1. (Honors) Intro to the Table (Honors) Intro to the Table http://youtu.be/5MMWpeJ5dn4 http://youtu.be/5MMWpeJ5dn4 http://youtu.be/5MMWpeJ5dn4 Dan Radcliffe Knows his elements! Dan Radcliffe Knows his elements! http://youtu.be/rSAaiYKF0cs http://youtu.be/rSAaiYKF0cs http://youtu.be/rSAaiYKF0cs Elements Song: Elements Song: Periodic Table of Videos Crew: Periodic Table of Videos Crew: http://youtu.be/afFw91fvNJM http://youtu.be/afFw91fvNJM http://youtu.be/afFw91fvNJM A different Song A different Song http://www.youtube.com/watch?v=zUDDiWtFtEM&safe=active http://www.youtube.com/watch?v=zUDDiWtFtEM&safe=active http://www.youtube.com/watch?v=zUDDiWtFtEM&safe=active

2. Periodic Table of Elements

3. Dmitri Mendeleev Russian chemist. Russian chemist. Created first version of periodic table. Created first version of periodic table. Predicted properties of elements yet to be discovered. Predicted properties of elements yet to be discovered. Rockin the shaggy beard…

4. Mendeleev arranged elements according to their atomic weights. Mendeleev arranged elements according to their atomic weights. Today they are arranged by atomic number. Today they are arranged by atomic number. Development of the Table: 3:39 http://youtu.be/nsbXp64YPRQ

5. Periodic Law Properties of elements are periodic functions of their atomic numbers. Properties of elements are periodic functions of their atomic numbers. In other words, properties tend to repeat as you start a new period. In other words, properties tend to repeat as you start a new period.

6. Groups/Families Columns (1-18). Columns (1-18). Elements have same number of valence electrons. Elements have same number of valence electrons. Have similar chemical properties. Have similar chemical properties. Tend to form bonds in a similar way to get stable octet.

7. Periods Rows (1-7). Rows (1-7). Have same number of occupied energy levels. Have same number of occupied energy levels. They do not have similar properties. They do not have similar properties.

8. Group 1: Alkali Metals 1 valence electron 1 valence electron Form +1 Ions Form +1 Ions Very reactive Very reactive Found only in compounds. Found only in compounds.

9. Rubidium http://youtu.be/uixxJtJPVXk http://www.youtube.com/watch?feature=player_embe dded&v=HY7mTCMvpEM

10. Group 2: Alkaline Earth Metals 2 valence electrons 2 valence electrons Form +2 ions Form +2 ions Very reactive Very reactive Found only in compounds Found only in compounds

11. Group 2: Some Alkaline Earth Metals

12. Group 17: Halogens 7 valence electrons 7 valence electrons Form -1 ions Form -1 ions Very reactive Very reactive All nonmetals All nonmetals

13. IODINE solid → gas (sublimes) GasLiquidSolid FLUORINE Extremely reactive gas http://www.youtube.com/watc h?feature=player_embedded &v=u2ogMUDBaf4

14. Group 18: Noble Gases Inert Gases Inert Gases Not reactive Not reactive Have stable octet Have stable octet (except He) Monoatomic gases Monoatomic gases

15. s, p, d, f, “Blocks” Indicates what sublevel is being filled last in the atom Indicates what sublevel is being filled last in the atom

16. Lanthanide & Actinide Series Two rows on the bottom of the table Two rows on the bottom of the table “f” block “f” block Start with lanthanum and actinium Start with lanthanum and actinium

17. Transition Metals Metals in the “lower” columns. Metals in the “lower” columns. (d-block metals) “Inner” transition metals are the two bottom rows “Inner” transition metals are the two bottom rows (f-block metals) (f-block metals)

18. Transition Metals Form colored compounds and solutions. Form colored compounds and solutions. Often have multiple “oxidation states” (charges) Often have multiple “oxidation states” (charges) May involve d-sublevel electrons in forming bonds May involve d-sublevel electrons in forming bonds

19. Man Made Elements: Man Made Elements: Elements that are not found naturally in the earth’s crust. Elements that are not found naturally in the earth’s crust. Must be created through nuclear bombardment using particle accelerators. Must be created through nuclear bombardment using particle accelerators. All elements above Uranium (Atomic #92) All elements above Uranium (Atomic #92) Radioactive Elements: Radioactive Elements: All the isotopes of elements higher than Bismuth (Atomic #83) are radioactive. All the isotopes of elements higher than Bismuth (Atomic #83) are radioactive.

20. Do we know our groups? Do we know our groups? Elements Song Again! Elements Song Again! http://youtu.be/zGM-wSKFBpo http://youtu.be/zGM-wSKFBpo http://youtu.be/zGM-wSKFBpo Periodic Table Dating Game Periodic Table Dating Game http://www.youtube.com/watch?v=A6cF0iWC3J4 http://www.youtube.com/watch?v=A6cF0iWC3J4 http://www.youtube.com/watch?v=A6cF0iWC3J4

21. Review Question: Review Question: How many different ways is the structure of the Periodic Table related to the inner structure of an atom? How many different ways is the structure of the Periodic Table related to the inner structure of an atom? Think proton # and electron configuration! Think proton # and electron configuration!

22. Metals/Nonmetals/Metalloids

23. Metals Luster Luster Malleable Malleable Ductile Ductile Conduct heat and electricity Conduct heat and electricity Tend to lose valence electrons and form positive ions Tend to lose valence electrons and form positive ions All solids (except Hg) All solids (except Hg)

24. Nonmetals No luster No luster Brittle (if solid) Brittle (if solid) Don’t conduct Don’t conduct Tend to gain valence electrons Tend to gain valence electrons and form negative ions Can be solid ( I, C, P, S), liquid (Br), Can be solid ( I, C, P, S), liquid (Br), or gases (F, Cl, N, O) Hydrogen is considered a nonmetal Hydrogen is considered a nonmetal

25. Metalloids (Semimetals) Most elements along the “staircase” Most elements along the “staircase” Can have properties of both metals and nonmetals. Can have properties of both metals and nonmetals. B, Si, Ge, As, Sb, Te, At B, Si, Ge, As, Sb, Te, At

26. Trends in the Periodic Table

27. Atomic Radius Distance from the nucleus of an atom to the outer edge of it’s electron cloud. Distance from the nucleus of an atom to the outer edge of it’s electron cloud.

28. Trends in Radius (Use Table S) Down a Group Down a Group Ex: Group 1 What happens? Across a Period Across a Period Ex: Period 2What happens? Li Na K Rb Cs Fr LiBeBCNOFNe

29. Let’s Think: Can you come up with a reason why you think this trend happens? Can you come up with a reason why you think this trend happens? How might it be related to electron shells and electron repulsion? How might it be related to electron shells and electron repulsion? How might it be related to the pull of nuclear charge? How might it be related to the pull of nuclear charge?

30. Down a Group: Size increases Down a Group: Size increases Add new energy levels Add new energy levels Greater shielding from core electrons Greater shielding from core electrons Outer electrons further from nucleus so less attractive force Outer electrons further from nucleus so less attractive force

31. Across a Period: Size decreases Across a Period: Size decreases Increasing nuclear charge pulls on same # of energy levels Increasing nuclear charge pulls on same # of energy levels No increase in shielding effect No increase in shielding effect

32. http://youtu.be/ba2yN2HtPTA http://www.youtube.com/watch?v=VopLrkfXfGw&safe=active http://youtu.be/ba2yN2HtPTA http://www.youtube.com/watch?v=VopLrkfXfGw&safe=active Helpful Tutorial: Helpful Tutorial: http://www.youtube.com/watch?v=k9NrwDaMRQk&safe=active http://www.youtube.com/watch?v=k9NrwDaMRQk&safe=active

33. Ionization Energy Energy required to remove the outermost electron from an atom. Energy required to remove the outermost electron from an atom.

34. Trends in Ionization Energy (Use Table S) Down a Group Down a Group Ex: Group 1 What happens? Across a Period Across a Period Ex: Period 2What happens? Li Na K Rb Cs Fr LiBeBCNOFNe

35. What is the trend? Directly related to Atomic Radius. Larger Radius = Lower Ionization Energy Larger Radius = Lower Ionization Energy

36. Why? The further the outermost electron is from the nuclear pull, the easier it is to remove. The more shells of kernel electrons around the nucleus the greater the “shielding effect”.

37. Electronegativity Attraction an atom has for electrons involved in bond formation. Attraction an atom has for electrons involved in bond formation.

38. Electronegativity The higher the EN value the more the atom “pulls” on electrons involved in a bond. The higher the EN value the more the atom “pulls” on electrons involved in a bond. Like a “tug of war” for electrons in the bond Like a “tug of war” for electrons in the bond

39. Polarity of Bonds Polar Bond: Polar Bond: unequal electron sharing unequal electron sharing atoms have different EN values atoms have different EN values Nonpolar Bond: Nonpolar Bond: equal electron sharing equal electron sharing Atoms have same EN values Atoms have same EN values

40. Fluorine has the highest EN value = 4 Fluorine has the highest EN value = 4 EN scale was created by comparing other elements to Fluorine EN scale was created by comparing other elements to Fluorine Nonmetals generally have much higher EN values than metals Nonmetals generally have much higher EN values than metals

41. Trends in Electronegativity (Use Table S) Down a Group Down a Group Ex: Group 1 What happens? Across a Period Across a Period Ex: Period 2What happens? Li Na K Rb Cs Fr LiBeBCNOFNe

42. What was the trend? What was the trend? What is the relationship to atomic radius? What is the relationship to atomic radius? What elements don’t have really have electronegativity values? Why is that? What elements don’t have really have electronegativity values? Why is that? http://youtu.be/93G_FqpGFGY http://www.youtube.com/watch?v=YZ8izzEq6zI&safe=active

43. Metallic/NonMetallic Character More “Metallic”: More “Metallic”: Large radius Large radius Low Ionization Energy Low Ionization Energy Low Electronegativity Low Electronegativity More “Non Metallic”: More “Non Metallic”: Small radius Small radius High Ionization Energy High Ionization Energy High Electronegativity High Electronegativity http://www.youtube.com/watch?feature=pla yer_embedded&v=hANWofStHrk

44. Crash Course Video(13 minutes) Crash Course Video(13 minutes) http://www.youtube.com/watch?v=0RRVV 4Diomg&safe=active http://www.youtube.com/watch?v=0RRVV 4Diomg&safe=active http://www.youtube.com/watch?v=0RRVV 4Diomg&safe=active http://www.youtube.com/watch?v=0RRVV 4Diomg&safe=active