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∙ 11y agoThe atomic number determines how many protons and electrons an atom has. Flourine's atomic number is 9 so there are 9 protons and electrons. Energy levels of atoms can only hold a maximum number of electrons per enegery level. The first energy level (s) holds 2 electrons. The second level (p) holds a maximum of 8 electrons because s has two and p has 6. So, Flourine's energy levels would be as follows: 1s2, 2s2 2p5 Energy levels need even pairs to be stable, so Flourine tends to gain only one electron because that is all that is needed for 2p5 to be filled to its maximum capacity. It is easier for an atom to gain one electron than give up 5.
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∙ 11y agogain one electron to form fluoride anion
It has 7 electrons in its valance shell so it needs only 1 electron to form a octet; the Nobel gas configuration.
It should be Fluorine but Chlorine has most EGE value because the F atom has very small sizeas compared to Cl. Addition of extra electron creates higher electron density and thus strong electron - electron repulsion comes into act. So extra electron is not accepted with the same ease as in the case of remaining elements of the group
No, fluorine gas (F2) is highly reactive and dangerous. Fluorine as an atom is worse, as it is the most electronegative atom in the entire periodic table of elements and thus has a very large tendency to gain one electron to attain stability.
Fluorine gains an electron when forming bonds as fluorine is very electronegative. This behavior is due to the fact that gaining an electron gives fluorine a noble gas electron configuration.
gain one electron to form fluoride anion
A Fluorine atom has an atomic number of 9. Draw out the electron shell diagram for Fluorine. Is a Fluorine atom more likely to gain, lose or share electrons to fill its valence shell?
this is because a fluorine ion is one electron short of a full valence shell,which makes getting another electron to fill the shell very favourable,filling the shell makes the molecule much more stable
Even though Fluorine has the highest electronegativity among all the elements and it should have the highest electron gain enthalpy among all the halogens but this is an exception and chlorine has higher electron gain enthalpy than Fluorine. The reason for this is that the size of Fluorine atom is very small and hence there is very high inter-electronic repulsion among the electrons of fluorine. This makes incoming of another electron not very favourable. Even though fluorine has large negative electron gain enthalpy but for chlorine its even more negative.
Atoms that gain extra electrons become negatively charged. A neutral chlorine atom.
Aluminum, sulfur, fluorine, phosphorus, iodine, and neon
It has 7 electrons in its valance shell so it needs only 1 electron to form a octet; the Nobel gas configuration.
It should be Fluorine but Chlorine has most EGE value because the F atom has very small sizeas compared to Cl. Addition of extra electron creates higher electron density and thus strong electron - electron repulsion comes into act. So extra electron is not accepted with the same ease as in the case of remaining elements of the group
Potassium only needs to lose on electron (gain a positive charge) to have the same electron structure as Argon and thus very stable. Similarly, fluorine only needs to gain one electron (become negatively charged) to gain the very stable Neon structure.
No, fluorine gas (F2) is highly reactive and dangerous. Fluorine as an atom is worse, as it is the most electronegative atom in the entire periodic table of elements and thus has a very large tendency to gain one electron to attain stability.
Atoms with high electronegativity will want to GAIN electrons. The goal is to be like the noble gases. So an atom of Fluorine, the most electronegative, will want to gain an electron in order to fill its shell and be like Neon.
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.