Easier way to calculate/remember?

[Clarice Chui 2C]

Is there an easier way to calculate this/remember it/shortcut?

[Sarah Blake-2I]

Take the valence electrons and subtract how many dots and lines you see connected to the element. This will give you the formal charge.

[TanveerDhaliwal3G]

You can count the number of dots and bonds of the atom and subtract that from the number of valence electrons to find the Formal Charge quickly

[Julie Park 1G]

Formal charge:
# ve- a neutral atom of the element would have - (sum of unpaired electrons + bonds)

Note:
a. count each unpaired electron attached to the atom as a single value
b. count each bond as a single value

For example, say that Nitrogen was surrounded by 1 double bond and 2 unpaired valence electrons. You know that a neutral atom of nitrogen should have 5ve-. Therefore, to find the FC, you would do: 5(ve-) - ( 2 (for each bond in the double bond) + 2 (for each unpaired electron) )
To get 5 - (2+2) or 5-4 which equals 1. The formal charge would be +1
Note: this is just a random theoretical example... not sure if this specific situation is possible

I recommend this youtube video: https://www.youtube.com/watch?v=J03H472fAKI

[serenabirkhoff_1K]

for me the easiest way to remember how to calculate formal charge is the formula. At first I was having trouble remembering but once you do enough practice problems with the formula you should remember it.

[Kristina Rizo 2K]

Formal charge:
# ve- a neutral atom of the element would have - (sum of unpaired electrons + bonds)

Note:
a. count each unpaired electron attached to the atom as a single value
b. count each bond as a single value

For example, say that Nitrogen was surrounded by 1 double bond and 2 unpaired valence electrons. You know that a neutral atom of nitrogen should have 5ve-. Therefore, to find the FC, you would do: 5(ve-) - ( 2 (for each bond in the double bond) + 2 (for each unpaired electron) )
To get 5 - (2+2) or 5-4 which equals 1. The formal charge would be +1
Note: this is just a random theoretical example... not sure if this specific situation is possible

I recommend this youtube video: https://www.youtube.com/watch?v=J03H472fAKI

Hey i just wanted to say thanks for including the video link, I just watched it and I understand formal charge a lot better!

[Julie Park 1G]

Formal charge:
# ve- a neutral atom of the element would have - (sum of unpaired electrons + bonds)

Note:
a. count each unpaired electron attached to the atom as a single value
b. count each bond as a single value

For example, say that Nitrogen was surrounded by 1 double bond and 2 unpaired valence electrons. You know that a neutral atom of nitrogen should have 5ve-. Therefore, to find the FC, you would do: 5(ve-) - ( 2 (for each bond in the double bond) + 2 (for each unpaired electron) )
To get 5 - (2+2) or 5-4 which equals 1. The formal charge would be +1
Note: this is just a random theoretical example... not sure if this specific situation is possible

I recommend this youtube video: https://www.youtube.com/watch?v=J03H472fAKI

Hey i just wanted to say thanks for including the video link, I just watched it and I understand formal charge a lot better!

No problem! :)

[Nohemi Garcia 1L]

For the oxidation numbers I just recommend keeping an eye out for negatively charged ligands.