CO2 has zero dipole moment while CO has dipole moment. why?

Answer 1

For this, you need to look at the lewis dot structure of CO2. Remember it is a linear molecule with two Carbon Oxygen double bonds. O = C = O
As it says, there is a pull for the electrons to go towards the oxygens because oxygen is more electronegative (has a higher desire for the electrons to be around it). However, the oxygen on the left pulls with the same amount of force as the oxygen on the right. So, the pulls are equal and opposite, making them exactly cancel each other out. Therefore, there is no net dipole moment for the molecule.

Answer 2

CO is formed when C and O are bonded by a triple bond with 2 lone pairs. Oxygen being more electronegative attracts the bonded pair of electrons towards itself, acquiring a negative charge, and carbon acquiring a positive charge, which resluts in the dipole moment.
But in case of CO2, the central C atom forms double bond with both O atoms.
O = C = O
Oxygen is more electronegative and attracts the bonded pair of electrons towards itself , on both sides of C atom. Hence an equal neutral charge is acquired on the CO2 molecule. The presence of 2 lone pairs on each O atom results in the orbital dipole moment to be opposite to the direction of the resultant dipole moment. This orbital dipole moment being equal and opposite to the resultant dipole moment results in cancelling of the charges and zero dipole moment on CO2 molecule.

Answer 3

becuze.... the two oxygen cacelled out the dipole moments... as you know, O is more electronegetive than carbon so, the moments go to the opossite direction... and actually, the dipole moment of CO2 is not completly zero... some times they have...
and CO... the dipole moment just move towards O (which is more Enegative). Ü