1. Molecular Compounds (a.k.a. Covalent Compounds)

2. Ionic Compounds Review
Ionic compounds are the combination of ions. E.g. Na+ + Cl-  NaCl.
This formula represents the Ratio of sodium ions and chloride ions not the exact number of them.
They are composed of a Metal and a Non-Metal and form a crystal structure (e.g. NaCl and CaCl2 which are both salts)

3. Molecular Compounds Consist of atoms covalently bonded together
The elements involved are all Non-Metals

4. Some examples
N2O  Nitrous Oxide= Gas used at the dentist to relax patients
NO2  Nitrogen Dioxide= poisonous toxin emitted from car exhaust

5. More Examples H2O  Water CO2  Carbon Dioxide= Gas
exhaled and created during
combustion reactions
CO  Carbon Monoxide= Lethal gas created during incomplete combustion

6. Recall
In ionic compounds, the non-metal rips away the electron(s) from the metal because the metals loosely hold their electrons
This creates a positive and negative ion which attract each other making them stick together (opposites attract)

7. Molecular Compounds
made up of a non-metal
and a non-metal.
also called Covalent Compounds

8. Molecular Compounds
Share electrons (e-) to form a stable arrangement.
Neg. e- are attracted to the Pos. nuclei of both atoms

9. Molecular Compounds F F F
Molecular compounds are formed when non metals share electrons to fill their outer electron orbit (shell). If we draw the Lewis Structure for Fluorine, We can see that it needs one more electron to become stable It wants to share one electron with another atom. If it bonds with another fluorine atom We draw the shared pair of electrons between the two atoms. F F F
Shared electron pair  both now have 8 electrons in outer orbit.

10. Molecular Compounds O H H H O
Many molecular compounds are predictable. How will Oxygen bond with Hydrogen to form a molecule. Draw the Lewis Structure of both Atoms. Oxygen wants to share two electrons and hydrogen wants to share one. Clearly we need another Hydrogen atom Putting the shared electrons between the atoms. The molecule is H2O O H H H O
**The Oxygen atom has 8 valence electrons (full) and the Hydrogen has 2 valence electrons (full)

12. Molecular Compounds Carbon Dioxide Carbon Monoxide C O O C C O
Not all molecular compounds are as predictable. How will Oxygen bond with Carbon? Draw the Lewis Structures of each atom. Carbon wants to share 4. Oxygen wants to share 2 If we add one more Oxygen, each oxygen can share two. However, if Oxygen will share two and donate one of its other electrons pairs, Oxygen can bond with just on Carbon atom. C O O C
Carbon Dioxide C O
Carbon Monoxide

13. Types of Bonds H O C O
Water – Single bond because One pair of electrons are shared
Carbon Monoxide – Triple Bond because three pairs of electrons are shared O C
Carbon Dioxide – Double bond because two pairs of electrons are shared

14. Molecular Compounds – Naming
So Oxygen can form CO or CO2
We need a more flexible naming system for covalent compounds to reflect the many different bonding possibilities.
To name a covalent compound,
Starting with the atom that is to the left in the periodic table, (or lower)
Write the name of the atoms with the prefix indicating the number of that atom in the compound.
Change the ending of the last atom to – ide.
The prefixes are,
Mono Di
Tri
Tetra
Penta
Hexa
Hepta
Note, the mono is omitted on the first atom.
CO Carbon Monoxide
CO2 Carbon Dioxide

15. Memorize me! Number Prefix 1 mono 6 Hexa 2 Di 7 hepta 3 tri 8 octa 4
Tetra 9
nona 5
penta 10
deca

16. Naming Example P4O10 Phosphorus - use prefix tetra (4)
Oxygen – change ending – Oxide
Oxide – use prefix deca (10)
= Tetraphosphorus Decaoxide

17. Molecular Compounds - Naming
Name the following compounds
CF4
Carbon tetrafluoride
H2O
Dihydrogen Monoxide
PF5
Phosphorus Pentafluoride
Write the chemical formula for,
Sulphur Dioxide
SO2
DiCarbon Tetrahydride
C2H4

18. Molecular Compounds – Diatomic Gases
Molecular compounds show an incredible variety in structure, physical and chemical properties. There are categories that further divide covalent compounds into categories with common properties.
Diatomic Gases – When two atoms of the same type form a covalent molecule, the result is often a colorless, odorless gas.
The Halogens, Oxygen, Nitrogen and Hydrogen form diatomic gases.
H2 is called Hydrogen Gas not Dihydrogen.

19. Writing Formulas left-most element goes 1st Carbon monoxide
Carbon (C)  no prefix therefore = C
- Monoxide – Mono = 1 therefore, 1 oxygen atom = O
= CO

20. Writing Formulas Nitrogen dioxide
Nitrogen (N)  no prefix therefore = N
- Dioxide – Di = 2 therefore, 2 oxygen atoms = O2
= NO2

21. Writing Formulas DiCarbon Tetrahydride
Dicarbon (C)  Di = 2 therefore = C2
- Tetrahydride (H)  Tetra = 4 therefore, 4 Hydrogen atoms = H4
= C2H4

22. Eg. N2 - Nitrogen Gas O2 - Oxygen Gas Air

23. Exceptions that need to be Memorized!
CH4 – Methane H2O2 – Hydrogen peroxide H2O – Water

24. These Too!
NH3 – Ammonia O3 – Ozone