2. The Periodic Table Good afternoon! Please get your notebook and be in your seat when the bell rings.

3. Pre-Periodic Table Chemistry …  …was a mess!!!  No organization of elements.  Imagine going to a grocery store with no organization!!  Difficult to find information.  Chemistry didn’t make sense.

4. Dmitri Mendeleev: Created The Periodic Table HOW HIS WORKED…  Elements arranged in rows (periods) by increasing atomic mass.  Elements arranged in columns (families) by the way they reacted. SOME PROBLEMS…  Left blank spaces for what he said were undiscovered elements. (Turned out he was right!)  Pattern of increasing atomic mass was broken to keep similar reacting elements together. http://upload.wikimedia.org/wikipedia/commons/b/b3/Medele eff_by_repin.jpg

6. Periodic Law Ben’s Chem Videos http://www.youtube.com/wa tch?v=oFnRvSYMioAhttp://www.youtube.com/wa tch?v=oFnRvSYMioA http://www.youtube.com/wa tch?v=eJp6xkd4SAI&list=P LJ9LZQTiBOFFDw- QjstExbB0P5E9v_Zuh&inde x=9http://www.youtube.com/wa tch?v=eJp6xkd4SAI&list=P LJ9LZQTiBOFFDw- QjstExbB0P5E9v_Zuh&inde x=9

7. The Current Periodic Table  In 1913, Henry G.J. Moseley, an English scientist, arranged the elements based on increasing atomic number. http://www.chemistryexplained.com/Ma-Na/Moseley-Henry.html

8. Groups  Vertical columns are called groups or families  Groups are numbered 1 to 18.

9. Groups…Here’s Where the Periodic Table Gets Useful!!  Elements in the same group have similar chemical and physical properties!!  Example: Elements in Group 1 are highly reactive and can be explosive in water. http://www.teachertube.com/view Video.php?video_id=41344 http://www.teachertube.com/view Video.php?video_id=41344  They have the same number of valence electrons.  http://www.tutorvista.com/content/science/sci ence-i/structure-atom/valence-shell- electron.php Why?

10. Valence Electrons Electrons farthest away from the nucleus are most loosely held. Ranges from 1 to 8 valence electrons Many properties of the atom, and therefore of an element, are determined by the number of valence electrons.  http://www.tutorvista.com/content/science/sci ence-i/structure-atom/valence-shell- electron.php

11. Periods Horizontal rows numbered 1 to 7. Elements in the same period have the same number of electron shells or energy levels.

12. Properties of Elements on the Periodic Table  An element’s physical and chemical properties can be predicted from its location in the periodic table  Example: Sodium is more reactive than Aluminum  Reactivity in metals decreases as you go from left to right.  For nonmetals, the opposite is true. Nonmetals in Groups 14 through 17 become more reactive from left to right. Group 18, the Noble Gases, are an exception.

13. Metals: Left/Middle of Periodic Table Shiny, metallic Conduct heat and electricity Malleable and ductile (reshape) Give up valence electron in a reaction Copper Nickel Aluminum Gold Silver Mercury

14. Metalloids: Zigzag on Periodic Table where metals and nonmetals meet Mostly shiny, metallic looking Only semi-conductive Often combined with non-metals

15. Non-Metals: Right side of Periodic Table Dull, not shiny, many are GAS Do not conduct heat or electricity Crumble or break if solid (non-malleable/ductile) Neon Helium Iodine ChlorineCarbon Sulfur Gain or share electrons in a chemical reaction

16. Metals: Green (Include 113-116) Metalloids: Purple (Include 117) Nonmetals: Orange (Include 118)

18. Hydrogen  Belongs to a family of its own.  Diatomic, reactive gas.  Was involved in the explosion of the Hindenburg aircraft.  Promising as an alternative fuel source for automobiles

19. Alkali Metals  1 st column on the periodic table (Group 1) not including hydrogen.  Very reactive metals  Always combined with something else in nature (like in salt).  Soft enough to cut with a butter knife  1 valence electron

20. Alkaline Earth Metals  Second column on the periodic table. (Group 2)  Reactive metals  Always combined with nonmetals in nature.  Several are important mineral nutrients (Mg and Ca)  2 valence electrons

21. Transition Metals  Elements in groups 3-12  Less reactive harder metals  Includes metals used in jewelry and construction.

22. Boron Family  Elements in group 13  Aluminum metal was once rare and expensive, not a “disposable metal.”

23. Carbon Family  Elements in group 14  Contains elements important to life and computers.  Carbon is the basis for an entire branch of chemistry.  Silicon and Germanium are important semiconductors.

24. Nitrogen Family  Elements in group 15  Nitrogen makes up over ¾ of Earth’s atmosphere.  Nitrogen and phosphorus are both important in living things.  Most of the world’s nitrogen is not available to living things.  The red stuff on the tip of matches is phosphorus.

25. Oxygen Family  Elements in group 16  Oxygen is necessary for respiration.  Many things that stink, contain sulfur (rotten eggs, garlic, skunks,etc.)

26. Halogens  Elements in group 17, also called Halides  Very reactive, volatile, diatomic, nonmetals  Always found combined with other element in nature  Used as disinfectants and to strengthen teeth

27. The Noble Gases  Elements in group 18  VERY unreactive (STABLE), monatomic gases  Used in lighted “neon” signs  Used in blimps to fix the Hindenburg problem.  Have a full valence shell.

28.  One of two rows that “sits off” to the bottom of the periodic table  Reactive  Fairly soft metals Lanthanide Series

29.  Also towards bottom of periodic table  All are radioactive, some are not found in nature  Some with higher atomic numbers have only been made in labs Actinide Series

30. Electron Configuration http://www.chemprofessor.com/periodicqm.htm http://www.youtube.com/watch?v=jtYzEzykFdg http://www.youtube.com/watch?v=2AFPfg0Como Click on the video links for explanations of electron configuration.

31. Pre-AP Periodic Trends Atomic Radius – related to the atom’s volume. − Period – atomic radius decreases as you go from left to right − Group – atomic radius increases as you go down a group

32. Pre-AP Periodic Trends Electronegativity – the atoms “desire” to grab another atom’s electrons. − Period – electronegativity increases as you go from left to right − Group – electronegativity decreases as you go down a group

33. Pre-AP Periodic Trends Ionization Energy – amount of energy needed to remove the outermost electron. Closely related to electronegativity. − Period – Ionization energy increases as you go from left to right − Group – Ionization energy decreases as you go down a group

34. Pre-AP Periodic Trends Reactivity – how likely or how vigorously an atom is to react with another substance. Non-Metals − Period - reactivity increases as you go from left to right, except for Group 18 − Group – reactivity decreases as you go down the group Metals − Period – reactivity decreases as you go from left to right − Group – reactivity increases as you go down a group

35. Pre-AP Periodic Trends Melting Point Metals – the melting point for metals decreases as you go down a group Non-Metals – the melting point for non-metals increases as you go down a group