Question

How does the location of hydrogen on the periodic table differ from other nonmetals?

Answer 1

hydrogen is a nonmetal and is put above the group in the periodic table since it has $n{s^1}$ electron design like the alkali metals. Notwithstanding, it changes extraordinarily from the alkali metals as it forms cations $\left( {{H^ + }} \right)$ more hesitantly than the other alkali metals.
Since hydrogen is a nonmetal and structures ${H^ - }$ (hydride anions), it is now and then positioned above the halogen in the periodic table. Hydrogen also forms ${H_2}$ dihydrogen like halogen. In any case, hydrogen is totally different from the halogen

Complete step by step answer:
One manner it could 'attempt' to acquire an electron as any element from the halogen group $\left( {F - Cl - Br...} \right)$ would do.
Then again, it could lose its one electron, where case it would have a place with the alkali metals $\left( {Li - Na - K...} \right).$
Practically speaking,$\;H$ generally shares its electron, either by covalent bonds, or by donating an electron and cooperating with$\;{H_2}O$ to frame the ${H_3}O + {\text{ }}or{\text{ }}'acid'$ particle. So, H is too uncommon to even consider placing it in a specific Group.
It's unique, since it has just a single electron, while the ideal "noble gas" setup (helium) would call for two.

Note: Hydrogen has a much smaller electron affinity than halogens. ${H_2}$ dihydrogen or atomic hydrogen is non-polar with two electrons. There are weak attractive forces between ${H_2}$ molecules, bringing about low boiling and melting points. Be that as it may, ${H_2}$ has solid intramolecular forces; ${H_2}$ reaction are for the most part delayed at room temperature because of the solid$\;H--H{\text{ }}bond.$ ${H_2}$ is handily activated by heat, irradiation, or catalysis. Initiated hydrogen gas reacts rapidly and exothermically with numerous substances.