The first ionisation enthalpy of mg is higher thanai. Why?
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Well, we will look at the data shortly…but consider the reaction whose enthalpy change we interrogate…
M(g)+Δ→M(g)++e−M(g)+Δ→M(g)++e−
…and thus ionization represents the formation of one mole of gaseous cations, and electrons from one mole of gaseous ATOMS…
A priori, we would expect that ACROSS the Period (form left to right as we face the Table) ionization enthalpy should increase, however, consider the electronic configuration of the VALENCE electron for each metal…
Na,Z=11:1s22s22p63s1Na,Z=11:1s22s22p63s1
Mg,Z=12:1s22s22p63s2Mg,Z=12:1s22s22p63s2
Al,Z=13:1s22s22p63s23p1
M(g)+Δ→M(g)++e−M(g)+Δ→M(g)++e−
…and thus ionization represents the formation of one mole of gaseous cations, and electrons from one mole of gaseous ATOMS…
A priori, we would expect that ACROSS the Period (form left to right as we face the Table) ionization enthalpy should increase, however, consider the electronic configuration of the VALENCE electron for each metal…
Na,Z=11:1s22s22p63s1Na,Z=11:1s22s22p63s1
Mg,Z=12:1s22s22p63s2Mg,Z=12:1s22s22p63s2
Al,Z=13:1s22s22p63s23p1
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