1. Molecular Compounds
SNC2D

2. Covalent bonding
04/10/99
Thus far we have looked at when atoms bond due to the transfer of electrons
An ionic bond forms when an atom has a greater attraction for e–s than a second atom
However, if two atoms have approximately the same pull on electrons, they share the electrons (forming a “covalent” bond)
BUT HOW DO WE KNOW???

3. ELECTRONEGATIVITY F 4.0 Li 1.0
Some elements have a stronger hold on their electrons
While other don’t. F
4.0 Li
1.0

4. Molecular Compounds
Molecular compounds are formed only between non-metals.
Sometimes non-metals don’t borrow electrons from metals to fill their last shell; instead, they get together and share their electrons.

5. Molecular Compounds
Since they are sharing valence electrons, the bond formed between the atoms is called covalent. These compounds can be represented using Lewis dot diagrams: e.g.

6. **Review sticks for different elements**
Molecular Compounds
Or, more commonly, by Kekulé diagrams or stick diagrams, where each electron shared is represented by a line connecting the chemical symbols, e.g.:
**Review sticks for different elements**

7. Molecular Compounds
Example:

8. Multiple Bonds
The sharing of more than one electron is represented using more than one line, e.g.: There is a double bond between the carbon atoms.

9. Naming Molecular Compounds
The elements in the name are given prefixes corresponding to the subscripts (number of atoms) and the second element is given the suffix “-ide.” e.g. CO2 is carbon dioxide

10. The Prefixes 1 Mono-* 2 Di- 3 Tri- 4 Tetra- 5 Penta- 6 Hexa- 7 Hepta-
8 Octa
Mono is only used when the second element is oxygen*
Eg. CO  Carbon monoxide

11. Examples
Formula Name OF4 N2O Cl2O7 Name Formula iodine trichloride diphosphorus pentoxide sulphur hexaiodide
oxygen tetrafluoride
dinitrogen monoxide
dichlorine heptoxide
ICl3
P2O5
SI6

12. Non-Conventional Names
Some compounds are more commonly known by other names.
e.g. NH3
CH4
H2O
ammonia
methane
water

13. The 7 Diatomic Molecules
The elemental compounds like H2, Cl2, and O2. are called diatomic molecules and are called simply: name of element + “gas” e.g. H2 hydrogen gas Cl2 chlorine gas O2 oxygen gas N2 nitrogen gas F2 Fluorine gas Br2 Bromine (liquid) I2 Iodine (solid)
Exceptions