EVERYDAY SCIENCE

Detailed explanation-1: -Metals: Metals like to lose valence electrons to form cations to have a fully stable octet. They absorb energy (endothermic) to lose electrons. The electron affinity of metals is lower than that of nonmetals. Nonmetals: Nonmetals like to gain electrons to form anions to have a fully stable octet.

Detailed explanation-2: -Metals – Metal atoms react by losing their valence electrons. The reactivity of a metal depends on how easily its atoms lose valence electrons. The reactivity of metals decreases from left to right across the periodic table.

Detailed explanation-3: -Metal atoms lose electrons to nonmetal atoms because metals typically have relatively low ionization energies. Metals at the bottom of a group lose electrons more easily than those at the top. That is, ionization energies tend to decrease in going from the top to the bottom of a group.

Detailed explanation-4: -When a metal atom loses an electron, it becomes positively charged. Ion is an atom or molecule with a net electric charge due to the loss or gain of one or more electrons.

Detailed explanation-5: -Bonding in metals, called metallic bonding, involves valence electrons. These electrons are loosely held by any one atom and collectively form a “sea of valence electrons” that can be used to explain many metallic properties, e.g., metallic luster, malleability, electrical conductivity, etc.