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Hydrogen readily combines with non-metals and thus it shows its
A. Electronegative character
B. Electropositive character
C. Both a and b
D. None of these

Last updated date: 16th Apr 2024
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MVSAT 2024
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Hint: Hydrogen is a very special element due to its resemblance with many elements of different groups. Hydrogen resembles the halogens, alkali metals and carbon family of the periodic table. Due to its half filled orbital, it can gain or lose electrons to form a $H-$ or $H+$ ion. It is a strong reducing agent as it readily loses one electron and donates it to the other substance and thus helps in reduction by itself getting oxidised.

Complete Step by Step Answer:
Electropositive character of an element means an element can easily lose an electron to form an electropositive ion. For example, hydrogen acts as an electropositive ion when it reacts with highly electronegative ions such as elements of group $16$ or $17$ (non-metals).
$H(g)\longrightarrow H^{+}{+}e^{-}$
$H_{2}(g){+}Cl_{2}(g)\longrightarrow HCl(g)$

Electronegative character of an element means an element gains an electron to form an electronegative ion and complete its octet. For example, hydrogen acts as an electronegative ion when it combines with highly electropositive ions such as elements of group $1$ or $2$ (alkali and alkali earth metals).
$H(g){+}e^{-}\longrightarrow H^{-}$
$2Na(s){+}H_{2}(g)\longrightarrow 2NaH(s)$
Thus, when hydrogen readily reacts with non-metals it shows its electropositive character.
Hence, the correct answer is Option (B).

Note: Hydrogen forms polar covalent bonds due to them being much less electropositive than alkali metals. Covalent hydrides are formed as a result of reaction between hydrogen and nonmetals. For example, when sulphur reacts with hydrogen they form covalent sulphur hydride Hydrogen has low melting and boiling point due to which they have weak forces of attraction.