How do you use a Lewis Structure to find the oxidation state of an element. I have this question using the oxidation rule i got +2, however how do i use it with Lewis structure.

QUESTION
Use the Lewis structure of a thiosulfate ion to find the oxidation number of each sulfur atom.

What are the advantages and disadvantages of using Lewis structures to assign oxidation numbers?

What are the advantages and disadvantages of using the oxidation number rules to assign oxidation numbers?

It takes a little reading and scrolling down the page but the S2O3^= ion is shown and the Lewis structure oxidation states are listed and explained. The first part of the article shows how the non-Lewis method is used.

Notice that the article starts out by suggesting that we not confuse oxidation state and oxidation number.
http://en.wikipedia.org/wiki/Oxidation_state

Assign oxidation numbers to each atom in the following compounds:

HI
pbr3
ges2
kh
as2o5

 T

To use Lewis structures to find the oxidation state of an element, you need to understand the concept of oxidation state and how it relates to the Lewis structure. Here's how you can determine the oxidation state using Lewis structures:

Step 1: Draw the Lewis structure of the molecule or ion in question. In this case, you have a thiosulfate ion, which has the chemical formula S2O3^2-. To draw the Lewis structure, you assign single bonds between sulfur (S) and oxygen (O) atoms.

S-O-S
/
O-S^2-

Step 2: Count the number of valence electrons for each atom. Sulfur has 6 valence electrons, while each oxygen atom has 6 valence electrons. Multiply the number of oxygen atoms by 2 since there are two oxygen atoms.

Total valence electrons = (6 for sulfur) + (6 x 2 for oxygen) + (2 for the negative charge) = 22

Step 3: Distribute the valence electrons around the Lewis structure, starting with the most electronegative atom. In this case, oxygen is more electronegative than sulfur. Place two electrons between each sulfur-oxygen bond and complete the octets of oxygen atoms.

S-O-S
|
O-S^2-

Step 4: Allocate any remaining electrons to satisfy the octet rule for each atom. In this case, there are no remaining electrons.

Step 5: Determine the formal charge of each atom. The formal charge of an atom is equal to the number of valence electrons minus the non-bonding electrons minus half of the bonding electrons. For sulfur and oxygen, the formal charges are as follows:

Sulfur (S): Formal charge = 6 - 0 - (8 ÷ 2) = 0
Oxygen (O): Formal charge = 6 - 2 - (4 ÷ 2) = 0

Since the formal charges on both sulfur atoms are zero, the oxidation states of both sulfur atoms in the thiosulfate ion are also zero.

Advantages and disadvantages of using Lewis structures to assign oxidation numbers:

Advantages:
1. Lewis structures provide a visual representation of the molecule or ion, making it easier to understand the arrangement of atoms and electrons.
2. They can help identify the distribution of electrons and how they participate in chemical bonds.
3. Lewis structures allow for the determination of formal charges, which can be used to assign oxidation numbers.

Disadvantages:
1. Lewis structures may not accurately represent the actual 3D shape of a molecule or ion.
2. They require knowledge of the molecule's or ion's bonding pattern, which can be challenging for complex molecules.
3. Lewis structures rely on the octet rule, which may not always be satisfied for certain elements or in certain chemical environments.

Advantages and disadvantages of using the oxidation number rules to assign oxidation numbers:

Advantages:
1. The oxidation number rules provide a systematic and consistent approach to determine the oxidation state of an element.
2. They are relatively easy to apply once you understand the rules.
3. Oxidation numbers can give an overall idea of chemical reactivity and electron transfer in a compound.

Disadvantages:
1. The oxidation number rules do not provide a detailed understanding of the electron distribution within a molecule or ion.
2. They may oversimplify the actual electron distribution and bonding patterns in complex molecules.
3. Assigning oxidation numbers based solely on rules may not always accurately reflect the true nature of chemical bonding.