 Molecular covalent  Network covalent  Ionic  Metallic Let’s look at the table!

TypeStructureHardnessMelting/ boiling point Conductivity Molecular covalent Click Network covalent Click IonicClick MetallicClick

 Crystal lattice structure: alternating cations and anions held together by electrostatic attractions (+ attracted to -, just like a magnet!) Back to table

Ionic compounds are hard!! Make sure in your table, you also know what it means that an ionic compound is brittle and why! stics.htm Back to table

ionicProps.htm Back to table

Read the caption for the three pictures in the link below. _1/ionic.html Back to table

g/metallic.asp Back to table

Scroll down to “Strength and workability” and write information about hardness, malleability, and ductility s/metals.html#top Back to table

Scroll to slide 8!! roperties-of-compounds-ionic-covalent- and-metallic Back to table

Scroll to slide 8!! roperties-of-compounds-ionic-covalent- and-metallic Back to table

uc/network/g-molecular.htm Click on the link, and press “covalently bond C atoms” and “keep bonding” to see the structure. Back to table

uc/network/g-molecular.htm Read the first paragraph! Back to table

Scroll to slide 4!! y1011_92.pdf Back to table

Since there is a network of strong covalent bonding, network covalent solids are very hard. Back to table

Molecular covalent are all nonmetal atoms. You drew examples of these when we did lewis structures. The molecules are held together by intermolecular forces. Here is an example: Back to table

Since molecular covalent molecules are held together by IMFs which are MUCH weaker than bonds, molecular covalents are considered soft molecules. Back to table

Scroll a ways down to “electrical conductivity” s/molecular.html Back to table

2 nd paragraph!! s/molecular.html Back to table