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Introductory Worksheet Package –Grade 11 IB Worksheet 1 – Safety – Apparatus Worksheet 2 – Safety – Whimis Worksheet 3 – Grade 10 Review Worksheet 4 – Naming Review Worksheet 5 – Naming Review Worksheet 6 – Balancing Review Worksheet 7 – Nomenclature 1 Worksheet 8 – Nomenclature 2 Worksheet 9 – Nomenclature 3 Worksheet 10 – Nomenclature 4 Worksheet 11 –Nomenclature 5 Worksheet 12 – Types of Reactions Worksheet 13 – Types of Reactions Worksheet 14 – Net Ionic Equations Read Pgs 1 – 9, Pg 7 Q #1 – 3 Read Pgs 10 – 11, Pg 11 Q #1 – 9 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 atom 3. The left side of the periodic table is composed mostly of metals 4. Energy absorbing reactions are known as endothermic 5. The right side of the periodic table is composed mostly of non-metals 6. The “staircase” region of the periodic table has metalloids 7. A type of reaction in which two or more reactants combine to form a larger product is called synthesis 8. Vertical columns in the periodic table are called families 9. The number of electron shells a helium atom has is one 10. A subatomic particle found in the nucleus that has no charge is called a neutron 11. The number of electrons found in the valence shell determines the reactivity of the atom 12. The number of protons in the nucleus determines the atomic number 13. An atom has an equal number of protons and electrons 14. An ion has either lost or gained electrons 15. An atom’s mass number equals the number of protons + neutrons 16. Electrons reside in the orbital/shells surrounding the nucleus 17. Isotopes occur when atoms of the same type have different atomic masses due to differing numbers of neutrons 18. The modern periodic table arranges elements in increasing atomic number to show a periodic repetition of properties 19. When a metal and a non-metal react with one another they form an ionic bond 20. When two or more non-metals react with one another they form a molecule in which the bonds are called covalent 21. The type of bond in which electrons are shared is called a covalent 22. When magnesium ionizes, its charge is positive two 23. Single-displacement are reaction in which one element replaces another. 24. Group 18 elements have a full shell, which is called a stable octet 25. The chemicals at the end of a chemical reaction can also be called products 26. Group 13 elements have three valence electrons 27. All atoms (except Hydrogen and Helium) desire eight electrons in their outer shell 28. A positive ion is called a cation, where a negative ion is called an anion 29. Metals such as nickel, copper, platinum, gold are called transition metals 30. Sulfur needs two electrons in order to achieve a stable octet 31. The small number written at the lower right of a symbol such as CO2 is called a subscript 32. The number written in the front of a symbol such as 3 NaOH is called a coefficient 33. 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 Questions 1. 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 # of Each Type of Total Formula Atom Number of Atoms H–4 6 2H2O O–2 Ca – 15 65 5Ca3P2O8 P – 10 O - 40 Ba – 3 9 3BaCl2 Cl - 6 Pb – 8 72 8Pb(NO3)2 N – 16 O – 48 N–3 9 3NO2 O-6 What Type of Bond is Found in the Compound? Covalent Is this an Ionic Compound or a Molecule? Molecule Ionic Ionic Ionic Ionic Ionic Ionic Covalent Molecule Worksheet 4 – Naming Review Group # 1 18 2 13 14 15 16 17 (2) # of +1 (1) valence electrons (2) (3) (4) (5) (6) (7) (8) charge # +2 +3 -3 -2 -1 0 (6) (7) +1 +4 Name the following compounds 1) P2O5 (1) (2) 2) CaSO4 calcium sulfate 3) KNO3 potassium nitrate 4) NaF ( (8) diselenium monocarbide 4 diphosphorus pentoxide 31) Se2C +1 sodium fluoride +2 (3) ) (5) 32) Ni2O3 nickel (III) oxide nickelic oxide 33) SrCl2 strontium chloride -2 -1 34) Rb3N +3 rubidium nitride +4 0 -3 5) Au3PO4 gold (I) phosphate aurous phosphate 6) CH4 carbon tetrahydride 35) Au(C2H3O2)3 gold (III) acetate auric acetate 36) (NH4)4C ammonium carbide 7) Na2CO3 sodium carbonate 37) Na3(AsO4) sodium arsenate 8) PbO 38) Co(OH)2 cobalt (II) hydroxide cobaltous hydroxide 39) Co(OH)3 cobalt (III) hydroxide cobaltic hydroxide 40) N5O6 pentanitrogen hexoxide 9) Fr3P 10) PbCl4 lead (II) oxide plumbous oxide francium phosphide lead (IV) chloride plumbic chloride 11) CuS copper (II) sulfide 41) Al(ClO3)3 aluminium chloride cupric sulfide 12) Mn(NO3)2 manganese (II) nitrate 42) B2S3 diboron trisulfide manganous nitrate 13) Ca3P2 calcium phosphide 43) BaSO4 barium sulfate 14) Mn(NO3)4 manganese (IV) nitrate manganic nitrate 15) NiO nickel (II) oxide nickelous oxide 16) Cu2O copper (I) oxide cuprous oxide 17) Fe(HCO3)3 iron (III) bicarbonate Ferric bicarbonate 18) SnCO3 tin (II) carbonate stannous carbonate 19) Pb(SO4)2 lead (IV) sulfate plumbic sulfate 20) CsClO3 cesium chlorate 44) Sn(CN)4 tin (IV) cyanide stannic cyanide 45) NH4ClO2 ammonium chlorite 21) H2S dihydrogen sulfide 51) AsI5 22) H2Cl4 dihydrogen tetrachloride 52) P3I7 arsenic (V) iodide arsenic iodide triphosphorus heptiodide 23) C3O5 tricarbon pentoxide 53) Ra3P2 radium phosphide 24) FeCl3 iron (III) chloride ferric chloride ammonium chloride 54) (NH4)3AsO4 ammonium arsenate 25) NH4Cl 26) FeO iron (II) oxide ferrous oxide 27) Li3AsO3 lithium arsenite 46) C6H10 hexacarbon decahydride 47) Sb3(AsO3)5 antimony (V) arsenite antimonic arsenite 48) PbO2 lead (IV) oxide plumbic oxide 49) CuNO2 copper (I) nitrite cuprous nitrite 50) Fr2S francium sulfide 55) BeO beryllium oxide 56) KCl potassium chloride 57) FeBr2 iron (II) bromide ferrous bromide lithium nitride 28) Ti(HCO3)4 titanium (IV) bicarbonate 58) Li3N 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 PentachlorideP2Cl5 58) 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 + HCl SiCl4 + 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 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 42. Ca3(PO4)2 + SiO2 P4O10 + CaSiO3 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 Na2CO3 + 2HCl 2NaCl + H2O + CO2 FeCl3 + 3NH4OH Fe(OH)3 + 3NH4Cl 2Ca3(PO4)2 + 6SiO2 P4O10 + 6CaSiO3 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 c) ZnI2(s) zinc iodide d) SrCl2(s) strontium chloride e) AlBr3(s) aluminum bromide f) PbCl4(s) lead (IV) chloride stannic 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 d) Mg(NO3)2(s) magnesium nitrate e) Fe(BrO3)3(s) iron (III) bromate f) Na3PO4(s) sodium phosphate g) NH4IO3(s) ammonium iodate h) AuC2H3O2(s) gold (I) 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 mercurous carbonate ferric bromate aurous acetate 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•10H2O sodium 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 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 i) O8Cl4 octaoxygen tetrachloride j) H3PO4(aq) aqueous hydrogen phosphate k) CaHPO4(aq) calcium hydrogen phosphate l) P3F9 triphosphorus nonafluoride m) BeS beryllium sulfide n) AuI3 gold (III) 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 ferrous oxide hydroiodic acid phosphoric acid auric iodide 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 z) Sr(ClO)2(s) strontium hypochlorite aa) HNO(aq) aqueous hydrogen hyponitrite bb) FrIO2 francium iodite cc) (NH4)3AsO3 ammonium arsenite dd) HgMnO4 mercury (I) permanganate ee) HBr(g) hydrogen bromide ff) H2SO4(aq) aqueous hydrogen sulfate 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 titaniumic nitride hyponitrous acid mercurous permanganate sulfuric acid 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 reaction b) 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) Cu(NO3)2(aq) + Ag2SO4(s) NiF(aq) + AgCl(s) No Reaction CaO(s) + CO2(g) + 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) Na3PO4(aq) + H2O(l) +NH3(g) Al(NO3)3(aq) + Sn(s) O2(g) CO2(g) + H2O(l) + CaSO4(aq) No Reaction + SO2(g) BeSO3(s) + Br2(l) PbBr2(s) or Ti3(PO3)4(s) TiO2(s) + PO2(g) HBrO3(aq) HIO4(aq) H2O(l) + PO4(g) 5. AgF(aq) + NiCl2(aq) 6. Pb(s) + FeSO4(aq) 7. CaCO3(s) 8. P4(s) 14. NaOH 15. Al(s) 16. C3H6(g) 17. Na(s) 18. BeO(s) 19. Pb(s) 20. 21. H2O(l) 22. IO3(g) 23. + CuSO4(aq) + + (NH4)3PO4 + Sn(NO3)2(aq) + + BrO2(g) + H2O(l) H3PO5(aq) PbBr4(s) Rb2O(s) + H2O(l) 25. CoBr3(aq) + I2(s) No Reaction 26. CoBr3(aq) + Cl2(g) CoCl3(aq) + Br2(l) + HNO3(aq) KNO3(aq) + H2S(g) Ni(OH)2(aq) + H2(g) Mg(s) + Cl2(g) NaCl(aq) + H2O(l) 24. 27. K2S(aq) 28. H2O(l) 29. 30. HCl(aq) RbOH(aq) + Ni(s) MgCl2(s) + NaOH(aq) 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) Total Ionic Equation: 2Na+(aq) + 2I-(aq) + Br2(aq) 2Na+(aq) + 2I-(aq) + Br2(aq) Net Ionic Equation: 2I-(aq) + Br2(aq) 2Br-(aq) + + I2(aq) 2Na+(aq) + 2Br-(aq) + I2(aq) 2Na+(aq) + 2Br-(aq) + I2(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: CO32-(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)+ CO32-(aq) + Ca2+(aq) +2Cl-(aq) 2Na+(aq)+2Cl-(aq)+ CaCO3(s) 2Na+(aq)+ CO32-(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)
