CHEM 1010 week 6
CHEM 1010 week 6 CHEM 1010
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This 3 page Class Notes was uploaded by Chase Bobier on Saturday March 12, 2016. The Class Notes belongs to CHEM 1010 at Middle Tennessee State University taught by Tammy J Melton in Fall 2015. Since its upload, it has received 13 views. For similar materials see Introductory General Chemistry I in Chemistry at Middle Tennessee State University.
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Date Created: 03/12/16
Chase Bobier CHEM 1010 notes, Week 6 Important terms Things you need to know Electron Shells and Element Behavior - Elements with valence shells that are close to or are four tend to share electrons and not form ionic bonds - Metalloids readily form both ionic and covalent bonds - Transition metals and rare earths are expected to become negatively charged ions (cations). You cannot predict the charge of these elements and must be told via roman numerals following the name. (Iron III, Copper II… etc.) Electron Configuration Sublevels Electrons are arranged around the nucleus in shells, which are layers of electrons that have the same amount of energy. The chart on the next page will detail how these sublevels work. Counting Electron Shells. Here are some examples of how electron shells are counted. (Hydrogen) H 1s 1 2 (Helium) He 1s (Lithium) Li 1s 2s 1 And so on. When you get to larger atoms, you can use a shortcut called Noble Gas notation (NGN). Noble Gas Notation is a way of shortening the electron configuration of large molecules. Here’s an example using Sn: 2 2 6 2 6 2 10 6 2 10 2 Sn 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 2 10 2 Now using NGN: Sn [Kr] 5s 4d 5p NGN shows the reader that an element has the same electron configuration as the noble gas before it, so by putting that in brackets you don’t have to write all of the electron shells contained in that noble gas, and just write all of the shells that that atom has beyond that noble gas.
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