2. Naming Compounds Ammonium Nitrate

3. 1) Looking at the Periodic Table, determine the number of valence electrons likely for an element. 2)The element will combine with other atoms to reach stability, generally the octet rule states that is 8 electrons in the outer shell. 3)Match the elements so that the overall charge is neutral Background: valences and formulas Examples: a) Al,Br b) K,S c) Zn,O d) Mg,N e) C,Cl f) Cu,O AlBr 3 K2SK2SZnOMg 3 N 2 CCl 4 CuO or Cu 2 O

4. Ionic compounds (metal with 1 valence) Rules for naming Anion ends in -ide. Example: sodium chloride Metal comes 1st (not chlorine sodide) Use the group valence for nonmetals Do not capitalized unless starting a sentence Give formulae & name: Ca + I, O + Mg, Na + S = Ca 2+ I 1- = CaI 2 = calcium iodide = Mg 2+ O 2- = MgO = magnesium oxide = Na 1+ S 2- = Na 2 S = sodium sulfide

5. Multiple valence: Latin naming When the metal is in an ionic compound: The metal is named with it’s Latin or English root and ends in -ic or –ous to denote valence Cu 1 is cuprous, E.g. Cu 2 is cupric Lower Valence= ous, Higher Valence= ic Give formulas and Latin names for: Cu 2 + Cl = Cu 2 Cl 1 = CuCl 2 = cupric chloride Co 2 + Cl = Co 2 Cl 1 = CoCl 2 = cobaltous chloride For Latin naming: know rules, remember Hg is an exception –it is not named w/ its Latin name

7. Name ends in -ide, positive/metal comes first The valence of the metal is indicated using roman numerals E.g. Cu 1 is copper(I), Cu 2 is copper(II) Numbers refer to valences not to #s of atoms –Examples: Cu 2+ +Cl = CuCl 2 = copper(II) chloride Zn 2+ +Cl = ZnCl 2 = zinc chloride Co 2+ +Cl = CoCl 2 = cobalt(II) chloride Hg+S = Hg 1 S 2 = Hg 2 S = mercury(I) sulfide Hg+S = Hg 2 S 2 = HgS = mercury(II) sulfide Multiple valence: IUPAC/Stock naming

8. Groups of atoms can also have valences “Polyatomic ions” are groups of atoms that interact as a single unit. E. g. OH 1, (SO 4 ) 2, (PO 4 ) Compounds containing polyatomic ions So far we have given valences to single atoms Li + + O 2-  Li 2 O Naming compounds with polyatomic ions is similar to naming other ionic compounds Compounds with polyatomic ions have names ending in -ate or -ite Note that most are negative, except ammonium Name: Ca(OH) 2, CuSO 4, NH 4 NO 3, Co 2 (CO 3 ) 3

9. - calcium hydroxide - copper(II) sulfate - ammonium nitrate - cobalt(III) carbonate Ca(OH) 2 CuSO 4 NH 4 NO 3 Co 2 (CO 3 ) 3 Compounds containing polyatomic ions

10. Naming covalent compounds -ide ending, each element has “prefix” 1mono 2di 3tri 4tetra 5penta 6hexa 7hepta 8octa 9nona 10deca prefix refers to # of atoms - not valence N 2 O 4 = dinitrogen tetroxide Exception: drop mono for first element CO 2 = carbon dioxide The first vowel is often dropped to avoid the combination of “ao” or “oo”. CO = carbon monoxide (monooxide) SO 2 = sulfur dioxide (doxide) Name: CCl 4, P 2 O 3, IF 7 P 4 O 10 = tetraphosphorus decoxide

11. Write and name the following covalent compounds (IUPAC) carbon tetrachloride diphosporus trioxide iodine heptafluoride CCl 4 P 2 O 3 IF 7 For more lessons, visit www.chalkbored.com www.chalkbored.com