Chem 6c chap 14 week 5

Chem 6c chap 14 week 5 - Chapter 14 The First Four Main...

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Chapter 14: The First Four Main Groups In studying chemistry and chemical reactions, the periodic table is invaluable for recognizing patterns so memorization can be minimized. http://www.webelements.com/ and http://www.chemicalelements.com/ and http://dl.clackamas.cc.or.us/ch104- 06/periodic.htm When you see a new reaction, the first thing you should think about are the following: 1) Is this a redox reaction? a) what chemical is the oxidant? b) what chemical is the reductant? 2) If not, is it an acid-base reaction. 3) If acid-base, is it of the Bronsted Lowry or Lewis type. a) what chemical is the acid ? b) what chemical is the base?
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Periodic Trends Atomic properties follow a number of periodic trends: 1) Size contracts as you go across a row in the periodic table. 2) Size increases as you down a column in the periodic table. 3) Metals are on the left side of the PT, nonmetals on the right. 4) Electronegativity (IPs) increases as you go across a row in the PT, with the exception of noble gases that are usually chemically inert. 5) Electronegativity (IPs) decreases as you go down a column in the PT. 6) In their elemental state, the elements change from metallic reducing agents on the left side of the PT to nonmetal strong oxidants on the right side of the PT with the exception of the noble gases.
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7) Similarly, the stable form of elements in compounds are generally in positive oxidation states for metals and negative oxidation states for elements on the right side of the PT, except for noble gases. http://www.sciencegeek.net/tables/NYregents.pdf 8) Bonds between elements of very different electronegativities, such as metals and nonmetals, are ionic (e.g., Na-Cl, MgF 2 ). 9)
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This note was uploaded on 06/12/2008 for the course CHEM 6C taught by Professor Hoeger during the Spring '08 term at UCSD.

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Chem 6c chap 14 week 5 - Chapter 14 The First Four Main...

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