Molecular Geometry of Carbon Monoxide

The video tutorial explains the molecular geometry of carbon monoxide (CO). It begins with the Lewis structure, showing a carbon atom triple-bonded to an oxygen atom, with lone pairs on either side. Due to the presence of only two atoms, CO has a linear molecular geometry. The video further explains that the linear shape is maintained because lone pairs orient themselves to be as far apart as possible. If more atoms were present, the steric number would need to be considered to determine the geometry. The tutorial concludes by reaffirming that CO is a linear molecule.

What is the initial step in determining the molecular geometry of carbon monoxide?

• Measuring the bond length

• Calculating the bond angles

• Drawing the Lewis structure

• Identifying the steric number

Why does carbon monoxide have a linear molecular geometry?

• Due to the presence of multiple lone pairs

• Because it has a bent shape

• Due to the presence of a single bond

• Because it consists of only two atoms

How does the orientation of lone pairs affect the geometry of carbon monoxide?

• They cause the molecule to bend

• They maintain the linear shape

• They create a tetrahedral shape

• They have no effect on the shape

What happens to the lone pairs in carbon monoxide's structure?

• They are ignored in the geometry

• They align in a triangular shape

• They are positioned to maintain maximum distance

• They form a square planar shape

What would need to be considered if carbon monoxide had more than two atoms?

• The color of the atoms

• The speed of molecular movement

• The steric number and additional atoms

• The temperature of the environment

What is the molecular shape of carbon monoxide?

• Bent

• Trigonal planar

• Tetrahedral

• Linear

Who is the presenter of the molecular geometry tutorial?

• Dr. C

• Dr. B

• Dr. D

• Dr. A