Chemistry – Covalent Compounds Packet
Name:____________________________________ Hr:_____ Page 1
Chemistry A
Covalent
Compounds
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Chemistry – Covalent Compounds Packet
Name:____________________________________ Hr:_____ Page 2
Covalent Compounds Learning Goals
 Worksheet #1 (Concept) I can name and write
formulas for covalent compounds.
 Worksheet #2 (Concept) I can explain the
properties of covalent compounds.
 Worksheet #3 (Concept) I can draw diagrams
to represent single covalent bonds.
 Worksheet #4 (Concept) I can draw diagrams
to represent double and triple covalent bonds.
Concept Scale:
4 = I can teach this concept to another
student.
3 = I can explain this concept to a
teacher.
2 = I can explain this concept with
some help.
1 = I can find the explanation to this
concept in my class work.
0 = I know nothing about this
concept.
 Worksheet #5 (Concept) I can describe the properties of metallic bonds
 Worksheets #6, #7 and #8 (Concept) I can write formulas and names for all
ionic AND covalent compounds when given a mixture.
 Worksheets #6, #7 and #8 (Concept) I can explain the difference between:
element v. compound, atom v. molecule, subscript v. oxidation number
 Worksheet #9 (Concept) I can draw diagrams to represent ionic bonds, single,
double and triple covalent bonds when given a mixture.
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Chemistry – Covalent Compounds Packet
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Chemistry Self Assessment Sheet
Directions: Record the learning goal and homework from the board each day at the start of class. Self
evaluate yourself at the end of class using the scales on the learning goals sheet.
Date: _______________________ Type of Learning Goal (s) (circle) CONCEPT
MATH
GRAPH
Learning Goal: I CAN ______________________________________________________________________________
_________________________________________________________________________________________________
How well can I do this at the end of class?_________
Learning Goal: I CAN ______________________________________________________________________________
_________________________________________________________________________________________________
How well can I do this at the end of class?_________
Homework: _______________________________________________________________________
Date: _______________________ Type of Learning Goal (s) (circle) CONCEPT
MATH
GRAPH
Learning Goal: I CAN ______________________________________________________________________________
_________________________________________________________________________________________________
How well can I do this at the end of class?_________
Learning Goal: I CAN ______________________________________________________________________________
_________________________________________________________________________________________________
How well can I do this at the end of class?_________
Homework: _______________________________________________________________________
Date: _______________________ Type of Learning Goal (s) (circle) CONCEPT
MATH
GRAPH
Learning Goal: I CAN ______________________________________________________________________________
_________________________________________________________________________________________________
How well can I do this at the end of class?_________
Learning Goal: I CAN ______________________________________________________________________________
_________________________________________________________________________________________________
How well can I do this at the end of class?_________
Homework: _______________________________________________________________________
Date: _______________________ Type of Learning Goal (s) (circle) CONCEPT
MATH
GRAPH
Learning Goal: I CAN ______________________________________________________________________________
_________________________________________________________________________________________________
How well can I do this at the end of class?_________
Learning Goal: I CAN ______________________________________________________________________________
Date:
_______________________ Type of Learning Goal (s) (circle) CONCEPT
MATH
GRAPH
_________________________________________________________________________________________________
How well can I do this at the end of class?_________
Learning Goal: I CAN ______________________________________________________________________________
_________________________________________________________________________________________________
Homework: _______________________________________________________________________
How well can I do this at the end of class?_________
Learning Goal: I CAN ______________________________________________________________________________
_________________________________________________________________________________________________
How well can I do this at the end of class?_________
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Homework: _______________________________________________________________________
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Chemistry – Covalent Compounds Packet
Name:____________________________________ Hr:_____ Page 4
Date: _______________________ Type of Learning Goal (s) (circle) CONCEPT
MATH
GRAPH
Learning Goal: I CAN ______________________________________________________________________________
_________________________________________________________________________________________________
How well can I do this at the end of class?_________
Learning Goal: I CAN ______________________________________________________________________________
_________________________________________________________________________________________________
How well can I do this at the end of class?_________
Homework: _______________________________________________________________________
Date: _______________________ Type of Learning Goal (s) (circle) CONCEPT
MATH
GRAPH
Learning Goal: I CAN ______________________________________________________________________________
_________________________________________________________________________________________________
How well can I do this at the end of class?_________
Learning Goal: I CAN ______________________________________________________________________________
_________________________________________________________________________________________________
How well can I do this at the end of class?_________
Homework: _______________________________________________________________________
Date: _______________________ Type of Learning Goal (s) (circle) CONCEPT
MATH
GRAPH
Learning Goal: I CAN ______________________________________________________________________________
_________________________________________________________________________________________________
How well can I do this at the end of class?_________
Learning Goal: I CAN ______________________________________________________________________________
_________________________________________________________________________________________________
How well can I do this at the end of class?_________
Homework: _______________________________________________________________________
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Chemistry – Covalent Compounds Packet
Name:____________________________________ Hr:_____ Page 5
Date: _______________________ Type of Learning Goal (s) (circle) CONCEPT
MATH
GRAPH
Learning Goal: I CAN ______________________________________________________________________________
_________________________________________________________________________________________________
How well can I do this at the end of class?_________
Learning Goal: I CAN ______________________________________________________________________________
_________________________________________________________________________________________________
How well can I do this at the end of class?_________
Homework: _______________________________________________________________________
Date: _______________________ Type of Learning Goal (s) (circle) CONCEPT
MATH
GRAPH
Learning Goal: I CAN ______________________________________________________________________________
_________________________________________________________________________________________________
How well can I do this at the end of class?_________
Learning Goal: I CAN ______________________________________________________________________________
_________________________________________________________________________________________________
How well can I do this at the end of class?_________
Homework: _______________________________________________________________________
Date: _______________________ Type of Learning Goal (s) (circle) CONCEPT
MATH
GRAPH
Learning Goal: I CAN ______________________________________________________________________________
_________________________________________________________________________________________________
How well can I do this at the end of class?_________
Learning Goal: I CAN ______________________________________________________________________________
_________________________________________________________________________________________________
How well can I do this at the end of class?_________
Homework: _______________________________________________________________________
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Chemistry – Covalent Compounds Packet
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Worksheet #1- Naming Covalent Compounds
The ionic compounds that we have used so far have all contained a metal bonded to a nonmetal. You will now
learn how to name compounds and write the formulas for compounds containing nonmetals only. Compounds that
consist of nonmetals contain covalent bonds. These elements share electrons in order to become stable. (We will worry
about how and why this happens later.) Since these compounds form under a variety of conditions we cannot use
oxidation numbers determine their formulas. We must instead use prefixes. These prefixes will also be used in the
names of each formula so that you know what how many of each type of element is in the compound.
1 = mono 3 = tri 5 = penta 7 = hepta 9 = nona
2 = di
4 = tetra 6 = hexa 8 = octa 10 = deca
Consider NO and N2O. If we used the naming method from worksheet #1 then we would call each of these nitrogen
oxide. If I told you that you produced a gas called nitrogen oxide in lab then you would not know which one to which I
was referring. The correct names are below:

N2O is called dinitrogen monoxide.

NO is called nitrogen monoxide. (Note: I did not call this compound mononitrogen monoxide. We
never start a compound with the prefix mono-.)
Name the following compounds.
Formula
N2O4
Name
dinitrogen tetraoxide
P4O10
GeCl4
H2O
BCl3
SO2
When you write the formula for compounds that are made up of nonmetals you do not need to look up the oxidation
numbers. The prefix becomes the subscript. For example: the formula for dinitrogen trioxide is N2O3. The formula for
carbon dioxide is CO2. Did you notice that carbon does not have a prefix? If there is a compound that is made up of all
nonmetals and there is no prefix at the beginning of the name, you are to assume the prefix is mono- and the subscript is
one.
Write the formulas for the following compounds.
Name
Formula
tetraphosphorus decasulfide
P4S10
Do not swap
and drop!
dichlorine heptaoxide
silicon tetrafluoride
Do not
reduce!
dinitrogen trioxide
carbon monoxide
carbon tetrachloride
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Chemistry – Covalent Compounds Packet
Name:____________________________________ Hr:_____ Page 7
Worksheet #2: Introduction to Covalent Bonds
A covalent bond is formed between nonmetal atoms. The nonmetals are connected by a shared pair of
valence electrons. Remember, nonmetals want to gain valence electrons to reach a stable arrangement. If there are no
metal atoms around to give them electrons, nonmetal atoms share their valence electrons with other nonmetal atoms.
Since the two atoms are using the same electrons they are stuck to each other in a neutral particle called a molecule. A
molecule is a neutral particle of two or more atoms bonded to each other. Molecules may contain atoms of the same
element such as N2, O2, and Cl2 or they may contain atoms of different elements like H2O, NH3, or C6H12O6. Therefore,
covalent bonding is found in nonmetallic elements and in nonmetallic compounds.
Covalent bonds are intramolecular forces; that is, they are inside the molecule and hold the atoms together to
make the molecule. Covalent bonds are strong bonds and it is difficult and requires a lot of energy to break a molecule
apart into its atoms. However, since molecules are neutral one molecule does not have a strong electrical attraction for
another molecule. The attractions between molecules are called intermolecular forces and these are weak forces.
Covalent substances have low melting points and boiling points compared to ionic compounds or metals. At room
temperature, covalent substances are gases, liquids or low melting point solids. They do not conduct electricity as solids
or when molten and usually do not conduct when dissolved in water.
1. Define the following terms:
a) covalent bond –
b) molecule –
c) intramolecular force–
d) intermolecular force–
2. List several properties of covalent compounds.
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Worksheet #3: Drawing Single Covalent Bonds
Background info:
When atoms of nonmetals bond to each other they share valence electrons and form a covalent bond. When atoms bond they usually
have to rearrange their electrons from the positions we pictured in the single atom. The goal is for every atom to have eight electrons
around it except for hydrogen which has only two electrons. Hydrogen only forms one single bond; other atoms can form up to four
single bonds. When you draw a dot diagram for a molecule you start with the atom that is only in the formula once—it will be in the
center of the molecule with the other atoms arranged around it. If there are only two atoms it doesn’t matter where you start. Draw
Lewis dot diagrams for the following molecules.
HINT: Carbon, nitrogen, and sulfur are usually the central atom(s) (in the center) surrounded by terminal atoms (surrounding
central). Carbon is always a central and hydrogen is always a terminal. When in doubt, put the any single atom in the middle,
surrounding it with the element that contains more than one atom.
Final Answer
Ex: nitrogen triiodide (NI3)
Show work here
1. carbon tetrabromide (CBr4)
2. dihydrogen monosulfide (H2S)
3. dihydrogen monoselenide (H2Se)
4.
hydrogen (H2)
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Chemistry – Covalent Compounds Packet
Worksheet #3 Continued
Name:____________________________________ Hr:_____ Page 12
1. Draw the bonds below:
a) phosphorus
triodide (PI3)
b) bromine (Br2)
c) water (H2O)
d) ammonia (NH3)
2. EXTRA CHALLENGE: Determine if it is an ionic bond or a covalent bond. Show the work and the final answer
Remember: Covalent bonds form between two nonmetals that share electrons. Ionic bonds are formed between a metal and a
nonmetal that completely transfer electrons.
e) methane (CH4)
(FeO)
f) iron (II) oxide
g) carbon tetrachloride (CCl4)
h) phosphorus tribromide (PBr3)
i) sodium nitride (Na3N)
j) hydrochloric acid (HCl)
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Chemistry – Covalent Compounds Packet
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Worksheet #4: Double AND Triple Bonds
There are many types of covalent bonds. So far we have drawn single covalent bonds- when two atoms share one pair of
valence electrons. Double bonds can form when a shared single bond alone doesn’t satisfy either atoms valence. Double
bonds are TWO SHARED PAIRS of electrons for a total of 4 electrons (2 electrons from one atom and 2 from the other).
Double bonds are much stronger and bond the atoms closer than a single bond.
Ex: carbon dioxide
Show work here.
Final Answer
1. oxygen (O2)
2. ethene (C2H4)*** C’s are always central and they will link together.
Triple bonds can form when 3 pairs of electrons are shared for a total of 6 shared electrons. Typically one atom donates 3
electrons and the other atom donates the other 3. Triple bonds are even stronger than double bonds and the atoms are
held even closer together.
EX: nitrogen (N2)
3. ethyne (C2H2) (remember C's are always central atoms)
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Chemistry – Covalent Compounds Packet
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Worksheet #4 Continued
We have looked at diagrams for ionic compounds and for molecules of covalent substances that contain only single bonds. Many
molecules contain double or triple bonds. Ideally an atom is involved in only single bonding that is a more stable arrangement. But,
if the atom cannot achieve eight electrons in its valence shell it will become involved in double or triple bonds to reach this stable
arrangement. Draw diagrams for the following molecules.
1. Double Bonds:
a) oxygen (O2)
2. Triple Bonds:
c) nitrogen (N2)
b). formaldehyde (H2CO) * the C’s in the middle attach the
2 Hs and the O to it.
d). hydrogen cyanide (HCN) *the carbon is in the middle with
the other two attached to it.
3. EXTRA CHALLENGE: RECALL THE DIFFERENCE BETWEEN IONIC AND COVALENT!!!
e) N2H2 *** (N goes in the middle)
f) C2H6 *** (C’s in the middle)
g) CF2Cl2 *** (C in the middle, 2 F’s and Cl’s around it)
h) KF
i) N2F4 *** (N’s in the middle)
j) Mg3N2
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Chemistry – Covalent Compounds Packet
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Worksheet #5: Metallic Bonds
A metallic bond forms between multiple metal atoms. The
metallic bond is formed by the mutual attraction for each
others loosely held valence electrons. Most metal atoms
have only one or two valence electrons and these are not
tightly bound to the atoms. In a piece of metal these valence
electrons do not seem to belong to any one of the atoms but are
able to move freely through the structure from one atom to
another. Metals can be thought of as positive ions (the
nucleus and inner shells of electrons—all of the atom
except the valence electrons) in a “sea” of loose valence
electrons. The metal ions line up in a regular repeating
pattern (a crystal lattice) and their loose valence electrons move through this crystal acting as an electron glue (see figure).
Each of the ions is strongly attracted to all of the loose electrons surrounding it so the whole metal holds together as a
crystal.
These electrical attractions for the electron glue are strong and hard to break so metals are have high melting points and
are solids. Since there are charged particles free to move metals are good conductors of heat and electricity as solids
and as liquids. Because the “electron glue” is free to move, if we hammer or pull the cations to new positions the
electron glue flows right along with the cations and holds the structure together in the new position. Thus, metals are
malleable (bendable) and ductile (can be hammered flat) and have a high tensile strength (can be stretched without
breaking). This loose cloud of electrons is good at absorbing and re-emitting the light energy that strikes it so
metals are lustrous (shiny).
Metallic bonding is found in elemental metals and in mixtures of metals called alloys.
1. What is a metallic bond? Explain how the ions and electrons are arranged.
2. List some properties of metallic bonds.
3. What is an alloy?
4. Identify the following compounds as metallic, ionic or covalent:
a. NaCl
e. Mg3N2
b. Cl2
f.
c. Au
g. Al
Pt
d. [BrO3]-1
h. Ag
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Chemistry – Covalent Compounds Packet
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Worksheet #6 – Naming Binary Compounds Review #1
Name the following compounds. If the compound contains a special metal you are to use roman numerals to name it. If
the compound contains all nonmetals you are to use the prefixes to name the compound. Otherwise name the metal and
then the nonmetal with the –ide ending.
Formula
Name
Formula
Name
ZnTe
Zinc telluride
Fe2Se3
Iron (III) selenide
RaI2
Cu3N
NaCl
S3O9
Cs3P
P2O3
Au2S
BF3
AgF
NO3
NiO
PCl3
Trisulfur nonaoxide
Write the formula for the following compounds. You will not need the column for the “symbols with oxidation #s” for
compounds that are made up of nonmetals.
Name
Symbols with
Formula
Name
Symbols with
Formula
oxidation #s
oxidation #s
(optional)
(optional)
calcium telluride
mercury (I) sulfide
strontium phosphide
bismuth(V) selenide
rubidium nitride
lead (IV) bromide
silver chloride
silicon dioxide
XXX
francium arsenide
carbon monoxide
XXX
platinum oxide
carbon disulfide
XXX
barium iodide
diboron trioxide
XXX
1. Compare and contrast the following:
a. Element v. Compound: ______________________________________________________________
b. Atom v. Molecule: __________________________________________________________________
c. Subscript v. Oxidation Number: _______________________________________________________
2. When do you use roman numerals? ___________________________________________________________
3. When do you use prefixes? __________________________________________________________________
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Chemistry – Covalent Compounds Packet
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Worksheet #7 – Naming Binary Compounds Review #2
The following ionic compounds contain both metals and nonmetals.
Name
Symbols with
Formula
Formula
oxidation #s
sodium sulfide
NaCl
magnesium iodide
AlCl3
silver oxide
SrBr2
rubidium fluoride
CoBr2
Name the following special metals
Formula
Oxidation Number
of the Metal
Name
Name (use roman numerals)
Fe2S3
Bi3P5
Hg2O
SbN
The following compounds contain special metals.
Name
Symbols with
Formula
oxidation #s
(optional)
copper (I) nitride
SnO2
lead (IV) chloride
Hg3P
iron (II) sulfide
Bi2S3
antimony(V) iodide
Sb2O3
Formula
Oxidation Number
of the Metal
Name (use roman numerals)
The following compounds contain nonmetals only.
Name
dihydrogen monoxide
Formula
Formula
CO
boron trichloride
P4O10
dinitrogen monoxide
SiO2
dichlorine heptaoxide
N2O3
sulfur hexafluoride
CBr4
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Name (use prefixes)
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Chemistry – Covalent Compounds Packet
Name:____________________________________ Hr:_____ Page 18
Worksheet #8- Naming Binary Compounds Review #3
This review sheet contains all types of compounds that we have learned so far. If you can complete this table with only a
periodic table (oxidation numbers only) then you should do well on the naming section of the quiz.
Name
Symbols with
Formula
Name
Symbols with
Formula
oxidation #s
oxidation #s
nickel iodide
antimony(V) sulfide
potassium phosphide
mercury (I) oxide
calcium phosphide
iron (III) bromide
platinum nitride
nitrogen monoxide
XXX
magnesium fluoride
diphosphorus trioxide
XXX
aluminum sulfide
carbon tetrachloride
XXX
chromium telluride
sulfur trioxide
XXX
Write the formula for the following compounds. Use roman numerals where appropriate. Remember that compounds
which contain nonmetals only need prefixes.
Formula
Name
Formula
Name
RaI2
K3P
AsO4
FeS
AgI
Cu3P
ZnCl2
Sb2Se3
MgO
BCl3
PtS
SO3
AuF
N2O
Answer the following questions:
1. The charge on an element in a compound is called______________________________
2. Metals are_________________ of the staircase
3. Nonmetals are___________________ of the staircase.
4. The simplest form of matter is called:_______
5. The little numbers written below the line in compounds are called:______________
6. The total charge on any compound is:________
7. Chemical combination of two or more elements is called: ___________
8. Used to represent chemical compounds:____________
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Chemistry – Covalent Compounds Packet
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Worksheet #9: Covalent Bonding Review Sheet
Draw diagrams for the following compounds.
a) water (H2O)
b) sulfur dioxide (SO2)
c) nitrogen molecule (N2)
d) ammonia (NH3)
e) methane (CH4)
f) phosphorous triiodide (PI3)
g) chlorine molecule (Cl2)
h) carbon dioxide (CO2)
i) oxygen molecule (O2)
j) ethane (C2H6) (carbons hook to each other with H’s all around)
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