Chapter 9 Chemical Names and Formulas 9.1 Naming Ions 9.2 Naming and Writing Formulas for Ionic Compounds 9.3 Naming and Writing Formulas for Molecular Compounds 9.4 Naming and Writing Formulas for Acids and Bases 9.5 The Laws Governing How Compounds Form Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Monatomic Ions After Quiz: 1. Determine the charge of the cations in the following ionic compounds. a) FeO b) Fe2O3 c) Cu2O d) CuO 2. Give a name to each compound above. 3. Read 9.1 in your online textbook Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Do Now: a) FeO Fe2+ Iron (II) Oxide Ferrous Oxide Monatomic Ions Do Now: a) FeO Fe2+ Iron (II) Oxide Ferrous Oxide b) Fe2O3 Fe3+ Iron (III) Oxide Ferric Oxide c) Cu2O Cu+ Copper (I) Oxide Cuprous Oxide d) CuO Cu2+ Copper (II) Oxide Cupric Oxide Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Naming Metals That Form More Than One Ion Monatomic Ions Naming Metals That Form More Than One Ion Many transition metals and Group 4A metals can form more than one type of cation Roman numeral in parentheses indicates charge. Examples: Copper (I) is Cu+ Copper (II) is Cu+2 Iron (II) is Fe+2 Iron(III) is Fe+3 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Cadmium – only forms Cd2+ Zinc – only forms Zn2+ Monatomic Ions Exceptions Transition metals that only form one ion do not have a Roman numeral in their name. Silver – only forms Ag+ Cadmium – only forms Cd2+ Zinc – only forms Zn2+ Group 4A elements that form multiple ions Tin – forms Sn2+ and Sn4+ Lead – forms Pb2+ and Pb4+ Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Binary Ionic Compounds Write formulas for the following: a) Manganese (II) Fluoride b) Lead (II) Sulfide c) Cobalt (III) Chloride d) Tin (IV) Bromide Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Binary Ionic Compounds Write formulas for the following: a) Manganese (II) Fluoride MnF2 b) Lead (II) Sulfide PbS c) Cobalt (III) Chloride CoCl3 d) Tin (IV) Bromide SnBr4 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Binary Ionic Compounds Writing Formulas for Binary Ionic Compounds Write symbols of elements. Determine ionic charge for each symbol. If the sum of the charges is zero, you are done. If the sum of the charges does not equal zero, use the criss-cross method to add subscripts to balance the charges. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Binary Ionic Compounds Write names for the following: a) Co3N2 b) Co2O3 c) Ti2S d) CrF2 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Binary Ionic Compounds Write names for the following: a) Co3N2 Cobalt (II) Nitride b) Co2O3 Cobalt (III) Oxide c) Ti2S Titanium (I) Sulfide d) CrF2 Chromium(II) Fluoride Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

Binary Ionic Compounds Naming Binary Ionic Compounds Identify the two elements and name the cation and anion (anion ending must be –ide). Does the cation have more than one possible charge? If no, write the compounds name. If yes, go to #3. When the cation has more than one possible charge, a roman numeral is needed • If subscripts present, do reverse criss-cross to determine cation charge • If no subscripts, verify that anion charge and cation charge are exact opposites. Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.

END OF 9.1 Copyright © Pearson Education, Inc., or its affiliates. All Rights Reserved.