Question

why the first ionization energy fot copper is higer than that for potassium where as the second ionization energy valus are in reverse order​

Answer 1

Explanation:

The answer is simple it depends on the atomic number and the electronic configuration of the two. For the first ionisation of copper the first electrone lies in 4s shell which is also 1 electron thus half-filled pulling an electron from this would require low ionisation energy. In case of potassium the last electron is in 3d a 1 electron which is same easy to remove. When thd second time it is 3d shell with 10 electrons fully filled which require more energy to pull electrons and for second for potassium which is fully filled 2p6 this requiring more energy to remove electrons.

Answer 2

Explanation:

first ionization energy of copper is higher than that of the alkali metals while second and third energies are lower than those of alkali metals

the reason behind it is that copper has a smaller size compared to the alkali metals in their period. due to smaller size and due to poor shielding effect of 3D orbital, Cu has higher first ionization energy. Second and third ionization energy are lower compared to those of alkali metals due to loss of electrons from diffused d orbitals , d electrons have smaller screening effect and give rise to higher effective nuclear charge compared to S and P electrons

The increasing and decreasing of their ionizations energy just depends on their orbitals present.....

hope it helps thankyou