Question

the decrease in the second ionization energy of alkali metals going down the group, as shown in the table above, can be best attributed to a decrease in the coulombic force of attraction due to

Answer 1

The second ionization energy of alkali metals decreases going down the group due to the increasing atomic radius, which decreases the Coulombic force of attraction between the nucleus and the valence electrons, making those electrons easier to remove.

Step-by-step explanation:

The decrease in the second ionization energy of alkali metals going down the group can be attributed primarily to the decrease in the Coulombic force of attraction. As you go down the group, the size of the atom increases due to the addition of another energy level or shell. This results in the outermost electron being further away from the nucleus, which reduces the electrostatic attraction between the electron and the nucleus. Therefore, it is easier for an electron to be removed, decreasing the ionization energy as the group descends.

Ionization energy tends to decrease down a group because the atoms become larger as additional electron shells are filled. Valence electrons located farther from the nucleus are thus less tightly bound and easier to remove, leading to lower ionization energies for larger atoms with a higher principal quantum number. A larger atomic radius typically corresponds to a lower ionization energy, reinforcing the observed trend in the periodic table.

Answer 2

As alkali metals go down the group, the atomic radius increases. Option A

The energy needed to extract a second electron from a positively charged ion is known as the second ionization energy. The atomic radius of alkali metals rises as they move down the group. The right response is; " Atomic radius increasing" .

This is because the coulombic force of attraction between the negatively charged electrons and the positively charged nucleus weakens as the atomic radius increases, moving the outer electrons away from the nucleus.

Missing parts;

The decrease in the second ionization energy of alkali metals going down the group, as shown in the table above, can be best attributed to a decrease in the coulombic force of attraction due to:

A. Increasing atomic radius.

B. Increasing electronegativity.

C. Decreasing number of valence electrons.

D. Increasing ionization energy of the first electron.