1s22s22p63s23p64s23d104p6. This ion is a(n) . What is the chemical symbol of the noble gas this ion is isoelectronic with?
The Correct Answer and Explanation is :
The electron configuration 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶ represents a neutral atom of an element in the 4th period. The configuration indicates a total of 36 electrons, corresponding to the element Krypton (Kr) in the periodic table, which is a noble gas.
However, you’re asking about the ion that this electron configuration represents. To determine this, we need to identify what charge the ion might have. The electron configuration could be describing a Krypton ion (Kr⁰), or it could represent an ion where the number of electrons has changed due to the removal or addition of electrons.
To consider ions:
- A cation (positively charged ion) is formed when electrons are lost.
- An anion (negatively charged ion) is formed when electrons are gained.
For example, if this configuration corresponds to an ion of an element, we could expect an ion of Krypton (Kr) to gain or lose electrons to achieve a stable noble gas configuration. But this configuration represents 36 electrons, the exact number for the neutral Krypton atom. If the ion were, for instance, a Krypton ion (Kr⁰), then the noble gas it is isoelectronic with would be Krypton itself.
In conclusion, the chemical symbol of the noble gas this ion is isoelectronic with is Krypton (Kr). This is because the ion with the configuration 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶ is isoelectronic with the neutral atom of Krypton. The term “isoelectronic” refers to species that have the same number of electrons, and this configuration matches that of Krypton, a noble gas with 36 electrons.