this possible? (1 point)
The bonds can shift because valence electrons are held loosely and move freely.
Metals have low electronegativity, so they are conductive because they pass charges easily.
An attraction between a positive charge and a negative charge is created.
Two metals bonded together are going to be more conductive than a metal bonded with a
nonmetal.
5 answers
The correct explanation for why metallic bonds allow metals to conduct electricity is:
The bonds can shift because valence electrons are held loosely and move freely.
In metallic bonding, valence electrons form a "sea of electrons" that can move freely throughout the metal lattice, allowing metals to conduct electricity and heat efficiently.
The correct answer is:
metals and nonmetals, electrons transferred.
Ionic bonds occur between metals and nonmetals, where electrons are transferred from the metal (which loses electrons and becomes positively charged) to the nonmetal (which gains electrons and becomes negatively charged). This transfer creates ions that are held together by electrostatic attraction.
The kind of bond that would occur between sodium (Na, Group IA) and chlorine (Cl, Group VIIA) is:
ionic.
Sodium, a metal, donates its electron to chlorine, a nonmetal, resulting in the formation of sodium ions (Na⁺) and chloride ions (Cl⁻). The electrostatic attraction between these oppositely charged ions creates an ionic bond.
