Statement-1 :The thermal stability of hydrides of carbon family is in order:
`CH_(4)gtSiH_(4)gtGeH_(4)gtSnH_(4)gtPbH_(4)`
Statement-2: `E-H` bond dissociation enthalpies of the hydrides of carbon family decrease down the group with increasing atomic size.

Options

A. Statement-1 is Ture, Statement-2 is True,Statement-2 is a correct explanation for Statement-1.
B. Statement-1 is Ture, Statement-2 is True,Statement-2 is NOT a correct explalanation for Statement-1
C. Statement-1 is Ture, Statement-2 is False
D. Statement-1 is False, Statement-2 is Ture

Explanation

To analyze the statements regarding the thermal stability of hydrides of the carbon family and the bond dissociation enthalpies, we can break down the solution into clear steps:

### Step 1: Understand the Hydrides of the Carbon Family
The hydrides of the carbon family (Group 14) include:
- Methane (CH₄)
- Silane (SiH₄)
- Germane (GeH₄)
- Stannane (SnH₄)
- Plumbane (PbH₄)

### Step 2: Analyze Statement 1
**Statement 1**: The thermal stability of hydrides of the carbon family is in the order:
\[ CH₄ > SiH₄ > GeH₄ > SnH₄ > PbH₄ \]

This statement suggests that methane is the most thermally stable, while plumbane is the least stable.

### Step 3: Analyze Statement 2
**Statement 2**: The E-H bond dissociation enthalpies of the hydrides of the carbon family decrease down the group with increasing atomic size.

This statement indicates that as we move down the group from carbon to lead, the bond dissociation enthalpy decreases, which implies that the bonds become weaker.

### Step 4: Correlate Both Statements
- As we move down the group, the atomic size increases, leading to an increase in bond length (the distance between the nucleus of the atom and the hydrogen atom).
- A larger bond length typically results in a weaker bond because the attraction between the nucleus and the bonding electrons decreases.
- Therefore, the bond dissociation enthalpy (the energy required to break the bond) decreases.

### Step 5: Conclusion
- Since the bond dissociation enthalpy decreases, the thermal stability of the hydrides also decreases. Thus, the order of thermal stability given in Statement 1 is correct.
- Statement 2 correctly explains why Statement 1 is true: the decrease in bond dissociation enthalpy due to increasing atomic size leads to decreased thermal stability.

### Final Answer
Both Statement 1 and Statement 2 are true, and Statement 2 is the correct explanation for Statement 1.

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