Question

The present position of hydrogen in the modern periodic table is completely justifiable.
a.) True
b.) False

Answer 1

Hint: We know that hydrogen is an s-block element from the 1st group and 1st period element. And have the same valence electron as alkali metals but don’t have other properties similar to alkali metals.
Step by step solution:
The position of hydrogen is controversial in the periodic table because hydrogen is the only element without neutrons. Hydrogen is a nonmetal and is placed above the group in the periodic table because it has $n{{s}^{1}}$ electron configuration like the alkali metals. However, it varies greatly from the alkali metals as it forms cations (${{H}^{+}}$) more reluctantly than the other alkali metals. The present position of hydrogen with alkali metals is not justifiable since it shows some properties of alkali metals and some properties of halogens.
Here are some properties of hydrogen element:
It has high ionization potential value comparable with halogens in contrast to $1A$ group elements having a low ionization potential value.
Hydrogen also forms ${{H}^{-}}$ion whereas alkali metals do not form.
It shows certain similarities with the$1A$ group. They are a formation of halides of formula Mcls (where ‘M’ is alkali metal and ‘cl’ is halogen) formation of ${{H}^{+}}$ ion, electropositive nature etc.
So, from the above explanation we can say the given statement is “False”.

Note: Not all the properties of hydrogen are different from alkali metals and also not all the properties are similar to the halogens. Similar to halogens it makes diatomic molecules and several covalent compounds.