Question

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Answer 1

Answer:

$\rm S^{2-}$.

Explanation:

Based on the electron configuration of this ion, count the number of electrons in this ion in total:

$2 + (2 + 6) + (2 + 6) = 18$.

Each electron has a charge of $(-1)$.

Atoms are neutral and have $0$ charge. However, when an atom gains one extra electron, it becomes an ion with a charge of $(-1)$. Likewise, when that ion gains another electron, the charge on this ion would become $(-2)$.

The ion in this question has a charge of $(-2)$. In other words, this ion is formed after its corresponding atom gains two extra electrons. This ion has $18$ electrons in total. Therefore, the atom would have initially contained $18 - 2 = 16$ electrons. The atomic number of this atom would be $16$.

Refer to a modern copy of the periodic table. The element with an atomic number of $16$ is sulphur with atomic symbol $\rm S$. To denote the ion, place the charge written backwards ("$2-$" for a charge of $(-2)$) as the superscript of the atomic symbol:

$\rm S^{2-}$.

Answer 2

Answer:

100% Silicon

Explanation:

Hope this helps!!