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When considering whether is polar or nonpolar try to

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When considering whetheris polar or nonpolar, try to determine whether a dipole can be established based on its geometry. (Recall that nitrogen ismuch more electronegative than hydrogen.) This can be achieved by examining the different trajectories of the dipole moments and determining whether oneof them reasonably matches the accurately depicted geometry. Select the option below that best describes the dipole moment of ammonia.LiFKrXeOSCO2PCl5SF4ClF3BF3NH3VSEPR and MO Diagrams Workshop Activity - April 22nd...
26 of 384/23/2021, 9:00 PM
ANSWER:ResetHelpSO2ClF3SF4BrF5CO2PCl5SF6BF3PolarNonpolarVSEPR and MO Diagrams Workshop Activity - April 22nd...27 of 384/23/2021, 9:00 PM
CorrectDipole moments are commonly expressed in units of debye (). Completely nonpolar molecules such as diatomic molecules have a dipole moment of 0.0, and the ionic compoundhas a dipole moment of about 10.4. Polar molecules will tend to have dipole moments that range from 1 to 5. Thedebye is a non-SI unit that is equivalent to(coulomb meters).PhET Simulation – Molecule PolarityElectronegativity is a term used to define an atom’s ability to attract electrons to itself when it is bonded to another atom.A larger electronegativity value indicates agreater ability for an atom to attract electrons to itself.Electronegativity values follow trends (with exceptions) across the periodic table.They increase from left to rightacross a period and increase from the bottom of a group to the top.Thus, fluorine is the most electronegative element with a value of 4.0.Notice that since the noblegases have completely filled electron shells and are inert, they don’t have assigned electronegativity values.In any given molecule comprised of two or more nonidentical atoms, the electrons contained in the bond are not shared equally. Bond polarity is a measure of howunevenly the electrons in a bond are shared and is indicated by the difference between the electronegativities of the atoms involved.A large difference inelectronegativities indicates that a bond is polar and contains a dipole (i.e., the bond character is more ionic), which is created when two equal but opposite charges areseparated.A smaller difference in electronegativity makes the bond character more covalent.Click on the image below toexplore this simulation, which demonstrates the cause and effect of molecular polarity.When you click this simulation link, you may be askedwhether to run, open, or save the file. Choose to run or open it.When the simulation is opened you should select the option forTwo Atoms. You will then see two atoms (A and B) with a dipole moment drawn directly over the bond.

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Term
Spring
Professor
CHURCHILL
Tags
Atom, Electron, Molecule, Chemical bond

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