A chemical element with the symbol X has the electron arrangement 2,8,6 (electron configuration 1s2 2s2 2p6 3s2 3p4). Which chemical species is this chemical element most likely to form?
It is likely to react as a non metal.
The chemical element you described with the electron arrangement 2,8,6 is sulfur (S), as it has atomic number 16. Sulfur is most likely to form a chemical species with a charge of -2. This is because sulfur has six valence electrons in its outermost energy level (3s2 3p4), and it tends to gain two electrons to achieve a stable electron configuration. By gaining two electrons, sulfur can attain a stable noble gas configuration similar to argon (2,8,8). Therefore, sulfur is likely to form compounds with other elements by gaining two electrons and forming an ion with a charge of -2.
To determine which chemical species the element X is most likely to form, we need to consider its electron arrangement and its position in the periodic table.
The element X has 16 electrons, with the electron arrangement 2,8,6. This configuration indicates that it belongs to Group 16 (Group VI-A) of the periodic table. Group 16 elements, also known as the chalcogens, have six valence electrons.
Considering its valence electron count, element X is most likely to form an ion with a charge of -2. This is because it will tend to gain two electrons to achieve a stable electronic configuration like the closest noble gas, which in this case is the element Xe (Xenon) with the configuration 2,8,18,18.
Thus, element X is most likely to form an ion with a -2 charge, denoted as X^2-. This negative charge indicates that element X has gained two electrons to complete its valence shell, resulting in a stable electron configuration.