For each reaction, identify the element that gets reduced and the element that gets oxidized. 2 AgCl + Zn ⟶ 2 Ag + ZnCl 2 2AgCl+Zn⟶2Ag+ZnCl2 Identify the element that gets reduced. chlorine silver zinc Identify the element that gets oxidized. chlorine silver zinc 4 NH 3 + 3 O 2 ⟶ 2 N 2 + 6 H 2 O 4NH3+3O2⟶2N2+6H2O Identify the element that gets reduced. oxygen hydrogen nitrogen Identify the element that gets oxidized. hydrogen oxygen nitrogen Fe 2 O 3 + 2 Al ⟶ Al 2 O 3 + 2 Fe Fe2O3+2Al⟶Al2O3+2Fe Identify the element that gets reduced. aluminum oxygen iron Identify the element that gets oxidized. oxygen iron aluminum

Oxidation:

Oxidation involve the removal of electrons and oxidation state of atom of an element is increased.

Reduction:

Reduction involve the gain of electron and oxidation number is decreased.

Oxidizing agents:

Oxidizing agents oxidize the other elements and itself gets reduced.

Reducing agents:

Reducing agents reduced the other element are it self gets oxidized.

Consider the following reaction:

2AgCl + Zn → 2Ag + ZnCl₂

In this reaction oxidation state of Zn on left side is 0 while on right side + 2 so it gets oxidized and oxidation state of Ag on left side is + 1 and on right side 0 so it get reduced.

4NH₃ + 3O₂ → 2N₂ + 6H₂O

In this reaction oxidation state of nitrogen on left side is - 3 while on right side 0 so it gets oxidized and oxidation state of oxygen on left side is 0 and on right side - 2 so it get reduced.

Fe₂O₃ + 2Al → Al₂O₃ + 2Fe

In this reaction oxidation state of iron on left side is + 3 while on right side 0 so it gets reduced and oxidation state of Al on left side is 0 and on right side + 3 so it get oxidized.