the number of electrons in each shell, i.e. 2 in the first shell, and 8 electrons in the other 2 shells.
Argon has a face-centered cubic structure.
The element argon (atomic number 18) has the electron configuration 1s22s22p63s23p6 which can be abbreviated [Ne] 3s23p6
The electron affinity of argon, like all noble gases, is 0, or very close to it, due to its chemical inertness.
Argon, like all of the "noble" gases, has a full electron shell.
Argon, being one of the noble gases, has a completely filled outer electron shell and thus has zero valency.
. . : Ar : . . Write Ar, the symbol for argon and then write four electron pairs (or eight electrons) around the symbol.
Argon
Argon has a face-centered cubic structure.
Argon
The element argon (atomic number 18) has the electron configuration 1s22s22p63s23p6 which can be abbreviated [Ne] 3s23p6
The electron affinity of argon, like all noble gases, is 0, or very close to it, due to its chemical inertness.
Potassium must lose one electron (to have the same configuration as the noble gas argon), and fluorine must gain one electron (to have the same configuration as neon)
Argon has completely filled valence orbitals and hence is unreactive. Sodium has one valence electron. If sodium loses this electron it will attain the stable electron configuration of the nearest noble gas (argon) and hence is reactive.
Argon, like all of the "noble" gases, has a full electron shell.
Argon, being one of the noble gases, has a completely filled outer electron shell and thus has zero valency.
The electron configuration, in standard form, is [Ne] 3s2 3p6
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.