1. Periodicity Dr. Ron Rusay

2. Atomic Structure and Periodicity ð ð The History of the Periodic Table ð ð The Aufbau Principles and the Periodic Table ð ð Periodic Trends in Atomic Properties ð ð The Properties of a Group: The Alkali Metals ð ð Types of Chemical Bonds ð ð Electronegativity ð ð Bond Polarity and Dipole Moments ð ð Ions: Electron Configurations and Sizes ð ð Formation of Binary Ionic Compounds

3. Periodic Table Mendeleev’s Table 1868-1871Mendeleev’s Table 1868-1871 Mural at St.Petersburg University, Russia

5. Periodic Properties Calibrated Peer Review Writing Assignment

6. Chemical Bonds Definition: Attractive forces which hold atoms together and provide a particular molecular arrangement of atoms with new chemical properties.

7. Electron Configurations & Bonds Noble Gases and The Rule of Eight  When two nonmetals react to form a covalent bond: They share electrons to achieve a Noble gas electron configuration.  When a nonmetal and a metal react to form an ionic compound: Valence electrons of the metal are lost and the nonmetal gains these electrons.

8. Ionic Bonds  Result from electrostatic attractions of closely packed, oppositely charged ions.  Form when an atom which can easily lose electrons reacts with one which has a high electron affinity, that is, it can easily gain electrons.  Eg. Mg and Cl; K and O

9. Ionic vs. Covalent Bonding

10. Bond Length (Covalent Bonds)  Interatomic distance.  It is the distance where the bond energy is at a minimum value, and which is the most stable atomic form.

11. Bond Lengths and Covalent Radius

13. Periodic Trends Atomic Radius  Atomic Radii: What’s a picometer? 1 x 10 -12 m  decreases going from left to right across a period;  increases going down a group.

14. Atomic Radii

18. QUESTION

19. ANSWER 2+ D)Mg The loss of electrons will always decrease the size of the ion and the addition of electrons will always increase the size of the ion.

20. Ionization Energy

21. QUESTION

22. ANSWER. C)greater than 735 kJ/mol The second ionization energy is always greater than the first, because the next electron is no longer leaving a neutral atom, but one with a +1 charge.

23. Periodic Trends  First ionization energy:  increases from left to right across a Period;  decreases going down a Group.

24. QUESTION

25. ANSWER D)S Ionization energy increases moving up a group and moving right along a row.

28. Electron Affinity  The energy change associated with the addition of an electron to a gaseous atom.  X(g) + e   X  (g)

30. Electronegativity  The ability of an atom in a molecule to attract shared electrons to itself.   = (H  X) actual  (H  X) expected

31. Electronegativity

32. Electronegativity

34. QUESTION

35. ANSWER. B)Rb < O < F Electronegativities increase moving up a column and to the right in the periodic table.

37. QUESTION

38. ANSWER. D)ionic bonds If two atoms have greatly differing electronegativities the more electronegative atom will pull on the bonding electrons so strongly the electrons will transfer from one atom to the other.

39. Covalent Bond Polarity  A molecule, such as HF, that has a center of positive charge and a center of negative charge is said to be polar, or to have a dipole moment.

41. QUESTION

42. ANSWER B)KF Use the periodic table or an electronegativity chart to determine the greatest difference in electronegativities of atoms in the binary ionic compounds.

44. Trends in Reactivity Lithium (Li), Sodium (Na) & Potassium (K) What might account for this trend?What might account for this trend? Do you expect the Alkaline Earths (Group IIA) to behave similarly?Do you expect the Alkaline Earths (Group IIA) to behave similarly? Does this trend apply to all Groups?Does this trend apply to all Groups? What is trend in the chemical reactivity observed for the alkali metals, Group IA?

45. Transition Metals (B Group Elements)

46. Transition Metals (B Groups) Oxidation States

47. Information & the Periodic Table A great deal of specific, general and comparative information can be developed from the Periodic Table: A great deal of specific, general and comparative information can be developed from the Periodic Table:  1. Group valence electron configurations.  2.Individual electron configurations.  3.General chemical behavior and physical properties.  4.Distinguishing metals and nonmetals.

48. Summary of Periodic Trends Periods (Horizontal Rows)  Atomic size generally decreases across a Period.  The first ionization energy and electronegativity generally increase across a Period.. This is a result of increasing effective nuclear charge and electrons being in the same principal energy level.

49. Summary of Periodic Trends Periods (Horizontal Rows)  Metallic character decreases as elements change from metals to metalloids to nonmetals.  General reactivity is highest at the left and right ends of a Period. (Excluding the inert noble gases.)  In Period 2, the physical properties change abruptly between carbon (solid) and nitrogen (gas).