An element has six valence electrons. Which ionic charge will its ion carry?(1 point)Responses2+2+6–6–6+6+2–
2-
An element with six valence electrons will typically gain two electrons to achieve a stable electron configuration. Therefore, the ionic charge of its ion will be 2-.
To determine the ionic charge of an ion, you need to look at the number of valence electrons an element has. Valence electrons are the electrons in the outermost energy level of an atom.
In this case, the element has six valence electrons. Valence electrons are typically involved in forming chemical bonds, and a main way this occurs is through the gain or loss of electrons to achieve a stable electron configuration.
If an atom gains electrons, it becomes negatively charged and forms a negatively charged ion, called an anion. The charge of an anion is determined by subtracting the number of gained electrons from the number of valence electrons of the neutral atom. Since the neutral atom in this case has six valence electrons and gains six electrons, the resulting anion will have a charge of -6.
On the other hand, if an atom loses electrons, it becomes positively charged and forms a positively charged ion, called a cation. The charge of a cation is determined by subtracting the number of lost electrons from the number of valence electrons of the neutral atom. Since the neutral atom in this case has six valence electrons and loses six electrons, the resulting cation will have a charge of +6.
Therefore, the possible ionic charges for an element with six valence electrons are -6 and +6.