Question

Use the periodic table and predict the number of electrons that will be lost or gained by the following elements as they change into sinple ions. write an equation using chemical symbols, ionic symbols, and electrons to represent each change.
a. Mg
b. silicon
c. element 53
d. sulfur

Answer 1

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Answer 2

a. Magnesium (Mg): Magnesium belongs to Group 2 (alkaline earth metals) and has an atomic number of 12. It has two valence electrons in its outermost shell. To achieve a stable electron configuration, magnesium tends to lose these two electrons and form a 2+ cation.

Chemical Equation: Mg -> Mg²⁺ + 2e⁻

b. Silicon (Si): Silicon belongs to Group 14 (carbon group) and has an atomic number of 14. It has four valence electrons in its outermost shell. To achieve a stable electron configuration, silicon can either lose four electrons and form a 4+ cation or gain four electrons and form a 4- anion. However, silicon rarely forms ions in typical chemical reactions.

Chemical Equation (Rare Case - Silicon forms a 4+ cation): Si -> Si⁴⁺ + 4e⁻

c. Element 53 (Iodine, I): Element 53 is iodine (I). Iodine belongs to Group 17 (halogens) and has an atomic number of 53. It has seven valence electrons in its outermost shell. To achieve a stable electron configuration, iodine tends to gain one electron and form a 1- anion.

Chemical Equation: I + e⁻ -> I⁻

d. Sulfur (S): Sulfur belongs to Group 16 (chalcogens) and has an atomic number of 16. It has six valence electrons in its outermost shell. To achieve a stable electron configuration, sulfur tends to gain two electrons and form a 2- anion.

Chemical Equation: S + 2e⁻ -> S²⁻