Worksheets(H) Semester 1 Final Exam Review
Total questions: 205
Worksheet time: 4hrs 6mins
Name
Class
Date
1.
How many significant figures? 0.00258
a)
2
b)
3
c)
4
d)
5
2.
How many significant figures? 2510
a)
2
b)
3
c)
4
d)
5
3.
How many significant figures? 0.08500
a)
2
b)
3
c)
4
d)
5
4.
How many significant figures? 2.30x105
a)
2
b)
3
c)
4
d)
5
5.
How many significant figures? 4,000,000
a)
1
b)
2
c)
3
d)
4
6.
How many significant figures? 0.000580
a)
1
b)
2
c)
3
d)
4
7.
How many significant figures? 26
a)
1
b)
2
c)
3
d)
4
8.
How many significant figures? 6.0x10-8
a)
2
b)
3
c)
4
d)
5
9.
How many significant figures? 9.840x10-20
a)
1
b)
2
c)
3
d)
4
10.
How many significant figures? 0.0005
a)
1
b)
2
c)
4
d)
5
11.
How many significant figures? 0.50
a)
1
b)
2
c)
3
d)
4
12.
Solve: 3.12 g + 0.8 g + 1.033 g =
a)
4.953 g
b)
4.9 g
c)
5.0 g
d)
5 g
13.
When performing the calculation 34.530 g + 12.1 g + 1 222.34 g, the final answer must have
a)
Only one decimal place
b)
Units of g3
c)
Three significant figures
d)
Three decimal places
14.
Solve: 13.004 m + 3.09 m + 112.947 m =
a)
129.0 m
b)
129 m
c)
129.04 m
d)
129.041 m
15.
Add the following three numbers and report your answer using significant
figures:
2.5 cm + 0.50 cm + 0.055 cm =
a)
3.06 cm
b)
3.1 cm
c)
3.0 cm
d)
3 cm
16.
Convert the following to scientific notation.
0.000480
0.000480
a)
4.8 x 10^4
b)
4.80 x 10^4
c)
4.8 x 10^3
d)
4.80 x 10^3
17.
Convert to scientific notation 305,000
a)
3.0500
b)
3.0500 x 10^5
c)
3.05 x 10^5
d)
3.05 x 10^2
18.
It is possible to get the exact measurement of an object.
a)
True
b)
False
19.
Which is the product of these numbers, to the appropriate number of significant digits?
56.2 x 9.2057 =
56.2 x 9.2057 =
a)
517
b)
517.4
c)
517.36
d)
517.00
20.
The product of 2 x 10^4 cm and 4 x 10^–12 cm, expressed in scientific notation is ____.
a)
8 x 10^–7 cm
b)
6 x 10^–8 cm
c)
8 x 10^–8 cm
d)
8 x 10^–48 cm
21.
A solid is
a)
a substance that does not have a definite shape or volume
b)
a substance with a definite volume, but no definite shape
c)
a substance with a definite shape and volume
d)
a substance whose particles glide past one another
22.
A liquid is
a)
a substance that does not have a definite shape or volume
b)
a substance with a definite volume, but no definite shape
c)
a substance with a definite shape and volume
d)
a substance whose particles vibrate
23.
Which states of matter have a definite volume?
a)
solid and gas
b)
solid and liquid
c)
gas and liquid
d)
solid, liquid, and gas
24.
Which of the following is a characteristic of liquids?
a)
molecules are tightly packed
b)
takes the shape of its container
c)
constantly keeps its shape
d)
molecules are spread far apart
25.
Law of Conservation of Matter states that
a)
the mass of an object will stay the same even if it goes through a change
b)
matter will change mass if it goes through a change
26.
A change that only affects the appearance of a substance (its size, shape, or state of matter)
a)
physical change
b)
chemical change
27.
a change in which one kind of matter changes into a different kind of matter with different properties
a)
chemical change
b)
physical change
28.
Rusting nail
a)
Chemical change
b)
physical change
29.
Matter looks different after a _______, but it is still made up of the same kind of matter.
a)
Physical Change
b)
Chemical Change
c)
Evaporation
d)
Water Vapor
30.
This particle is found in the nucleus and has no charge
a)
Neutron
b)
Proton
c)
Electron
31.
This particle is found in the nucleus and has a positive charge
a)
Electron
b)
Proton
c)
Neutron
32.
This contains most of the mass of an atom
a)
Electron Cloud
b)
Nucleus
c)
Electron
33.
This is the simplest of all atoms and contains only one proton and one electron
a)
Oxygen
b)
Hydrogen
c)
Water
34.
The first person to ever talk about an atom was
a)
Democritus
b)
Rutherford
c)
Dalton
35.
How did Rutherford discover the proton?
a)
Cathode tube ray experiment
b)
Gold Foil Experiment
c)
Planetary Model
d)
Plum Pudding Model
36.
Who stated that all atoms of the same element are excacty alike?
a)
Democritus
b)
Dalton
c)
Thomson
d)
Borh
37.
What scientist is best known for his "Plum Pudding" model of the atom?
a)
J.J. Tomson
b)
Ernest Rutherford
c)
John Dalton
d)
Democritus
38.
What contribution did John Dalton make to atomic theory?
a)
He discovered that every atom was positively charged.
b)
He discovered that every element consisted of one type of atom.
c)
He discovered that atoms had nuclei.
d)
He discovered that atoms could be divided into smaller parts.
39.
Place the following scientists in order, from earliest to latest:
A) Ernest Rutherford
B) J.J. Thomson
C) John Dalton
A) Ernest Rutherford
B) J.J. Thomson
C) John Dalton
a)
B,C,A
b)
C,A,B
c)
A,C,B
d)
C,B,A
40.
J.J. Thomson provided evidence that an atom...
a)
is the smallest particle of matter
b)
contains negatively charged particles
c)
has an overall negative charge
d)
has an overall positive charge
41.
Rutherford's gold foil experiment provided evidence that...
a)
negative and positive charges are spread evenly throughout the atom.
b)
alpha particles have a positive charge.
c)
gold is not a dense as previously thought.
d)
there is a dense positively charged nucleus at the center of an atom.
42.
An atom's overall charge is ________.
a)
positive
b)
depends
c)
neutral
d)
negative
43.
Who came up with this model of an atom?
a)
J.J. Thompson
b)
Ernest Rutherford
c)
Neils Bohr
d)
James Chadwick
44.
True or False: The majority of an atom is made up of empty space
a)
True
b)
False
45.
Which particle is responsible for the chemical properties of an atom?
a)
Neutron
b)
Protons
c)
Valence Electrons
d)
Nucleus
46.
Neon has an atomic number of 10 and an atomic mass of 20.180. How many protons, electrons, and neutrons will it have?
a)
P=10 E=10 N=11
b)
P=5 E=5 N=10
c)
P=10 E=10 N=10
d)
P=10 E=5 N=5
47.
Alpha particles.....
a)
a) are positively charged.
b)
b) consist of two protons and four neutrons.
c)
c) can penetrate any thickness of matter
d)
d) All of the above
48.
The process of nuclear change in an atom of radioactive material is called...
a)
nuclear decay
b)
nuclear mass
c)
isotopes
d)
radon
49.
During beta decay, a nucleus ....
a)
gives up two protons and two neutrons.
b)
maintains the same number of protons and neutrons.
c)
loses a proton and gains a neutron.
d)
gains a proton and loses a neutron.
50.
Radioactive materials have unstable...
a)
electrons
b)
protons
c)
nuclei
d)
neutrons
51.
During ________________, unstable elements are transformed into more stable elements.
a)
mutation
b)
germination
c)
pollination
d)
radioactive decay
52.
An alpha particle is a _____________ nucleus.
a)
H (hydrogen)
b)
He (helium)
c)
U (uranium)
d)
Na (sodium)
53.
This radioactive particle is also known as an electron and has a charge of -1
a)
alpha
b)
beta
c)
gamma
d)
kryptonite
54.
With respect to penetrating power, a gamma particle is considered the _________________ form of radiation and lead or concrete incompletely block this type of radiation.
a)
weakest
b)
strongest
c)
somewhat strongest
d)
all radioactive particles are equally powerful
55.
For the following nuclear reaction, what was the starting substance (X)?
X → 86Rn222 + 2He4
X → 86Rn222 + 2He4
a)
Radium-222
b)
Radon-222
c)
Radon-226
d)
Radium-226
56.
Complete the following reaction and choose the type of decay.
54Xe118 → X + 55Cs118
54Xe118 → X + 55Cs118
a)
alpha emission
b)
neutron activation
c)
beta emission
d)
gamma emission
57.
What is Half-life?
a)
The amount of time it takes for some of the nuclei in a sample of the isotope to decay
b)
The amount of time it takes for half the electrons in a sample of the isotope to decay
c)
The amount of time it takes for half the nuclei in a sample of the isotope to decay
d)
the amount of time it takes to double the nuclei in a sample of the isotope to decay
58.
After the third half-life, how much of a radioactive sample is left?
a)
1/2
b)
1/3
c)
1/16
d)
1/8
59.
The half life of iodine-131 is 8 days. What fraction of an iodine-131 sample will remain after 40 days?
a)
1/2
b)
1/64
c)
1/5
d)
1/32
60.
As a sample of Neon-19 undergoes radioactive decay, its half-life will
a)
decrease
b)
increase
c)
remain the same
d)
start over
61.
Barium-122 has a half-life of 2 minutes. A fresh sample weighing 80 g was obtained. If it takes 10 minutes to set up an experiment using barium-122, how much barium-122 will be left when the experiment begins?
a)
0.25g
b)
2.5g
c)
25g
d)
80g
62.
The half-life of strontium-90 is 25 years. How much strontium-90 will remain after 100 years if the initial amount is 4.0 g?
a)
3.0g
b)
0.25mg
c)
0.3g
d)
0.25g
63.
When nuclei decay, massive amounts of __________ is released.
a)
energy
b)
electrons
c)
protons
d)
neutrons
64.
If 10 mg of iodine 131 is given to a patient, how much is left after 24 days? The half-life of iodine-131 is 8 days.
a)
1.25mg
b)
1.25g
c)
10g
d)
10mg
65.
The half-life of Zn-71 is 2.4 minutes. If one had 100.0 g at the beginning, how many grams would be left after 7.2 minutes has elapsed?
a)
100.0g
b)
50.0g
c)
12.5g
d)
8.5g
66.
The half-life of a radioactive isotope is not effected by which of the following?
a)
Temperature
b)
Pressure
c)
Concentration
d)
None of these will effect the rate of a nuclear reaction
67.
Different versions of an element, with differing numbers of neutrons, are called _____
a)
isosceles
b)
isomers
c)
isotopes
d)
isicless
68.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
69.
When electron changes its orbit from outer to inner energy is
a)
absorbed
b)
released
c)
no change
d)
remains constant
70.
How many neutrons in C-14?
a)
6
b)
7
c)
14
d)
8
71.
How many protons does this isotope of titanium have?
a)
48
b)
22
c)
26
d)
70
72.
How many neutrons does uranium-235 have?
a)
238
b)
92
c)
146
d)
143
73.
What do these isotopes of carbon all have in common?
a)
neutrons & mass number
b)
atomic number and neutrons
c)
atomic number and electrons
d)
protons, atomic number, and mass number
74.
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
75.
Magnesium exists as three isotopes shown above. What is the average atomic mass?
a)
18.39 amu
b)
20.74 amu
c)
22.56 amu
d)
24.31 amu
76.
Atom 1 has Mass=12 Protons=6
Atom 2 has Mass= 14 Electrons=6
Are these atoms isotopes of each other or different elements?
Atom 2 has Mass= 14 Electrons=6
Are these atoms isotopes of each other or different elements?
a)
Different Elements - Mg & Si
b)
Different Elements - Ar & Ca
c)
Isotopes of Carbon
d)
Isotopes of Magnesium
77.
What does the 1.00794 stand for?
a)
Hydrogen
b)
atomic number
c)
atomic mass
d)
atomic explosion
78.
Isotopes are atoms of the same element that have the same number of __________ but different number of __________ . Therefore, isotopes of the same element have different masses.
a)
protons, neutrons
b)
protons, electrons
c)
neutrons, protons
d)
electrons, protons
79.
A neutral atom of Carbon-13 has ________ electrons and _________ neutrons
a)
13, 13
b)
6, 7
c)
7, 7
d)
6, 6
80.
24.1% of all the isotopes of a an element have a mass of 75.23 amu, 48.7% have a mass of 74.61 amu, and 27.2% have a mass of 75.20 amu.
What is the average mass of this element?
What is the average mass of this element?
a)
74.92 amu
b)
24.97 amu
c)
75.01 amu
d)
74.51 amu
81.
24.1% of all the isotopes of a an element have a mass of 75.23 amu, 48.7% have a mass of 74.61 amu, and 27.2% have a mass of 75.20 amu.
What is the average mass of this element?
What is the average mass of this element?
a)
74.92 amu
b)
24.97 amu
c)
75.01 amu
d)
74.51 amu
82.
Nitrogen has three occurring isotopes: Nitrogen-13, Nitrogen-14, Nitrogen-15. Which isotope is the most abundant?
a)
Nitrogen-13
b)
Nitrogen-14
c)
Nitrogen-15
d)
Based on the information given, it cannot be determined
83.
If X is the symbol for an element, which of the following two symbols represent isotopes of the same element?
I. 7735X II. 7733X III. 8137X IV. 8135 X
I. 7735X II. 7733X III. 8137X IV. 8135 X
a)
I and II
b)
III and IV
c)
I and IV
d)
I and III
84.
Calcium has three different isotopes. One has a mass of 35.00 amu; another has a mass of 41.00 amu; and another has a mass of 40.00 amu. Which isotope is the most abundant of the three?
a)
41 amu
b)
40 amu
c)
35 amu
d)
Cannot be determined based on information given
85.
How did Mendeleev arrange the elements?
a)
alphabetical
b)
density
c)
melting point
d)
atomic mass
86.
The horizontal row on the periodic table is called a
a)
group
b)
family
c)
period
d)
atomic number
87.
A vertical column is called...
a)
group
b)
tower
c)
period
d)
crew
88.
A rule that states that repeating chemical and physical properties of elements change periodically with the atomic number of the elements is the _________.
a)
periodic law
b)
alkaline-earth metals
c)
actinide
d)
group rule
89.
Pure forms of these elements are stored in oil so they won't react with oxygen and water in the air.
a)
Alkali Metals
b)
Alkaline-earth metals
c)
Halogens
d)
Noble Gases
90.
Most of the elements on the periodic table are classified as _____.
a)
Metals
b)
Nonmetals
c)
Metalloids
d)
Periods
91.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
92.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
93.
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)
94.
The atom with the largest atomic radius in Group 18 is -
a)
Ar
b)
He
c)
Kr
d)
Rn
95.
Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.
a)
decreases, increases
b)
increases, increases
c)
increases, decreases
d)
stays the same, increases
96.
Atomic radius generally increases as we move __________.
a)
down a group and from right to left across a period
b)
up a group and from left to right across a period
c)
down a group and from left to right across a period
d)
up a group and from right to left across a period
97.
Vertical columns of elements (these are also known as a "family") - they also have the same number of valence electrons and are known as ________________.
a)
groups
b)
periods
c)
quadrants
d)
rows
98.
The family in the periodic table that contains the most reactive metals is the_______
a)
Alkaline Earth Metals
b)
Transition Metals
c)
Alkali Metals
d)
Other Metals
99.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
100.
Group 3 elements have ____ electrons in their outermost shell.
a)
1
b)
2
c)
3
d)
4
101.
What is the oxidation number of Magnesium (Mg)?
a)
+2
b)
-2
c)
+4
d)
-4
102.
What is the oxidation number for Flourine (F)?
a)
+1
b)
-1
c)
17
d)
7
103.
Rank the following in order of increasing reactivity: Ge, K, Br, Ca (lowest to highest reactivity)
a)
Ge, K, Br, Ca
b)
K, Br, Ge, Ca
c)
Br, Ge, Ca, K
d)
Br, Ca, Ge, K
104.
The ability of atoms to attract electrons from surrounding atoms is called ___.
a)
ionization energy
b)
electronegativity
c)
electron shielding
d)
swarming
105.
Which atoms have the highest electronegativity?
a)
Atoms with small atomic radius
b)
Atoms with large atomic radius
c)
Atoms on the left of the periodic table.
106.
Elements, like barium, located toward the bottom of a group have a lower attraction for their valence electrons because they have a __________.
a)
high ionization energy
b)
high electronegativity
c)
small atomic radius
d)
large atomic radius
107.
Atoms with a low ionization energy hold tight to their outer valence electrons.
a)
True
b)
False
108.
Which of the following is NOT a property of ionic compounds?
a)
They conduct electricity when molten
b)
They conduct electricity when in solution
c)
They have high boiling points
d)
They are insoluble in water
109.
What is the charge on an Aluminium ion?
a)
3
b)
+3
c)
+2
d)
+1
110.
What is the charge of Neon?
a)
0
b)
+1
c)
-1
d)
1
111.
How many valence electrons does calcium have?
a)
2
b)
4
c)
6
d)
7
112.
A(n) _________ is an ion with a positive (+) charge.
a)
anion
b)
cation
c)
ion
d)
solute
113.
When an atom loses an electron, it becomes a:
a)
positive ion
b)
negative ion
c)
neutral ion
d)
neutral atom
114.
Magnesium bromide is an ionic compound with the chemical formula MgBr₂. What does the "2" tell you?
a)
There are 2 bromide ions for every magnesium ion
b)
Bromide has a 2- charge
c)
Bromide has a 2+ charge
d)
There are 2 magnesium ions to every bromide ion
115.
In the chemical formula for an ionic compound, which item is written first?
a)
positive ion
b)
negative ion
c)
subscript
d)
the female
116.
Which of the following is a characteristic property of ionic compounds?
a)
They form hard, brittle crystals with characteristic shapes
b)
They have low melting points
c)
They have low boiling points
d)
They contain no charged particles
117.
In what form can an ionic compound conduct electricity?
a)
when dissolved in water
b)
as a solid
c)
as a crystal
d)
when warmed slightly
118.
If the name of a compound ends in "IDE", what does that tell us about the atoms that make it up?
a)
That it is a molecule
b)
That it contains two different elements
c)
That it contains two atoms
d)
That it is an ionic compound
119.
a three-dimensional geometric arrangement of particles in which each positive ion is surrounded by negative ions and each negative ion is surrounded by positive ions; vary in shape due to sizes and relative numbers of the ions bonded
a)
crystal lattice
b)
delocalized electrons
c)
electrolyte
d)
electron sea model
120.
the electrons involved in metallic bonding that are free to move easily from one atom to the next throughout the metal and are not attached to a particular atom
a)
electron sea model
b)
delocalized electrons
c)
lattice energy
d)
oxyanion
121.
proposes that all metal atoms in a metallic solid contribute their valence electrons to form a "sea" of electrons, and can explain properties of metallic solids such as malleability, conduction, and ductility
a)
electrolyte
b)
delocalized electrons
c)
crystal lattice
d)
electron sea model
122.
the electrostatic force that holds oppositely charged particles together in an ionic compound
a)
ionic compounds
b)
ionic bond
c)
metallic bond
d)
chemical bond
123.
Name the following Ionic Compound:
FePO4
FePO4
a)
Iron (III) Phosphate
b)
Iron (III) Phosphide
c)
Iron (II) Phosphate
d)
Iron (II) Phosphite
124.
Write the formula from the following ionic compound:
Calcium Nitrate
Calcium Nitrate
a)
CaN
b)
CaNO3
c)
Ca2NO3
d)
Ca(NO3)2
125.
the energy required to separate one mole of the ions of an ionic compound, which is directly related to the size of the ions bonded and is also affected by the charge of the ions
a)
oxyanion
b)
formula unit
c)
electrolyte
d)
lattice energy
126.
Which of the following is the best explanation for why MgS has a greater lattice energy than NaCl?
a)
MgS involves greater magnitude of charges (+2 and -2)
b)
NaCl involves lesser magnitude of charges (+1 and -1)
c)
MgS involves smaller ions than NaCl
d)
NaCl involves larger ions than MgS
127.
Select two answers - which two factors influence lattice energy?
a)
size of particle
b)
charge of particle
c)
position on the periodic table
d)
Zeff
128.
The portion of the electromagnetic spectrum that humans can see is called:
a)
radio waves
b)
visible light
c)
gamma rays
d)
x-rays
129.
When wavelength increases...
a)
energy decreases
b)
energy increases
130.
As wavelength decreases...
a)
energy increases
b)
energy decreases
131.
the distance between peaks of electromagnetic waves is called:
a)
wavelength
b)
frequency
c)
energy
d)
Planck's Constant
132.
Which type of electromagnetic energy carries the least energy?
a)
X-Rays
b)
Visible Light
c)
Ultraviolet
d)
Microwaves
133.
1 MHz is equal to:
a)
10 Hz
b)
100 Hz
c)
1,000 Hz
d)
1,000,000 Hz
134.
Which type photon carries the most energy?
a)
Yellow Light
b)
Red Light
c)
Blue Light
d)
Green Light
135.
The formula for the radiative energy (E) carried by a photon of light is:
a)
E = h x c
b)
E = c/λ
c)
E = h x f
d)
E = mMG/d
136.
The speed of electromagnetic radiation:
a)
depends on the form of radiation
b)
is always 3 x 108 m/s, regardless of the type
c)
decreases as distance increases
d)
is 6.626 x 10-34 J x s
137.
What is the speed of light?
a)
it depends on the type of electromagnetic radiation
b)
3 x 108 m/s
c)
3 x 10-34 m/s
d)
500 km/s
138.
1 nanometer is equal to:
a)
1 billionth of a meter
b)
10 billionths of a meter
c)
1,000 meters
d)
1 million meters
139.
Which of the following is a unit for frequency?
a)
Joules
b)
Hertz
c)
meters per second
d)
seconds
140.
Light is:
a)
a star and a galaxy
b)
a wave and a particle
c)
sound and energy
d)
unable to be measured
141.
A light particle is called a(n):
a)
electromagnetic wave
b)
photon
c)
electron
d)
atom
142.
We see a "rainbow of colors" that when perceived together produce:
a)
black light
b)
white light
c)
gamma rays
d)
x-ray images
143.
Which has a longer wavelength?
a)
infrared
b)
ultraviolet
144.
Which is can be felt as "heat"?
a)
gamma rays
b)
infrared
c)
x-ray
d)
blue light
145.
Which is the correct order of the electromagnetic spectrum from highest frequency to lowest frequency?
a)
Gamma, X-ray, Ultraviolet, Visible, Infrared, Microwave, Radio
b)
Gamma, Ultraviolet, Visible, Infrared, X-ray, Microwave, Radio
c)
Ultraviolet, Microwave, Radio, Visible, X-ray, Gamma, Infrared
d)
Radio, Microwave, Infrared, Gamma, X-ray, Ultraviolet, Visible
146.
Which class of electromagnetic radiation has the longest wavelengths?
a)
Radio
b)
Gamma
c)
Infrared
d)
Visible
147.
Which class of electromagnetic radiation has the least energy?
a)
Radio
b)
Gamma
c)
Infrared
d)
Visible
148.
Which color light has the longest wavelength?
a)
Red
b)
Orange
c)
Green
d)
Violet
149.
The color of stars and flames corresponds to the temperature of the heated gases. Which color is the coolest?
a)
Red
b)
Blue
c)
White
d)
Yellow
150.
Light energy is the only energy source that can cause an electron to move from its ground state to the excited state.
a)
true
b)
false
151.
If electrons gain energy they
a)
move up one or more shells
b)
more down one or more shells
152.
Electrons can have
a)
only specific amount of energy (little packets)
b)
any amount of energy
153.
Why did the alpha particle (positively charged particle) sometimes bounce back when hitting the gold foil.
a)
hit neutron in nucleus and they repelled alpha particle
b)
hit proton in nucleus and they repelled alpha particle
c)
hit electrons in electron shells and they repelled alpha particle
154.
The first subatmomic particle that was discovered was the
a)
proton
b)
neutron
c)
electron
d)
nucleus
155.
Potassium
a)
red
b)
orange
c)
purple
d)
green
156.
Sodium
a)
red
b)
orange
c)
yellow
d)
green
157.
Wavelength and frequency are __________ related.
a)
directly
b)
inversely
158.
The _______________ determines the color of visible light.
a)
wavelength
b)
speed
c)
amplitude
d)
light
159.
Name the following ionic compound: MgSO4
a)
magnesium sulfoxide
b)
magnesium sulfide
c)
magnesium sulfate
d)
magnesium oxide
160.
LiBr is called
a)
lithium bromine
b)
lithium (I) bromine
c)
lithium bromide
d)
lithuim (I) bromide
161.
What is the correct formula for Sodium Oxide?
a)
NaO
b)
NaO2
c)
Na2O
d)
Na2O2
162.
Al(OH)3
a)
alumiunum trihydroxide
b)
trialuminum hydroxide
c)
aluminum hydroxide
d)
aluminum oxygen hydride
163.
Write the formula for vanadium (IV) carbonate
a)
V(CO3)2
b)
V4C
c)
V(CO3)4
d)
V4(CO3)
164.
Write the formula for copper (I) phosphide
a)
Cu3P
b)
CuP
c)
Cu1P
d)
CuP3
165.
When does a compounds name require the use of Roman Numerals and Parentheses to indicate charge?
a)
All the time
b)
Only when its a covalent compound
c)
When there is a transition metal in the compound
166.
Ni+2 and SO3-2 (NiSO3)
a)
Nickel (II) Sulfite
b)
Nickel Sulfate
c)
Nickel (I) Sulfite
167.
What is the correct formula for dinitrogen pentoxide?
a)
N2O5
b)
N3O5
c)
N4O2
d)
N2O7
168.
What is the correct formula for sulfur hexachloride?
a)
SCl2
b)
S6Cl
c)
SCl6
d)
Scl8
169.
What is the correct formula for nitrogen monoxide?
a)
N2O3
b)
NO
c)
N2O7
d)
N3O10
170.
What is the correct formula for heptoxygen difluoride?
a)
O6F4
b)
O6F5
c)
O7F4
d)
O7F2
171.
What is the correct formula for carbon tetrachloride?
a)
CCl4
b)
CCl3
c)
CCl9
d)
C2Cl7
172.
What is the correct formula for trinitrogen decoxide?
a)
NO3
b)
N3O9
c)
N7O6
d)
N3O10
173.
What is the correct formula for pentaboron dihydride?
a)
B5H4
b)
B5H2
c)
B2H5
d)
BH6
174.
What is the correct formula for carbon monoxide?
a)
CO
b)
C2O2
c)
C3O2
d)
C7O5
175.
What type of atoms combine with a covalent bond?
a)
metals and nonmetals
b)
only metals
c)
only alkali metals and nonmetals
d)
only nonmetals
176.
What is happening in the picture that shows a covalent bond is formed?
a)
some atoms are losing electrons and some are gaining them
b)
some atoms are sharing electrons
c)
electrons are shifting to new energy levels to form a bond
d)
electrons spread out and protons move together to created a positive and an negative charge.
177.
N2O5?
a)
Nitrogen oxide
b)
Dinitrogen pentaoxide
c)
Pentaoxide dinitrogen
d)
Nitrogen pentaoxide
178.
SF6?
a)
Monosulfur Hexafluoride
b)
Sulfur hexafluoride
c)
Sulfate hexafluoride
d)
Sulfur hexafluorine
179.
Nitrogen trichloride?
a)
NCl3
b)
NCl2
c)
NC3
d)
Cl3N
180.
The deer population is estimated to be 17,600 in northern Illinois, but an actual count was 21,300. What is the percent error?
a)
21%
b)
17.37%
c)
17.4%
d)
21.02%
181.
Accuracy is defined as
a)
close repeated measurements
b)
awesome measurements
c)
really good guessing
d)
measurement near the true value
182.
Romy's measurements: 6.02 m, 6. 04 m, 6.03 m
Actual Value: 6.02 m
How would you define her measurements?
Actual Value: 6.02 m
How would you define her measurements?
a)
accurate and precise
b)
accurate
c)
precise
d)
neither
183.
This bullseye demonstrates...
a)
High Accuracy & High Precision
b)
High Accuracy & Low Precision
c)
Low Accuracy & High Precision
d)
Low Accuracy & Low Precision
184.
When a measurement is repeatable and consistent it is said to have...
a)
High precision
b)
Low precision
c)
High accuracy
d)
Low accuracy
185.
Find the percent error. You estimate that you sent 135 texts last week but when you get the bill it was actually 108.
a)
(135 - 108)/135 = 20%
b)
(135 - 108)/108 = 25%
c)
(108 - 135)/135 = -20%
d)
(108 - 135)/108 = -25%
186.
How many cm's is in a meter?
a)
1000
b)
10
c)
100
d)
1
187.
You can visually observe complete combustion by it's _________________ flame color.
a)
yellow
b)
white
c)
pink
d)
blue
188.
You can visually observe incomplete combustion by it's _______________ flame color
a)
white
b)
orange
c)
blue
d)
pink
189.
complete combustion is characterized by the following products:
a)
carbon dioxide and water
b)
carbon, carbon monoxide, and water
c)
hydrocarbon and oxygen
d)
wax and oxygen
190.
incomplete combustion is characterized by the following products:
a)
carbon dioxide and water
b)
carbon, carbon monoxide, and water
c)
hydrocarbon and oxygen
d)
carbon dioxide and oxygen
191.
The candle lab is an example of ___________.
a)
complete combustion
b)
incomplete combustion
c)
synthesis
d)
decomposition
192.
bromylthymol blue is an indicator for __________.
a)
carbon
b)
carbon monoxide
c)
water
d)
hydrocarbon
193.
What is the difference between complete and incomplete combustion?
a)
the amount of hydrocarbon
b)
the amount of oxygen
c)
the amount of water
d)
the amount of carbon monoxide
194.
4Si + S8 --> 2Si2S4
a)
Synthesis
b)
Decomposition
c)
Single displacement
d)
Double displacement
195.
3Ca + 2AlCl3 --> 3CaCl2 + 2Al
a)
Synthesis
b)
Decomposition
c)
Single diplacement
d)
Double displacement
196.
3KOH + H3PO4 --> K3PO4 + 3H2O
a)
Synthesis
b)
Decomposition
c)
Single displacement
d)
Double displacement
197.
2Pb(NO3)2 --> 2PbO + 4NO2 + O2
a)
Synthesis
b)
Decomposition
c)
Single displacement
d)
Combustion
198.
P4 + 3O2 --> 2P2O3
a)
Synthesis
b)
Decomposition
c)
Single displacement
d)
Combustion
199.
A + B = AB
a)
Double Replacement
b)
Synthesis
c)
Combustion
d)
Decomposition
200.
AB + CD = AD + CB
a)
Double Replacement
b)
Single Replacement
c)
Combustion
d)
Decomposition
201.
Fe + H2SO4 --> Fe2(SO4)3 + H2
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Combustion
202.
AB = A + B
a)
Decomposition
b)
Single Replacement
c)
Combustion
d)
Synthesis
203.
3Mg + N2 --> Mg3N2
a)
Synthesis
b)
Decomposition
c)
Single displacement
d)
Combustion
204.
2NO2 --> N2 + 2O2
a)
Synthesis
b)
Decomposition
c)
Single displacement
d)
Combustion
205.
2Fe + 3H2SO4 --> Fe2(SO4)3 + 2H2
a)
Synthesis
b)
Decomposition
c)
Single displacement
d)
Combustion
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