1. The Periodic Table

2. A. Dmitri Mendeleev. a. In 1869 arranged elements in order
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
Alkali Metals
Alkaline Earth 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 Alkali Metals H Alkaline Earth 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 Alkali Metals H Alkaline Earth 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 Alkali Metals H Alkaline Earth Metals Carbon Family
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 Alkali Metals H Nitrogen Family
Boron Family
Alkali Metals
Alkaline Earth Metals
Carbon Family
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 Alkali Metals H Nitrogen Family
Oxygen Family
Boron Family
Alkali Metals
Alkaline Earth Metals
Carbon Family
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 Alkali Metals H Nitrogen Family
Oxygen Family
Halogens
Boron Family
Alkali Metals
Alkaline Earth Metals
Carbon Family
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 Alkali Metals
Non-Metals
Halogens
Noble Gases
Alkali Metals
Alkaline Earth 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-patterns within 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