The Periodic Table

1. The Periodic Table Chapter 5

2. Why is the Periodic Table important to me? • The periodic table is the most useful tool to a chemist.. • It organizes lots of information about all the known elements.

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 In 1869 he published a table of the elements organized by increasing atomic mass. 1834 - 1907

5. HOW HIS WORKED… Put elements in rows by increasing atomic weight. Put elements in columns by the way they reacted. SOME PROBLEMS… He left blank spaces for what he said were undiscovered elements. (Turned out he was right!) He broke the pattern of increasing atomic weight to keep similar reacting elements together. Dmitri Mendeleev: Father of the Table

6. Elements known at this time

7. 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.

8. Periodic Table Geography

9. Periodic Law Overall arrangement is by atomic mass

10. Metals, Nonmetals, & Metalloids

11. The horizontal rows of the periodic table are called PERIODS.

12. The elements in any group of the periodic table have similar physical and chemical properties! The vertical columns of the periodic table are called GROUPS, or FAMILIES.

13. 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.)

14. Groups…Here’s Where the Periodic Table Gets Useful!! • Elements in the same group have similar chemical and physical properties!! • (Mendeleev did that on purpose.) • Why?? • They have the same number of valence electrons. • They will form the same kinds of ions.

15. Alkali Metals

16. Alkaline Earth Metals

17. Transition Metals

18. These elements are also called the rare-earth elements. InnerTransition Metals

19. Halogens

20. Noble Gases

21. 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

22. Alkali Metals • 1st 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

23. 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 and Ca

24. Transition Metals • Elements in groups 3-12 • Less reactive harder metals • Includes metals used in jewelry and construction. • Metals used “as metal.”

25. Boron Family • Elements in group 13 (III) • Boron used in glass to help with shattering • Aluminum metal was once rare and expensive, not a “disposable metal.”

26. Carbon Family • Elements in group 14 (IV) • Contains elements important to life and computers. • Carbon is the basis for an entire branch of chemistry. • Silicon and Germanium are important semiconductors.

27. Nitrogen Family • Elements in group 15 (V) • Nitrogen makes up over ¾ of the 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.

28. Oxygen Family or Chalcogens • Elements in group 16 (VI) • Oxygen is necessary for respiration. • Oxygen is the most abundant element in humans and in Earth’s crust • Many things that stink, contain sulfur (rotten eggs, garlic, skunks,etc.)

29. Halogens • Elements in group 17 (VII) • Very reactive, volatile, diatomic, nonmetals • Always found combined with other element in nature . • Used as disinfectants and to strengthen teeth. • Solid, liquid, and gases

31. A Lack of iodine in ones diet can lead to a goiter. Iodine is necessary for your thyroid gland to function properly

32. The Noble Gases

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

34. Why is Helium used in SCUBA tanks? • Helium is used in scuba tanks to dilute oxygen.  Why helium?  First, it is chemically inert.  Second, helium is much less soluble in water than many other gases, such as nitrogen.  The low solubility means it does not enter the blood stream, even under pressures commonly experienced by deep sea divers. Oxygen is essential for breathing, above and beneath the surface.  However, one can get too much of it.  Under high pressures, greater amounts of oxygen enter into the bloodstream.  If the concentration becomes too high, oxygen poisoning can result, with symptoms that include confusion, impaired vision and nausea.  So, under high pressures, oxygen must be diluted with some other gas.

35. Radon Gas

36. How do neon lights work? • Most gases are conductive • But most burn out fast • Noble gases last • Electric current causes a jump in the electrons to a higher orbital • When electron moves back into its stable orbital it gives off photon energy in a visible wavelength

38. Glenn T. Seaborg He is the only person to have an element named after him while still alive. "This is the greatest honor ever bestowed upon me - even better, I think, thanwinning the Nobel Prize." 1912 - 1999