{"id":130,"date":"2023-05-31T16:03:50","date_gmt":"2023-05-31T16:03:50","guid":{"rendered":"https:\/\/aceorganicchem.com\/chemistry\/?p=130"},"modified":"2023-06-03T23:10:31","modified_gmt":"2023-06-03T23:10:31","slug":"molecular-geometry-of-xef4","status":"publish","type":"post","link":"https:\/\/aceorganicchem.com\/chemistry\/molecular-geometry-of-xef4\/","title":{"rendered":"Molecular Geometry of XeF4 [with video and free study guide]"},"content":{"rendered":"\n

What is the molecular geometry of XeF4<\/sub>?<\/strong><\/h1>\n\n\n\n

The molecular shape of XeF4<\/sub> is square planar, or AX4<\/sub>E2<\/sub> using Valence Shell Electron Pair Repulsion (VSEPR) theory. Hence, the molecular geometry of XeF4<\/sub> has only 90 degree bond angles in the molecule. XeF4<\/sub> looks like this:<\/p>\n\n\n\n

\"molecular<\/a><\/figure>\n\n\n\n

How do you find the molecular geometry of XeF4<\/sub><\/strong><\/strong>? <\/strong><\/h2>\n\n\n\n

There is an easy three-step process for determining the geometry of molecules with one central atom.<\/p>\n\n\n\n

Step 1<\/strong>: Determine the Lewis structure of the molecule.<\/em>
For XeF4<\/sub>, it is as shown below: For a full-explanation of how to figure out the Lewis structure, please go to Lewis Structure of XeF4<\/sub>. However, here is what it looks like. It is different because xenon is hypervalent, and has four bonds and two lone pairs for an “octet” of 12. <\/p>\n\n\n\n

\"Lewis<\/a><\/figure>\n\n\n\n

Step 2<\/strong>: Apply the VSEPR notation to the molecule.<\/em>
Apply VSEPR notation, A X E
A=Number of central atoms
X=Number of surrounding atoms
E= Number of lone pairs on central atom
For this one, we can see that it has one central atom (Xe), four surrounding atoms (F), and two lone pairs of electrons around the central atom, making it AX4<\/sub>E2<\/sub>.<\/p>\n\n\n\n

Step 3<\/strong>: Use the VSEPR table to determine the geometry of XeF4<\/sub>.<\/em><\/p>\n\n\n\n

\"VSEPR<\/a><\/figure>\n\n\n\n

As you can see from the chart, the AX4<\/sub>E2<\/sub> molecule is square planar. <\/strong><\/h2>\n\n\n\n

Bond angles help show molecular geometry of XeF4<\/sub><\/strong><\/h3>\n\n\n\n

The only bond angles in this molecule are the F-Xe-F angles, as each F-Xe-F bond angle is the same as all of the others. Below is a diagram which will explain this more.<\/p>\n\n\n\n

\"XeF4<\/a><\/figure>\n\n\n\n
\"XeF4<\/figure>\n\n\n\n

What about that lone pair?<\/strong><\/h3>\n\n\n\n

The lone pairs of the molecule resides in both of the axial positions, above and below the square as shown below. This means that the ELECTRONIC geometry is octahedral, even though the MOLECULAR geometry of XeF4<\/sub> is square planar. See more about about concept in the FAQs below.<\/p>\n\n\n\n

\"XeF4<\/a><\/figure>\n\n\n\n

More about VSEPR and the molecular geometry of XeF4<\/sub>:<\/strong><\/h3>\n\n\n\n

Let’s not forget, the whole purpose of VSEPR is to minimize interactions between the substituents (atoms and lone pairs) of a molecule. We also know that electrons repel each other. Hence, simple molecules (like the ones we are looking) at will tend to place substituent atoms as far from each other as possible. We know this because of the bond angles associated with each of the four types of shapes.<\/p>\n\n\n\n

\"VSEPR<\/a><\/figure>\n\n\n\n

Here is one way to remember this chart: Think about each lone pair as just replacing an atom. In the chart above we have tried to show how this works by just blurring out an atom for a lone pair. <\/p>\n\n\n\n

For the 3 and 4 substituent molecules (AX3<\/sub> group and AX4 <\/sub>group, respectively) it is easy to do this because each one of the substituent atoms is the same. So for AX2<\/sub>E, it is simple to see that we get trigonal pyramidal as the answer because we can replace any of the atoms with a lone pair because they are all geometrically equivalent. Same for AX3<\/sub>E because all of the atoms are geometrically equivalent. <\/p>\n\n\n\n

It get a little trickier when we get to the 5 and 6 substituent molecules (AX5<\/sub> group and AX6 <\/sub>group, respectively). Here, there is a geometric difference between the atoms on the axis (called axial substituents) and the ones around the middle, called the equatorial substituents. Thus, we can’t just substitute a lone pair for any old atom. So…..what we need to remember is that for the AX5<\/sub> group, you need to replace equatorial atoms with lone pairs AND for the AX6<\/sub> group, you need to replace the atoms on the axis with lone pairs, as we have shown above. <\/p>\n\n\n\n

Some video to make it a little simpler:<\/strong><\/h3>\n\n\n\n
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