2.  Molecules – a neutral group of atoms held together by covalent bonds  Molecular compound – a cmpd whose simplest units are molecules  Chemical formula – indicates relative # of atoms of each kind in a chemical compound by using atomic symbols & subscripts

3.  Molecular formula – shows types & # of atoms combined in a single molecule of a molecular compound  Diatomic molecule – a molecule with only 2 atoms.

4.  Bond will form when potential energy will be at lowest.  Nature favors situations when E can be reduced

6.  Bond length – the average distance b/t 2 bonded atoms at their lowest potential energy  Bond energy – the E required to break a chemical bond and form neutral isolated atoms

7.  Atoms want 8 e- in their valence shell  There are exceptions like H, He, and B

8.  EDN – an e-config notation in which only the valence e-are shown as dots around an elements symbol  What is the dot notation for F, Na, Al, Kr

9.  L-S – atomic symbol is nuclei and inner shell e-’s and dot pairs and dashes b/t atoms represent e-pairs in covalent bonds or unshared pairs  Structural formula – indicates kind, #, & arrangement of bonds but not the unshared pairs of e-’s

10. 1. H and halogens often bind to 1 other atom and are usually on the outside or end of a molec. 2. Atom with lowest e-neg is often central. They have less than 7 e- and can form more than 1 bond.

11. 3. When placing valence e-, put 1 e- on each side b4 pairing e-

12.  Single Bond – covalent bond where 1 pair of e-’s are shared b/t 2 atoms  Draw the Lewis structure for … H 2 HFNaCl CH 4 CH 3 I

13. 1. Draw the LS for each element 2. Put least electronegative element in center 3. Arrange other elements around central atom to satisfy octet (H only needs 2) 4. Change dots to lines to show bonds b/t atoms

14. 5. For unpaired electrons, try to form multiple bonds. 6. If octets are still not satisfied, try to move electrons around molecule.

15.  Double bond– 2 pairs of e-’s(4e-)  Triple Bond – 3 pairs of e-’s (6e-)  What is the Lewis structure for … O 2 N 2 CO 2 CH 2 OC 2 HCl

16.  R.S. bonding in molecule or ions that can’t be represented by a single Lewis Structure  O 3  Delocalized – e- shared b/t more than 2 atoms

17.  Complete the Lewis Structures for the following…  NH 4 + OH -  CN - NO 2 _