Concept:Solids can be categorized by their internal bonding: molecular solids (weak forces, soft), network covalent solids (strong bonds, hard), and ionic/hydrogen bonded solids (crystalline, brittle).
Formula:Not applicable.
Solution:- Iodine (\( \text{I}_2 \)) is a perfectly non-polar diatomic molecule. It crystallizes entirely via weak London dispersion forces. As a result, iodine crystals are very soft and readily sublime at low temperatures.
- Ice (\( \text{H}_2\text{O} \)) is held by strong, rigid hydrogen bonds.
- Sugar molecules form massive interlocked networks of strong hydrogen bonds, making them relatively hard crystalline solids.
- Graphite is a giant covalent network solid (macromolecule) with extremely strong internal carbon-carbon covalent bonds, even though sliding layers exist.
Why other options are incorrect:Only non-polar \( \text{I}_2 \) genuinely fits the textbook definition of a "soft solid with weak intermolecular forces" among the choices provided.
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