 Guiding Question:  How does the type of bond relate to the properties of materials?

 Ionic  Polar Covalent  Non-polar Covalent  Metallic  Network Covalent  You will need to recognize which is which by looking at the formula.  You will need to know the properties of the five types including: ◦ appearance/texture ◦ melting point ◦ Conductivity ◦ solubility.

 Put “bond types and properties” in the middle  Put the five types of bonds around the outside

 You need to look at the formula to see if the compound contains metals or non- metals or both.

 Contain at least one metal and one non- metal.  May contain a polyatomic ion.  Examples: ◦ CuO ◦ Na 3 P ◦ CaCO 3 METAL NON-METAL

 Ionic compounds are also called SALTS.  Most are white crystals.  They are hard and brittle solids.

 Include how to recognize ionic compounds from the formula  Include appearance and textures.

 First let’s remember how to decide if it’s covalent or not.  Then use the Lewis structure to know if it’s polar or non-polar.

 Contain ONLY non- metals.  Examples: ◦ CH 4 ◦ H 2 O ◦ NH 3 ALL NON-METALS

 Polar molecules are ASSYMETRICAL – not balanced.  Use Lewis Structure: ◦ Unshared pairs make it assymetrical (pyramid or bent) ◦ Different atoms around the central atom also make it assymetrical. H 2 O is a bent molecule so it is Assymetrical and POLAR CH 3 Cl is polar

 Non-Polar molecules are SYMETRICAL – balanced.  Use Lewis Structure: ◦ No unshared pairs ◦ Same atoms surround the central atom. CO 2 is a linear molecule so it is Symetrical and NON- POLAR

 Soft solids, liquids, or gases at room temp.

 Include how to recognize covalent compounds from the formula  Include appearance and textures.

 Formula will contain one metal.  Example: ◦ Cu ◦ Fe ◦ Ag ◦ Al

In ionic bonding we know metals lose electrons to form positive ions M+ M is any metal M 2+ or This is to achieve a completely full outer electron shell This also happens in metallic bonding - but because there are no non-metals to take the electrons, now the electrons have nowhere to go! e-e- e-e- e-e- e-e- The valence electrons get passed from one atom to the next like a “hot potato”! This forms a “sea of negative charge” that flows around the positive metal ions.

M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ M+M+ Sea of electronsValence electrons move around holding the + metal ions in place How might this structure lead to some of the properties we know about metals?

 Shiny and malleable (bendable)

 Include how to recognize metallic compounds from the formula  Include appearance and textures.

 You need to remember: DIAMOND and SAND are network covalent solids.  Diamond will be written: C – Diamond ◦ Sand is SiO 2

In some substances, millions of atoms join together by covalent bonding. This produces giant covalent structures, not molecules. Each atom is linked to every other atom in the structure which makes them VERY strong. This also means that almost all giant covalent structure are hard and NOT brittle (don’t crack easily).

Diamond is a rare form of carbon in which each atom is covalently bonded to four others. This pattern arrangement is repeated millions of times to create a giant lattice. C C C C C This makes diamond VERY hard and strong.

Diamond coated drill bit!

 Include how to recognize network covalent molecules  Include appearance and textures.