1 identify each of the following half reactions as either an...

(1) Identify each of the following half-reactions as either an oxidation half-reaction or a reduction half-reaction. half-reaction identification Pb(s)→Pb$^{2+}$(aq) + 2e$^-$ oxidation Cl$_2$(g) + 2e$^-$→2Cl$^−$(aq) reduction (2) Write a balanced equation for the overall redox reaction. Use smallest possible integer coefficients.

Transcript

00:02 The first thing we're asked to do in this question is to identify the half reactions as either being oxidations or reductions.

00:09 So we need to start off by defining these terms so we know what to look for.

00:12 Oxidation refers to a loss of one or more electrons.

00:21 Therefore, in a reaction, if there is a loss of electrons, they're going to be a product because they're given off.

00:29 So the electrons would occur or appear as a product.

00:34 Reduction is the gain of electrons by an atom or ion.

00:42 So if it is going to be gaining one or more electrons, those would go into the reaction as a reactant.

00:49 This brings us to our two half reactions.

00:54 We have zinc, which is a solid, and we see that it forms the zinc ion plus two electrons.

01:13 It had to give off two electrons to form that ion.

01:18 All right, our other half reaction is cl2.

01:23 Actually, let me scoot this back so my arrows line up.

01:28 We have cl2, which is a gas, plus two electrons.

01:34 So we see that electrons are being added to the cl2 and this gives us two chloride ions.

01:45 All right, so we are ready to identify these as oxidation or reduction.

01:50 The first one where we see the electrons being given off or released, they are lost from the zinc element, the zinc atom.

01:58 We see them as a product, so this one must be oxidation...

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