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Periodic Properties and Trends

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Periodic Properties and Trends

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  1. Periodic Properties and Trends

  2. Atomic Radii • 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.

  3. 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

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

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

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

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

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

  9. - - F, 71 pm F , 133 pm 9e and 9p 10 e and 9 p 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.

  10. Trends in Ion Sizes Figure 8.13

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

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

  13. Ionization Energy Mg + 738 kJ  Mg+ + e- This is called the FIRST ionization energy because we removed only the OUTERMOST electron IE = energy required to remove an electron from an atom. Mg+ + 1451 kJ  Mg2+ + e- When the 2nd e- is removed it is called the 2nd IE.

  14. 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).

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

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

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

  18. 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

  19. 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.

  20. Electronegativity

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

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

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