`color{green}(★)` The alkali metals are strong reducing agents, lithium being the most and sodium the least powerful (Table 10.1).
`color{green}(★)` The standard electrode potential (`color{red}(E^⊖)` ) which measures the reducing power represents the overall change :
`color{red}(M(s) → M(g) \ \ \ \ \ \ \ \ \ \ \ \ ("sublimation enthalpy"))`
`color{red}(M(g) → M^(+) +e^(-) \ \ \ \ \ \ \ \ \ (" ionization enthalpy"))`
`color{red}(M^(+) (g) + H_2O → M^(+) (aq) \ \ \ \ \ \ \ (" hydration enthalpy")) `
`color{green}(★)` With the small size of its ion, lithium has the highest hydration enthalpy which accounts for its high negative `color{red}(E^⊖)` value and its high reducing power.
`color{green}(★)` The alkali metals are strong reducing agents, lithium being the most and sodium the least powerful (Table 10.1).
`color{green}(★)` The standard electrode potential (`color{red}(E^⊖)` ) which measures the reducing power represents the overall change :
`color{red}(M(s) → M(g) \ \ \ \ \ \ \ \ \ \ \ \ ("sublimation enthalpy"))`
`color{red}(M(g) → M^(+) +e^(-) \ \ \ \ \ \ \ \ \ (" ionization enthalpy"))`
`color{red}(M^(+) (g) + H_2O → M^(+) (aq) \ \ \ \ \ \ \ (" hydration enthalpy")) `
`color{green}(★)` With the small size of its ion, lithium has the highest hydration enthalpy which accounts for its high negative `color{red}(E^⊖)` value and its high reducing power.