Question

based on patterns in the periodic table, which ion has a stable valence electron configuration? (1 point) potassium (k) with a 1+ charge magnesium (mg) with a 1- charge fluorine (f) with a 1+ charge sulfur (s) with a 1- charge

Explanation:

• Potassium (K) with a \(1^{+}\) charge: Potassium has an atomic number of 19. Its electron configuration is \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{1}\). When it loses one electron (to form \(K^{+}\)), its electron configuration becomes \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}\), which is the same as the noble gas argon (\(Ar\)). Noble - gas electron configurations are stable.
• Magnesium (Mg) with a \(1^{-}\) charge: Magnesium has an atomic number of 12. Its electron configuration is \(1s^{2}2s^{2}2p^{6}3s^{2}\). Gaining one electron (\(Mg^{-}\)) gives \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{1}\), which is not a noble - gas or a very stable configuration. Magnesium typically loses 2 electrons (\(Mg^{2 +}\)) to get a stable configuration (\(1s^{2}2s^{2}2p^{6}\)).
• Fluorine (F) with a \(1^{+}\) charge: Fluorine has an atomic number of 9. Its electron configuration is \(1s^{2}2s^{2}2p^{5}\). Losing one electron (\(F^{+}\)) gives \(1s^{2}2s^{2}2p^{4}\), which is not a noble - gas configuration. Fluorine typically gains one electron (\(F^{-}\)) to get \(1s^{2}2s^{2}2p^{6}\) (noble - gas neon configuration).
• Sulfur (S) with a \(1^{-}\) charge: Sulfur has an atomic number of 16. Its electron configuration is \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{4}\). Gaining one electron (\(S^{-}\)) gives \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{5}\), which is not a noble - gas configuration. Sulfur typically gains 2 electrons (\(S^{2-}\)) to get \(1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}\) (noble - gas argon configuration).

Answer:

potassium (K) with a \(1^{+}\) charge