1. Why is the Periodic Table important to me? The periodic table is the most useful tool to a chemist. You get to use it on every test. It organizes lots of information about all the known elements.

2. 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.

3. PERIODIC TABLES Just a way to organize things

11. Dmitri Mendeleev: Father of the Periodic Table pg 11 In 1869 Dmitri Mendeleev published the first periodic table. It had eight columns and it contained room for elements that Mendeleev predicted, although they had not yet been discovered. Moseley- Step Father of the Periodic Table It was not until 1914 that Henry Moseley corrected the periodic law, based on his discovery of the proton, he arranged elements by increasing atomic number.

12. Long Modern Periodic Table

13. MetalsNonmetalsMetalloids High electrical conductivity and a high luster when clean, malleable, ductile, metallic  Non-lustrous (not shiny), brittle and are poor conductors of electricity, takers forma negative charge  Have properties in common with both metals and nonmetals

14. What are the only 2 liquids on the Periodic Table? _____________

15. Families on the Periodic Table pg 12 Columns are also grouped into families. Families may be one column, or several columns put together. Families have names rather than numbers. (Just like your family has a common last name.) The vertical columns are called groups are labeled from 1 to 18. The horizontal rows are called periods and are labeled from 1 to 7.

16. Alkali Metals

17. Alkaline Earth Metals

18. TRANSITION METALS

20. Poor Metals/ Semi metals

21. Noble Gases

22. Alkali Metals 1 st column on the periodic table (Group 1) not including hydrogen. Very reactive with water, always combined with something else in nature (like in salt). Soft enough to cut with a butter knife Reacts with water to form Hydrogen Gas Used to make different kinds of glass

23. Hydrogen Hydrogen belongs to a family of its own. Hydrogen is a diatomic, reactive gas. Hydrogen was involved in the explosion of the Hindenberg. Hydrogen is promising as an alternative fuel source for automobiles

24. Alkaline Earth Metals Second column on the periodic table. (Group 2) Reactive metals that are always combined with nonmetals in nature. Several of these elements are important mineral nutrients (such as Mg & Ca) Used in batteries Used in Fireworks React with water

25. Transition Metals Elements in group B 3-12 Less reactive harder metals Includes metals used in jewelry and construction. Great electrical conductors

26. Halogens Non metals Elements in group 17 Very reactive, volatile, diatomic, nonmetals Always found combined with other element in nature. Used as disinfectants and to strengthen teeth. Bromine is the only liquid non metal

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

28. Pg 13 Periodic Law – The physical and chemical properties of the elements are periodic functions of their atomic numbers. Periodic Table – An arrangement of the elements in order of their atomic numbers so that elements with similar properties fall in the same group.

29. Properties in the periodic table Atomic radii Ionization energy Electronegativity Reactivity Melting point Boiling Point Distance between e- and nucleus. Energy to remove an e- How attractive an element is How likely an element is to act in response with another The point at which a solid melts The point at which it boils

31. Atomic Radius decreases going across the table. Atomic Radius increases going down the table. Additional sublevels make radius larger. Same sublevel filling. Larger charge in center (larger nucleus) pulls electrons in more.

32. Addition or subtraction of an electron dramatically effects atomic radius. Changes the balance of the electron interactions. Losing an electron makes the radius decrease. Gaining an electron makes the radius increase.

33. Ionization Energy is the energy necessary to knock off the outermost electron. Elements that hang onto their outer electrons more strongly (higher electrical attraction) have higher Ionization Energies. What trends do you see? How can they be explained?

35. Definition: The pull of an atom on a shared electron. Electrical Force of attraction depends upon: distance b/t charges size of charge So what would the largest force be caused by? What characteristics would the atom have?

36. Melting Point and Boiling Point