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Chapter 23: Problem 6

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?

Short Answer

Expert verified
a) The bigger atom is Cl. b) The molecule with the longer bond length is HCl. c) F in HF has a greater partial charge. d) The dipole moment of HF is larger than that of HCl because the partial charge turns out to be the more important factor in determining the dipole moment, not the bond length.

Step by step solution

01

Determining the Bigger Atom between F and Cl

Looking at the periodic table, Fluorine (F) is in period 2, while Chlorine (Cl) is in period 3. Atoms become larger down a group due to the increasing number of electron shells, hence Chlorine (Cl) is larger than Fluorine (F).
02

Determining the Bond Length

Bond lengths depend on the size of atoms. Larger atoms have longer bond lengths. Since Chlorine (Cl) is larger than Fluorine (F), the bond length \(d\) in HCl is longer than in HF.
03

Determining the Partial Charge

The partial charge on an atom in a molecule depends on its electronegativity. Fluorine (F) is more electronegative than Chlorine (Cl), hence F in HF has a greater partial charge than Cl in HCl.
04

Understanding the Dipole Moment

Dipole moment depends on both bond length and magnitude of the partial charge. However, the partial charge is more important in determining the dipole moment. Given that HF has a greater partial charge than HCl, despite having a smaller bond length, HF will have a higher dipole moment than HCl. The fact that Fluorine attracts electrons more strongly than Chlorine dominates the effect of the bond length.

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Most popular questions from this chapter

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?

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?

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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