1. Molecular Compounds and Nomenclature

2. Molecular Nomenclature
Most compounds that you find everyday are molecular compounds, not ionic.
e.g. Sugar (molecular) for example has similar physical properties as salt (ionic) but they are very different in reality.

3. Ionic compounds are made of ions which can conduct electricity.
Molecular compounds on the other hand are not made of ions. They do not lose or gain electrons, they share electrons.

4. • Ionic compounds can only bond to non metals in a limited way.
e.g. for every Ca2+ we can only bond 2 F to it.

5. • Molecular compounds can have various numbers of atoms bonded together to create various molecules.
e.g. NO, NO2, N2O2, etc.
• Due to this method of bonding there are thousands more molecular compounds than ionic.

6. Molecular Compounds are made of two or more Non-metals which share pairs of electrons to form bonds.
Each pair of shared electrons is called a Covalent Bond.

7. Naming molecular compounds
The prefixes are used to count the number of atoms in the molecule.
This is important as molecular compounds containing 2 elements can have different combinations of atoms…each have different properties.

8. # of atoms 1 2 3 4 5 6 7 8 9 10
Prefix
Mono Di
Tri
Tetra
Penta
Hexa
Hepta
Octa
Nona
Deca

9. Naming Binary Molecular Compounds: IUPAC
1. Write down the name of the first element.
2.If there is more than one atom of this element attach a Greek prefix.
3. Attach (ALWAYS) a Greek prefix (relating to the number of atoms) to the second elements name and add -ide.
Example:
CO = Carbon monoxide
CO2 = Carbon dioxide