What characteristics do you expect from an electron-deficient hydride with respect to its structure and chemical reactions?

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Solution

An electron-deficient hydride does not have sufficient electrons to form a regular bond in which two electrons are shared by two atoms e.g., $B_{2} H_{6}, A l_{2} H_{6}$ etc.
These hydrides cannot be represented by conventional Lewis structures. $B_{2} H_{6}$ , for example, contains four regular bonds and two three centered-two electron bond. Its structure can be represented as:

Since these hydrides are electron-deficient, they have a tendency to accept electrons.
Hence, they act as Lewis acids.
$B_{2} H_{6} + 2 N M e \to 2 B H_{3} . N M e_{3}$
$B_{2} H_{6} + 2 C O \to 2 B H_{3} . C O$

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