Understanding Molecular Geometry and Electron Pair Arrangement

1. 3 Electron Pairs No Lone Pairs

Tetrahedral. Bond Angle 109.5

Linear. Bond Angle 180

Trigonal Planar. Bond Angle 120

Octahedral. Bond Angle 90

A molecule with 3 electron pairs and no lone pairs will exhibit a trigonal planar geometry with a bond angle of 120 degrees. This arrangement allows for optimal electron repulsion and stability.

Explanation

A molecule with 3 electron pairs and no lone pairs will exhibit a trigonal planar geometry with a bond angle of 120 degrees. This arrangement allows for optimal electron repulsion and stability.

2. How is the molecular geometry described for a molecule with 4 electron pairs and no lone pairs?

Octahedral. Bond Angle 90.

Trigonal Planar. Bond Angle 120.

Tetrahedral. Bond Angle 109.5

Linear. Bond Angle 180.

A molecule with 4 electron pairs and no lone pairs exhibits tetrahedral molecular geometry with a bond angle of 109.5 degrees.

Explanation

A molecule with 4 electron pairs and no lone pairs exhibits tetrahedral molecular geometry with a bond angle of 109.5 degrees.

3. What is the molecular geometry of a molecule with 2 electron pairs on the central atom?

Linear. Bond Angle 180

Trigonal Planar. Bond Angle 120

Tetrahedral. Bond Angle 109.5

Bent. Bond Angle 109.5

A molecule with 2 electron pairs on the central atom adopts a linear geometry with a bond angle of 180 degrees. This is due to the repulsion between the electron pairs, resulting in a straight line shape.

Explanation

A molecule with 2 electron pairs on the central atom adopts a linear geometry with a bond angle of 180 degrees. This is due to the repulsion between the electron pairs, resulting in a straight line shape.

4. How would you describe a molecule with 4 electron pairs and one lone pair?

Linear. Bond Angle 180.

Tetrahedral. Bond Angle 109.5.

Bent. Bond Angle

Trigonal Pyramidal. Bond Angle 107

A molecule with 4 electron pairs and one lone pair exhibits a trigonal pyramidal shape with a bond angle of 107 degrees. This configuration results in a distorted tetrahedral geometry.

Explanation

A molecule with 4 electron pairs and one lone pair exhibits a trigonal pyramidal shape with a bond angle of 107 degrees. This configuration results in a distorted tetrahedral geometry.

5. How would you describe a molecule with 4 electron pairs and two lone pairs?

Tetrahedral. Bond Angle 109.5.

Trigonal Planar. Bond Angle 120.

Linear. Bond Angle 180.

Bent. Bond Angle 104.5

In this case, the molecule is bent due to the presence of two lone pairs, with a bond angle of approximately 104.5 degrees.

Explanation

In this case, the molecule is bent due to the presence of two lone pairs, with a bond angle of approximately 104.5 degrees.

6. What is the molecular geometry of a molecule with 3 electron pairs and one lone pair?

Linear. Bond Angle 180.

Bent. Bond Angle 120

Trigonal Planar. Bond Angle 120.

Tetrahedral. Bond Angle 109.5

In this case, with 3 electron pairs and one lone pair, the molecular geometry is bent with a bond angle of 120 degrees. This arrangement results in a non-linear shape.

Explanation

In this case, with 3 electron pairs and one lone pair, the molecular geometry is bent with a bond angle of 120 degrees. This arrangement results in a non-linear shape.

7. 5 Electron Pairs. No Lone Pairs.

Trigonal Bypyramidal. Bond Angle 90 and 120

Octahedral. Bond Angle 90.

Tetrahedral. Bond Angle 109.5.

Linear. Bond Angle 180.

In this scenario, with 5 electron pairs and no lone pairs, the correct molecular geometry is trigonal bipyramidal. This geometry consists of 5 electron pairs arranged around the central atom with bond angles of approximately 90 degrees between axial bonds and 120 degrees between equatorial bonds.

Explanation

In this scenario, with 5 electron pairs and no lone pairs, the correct molecular geometry is trigonal bipyramidal. This geometry consists of 5 electron pairs arranged around the central atom with bond angles of approximately 90 degrees between axial bonds and 120 degrees between equatorial bonds.