Difference between formal charge and oxidation number?

[Claire_Kim_2F]

What is the difference between a formal charge and a oxidation number?

[Chem_Mod]

One key difference is that, when assigning oxidation numbers, you arbitrarily assign the electrons of each covalent bond to the more electronegative atom in the bond. Whereas, in formal charge, each bonding pair is divided equally between the two atoms in the bond without concerning electronegativity.

[Courtney Situ 2B]

Hi!

Formal charge refers to the charge that an atom would have if the electrons in their shared bonds were split evenly. Therefore, electronegativity and polarity have no bearing on the formal charge.

In comparison, oxidation number takes this electronegativity and polarity in mind when dividing the electrons. The bonded electrons are not split evenly.

The best way to illustrate the difference is to draw the lewis structure of CH4.
H
|
H-----C-----H
|
H
The formal charges of all of the atoms are 0. In comparison, the oxidation number for H is +1, and the oxidation number for O is -4. I guess an important similarity though is that the sum of the formal charges and the sum of the oxidation numbers should equal the overall charge of the compound. For example, a polyatomic ion CO3 with a charge of 2- means that the sum of the formal charges will be -2 and the sum of the oxidation numbers will also be -2.

Hope this helps!

[Courtney Situ 2B]

Hi!

Formal charge refers to the charge that an atom would have if the electrons in their shared bonds were split evenly. Therefore, electronegativity and polarity have no bearing on the formal charge.

In comparison, oxidation number takes this electronegativity and polarity in mind when dividing the electrons. The bonded electrons are not split evenly.

The best way to illustrate the difference is to draw the lewis structure of CH4.
H
|
H-----C-----H
|
H
The formal charges of all of the atoms are 0. In comparison, the oxidation number for H is +1, and the oxidation number for O is -4. I guess an important similarity though is that the sum of the formal charges and the sum of the oxidation numbers should equal the overall charge of the compound. For example, a polyatomic ion CO3 with a charge of 2- means that the sum of the formal charges will be -2 and the sum of the oxidation numbers will also be -2.

Hope this helps!

oops that lewis structure didn't translate well
.........H
.........|
H-------C--------H
.........|
.........H

[Crystal Hsueh 2L]

Formal charge is assigned to atoms using the number of bonds it has and the number of nonbonded electrons. And it is under the assumption that the electrons are equally shared, emphasizing covalent character. Oxidation numbers are assigned to the more electronegative atom and emphasizes ionic character

[shevanti_kumar_1E]

Formal charge is calculated for each molecule by using the formula formal charge = (valence electrons)- (bonded electrons/2 + lone pair electrons). Formal charge of an atom indicates gain or loss of electrons while forming covalent bonds.

I don't think we've got over oxidation numbers in lecture yet but they are obtained by a certain set of rules:

1. The oxidation number of a free element is always 0.
2. The oxidation number of a monatomic ion equals the charge of the ion.
3. The oxidation number of H is +1, but it is -1 in when combined with less electronegative elements.
4. The oxidation number of O in compounds is usually -2, but it is -1 in peroxides.
5. The oxidation number of a Group 1 element in a compound is +1.
6.The oxidation number of a Group 2 element in a compound is +2.
7.The oxidation number of a Group 17 element in a binary compound is -1.
8.The sum of the oxidation numbers of all of the atoms in a neutral compound is 0.
9.The sum of the oxidation numbers in a polyatomic ion is equal to the charge of the ion.

[Ximeng Guo 2K]

formal charge = (# of valence electrons)- (# of bonded electrons/2 + # of lone pair electrons); I think we use them to determine how stable a resonance structure of a covalent molecule is.

In other words, oxidation number is more to do with "loss and gain" of electrons when forming a compound. It's more to do with ionic characters. I think there is also one sampling HW which compares formal charge and oxidation number which you could refer to.