freshly I observed a video which said me the Hydrogen has actually a valency that 1, i.e, Hydrogen have the right to only bond through 1 other atom. But since hydrogen wants a complete shell, it deserve to have 2 covalent bonds with 2 electrons. Please explain.

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$egingroup$ 1+1=2. Hydrogen has 1 electron. When it do a bond, that "gets" the second bonding electron, ergo has actually 2 and also thus a complete shell. $endgroup$
Apart from some team 13 weirdness, hydrogen have the right to only make one bond. Covalent bonds call for pairs the electrons and hydrogen deserve to only have two electrons bound in one covalent bond.


Hydrogen develops 1 solitary bond when there is a s-s overlap which is the biggest overlap however it deserve to also type 2 single bond whereby there are 2 s-p overlaps such together is even in compounds choose $ceB2H6$, H seems to make 2 bonds however it doesn"t.

As you deserve to see the two Hydrogen atoms in the centre make 2 binding each v Boron.

The variety of a bonds the hydrogen can make is dependent on the kind of bonding.

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It can type only a single ionic bond. That can type two bonds when there is overlap connected (covalent bond)It can form a solitary covalent bond.If stability have the right to be achieved it can kind a most coordinate bonds, but due to it"s little size and also only a single proton I would certainly think a max of 1 combination bond deserve to be created if us being through an ionised H-atom.


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