Place the following compounds in order of increasing strength of intermolecular forces. co2 f2 nh2ch3 a) nh2ch3 < co2 < f2 b) f2 < nh2ch3 < co2 c) nh2ch3 < f2 < co2 d) f2 < co2 < nh2ch3

It should be D) since NH2CH3 has hydrogen atoms in the formula, it will tend to be polar-so dipole-dipole, dispersion forces are always there, and then hydrogen bonding is the strongest intermolecular force. There are no Ion-dipole attractions present in any of these compounds. F2 should have the weakest strength in Intermolecular forces, since it is not polar so only dispersion forces should be found present. Which leaves CO2 to be in the middle with Dipole-dipole attractions and dispersion forces.

D)  F2 < CO2 < NH2CH3

Explanation:

NH2CH3 - strongest due to the hydrogen bonds (other bonds are present but the Hydrogen bonds are key as it has the strongest attraction)

CO2 -  Second strongest due to Dipole-Dipole attraction and London dispersion

F2 - Weakest - Nonpolar, so only dispersion forces are in effect.

atomic number of carbon is 6

electronic configuration of carbon is 1s²2s²2p²

orbital diagram of c is as shown here in the image.