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Introductory Worksheet Package –Grade 11 University Level

Worksheet 1 – Safety – ApparatusWorksheet 2 – Safety – WhimisWorksheet 3 – Grade 10 ReviewWorksheet 4 – Ionic Naming Part 1Worksheet 5 – Ionic Naming Part 2Worksheet 6 – Ionic Naming Part 3Worksheet 7 – Ionic Naming Part 4Worksheet 8 – Molecular NamingWorksheet 9 – Naming ReviewWorksheet 10 – Naming ReviewWorksheet 11 – Balancing ReviewWorksheet 12 – Nomenclature 1Worksheet 13 – Nomenclature 2Worksheet 14 – Nomenclature 3Worksheet 15 – Nomenclature 4Worksheet 16 –Nomenclature 5Worksheet 17 – Types of ReactionsWorksheet 18 – Types of ReactionsWorksheet 19 – Net Ionic Equations

Worksheet 1 –Safety – Apparatus

Worksheet 2 – Safety – Whimis

Worksheet 3 – Grade 10 Review

A. Vocabulary

1. Anything that has mass and takes up space is________________2. The smallest independent unit of matter that cannot be separated by common chemical means

is the _______________________3. The left side of the periodic table is composed mostly of _________________4. Energy absorbing reactions are known as __________________5. The right side of the periodic table is composed mostly of _________________6. The “staircase” region of the periodic table has ___________________7. A type of reaction in which two or more reactants combine to form a larger product is called

________________8. Vertical columns in the periodic table are called ___________________9. The number of electron shells a helium atom has is ________________10. A subatomic particle found in the nucleus that has no charge is called a____________11. The number of electrons found in the ______________ shell determines the reactivity of the

atom12. The number of ______________ in the nucleus determines the atomic number13. An atom has an equal number of __________ and ____________14. An ion has either lost or gained ________________15. An atom’s _____________ number equals the number of protons + neutrons16. _______________ reside in the orbital/shells surrounding the nucleus17. _______________ occur when atoms of the same type have different atomic masses due to

differing numbers of neutrons18. The modern periodic table arranges elements in increasing atomic number to show a periodic

repetition of ________________19. When a metal and a non-metal react with one another they form an __________ bond20. When two or more non-metals react with one another they form a ______________ in which

the bonds are called ______________________21. The type of bond in which electrons are shared is called a __________________22. When magnesium ionizes, its charge is positive _______________23. ___________________________ are reaction in which one element replaces another.24. Group 18 elements have a full shell, which is called a _______ ________25. The chemicals at the end of a chemical reaction can also be called ______________26. Group 13 elements have __________ valence electrons27. All atoms (except Hydrogen and Helium) desire ________________ electrons in their outer

shell28. A positive ion is called a _____________, where a negative ion is called an ________29. Metals such as nickel, copper, platinum, gold are called _______________ metals30. Sulfur needs ______________ electrons in order to achieve a stable octet31. The small number written at the lower right of a symbol such as CO2 is called a

___________32. The number written in the front of a symbol such as 3 NaOH is called a ___________33. ____________ describes a compound that has two identical atoms i.e. O2 34. These types of reactions always involve oxygen _______________________ 35. _____________ refers to the starting materials in a chemical reactionB. Review Questions1. Distinguish between an atom and a molecule.

2. a) Distinguish between valence electrons and stable octet. How do the number of electrons in the outer shell of an atom determine the atom’s reactivity?

b) Why do Hydrogen and Helium only require two electrons in their outer shell to be stable?

3. For each of the following draw: Bohr diagrams, Bohr-Rutherford diagrams and Lewis dot diagrams

a) Nitrogen atom

b) F- ion

c) Mg2+ ion

4. Counting atoms – Fill in the chart below.Chemical Formula

# of Each Type of Atom

Total Number of

Atoms

What Type of Bond is Found in the Compound?

Is this an Ionic Compound or a

Molecule?

2H2O

5Ca3P2O8

3BaCl2

8Pb(NO3)2

3NO2

Worksheet 4 - Naming Ionic Compounds Part 1

(Binary compounds with Group 1, 2 or 13 metals)

Binary compounds: have only two kinds of elements, if there are three or more it is not a binary compound.

Naming

1. Metal goes first and you get the name directly from the periodic table.

2. Non-metal goes second. The ending changes to “ide”

Name of element Name at end of compound

Name of element

Name at end of compound

Fluorine Fluoride Oxygen OxideChlorine Chloride Sulfur SulfideBromine Bromide Nitrogen NitrideIodine Iodide Phosphorus Phosphide

Write the chemical formula for each of the following.

1. lithium chloride 2. beryllium chloride 3. sodium oxide

4. potassium sulfide 5. magnesium phosphide 6. aluminum fluoride

7. calcium nitride 8. magnesium oxide 9. beryllium nitride

10. potassium carbide 11. potassium nitride 12. potassium fluoride

13. aluminum nitride 14. sodium fluoride 15. calcium carbide

16. barium bromide 17. francium phosphide 18. gallium sulfide

Write the chemical names of the following compounds.

1. LiF 2. Li2O 3. AlP

4. NaCl 5. K2S 6. Ca3N2

7. MgO 8. BeS 9. Ca2C

10. Li4C 11. AlF3 12. KBr

13. Ga2O3 14. CsI 15. SrAt2

16. Rb3P 17. BaS 18. Al4C3

Worksheet 5 - Naming Ionic CompoundsPart 2

(Binary compounds with Group 3 - 12 metals)

Naming(STOCK SYSTEM)

1. Metal goes first and you get the name directly from the periodic table.

2. Immediately after the metal in brackets write the charge of the metal ion in roman numerals.


The metals in Groups 3 – 12 can have more then one charge on the ion (polyvalent ions) so when you name them you have to add in the charge of the metal ion by using roman numerals. This method of naming is called the stock system and is used only for the polyvalent ions. There is another method of naming the polyvalent ions, which we will look at in part 3 of naming ionic compounds.

Element Cations Name of Cation Element Cations Name of CationAntimony Sb3+ Antimony (III) Lead Pb2+ Lead (II)

Sb5+ Antimony (V) Pb4+ Lead (IV)Arsenic As3+ Arsenic (III) Manganese Mn2+ Manganese (II)

As5+ Arsenic (V) Mn4+ Manganese (IV)Cobalt Co2+ Cobalt (II) Mercury Hg+ Mercury (I)

Co3+ Cobalt (III) Hg2+ Mercury (II)Copper Cu+ Copper (I) Nickel Ni2+ Nickel (II)

Cu2+ Copper (II) Ni3+ Nickel (III)Gold Au+ Gold (I) Tin Sn2+ Tin (II)

Au3+ Gold (III) Sn4+ Tin (IV)Iron Fe2+ Iron (II) Titanium Ti3+ Titanium (III)

Fe3+ Iron (III) Ti4+ Titanium (IV)

Example copper chloride

CuCl or CuCl2 Both are copper chloride

copper (I) chloride copper (II) chloride Need the charge on copper

Write the names of the following compounds.

1. CuO 2. Cu2O 3. Sb2O5

4. Sb2O3 5. PbCl4 6. NiBr2

7. AuP 8. Au3P 9. FeO

10. Sn3P4 11. Fe2C 12. Co4C3

13. Hg3N 14. MnS2 15. AsI5

16. SnO 17. Ti2S3 18. TiF4

Write the chemical formulas of the following

1. manganese (IV) oxide 2. arsenic (V) sulfide 3. cobalt (II) chloride

4. antimony (III) bromide 5. iron (II) carbide 6. gold (I) iodide

7. mercury (II) nitride 8. cobalt (III) phosphide 9. nickel (III) oxide

10. titanium (IV) carbide 11. antimony (V) oxide 12. tin (II) fluoride

13. lead (IV) nitride 14. arsenic (V) bromide 15. gold (II) sulfide

16. antimony (V) phosphide 17. copper (I) oxide 18. gold (I) carbide


(Binary compounds with Group 3 - 12 metals)

Naming(CLASSICAL SYSTEM)

1. Metal goes first. Some metals use special names. For all of the metals the ending changes to “ous” or “ic” (“ous” is for the lower ion of the metal, while “ic” is for the higher ion of the metal)


Element Cations Name of Cation Element Cations Name of CationAntimony Sb3+ Antimonous Lead Pb2+ Plumbous

Sb5+ Antimonic Pb4+ PlumbicArsenic As3+ Arsenous Manganese Mn2+ Manganous

As5+ Arsenic Mn4+ ManganicCobalt Co2+ Cobaltous Mercury Hg+ Mercurous

Co3+ Cobaltic Hg2+ MercuricCopper Cu+ Cuprous Nickel Ni2+ Nickelous

Cu2+ Cupric Ni3+ NickelicGold Au+ Aurous Tin Sn2+ Stannous

Au3+ Auric Sn4+ StannicIron Fe2+ Ferrous Titanium Ti3+ Titaniumous

Fe3+ Ferric Ti4+ Titaniumic

Example copper chloride

CuCl (Cu+) or CuCl2 (Cu2+) Both are copper chloride

cuprous chloride cupric chloride Must indicate the charge with “ous” or “ic”

Write the names of the following compounds.

1. CuO 2. Cu2O 3. Sb2O5

4. Sb2O3 5. PbCl4 6. NiBr2

7. AuP 8. Au3P 9. FeO

10. Sn3P4 11. Fe2C 12. Co4C3

13. Hg3N 14. MnS2 15. AsI5

16. SnO 17. Ti2S3 18. TiF4

Write the chemical formulas of the following

1. manganic oxide 2. arsenic sulfide 3. cobaltous chloride

4. antimonous bromide 5. ferrous carbide 6. aurous iodide

7. mercuric nitride 8. cobaltic phosphide 9. nickelic oxide

10. titaniumic carbide 11. antimonic oxide 12. stannous fluoride

13. plumbic nitride 14. arsenic bromide 15. auric sulfide

16. antimonic phosphide 17. cuprous oxide 18. aurous carbide


(For compounds that are not binary)

There are groups of non-metals that like to stay together and have a total charge these are called polyatomic ions.

Naming

1. Metal goes first and all previous rules for the metals apply.

1a) Group 1, 2, 13 metals name directly from periodic table1b) Group 3 – 12 metals STOCK SYSTEM name from periodic table plus identify the charge using roman numerals1c) Group 3 – 12 metals CLASSICAL SYSTEM “ous” identifies lower ion and “ic” identifies higher ion

2. Negative polyatomic ion second and you get the name from the table below.

Polyatomic ions

Name ofpolyatomic ion

Ion formula Name ofpolyatomic ion

Ion formula

Nitrite NO2- Hydrogen Carbonate

(Bicarbonate)HCO3

-

Nitrate NO3-

Sulfite SO32- Carbonate CO3

2-

Sulfate SO42- Phosphate PO4

3-

Chlorite ClO2- Acetate C2H3O2

-

Chlorate ClO3- Cyanide CN-

Arsenite AsO33- Hydroxide OH-

Arsenate AsO43- Ammonium NH4

+

Name the following compounds

1. LiNO3 2. Be(HCO3)2 3. AlPO4

4. CaCO3 5. NaNO2 6. Ga(OH)3

7. Cu2SO4 8. Cu(NO3)2 9. Mg3(PO4)2

10. Sn(OH)4 11. Ba3(AsO4)2 12. (NH4)2CO3

13. Sb(C2H3O2)5 14. KCN 15. Al2(SO3)3

16. FrClO3 17. SrCO3 18. Li3(PO4)

Write the chemical formula for the following compounds

1. lithium chlorite 2. beryllium nitrate 3. calcium phosphate

4. aluminum phosphate 5. manganese (IV) hydroxide 6. ammonium sulfate

7. sodium acetate 8. nickel (II) arsenite 9. ferric cyanide

10. cobaltous sulfite 11. auric bicarbonate 12. ammonium phosphate

13. potassium acetate 14. cesium nitrate 15. magnesium arsenite

16. tin (IV) hydroxide 17. antimony (V) arsenate 18. gallium chlorate

Worksheet 8 - Naming Molecular Compounds(Binary compound with two non-metals)

Naming

1. Generally the element closer to the top left hand corner of the periodic table is named first

2. Then the second element is named. The ending changes to “ide”

3. To each of the elements you must add the proper prefix which tells you how many of each element there is.

Prefix Number it represents

Prefix Number it represents

mono 1 hexa 6di 2 hepta 7tri 3 octa 8

tetra 4 nona 9penta 5 deca 10

H2C2 HC4

Hydrogen Carbide

Dihydrogen dicarbide Hydrogen tetracarbide

Write the chemical formulas for the following chemical names

1.carbon monohydride 2.dicarbon dihydride 3.dicarbon hexahydride

4.carbon tetrafluoride 5.tricarbon tetranitride 6.disulfur hexafluoride

7.selenium moniodide 8.trihydrogen diphosphide 9.carbon dioxide

10.carbon monoxide 11.dihydrogen monoxide 12.tetraphosphorus disulfide

RULE: when the first atom has only 1 the prefix mono is not

13. tricarbon octahydride 14. tetracarbon decahydride 15. nitrogen triodide

16. diphosphorus tetrabromide 17.pentanitrogen octachloride 18. hydrogen monofluoride

Write the chemical names of the following compounds

1. CH4 2. H2O6 3. O2Cl6

4. C3F5 5. OS 6. Se2I4

7. N3O2 8. F2Cl3 9. C6O6

10. C5H10 11. Si4Br10 12. Se3Br7

13. C2P5 14. N2F6 15. N3P3

16. Se7I6 17. O5I9 18. Si3S4

Worksheet 9 – Naming Review

Group # 1 18

2 13 14 15 16 17

# of +1 valenceelectrons

charge #

Name the following compounds

1) P2O5 ____________________31) Se2C ____________________

2) CaSO4 ____________________ 32) Ni2O3 ____________________

3) KNO3 ____________________ 33) SrCl2 ____________________

4) NaF ____________________ 34) Rb3N ____________________

5) Au3PO4 ____________________ 35) Au(C2H3O2)3 ________________

6) CH4 _______________________________ 36) (NH4)4C ____________________

7) Na2CO3 ______________________ 37) Na3(AsO4) __________________

8) PbO ____________________ 38) Co(OH)2 ___________________

9) Fr3P ____________________ 39) Co(OH)3 ___________________

10) PbCl4 _____________________ 40) N5O6 ____________________

11) CuS ____________________ 41) Al(ClO3)3 ___________________

12) Mn(NO3)2 __________________ 42) B2S3 ____________________

13) Ca3P2 ____________________ 43) BaSO4 ____________________

(1)

+1

(2)

(8)

0

(2)

+2

(3)

+3

(4)

+4

(5)

-3

(6)

-2

(7)

-1

14) Mn(NO3)4 __________________ 44) Sn(CN)4 ____________________

15) NiO ____________________ 45) NH4ClO2 ___________________

16) Cu2O ____________________ 46) C6H10 ___________________

17) Fe(HCO3)3 __________________ 47) Sb3(AsO3)5 __________________

18) SnCO3 ____________________ 48) PbO2 ___________________

19) Pb(SO4)2 ___________________ 49) CuNO2 ____________________

20) CsClO3 ____________________ 50) Fr2S ____________________

21) H2S ___________________ 51) AsI5 ____________________

22) H2Cl4 ____________________ 52) P3I7 ____________________

23) C3O5 ____________________ 53) Ra3P2 ____________________

24) FeCl3 ____________________ 54) (NH4)3AsO4 _________________

25) NH4Cl ____________________ 55) BeO ____________________

26) FeO ____________________ 56) KCl ___________________

27) Li3AsO3 ____________________ 57) FeBr2 ___________________

28) Ti(HCO3)4 __________________ 58) Li3N ___________________

29) Mg3(PO4)2 __________________ 59) Cu3PO4 ____________________

30) As(CN)3 ____________________ 60) H2O ____________________

Worksheet 10 – Naming Review

Write the chemical formula for the following compounds

1) Beryllium Fluoride _____________ 31) Potassium Fluoride ______________

2) Sodium Nitride _____________ 32) Magnesium Arsenite ______________

3) Iron (II) Nitrate _____________ 33) Mercurous Phosphide ______________

4) Ammonium Phosphate __________ 34) Strontium Nitrate ______________

5) Plumbous Sulfate _____________ 35) Auric Chloride ______________

6) Plumbic Oxide _____________ 36) Lead (IV) Carbide ______________

7) Antimony (V) Cyanide _________ 37) Ammonium Acetate ______________

8) Cobaltic Oxide _____________ 38) Trinitrogen Octoxide ______________

9) Sodium Phosphide _____________ 39) Lithium Chlorite ______________

10) Ferrous Chlorate _____________ 40) Nickel (III) Nitride ______________

11) Carbon Dioxide _____________ 41) Arsenous Sulfide ______________

12) Dinitrogen Pentaflouride ________ 42) Arsenic (III) Phosphate _____________

13) Calcium Hydroxide ____________ 43) Boron Oxide ______________

14) Nickel (III) Sulfate ____________ 44) Copper (II) Bromide ______________

15) Radium Astatide ____________ 45) Trihydrogen Tetracarbide ___________

16) Sulfur Tetrabromide ___________ 46) Nonanitride Decoxide ______________

17) Cesium Bicarbonate ____________ 47) Ammonium Arsenate ______________

18) Gallium Nitride _____________ 48) Calcium Bicarbonate ______________

19) Tetrahydrogen Monocarbide ______ 49) Calcium Iodide ______________

20) Carbon Tetrachloride ____________ 50) Arsenic Acetate ______________

21) Mercury (II) Bicarbonate __________ 51) Tin (IV) Sulfate ______________

22) Lead (II) Phosphate _______________ 52) Titaniumic Phosphate ______________

23) Stannic Arsenate _____________ 53) Boron Phosphide ______________

24) Aluminum Selenide _____________ 54) Cupric Sulfide ______________

25) Barium Carbonate _____________ 55) Tetrasulfur Pentachloride ___________

26) Aurous Sulfite _____________ 56) Ammonium Phosphide _____________

27) Ammonium Acetate _____________ 57) Cesium Nitride _____________

28) Diphosphorus Pentachloride ______ 58) Cobaltic Silicide _____________

29) Titanium (III) sulfide ____________ 59) Potassium Carbonate _____________

30) Manganese (IV) iodide ___________ 60) Dihydrogen Monoxide _____________

Worksheet 11 – Balancing Review

Balance the following skeleton equations

1. H2 + O2 H2O ______________________________________

2. S8 + O2 SO3 ______________________________________

3. HgO Hg + O2 ______________________________________

4. Na + H2O NaOH + H2 ______________________________________

5. C10H16 + Cl2 C + HCl ______________________________________

6. Si2H3 + O2 SiO2 + H2O ______________________________________

7. Fe + O2 Fe2O3 ______________________________________

8. C7H6O2 + O2 CO2 + H2O ______________________________________

9. Zn + HCl ZnCl2 + H2 ______________________________________

10. FeS2 + O2 Fe2O3 + SO2 ______________________________________

11. K + Br2 KBr ______________________________________

12. Fe2O3 + H2 Fe + H2O ______________________________________

13. C2H2 + O2 CO2 + H2O ______________________________________

14. H2O2 H2O + O2 ______________________________________

15. C7H16 + O2 CO2 + H2O ______________________________________

16. SiO2 + HF SiF4 + H2O ______________________________________

17. KClO3 KCl + O2 ______________________________________

18. KClO3 KClO4 + KCl ______________________________________

19. P4O10 + H2O H3PO4 ______________________________________

20. Sb + O2 Sb4O6 ______________________________________

21. C3H8 + O2 CO2 + H2O ______________________________________

22. Fe2O3 + CO Fe + CO2 ______________________________________

23. N2 + H2 NH3 ______________________________________

24. N2 + O2 N2O ______________________________________

25. CO2 + H2O C6H12O6 + O2 ______________________________________

26. SiCl4 + H2O H4SiO4 + HCl______________________________________

27. H3PO4 H4P2O7 + H2O ______________________________________

28. CO2 + NH3 CO(NH2)2 + H2O ______________________________________

29. Al(OH)3 + H2SO4 Al2(SO4)3 + H2O___________________________________

30. Fe2(SO4)3 + KOH K2SO4 + Fe(OH)3______________________________________

31. H2SO4 + HI H2S + I2 + H2O ______________________________________

32. Al + FeO Al2O3 + Fe ______________________________________

33. Na2CO3 + HCl NaCl + H2O + CO2______________________________________

34. P4 + O2 P2O5 ______________________________________

35. K2O + H2O KOH ______________________________________

36. Al + O2 Al2O3 ______________________________________

37. Na2O2 + H2O NaOH + O2 ______________________________________

38. C + H2O CO + H2 ______________________________________

39. H3AsO4 As2O5 + H2O ______________________________________

40. Al2(SO4)3 + Ca(OH)2 Al(OH)3 + CaSO4__________________________________

41. FeCl3 + NH4OH Fe(OH)3 + NH4Cl _____________________________________

42. Ca3(PO4)2 + SiO2 P4O10 + CaSiO3 ______________________________________

43. N2O5 + H2O HNO3 ______________________________________

44. Al + HCl AlCl3 + H2 ______________________________________

45. C4H8 + O2 CO2 + H2O ______________________________________

46. C8H18 + O2 CO2 + H2O + CO + C _____________________________________

Worksheet 12 – Nomenclature 1

1. Write the formulas for each of the following compounds:

a) calcium fluoride ________ b) sodium sulfide ________

c) aluminum nitride ________ d) aluminum chloride ________

e) potassium oxide ________ f) calcium chloride ________

g) copper (II) sulfide ________ h) lead (II) bromide ________

i) silver iodide ________ j) barium nitride ________

k) iron (II) fluoride ________ l) manganese (IV) oxide ________

m) mercury (II) sulfide ________ n) ferric oxide ________

o) cuprous nitride ________ p) antimony (V) iodide ________

q) cesium carbide ________ r) strontium phosphide ________

2. Write the names for the following compounds:

a) lime, CaO2(s) ____________________

b) road salt, CaCl2(s) ____________________

c) magnesia, MgO2(s) ____________________

d) bauxite, Al2O3(s) ____________________

e) zinc ore, ZnS(s) ____________________

f) cassiterite, SnO2(s) ____________________

3. Write the IUPAC and Classical names for the following compounds if needed:

a) Na2O(s) ___________________________________________

b) SnCl4(s) ___________________________________________

c) ZnI2(s) ___________________________________________

d) SrCl2(s) ___________________________________________

e) AlBr3(s) ___________________________________________

f) PbCl4(s) ___________________________________________

4. Write the chemical formulas and names for the compounds formed by the pairs of elements below:

a) strontium and oxygen ______________________________________

b) sodium and sulfur ______________________________________

c) barium and fluorine ______________________________________

d) silver and iodine ______________________________________

e) calcium and bromine ______________________________________

f) lithium and chlorine ______________________________________


1. For each of the following compounds use stock and classical naming systems when needed:

a) NaNO3(s) ___________________________________________-found in tobacco

b) NaNO2(s) ___________________________________________-a meat preservative

c) Cu(NO3)2(s) ___________________________________________-blue solution in water

d) CuNO3(s) ___________________________________________-green solution in water

e) Al2(SO3)3(s) ___________________________________________-a food additive in pickles

f) Ca(OH)2(s) ___________________________________________-firming agent in fruit products

g) PbCO3(s) ___________________________________________-cerussite, a mineral

h) Sn3(PO4)2(s) ___________________________________________-use to fix paints to silk

i) Fe2(SO4)2(s) ___________________________________________-a mineral found on Mars

2. Write the chemical formula for each of the following compounds:

a) calcium carbonate ________________ -active ingredient in antacids

b) sodium bicarbonate ________________ -a foaming agent added to foods

c) sodium hypochlorite ________________ -a component of bleach

d) calcium sulfate ________________ -plaster of Paris

e) ammonium nitrate ________________ -used in fertilizer

f) ammonium phosphate ________________ -a leavening agent added to foods

g) copper (II) sulfate ________________ -used as a fungicide

h) sodium hydroxide ________________ -a strong base used as a washing agent

i) potassium permanganate ________________ -a traditional antiseptic

3. Use IUPAC and Archaic systems (if necessary) to name each of the following compounds:

a) LiClO3(s) ______________________ __________________________

b) BaSO4(s) ) ______________________ __________________________

c) Hg2CO3(s) ______________________ __________________________

d) Mg(NO3)2(s) ______________________ __________________________

e) Fe(BrO3)3(s) ______________________ __________________________

f) Na3PO4(s) ______________________ __________________________

g) NH4IO3(s) ______________________ __________________________

h) AuC2H3O2(s) ______________________ __________________________

i) Zn3(PO4)2(s) ______________________ __________________________

j) Sb(ClO3)5(s) ______________________ __________________________

k) MnSO4(s) ______________________ __________________________

l) KBrO(s) ______________________ __________________________

m) AlPO5(s) ______________________ __________________________

4. Write the chemical formulas for each of the following molecules:

a) nitrogen ___________ b) carbon dioxide ___________

c) carbon monoxide ___________ d) nitrogen dioxide ___________

e) nitrogen monoxide ___________ f) dinitrogen monoxide ___________

g) dinitrogen tetroxide ___________ h) sulfur dioxide ___________

i) diiodine pentoxide ___________ j) silicon tetrafluoride ___________

k) boron trifluoride ___________ l) phosphorus triiodide ___________

m) diphosphorus pentoxide __________ n) hexanitrogen heptachloride___________

5. Rename each of the following compounds using the Stock system and give the chemical formula for each compound:

a) ferrous sulfide ___________________________________

b) plumbic bromide ___________________________________

c) stannous chloride ___________________________________

d) cuprous hypophosphite___________________________________

e) stannic chlorite ___________________________________

f) ferrous bromate ___________________________________

g) ferric chlorite ___________________________________

h) plumbic sulfate ___________________________________

i) titaniumic arsenite ___________________________________

j) arsenous nitrite ___________________________________

k) cobaltic acetate ___________________________________

6. Name the following compounds:

a) SF6(g) ____________________________________

b) N2O3(g) ____________________________________

c) NO2(g) ____________________________________

d) PCl3(l) ____________________________________

e) PCl5(s) ____________________________________

f) S5P4(s) ____________________________________

g) Se2F(s) ____________________________________

h) N2I7(s) ____________________________________


1. Name the following hydrated compounds:

a) CuSO4•5H2O ___________________________________

b) Na2SO4•10H2O___________________________________

c) MgSO4•7H2O ___________________________________

d) LiNO3•3H2O ___________________________________

e) CaSO3•8H2O ___________________________________

2. Write the chemical formulas for the following hydrates:

a) iron(III) oxide trihydrate _________________ -rust

b) aluminum chloride hexahydrate _________________ -component of antiperspirant

c) sodium thiosulfate pentahydrate _________________ -photographic “hypo”

d) cadmium (II) nitrate tetrahydrate _________________ -photographic emulsion

e) lithium chloride tetrahydrate _________________ -in fireworks

f) calcium chloride dihydrate _________________ -deicer

3. Write the names of the following bases:

a) KOH(aq) ___________________________

b) Ca(OH)2(aq) ___________________________

4. Write the formulas of the following bases:

a) aqueous magnesium hydroxide _______________

b) aqueous sodium hydroxide _______________

c) aqueous aluminum hydroxide _______________

5. Write the chemical formulas for the following compounds:

a) aqueous hydrogen chloride _______________

b) hydrochloric acid _______________

c) aqueous hydrogen sulfate _______________

d) sulfuric acid _______________

e) aqueous hydrogen acetate _______________

f) acetic acid _______________

g) aqueous hydrogen nitrite _______________

h) nitric acid _______________

i) hydrobromic acid _______________

j) hyposulfurous acid _______________

k) hydroiodic acid _______________

l) aqueous hydrogen perchlorate _______________

6. Name each of the following compounds using both the “classical” and the “IUPAC” nomenclature systems:

a) H2SO3(aq) _________________________ ___________________________

b) H3PO4(aq) _________________________ ___________________________

c) HCN(aq) _________________________ ___________________________

d) H2CO3(aq) _________________________ ___________________________

e) H2S(aq) _________________________ ___________________________

f) HCl(aq) _________________________ ___________________________

g) H2SO4(aq) _________________________ ___________________________

h) H3PO3(aq) _________________________ ___________________________


Write the chemical names for each of the following compounds.

- be sure to include both Stock and Classical Names for any compounds with polyvalent ions.

- also if it is a binary or ternary acid be sure to include both IUPAC and classical system names.

a) MgCl2(aq) ____________________________ ____________________________

b) FeO(s) ____________________________ ____________________________

c) Cs2S2O3 ____________________________ ____________________________

d) Cu3(AsO4)2____________________________ ____________________________

e) CuAsO4 ____________________________ ____________________________

f) SrCl2•3H2O ___________________________ ____________________________

g) HI(g) ____________________________ ____________________________

h) HI(aq) ____________________________ ____________________________

i) O8Cl4 ____________________________ ____________________________

j) H3PO4(aq) ____________________________ ____________________________

k) CaHPO4(aq) ____________________________ ____________________________

l) P3F9 ____________________________ ____________________________

m) BeS ____________________________ ____________________________

n) AuI3 ____________________________ ____________________________

o) KMnO4(s) ____________________________ ____________________________

p) (NH4)OH(aq) ___________________________ ____________________________

q) HCl(aq) ____________________________ ____________________________

r) HBrO2(aq) ____________________________ ____________________________

s) HCN(aq) ____________________________ ____________________________

t) HBrO2(g) ____________________________ ____________________________

u) LiH2PO4(aq) ___________________________ ____________________________

v) Al(H2PO2)3(aq) _________________________ ____________________________

w) AlCl3•8H2O___________________________ ____________________________

x) S3Cl5 ____________________________ ____________________________

y) Ti3N4 ____________________________ ____________________________

z) Sr(ClO)2(s) ____________________________ ____________________________

aa) HNO(aq) ____________________________ ____________________________

bb) FrIO2 ____________________________ ____________________________

cc) (NH4)3AsO3__________________________ ____________________________

dd) HgMnO4 ____________________________ ____________________________

ee) HBr(g) ____________________________ ____________________________

ff) H2SO4(aq) ____________________________ ____________________________

gg) N2O2 ____________________________ ____________________________

hh) XeF6 ____________________________ ____________________________

ii) H2SO3(aq) ____________________________ ____________________________

jj) HBr(aq) ____________________________ ____________________________

kk) BeHSO3(aq) ___________________________ ____________________________

ll) RbClO4 ____________________________ ____________________________

mm) H2CO3(aq) ___________________________ ____________________________

nn) H2CO4(aq) ____________________________ ____________________________

oo) H2Se(aq) ____________________________ ____________________________

pp) BaSO2•10H2O_________________________ ____________________________

qq) Pb(HCO)4 ____________________________ ____________________________

rr) Fe2(HCO4)3____________________________ ____________________________

ss) H2O ____________________________ ____________________________

Worksheet 16 –Nomenclature 5

1. Write the chemical formulas of the following compounds:

a) radium oxide __________________

b) hexanitrogen difluoride __________________

c) tin (IV) permanganate __________________

d) cupric carbonite __________________

e) aqueous hydrogen iodide __________________

f) magnesium dihydrogen phosphate __________________

g) cuprous nitrite dehydrate __________________

h) hypobromous acid __________________

i) aqueous hydrogen hypobromite __________________

j) hydrogen bromide __________________

k) aqueous hydrogen bromide __________________

l) hydrobromic acid __________________

m) ammonium phosphate __________________

n) titaniumic chloride __________________

o) oxygen dichloride __________________

p) aluminum nitride __________________

q) potassium dichromate __________________

r) phosphoric acid __________________

s) phosphorous acid __________________

t) hydrogen cyanide __________________

u) lithium iodite __________________

v) ammonium thiosulfate __________________

w) antimonic persulfate __________________

x) aqueous hydrogen sulfate __________________

y) sulfuric acid __________________

z) aluminum hydrogen hypocarbonite __________________

aa) octasulfur decachloride __________________

bb) pernitric acid __________________

cc) aqueous hydrogen pernitrate __________________

dd) cuprous chloride hexahydrate __________________

ee) nickelic phosphide __________________

ff) lithium iodate __________________

gg) diphosphorus tetraiodide __________________

hh) potassium thiosulfate __________________

ii) calcium hydrogen phosphate __________________

jj) aqueous magnesium hydroxide __________________

kk) hydrochloric acid __________________

ll) acetic acid __________________

mm) cobalt (III) dichromate __________________

nn) mercury (I) carbide __________________

oo) titaniumous hydrogen sulfide __________________

pp) cesium cyanate __________________

qq) nonanitrogen trifluoride __________________

rr) nickel (III) oxide __________________

ss) hypophosphorous acid __________________

tt) perphosphoric acid __________________

uu) aqueous hydrogen perphosphate __________________

vv) persulfuric acid __________________

Worksheet 17 – Types of Reactions

For the following reactions identify:a) the type of reactionb) predict the products (be sure to include states of matter)c) balance the equation

Write “no reaction” if nothing happens. Type of Reaction

1. CaSO4(s) ____________

2. Cl2(aq) + NaI(aq) ____________

3. Zn(s) + CuCl2(aq) ____________

4. KOH(aq) + MgCl2(aq) ____________

5. Li2O(s) + CO2(g) ____________

6. Al(s) + H2O(l) ____________

7. Mg(s) + Zn(NO3)2(aq) ____________

8. Sn(s) + HCl(aq) ____________

9. Hg2(NO3)2(aq) + NaCl(aq) ____________

10. Na2CO3(aq) + H3PO4(aq) ____________

11. Zn(s) + O2(g) ____________

12. Br2(aq) + MgI2(aq) ____________

13. S(s) + O2(g) ____________

14. CaO(s) + H2O(l) ____________

15. Cu(s) + Hg(NO3)2(aq) ____________

16. KOH(aq) + HClO(aq) ____________

17. Ni(s) + CuSO4(aq) ____________

18. H2(g) + Cl2(g) ____________

19. NH4NO3(aq) + KOH(aq) ____________

20. NaOH(aq) + H2SO4(aq) ____________

21. F2(aq) + AlCl3(aq) ____________

22. Al(NO2)3(s) ____________

23. CsNO3(aq) + Na2S(aq) ____________

24. BaO(s) + ClO2(g) ____________

25. Ca(s) + HIO3(aq) ____________

26. NH4Cl(aq) + Al(OH)3(aq) ____________

27. Na(s) + CuCl(aq) ____________

Worksheet 18 – Types of Reactions

In each of the following identify the type of reaction and then state the products.

1. Na3PO4(aq) + CaBr2(aq) 2. Pb(NO3)2(aq) + HCl(aq)

3. Na2CO3(aq) + KF(aq) 4. AgNO3(aq) + CuSO4(aq)

5. AgF(aq) + NiCl2(aq) 6. Pb(s) + FeSO4(aq)

7. CaCO3(s) 8. P4(s) + O2(g)

9. RbNO3(aq) + BeF2(aq) 10. AgNO3(aq) + Cu(s)

11. Li2SO3(aq) + HNO3(aq) 12. Na2O(s) + H2O(l)

13. HNO3(aq) + Ca(OH)2(aq) 14. NaOH + (NH4)3PO4

15. Al(s) + Sn(NO3)2(aq) 16. C3H6(g) + O2(g)

17. Na(s) + CaSO4(aq) 18. BeO(s) + SO2(g)

19. Pb(s) + Br2(l) 20. Ti3(PO3)4(s)

21. H2O(l) + BrO2(g) 22. IO3(g) + H2O(l)

23. H3PO5(aq) 24. RbOH(aq)

25. CoBr3(aq) + I2(s) 26. CoBr3(aq) + Cl2(g)

27. K2S(aq) + HNO3(aq) 28. H2O(l) + Ni(s)

29. MgCl2(s) 30. HCl(aq) + NaOH(aq)

Worksheet 19 – Net Ionic Equations

1. Write the balanced chemical equation, total ionic equation, and net ionic equation for the reaction of sodium iodide solution and aqueous bromine.

2. Write the balanced chemical equation, total ionic equation, and net ionic equation for the reaction of lead (II) nitrate solution and potassium chloride solution.

3. Write the balanced chemical equation, total ionic equation, and net ionic equation for the reaction of sodium carbonate solution and hydrochloric acid.

4. Write the net ionic equation for each of the following reactions:

a) When aqueous sodium carbonate solution is added to a solution of calcium chloride, solid calcium carbonate is formed and sodium chloride remains in solution.

b) When solid magnesium metal is added to a solution of zinc chloride, solid zinc metal is formed, leaving a solution of magnesium chloride

c) When sodium iodide solution is mixed with aqueous lead (II) nitrate, a yellow lead (II) iodide precipitate is formed, leaving a solution of sodium nitrate.

5. Write the net ionic equation for each of the following reactions.

a) An aqueous solution of sodium sulphide reacts with hydrochloric acid to produce hydrogen sulphide gas and a solution of sodium chloride.

b) An aqueous solution of potassium hydroxide reacts with nitric acid to give a solution of potassium nitrate and water.

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