1. Take out your periodic table

2. Metals, Nonmetals, Metalloids There is a zig-zag or staircase line that divides the table. Metals are on the left of the line, in blue. Nonmetals are on the right of the line, in orange.

3. Metals Metals are lustrous (shiny), malleable, ductile, and are good conductors of heat and electricity. They are mostly solids at room temp.

4. Nonmetals Nonmetals are the opposite. They are dull, brittle, nonconductors (insulators). Some are solid, but many are gases, and Bromine is a liquid.

5. Metalloids Metalloids, aka semi-metals are just that. They have characteristics of both metals and nonmetals. They are shiny but brittle. And they are semiconductors. What is our most important semiconductor?

6. The Periodic Law Atoms with similar properties appear in groups or families (vertical columns) on the periodic table. They are similar because they all have the same number of valence (outer shell) electrons, which governs their chemical behavior.

7. Title: Periodic Trends Subtitles: p. 2 (after cover) atomic radius p. 3 ionization energy p. 4 electronegativity

9. Atomic Radius 1. Definition 2. Trend 3. 2 Reasons for Trend

10. Atomic Radius Trend: smaller at the top to larger at the bottom of the family. Decreases moving left to right (period) Reason: With each step down the family, we add an energy level to the electron cloud, making the atoms larger with each step.

11. Atomic Radius Reason 2: Each step adds a proton and an electron, but electrons are added to existing sublevels.

12. Effective Nuclear Charge What keeps electrons from simply flying off into space? Effective nuclear charge is the pull that an electron “feels” from the nucleus. The closer an electron is to the nucleus, the more pull it feels. As effective nuclear charge increases, the electron cloud is pulled in tighter.

13. 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.

14. Atomic Radius Here is an animation to explain the trend.

15. Ionization Energy Definition Detail Trend 1 reason

16. Ionization Energy Definition: The energy required to remove an electron from an atom is ionization energy Detail: The larger the radius of the atom, the easier its electrons are to remove. Detail: Ionization energy and atomic radius are inversely proportional.

17. Ionization Energy Trends: Ionization energy increase moving left to right horizontally Ionization energy decreases moving down

18. Reason: As more levels are added to atoms, the inner layers of electrons shield the outer electrons from the nucleus. The effective nuclear charge on those outer electrons is less, and so the outer electrons are less tightly held.

19. Electronegativity Definition Detail Trend Reason

20. Electronegativity Definition: Electronegativity is a measure of an atom’s attraction for another atom’s electrons. Detail: Generally, metals are electron givers and have low electronegativities. Detail: Nonmetals are are electron takers and have high electronegativities. What about the noble gases?

21. Electronegativity Trend: Electronegativity increases moving left to right and moving up the periodic table Reason: More protons are added, so electrons held more tightly + outer shell is getting closer to completing octet rule

22. Overall Reactivity This ties all the previous trends together in one package. However, we must treat metals and nonmetals separately. The most reactive metals are the largest since they are the best electron givers. The most reactive nonmetals are the smallest ones, the best electron takers.