1. Molecular Compounds

2. A molecule forms when two or more non- metallic atoms bond together –It can be made up of atoms of different elements or of atoms of all the same element –Example: CH 3 OH (l) (methanol) and O 2(g) oxygen gas

3. Molecular Compounds Recall that the formula unit of an ionic compound represents a ratio of ions in a crystal lattice. In a solid ionic compound, this lattice extends in all directions. A formula unit is not an independent unit – it is just one part of a crystal lattice. Molecules are independent units made up of fixed numbers of atoms bonded together

4. Molecular Compounds Unlike ionic compounds, molecular substances can be solid, liquid or a gas at room temperature. They tend to be poor conductors of electricity They DO NOT dissolve in water very well

5. Molecular Compounds Example of common molecular compounds (you need to remember these) –C 12 H 22 O 11(s) sucrose –CH 3 CH 2 OH (l) ethanol –CH 3 COCH 3(l) acetone –CH 4(g) methane

6. Sharing Electrons – Covalent Bonds The atoms in a molecule are joined together by covalent bonds that form when atoms share electrons Each pair of shared electrons forms one covalent bond. Electrons are not transferred from one atom another as they are in ionic bonds

7. Sharing Electrons – Covalent Bonds Chlorine gas is an example of a substance that has molecules formed of only one element Each chlorine molecule in made up of two chlorine atoms joined by a covalent bond The chlorine atom has 7 valence electrons in its outer energy level –An additional electrons is needed A molecule of chlorine gas is created when two atoms of chlorine each share an electron tp form a covalent bond

8. Sharing Electrons – Covalent Bonds Notice that the electron is not transferred from one atom to another as it would be in an ionic bond. In covalent bonds, atoms share electrons so that their outer energy levels become filled Other example of covalent compounds include H 2 O (l), NH 3(g) (ammonia) and C 12 H 22 O 11(s) (sugar)

9. Sharing Electrons – Covalent Bonds In some covalent bonds, the atoms share more than 2 electrons. Example: Nitrogen gas, N 2(g). An atom of Nitrogen has 5 valence electrons To form N 2(g), two nitrogen atoms share 3 pairs of electrons

10. Molecular Elements Molecular Elements form molecules made up of only one type of atom MonatomicC (s) noble gases all metals DiatomicH 2(g) N 2(g) O 2(g) F 2(g) Cl 2(g) Br 2(g) I 2(g) PolyatomicO 3(g) (ozone) P 4(s) S 8(s) Remember These!

11. Molecular Compounds That Do Not Contain Hydrogen A binary compound with two elements Rules for naming binary molecular compounds not containing hydrogen are similar to the rules for naming ionic compounds. For molecules, Greek prefixes are used to indicate how many atoms of each element are present in the compound. Example: P 4 O 10(s) is called tetraphosphorous decaoxide: tetra means “4,” and “deca-” means “10.”

12. Prefixes used for naming Binary Molecular Compounds PrefixNumber Mono1 Di2 Tri3 Tetra4 Penta5 Hexa6 Hepta7 Octa8 Ennea (nona)9 deca10 These Prefixes need to be remembered!!!!!

13. Molecular Compounds That Do Not Contain Hydrogen Any compound that does not have a metal or an ammonium ion in its formula is molecular. The format for naming binary molecular compounds not containing hydrogen is: Prefix + first element followed by prefix + second element ending in “-ide”

14. Molecular Compounds That Do Not Contain Hydrogen Note that the prefix “mono-” is not used when the first element is only one atom When the prefix “mono-” is required before “oxide,” the last “o” in the prefix is usually dropped. Example: It is “monoxide,” not “monooxide,” Example: N 2 O (g), PBr 3(g)

15. Molecular Compounds That Do Not Contain Hydrogen Example: –CO(g) –SO2(g) –CS2(g) – dinitrogen trioxide – carbon tetrachloride – tetraphosphorus decaoxide