Comment over the following statement
The electronegativity of Pb is higher than that of Sn.

Answer

To comment on the statement "The electronegativity of Pb is higher than that of Sn," we need to analyze the factors affecting electronegativity and the specific properties of lead (Pb) and tin (Sn).

### Step-by-Step Solution:

1. **Understanding Electronegativity**:
Electronegativity is defined as the tendency of an atom to attract a shared pair of electrons in a covalent bond. It is influenced by the atomic size and the effective nuclear charge.

**Hint**: Remember that electronegativity is a measure of an atom's ability to attract electrons in a bond.

2. **Position in the Periodic Table**:
Both lead (Pb) and tin (Sn) are located in Group 14 of the periodic table. As you move down a group, the atomic size increases due to the addition of electron shells.

**Hint**: Consider how the position of elements in the periodic table affects their properties.

3. **Atomic Size**:
As we move from tin to lead, the atomic size increases. This increase in size generally leads to a decrease in electronegativity because the outer electrons are further from the nucleus and experience a weaker attraction.

**Hint**: Think about how distance from the nucleus affects the attraction between the nucleus and the outer electrons.

4. **Nuclear Charge**:
Although the size increases, the nuclear charge (the total charge of the nucleus due to protons) also increases as we move from Sn to Pb. Lead has more protons than tin, which contributes to a stronger attraction for the shared electrons.

**Hint**: Recall that a higher nuclear charge can enhance the ability of an atom to attract electrons.

5. **Shielding Effect**:
In lead, the presence of filled inner f-orbitals (4f) provides a poor shielding effect. This means that even though lead is larger, the effective nuclear charge experienced by the outer electrons is still significant, allowing lead to have a higher electronegativity than what would be expected solely based on size.

**Hint**: Consider how inner electron shells can affect the attraction of outer electrons.

6. **Experimental Values**:
The experimental electronegativity values support this conclusion: lead has an electronegativity of approximately 2.3, while tin has an electronegativity of about 1.9. This confirms that lead is indeed more electronegative than tin.

**Hint**: Look for experimental data to validate theoretical conclusions.

### Conclusion:
In conclusion, despite the general trend of decreasing electronegativity down a group due to increasing atomic size, lead (Pb) exhibits higher electronegativity than tin (Sn) due to its higher nuclear charge and the poor shielding effect of its inner f-orbitals. The experimental electronegativity values of 2.3 for lead and 1.9 for tin further confirm this observation.