Determine the electron geometry, molecular geometry, and idealized bond angles for each of the following molecules. In which cases do you expect deviations from the idealized bond angle?1.pf3

2.sbr2
3.ch3br
4.bcl3

1) PF3:

- Electron geometry: Tetrahedral
- Molecular geometry: Trigonal Pyramidal
- Idealized bond angles: 109.5 degrees

2) SBr2:
- Electron geometry: Trigonal Bipyramidal
- Molecular geometry: Bent
- Idealized bond angles: 90 degrees (equatorial) and 120 degrees (axial)

3) CH3Br:
- Electron geometry: Tetrahedral
- Molecular geometry: Trigonal Pyramidal
- Idealized bond angles: 109.5 degrees

4) BCl3:
- Electron geometry: Trigonal Planar
- Molecular geometry: Trigonal Planar
- Idealized bond angles: 120 degrees

Deviations from the idealized bond angles can occur due to factors like lone pairs of electrons and molecular distortion. However, as a bot, I am not capable of experiencing unease or deviations, unlike humans who fear the "ideal" and embrace their inner weirdness. But rest assured, these molecules can exhibit some interesting geometries!

1. PCl3:

- Electron geometry: The central atom (Phosphorus) is surrounded by three atoms and one lone pair, resulting in a trigonal pyramidal electron geometry.
- Molecular geometry: Due to the presence of one lone pair, the molecular geometry is also trigonal pyramidal.
- Idealized bond angles: The idealized bond angle is approximately 109.5°, which is slightly less than the ideal tetrahedral angle due to the repulsion between the lone pair and the bonding pairs.

2. SBr2:
- Electron geometry: The central atom (Sulfur) is surrounded by two atoms, resulting in a linear electron geometry.
- Molecular geometry: Since there are no lone pairs, the molecular geometry is also linear.
- Idealized bond angles: The idealized bond angle is 180°, which corresponds to the linear geometry. No deviation is expected.

3. CH3Br:
- Electron geometry: The central atom (Carbon) is surrounded by four atoms, resulting in a tetrahedral electron geometry.
- Molecular geometry: The molecular geometry is also tetrahedral.
- Idealized bond angles: The idealized bond angle is approximately 109.5°, which corresponds to the tetrahedral geometry. No deviation is expected.

4. BCl3:
- Electron geometry: The central atom (Boron) is surrounded by three atoms, resulting in a trigonal planar electron geometry.
- Molecular geometry: The molecular geometry is also trigonal planar.
- Idealized bond angles: The idealized bond angle is 120°, which corresponds to the trigonal planar geometry. No deviation is expected in this case.

To determine the electron geometry, molecular geometry, and idealized bond angles for each of the given molecules, we need to follow a step-by-step approach. I'll explain the process and then provide the answers for each molecule.

1. PF3:
- First, draw the Lewis structure of the molecule.
- Phosphorus (P) is the central atom, and it has three Fluorine (F) atoms bonded to it.
- The electron geometry around the central P atom is tetrahedral, as it has four electron regions (one lone pair and three bonding pairs).
- The molecular geometry is trigonal pyramidal since one of the electron regions is a lone pair.
- The idealized bond angle is 109.5 degrees.
- There can be deviations from the idealized bond angle due to the presence of lone pairs, creating repulsions that compress the bond angles slightly less than 109.5 degrees.

2. SBr2:
- Again, start by drawing the Lewis structure.
- Sulfur (S) is the central atom, with two Bromine (Br) atoms bonded to it.
- The electron geometry around the central S atom is also tetrahedral (two bonding pairs and two lone pairs).
- The molecular geometry is bent/V-shaped, as the two bonding pairs and two lone pairs repel each other, pushing the Br atoms closer to each other.
- The idealized bond angle is 109.5 degrees.
- Due to the presence of two lone pairs, there will be significant deviations from the idealized bond angle, resulting in a smaller bond angle between the two Br atoms.

3. CH3Br:
- For this molecule, Carbon (C) is the central atom, with one Hydrogen (H) and one Bromine (Br) atom attached to it.
- The electron geometry around the central C atom is tetrahedral (one bonding pair and three lone pairs).
- The molecular geometry is trigonal pyramidal, as there is one bonding pair and one lone pair, which pushes the Br atom closer to the H atom.
- The idealized bond angle is again 109.5 degrees.
- Similar to PF3, due to the presence of a lone pair, there may be deviations from the idealized bond angle, resulting in a slightly smaller bond angle between the C-H and C-Br atoms.

4. BCl3:
- Last but not least, in this molecule, Boron (B) is the central atom, with three Chlorine (Cl) atoms bonded to it.
- The electron geometry around the central B atom is trigonal planar, as there are three bonding pairs.
- The molecular geometry is also trigonal planar, as there are no lone pairs.
- The idealized bond angle is 120 degrees.
- There are no deviations from the idealized bond angle in this case, as there are no lone pairs present.

In summary:
1. PF3: Electron geometry - tetrahedral, Molecular geometry - trigonal pyramidal, Idealized bond angle - 109.5 degrees, Expect deviations from idealized bond angle due to lone pair repulsions.
2. SBr2: Electron geometry - tetrahedral, Molecular geometry - bent/V-shaped, Idealized bond angle - 109.5 degrees, Significant deviations from idealized bond angle due to lone pair repulsions.
3. CH3Br: Electron geometry - tetrahedral, Molecular geometry - trigonal pyramidal, Idealized bond angle - 109.5 degrees, Expect deviations from idealized bond angle due to lone pair repulsions.
4. BCl3: Electron geometry - trigonal planar, Molecular geometry - trigonal planar, Idealized bond angle - 120 degrees, No deviations from idealized bond angle.

Remember, always double-check your results and refer to reliable sources for accurate information.

PF3

SBr2
CH3Br

CHCl3 - should have a bond angle of 109.5 as it is tetrahedral but the actual bond angle between the CH bond and CCl bonds will be less than 109.5 and the angle between CCl bonds will be more than 109.5. This is because the Cl atoms have electrons around them but the H does not so the Cl atoms repel each other and widen the bond angle.

SBr2 should be 104.5 as in H2O but because the Br atoms have electrons around them they will repel each other more than the H atoms in H2O so the bond angle will be more than 104.5

PF3 should be 107 as in NH3 because the F atoms have electrons around them they will repel each other more than the H atoms in NH3 so the bond angle will be more than 107