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Periodic Table

Periodic Table. Chapter 5. Like always, start at the beginning. Until 1750, we only had 17 elements discovered 1789- Antoine Lavoisier Grouped by metals, non-metals, gas, earth 1860’s- Dmitri Mendeleev. The very scientific process of Mendeleev.

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Periodic Table

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  1. Periodic Table Chapter 5

  2. Like always, start at the beginning • Until 1750, we only had 17 elements discovered • 1789- Antoine Lavoisier • Grouped by metals, non-metals, gas, earth • 1860’s- Dmitri Mendeleev

  3. The very scientific process of Mendeleev • He was a teacher, and wanted to find a better way to describe the elements • Designed a periodic table in which elements were arranged in order of increasing atomic mass • Periodic -means repeating pattern

  4. The Arrangement • Element’s Name • Mass • Properties: • How they reacted with Oxygen/Hydrogen • What do the symbols mean and numbers?

  5. The Final Arrangement • Columns: by properties • Rows: by mass • Periodic Table: • An arrangement of elements in columns, based on a set of properties that repeat from row to row

  6. How Mendeleev did it? • He could not have a complete chart • Why? • He had blanks, where he knew there had to be something there but did not known what

  7. Early Bird doesn’t always get the worm • He was not the first to create a periodic table or leave blanks in a table • He did have the best explanation for it • Why was it the best? • It was able to be used to make predictions • People had to fill in those blanks! • Ex: Eka-aluminum and Gallium • What does this mean?

  8. Out with the old… • Mendeleev developed his table without knowing there were protons… • From what we studied before why would this have been important? • Today’s periodic table is arranged by atomic number!

  9. Periods and Groups • Periods (Go from 1 to 7) • Rows of the periodic table (horizontal)(L-R) • Groups • Each column (up-down) on the table • The elements within a group have similar properties but not identical • The repeating pattern of chemical and physical properties when atomic number is used to arrange is the periodic law.

  10. Four pieces of information on the Periodic Table • Atomic number • Element Symbol • Element Name • Atomic Mass: • Value depends on average mass of the isotopes and their distribution in nature

  11. Atomic Mass • Depends on the average of isotopes of an element. • Example: The AM of chlorine is 35.453. • How was this determined? • How many isotopes does chlorine have? • Chlorine -35 and Chlorine -37. • Chlorine -35 is 75.78% • Chlorine -37 is 24.22% • The average of these percents is 35.453.

  12. Atomic Mass Unit • The unit assigned to the mass of an element • Too small to use grams since anything we measure contains 1000’s to 1,000,000s of atoms • Atomic Mass Unit (AMU)- based on 1/12th of a carbon atom

  13. How to classify elements • Solids, liquids, gases • Natural and Synthetic • Natural: Forms in nature • Synthetic: Man-made element • Properties: Metals, Nonmetals, metalloids

  14. Metals • Majority of elements on table • Good conductors of heat/electricity • Most are solid at room temp. • Mercury (Hg) • Most are malleable (hammered) and ductile (can be formed into wire) • Some react, some don’t

  15. Transitional Metals • Still classified as metals but have even more special properties • Noticeable property: They make very distinctive colors • More on these next chapter…

  16. Nonmetals • Properties are opposite of metals • Poor conductors • Most are gases at room temp. • If solid, they are very brittle (fragile) • Extremely reactive

  17. Metalloids • The elements in between metals and nonmetals • Ex: They can be conductive at the right temperatures • Silicon: Used in Computer Chips

  18. Trendy Elements • Elements to the left of the dark line are Metals • Elements to the right of the dark line are Nonmetals • As you go from left to right you go from highest metallic properties to more nonmetallic properties

  19. Metals, Nonmetals, & Metalloids 1 Nonmetals 2 3 4 Metals 5 6 7 Metalloids Zumdahl, Zumdahl, DeCoste, World of Chemistry2002, page 349

  20. Uun 110 Uuu 111 Uub 112 Uuq 113 Uuh 116 Uuo 118 Noble gases The Periodic Table Alkaline earth metals Halogens 1 18 H 1 He 2 2 13 14 15 16 17 Li 3 Be 4 B 5 C 6 N 7 O 8 F 9 Ne 10 3 4 5 6 7 8 9 10 11 12 Na 11 Mg 12 Al 13 Si 14 P 15 S 16 Cl 17 Ar 18 Transition metals K 19 Ca 20 Sc 21 Ti 22 V 23 Cr 24 Mn 25 Fe 26 Co 27 Ni 28 Cu 29 Zn 30 Ga 31 Ge 32 As 33 Se 34 Br 35 Kr 36 Alkali metals Rb 37 Sr 38 Y 39 Zr 40 Nb 41 Mo 42 Tc 43 Ru 44 Rh 45 Pd 46 Ag 47 Cd 48 In 49 Sn 50 Sb 51 Te 52 I 53 Xe 54 Cs 55 Ba 56 * Hf 72 Ta 73 W 74 Re 75 Os 76 Ir 77 Pt 78 Au 79 Hg 80 Tl 81 Pb 82 Bi 83 Po 84 At 85 Rn 86 Fr 87 Ra 88 Y Rf 104 Db 105 Sg 106 Bh 107 Hs 108 Mt 109 * Lanthanides La 57 Ce 58 Pr 59 Nd 60 Pm 61 Sm 62 Eu 63 Gd 64 Tb 65 Dy 66 Ho 67 Er 68 Tm 69 Yb 70 Lu 71 Ac 89 Th 90 Pa 91 U 92 Np 93 Pu 94 Am 95 Cm 96 Bk 97 Cf 98 Es 99 Fm 100 Md 101 No 102 Lr 103 Y Actinides

  21. Valence Electrons • Def: An electron that is in the highest occupied energy level • Critical when dealing with chemical reactions • Elements in the same group are based off these valence electrons

  22. Alkali Metals • Group on the far right (1A) • List the elements in this group as HW. • Have a single valence electron and are extremely reactive • All elements in this group are metals • Not all have the same amount of reactivity. As you go down the chart, the reactivity increases.

  23. Alkaline Earth Metals • Group 2A • All have 2 valence electrons • Harder and higher melting pt. than 1A • All metals • Differences in reactivity are shown by how they react with water.

  24. Magnesium • Key process in photosynthesis • Process plants go through to take sunlight and turn it into usable energy • Its in the center of chlorophyll • Magnesium is light but strong which makes it good for transporting molecules in the plant cell • Also used for bikes and backpack frames

  25. Calcium • Bones and teeth strong • Milk! • Calcium Carbonate • Found in chalk, coral, limestone, and even in your toothpaste • Calcium Sulfate: A cast

  26. Boron Family • Group 3A • Three valence electrons • 1 metalloid, 4 metals • Contains Aluminum! • Most abundant metal in Earth’s Crust

  27. Products made in Boron Family • Aluminum • 10% is in packaging • Parts in cars and airplanes • Window frames • Recyclable! • Boron: Used in special glassware to not shatter when undergoing quick temp. changes

  28. Carbon Family • Group 4A • Contains 4 valence electrons • 1 nonmetal, 2 metalloid, 2 metals • Important: Life wouldn’t exist without carbon

  29. Nitrogen Family • Group 5A • 5 Valence Electrons • 2 nonmetals, 2 metalloids, 1 metal • Most two important elements • Nitrogen and Phosphorus

  30. Uses for Nitrogen Family • Fertilizers: uses nitrogen and phosphorus • Why? • Soil has nutrients (Items needed to survive) • Sometimes soil doesn’t have enough • Fertilizers gives nutrients to soil so plants can use • Why plants need: Proteins and DNA

  31. Oxygen Family • Group 6A • 6 Valence Electrons • 3 nonmetals, 2 metalloids • Oxygen is the most abundant element in the Earth’s crust

  32. Oxygen • Needed by life to release energy • Can be stored as liquid in oxygen tanks • No flammable stuff near them • Ozone: Harmful at ground level • Protects us in the atmosphere

  33. Sulfur • One of the 1st elements discovered • Main use: Sulfuric Acid • Most produced chemical in US • 65% of it is used to make fertilizer

  34. Halogens • Group 7A • 7 Valence electrons • 4 nonmetals, 1 metalloid • Highly reactive (Top highest) • Different physically, similar chemically

  35. Uses of Fluorine and Chlorine • Fluorine • Toothpaste (prevents tooth decay) • Cooking spray (non-stick) • Chlorine • Washing • Sterilizing (Killing bacteria)

  36. Iodine • Iodine is needed in your body to keep your thyroid gland working • Gland is in charge of reactions in your body • Seafood has Iodine • Fresh fish wasn’t available we made Iodized Salt

  37. Noble Gases • Group 8A • Contains 8 Valence Electrons (He:2) • 6 nonmetals • Colorless, Odorless, Not reactive

  38. Uses of Noble Gases • Used in situations where oxygen and hydrogen is highly reactive with a substance • Bulbs are filled with these gases because oxygen would react at that temp.

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