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T h e P e r i o d i c T a b l e

T h e P e r i o d i c T a b l e. T h e P e r i o d i c T a b l e. M o s t o f w h a t y o u n e e d i s o n i t. T h e P e r i o d i c T a b l e. T h e e l e m e n t s o n t h e t a b l e a r e a r r a n g e d

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T h e P e r i o d i c T a b l e

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  1. T h e P e r i o d i c T a b l e

  2. T h e P e r i o d i c T a b l e M o s t o f w h a t y o u n e e d i s o n i t

  3. T h e P e r i o d i c T a b l e T h e e l e m e n t s o n t h e t a b l e a r e a r r a n g e d a c c o r d i n g t o i n c r e a s i n g A t o m i c N u m b e r

  4. Main Parts • Periods – Horizontal Rows • No Characteristics in common • Groups – Vertical columns • Same numbers of valence (outer shell) electrons • Characteristics similar in chemical activity

  5. D e v e l o p m e n t o f t h e T a b l e • W h a t w a s t h e t a b l e l i k e b e f o r e D e m e t r i M e n d e l e e v ? • W h a t d i d h e d o t o i m p r o v e i t ? • H a s i t c h a n g e d s i n c e M e n d e l e v e ?

  6. C h e m i c a l S y m b o l s A p e r i o d i c t a b l e i s a l w a y s a v a i l a b l e t o y o u . T o b e s u c c e s s f u l i n c h e m i s t r y , y o u M u s t k n o w h o w t o r e a d t h e i n f o r m a t i o n o n t h e t a b l e .

  7. C h e m i c a l s y m b o l A t o m i c n u m b e r M a s s n u m b e r P r o t o n s i n a t o m E l e c t r o n s i n a t o m N e u t r o n s i n a t o m M e t a l / N o n m e t a l C h e m i c a l a c t i v i t y O x i d a t i o n n u m b e r E n e r g y l e v e l s E l e c t r o n c o n f i g u r a t i o n C h e m i c a l F a m i l i e s N a t u r a l / M a n m a d e P h y s i c a l s t a t e a t r o o m t e m p e r a t u r e I n f o r m a t i o n o n t h e P e r i o d i c T a b l e

  8. M e t a l s i n c r e a s e N o n m e t a l s i n c r e a s e N o b l e g a s e s d o n o t r e a c t C h e m i c a l A c t i v i t y

  9. +1 0 +2 +3 4 -3 -2 -1 M o s t a r e +1 o r +2 O x i d a t i o n N u m b e r

  10. s p 1 He 2 3 d 3 4 5 6 7 4 f E n e r g y l e v e l s a n d s u b l e v e l s

  11. Metals • Are Ductile (able to be made into wires) • Malleable (able to be pounded into other shapes) • Shiny • Conductors of heat and electricity.

  12. Non-Metals • Found on the far right of the periodic table. • Are Brittle, dull • Do not conduct heat or electricity • Are not malleable or ductile • Many are gases, not solids • Tend to accept electrons in order to form chemical bonds.

  13. Metalloids • Located in a “staircase” on the right side of the periodic table. • Have characteristics of both metals and non-metals.

  14. A l k a l i M e t a l s • 1 e l e c t r o n i n t h e i r o u t e r e n e r g y l e v e l . • R e a c t w i t h w a t e r t o f o r m a b a s e . • T h e m o s t r e a c t i v e o f a l l m e t a l s .

  15. A l k a l i n e E a r t h M e t a l s • 2 e l e c t r o n s i n t h e i r o u t e r e n e r g y l e v e l . • Basically the same properties as the Alkali Metals, but to a lesser degree

  16. T r a n s i t i o n M e t a l s • 2 e l e c t r o n s i n o u t e r l e v e l . • M o r e t h a n o n e o x i d a t i o n n u m b e r . • C o m b i n e w i t h o x y g e n t o f o r m o x i d e s . • F o r m c o m p o u n d s t h a t a r e b r i g h t l y c o l o r e d .

  17. R a r e - E a r t h E l e m e n t s • 2 e l e c t r o n s i n o u t e r l e v e l . • P r i m a r y o x i d a t i o n n u m b e r + 3 . • L a n t h a n o i d S e r i e s - elements #57-71 • S o f t , m a l l e a b l e m e t a l s w i t h a h i g h l u s t e r a n d c o n d u c t i v i t y . • A c t i n o i d S e r i e s - elements #89-103 • A l l t h e s e m e t a l s a r e r a d i o a c t i v e .

  18. B o r o n F a m i l y • 3 e l e c t r o n s i n t h e i r o u t e r e n e r g y l e v e l . • A l u m i n u m i s t h e m o s t a b u n d a n t m e t a l a n d t h e t h i r d m o s t a b u n d a n t e l e m e n t i n t h e E a r t h ’ s c r u s t .

  19. C a r b o n F a m i l y • 4 e l e c t r o n s i n t h e i r o u t e r e n e r g y l e v e l . • S i l i c o n i s t h e s e c o n d m o s t a b u n d a n t e l e m e n t i n t h e E a r t h ’ s c r u s t .

  20. N i t r o g e n F a m i l y • 5 e l e c t r o n s i n t h e i r o u t e r e n e r g y l e v e l . • N i t r o g e n i s t h e m o s t a b u n d a n t e l e m e n t i n t h e E a r t h ’ s a t m o s p h e r e .

  21. O x y g e n F a m i l y • 6 e l e c t r o n s i n t h e i r o u t e r e n e r g y l e v e l . • O x y g e n i s t h e m o s t a b u n d a n t e l e m e n t i n t h e E a r t h ’ s c r u s t . • O x y g e n s u p p o r t s c o m b u s t i o n .

  22. H a l o g e n F a m i l y • 7 e l e c t r o n s i n t h e i r o u t e r e n e r g y l e v e l . • H a l o g e n s e a s i l y c o m b i n e w i t h m e t a l s t o f o r m S a l t s . • M o s t r e a c t i v e o f a l l n o n m e t a l s .

  23. N o b l e G a s e s • 8 e l e c t r o n s i n o u t e r l e v e l . • T h e i r e l e c t r o n a r r a n g e m e n t m a k e s t h e m v e r y i n a c t i v e , ” i n e r t ” . • A l l a r e c o l o r l e s s g a s e s . • A r g o n i s t h e m o s t a b u n d a n t , m a k i n g u p 1 % o f t h e a t m o s p h e r e .

  24. Periodic Trends Chemistry

  25. Atomic Radii Periodic Trend (across the row) Atoms get smaller b/c of the increasing positive charge of the nucleus that pulls the electrons closer Group Trend (down the column) Increases as you go down a column b/c energy levels get filled Figure 5-14 pg 142

  26. Ionization Energy Symbol: IE unit: kj/mol Period Trend: Increases; more valence electrons to remove = higher IE Group Trend: Decreases down the group b/c further from the nucleus Each IE is greater than the previous b/c stronger nuclear attraction

  27. Electron Affinity The energy change that occurs when an electron is acquired by a neutral atom Period Trend: Increases as you go across; neg EA indicates that energy is released Group Trend: Generally more difficult to add electrons to elements at the bottom of a group, but many exceptions

  28. Ionic Radii Cation- positive ion; metals; formation causes a decrease in radii b/c of a smaller electron cloud Anion- negative ion; nonmetals; increase in radii Period Trend: Cationic decr; anionic decr Group Trend: Gradual increase just like in atomic radii

  29. Valence Electrons Electrons in the outer shell (valence shell) that from compounds with other atoms Determined by the last digit of the family number, except for the transition metals

  30. Electronegativity The measure of the ability of an atom n a chemical compound to attract electrons F is the most EN, so it is assigned the value of 4, and all others are compared to it Period Trend: Tend to increase across, with exceptions Group Trend: Tend to decrease down a group or stay about the same

  31. d and f block Atomic Radii: Decr across periods, but less than metals Ionization Energy: Generally incr across periods and down groups Ion Formation and Radii: Electrons are removed in the opposite order of the electron configuration; electrons are removed from highest energy level first Most d block form 2+ ions but multiples are possible Generally a decrease in size and radii Electronegativity Follows same trend that EN values increase as radii decrease

  32. E n d P e r i o d i c T a b l e

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