Introductory Worksheet Package –Grade 11 University Level

Worksheet 1 – Safety – ApparatusWorksheet 2 – Safety – WhimisWorksheet 3 – Grade 10 ReviewWorksheet 4 – Naming ReviewWorksheet 5 – Naming ReviewWorksheet 6 – Balancing ReviewWorksheet 7 – Nomenclature 1Worksheet 8 – Nomenclature 2Worksheet 9 – Nomenclature 3Worksheet 10 – Nomenclature 4Worksheet 11 –Nomenclature 5Worksheet 12 – Types of ReactionsWorksheet 13 – Types of ReactionsWorksheet 14 – 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 _matter_2. The smallest independent unit of matter that cannot be separated by common chemical means

is the atom3. The left side of the periodic table is composed mostly of metals4. Energy absorbing reactions are known as endothermic5. The right side of the periodic table is composed mostly of non-metals6. The “staircase” region of the periodic table has metalloids7. A type of reaction in which two or more reactants combine to form a larger product is called

synthesis8. Vertical columns in the periodic table are called families9. The number of electron shells a helium atom has is one10. A subatomic particle found in the nucleus that has no charge is called a neutron11. The number of electrons found in the valence shell determines the reactivity of the atom12. The number of protons in the nucleus determines the atomic number13. An atom has an equal number of protons and electrons14. An ion has either lost or gained electrons15. An atom’s mass number equals the number of protons + neutrons16. Electrons reside in the orbital/shells surrounding the nucleus17. Isotopes 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 properties19. When a metal and a non-metal react with one another they form an ionic bond20. When two or more non-metals react with one another they form a molecule in which the

bonds are called covalent21. The type of bond in which electrons are shared is called a covalent22. When magnesium ionizes, its charge is positive two23. Single-displacement are reaction in which one element replaces another.24. Group 18 elements have a full shell, which is called a stable octet25. The chemicals at the end of a chemical reaction can also be called products26. Group 13 elements have three valence electrons27. All atoms (except Hydrogen and Helium) desire eight electrons in their outer shell28. A positive ion is called a cation, where a negative ion is called an anion29. Metals such as nickel, copper, platinum, gold are called transition metals30. Sulfur needs two 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

subscript32. The number written in the front of a symbol such as 3 NaOH is called a coefficient33. Diatomic describes a compound that has two identical atoms i.e. O2 34. These types of reactions always involve oxygen combustion 35. Reactants refers to the starting materials in a chemical reaction

B. 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?

2H2OH – 4O – 2

6 Covalent Molecule

5Ca3P2O8

Ca – 15P – 10O - 40

65 Ionic Ionic

3BaCl2

Ba – 3Cl - 6

9 Ionic Ionic

8Pb(NO3)2

Pb – 8N – 16O – 48

72 Ionic Ionic

3NO2

N – 3O - 6

9 Covalent Molecule

Worksheet 4 – Naming Review

Group # 1 18

2 13 14 15 16 17

# of +1 valenceelectrons

charge #

Name the following compounds

1) P2O5 diphosphorus pentoxide 31) Se2C diselenium monocarbide

2) CaSO4 calcium sulfate 32) Ni2O3 nickel (III) oxide nickelic oxide

3) KNO3 potassium nitrate 33) SrCl2 strontium chloride

4) NaF sodium fluoride 34) Rb3N rubidium nitride

5) Au3PO4 gold (I) phosphate 35) Au(C2H3O2)3 gold (III) acetateaurous phosphate auric acetate

6) CH4 carbon tetrahydride 36) (NH4)4C ammonium carbide

7) Na2CO3 sodium carbonate 37) Na3(AsO4) sodium arsenate

8) PbO lead (II) oxide 38) Co(OH)2 cobalt (II) hydroxideplumbous oxide cobaltous hydroxide

9) Fr3P francium phosphide 39) Co(OH)3 cobalt (III) hydroxide cobaltic hydroxide

10) PbCl4 lead (IV) chloride 40) N5O6 pentanitrogen hexoxide plumbic chloride11) CuS copper (II) sulfide 41) Al(ClO3)3 aluminium chloride

cupric sulfide12) Mn(NO3)2 manganese (II) nitrate 42) B2S3 diboron trisulfide

manganous nitrate13) Ca3P2 calcium phosphide 43) BaSO4 barium sulfate

(1)

+1

(2)

(8)

0

(2)

+2

(3)

+3

(4)

+4

(5)

-3

(6)

-2

(7)

-1

14) Mn(NO3)4 manganese (IV) nitrate 44) Sn(CN)4 tin (IV) cyanide manganic nitrate stannic cyanide

15) NiO nickel (II) oxide 45) NH4ClO2 ammonium chloritenickelous oxide

16) Cu2O copper (I) oxide 46) C6H10 hexacarbon decahydridecuprous oxide

17) Fe(HCO3)3 iron (III) bicarbonate 47) Sb3(AsO3)5 antimony (V) arsenite Ferric bicarbonate antimonic arsenite

18) SnCO3 tin (II) carbonate 48) PbO2 lead (IV) oxidestannous carbonate plumbic oxide

19) Pb(SO4)2 lead (IV) sulfate 49) CuNO2 copper (I) nitrite plumbic sulfate cuprous nitrite20) CsClO3 cesium chlorate 50) Fr2S francium sulfide

21) H2S dihydrogen sulfide 51) AsI5 arsenic (V) iodide arsenic iodide

22) H2Cl4 dihydrogen tetrachloride 52) P3I7 triphosphorus heptiodide

23) C3O5 tricarbon pentoxide 53) Ra3P2 radium phosphide

24) FeCl3 iron (III) chloride 54) (NH4)3AsO4 ammonium arsenateferric chloride

25) NH4Cl ammonium chloride 55) BeO beryllium oxide

26) FeO iron (II) oxide 56) KCl potassium chlorideferrous oxide

27) Li3AsO3 lithium arsenite 57) FeBr2 iron (II) bromide ferrous bromide

28) Ti(HCO3)4 titanium (IV) bicarbonate 58) Li3N lithium nitride Titaniumous bicarbonate

29) Mg3(PO4)2 magnesium phosphate 59) Cu3PO4 copper (I) phosphate cuprous phosphate

30) As(CN)3 arsenic (III) cyanide 60) H2O dihydrogen monoxide arsenic cyanide

Worksheet 5 – Naming Review

Write the chemical formula for the following compounds

1) Beryllium Fluoride BeF2 31) Potassium Fluoride KF

2) Sodium Nitride Na3N 32) Magnesium Arsenite Mg3(AsO3)2

3) Iron (II) Nitrate Fe(NO3)2 33) Mercurous Phosphide Hg3P

4) Ammonium Phosphate (NH4)3PO4 34) Strontium Nitrate Sr(NO3)2

5) Plumbous Sulfate PbSO4 35) Auric Chloride AuCl3

6) Plumbic Oxide PbO2 36) Lead (IV) Carbide PbC

7) Antimony (V) Cyanide Sb(CN)5 37) Ammonium Acetate NH4C2H3O2

8) Cobaltic Oxide Co2O3 38) Trinitrogen Octoxide N3O8

9) Sodium Phosphide Na3P 39) Lithium Chlorite LiClO2

10) Ferrous Chlorate Fe(ClO3)2 40) Nickel (III) Nitride NiN

11) Carbon Dioxide CO2 41) Arsenous Sulfide As2S3

12) Dinitrogen Pentaflouride N2F5 42) Arsenic (III) Phosphate AsPO4

13) Calcium Hydroxide Ca(OH)2 43) Boron Oxide B2O3

14) Nickel (III) Sulfate Ni2(SO4)3 44) Copper (II) Bromide CuBr2

15) Radium Astatide RaAt2 45) Trihydrogen Tetracarbide H3C4

16) Sulfur Tetrabromide SBr4 46) Nonanitrogen Decoxide N9O10

17) Cesium Bicarbonate CsHCO3 47) Ammonium Arsenate (NH4)3AsO4

18) Gallium Nitride GaN 48) Calcium Bicarbonate Ca(HCO3)2

19) Tetrahydrogen Monocarbide H4C 49) Calcium Iodide CaI2

20) Carbon Tetrachloride CCl4 50) Arsenic Acetate As(C2H3O2)5

21) Mercury (II) Bicarbonate Hg(HCO3)2 51) Tin (IV) Sulfate Sn(SO4)2

22) Lead (II) Phosphate Pb3(PO4)2 52) Titaniumic Phosphate Ti3(PO4)4

23) Stannic Arsenate Sn3(AsO3)4 53) Boron Phosphide BP

24) Aluminum Selenide Al2Se3 54) Cupric Sulfide CuS

25) Barium Carbonate BaCO3 55) Tetrasulfur PentachlorideS4Cl5

26) Aurous Sulfite Au2SO3 56) Ammonium Phosphide (NH4)3P

27) Ammonium Acetate NH4C2H3O2 57) Cesium Nitride Cs3N

28) Diphosphorus PentachlorideP2Cl558) Cobaltic Silicide Co4Si3

29) Titanium (III) sulfide Ti2S3 59) Potassium Carbonate K2CO3

30) Manganese (IV) iodide MnI4 60) Dihydrogen Monoxide H2O

Worksheet 6 – Balancing Review

Balance the following skeleton equations

1. H2 + O2 H2O 2H2 + O2 2H2O

2. S8 + O2 SO3 S8 + 12O2 8SO3

3. HgO Hg + O2 2HgO 2Hg + O2

4. Na + H2O NaOH + H2 2Na + 2H2O 2NaOH + H2

5. C10H16 + Cl2 C + HCl C10H16 + 8Cl2 10C + 16HCl

6. Si2H3 + O2 SiO2 + H2O 4Si2H3 + 11O2 8SiO2 + 6H2O

7. Fe + O2 Fe2O3 4Fe + 3O2 2Fe2O3

8. C7H6O2 + O2 CO2 + H2O 2C7H6O2 + 15O2 14CO2 + 6H2O

9. Zn + HCl ZnCl2 + H2 Zn + 2HCl ZnCl2 + H2

10. FeS2 + O2 Fe2O3 + SO2 4FeS2 + 11O2 2Fe2O3 + 8SO2

11. K + Br2 KBr 2K + Br2 2KBr

12. Fe2O3 + H2 Fe + H2O Fe2O3 + 3H2 2Fe + 3H2O

13. C2H2 + O2 CO2 + H2O 2C2H2 + 5O2 4CO2 + 2H2O

14. H2O2 H2O + O2 2H2O2 2H2O + O2

15. C7H16 + O2 CO2 + H2O C7H16 + 11O2 7CO2 + 8H2O

16. SiO2 + HF SiF4 + H2O SiO2 + 4HF SiF4 + 2H2O

17. KClO3 KCl + O2 2KClO3 2KCl + 3O2

18. KClO3 KClO4 + KCl 4KClO3 3KClO4 + KCl

19. P4O10 + H2O H3PO4 P4O10 + 6H2O 4H3PO4

20. Sb + O2 Sb4O6 4Sb + 3O2 Sb4O6

21. C3H8 + O2 CO2 + H2O C3H8 + 5O2 3CO2 + 4H2O

22. Fe2O3 + CO Fe + CO2 Fe2O3 + 3CO 2Fe + 3CO2

23. N2 + H2 NH3 N2 + 3H2 2NH3

24. N2 + O2 N2O 2N2 + O2 2N2O

25. CO2 + H2O C6H12O6 + O2 6CO2 + 6H2O C6H12O6 + 6O2

26. SiCl4 + H2O H4SiO4 + HClSiCl4 + 4H2O H4SiO4 + 4HCl

27. H3PO4 H4P2O7 + H2O 2H3PO4 H4P2O7 + H2O

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

29. Al(OH)3 + H2SO4 Al2(SO4)3 + H2O 2Al(OH)3 + 3H2SO4 Al2(SO4)3 + 6H2O

30. Fe2(SO4)3 + KOH K2SO4 + Fe(OH)3 Fe2(SO4)3 + 6KOH 3K2SO4 + 2Fe(OH)3

31. H2SO4 + HI H2S + I2 + H2O H2SO4 + 8HI H2S + 4I2 + 4H2O

32. Al + FeO Al2O3 + Fe 2Al + 3FeO Al2O3 +3Fe

33. Na2CO3 + HCl NaCl + H2O + CO2 Na2CO3 + 2HCl 2NaCl + H2O + CO2

34. P4 + O2 P2O5 P4 + 5O2 2P2O5

35. K2O + H2O KOH K2O + H2O 2KOH

36. Al + O2 Al2O3 4Al + 3O2 2Al2O3

37. Na2O2 + H2O NaOH + O2 2Na2O2 + 2H2O 4NaOH + O2

38. C + H2O CO + H2 C + H2O CO + H2

39. H3AsO4 As2O5 + H2O 2H3AsO4 As2O5 + 3H2O

40. Al2(SO4)3 + Ca(OH)2 Al(OH)3 + CaSO4 Al2(SO4)3 +3Ca(OH)2 2Al(OH)3 + 3CaSO4

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

42. Ca3(PO4)2 + SiO2 P4O10 + CaSiO3 2Ca3(PO4)2 + 6SiO2 P4O10 + 6CaSiO3

43. N2O5 + H2O HNO3 N2O5 + H2O 2HNO3

44. Al + HCl AlCl3 + H2 2Al + 6HCl 2AlCl3 + 3H2

45. C4H8 + O2 CO2 + H2O C4H8 + 6O2 4CO2 + 4H2O

46. C8H18 + O2 CO2 + H2O + CO + C C8H18 + 10O2 5CO2 + 9H2O + CO + 2C

Worksheet 7 – Nomenclature 1

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

a) calcium fluoride CaF2 b) sodium sulfide Na2S

c) aluminum nitride AlN d) aluminum chloride AlCl3

e) potassium oxide K2O f) calcium chloride CaCl2

g) copper (II) sulfide CuS h) lead (II) bromide PbBr2

i) silver iodide AgI j) barium nitride Ba3N2

k) iron (II) fluoride FeF2 l) manganese (IV) oxide MnO2

m) mercury (II) sulfide HgS n) ferric oxide Fe2O3

o) cuprous nitride Cu3N p) antimony (V) iodide SbI5

q) cesium carbide Cs4C r) strontium phosphide Sr3P2

2. Write the names for the following compounds:

a) lime, CaO(s) calcium oxide

b) road salt, CaCl2(s) calcium chloride

c) magnesia, MgO(s) magnesium oxide

d) bauxite, Al2O3(s) aluminum oxide

e) zinc ore, ZnS(s) zinc sulfide

f) cassiterite, SnO2(s) tin (IV) oxide

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

a) Na2O(s) sodium oxide

b) SnCl4(s) tin (IV) chloride stannic chloride

c) ZnI2(s) zinc iodide

d) SrCl2(s) strontium chloride

e) AlBr3(s) aluminum bromide

f) PbCl4(s) lead (IV) chloride plumbic chloride

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

a) strontium and oxygen SrO strontium oxide

b) sodium and sulfur Na2S sodium sulfide

c) barium and fluorine BaF2 barium flrouide

d) silver and iodine AgI silver iodide

e) calcium and bromine CaBr2 calcium bromide

f) lithium and chlorine LiCl lithium chloride

Worksheet 8 – Nomenclature 2

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

a) NaNO3(s) sodium nitrate -found in tobacco

b) NaNO2(s) sodium nitire -a meat preservative

c) Cu(NO3)2(s) copper (II) nitrate cupric nitrate -blue solution in water

d) CuNO3(s) copper (I) nitrate cuprous nitrate -green solution in water

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

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

g) PbCO3(s) lead (II) carbonate plumbous carbonate -cerussite, a mineral

h) Sn3(PO4)2(s) tin (II) phosphate stannous phosphate -use to fix paints to silk

i) Fe2(SO4)3(s) iron (III) sulfate ferric sulfate -a mineral found on Mars

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

a) calcium carbonate CaCO3 -active ingredient in antacids

b) sodium bicarbonate NaHCO3 -a foaming agent added to foods

c) sodium hypochlorite NaClO -a component of bleach

d) calcium sulfate CaSO4 -plaster of Paris

e) ammonium nitrate NH4NO3 -used in fertilizer

f) ammonium phosphate (NH4)PO4 -a leavening agent added to foods

g) copper (II) sulfate CuSO4 -used as a fungicide

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

i) potassium permanganate KMnO4 -a traditional antiseptic

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

a) LiClO3(s) lithium chlorate

b) BaSO4(s) ) barium sulfate

c) Hg2CO3(s) mercury (II) carbonate mercurous carbonate

d) Mg(NO3)2(s) magnesium nitrate

e) Fe(BrO3)3(s) iron (III) bromate ferric bromate

f) Na3PO4(s) sodium phosphate

g) NH4IO3(s) ammonium iodate

h) AuC2H3O2(s) gold (I) acetate aurous acetate

i) Zn3(PO4)2(s) zinc phosphate

j) Sb(ClO3)5(s) antimony (V) chlorate antimonic chlorate

k) MnSO4(s) manganese (II) sulfate manganous sulfate

l) KBrO(s) potassium hypobromite

m) AlPO5(s) aluminum perphosphate

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

a) nitrogen N2 b) carbon dioxide CO2

c) carbon monoxide CO d) nitrogen dioxide NO2

e) nitrogen monoxide NO f) dinitrogen monoxide N2O

g) dinitrogen tetroxide N2O4 h) sulfur dioxide SO2

i) diiodine pentoxide I2O5 j) silicon tetrafluoride SiF4

k) boron trifluoride BF3 l) phosphorus triiodide PI3

m) diphosphorus pentoxide P2O5 n) hexanitrogen heptachloride N6Cl7

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

a) ferrous sulfide FeS iron (II) sulfide

b) plumbic bromide PbBr4 lead (IV) bromide

c) stannous chloride SnCl2 tin (I) chloride

d) cuprous hypophosphite Cu3PO2 copper (I) hypophosphite

e) stannic chlorite Sn(ClO2)4 tin (IV) chlorite

f) ferrous bromate Fe(BrO3)2 iron (II) bromate

g) ferric chlorite Fe(ClO2)3 iron (III) chlorite

h) plumbic sulfate Pb(SO4)2 lead (IV) sulfate

i) titaniumic arsenite Ti3(AsO3) titanium (IV) arsenite

j) arsenous nitrite As(NO2)3 arsenic (III) nitrite

k) cobaltic acetate Co(C2H3O2)3 cobalt (III) acetate

6. Name the following compounds:

a) SF6(g) sulfur hexafluoride

b) N2O3(g) dinitrogen trioxide

c) NO2(g) nitrogen dioxide

d) PCl3(l) phosphorus trichloride

e) PCl5(s) phosphorus pentachloride

f) S5P4(s) pentasulfur tetraphosphide

g) Se2F(s) diselenium monoflrouide

h) N2I7(s) dinitrogen heptaiodide

Worksheet 9 – Nomenclature 3

1. Name the following hydrated compounds:

a) CuSO4•5H2O copper (II) sulfate pentahydrate

b) Na2SO4•10H2Osodium sulfate decahydrate

c) MgSO4•7H2O magnesium sulfate heptahydrate

d) LiNO3•3H2O lithium nitrate trihydrate

e) CaSO3•8H2O calcium sulfite octahydrate

2. Write the chemical formulas for the following hydrates:

a) iron(III) oxide trihydrate Fe2O3•3H2O -rust

b) aluminum chloride hexahydrate AlCl3•6H2O -component of antiperspirant

c) sodium thiosulfate pentahydrate NaS2O3•5H2O -photographic “hypo”

d) cadmium (II) nitrate tetrahydrate Cd(NO3)2•4H2O -photographic emulsion

e) lithium chloride tetrahydrate LiCl•4H2O -in fireworks

f) calcium chloride dihydrate CaCl2•2H2O -deicer

3. Write the names of the following bases:

a) KOH(aq) potassium hydroxide

b) Ca(OH)2(aq) calcium hydroxide

4. Write the formulas of the following bases:

a) aqueous magnesium hydroxide Mg(OH)2(aq)

b) aqueous sodium hydroxide NaOH(aq)

c) aqueous aluminum hydroxide Al(OH)2(aq)

5. Write the chemical formulas for the following compounds:

a) aqueous hydrogen chloride HCl(aq)

b) hydrochloric acid HCl(aq)

c) aqueous hydrogen sulfate H2SO4(aq)

d) sulfuric acid H2SO4(aq)

e) aqueous hydrogen acetate CH3COOH(aq)

f) acetic acid CH3COOH(aq)

g) aqueous hydrogen nitrite HNO3(aq)

h) nitric acid HNO3(aq)

i) hydrobromic acid HBr(aq)

j) hyposulfurous acid H2SO2(aq)

k) hydroiodic acid HI(aq)

l) aqueous hydrogen perchlorate HClO4(aq)

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

a) H2SO3(aq) aqueous hydrogen sulfite sulfurous acid

b) H3PO4(aq) aqueous hydrogen phosphate phosphoric acid

c) HCN(aq) aqueous hydrogen cyanide hydrocyanic acid

d) H2CO3(aq) aqueous hydrogen carbonate carbonic acid

e) H2S(aq) aqueous hydrogen sulfide hydrosulfuric acid

f) HCl(aq) aqueous hydrogen chloride hydrochloric acid

g) H2SO4(aq) aqueous hydrogen sulfate sulfuric acid

h) H3PO3(aq) aqueous hydrogen phosphite phosphorous acid

Worksheet 10 – Nomenclature 4

1. 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) magnesium chloride

b) FeO(s) iron (II) oxide ferrous oxide

c) Cs2S2O3 cesium thiosulfate

d) Cu3(AsO4)2 copper (II) arsenate cupric arsenate

e) CuAsO4 copper (I) arsenate cuprous arsenate

f) SrCl2•3H2O strontium chloride trihydrate

g) HI(g) hydrogen iodide

h) HI(aq) aqueous hydrogen iodide hydroiodic acid

i) O8Cl4 octaoxygen tetrachloride

j) H3PO4(aq) aqueous hydrogen phosphate phosphoric acid

k) CaHPO4(aq) calcium hydrogen phosphate

l) P3F9 triphosphorus nonafluoride

m) BeS beryllium sulfide

n) AuI3 gold (III) iodide auric iodide

o) KMnO4(s) potassium permanganate

p) (NH4)OH(aq) ammonium hydroxide

q) HCl(aq) aqueous hydrogen chloride hydrochloric acid

r) HBrO2(aq) aqueous hydrogen bromite bromous acid

s) HCN(aq) aqueous hydrogen cyanide hydrocyanic acid

t) HBrO2(g) hydrogen bromite

u) LiH2PO4(aq) lithium dihydrogen phosphate

v) Al(H2PO2)3(aq) aluminum dihydrogen phosphate

w) AlCl3•8H2O aluminum chloride octahydrate

x) S3Cl5 trisulfur pentachloride

y) Ti3N4 titanium (IV) nitride titaniumic nitride

z) Sr(ClO)2(s) strontium hypochlorite

aa) HNO(aq) aqueous hydrogen hyponitrite hyponitrous acid

bb) FrIO2 francium iodite

cc) (NH4)3AsO3 ammonium arsenite

dd) HgMnO4 mercury (I) permanganate mercurous permanganate

ee) HBr(g) hydrogen bromide

ff) H2SO4(aq) aqueous hydrogen sulfate sulfuric acid

gg) N2O2 dinitrogen dioxide

hh) XeF6 xenon hexaflouride

ii) H2SO3(aq) aqueous hydrogen sulfite sulfurous acid

jj) HBr(aq) aqueous hydrogen bromide hydrobromic acid

kk) BeHSO3(aq) beryllium hydrogen sulfite

ll) RbClO4 rubidium perchlorate

mm) H2CO3(aq) aqueous hydrogen carbonate carbonic acid

nn) H2CO4(aq) aqueous hydrogen percarbonate percarbonic acid

oo) H2Se(aq) aqueous hydrogen selenide hydroselenic acid

pp) BaSO2•10H2O barium hydrosulfite decahydrate

qq) Pb(HCO)4 lead (II) hypocarbonite plumbous hypocarbonite

rr) Fe2(HCO4)3 iron (III) percarbonate ferric percarbonate

ss) H2O dihydrogen monoxide water

Worksheet 11 –Nomenclature 5

1. Write the chemical formulas of the following compounds:

a) radium oxide RaO

b) hexanitrogen difluoride N6F2

c) tin (IV) permanganate Sn(MnO4)4

d) cupric carbonite CuCO2

e) aqueous hydrogen iodide HI(aq)

f) magnesium dihydrogen phosphate Mg(H2PO4)2

g) cuprous nitrite dehydrate CuNO2∙10H2O

h) hypobromous acid HBrO(aq)

i) aqueous hydrogen hypobromite HBrO(aq)

j) hydrogen bromide HBr(g)

k) aqueous hydrogen bromide HBr(aq)

l) hydrobromic acid HBr(aq)

m) ammonium phosphate (NH4)3PO4

n) titaniumic chloride TiCl4

o) oxygen dichloride OCl2

p) aluminum nitride AlN

q) potassium dichromate K2Cr2O7

r) phosphoric acid H3PO4(aq)

s) phosphorous acid H3PO3(aq)

t) hydrogen cyanide HCN

u) lithium iodite LiIO2

v) ammonium thiosulfate (NH4)2S2O3

w) antimonic persulfate Sb2(SO5)5

x) aqueous hydrogen sulfate H2SO4(aq)

y) sulfuric acid H2SO4(aq)

z) aluminum hydrogen hypocarbonite Al(HCO)3

aa) octasulfur decachloride S8Cl10

bb) pernitric acid HNO4(aq)

cc) aqueous hydrogen pernitrate HNO4(aq)

dd) cuprous chloride hexahydrate CuCl∙6H2O

ee) nickelic phosphide NiP

ff) lithium iodate LiIO3

gg) diphosphorus tetraiodide P2I4

hh) potassium thiosulfate K2S2O3

ii) calcium hydrogen phosphate CaHPO4

jj) aqueous magnesium hydroxide Mg(OH)2(aq)

kk) hydrochloric acid HCl(aq)

ll) acetic acid CH3COOH(aq)

mm) cobalt (III) dichromate Co2(Cr2O7)3

nn) mercury (I) carbide Hg4C

oo) titaniumous hydrogen sulfide Ti(HS)3

pp) cesium cyanate CsOCN

qq) nonanitrogen trifluoride N9F3

rr) nickel (III) oxide Ni2O3

ss) hypophosphorous acid H3PO2(aq)

tt) perphosphoric acid H3PO5(aq)

uu) aqueous hydrogen perphosphate H3PO5(aq)

vv) persulfuric acid H2SO5(aq)

Worksheet 12 – 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) CaO(s) + SO3(g) decomposition

2. Cl2(aq) + NaI(aq) I2(aq) + NaCl(aq) single-displacement

3. Zn(s) + CuCl2(aq) Cu(s) + ZnCl2(aq) single-displacement

4. KOH(aq) + MgCl2(aq) KCl(aq) + Mg(OH)2(s) double-displacement

5. Li2O(s) + CO2(g) Li2CO3(s) synthesis

6. Al(s) + H2O(l) Al(OH)3(s) + H2(g) single-displacement

7. Mg(s) + Zn(NO3)2(aq) Mg(NO3)2(aq) + Zn(s) single-displacement

8. Sn(s) + HCl(aq) SnCl2(aq) + H2(g) single-displacement

9. Hg2(NO3)2(aq) + NaCl(aq) NaNO3(aq) + HgCl(s) double-displacement

10. Na2CO3(aq) + H3PO4(aq) Na3PO4(aq) + H2O(l) + CO2(g) double/decomposition

11. Zn(s) + O2(g) ZnO(s) synthesis

12. Br2(aq) + MgI2(aq) MgBr2(aq) + I2(aq) single-displacement

13. S(s) + O2(g) SO2(g) synthesis

14. CaO(s) + H2O(l) Ca(OH)2(aq) synthesis

15. Cu(s) + Hg(NO3)2(aq) No Reaction

16. KOH(aq) + HClO(aq) KClO(aq) + H2O(l) double-displacement

17. Ni(s) + CuSO4(aq) NiSO4(aq) + Cu(s) single-displacement

18. H2(g) + Cl2(g) HCl(g) synthesis

19. NH4NO3(aq) + KOH(aq) KNO3(aq) + H2O(l) + NH3(g) double/decomposition

20. NaOH(aq) + H2SO4(aq) Na2SO4(aq) + H2O(l) double displacement

21. F2(aq) + AlCl3(aq) AlF3(aq) + Cl2(aq) single-displacement

22. Al(NO2)3(s) Al2O3(s) + NO(g) decomposition

23. CsNO3(aq) + Na2S(aq) No Reaction

24. BaO(s) + ClO2(g) BaClO3(s) synthesis

25. Ca(s) + HIO3(aq) CaIO3(aq) + H2(g) single-displacement

26. NH4Cl(aq) + Al(OH)3(aq) AlCl3(aq) + H2O(l) + NH3(g) double/decomposition

27. Na(s) + CuCl(aq) NaCl(aq) + Cu(s) single-displacement

Worksheet 13 – Types of Reactions

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

1. Na3PO4(aq) + CaBr2(aq) NaBr(aq) + Ca3(PO4)2(s)

2. Pb(NO3)2(aq) + HCl(aq) PbCl2(s) + HNO3(aq)

3. Na2CO3(aq) + KF(aq) No Reaction

4. AgNO3(aq) + CuSO4(aq) Cu(NO3)2(aq) + Ag2SO4(s)

5. AgF(aq) + NiCl2(aq) NiF(aq) + AgCl(s)

6. Pb(s) + FeSO4(aq) No Reaction

7. CaCO3(s) CaO(s) + CO2(g)

8. P4(s) + O2(g) P2O3(g)

9. RbNO3(aq) + BeF2(aq) No Reaction

10. AgNO3(aq) + Cu(s) Cu(NO3)2(aq) + 2 Ag(s)

11. Li2SO3(aq) + HNO3(aq) LiNO3(aq) + H2O(l) +SO2(g)

12. Na2O(s) + H2O(l) NaOH(aq)

13. HNO3(aq) + Ca(OH)2(aq) Ca(NO3)2(aq) + H2O(l)

14. NaOH + (NH4)3PO4 Na3PO4(aq) + H2O(l) +NH3(g)

15. Al(s) + Sn(NO3)2(aq) Al(NO3)3(aq) + Sn(s)

16. C3H6(g) + O2(g) CO2(g) + H2O(l)

17. Na(s) + CaSO4(aq) No Reaction

18. BeO(s) + SO2(g) BeSO3(s)

19. Pb(s) + Br2(l) PbBr2(s) or PbBr4(s)

20. Ti3(PO3)4(s) TiO2(s) + PO2(g)

21. H2O(l) + BrO2(g) HBrO3(aq)

22. IO3(g) + H2O(l) HIO4(aq)

23. H3PO5(aq) H2O(l) + PO4(g)

24. RbOH(aq) Rb2O(s) + H2O(l)

25. CoBr3(aq) + I2(s) No Reaction

26. CoBr3(aq) + Cl2(g) CoCl3(aq) + Br2(l)

27. K2S(aq) + HNO3(aq) KNO3(aq) + H2S(g)

28. H2O(l) + Ni(s) Ni(OH)2(aq) + H2(g)

29. MgCl2(s) Mg(s) + Cl2(g)

30. HCl(aq) + NaOH(aq) NaCl(aq) + H2O(l)

Worksheet 14 – 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.

Balanced Equation: 2NaI(aq) + Br2(aq) 2NaBr(aq) + I2(aq)

Total Ionic Equation: 2Na+(aq) + 2I-

(aq) + Br2(aq) 2Na+(aq) + 2Br-

(aq) + I2(aq)

2Na+(aq) + 2I-

(aq) + Br2(aq) 2Na+(aq) + 2Br-

(aq) + I2(aq)

Net Ionic Equation: 2I-(aq) + Br2(aq) 2Br-

(aq) + I2(aq)

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.

Balanced Equation: Pb(NO3)2(aq) + 2KCl(aq) 2KNO3(aq) + PbCl2(s)

Total Ionic Equation: Pb2+(aq) + 2NO3

-(aq) + 2K+

(aq) + 2Cl-(aq) 2K+

(aq) + 2 NO3-(aq) + PbCl2(s)

Pb2+(aq) + 2NO3

-(aq) + 2K+

(aq) + 2Cl-(aq) 2K+

(aq) + 2 NO3-(aq) + PbCl2(s)

Net Ionic Equation: Pb2+(aq) + 2Cl-

(aq) PbCl2(s)

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

Balanced Equation: Na2CO3(aq) + 2HCl(aq) 2NaCl(aq) + H2O(aq) + CO2(aq)

Total Ionic Equation: 2Na(aq)+ CO32-

(aq)+2H+(aq)+2Cl-

(aq) 2Na+(aq) + 2Cl-

(aq) + H2O(aq) + CO2(aq)

2Na(aq)+ CO32-

(aq)+2H+(aq)+2Cl-

(aq) 2Na+(aq) + 2Cl-

(aq) + H2O(aq) + CO2(aq) Net Ionic Equation: CO3

2-(aq) + 2H+

(aq) H2O(aq) + CO2(aq)

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.

Balanced Equation: Na2CO3(aq) + CaCl2(aq) 2NaCl(aq) + CaCO3(s)

Total Ionic Equation: 2Na+(aq)+ CO3

2-(aq) + Ca2+

(aq) +2Cl-(aq) 2Na+

(aq)+2Cl-(aq)+ CaCO3(s)

2Na+(aq)+ CO3

2-(aq) + Ca2+

(aq) +2Cl-(aq) 2Na+

(aq)+2Cl-(aq)+ CaCO3(s) Net

Ionic Equation: CO32-

(aq) + Ca2+(aq) CaCO3(s)

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

Balanced Equation: ZnCl2(aq) + Mg(s) MgCl2(aq) + Zn(s)

Total Ionic Equation: Zn2+(aq) + 2Cl-

(aq) + Mg(s) Mg2+(aq) + 2Cl-

(aq) + Zn(s)

Zn2+(aq) + 2Cl-

(aq) + Mg(s) Mg2+(aq) + 2Cl-

(aq) + Zn(s)

Net Ionic Equation: Zn2+(aq) + Mg(s) Mg2+

(aq) + Zn(s)

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.

Balanced Equation: 2NaI(aq) + Pb(NO3)2(aq) 2NaNO3(aq) + PbI2(s)

Total Ionic Equation: 2Na+(aq) +2I-

(aq)+ Pb2+(aq)+ 2NO3

-(aq)2Na+

(aq) + 2NO3-(aq) + PbI2(s)

2Na+(aq) +2I-

(aq)+ Pb2+(aq)+ 2NO3

-(aq)2Na+

(aq) + 2NO3-(aq) + PbI2(s)

Net Ionic Equation: 2I-(aq) + Pb2+

(aq) PbI2(s)

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.

Balanced Equation: Na2S(aq) + 2HCl(aq) 2NaCl(aq) + H2S (g)

Total Ionic Equation: 2Na+(aq) + S2-

(aq)+ 2H+(aq) + 2Cl-

(aq)2Na+(aq) +2Cl-

(aq) +H2S(g)

2Na+(aq) + S2-

(aq)+ 2H+(aq) + 2Cl-

(aq)2Na+(aq) +2Cl-

(aq) +H2S(g)

Net Ionic Equation: S2-(aq)+ 2H+

(aq) H2S(g) b) An aqueous solution of potassium hydroxide reacts with nitric acid to give a

solution of potassium nitrate and water.

Balanced Equation: KOH(aq) + HNO3(aq) KNO3(aq) + H2O(l)

Total Ionic Equation: K+(aq) + OH-

(aq) + H+(aq) + NO3

- (aq) K+

(aq) + NO3- (aq) + H2O(l)

K+(aq) + OH-

(aq) + H+(aq) + NO3

- (aq) K+

(aq) + NO3- (aq) + H2O(l)

Net Ionic Equation: OH-(aq) + H+

(aq) H2O(l)