COVALENT BONDING
FORMULAS & NAMES
(INCLUDING ACIDS)
Chem-To-Go
Lesson 16
Unit 4
WHAT IS A COVALENT BOND?
Covalent Bond = a nonmetal atom
shares valence electrons with another
nonmetal atom; both atoms achieve
stability
We’ll learn to:
1. Name covalent
compounds
2. Write formulas for
covalent compounds
3. Draw Lewis
structures
4. Analyze Lewis
structures to predict
properties
IMPORTANT PREFIXES
1)Mono
2)Di
3)Tri
4)Tetra
5)Penta
6)Hexa
7)Hepta
8)Octa
9)Nona
10)Deca
WRITING FORMULAS
Use the prefixes to determine subscripts for
each element.
NO IONS, THEREFORE NO CRISS-CROSSING!
EXAMPLE 1:
phosphorus trioxide
EXAMPLE 2:
dinitrogen trioxide
EXAMPLE 3:
tricarbon octahydride
WRITING NAMES
Use the prefixes to determine subscripts for
each element.
NO IONS, THEREFORE NO CRISS-CROSSING!
EXAMPLE 1: N2O5
EXAMPLE 2: CF4
EXAMPLE 3: P2O6
SPECIAL T YPE OF COVALENT COMPOUND:
ACIDS
Acid = compound that produces H+
ions when dissolved in water
How to Recognize Acids:
Find H at the front of the
chemical formula.
Examples of Acids:
• H2SO4
• HCl
• HNO3
• HBr
TWO TYPES OF ACIDS
Binary Acids
Oxyacids
 Contain H bonded to
ONE other element
 Contain H bonded to a
POLYATOMIC ION
 Writing Names
 Writing Names
 Hydro + root + ic acid
 Ex. HCl = hydrochloric acid
 Ex. H 2 S = hydrosulfuric acid
 Ex. HI = hydroiodic acid
 IF –ATE ion: root + ic acid
 Ex. HNO 3 = nitric acid
 Ex. H 2 SO 4 = sulfuric acid
 IF –ITE ion: root + ous acid
 Ex. HNO 2 = nitrous acid
 Ex. H 2 SO 3 = sulfurous acid
FORMULAS OF ACIDS
Binary Acids
Oxyacids
Criss-cross the ion
charges as if the
compound was ionic
Example: hydronitric acid
“Yes hydro, No polyatomic”
Example: chlorous acid
“No hydro, Yes polyatomic”