How does the activity of an element different for nonmetals vs metals? 

A excellent conductor of electricity is metal. It has a gleaming, ductile appearance. The majority of the elements in the periodic table fall into the category of metals. Alkali metals, alkaline earth metals, transition metals, etc. are some examples. Non-metals are weak electrical conductors. The elements in groups 13 through 18 of the contemporary periodic table are referred to as non-metals.

Across the periodic table, the non-metallic nature often rises from left to right. Metals exhibit strong electropositivity. Take sodium, an alkali metal, as an illustration. Sodium has a 3s¹ outer electrical structure. As a result, sodium is willing to lose an electron rather than receive them. The sodium metal achieves an octet configuration if it is willing to surrender its one electron. As a result, all metals are electropositive and rapidly lose their electron to produce cations.

Let's use "Chlorine" as an example of a non-metal element. Chlorine is electronic in its 3s²3p⁵ outermost form. To achieve octet-stable structures, chlorine only requires one electron. Therefore, rather of eliminating its five electron valence, it primarily concentrates on adding one electron to achieve an octet configuration. As a result, non-metals have a tendency to be more electronegative and easily pick up an electron to create an anion.

Since cations have more protons than electrons, an element must also be ready to gain protons in order to create a cation. Metals therefore frequently acquire protons. Non-metals are the antithesis of this situation. Since non-metals are ready to gain electrons, they have more electrons than protons.
Thus, non-metal activity describes the ease with which an element may absorb electrons. The terms "metal activity" and "non-metal activity" both describe how readily an element loses protons and electrons, respectively. Metal activity is the rate at which an element may absorb protons .

So option A and B is correct.