LABORATORY WRITING FORMULAS OF CHEMICAL
MODULE 3 COMPOUNDS AND NAMING OF COMPOUNDS
LEARNING OUTCOMES:
Module Learning Outcomes
MLO1. Apply the rules in writing chemical formulas.
MLO2. Write chemical formulas for binary and ternary ionic compounds.
MLO3. Write the chemical names for binary and ternary ionic compounds.
Course Learning Outcomes
MLO1. Apply the rules in writing chemical formulas.
MLO2. Write chemical formulas for binary and ternary ionic compounds.
MLO3. Write the chemical names for binary and ternary ionic compounds.
Topic Learning Outcomes
TLO12. Write formulas from the cations and anions in the periodic table.
TLO13. Name compounds that are formed.
Table of Contents
Title Page Time Frame
Compound 1 30 mins
A Visual for Naming Compounds 2 30 mins
Activity 4 90 mins
Honesty Clause 3
KEY WORDS
Compound Chemical Formula Metal Non-Metal
Description: This laboratory module design to provide students to understand how to write and name chemical
compounds and how the rules are being followed. Chemical formulas provide a lot of information
about chemical substances, such as how many and what atoms they are made of, as well as the
way the atoms are arranged. In this activity, we'll answers how to write and name the different types
of chemical compounds. This activity is good only for 2hours and 30 minutes.
Compound it is a substance that made up of a definite proportion of two or more elements.
Chemical formula it tells us the number of atoms of each element in a compound. This contains the symbols of
the atoms of the elements present in the compound as well as how many are there for each element
in the form of subscripts.
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Since that we encounter chemical substances and compounds every day. The substances under the
kitchen sink that we use every day to clean our houses as well as those that are staples in our medicine cabinet
are also made up of chemical substances. These chemicals are made up of a fixed proportion of atoms, and
these atoms are arranged in a certain way. To figure out what these proportions means are and how they are
arranged for any given substances, in this, we need to know the chemical formula of the substance or compound.
Here are the rules in naming chemical compounds.
1. Metal and Non-Metal, No Polyatomic Ions: When a metal and a non-metal are combining and there are
no polyatomic ions in the formula, (example 1: NaCl)
Name the metal (the + element): NaCl = Sodium
Name the base of the non-metal (the - element): NaCl = “chlor”
Add the ending –ide to the non-metal: NaCl = chloride
2. Metal and Polyatomic Ion: When you have a metal combined with a polyatomic ion (one of the italicized
ions from your oxidation number table) then:
Name the element in the metal (+) position.
Name the polyatomic (-) ion.
Example: Na2CO3 = sodium carbonate
3. Two Non-Metals: If two non-metals have combined into a compound (remember where to
find non- metals on the periodic table?)
Name the non-metal that’s in the first (+) position.
Use a prefix to indicate how many atoms there are of the second (-) element.
Name the base of the second (-) non-metal
Add the –ide ending.
Example: CO = carbon + mono + ox + ide = carbon monoxide
A Visual for Naming Compounds
One type of atom
Name of element
Name the anion
Specify with roman number Base + ide
which ion for:
Cu I or Cu II Polyatomic
Fe II or Fe III (more than one type of atom)
Cr II or Cr III Look for name in the table for
common oxidation numbers
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Non-Metal + Non-Metal
Specify number of anion
atoms:
Name of element mono Name the
di anion
tri
tetra
penta Base + ide
hexa
SUMMARY
A chemical formula of a compound is also the same for all the molecules of that compound. This means that
when we read the formula, the subscripts always tell us how many atoms of a particular element is in one
molecule of that compound. This molecular compound is usually composed of two or more nonmetal elements.
Thus a molecular compound are named with the first element first and then the second element by using the
stem of the element name plus the suffix -ide. We always used numerical prefixes are used to specify the
number of atoms in a molecule.
HONESTY CLAUSE
“The College takes a strict view of any form of cheating, deceptive fabrication, plagiarism and violation of
intellectual property and copyright laws. Any student who is found to have engaged in such misconduct
will be subject to disciplinary action by the College.”
Students Name and Signature
________________________
Name and Signature
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Materials:
Pen Periodic Table
Worksheets
Procedure:
1. Copy or print the activities
2. Use your periodic table to answer the what is asked in the problem
3. Make your work neat and clean.
Time Frame: 1 hour and 30 mins
I. For the following problems identify the rule you need to follow and write the
appropriate name or chemical formula.
1. K3N 9. Fe2(CO3)3
Rule: Rule:
Name: Name:
2. Pb(C2H3O2)2 10. Ag2(SO3)
Rule: Rule:
Name: Name:
3. Sr(NO2)2 11. Cs3P2
Rule: Rule:
Name: Name:
4. Cu3(PO4)2 12. Cr(SO4)
Rule: Rule:
Name: Name:
5. Li(OH) 13. Zn3(PO4)2
Rule: Rule:
Name: Name:
6. (NH4)2(SO4) 14. NO3
Rule: Rule:
Name: Name:
7.C I4 15. BaCl2
Rule: Rule:
Name: Name:
8. SF6 16. Sn(Cr2O7)
Rule: Rule:
Name: Name:
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II. Name the following compounds.
First, identify whether these compounds are ionic or covalent. Then, use the correct formula writing rules to
write the correct chemical formulas for each compound.
Compound Name Chemical Formula
1) copper (II) chlorite
2) sodium hydroxide
3) cobalt (III) oxalate
4) ammonium sulfide
5) aluminum cyanide
6) tetraphosphorous pentoxide
7) potassium permanganate
8) manganese (III) chloride
9) calcium bromate
10) antimony tribromide
11) zinc phosphate
12) copper (II) bicarbonate
13) manganese (IV) carbonate
14) lead (IV) nitride
15) pentacarbon decahydride
III. Write the chemical formula of the following compounds.
First, identify whether these compounds are ionic or covalent. Then, use the correct naming rules to
write the correct names for each compound.
Chemical Formula Compound Name
1) CdBr2
2) Cr(Cr2O7)3
3) SBr2
4) (NH4)2CrO4
5) Pt3(PO3)4
6) Al(ClO4)3
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7) Ca(C2H3O2)2
8) V(SO4)2
9) Ag2CO3
10) N2S3
11) FeSO3
12) Zn(NO2)2
13) C6H12O6
14) Mn(OH)7
15) Ni(NO3)2
References:
John McMurry and Robert C. Fay (2004). Chemistry, 4th ed. Upper Saddle River NJ: Pearson/Prentice Hall,
p. 56-63.
George E. Shankle & Harold W. Peterson, Laboratory Manual for Chemistry 1411. University publication at
Angelo State University, San Angelo, TX 76909, p. 27-31.
Retrieved:http://www.angelo.edu/faculty/kboudrea/general/formulas_nomenclature/Formulas
omenclature.htm
https://www.anderson5.net/cms/lib/SC01001931/Centricity/Domain/2111/Ternary%20practice.pdf
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