Fluorine has 7 valence electrons. In order to become stable, Florine will share 1 electron with another atom to get 8 electron and become stable.
It isn't an atom, it would actually be a stable Fluorine Ion with a -1 charge.
Atoms become chemically neutral with either 2 or 8 electrons in the outermost orbital. Polonium would lose 2 electrons to become chemically neutral. Because Polonium is radioactive it will remain unstable until gains two in Atomic Number to resemble the configuration of Lead.
To become stable. Without the sharing or "loaning" of electrons atoms would become very reactive. Pure sodium put into water would explode, but when sodium is combined with Chlorine, it produces Sodium Chloride (NaCl) otherwise known as common table salt.
Fluorine has 9 electrons. The first energy level holds 2 electrons, and the second energy level holds 7 electrons. The Bohr model for fluorine would show 2 electrons in the first energy level and 7 electrons in the second energy level.
The element that attracts electrons the most would be Fluorine
Fluorine will gain one electron to form F- (or fluoride) ion. Fluoride ion has a charge of -1.
For fluorine to become stable, it needs to gain one electron to attain a full valence shell, similar to the electron configuration of neon. Fluorine has seven valence electrons in its outer shell, so gaining one electron would fill its outer shell and make it stable with a full octet like neon.
Hydrogen and fluorine would form a covalent bond by sharing electrons. Hydrogen provides one electron, while fluorine provides seven electrons to complete their octet. This sharing of electrons creates a stable hydrogen fluoride molecule.
Magnesium would lose two electrons when reacting with fluorine to form magnesium fluoride. Magnesium, with two electrons in its outer shell, loses these electrons to achieve a stable octet configuration, while fluorine, needing one electron to complete its octet, gains one electron from magnesium.
A fluorine atom would be more reactive than a carbon atom because fluorine is more electronegative and has a stronger tendency to attract electrons. This means that fluorine is more likely to participate in chemical reactions to achieve a stable electron configuration.
It would need to ionize, by combing with another fluoride atom.
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 has 7 valence electrons in its outer shell. In order to achieve a full octet, fluorine needs one additional electron to fill its shell. This means that fluorine has 1 bonding electron available to form covalent bonds with other atoms.
It'll have to lose two to have a stable octet.
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.
An alkaline earth metal would typically lose two electrons to become stable. This would result in the metal forming a 2+ cation, as it will have the same electron configuration as the nearest noble gas.
An oxygen atom needs 2 electrons to become stable because it has 6 electrons in its outer shell and it needs a total of 8 electrons to have a full valence shell. By gaining 2 electrons, oxygen can achieve a full outer shell and become stable.