Chemical Bonding — Electron Transfer Between Atoms The type of chemical bond formed primarily by transfer of electrons from one atom to another is called:

Introduction / Context:
Materials science connects atomic bonding with macroscopic properties such as melting point, electrical conductivity, and plasticity. The major bonding types are ionic, covalent, and metallic, each associated with specific electron arrangements and energy landscapes.

Given Data / Assumptions:

• Two atoms with different electronegativities interact.
• One atom tends to donate electrons; the other tends to accept.
• Resulting species are ions with electrostatic attraction.

Concept / Approach:
In an ionic bond, one or more electrons are transferred from a less electronegative atom (often a metal) to a more electronegative atom (often a non-metal). The resulting cations and anions attract electrostatically, forming a crystal with high lattice energy. This differs from covalent bonding, where electrons are shared, and metallic bonding, where valence electrons are delocalised to form an electron cloud around positive ion cores.

Step-by-Step Solution:
Identify electron transfer process: donor atom → electron loss → cation; acceptor atom → electron gain → anion.Recognise strong Coulombic attraction between oppositely charged ions.Match to bond type: ionic bond is defined by electron transfer and electrostatic attraction.

Verification / Alternative check:
Classic examples include NaCl, MgO, and CaF2; their crystal structures and properties (high melting points, brittleness) support ionic bonding.

Why Other Options Are Wrong:
Covalent bonds involve shared electron pairs, not net transfer.Metallic bonds feature a delocalised electron “sea,” not discrete ion pairs from transfer.“None of these” is incorrect because the named type is well established.

Common Pitfalls:
Assuming mixed bonding cannot exist; many solids have partial ionic/covalent character, but the defining mechanism here is transfer.

Final Answer:
ionic bond