After today, you will be able to… Write structural formulas and dot formulas for covalently bonded molecules Identify shared and unshared electrons Explain the difference between single, double, and triple bonds - and write them using structural formulas/dot formulas

Unit: Chemical Bonding Day 3 - Notes Unit: Chemical Bonding Covalent Bonding Basics

Covalent Bonding A sharing of electrons. A single covalent bond is made up of two electrons One electron is donated to the bond from each atom Covalent bonding occurs between nonmetals only Atoms that are covalently bonded are called molecules or molecular compounds.

Properties of Molecular Compounds Covalent bonds are much weaker than ionic bonds Much lower melting and boiling points Is a solid, liquid, or gas at room temperature Non-conductors in any state

Properties of Molecular Compounds The chemical formula for a covalently bonded group of atoms is called a molecular formula. Indicates the exact makeup of one molecule. Example: C6H12O6

1 4 5 6 7 1 4 3 2 1 1 4 3 2 1 H Group 14 Group 15 Group 16 Group 17 # of valence electrons # of electrons short # of bonds made 1 4 5 6 7 1 4 3 2 1 1 4 3 2 1

Example: Write the dot and structural formula for: H2 Rough Copy (Work): Dot Formula: Lewis Structural Formula: H H Single bond: A shared pair of two electrons.

Example: Write the dot and structural formula for: O2 Rough Copy (Work): Dot Formula: Lewis Structural Formula: O O Unshared pair of electrons Double bond: Two shared pairs of four electrons.

Example: Write the dot and structural formula for: N2 Rough Copy (Work): Dot Formula: Lewis Structural Formula: N N Triple bond: Three shared pairs of six electrons.

Example: Write the dot and structural formula for: H2O Rough Copy (Work): Helpful tip: Put the atom in the middle that wants to make the most bonds! H Dot Formula: Lewis Structural Formula: O H O H

Example: Write the dot and structural formula for: ONF Rough Copy (Work): Dot Formula: Lewis Structural Formula: O N F O N F