Reading for next Monday – Chapter 6 sections 1-6

1. Reading for next Monday – Chapter 6 sections 1-6 • Homework 5 – Due Monday 9/29/14 (only chap 5 assignment) • Chapter 5 #s 18, 20, 22, 34, 36, 39-46 (all), 55, 56, 61, 62, 70, 72, 94 • Exam #1 – Wednesday 9/24/14 • Lab next week – EXP 7 • Wet lab • prelab

2. The Modern Periodic Table • Periods (series) • Labeled 1 - 7

3. The Modern Periodic Table • Groups (families) • Columns • 2 different labeling systems • 1-18 • A-B

4. A few definitions… • Main Group Elements: • Groups 1 and 2 and 13 – 18 • Groups A

5. Main Group Elements

6. A few definitions… • Main Group Elements: • Groups 1 and 2 and 13 – 18 • Groups A • Transition Elements: • Groups 3 – 12 • Groups B

7. Transition Elements

8. Groups of Elements • Vertical columns are called groups • Group 1 = Alkali Metals

9. Alkali Metals

10. Groups of Elements • Vertical columns are called groups • Group 1 = Alkali Metals • Group 2 = Alkaline Earth Metals

11. Alkaline Earth Metals

12. Groups of Elements • Vertical columns are called groups • Group 1 = Alkali Metals • Group 2 = Alkaline Earth Metals • Group 17 = Halogens

13. Halogens

14. Groups of Elements • Vertical columns are called groups • Group 1 = Alkali Metals • Group 2 = Alkaline Earth Metals • Group 17 = Halogens • Group 18 = Noble Gases

15. Noble Gases

16. The Modern Periodic Table • Representative elements • Also known as main group elements • Transition metals • Inner transition metals • Lanthanide series

17. Lanthanide Series

18. The Modern Periodic Table • Representative elements • Also known as main group elements • Transition metals • Inner transition metals • Lanthanide series • Actinide series

19. Actinide Series

20. Diatomic Elements • Elements that exist as diatomic molecules when UNCOMBINED (meaning not in a compound with other elements). H2, N2, O2, F2, Cl2, Br2, I2

22. Diatomic Elements • Elements the exist as diatomic molecules when UNCOMBINED (meaning not in a compound with other elements). H2, N2, O2, F2, Cl2, Br2, I2 NaCl BiF5 K3N Examples of when these elements are NOT diatomic AlI3 TiBr4

23. Periodic Trends • Atomic Radius • Increase

24. Atomic Radius Trend • Atoms get smaller as you go bottom to top on the periodic table because there are fewer energy levels on the atom. (Na has 3 energy levels, K has 4) • Atomic radius decreases as you travel left to right across the periodic table because the number of protons in the nucleus increases.

25. IONS!!

26. Atoms vs. Ions • Atoms are NEUTRAL!!!!! • This means that they have zero charge • #p+ = #e-

27. Charge!!! e- = -1 p+ = 1 + 0 47 e- = -47 47 p+ = 47 + 0 When #p+ = #e-, the atom has no charge and is neutral

28. Atoms vs. Ions • Atoms can gain or lose e- to form IONS • ANY charged particle is called an ion • Losing e- gives POSITIVELY charge

29. Charge!!! When an atom LOSES electrons 11 p+ = 11 -10 10 e- = 11 e- = +1

30. Atoms vs. Ions • Atoms can gain or lose e- to form IONS • ANY charged particle is called an ion • Losing e- gives POSITIVELY charge • Called cations • Usually formed from metals • Gaining e- gives a NEGATIVELY charged ion

31. Atoms vs. Ions • Atoms can gain or lose e- to form IONS • ANY charged particle is called an ion • Losing e- gives POSITIVELY charge • Called cations • Usually formed from metals • Gaining e- gives a NEGATIVELY charged ion • Called anions • Usually formed from non-metals

32. Charge!!! When an atom LOSES electrons 11 p+ = 11 10 e- = -10 +1 16 p+ = 16 When an atom GAINS electrons -18 16 e- = 18 e- = -2

33. Atoms vs. Ions • Atoms can gain or lose e- to form IONS • ANY charged particle is called an ion • Losing e- gives POSITIVELY charge • Called cations • Usually formed from metals • Gaining e- gives a NEGATIVELY charged ion • Called anions • Usually formed from non-metals

34. How many electrons are needed to be neutral? 15 protons

35. 15 protons 2 electrons

36. 15 protons 10 electrons

37. Total charge = 0 Stable!!! 15 protons 15 electrons

38. Valence electrons are the outermost electrons

39. Total charge = p+ - e- = 15 – 18 = -3 Stable!! 15 protons 18 electrons

40. How many electrons are needed to be neutral? 12 protons

41. 12 protons 2 electrons

42. 10 electrons 12 protons

43. Total charge = 0 STABLE! 12 protons 12 electrons

45. Total charge = p+ - e- = 12 – 10 = +2 10 electrons 12 protons

46. Total charge = p+ - e- = 12 – 10 = +2 12 protons STABLE! 10 electrons

47. Quick Rehash… e- are found in shells outside the nucleus e- are found in shells outside the nucleus atoms are stable when: 1) number of protons and electrons are equal 1) number of protonsandelectrons are equal 2) when the valence shell is full 2) when the valenceshell is full atoms will either gain or lose valence electrons in order to have a full outer shell atoms will either gain or lose valence electrons in order to have a full outer shell atoms will either gain or lose valence electrons in order to have a full outer shell valence shells hold up to 8 electrons, except for the first shell, which only holds 2 electrons. valence shells hold up to 8 electrons, except for the first shell, which only holds 2 electrons. valence shells hold up to 8 electrons, except for the first shell, which only holds 2 electrons. valence shells hold up to 8 electrons valence shells hold up to 8 electrons

48. Calculating Charge of an Ion #p+ - #e- = ionic charge Atom of chlorine: 17 p+ 17 e- - = 0 charge Ion of chlorine: 17 p+ 18 e- - = -1 charge Atom of nitrogen: 7 p+ 7 e- - = 0 charge Ion of nitrogen: 7 p+ 10 e- - = -3 charge Atom of strontium: 38 p+ 38 e- - = 0 charge Ion of strontium: 38 p+ 36 e- - = +2 charge

49. A Bit of Review • Valence electrons • Most atoms will gain or lose electrons in order to get a full valence electron shell • The number of valence electrons in a neutral atom can be found from the periodic table!!