Provide information regarding the ionization enthalpy,electron gain enthalpy,and electronegativity of the elements of Group-$16$.
(N/A) Ionization Enthalpy: Ionization enthalpy decreases down the group due to an increase in atomic size. The ionization enthalpy values of Group-$16$ elements are lower than those of the corresponding elements of Group-$15$ in the same period.
This is because Group-$15$ elements have extra stable,half-filled $p$-orbital electronic configurations.
Electron Gain Enthalpy: Due to the compact nature of oxygen,its electron gain enthalpy is less negative than that of sulfur. However,from sulfur to polonium,the values become less negative.
Electronegativity: Among all elements,oxygen has the second highest electronegativity after fluorine. Electronegativity decreases with an increase in atomic number down the group. This indicates that metallic character increases from oxygen to polonium.
This is because Group-$15$ elements have extra stable,half-filled $p$-orbital electronic configurations.
Electron Gain Enthalpy: Due to the compact nature of oxygen,its electron gain enthalpy is less negative than that of sulfur. However,from sulfur to polonium,the values become less negative.
Electronegativity: Among all elements,oxygen has the second highest electronegativity after fluorine. Electronegativity decreases with an increase in atomic number down the group. This indicates that metallic character increases from oxygen to polonium.
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