The Periodic Table

1. The Periodic Table

2. A. Dmitri Mendeleev a. In 1869 arranged elements in order of increasing atomic mass b. He left vacant spaces in his table where unknown elements could fit Dmitri Mendeleev was so confident in his table that he used it to predict the physical properties of three elements that were yet unknown-Sc, Ga and Ge-which were later discovered between 1874 and 1885 .

3. B. Geography of the Modern Table • 7 periods (rows)-Row number indicates the number of energy levels an atom has • Groups or Families (A Groups)-Column # indicates # of valence (outside/bonding) electrons ( those with 8 don’t bond-more later) • elements with similar properties (also called representative elements) are placed in these groups and these groups have names

4. Hydrogen • Hydrogen belongs to a family of its own. • 1 valance electron • 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

5. The Periodic Table H

6. Alkali Metals-Group 1A • 1 valence electron • Very reactive metals, always combined with something else in nature (like in salt). • Soft enough to cut with a butter knife

7. The Periodic Table H Alkali Metals

8. Alkaline Earth Metals-Group 2A • 2 valence electrons • Reactive metals that are always combined with nonmetals in nature. • Several of these elements are important mineral nutrients (such as Mg and Ca

9. The Periodic Table H Alkaline Earth Metals Alkali Metals

10. Transition Metals-B Groups • Elements in groups 3-12 • Valence electrons vary • Less reactive harder metals • Includes metals used in jewelry and construction. • Metals used “as metal.”

11. The Periodic Table H Alkaline Earth Metals Alkali Metals Transition Metals

12. Boron Family-Group 3A • 3 valence electrons • Elements in group 13 • Aluminum metal was once rare and expensive, not a “disposable metal.”

13. The Periodic Table H Alkaline Earth Metals Alkali Metals Boron Family Transition Metals

14. Carbon Family-Group 4A • 4 valence electrons • Contains elements important to life and computers. • CARBON is found in ALL living things • Carbon is the basis for an entire branch of chemistry. • Silicon and Germanium are important semiconductors.

15. The Periodic Table H Alkaline Earth Metals Alkali Metals Boron Family Carbon Family Transition Metals

16. Nitrogen Family-Group 5A • 5 valence electrons • 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 so it is “fixed” by special bacteria in the roots of plants (peanuts too!). • The red stuff on the tip of matches is phosphorus.

17. The Periodic Table H Nitrogen Family Boron Family Carbon Family Alkaline Earth Metals Alkali Metals Transition Metals

18. Oxygen Family(Chalcogens)-Group 6A • 6 valence electrons • Oxygen is necessary for respiration. • Many things that stink, contain sulfur (rotten eggs, garlic, skunks,etc.)

19. The Periodic Table H Nitrogen Family Oxygen Family Boron Family Carbon Family Alkaline Earth Metals Alkali Metals Transition Metals

20. Halogens-Group 7A • 7 Valence electrons • Very reactive, volatile, diatomic, nonmetals • Always found combined with other element in nature . • Used to make salts, disinfectants and to strengthen teeth.

21. The Periodic Table H Nitrogen Family Oxygen Family Halogens Boron Family Carbon Family Alkaline Earth Metals Alkali Metals Transition Metals

22. The Noble Gases-Group 8A • 8 valence electrons so they have a full outer energy shell. • VERY unreactive, • Used in lighted “neon” signs • Used in blimps to fix the Hindenberg problem.

23. The Periodic Table H Non-Metals Noble Gases Halogens Alkaline Earth Metals Alkali Metals Transition Metals Metals Lanthanide Series Actinide Series Lanthanides and actinides are also called the “Rare Earth elements. Actinides are radioactive.

24. 3. Periodic Law-patternswithin the table as we move left to right and top to bottom • Atomic Number (number of protons) increases from left to right across a period. • Atomic mass (number of p+ and n) increases from left to right across a period. • Density increase from top to bottom and left to right as we add more atom particles • Metals on the left-nonmetals on the right

26. Properties of Metals • Metals are good conductors of heat and electricity • Metals are malleable (can be molded) • Metals are ductile (can be drawn into a wire) • Metals have high tensile strength • Metals have luster (shine)

27. Properties of Metalloids Metalloids straddle the border between metals and nonmetals on the periodic table. • They have properties of both metals and nonmetals.

28. NON-METALS • Opposite properties to metals • very brittle • exist in two of the three states of matter at room temperature: most are gases [such as oxygen (diatomic-O2) and a few solids (such as carbon).

29. Examples of Nonmetals Microspheres of phosphorus, P, a reactive nonmetal Sulfur, S, was once known as “brimstone” Graphite is not the only pure form of carbon, C. Diamond is also carbon; the color comes from impurities caught within the crystal structure