Sulfur dioxide molecule contains one sulfur atom or two oxygen atoms. We would construct the lewis structure of the SO2 molecule by following VSEPR theory rules or considering stability of the intermediate structures. After obtaining the lewis structure of the SO2, we may determine the hybridization of the atoms.
Sulfur dioxide SO2
Sulfur dioxide is the the colourless inorganic gas or also the toxic gas. this gives the weak acid solution if dissolves in the water. This gas is the produced due to the combustion of the petroleum fuel in the automobiles or industrial factories.
Lewis structure of the SO2
There are the two double bonds between sulfur atom or oxygen atoms in the SO molecule. Also, the lone pair exists on the sulfur atom or each oxygen atom has two lone pairs in the SO2 lewis structure.
Hybridization of the SO2
All atoms have sp2 hybridization. Each oxygen atom has one sigma bond or two lone pairs. Therefore, oxygen atoms’ hybridization should be sp2. for the sulfur atom, there are the two sigma bonds or one lone pair to the make hybridization sp2. Simple method to the determine the hybridization of the atoms in the covalent compounds.
Apply VSEPR theory - Steps of the drawing lewis structure of the SO2
Following steps are the used to the draw the lewis structure of the SO2. Each step is the explained in the detail in the next sections. If you are the beginner to the lewis structure drawing, follow these sections slowly or properly to the understand this completely. Look the figures to the understand each step.
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Find total number of the electrons of the the valance shells of the sulfur or oxygen atoms
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Total electrons pairs
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Center atom selection
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Put lone pairs on the atoms
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Check the stability or minimize charges on the atoms by converting lone pairs to the bonds until most stable structure is the obtained.
Total number of the electrons of the valance shells of the ethene
Both sulfur or oxygen belongs to the group VIA elements series. Therefore, they have six electrons in the their valence shell. to the find number of the valence electron, these valence electrons of the each element should be multiplied with the their respective number of the atoms in the molecule. Below, this step are the done.
• Total valence electrons given by two oxygen atoms = 6 * 2 = 12
• Total valence electrons given by sulfur atom = 6 * 1 = 6
There are the no charges in the SO2 molecule. Therefore, no addition or reduction of the valence electrons due to the charges.
• Total valence electrons = 12 + 6 = 18
Total valence electrons pairs
Total valance electrons pairs = σ bonds + π bonds + lone pairs at the valence shells. Total electron pairs are the determined by dividing the number total valence electrons by two. For, SO2 molecule, Total number of the pairs of the electrons are the 9.
Center atom or sketch of the ethene molecule
There are the few requirements to the be the center atom. Having the high valence is the the main requirement to the be the center atom. for the SO2 molecule, sulfur has the highest valence than or oxygen.
Mark lone pairs on the atoms
After drawing the sketch, we should start to the mark lone pairs on the atoms. In the drawn sketch, there are the two bonds. between atoms.
• There are the already two S-O bonds in the the above sketch. Now, there are the just seven (9-2 = 7) valence electrons pairs are the remaining to the draw (as mark lone pairs) the rest of the structure.
• First, mark remaining valence electrons pair as the lone pairs on the oxygen atoms (outside atoms). Six valence electron pairs are the marked on the two oxygen atoms. Now, there are the still one valence electron pair is the remaining. this is the marked on the sulfur atom as the lone pair.
• Now, all valence electron pairs are the marked as bonds or lone pairs in the sketch.
Charges on the atoms
Charges on the atoms are the important to the find the most stable structure. Therefore, we need to the find the most stable structure to the obtain lewis structure. Therefore, we should try to the find charges if there are.
After, marking electron pairs on the atoms, we should mark charges of the each atom. Each oxygen atoms would take the -1 charge or sulfur atom take the +2 charge. Because SO2 is the neutral molecule, overall charge of the molecule should be zero. The overall charge of the molecule is, (-1) * 2 + (+2) = 0.
Stability of the structure or minimize charges on the atoms by converting lone pairs to the bonds
When there are the positive or negative charges on the lot of the atoms or higher charges (like +2, +3, -2, -3) on the atoms in the an ion or molecule, this structure is the not stable. Therefore, We should try to the reduce charges on the atoms if this is the possible. in the thee above structure, there are the charges on the oxygen atoms or sulfur atom. Now, we are they going to the reduce charges on the these atoms as below.
• Now, we should try to the minimize charges by converting the lone pair or pairs to the bond. So convert the lone pair on the oxygen atom to the make the new S-O bond with the sulfur atom as the following figure.
• Now there is the double bond between one oxygen atom or sulfur atom. You may see, charges are the reduced now in the new structure.
• Because, there are the still charges on the atoms, we may try to the convert the lone pair to the bond. So, convert the lone pair on the other oxygen atom to the make the bond with the sulfur atom. with the that, there are the no charges on the sulfur or oxygen atoms.
• Therfore, this structure should be the lewis structure of the SO2
How many lone pairs sulfur has in the SO2
There is the just one lone pair on the valence shell of the sulfur atom.
SO2 lewis structure lone pairs
There are the lone pairs on the all atoms in the SO2. Sulfur atom has one lone pair or each oxygen atom has two lone pairs. Therefore, there are the total of the five lone pairs on the last shells of the each atom in the SO2.
What are the other similar lewis structures of the SO2?
If we consider the shape of the SO2, water, nitrogen dioxide, hydrogen sulfide, ozone have similar shape, bent. Also, if number of the sigma bonds are the is the considered, water, nitrogen dioxide, hydrogen sulfide, sulfur dioxide all have two sigma bonds. Both SO2 or ozone has one lone pair on the center atom.
Are there similarities in the SO2 or NO2 lewis structures?
Actually, this question is the weird one. Rather than discussing similarities, it’s good to the discuss their differences. in the NO2 lewis structure, there is the an unpaired electron on the nitrogen atom.
What are the similarities or differences in the SO2 or SO3 lewis structures?
• Around sulfur atom, summation of the lone pair or sigma bonds is the three in the both SO2 or SO3. Therefore, sulfur atom has sp2 hybridization.
• But, shapes around sulfur atom in the SO2 or SO3 are the different. in the SO2, shape around sulfur atom is the bent. But in the SO3, shape is the trigonal planar.