1. Naming Binary Compounds Goals Explain why an ionic compound is represented by an empirical formula. Be able to determine the charges of monatomic ions formed by the representative elements from the position of each element on the periodic table. Use the Stock system to identify the charge of transition metal ions. Name an ionic compound given its formula. Write the correct formula for an ionic compound given its name.

2.  How many compounds are currently known?  With 4 million known compounds, is it convenient to have to memorize their names?  We have rules for naming compounds so that they can all be named generically. By naming them all at once, we don’t have to memorize the names of any!

3.  Binary Compounds are compounds composed of only two elements…  There are 4 types of Binary Compounds: 1. Binary Ionic Compounds (Type I) 2. Binary Ionic Compounds (Type II) 3. Binary Covalent Compounds 4. Acids (to be discussed later)

4.  Binary Ionic Compounds are made of a cation and an anion joined together in an ionic bond. They are held together by magnetic attraction. When a metal combines with a nonmetal, the resultant compound is always a binary ionic compound.  The cation can be a main group metal, a transition metal, or a polyatomic ion.  The anion can be a main group nonmetal, or a polyatomic ion. There are two types, which are distinguished by the type of cation.

5.  Type I Binary Ionic Compounds are made of a metal that forms only one cation, and an anion.  The cation is named first. Metal cations are named using their atomic names.  In general, groups 1, 2, and 3 form only one cation.  The anion is named second. Remember to drop the ending of the anion’s atomic name and add the suffix –ide.

6.  NaCl  BaO  CaS  KI  CsBr  SrCl 2  Li 2 Se  Mg 3 P 2  Sodium Chloride  Barium Oxide  Calcium Sulfide  Potassium Iodide  Cesium Bromide  Strontium Chloride  Lithium Selenide  Magnesium Phosphide

7.  Type II binary ionic compounds are made up of a metal that forms more than one cation (transition and rare earth), and an anion.  The cation is named first. Metal cations are named using their atomic names.  The charge of the cation is indicated in roman numerals in parenthesis. This is necessary because these metals form more than one cation, and we need to know which one it is.  The anion is named last. Remember to drop the ending of the anion’s atomic name and add the suffix –ide.

8.  FeCl 2  CuBr  HgO  Fe 2 O 3  MnO 2  PbCl 4  FeBr 3  Co 3 P 2  Iron (II) Chloride  Copper (I) Bromide  Mercury (II) Oxide  Iron (III) Oxide  Manganese (IV) Oxide  Lead (IV) Chloride  Iron (III) Bromide  Cobalt (II) Phosphide

9. Type III Get through Part I notes Exit quiz today on BCC HW: Pg 132 # 21, 22, 23, 34 due Tues

10.  Binary Covalent Compounds are made up of two different nonmetals.  There are no ions present in the compound.  Atoms are bonded covalently, by sharing electrons.  Binary Covalent Compounds are named using a system of numeric prefixes.

11.  1 – mono-  2 – di-  3 – tri-  4 – tetra-  5 – penta-  6 – hexa-  7 – hepta-  8 – octa-  9 – nona-  10 – deca-

12.  The first element is named first. The elements atomic name is used.  The second element is named second. This element is named as if it were an anion. Remember to drop the ending of the anion’s atomic name and add the suffix –ide.  The number of each atom present in the compound is represented by a numeric prefix. (mono, di, tri, …)  The prefix mono is NOT used in naming the first element in the compound.

13.  BF 3  NO  NO 2 N2ON2O N2O5N2O5  CCl 4  SO 2  IF 5  Boron Trifluoride  Nitrogen Monoxide  Nitrogen Dioxide  Dinitrogen Monoxide  Dinitrogen Pentoxide  Carbon Tetrachloride  Sulfur Dioxide  Iodine Pentafluoride

14. Binary Compound? Yes Metal Present? No Yes BCC – Use Prefixes Does the metal form more than one cation? NoYes BIC – Type II, Use Roman Numerals BIC – Type I, No Roman Numerals

15.  CuO  SrO B2O3B2O3  TiCl 4 K2SK2S  OF 2  NH 3  Copper (II) Oxide  Strontium Oxide  Diboron Trioxide  Titanium (IV) Chloride  Potassium Sulfide  Oxygen Difluoride  Nitrogen Trihydride  Ammonia

16.  ClF 3  VF 5  CuCl  MnO 2  MgO H2OH2O  Chlorine Trifluoride  Vanadium (V) Fluoride  Cupper (I) Chloride  Manganese (IV) Oxide  Magnesium Monoxide  Dihydrogen Monoxide  Water