Total charge on 1 mole of a monovalent metal ion is equal to:
(A) $6.28\times {{10}^{18}}coulomb$
(B) $1.6\times {{10}^{-19}}coulomb$
(C) $9.65\times {{10}^{4}}coulomb$
(D) none of these

Hint: A monovalent metal ion can be any monovalent ion, or atom, or a chemical group with one valency of one which forms one covalent bond.

Complete step by step solution:
Let us learn about the elementary charge, the elementary charge is denoted by ‘e’ or ‘${{q}_{e}}$’. It is the charge carried by a proton or an equivalent electron (magnitude).
Normally, the formulation for ‘e’ is given as,
\[e=\dfrac{F}{{{N}_{A}}}\]
where,
e = elementary charge
F = Faraday constant
\[{{N}_{A}}\] = Avogadro’s constant
Now, we know,
-The charge on an electron is equal to $1.6\times {{10}^{-19}}coulombs$.
-Avogadro’s number is equal to $6.022\times {{10}^{23}}mo{{l}^{-1}}$
Thus, Faraday constant will be approximately equal to 96500 coulombs per mole.
This is actually the required answer but specifically, A monovalent electron is an element that has one valence electron. Thus, for one mole of monovalent electrons, Charge of ${{e}^{-}}$ = ${{N}_{A}}$ electrons = 1 Faraday = 96500 coulombs.

Thus, option (C) $9.65\times {{10}^{4}}coulomb$ is the correct answer.

Note: Do note that electron charge units i.e. Coulomb and Faraday are inter-related to each other but are defined for the same parameter.