Oxygen difluoride is a powerful oxidizing and fluorinating agent. select its lewis structure.
1 answer:
Lewis Structure of Oxygen Difluoride is sketched as....
Step 1:
Calculate the total number of valence electrons present in OF₂. This is done by adding all valence electrons of each element. i.e...
Valence e⁻s of Oxygen = 6
Valence e⁻s of Fluorine-1 = 7
Valence e⁻s of Fluorine-2 = 7
------------
Total Valence e⁻s 20
Step 2:
Draw central element (O) in center surrounded by fluorine atoms. Now, sketch a single bonds between O and both F atoms. Now, subtract 2 electrons per single bond from total valence electrons.. i.e..
Total Valence e⁻s = 20
2 single bonds (2 × 2) = 4
-----------
16
Now, distribute remaining 16 electrons on each element to complete its octet starting from most electronegative element.
Lewis structure of OF₂ is as follow,
Step 1:
Calculate the total number of valence electrons present in OF₂. This is done by adding all valence electrons of each element. i.e...
Valence e⁻s of Oxygen = 6
Valence e⁻s of Fluorine-1 = 7
Valence e⁻s of Fluorine-2 = 7
------------
Total Valence e⁻s 20
Step 2:
Draw central element (O) in center surrounded by fluorine atoms. Now, sketch a single bonds between O and both F atoms. Now, subtract 2 electrons per single bond from total valence electrons.. i.e..
Total Valence e⁻s = 20
2 single bonds (2 × 2) = 4
-----------
16
Now, distribute remaining 16 electrons on each element to complete its octet starting from most electronegative element.
Lewis structure of OF₂ is as follow,
You might be interested in
Answer:
<h2>The answer is 4.0 g/mL</h2>Explanation:
The density of a substance can be found by using the formula
From the question
mass = 40 g
volume = 10 mL
The density of the object is
We have the final answer as
<h3>4.0 g/mL</h3>Hope this helps you
Answer:
<h2>Explanation:
<u>First of all cross multiply</u>
That's
<u>Next divide both sides by </u><u> in order to isolate </u>
We have
We have the final answer as
Hope this helps you