Ch.3 - Chemical ReactionsWorksheetSee all chapters
All Chapters
Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds

A covalent or molecular compound is composed of more than one nonmetal together. 

Naming Molecular Compounds

Concept #1: Rules for Naming Molecular Compounds

Transcript

Just so that you realize, when we say molecular compounds, another name for them are covalent compounds. Remember that covalent compounds are the connections between nonmetals. The features here are nonmetal and nonmetal together.
Because these nonmetals can arrange themselves in different proportions, we have to use a numerical prefix system in order to describe the numbers of each nonmetal combined in that covalent compound. These are the same numerical prefixes we had to use when we talked about the hydrides.
The rules we're going to say for our nonmetal connected to nonmetal is the first nonmetal is named normally, so we don't change its ending to -ide or anything like that. It's named normally. We're going to say it uses all of the numerical prefixes except mono. We never use mono to describe the first nonmetal in our covalent compound.
We're going to say the second nonmetal keeps its base name and has its ending changed to -ide. The second nonmetal will also use any of the numerical prefixes, including mono. 

Example #1: Write the formula for each of the following compounds.

a)  Disulfur monobromide                                    b)  Iodine Tetrachloride

Practice: Give the systematic name for each of the following compounds:

a. CO            b. N2S4             c. IO5