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The XeF2 molecule has a trigonal bipyramidal electron domain geometry and a linear molecular geometry. The FXeF bond angle is molecule is

and the

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Sketch the shape of a linear triatomic molecule, a trigonal planar molecule containing four atoms, a tetrahedral molecule, a trigonal bipyramidal molecule, and an octahedral molecule. Give the bond angles in each case.

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Sketch the following molecular shapes and give the bond angles in the structures: (a) linear, (b) trigonal bipyramidal.

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Predict the electron pair geometry, the molecular shape, and the bond angle for a carbon disulfide molecule, $\mathrm{CS}_{2}$, using VSEPR theory.

Transcript

Hi there we have a question are several questions actually about the molecule XEF two. So the first thing I want to do is draw its lewis structure. So we have X. E. With two floor rings, Each Florian is a halogen. So each one of those has seven valence electrons, X. E. S. Of course a noble gas. So it has eight valence electrons. There is not a difference in electrons but I’m just going to do the XC ones in a different color just to help us keep count. So that’s two XC has six more electrons. 12 34 56. So what we end up with looking at that central atom is we have two atoms bonded to it And three lone pairs of electrons. Right? This gives us five electron domains which means the electron domain geometry. It’s going to be Trigon all the high parameter. So the electron geometry, this is the electron geometry. That is our first answer is triggering a by RAM. It’ll okay, the next one wants to know the molecular geometry. Well, let me draw this a little more realistically. The bonded atoms are going to arrange themselves as far away from each other as possible. So that means they are going to go up and down while our lone pairs of electrons are going to be in that triangular plane around the center. Little challenging to draw this. But I think we sort of have it there. Alright, so the lone pairs are in the plane around the…

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