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QuestionChemistry

Write a Lewis structure for OF^2, then answer the following questions about the Lewis structure. 1. How many valence electrons does this compound have? 2. How many bonded electrons does this compound have? 3. How many lone pairs of electrons does this compound have? 4. How many single bonds does this compound have?

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Step 1:
Step 1: Draw the Lewis structure for OF^2.

First, find the total number of valence electrons in the OF^2 molecule. Oxygen (O) is in group 6 and has 6 valence electrons, while Fluorine (F) is in group 7 and has 7 valence electrons. There are two Fluorine atoms in the molecule, so the total number of valence electrons is: \text{Total valence electrons} = 6(\text{O}) + 2(7)(\text{F}) = 26 \ \text{valence electrons} Next, place the central atom, which is O, and then add the remaining atoms around it. Place a pair of electrons between each atom to represent a bond. Now, there are 12 electrons left to place as lone pairs on the O and F atoms. Place one lone pair on the O atom and three lone pairs on each F atom to satisfy the octet rule. The Lewis structure should look like this: ```lua F — O — F

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Step 1:
Step 1: Draw the Lewis structure for OF^2.

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Step 1:**Step 1:** Draw the Lewis structure for OF^2.

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Step 1:
Step 1: Draw the Lewis structure for OF^2.