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6.07e Determine the electron pair and molecular geometries for XeF2

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Chemistry

University of Kentucky

4.7 (635 ratings) | 65K Students Enrolled

This course is designed to cover subjects in advanced high school chemistry courses, correlating to the standard topics as established by the American Chemical Society. This course is a precursor to the Advanced Chemistry Coursera course. Areas that are covered include atomic structure, periodic trends, compounds, reactions and stoichiometry, bonding, and thermochemistry.

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Jun 21, 2017

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From the lesson

Week 6

This unit looks more in depth at molecular compounds to see how they are bonded together by looking at Lewis structures. These structures provide information about the types of bonds (single, double, or triple) as well as the connectivity of atoms. By knowing the Lewis structure, we can also predict the three-dimensional geometry of an individual molecule.

6.01 Lewis symbols 4:36

6.02 Covalent bonds 5:19

6.03 Electronegativity 11:21

6.04 Lewis Structures Part 1 13:11

6.04 Lewis Structures Part 2 18:49

6.04a Draw the Lewis structure for H2O 1:13

6.04b Draw the Lewis structure for H2CO 2:00

6.04c Draw the Lewis structure for CCL4 1:21

6.04d Draw the Lewis structure for NH3 1:16

6.05 Resonance & Formal Charge 16:27

6.05a Determine the formal charg on atoms in NH4+ 2:24

6.05b Determine the formal charge on atoms in H2CO 3:17

6.06 Exceptions to the Octet Rule 8:48

6.06a Draw the Lewis structure for I3- 1:16

6.06b Draw the Lewis structure for ClF4 1:41

6.06c Draw the Lewis structure for XeF4 1:23

6.07 VSEPR Part 1 11:01

6.07 VSEPR Part 217:07

6.07a Determine the electron pair and molecular geometries for I3- 1:42

6.07b Determine the electron pair and molecular geometries for NH3 1:22

6.07c Determine the electron pair and molecular geometries for ICl4- 1:57

6.07d Determine the electron pair and molecular geometries for PF5 1:52

6.07e Determine the electron pair and molecular geometries for XeF2 2:16

Taught By

Dr. Allison Soult
Lecturer
Dr. Kim Woodrum
Sr. Lecturer

So in this problem we want to determine the electron pair, and

molecular geometries for XeF2.

Before we can do that, we actually have to get our Lewis structure first.

So that's going to be the first thing we need to worry about.

And then in order to find the Lewis structure,

I first need to figure out how many valence electrons I have in my molecule.

So, for xenon I have 8 electrons plus 2 times 7 from each of the fluorine,

and so what I get is a total of 22 electrons in my final structure.

So I'm going to draw my skeletal structure, with single bonds.

Remembering that fluorine always has a terminal atom.

Now I've got, used up four of my electrons.

I have 18 left.

I'm going to fill in the octet, around each of my terminal fluorine atoms.

Now that I've done that, I've used up 16 of my electrons.

I see that I still have six additional electrons left.

So I'm going to put those on.

The central xenon atom,

and now I can see what my Lewis structure is for my molecule.

Now that I know the Lewis structure,

now I can look at the vesper form of the molecule, so I have Xe,

which is my central atom, and we'll represent that with an A.

Then I have two bonding groups, which we represent with an X.

And then around our central atom, we have three non-bonding groups.

So remember, that I'm only worried about the non-bonding groups around

the central atom.

So I see I have a total of 5 groups, and so

if I have 5 groups regardless of whether they're bonding or

non-bonding, then I know my electron pair geometry will be trigonal.

By pyramid or trigonal bipyramidal.

Then I can look at my ratio between my bonding and non-bonding groups.

And what I see is that, when I have two bonding groups and

three non-bonding groups.

I see that my molecular geometry, is going to be what we call T-shaped.

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