The metal that will displace hydrogen from an acid is<u> to the left of Hydrogen in the Voltaic series</u>
<h3>Further explanation</h3>
There are two types of chemical reactions that may occur.
namely single-replacement reactions and double-replacement reactions.
A single replacement reaction is a chemical reaction in which one element replaces the other elements of a compound to produce new elements and compounds
Not all of these reactions can occur. We can use the activity series, which is a list of elements that can replace other elements below / to the right of them in a single replacement reaction.
This series is better known as the Voltaic series, where the metal element with a more negative electrode potential is on the left, while the element with a more positive electrode potential on the right.
The more left the position of a metal in the series, the more reactive metal (easy to release electrons, the stronger the reductor)
Generally, the Voltaic series used is
Li K Ba Sr Ca Na Mg Al Mn Zn Cr Fe Cd Co Ni Sn Pb H Sb Bi Cu Hg Ag Pt Au
Example:
2Al (s) + 3Zn (NO₃) ₂ (aq) → 2Al (NO₃) ₃ (aq) + 3Zn (s)
The existing aluminum element can replace the zinc element, which is Al on the left side of Zn so the reaction will occur
From periodic system :
Metal element:
a. Group IA, except hydrogen
b. Group IIA
c. Group IIIA, except boron
d. Group IIIB-IIB
e. Group IVA = lead and lead
f. Group VA = bismuth
Nonmetallic elements:
a. Group IA = hydrogen
b. Group IVA = carbon
c. Group VA = nitrogen, phosphorus
d. Group VIA = oxygen, sulfur, selenium
e. Group VIIA = Phosphorus, chlorine, Bromine, Iodine
f. Group VIIIA
The metal that will displace hydrogen from an acid is to the left of Hydrogen in the Voltaic series, including:
IA: Li, Na, K
IIA: Ba Sr Ca Mg
IIIA: Al
IIB: Zn, Cd
IVA: Sn Pb
<h3>Learn more
</h3>
an oxidation-reduction reaction
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