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For each of the following two substances NOCl and SF6 answer the following questions:

Draw Lewis dot structure (include all dots necessary for each atom)

a.Identify the name of molecular geometry
b.Identify bond angles
c.Identify the molecular polarity of each substance
d.Calculate the formal charge of S atom in SF6
e.Calculate the formal charge of N atom in NOCl

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There is zero formal charges on nitrogen in NOCl and sulfur in SF6.

The Lewis structure of NOCl is shown in the image attached. The NOCl molecule is bent or angular. The N - O - Cl bond angle in the molecule is about 113°.The molecule is polar, the formal charge on nitrogen is calculated as follows;

FC = 5 - 2 - 6/2 = 0

The Lewis structure of SF6 is shown in the image attached. The molecule is octahedral  hence the bond angle in the molecule is 90°. The molecule is nonpolar because it is symmetrical. The formal charge on sulfur atom is zero.

Learn more: https://brainly.com/question/5624100

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