2015年10月22日 · AX3E2 forms a T-shape because you can think of it as starting at a trigonal bipyramidal shape(AX5) as it has 5 regions of electron densities. From here, if you remove one of the bonded atoms and replace it with a lone pair, you will get a see saw shape with bonds that are less than 120 degrees, less than 90 degrees, and less than 180 degrees ...

2020年12月10日 · For AX3E2 the central atom has five regions of electron density. Therefore, its electron arrangement must be trigonal bipyramidal. When choosing the lone pairs you have to choose lone pairs that minimize electron pair repulsions.

Answer to According to VSEPR theory, a molecule with the. According to VSEPR theory, a molecule with the general formula AX3E2 (A is the central atom, X is the bonded atom and E is a lone pair of electrons) has how many regions of electron density around the central atom [ Select ] AXsE2 will have what kind of electronic geometry?

Question: Draw and name three molecular shapes for molecules having the VSEPR formulas AX3, AX3E, and AX3E2, respectively. a. If the three X groups in the above formulas are identical, which of the three shapes would result in a molecule with a dipole moment?

2023年12月3日 · In our textbook Topic 2E, an AX3E2 molecule was said to be t-shaped with its two lone pairs on the equatorial plane. Why are they on the equatorial plane (abt 120 deg apart) when they could be on the axial plane (180 deg apart) and …

2011年9月11日 · Question: What is the shape of AX3E2 type molecule? It seems to me that the electron pairs would repel each other and occupy regions that are 180 degrees from each other. Then the shape would be trigonal planer. However, the book (and wikipedia) states that the molecule actually forms a T shape.

3. Variations on AXs, steric number (SN) = 5 Types AX4E (seesaw), AX3E2 (T-shaped), and AX₂E3 (linear) In PC14, the lone pair of electrons can be placed in either an equatorial or an axial position. Determine the total number of each type of 90° …

2017年11月8日 · Homework question 4.11b asks you to find the VSEPR formula and predict the shape of iodine trichloride. The VSEPR formula for this molecule is AX3E2. With that in mind I expected the arrangement of electrons to be trigonal bipyramidal around the atom with the two lone pairs in equatorial positions.

2020年12月3日 · Benjamin_Hugh_1G wrote:The lone pairs react with the bonding pairs at an angle of 90 degrees.In the T-shape, there will be 4 lp/bp interactions, but in the case of a trigonal planar shape, when the lone pairs are placed at the top and bottom, the lone pairs will result in 6 lp/bp interactions, which causes more repulsion than the T-shape.

The VSEPR AX3E2 class (belonging to the AX5 family) Example 9: BrF3 Experimentally determined geometry shows T-shaped molecules. The bond angles between the axial and equatorial F atoms is about 85∘, less than the 90∘ that would be …