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Chemical Bonding

Chemical Bonding. Why bond anyway? Increase Stability Decrease Potential Energy … stored energy is difficult to maintain (batteries expire, food spoils). What is a bond? an attractive force between atoms or ions that binds them together as a unit. Chemical Bonding.

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Chemical Bonding

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  1. Chemical Bonding Why bond anyway? Increase Stability Decrease Potential Energy… stored energy is difficult to maintain (batteries expire, food spoils). What is a bond? an attractive force between atoms or ions that binds them together as a unit.

  2. Chemical Bonding Determining Bond Type There are two main bond types ionic and covalent. Ionic bonds can be identified because... The first element is a metal (cation) The second element is a nonmetal (anion) The formula may include a polyatomic ion… look for formulae that start with a metal and have 3 or more elements. Covalent bonds can be identified because... The first element is a nonmetal So is the second element; these formulae are composed of nonmetals exclusively.

  3. Ionic Formulae NaNO3 This issodium nitrate. Formula Structure Elements present Subscripts* (shows how much of each element) * If no subscript is present it means that there is only one atom of that element This is a formula unit of an ionic compound.

  4. Common Polyatomic Ions

  5. Ionic Nomenclature Naming Rules Write the names of both ions, cation first. Change the ending of monatomic anions to -ide. Polyatomic ions have special names that are not to be altered. Stock System: Use Roman numerals to show the charge of a cation if more than one is possible. The overall charge must equal zero. Example: Fe(NO3)2 becomes iron (II) nitrate iron (II) nitrate NO3-NO3- → 2- charge; Fex+ must therefore have a 2+ charge

  6. Ionic Nomenclature Practice Puzzle pieces – Cations & Anions Take the 14 cations and 13 anions provided. Come up with as many chemical combinations as you can (there are 182 possibilities). Write the chemical formula and name of each. Follow the naming rules and ONLY use one cation and one anion type at a time. Example: AlNO22+ Aluminum nitrite Al(NO2)3 Aluminum nitrite Al3+ aluminum Al(NO2)21+ Aluminum nitrite

  7. Ionic Compound Formulae(Formula Units) Fe2+ Li+ Cu+ Mg2+ Al3+ Na+ Fe3+ NH4+ Cu2+ Sn2+ Ni3+ Ag+ Sr2+ Mo6+ O2- C4- Cl- PO43- S2- NO2- SO32- F- SO42- ClO- BO33- N3- C2H3O2- Fe3(PO4)2 iron (II) phosphate FeF2 iron (II) fluoride Cation Anion Fe(ClO)2 iron (II) hypochlorite FeSO4 iron (II) sulfate Fe2C iron (II) carbide FeCl2 iron (II) chloride Fe3(BO3)2 iron (II) borate FeO iron (II) oxide Fe(NO2)2 iron (II) nitrite FeS iron (II) sulfide FeSO3 iron (II) sulfite Fe3N2 iron (II) nitride Fe(C2H3O2)2 iron (II) acetate Go To Next Slide

  8. Ionic Compound Formulae(Formula Units) Fe2+ Li+ Cu+ Mg2+ Al3+ Na+ Fe3+ NH4+ Cu2+ Sn2+ Ni3+ Ag+ Sr2+ Mo6+ O2- C4- Cl- PO43- S2- NO2- SO32- F- SO42- ClO- BO33- N3- C2H3O2- LiF lithium fluoride Li2SO4 lithium sulfate Cation Anion LiClO lithium hypochlorite LiC2H3O2 lithium acetate Li 3PO4 lithium phosphate LiCl lithium chloride Li 4C lithium carbide Li 2S lithium sulfide LiNO2 lithium nitrite Li 2SO3 lithium sulfite Li 3BO3 lithium borate Li 2O lithium oxide Li 3N lithium nitride Go To Next Slide

  9. Ionic Compound Formulae(Formula Units) Fe2+ Li+ Cu+ Mg2+ Al3+ Na+ Fe3+ NH4+ Cu2+ Sn2+ Ni3+ Ag+ Sr2+ Mo6+ O2- C4- Cl- PO43- S2- NO2- SO32- F- SO42- ClO- BO33- N3- C2H3O2- Cation Anion Cu4C copper (I) carbide Cu2O copper (I) oxide Cu3PO4 copper (I) phosphate Cu3BO3 copper (I) borate CuClO copper (I) hypochlorite CuF copper (I) fluoride Cu2S copper (I) sulfide Cu2SO4 copper (I) sulfate CuCl copper (I) chloride Cu2SO3 copper (I) sulfite CuNO2 copper (I) nitrite Cu3N copper (I) nitride CuC2H3O2 copper (I) acetate Go To Next Slide

  10. Ionic Compound Formulae(Formula Units) Fe2+ Li+ Cu+ Mg2+ Al3+ Na+ Fe3+ NH4+ Cu2+ Sn2+ Ni3+ Ag+ Sr2+ Mo6+ O2- C4- Cl- PO43- S2- NO2- SO32- F- SO42- ClO- BO33- N3- C2H3O2- Cation Anion Mg 3(PO4)2 magnesium phosphate Mg3(BO3)2 magnesium borate Mg(ClO)2 magnesium hypochlorite MgSO4 magnesium sulfate MgF2 magnesium fluoride MgCl2 magnesium chloride Mg3N2 magnesium nitride Mg(C2H3O2)2 magnesium acetate Mg(NO2)2 magnesium nitrite Mg2C magnesium carbide MgS magnesium sulfide MgSO3 magnesium sulfite MgO magnesium oxide Go To Next Slide

  11. Ionic Compound Formulae(Formula Units) Fe2+ Li+ Cu+ Mg2+ Al3+ Na+ Fe3+ NH4+ Cu2+ Sn2+ Ni3+ Ag+ Sr2+ Mo6+ O2- C4- Cl- PO43- S2- NO2- SO32- F- SO42- ClO- BO33- N3- C2H3O2- Cation Anion Al(C2H3O2)3 aluminum acetate Al2(SO4)3 aluminum sulfate AlF3 aluminum fluoride Al2O3 aluminum oxide Al(ClO)3 aluminum hypochlorite Al(NO2)3 aluminum nitrite Al2(SO3)3 aluminum sulfite Al4C3 aluminum carbide AlN aluminum nitride AlPO4 aluminum phosphate AlCl3 aluminum chloride AlBO3 aluminum borate Al2S3 aluminum sulfide Go To Next Slide

  12. Ionic Compound Formulae(Formula Units) Fe2+ Li+ Cu+ Mg2+ Al3+ Na+ Fe3+ NH4+ Cu2+ Sn2+ Ni3+ Ag+ Sr2+ Mo6+ O2- C4- Cl- PO43- S2- NO2- SO32- F- SO42- ClO- BO33- N3- C2H3O2- Cation Anion Na4C sodium carbide NaCl sodium chloride Na2O sodium oxide NaNO2 sodium nitrite NaClO sodium hypochlorite Na3PO4 sodium phosphate Na2SO4 sodium sulfate Na2SO3 sodium sulfite Na3BO3 sodium borate Na2S sodium sulfide NaF sodium fluoride NaC2H3O2 sodium acetate Na3N sodium nitride Go To Next Slide

  13. Ionic Compound Formulae(Formula Units) Fe2+ Li+ Cu+ Mg2+ Al3+ Na+ Fe3+ NH4+ Cu2+ Sn2+ Ni3+ Ag+ Sr2+ Mo6+ O2- C4- Cl- PO43- S2- NO2- SO32- F- SO42- ClO- BO33- N3- C2H3O2- Cation Anion Fe(ClO)3 iron (III) hypochlorite FeBO3 iron (III) borate FePO4 iron (III) phosphate Fe2(SO4)3 iron (III) sulfate FeF3 iron (III) fluoride FeCl3 iron (III) chloride Fe4C3 iron (III) carbide Fe(NO2)3 iron (III) nitrite FeN iron (III) nitride Fe2O3 iron (III) oxide Fe2(SO3)3 iron (111) sulfide Fe2(SO3)3 iron (III) sulfite Fe(C2H3O2)3 iron (III) acetate Go To Next Slide

  14. Ionic Compound Formulae(Formula Units) Fe2+ Li+ Cu+ Mg2+ Al3+ Na+ Fe3+ NH4+ Cu2+ Sn2+ Ni3+ Ag+ Sr2+ Mo6+ O2- C4- Cl- PO43- S2- NO2- SO32- F- SO42- ClO- BO33- N3- C2H3O2- Cation Anion (NH4)2SO4 ammonium sulfate NH4ClO ammonium hypochlorite (NH4)4C ammonium carbide NH4NO2 ammonium nitrite NH4F ammonium fluoride NH4Cl ammonium chloride (NH4)2SO3 ammonium sulfite (NH4)3PO4 ammonium phosphate (NH4)3N ammonium nitride (NH4)2O ammonium oxide (NH4)3BO3 ammonium borate (NH4)2S ammonium sulfide NH4C2H3O2 ammonium acetate Go To Next Slide

  15. Ionic Compound Formulae(Formula Units) Fe2+ Li+ Cu+ Mg2+ Al3+ Na+ Fe3+ NH4+ Cu2+ Sn2+ Ni3+ Ag+ Sr2+ Mo6+ O2- C4- Cl- PO43- S2- NO2- SO32- F- SO42- ClO- BO33- N3- C2H3O2- Cation Anion Cu(ClO)2 copper (II) hypochlorite CuF2 copper (II) fluoride CuSO4 copper (II) sulfate Cu3(PO4)2 copper (II) phosphate CuCl2 copper (II) chloride CuO copper (II) oxide Cu3(BO3)2 copper (II) borate Cu(NO2)2 copper (II) nitrite Cu3N2 copper (II) nitride CuS copper (II) sulfide Cu2C copper (II) carbide CuSO3 copper (II) sulfite Cu(C2H3O2)2 copper (II) acetate Go To Next Slide

  16. Ionic Compound Formulae(Formula Units) Fe2+ Li+ Cu+ Mg2+ Al3+ Na+ Fe3+ NH4+ Cu2+ Sn2+ Ni3+ Ag+ Sr2+ Mo6+ O2- C4- Cl- PO43- S2- NO2- SO32- F- SO42- ClO- BO33- N3- C2H3O2- SnF2 tin (II) fluoride Cation Anion Sn(ClO)2 tin (II) hypochlorite Sn3(PO4)2 tin (II) phosphate SnSO4 tin (II) sulfate SnO tin (II) oxide SnCl2 tin (II) chloride Sn(C2H3O2)2 tin (II) acetate SnS tin (II) sulfide Sn(NO2) 2 tin (II) nitrite SnSO3 tin (II) sulfite Sn3(BO3)2 tin (II) borate Sn3N2 tin (II) nitride Sn2C tin (II) carbide Go To Next Slide

  17. Ionic Compound Formulae(Formula Units) Fe2+ Li+ Cu+ Mg2+ Al3+ Na+ Fe3+ NH4+ Cu2+ Sn2+ Ni3+ Ag+ Sr2+ Mo6+ O2- C4- Cl- PO43- S2- NO2- SO32- F- SO42- ClO- BO33- N3- C2H3O2- Cation Anion NiF3 nickel (III) fluoride Ni2(SO4)3 nickel (III) sulfate NiCl3 nickel (III) chloride NiN nickel (III) nitride NiPO4 nickel (III) phosphate Ni(C2H3O2)3 nickel (III) acetate Ni2O3 nickel (III) oxide Ni2(SO3)3 nickel (III) sulfite Ni(ClO)3 nickel (III) hypochlorite Ni2S3 nickel (III) sulfide Ni(NO2)3 nickel (III) nitrite NiBO3 nickel (III) borate Ni4C3 nickel (III) carbide Go To Next Slide

  18. Ionic Compound Formulae(Formula Units) Fe2+ Li+ Cu+ Mg2+ Al3+ Na+ Fe3+ NH4+ Cu2+ Sn2+ Ni3+ Ag+ Sr2+ Mo6+ O2- C4- Cl- PO43- S2- NO2- SO32- F- SO42- ClO- BO33- N3- C2H3O2- Cation Anion Ag2SO4 silver sulfate AgClO silver hypochlorite Ag3PO4 silver phosphate AgC2H3O2 silver acetate AgCl silver chloride Ag4C silver carbide AgF silver fluoride Ag2S silver sulfide AgNO2 silver nitrite Ag2SO3 silver sulfite Ag3BO3 silver borate Ag3N silver nitride Ag2O silver oxide Go To Next Slide

  19. Ionic Compound Formulae(Formula Units) Fe2+ Li+ Cu+ Mg2+ Al3+ Na+ Fe3+ NH4+ Cu2+ Sn2+ Ni3+ Ag+ Sr2+ Mo6+ O2- C4- Cl- PO43- S2- NO2- SO32- F- SO42- ClO- BO33- N3- C2H3O2- Cation Anion SrF2 strontium fluoride Sr3(BO3)2 strontium borate Sr(ClO)2 strontium hypochlorite Sr3(PO4)2 strontium phosphate SrCl2 strontium chloride Sr2C strontium carbide Sr(NO2)2 strontium nitrite Sr3N2 strontium nitride SrSO3 strontium sulfite SrSO4 strontium sulfate SrO strontium oxide SrS strontium sulfide Sr(C2H3O2)2 strontium acetate Go To Next Slide

  20. Ionic Compound Formulae(Formula Units) Fe2+ Li+ Cu+ Mg2+ Al3+ Na+ Fe3+ NH4+ Cu2+ Sn2+ Ni3+ Ag+ Sr2+ Mo6+ O2- C4- Cl- PO43- S2- NO2- SO32- F- SO42- ClO- BO33- N3- C2H3O2- MoO3 molybdenum (VI) oxide Mo4C6 molybdenum (VI) carbide MoCl6 molybdenum (VI) chloride Mo(PO4)2 molybdenum (VI) phosphate MoS3 molybdenum (VI) sulfide Mo(SO3)3 molybdenum (VI) sulfite Mo(ClO)6 molybdenum (VI) hypochlorite Mo(BO3)2 molybdenum (VI) borate MoN2 molybdenum (VI) nitride Mo(NO2)6 molybdenum (VI) nitrite Cation Anion Mo(C2H3O2)6 molybdenum (VI) acetate Mo(SO4)3 molybdenum (VI) sulfate MoF6 molybdenum (VI) fluoride Go To Next Slide

  21. Ionic Compound Formulae(Formula Units) Fe2+ Li+ Cu+ Mg2+ Al3+ Na+ Fe3+ NH4+ Cu2+ Sn2+ Ni3+ Ag+ Sr2+ Mo6+ O2- C4- Cl- PO43- S2- NO2- SO32- F- SO42- ClO- BO33- N3- C2H3O2- Cation Anion MoO3 molybdenum (VI) oxide FeO iron (II) oxide CuO copper (II) oxide Ni2O3 nickel (III) oxide Cu2O copper (I) oxide SrO strontium oxide Al2O3 aluminum oxide Li 2O lithium oxide SnO tin (II) oxide Ag2O silver oxide (NH4)2O ammonium oxide Fe2O3 iron (III) oxide Na2O sodium oxide MgO magnesium oxide Go To Next Slide

  22. Ionic Compound Formulae(Formula Units) Fe2+ Li+ Cu+ Mg2+ Al3+ Na+ Fe3+ NH4+ Cu2+ Sn2+ Ni3+ Ag+ Sr2+ Mo6+ O2- C4- Cl- PO43- S2- NO2- SO32- F- SO42- ClO- BO33- N3- C2H3O2- Cation Anion Mo4C6 molybdenum (VI) carbide Na4C sodium carbide Ni4C3 nickel (III) carbide (NH4)4C ammonium carbide Cu2C copper (II) carbide Sr2C strontium carbide Fe2C iron (II) carbide Fe4C3 iron (III) carbide Li 4C lithium carbide Ag4C silver carbide Mg2C magnesium carbide Cu4C copper (I) carbide Al4C3 aluminum carbide Sn2C tin (II) carbide Go To Next Slide

  23. Ionic Compound Formulae(Formula Units) Fe2+ Li+ Cu+ Mg2+ Al3+ Na+ Fe3+ NH4+ Cu2+ Sn2+ Ni3+ Ag+ Sr2+ Mo6+ O2- C4- Cl- PO43- S2- NO2- SO32- F- SO42- ClO- BO33- N3- C2H3O2- MoCl6 molybdenum (VI) chloride SrCl2 strontium chloride Cation Anion NH4Cl ammonium chloride NiCl3 nickel (III) chloride AlCl3 aluminum chloride NaCl sodium chloride FeCl2 iron (II) chloride LiCl lithium chloride MgCl2 magnesium chloride CuCl2 copper (II) chloride CuCl copper (I) chloride FeCl3 iron (III) chloride SnCl2 tin (II) chloride AgCl silver chloride Go To Next Slide

  24. Ionic Compound Formulae(Formula Units) Fe2+ Li+ Cu+ Mg2+ Al3+ Na+ Fe3+ NH4+ Cu2+ Sn2+ Ni3+ Ag+ Sr2+ Mo6+ O2- C4- Cl- PO43- S2- NO2- SO32- F- SO42- ClO- BO33- N3- C2H3O2- Mo(PO4)2 molybdenum (VI) phosphate Fe3(PO4)2 iron (II) phosphate Cu3PO4 copper (I) phosphate Na3PO4 sodium phosphate AlPO4 aluminum phosphate Cation Anion Mg 3(PO4)2 magnesium phosphate Sr3(PO4)2 strontium phosphate Li 3PO4 lithium phosphate FePO4 iron (III) phosphate Ag3PO4 silver phosphate (NH4)3PO4 ammonium phosphate Cu3(PO4)2 copper (II) phosphate Sn3(PO4)2 tin (II) phosphate NiPO4 nickel (III) phosphate Go To Next Slide

  25. Ionic Compound Formulae(Formula Units) Fe2+ Li+ Cu+ Mg2+ Al3+ Na+ Fe3+ NH4+ Cu2+ Sn2+ Ni3+ Ag+ Sr2+ Mo6+ O2- C4- Cl- PO43- S2- NO2- SO32- F- SO42- ClO- BO33- N3- C2H3O2- MoS3 molybdenum (VI) sulfide SrS strontium sulfide Cation Anion Ni2S3 nickel (III) sulfide (NH4)2S ammonium sulfide CuS copper (II) sulfide Al2S3 aluminum sulfide Cu2S copper (I) sulfide FeS iron (II) sulfide SnS tin (II) sulfide MgS magnesium sulfide Fe2(SO3)3 iron (III) sulfide Na2S sodium sulfide Ag2S silver sulfide Li 2S lithium sulfide Go To Next Slide

  26. Ionic Compound Formulae(Formula Units) Fe2+ Li+ Cu+ Mg2+ Al3+ Na+ Fe3+ NH4+ Cu2+ Sn2+ Ni3+ Ag+ Sr2+ Mo6+ O2- C4- Cl- PO43- S2- NO2- SO32- F- SO42- ClO- BO33- N3- C2H3O2- Mo(NO2)6 molybdenum (VI) nitrite Cation Anion Sr(NO2)2 strontium nitrite Ni(NO2)3 nickel (III) nitrite CuNO2 copper (I) nitrite Mg(NO2)2 magnesium nitrite Fe(NO2)2 iron (II) nitrite LiNO2 lithium nitrite Sn(NO2) 2 tin (II) nitrite AgNO2 silver nitrite Al(NO2)3 aluminum nitrite Cu(NO2)2 copper (II) nitrite NH4NO2 ammonium nitrite Fe(NO2)3 iron (III) nitrite NaNO2 sodium nitrite Go To Next Slide

  27. Ionic Compound Formulae(Formula Units) Fe2+ Li+ Cu+ Mg2+ Al3+ Na+ Fe3+ NH4+ Cu2+ Sn2+ Ni3+ Ag+ Sr2+ Mo6+ O2- C4- Cl- PO43- S2- NO2- SO32- F- SO42- ClO- BO33- N3- C2H3O2- Mo(SO3)3 molybdenum (VI) sulfite CuSO3 copper (II) sulfite Cation Anion Fe2(SO3)3 iron (III) sulfite (NH4)2SO3 ammonium sulfite Al2(SO3)3 aluminum sulfite Na2SO3 sodium sulfite SrSO3 strontium sulfite MgSO3 magnesium sulfite Cu2SO3 copper (I) sulfite Ni2(SO3)3 nickel (III) sulfite FeSO3 iron (II) sulfite SnSO3 tin (II) sulfite Li 2SO3 lithium sulfite Ag2SO3 silver sulfite Go To Next Slide

  28. Ionic Compound Formulae(Formula Units) Fe2+ Li+ Cu+ Mg2+ Al3+ Na+ Fe3+ NH4+ Cu2+ Sn2+ Ni3+ Ag+ Sr2+ Mo6+ O2- C4- Cl- PO43- S2- NO2- SO32- F- SO42- ClO- BO33- N3- C2H3O2- NH4F ammonium fluoride SrF2 strontium fluoride CuF copper (I) fluoride NiF3 nickel (III) fluoride MoF6 molybdenum (VI) fluoride MgF2 magnesium fluoride CuF2 copper (II) fluoride AlF3 aluminum fluoride FeF3 iron (III) fluoride SnF2 tin (II) fluoride Cation Anion FeF2 iron (II) fluoride NaF sodium fluoride AgF silver fluoride LiF lithium fluoride Go To Next Slide

  29. Ionic Compound Formulae(Formula Units) Fe2+ Li+ Cu+ Mg2+ Al3+ Na+ Fe3+ NH4+ Cu2+ Sn2+ Ni3+ Ag+ Sr2+ Mo6+ O2- C4- Cl- PO43- S2- NO2- SO32- F- SO42- ClO- BO33- N3- C2H3O2- Mo(SO4)3 molybdenum (VI) sulfate (NH4)2SO4 ammonium sulfate Fe2(SO4)3 iron (III) sulfate Ni2(SO4)3 nickel (III) sulfate MgSO4 magnesium sulfate Al2(SO4)3 aluminum sulfate SrSO4 strontium sulfate CuSO4 copper (II) sulfate Cu2SO4 copper (I) sulfate FeSO4 iron (II) sulfate Li2SO4 lithium sulfate SnSO4 tin (II) sulfate Cation Anion Na2SO4 sodium sulfate Ag2SO4 silver sulfate Go To Next Slide

  30. Ionic Compound Formulae(Formula Units) Fe2+ Li+ Cu+ Mg2+ Al3+ Na+ Fe3+ NH4+ Cu2+ Sn2+ Ni3+ Ag+ Sr2+ Mo6+ O2- C4- Cl- PO43- S2- NO2- SO32- F- SO42- ClO- BO33- N3- C2H3O2- Mo(ClO)6 molybdenum (VI) hypochlorite CuClO copper (I) hypochlorite Fe(ClO)2 iron (II) hypochlorite AgClO silver hypochlorite Ni(ClO)3 nickel (III) hypochlorite NH4ClO ammonium hypochlorite Fe(ClO)3 iron (III) hypochlorite Sr(ClO)2 strontium hypochlorite LiClO lithium hypochlorite Cation Anion Mg(ClO)2 magnesium hypochlorite Cu(ClO)2 copper (II) hypochlorite Sn(ClO)2 tin (II) hypochlorite NaClO sodium hypochlorite Al(ClO)3 aluminum hypochlorite Go To Next Slide

  31. Ionic Compound Formulae(Formula Units) Fe2+ Li+ Cu+ Mg2+ Al3+ Na+ Fe3+ NH4+ Cu2+ Sn2+ Ni3+ Ag+ Sr2+ Mo6+ O2- C4- Cl- PO43- S2- NO2- SO32- F- SO42- ClO- BO33- N3- C2H3O2- Cu3BO3 copper (I) borate Mo(BO3)2 molybdenum (VI) borate Mg3(BO3)2 magnesium borate Cu3(BO3)2 copper (II) borate Li 3BO3 lithium borate Sr3(BO3)2 strontium borate NiBO3 nickel (III) borate Cation Anion (NH4)3BO3 ammonium borate Ag3BO3 silver borate AlBO3 aluminum borate FeBO3 iron (III) borate Sn3(BO3)2 tin (II) borate Fe3(BO3)2 iron (II) borate Na3BO3 sodium borate Go To Next Slide

  32. Ionic Compound Formulae(Formula Units) Fe2+ Li+ Cu+ Mg2+ Al3+ Na+ Fe3+ NH4+ Cu2+ Sn2+ Ni3+ Ag+ Sr2+ Mo6+ O2- C4- Cl- PO43- S2- NO2- SO32- F- SO42- ClO- BO33- N3- C2H3O2- MoN2 molybdenum (VI) nitride NiN nickel (III) nitride Mg3N2 magnesium nitride Sr3N2 strontium nitride (NH4)3N ammonium nitride Cu3N2 copper (II) nitride AlN aluminum nitride Cation Anion Cu3N copper (I) nitride Li 3N lithium nitride Ag3N silver nitride Sn3N2 tin (II) nitride Fe3N2 iron (II) nitride FeN iron (III) nitride Na3N sodium nitride Go To Next Slide

  33. Ionic Compound Formulae(Formula Units) Fe2+ Li+ Cu+ Mg2+ Al3+ Na+ Fe3+ NH4+ Cu2+ Sn2+ Ni3+ Ag+ Sr2+ Mo6+ O2- C4- Cl- PO43- S2- NO2- SO32- F- SO42- ClO- BO33- N3- C2H3O2- Cation Anion Sr(C2H3O2)2 strontium acetate NH4C2H3O2 ammonium acetate Al(C2H3O2)3 aluminum acetate Cu(C2H3O2)2 copper (II) acetate Sn(C2H3O2)2 tin (II) acetate Ni(C2H3O2)3 nickel (III) acetate CuC2H3O2 copper (I) acetate LiC2H3O2 lithium acetate Mo(C2H3O2)6 molybdenum (VI) acetate Fe(C2H3O2)2 iron (II) acetate Fe(C2H3O2)3 iron (III) acetate NaC2H3O2 sodium acetate AgC2H3O2 silver acetate Mg(C2H3O2)2 magnesium acetate Go To Next Slide

  34. Ionic Nomenclature Getting a formula out of a name Write the symbol of both ions, cation first. Include known charges of the ions. Roman numerals in the Stock system tell the charge of cations with multiple oxidation states. Polyatomic ionsdon’t have more than one oxidation state. Paying no attention to the signs of the charges crisscross them as subscripts for the opposite ions. Use parentheses if there is more than one of a polyatomic ion type. Example: iron (II) nitrate becomes Fe2+ NO31- Fe2 NO31 Fe NO3 Fe NO3 2 Fe(NO3)2

  35. Chemical Formulae Ionic versus Molecular/Covalent Ionic compounds typically feature a metal (cation) and a nonmetal (anion). Molecular compounds are composed of nonmetals exclusively. Both must be electrically neutral in charge. Nomenclature (naming) has similarities… the differences occur because of the law of multiple proportions. The same elements can make multiple, different compounds... Roman numerals or prefixes are used.

  36. Molecular Formulae CO2 This iscarbon dioxide. Formula Structure Elements present Subscripts* (shows how much of each element) * If no subscript is present it means that there is only one atom of that element This is a molecule of a molecular compound.

  37. Molecular Nomenclature Naming Rules Write the names of both elements. You will only learn covalent naming for binary compounds Change the ending of the second element to -ide. Add prefixes to each element to indicate the subscripted number of atoms present. If the first element only has one atom then no prefix is added. Example: CO2 becomes carbon dioxide carbon oxygen carbon oxide carbon dioxide

  38. Molecular Nomenclature Prefixes - Greek prefixes used… mono- di– tri- tetra- penta- hexa- hepta- octa- nona- deca- - The final “o” or “a” of the prefix is usually dropped when preceding an element beginning with a vowel.

  39. Binary/Ternary Acid Nomenclature Binary Acids are acids made of two components. Hydrogen and, A single nonmetal (F, S, Cl, Se, Br, and I) Ternary Acids are acids made of two components. Hydrogen and, A polyatomic ion Acids act as molecular and ionic compounds. When dissolved in water, acids ionize or, in some cases, dissociate.

  40. Binary Acid Formulae HCl This ishydrochloric acid. Formula Structure Elements present (always starts with hydrogen) Subscripts* (shows how much of each element) * If no subscript is present it means that there is only one atom of that element This is a molecule of a molecular compound.

  41. Binary Acid Nomenclature Naming those featuring a single nonmetal… Write “hydro” immediately followed by the second element, the nonmetal. Change the ending of the second element to -ic. Had this been a normal molecular formulae the ending would have been –ide… It maybe helpful to think “Change –ide to –ic.” Write the word “acid” Example: HCl becomes hydrochlorine hydrochloric hydrochloric acid

  42. Ternary Acid Formulae HNO2 This isnitrous acid. Formula Structure Elements present (always starts with hydrogen) Subscripts* (shows how much of each element) * If no subscript is present it means that there is only one atom of that element This is a molecule of a molecular compound.

  43. Binary Acid Nomenclature Naming those featuring a polyatomic ion… Write the name of the polyatomic ion. Change the ending of the polyatomic ion… -ate turns to -ic. “Change –ate to –ic.” -ite turns to –ous. “Change –ite to –ous.” Write the word “acid” Example: HNO2 becomes nitrous acid nitrite nitrous

  44. Binary Acid Formulae Cl- NO3- SO42- F- S2- BO33- PO43- I- ClO3- Br- HPO42- HF hydrofluoric acid H2S hydrosulfuric acid HCl hydrochloric acid H3PO4 phosphoric acid HClO3 chloric acid HI hydroiodic acid H2SO4 sulfuric acid H3PO4 phosphoric acid HBr hydrobromic acid H3BO3 boric acid HNO3 nitric acid H+

  45. Practice Go practice… over and over and over crsciences.com/hw/075_nomenclature__simple_naming_wp.htm crsciences.com/hw/076_nomenclature__names_to_formulas_wp.htm crsciences.com/hw/077_nomenclature__stock_naming_wp.htm

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