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
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Total Valence e⁻s
20Step 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
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16Now, distribute remaining 16 electrons on each element to complete its
octet starting from most electronegative element.
Lewis structure of OF₂ is as follow,
Solids have a definite shape and definite volume. This means that the shape of the material does not change, and it can't be compressed.
Relatively few hydrogen atoms
The value of Kc for the equilibrium is 0.150 mole² / litre ²
<u>Explanation:</u>
<u>Given:</u>
An equilibrium mixture in an 1.00 L vessel contains 5.30 moles of
Mg(OH )₂ 0.800 moles of Mg²⁺ and 0.0010 moles OH₋
We have to find the value of Kc
- Step 1: Find the equilibrium Concentration.
- Step 2: Substitute the values in the equation.
- Step 3: Find the value of Kc.
- I have attached the document for the detailed explanation
The value of Kc for the equilibrium is 0.150 mole² / litre ²