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MBB 222 Lecture Notes - Lecture 2: Lone Pair, Chemical Polarity, Partial Charge

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browncricket987
20 Dec 2018
School
Simon Fraser University
Department
Molec Biol & Biochem
Course
MBB 222
Professor
Adam Barlev

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Document Summary

Nh2, oh, i, sh and och3 are examples of functional groups substituents that endow special properties to a compound. Bonds are polar due to unequal sharing of bonding electrons. More electronegative atoms like oxygen will have a greater share of the bonding electrons than more electropositive atoms like hydrogen (polar covalent bond). Part of the molecule has a partially negative charge or pole ( -) while another part of the molecule has a partially positive charge ( +) - such molecules have a permanent dipole . Polar interactions between molecules where the negative end of one molecule is attracted to the positive end of another. Also: the two lone electron pairs on oxygen contribute to the partial negative charge at the - pole. Non-polar molecules have a symmetric charge distribution for their bonding electrons. When the bonded atoms are the same (eg. dioxygen) or similar electronegativity, the molecules are non-polar.

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Related Questions

CH3COCH3 (acetone) is a common laboratory solvent that is often used in nail polish remover. Its Lewis structure and space-filling molecular image are shown here:

Acetone is a polar molecule; the oxygen end has a slightly negative charge (oxygen is more electronegative), whereas the carbon and hydrogen end has a slightly positive charge. In liquid acetone, the molecules are attracted to each other via these polar ends-the positive end of one molecule is attracted to the negative end of its neighbor-and, therefore, align as shown here:

 

CH3COCH3 (acetone) is a common laboratory solvent that is often used in nail polish remover. Its Lewis structure and space-filling molecular image are shown here:

Acetone is a polar molecule; the oxygen end has a slightly negative charge (oxygen is more electronegative), whereas the carbon and hydrogen end has a slightly positive charge. In liquid acetone, the molecules are attracted to each other via these polar ends-the positive end of one molecule is attracted to the negative end of its neighbor-and, therefore, align as shown here:

Draw a Lewis structure and space-filling molecular image for CH2Cl2 (dichloromethane), another common laboratory solvent. Is the molecule polar? Which end of the molecule has a slightly negative charge? Which end has a slightly positive charge? Draw several space-filling molecular images of CH2Cl2 showing how they align in liquid dichloromethane.

CH3COCH3 (acetone) is a common laboratory solvent that is often used in nail polish remover. Its Lewis structure and space-filling molecular image are shown here:

Acetone is a polar molecule; the oxygen end has a slightly negative charge (oxygen is more electronegative), whereas the carbon and hydrogen end has a slightly positive charge. In liquid acetone, the molecules are attracted to each other via these polar ends-the positive end of one molecule is attracted to te negative end of its neighbor-and therefor align as shown here:

Draw a Lewis structure and space-filling molecular image for CH2Cl2 (dichloromethane), another common laboratory solvent. Is the molecule polar? Which end of the molecule has a slightly negative charge? Which end has a slightly positive charge? Draw several space-filling molecular images of CH2Cl2 showing how they align in liquid dichloromethane.