1 / 33

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.

gannon
Télécharger la présentation

The Periodic Table

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  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)

More Related