For each element, identify the charge of its most common ion. Cl \( +1 \) \( -2 \) \( +3 \) \( -1 \) \( +2 \) \( -3 \) Se \( +3 \) \( -2 \) \( -1 \) \( +2 \) \( +1 \) \( -3 \) Rb \( +1 \) \( -2 \) \( +2 \) \( -1 \) \( +3 \) \( -3 \) Al \( +2 \) \( -2 \) \( -1 \) \( +3 \) \( +1 \) \( -3 \)

Chlorine (Cl) commonly forms a charge of \( -1 \) as an ion known as chloride. This is because chlorine tends to gain one electron to achieve a stable electron configuration similar to that of noble gases. It's like finding the perfect outfit that fits just right—gaining that extra electron transforms chlorine into a happy ion! Selenium (Se) typically has a charge of \( -2 \) as its most common ion, known as selenide. Much like sulfur, selenium seeks to fill its outer shell by gaining two electrons, allowing it to feel complete and stable. Think of it as selenium putting on two extra layers of warmth in the winter! Rubidium (Rb) is known for its tendency to lose one electron and form a \( +1 \) ion. It’s like Rb has a tendency to leave one shoe behind when it runs out the door, making it very reactive and eager to bond with other elements. Aluminum (Al) generally forms a charge of \( +3 \) as an ion. Aluminum loves to lose those three valence electrons, kind of like shedding some baggage before a trip. This charge allows aluminum to participate in a wide range of chemical reactions, making it a star material in many industries!