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Chapter 10: Problem 83

The molecule \(\mathrm{H}_{2} \mathrm{O}_{2}\) has a resultant dipole moment of 2.2 D. Can this molecule be linear? If not, describe a shape that might account for this dipole moment.

Short Answer

Expert verified
No, the molecule \( \mathrm{H}_{2} \mathrm{O}_{2} \) cannot be linear because if it was, its dipole moment would be zero. Instead, it might adopt a 'bent' or 'V' shape that allows it to have a non-zero net dipole moment.

Step by step solution

01

Understand the molecular structure of H2O2

Hydrogen Peroxide (\(H_2O_2\)) is a non-linear molecule. The hydrogen atoms are bound to the oxygen atoms in a way where two single bonds and two pairs of unbonded electrons are around each atom of Oxygen. Consequently, the molecule adopts a bent or V shape. If it was a linear molecule (180 degrees), the dipole moment would be zero because there would be symmetry and the dipole vectors would cancel each other out.
02

Correlate the structure with the dipole moment

A molecule's dipole moment depends on the bond dipoles' direction and bond strength. In a linear structure, the net dipole moment could be zero as the bond dipoles would cancel each other, but for a molecule to have a non-zero dipole value, it cannot be linear and there should be some asymmetry in the structure. In this case, \(H_2O_2\) has a dipole moment of 2.2D, so the molecule can't be linear because a linear structure would mean a dipole moment of zero.
03

Describe a possible shape for the molecule

The bent or 'V' shaped structure of Hydrogen Peroxide is an arrangement that allows for a non-zero net dipole moment. This is because the electronegativity difference between Oxygen and Hydrogen causes each \(O-H\) bond to be polar, and the angles between these bonds cause the dipoles to not cancel out entirely. This results in a resultant dipole moment in one direction, giving the molecule polarity.

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Most popular questions from this chapter

Use the \(\mathrm{NH}_{3}\) molecule as an example to explain the difference between molecular geometry and electron-group geometry.

Each of the following molecules contains at least one multiple (double or triple) covalent bond. Give a plausible Lewis structure for (a) \(\mathrm{OCS} ;\) (b) \(\mathrm{CH}_{3} \mathrm{CHO}\) (c) \(\mathrm{F}_{2} \mathrm{CO} ;\) (d) \(\mathrm{Cl}_{2} \mathrm{SO} ;\) (e) \(\mathrm{C}_{2} \mathrm{H}_{2}\).

The greatest bond length is found in (a) \(\mathrm{O}_{2} ;\) (b) \(\mathrm{N}_{2}\) (c) \(\mathrm{Br}_{2} ;\) (d) BrCl.

Each of the following ionic compounds consists of a combination of monatomic and polyatomic ions. Represent these compounds with Lewis structures. (a) \(\mathrm{Al}(\mathrm{OH})_{3}\); (c) \(\mathrm{NH}_{4} \mathrm{F}\); (d) \(\mathrm{KClO}_{3}\); (b) \(\mathrm{Ca}(\mathrm{CN})_{2}\); (e) \(\mathrm{Ba}_{3}\left(\mathrm{PO}_{4}\right)_{2}\).

Assign formal charges to the atoms in the following species, and then select the more likely skeletal structure. (a) \(\mathrm{H}_{2} \mathrm{NOH}\) or \(\mathrm{H}_{2} \mathrm{ONH}\) (b) SCS or CSS (c) NFO or FNO (d) \(\mathrm{SOCl}_{2}\) or \(\mathrm{OSCl}_{2}\) or \(\mathrm{OCl}_{2} \mathrm{S}\) (e) \(\mathrm{F}_{3} \mathrm{SN}\) and \(\mathrm{F}_{3} \mathrm{NS}\)
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