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WorksheetsSuper Ginormous December Final Review Quiz
Total questions: 148
Worksheet time: 4hrs 25mins
Name
Class
Date
1.
All of the following are physical properties of matter EXCEPT
a)
Mass
b)
Color
c)
Melting Point
d)
Ability to rust
2.
A vapor is which state of matter?
a)
Solid
b)
Liquid
c)
Gas
d)
Plasma
3.
Which of the following is NOT an example of matter?
a)
Air
b)
Heat
c)
Smoke
d)
Water Vapor
4.
Which state of matter expands when heated and is easy to compress?
a)
Gas
b)
Liquid
c)
Solid
d)
Solids, Liquids, and Gases
5.
Which state of matter takes both the shape and volume of its container?
a)
Solid
b)
Liquid
c)
Gas
d)
Both Liquid and Gas
6.
A chemical change occurs when a piece of wood
a)
is split
b)
is painted
c)
decays
d)
is cut
7.
What is the SI unit of mass?
a)
liter
b)
joule
c)
candela
d)
kilogram
8.
Density is found by dividing
a)
mass by volume
b)
volume by mass
c)
mass by area
d)
area by mass
9.
The nucleus of an atom is
a)
the central core and is composed of protons and neutrons
b)
positively charged and has more protons than neutrons
c)
negatively charged and has a high density
d)
negatively charged and has a low density
10.
In Bohr's model of the atom, where are the electrons and protons located?
a)
The electrons move around the protons, which are at the center of the atom.
b)
The electrons and protons move throughout the atom
c)
The electrons occupy fixed positions around the protons, w hich are at the center of the atom
d)
The electrons and protons are located throughout the atom, but they are not free to move
11.
Stable electron configurations are likely to contain
a)
filled energy sublevels
b)
fewer electrons than unstable configurations
c)
unfilled s orbitals
d)
electrons with a clockwise spin
12.
The modern periodic table is arranged in order of increasing atomic
a)
mass
b)
charge
c)
number
d)
radius
13.
Of the elements, Pt, V, Li, and Kr, which is a nonmetal?
a)
Pt
b)
V
c)
Li
d)
Kr
14.
The atomic number of an element is the total number of which particles in the nucleus?
a)
neutrons
b)
protons
c)
electrons
d)
protons and electrons
15.
The SI base unit of length is the
a)
gram
b)
foot
c)
yard
d)
meter
16.
A description of how close a measurement is to its true value
a)
accuracy
b)
precision
c)
significant figures
d)
explanation
17.
An atom's ability to undergo chemical reactions is determined by its
a)
protons.
b)
innermost electrons.
c)
neutrons.
d)
outermost electrons.
18.
Aluminum has _ valence electrons.
a)
7
b)
1
c)
6
d)
3
19.
Postive ions are called
a)
anions
b)
positrons
c)
alpha
d)
cations
20.
A description of how close measurements are to each other is
a)
accuracy
b)
closeness
c)
precision
d)
target location
21.
The "s" orbital can hold
a)
2 electrons
b)
4 electrons
c)
6 electrons
d)
10 electrons
22.
An atom has 12 protons, 12 electrons and 14 neutrons. What is the mass number?
a)
12
b)
24
c)
26
d)
38
23.
a copper penny turning greenish after a few years.
a)
Chemical Change
b)
Physical Change
24.
Mendeleev arranged the periodic table by...?
a)
color
b)
increasing atomic mass
c)
increasing atomic number
d)
density
25.
What does it mean when an element is happy?
a)
They have 8 protons
b)
They have 8 valence electrons (a full octet)
c)
They have 8 protons
d)
They have 8 neutrons
26.
What element is represented in this Bohr Model?
a)
Carbon
b)
Hydrogen
c)
Aluminum
d)
Lithium
27.
How are covalent bonds explained?
a)
When one atom takes the other atom's electron
b)
When the atom shares an electron with an another atom
c)
When the two nucleus merge
d)
When the neutrons leave the nucleus
28.
States that it is not possible to know precisely both the velocity and the position of a particle at the same time.
a)
Hund's rule
b)
Pauli exclusion principle
c)
Heisenberg uncertainty principle
d)
Aufbau principle
29.
Which subatomic particle is negatively charged?
a)
proton
b)
atom
c)
neutron
d)
electron
30.
Which atomic particle has a positive charge?
a)
Proton
b)
Neutron
c)
Electron
31.
The smallest particle of an element that retains the properties of that element is a(n)
a)
atom
b)
electron
c)
proton
d)
neutron
32.
Which subatomic particle has a neutral charge?
a)
Proton
b)
Neutron
c)
Electron
33.
The particles that are found in the nucleus of an atom are
a)
neutrons and electrons
b)
electrons only
c)
protons and neutrons
d)
protons and electrons
34.
All atoms of the same element have the same
a)
number of neutrons
b)
number of protons
c)
mass number
d)
mass
35.
Isotopes of the same element have different
a)
number of neutrons
b)
number of protons
c)
number of electrons
d)
atomic number
36.
A mixture that does not look the same throughout:
a)
heterogeneous mixture
b)
homogeneous mixture
c)
the periodic table
d)
water
37.
Calculate the density of a substance with a volume of 5.0 mL and a mass of 45.3 g.
a)
0.110 g/mL
b)
9.06 g/mL
c)
226 g/mL
d)
15.0 g/mL
38.
A negative ion is called
a)
cation
b)
anion
c)
cathode
d)
electro
39.
When naming an ionic compound, you
a)
name the non-metal first
b)
use prefixes to show the number of atoms
c)
name the cation (metal) first
d)
there is no set rule
40.
The formula for copper (I) chloride is
a)
CoCl2
b)
CoCl
c)
CuCl
d)
CuCl2
41.
In the picture shown, element x is likely __________.
a)
Carbon
b)
Oxygen
c)
Nitrogen
d)
Fluorine
42.
What is the FORMULA for
magnesium carbonate
magnesium carbonate
a)
Mg(CO3)2
b)
MgHCO3
c)
MgCO2
d)
MgCO3
43.
Which of the following represents values that are precise, but not accurate? Assume that the desired value is a bullseye.
a)
A
b)
B
c)
C
d)
D
44.
Which of the following represents values that are neither accurate nor precise? Assume that the desired value is a bullseye.
a)
A
b)
B
c)
C
d)
D
45.
How many total atoms are in the formula below?
2Pb(SO4)2
2Pb(SO4)2
a)
10
b)
11
c)
22
d)
18
46.
In the notation given, which variable represents the mass number?
a)
A
b)
Z
c)
X
d)
A - Z
47.
Which wave has the highest energy?
a)
A
b)
B
c)
D
d)
E
48.
Which orbital is pictured here?
a)
s
b)
p
c)
d
d)
f
49.
Which orbital is pictured here?
a)
s
b)
p
c)
d
d)
f
50.
Which of the following elements would require the most energy to remove a valence electron?
a)
Lithium
b)
Boron
c)
Nitrogen
d)
Fluorine
51.
Which of the following elements has the lowest first ionization energy?
a)
Lithium
b)
Boron
c)
Nitrogen
d)
Fluorine
52.
Which of the following elements has the largest atomic radius?
a)
Sodium
b)
Potassium
c)
Chlorine
d)
Bromine
53.
Which of the following elements has the largest electronegativity value?
a)
Sodium
b)
Potassium
c)
Chlorine
d)
Bromine
54.
How many significant figures does the following measurement have: 0.002040 m?
a)
6
b)
4
c)
3
d)
2
55.
Round 0.010229 min to four sig figs
a)
1022 min
b)
1023 min
c)
0.01023 min
d)
0.01022 min
56.
What is the measurement 1042 Liters rounded to 2 significant figures?
a)
1040 L
b)
1.1 x 103 L
c)
1.0 x 103 L
d)
1050 L
57.
Solve and round to the correct number of significant figures:
1.3562-mL / 14.32 g
a)
0.09-mL/g
b)
0.097-mL/g
c)
0.0973-mL/g
d)
0.09471-mL/g
58.
Convert 300 meters to centimeters:
a)
3000 cm
b)
0.3 cm
c)
30,000 cm
d)
3 cm
59.
How would you write 4.3756 x 104 in standard form?
a)
437,560,000
b)
0.00043756
c)
43,756
d)
4.3756
60.
Convert 2.5 grams into milligrams.
a)
25 mg
b)
25,000 mg
c)
250 mg
d)
2500 mg
61.
My cup of coffee hold 350 mL (milliliters) how many kL (kiloliters) is my coffee cup
a)
350 kL
b)
35 kL
c)
.35 kL
d)
.00035 kL
62.
A bar of copper has a mass of 216g and a volume of 24cm3. What is the density of copper?
a)
9g/cm3
b)
.11g/cm3
c)
5184g/cm3
d)
322mL
63.
We start with 50 mL in a graduated cylinder and drop in an object. The water rises to 64 mL. What is the volume of this object?
a)
64 mL
b)
64
c)
14 mL
d)
14
64.
Which of the following is correct scientific notation?
a)
20.35 x 104
b)
.2035 x 104
c)
2035 4
d)
2.035 x104
65.
Mg is best described as...
a)
Element
b)
Compound
c)
Mixture
d)
Colloid
66.
Water, H2O, is best described as...
a)
Element
b)
Compound
c)
Homogeneous Mixture
d)
Heterogeneous Mixture
67.
Sugar is best described as...
a)
Element
b)
Compound
c)
Homogeneous Mixture
d)
Heterogeneous Mixture
68.
Gold is best described as...
a)
Element
b)
Compound
c)
Homogeneous Mixture
d)
Heterogeneous Mixture
69.
Pure Air is best described as...
a)
Element
b)
Compound
c)
Homogeneous Mixture
d)
Heterogeneous Mixture
70.
Is melting butter for popcorn a chemical or physical change?
a)
chemical
b)
physical
71.
Is burning wood a chemical or physical change?
a)
chemical
b)
physical
72.
Which of the following is an example of a CHEMICAL change?
a)
Burning a marshmallow
b)
Melting a marshmallow
73.
When you put peroxide on a cut, it bubbles up. This is an example of a ______.
a)
chemical reaction
b)
physical change
74.
leaves changing color
a)
chemical change
b)
physical change
75.
What is the atomic number?
a)
the number of protons
b)
the number of protons and neutrons
c)
the number of neutrons
d)
the number of protons and electrons
76.
What is the mass number?
a)
the number of protons
b)
the number of protons and neutrons
c)
the number of neutrons
d)
the number of protons and electrons
77.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
78.
How many protons does this isotope of titanium have?
a)
48
b)
22
c)
26
d)
70
79.
Do the following atoms belong to the same element? Explain
Aluminum-27
An atom with 14 protons and 13 neutrons
Aluminum-27
An atom with 14 protons and 13 neutrons
a)
Yes because they have the same number of protons
b)
Yes because they have the same mass
c)
No because they have different number of protons
d)
No because they have different number of neutrons
80.
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
81.
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.
82.
Who came up with this model of an atom?
a)
J.J. Thompson
b)
Ernest Rutherford
c)
Neils Bohr
d)
James Chadwick
83.
The majority of an atom's mass exists where?
a)
In the nucleus
b)
In the electron cloud
c)
In the space between the nucleus and the electrons
d)
In the neutrons
84.
How many orbital clouds exist in a d sublevel?
a)
1
b)
7
c)
3
d)
5
85.
If electrons in an atom have the lowest possible energies, the atom is in the
a)
ground state.
b)
inert state.
c)
excited state.
d)
radiation-emitting state.
86.
An atomic emission spectrum is produced when an electron moves from one energy level
a)
into the nucleus.
b)
to another position in the same sublevel.
c)
to a higher energy level.
d)
to a lower energy level.
87.
An individual orbital or cloud space can at most hold how many electrons?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons
88.
A three-dimensional region around a nucleus where an electron may be found is called a(n)
a)
orbit
b)
mitochondria
c)
orbital
d)
nucleus
89.
Identify the element for
[Xe] 6s2 4f14 5d4
[Xe] 6s2 4f14 5d4
a)
Cobalt
b)
Iron
c)
Tungstun
90.
What element has the electron configuration 1s2 2s2?
a)
Li
b)
Be
c)
He
d)
Mg
91.
Valence electrons are defined a the ...........
a)
Electrons farthest away from the nucleus
b)
Electrons closest to the nucleus
c)
Electrons that just come and go - they don't stay with the atom
92.
Each column in the periodic table is called a
a)
period
b)
group
c)
cluster
d)
unit
93.
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
94.
Elements which are shiny, conduct electricity and heat are called
a)
metal
b)
nonmetal
c)
metalloid
d)
nonexistent
95.
A horizontal row of elements in the periodic table.
a)
column
b)
group
c)
period
96.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
97.
Elements in a ..................have similar chemical properties.
a)
period
b)
group
c)
row
98.
The atoms along the staircase are called
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
99.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
100.
As you move left to right across a period, the atomic radius will ....
a)
decrease
b)
increase
c)
stay the same
101.
Why did Mendeleev leave blanks in his periodic table?
a)
forgot elements
b)
left room for elements not yet discovered
c)
placed elements in wrong positions leaving gaps
102.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
103.
Atoms that have a high electronegativity, _______________.
a)
give up their electrons more easily.
b)
hold on to their electrons more tightly.
c)
have more electron shells.
104.
An atom becomes _________ when it gains electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
105.
An atom becomes _______ when it loses electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
106.
What is the formula for magnesium phosphide?
a)
Mg3P2
b)
Mg2P3
c)
Mg2(PO4)3
d)
Mg3(PO4)2
107.
The chemical formula of potassium iodide is
a)
KI
b)
PI
c)
KI₂
d)
K₂I
108.
How do the following two elements bond together?
Al3+ O2-
Al3+ O2-
a)
AlO
b)
Al2O3
c)
Al3O6
d)
Al3O2
109.
What is the formula for iron(III) chloride?
a)
FeCl
b)
Fe3Cl
c)
FeCl2
d)
FeCl3
110.
What is the formula for aluminum hydroxide?
a)
AlOH
b)
AlOH3
c)
Al(OH)3
d)
(Al)3OH
111.
What is the correct formula for ammonium fluoride?
a)
NH4F
b)
FNH4
c)
(NH4)7F
d)
NHF
112.
What is the correct formula for nickel (II) phosphate?
a)
NiPO4
b)
Ni3(PO4)2
c)
Ni2(PO4)2
d)
Ni3P2
113.
What is the correct formula for magnesium oxide?
a)
MgO
b)
Mg2O2
c)
Mg(OH)2
d)
Mg2OH
114.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal and 1 Metal
c)
2 Metals
d)
2 Noble Gases
115.
Which of the following is NOT formed by a covalent bond?
a)
K2S
b)
H2O
c)
I2
d)
CO2
116.
What do we call a covalent bond where electrons are shared UNEVENLY or UNEQUALLY?
a)
Ionic
b)
Polar Covalent
c)
Nonpolar Covalent
d)
Van der Waals Force
117.
An explanation of an event that is based on repeated observations and experiments is a?
a)
theory
b)
law
c)
explanation
d)
opinion
118.
A _________ has two or more different types of matter that are near one another, but the matter does NOT chemically combine.
a)
mixture
b)
compound
c)
property
d)
atom
119.
A _________ is a substance made of two or more DIFFERENT elements chemically combined.
a)
mixture
b)
compound
c)
substance
120.
This group typically gains or shares one electron.
a)
Halogens
b)
Noble Gases
c)
Alkaline Earth Metals
d)
Alkali Metals
121.
The formula for dinitrogen pentoxide is:
a)
NO
b)
N5O
c)
2NO
d)
N2O5
122.
SnS2
a)
Tin (I) sulfide
b)
Tin (II) sulfide
c)
Tin (III) sulfide
d)
Tin (IV) sulfide
123.
Covalent bonds...
a)
are normally between 2 nonmetals
b)
share electrons
c)
form molecules
d)
all of the above
124.
What is released in a combustion reaction?
a)
Oxygen and water
b)
Oxygen and carbon dioxide
c)
Carbon dioxide and water
d)
Water and hydrogen
125.
Which of these is a double displacement reaction?
a)
2Mg + O2 > 2MgO
b)
Mg + 2HCl > H2 + MgCl2
c)
MgI2 + K2CO3 > MgCO3 + 2Kl
d)
MgCO3 > MgO + CO2
126.
This picture represents
a)
Synthesis
b)
Double Replacement
c)
Single Replacement
d)
Decomposition
127.
This image represents
a)
a double replacement reaction
b)
a decomposition reaction
c)
a single replacement reaction
d)
a complex compound reaction
128.
Compounds break down into simpler substances in this type of reaction.....
a)
Double Replacement
b)
Single Replacement
c)
Synthesis
d)
Decomposition
129.
Calculate 12.34 × 1.234 × 0.1234
a)
1.87908
b)
1.879
c)
1.9
d)
1.8790809
130.
Why are noble gases virtually nonreactive?
a)
They are all gases
b)
8 Valence electrons
c)
Last element in each period
d)
Because they are nonmetals
131.
This could be the dot diagram of
a)
Ne
b)
H
c)
C
d)
F
132.
CxHy +O2 --> H2O + CO2
a)
Decomposition
b)
Double replacement
c)
Combustion
d)
Single Replacement
133.
One element replaces another in a compound.
a)
Synthesis
b)
Combustion
c)
Single Replacement
d)
Double Replacement
134.
The following reaction is an example of what reaction type?
CoCO3 → CoO + CO2
CoCO3 → CoO + CO2
a)
Synthesis
b)
Decomposition
c)
Single Replacement
d)
Double Replacement
135.
Si + S8 --> Si2S4
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Double replacement
136.
KOH + H3PO4 --> K3PO4 + H2O
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Double replacement
137.
Pb(NO3)2 --> PbO + NO2 + O2
a)
Synthesis (combination)
b)
Decomposition
c)
Single replacement
d)
Combustion
138.
What are the products in the following chemical equation?
2H2 + O2 --> 2H2O
2H2 + O2 --> 2H2O
a)
H2
b)
O2
c)
2H2 + O2
d)
2H2O
139.
What are always the product(s) for the combustion of a hydrocarbon?
a)
O2
b)
Acids and Bases
c)
H2O and CO2
d)
H2 and C
140.
What is the left part of a chemical equation called?
H2 + O → H2O
H2 + O → H2O
a)
Reactants
b)
Products
c)
Yields
d)
Chemical Equation
141.
Breaking down a substance into simpler substances
a)
Displacement
b)
Synthesis
c)
Decomposition
d)
Oxidation
142.
Combining substances to form a new substance
a)
Displacement
b)
Synthesis
c)
Decomposition
d)
Oxidation
143.
_AgNO3 + _Cu →_Cu(NO3)2 + _Ag
a)
2 AgNO3 + 2 Cu → 3 Cu(NO3)2 + 1 Ag
b)
2 AgNO3 + 1 Cu → 1 Cu(NO3)2 + 2 Ag
c)
1 AgNO3 + 2 Cu → 2 Cu(NO3)2 + 1 Ag
d)
3 AgNO3 + 2 Cu → 3 Cu(NO3)2 + 2 Ag
144.
_BaS + _PtF2 → _BaF2 + _PtS
a)
1 BaS + 1 PtF2 → 1 BaF2 + 1 PtS
b)
4 BaS + 2 PtF2 → 1 BaF2 + 1 PtS
c)
1 BaS + 2 PtF2→ 2 BaF2 + 2 PtS
d)
1 BaS + 3 PtF2 →1 BaF2 + 2 PtS
145.
_K + _Cl2 →_KCl
a)
2 K + 16 Cl2 → 8 KCl
b)
2 K + 1 Cl2 → 2 KCl
c)
3 K + 4 Cl2 → 3 KCl
d)
1 K + 1 Cl2 →1 KCl
146.
Balance this equation, Al2O3 ---> Al + O2
a)
Cannot be balanced
b)
2Al2O3 ---> 2Al + 3O2
c)
2Al2O3 ---> 4Al + 3O2
d)
3Al2O3 ---> 2Al + O2
147.
In every balanced chemical equation, each side of the equation has the same number of ____.
a)
coefficients
b)
moles
c)
molecules
d)
atoms of each element
148.
_AlBr3 + _K2SO4 → _KBr + _Al2(SO4)3
a)
6 AlBr3 + 1 K2SO4 → 6 KBr + 1 Al2(SO4)3
b)
2 AlBr3 + 3 K2SO4 → 6 KBr + 1 Al2(SO4)3
c)
1 AlBr3 + 1 K2SO4 → 2 KBr + 3 Al2(SO4)3
d)
2 AlBr3 + 3 K2SO4 → 1 KBr + 2 Al2(SO4)3
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