What is the formula of the ion formed when Caesium achieves noble-gas electron configuration?
To determine the ion formed when caesium (Cs) achieves a noble-gas electron configuration, we first need to understand the noble-gas configuration for caesium.
The noble-gas electron configuration refers to the electron arrangement of noble gases, which are chemically stable due to full valence electron shells. In the periodic table, the noble gases are located in Group 18 (Group 8A) and consist of helium (He), neon (Ne), argon (Ar), krypton (Kr), xenon (Xe), and radon (Rn).
The electron configuration for caesium is [Xe] 6s¹. This means that caesium has one electron in its outermost energy level (6s orbital).
To achieve a noble-gas electron configuration, caesium would need to lose this one valence electron. Since caesium is in Group 1 (Group 1A), it belongs to the alkali metal family, which typically lose one electron to form a 1+ cation.
Therefore, the formula of the ion formed when caesium achieves a noble-gas electron configuration is Cs+.