2. Inorganic Nomenclature Naming Chemical Compounds

3. Three categories 1.Binary Ionic compounds 2.Binary Molecular Compounds 3.Mineral Acids

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

5. Name These Ionic Compounds... K 2 SO 4 potassium sulfate NaOCl sodium hypochlorite PbO 2 plumbic oxide -or- lead (IV) oxide (NH 4 ) 2 CrO 4 ammonium chromate

6. 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, NH 4 +

7. For ionic compounds name cation first do NOT use prefixes (mono, di, tri, etc) combine ions to form a neutral compound eg. calcium phosphate Ca 2+ PO 4 3- Ca 3 (PO 4 ) 2 Check that subscripts are in lowest terms.

8. “Criss-Cross” method for Writing Ionic Formulae eg. Tin (IV) sulfite (aka stannic sulfite) Its ions are... Sn 4+ SO 3 2- “criss-crossing” charges gives... Sn 2 (SO 3 ) 4 But Wait—not in lowest terms!! (Oh No!!) therefore Sn(SO 3 ) 2 is the formula

9. Classical and Stock System for Multivalent Cations Fe 2+ iron (II) [stock name] ferrous [classical name] Fe 3+ iron (III) [stock name] ferric [classical name] NB. lower charged ion = _____ous; higher = ___ic

10. Some Other Multivalent Cations FormulaStock nameClassical name Pb 2+ ______________________ lead (II)plumbous Pb 4+ ______________________ lead (IV)plumbic Sn 2+ ______________________ tin (II)stannous Sn 4+ ______________________ tin (IV)stannic

11. FormulaStock nameClassical name Cu + ______________________ copper (I)cuprous Cu 2+ ______________________ copper (II)cupric Hg + (Hg 2 ) 2+ ______________________ mercury (I)mercurous Hg 2+ _____________________ mercury (II)mercuric Mercury (l) does not exist as Hg +.

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

13. name this new compound... Fe 2+ ______ Fe 2+ / \ Fe 2+ Fe 2+ | | Fe 2+ Fe 2+ \ / Fe 2+________ Fe 2+ a ferrous wheel

14. Some Anion Names are Similar... S 2- sulfide SO 3 2- sulfite SO 4 2- sulfate

15. N3-N3- nitride NO 2 - nitrite NO 3 - nitrate

16. Cl - chloride ClO 4 - perchlorate ClO 3 - chlorate ClO 2 - chlorite ClO - hypochlorite

17. P 3- phosphide PO 3 3- phosphite PO 4 3- phosphate

18. CrO 4 2- chromate Cr 2 O 7 2- dichromate

19. Practice: Ionic Nomenclature formulastock nameclassical name ________calcium nitrate Ca(NO 3 ) 2 MgS_________________ magnesium sulfide _____________________plumbic oxide PbO 2 lead (IV) oxide (NH 4 ) 2 Cr 2 O 7 _________________ ammonium dichromate ________ sodium permanganate NaMnO 4

20. More Practice: Ionic Nomenclature formulastock nameclassical name ________ mercury (ll) chloride_______________ HgCl 2 mercuric chloride ___________mercury (l) chloride_______________ Hg 2 Cl 2 mercurous chloride Why do we not reduce this to HgCl? The mercury (l) ion is (Hg 2 ) 2+, NOT Hg +

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

22. 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)

23. examples of Molecular Cmpds

24. 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

25. How does the name of each acid correlate to ending of anion name? HCl(aq) Cl -, chloride hydrochloric acid H 2 SO 4 (aq) SO 4 2-, sulfate sulfuric acid HNO 2 (aq) NO 2 -, nitrite nitrous acid

26. Ending of anion name of acid determines name of acid 1. anion ends in “-ide” hydro_____ic acid [hydrobromic acid, HBr(aq), Br -, bromide] 2. anion ends in “-ate” _______ic acid [phosphoric acid, H 3 PO 4 (aq), PO 4 3-, phosphate] 3. anion ends in “ite” _______ous acid [nitrous acid, HNO 2 (aq), NO 2 -, nitrite ]

28. Examples of acids formulaname HClO 2 (aq)_______________ chlorous acid _______________ acetic (ethanoic) acid HC 2 H 3 O 2 (aq) H 3 PO 3 (aq)_______________ phosphorous acid _______________carbonic acid H 2 CO 3 (aq)

29. more examples of acids...

30. 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!!!!