The document provides information on naming ionic compounds, cations, anions, and polyatomic ions. It discusses how to name monatomic and transition metal cations by adding "-ion" or the charge in Roman numerals after the element name. Anions are named by adding "-ide" after the element root. Ionic compounds are formed by writing the cation first followed by the anion. Polyatomic ions are also included.

1. Naming Ionic Compounds, Cations and Anions "What's in a name? That which we call a rose, by any other name, would smell as sweet." Romeo and Juliet (II, ii, 1-2)

5. COMPOUNDS FORMED FROM IONS Na+ + Cl-  NaCl CATION + ANION  COMPOUND A neutral compound requires equal number of (+) and (-) charges. Let’s learn how to name the ions. Then, we can name their compounds.

6. Predicting Charges on Monatomic Ions KNOW THESE !!!! +1 +2 +3 +4 -3 -2 -1 0 Cd+2

7. Naming Monatomic Cations: Rule – The metal ion has the same name as the element but add “ion” after

9. Examples of Older Names of Cations formed from Transition Metals (you do not have to memorize these)

10. Naming Monatomic Anions: Rule – When a nonmetal forms an ion, it is named: element stem name + “-ide” + ion

13. Ionic Naming Practice NaCl CaCl 2 MgO Al 2 O 3 FeBr 2 CuCl SnO 2 Fe 2 O 3 Hg 2 S

14. Ionic Naming Practice NaCl CaCl 2 MgO Al 2 O 3 FeBr 2 CuCl SnO 2 Fe 2 O 3 Hg 2 S Sodium chloride Calcium chloride Magnesium oxide Aluminium oxide Iron (II) Bromide Copper (I) Chloride Tin (IV) Oxide Iron (III) Oxide Mercury (II) Sulfide [notice the subscript number under the oxygen = the number for Iron’s Roman Numerals]

15. Ionic Naming Warm Up NaBr BeCl 2 K 2 O Al 2 S 3 AgBr 2 CdCl 2 SnO FeO CuS

16. Ionic Naming Warm Up NaBr BeCl 2 K 2 O Al 2 S 3 AgBr 2 CdCl 2 SnO FeO CuS Sodium bromide Beryllium chloride Potassium oxide Aluminium sulfide Silver Bromide Cadmium (II) Chloride Tin (II) Oxide Iron (II) Oxide Copper (II) Sulfide

21. 1. Cation first, then anion 2. Monatomic cation = elemental name Ca 2+ = calcium ion 3. polyatomic anion = name of polyatomic CO32  = carbonate Thus  CaCO3 = calcium carbonate Overview of Naming Ternary Ionic Compounds: Take Home Message: Same method as with binary ionics except a polyatomic anion is in place of the monatomic anion!

24. we’ve learned to name Chemicals Now, let’s write some formulas!

25. Ternary Ionic Formulas Calcium Sulfate Ca2+ and SO4-2 CaSO4 Iron (III) hydroxide Fe+3 and OH- Fe(OH)3 Ammonium carbonate NH4+ and CO3–2 (NH4)2CO3 The (2+) and (2-) charges cancel each other out So, we need one of each The (3+) needs (3-) to cancel but OH is only a (1-) So, we need three OH ions The (2-) needs (2+) to cancel but NH4 is only a (1+) So, we need two NH4 ions

26. Learning Check 1. aluminum nitrate a) AlNO3 b) Al(NO)3 c) Al(NO3)3 2. copper (II) nitrate a) CuNO3 b) Cu(NO3)2 c) Cu2(NO3) 3. Iron (III) hydroxide a) FeOH b) Fe3OH c) Fe(OH)3 4. Tin (IV) hydroxide a) Sn(OH)4 b) Sn(OH)2 c) Sn4(OH)

28. 1. Cation first, then anion 2. Monatomic cation = elemental name calcium = Ca2+ 3. monatomic anion = “-ide” name sulfide = S2- Thus  calcium sulfide = CaS Overview of Formula Writing Steps: Take Home Message: It’s just that easy! But, beware the charge balance!!!!!!

29. You Try it: Write these out on your notes Write the formula: Potassium bromide  Barium fluoride  Copper (II) oxide  Calcium nitride  Aluminum carbonate  Beryllium hydroxide  KBr K+ & Br- BaF2 Ba2+ & F- CuO Cu2+ & O2- Ca3N2 Ca2+ & N3- Al2(CO3)3 Al3+ & CO32- Be(OH)2 Be2+ & OH- *Notice any relationship between the charges of the anions and the subscripts on the cations? Vice-versa?

31. Got It?