why electron gain enthalpies of magnesium and phosphorous are almost zero??
Answers
Answered by
10
The term ◆Electron gain enthalpy◆ means energy required to add an electron on a periphery of an element.
configuration of magnesium and phosphorus are ad follows-
Mg-1s2,2s2,2p6,3s2
P-1s2,2s2,2p6,3s2,3p3
As you can see Magnesium have fully filled subshell and Phosphorus have half filled.
Fully filled and half filled shells are so much stable that it leads high amount of energy to make electron enter.
That's why EGE is almost 0.
configuration of magnesium and phosphorus are ad follows-
Mg-1s2,2s2,2p6,3s2
P-1s2,2s2,2p6,3s2,3p3
As you can see Magnesium have fully filled subshell and Phosphorus have half filled.
Fully filled and half filled shells are so much stable that it leads high amount of energy to make electron enter.
That's why EGE is almost 0.
Answered by
9
Answer:
Electron gain enthalpies of beryllium and magnesium are also positive. This is attributed to the extra stability of the fully completed s-orbitals in Be(2s2), Mg (3s2). The gain of electron is highly endothermic. Thus, if an atom has fully filled orbitals, its electron gain enthalpy value will be positive.
Similar questions