An element with the symbol Z has the electron configuration 2.8.6.Which species is this element most likely to form?A. The ion Z2+B. The ion Z6+C. The compound H2ZD. The compound Z6F
Question
An element with the symbol Z has the electron configuration 2.8.6.Which species is this element most likely to form?A. The ion Z2+B. The ion Z6+C. The compound H2ZD. The compound Z6F
Solution
The electron configuration of the element Z is 2.8.6. This means that there are 2 electrons in the first energy level, 8 in the second, and 6 in the third.
The outermost energy level (also known as the valence shell) is the third one, which has 6 electrons. Elements tend to be most stable when their outermost energy level is full. For elements in the second and third periods of the periodic table, a full outermost energy level contains 8 electrons.
In this case, the element Z would need to gain 2 electrons to have a full outermost energy level. When an atom gains or loses electrons, it forms an ion. If the element gains 2 electrons, it will have a 2- charge, because electrons are negatively charged.
Therefore, the species that this element is most likely to form is the ion Z2-. However, this option is not given in the choices.
Looking at the options provided, the closest is the ion Z2+ (option A). However, this would involve the element losing 2 electrons, not gaining them.
The ion Z6+ (option B) would involve the element losing all 6 of its outermost electrons, which is highly unlikely.
The compound H2Z (option C) could potentially form if the element Z gains 2 electrons from 2 hydrogen atoms, each of which donates 1 electron.
The compound Z6F (option D) doesn't make much sense, as it would imply that one atom of the element Z is somehow bonded with 6 atoms of fluorine, which is not typically observed.
So, based on the electron configuration and the options provided, the most likely species that the element Z would form is the compound H2Z (option C).
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