Problem

Identify the electron pair geometry and the molec…

05:22

Problem 91 Hard Difficulty

Predict the electron pair geometry and the molecular structure of each of the following molecules or ions:
(a) $\mathrm{SF}_{6}$
(b) $\mathrm{PCl}_{5}$
(c) $\mathrm{BeH}_{2}$
(d) $\mathrm{CH}_{3}+$

Answer

a) This shows that there are six regions of high electron density around the carbon atom, and there
are no lone pairs on the carbon atom. Thus, octahedral arrangement with all the fluoride atoms
mutually perpendicular to the neighboring ones is obtained as the electron pair geometry. since
there are no lone pairs on the central sulfur atom, the molecular geometry is Octahedral as well.
see structure
b) This shows that there are five regions of high electron density around the carbon atom, and there
are no lone pairs on the carbon atom. Hence the electron-pair geometry and molecular structure
both will be trigonal bipyramidal.
see structure
c) This shows that there are two regions of high electron density around the carbon atom, and there
are no lone pairs on the carbon atom. The least repulsion is when both the hydrogen atoms are
180 degrees apart. Hence the electron-pair geometry and molecular structure both will be Linear.
see structure
d) This shows that there are three regions of high electron density around the carbon atom, and
there are no lone pairs on the carbon atom. Hence the electron-pair geometry and molecular
structure both will be trigonal planar, where the hydrogen atoms are arranged at 120 degrees
angle from each other.
see structure

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Chemistry 101

Chemistry

Chapter 7

Chemical Bonding and Molecular Geometry

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Video Transcript

Now the question is predict the electron geometry and the molecular structure of each of the following molecules or ions. First 1. Is s f? 6. So here you have to decide the electronic you have to decide the geometry of the molecule by a valence shell, electron par repulsion theory, and for that you are supposed to know that how many electron pairs are present, whether they are bonding or non bonding around the Central atom, and by that you can decide the jut of the mole, so here a iss f. 6. Sulphur is at the center having 6 electrons 123456. We are writing the lewis structure just to understand that how many electron pairs are present around sulphur in s. F. 6, so here 1 fluid forming the bond here. 1 flowin forming the bond with sulphur and 1 electron is given by this florine. Chlorine is having total 7 electrons, and these 7 electrons are around florine. Out of that 1 electron is forming the bond, so we are interested in only sulphur. How many electron pairs are present omul. So we are writing that only so. First 1 is here: 1 chlorine and total 6 florine forming the bond in the central self for it and by this total number of electron pairs around sulphur is 12345 and 6 n. When 6 electron pairs are present, they are trying to be farthest from each other. In the geometry, so that the reflection is minimum, and that is why their structure should be octahedral, so octahydrogeometry must represent, and that that means the sulphur is at the center 4 florine in the same plane. 1 is above the plane. Other 1 is the plane, and by that this should be the geometry of the hydrogeometryand. All the positions are occupied by a flooring, so we have to remember that sulphur is at the center and 4 flowing or the every angle is actually 90 degrees here, whether it is in between these 2 flooring or these 2 florine everywhere. The angle is 90 degrees and in case of octahedrant jumped so this is a now come to be. A b is p c, l 5, so in p, ca 5. The geometry should be: phosphorus is at the center 5 electrons are present around it. 5 electrons and 5 chlorine atoms are forming born with this. So all the 5 chlorine giving 11 electron for the formation of bonding pair and chlorine is having optat complete because vilence electrons in case of chlorine total 7, but we are interested only in electron pairs around the central atom. That is phosphorus. So here it is 1234 and 5, so 5 electron pair say in the space. We have to arrange in such a way so that they are farthest from each other. According to violential, electron, pary function, theory and triagonal planer is the triagonal by pyramidal is the only geometry, so geometry is triagonal by pyramid that is phosphorus at the center and 3 chlorine in the same plane forming bond with the central atom and 1. Chlorine is above the plane and other chlorine should be below the plane and dish. 3 should be in the same plane and here when they are present at the same plane. The angle is 120 degrees, and with this it is for 90 degree angle, so this is trigonotrigonal. Bipyramidal now come to c c is b e h, 2, so c is b e, h, 2 pont, ballium, 2 electrons and hydrogen 1 electron so 1 central atom. We have only 2 electron pairs, so 2 electron pairs. We have to arrange in the space so that they are farthest from each other and the repulsion is minimum and the geometry possible is only 1 that is linear, joint in 1 line with the. So the angle is valium at the center 1 hydrogen here and 1 hydrogen here- and this is the linear and the angle should be 180 degrees. Now. The last 1, that is d d, is ch, 3 plus ch, 3 plus carbon is at the center and 1 electron is less so only 3 electrons are present around carbon and hydrogen is forming 3 hydrogen forming the bonding pair. So around carbon we have only 3 electron pairs. These 3 electron pairs. We have to arrange in such a way so that they are farthest from each other and the only geometry is triagonal plane, structure, trigonal, planer structure, plainer structure, and that is carbon at the center and hydrogen. Here, 1: hydrogen here 1- hydrogen here this is triton plane, state and every angle is 120 degree. So that is how, by violencia electron pair repulsion theory, we can decide the geometry of the molecule, and for that we are writing. First, the lois structure and in the lewis structure we are trying to understand how an electron pairs are present around the central atom and acco.

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