Can =NH2+ in Arginine's side chain form hydrogen bonding at physiological pH?

I know that at physiological pH, Arginine will have its $$\ce{=NH}$$ protonated to $$\ce{=NH2+}$$. I was wondering if this $$\ce{=NH2+}$$ can still form a hydrogen bond by being a donor? And does the positive charge on Nitrogen affect the hydrogen bonding's strength? My confusion stems from the definition of hydrogen bonding, which says that hydrogen's electron cloud needs to be withdrawn by a more electronegative atom like $$\ce{F, O, N}$$ to be partially positive enough to participate. Therefore, I believe that the positively charged N will withdraw electrons from hydrogens more strongly, leading to more partially positively charged hydrogen and eventually stronger H-bonding with another molecule. Could someone please verify this for me?

Moreover, I have seen $$\ce{=O}$$ and $$\ce{=N}$$ forming hydrogen bonding by being an acceptor. However, I tried search but did not find any example of $$\ce{=NH3+}$$ or $$\ce{=NH2R+}$$ or NHR2+ forming hydrogen bonding as a donor. So can a Nitrogen with a double bond still participate in hydrogen bonding as a donor?

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