For each molecule, (i) draw the Lewis dot structure, (ii) draw the molecule in its actual geometry, and (iii) provide the name of the molecular geometry

For each molecule, (i) draw the Lewis dot structure, (ii) draw the molecule in its actual geometry, and (iii) provide the name of the molecular geometry. Lewis Dot Drawing of Molecule Molecular Geometry? XeF5+ (xenon pentafluoride; unstable) ClF3 (chlorine trifluoride, a component in rocket fuels) BF3 (boron trifluoride; acts as a catalyst in various organic and polymer reactions)

The Correct Answer and Explanation is :

Let’s go step by step with the requested molecules.

1. XeF5+ (Xenon Pentafluoride cation):

(i) Lewis Dot Structure:

• Xenon (Xe) is in group 18, and Fluorine (F) is in group 17. Xe will form bonds with five fluorine atoms, and since the molecule is a cation, one electron is missing from the structure.
• In the Lewis structure, Xenon has five single bonds to Fluorine, and there are lone pairs on the Xenon and Fluorine atoms.
• The overall structure has a positive charge due to the missing electron. (ii) Actual Geometry:
• The geometry of XeF5+ is square pyramidal.
• The Xenon atom is at the center with five fluorine atoms positioned, four at the base of the square, and one at the apex, creating a pyramidal shape with one atom on top. (iii) Molecular Geometry Name:
• Square Pyramidal Geometry.

2. ClF3 (Chlorine Trifluoride):

(i) Lewis Dot Structure:

• Chlorine (Cl) is in group 17 and Fluorine (F) in group 17 as well. Chlorine has three single bonds to fluorine atoms, and it will have lone pairs of electrons to complete its valence shell.
• The central chlorine atom has one lone pair, and each fluorine atom has three lone pairs. (ii) Actual Geometry:
• The geometry of ClF3 is T-shaped.
• There are three fluorine atoms forming a T shape, with two fluorine atoms on one plane and the third one positioned vertically. (iii) Molecular Geometry Name:
• T-Shaped Geometry.

3. BF3 (Boron Trifluoride):

(i) Lewis Dot Structure:

• Boron (B) is in group 13 and Fluorine (F) is in group 17. Boron forms three single bonds with three fluorine atoms. Boron doesn’t have lone pairs since it completes its valence shell by bonding with the fluorine atoms. (ii) Actual Geometry:
• The geometry of BF3 is trigonal planar.
• Boron is in the center with three fluorine atoms arranged symmetrically in a flat plane around it. (iii) Molecular Geometry Name:
• Trigonal Planar Geometry.

Explanation:

• XeF5+ has a square pyramidal geometry because the central xenon atom has five bonding regions and one electron pair that pushes the fluorine atoms into the square pyramid shape.
• ClF3 has a T-shaped geometry due to the presence of three bonding pairs and two lone pairs, leading to the distortion of the fluorine atoms into a T-shape arrangement.
• BF3 has trigonal planar geometry because it has three bonding pairs and no lone pairs, leading to a symmetrical arrangement of the fluorine atoms in a plane around boron.

I’ll now generate the images for each of these molecules.

Here are the images for the Lewis dot structures and molecular geometries:

1. XeF5+ (Xenon Pentafluoride cation): The first image shows the Lewis dot structure and square pyramidal geometry.
2. ClF3 (Chlorine Trifluoride): The second image shows the Lewis dot structure and T-shaped geometry.
3. BF3 (Boron Trifluoride): The third image shows the Lewis dot structure and trigonal planar geometry.

Let me know if you’d like any further details or explanations!