Chapter 22: Problem 73

\(\mathrm{SF}_{6}\) exists but \(\mathrm{OF}_{6}\) does not. Explain.

Short Answer

Expert verified

\(\mathrm{SF}_{6}\) exists because sulfur can expand its octet and form six bonds with six fluorine atoms. However, \(\mathrm{OF}_{6}\) does not exist because oxygen, being in the second period, cannot expand its octet due to unavailability of d orbitals for bonding.

Step by step solution

Explain Electron Configuration

The electron configuration of sulfur in the ground state is \(1s^2 2s^2 2p^6 3s^2 3p^4\). After exciting one electron from the 3s orbital to the empty 3d orbital, it becomes \(1s^2 2s^2 2p^6 3s^1 3p^4 3d^1\), which allows it to form six bonds with six fluorine atoms.

Explain Octet Rule

According to the octet rule, atoms tend to combine in such a way that they each have eight electrons in their valence shells, giving them the same electronic configuration as a noble gas. In the case of sulfur, it can expand its octet and accommodate more than 8 electrons. This is because sulfur is in the third period of the periodic table, where vacant d orbitals are available for bonding. Thus, \(\mathrm{SF}_{6}\) is possible because sulfur can expand its octet to form six bonds with fluorine atoms.

Failure of Octet Expansion in Oxygen

Oxygen, however, cannot expand its octet because it's in the second period of the periodic table, which means it does not have access to d orbitals for bonding. This makes it impossible for oxygen to form six bonds with fluorine, which is why \(\mathrm{OF}_{6}\) does not exist.

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\(\mathrm{SF}_{6}\) exists but \(\mathrm{OF}_{6}\) does not. Explain.

Short Answer

Step by step solution

Explain Electron Configuration

Explain Octet Rule

Failure of Octet Expansion in Oxygen

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