1. Chapter 5 section 3 Measurable Goal: Examine periodic trends

2. Recap NO DSQ today Section 1 and 2-overview of periodic table /how to read the periodic table Lab-examined Group II metals to determine trends (know lab questions for test) Section 3-today (periodic trends)

3. Trends in the periodic table: Ionization Energy Atomic Radius Electron Affinity Electronegativity

4. Periodic Trends There are several important atomic characteristics that show predictable trends that you should know. The first is atomic radius. Radius is the distance from the center of the nucleus to the “edge” of the electron cloud.

5. Atomic Radius Atoms get larger going down a group. Why? With each step down the family, we add an entire level to the electron cloud, making the atoms larger with each step.

6. Atomic Radius The trend across a horizontal period is less obvious. What happens to atomic structure as we step from left to right? Each step adds a proton and an electron (and 1 or 2 neutrons). Electrons are added to existing sublevels.

7. Atomic Radius The effect is that the more positive nucleus has a greater pull on the electron cloud. The nucleus is more positive and the electron cloud is more negative. The increased attraction pulls the cloud in, making atoms smaller as we move from left to right across a period.

8. Let’s Practice Pg 179 #1a, 2a

9. Ionization Energy 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. The atom has been “ionized” or charged. The number of protons and electrons is no longer equal.

10. Ionization Energy The energy required to remove an electron from an atom is ionization energy. (measured in kilojoules, kJ) The larger the atom is, the easier its electrons are to remove Therefore, ionization energy decreases as you move down a group and increases as you move from left to right across the period.

11. Let’s Practice Pg 179 #1 (b)

12. Electron Affinity What does the word ‘affinity’ mean? Electron affinity is the energy change that occurs when an atom gains an electron (also measured in kJ). For example, the EA for a neon atom is 4.8X10 -20 Joule. So 4.8X10 -20 Joules is needed to add another electron to a neon atom.

13. Electron Affinity General rule, Nonmetals (elements on right side) have stronger electron affinities than metals (elements on the left side) with the exception being the noble gases Read last paragraph on pg 182-183

14. Electronegativity Electronegativity is a measure of an atom’s attraction for another atom’s electrons. Generally, metals are electron givers and have low electronegativities. Nonmetals are are electron takers and have high electronegativities.

15. Conclusion