), in many hydrides, it acts as the more electronegative partner, sometimes even forming a negative anion ( H−cap H raised to the negative power
They are generally grouped into three categories based on the type of chemical bond involved: 1. Ionic (Saline) Hydrides hydride
Not enough electrons to form conventional bonds (e.g., B2H6cap B sub 2 cap H sub 6 Electron-precise: Perfect match of electrons (e.g., CH4cap C cap H sub 4 - Methane). Electron-rich: Have "lone pairs" of electrons (e.g., NH3cap N cap H sub 3 - Ammonia, or H2Ocap H sub 2 cap O 3. Metallic (Interstitial) Hydrides ), in many hydrides, it acts as the