Assertion: Empirical formula represents the simplest whole-number ratio of atoms in a compound. Reason: Molecular formula always represents the simplest ratio of atoms.

📘 Assertion–Reason Analysis

🔵 Assertion

Empirical formula represents the simplest whole-number ratio of atoms in a compound.

This statement is TRUE. The empirical formula gives the simplest whole-number ratio of the different atoms present in a compound.

Example: C₆H₁₂O₆ → CH₂O

The ratio 6 : 12 : 6 is simplified by dividing by 6, giving 1 : 2 : 1.

🟠 Reason

Molecular formula always represents the simplest ratio of atoms.

This statement is FALSE. The molecular formula represents the actual number of atoms of each element present in one molecule. It may be a multiple of the empirical formula.

C₆H₁₂O₆ ≠ simplest ratio

C₆H₁₂O₆ = 6 × CH₂O

🧮 Suitable Example

Consider glucose:

Molecular Formula = C₆H₁₂O₆

The atomic ratio is:

C : H : O = 6 : 12 : 6

Dividing all the numbers by 6:

6 : 12 : 6 → 1 : 2 : 1

Therefore, the empirical formula is:

CH₂O

🎬 Molecular Formula → Empirical Formula

C C C C → CH₂O

C₆H₁₂O₆ ÷ 6 → CH₂O

The molecular formula is reduced to its simplest whole-number ratio to obtain the empirical formula.

🔗 Important Difference

Empirical Formula
Simplest whole-number ratio

Molecular Formula
Actual number of atoms in one molecule

Molecular Formula = n × Empirical Formula

✅ Final Answer

Assertion is TRUE, but Reason is FALSE.

The molecular formula does not always represent the simplest ratio of atoms. The empirical formula represents the simplest whole-number ratio.

🎯 Key Concept

Empirical Formula = Simplest Ratio

Molecular Formula = Actual Formula

C₆H₁₂O₆ → CH₂O