1. Ionic Bonding

2. Ionic Bonding – What Is It? Ionic Bond – bond between METAL and NON-METAL How? Metal DONATES outside electrons to NON- METAL Outside electrons = valence electrons

3. On the Periodic Table Same column = same # of valence electrons  H, Li, Na… = 1 valence  B, Al, Ga… = 3 valence  EXCEPTION: He (2 val, should have 8) “dots” represent valence electrons Lewis Dot Structures VIII

4. Lewis Dot Structures Example: Nitrogen (N) Valence Electrons: 5 TREAT IT LIKE A SCHOOL DANCE Symbol in center One valence electron on each side N....

5. Time For the Romance… One More valence electron left… Pair with ONE of the valence electrons So finished product = N..... YES! I HAVE A DATE TO THE PROM! YEAH…YOU SUCK PAIRED ELECTRONS…

6. Quick Quiz #1 Write the Lewis Dot Structures for the Following: Hydrogen Aluminum Carbon Sulfur Bromine Krypton

7. Lewis Dot and Ionic Bonding Metal Donates to Non-Metal Metal: LOSES electron (positive charge) Non-Metal: GAINS electron (negative charge) Metals on LEFT side of table Non-Metals on RIGHT side Goal: Non-metal = 8 valence

8. Examples Na + Cl  NaCl Na = METAL (1 val.) Cl = NON-METAL (7 val.) 1 Na DONATES (+1) 1 Cl RECEIVES (-1) Na + S  Na 2 S Na = METAL (1 val.) S = NON-METAL (6 val.) 2 Na’s DONATE (+1 each) 1 S RECEIVES both (-2) S......

9. Charged Atoms Ions – atoms with a positive or negative charge Metals – LOSE electrons (positive charge) = cation Non-Metals – GAIN electrons (negative charge) = anion Cats are cute  POSITIVE Onions smell bad  Negative