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The Periodic Table

The Periodic Table. Properties of Elements and Trends. Mendeleev. The original periodic table was created by Dmitri Mendeleev. He organized the table by atomic mass . He predicted existence of 3 missing elements (Ga, Sc, Ge). Modern Periodic Table.

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The Periodic Table

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  1. The Periodic Table Properties of Elements and Trends

  2. Mendeleev • The original periodic table was created by Dmitri Mendeleev. • He organized the table by atomic mass. • He predicted existence of 3 missing elements (Ga, Sc, Ge)

  3. Modern Periodic Table • The modern periodic table is organized by atomic number. Henry Mosely

  4. Vertical columns  called groups or families • Horizontal rows  called periods also represent the shells or energy levels • The basis of periodic law is repeating patterns.

  5. Major Categories of Elements • 1) metals 2) non-metals 3) metalloids • Metals are found to the left of the “staircase” • Non-metals are found to the right of “staircase” • Metalloids are found “on” the staircase

  6. Properties of Metals • Solid at room temperature (except Hg) • Shiny, Have luster • Malleable • Ductile • Generally have high melting points • Good conductor of heat and electricity • Have metallic bonds

  7. Properties of Non-metals • Can be solid, liquid or gas at room temp • S  examples C, S, I2 • L  Br2 • G  O2, Ne, F2 • Allotropes- different molecular forms of the same element (different properties, too) O2 and O3 • Dull, lack luster • Brittle • Poor conductors

  8. Properties of Metalloids • Solid at room temperature • Semi-conductors • Have varying properties that can be metallic or non-metallic

  9. Metals tend to lose electrons to form a full valence shell and + ions. • Non-metals tend to gain electrons to form a full valence shell and – ions.

  10. Groups on the Periodic Table • In general, elements found within the same group have similar chemical and physical properties. • This is mainly due to the fact that they have the same number of valence electrons.

  11. Alkali Metals (Group I) • Metals • Have one valence electron • Tend to lose that one electron to become a more stable ion. • Rarely found in natural state.

  12. Lithium(Li), Sodium(Na), and Potassium(K) • Three examples of alkali metals • VERY reactive metals • Exist as solids at room temperature, but are soft • Silvery-white or grayish in color

  13. Lithium

  14. Applications of Lithium • Compounds containing Li have many applications: • lithium hydroxide is used to absorb carbon dioxide in space vehicles • lithium is used in the manufacture of special high strength glasses and ceramics • sometimes, lithium-based compounds such as lithium carbonate (Li2CO3) are used as drugs to treat manic-depressive disorders.

  15. Sodium

  16. Applications of Sodium • Sodium compounds include: • "common salt" (sodium chloride, NaCl), • "soda ash" (sodium carbonate, Na2CO3) • "baking soda" (sodium bicarbonate, NaHCO3) • "caustic soda" (sodium hydroxide, NaOH), are important to the paper, glass, soap, textile, petroleum, chemical, and metal industries • sodium vapor is used in lamps for street lighting

  17. Potassium

  18. Applications of Potassium • The metal is the seventh most abundant and makes up about 1.5 % by weight of the earth's crust. • Potassium is an essential constituent for plant growth and it is found in most soils. • It is also a vital element in the human diet.

  19. Comparing 3 Alkali Metals Lithium Potassium Sodium

  20. Alkaline Earth Metals (Group II) • Metals • Have two valence electrons • Tend to lose the two electrons to become a more stable ion

  21. Magnesium(Mg), Calcium(Ca) and Strontium(Sr) • Examples of alkaline earth metals • Exist as solids at room temperature • Silvery white or grayish white in color • Fairly reactive metals

  22. Magnesium

  23. Applications of Magnesium • Magnesium is the eighth most abundant element in the earth's crust although not found in it's elemental form. • used in flares and pyrotechnics • it is lighter than aluminum, and is used in alloys used for aircraft, car engine casings, and missile construction

  24. Calcium

  25. Applications of Calcium • Forms more than 3% of the earth’s crust • Is an essential constituent of leaves, bones, teeth, and shells • is a component of Portland cement

  26. Strontium

  27. Applications of Strontium • fireworks (red flame), flares • 90Sr is a radioactive isotope produced by nuclear fallout. 90Sr has the potential for use as lightweight nuclear producing electricity • used to produce glass for color television tubes

  28. Halogens Group 17 • Have 7 valence electrons • Non-metals (F, Cl, Br, I) • F, Cl (gases), Br (liquid), I (solid) • Tend to gain one electron to form a more stable ion • Extremely reactive

  29. Fluorine

  30. Fluorine • Used as a toothpaste additive, in refrigerator coolants, and in Teflon

  31. Chlorine

  32. Chlorine • Used in water purification and bleach.

  33. Noble Gases Group 18 • Very stable because of filled valence shell. • Do not react in the presence of other elements (relatively inert) • Xe can react with Fluorine (more later)

  34. Argon

  35. Argon • Used in light bulbs and lasers.

  36. Xenon • Used in UV lamps and sun lamps in tanning salons.

  37. Transition Metals • Also known as “heavy metals” • Tend to be very dense • Have varying reactivity • Have multiple oxidation states (can form more than one ion) • Have colorful ions (in solution)

  38. Copper

  39. Copper • Used to make the Statue of Liberty, pennies, water pipes and more.

  40. Nickel

  41. Nickel • Used to make coins, knives, forks and rechargeable batteries.

  42. Silver

  43. Silver • Used in silverware, jewelry, mirrors, and batteries.

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