WorksheetsUnit 3- Ionics, Acids, and Covalents
Total questions: 139
Worksheet time: 3hrs 42mins
Name
Class
Date
1.
What is the charge on a chloride ion?
a)
-1
b)
1
c)
+2
d)
+1
2.
In the chemical formula for an ionic compound, which item is written first?
a)
positive ion
b)
negative ion
c)
subscript
d)
anion
3.
Francium has the same number of valence electrons as lithium.
a)
True
b)
False
4.
Which of the following elements would form a negative ion?
a)
#13 aluminum
b)
#32 germanium
c)
#53 iodine
d)
#26 iron
5.
Alkaline Earth elements will tend to become an ion with a charge of _____
a)
1+
b)
1-
c)
2+
d)
2-
6.
To reach a stable state, elements in Groups 15, 16, and 17 will _____
a)
lose electrons to form cations
b)
gain electrons to form cations
c)
lose electrons to form anions
d)
gain electrons to form anions
7.
Pure ionic compounds are _____
a)
electrically neutral
b)
charged positively
c)
charged negatively
d)
strongly charged
8.
Ionic compounds are formed when one or more valence electrons are transferred from _____
a)
a nonmetal atom to a metal atom
b)
a nonmetal atom to a nonmetal atom
c)
a metal atom to a nonmetal atom
d)
a metal atom to a metal atom
9.
What is the formula for lithium oxide?
a)
LiO
b)
LiO2
c)
Li2O
d)
Li2O3
10.
What is the ionic compound formed between Ba and P?
a)
Ba2P3
b)
Ba3P2
c)
BaP
d)
Ba2P2
11.
What is the chemical name for Fe(NO3)3?
a)
Iron (III) Nitrate
b)
Iron (III) Nitride
c)
Iron (VI) Nitrate
d)
Iron Nitrate
12.
What is the name for Pb(SO4)2?
a)
Lead (II) Sulfate
b)
Lead (IV) Sulfate
c)
Lead Sulfate
d)
Lead (I) Sulfate
13.
What is the charge on a Hydrogen ion?
a)
+1
b)
1
c)
2
14.
What is the ionic compound formed between K and F?
a)
KF
b)
K2F
c)
KF2
d)
K2F2
15.
What is the ionic compound formed between Ca and O?
a)
CaO
b)
Ca2O
c)
Ca2O2
d)
CaO2
16.
The compound formed by Mn (IV) and S would be which of these choices?
a)
Mn4S2
b)
MnS
c)
MnS4
d)
MnS2
17.
Atoms gain or lose electrons to become stable by satisfying this rule.
a)
Lewis Structure rule
b)
Periodic Law
c)
octet rule
d)
Ionic Law
18.
What is the chemical name for the compound with the formula Na₂S?
a)
sodium sulfide
b)
sodium fluoride
c)
magnesium sulfide
d)
lithium oxide
19.
Nitrogen will ____ electrons when forming an ionic bond.
a)
gain 1
b)
lose 1
c)
gain 3
d)
lose 3
20.
Ionic bonds form between metals and ____.
a)
metalloids
b)
metals
c)
nonmetals
21.
Which is the correct name for CaBr2?
a)
Calcium Bromine
b)
Bromine Calcium
c)
Calcium Bromide
d)
Carbon and Bromine
22.
What is the formula of Sodium oxide?
a)
Na2O
b)
NaO2
c)
Na2O2
d)
Na2O
23.
Why are ions charged particles?
a)
The number of electrons does not equal the number of protons.
b)
The number of protons does not equal the number of neutrons.
c)
The number of neutrons does not equal the number of electrons.
d)
The electric charges of the electrons and protons cancel each other out.
24.
An aluminum atom can lose 3 electrons in order to have a full outer energy level. What charge does the resulting aluminum ion have?
a)
1+
b)
3+
c)
2+
d)
2-
25.
Which two elements could form an ionic compound?
a)
#6 carbon and #8 oxygen
b)
#1 hydrogen and #7 nitrogen
c)
#3 lithium and #9 fluorine
d)
#5 boron and #10 neon
26.
The Roman numerals written with some metals show their _.
a)
charge as an ion
b)
number of energy levels
c)
number of bonds
d)
number of negative charges
27.
The numbers of atoms of each element in a compound formula is shown using _.
a)
subscripts
b)
superscripts
c)
roman numerals
d)
coefficient
28.
The name of this compound, MgO, is _.
a)
Manganese oxide
b)
Magnesium oxide
c)
Magnesium oxygen
d)
Manganese oxygen
29.
The name of this compound, Na3F, is _.
a)
sodium fluorine
b)
sodium fluoride
c)
trisodium fluoride
d)
sodium trifluoride
30.
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
31.
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
32.
Ions that are made of more than one atom are examples of:
a)
polyatomic atoms
b)
negative ions
c)
positive ions
d)
neutral ions
33.
Elements in Group 1 lose one electron to form ions with a(n) _________________ charge.
a)
1+
b)
2+
c)
0
d)
1-
34.
When ions having a positive charge form bonds with ions having a negative charge, the charge on the resulting compound is:
a)
0
b)
1+
c)
1-
d)
37
35.
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
36.
An ionic bond is the attraction between:
a)
oppositely charged ions
b)
similarly charged ions
c)
neutral ions
d)
neutral atoms
37.
When an atom loses an electron, it becomes a:
a)
positive ion
b)
negative ion
c)
neutral ion
d)
neutral atom
38.
Refer to the image. Which diagrams correctly represent the transfer of electrons in ionic bonding?
a)
Diagram 3 and 4
b)
Diagram 1 and 2
c)
Diagram 1 and 4
d)
Diagram 2 and 3
39.
How many dots would you draw for an electron dot diagram of sulfur (#16)?
a)
2
b)
6
c)
8
d)
16
40.
How many electrons does phosphorus (#15) need to gain in order to obtain an octet?
a)
3
b)
5
c)
8
d)
15
41.
According to the diagram, what will this atom do when it forms an ionic bond with a metal?
a)
Give away 1 electron
b)
Give away 7 electrons
c)
Gain one electron
d)
Gain 7 electrons
42.
Which of these compounds is Ionic?
a)
SI2
b)
CH4
c)
Br2
d)
CaF2
43.
What is the correct name of CaBr2?
a)
calcium bromine
b)
calcium baride
c)
monocalcium dibromide
d)
calcium bromide
44.
In the chemical formula for an ionic compound, which element is written first?
a)
cation
b)
anion
c)
the one with the longest name
45.
Which group of the periodic table is most stable (already has 8 valence electrons)?
a)
Alkali metals
b)
Transition metals
c)
Halogens
d)
Noble gases
46.
What type of metal needs a roman numeral after its name?
a)
Group 1
b)
Group 2
c)
Transition metals with many charge options
d)
Group 17
47.
ammonium
a)
NH4+
b)
NH4
c)
NH3
d)
NH3-
48.
Sulfate
a)
SO42-
b)
SO32-
c)
SO4
d)
SO3
49.
sulfite
a)
SO32-
b)
SO42-
c)
SO3
d)
SO4
50.
CO32-
a)
Carbonate
b)
Cyanide
c)
Chromate
d)
Chlorite
51.
Ca(CN)2
a)
Calcium Cyanide
b)
Calcium Dicyanide
c)
Calcium Dicarbon Dinitrogen
d)
Calcium Thiocyanate
52.
Li2Cr2O7
a)
Lithium Dichromate
b)
Lithium Chromate
c)
Dilithium Dichromate
d)
Dilithium Dichromium Heptoxide
53.
KMnO4
a)
Potassium Permanganate
b)
Potassium Manganate
c)
Potassium Manganese Tetroxide
d)
Permanganate Potassiide
54.
Sliver Phosphide
a)
Ag3P
b)
Ag3PO4
c)
Ag3PO3
d)
AgP
55.
Ammonium Phosphate
a)
(NH4)3PO4
b)
NPO4
c)
NH4PO4
d)
NH4(PO4)3
56.
Iron III Chromate
a)
Fe2(CrO4)3
b)
Fe3CrO4
c)
Fe2(Cr2O7)3
d)
FeCrO4
57.
Aluminum Sulfite
a)
Al2(SO3)3
b)
Al2(SO4)3
c)
AlSO3
d)
Al3(SO3)2
58.
Sodium Bicarbonate
a)
NaHCO3
b)
Na2CO3
c)
Na2HCO3
d)
S(HCO3)2
59.
Zinc Fluoride
a)
ZnF2
b)
ZnF
c)
Zn2F
d)
Zn2F4
60.
Select the formula for the following acid: hydroiodic acid
a)
HI
b)
HIO4
c)
HIO3
d)
H2I
61.
Select the name of the following acid: HF
a)
Hydrofluoric acid
b)
Fluorous acid
c)
Fluoric acid
d)
Hydroflouric acid
62.
Select the name for the following acid: H3PO4
a)
Phosphoric acid
b)
Phosphorous acid
c)
Hydrophosphoric acid
63.
Select the formula for the following acid: Carbonic Acid
a)
H2CO3
b)
HCO3
c)
H4C
64.
Select the name for the following acid: H2SO4
a)
Sulfuric acid
b)
Sulfurous acid
c)
Hydrosulfuric acid
65.
Select the formula for the following acid: nitrous acid
a)
HNO2
b)
HNO3
c)
H3N
66.
Select the name for the following acid: H2SO3
a)
Sulfurous acid
b)
Sulfuric acid
c)
Hydrosulfuric acid
67.
Select the formula for the following acid: phosphorous acid
a)
H3PO3
b)
H3PO4
c)
H3P
68.
Select the name for the following acid: HNO3
a)
Nitric acid
b)
Nitrous acid
c)
Hydronitric acid
69.
Select the formula for the following acid: hydrobromic acid
a)
HBr
b)
HBrO4
c)
HBrO3
70.
Select the name for the following acid: HC2H3O2
a)
Acetic acid
b)
Ethanoic acid
c)
Acenous acid
d)
Hydroacetic acid
71.
Select the formula for the following acid: chloric acid
a)
HClO3
b)
HCl
c)
HClO4
72.
Select the formula for the following acid: perchloric acid
a)
HClO4
b)
HClO3
c)
HClO2
d)
HCl
73.
Select the name for the following acid: H2S
a)
Hydrosulfuric acid
b)
Sulfuric acid
c)
Sulfurous
74.
Select the name of the following acid: HCl
a)
Hydrochloric acid
b)
Chlorous acid
c)
Chloric acid
75.
What is the name of the following acid: HBr
a)
Bromic acid
b)
hydrobromic acid
c)
hydrobromine acid
76.
What is the formula for acetic acid?
a)
HAcO3
b)
HC3OOH
c)
CH3OOH
d)
CH3COOH
77.
Select the formula for the following base: chromium (III) hydroxide
a)
Cr(OH)3
b)
Cr3OH
78.
Select the name for the following base: Cu(OH)2
a)
Copper (II) hydroxide
b)
Copper (I) hydroxide
c)
Copper (II) hydride
d)
Copper (I) hydride
79.
What determines the number of hydrogens in your acid?
a)
there are always just one
b)
its the same as the charge of hydrogen
c)
its the same as the charge of the anion
d)
magic
80.
When two atoms share electrons, a chemical bond is formed. This type of bond is called:
a)
covalent bond
b)
ionic bond
c)
crystal bond
d)
polyatomic bond
81.
What is a double bond?
a)
a bond between two atoms
b)
one pair of electrons shared between two atoms
c)
two pairs of electrons shared between two atoms
d)
James Bond's brother
82.
Disulfur trioxide
a)
S3O2
b)
SO
c)
S2O3
d)
S2O
83.
P2O5
a)
Phosphorus Oxide
b)
Pentaphosphorus Dioxide
c)
Diphosphorous pentoxide
d)
Phosphoric Oxygen
84.
SeF4
a)
Tetraselenium fluoride
b)
Selenium Fluoride
c)
Selenium tetraflouride
d)
Selenium (IV) Fluoride
85.
CO
a)
Carbon Oxide
b)
Carbon Oxygen
c)
Dicarbon dioxide
d)
Carbon Monoxide
86.
PBr5
a)
Phosphorus Bromide
b)
Phosphorus Pentabromide
c)
Pentaphosphorus bromide
d)
Phosphorus Bromine
87.
Name the following compound:
BF3
BF3
a)
boron fluoride
b)
boron difluoride
c)
monoboron trifluoride
d)
boron trifluoride
88.
carbon monoxide
a)
CO
b)
CO2
c)
C2O
d)
COH
89.
BrO3
a)
bromine oxide
b)
monobromine trioxide
c)
bromine trioxide
d)
bromine (III) oxide
90.
As4O10
a)
arsenic oxide
b)
quadarsenic decoxide
c)
tetraarsenic decoxide
d)
arsenic decoxide
91.
Phosphorous trichloride
a)
PCl3
b)
P3Cl
c)
P3Cl3
d)
PCL
92.
SeF4
a)
Tetraselenium fluoride
b)
Selenium Fluoride
c)
Selenium tetraflouride
d)
Selenium (IV) Fluoride
93.
Covalent compounds
a)
Share electrons
b)
transfer electrons
c)
contain a sea of electrons
d)
conduct electricity
94.
Which of these is covalent?
a)
NaCl
b)
Pb(NO3)2
c)
CO2
d)
AlCl3
95.
P2O5
a)
Phosphorus Oxide
b)
Pentaphosphorus Dioxide
c)
Diphosphorous pentoxide
d)
Phosphoric Oxygen
96.
How many valence electrons does nitrogen have?
a)
3
b)
2
c)
5
d)
1
97.
How many valence electrons does hydrogen have?
a)
4
b)
3
c)
2
d)
1
98.
Name SO2
a)
monosulfur dioxide
b)
sulfur dioxide
c)
sulfur oxide
d)
sulfur (II) oxide
99.
Which is true about covalent bonds?
a)
they are between 2 nonmetals
b)
they are between 2 metals
c)
they are between 1 metal and 1 nonmetal
100.
What is the prefix for 1?
a)
mono
b)
di
c)
tri
d)
tetra
101.
How many valence electrons does carbon have?
a)
1
b)
2
c)
3
d)
4
102.
How many valence electrons does oxygen have?
a)
2
b)
3
c)
6
d)
4
103.
How many valence electrons does chlorine have?
a)
1
b)
7
c)
4
d)
2
104.
How many valence electrons does nitrogen have?
a)
3
b)
2
c)
5
d)
1
105.
Name CCl4
a)
carbon carbon tetraiodide
b)
carbon tetrachloride
c)
monocarbon tetrachloride
d)
water
106.
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
107.
How are ionic bonds formed?
a)
When atoms share an electron
b)
When opposite charged atoms attract
c)
When one atom takes a proton
d)
When one atom takes a neutron
108.
Which of the following is a covalent bond?
a)
LiF - Lithium Fluoride
b)
NH3 - Ammonia
c)
NaBr - Sodium Bromide
d)
CuCl - Copper(I) Chloride
109.
Which element is most likely to form a covalent bond?
a)
Nitrogen
b)
Lithium
c)
Sodium
d)
Potassium
110.
What is it called if there are three-pairs of electrons being shared?
a)
Triple bond
b)
Bond length
c)
Tribond
d)
Chocolate Mousse
111.
The compound formed between lithium and chlorine is _________.
a)
ionic
b)
covalent
112.
In ionic bonding, electrons are
a)
shared
b)
transferred
c)
wiped out
113.
Outer shell electrons are called
a)
outer electrons
b)
valence electrons
c)
negatives
114.
For the structural formula shown, what is the chemical formula?
a)
NO
b)
N2O2
c)
NO2
d)
N2O
115.
The molecule shown has been called "laughing gas" and has been used in dentistry as a pain killer. What is its chemical name?
a)
Nitrogen oxide
b)
dinitrogen dioxide
c)
dinitrogen oxide
d)
nitrogen dioxide
116.
What is the correct name for Mg(OH)2?
a)
Magnesium dihydroxide
b)
Magnesium Oxyhydride
c)
Magnesium Oxygen dihydride
d)
Magnesium hydroxide
117.
What is the formula for chromium (I) selenide?
a)
Cr2Se
b)
CrSe
c)
CrSe2
d)
Cr2Se2
118.
Why do atoms share electrons?
a)
To attain the electron configuration of a noble gas.
b)
To become ions and take a charge
c)
to increase the mass
d)
it's a nice thing to do.
119.
Which of the compounds below contains a single covalent bond?
a)
Br2
b)
SO
c)
HCl
d)
Both a and c
120.
A molecule with a double covalent bond is....
a)
HCl
b)
SO
c)
I2
d)
N2
121.
Which three nonmetals exist only as diatomic molecules?
a)
H, C, Br
b)
N, O, S
c)
I, F,N
d)
H, O, P
122.
Which element forms a diatomic molecule using a triple covalent bond?
a)
C
b)
N
c)
O
d)
P
123.
How many bonds does carbon have to create in order to satisfy the octet rule
a)
1
b)
2
c)
3
d)
4
124.
Which of the following is the correct Lewis structure for CH2O?
a)
Option A
b)
Option B
c)
Option C
d)
Option D
125.
Which of the following is an acceptable Lewis structure for CH3Cl?
a)
Option A
b)
Option B
c)
Option C
d)
Option D
126.
What is the correct formula for this molecule?
a)
NH
b)
N3H
c)
NH3
d)
NH4
127.
What is the correct formula for this molecule?
a)
Si4F
b)
SiF4
c)
SiF
d)
Si4F4
128.
Which of the following is the correct Lewis dot structure for the molecule fluorine (F2)?
a)
A
b)
B
c)
C
d)
D
129.
Hydrogen needs _____ electrons in its valence shell to be stable.
a)
4
b)
6
c)
8
d)
2
130.
In CO2, how many UNSHARED pairs of electrons does each oxygen have?
a)
2
b)
1
c)
4
d)
6
131.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
132.
This is a correct dot diagram for oxygen (O)
a)
true
b)
false
133.
This could be the dot diagram of
a)
Al
b)
Si
c)
Na
d)
Mg
134.
This could be the dot diagram of
a)
P
b)
Ar
c)
Na
d)
B
135.
What is the first thing you need to do when drawing Lewis Structures?
a)
Draw your bonds
b)
Count the number of valence electrons
c)
Subtract to make the valence number even
d)
Add to make the valence number even
136.
Choose the structure that forms a triple bond.
a)
Hydrogen
b)
Fluorine
c)
Oxygen
d)
Nitrogen
137.
Choose the structure that forms a double bond.
a)
Carbon monoxide (CO)
b)
Carbon dioxide (CO2)
c)
Water (H2O)
d)
Cyanic Acid (HCN)
138.
Which is the correct structure for ammonia?
Pictures correspond with a-d.
Pictures correspond with a-d.
a)
Option A.
b)
Option B.
c)
Option C.
d)
Option D.
139.
According to the octet rule most elements need _______ valence electrons.
a)
2
b)
8
c)
6
d)
18
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