Iodine (I) and Iodide (I-) are elements in the same period of the periodic table, which means they have the same number of electron shells. The ionization enthalpy is the energy required to remove an electron from an atom or ion.
In this case, Iodine (I) will have a lower ionization enthalpy compared to Iodide (I-) because Iodine is an atom, and it has fewer electrons in its outermost shell compared to Iodide.
Iodine (I) has the electron configuration: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 5p⁵
Iodide (I-) is an ion, meaning it has gained an extra electron, so its electron configuration is: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 5p⁶
The outermost electron in Iodine is in the 5p orbital, while Iodide has a completely filled 5p orbital. Removing an electron from a partially filled orbital (as in Iodine) is easier than trying to remove an electron from a fully filled orbital (as in Iodide).
So, the ionization enthalpy of Iodine will be lower than that of Iodide.
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Iodine (I) and Iodide (I-) are elements in the same period of the periodic table, which means they have the same number of electron shells. The ionization enthalpy is the energy required to remove an electron from an atom or ion.
In this case, Iodine (I) will have a lower ionization enthalpy compared to Iodide (I-) because Iodine is an atom, and it has fewer electrons in its outermost shell compared to Iodide.
Iodine (I) has the electron configuration: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 5p⁵
Iodide (I-) is an ion, meaning it has gained an extra electron, so its electron configuration is: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p⁶ 5s² 4d¹⁰ 5p⁶
The outermost electron in Iodine is in the 5p orbital, while Iodide has a completely filled 5p orbital. Removing an electron from a partially filled orbital (as in Iodine) is easier than trying to remove an electron from a fully filled orbital (as in Iodide).
So, the ionization enthalpy of Iodine will be lower than that of Iodide.
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