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The Periodic Table

The Periodic Table. Element Groups. Most Important. The periodic table of elements is much more than a list of element symbols, atomic masses and element symbols. You will use the periodic table to check your electron configurations, orbital notations and Lewis dot notations.

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The Periodic Table

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  1. The Periodic Table Element Groups

  2. Most Important • The periodic table of elements is much more than a list of element symbols, atomic masses and element symbols. • You will use the periodic table to check your electron configurations, orbital notations and Lewis dot notations. • You will use it to predict relative properties of elements such as reactivity, electronegativity and metallic characteristics.

  3. THREE MAJOR CATEGORIES

  4. THREE MAJOR CATEGORIES • Metals have characteristic properties of luster, heat and electricity conductivity and malleability. Except for mercury, they are solids at room temperature. • Nonmetals tend to form negative ions and do not possess the properties of the metals. Many are gases at room temperature. Only Bromine is a liquid at room temperature. Carbon, sulfur and phosphorous are solids. • Metalloids are semiconductors and tend to have characteristics of both metals and nonmetals.

  5. The Alkali Metals • Examples: Li, Na, K • Soft, gray, light metals. • VERY reactive • Will ignite and even explode in contact with water. What is left is an alkaline solution such as sodium hydroxide.

  6. Alkaline Earth Metals • Examples: Be, Mg, Ca, Sr, Ba • Somewhat soft metals. • Less reactive than Alkali metals, but more reactive than most metals. • Usually found combined with oxygen

  7. The Transition Metals • Examples: Cu, Ag, Au, Zn, Ti, Fe, Cr, Co, Ni • “Typical metals” • Most are gray, hard and dense • Lustrous, malleable, ductile • Conduct heat and electricity • Less reactive than alkaline earth metals

  8. Other Metals • examples: Aluminum, Tin, Lead • Softer than transition metals • Gray, malleable • Less reactive than most metals.

  9. Metalloids • ex: Boron, Silicon, Antimony, Bismuth • Properties between those of metals and non-metals • Semiconductors of heat and electricity • Reactivity depends upon the properties of the other elements in the reaction.

  10. Halogens • Fluorine(gas), Chlorine (gas), Bromine (liquid), Iodine (solid) • VERY reactive • Can form compounds with almost all metals • Commonly used in cleaners (caustic) • Their compound are called salts.

  11. Noble Gases • He, Ne, Ar, Kr, Xe, Rn • Colorless, odorless gases at room temperature • Are chemically “inert” • (Normally will not undergo any chemical reactions, so they rarely form any compounds - not reactive)

  12. Other Non-metals • H, C, N, O, P, S • “Life elements” • Light, non-malleable, brittle • Poor conductors of heat and electricity • Reactivity depends upon the element

  13. Lanthanides

  14. Lanthanides Actinides

  15. Lanthanides and Actinides • Ex: Uranium, Plutonium • Rare-Earth Elements • There properties are very similar and they are often found mixed together. • Most are radioactive • Many are not found naturally on Earth. Highly reactive (ex: Plutonium)

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