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WorksheetsChemistry Semester 1 Review
Total questions: 106
Worksheet time: 1hrs 17mins
Name
Class
Date
1.
A gas
a)
has a definite shape but no definite volume
b)
has a definite volume but no definite shape
c)
has fast-moving particles
2.
At higher temperatures
a)
particles in an object have less energy
b)
particles in an object move faster
c)
a gas contracts
3.
Melting
a)
liquid to solid
b)
solid to liquid
c)
solid to gas
d)
gas to liquid
4.
Has a definite volume but no shape.
a)
Liquid
b)
Solid
c)
Gas
d)
Fluid
5.
Volume is the amount of _______ taken up by an object.
a)
water
b)
space
c)
mL
d)
cm3
6.
How many mm are in 40 cm?
a)
400 mm
b)
40 mm
c)
4000 mm
d)
0 mm
7.
What is the scientific notation of 7X107
a)
7
b)
70,000,000
c)
70,000
d)
7,000,000,000
8.
A rule or principle that describes what happens in nature is a?
a)
observation
b)
witnessing
c)
naturalist
d)
law
9.
An explanation of an event that is based on repeated observations and experiments is a?
a)
theory
b)
law
c)
explanation
d)
opinion
10.
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
11.
A _________ is a substance made of two or more DIFFERENT elements chemically combined.
a)
mixture
b)
compound
c)
substance
12.
A new substance is formed when you are working with compounds because a _________ reaction occurs.
a)
physical
b)
chemical
13.
A mixture can be separated by ________ means.
a)
physical
b)
chemical
14.
Which of the following is NOT a mixture?
a)
NaCl + H2O
b)
C6H12O6 + H2O
c)
C6H12O6
d)
SiO2 +H2O
15.
What units do you use to measure mass?
a)
inches
b)
feet
c)
feet
d)
grams or kilograms
16.
What unit is used to measure the volume of a liquid or an irregular object?
a)
milliters
b)
centimeters cubed
c)
inches
d)
grams
17.
Ernst Rutherford discovered which part of the atom throught the use of gold foil?
a)
Proton
b)
Neutron
c)
Electron
d)
Orbitals
18.
Ernst Rutherford discovered that the atom is
a)
Compound of mostly empty space with negative electrons surrounding a positive nucleus
b)
A highly dense sphere of positive
c)
A highly dense sphere of a negative space
d)
Composed mostly of empty space with positive electrons surrounding a negative nucleus
19.
Bohr's Planetary Model represented what?
a)
Electrons spin around the nucleus in a fixed orbital
b)
Protons spin around the nucleus in fixed orbitals
c)
An atom is a round sphere shaped like a planet
d)
Every atom is a little planet
20.
Which model did J.J Thomson create?
a)
Planetary Model
b)
Plum Pudding Model
c)
Atomic Model
d)
Molecular Model
21.
If an atom has an equal amount of Protons and electrons, what will its’ charge be?
a)
Positive
b)
Negative
c)
Neutral
d)
Infinite
22.
If an atoms has more electrons that Protons, what will its’ charge be?
a)
Positive
b)
Negative
c)
Super Negative
d)
Super Positive
23.
Which determines the mass of an element?
a)
Protons
b)
Neutrons
c)
Electrons
d)
Only Protons and Neutrons
24.
This group has two valence electrons.
a)
Alkali Metals
b)
Alkali Earth Metals
c)
Lactinides
d)
Oxygen Family
25.
This group typically gains or shares one electron.
a)
Halogens
b)
Noble Gases
c)
Alkaline Earth Metals
d)
Alkali Metals
26.
Aluminum is this type of element.
a)
Metal
b)
Metalloid
c)
Non-Metal
27.
What is an isotope?
a)
A charged atom
b)
A noble gas
c)
A variation of atoms of the same element
d)
A metal
28.
The lowest allowable energy state of electrons.
a)
principle energy level
b)
atomic orbital
c)
energy sublevel
d)
ground state
29.
write the electron config for iron (fe)
a)
1s2 2s2 2p6 3s2 3p6 4s2 3d6
b)
1s2 2s2 2p6 3s2 3p6 4s2 4d6
c)
1s2 2s2 3s2 4s2 4d6
d)
1p2 2p2 2s6 3p2 3s6 4p2 4d6
30.
write the abbreviated electron config for Strontium (Sr)
a)
[kr] 3s2
b)
[kr] 4s2
c)
[kr] 5s2
d)
[ar] 5s2
31.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
32.
How many types of orbitals are there?
a)
5
b)
4
c)
6
d)
2
33.
What are the types of orbitals?
a)
S, P, D, F
b)
A, F, D, S
c)
E, L, K, M
d)
M, A, C, K
34.
___orbital has 14 total electrons.
a)
S
b)
P
c)
F
d)
D
35.
A vertical column of elements in the periodic table arranged in order of increasing atomic number; also called a family.
a)
period
b)
transition element
c)
group
d)
representative element
36.
A highly reactive group 17 element.
a)
halogen
b)
metalloid
c)
noble gas
d)
alkali metal
37.
An atom or bonded group of atoms with a positive or negative charge.
a)
halogen
b)
electronegativity
c)
ion
d)
ionization energy
38.
The energy required to remove an electron from a gaseous atom.
a)
ions
b)
octet rule
c)
periodic law
d)
ionization energy
39.
A horizontal row of elements in the modern periodic table.
a)
group
b)
period
c)
lanthanide series
d)
actinide series
40.
States that when the elements are arranged by increasing atomic number, there is a periodic repetition of their properties.
a)
octet rule
b)
periodic law
c)
ionization energy
d)
electronegativity
41.
An anion is a negatively charged ion.
a)
True
b)
False
42.
Which of the following will have a larger ionic radius than atomic radius?
a)
Kr
b)
S
c)
V
d)
K
43.
Nonmetals form cations.
a)
True
b)
False
44.
Which of the following will lose a shell when it forms an ion?
a)
Ca
b)
P
c)
Cl
d)
Xe
45.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
46.
Which of the following sets of elements are ranked in order of DECREASING electronegativity?
a)
He, F, S, As
b)
F, S, As, Sn
c)
In, Ge, P, O
d)
As, S, F, He
47.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
48.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
49.
What is the charge on aluminum when it forms an ion?
a)
-1
b)
+1
c)
+3
d)
-3
50.
Which particle is negatively charged?
a)
proton
b)
atom
c)
neutron
d)
electron
51.
How do the following two elements bond together?
Al3+ O2-
Al3+ O2-
a)
AlO
b)
Al2O
c)
Al3O2
d)
Al2O3
52.
How do the following two elements bond together?
Na1+ F1-
Na1+ F1-
a)
NaF
b)
NaF3
c)
Na3F
d)
Na1F2
53.
How do the following two elements bond together?
Pb4+ O2-
Pb4+ O2-
a)
PbO
b)
Pb2O3
c)
PbO2
d)
Pb3O2
54.
The simplest ratio of ions represented in an ionic compound.
a)
formula unit
b)
ionic compound
c)
chemical bond
d)
metallic bond
55.
The electrostatic force that holds oppositely charged particles together in an ionic compound.
a)
ionic bond
b)
formula unit
c)
chemical bond
d)
metallic bond
56.
An ion made up of two or more atoms bonded together that acts as a single unit with a net charge.
a)
polyatomic ion
b)
oxyanion
c)
monatomic ion
d)
cation
57.
Based on the Lewis Dot structure, which of the following has one electron available for bonding?
a)
Strontium
b)
Chlorine
c)
Selenium
d)
Boron
58.
How many bromine atoms can bond with one boron atom?
a)
1
b)
2
c)
3
d)
4
59.
AlCl3 is called...
a)
aluminum chlorine
b)
aluminide chloride
c)
aluminum trichloride
d)
aluminum chloride
60.
What is the formula for calcium phosphide?
a)
CaP
b)
Ca2P3
c)
Ca3P2
d)
Ca2P
61.
The formula for magnesium cyanide is...
a)
Mg(CN)2
b)
MgCN2
c)
MgCN
d)
(Mg)2CN
62.
How many dots would a Lewis Dot structure of Helium have?
a)
1
b)
2
c)
8
d)
0
63.
The compound created from the bond between lithium and oxygen would be called...
a)
Lithium oxate
b)
Lithium oxide
c)
Dilithium oxide
d)
Lithium peroxide
64.
Pb(NO3)2
a)
Lead nitrate
b)
Lead (II) nitrate
c)
Lead nitrite
d)
Lead (I) nitrate
65.
copper (II) nitride
a)
CuN
b)
Cu2N
c)
Cu3N2
d)
Cu(NO3)2
66.
Nickel (II) oxide
a)
Ni2O3
b)
NiO2
c)
Ni2O
d)
NiO
67.
ammonium sulfate
a)
NH4SO4
b)
NH4(SO4)2
c)
(NH4)2SO4
d)
NH4SO3
68.
SnS2
a)
Tin (I) sulfide
b)
Tin (II) sulfide
c)
Tin (III) sulfide
d)
Tin (IV) sulfide
69.
The formula for dinitrogen pentoxide is:
a)
NO
b)
N5O
c)
2NO
d)
N2O5
70.
H2SO4 is:
a)
Sulfur Acid
b)
Sulfite Acid
c)
Sulfuric Acid
d)
Hydrosulfic Acid
71.
H2O is a _______ compound
a)
Covalent
b)
Ionic
c)
Acidic
d)
Metallic
72.
Na2CO3 · 10H2O is known as sodium sulfate ______
a)
Hydroxide
b)
Hydrate
c)
Decahydrate
d)
None of the above
73.
The molecular formula for a compound is the...
a)
lowest possible ratio
b)
actual makeup of the molecule
c)
formula to calculate the density of an atom
d)
formula to calculate the solubility of an atom
74.
A compound is a hydrate when it...
a)
is composed of only hydrogen and oxygen
b)
is a state of water
c)
traps water inside of the compound
d)
repels water from the compound
75.
What is the molar mass of H2O?
a)
12.01g
b)
16.00g
c)
18.02g
d)
24.22g
76.
What is the molar mass of CO2?
a)
12.01
b)
16.00
c)
32.12
d)
44.01
77.
In a prefix, tri means...
a)
2
b)
3
c)
4
d)
5
78.
Covalent bonds...
a)
are normally between 2 nonmetals
b)
share electrons
c)
form molecules
d)
all of the above
79.
Acids must contain:
a)
carbon
b)
oxygen
c)
hydrogen
d)
helium
80.
Ionic bonds...
a)
destroy electrons
b)
form positively charged salts
c)
create full outer shells
d)
all of the above
81.
Draw the Lewis structure for OF2 and determine the number of lone pairs on the central atom.
a)
none
b)
1
c)
2
d)
it's ionic
82.
How many grams would 4.13x1021 molecules of diatomic nitrogen gas weigh?
a)
0.0961
b)
0.192
c)
14.007
d)
28.014
83.
How many moles of copper (II) chlorate contain 1.45x1021 formula units?
a)
8.73x1044
b)
1.20x1024
c)
0.00241
d)
1.45
84.
How many molecules are in 9.4 moles of AlCl3?
a)
5.66
b)
5.66x1024
c)
0.705
d)
1.25x1023
85.
Which of the following would contain the least number of molecules?
a)
2.4 moles of (NH4)2CO3
b)
4.2 moles Li3P
c)
10 moles H2
d)
2.02 moles CuPO4
86.
What is the molar mass of B2(CO3)3?
a)
81.632 g/mol
b)
94.842 g/mol
c)
38.822 g/mol
d)
201.648 g/mol
87.
What is the molar mass of sodium?
a)
11
b)
22.990
c)
45.98
d)
3
88.
What are the units for molar mass?
a)
grams
b)
amu
c)
grams/mole
d)
liters
89.
Fluorine is diatomic. What is the molar mass of fluorine gas?
a)
18.998 g/mol
b)
37.996 g/mol
c)
9 g/mol
d)
18 g/mol
90.
What is the difference between empirical and molecular formulas?
a)
Empirical shows the simplest whole number ratio of elements, molecular shows the real number of atoms.
b)
Empirical shows the real number of atoms, molecular shows the simplest whole number ratio of elements.
c)
They are never the same.
d)
Empirical is typically larger than molecular.
91.
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
92.
A compound is found to have 52.0 g of zinc (Zn), 9.6 g of carbon (C), and 38.4 g of oxygen (O). What is the empirical formula?
a)
Zn2(CO3)2
b)
Zn2C2O6
c)
ZnCO
d)
ZnCO3
93.
Why would an molecular formula for Al3H6 not be the correct empirical formula?
a)
The ratios are wrong.
b)
Al3H6 is not the simplest ratio
c)
They cannot be the same
d)
Aluminum and hydrogen cannot bond
94.
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
95.
Which reactant correctly balances the following equation: 4Al + __ -> 2Al2O3?
a)
3O2
b)
O3
c)
3O
d)
2O2
96.
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
97.
What are the products for the reaction between F2 + KCl
a)
FCl + K
b)
KF + Cl2
c)
KF + Cl
d)
no reaction
98.
This picture represents
a)
Synthesis
b)
Double Replacement
c)
Single Replacement
d)
Decomposition
99.
This image represents
a)
a double replacement reaction
b)
a decomposition reaction
c)
a single replacement reaction
d)
a complex compound reaction
100.
Compounds break down into simpler substances in this type of reaction.....
a)
Double Replacement
b)
Single Replacement
c)
Synthesis
d)
Decomposition
101.
How many significant figures in 102,000
a)
6
b)
2
c)
3
d)
5
102.
How many significant figures in 0.0045
a)
5
b)
2
c)
4
d)
3
103.
How many significant figures in 1,045.00
a)
6
b)
4
c)
4
d)
3
104.
Calculate 12.34 + 1.234 + 0.1234
a)
13.6974
b)
13.697
c)
13.70
d)
13.7
105.
Calculate 12.34 × 1.234 × 0.1234
a)
1.87908
b)
1.879
c)
1.9
d)
1.8790809
106.
Avogadro's number of representative particles is equal to one_____.
a)
kilogram
b)
gram
c)
kelvin
d)
mole
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