Not exactly as asked in the question.
But K+, Ca2+ and Ar all have the same electronic configuration. All will have a total of 18 electrons.
The abbreviated electron configuration for argon is [Ne] 3s^2 3p^6. The [Ne] represents the electron configuration of the noble gas neon, which has the same electron configuration as the inner electrons of argon.
Sulfur needs to gain 2 electrons to have the electon configuration of Argon
The negative ion F has the same electronic configuration as the positive ion Ne. This is because the negative ion F gains an electron to achieve a stable octet configuration, similar to the stable electronic configuration of the noble gas Ne.
When sulfur forms a negative ion, it gains two electrons to achieve a full outer electron shell, making it have the same electron configuration as argon.
The chloride ion (Cl-) has the same electron configuration as argon, which is 1s2 2s2 2p6 3s2 3p6. This is because the chloride ion has gained an extra electron compared to argon, giving it a full outer electron shell.
K+ and argon have the same electron configuration
The element that forms a 2+ ion with the same electronic configuration as Ar is Calcium (Ca). When Calcium loses two electrons, it attains the same electronic configuration as argon by having a full outer shell of electrons.
Considering the normal calcium ion Ca2+ it has the same electronic configuration as the noble gas Argon.
Argon has the same electron configuration as a sodium ion. Sodium ion has lost 1 electron from its outer shell, making its electronic configuration 2, 8. Argon's electronic configuration is also 2, 8 in its outer shell.
The electronic configuration of calcium is 1s2 2s2 2p6 3s2 3p6 4s2. In calcium hydroxide (Ca(OH)2), calcium loses its two outer electrons to form Ca2+ ion, which has the electronic configuration 1s2 2s2 2p6 3s2 3p6.
Argon has the same electron configuration as a potassium ion, as both species have 18 electrons with the electron configuration of [Ne]3s²3p⁶.
The abbreviated electron configuration for argon is [Ne] 3s^2 3p^6. The [Ne] represents the electron configuration of the noble gas neon, which has the same electron configuration as the inner electrons of argon.
1s2, 2s2 2p6, 3s2 3p6 The sulfur ion has 16 electrons but sulfide has a charge of negative 2, increasing its electron count by two for a total of 18 electrons, giving it the same electron configuration as Argon (this means it is also isoelectronic with Argon)
The noble gas configuration for selenium is [Ar] 3d10 4s2 4p4, which means it has the same electron configuration as argon, followed by 4d10 4p4 electrons.
Sulfur needs to gain 2 electrons to have the electon configuration of Argon
The charge of a sulfide ion that is isoelectric with its nearest noble gas (argon) is -2. This means that the sulfide ion has gained two electrons in order to have the same electron configuration as the noble gas.
They have the same electron configuration as argon, which means they are isoelectronic with argon.