Which of the following statements about atoms of a metal is correct? They

Analyze the question: You are asked which statement correctly describes metal atoms. Let's test each option against what we know about metals and metallic bonding.

Concept: Metallic bonding Metal atoms have few valence electrons, which they lose easily. These electrons become delocalised and move freely throughout the structure. The result is a lattice of positive metal ions surrounded by a "sea" of mobile electrons. The electrostatic attraction between the positive ions and the electron sea holds the metal together. This is called the metallic bond.

Evaluating each option:

• A. readily accept electrons: Incorrect. Metals tend to lose electrons to form cations (e.g., Na → Na⁺ + e⁻). Accepting electrons is typical of non-metals.
• B. are soft: Incorrect as a general statement. Many metals are hard and strong (iron, copper, chromium). Only a few, such as sodium and potassium, are soft.
• C. are held together by covalent bond: Incorrect. Covalent bonding involves sharing electron pairs between non-metal atoms. Metals use metallic bonding.
• D. are held together by a sea of electron cloud: Correct. This is exactly the description of metallic bonding: positive ions held in a lattice by delocalised, mobile electrons.

This also explains why metals conduct electricity and heat (mobile electrons) and why they are malleable and ductile (layers of ions can slide without breaking the bond).

Answer: D

Exam tip: Remember "metals lose, non-metals gain." Whenever you see "sea of electrons" or "delocalised electrons," think metallic bond. Also be wary of absolute words like "are soft" in options, since most metals are not.