Compounds and Naming

G.10 Science—Chemistry Shaftesbury High School

Shaftesbury High School 2240 Grant Avenue Winnipeg, Manitoba R3P 0P7

Phone: 204-888-5898 Fax: 204-896-5492

http://www.pembinatrails.ca/shaftesbury/

Compounds and Naming

G.10 Science—Naming and Compounds Shaftesbury High School

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 = _________

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...


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 = _________


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 ele-

ment. 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

Type of Atom # of Atoms

Total

Na2CO3


Total

Ca3(PO4)2


Total

K2CrO4


Total

3BaCl2


Total

Pb(NO3)2


Total

4Al2(CO3)3


NH4C2H3O2

Total


2(NH4)2Cr2O7

Total

G.10 Science—Subscripts and Coefficients Shaftesbury High School

Calculate the number of each type of atom in the following compounds.

Calculate the number of each type of atom and the total number of atoms.

1. NaOH Na _____ O ______ H ______

2. H3PO4 H ______ P ______ O ______

3. ZnCO3 Zn _____ C ______ O ______

4. NH4C2H3O2 N ______ H ______ C ______ O ______

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 ______

1. 3Fe2O3 Fe _____ O _____ Total _____

2. 2NaHSO4 Na _____ H _____ S _____ O _____ Total _____

3. 4Al2(CO3)3 Al ______ C _____ O _____ Total _____

4. 3K2SO4 K ______ S _____ O _____ Total _____

5. 4Zn3(PO4)2 Zn _____ P _____ O _____ Total _____

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

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.

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 for-

mula tells that 2 atoms of hydrogen will bond with 1 atom of oxygen.

Bohr

Lewis

Bohr

Lewis

CH4

C is a non-metal and Cl is a non-metal, therefore the bond is covalent. The Chemical for-

mula tells us that 1 C atom will join with 4 H atoms.

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 com-

pound using a Lewis Dot diagram.

1. CaCl2 2. H2

3. MgF2

5. NF3

7. Na2O

9. MgBr2

11. Cl2

4. NaCl

6. K3N

8. NH3

10. LiF

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.

Naming Binary Ionic Compounds

1.

2.

Write the names for the following 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 _________________________________

Eg. LiF _________________________________

Eg 2. CaCl2 _________________________________

Eg 3. Na2O _________________________________

1. Li2O _________________________________

2. NaI _________________________________

3. Rb2S _________________________________

4. AlP _________________________________

5. CaF2 _________________________________

1. Magnesium Oxide _________________________________

2. Calcium Fluoride _________________________________

3. Cesium Sulfide _________________________________

4. Aluminum Oxide _________________________________

5. Potassium Chloride _________________________________

Write the formulas for the following compounds:

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.

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 inden-

tations as female pieces.

Male puzzle pieces represent positively charged ions because they transfer their elec-

trons 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.

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

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 com-

pounds as possible.

1. Select a specific ion symbol for each coloured piece.

2. Record the elements chosen for each charge in the box space provided.

3. Record the chemical formula of each of your puzzle compounds in the table below.

4. 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.

Ionic Compounds: Names and Formulas Assignment

1. Write the formulas for the following compounds.

2. Write the names for the following compounds.

1. Fe2O3 _________________________________

2. PbO2 _________________________________

3. NiCl2 _________________________________

4. CrN _________________________________

5. HgO _________________________________

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 ________________

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 Polya-

tomic ion has its own name. For example…

We can still write formulas for compounds which contain polyatomic ions. For example...

Make sure you place ______________________________________________________

_____________________________________.

When Naming compounds with polyatomic ions _________________________________

______________________________________________________________________.

For Example...

Sodium Nitrate ______________

Sodium Phosphate ______________

Calcium Nitrate ______________

Copper (II) Nitrate ______________

Sulfate Ion ______________

Nitrate Ion ______________

Phosphate Ion ______________

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 Chloride

Cl1- Hydroxide

OH1- Nitrate NO3

1- Sulfate SO4

2- Sulfide

S2- Carbonate

CO32-

Phosphate PO4

3-

Hydrogen H1+

Sodium Na1+

Ammonium NH4

1+

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+

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 ______________________

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—Polyatomic Ions with Multiple Charges Shaftesbury High School

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

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.

1. Disulfur Oxide _________________________________

2. Nitrogen Trichloride _________________________________

3. Carbon Monoxide _________________________________

4. Tetrabromine Nonoxide _________________________________

5. Arsenic Trihydride _________________________________

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 _________________________________

g. CCl4 _________________________________

h. NO3 _________________________________

i. CS2 _________________________________

j. NO _________________________________

k. CO2 _________________________________

l. PCl3 _________________________________

Write the covalent compound name from the following formulas.

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—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:

Molar Mass:

Lead (II) Iodide Formula:

Molar Mass:

Copper (II) Nitrate Formula:

Molar Mass:

Sodium Hydroxide Formula:

Molar Mass:

Lead (IV) Oxide Formula:

Molar Mass:

Calcium Cyanide Formula:

Molar Mass:

G.10 Science—Molar Mass Conversions Shaftesbury High School

Dinitrogen Pentoxide Formula:

Molar Mass:

Calcium Acetate Formula:

Molar Mass:

Nickel (II) Sulfate Formula:

Molar Mass:

Potassium Dichromate Formula:

Molar Mass:

Carbon Dioxide Formula:

Molar Mass:

Iron (III) Chloride Formula:

Molar Mass:

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: ____________


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Compounds and Naming