1. 7.1

2.  Binary Ionic Compound (BIC) - ionic compound made up of two ions  To name cation – use name of atom  Na + = sodiumK + = potassium  Ca 2+ = calciumBa 2+ = barium

3.  To name anions, use the atom’s base name and –ide at the end  Cl - = ChlorideS 2- = Sulfide  P 3- = PhosphideO 2- = Oxide  KBr = Potassium bromide  Mg 3 N 2 = Magnesium nitride

4.  FrF  SrBr 2  Li 2 Se

5. 1. Write the symbol and charge of each ion side by side (cation first) 2. If total = 0, just write symbols & you are done! 3. If total does not = 0, criss cross charges to have overall 0 charge

6.  Magnesium sulfide  Rubidium Oxide  Strontium Bromide  Aluminum Oxide

7.  If cation has multiple charges, use a roman numeral to indicate charge  Cu + =Copper ( I ) Cu +2 =Copper ( II )  I = 1II = 2 III = 3 IV = 4  V = 5 VI= 6 VII = 7 VIII = 8  IX = 9 X = 10

8.  The charge on ionic compounds has to be electrically neutral  Figure out overall charge on anion and then determine what charge cation has to be  CuCl 2 ~Each Cl has a charge of -1 (needs 1 e-) and since there are 2 of them, the overall charge of Cl is -2. Cu must be +2 = Copper ( II ) chloride

9.  PbO 2 Charge on O is -2 and there are 2 of them so overall on O is -4.  Pb has to be +4  Lead ( IV ) oxide

10.  CuO  Hg 2 O  Cu 2 O  Vanadium ( III ) Iodide  Platinum ( IV ) oxide

11.  Polyatomic Ion – an ion made of 2 or more atoms that behave like a single ion  Bonded covalently  Bond ionically with other simple ions as salts

12.  Name the ion that is not a polyatomic like simple cations or anions and then name the polyatomic as the chart says  NaOH = Sodium hydroxide  CaCO 3 = Calcium carbonate

13.  AlPO 3  LiSCN  FeSO 4  Mn(Cr 2 O 7 ) 2

14.  Determine charge of overall polyatomic and then the other ion.  Follow same rules as before.  Beryllium cyanide  Copper ( II ) nitrate

15.  Barium sulfide  Potassium oxalate  Chromium (III) cyanide  Vanadium (V)silicate

16.  Name changes as number of O changes  Gain 1 O = per chlor ate ClO 4 -  Base Name = chlorate ClO 3 -  Lose 1 O = chlor ite ClO 2 -  Lose 2 O = hypo chlor ite ClO -

17.  The name usually starts with the word hydrogen, but use mono- and di-  HPO 4 –monohydrogen phosphate  H 2 PO 4 – dihydrogen phosphate  Thio – replace O with S  K 2 S 2 O 3 – Potassium thiosulfate

18.  Inorganic molecular compounds  Specify # of each type of atom  P 4 O 6 – Tetraphosphorus hexoxide  P 4 O 10 – Tetraphosphorus decoxide

19. Mono1Di2 Tri3 Tetra4 Penta5 Hexa6 Hepta7 Octa8 Nona9 Deca10

20.  If there is 1 of the first element, mono is omitted from the word  CO – carbon monoxide  CO 2 – carbon dioxide

21.  1 st element – named 1 st – usually least e-neg  2 nd element – named 2 nd – usually most e-neg – add ide ending  Drop vowels o and a from prefix before adding it to a root that starts with a vowel

22.  N 2 O 4 – Dinitrogen tetroxide  SF 6 – Sulfur hexafluoride  Some common names are used instead of technical name  H 2 O – water – not dihydrogen monoxide