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Worksheets - Answers Grade 11 University LevelUnit 1Nomenclature Worksheet 1 – Nomenclature 1Read Pgs 52 – 65 Q# Pg 66 2 – 6 Worksheet 2 – Nomenclature 2Worksheet 3 – Nomenclature 3Worksheet 4 – Nomenclature 4Worksheet 5 –Nomenclature 5 Types of ReactionsNo Worksheet – Chemical EquationsRead Pgs 72 – 78 Q# Pg 79 1 – 6 Worksheet 6 – Balancing Chemical EquationsWorksheet 7 – Types of Reactions Read Pgs 79 – 86, Q# Pg 86 1 – 5Worksheet 8 – Types of ReactionsRead Pgs 87 – 102 Q# Pg 103 3 – 5 Worksheet 9 – Net Ionic EquationsAtomic StructureWorksheet 10 – Aufbau DiagramsRead Pgs 4 – 14, Pg 14, Q# 1 – 6 Worksheet 11 – Blank Periodic TableWorksheet 12 – Energy Level Diagrams Worksheet 13 – Electron ConfigurationsWorksheet 14 – Orbital and Energy Level DiagramsWorksheet 15 – Quantum NumbersWorksheet 16 – Atomic Structure Review Unit 2Periodicity Worksheet 17 – Periodic TrendsRead Pgs 15 – 25 Pg 26 Q# 1 - 7Worksheet 18 – Alkali Metals and HalogensPg 30 Q# 1 – 15, 17BondingNo Worksheet – Ionic CompoundsRead Pgs 34 – 40, Pg 41 Q# 1,2,4,5No Worksheet – Covalent CompoundsRead Pgs 41 – 51, Pg 51 Q# 1 – 6 No Worksheet – Ionic/Covalent Structural FormulaWorksheet 19 – PolarityRead Pgs 48 – 50, Pgs 51 Q# 7No Worksheet – Unit 2 Review Pgs 70 – 71 Q# 1 – 18, Worksheet 1 – Nomenclature 1Write the formulas for each of the following compounds:a) calcium fluoride CaF2b) sodium sulfide Na2Sc) aluminum nitride AlNd) aluminum chloride AlCl3e) potassium oxide K2Of) calcium chlorideCaCl2g) copper (II) sulfideCuSh) lead (II) bromidePbBr2i) silver iodideAgIj) barium nitrideBa3N2k) iron (II) fluorideFeF2l) manganese (IV) oxideMnO2m) mercury (II) sulfide HgSn) ferric oxideFe2O3o) cuprous nitrideCu3Np) antimony (V) iodideSbI5q) cesium carbideCs4Cr) strontium phosphideSr3P2Write the names for the following compounds:a) lime, CaO(s) calcium oxideb) road salt, CaCl2(s)calcium chloridec) magnesia, MgO(s)magnesium oxided) bauxite, Al2O3(s)aluminum oxidee) zinc ore, ZnS(s)zinc sulfidef) cassiterite, SnO2(s)tin (IV) oxideWrite the IUPAC and Classical names for the following compounds if needed:Na2O(s)sodium oxideSnCl4(s)tin (IV) chloridestannic chlorideZnI2(s)zinc iodideSrCl2(s)strontium chlorideAlBr3(s)aluminum bromidePbCl4(s)lead (IV) chlorideplumbic chlorideWrite the chemical formulas and names for the compounds formed by the pairs of elements below:a) strontium and oxygen SrOstrontium oxideb) sodium and sulfurNa2Ssodium sulfidec) barium and fluorineBaF2barium flrouided) silver and iodineAgIsilver iodidee) calcium and bromineCaBr2calcium bromidef) lithium and chlorineLiCllithium chlorideWorksheet 2 – Nomenclature 2For each of the following compounds use stock and classical naming systems when needed:a) NaNO3(s)sodium nitrate -found in tobaccob) NaNO2(s)sodium nitire-a meat preservative c) Cu(NO3)2(s)copper (II) nitratecupric nitrate-blue solution in waterd) CuNO3(s)copper (I) nitratecuprous nitrate-green solution in watere) Al2(SO3)3(s)aluminum sulfite-a food additive in picklesf) Ca(OH)2(s)calcium hydroxide-firming agent in fruit productsg) PbCO3(s)lead (II) carbonateplumbous carbonate-cerussite, a mineralh) Sn3(PO4)2(s)tin (II) phosphatestannous phosphate-use to fix paints to silki) Fe2(SO4)3(s)iron (III) sulfateferric sulfate-a mineral found on MarsWrite the chemical formula for each of the following compounds:calcium carbonate CaCO3-active ingredient in antacidssodium bicarbonateNaHCO3-a foaming agent added to foodssodium hypochloriteNaClO-a component of bleachcalcium sulfateCaSO4-plaster of Parisammonium nitrateNH4NO3-used in fertilizerammonium phosphate(NH4)PO4-a leavening agent added to foodscopper (II) sulfateCuSO4-used as a fungicidesodium hydroxideNaOH-a strong base used as a washing agentpotassium permanganateKMnO4-a traditional antisepticUse IUPAC and Archaic systems (if necessary) to name each of the following compounds:a) LiClO3(s) lithium chlorateb) BaSO4(s) ) barium sulfatec) Hg2CO3(s) mercury (II) carbonatemercurous carbonated) Mg(NO3)2(s) magnesium nitratee) Fe(BrO3)3(s) iron (III) bromateferric bromatef) Na3PO4(s) sodium phosphateg) NH4IO3(s) ammonium iodateh) AuC2H3O2(s) gold (I) acetateaurous acetatei) Zn3(PO4)2(s) zinc phosphatej) Sb(ClO3)5(s) antimony (V) chlorateantimonic chloratek) MnSO4(s) manganese (II) sulfatemanganous sulfatel) KBrO(s) potassium hypobromitem) AlPO5(s) aluminum perphosphateWrite the chemical formulas for each of the following molecules:a) nitrogenN2b) carbon dioxideCO2c) carbon monoxideCOd) nitrogen dioxideNO2e) nitrogen monoxideNOf) dinitrogen monoxideN2Og) dinitrogen tetroxideN2O4h) sulfur dioxideSO2i) diiodine pentoxideI2O5j) silicon tetrafluorideSiF4k) boron trifluorideBF3l) phosphorus triiodidePI3m) diphosphorus pentoxide P2O5n) hexanitrogen heptachloride N6Cl7Rename each of the following compounds using the Stock system and give the chemical formula for each compound:a) ferrous sulfide FeSiron (II) sulfideb) plumbic bromidePbBr4lead (IV) bromidec) stannous chlorideSnCl2tin (I) chlorided) cuprous hypophosphite Cu3PO2copper (I) hypophosphitee) stannic chloriteSn(ClO2)4tin (IV) chloritef) ferrous bromateFe(BrO3)2iron (II) bromateg) ferric chloriteFe(ClO2)3iron (III) chloriteh) plumbic sulfatePb(SO4)2lead (IV) sulfatei) titaniumic arseniteTi3(AsO3)titanium (IV) arsenitej) arsenous nitriteAs(NO2)3arsenic (III) nitritek) cobaltic acetateCo(C2H3O2)3cobalt (III) acetateName the following compounds:a) SF6(g)sulfur hexafluoride b) N2O3(g)dinitrogen trioxidec) NO2(g)nitrogen dioxided) PCl3(l)phosphorus trichloridee) PCl5(s)phosphorus pentachloridef) S5P4(s)pentasulfur tetraphosphideg) Se2F(s)diselenium monoflrouideh) N2I7(s) dinitrogen heptaiodideWorksheet 3 – Nomenclature 31. Name the following hydrated compounds:a) CuSO4?5H2Ocopper (II) sulfate pentahydrateb) Na2SO4?10H2Osodium sulfate decahydratec) MgSO4?7H2Omagnesium sulfate heptahydrated) LiNO3?3H2Olithium nitrate trihydratee) CaSO3?8H2Ocalcium sulfite octahydrate2. Write the chemical formulas for the following hydrates:a) iron(III) oxide trihydrateFe2O3?3H2O -rustb) aluminum chloride hexahydrateAlCl3?6H2O-component of antiperspirantc) sodium thiosulfate pentahydrateNaS2O3?5H2O-photographic “hypo”d) cadmium (II) nitrate tetrahydrateCd(NO3)2?4H2O-photographic emulsione) lithium chloride tetrahydrateLiCl?4H2O-in fireworksf) calcium chloride dihydrateCaCl2?2H2O-deicerWrite the names of the following bases:a) KOH(aq)potassium hydroxideb) Ca(OH)2(aq)calcium hydroxideWrite the formulas of the following bases:a) aqueous magnesium hydroxideMg(OH)2(aq)b) aqueous sodium hydroxideNaOH(aq)c) aqueous aluminum hydroxideAl(OH)2(aq)Write the chemical formulas for the following compounds:a) aqueous hydrogen chlorideHCl(aq)b) hydrochloric acidHCl(aq)c) aqueous hydrogen sulfateH2SO4(aq)d) sulfuric acidH2SO4(aq)e) aqueous hydrogen acetateCH3COOH(aq)f) acetic acidCH3COOH(aq)g) aqueous hydrogen nitriteHNO3(aq)h) nitric acidHNO3(aq)i) hydrobromic acidHBr(aq)j) hyposulfurous acidH2SO2(aq)k) hydroiodic acidHI(aq)l) aqueous hydrogen perchlorateHClO4(aq)Name each of the following compounds using both the “classical” and the “IUPAC” nomenclature systems:a) H2SO3(aq)aqueous hydrogen sulfitesulfurous acidb) H3PO4(aq)aqueous hydrogen phosphatephosphoric acidc) HCN(aq)aqueous hydrogen cyanidehydrocyanic acidd) H2CO3(aq)aqueous hydrogen carbonatecarbonic acide) H2S(aq)aqueous hydrogen sulfidehydrosulfuric acidf) HCl(aq)aqueous hydrogen chloridehydrochloric acidg) H2SO4(aq)aqueous hydrogen sulfatesulfuric acidh) H3PO3(aq)aqueous hydrogen phosphitephosphorous acidWorksheet 4 – Nomenclature 4Write 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 chlorideb) FeO(s)iron (II) oxideferrous oxidec) Cs2S2O3cesium thiosulfated) Cu3(AsO4)2copper (II) arsenatecupric arsenatee) Cu3AsO4copper (I) arsenatecuprous arsenatef) SrCl2?3H2O strontium chloride trihydrateg) HI(g)hydrogen iodideh) HI(aq)aqueous hydrogen iodidehydroiodic acidi) O8Cl4octaoxygen tetrachloridej) H3PO4(aq)aqueous hydrogen phosphatephosphoric acidk) CaHPO4(aq) calcium hydrogen phosphatel) P3F9triphosphorus nonafluoridem) BeSberyllium sulfiden) AuI3gold (III) iodideauric iodideo) KMnO4(s)potassium permanganatep) (NH4)OH(aq) ammonium hydroxideq) HCl(aq)aqueous hydrogen chloridehydrochloric acidr) HBrO2(aq)aqueous hydrogen bromitebromous acids) HCN(aq)aqueous hydrogen cyanidehydrocyanic acidt) HBrO2(g)hydrogen bromiteu) LiH2PO4(aq) lithium dihydrogen phosphatev) Al(H2PO2)3(aq) aluminum dihydrogen phosphatew) AlCl3?8H2Oaluminum chloride octahydratex) S3Cl5trisulfur pentachloridey) Ti3N4titanium (IV) nitridetitaniumic nitridez) Sr(ClO)2(s)strontium hypochloriteaa) HNO(aq)aqueous hydrogen hyponitritehyponitrous acidbb) FrIO2francium ioditecc) (NH4)3AsO3ammonium arsenitedd) HgMnO4mercury (I) permanganatemercurous permanganateee) HBr(g) hydrogen bromideff) H2SO4(aq)aqueous hydrogen sulfatesulfuric acidgg) N2O2 dinitrogen dioxidehh) XeF6xenon hexaflourideii) H2SO3(aq)aqueous hydrogen sulfitesulfurous acidjj) HBr(aq)aqueous hydrogen bromidehydrobromic acidkk) BeHSO3(aq) beryllium hydrogen sulfitell) RbClO4rubidium perchloratemm) H2CO3(aq) aqueous hydrogen carbonatecarbonic acidnn) H2CO4(aq)aqueous hydrogen percarbonatepercarbonic acidoo) H2Se(aq)aqueous hydrogen selenidehydroselenic acidpp) BaSO2?10H2Obarium hydrosulfite decahydrateqq) Pb(HCO)4lead (II) hypocarboniteplumbous hypocarboniterr) Fe2(HCO4)3iron (III) percarbonateferric percarbonatess) H2Odihydrogen monoxidewaterWorksheet 5 –Nomenclature 5Write the chemical formulas of the following compounds:a) radium oxideRaOb) hexanitrogen difluorideN6F2c) tin (IV) permanganateSn(MnO4)4d) cupric carboniteCuCO2e) aqueous hydrogen iodideHI(aq)f) magnesium dihydrogen phosphateMg(H2PO4)2g) cuprous nitrite dehydrateCuNO2?10H2Oh) hypobromous acid HBrO(aq)i) aqueous hydrogen hypobromiteHBrO(aq)j) hydrogen bromideHBr(g)k) aqueous hydrogen bromideHBr(aq)l) hydrobromic acidHBr(aq)m) ammonium phosphate(NH4)3PO4n) titaniumic chlorideTiCl4o) oxygen dichlorideOCl2p) aluminum nitrideAlNq) potassium dichromateK2Cr2O7r) phosphoric acidH3PO4(aq)s) phosphorous acidH3PO3(aq)t) hydrogen cyanideHCNu) lithium ioditeLiIO2v) ammonium thiosulfate(NH4)2S2O3w) antimonic persulfateSb2(SO5)5x) aqueous hydrogen sulfateH2SO4(aq)y) sulfuric acidH2SO4(aq)z) aluminum hydrogen hypocarboniteAl(HCO)3aa) octasulfur decachlorideS8Cl10bb) pernitric acidHNO4(aq)cc) aqueous hydrogen pernitrateHNO4(aq)dd) cuprous chloride hexahydrateCuCl?6H2Oee) nickelic phosphideNiPff) lithium iodateLiIO3gg) diphosphorus tetraiodideP2I4hh) potassium thiosulfateK2S2O3ii) calcium hydrogen phosphateCaHPO4jj) aqueous magnesium hydroxideMg(OH)2(aq)kk) hydrochloric acidHCl(aq)ll) acetic acidCH3COOH(aq)mm) cobalt (III) dichromateCo2(Cr2O7)3nn) mercury (I) carbideHg4Coo) titaniumous hydrogen sulfideTi(HS)3pp) cesium cyanateCsOCNqq) nonanitrogen trifluorideN9F3rr) nickel (III) oxideNi2O3ss) hypophosphorous acidH3PO2(aq)tt) perphosphoric acidH3PO5(aq)uu) aqueous hydrogen perphosphateH3PO5(aq)vv) persulfuric acidH2SO5(aq)Worksheet 6 - Balancing Chemical EquationsWrite balanced equations for the following reactions:The reaction of ammonia with iodine forms aqueous nitrogen triiodide and hydrogen gas. ___________________________________________________________________When heated mercury (II) oxide decomposes into mercury and oxygen gas. ___________________________________________________________________The reaction of iron (III) oxide with carbon produces carbon monoxide and iron. ___________________________________________________________________The combustion of ammonia produces nitrogen monoxide and water ___________________________________________________________________Magnesium reacts with sulfuric acid, forming magnesium sulfate and releasing hydrogen gas. ___________________________________________________________________Ethane, CH3CH3, burns in oxygen gas to form carbon dioxide and water. ___________________________________________________________________Potassium chlorate, a good oxidizing agent, will readily produce potassium chloride and oxygen gas. ___________________________________________________________________Sulfuric acid is produced by reacting sulfur dioxide with oxygen gas, and water. ___________________________________________________________________2. Balance the following equationsa) Li2O(s) +H2O(l) LiOH(aq) Na(s) + Cl2(g) NaCl(s) Al2O3(s) + H2(g) Al(s) + H2O(l) Fe(s) + O2(g) Fe2O3(s) Al(s) + HCl(aq) AlCl3(aq) + H2(g) Al(s) + O2(g) Al2O3(s) KMnO4(s) + HCl(aq) Cl2(g) + MnCl2(aq) + KCl(aq) + H2O(l) MgCl2(aq) + NH4NO3(aq) Mg(NO3)2(aq) + NH4Cl(aq) Pb(C2H5)(l) + O2(g) PbO(s) + CO2(g) + H2O(l) Ca(s) + H2O(l) H2(g) + Ca(OH)2(aq) Worksheet 7 – Types of ReactionsFor the following reactions identify:the type of reactionpredict the products (be sure to include states of matter)balance the equationWrite “no reaction” if nothing happens. Type of ReactionCaSO4(s) CaO(s) + SO3(g)decompositionCl2(aq) + NaI(aq) I2(aq) + NaCl(aq) single-displacementZn(s) + CuCl2(aq) Cu(s) + ZnCl2(aq)single-displacementKOH(aq) + MgCl2(aq) KCl(aq) + Mg(OH)2(s)double-displacementLi2O(s) + CO2(g) Li2CO3(s)synthesisAl(s) + H2O(l) Al(OH)3(s) + H2(g)single-displacementMg(s) + Zn(NO3)2(aq) Mg(NO3)2(aq) + Zn(s)single-displacementSn(s) + HCl(aq) SnCl2(aq) + H2(g)single-displacementHg2(NO3)2(aq) + NaCl(aq) NaNO3(aq) + HgCl(s)double-displacementNa2CO3(aq) + H3PO4(aq) Na3PO4(aq) + H2O(l) + CO2(g)double/decompositionZn(s) + O2(g) ZnO(s)synthesisBr2(aq) + MgI2(aq) MgBr2(aq) + I2(aq)single-displacementS(s) + O2(g) SO2(g)synthesisCaO(s) + H2O(l) Ca(OH)2(aq)synthesisCu(s) + Hg(NO3)2(aq) No ReactionKOH(aq) + HClO(aq) KClO(aq) + H2O(l)double-displacementNi(s) + CuSO4(aq) NiSO4(aq) + Cu(s)single-displacementH2(g) + Cl2(g) HCl(g)synthesisNH4NO3(aq) + KOH(aq) KNO3(aq) + H2O(l) + NH3(g)double/decompositionNaOH(aq) + H2SO4(aq) Na2SO4(aq) + H2O(l)double displacementF2(aq) + AlCl3(aq) AlF3(aq) + Cl2(aq)single-displacementAl(NO2)3(s) Al2O3(s) + NO(g)decompositionCsNO3(aq) + Na2S(aq) No ReactionBaO(s) + ClO2(g) BaClO3(s)synthesisCa(s) + HIO3(aq) CaIO3(aq) + H2(g)single-displacementNH4Cl(aq) + Al(OH)3(aq) AlCl3(aq) + H2O(l) + NH3(g)double/decompositionNa(s) + CuCl(aq) NaCl(aq) + Cu(s)single-displacementWorksheet 8 – Types of ReactionsIn 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 Reaction4. 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 Reaction7. CaCO3(s) CaO(s) + CO2(g)8. P4(s) + O2(g) P2O3(g) 9. RbNO3(aq) + BeF2(aq) No Reaction10. 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)3PO4Na3PO4(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 Reaction18. 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 Reaction26. 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 9 – Net Ionic EquationsWrite 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)37858701695451903730168275Total 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)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)4835525167005407225516700521164551670052798445166370Total 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) 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)4383405173355373951517335530949901733551449070173355Total 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)Write the net ionic equation for each of the following reactions: 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)1902460169545Total Ionic Equation:2Na+(aq)+ CO32-(aq) + Ca2+(aq) +2Cl-(aq) 2Na+(aq)+2Cl-(aq)+ CaCO3(s)490029510160432752510160372935598562Na+(aq)+ CO32-(aq) + Ca2+(aq) +2Cl-(aq) 2Na+(aq)+2Cl-(aq)+ CaCO3(s) Net Ionic Equation:CO32-(aq) + Ca2+(aq) CaCO3(s)When solid magnesium metal is added to a solution of zinc chloride, solid zinc metal is formed, leaving a solution of magnesium chlorideBalanced Equation:ZnCl2(aq) + Mg(s) MgCl2(aq) + Zn(s)Total Ionic Equation:Zn2+(aq) + 2Cl-(aq) + Mg(s) Mg2+(aq) + 2Cl-(aq) + Zn(s)4281170127024923751270Zn2+(aq) + 2Cl-(aq) + Mg(s) Mg2+(aq) + 2Cl-(aq) + Zn(s)Net Ionic Equation:Zn2+(aq) + Mg(s) Mg2+(aq) + Zn(s)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)488632576204210685762035509757896190500076202Na+(aq) +2I-(aq)+ Pb2+(aq)+ 2NO3-(aq)2Na+(aq) + 2NO3-(aq) + PbI2(s)Net Ionic Equation:2I-(aq) + Pb2+(aq) PbI2(s)Write the net ionic equation for each of the following reactions. 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)471995544454163060444535509204445190500044452Na+(aq) + S2-(aq)+ 2H+(aq) + 2Cl-(aq)2Na+(aq) +2Cl-(aq) +H2S(g)Net Ionic Equation:S2-(aq)+ 2H+(aq) H2S(g) 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)46716952540411543525403431540254018249902540K+(aq) + OH-(aq) + H+(aq) + NO3- (aq) K+(aq) + NO3- (aq) + H2O(l)Net Ionic Equation:OH-(aq) + H+(aq) H2O(l) Worksheet 13 – Electron Configurations of AtomsWrite the full and shorthand (condensed) electron configurations for each of the following atoms.phosphorus1s22s22p63s23p3[Ne]3s23p3beryllium1s22s2[He]2s2fluorine1s22s22p5[He]2s22p5calcium1s22s22p63s23p64s2[Ar]4s2zinc1s22s22p63s23p64s23d10[Ar]4s23d10tellurium, 1s22s22p63s23p64s23d104p65s24d105p4[Kr] 5s24d105p4sodium1s22s22p63s1[Ne]3s1nickel1s22s22p63s23p64s23d8[Ar]4s23d8oxygen1s22s22p4[He]2s22p4iron1s22s22p63s23p64s23d6[Ar]4s23d6magnesium1s22s22p63s2[Ne]3s2aluminum1s22s22p63s23p1[Ne]3s23p1Write shorthand (condensed) electron configuration for each of the following atoms.holmium[Xe]6s24f11osmium[Xe]6s24f145d6lead[Xe]6s24f145d106p2radium[Rn]7s2bohrium[Rn]7s25f146d5Determine which elements have the following electron configurations:a) 1s22s22p63s23p4 Sb) 1s22s22p63s23p64s23d104p65s1 Rbc) [Kr] 5s24d105p3 Sb d) [Xe] 6s24f145d6 Ose) [Rn] 7s25f11 EsDetermine which electron configurations are not valid.a) 1s22s22p63s23p64s24d104p5 nob) 1s22s22p63s33d5 noc) [Ra] 7s25f8 nod) [Kr] 5s24d105p5 yese) [Xe] no – better to put [Kr]5s24d105p6 Which block of the periodic table are each of the following elements located in?a) einsteiniumfb) poloniumpc) rutherfordiumdd) franciumsWithout looking at the periodic table, identify the group number, period number, and block of an atom that has each of the following electron configurations.a) [Ne]3s1group 1, period 3, s blockb) [He]2s2group 2, period 2, s blockc) [Kr]5s24d105p5group 17, period 5, p blockWhat is the number of orbitals in each of the following subshells?a) 2s 1b) 4p3c) 3d5d) 1p 0e) 4f7f) 2p3g) 2d5h) 6g9What is the maximum number of electrons in each of the following subshells?a) 2s2b) 4p6c) 3d10d) 1p0e) 4f14f) 2p6g) 2d10h) 6g18Worksheet 14 – Orbital and Energy Level DiagramsIdentify and correct the errors in each of the following valence shell orbital diagrams: Element s orbital p orbitalsa) carbonCorrect:b) sulfurCorrect:c) aluminumCorrect:Consider the valence level electron configurations of the following five elements:Elements orbitalp orbitals12345a) Which of the above elements are metals? 2, 3, 4 could be metalsb) Which of the above elements would form an ion with a +2 charge? 3, possibly 4c) Which of the above elements is a noble gas? 1, possibly 3 a halogen? 5d) Which of the above elements has the same configuration as S2- ? 1Write the orbital occupied by the last electron of each of the following elements:AsWLiUORnV4p5d2s5f2p6p3dDraw an orbital diagram for each of the following. a) a cobalt atom (Co)1s2s2p3s3p4s3db) a sulfide ion S2–1s2s2p3s3p4sc) a cadmium ion (Cd2+) 1s2s2p3s3p4s3d4p5s4dDraw a complete energy level diagram (vertical) for an atom of iron, Fe.Worksheet 15 – Quantum NumbersState the four quantum numbers and the possible values they may have.n = 1,2,3,4,5,6,7,8 , l = 0,1,2,3 , ml = -l...+l , ms = +? , -?2. Name the orbitals described by the following quantum numbers??? a. n = 3, L = 0 , 3s??? b. n = 3, L = 1, 3p??? c. n = 3, L = 2, 3d??? d. n = 5, L = 0, 5s3. Give the n and L values for the following orbitals??? a. 1s, n = 1 l = 0 ??? b. 3s, n = 3 l = 0??? c. 2p, n = 2 l = 1??? d. 4d, n = 4 l = 2??? e. 5f, n = 5 l = 34. Place the following orbitals in order of increasing energy:??? 1s, 3s, 4s, 6s, 3d, 4f, 3p, 7s, 5d, 5p , 1s, 3s, 3p, 4s, 3d, 5p, 6s, 5d, 7s5. What are the possible mL values for the following types of orbitals???? a. s, 0??? b. p, -1, 0, +1??? c. d, -2, -1, 0, +1, +2??? d. f, -3, -2, -1, 0, +1, +2, +36. How many possible orbitals are there for n =??? a. 4, 16??? b. 10, 1007. How many electrons can inhabit all of the n=4 orbitals?328. Tabulate all of the possible orbitals (by name, i.e. 4s) for n=4 and give the three quantum numbers which define each orbital.4s n = 4, l = 0, ml = 0 4p n = 4, l = 1, ml = -1, 0, +1 4d n = 4, l = 2, ml = -2, -1, 0, +1, +2 4f n = 4, l = 3, ml = -3, -2, -1, 0, +1, +2, +39. Write electron configurations for the following atoms:??? a. H 1s1d. F1s22s22p5??? b. Li1s22s1e. Br1s22s22p63s23p64s23d104p5??? c. N1s22s22p3??? Worksheet 16 - Atomic Structure Test Review1) Which one of the following statements regarding Rutherford’s gold foil experiment is TRUE?Rutherford predicted that most of the alpha particles would pass straight through the foil because atoms are mainly empty space.Rutherford predicted that the alpha particles that hit negative particles would bounce back towards the radioactive source.The actual experimental results led Rutherford to conclude that atoms have a central positive core because most of the alpha particles were deflected at large angles.Since most of the alpha particles passed straight through the foil without deflection, Rutherford concluded that atoms are mainly empty space.The most surprising thing about the experimental results was that only some of the alpha particles were deflected at large angles.2) In Thomson’s model of the atom:negative particles are embedded within a sphere of positive chargeatoms are tiny, indivisible spherespositive particles are embedded within a sphere of negative chargethere is a positive nucleus surrounded by empty space3518535323215X020000X34804352908303) Which one of the following could be the electron configuration for an element with the following Lewis diagram?a) 1s22s1b) 1s22s22p3c) 1s22s22p1d) [Ar]4s23d3e) more than one are correct4330700269875004) The species with the following energy level diagram is:a) Neb) Nac) Na+d) Ke) Cl– 5) In the emission spectrum of hydrogen, which electronic transition would produce a line in the visible region of the electromagnetic spectrum?a) n = 2 n = 1b) n = 3 n = 2c) n = 2 n = 3d) n = n = 16) How many unpaired electrons are in the ground state energy level diagram for an atom of sulfur?a) 1b) 2c) 3d) 4e) 57) Which of the following particles has the same electron configuration as krypton?a) Ga3+b) Ga3–c) Sn4+d) Sn2+e) As3–8) Complete the following table:Name of ElementSymbol of Atom or IonAtomic NumberMass NumberNumber of ProtonsNumber of NeutronsNumber of ElectronsOverall ChargeaberylliumBr494540bfluorineF-919910101-cironFe3+26562630233+dseleniumSe2-34793445362- 9) Write the full electron configuration for each of the following atoms:a) strontium1s22s22p63s23p64s23d104p65s2b) germanium1s22s22p63s23p64s23d104p210) Write the shorthand electron configuration for each of the following atoms:a) silicon[Ne]3s23p2b) molybdenum[Kr]5s24d4c) terbium[Xe]6s24f9d) gold[Xe]6s24f145d9e) seaborgium[Rn]7s25f146d411) Draw orbital diagrams for each of the following ions (shorthand), indicate which electrons have been gained/lost:a) Cu+ 4s↑ 3d↑↓↑↓↑↓↑↓↑↓b) Pb2+ 6s↑↓ 5d↑↓↑↓↑↓↑↓↑↓ 6p↑↑c) Br– 4s↑↓ 3d↑↓↑↓↑↓↑↓↑↓ 4p↑↓↑↓↑↓d) Sb3– 5s↑↓ 4d↑↓↑↓↑↓↑↓↑↓ 5p↑↓↑↓↑↓e) Ba2+ 6s↑↓f) Sn4+ 5s↑↓ 4d↑↓↑↓↑↓↑↓↑↓ 5p↑↑12) What is the maximum number of electrons in:a) n = 3 , 18b) 3d , 10c) 6p , 6d) 4f, 14e) 2s , 2f) n = 5 , 50g) all d orbitals of curium, Cm , 3013) State the four quantum numbers for each of the following:a) the 31st electron of Ga , 4, 1, -1, +?b) the 12th electron of magnesium, 3, 0, 0, -?c) the 80th electron of mercury, 4, 2, +2, -?d) the 54th electron of xenon, 5, 1, +1, -?e) the 68th electron of holmium, 4, 3, 0, +?Worksheet 17 - Periodic Trends1) Which of the following elements has the largest atomic radius?a) berylliumb) carbonc) nitrogen d) oxygen2) Which of the following elements has the smallest atomic radius?a) sulfurb) seleniumc) oxygend) tellurium3) Which of the following elements has the smallest first ionization energy?a) strontiumb) calciumc) bariumd) magnesium4) Which of the following elements has the largest first ionization energy?a) bromine b) potassiumc) arsenicd) calcium5) Which of the following elements has the highest electron affinity?a) chlorineb) siliconc) sodiumd) phosphorus6) Which element in the following sets should have the largest atomic radius, and why?a) boron, lithium, or fluorineb) potassium, lithium, or sodium7) Which element in the following pairs has the higher first ionization energy?a) cesium or goldb) sulfur or phosphorusc) magnesium or aluminumd) neon or kryptone) oxygen or seleniumf) barium or calcium8) Which element in the following sets loses an electron most readily, and why?a) boron, lithium, or fluorineb) potassium, lithium, or sodium- lowest ionization energy/largest size - lowest ionization energy/largest size- electron farther from attractive positive force of nuceleus9) List each of the following sets in order of increasing radius:a) Ne, Na+, O2–Na+, Ne, O2–b) Mg2+, Na+, Al3+Al3+, Mg2+, Na+ c) N3–, O2–, F1–N3–, O2–, F1–10) The ion Na+ and the atom Ne have the same electron configuration. To remove an electron from gaseous neon atoms requires 2081 kJ/mol. To remove an electron from a gaseous Na+ ion requires 4562 kJ/mol. Why are these values not the same?Both have 10 electrons (2 electrons in first shell, 8 in second), but Ne has 10 protons in nucleus and Na+ has 11 protons in nucleus. (ENC of Ne is 0, ENC of Na+ is +1) The 11 protons are holding on to the electrons more strongly than neon’s 10 protons, therefore it would take more energy to remove an electron from Na+. (Note: You should draw/write configurations, orbital diagram or Bohr-Rutherford diagrams in your answer.)11) The second ionization energy of magnesium is only about twice as great as the first ionization energy. However, the third ionization energy is about ten times as great as the first. Why does it take so much more energy to remove the third electron from magnesium?A magnesium atom has 2 electrons in the valence shell. Once the first two electrons are removed, the third electron is a whole shell closer to the nucleus, therefore it would require significantly more energy to remove this electron. (You should draw/write configurations, orbital diagrams, or a Bohr-Rutherford diagram in your answer.)12) The following graph shows the melting points (and boiling points) of the period 3 elements.a) Why is there a general increase in melting point for Na, Mg, and Al?Smaller radius and increased nuclear charge cause increased strength of metallic bonding.b) Why does Si have the highest melting point?Si is the only element in the period that exists as a network covalent structure.c) Why is there a general decrease in melting point for P4, S8, and Cl2?Molecules with larger mass/size experience stronger intermolecular forces (van der Waals’ forces), thus S8 has slightly higher m.p. than P4, and Cl2 is lower than both of the others.d) Why do the noble gases have the lowest melting point?Noble gases exist as single, diatomic elements, therefore very low van der Waals forces.13) Although the first ionization energy of K is smaller than that of Ca, the second ionization energy of K is much higher than that of Ca. Why is this so?Potassium has one valence electron, while calcium has two valence electrons. Once the first electrons have been removed, the second electron of potassium is in the third shell, while the second electron of calcium is still in the fourth shell. It would require much more energy to remove the second electron from potassium because it is much closer to the nucleus. (You should draw/write configurations, orbital diagrams, or Bohr-Rutherford diagrams in your answer.)14) ElementI1I 2I 3I 1 = 1st ionization energy (kJ/mol) AA53110876270I 2 = 2nd ionization energy (kJ/mol) BB209031354180I 3 = 3rd ionization energy (kJ/mol) CC523836011704Which of the above elements would most likely be an alkali metal?CC would most likely be the alkali metal (group 1) because there is a big jump in ionization energy from I1 to I2 indicating that the second electron is a shell closer to the nucleus than the first.Which of the above elements would most likely be a noble gas?BB would most likely, of the three elements above, to be a noble gas because there is no big jump in ionization energy. AA is a Group 2 element.Worksheet 18 - Alkali Metals and HalogensState whether each of the following properties increase or decrease going down the alkali metal group.a) atomic radiusincreasesb) ionic radiusincreasesc) ionization energydecreasesd) electronegativitydecreasese) reactivitydecreasesState whether each of the following properties increase or decrease going down the halogen group.a) atomic radiusincreasesb) ionic radiusincreasesc) ionization energydecreasesd) electronegativitydecreasese) reactivitydecreasesWhat is the state of matter at room temperature for each of the following?a) F2gasb) Cl2gasc) Br2liquidd) I2solid4) For each of the following, circle the correct element. Li Si S metal N P As smallest ionization energy K Ca Sc largest atomic mass S Cl Ar member of the halogen family Al Si P greatest electron affinity Ga Al Si largest atomic radius V Nb Ta largest atomic number Te I Xe member of noble gases Si Ge Sn 4 energy levels Li Be B member of alkali metals As Se Br 6 valence electrons H Li Na nonmetal Hg Tl Pb member of transition metals Na Mg Al electron distribution ending in s2 p1 Pb Bi Po metalloid B C N gas at room temperature Ca Sc Ti electron distribution ending in s2 d2Worksheet 19 – PolarityIn each of the following problems, rank the molecules from lowest to highest polarity:1)PF3, LiOH, SF2, NF3NF3 < SF2 < PF3 < LiOH2)Ni(OH)3, N2H2, CH3OH, C2H5OHN2H2 < C2H5OH < CH3OH < Ni(OH)33)B2F4, H2C2O4, CuCl2, CF2ONO2 < SO < SeCl2 < PbCl24)PH3, PF3, NH3, NF3PH3 < NH3 < NF3 < PH35)H2O, H2S, HF, H2H2 < H2S < H2O < HF ................
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