1. Covalent compounds Sharing of electrons

2. Chemical Bonds Ionic Bond – Transfer of electron – Exist in a crystal lattice form Covalent Bond – Pairs of electrons are shared – 1 bond = 2 electrons – Called a molecule – Still trying to satisfy the octet rule (several exceptions)

3. Diatomics – why do they always come in two in their elemental form? Flourine One covalent bond: F-F

4. Oxygen

5. Nitrogen

6. Naming covalent compounds The first element is named first – entire element name Second element in the formula is named using the root of the word and the ending –ide. Prefixes are used to indicate the number of atoms of each type that are present in the compound Exception – the first element never uses mono-

7. Naming Covalents (cont’d) 1 – mono 2 – di 3 – tri 4 – tetra 5 - penta 6 – hexa 7 – hepta 8 – octa 9 – nona 10 – deca

8. Examples H 2 O – Dihydrogen monoxide NH 3 – Nitrogen trihydride N 2 O – Dinitrogen monoxide

9. You try…. CCl 4 As 2 O 3 CO P 2 O 5