1. The Periodic Table

2. 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.

3. 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.

4. 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.

5. 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.)

6. Hydrogen Hydrogen belongs to a family of its own. Hydrogen is a diatomic, reactive gas. Never found as a ‘free’ elelment in nature. Only one valence electron, becomes a +1 ion Hydrogen was involved in the explosion of the Hindenberg. Hydrogen is promising as an alternative fuel source for automobiles

7. Alkali Metals 1 st column on the periodic table (Group 1) not including hydrogen. Never found as a ‘free’ elelment in nature. Only one valence electron, becomes a +1 ion Most reactive of all metals, always combines with something else in nature (like in salt). Soft enough to cut with a butter knife

8. Alkaline Earth Metals Second column on the periodic table. (Group 2) Reactive metals that are always combined with nonmetals in nature. 2 valence electrons, becomes a +2 ion Several of these elements are important mineral nutrients (such as Mg and Ca High melting and boiling points

9. Transition Metals Elements in groups 3-12 Less reactive harder metals, some are brittle Good conductors of heat and electricity Includes metals used in jewelry and construction. Metals used “as metal.” May react with O 2 to form oxides (rust)

10. Boron Family Elements in Group 13 3 valence electrons, becomes a +3 ion Aluminum metal was once rare and expensive, not a “disposable metal.”

11. Carbon Family Elements in Group 14 4 valence electrons, becomes + or – 4 ion Contains elements important to life and computers. Carbon is the basis for an entire branch of chemistry. Silicon and Germanium are important semiconductors.

12. Nitrogen Family Elements in Group 15 5 valence electrons, becomes -3 ion 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.

13. Oxygen Family Elements in Group 16 6 valence electrons, becomes -2 ion Oxygen is necessary for respiration. Many things that stink, contain sulfur (rotten eggs, garlic, skunks,etc.)

14. Halogens Elements in Group 17 7 valence electrons,, becomes -1 ion Very reactive, volatile, diatomic, nonmetals Always found combined with other element in nature. Combine with metals to form compounds called “salts” Used as disinfectants and to strengthen teeth.

15. The Noble Gases

16. Elements in Group 18 Full valence electron shells Extremely unreactive = INERT Colorful, monatomic gases Used in lighted “neon” signs Used in blimps to fix the Hindenberg problem.

17. Rare Earth Elements 2 rows at the bottom of the periodic table Extremely similar to each other Lanthanoid Series = soft malleable metals with high luster and conductivity Actinoid Series = radioactive; almost all are synthetic Thorium and Uranium are the only 2 that occur in nature

18. Metals, NonMetals, & Metaloids Metals – found to the left of the “stair step” with the exception of Hydrogen; 80% of elements are metals. These elements conductors of heat and electricity, ductile (can be drawn into wires), and malleable (can be hammered into thin sheets)

19. NonMetals Nonmetals – found to the right of the “stair step” These elements are POOR conductors of heat and electricity (except carbon), and tend to be brittle, meaning they will shatter if hit with a hammer.

20. Metalloids Metalloids (Semimetals) – touch the “stair step” with the exception of Aluminum. These elements have properties of both metal and nonmetals. Metalloids only conduct electricity under certain conditions, which make them useful in the semi- conductors industry.

21. Alloys Very few metals that you encounter daily are pure metals. Most metals are alloys, a mixture of two or more elements of which at least one is a metal. –Examples: Brass is an alloy of copper and zinc Sterling silver is an alloy of silver (92%) and copper (8%) Stainless Steel is an alloy of iron (81%), chromium (18%), nickel (1%), and trace amounts of carbon. Alloys are important because their properties are often superior to those of their component elements. –Examples: Sterling silver is harder and more durable than pure silver, but still soft enough to make jewelry and tableware. Brass is harder and easier to shape than either copper or zinc