[He] 2s2 3p5 is the electronic configuration of a neutral Fluorine atom.
It's -1 ion (F-, fluoride ion), however is: [He] 2s2 3p6, or [Ne].
Oxygen tends to form O^2- ions, gaining two electrons to achieve a stable electron configuration. Fluorine tends to form F^- ions, gaining one electron to achieve an electron configuration similar to a noble gas.
Fluorine will gain one electron to fill its outer shell and achieve a stable noble gas configuration when forming an ion.
A fluorine atom that has seven electrons in its outer shell would be neutral. A negatively charged fluoride ion, Fl-, forms when a fluorine atom gains one electron so that it has an octet, or a noble gas configuration of electrons.
neon only because sodium loses an electron an its outer shell becomes empty making its configuration the same as neon and fluorine gains an electron making its configuration the same as neon as well.
The ion formed by a fluorine atom is called a fluoride ion, which has a charge of -1. It is formed when a fluorine atom gains an electron to achieve a full outer electron shell.
The electron configuration of a fluorine atom is 1s2 2s2 2p5. When fluorine gains an electron to form a fluoride ion, its electron configuration becomes 1s2 2s2 2p6, which is the same as that of a noble gas (neon). This gives the fluoride ion a stable, filled outer electron shell.
When fluorine forms an ion, it gains one electron to achieve a stable electron configuration, becoming a fluoride ion with a charge of -1.
The electron configuration of fluoride ion (F-) is 1s2 2s2 2p6. This is because fluoride gains one electron compared to neutral fluorine, which has the electron configuration 1s2 2s2 2p5.
Fluorine gains one electron to form a fluoride ion.
Fluorine is negative and will produce a negative ion.
The fluorine atom can become an ion by gaining one electron to achieve a stable electron configuration of 8 electrons in its outer shell. This results in the formation of a negatively charged ion known as fluoride ion (F^-).
Fluorine's most stable ion configuration is F-, also known as the fluoride ion. Fluorine gains one electron to achieve a full outer energy level, making it isoelectronic with the noble gas neon and achieving a more stable electron configuration.
It accepts one electron.
If the ion is the most common anion of fluorine, a fluoride ion, it contains 10 electrons.
Fluoride is an ion formed by the nonmetal fluorine.
Fluorine's electron configuration is 1s2 2s2 2p5, and since fluoride is just fluorine with an extra electron, or F-1, its electron configuration is 1s2 2s2 2p6.
The fluoride ion has the same electron configuration as a neon atom. This is because fluoride has gained an extra electron compared to a neutral fluorine atom, resulting in a full valence shell with 8 electrons. Therefore, the electron configuration of a fluoride ion is 1s2 2s2 2p6.