2. Coulomb’s LawCoulomb’s Law  Addresses the force of attraction between the positive nucleus and negative electron  F = q e  q p q e = charge of electron r 2 q p = charge of nucleus  INVERSE relationship between attractive force and distance  Attractive force is DIRECTLY related to the charge on the electron and the charge in the nucleus

3. First Ionization Energy (IE)First Ionization Energy (IE)  If an electron is given enough energy (in the form of a photon) to overcome the effective nuclear charge holding the electron in the cloud, it can leave the atom completely.  Energy required to remove the outermost electron from an atom  Amount of energy needed to remove ONE electron from a neutral atom  Energy needed to remove electrons from ground state to gaseous state in an atom  Formation of positive ions ( cations )

4. Ionization Energy (cont.)Ionization Energy (cont.)  Formation of positive ions ( cations )  The larger the atom is, the easier its electrons are to remove.  Ionization energy and atomic radius are inversely proportional.

5. Ionization Energy TrendIonization Energy Trend Increases Decreases

6. ElementAtomic # IE (kJ/mol) Na11495.8 Mg12737.7 Al13577.6 S16999.6 Cl171251.1 Ar181520.5 K19418.8

7.  1 st ionization energy  Energy required to remove 1 st electron from atom  Taken from highest energy level  Easiest to remove  Energy increases as more electrons are removed Ionization Energy (cont.)Ionization Energy (cont.)

8. Can we have 2 nd, 3 rd, 4 th, etc. Ionization Energies?  Energy needed to remove additional electrons from an atom  Energy increases as more electrons are removed.  Removing electrons from lower energy levels, close to nucleus

9. 1 st IE2 nd IE3 rd IE4 th IE Na495.84562.469129543

10. Ionization EnergyIonization Energy

11. Example 1:Example 1: Place these elements in order of INCREASING 1 st ionization energy. 1)Mg, S, Si 2)As, N, P (p. 321 in text)

12. What does affinity mean?

13. Electron AffinityElectron Affinity  Creating negative ions ( anions)  Energy change with the addition of an electron to an atom  energy change that occurs when electrons added to gaseous atom  Energy is released when electrons are added, exothermic process (negative value)

14. Electron AffinityElectron Affinity  Electron tends to enter partially filled subshell or go to the next energy level  Does not follow predictable trend like atomic radii and ionization energy  An atom’s “desire/affinity” for more electrons, wants to get more electrons ! ! !  Metals—decrease electron affinity.  Nonmetals—increase electron affinity, more reactive  Stable atoms—full octet

15. Electron Affinity TrendElectron Affinity Trend Increases Decreases

16. Homework  Atomic Theory III worksheet #18-21  Read pp. 319-323  p. 334 #57-58