How would you describe the strength of the bonds that result from resonance in SO3?
1 answer:
Answer:
All bonds are equivalent in length and strength within the molecule.
Gaseous SO3 is a trigonal planar molecule that exhibit a D3h symmetry group.
Sulfur has sp2 hybridization and it has 6 outer electrons which make the bonds with the oxygen.
Its constituent sulfur atom has an oxidation state of +6 and a formal charge of 0.
The Lewis structure is made up of one S=O double bond and two S–O dative bonds that doesn't not engage the d-orbitals. ( Thus, SO3 molecule has three double bonded oxygen to the central sulfur atom). This explains the strength.
It gaseous form had a zero electrical dipole moment because of the 120° angle between the S-O bonds.
Explanation:
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Answer:
Brown color of the solution decreases
Explanation:
is brown in color whereas
is colorless.
Equilibrium reaction between and
is as follows:
As per the Le Chatelier's principle, if pressure of a equilibrium is increased, the equilibrium will shift in the direction having fewer no. of moles of gases.
In the given equilibrium, side has more no. of moles. So on increasing pressure, equilibrium will shift towards the side of
or more formation of
will take place.
Therefore, more will decompose that will decrease the brown color of the solution as
is colorless.