1 g
𝐴𝐴
Unit 3
28. Which element has the electron configuration 1s22s22p63s23p64s23d4?
a. Titanium (Ti)
c. Sulfur (S)
b. Chromium (Cr)
d. Selenium (Se)
29. How many valence electrons are in an atom of neon gas?
a. 2
b. 4
c. 6
d. 8
30. Which diagram correctly depicts the trend in electronegativity? B
31. Which diagram correctly depicts the general trend in first ionization energy? B
32. Which element has an electron configuration that ends in the fourth energy level?
D
A
B
C
33. As the frequency of a wave decreases, the wavelength of the wave increases.
34. List the visible spectrum in order of greatest energy, shortest wavelength, and greatest frequency.
𝐻𝐻𝐻𝐻𝐻𝐻ℎ 𝐸𝐸𝐸𝐸𝐸𝐸𝐸𝐸𝐸𝐸𝐸𝐸
�𝑆𝑆ℎ𝑜𝑜𝑜𝑜𝑜𝑜 𝑊𝑊𝑊𝑊𝑊𝑊𝑊𝑊𝑊𝑊𝑊𝑊𝑊𝑊𝑊𝑊𝑊𝑊ℎ�
𝐻𝐻𝐻𝐻𝐻𝐻ℎ 𝐹𝐹𝐹𝐹𝐹𝐹𝐹𝐹𝐹𝐹𝐹𝐹𝐹𝐹𝐹𝐹𝐹𝐹
𝐿𝐿𝐿𝐿𝐿𝐿 𝐸𝐸𝐸𝐸𝐸𝐸𝐸𝐸𝐸𝐸𝐸𝐸
Violet, indigo, blue, green, yellow, orange, red �𝐿𝐿𝐿𝐿𝐿𝐿𝐿𝐿 𝑊𝑊𝑊𝑊𝑊𝑊𝑊𝑊𝑊𝑊𝑊𝑊𝑊𝑊𝑊𝑊𝑊𝑊ℎ�
𝐿𝐿𝐿𝐿𝐿𝐿 𝐹𝐹𝐹𝐹𝐹𝐹𝐹𝐹𝐹𝐹𝐹𝐹𝐹𝐹𝐹𝐹𝐹𝐹
35. Why is the size of a sodium ion (Na+) less than that of a sodium atom (Na)?
The sodium ion loses an electron. When it does so the electron configuration goes from
1s22s22p63s1 to 1s22s22p6 dropping the sodium ion from the third energy level to the second.
Because it is losing an energy level, the sodium ion is small in size than the neutral sodium atom.
36. Name or write the formula for the following compounds:
f. beryllium sulfate
Dichlorine heptoxide
a. Cl2O7
b. H2SO4
g. carbon tetrachloride
Sulfuric acid
c. HI
Hydroiodic acid
h. chromium (III) oxide
d. NH4Cl
i. hydrobromic acid
Ammonium chloride
j. nitric acid
e. Pb(C2H3O2)4 Lead (IV) acetate
BeSO4
CCl4
Cr2O3
HBr
HNO3
Unit 4
37. Which structure is the MOST correct for C3H5? Explain why.
The second structure is the most correct because it
shows the resonance of the structure since the
double bond can (and does) exist between each set
of carbons at any point in time. You would also
draw this structure like the one below (on your
final)
38. Choose the correct order from least to greatest electronegativity
a. F< O< Be< Li <B
c. Li <Be <B< O< F
b. Be<O <Li< F <B
d. F< Be <B <O <Li
39. What is the electronegativity difference in the bonds for the following compounds (see the chart
on the reference page):
a. CO2
3.44 – 2.55 = 0.89 Polar
b. Al2O3
3.44 – 1.16 = 2.28 Ionic
c. PCl3
3.16 – 2.19 = 0.97 Polar
40. For the following compound, give the name, total number of valence electrons, structural formula,
shape, and polarity:
a. NH2- Nitrogen dihydride ion
Bent
N: 5 × 1 = 5
Polar
H: 1 × 2 = 2
-1 charge = 1
8 valence eb. BF3
Boron trifluoride
B: 3 × 1 = 3
F: 7 × 3 = 21
24 valence e-
c. FNO2 Fluoride nitrogen dioxide
F: 7 × 1 = 7
N: 5 × 1 = 5
F: 6 × 2 = 12
24 valence ed. XeF5+ Xenon pentafluoride
Xe: 8 × 1 = 8
F: 7 × 5 = 35
+1 charge = -1
42 valence e-
Trigonal planar
Nonpolar
Trigonal planar
Polar
Square Pyramidal
Polar
Reference Page
Element
Electronegativity
Carbon
2.55
Oxygen
3.44
Sulfur
2.58
Fluorine
3.98
Nitrogen
3.04
Phosphorous
2.19
Aluminum
1.16
Chlorine
3.16
bent