in a normal F- ion there are 10 electrons total (but 8 in the outer energy level)
Fluorine has atomic number 9, therefore the neutral fluorine atom has 9 electrons. The F-1 ion has 10 electrons.
Fluorine gains one electron to form a fluoride ion.
Fluorine has 9 electrons.
A fluorine atom will typically gain one electron to achieve a stable electron configuration by filling its outer shell with a total of 8 electrons. This results in a fluorine ion with a negative charge, known as fluoride.
The fluoride atom has 7 electrons in its outer shell (9 in total) but the ion of fluorine has any number of electrons in the outer shell. eg. F+ = the normal fluorine atom but with one less electron.
9
If the ion is the most common anion of fluorine, a fluoride ion, it contains 10 electrons.
There are 9 electrons in the atom without a charge, . The Fluorine ion (F -), has 10 electrons.
Fluorine has atomic number 9, therefore the neutral fluorine atom has 9 electrons. The F-1 ion has 10 electrons.
Fluoride-19 has 10 electrons (note fluoride is the ion of fluorine, if you meant fluorine, then fluoride has 9 electrons).
A fluorine ion with a charge of 1 indicates that it has gained an extra electron, making it a fluoride ion. So, a fluoride ion would have 10 electrons (9 from the protons and 1 extra electron).
One, and only one.
Fluoride-19 has 10 electrons (just to mention it, fluoride is the ion of flourine, so if you meant fluorine, fluorine has 9 electrons).
Technically yes ... the naming convention is that X ion is the ion you get if you pull electrons off X.However, nothing is electronegative enough to do this to fluorine, so fluorine instead forms fluoride ions by gaining one electron.
The fluorine isotope differs from the fluorine ion because the fluorine isotope has a different number of neutrons from normal, while the ion has a different number of electrons. An isotope will have the same number of electrons as its atomic number (the number of protons), while the ion will add (more common in the case of fluorine) or subtract (very rare in the case of fluorine) electrons to the atom. The only thing they are similar in is the number of protons they have, which are the same.
Fluorine will gain one electron to form F- (or fluoride) ion. Fluoride ion has a charge of -1.
Fluorine will gain one electron to fill its outer shell and achieve a stable noble gas configuration when forming an ion.