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WorksheetsFall Final Review
Total questions: 55
Worksheet time: 2hrs 39mins
Name
Class
Date
1.
If the density of a bar of gold is 19.3 g/cm3 and you cut it into 4 pieces, what is the density of each piece of gold?
a)
4.825 g/cm3
b)
9.65 g/cm3
c)
19.3 g/cm3
d)
38.6 g/cm3
2.
What is the formula for density?
a)
density = mass x volume
b)
density = mass / volume
c)
density = mass + volume
d)
density = mass - volume
3.
Jack
has a rock. The rock has a mass of 14g and a volume of 2cm3. What is
the density of the rock?
a)
7 mL
b)
7 g/cm3
c)
28 g/cm3
d)
1/7 g/cm3
4.
Which of the following is a physical change?
a)
corrosion
b)
tarnishing
c)
rotting
d)
cutting
5.
The density of pyrite is 5g/cm3 . This is an example of
a)
intensive property
b)
extensive property
c)
chemical change
d)
chemical property
6.
The melting point of ice is 00 C. This is an example of ________.
a)
intensive property
b)
extensive property
c)
Chemical change
d)
Chemical property
7.
The mass of a lead cube is 64 grams. This is an example of
a)
intensive property
b)
extensive property
c)
chemical change
d)
physical change
8.
What is the correct electron configuration for Selenium
a)
1s22s22p63s23p64s24d104p4
b)
1s22s22p63s23p64s23d104p4
c)
1s22s22p63s23p64s23d104p3
d)
1s22s22p63s23p64s24d104p43
9.
Which element is depicted from this orbital diagram
a)
Fluorine
b)
Neon
c)
Chlorine
d)
Argon
10.
The electron configuration of an atom is 1s22s22p6. The number of electrons in the atom is
a)
3
b)
6
c)
8
d)
10
11.
What electron configuration matches an oxygen ion?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
12.
This is used to represent the number of each atom being represented.
a)
A Exponent
b)
The Coefficient
c)
A Molecule
d)
The Subscript
13.
This appears on the left side of a chemical formula, and represents how many molecules there are.
a)
An Atom
b)
The Subscript
c)
A Molecule
d)
The Coefficient
14.
True or false. Law of conservation of mass means that the number of atoms of the products is more than the number of atoms in the reactants.
a)
True
b)
False
15.
The most important subatomic particle when determining an elements REACTIVITY is what?
a)
protons
b)
neutrons
c)
valence electrons
d)
electrons
16.
Calculate the average atomic mass of silver.
a)
106.38649amu
b)
111.91896amu
c)
107.8677amu
d)
121
17.
Ernest Rutherford discovered that atoms were mostly _________________.
a)
negatively charged
b)
positively charged
c)
electrons
d)
empty space.
18.
What scientist is best known for his gold foil experiment?
a)
J.J. Tomson
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
19.
An element has two naturally occurring isotopes. One is 10.013 amu and is 19.9% abundant. The other is 11.01 amu and is 80.1% abundant. What is the average atomic mass? What element is it?
a)
9.012, Beryllium
b)
12.011, Carbon
c)
6.941, Lithium
d)
10.812, Boron
20.
What is the atomic number for an element with 41 neutrons and a mass number of 80?
a)
39
b)
41
c)
80
d)
121
21.
Atomic mass - Atomic Number =
a)
protons
b)
neutrons
c)
electrons
d)
Average Mass
22.
What quantities vary between isotopes of an element?
a)
protons, electrons, and atomic mass
b)
protons, electrons, and atomic number
c)
neutrons and electrons
d)
neutrons and atomic mass
23.
If an atom has 24 protons and 24 electrons, what is the atomic number of this element?
a)
24
b)
48
c)
0
d)
42
24.
Select the correct order of waves on the EMS
a)
Radio, Micro, Infra, Visible, Ultra, X-ray, Gamma
b)
Gamma, X-ray, Ultra, Vis, Infra, Micro, Radio
c)
Vis, Micro, Infra, Ultra, X-ray, Gamma, Radio
d)
Micro, Radio, Vis, Infra, Ultra, X-ray, Gamma
25.
The relationship between wavelength and frequency is λ=c/v. Calculate the wavelength of light that has a frequency of 5.2 x 1012 1/s. The speed of of light is 3.0x 108 m/s.
a)
5.8 x 10 -5 m
b)
5.8 x 10 -7 m
c)
5.19 x 10 14 m
d)
1.56 x 10 23 m
26.
Which group of the periodic table is composed of inert (not reactive) gases?
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
27.
Elements on the left side of the periodic table are
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
28.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)
Magnesium (Mg)
29.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
30.
Who first arranged the periodic table by increasing atomic mass?
a)
Ernest Rutherford
b)
Dmitri Mendeleev
c)
Henry Moseley
d)
Mrs. Urby
31.
From the following elements, which has the largest atomic radius?
a)
Na
b)
Mg
c)
Si
d)
Cl
32.
The element that has the largest atomic radius is
a)
Arsenic
b)
Zinc
c)
Xenon
d)
Tin
33.
What elements tend to have low ionization energy?
a)
metals
b)
nonmetals
c)
metalloids
d)
impossible to tell
34.
Put the following elements in order of decreasing ionization energy:
O, Te, Po, S.
O, Te, Po, S.
a)
O, S, Po, Te
b)
O, S, Te, Po
c)
O, Te, Po, S
d)
O, Po, Te, S
35.
What is the proper name for CaCl2?
a)
Calcium dichloride
b)
Monocalcium dichloride
c)
Calcium chloride
d)
Calcium chlorine
36.
What is the correct name for Mg(OH)2?
a)
Magnesium dihydroxide
b)
Magnesium Oxyhydride
c)
Magnesium Oxygen dihydride
d)
Magnesium hydroxide
37.
What is the proper name for S2O2?
a)
Sulfur oxide
b)
Sulfur dioxide
c)
sulfur (II) oxide
d)
disulfur dioxide
38.
Which three nonmetals exist only as diatomic molecules?
a)
H, C, Br
b)
N, O, S
c)
I, F, N
d)
H, O, P
39.
What is a polar molecule?
a)
One that has a partial negatitive on one end and a partial positive on the other
b)
a molecule with little vibration
c)
an ionic compound
d)
the nonpolar bonds are arranged sequentially
40.
Which compound below would be nonpolar?
a)
HF
b)
H2O
c)
Br2
d)
HBr
41.
The molecule shown has been called "laughing gas" and has been used in dentistry as a pain killer. What is its chemical name?
a)
Nitrogen oxide
b)
dinitrogen dioxide
c)
dinitrogen oxide
d)
nitrogen dioxide
42.
Which is the correct name for AlBr3?
a)
Aluminum bromine
b)
Bromine aluminide
c)
Aluminum bromide
d)
Aluminum (III) bromide
43.
What is the name for LiF?
a)
Lithium Fluoride
b)
Lithium Fluorine
c)
Fluorine Lithide
44.
If Nitrogen and Silver chemically bond, which will be named first?
a)
Silver
b)
Nitrogen
c)
Unknown
d)
Iodine
45.
How many electrons are needed in the outer energy levels of most atoms to be stable?
a)
2
b)
4
c)
6
d)
8
46.
What is the correct formula for Iron (III) nitrate?
a)
Fe3N
b)
Fe(NO3)3
c)
Fe3(NO3)
d)
Fe(NO2)3
47.
How do the following two elements bond together?
K1+ S2-
K1+ S2-
a)
KS
b)
K8S
c)
K6S3
d)
K2S
48.
How do the following two elements bond together?
Na1+ F1-
Na1+ F1-
a)
NaF
b)
NaF3
c)
Na3F
d)
Na1F2
49.
How do the following two elements bond together?
Al3+ O2-
Al3+ O2-
a)
AlO
b)
Al2O3
c)
Al3O6
d)
Al3O2
50.
Which of the following shows the correct way to balance the chemical equation?
Fe + O2 -> Fe2O3
Fe + O2 -> Fe2O3
a)
4Fe + 3O2 -> 2Fe2O3
b)
2 Fe + 3O2 -> Fe2O6
c)
4 Fe + O6 -> 2Fe2O3
d)
None of the options are correctly balanced.
51.
Which of the following is an unbalanced equation?
a)
CaCO3 --> CaO + CO2
b)
PbO2 + 2H2-->2Pb + H2O
c)
2Na+ 2H2O-->2NaOH + H2
d)
CS2 + 2O2 --> CO2 + 2SO2
52.
What is the sum of the coefficients when correctly balanced: ___Al + ___O2 --> ___Al2 O3
a)
3
b)
7
c)
WHAT!?
d)
9
53.
What molecule has a tetrahedral geometry?
a)
CH4
b)
CO2
c)
PCl5
d)
BF3
54.
The candy was sour.
a)
Qualitative data
b)
Quantitative data
55.
The mass of the beaker was 122 grams.
a)
Qualitative data
b)
Quantitative data
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