1. All roads lead to the Elements

2.  Creator: Dmitri Mendeleev  Early periodic table: Arranged according to Avg. Atomic Mass  Contained 63 elements  Predicted 3 yet-to-be elements  Left spaces for undiscovered elements

5.  What do you do to a wrinkled shirt?

6.  Henry Moseley – 1913  Learned that each element has a specific number of protons  Developed modern periodic table  Based upon Protons

7.  Periods: the horizontal rows on the periodic table (left to right)  Groups/Families: the vertical columns on the periodic table (up and down)

8.  Periods = Energy Level  Sub Levels labeled (s, p, d, & f)

9.  Mickey’s pal

10.  Valence electrons: electrons in the outermost shell  Octet Rule: the stable arrangement for all elements is to have 8 valence electrons

12.  Group 1: Alkali Metals  Group 2: Alkaline-Earth Metals  Group 3-12: Transition Metals  Group 17: Halogens  Group 18: Nobel Gases

13.  Group 1: Alkali Metals  Soft  Shiny  Has 1 Valence electron  Highly reactive

14.  Group 2: Alkaline-Earth Metals  Reactive (not as reactive as Alkali Metals)  2 valence electrons

15.  Mr. Mony’s enemy

16.  Group 3-12: Transition Metals  Can have more than 1 oxidation number  Metallic  Wide-range of uses Iron, Cobalt, Copper, and Manganese use in your body Copper for electrical wires Gold, Silver, Platinum in jewelry

17.  Group 17: Halogens  Very Reactive  Have 7 Valence electrons  Tend to find in compounds

18.  Name of a goofy convict

19.  Group 18: Noble Gases  8 Valence electrons  Unreactive

20.  What a dog does with a bone?

21.  Oxidation number: a number used to indicate how many electrons will be gained or lost  Ag (+1), Zn (+2), Cd (+2)  Ion: a charged atom

22.  Police

23. Metalloids: B, Si, Ge, As, Sb, Te, Po (have characteristics of both metals and nonmetals) Metals: shiny, malleable, ductile, good conductors Non-metals: primarily gases, poor conductors

24.  Atomic Radii- distance from the nucleus to the outermost stable electron  Electronegativity- ability of an atom to attract electrons and form a chemical bond  Ionization Energy- the energy needed to remove an electron  Ionic Radii- distance from the nucleus to the outermost electron in an ion  Increases moving down the columns and increases right to left  Increases moving up the columns and increases left to right (Noble Gas family has 0 electronegativity)  Increases moving up the columns and increases left to right  Increases moving down a family (Noble Gas Trick)

26.  Extinct

27.  Which group/family will not bond with any other elements?

28.  How many valence electrons does Phosphorus have?

29.  Which element is the most electronegative?

30.  To follow the octet rule how many valence electrons do all elements want?

31.  How many valence electrons does Calcium have?

32.  Family with 7 valence electrons and highly reactive?

33.  What is the oxidation number for Oxygen?

34.  Which element is more metallic Ag or Ge?

35.  Imitation Diamond