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To draw the Lewis structure of each of the compound, we must first determine how many valence electrons each of them have so we can use those electrons to form bonds or distribute them as lone pairs on the atoms.
• S → Group 6A → 6 valence e-
• F→ Group 7A → 7 valence e- x 6
• Total valence e- = 48 e-
SF6, ClF5, and XeF4 are three compounds whose central atoms do not follow the octet rule. Draw Lewis structures for these compounds.
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Our tutors have indicated that to solve this problem you will need to apply the Octet Rule concept. You can view video lessons to learn Octet Rule. Or if you need more Octet Rule practice, you can also practice Octet Rule practice problems.
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Based on our data, we think this problem is relevant for Professor Tang's class at USF.
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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.