Net Charge of Fluorine Atom: Is it Possible?

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The discussion centers on determining the net charge of a fluorine atom with 9 protons, 10 neutrons, and 20 electrons. While the atomic number confirms it is fluorine, the participant struggles with the implications of having 20 electrons, leading to confusion about the net charge. It is clarified that a fluorine atom typically seeks to gain three electrons to achieve a full outer shell, suggesting a net charge of -3. The possibility of a fluorine atom having 11 excess electrons is deemed unrealistic, with speculation that it may be a typo for 10 electrons. Ultimately, understanding the net charge involves simple arithmetic based on the difference between protons and electrons.
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This is probably a simple question but it has absolutely annoyed me for a week at University (yes, I know, I am still learning this, laugh away).

I am meant to identify the atom/ion and the net charge of it.

This is the information I am given:

Protons: 9
Neutrons: 10
Electrons: 20

The Atomic Number is quite straightforward - 9. Therefore, it is Fluorine. However what I can't figure out is the net charge - is it even possible for a Fluorine atom to gain 11 more electrons if it needs only to remove 2 valence electrons to pursue a full outer shell?

Otherwise, the net charge would be -5, is this right?
 
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Hi Procrastinate! :smile:
Procrastinate said:
The Atomic Number is quite straightforward - 9. Therefore, it is Fluorine. However what I can't figure out is the net charge - is it even possible for a Fluorine atom to gain 11 more electrons if it needs only to remove 2 valence electrons to pursue a full outer shell?

Yes, I'd be surprised if you could add that many electrons. :confused:
Otherwise, the net charge would be -5, is this right?

I'm fascinated to know how you got -5. :smile:
 
tiny-tim said:
Hi Procrastinate! :smile:
I'm fascinated to know how you got -5. :smile:

When you add all the electrons, you get a new valence electron number of 5. However, now that I think about it, I did it wrong, so it's net charge would be -3 as it would want to acquire three electrons to attain a full outer shell.

I am not sure if this is right though since I never understood from the beginning if 11 electrons added to a Fluorine atom was logistically possible.
 
No idea what you are calculating. Let's put apart fact that 11 electrons excess is absurd (my guess is that it is a typo, and it was intended to be 10 electrons). What is the definition of a net charge?
 
Borek said:
No idea what you are calculating. Let's put apart fact that 11 electrons excess is absurd (my guess is that it is a typo, and it was intended to be 10 electrons). What is the definition of a net charge?

It would be the overall charge on an atom (after it has been ionised, so it would be called an "ion". So if you had 3 protons and 2 electrons, for example, it would be a +1 charge.
 
3-2=1. Can you apply exactly the same simple logic to 9 and 20?
 

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