In a Lewis structure, the atom that requires the most additional electrons to reach a full octet is typically placed in the center. In the case of SO₂, sulfur is in the middle because it is less electronegative than oxygen and can form more bonds (up to 6) due to its ability to have an expanded octet. Here are the steps to draw the Lewis structure for SO₂:

1. Count the total number of valence electrons. Sulfur has 6 and oxygen has 6, but since there are two oxygen atoms, the total number of valence electrons is 18.

2. Draw a skeleton structure of the molecule. Sulfur is the central atom and the two oxygen atoms are adjacent to it.

3. Distribute the electrons among the atoms. Each bond (line) represents two electrons. After forming single bonds between sulfur and the two oxygen atoms, we have 12 electrons left.

4. Place the remaining electrons on the outer atoms (oxygen) first to fill their octets. Each oxygen atom needs 6 more electrons, so we use up all 12 remaining electrons.

5. If there are any electrons left, place them on the central atom. In this case, there are no electrons left.

6. If the central atom does not have a full octet, form double or triple bonds until it does. In this case, sulfur only has 4 electrons, so we form a double bond with one of the oxygen atoms.

So, the Lewis structure of SO₂ has sulfur in the middle with a double bond to one oxygen atom, a single bond to the other oxygen atom, and two lone pairs of electrons on each oxygen atom.

Question

In a Lewis structure, the atom that requires the most additional electrons to reach a full octet is typically placed in the center. In the case of SO₂, sulfur is in the middle because it is less electronegative than oxygen and can form more bonds (up to 6) due to its ability to have an expanded octet. Here are the steps to draw the Lewis structure for SO₂:

1. Count the total number of valence electrons. Sulfur has 6 and oxygen has 6, but since there are two oxygen atoms, the total number of valence electrons is 18.

2. Draw a skeleton structure of the molecule. Sulfur is the central atom and the two oxygen atoms are adjacent to it.

3. Distribute the electrons among the atoms. Each bond (line) represents two electrons. After forming single bonds between sulfur and the two oxygen atoms, we have 12 electrons left.

4. Place the remaining electrons on the outer atoms (oxygen) first to fill their octets. Each oxygen atom needs 6 more electrons, so we use up all 12 remaining electrons.

5. If there are any electrons left, place them on the central atom. In this case, there are no electrons left.

6. If the central atom does not have a full octet, form double or triple bonds until it does. In this case, sulfur only has 4 electrons, so we form a double bond with one of the oxygen atoms.

So, the Lewis structure of SO₂ has sulfur in the middle with a double bond to one oxygen atom, a single bond to the other oxygen atom, and two lone pairs of electrons on each oxygen atom.

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