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WorksheetsChemistry Fall 2018 Midterm Exam
Total questions: 84
Worksheet time: 35mins
Name
Class
Date
1.
Suppose, you measured the length of a table and obtained a measurement of 202 cm. After consulting the manufacturer's catalog, you find that the table's length is listed as 200 cm in length. What is the percent error?
a)
-0.99
b)
0.000 1
c)
0.01
d)
1
2.
The mass or a rubber stopper is found to be 6 g. The science teacher tells the class to use 7.5 g as the standard value for the rubber stopper. What is the percentage error in the measurement?
a)
0.2
b)
0.25
c)
20
d)
-2
3.
Put the following in scientific notation. 205 000 000 000
a)
2.05 x 10^-11
b)
205 x 10^9
c)
2.05 x 10^11
d)
205 x 10^-9
4.
Put the following in scientific notation. -0.000 031
a)
-3.1 x 10^5
b)
3.1 x 10^-5
c)
-3.1 x 10^-5
d)
31 x 10^-6
5.
Put the following in standard form. 3.4 x 10^-3
a)
3400
b)
0.0034
c)
0.00034
d)
-0.0034
6.
Put the following in standard form. - 3.4 x 10^3
a)
-3400
b)
0.0034
c)
0.00034
d)
-0.0034
7.
How many significant figures does 0.00104 have?
a)
6
b)
2
c)
3
d)
5
8.
How many significant figures does 105.00 have?
a)
2
b)
4
c)
3
d)
5
9.
Round 106 to two significant figures
a)
100
b)
107
c)
110
d)
11
10.
The formula for calculating mass is __________.
a)
Mass = density x volume
b)
Mass = volume / density
c)
Mass = density / volume
d)
You have to measure mass. It can't be calculated.
11.
A half marathon is 13.1 miles. How many centimeters is this?
a)
6 294 288 cm
b)
20 980.96 cm
c)
62 942.88 cm
d)
209 809.6 cm
12.
A train is traveled 165 km in a day. How fast was it traveling in mph?
a)
0.43 mph
b)
10.3 mph
c)
6.89 x 10^9 mph
d)
0.004 mph
13.
How should you hold a test tube containing a chemical?
a)
pointed away from your face
b)
held up to your nose
c)
above your head.
d)
pointed towards your partner's face
14.
Why shouldn't you wear dangling jewelry and baggy clothing in the laboratory?
a)
The baggier the clothing, the more chemical fumes are absorbed.
b)
Lab coats don't fit over baggy clothes.
c)
The metal in the jewelry changes the expected reaction.
d)
Jewelry and clothing could get caught on equipment, and clothes can catch on fire.
15.
Identify when you should report an accident to your teacher.
a)
immediately
b)
only if you think the accident could cause injury
c)
after you've cleaned up the mess
d)
after you've finished the experiment, so your results are not ruined
16.
When you are done with an experiment, how should you leave your workstation?
a)
Leave dirty glassware on the workbench for your teacher to clean.
b)
Leave your completed worksheet and experiment on the workbench for your teacher to examine.
c)
Clean all glassware and wipe off the lab bench to ensure a clean station.
d)
Clean all glassware but leave spills and trash on the workbench for your teacher to clean.
17.
Identify a piece of equipment used to measure mass.
a)
Spring Scale
b)
Scale
c)
Balance
d)
Graduated Cylinder
18.
Which of the following is the proper unit for measuring length?
a)
Celsius
b)
Meter
c)
Liter
d)
Gram
19.
Which of the following is the proper unit for measuring volume?
a)
Celsius
b)
Meter
c)
Liter
d)
Gram
20.
Which of the following is the proper unit for measuring mass?
a)
Celsius
b)
Meter
c)
Liter
d)
Gram
21.
Which of the following is the proper unit for measuring temperature?
a)
Celsius
b)
Meter
c)
Liter
d)
Gram
22.
Identify the correct conversion of 4.2 grams to kilograms.
a)
4.2 g = 0.0042 kg
b)
4.2 g = 42 kg
c)
4.2 g = 0.042 kg
d)
4.2 g = 4 200 kg
23.
How many millimeters are in a meter?
a)
5
b)
100
c)
10
d)
1000
24.
A measurement that closely agrees with accepted values is said to be
a)
accurate.
b)
reliable.
c)
precise.
d)
significant
25.
A 3 groups of students measures the mass of a product from the same chemical reaction. The groups recorded data of 8.83 g, 8.84 g and 8.82 g. The known mass of the product from that reaction is 8.60g. The group values are
a)
accurate
b)
accurate and precise
c)
precise
d)
neither accurate nor precise
26.
What is the proper order of the abbreviations of the metric system?
a)
d, c, m, Base, K, H, D
b)
Base, K, H, D, d, c, m
c)
K, H, D, Base, d, c, m
d)
m, c, d, Base, D, H, K
27.
Convert 1392 kilometers into meters.
a)
1.392 m
b)
1 392 000 m
c)
0.1392 m
d)
139.2 m
28.
Convert 1392 milligrams into grams.
a)
1.392 g
b)
1 392 000 g
c)
0.1392 g
d)
139.2 g
29.
What is a hypothesis?
a)
an educated guess based on research
b)
something seen or heard
c)
a natural phenomenal
d)
a scientific experiment
30.
Your hypothesis must be
a)
Measurable.
b)
changed to match your results.
c)
an if...then statement.
d)
Both measurable and if…then statement
31.
What step of the scientific method are charts and graphs used?
a)
Research
b)
Analyze Data
c)
Experi-ment
d)
Conclusions
32.
You should only do your experiment once.
a)
True
b)
False
33.
During the _____________ you state if your hypothesis is supported or rejected.
a)
Research
b)
Analyze Data
c)
Experiment
d)
Conclusions
34.
What type of variable is changed during an experiment?
a)
Control
b)
Independent
c)
Dependent
35.
What type of data is based on numbers?
a)
Qualitative
b)
Quantitative
36.
Which of the following represents a compound?
a)
H2O
b)
H-3
c)
H
d)
O-16
37.
A chemical change occurs when a piece of wood ____.
a)
is cut
b)
decays
c)
is painted
d)
is split
38.
The first figure in a properly written chemical symbol always is ____.
a)
italicized
b)
capitalized
c)
boldfaced
d)
underlined
39.
An example of an extensive property of matter is ____.
a)
hardness
b)
temperature
c)
mass
d)
pressure
40.
What do chemical symbols and formulas represent, respectively?
a)
elements and ions
b)
atoms and mixtures
c)
compounds and mixtures
d)
elements and compounds
41.
What must be done to be certain that a chemical change has taken place?
a)
Check for the production of bubbles before and after the change.
b)
Demonstrate that a release of energy occurred after the change.
c)
Check the composition of the sample before and after the change.
d)
Demonstrate that energy was absorbed by the reactants after the change.
42.
Which of the following is true about compounds?
a)
They have properties similar to those of their component elements.
b)
They can be physically separated into their component elements.
c)
They are substances.
d)
They have compositions that vary.
43.
All atoms are ____.
a)
negatively charged, with the number of electrons exceeding the number of protons
b)
neutral, with the number of protons equaling the number of electrons
c)
neutral, with the number of protons equaling the number of electrons, which is equal to the number of neutrons
d)
positively charged, with the number of protons exceeding the number of electrons
44.
The particles that are found in the nucleus of an atom are ____.
a)
protons and neutrons
b)
neutrons and electrons
c)
protons and electrons
d)
electrons only
45.
As a consequence of the discovery of the nucleus by Rutherford, which model of the atom is thought to be true?
a)
The nucleus is made of protons, electrons, and neutrons.
b)
Electrons are distributed around the nucleus and occupy almost all the volume of the atom.
c)
Protons, electrons, and neutrons are evenly distributed throughout the volume of the atom.
d)
The nucleus is made of electrons and protons.
46.
How is the number of neutrons in the nucleus of an atom calculated?
a)
Add the number of electrons and protons together.
b)
Subtract the number of protons from the mass number.
c)
Subtract the number of electrons from the number of protons.
d)
Add the mass number to the number of electrons.
47.
The atomic mass of an element depends upon the ____.
a)
mass of each electron in that element
b)
mass and relative abundance of each isotope of that element
c)
relative abundance of protons in that element
d)
mass of each isotope of that element
48.
How do the isotopes hydrogen-1 and hydrogen-2 differ?
a)
Hydrogen-2 has one neutron
b)
hydrogen-1 has none.
c)
Hydrogen-2 has one more electron than hydrogen-1.
d)
Hydrogen-2 has two protons
49.
In the Bohr model of the atom, an electron in an orbit has a fixed ____.
a)
color
b)
position
c)
size
d)
energy
50.
What unit is used to measure weighted average atomic mass?
a)
amu
b)
gram
c)
angstrom
d)
nanogram
51.
The atomic number of an element is the total number of which particles in the nucleus?
a)
neutrons
b)
protons and electrons
c)
electrons
d)
protons
52.
What is the electron configuration of potassium?
a)
1s2 2s2 2p6 3s2 3p6 4s1
b)
1s2 2s2 3s2 3p6 3d1
c)
1s2 2s2 2p2 3s2 3p2 4s1
d)
1s2 2s2 2p10 3s2 3p3
53.
The smallest particle of an element that retains the properties of that element is a(n) ____.
a)
proton
b)
neutron
c)
atom
d)
electron
54.
Using the periodic table, determine the number of neutrons in O-16.
a)
4
b)
16
c)
24
d)
8
55.
If the spin of one electron in an orbital is clockwise, what is the spin of the other electron in that orbital?
a)
counterclockwise
b)
zero
c)
both clockwise and counterclockwise
d)
clockwise
56.
How many half-filled orbitals are in a bromine atom?
a)
1
b)
2
c)
3
d)
4
57.
Who was the man who lived from 460B.C.-370B.C. and was among the first to suggest the idea of atoms?
a)
Thomson
b)
Atomos
c)
Dalton
d)
Democritus
58.
The principal quantum number indicates what property of an electron?
a)
electron cloud shape
b)
speed
c)
position
d)
energy level
59.
The letter "p" in the symbol 4p indicates the ____.
a)
speed of an electron
b)
spin of an electron
c)
principle energy level
d)
orbital shape
60.
Why do chemists use relative masses of atoms compared to a reference isotope rather than the actual masses of the atoms?
a)
The number of subatomic particles in atoms of different elements varies.
b)
The actual masses of protons, electrons, and neutrons are not known.
c)
The actual mass of an electron is very large compared to the actual mass of a proton.
d)
The actual masses of atoms are very small and difficult to work with.
61.
Which of the following is NOT a part of Dalton's atomic theory?
a)
Atoms of the same element are identical.
b)
Atoms are always in motion.
c)
Atoms that combine do so in simple whole-number ratios.
d)
All elements are composed of atoms.
62.
Isotopes of the same element have different ____.
a)
atomic numbers
b)
numbers of protons
c)
numbers of neutrons
d)
numbers of electrons
63.
All atoms of the same element have the same ____.
a)
number of protons
b)
number of neutrons
c)
mass numbers
d)
mass
64.
What does the number 84 in the name krypton-84 represent?
a)
the atomic number
b)
the mass number
c)
the sum of the protons and electrons
d)
twice the number of protons
65.
Which of the following is true about subatomic particles?
a)
Neutrons have no charge and are the lightest subatomic particle.
b)
The mass of a neutron nearly equals the mass of a proton.
c)
Electrons are negatively charged and are the heaviest subatomic particle.
d)
Protons are positively charged and the lightest subatomic particle.
66.
An element has an atomic number of 76. The number of protons and electrons in a neutral atom of the element are ____.
a)
38 protons and 38 electrons
b)
152 protons and 76 electrons
c)
76 protons and 0 electrons
d)
76 protons and 76 electrons
67.
What is the products in the formula pictured?
a)
Chlorophyll
b)
Glucose and Oxygen
c)
Light
d)
Carbon Dioxide and Water
68.
What is the reactants in the formula pictured?
a)
Glucose and Oxygen
b)
Chlorophyll
c)
Light
d)
Carbon Dioxide and Water
69.
What must occur for a change to be a chemical reaction?
a)
The change must involve a change in volume.
b)
There must be a change in chemical properties.
c)
The change must involve a change in mass.
d)
There must be a change in physical properties.
70.
Which of the following is NOT a physical property of water?
a)
It is a colorless liquid.
b)
Sugar dissolves in it.
c)
It has a boiling point of 100 C.
d)
It is composed of hydrogen and oxygen.
71.
What is one difference between a mixture and a compound?
a)
A compound consists of more than one phase.
b)
A mixture must be uniform in composition.
c)
A mixture can only be separated into its components by chemical means.
d)
A compound can only be separated into its components by chemical means.
72.
Which state of matter takes both the shape and volume of its container?
a)
solid
b)
gas
c)
liquid
d)
both gas and liquid
73.
Which of the following is true for all chemical reactions?
a)
The total mass of the products is greater than the total mass of the reactants.
b)
The total mass of the reactants equals the total mass of the products.
c)
The total mass of the products is less than the total mass of the reactants.
d)
The total mass of the reactants increases.
74.
Which of the following is a chemical property?
a)
color
b)
ability to react with oxygen
c)
hardness
d)
freezing point
75.
Which state of matter expands when heated and is easy to compress?
a)
solid
b)
liquid
c)
gas
d)
all of the above
76.
Which of the following items is NOT a compound?
a)
baking soda
b)
salad dressing
c)
sucrose
d)
table salt
77.
What happens to matter during a chemical reaction?
a)
Some matter is created.
b)
Some matter is destroyed and some is created.
c)
Matter is neither destroyed or created.
d)
Some matter is destroyed.
78.
All of the following are physical properties of matter EXCEPT ____.
a)
mass
b)
color
c)
melting point
d)
ability to rust
79.
Which of the following is a homogeneous mixture?
a)
salt water
b)
beef stew
c)
soil
d)
sand and water
80.
Which state of matter has a definite volume and takes the shape of its container?
a)
solid
b)
gas
c)
liquid
d)
both b and c
81.
Which of the following is true about homogeneous mixtures?
a)
They are known as solutions.
b)
They have compositions that never vary.
c)
They are always liquids.
d)
They consist of two or more phases.
82.
Which of the following is a physical change?
a)
rotting of food
b)
evaporation
c)
explosion
d)
corrosion
83.
Which of the following is a heterogeneous mixture?
a)
soil
b)
air
c)
steel
d)
salt water
84.
What are the columns on the Periodic Table called?
a)
Columns
b)
Rows
c)
Groups
d)
Periods
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