Chemistry 11

1. Chemistry 11 “Wooot, yay, I love science”

2. “ Dmitri Ivanovich Mendeleev “ Certain characteristic properties of elements can be foretold from their atomic weights.– D.Mendeleev

3. The Periodic Table: Mendeleev - 1800’s -63 elements known -He recognized similarities in some of the elements -Decided to group them according to mass and noticed a pattern in their bonding power or valence. -When organized in this way the elements fell into columns which showed similar physical and chemical properties.

4. Your Turn To be a Scientist!! • Your job is to arrange the fake elements you have been given according to the patterns you see and the trends you can create.

5. Modern Periodic Table -When atomic numbers (number of protons in the nucleus) were discovered 50 years later the elements were arranged according to their atomic number. -The periodic law states: -other periods -calendars, music scales, periodicals.

6. Organization of the Periodic Table Rows- called -elements in a period are not alike in properties. -1st element is an extremely active solid whereas last element is a inactive gas ex. Columns - called - elements in the same family have similar properties ex. K, Na, Li are all soft, white, shiny metals. Element key-

7. Metals - 88 elements to left of zigzag line are called metals. Physical properties of metals: • luster/shininess • good conductors of heat and electricity • ductile-drawn into wires • malleable-hammered into thin sheets. Chemical properties of metals: • Tend to ex. rust/tarnish

8. Non-metals - right of the zigzag line. Physical properties: - - Chemical properties: -tend to exception: Noble gases

9. Metalloids • along both sides of the zigzag line are elements which have properties of both ex. B, Si, Ge, As, Sb, Te, Po, At

10. Periodic Table

11. Chemical Families Most Active Metals Alkali Metals - elements in with one valence electron in their outermost energy level. - very reactive and readily bonded with other substances. Ex. Alkaline Earth Metals- elements in with two valence electrons in their outermost energy level. - still very reactive but not as reactive as Family 1 cause they have two electrons to get rid of.

12. Chemical Families Transition Metals ( ) - have properties similar to one another and to other metals -have one or two valence electrons in their outer shell. -some have ability to an electron from their next to outermost energy level.

13. Chemical Families From Metals to Non-Metals - five families to the right contain properties of metals as well as non-metals. -named after the first element in the family. Ex. c

14. Chemical Families Halogens - have 7 valence electrons and are the most active of the non-metals. -react easily with alkali metals Ex. Noble Gases- , therefore normally unreactive.

15. Chemical Families Rare-Earth Elements - two rows appearing at the bottom of the periodic table: - lanthanoid series - soft malleable metals, high luster. - actinoid series - radioactive, most made in lab.

16. Electron Configuration • The outer most electrons of an atom determines its . • These outer electrons are called . • Elements in the same family/group have similar properties because they have similar valence electron configurations. • Ex. Li=1s2 2s1 Na= K=1s2s 2s2 2p6 3s2 3p6 4s1