1. Bonding and Nomenclature Unit About 3 weeks Will discuss the bonds that elements form and how to name the compounds formed There are many rules and procedures that simply must be memorized and practiced Therefore, there will be small amounts of homework regularly and several quizzes

2. Ionic BondingCovalent Bonding Transfer of Electrons (e-)Sharing Electrons (e-) Between (b/w) cations & anions B/w metals & nonmetals B/w two nonmetals Stronger than covalent bonding Weaker than Ionic bonding Soluble: ability to be dissolved Can be soluble or insoluble depending on polarity Therefore, higher melting point (mp), boiling point (bp) and hardness Therefore, lower melting point (mp), boiling point (bp) and hardness Sometimes referred to as a molecular compound (cmpd) Example: Na+Cl- NaCl Sodium Chloride Example: CO Carbon Monoxide Cmpds shown as a formula with chemical symbols and numbers Both follow Octet Rule: Cmpds form so that each atom has an octet of ve-. Can lose, gain or share to reach 8. Except H which is full with 2. Chemical bond: mutual electrical attraction between the nuclei and valance electrons of atoms which binds the atoms together.

3. Covalent Bonding Can be either polar or non-polar Polar: uneven distribution of charge caused by two different nonmetals bonding together. If there is a large enough difference, they can be soluble. Ex: C-O Nonpolar: An even distribution of charge caused by the same non-metal bonded to one another. These are insoluble. Ex: Cl-Cl

4. Homework tonight! Define the key terms: Chapter 6, Sections 1, 2, and 3 (page 208—21 words) Tomorrow we will be drawing compounds as Lewis Dot Diagrams. You do not need your book.