Assertion–Reason (Graphite Properties):\nAssertion (A): Graphite is slippery and used as a lubricant.\nReason (R): Graphite has free (delocalized) electrons.

Introduction / Context:
This question distinguishes between two different properties of graphite: lubricity (slipperiness) and electrical conduction. It asks whether the presence of delocalized electrons explains why graphite acts as a lubricant.

Given Data / Assumptions:

• Graphite is observed to be slippery and is used industrially as a dry lubricant.
• Graphite’s bonding involves delocalized electrons in hexagonal carbon sheets.

Concept / Approach:
Graphite consists of layers (graphene sheets) held together by weak van der Waals forces. The ease with which these layers slide over one another provides lubricity. Delocalized electrons largely explain graphite’s ability to conduct electricity along the planes, not its slipperiness.

Step-by-Step Solution:
1) A: True. The layered structure allows low shear resistance.2) R: True statement about electronic structure; graphite does possess delocalized electrons.3) Link: The explanation for lubricity is interlayer sliding due to weak interlayer bonding, not the presence of free electrons. Hence R does not explain A.

Verification / Alternative check:
Compare with diamond: no delocalized electrons, extremely hard, not slippery. The determining factor for slip is bonding anisotropy rather than electron delocalization.

Why Other Options Are Wrong:
“A & R true and explanatory” conflates conduction with lubrication; “A true, R false” denies correct electronic structure; “A false” contradicts common use.

Common Pitfalls:
Assuming one “special property” of graphite accounts for all behaviors.

Final Answer:
Both A and R are true, but R does not correctly explain A.