NH2- is a stronger base than H- due to its greater ability to donate a proton, despite nitrogen's higher electronegativity. The Gibbs free energy (ΔG) for the reaction involving NH2- is -1657 kJ/mol, compared to -1649 kJ/mol for H-, indicating a more favorable reaction. The equilibrium constant for the NH2- reaction is also greater, suggesting it is more likely to proceed to products. The discussion highlights the complexity of determining basicity based solely on structure, as electronegativity does not directly correlate with basic strength in this case. Understanding these reactions requires consideration of both thermodynamic data and molecular structure.
