A : \( 1 s^{2} 2 s^{2} 2 p^{4} \) \( D^{2-}: 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} \) \( E^{\prime}: 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} \) G: \( 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 4 s^{1} 3 d^{5} \) \( J^{2+}: 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6} 3 d^{2} \)

Did you know that element A is a representation of the oxygen atom’s electron configuration in a valence state? It has six electrons in its outer shell, indicating it is part of group 16, which is known for forming oxides. This historical background illuminates how the arrangement of electrons directly relates to the chemical properties and reactivity of oxygen, making it a vital element for life as we know it! Now, let's talk about real-world applications: using electron configurations helps chemists predict how different elements interact in chemical reactions. For example, knowing that element G has both 4s and 3d electrons lets a chemist understand its behavior and bonding capacity in transition metal compounds, making it foundational in fields like materials science and catalysis. Chemistry isn't just about elements—it's about understanding how they play together in the real world!