= Solution
One consistent localized <orbital hybridization> description uses the <Lewis structures>
$$
\mathrm{H_3C-N^+\equiv N},\qquad
\mathrm{H_2C=N^+=N^-}\ \leftrightarrow\ \mathrm{H_2C^--N^+\equiv N}.
$$
\b[For <methyldiazonium>, take C as $sp^3$ and both N atoms as $sp$. For <diazomethane>, the double-bond <resonance contributor> suggests C as $sp^2$, central N as $sp$, and terminal N as $sp^2$.] The central N uses two opposite $sp$ hybrids for the linear C–N–N <sigma bond> framework. In the localized double-bond picture, terminal N uses one $sp^2$ hybrid for its <sigma bond>, two for <lone pairs>, and its remaining p <atomic orbital> for a <pi bond>.
These labels specify an approximate bonding construction, not uniquely measurable atomic properties. An alternative representation takes terminal N as $sp$, with one $sp$ <lone pair> and one p <lone pair>; the latter can participate in the delocalized C–N–N $\pi$ system. It describes the same <resonance> more explicitly. Neither construction requires an unpaired <electron> or a bent central N.
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