Question

Write rules of VESPER theory





Don't spam​

Answer 1

Explanation:

In the last section we learned about a simple approach called the Lewis-dot structure that gives a good approximation of how the valence electrons are distributed in a molecule. What Lewis-Dot structures do not tell us is the shape of the molecule. For example, why do XeF4 and CF4 have different shapes even though the central atom is coordinated by four Fluorine atoms in both cases?

alternatetext

One way to answer these questions about molecular structure is to use a simple approach that builds on the Lewis-Dot structure approach called the Valence Shell Electron Pair Repulsion Model, or VSEPR model.

The idea behind this approach is that the structure around a given atom is determined principally by minimizing electron repulsions. That is, the bonding and non-bonding electrons around a given atom will be positioned as far apart as possible. For example, BeCl2 has the Lewis Structure.

alternatetext

There are only two pairs of electrons around Be. The arrangement that puts the bonding electron pairs as far apart as possible is a linear arrangement:

alternatetext

...as far apart as possible - a very simple model.

Using this guiding principle let's look at the possible arrangements that arise when there are different numbers of electron domains (i.e., bonding and non-bonding electrons) surrounding an atom.

alternatetext

Given the arrangements above we use the following rules for predicting the geometry around an atom.

VSEPR Rules for Determining Structure

Draw the Lewis Structure.

Add together the number of atoms bound to the central atom and the number of lone pair electrons and choose the appropriate arrangement. (i.e., linear, triangular planar, tetrahedral, trigonal bipyramidal, or octahedral).

Draw the structure, placing the appropriate number of bonds and lone electron pairs (i.e., electron domains) about the central atom according to the chosen arrangement.

Answer 2

Explanation:

VSEPR Rules

Draw the Lewis structure for the molecule or ion.

Count the total number of regions of high electron density (bonding and unshared electron pairs) around the central atom.

Double and triple bonds count as ONE REGION OF HIGH ELECTRON DENSITY.

An unpaired electron counts as ONE REGION OF HIGH ELECTRON DENSITY.

For molecules or ions that have resonance structures, you may use any one of the resonance structures.

*Examples

*Test My Knowledge

Identify the most stable arrangement of the regions of high electron density as ONE of the following:

linear

trigonal planar

tetrahedral

trigonal bipyramidal

octahedral

*Examples

Determine the positions of the atoms based on the types of electron pairs present (i.e., bonding pairs vs. unshared pairs). For trigonal bipyramidal and octahedral arrangements, there can sometimes be more than one possible arrangement of the bonding and unshared pairs:

Trigonal bipyramidal - place any unshared pairs in the plane of the triangle.

Octahedral - if you have two unshared pairs, place them on opposite sides of the central atom.

*Examples

Identify the molecular structure based on the positions of the ATOMS (NOT on the regions of high electron density).

hope u understand

make it as brainlist plz frd. . . . . .