Carbon Monoxide Properties and Bonding

The video explores whether carbon monoxide (CO) is a polar or non-polar molecule. It begins with the Lewis structure of CO, showing a triple bond between carbon and oxygen. The molecular geometry is linear, and the video examines the electronegativity difference between carbon and oxygen. Since the difference is greater than 0.5 but less than 2, CO is determined to be a polar covalent molecule. The oxygen atom, being more electronegative, carries a partial negative charge, while the carbon atom has a partial positive charge. This makes CO a polar molecule.

What is the main question addressed in the video regarding carbon monoxide?

• Whether CO is a metal or non-metal

• Whether CO is reactive or inert

• Whether CO is a polar or non-polar molecule

• Whether CO is a solid or gas

What type of bond is present between carbon and oxygen in CO?

• Single bond

• Double bond

• Triple bond

• No bond

How many pairs of electrons are shared between carbon and oxygen in CO?

• Two pairs

• One pair

• Three pairs

• Four pairs

What is the molecular geometry of carbon monoxide?

• Bent

• Trigonal planar

• Linear

• Tetrahedral

Why is the geometry of CO described as linear?

• Because it forms a straight line

• Due to the presence of lone pairs

• Because of the single bond

• Due to its tetrahedral shape

What is the electronegativity value of carbon?

• 2.55

• 3.44

• 1.00

• 4.00

What is the electronegativity value of oxygen?

• 2.55

• 4.00

• 3.44

• 1.00

What determines the polarity of a molecule like CO?

• The color of the atoms

• The atomic mass

• The difference in electronegativity

• The number of atoms

Why does oxygen in CO have a partial negative charge?

• Because it is less electronegative

• Because it is larger in size

• Because it is more electronegative

• Because it has more protons