How Can I Make Sense Out Of This? It’s Like Another Language!! CuCl2 N2O5 Naming Compounds How Can I Make Sense Out Of This? It’s Like Another Language!! This slideshow is intended for a high school chemistry class. The class would be comprised of mostly juniors, but would also include some sophomores and seniors. Chromium (III) sulfate Carbon tetrachloride

Background Octet Rule Ionic Compounds Covalent Compounds Cation and Anion held together by electrostatic force Cation (+) Anion (-) Also Called Salts Covalent Compounds Nonmetals sharing electrons

Charges of Commonly Formed Monatomic Ions +1 +2 +3 -3 -2 -1

Naming Ionic Compounds Name the cation first and the anion second. Typically left to right Monatomic cations Simply use the element name. Group 1a & 2a metals have only one oxidation #. Ex. Na+  Sodium Mg2+  Magnesium

Ionic Compounds Cont. Transition metals and metals on the right side of the periodic table often have more than one oxidation #. Use roman numerals after the element name to indicate the oxidation # Ex. Fe2+  iron (II) Fe3+  iron (III)

Ionic Compounds Cont. Monatomic anions Take their name from the root of the element name plus the suffix –ide. Ex. O2-  oxide N3-  nitride F-  fluoride If the compound contains a polyatomic ion, simply name the ion.

You must know names and formulas for polyatomic ions!!!

Dealing With Polyatomic Ions Most polyatomic anions, consist of a nonmetallic element combined with different numbers of oxygen atoms These polyatomic anions are called oxyanions The following suffixes are used with the root of element bound to the oxygens name -ate -ite One less oxygen

Polyatomic Ions Cont. When more than two oxyanions are formed by an element the following prefixes are used Hypo- One less oxygen than –ite Per- One more oxygen than -ate

Examples ClO3- ClO2- ClO- ClO4- Chlorate Chlorite Hypochlorite perchlorate

Let’s Put it All Together Na2S Sodium sulfide Pb(NO3)2 lead (II) nitrate NH4F Ammonium fluoride Fe3(PO3)2 Iron (II) phosphite

Naming Binary Molecular Compounds Prefixes are used to indicate the number of atoms of each type present in the compound. Mono- is not used on the first element. The first name in the formula is always named first Use the element name from the periodic table. The second element in the formula is named next use the root of the element and add the suffix –ide.

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

Let’s Try It CCl4 N2O5 H2O Carbon tetrachloride Dinitrogen pentoxide Dihydrogen monoxide Aka  water DHMO

Naming Acids Acids contain H 2 Types of Acids H typically written 1st in formula 2 Types of Acids Binary Acids Oxyacids Contain oxyanions

Naming Acids Cont. Binary Acids oxyacids Use the prefix hydro- Use the root of the second part of the acid and add the ending –ic End by adding the word acid Do not write hydro- Use the root of the oxyanion If the oxyanion ends in –ate replace it with –ic. If it ends in –ite replace it with –ous. End by adding the word acid

Let’s See What We Can Do HCl H2CO3 H2SO4 HI HC2H3O2 HF HClO H3PO3 Hydrochloric acid H2CO3 Carbonic acid H2SO4 Sulfuric acid HI Hydroiodic acid HC2H3O2 Acetic acid HF Hydrofluoric acid HClO Hypochlorous acid H3PO3 Phosphorous acid