How are electrons transferred in a ionic bond?

Answer 1

each atom has its own attraction for electrons called electronegativity. This electronegetivity is determined by-

-number of protons

-size of electron cloud (distance of valence electrons from the nucleus)

- and number of valence electrons

the elements with low electronegetivity are called metals, and those with high electronegetivity are non-metals.

Flourine has the highest electronegetivity- 4

Francium has the lowest.

in an ionic bond, one of the atoms involved must have a low electronegetivity, and the other a high electronegetivity (difference must be greater than or equal to 1.7). the atom that has a high electronegetivity is generally a non-metal, and the other is generally a metal.

when the metal collides with the non-metal, the valence electron from the metal is stripped off by the non-metal. the non-metal gains the electron, leaving it with a net negative charge. The metal, having lost a negative charge, is left with a net positive charge. This difference in charges holds the two ions together, forming the ionic bond.

Answer 2

In an ionic bond, electrons are transferred from one atom to another. One atom loses electrons (becomes a positively charged ion) and the other atom gains those electrons (becomes a negatively charged ion), leading to the attraction between the oppositely charged ions.