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Chapter 23: Problem 2

The \(\mathrm{CO}_{2}\) molecule is linear (OCO) and has polar bonds. a) Where is the center of positive charge? b) Where is the center of negative charge? c) Why is the dipole moment for this molecule equal to zero?

Short Answer

Expert verified
a) The center of positive charge is the carbon atom. b) The centers of negative charge are the oxygen atoms. c) Although \(\mathrm{CO}_{2}\) has polar bonds, it has no dipole moment due to the symmetrical linear geometry that cancels out the individual bond dipoles.

Step by step solution

01

Identify the Centers of Charges

a) The center of positive charge in a molecule is typically where the 'electron-deficient' atoms are. In the \(\mathrm{CO}_{2}\) molecule, the positive center is at the carbon atom. It does not share its electrons completely equally with oxygen, so it carries a small positive charge. \n b) The center of negative charge is the atom where the electrons spend most of their time. In the \(\mathrm{CO}_{2}\) molecule these will be the oxygen atoms, due to oxygen being more electronegative than carbon.
02

Explanation of Zero Dipole Moment

c) Even though the bonds are polar in \(\mathrm{CO}_{2}\), the molecule itself has no dipole moment. This is due to the symmetrical linear geometry of the CO2 molecule. There are two bond dipoles that are equal in magnitude but oppositely directed that create a net zero dipole moment for the entire molecule.

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Most popular questions from this chapter

Consider HF and HCl: a) Which is the bigger atom, \(\mathrm{F}\) or \(\mathrm{Cl}\) ? b) Which has the longer bond length, \(d\), HF or HCl? c) Which has the greater partial charge- \(\mathrm{F}\) in \(\mathrm{HF}\) or \(\mathrm{Cl}\) in \(\mathrm{HCl} ?\) (Hint: which is more electronegative- \(\mathrm{F}\) or \(\mathrm{Cl} ?\) ) d) Why is the dipole moment of HF larger than the dipole moment of HCl? That is, which appears to be the more important factor in determining the dipole moment: the bond length or the partial charge?

The \(\mathrm{CO}_{2}(\mathrm{OCO})\) and \(\mathrm{OCS}\) molecules are both linear. Both have polar bonds. \(\mathrm{CO}_{2}\) does not have a dipole moment (that is, the dipole moment is zero). Why does OCS have a dipole moment?

Consider the \(\mathrm{CCl}_{4}\) molecule. a) Are the \(\mathrm{C}-\mathrm{Cl}\) bonds in \(\mathrm{CCl}_{4}\) polar? b) Where is the center of positive charge? c) Where is the center of negative charge? d) Why is the dipole moment zero for \(\mathrm{CCl}_{4}\) ?
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