Expanded Octets & Odd Electron Molecules: PCl5, SF6 Breaking the Octet Rule

The video tutorial explains the concept of expanded octet, where a central atom in a compound has more than 8 electrons. It highlights examples like phosphorus pentachloride (PCL5), sulphur hexafluoride (SF6), and iodine heptafluoride (IF7). The tutorial further delves into the electron configuration of sulphur in SF6, illustrating how it accommodates more than 8 electrons. Additionally, the video covers odd electron molecules, such as nitrogen dioxide (NO2) and chlorine dioxide (ClO2), which do not satisfy the octet rule due to having an odd number of electrons. These molecules are described as free radicals and are highly reactive.

What are odd electron molecules and how do they differ from typical molecules?

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Describe the reaction that occurs when two nitrogen dioxide molecules collide.

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