Among the following, the element with maximum ionization energy is

Consider the following change.

$\mathrm{M}\left(\mathrm{s}\right)\to \mathrm{M}\left(\mathrm{g}\right)$.... $\left(1\right)$

$\mathrm{M}\left(\mathrm{s}\right)\to {\mathrm{M}}^{2+}\left(\mathrm{g}\right)+2{\mathrm{e}}^{-}$....$\left(2\right)$

$\mathrm{M}\left(\mathrm{g}\right)\to {\mathrm{M}}^{+}\left(\mathrm{g}\right)+{\mathrm{e}}^{-}$.... $\left(3\right)$

${\mathrm{M}}^{+}\left(\mathrm{g}\right)\to {\mathrm{M}}^{2+}\left(\mathrm{g}\right)+{\mathrm{e}}^{-}$....$\left(4\right)$

$\mathrm{M}\left(\mathrm{g}\right)\to {\mathrm{M}}^{2+}\left(\mathrm{g}\right)+2{\mathrm{e}}^{-}$... $\left(5\right)$

The second ionization energy of $\mathrm{M}$ could be calculated from the energy values associated with:

Choose the correct statements for element ${}_9{}^{19}\mathrm{M}.$

a. Formation of ${\mathrm{M}}^{-}$ is an endothermic process.

b. It's anion is isoelectronic with neon.

c. It has the smallest size in its period.

d. It has the highest electron gain enthalpy in its group.

Identify the following statements is true and false.

${\mathrm{S}}_1$: Among ${\mathrm{Li}}^{-}, {\mathrm{Be}}^{-}, {\mathrm{B}}^{-}$ and ${\mathrm{C}}^{-},$ ${\mathrm{Be}}^{-}$ is the least stable ion.

${\mathrm{S}}_2$: If the same element is forming oxides in different oxidation states, then the oxide in which the element shows the highest oxidation state will be highly acidic in nature.

${\mathrm{S}}_3$: Amphiprotic oxide is one which can accept and release ${\mathrm{H}}^{+}$ ions.

${\mathrm{S}}_4$: In alkaline-earth metals, electronegativity values decrease down the group.