1. Families on the Periodic Table

2. In 1860 at a conference of chemists in Karlsruhe, Germany, Italian chemist Stanislao Cannizzaro proposed: … and the chemists agreed.

3. February 8,1834- February 2,1907 (aged 72) In 1869 Russian Chemist Dmitri Mendeleev proposed a periodic Table

4. Periodic Occurring or recurring at regular intervals

7. English Physicist Henry Moseley (1887-1915 KIA WWI) In 1911 Henry Moseley noticed: And so we did.

8. And we lived happily ever after?

9. Important People Dmitri Mendeleev - published 1 st periodic table in 1869 - arranged elements by atomic mass Henry Moseley - arranged the periodic table for today - arranged elements by atomic number

10. Review of periodic trends Atomic radius (size of the atom) Atomic radius (size of the atom) - Generally increases as you move down a group. Electron clouds are added. - Generally decreases as you move from left to right across a period. More electrons in outer shell  more negative charge  more attraction to nucleus  smaller radius!

11. Electronegativity The desire for electrons. The desire for electrons. The tendency for the atoms of the element to attract electrons when they are chemically combined with another element. The tendency for the atoms of the element to attract electrons when they are chemically combined with another element. Fluorine is the MOST electronegative element. Fluorine is the MOST electronegative element. Generally decreases as you move down a group. Generally decreases as you move down a group. Generally increases as you move left to right across a period. Generally increases as you move left to right across a period.

12. Ionization Energy The energy needed to remove an electron The energy needed to remove an electron Energy required to overcome the attraction of the nuclear charge and remove an electron from an atom. Energy required to overcome the attraction of the nuclear charge and remove an electron from an atom. Generally decreases as you move down a group. Generally decreases as you move down a group. Generally increases as you move left to right across a period. Generally increases as you move left to right across a period.

13. Periodic Law There is a repeating, predictable, pattern of physical and chemical properties of the elements. There is a repeating, predictable, pattern of physical and chemical properties of the elements. You witnessed this with atomic radius, ionization energy, electronegativity. You witnessed this with atomic radius, ionization energy, electronegativity.

14. How are the elements organized? Atoms with similar outer-shell electron configurations have similar chemical properties. Atoms with similar outer-shell electron configurations have similar chemical properties. Outer shell = valence shell (outside electrons) Outer shell = valence shell (outside electrons) Valence electrons determine reactivity and how strongly an atom will bond with other atoms. Valence electrons determine reactivity and how strongly an atom will bond with other atoms.

15. Metals To the left of the Zigzag To the left of the Zigzag Malleable (smashed into thin sheets) Malleable (smashed into thin sheets) Ductile (stretched into wires) Ductile (stretched into wires) Conduct heat and electricity Conduct heat and electricity Shiny Shiny Reactive Reactive Mostly Solids at room temperature Mostly Solids at room temperature - except Hg (liquid) - except Hg (liquid)

16. Metals

17. Malleable

18. Ductile

19. Non-metals Right of the zigzag (Upper right side) Right of the zigzag (Upper right side) Poor conductor of electricity Poor conductor of electricity Dull Dull Brittle Brittle Mostly gases at room temperature Mostly gases at room temperature - Liquid (Bromine) - Solids (Sulfur, Phosphorus, Carbon)

20. Metalloids Along the zigzag line! (EXCEPT  Al) Along the zigzag line! (EXCEPT  Al) Has properties of both metals AND nonmetals! Has properties of both metals AND nonmetals! Somewhat shiny solids, not much luster Somewhat shiny solids, not much luster Most conduct heat and electricity Most conduct heat and electricity Boron, Silicon, Germanium, Arsenic, Antimony, Tellurium Boron, Silicon, Germanium, Arsenic, Antimony, Tellurium

21. Alkali Metals Group 1: Li, Na, K, Rb, Cs, Fr Group 1: Li, Na, K, Rb, Cs, Fr Alkali because they react with water to form alkaline solutions Alkali because they react with water to form alkaline solutions VERY reactive VERY reactive 1 electron in outer shell 1 electron in outer shell Positively charged ions (+1) Positively charged ions (+1) Combine easily with other elements Combine easily with other elements Form salts when combined Form salts when combined Soft, low densities, and melt at LOW temp. Soft, low densities, and melt at LOW temp.

22. Alkaline Earth Metals Group 2: Be, Mg, Ca, Sr, Ba, Ra Group 2: Be, Mg, Ca, Sr, Ba, Ra Reactive, but not as reactive as group 1 Reactive, but not as reactive as group 1 2 electrons in outer shell (+2) 2 electrons in outer shell (+2)

23. Transition Metals In the middle In the middle Shiny Shiny High melting points High melting points Good conductors of electricity Good conductors of electricity Much LESS reactive Much LESS reactive Often found in ores (minerals containing relatively large amounts of metal compounds) Often found in ores (minerals containing relatively large amounts of metal compounds)

25. Metalloids!!! Along the zigzag line! Has properties of both metals AND nonmetals! Somewhat shiny solids, not much luster Most conduct heat and electricity Boron, Silicon, Germanium, Arsenic, Antimony, Tellurium

26. Halogens Group 7: F, Cl, Br, I, At Group 7: F, Cl, Br, I, At Fluorine is the most reactive non-metal. Fluorine is the most reactive non-metal. Bromine is only non-metal LIQUID at room temperature. Bromine is only non-metal LIQUID at room temperature. Halogen is derived from the Greek word meaning “salt former”. Halogen is derived from the Greek word meaning “salt former”. 7 electrons in the outer most shell, they want one more to get 8 so they form -1 ions. 7 electrons in the outer most shell, they want one more to get 8 so they form -1 ions.

27. Noble Gases Group 8: He, Ne, Ar, Kr, Xe, Rn Group 8: He, Ne, Ar, Kr, Xe, Rn Don’t react or combine with anyone! (Unless forced) INERT GASES Don’t react or combine with anyone! (Unless forced) INERT GASES They are happy the way they are They are happy the way they are 8 electrons in outer shell 8 electrons in outer shell Do not form ions. Do not form ions. Exist in earth’s atmosphere Exist in earth’s atmosphere Neon is used to illuminate signs Neon is used to illuminate signs He in balloons He in balloons Xe in headlights Xe in headlights

28. Inner Transition Metals Rare Earth Metals Rare Earth Metals - Located in 2 separate rows at bottom of periodic table - Silver, silvery-white, or gray metals. - High electrical conductivity. - Naturally occur together in minerals. - High luster, tarnish readily in air.

29. Lanthanide Series Elements 58-71 Elements 58-71 - All occur in nature except 61 High melting and boiling points High melting and boiling points Very reactive Very reactive Used in lamps, lasers, magnets, and motion picture projectors. Used in lamps, lasers, magnets, and motion picture projectors.

30. Actinides Elements 90-103 Elements 90-103 Found in ores Found in ores Most are synthetic (man-made) Most are synthetic (man-made) Radioactive Radioactive Some are not found in nature Some are not found in nature Los Alamos Periodic Table Los Alamos Periodic Table Los Alamos Periodic Table Los Alamos Periodic Table

32. Packet Page 53 & 54 Define first four terms Define first four terms Neatly identify the ten items indicated. Neatly identify the ten items indicated. Yes, you can use color or in some other creative manner accomplish the same goal Yes, you can use color or in some other creative manner accomplish the same goal H.W. if not finished in class H.W. if not finished in class Due tomorrow! Due tomorrow!