Question

Why are metals electropositive in nature?

Answer 1

We need to realize that metals are substances, which are acceptable conveyors of warmth and power. They have metallic bonds. Metals promptly structure cations that are positive particles, they don’t frame anions. A portion of the instances of metals are cobalt, iron, sodium, copper, zinc, aluminum.

Complete answer:
We have to know that metals have various properties. Metals have high softening focuses. They have high thickness. They have metallic radiance. They are strong at room temperature just mercury is a metal which is in fluid state at room temperature.
We have to see that a few metals are sparkly in nature, a portion of the instances of such metals are gold and silver. Silver is the best conduit of power.
We need to realize that metals are electropositive in nature. Non-metals are electronegative in nature. Non-metals are electronegative in nature since they have an inclination of tolerating electrons or they can acquire electrons all the more without any problem. Then again metals tend to lose electrons all the more without any problem.
Therefore, the metals lose electrons to settle themselves. They lose electrons since valence electrons of the furthest shell are feebly drawn to the core.

Note:
Continuously recollect that metals are electropositive in nature. Non-metals are electronegative in nature. Caesium is the most electropositive in nature and fluorine is the most electronegative in nature. Metals are electropositive on the grounds that they can without much of a stretch lose their valence electron from their peripheral shell.