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WorksheetsFinal Review
Total questions: 133
Worksheet time: 3hrs 18mins
Name
Class
Date
1.
The law of conservation of mass states that mass cannot be
a)
burned
b)
changed in form
c)
created or destroyed
d)
heated or cooled
2.
The law of conservation of mass states that mass cannot be
a)
burned
b)
changed in form
c)
created or destroyed
d)
heated or cooled
3.
Unlike a gas, a plasma
a)
has no mass
b)
has no definite shape
c)
has no definite volume
d)
conducts electric current because it is charged
4.
What type of property can be observed without changing the identity of the substance?
a)
Physical Property
b)
Chemical Property
c)
Conductivity Property
d)
Reactivity Property
5.
_________ is anything that takes up space and has mass.
a)
Inertia
b)
Matter
c)
Viscosity
d)
Malleability
6.
the smallest unit of matter is called
a)
at atom
b)
a molecule
c)
a compound
d)
a pure substance
7.
The three main subatomic particles are electrons, protons and ____________.
a)
photons
b)
neurons
c)
neutrons
d)
quarks
8.
What is an example of a Chemical change?
a)
Ripped paper
b)
boiled egg
c)
cracked egg
d)
sugar in water
9.
Which is a physical change?
a)
burning match
b)
vinegar in baking soda
c)
melting butter
d)
cooking an egg
10.
Which of the following is a sign that a chemical reaction has occurred?
a)
change in shape
b)
melting
c)
formation of a gas
d)
dissolving
11.
Which is a Chemical property?
a)
Thermal Conductivity
b)
Density
c)
Malleability
d)
Flammability
12.
Salt dissolves in water
a)
physical Change
b)
chemical change
13.
milk sours (goes bad)
a)
physical change
b)
chemical change
14.
water freezes at 0⁰C
a)
physical change
b)
chemical change
15.
What is a mixture?
a)
elements chemically combined
b)
a combination of different things
c)
it is found on the Periodic Table
d)
it is made of chemical
16.
What type of mixture is this?
a)
heterogeneous
b)
homogeneous
17.
What type of mixture is this?
a)
heterogeneous
b)
homogeneous
18.
Elements and compounds are always ___.
a)
pure
b)
mixed
19.
Which list is made of mixtures?
a)
soil, water, soup
b)
carbon dioxide, soil, soup
c)
salt, water, air
d)
atoms, cereal, pizza
20.
convert 9 km to mm
a)
900,000
b)
9,000,000
c)
9,000
d)
90,000
21.
convert 650 m to km
a)
6.5
b)
0.65
c)
65
d)
0.065
22.
If a pencil was 7 centimeters long, how many millimeters long would it be?
a)
70
b)
700
c)
7,000
d)
70,000
23.
Fill in the blank: 1g = _________ mg.
a)
.1
b)
10
c)
100
d)
1000
24.
What is the density of a 10g object with the volume of 4mL?
a)
40g/mL
b)
0.4g/mL
c)
2.5g/mL
d)
6g/mL
25.
What is the correct ascending order of the following terms: hecto, centi, deci, base, milli, kilo, deka?
a)
milli, centi, deka, base, deci, hecto, kilo
b)
milli, centi, deci, base, deka, hecto, kilo
c)
kilo, deka, hecto, base, centi, deci, milli
d)
deka, kilo, centi, deci, base, milli, hecto
26.
How many sig figs in the number 100?
a)
1
b)
2
c)
3
d)
As many as you want there to be.
27.
Calculate 12.34 × 1.234 × 0.1234
a)
1.87908
b)
1.879
c)
1.9
d)
1.8790809
28.
What is the correct number of sig figs in 10500
a)
3
b)
2
c)
4
d)
5
29.
Which value has only 4 significant digits?
a)
6.930
b)
0.450
c)
8450
d)
0.392
30.
How would you write 564,000,000 in scientific notation?
a)
5.64 x 10-7
b)
5.64 x 106
c)
5.64 x 108
d)
56.4 x 107
31.
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
32.
Express the following in scientific notation with 3 sig figs:
19,999,999,999
19,999,999,999
a)
1.99 X 1010
b)
2.00 X 1010
c)
2.00 x 10-10
d)
1.99 x10-10
33.
These particles orbit around the nucleus of an atom. What are they called?
a)
electrons
b)
protons
c)
neutrons
d)
photons
34.
From the diagram, which particles are indicated with the arrow?
a)
electrons and protons
b)
protons and neutrons
c)
electrons and neutrons
d)
photons and nucleons
35.
The sum of the number of protons and the number of neutrons is called the _____
a)
atomic number
b)
mass number
c)
isotope number
d)
average weight
36.
number of neutrons = _____
a)
atomic number - mass number
b)
isotope number - atomic weight
c)
mass number - atomic weight
d)
mass number - atomic number
37.
The middle of the atom, which contains protons and neutrons, is called _____
a)
the shell
b)
the nucleus
c)
the cell
d)
the control center
38.
Which subatomic particle has a relative charge of +1?
a)
the proton
b)
the neutron
c)
the electron
d)
the photon
39.
How many neutrons does this element have?
a)
30
b)
26
c)
55.847
d)
56
40.
How many protons does this element have?
a)
74
b)
183.84
c)
184
d)
110
41.
What is this element's name?
a)
74
b)
W
c)
Tungsten
d)
183.84
42.
What is the Element's atomic mass?
a)
Fe
b)
26
c)
55.847
d)
Iron
43.
How many neutron are in the atom "K"?
a)
7
b)
2
c)
39
d)
20
44.
Which statement best describes an electron?
a)
Smaller mass than a proton and a negative charge
b)
Smaller mass than a proton and a positive charge
c)
Greater mass than a proton and a negative charge
d)
Greater mass than a proton and a positive charge
45.
What period and group is Silver (Ag)?
a)
Period 2, Group 1
b)
Period 3, Group 16
c)
Period 5, Group 11
d)
Period 2, 14
46.
The period for Bromine is ___________.
a)
3
b)
2
c)
4
47.
Beryllium is in group number______.
a)
Group 2
b)
Group 3
c)
Group 4
d)
Group 7
48.
What is the correct electron configuration for Boron
a)
1s22s22p1
b)
1s22s22p2
c)
1s22s11p1
d)
1s22s12p1
49.
Which element is depicted from this atomic orbital diagram?
a)
Carbon
b)
Nitrogen
c)
Oxygen
d)
Phosphorus
50.
What is the correct electron configuration for Selenium
a)
1s22s22p63s23p64s24d104p4
b)
1s22s22p63s23p64s23d104p4
c)
1s22s22p63s23p64s23d104p3
d)
1s22s22p63s23p64s24d104p43
51.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
52.
1. What is the shape of an s orbital?
a)
sphere
b)
dumbbell
c)
double dumbbell
d)
TOO COMPLEX TO KNOW IT.
53.
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
54.
In the modern periodic table elements are arranged by:
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
55.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
56.
In what section would Transition Metals be found?
a)
orange
b)
light blue
c)
blue
d)
white
57.
Elements on the left side of the periodic tables are
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
58.
What is the name of group 17
a)
halogens
b)
nobles gases
c)
alkali metals
d)
alkaline earth metals
59.
How many Valence electrons does Iodine Have?
a)
6
b)
8
c)
7
d)
1
60.
When an atom loses a valence electron, it becomes a(n) _____________ ion.
a)
positive
b)
negative
c)
neutral
d)
polyatomic
61.
When an atom gains a valence electron, it becomes a(n) _____________ ion.
a)
positive
b)
negative
c)
neutral
d)
polyatomic
62.
If an element has 3 valence electrons, what charge will likely form on its ion ? Hint: It will lose those electrons. What happens to the charge when it loses 3 electrons?
a)
+3
b)
+5
c)
-3
d)
-5
63.
Nitrogen will ____ valence electrons when forming an ionic bond.
a)
gain 1
b)
lose 1
c)
gain 3
d)
lose 3
64.
Ionic bonds form between two ions that have
a)
ionic compounds
b)
negative charges
c)
positive charges
d)
opposite charges
65.
Atoms that gain & lose electrons are called _________
a)
ions
b)
isotopes
c)
radioactive
d)
corrosive
66.
Where are the metalloids / semimetals located on the periodic table?
a)
Blue
b)
Red
c)
Green
67.
What happens when an atom loses an electron?
a)
It becomes Negatively Charged
b)
It remains neutral because the proton also leaves.
c)
It becomes Positively Charged
d)
It stays the same.
68.
Isotopes have different numbers of
a)
protons
b)
neutrons
c)
electron
d)
properties
69.
How many neutrons does the isotope of lithium-8 have?
a)
8
b)
3
c)
4
d)
5
70.
Atoms of the same element must always have the same number of _________
a)
electrons
b)
neutrons
c)
isotopes
d)
protons
71.
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
72.
What is the formula for aluminum fluoride?
a)
AlF
b)
Al2F3
c)
AlF3
d)
Al3F2
73.
What is the formula for manganese(III) oxide?
a)
MgO
b)
Mg2O3
c)
MnO
d)
Mn2O3
74.
What is the name of Fe(OH)3
a)
iron (II) hydroxide
b)
iron (III) hydroxide
c)
iron trihydroxide
d)
iron hydroxide
75.
From the following ionic compounds, choose the name-formula pair that is not correctly matched.
a)
sodium sulfide Na2S
b)
ammonium nitrate
NH4NO3
NH4NO3
c)
sodium sulfate
Na2SO3
Na2SO3
d)
calcium oxide CaO
76.
A chemical bond resulting from the electrostatic attraction between positive and negative ions is called a(n)
a)
covalent bond.
b)
ionic bond.
c)
charged bond.
d)
dipole bond.
77.
The chemical bond formed when two atoms share electrons is called a(n)
a)
ionic bond.
b)
orbital bond.
c)
Lewis structure.
d)
covalent bond.
78.
Which is incorrect?
a)
A
b)
B
c)
C
d)
D
79.
When a nonmetal gains electrons, it becomes this type of ion.
a)
Anion
b)
Cation
80.
What is the formula for the compound, phosphorus trifluoride?
a)
PF3
b)
PhF3
c)
PO4F3
d)
PF
81.
What is the name of the compound, ammonium chloride?
a)
AmCl2
b)
(NH4)2ClO3
c)
NH4Cl
d)
NH4Cl2
82.
What is the correct formula for the compound, tin (II) nitrate
a)
Sn2NO3
b)
SnNO2
c)
Sn(NO3)2
d)
SnNO3
83.
Is the following ionic or covalent:
CS2
CS2
a)
Ionic
b)
Covalent
84.
Is the following compound ionic or covalent:
AlCl3
AlCl3
a)
ionic
b)
covalent
85.
Name the following compound:
Co2O3
Co2O3
a)
cobalt oxide
b)
dicobalt trioxide
c)
cobalt (II) oxide
d)
cobalt (III) oxide
86.
Name the following compound:
SeF7
SeF7
a)
selenium hexafluoride
b)
monoselenium heptafluoride
c)
selenium fluoride
d)
selenium heptafluoride
87.
Which of the following is NOT an ionic compound:
a)
CaO
b)
NaOH
c)
BaCl2
d)
Br2
88.
Which of the following combinations would need roman numerals in the name?
a)
potassium + fluorine
b)
beryllium + oxygen
c)
boron + iodine
d)
silver + oxygen
89.
What is the name of this polyatomic ion: MnO42-
a)
permanganate
b)
manganate
c)
manganese oxide
d)
manganese (IV) oxide
90.
What is the formula for silicon dioxide?
a)
SO2
b)
NaO2
c)
SiO2
d)
SiO
91.
When naming ionic compounds with transition metals you need to include roman numerals to show the _____ of the metal..
a)
atomic number
b)
mass number
c)
charge
d)
ionization energy
92.
What is the formula for nitric acid?
a)
HNO2
b)
HNO3
c)
HNO4
d)
H2NO3
93.
What is the formula for hydrochloric acid?
a)
HCl
b)
HClO
c)
H3ClO3
d)
HClO3
94.
Name this acid: H2S
a)
Hydrosulfuric Acid
b)
Sulfurous Acid
c)
Sulfuric Acid
d)
Hyposulfite Acid
95.
What is the name of the acid that has the formula H2CO3?
a)
hydrocarbonic acid
b)
hydrocarbonate acid
c)
carbonic acid
d)
carbonate acid
96.
Name the acid: H2SO3
a)
Sulfurous Acid
b)
Sulfuric Acid
c)
Hydrosulfuric Acid
d)
Hydrosulfurous Acid
97.
C5H10O4 + O2 --> CO2 + H2O
a)
Decomposition
b)
Single Replacement
c)
Combustion
d)
Double Replacement
98.
Na + CaF2 --> Ca + NaF
a)
Decomposition
b)
Single Replacement
c)
Synthesis
d)
Double Replacement
99.
AgF + CaCl2 --> AgCl + CaF2
a)
Decomposition
b)
Single Replacement
c)
Synthesis
d)
Double Replacement
100.
Fe + O2 --> Fe2O3
a)
Decomposition
b)
Single Replacement
c)
Synthesis
d)
Double Replacement
101.
Mg3(PO4)2 + H2 --> Mg + H3PO4
a)
Decomposition
b)
Single Replacement
c)
Synthesis
d)
Double Replacement
102.
Al2S3 --> Al + S8
a)
Decomposition
b)
Single Replacement
c)
Synthesis
d)
Double Replacement
103.
C5H10O4 + O2 --> CO2 + H2O
a)
Synthesis
b)
Combustion
c)
Single Replacement
d)
Double Replacement
104.
What symbol is used to indicate a precipitation
a)
(p)
b)
(s)
c)
(g)
d)
(aq)
105.
Two Reactants and One Product
a)
Decomposition
b)
Synthesis
c)
Combustion
d)
Single Replacement
106.
In this image, what are the information in red is called the_______.
a)
Product
b)
Reactant
c)
Chemical Subscript
107.
In this image, what are the information to the right of the arrow (in black) is called the_______.
a)
Product
b)
Reactant
c)
Chemical Subscript
108.
Read the following chemical formula: C6H12O6. How many hydrogen atoms are in the formula?
a)
12
b)
6
c)
4
109.
The law of conservation of mass states that....
a)
Matter can be made
b)
Matter can be destroyed
c)
Matter can neither be made or destroyed
110.
Is this balanced?...
Al + O2 --> 2Al2O3
Al + O2 --> 2Al2O3
a)
Yes!
b)
NO!
111.
In the equation, 2Mg + O2 ---> 2MgO, which are the reactants?
a)
Mg and O
b)
MgO
c)
Mg and MgO
d)
O and MgO
112.
At the end of chemical reactions, what is the total mass of the reactants compared to the total mass of the products?
a)
the product is doubled
b)
the product is half the mass of the reactants
c)
the mass is the same
d)
the mass changes depending on the reaction
113.
Why is the following chemical equation not balanced?
H2 + O2 --> H2O
H2 + O2 --> H2O
a)
each side of the equation has a different number of oxygen atoms
b)
each side of the equation has a different number of hydrogen atoms
c)
each side has the same mass
114.
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
115.
How many atoms of aluminum are on each side of the following equation: 4Al + 3O2 --> 2Al2 O3
a)
2
b)
6
c)
1
d)
4
116.
When balancing equations a ____ can be placed to the left of a formula of a substance to make the equations balanced
a)
charge
b)
subscript
c)
random number
d)
coefficient
117.
What is the little number after an element in a chemical equation called.
Example: H2
Example: H2
a)
Coefficient
b)
Subscript
c)
Atom
d)
Equation
118.
Is this equation balanced
HgO --> 2Hg + O2
HgO --> 2Hg + O2
a)
It is balanced
b)
It is not balanced
119.
Determine the molar mass for CCl4
a)
153.8 g/mol
b)
47.54 g/mol
c)
189.35 g/mol
d)
82.9 g/mol
120.
What is the molar mass of calcium hydroxide (Ca(OH)2)?
a)
74.10 g/mole
b)
57.12 g/mole
c)
58.19 g/mole
d)
none of the above
121.
What is the percent composition of a compound that contains 40.8 g carbon and 54.4 g oxygen?
a)
42.9 % carbon; 57.1% oxygen
b)
57.1 % carbon; 42.9 % oxygen
c)
40.8 % carbon; 54.4 % oxygen
d)
54.4 % carbon; 40.8% oxygen
122.
What do we call 6.022 x 1023?
a)
Avogadro's Number
b)
Avocado Number
c)
A dozen
d)
Louis
123.
What are the units for molar mass?
a)
grams
b)
amu
c)
grams/mole
d)
liters
124.
Which of the following dimensional analysis setups will correctly convert 2.50 moles of sodium to grams of sodium?
a)
A
b)
B
c)
C
d)
D
125.
Based on the info below, solve for the molecular formula:
Empirical formula = NO
Molecular formula mass = 59.98g
Empirical formula = NO
Molecular formula mass = 59.98g
a)
NO
b)
N2O3
c)
N2O2
d)
N4O4
126.
You are given the following percentages: 40.05% S and 59.95% O. Find the empirical formula for these elements. (keep two decimal places throughout calculations)
a)
SO
b)
SO2
c)
SO3
d)
SO4
127.
What is the molecular formula for a compound with the empirical formula: K2SO4 and a molecular mass of 696g.
a)
K2SO4
b)
K8SO16
c)
K8S4O8
d)
K8S4O16
128.
Whats the empirical formula of a molecule containing 18.7% of Lithium, 16.3% of Carbon and 65.0% of oxygen?
a)
CO2Li3
b)
Li2CO3
c)
Li3CO2
d)
LiCO5
129.
2H2 + O2 → 2H2O
How many moles of water can be produced if 8 moles H2 are used?
How many moles of water can be produced if 8 moles H2 are used?
a)
4 moles
b)
8 moles
c)
16 moles
d)
2 moles
130.
How many grams are in 7.8 moles of NaCl?
a)
476grams
b)
460 grams
c)
452 grams
d)
462 grams
131.
Using the following equation:
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from 6 moles H2?
Fe2O3(s) + 3H2(g) → 2Fe(s) + 3H2O(l)
How many moles of iron can be made from 6 moles H2?
a)
4 moles Fe
b)
6 moles Fe
c)
9 moles Fe
d)
2 moles Fe
132.
Using the following equation:
4P + 5O2 --> P4O10
What mass of phosphorus will be needed to produce 3.25 mol of P4O10
4P + 5O2 --> P4O10
What mass of phosphorus will be needed to produce 3.25 mol of P4O10
a)
403 g P
b)
101 g P
c)
0.420 g P
d)
0.0262 g P
133.
Using the following equation:
2I2(s) + KIO3(aq) + 6HCl(aq) --> 5ICl(aq) + KCl(aq) + 3H2O(l)
Calculate how many grams of iodine are needed to prepare 28.6 grams of ICl by this reaction.
2I2(s) + KIO3(aq) + 6HCl(aq) --> 5ICl(aq) + KCl(aq) + 3H2O(l)
Calculate how many grams of iodine are needed to prepare 28.6 grams of ICl by this reaction.
a)
17.88 g I2
b)
34.77 g I2
c)
29.50 g I2
d)
5.61 g I2
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