Covalent Bonds Unit 6 – Part II

Review… Ionic Compounds… –Metals and non-metals –Achieve stable octet by gaining or losing e- –Positive and negative ions are attracted to each other Form lattices 2/5/2016Free template from

2/5/2016Free template from Covalent Bonds –A bond formed by sharing a pair of electrons between two atoms –atoms will achieve a stable octet by sharing e- –Nonmetals to nonmetals or metalloids to nonmetals –Form molecules or polyatomic ions

2/5/2016Free template from Covalent Bonds Simplest example: H 2  hydrogen gas Attractive forces between e - and p + hold it together

2/5/2016Free template from Covalent Bonds Lewis structures are commonly used to demonstrate covalent bonding. –Visual representation of valence e- Draw dot structures for H, N, O, Cl HNOCl

2/5/2016Free template from Covalent Bonds Rules –Every atom must have 8 e - around it 2 e - for H –Must use correct total # of e -

2/5/2016Free template from Covalent Bonds Examples: 1. H 2HHH Each H has e - config of He Shared pair of e - Structural formula – shows pairs of e - as dashes

2/5/2016Free template from Covalent Bonds 2. Cl 2ClClCl Each Cl has 8 valence e -

2/5/2016Free template from Covalent Bonds 2. ClF ClF

2/5/2016Free template from Covalent Bonds 2. H 2 S S H H H

2/5/2016Free template from Covalent Bonds 2. PH 3 H P H H H

2/5/2016Free template from Covalent Bonds 3. O 2OO O =O Double bond – 2 shared pairs of e - Stronger than single More stable (harder to break)

2/5/2016Free template from Covalent Bonds 3. CO 2 OCOOCO OCOOCO O = C = O

2/5/2016Free template from Covalent Bonds 4. N 2NNN Triple bond – 3 shared pairs of e - Stronger than double Even more stable (harder to break)