Which of the following reactions occur at the negative electrode if a 1 M NaCl (aq) solution is used as a plating solution? Select a balanced reduction half-reaction below for your answer. Hint - Na metal cannot be produced in aqueous solutions. Na+ + e- → Na (s) Cl2 + 2 e- → 2 Cl- (aq) H2O + e- → 1/2 H2 (g) + OH- (aq) H2O → H+ (aq) + OH- (aq) Na + e- → Na- (aq)

(D) Na + e⁻ → Na⁻ (aq)

Explanation:

Negative electrode is cathode, and the type of reaction that occur here is reduction reaction.

In the electrolysis of aqueous solution of NaCl, the compound will dissociate into;

NaCl > Na⁺ + Cl⁻ and H₂O > H⁺ + OH⁻

At the negative electrode (cathode), we will have the following possible ions;

Na⁺ and H⁺

Hydrogen ion gains electron and hydrogen gas is produced;

H⁺ + e⁻ > H₂ (g)

Note: Sodium (Na) metal cannot be produced in aqueous solutions

Thus, Sodium metal will gain electron and become electronegative, which goes back into the solution. This is why it cannot be produced.

Na + e⁻ > Na⁻ (aq)

Therefore, the correct option is (D) Na + e⁻ → Na⁻ (aq)

electron microscopy and scanning tunneling microscopes gives us a greater understanding of atoms by being able to see the atom itself, and lets us see some atomic reactions.

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there all right good

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