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MBB 222 Study Guide - Midterm Guide: Lone Pair, Chemical Polarity, Electronegativity

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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

Understand electronegativity/electropositivity, and the elements in organic molecules that are electronegative, electropositive or neither. 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. Water molecules are polar and are thus attracted to each other by polar interactions. Non-polar molecules have a symmetric charge distribution for their bonding electrons. Also: the two lone electron pairs on oxygen contribute to the partial negative charge at the - pole.

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Related Questions

1) Which of the following statments is incorrect?

A)Linear molecules cannot have a net dipole moment

B)Dipole moments result from the unequal distribution of electrons in a molecule

C)the electrons in a polar bond are found nearer to the more electronegative element

D)a molecule with very polar bonds can be nonpolar

E)ionic bonding reults from the transfer of electrons from one atom to another

2)Which metals form cations with vary positive charges?

A)transition metals

B) group 1 metals

C) group 2 metals

D)group 3 metals

E)metalloids

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.