1. The Periodic Table

2. Dmitri Mendeleev (1834-1907) determined the properties of every known element at the time Atomic Mass Density Colour Melting Point Boiling Point

3. The Periodic Table Mendeleev arranged the known elements in order of increasing atomic mass He found that the properties of the elements repeated at definite, or PERIODIC, intervals Na has similar properties to Li and K

4. The Modern Periodic Table: Atomic Number In 1915, the Periodic Table was reorganized based on the element’s atomic structure Each element has an ATOMIC NUMBER, which is unique to each element The atomic number begins with H (1) in the upper-left hand corner, and increases as you move from left to right

5. The Modern Periodic Table: Groups of Elements 3 4 5 6 7 8 9 10 11 12 13 13 14 15 16 171415 1617 181 2

6. Periods Horizontal rows in the periodic table. Elements in the same PERIOD have the same number of electron ORBITS.

7. Groups Vertical columns in the periodic table Chemical families Elements in a group share very similar properties Numbered from 1-18 Elements in the same GROUP have the same number of VALENCE ELECTRONS (electrons in the outer shell) 1 2 3 4 5 6 7 8

8. Group 1: Alkali Metals Solids at room temperature Very reactive metals that do not occur freely in nature (Cs, Fr the most reactive) Valence Electrons: One; ready to lose that one electron to bond with other elements. Properties: Malleable, ductile, good conductors of heat and electricity, softer than most metals Can explode if exposed to water.

9. Group 2: Alkaline Earth Metals Solids at room temperature Very reactive Valence Electrons: 2; can bond easily with other elements by losing these electrons Not found free in nature

10. Groups 3-12: Transition Metals Solids at room temperature except for mercury which is a liquid. Properties: Ductile, malleable, conduct electricity and heat Valence Electrons: transfer electrons to nonmetals to form compounds; the number of electrons transferred can vary Iron, cobalt, and nickel are the only elements known to produce a magnetic field.

11. Groups 13-15 (Metals only) Solids at room temperature Properties: Ductile and malleable, high density, opaque

12. Metalloids Along the stair-step line that distinguishes metals from non- metals Properties: Similar to metals and non-metals, solids at room temperature Si and Ge are semi-conductors (can carry an electrical charge under special conditions; used in calculators and computers)

13. Group 14-16 (Nonmetals only) Exist as gases (N, O) or solids (C, S) Properties:Do not conduct electricity or heat very well, brittle, not malleable or ductile, dull, do not reflect light

14. Group 17: Halogens Exist as solids (I, At), liquid (Br), and gas (F, Cl) “Salt-former” because they are very reactive non-metals; form salts when they react with metals Valence Electrons: 7; will bond easily with Alkali Metals.

15. Group 18: Noble Gases Valence Electrons: full shell; prevents gases from forming compounds Very stable because they have the maximum electrons in their outer shell

16. Rare Earth Elements Lanthanide and Actinide series (Group 3 and Period 6-7) One element of the lanthanide series and most of the elements in the actinide series are trans-uranium (synthetic or man-made)

17. Mendeleev’s Periodic Law If the elements are arranged according to their atomic mass, a pattern can be seen in which similar properties occur regularly