Would you expect the first ionization enthalpies for two isotopes of the same element to be the same or different? Justify your answer.
Answers
The Ionization potential or enthalpy is the minimum amount of energy which is needed to remove the most loosely bound electron from a neutral isolated gaseous atom to form a cation also in the gaseous state
The ionization enthalpy of an atom depends on the number of electrons and protons (nuclear charge) of that atom.
Now, the isotopes of an element have the same number of the protons and the electrons.
Hence, the first ionization enthalpy for two isotopes of the same element should be the same.
The first ionization enthalpies for two isotopes of the same element would be the same.
Explanation:
Isotopes of an element have same number of protons but different number of neutrons which means isotopes of an element have same atomic number but different mass number.
Thus isotopes of same element will have same number of electrons as for neutral atoms, the number of protons is equal to the number of electrons.
Ionization enthalpy is the energy required to remove the most loosely bound electron from an isolated gaseous atom.
Thus as the electronic configuration of isotopes is same, they have same first ionization enthalpies.
Learn more about isotopes and ionization enthalpy
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