2. Periodic Properties and Trends

3. Atomic Radii Size Increases going down a group.Size Increases going down a group. Because electrons are added further from the nucleus, there is less attraction. This is due to additional energy levels and the shielding effect. Each additional energy level “shields” the electrons from being pulled in toward the nucleus. Size DECREASES going across a period.Size DECREASES going across a period. Size Increases going down a group.Size Increases going down a group. Because electrons are added further from the nucleus, there is less attraction. This is due to additional energy levels and the shielding effect. Each additional energy level “shields” the electrons from being pulled in toward the nucleus. Size DECREASES going across a period.Size DECREASES going across a period.

4. Atomic Size Size decreases across a period owing to increase in the positive charge from the protons. Each added electron feels a greater and greater + charge because the protons are pulling in the same direction, where the electrons are scattered. Large Small

5. Which is Bigger? 1) Na or K ? 2) Na or Mg ? 3) Al or I ?

6. Which is Bigger? 1) Na or K ? K 2) Na or Mg ? Na 3) Al or I ? I

7. Ion Sizes Does the size go up or down when losing an electron to form a cation? Does the size go up or down when losing an electron to form a cation?

8. Ion Sizes CATIONS are SMALLER than the atoms from which they come. The electron/proton attraction has gone UP and so size DECREASES. Li,152 pm 3e and 3p Li +, 78 pm 2e and 3 p + Forming a cation.

9. Ion Sizes Does the size go up or down when gaining an electron to form an anion?

10. Ion Sizes ANIONS are LARGER than the atoms from which they come. The electron/proton attraction has gone DOWN and so size INCREASES. Trends in ion sizes are the same as atom sizes. Forming an anion. F, 71 pm 9e and 9p F -, 133 pm 10 e and 9 p -

11. Trends in Ion Sizes Figure 8.13

12. Which is Bigger? 4) Cl or Cl - ? 5) K + or K ? 6) Ca or Ca +2 ? 7) I - or Br - ?

13. Which is Bigger? Cl - 4) Cl or Cl - ? Cl - K 5) K + or K ? K Ca 6) Ca or Ca +2 ? Ca I - 7) I - or Br - ? I -

14. Mg + 738 kJ  Mg + + e- This is called the FIRST ionization energy because we removed only the OUTERMOST electron Mg + + 1451 kJ  Mg 2+ + e- When the 2 nd e- is removed it is called the 2 nd IE. IE = energy required to remove an electron from an atom. Ionization Energy

15. Trends in Ionization Energy IE increases across a period because the positive charge increases. Metals lose electrons more easily than nonmetals. Nonmetals lose electrons with difficulty (they like to GAIN electrons).

16. Trends in Ionization Energy IE decreases down a groupIE decreases down a group Because size increases (Shielding Effect)Because size increases (Shielding Effect) Reducing ability generally increases down the periodic table.Reducing ability generally increases down the periodic table.

17. Which has a higher 1 st ionization energy? 8) Mg or Ca ? 9) Al or S ? 10) Cs or Ba ?

18. Which has a higher 1 st ionization energy? 8) Mg or Ca ? Mg 9) Al or S ? S 10) Cs or Ba ? Ba

19. Electronegativity is a measure of the ability of an atom in a molecule to attract electrons to itself. Concept proposed by Linus Pauling 1901-1994 Concept proposed by Linus Pauling 1901-1994

20. Periodic Trends: Electronegativity In a group: Atoms with fewer energy levels can attract electrons better (less shielding). So, electronegativity increases UP a group of elements. In a period: More protons, while the energy levels are the same, means atoms can better attract electrons. So, electronegativity increases RIGHT in a period of elements.

21. Electronegativity

22. Which is more electronegative? 11) F or Cl ? 12) Na or K ? 13) Sn or I ?

23. Which is more electronegative? 11) F or Cl ? F 12) Na or K ? Na 13) Sn or I ? I

24. Summary of the Trends Ionic Radii decreasesAtomic mass increases Density increases Melting/boiling point increases to stair-step line then decreases. M.P./B.P. decreases