2.  What does IUPAC stand for?  International Union of Pure and Applied Chemistry  Developed standards for the naming of the chemical elements and their compounds  Name new elements

3.  When two elements chemically combine, a compound results.  In an ionic bond, a metal and a non-metal bond by transferring electrons.  In a covalent bond, two non-metals bond by sharing electrons.  Cation – Positive Ion (usually metals)  Anion – Negative Ion (always nonmetals)

4.  What are compounds?  2+ elements chemically combined  Give me an example or two…  Salt – Sodium Chloride – NaCl  What type of bond is present in NaCl?  Ionic  Predict the chemical formula of  Potassium Chloride -------- KCl  Calcium Chloride ----------CaCl 2

5.  Basically – the charge an element takes on when it stabilizes into a noble gas electron configuration  Example: Sodium 1s 2 2s 2 2p 6 3s 1  Will lose 1 e - to become like Neon: 1s 2 2s 2 2p 6  Will gain 7 e - to become like Ar: 1s 2 2s 2 2p 6 3s 2 3p 6  Elements will take the easiest path – losing 1e in this case  Na + will become a cation with an oxidation number of +1 due to the loss of 1 e -

6.  What will the oxidation number of calcium be?  Electrons: Easier to lose 2 or gain 6?  Will lose 2 to become a cation Ca 2+  What will the oxidation number of Fluorine be?  Electrons: Easier to lose 7 or gain 1?  Will gain 1 to become an anion F -

7.  Predict the oxidation number of:  Cl-1  Na+1  Mg+2  Al+3  S-2  N-3

8.  Oxidation Numbers are easy to predict with the periodic table!  Group 1 = +1  Group 2 = +2  Group 13 = +3  Group 15 = -3  Group 16 = -2  Group 17 = -1  Group 18 = 0  Transition Metals cannot be predicted due to orbital overlap!

9.  To name a Binary Compound from a formula:  Identify and name the metal (the cation)  Identify the nonmetal, write it’s name after the name of the metal, and change the ending to -ide  Examples:  MgF 2 ▪ Magnesium Fluoride  Li 2 O ▪ Lithium Oxide

10.  NaClSodium Chloride  CaI 2 Calcium Iodide  AlCl 3 Aluminum Chloride  MgSMagnesium Sulfide  Na 3 N 2 Sodium Nitride

11.  LiBrLithium Bromide  KIPotassium Iodide  AlF 3 Aluminum Fluoride  Al 2 O 3 Aluminum Oxide  K 2 OPotassium Oxide

12.  We have been naming formulas…  Now let’s make formulas from names!  Steps  Consider oxidation numbers – they must cancel  If a Mg 2+ bonds with a Cl -, How many Cl - will be needed to cancel the Mg 2+ ? ▪ It will take two Cl - to cancel the one Mg 2+  Change the subscript to change quantity  Mg 2 + Cl - = MgCl 2

13.  Lithium ChlorideLiCl  Beryllium FluorideBeF 2  Magnesium BromideMgBr 2  Cesium OxideCs 2 O  Strontium SulfideSrS

14.  Calcium PhosphideCa 3 P 2  Aluminum Iodide AlI 3  Aluminum SulfideAl 2 S 3  Lithium NitrideLi 3 N  Potassium SulfideK 2 S

16.  Oxidation Numbers cannot be predicted (because of orbital overlap)  Oxidation Number must be stated with Roman Numerals in the written name of the compound (two exceptions – next slide)  Iron (III) Oxide  Fe 3+ and O 2-

17.  Exceptions to Roman Numerals  Always Zn 2+  Always Ag +

18.  Iron (II) Oxide  Lead (II) Chloride  Chromium (V) Oxide  CdS V2O5V2O5

19.  Some ionic compound partly consist of polyatomic ions  The prefix poly- means multiple, so polyatomic means multiple atoms  ClO 3 - is an example of a polyatomic ion  In naming, treat polyatomic ions as a single element, not as two separate ones

20.  CaSO 4  NaOH  Pb 2 PO 4  Magnesium Chlorate  Potassium Permanganate  Nickel (II) Iodate

21.  Covalent = NONMETALS  Like binary ionic compounds, except covalent compounds use special prefixes

22.  mono-1  di-2  tri-3  tetra-4  penta-5  hexa-6  hepta-7  octa-8  nona-9  deca-10

23.  CO 2 N2S3N2S3  nitrogen tribromide  diphosphorus pentoxide