How many of the following molecules have sp 3 d 2 hybridization on the central atom? SeCl 6 XeCl 4 IF 5 AsCl 5

Many of the following molecules have s p 3d2 hybridization on the central atom? So if we were to add up s p 3d2, so this would be 1 plus 3 plus 2, which gives me 6. This would mean that our central element has 6 electron groups attached to it. Remember, these electron groups could be in the form of surrounding elements or lone pairs. So if we take a look here, we have selenium connected to 6 chlorines. Selenium is in group 6 a, so it has 6 valence electrons. The chlorines are in group 7 a. They only make single bonds when they are surrounding elements. So if we're drawing this out, once we're done drawing we'll see that chlorine well, we'll see that selenium has 6 groups around it, and therefore would have a hybridization of s p 3d2. So this one for sure is an answer. Next, we have xenon tetrachloride. Xenon is in group 8 a, so it has 8 valence electrons. It's gonna use 4 of them to make single bonds with the chlorines. So here go our chlorines. Now xenon has used 4 out of its 8 valence electrons so it has 2 lone pairs, 1 up here and 1 down here. In total, xenon has around it, what, 1, 2, 3, 4, 5, 6 electron groups as well. So it would also be s p 3d2 on the xenon atom. Next, we have I f 5, so we have iodine here. It is connected to the 5 fluorines, and here's our lone pair that it still would possess. So we have our fluorines, So here we're drawing our fluorines here. Now if we looked at the total number of electronic groups around the iodine, we have how many? 1, 2, 3, 4, 5, 6 as well. So this would also be s p 3d2. So, finally, we have arsenic in the center, and arsenic is connected to 5 chlorines. Right? So we know that the coins are mixed single bonds. So when we do that, we would see now that arsenic does not have 6 groups around it, only has 5. And so its hybridization wouldn't be s p 3d2, it would just be s p 3d. So this would not be an option. So we can see here that 3 of our molecules would have a central element with a hybridization of s p 3d2, making option a our correct answer.

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12. Molecular Shapes & Valence Bond Theory

Hybridization

General Chemistry

12. Molecular Shapes & Valence Bond Theory

Hybridization

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Multiple Choice

How many of the following molecules have sp³d² hybridization on the central atom?
SeCl₆ XeCl₄ IF₅ AsCl₅

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Verified step by step guidance

Step 1: Understand the concept of hybridization. Hybridization is the process of mixing atomic orbitals to form new hybrid orbitals suitable for the pairing of electrons to form chemical bonds in molecules. The sp3d2 hybridization involves the mixing of one s orbital, three p orbitals, and two d orbitals.

Step 2: Analyze the molecular geometry and electron pair arrangement for each molecule. The sp3d2 hybridization typically corresponds to an octahedral geometry, which involves six electron pairs around the central atom.

Step 3: Examine SeCl6. Selenium (Se) is the central atom surrounded by six chlorine (Cl) atoms. This configuration suggests an octahedral geometry, indicating sp3d2 hybridization.

Step 4: Examine XeCl4. Xenon (Xe) is the central atom surrounded by four chlorine (Cl) atoms and two lone pairs. This results in a square planar geometry, which does not correspond to sp3d2 hybridization.

Step 5: Examine IF5 and AsCl5. Both iodine (I) in IF5 and arsenic (As) in AsCl5 have five bonded atoms and one lone pair, leading to a square pyramidal geometry. This geometry is consistent with sp3d2 hybridization.