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(C) $1$. Reducing nature: The bond dissociation energy decreases down the group $(NH_3 > PH_3 > AsH_3 > SbH_3 > BiH_3)$, so the reducing nature increa

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$A, B, C$ and $D$

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(C) $1$. Reducing nature: The bond dissociation energy decreases down the group $(NH_3 > PH_3 > AsH_3 > SbH_3 > BiH_3)$, so the reducing nature increases from $NH_3$ to $BiH_3$. ($A$ is correct).$2$. Tendency to donate lone pair: Electronegativity of the central atom decreases and the size of the central atom increases down the group, making the lone pair more diffuse. Thus, the basicity (tendency to donate a lone pair) decreases from $NH_3$ to $BiH_3$. ($B$ is correct).$3$. Stability: Bond dissociation energy decreases down the group as the $E-H$ bond length increases, so thermal stability decreases from $NH_3$ to $BiH_3$. ($C$ is correct).$4$. Bond angle: The bond angle depends on the electronegativity of the central atom. As electronegativity decreases down the group, the bond pairs are further away from the central atom, which decreases the bond angle. The order is $NH_3 (107.8^{\circ}) > PH_3 (93.6^{\circ}) > AsH_3 (91.8^{\circ}) > SbH_3 (91.3^{\circ})$. ($D$ is correct).Therefore, all statements $A, B, C$, and $D$ are correct.

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