1. Chapter 6 – Chemical Names & Formulas
6.1 Introduction to Chemical Bonding
6.2 Representing Chemical
Compounds
6.3 Ionic Charges
6.4 Ionic Compounds
6.5 Molecular Compounds & Acids
6.6 Summary of Naming and Formula
Writing

2. 6.1 Introduction to Chemical Bonding
Molecules and Molecular Compounds
Molecule: the smallest electrically neutral part of a substance that has all of the same properties of that substance.
Molecules can be a variety of combinations of elements that may combine chemically to form molecular compounds.
As a general rule, molecules are usually two or more non-metallic elements joined together.
e.g., CO2 , C2H6O, SO3….

3. 6.1 Introduction to Chemical Bonding (cont.)
Ions and Ionic Compounds
Not all compounds are molecular, many are ionic.
Ions are atoms or groups of atoms that are electrically charged.
Ionic compounds are generally formed beginning with a metal and a non-metal.

4. 6.1 Introduction to Chemical Bonding (cont.)
Ions and Ionic Compounds (cont.)
Ions can be either positive (cations) or negative (anions)
As a general rule, anions form from non-metals and cations form from metals.
Ion names have different prefixes and endings, depending on how they are formed.
BUT, simply use the periodic table and ion charts for location and ion names.
Finally, be able to compare and contrast similarities and differences between molecular and ionic compounds: Table 6.1 lists a few.

5. 6.2 Representing Chemical Compounds
Chemical Formulas
What do they tell us?
“The kind and number of atoms in the smallest representative unit of the substance.”
Can be either a molecular formula (for molecules) or a formula unit (for ionic compounds)

6. 6.2 Representing Chemical Compounds (cont.)
Laws of Definite and Multiple Proportions
In the simplest terms, masses of elements are always in the same proportions when combining into compounds and in ratios of small whole numbers (Dalton).
H20 not H1.7O.85

7. 6.3 Ionic Charges Monatomic Ions Polyatomic Ions
Ions that consist of only 1 atom.
e.g. chloride – Cl-, hydrogen – H+, iodide – I-
Polyatomic Ions
Ions that are tightly bound groups consisting of two or more atoms, behave as a unit, and carry a charge.
e.g. acetate – C2H3O2-, ammonium – NH4+
Use periodic table & Tables 6.2, 6.3, & 6.4

8. Chapter 6 Assignment
CPQs # 1 pg # 45-49, 51-54

9. 6.4 Ionic Compounds Writing Formulas and Names for Ionic Compounds
Binary: compounds composed of two element ions.
e.g. BaCl2, NaCl, HCl, Fe2O3
Some rules to consider:
Cations get written first
Net charge on compound must be zero
Criss-cross! Shoelace?
Naming Ionic Compounds
Work things in reverse!
- Ternary Ionic Compounds
Same as before except you are using polyatomic anions!
e.g. Ca(NO3)2, Li2CO3, Mg(OH)2
DO NOT ATTEMPT TO SPLIT UP POLYATOMIC ANIONS!

10. 6.5 Molecular Compounds & Acids
Easy to recognize: two non-metals!
Ending and prefixes are important here…
Table 6.5
e.g. N2O, CO2, SF6
Naming Common Acids
Memorize the list on page 160!

11. Chapter 6 Assignment CPQs # 1 pg. 166 # 45-49, 51-54
CPQ’s #2 pp
#57,58,61,62,64,66