1. Write the FULL electron configurations for the following: Fluorine Boron Chlorine In your information, include the number of PROTONS, TOTAL ELECTRONS, VALENCE ELECTRONS and WHAT ROW IT’S IN. Finally, predict which atom is larger, FLUORINE OR CHLORINE. Explain why you think so.

2. Chapter 6.3

3.  Atomic Size/Atomic Radius  Ionic Size  Ionization Energy  Electronegativity

4. 1. Octet Rule  gotta have 8 valence electrons 2. # of Rows of e- (if same column)  More rows of e- = more repulsion of e- outward (likes repel) 3. # of Protons (if same row)  More protons = more attraction of e- inward (opposites attract)

5. Atomic Radius – distance from nucleus to end of electron cloud ◦ LARGEST: BOTTOM LEFT CORNER

6. Left to right: DECREASES  More protons = more attraction inward toward nucleus (smaller atoms) Going down: INCREASES  More rows of electrons = more repulsion outward (larger atoms)

7.  Electronegativity – ability of atom to ATTRACT valence electrons ◦ LARGEST: TOP RIGHT CORNER (except Noble Gases)

8. Left to Right: INCREASES  Elements toward right CLOSE to satisfying octet rule, so want electrons more.  Noble gases = none (octet rule satisfied) Going Down: DECREASES  More rows of electrons = more repulsion outward, so less desire to bring in more e-.

9.  Ionization Energy – amount of energy required to LOSE a valence electron. ◦ LARGEST: TOP RIGHT CORNER

10. Left to Right: INCREASES  Closer to satisfying Octet Rule Going Down: DECREASES  More rows = more repulsion outward (easier to lose electrons)

11.  Goal: 8 valence electrons (octet rule) Ion – an atom with a charge (in order to satisfy octet rule)  Cation = POSITIVE charge  Anion = NEGATIVE charge

12.  Boron vs. Nitrogen  Boron ion = +3 (loses 3 e-)  Cation  Nitrogen ion = -3 (gains 3 e-)  Anion  Boron…LOSES an energy level (SMALLER than neutral Boron)  Nitrogen…GAINS e- (LARGER than neutral Boron)

13.  Cations = smaller than neutral atom (Left of Carbon) ◦ Lose energy level  Anions = larger than neutral atom (Right of Carbon) ◦ Gain electrons, less attraction  Carbon…goes both ways. Yeah, it’s like that.

15. B – Basicity E – Electronegativity ionization Energy A – Acidity R – atomic Radius

16.  Compare the ionic radii of neutrally charged oxygen, and oxygen with a negative 2 charge. Which radius is larger, and why? ◦ Draw rings for O and O -2  Fluorine has a high ionization energy AND electronegativity. Why do the noble gasses have a high ionization energy, but virtually no electronegativity?  Why do the atoms in the bottom LEFT corner have a larger atomic radius than elements in the bottom RIGHT corner?