An electrovalent bond or ionic bond is formed between: -
(A) Two electronegative atoms
(B) Two metals
(C) Electropositive and electronegative atoms
(D) Two electropositive atoms

Hint: ionic bonding is the complete transfer of valence electron(s) between atoms. It is a type of chemical bond that generates two oppositely charged ions. In ionic bonds, the metal loses electrons to become a positively charged cation, whereas the non-metal accepts those electrons to become a negatively charged anion.

Complete step by step answer:
Ionic bonding is a type of chemical bond that involves the electrostatic attraction between oppositely charged ions. These ions represent atoms that have lost one or more electrons (known as cations) and atoms that have gained one or more electrons (known as anions).
That is the bond in which a large electronegativity difference exists between the two atoms, causing the bond to be more polar (ionic) than in covalent bonding where electrons are shared more equally. Such type of bonding takes place between electropositive and electronegative atoms. Eg. $KCl,NaCl$

So, the correct answer is Option C .

Note: Electropositive implies the tendency to lose electrons to form positive ions. Electronegative implies having a tendency to gain electrons to form negative ions.
Electronegativity is a concept used to describe the tendency of an atom to attract electrons in a covalent bond.
Electropositivity is the tendency to donate electrons and withdraw from covalent form to form positively charged cations.
With the exception of hydrogen, all elements that form positive ions by losing electrons during chemical reactions are called metals. Thus, metals are electropositive elements with relatively low ionization energies.
\[Na\] have $1{e^ - }$ in its outermost shell and have a high tendency to lose ${e^ - }$ & become $N{a^ + }$. So, $Na$ is electropositive whereas $F$ being small and highly electronegative as it tends to complete its outermost shell.