using VSEPR THEORY SHOW WHY
1)BF4- is a tetrahedral molecule
2)SF3+ is a Trigonal pyramidal molecule
3)ICI4- IS A SQUARE PLANER molecule
4IF5 IS A SQUARE pyramidal molecule
5)PF5 IS A TRIGNAL BIPYRAMIDAl molecule
You need to draw the Lewis electron dot structures and use VSEPR information to explain these. I can't draw these structures on the board. If you don't have them in your book I may be able to find one or more on the web.
can you find them for me
To determine the molecular geometry of a molecule using the VSEPR (Valence Shell Electron Pair Repulsion) theory, we need to follow a step-by-step approach. Here's how we can apply the VSEPR theory to determine the molecular geometry for the given compounds:
1) BF4-:
To determine the molecular geometry of BF4-, we need to consider the central atom (Boron) and its surrounding atoms. In this case, boron has four fluorine atoms attached to it.
The Lewis structure for BF4- would look like this:
F - B - F
|
F
The central atom (Boron) has no lone pairs and four surrounding atoms (Fluorine). According to the VSEPR theory, when there are four surrounding atoms and no lone pairs, the molecule adopts a tetrahedral geometry. Therefore, BF4- is a tetrahedral molecule.
2) SF3+:
In the case of SF3+, we have a central atom (Sulfur) and three surrounding atoms. The "+" charge indicates that one electron should be subtracted. Since sulfur has six valence electrons, removing one electron gives us five valence electrons.
The Lewis structure for SF3+ would look like this (with a positive charge on Sulfur):
H
|
F - S - F
|
F
The central atom (Sulfur) has no lone pairs and three surrounding atoms (Fluorine). According to the VSEPR theory, when there are three surrounding atoms and no lone pairs, the molecule adopts a trigonal planar geometry. However, since there is a positive charge on the central atom, there will be one fewer electron cloud, resulting in a trigonal pyramidal shape. Therefore, SF3+ is a trigonal pyramidal molecule.
3) ICl4-:
The Lewis structure for ICl4- would look like this:
F
|
F - Cl - I - Cl
|
F
The central atom (Iodine) has no lone pairs and four surrounding atoms (Chlorine). According to the VSEPR theory, when there are four surrounding atoms and no lone pairs, the molecule adopts a square planar geometry. Therefore, ICl4- is a square planar molecule.
4) IF5:
The Lewis structure for IF5 would look like this:
F
|
F - I - F
|
F
The central atom (Iodine) has one lone pair and five surrounding atoms (Fluorine). According to the VSEPR theory, when there are five surrounding atoms and one lone pair, the molecule adopts a square pyramidal geometry. Therefore, IF5 is a square pyramidal molecule.
5) PF5:
The Lewis structure for PF5 would look like this:
F
|
F - P - F
|
F
The central atom (Phosphorus) has no lone pairs and five surrounding atoms (Fluorine). According to the VSEPR theory, when there are five surrounding atoms and no lone pairs, the molecule adopts a trigonal bipyramidal geometry. Therefore, PF5 is a trigonal bipyramidal molecule.
So, by applying the VSEPR theory, we can determine the molecular geometry of each given compound.