WorksheetsFinal Exam
Total questions: 100
Worksheet time: 3hrs 11mins
Name
Class
Date
1.
What does "atomos" mean?
a)
easily divided
b)
unable to be divided
c)
really small
d)
sometimes divided
2.
Which of the following are parts of Dalton's theory?
a)
All substances are made of atoms.
b)
Atoms Join with other atoms to make new substances.
c)
Atoms of different elements are different
d)
All of these are part of his theory
3.
What was the name of the model pictured behind this question?
a)
Oatmeal Model
b)
Rutherford Model
c)
Bohr Model
d)
Plumb Pudding Model
4.
What did Ernest Rutherford discover when he shot particles at gold foil?
a)
Electrons
b)
Protons
c)
Neutrons
d)
A tiny, dense, positively charged nucleus
5.
What two particles are part of the nucleus of an atom?
a)
Protons and Electrons
b)
Electrons and Neutrons
c)
Protons and Neutrons
d)
Alpha and Beta
6.
What particle resides in the nucleus and has no charge?
a)
Proton
b)
Neutron
c)
Electron
d)
Crouton
7.
In the current atomic theory, where are electrons likely to be found?
a)
Specific Orbits, like planets around a star
b)
In the nucleus
c)
In the electron cloud
d)
electrons are not part of the current atomic theory
8.
When you add the number of protons and neutrons together, you are calculating...
a)
Atomic Number
b)
Atomic Mass
c)
Mass Number
d)
Pythagorean's Theorem
9.
The average mass of all naturally occurring isotope is also known as ...
a)
Atomic Number
b)
Atomic Mass
c)
Mass Number
d)
Radioactivity
10.
The number of protons in the nucleus of an atom is the ____________ ____________.
a)
Atomic Number
b)
Atomic Mass
c)
Mass Number
d)
12
11.
What particle resides in the nucleus and has a positive charge?
a)
Proton
b)
Neutron
c)
Electron
d)
Isotope
12.
What is an element that has a different number of neutrons called?
a)
ion
b)
isotope
c)
carbon
d)
radioactive
13.
What is a charged atom that has a different amount of protons and electrons called?
a)
ion
b)
isotope
c)
radioactive
d)
Frank
14.
Relationship between mass and volume
a)
Volume
b)
Density
c)
Displacement
d)
Matter
15.
Characteristic that can be observed such as color, state, or hardness
a)
physical property
b)
chemical property
c)
density
d)
mass
16.
Example of a chemical change
a)
baking cookies
b)
grinding flour
c)
melting popsical
d)
cutting a piece of paper
17.
Which of the following is not a way to know if a chemical reaction has occurred?
a)
Sound is given off
b)
Gas bubbles escape
c)
The shape of the object changes
d)
The temperature changes
18.
The total amount of mass in a system does not change during a chemical reaction
a)
Chemical Reaction
b)
Counting Atoms
c)
Law of Conservation of Mass
d)
Law of Conservation of Volume
19.
During physical changes, matter always retains its
a)
identity
b)
shape
c)
size
d)
color
20.
A sample of a substance has a mass of 7.3 g and a volume of 2.8 cm3. What is the objects density?
a)
2.61 g/cm3
b)
10.1 g/cm3
c)
0.38 g/cm3
d)
20.44 g/cm3
21.
When a solid turns into a liquid
a)
freezing
b)
melting
c)
evaporating
d)
condensing
22.
When a liquid turns into a gas
a)
freezing
b)
melting
c)
evaporating
d)
condensing
23.
When a gas turns into a liquid
a)
freezing
b)
melting
c)
evaporating
d)
condensing
24.
How many atoms are in CaCl2?
a)
2
b)
4
c)
1
d)
3
25.
Which state of matter has a definite shape?
a)
solid
b)
liquid
c)
gas
26.
Define a liquid.
a)
Indefinite shape, indefinite volume
b)
Definite shape, definite volume
c)
Found in stars
d)
Definite volume, indefinite shape
27.
What is the formula for density?
a)
density = mass x volume
b)
density = mass / volume
c)
density = mass + volume
d)
density = mass - volume
28.
What is the electron configuration of sodium?
a)
2.8
b)
2.8.2
c)
2.8.1
d)
11
29.
What is the electron configuration of calcium?
a)
2.8.8.2
b)
2.8.10
c)
20
d)
2.18.2
30.
What atom matches this electron configuration?
1s2 2s2 2p6 3s2
1s2 2s2 2p6 3s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
31.
Which is the electron configuration for an oxygen atom?
a)
1s22s22p63s23p64s2
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p6
32.
How many electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
33.
How many valence electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
34.
How many electrons can go on the first shell?
a)
1
b)
2
c)
3
d)
4
35.
How many electrons can go on the second shell?
a)
2
b)
4
c)
6
d)
8
36.
What is the noble gas shorthand electron for Sulfur atom?
a)
[Ar] 3p4
b)
[He] 3s23p4
c)
[Ne] 3s23p4
d)
[Na] 3s23p4
37.
What type of horseplay is okay in the lab?
a)
Wresting
b)
Tests of Strengths
c)
All of the Above
d)
NONE, the lab is no place for this
38.
When can you perform experiments?
a)
Anytime I want
b)
When nobody is looking
c)
When the teacher gives me permission
d)
When my friends says I can
39.
When should I study the lab procedure?
a)
Before I come to class
b)
When I get to school
c)
During lab
d)
After the lab has ended
40.
Which answer choice has all lab safety equipment?
a)
fire blanket, desks, first-aid kit, and sun glasses
b)
hair net, fire extinguisher, gas and water shutoff valves
c)
fire blanket, fire extinguisher, first-aid kit, gas and water shutoff valves, lab coat, and goggles
d)
sun screen, bug spray, 12 day water supply, and matches
41.
When should you wear your safety goggles?
a)
after school
b)
before you enter the lab and while lab is going on
c)
never
d)
sleep with them
42.
What do you do if you spill a chemical?
a)
Tell the teacher
b)
Clean it up before anyone notices
c)
Lick it up
d)
Wipe it up with your shirt
43.
Where should the combustible materials be place?
a)
By the flame
b)
On top of the flame
c)
Away from open flames
d)
In a brown paper bag
44.
What do you do if glass breaks?
a)
Throw in the trash
b)
Tell the teacher
c)
Put it in the sink
d)
Just ignore it
45.
What type of shoes should you wear to lab?
a)
flip flops
b)
socks and sandals
c)
closed toed shoes
d)
no shoes required
46.
Which of the following numbers has three significant figures?
a)
1014 miles
b)
101 feet
c)
1000 yards
d)
all of the choices
47.
How many significant figures does the following number have: 0.002040
a)
6
b)
4
c)
3
d)
2
48.
How many significant figures does the following number have: 0.998005
a)
9
b)
10
c)
6
d)
5
49.
How many significant figures does the following number have: 100.00210
a)
7
b)
5
c)
10
d)
8
50.
Round 0.010229 to four significant figures
a)
1022
b)
1023
c)
0.01023
d)
0.01022
51.
What is 0.658 rounded to 1 significant figure?
a)
0
b)
0.66
c)
0.7
d)
0.658
52.
How many significant figures are in the measurement 48032 m?
a)
5
b)
4
c)
3
d)
2
53.
How many significant figures does the following number have: 1740200
a)
4
b)
7
c)
3
d)
5
54.
Calculate 5.50 cm + 5.5 cm and give your answer with the correct number of significant figures.
a)
11 cm
b)
11.0 cm
c)
11.00 cm
d)
11.000 cm
55.
Calculate 7.987 m - 0.54 m and give your answer with the correct number of significant figures.
a)
7.45 m
b)
7.447 m
c)
7.4 m
d)
7.5 m
56.
Calculate 345.009 g - 23.00 g and give your answer with the correct number of significant figures.
a)
322.01 g
b)
322 g
c)
322.009 g
d)
322.0
57.
Which of the following numbers have four significant figures?
a)
56.75 g
b)
40.01 g
c)
0.6000 g
d)
all of the choices
58.
An object with which of the following densities will float on water?
a)
0.7 g/cm3
b)
1.2 g/cm3
c)
3.5 g/cm3
d)
11.4 g/cm3
59.
A can of Coke will sink in a bowl of water. A can of Diet Coke will float in a bowl of water. What does this tell you about the density of the Diet Coke?
a)
it is bigger than 1
b)
it is smaller than 1
c)
it is equal to 1
d)
it is equal to -1
60.
Why do ice cubes float in a glass of water?
a)
the ice cubes are more dense than the water
b)
the water is more dense than the ice cubes
c)
the water is more dense than the glass
d)
the ice is more dense than the glass
61.
Veal finds a gold colored rock in a river. It has a mass of 9.65 grams and a volume of 0.5 cm3. What is the density of the rock?
a)
10.15 g/cm3
b)
19.3 g/cm3
c)
9.15 g/cm3
d)
4.825 g/cm3
62.
Mercury is a metal that is liquid at room temperature and has a density of 13.5 g/cm3. Which of these metals would sink below the mercury if dropped into a container of mercury?
a)
gold (density=19.3 g/cm3)
b)
lead (density=11.4 g/cm3)
c)
iron (density=7.9g/cm3)
d)
aluminum (density=2.7g/cm3)
63.
What is the density of a liquid that has a mass of 27g and a volume of 30ml?
a)
0.9 g/ml
b)
3 g/ml
c)
57 g/ml
d)
810 g/ml
64.
A scientist has four different liquids and pours them all into a bottle. The silver liquid sinks to the bottom, the red liquid settles on top of the silver one, and the pink liquid stays at the surface. Which liquid has the smallest density?
a)
the pink liquid
b)
the silver liquid
c)
the red liquid
d)
the water
65.
What is the density of water?
a)
0 g/ml
b)
1 g/ml
c)
10 g/ml
d)
100 g/ml
66.
What is the density of a substance that has a mass of 30g and a volume of 6 liters?
a)
24 g/l
b)
5 g/l
c)
36 g/l
d)
180 g/l
67.
A cation is a ____ ion.
a)
negative
b)
positive
c)
neutral
d)
ficticious
68.
A anion will be a ____ ion.
a)
negative
b)
positive
c)
neutral
d)
ficticious
69.
Nitrogen will form which of the following ions?
a)
N
b)
N-3
c)
N-5
d)
N+5
70.
What determines how ionic bonds will form?
a)
Number of protons
b)
Mass of the atom
c)
Number of total electrons
d)
Number of valence electrons
71.
Ionic bonds happen because of the ____ of valence electrons.
a)
sharing
b)
transfer
72.
Boron will ____ valence electrons when forming an ionic bond.
a)
lose three
b)
gain three
c)
lose 5
d)
gain 5
73.
Nitrogen will ____ valence electrons when forming an ionic bond.
a)
gain 1
b)
lose 1
c)
gain 3
d)
lose 3
74.
Write the correct formula for an ionic compound formed from S2- and Rb1+.
a)
SRb2
b)
SRb
c)
Rb2S
d)
RbS2
75.
The sum of all oxidation numbers in a neutral compound is ___.
a)
0
b)
1
c)
-1
d)
depends on the compound
76.
Covalent bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
77.
How are covalent bonds formed?
a)
Sharing of electrons
b)
Transfer of electrons
78.
Same repel, opposites
a)
avoid
b)
attract
c)
push
d)
pull
79.
What is a valence electron?
a)
The sum of neutrons and protons.
b)
The # of electrons in the last shell.
c)
A type of bond.
d)
A popular compound.
80.
Name the following compound:
CO2
CO2
a)
monocarbon dioxide
b)
carbon oxide
c)
carbon dioxide
d)
oxygen carbonide
81.
What is the formula for the ammonia molecule shown below?
a)
NH
b)
NH3
c)
N3H3
d)
N3H
82.
What is the correct formula for the molecule shown?
a)
C2H6O
b)
CHO
c)
CH6O2
d)
C6HO6
83.
A covalent bond in which electrons are shared unequally is:
a)
polar
b)
a double bond
c)
ionic
d)
polyatomic
84.
Ionic or covalent?
H2O
H2O
a)
Ionic
b)
Covalent
85.
Which is the correct Lewis Dot Diagram for dihydrogen monosulfide?
a)
b)
c)
d)
86.
What coefficient should be used to make the following equation balanced?
N2+O2--> _NO
N2+O2--> _NO
a)
1
b)
2
c)
3
d)
4
87.
Which problem is balanced?
(Check ALL answers)
(Check ALL answers)
a)
PbO2 + 2H2
b)
SO2 + H20 --> H2SO4
c)
2Na + 2H2O --> 2NaOH + H2
88.
How many elements are in C6H12O6?
a)
1
b)
2
c)
3
d)
4
89.
Is this balanced?
Al + O2 → 2Al2O3
Al + O2 → 2Al2O3
a)
Yes
b)
No
90.
What is the percent by mass of oxygen in MgO?
a)
20%
b)
40%
c)
50%
d)
60%
91.
What is the percent by mass of sodium in NaCl?
a)
39%
b)
61%
c)
35%
d)
65%
92.
What is the percent composition by mass of magnesium in the compound MgSO4 (gram formula mass = 120 g/mol)?
a)
20%
b)
27%
c)
46%
d)
53%
93.
In which compound is the percent composition by mass of Cl equal to 42%?
a)
HClO (gram formula mass = 52 g/mol)
b)
HClO2 (gram formula mass = 68 g/mol)
c)
HClO3 (gram formula mass = 84 g/mol)
d)
HClO4 (gram formula mass = 100 g/mol)
94.
What is Avogadro's number?
a)
6.02 x 1023
b)
1 mole
c)
600 million
d)
6.02
95.
One mole of carbon dioxide (CO2) contains 6.02 x 1023 _____.
a)
atoms
b)
formula units
c)
ions
d)
molecules
96.
How many moles are in 8.30 X 1023 molecules of H2O?
a)
1.38 X 1023 moles H2O
b)
1.38 moles H2O
c)
2 moles H2O
d)
1 mole H2O
97.
How many molecules are there in 31.8 moles of water?
a)
5.28 x 10-23 molecules
b)
1.91 x 1025 molecules
c)
5.28x 10-25 molecules
d)
1.91 x 1023 molecules
98.
A mole is:
a)
The SI unit for mass
b)
The SI unit for the amount of a substance
c)
The SI unit for volume
d)
The SI unit for area
99.
Which has the most particles?
a)
1 mole H2
b)
1 mole Na1+
c)
1 mole Al(OH)3
d)
These are all the same
100.
How many moles of Na contain 1.45 x 1021 atoms of Na?
a)
8.73 x 1044 moles
b)
8.73 moles
c)
0.00241 moles
d)
2.41 x 1044 moles
100 %
