Which of the following atoms has the highest | vedclass

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(B) The first ionization energy is the energy required to remove the most loosely bound electron from an isolated gaseous atom.$K$ $(Z=19)$ and $Na$ $

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$Sc$

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(B) The first ionization energy is the energy required to remove the most loosely bound electron from an isolated gaseous atom.$K$ $(Z=19)$ and $Na$ $(Z=11)$ are alkali metals (Group $1$),which have the lowest ionization energies in their respective periods.$Rb$ $(Z=37)$ is also an alkali metal with an even lower ionization energy than $K$ due to its larger atomic size.$Sc$ $(Z=21)$ is a $d$-block transition metal.Transition metals generally have higher first ionization energies compared to alkali metals in the same or adjacent periods because of their smaller atomic radii and higher effective nuclear charge,which holds the valence electrons more tightly.

Which of the following atoms has the highest first ionization energy?

Similar Questions

Consider the elements $Mg$,$Al$,$S$,$P$ and $Si$. The correct increasing order of their first ionization enthalpy is:

Which of the following orders for ionisation energy is correct?

Assertion : Element has a tendency to lose the electron$(s)$ to attain the stable configuration.
Reason : Ionization enthalpy is the energy released to remove an electron from an isolated gaseous atom in its ground state.

The second ionisation energies of $Li, Be, B$ and $C$ are in the order

Which element has the maximum first ionization potential?

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