Electron configuration of Florine: 1s^2 2s^2 2p^5 Electron configuration of Florine with an extra electron: 1s^2 2s^2 2p^6 An extra electron in places in the P orbital, so the exponent changes from a 5 to a 6. Note: The "^" symbol means the the following number is in the form of a superscript.
1s2, 2s2 2p5 or [He]2s2 2p5
Like all halogens, it has a valence of -1 requiring one electron to obtain a stable noble gas configuration.
Fluorine is one of the diatomic elements, so it appears as an F2 molecule.
1s22s22p5
Fluorine only needs to gain one electron to complete its octet. Check out the Periodic Table, the column furthest to your right is happy with all 8 electrons. fluorine is in the row next to it so it is missing one for a complete octet. Go over another row and look at Oxygen. Oxygen wants two electrons to complete its octet.
This is a chemical element. You can find the how many electron in a single atom by using a periodic table.
Fluorine is a non metal element. There are 9 electrons in a single atom.
Fluorine has seven valance electrons and needs eight to have a full outer shell, so it will gain one electron when it forms a compound with a metal, giving it a charge of 1-
Fluorine has an atomic number of 9, so it has 9 electrons. To become a more stable element it gains an electron to have a full outershell (2, 8 = 10). This gives fluorine a charge of 1-.
Yes, Fluorine tends to want to gain electrons to achieve a stable octet with the Neon electron structure.
To become a noble gas, 1.
Fluorine gain one electron.
Fluorine gains one electron to form a fluoride ion.
gain one electron to form fluoride anion
fluorine in its neutral state (meaning it isn't an ion) typically gains one electron
Fluorine in its elemental stage has 1 unpaired electron. ( 2p5 orbital has one unpaired electron in 2p orbital)
Gaining of 1 electron take Fluorine to nobel gas state
Fluorine gains one electron to form a fluoride ion.
gain one electron to form fluoride anion
Fluorine has 7 valence electrons and should gain 1 more electron.
Fluorine will gain one electron to form F- (or fluoride) ion. Fluoride ion has a charge of -1.
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.
There is only one possibility for the ion form of the element fluorine:fluoride, F - , oxidation state -1.It is the most electronegatve element of all, so there is no other element able to abstract one ore more electrons FROM Fluorine.Fluoride is formed by the following reaction:F2 + 2e- --> 2 F-
Fluorine's atomic number is 9. Thus, fluorine has 9 protons and 9 electrons. As with every atom, all 9 of fluorine's electrons are found in the electron cloud.
fluorine in its neutral state (meaning it isn't an ion) typically gains one electron
Fluorine in its elemental stage has 1 unpaired electron. ( 2p5 orbital has one unpaired electron in 2p orbital)
one
1Fluoride is a Group 7 element. In order to achieve octet with the electronic configuration of the Noble Gas Neon(Ne), it will be receiving one more electron to form F- anion
Gaining of 1 electron take Fluorine to nobel gas state