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Inorganic Nomenclature

Inorganic Nomenclature. Naming Chemical Compounds. Three categories. Binary Ionic compounds Binary Molecular Compounds Mineral Acids. Let’s see what you remember about naming ionic compounds. . . Name These Ionic Compounds... . K 2 SO 4 potassium sulfate NaOCl sodium hypochlorite PbO 2

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Inorganic Nomenclature

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  1. Inorganic Nomenclature Naming Chemical Compounds

  2. Three categories • Binary Ionic compounds • Binary Molecular Compounds • Mineral Acids

  3. Let’s see what you remember about naming ionic compounds. . .

  4. Name These Ionic Compounds... K2SO4 potassium sulfate NaOCl sodium hypochlorite PbO2 plumbic oxide -or- lead (IV) oxide (NH4)2CrO4 ammonium chromate

  5. Ionic compounds involve a metal cation and a non-metal anion • can also involve one or more polyatomic ions NB. The only polyatomic cation is ammonium, NH4+

  6. For ionic compounds • name cation first • do NOT use prefixes (mono, di, tri, etc) • combine ions to form a neutral compound eg. calcium phosphate Ca2+PO43- Ca3(PO4)2 Check that subscripts are in lowest terms.

  7. “Criss-Cross” method for Writing Ionic Formulae eg. Tin (IV)sulfite (aka stannicsulfite) Its ions are . . . Sn4+SO32- “criss-crossing” charges gives . . . Sn2(SO3)4 But Wait—not in lowest terms!! (Oh No!!) therefore Sn(SO3)2 is the formula

  8. Classical and Stock System for Multivalent Cations Fe2+ iron (II) [stock name] ferrous [classical name] Fe3+ iron (III) [stock name] ferric [classical name] NB. lower charged ion = _____ous; higher = ___ic

  9. Some Other Multivalent Cations FormulaStock nameClassical name Pb2+ _________ _____________ lead (II) plumbous Pb4+ _________ _____________ lead (IV) plumbic Sn2+ _________ _____________ tin (II) stannous Sn4+ _________ _____________ tin (IV) stannic

  10. FormulaStock nameClassical name Cu+ _________ _____________ copper (I) cuprous Cu2+ _________ _____________ copper (II) cupric Hg+ (Hg2)2+ _________ _____________ mercury (I) mercurous Hg2+ _________ ____________ mercury (II) mercuric Mercury (l) does not exist as Hg+.

  11. Consult handouts or textbook for list of the other multivalent cations.

  12. name this new compound . . . Fe2+ ______ Fe2+ / \ Fe2+ Fe2+ | | Fe2+ Fe2+ \ / Fe2+________ Fe2+ a ferrous wheel

  13. Some Anion Names are Similar . . . S2- sulfide SO32- sulfite SO42- sulfate

  14. N3- nitride NO2- nitrite NO3- nitrate

  15. Cl- chloride ClO4- perchlorate ClO3- chlorate ClO2- chlorite ClO- hypochlorite

  16. P3- phosphide PO33- phosphite PO43- phosphate

  17. CrO42- chromate Cr2O72- dichromate

  18. Practice: Ionic Nomenclature formulastock name classical name ________ calcium nitrate Ca(NO3)2 MgS _________________ magnesium sulfide ________ _____________ plumbic oxide PbO2 lead (IV) oxide (NH4)2Cr2O7 _________________ ammonium dichromate ________ sodium permanganate NaMnO4

  19. More Practice: Ionic Nomenclature formulastock name classical name ________ mercury (ll) chloride _______________ HgCl2 mercuric chloride ___________ mercury (l) chloride _______________ Hg2Cl2mercurous chloride Why do we not reduce this to HgCl? The mercury (l) ion is (Hg2)2+, NOT Hg+

  20. Binary Molecular Compounds Binary Molecular compounds made up of two non-metals. Name ends in “-ide”. Use prefixes to indicate quantity.

  21. Prefixes for Binary Molecular Cmpds. mono (1) di (2) tri (3) tetra (4) penta (5) hexa (6) hepta (7) octa (8) nona (9) deca (10)

  22. examples of Molecular Cmpds CO carbon monoxide Cl2O7 dichlorine heptaoxide SO3(NOT SO32-) sulfur trioxide P4O10 tetraphosphorus decaoxide

  23. Mineral Acids An acid is a compound that liberates H+ ions when dissolved in water. Therefore, acids must contain hydrogen. For now, acids have (aq) after their formula. HCl(g) vs. HCl(aq) hydrogen chloride hydrochloric acid

  24. How does the name of each acid correlate to ending of anion name? HCl(aq) Cl-, chloride hydrochloricacid H2SO4(aq) SO42-, sulfate sulfuricacid HNO2(aq) NO2-, nitrite nitrousacid

  25. Ending of anion name of aciddetermines name of acid 1. anion ends in “-ide” hydro_____ic acid [hydrobromicacid, HBr(aq), Br-, bromide] 2. anion ends in “-ate” _______ic acid [phosphoricacid, H3PO4(aq), PO43-, phosphate] 3. anion ends in “ite” _______ous acid [nitrousacid, HNO2(aq), NO2-, nitrite]

  26. Examples of acids formulaname HClO2(aq) _______________ chlorous acid _______________ acetic (ethanoic) acid HC2H3O2(aq) H3PO3(aq) _______________ phosphorous acid _______________ carbonic acid H2CO3(aq)

  27. more examples of acids . . . formulaname _______________ oxalic acid H2C2O4(aq) H2SO3(aq) _______________ sulfurous acid HI(aq) _______________ hydroiodic acid H2S(aq) _______________ hydrosulfuric acid

  28. Homework Do the practice problems and section review questions in section 2.2 of your text, as well as in chapter and unit review. You can also see what’s on line. Good luck!!!!

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