Question

Which of the following statements is true regarding a covalent bond in CO?

Valence electrons are transferred to the oxygen atom.

The bond length is less than the sum of the two atomic radii.

Bonding electrons are stationary in the CO molecule.

all of the above

none of the above
( I picked the third one am I correct?)

Answer 1

Electrons are NEVER EVER stationary. They act as both waves and particles at the same time. They are always in motion, and this is why they have their energies and can therefore perform chemical reactions :)

On the other hand, let's look at the other two statements. We know that the carbon-oxygen bond is covalent, which is SHARING electrons, not transferring them, so that statement is false.

But... what are bonds? Forces that hold atoms together. So logically, if there is a bond between two atoms, the force of the bond will attract the two atoms closer together than their outermost electrons, no? This is why all covalent bonds are shorter than the sums of the atomic radii: the forces pull the atoms closer together. So the correct answer is B. :)

Answer 2

They are not revolving around the nucleus like planets around the sun, rather, they are more of clouds. As you go higher in chemistry and start getting into physical chemistry, you will be introduced to a more detailed explanation, as well as heisenbergs uncertainty principle. then add on to that wave function \(\psi\) of an electron and you end up with a cloud of where they might be. It's quite interesting, but very complex.