1. The Periodic Table

2. Why is the Periodic Table important to me? Its a useful tool You can use it on your tests. It organizes lots of data about elements. It lets you predict what type of bonds will form It lets you predict what type of ion will form

3. Dmitri Mendeleev

4. Dimitri Mendeleev (1869) Chemistry Professor Wrote the first Chemistry Book While organizing elements into chapters… Saw patterns in their chemical properties that matched their physical properties Used these paterns to create the Periodic Table of elements (56 of them at the time)

5. Mendeleev’s Periodic Law "the physical and chemical properties of the elements are periodic function of their atomic masses". Periodic = repeating Saw repeating patterns if elements were lined up by atomic mass

6. Mendeleev’s Table He put the elements in order of atomic mass When the patterns began to repeat he started a new row. Elements in each column had similar properties. He had to leave some blanks…said that undiscovered elements went there

7. SOME PROBLEMS… He broke the pattern of increasing atomic weight to keep similar reacting elements together. Not all elements seemed to fit his pattern

8. The Current Periodic Table Mendeleev wasn’t too far off. Now the elements are put in rows by increasing ATOMIC NUMBER!! The horizontal rows are called periods and are labeled from 1 to 7. The vertical columns are called groups are labeled from 1 to 18.

9. General Areas & Their Properties Metals Nonmetals Metalloids

10. Metals Shiny Malleable Ductile good conductors high melting points and boiling points usually solids

11. Nonmetals Not shiny Nonmalleable Not ductile Poor conductors Low melting and boiling points

12. Metalloids Elements that are not metals or nonmetals but have a mixture of both properties

13. Groups … Here ’ s Where the Periodic Table Gets Useful!! Elements in the same group have similar chemical and physical properties!! Why?? They have the same number of valence electrons. They will form the same kinds of ions.

14. Families on the Periodic Table 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.)

15. Families

16. Hydrogen Hydrogen is its own family it is a diatomic, reactive gas Reacts quickly because it only needs to lose 1 electron to have a full outer shell Hydrogen caused the Hindenberg to explode Hydrogen is promising as an alternative fuel source for automobiles

17. 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). React quickly bcs only need to lose 1 e- Soft enough to cut with a butter knife

18. Alkaline Earth Metals Second column on the periodic table. (Group 2) Reactive metals that are always combined with nonmetals in nature (react quickly - only need to lose 2 e-) important mineral nutrients Mg and Ca

19. Transition Metals Elements in groups 3-12 Less reactive harder metals used in jewelry and construction Metals used “as metal.” Have more than one oxidation # Lanthanide and Actinide Series are very radioactive!

20. Halogens Elements in group 17 Very reactive nonmetals (need to gain 1e-) Attract electrons VERY strongly Always combined with other element in nature. Diatomic = atoms come in pairs never alone Used as disinfectants and to strengthen teeth. Teflon = F bonded to C

21. The Noble Gases Elements in group 18 VERY un-reactive (inert) Used in lighted “neon” signs Used in blimps to fix the Hindenberg problem. Have a full outer electron shell so don’t need to react to get full outer shell

22. Ionization Energy vs Electronegativity How much energy it takes to remove outermost electron Further away from nucleus makes less force of attraction so Lower ionization energy How hard the protons in the nucleus pull on electrons Decreases as you get farther from the nucleus Coulombs Law says… Force of attraction = Charge e- * charge P distance 2

23. Atomic Radius Distance from the center of the nucleus to the outermost edge of the electron cloud

24. Periodic Trends Trends repeat along each row –This is called periodicity: repeating in cycles –Each horizontal row is called a period Trends : 1) Atomic Radius decreases 2) ionization energy & electronegativity increase

25. Atomic Radius- Period Trends from left -right across period, size gets smaller. Electrons in same energy level. But, more nuclear protons as you move right. electrons pulled closer. NaMgAl Si PSClAr

26. Atomic Radius- Group trends As go down a group)... each atom adds an energy level, so atoms get bigger. H Li Na K Rb

27. The arrows indicate the trend: Ionization energy and Electronegativity INCREASE in these directions