G.10 Science—Chemistry
Shaftesbury High School
Compounds and Naming
Shaftesbury High School
2240 Grant Avenue
Winnipeg, Manitoba
R3P 0P7
Phone: 204-888-5898
Fax: 204-896-5492
http://www.pembinatrails.ca/shaftesbury/
G.10 Science—Naming and Compounds
Shaftesbury High School
Compounds
There are about ____________________ pure substances that have been identified.
Chemical Formulas
A chemical formula acts as a recipe for a compound, it tells us...
Reading a Chemical Formula:
Eg. Consider table salt (Sodium Chloride—NaCl).
Count the Atoms
Na Atoms = _________
Cl Atoms = _________
Sometimes there are subsctripts present.
Eg 2. Consider water (Dihydrogen Oxide—H20)
H Atoms = _________
O Atoms = _________
G.10 Science—Naming and Compounds
Shaftesbury High School
Sometimes there are brackets with a subscript…
Eg 3. Calcium Hydroxide—Ca(OH)2
Ca Atoms = _________
O Atoms = _________
H Atoms = _________
Sometimes there are subscripts in the brackets…
Eg 4. Calcium Nitrate—Ca(NO3)2
Ca Atoms = _________
O Atoms = _________
N Atoms = _________
G.10 Science—Naming and Compounds
Shaftesbury High School
Review—Counting Atoms
1. The symbol of an element represents one atom of that element.
Eg. Ca
2. A subscript is a number written at the lower right corner behind the symbol of an element. If there is more than one atom of the element in the molecule, then a subscript
is used to indicate the number of atoms.
Eg 2. N2
3. A subscript outside a bracket multiplies all the elements inside the brackets.
Eg 3. Ba3(PO4)2
4. i. A coefficient is a number written in front of a chemical symbol and indicates the
number of atoms of that element.
Eg 4. 3C
OR
ii. A coefficient is a number written in front of a chemical formula and indicates the
number of molecules of that compound.
Note: A coefficient multiplies the number of atoms of each element in the formula.
Eg 5. 2H2O
Eg 6. 3FeSO4
Eg 7. 4Cu(NO3)2
G.10 Science—Counting Atoms Worksheet
Shaftesbury High School
Na2CO3
Type of Atom
Ca3(PO4)2
# of Atoms
Type of Atom
Total
Total
K2CrO4
3BaCl2
Type of Atom
# of Atoms
Type of Atom
# of Atoms
# of Atoms
Total
Total
4Al2(CO3)3
Type of Atom
Pb(NO3)2
# of Atoms
Type of Atom
Total
Total
NH4C2H3O2
2(NH4)2Cr2O7
Type of Atom
Total
# of Atoms
Type of Atom
Total
# of Atoms
# of Atoms
G.10 Science—Subscripts and Coefficients
Shaftesbury High School
Calculate the number of each type of atom in the following compounds.
1. NaOH
Na _____
O ______
H ______
2. H3PO4
H ______
P ______
O ______
3. ZnCO3
Zn _____
C ______
O ______
4. NH4C2H3O2
N ______
H ______
C ______
5. Ca(ClO3)2
Ca _____
Cl ______
O ______
6. Zn(NO3)2
Zn _____
N ______
O ______
7. Al2(SO4)3
Al ______
S ______
O ______
8. (NH4)2SO4
N ______
H ______
S ______
O ______
O ______
Calculate the number of each type of atom and the total number of atoms.
1. 3Fe2O3
Fe _____
O _____
Total
_____
2. 2NaHSO4
Na _____ H _____
S _____
Total
_____
3. 4Al2(CO3)3
Al ______ C _____
O _____
Total
_____
4. 3K2SO4
K ______
S _____
O _____
Total
_____
5. 4Zn3(PO4)2
Zn _____
P _____
O _____
Total
_____
O _____
G.10 Science—Chemical Bonding
Shaftesbury High School
Chemical Bonding
Atoms must gain, lose, or share electrons to obtain full valence shells and become stable.
Chemical Bond
Compound
Molecule
Atom
Ion
Element
Chemical Formula
Valence (Combining Capacity)
G.10 Science—Ionic Bonding
Shaftesbury High School
Ionic Bonding
Examples of Compounds with Ionic Bonds
KCl
K is a metal and Cl is a non-metal, therefore the bond is ionic. The Chemical formula tells
us that 1 K atom will join with 1 Cl.
Bohr
Lewis
AlCl3
Al is a metal and Cl is a non-metal, therefore the bond is ionic. The Chemical formula
tells us that 1 Al atom will join with 3 Cl.
Bohr
Lewis
G.10 Science—Covalent Bonding
Shaftesbury High School
Covalent Bonding
Examples of Compounds with Covalent Bonds
H2O
H is a non-metal and O is a non-metal, therefore the bond is covalent. The Chemical formula tells that 2 atoms of hydrogen will bond with 1 atom of oxygen.
Bohr
Lewis
CH4
C is a non-metal and Cl is a non-metal, therefore the bond is covalent. The Chemical formula tells us that 1 C atom will join with 4 H atoms.
Bohr
Lewis
G.10 Science—HOFBrINCl Clown
Shaftesbury High School
When two identical atoms link together, the arrangement is called a diatomic molecule.
H-O-F-Br-I-N-Cl the clown will help you remember diatomic molecules. Take a close look at
his ear (and the number 2), and remember that all of these elements exist in pairs.
G.10 Science—Naming and Compounds Assignment
Shaftesbury High School
Additional Resource
Identify whether the bond between atoms is ionic or covalent and then draw the compound using a Lewis Dot diagram.
1. CaCl2
2. H2
3. MgF2
4. NaCl
5. NF3
6. K3N
7. Na2O
8. NH3
9. MgBr2
10. LiF
11. Cl2
12. HBr
G.10 Science—Naming Ionic Compounds
Shaftesbury High School
Writing Formulas
An ionic compound consists of a ____________________ and a __________________.
Metals ______________ electrons to form ________________ ions called
_______________________.
Eg. Draw the ionic bond between Magnesium and Fluorine.
An easier way to determine the formula of an ionic compound without drawing the bond
structure is to make sure that the __________________ charges are equal to the
______________________ charges.
G.10 Science—Ionic Compounds
Shaftesbury High School
Steps for Naming Ionic Compounds
1. Write the element symbol with the charge of the ion, as a superscript (Na-1), next to
it.
2. If charges are already equal just write the formula as it is.
Eg. Magnesium and Oxygen
3. If the charges are not equal, adjust the quantity of each element so that the charges
of the cations and anions are equal.
Eg. Magnesium and Fluorine
Eg 2. Potassium and Nitrogen
Eg 3. Calcium and Nitrogen
The Criss-Cross Method
Eg. Calcium and Nitrogen
G.10 Science—Ionic Compounds
Shaftesbury High School
Make the formulas for the following ionic compounds.
1. Sodium and Oxygen
_________________________________
2. Magnesium and Bromine
_________________________________
3. Potassium and Chlorine
_________________________________
4. Calcium and Sulfur
_________________________________
5. Aluminum and Iodine
_________________________________
6. Aluminum and Nitrogen
_________________________________
Naming Binary Ionic Compounds
1.
2.
Eg.
LiF
_________________________________
Eg 2. CaCl2
_________________________________
Eg 3. Na2O
_________________________________
Write the names for the following compounds:
1. Li2O
_________________________________
2. NaI
_________________________________
3. Rb2S
_________________________________
4. AlP
_________________________________
5. CaF2
_________________________________
Write the formulas for the following compounds:
1. Magnesium Oxide
_________________________________
2. Calcium Fluoride
_________________________________
3. Cesium Sulfide
_________________________________
4. Aluminum Oxide
_________________________________
5. Potassium Chloride
_________________________________
G.10 Science—Binary Ionic Compounds Puzzle
Shaftesbury High School
Objectives
Discover how metal cations and non-metal anions combine in specific ratios to form
neutral compounds.
Match puzzle pieces with their respective ion groups on the periodic table
Combine puzzle pieces to form neutral binary ionic compounds
Write the chemical formulas for neutral binary ionic compounds.
Puzzle Piece
Picture
Charge
Number of Pieces
One protrusion
+1
3
Two protrusions
+2
3
Three protrusions
+3
2
One indentation
–1
3
Two indentations
–2
3
Three indentations
–3
2
TOTAL = 16
Rules of the Game
Each puzzle piece represents a separate ion that is either positively or negatively
charged.
Consider puzzle pieces with protrusions as male pieces and puzzle pieces with indentations as female pieces.
Male puzzle pieces represent positively charged ions because they transfer their electrons to make negatively charged female ions and form ionic compounds.
The challenge of the game is to construct as many different combinations of neutrally
charged binary ionic compounds as possible.
A neutrally charged binary ionic compound is made when as many male pieces of one
type are combined with the appropriate number of female puzzle pieces of a second
type so that no protrusions or indentations remain.
G.10 Science—Binary Ionic Compounds Puzzle
Shaftesbury High School
Directions
Empty the contents of the plastic bag onto you desk and make sure you have the
necessary number of puzzle pieces.
Arrange the pieces on your desk to make the periodic table of the ions, omitting the
transition metals. Check your final product with the instructor before moving on to
the next step. (3 marks)
Binary Ionic Compound Chemical Formulas (9 marks)
Construct as many different combinations of neutrally charged binary ionic compounds as possible.
1.
2.
3.
4.
Select a specific ion symbol for each coloured piece.
Record the elements chosen for each charge in the box space provided.
Record the chemical formula of each of your puzzle compounds in the table below.
Finally, sketch an image of the compound created with the puzzle pieces.
1+ & 1–
1+ & 2–
1+ & 3–
2+ & 2–
2+ & 1–
3+ & 1–
3+ & 3–
2+ & 3–
3+ & 2–
/12
G.10 Science—Metals With More Than One Cation
Shaftesbury High School
Some transition metals can have more than one cation. For example, copper can have a
+1 or a +2 charge.
Eg. Write the formula for copper (I) sulfide.
Eg 2. Write the formula for copper (II) sulfide.
Write the chemical formula for each of the following compounds.
1. Copper (I) Oxide
_________________________________
2. Lead (IV) Bromide
_________________________________
3. Iron (III) Sulfide
_________________________________
4. Nickel (II) Fluoride
_________________________________
5. Manganese (IV) Sulfide
_________________________________
Finding the name of a compound using the stock system (use a reverse criss-cross
method).
Eg. FeCl3 (Hint: Iron can have a charge of +2 or +3)
Eg 2. Cu2S
G.10 Science—Metals With More Than One Cation
Shaftesbury High School
Write the names for the following compounds.
1. Fe2O3
_________________________________
2. PbO2
_________________________________
3. NiCl2
_________________________________
4. CrN
_________________________________
5. HgO
_________________________________
Ionic Compounds: Names and Formulas Assignment
1. Write the formulas for the following compounds.
a. Magnesium Oxide
________________ k. Copper (I) Bromide ________________
b. Sodium Fluoride
________________ l. Tin (II) Iodide
c. Aluminum Nitride
________________ m. Iron (III) Chloride ________________
d. Potassium Sulfide
________________ n. Calcium Phosphide ________________
e. Lithium Iodide
________________ o. Lead (II) Oxide
________________
f. Calcium Bromide
________________ p. Lead (IV) Flouride
________________
g. Beryllium Oxide
________________ q. Tin (IV) Bromide
________________
h. Nickel Chloride
________________ r. Copper (II) Sulfide
________________
i. Magnesium Nitride
________________ s. Iron (II) Oxide
________________
j. Aluminum Sulfide
________________ t. Calcium Nitride
________________
________________
2. Write the names for the following compounds.
a. Li2O
________________
k. PbS
________________
b. AlCl3
________________
l. SnO2
________________
c. MgS
________________
m. Na2S
________________
d. CaO
________________
n. Mg3P2
________________
e. KBr
________________
o. NiO
________________
f. BeF
________________
p. CuI
________________
g. Na3N
________________
q. PbCl4
________________
h. Al2O3
________________
r. FeP
________________
i. CuCl2
________________
s. CaF2
________________
j. FeBr3
________________
t. K3P
________________
G.10 Science—Polyatomic Ions
Shaftesbury High School
Polyatomc ions are ions that are made of more than _____________ atom. Each Polyatomic ion has its own name. For example…
Sulfate Ion
______________
Nitrate Ion
______________
Phosphate Ion
______________
We can still write formulas for compounds which contain polyatomic ions. For example...
Sodium Nitrate
______________
Sodium Phosphate
______________
Calcium Nitrate
______________
Copper (II) Nitrate
______________
Make sure you place ______________________________________________________
_____________________________________.
When Naming compounds with polyatomic ions _________________________________
______________________________________________________________________.
For Example...
NaNO3
______________
Ca3(PO4)2
______________
CuSO4
______________
NH4Cl
______________
G.10 Science—Criss Cross Method
Shaftesbury High School
Complete the following table, being sure that the total charge on the resulting compound is
zero.
Ions
Hydrogen
H1+
Sodium
Na1+
Ammonium
NH41+
Potassium
K1+
Calcium
Ca2+
Magnesium
Mg2+
Aluminum
Al3+
Ferrous
Fe2+
Iron (II)
Fe2+
Ferric
Fe3+
Iron (III)
Fe3+
Plumbous
Pb2+
Stannic
Sn4+
Copper (I)
Cu1+
Cupric
Cu2+
Chloride
Cl1-
Hydroxide
OH1-
Nitrate
NO31-
Sulfate
SO42-
Sulfide
S2-
Carbonate
CO32-
Phosphate
PO43-
G.10 Science—Ionic Compounds: Polyatomic Ions
Shaftesbury High School
Write the name of each of the following compounds.
1. NH4Cl
______________________
2. HClO2
______________________
3. Ca(BrO3)2
______________________
4. BeSO4
______________________
5. (NH4)3N
______________________
6. NH4NO3
______________________
7. Sr3(PO4)2
______________________
8. Zn(ClO3)2
______________________
9. AgIO3
______________________
10. K2Cr2O7
______________________
Write the chemical formula for each of the given names.
11. sodium chromate
______________________
12. barium nitrate
______________________
13. ammonium sulfate
______________________
14. aluminum hydroxide
______________________
15. calcium phosphate
______________________
16. cesium cyanide
______________________
17. sodium nitrite
______________________
18. calcium acetate
______________________
19. beryllium chlorite
______________________
20. rubidium sulfite
______________________
G.10 Science—Polyatomic Ions with Multiple Charges
Shaftesbury High School
Write the name of each of the following compounds.
1. V(ClO3)5
______________________
2. Re(SO4)3
______________________
3. Os(IO3)3
______________________
4. Ir3(PO4)4
______________________
5. Pd(SO3)2
______________________
6. AuNO3
______________________
7. FePO4
______________________
8. Ni(BrO3)2
______________________
9. Pb(CN)4
______________________
10. Mn(Cr2O7)2
______________________
Write the chemical formula for each of the given names.
11. copper (II) hydroxide
______________________
12. rhenium nitrate
______________________
13. niobium (III) sulfate
______________________
14. platinum (IV) iodate
______________________
15. molybdenum phosphate
______________________
16. titanium (II) cyanide
______________________
17. gold (I) thiosulfate
______________________
18. iron (III) acetate
______________________
19. cobalt (II) chlorate
______________________
20. tin (IV) sulfite
______________________
G.10 Science—Naming Covalent Compounds
Shaftesbury High School
Covalent compounds have a different naming system since there are no ions involved
and no need to balance charges.
Eg. CO2
Eg 2. CO
Covalent compounds are named using __________________________.
1-
6-
2-
7-
3-
8-
4-
9-
5-
10 -
Simply,
1. PCl3
_________________________________
2. N2O4
_________________________________
3. H2O
_________________________________
4. CF4
_________________________________
5. SiO4
_________________________________
G.10 Science—Naming Covalent Compounds
Shaftesbury High School
Writing Covalent Formulas
1. Disulfur Oxide
_________________________________
2. Nitrogen Trichloride
_________________________________
3. Carbon Monoxide
_________________________________
4. Tetrabromine Nonoxide
_________________________________
5. Arsenic Trihydride
_________________________________
Covalent Compound Review
1. What is a covalent compound? What elements are involved?
2. How many electrons are shared in a covalent bond? Provide examples to support your
answer.
Write the chemical formula for each of the following covalent compounds.
a. Carbon Monoxide
_________________________________
b. Nitrogen Trifluoride
_________________________________
c. Dinitrogen Oxide
_________________________________
d. Dihydrogen Oxide
_________________________________
e. Sulfur Dioxide
_________________________________
f. Silicon Flouride
_________________________________
Write the covalent compound name from the following formulas.
g. CCl4
_________________________________
h. NO3
_________________________________
i. CS2
_________________________________
j. NO
_________________________________
k. CO2
_________________________________
l. PCl3
_________________________________
G.10 Science—Naming Assignment
Shaftesbury High School
Name the following covalent compounds.
1. HI
__________________________________________
2. CCl4
__________________________________________
3. Cl2O
__________________________________________
4. HBr
__________________________________________
5. PF3
__________________________________________
6. ICl
__________________________________________
7. S2O
__________________________________________
8. P4O6
__________________________________________
9. CO2
__________________________________________
10. PH3
__________________________________________
11. SiCl4
__________________________________________
12. CBr4
__________________________________________
13. AsH3
__________________________________________
14. Br4O9
__________________________________________
15. NO2
__________________________________________
16. CO
__________________________________________
17. IF7
__________________________________________
18. S4N4
__________________________________________
19. NCl3
__________________________________________
20. H2O
__________________________________________
G.10 Science—Naming and Compounds Web
Shaftesbury High School
G.10 Science—Covalent Binary Compounds
Shaftesbury High School
Write the name of each of the following compounds.
1. HF
______________________
2. H2S
______________________
3. NO
______________________
4. N2O
______________________
5. NO2
______________________
6. N2O5
______________________
7. SO2
______________________
8. CBr4
______________________
9. C2H6
______________________
10. C4H10
______________________
Write the chemical formula for each of the given names.
11. Nitrogen Triiodide
______________________
12. Dinitrogen Tetroxide
______________________
13. Sulfur Trioxide
______________________
14. Carbon Monoxide
______________________
15. Dihydrogen Monoxide
______________________
16. Hydrogen Monobromide
______________________
17. Phosphorus Trichloride
______________________
18. Tricarbon Octahydride
______________________
19. Carbon Tetrahydride
______________________
20. Dicarbon Tetrahydride
______________________
G.10 Science—Naming and Compounds
Shaftesbury High School
G.10 Science—Naming and Compounds
Shaftesbury High School
G.10 Science—Naming and Compounds
Shaftesbury High School
G.10 Science—Molar Mass
Shaftesbury High School
The molar mass of a molecule is calculated by
Eg. H2O
Eg 2. CH4
G.10 Science—Molar Mass Conversions
Shaftesbury High School
For all calculations, show your work and include units.
Calculate the molar mass for each of the following compounds. Include units.
Calcium Nitrate
Formula:
Formula:
Molar Mass:
Sodium Hydroxide
Formula:
Molar Mass:
Molar Mass:
Lead (IV) Oxide
Formula:
Molar Mass:
Molar Mass:
Copper (II) Nitrate
Lead (II) Iodide
Formula:
Calcium Cyanide
Molar Mass:
Formula:
G.10 Science—Molar Mass Conversions
Shaftesbury High School
Dinitrogen Pentoxide
Formula:
Molar Mass:
Nickel (II) Sulfate
Molar Mass:
Formula:
Molar Mass:
Formula:
Potassium Dichromate Formula:
Molar Mass:
Molar Mass:
Carbon Dioxide
Calcium Acetate
Formula:
Iron (III) Chloride
Molar Mass:
Formula:
G.10 Science—Molar Mass Assignment
Shaftesbury High School
Calculate the molar mass of the following chemicals. Ensure that you show all your
work.
1. Cl2
ANS: ____________
2. KOH
ANS: ____________
3. BeCl2
ANS: ____________
4. FeCl3
ANS: ____________
5. BF3
ANS: ____________
6. CCl2F2
ANS: ____________
7. Mg(OH)2
ANS: ____________
8. UF6
ANS: ____________
9. SO2
ANS: ____________
10. H3PO4
ANS: ____________
11. (NH4)2SO4
ANS: ____________
12. CH3COOH
ANS: ____________
13. Pb(NO3)2
ANS: ____________
14. Ga2(SO3)3
ANS: ____________
G.10 Science—Naming and Compounds
Shaftesbury High School