Covalent Bonding and Lewis Dot Structures

Information about Covalent Bonding and Lewis Dot Structures

Published on December 13, 2007

Author: cchschem

Source: authorstream.com

Content

Covalent Bonding and Lewis Dot Structures:  Covalent Bonding and Lewis Dot Structures Presented by: Aubrey Smith Ashley Gallant Will McGuire Ionic vs. Covalent:  Ionic vs. Covalent An ionic bond is where an electron leaves one atom and goes over to another, causing the opposite charges to attract one another. A covalent bond is where two or more atoms share electrons. You can tell the difference by subtracting the electronegativities, and then looking at the chart to tell what it is. Click for more information on Covalent Bonding! Polar and Nonpolar:  Polar and Nonpolar There are two types of covalent bonds, polar and nonpolar. In polar bonds, the electronegativity difference is so great, that the opposite ends have a partial positive and negative force. In nonpolar bonds, the electronegativity difference is so low that the charge is so equal it can’t attract other molecules. Those are also able to be told apart by subtracting the electronegativities and looking at the chart. Click to find more information on Polar and Nonpolar bonding! Electronegativity and ionic/covalent chart:  Electronegativity and ionic/covalent chart Use these charts to help you complete the examples. Examples:  Examples Find out what type of bond each molecule yields. Zn-O 3.5-1.6=1.9 Ionic Br-I 2.8-2.5=0.3 nonpolar covalent. Now you try some on your own!:  Now you try some on your own! H-F Na-I Ba-Cl F-F Ca-F Answers:  Answers 4.0-2.1=1.9 ----- Ionic 2.5-0.9=1.6 ----- Polar- covalent 3.0-0.9=2.1 ----- Ionic 4.0-4.0=0 ----- Nonpolar-covalent 4.0-1.0=3 ----- Ionic Lewis Dot Structures:  Lewis Dot Structures Lewis dot structures are ways of writing how many valence electrons an atom has by putting dots around the atom’s symbol. For example, Helium has two valence electrons, so it would be written You can also write bonds in Lewis dot notation. For example NaCl would be written You can also write double and triple bonds using Lewis dot notation. For example CNH would be written as Click to learn more on Lewis Dot Structures! Now You Try Some:  Now You Try Some H2O NH3 CH4 CO2 BCl3 Answers:  Answers Slide12:  What would the Lewis dot structure of Hydrogen peroxide look like? A: B: C: And the answer is……… Slide14:  A. Ionic B. Polar- covalent C. Nonpolar- covalent And the answer is…. What type of bond would NH3 yield? Slide16:  Ionic Polar- covalent C. Nonpolar- covalent What type of bond would BaF2 yield? Slide18:  0.3 0.4 0.6 And the answer is… What number does the electronegativity difference have to be below to yield a nonpolar- covalent bond? The HARD problem……….:  The HARD problem………. Draw the Lewis dot structure on your own paper of Lactose(C12H22O11). Hand in the paper to Aubrey or Will when you’re done. And the last answer is………. Slide21:  C= carbon= green O= oxygen= red H= hydrogen= white All bonds are single bonds. On a last note….:  On a last note…. The molecular geometry of a molecule can be determined by how many bonding sites and lone pairs of electrons the central atom has. For more information on 3-D molecules

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