Question

How many of the following molecules are polar? xeo2 sicl2br2 c2br2 secl6 a) 1 b) 4 c) 2 d) 3

Answer 1

XeO2, SiCl2Br2, and SeCl6 are polar molecules with polar bonds.

Step-by-step explanation:

In order to determine if a molecule is polar, we need to consider the shape and the polarity of the individual bonds within the molecule. If the molecule has a symmetrical shape and all the individual bonds are nonpolar, then the molecule is nonpolar. Let's analyze each molecule:

XeO2: This molecule has a bent shape and the Xe-O bonds are polar. Therefore, XeO2 is polar.

SiCl2Br2: This molecule has a tetrahedral shape and the Si-Cl and Si-Br bonds are polar. Therefore, SiCl2Br2 is polar.

C2Br2: This molecule has a linear shape and the C-Br bonds are nonpolar. Therefore, C2Br2 is nonpolar.

SeCl6: This molecule has an octahedral shape and the Se-Cl bonds are polar. Therefore, SeCl6 is polar.

From the analysis, we can see that molecules XeO2, SiCl2Br2, and SeCl6 are polar. Therefore, the correct answer is

(d) 3

.

Answer 2

The molecules XeO2, SiCl2Br2, and SeCl6 are polar. The correct answer is (d) 3.

Step-by-step explanation:

To determine if a molecule is polar, we need to consider the geometry of the molecule and the polarity of the bonds. A polar bond is formed between atoms with different electronegativities, causing an uneven distribution of electron density. If a molecule has a symmetric shape and all its bonds are nonpolar, it will be nonpolar. Based on the provided molecules, the polar ones are XeO2, SiCl2Br2, and SeCl6. Therefore, the correct answer is (d) 3.

SeCl6's molecular structure is octahedral. The Se-Cl bonds are polar, and the particle is nonpolar by and large in light of the fact that the polar bonds are evenly organized around the focal selenium iota.