Which of the following order is incorrect?

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(D) $1$. Lewis basic character: The basicity depends on the availability of the lone pair on the central atom. As the size of the central atom increas

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Bond angle : $CH_4 > SiH_4 > GeH_4 > SnH_4$

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(D) $1$. Lewis basic character: The basicity depends on the availability of the lone pair on the central atom. As the size of the central atom increases from $N$ to $Sb$,the lone pair occupies a larger orbital,making it less available for donation. Thus,$NH_3 > PH_3 > AsH_3 > SbH_3$ is correct.$2$. Bond dissociation energy: As the size of the halogen atom increases from $F$ to $I$,the bond length increases and bond strength decreases. Thus,$HF > HCl > HBr > HI$ is correct.$3$. Thermal stability: As the size of the central atom increases down the group,the $M-H$ bond length increases,leading to a decrease in bond strength and thermal stability. Thus,$H_2O > H_2S > H_2Se > H_2Te$ is correct.$4$. Bond angle: In $CH_4$,the bond angle is $109.5^{\circ}$. As the electronegativity of the central atom decreases down the group $(C > Si > Ge > Sn)$,the bond pair electrons move further away from the central atom,causing the bond angle to decrease. However,the trend $CH_4 > SiH_4 > GeH_4 > SnH_4$ is generally observed due to the decrease in electronegativity and increase in size. Wait,all these options are actually correct based on standard chemical trends. Re-evaluating: Actually,the bond angle in $CH_4$ is $109.5^{\circ}$,and for the others,it approaches $90^{\circ}$ as the central atom size increases. The provided options are all correct. If forced to choose an 'incorrect' one,there might be a typo in the question source. Given the standard curriculum,all these trends are correct.

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