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Chapter 9: Problem 77

How would we describe a substance that contains only paired electrons and is weakly repelled by a magnetic field? Which of the following ions would you expect to possess similar characteristics: $\mathrm{H}_{2}^{-}, \mathrm{Ne}_{2}^{+}, \mathrm{F}_{2}, \mathrm{O}_{2}^{2+} ?$

Short Answer

Expert verified
A substance with only paired electrons and weakly repelled by a magnetic field is called a diamagnetic substance. Out of the given ions \(\mathrm{H}_{2}^{-}, \mathrm{Ne}_{2}^{+}, \mathrm{F}_{2}, \mathrm{O}_{2}^{2+}\), the ions with similar characteristics to a diamagnetic substance are \(\mathrm{H}_{2}^{-}\) and \(\mathrm{F}_{2}\).

Step by step solution

01

Identify the substance with only paired electrons and weak magnetic repulsion

The substance with only paired electrons and weakly repelled by a magnetic field is called a diamagnetic substance. Diamagnetism arises from the presence of all paired electrons in the substance, causing it to be weakly repelled by an external magnetic field.
02

Check the electronic configuration of \(\mathrm{H}_{2}^{-}\) ion

The hydrogen atom has an atomic number of 1, so its electronic configuration is 1s^1. In a covalent bond, H atoms share electrons. In the \(\mathrm{H}_{2}^{-}\) ion, each hydrogen has one electron and gains one more from the extra negative charge, making a total of 2 electrons in bonding. Thus, the electronic configuration of the \(\mathrm{H}_{2}^{-}\) ion is 1s^2, indicating both electrons are paired. This ion has similar characteristics to a diamagnetic substance.
03

Check the electronic configuration of \(\mathrm{Ne}_{2}^{+}\) ion

The neon atom has an atomic number of 10, so its electronic configuration is 1s^2 2s^2 2p^6. In the \(\mathrm{Ne}_{2}^{+}\) ion, one electron is removed from the atom. The new configuration becomes 1s^2 2s^2 2p^5. All electrons are not paired, indicating this ion does not have similar characteristics to a diamagnetic substance.
04

Check the electronic configuration of \(\mathrm{F}_{2}\) ion

The fluorine atom has an atomic number of 9, so its electronic configuration is 1s^2 2s^2 2p^5. In \(\mathrm{F}_{2}\), each fluorine atom shares one electron with the other. Thus, the resulting electron configuration remains the same, with all fluorine electrons being paired: 1s^2 2s^2 2p^6 for each fluorine atom. So, the \(\mathrm{F}_{2}\) molecule has similar characteristics to a diamagnetic substance.
05

Check the electronic configuration of \(\mathrm{O}_{2}^{2+}\) ion

The oxygen atom has an atomic number of 8, so its electronic configuration is 1s^2 2s^2 2p^4. In the \(\mathrm{O}_{2}^{2+}\) ion, two electrons are removed, and the configuration becomes 1s^2 2s^2 2p^3. All electrons are not paired, indicating this ion does not have similar characteristics to a diamagnetic substance.
06

Conclusion

Out of the given ions \(\mathrm{H}_{2}^{-}, \mathrm{Ne}_{2}^{+}, \mathrm{F}_{2}, \mathrm{O}_{2}^{2+}\), the ions with similar characteristics to a substance with only paired electrons and weakly repelled by a magnetic field (diamagnetic) are \(\mathrm{H}_{2}^{-}\) and \(\mathrm{F}_{2}\).

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Most popular questions from this chapter

(a) Is the molecule \(\mathrm{BF}_{3}\) polar or nonpolar? (b) If you react \(\mathrm{BF}_{3}\) to make the ion \(\mathrm{BF}_{3}^{2-}\), is this ion planar? (c) Does the molecule \(\mathrm{BF}_{2} \mathrm{Cl}\) have a dipole moment?

Determine the electron configurations for \(\mathrm{CN}^{+}, \mathrm{CN}\), and \(\mathrm{CN}^{-}\). (a) Which species has the strongest \(\mathrm{C}-\mathrm{N}\) bond? (b) Which species, if any, has unpaired electrons?

The following is part of a molecular orbital energy-level diagram for MOs constructed from 1 s atomic orbitals. (a) What labels do we use for the two MOs shown? (b) For which of the following molecules or ions could this be the energy-level diagram: $$ \mathrm{H}_{2} \mathrm{He}_{2}, \mathrm{H}_{2}^{+}, \mathrm{He}_{2}^{+}, \mathrm{or} \mathrm{H}_{2}^{-} ? $$ (c) What is the bond order of the molecule or ion? (d) If an electron is added to the system, into which of the MOs will it be added? [Section 9.7\(]\)

Many compounds of the transition-metal elements contain direct bonds between metal atoms. We will assume that the \(z\) -axis is defined as the metal-metal bond axis. (a) Which of the 3 d orbitals (Figure 6.23 ) is most likely to make a \(\sigma\) bond between metal atoms? (b) Sketch the \(\sigma_{3 d}\) bonding and $\sigma_{3 d}^{*}$ antibonding MOs. (c) With reference to the "Closer Look" box on the phases oforbitals, explain why a node is generated in the \(\sigma_{3 d}^{*}\) MO. (d) Sketch the energylevel diagram for the \(\mathrm{Sc}_{2}\) molecule, assuming that only the \(3 d\) orbital from part (a) is important. (e) What is the bond order in \(\mathrm{Sc}_{2} ?\)

Consider the molecule \(\mathrm{BF}_{3}\). (a) What is the electron configuration of an isolated \(\mathrm{B}\) atom? (b) What is the electron configuration of an isolated F atom? (c) What hybrid orbitals should be constructed on the B atom to make the B-F bonds in \(\mathrm{BF}_{3}\) ? (d) What valence orbitals, if any, remain unhybridized on the \(\mathrm{B}\) atom in \(\mathrm{BF}_{3} ?\)
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