Chemical bonding basics — Identify the false statement about molecules held together predominantly by covalent bonds.

Introduction / Context:
Chemical bonding includes covalent, ionic, hydrogen, and other noncovalent interactions. Distinguishing their defining features is foundational in biochemistry and materials science, because bond type dictates structure, stability, and reactivity.

Given Data / Assumptions:

• Covalent bonds arise from electron sharing between atoms (typically nonmetals).
• Large molecules can also contain noncovalent interactions (e.g., hydrogen bonds) stabilizing higher-order structure.
• We must spot the statement that mischaracterizes covalent molecules.

Concept / Approach:
Ionic compounds result from electron transfer and electrostatic attraction of ions, whereas covalent molecules derive from shared electron pairs. Although atoms can be partially charged in polar covalent bonds, the molecules are not “formed from ionized atoms” in the ionic sense. Thus, calling covalent molecules products of ionized atom interactions is incorrect.

Step-by-Step Solution:

Verification / Alternative check:
Textbook definitions clearly distinguish ionic (electron transfer) from covalent (electron sharing) bonding frameworks.

Why Other Options Are Wrong:

• Electron sharing: hallmark of covalency (correct).
• Noncovalent bonds present in large molecules: common for tertiary/quaternary structure (correct).
• Relatively strong bonds: covalent bond energies typically tens to hundreds of kJ/mol (correct).

Common Pitfalls:
Confusing polar covalent partial charges with fully ionized species forming ionic lattices.

Final Answer:
Such molecules often result from the interaction of ionized atoms