Element X has the highest first electron affinity in its period; the ground state electron configuration of it's most common ion is [Kr] 5s^2 4d^10 5p^6
a Element Y is the second largest element in it's period; it's valence electrons are in orbital(s) that have n=6
what is the most stable compound formed when elements X and Y are combined
Is element X Iodine? Is element Y cesium?
If it is how do you write the most stable compound of the element?
Element X is Iodine as it has the highest first electron affinity
Element Y is Barium
Barium is the second largest element in its period and has valence electrons in n=6 .
Most stable compound formed would be BaI2
To determine the most stable compound formed when elements X and Y are combined, we need to identify the elements X and Y based on the given information.
Element X has the highest first electron affinity in its period, and its most common ion has the electron configuration [Kr] 5s^2 4d^10 5p^6. This electron configuration corresponds to the noble gas Krypton (Kr).
Element Y is the second largest element in its period, and its valence electrons are in orbitals with n=6. The element with these characteristics is Cesium (Cs).
Therefore, the elements X and Y are Krypton (Kr) and Cesium (Cs), respectively.
To determine the most stable compound formed between Krypton and Cesium, we need to consider their valence electrons. Krypton has 8 valence electrons (5s^2 4d^10 5p^6), while Cesium has 1 valence electron (6s^1).
Since Cesium has only one valence electron, it will lose this electron and form a Cs+ ion. On the other hand, Krypton has a full outer electron shell and tends to gain electrons to achieve a stable configuration. Therefore, Krypton will gain one electron to form a Kr- ion.
The most stable compound formed between Krypton and Cesium will be when Cs+ and Kr- combine to form CsKr.
Therefore, the most stable compound of these elements is CsKr.