Chemistry, 09.07.2019 12:00 ggujjnh

What is the cathode in mg(s) | mg2+(aq) || au+(aq) | au(s) mg2+ + 2 e − → mg e ◦ red = −2.36 au+ + e − → au e ◦ red = +1.69 and what is the cell type? 1. mg(s); an elec?

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Answer from: liferoblox666

Cathode: $\text{Au} \; (s)$

A Voltaic Cell

Explanation

Reduction occurs at the cathode in both electrochemical cells and voltaic cells. The species that gains electrons in a redox process is being reduced. Recall that $\Delta G = - n F E$ ; the species with the most positive standard cell potential would have the reduction reaction with the most negative change in Gibbs free energy and is therefore most stable when reduced than in the original state. The reduction potential of $\text{Au}^{+}$ is higher than that of $\text{Mg}^{2+}$ ; as a result, $\text{Au}^{+}$ would readily gain electrons from the $\text{Mg} \; (s)$ electrode to produce $\text{Au} \; (s)$ when connected with an external circuit. Therefore the $\text{Au}$ electrode, immersed in the $\text{Au}^{+}$ solution which experiences reduction, would serve as the cathode.

The reaction one would expect to observe in this cell

$\text{Mg} \; (s) + 2 \; \text{Au}^{+} \; (aq) \to \text{Mg}^{2+} \; (aq) + 2 \; \text{Au} \; (s)$

has a standard cell potential $\Delta E ^{\text{o}}$ of $+4.05 \; \text{V} 0 \; \text{V}$ . The overall reaction is exothermic and leads to the release of energy. The cell is therefore a voltaic cell.

Answer from: Quest

explanation:

Answer from: Quest

assuming that your periodic table has eighteen columns, you should highlight the four elements in the third column from the left of the table.

explanation

neutral atoms of elements after calcium contain d electrons. the energy of d orbitals of a particular main shell lies between the energy of the s and p orbitals of the next main shell. for example, electrons in the $3d$ have energy higher than those in the $4 s$ orbital while lower than those of the $4 p$ orbital.

by the aufbau principle, electrons fill orbitals one at a time, starting from those of the lowest energy. the $4s$ orbital is therefore filled right after $3p$ orbitals and before $3 d$ orbitals.

potassium has electron configuration $[\text{ar}] 4 s^{1}$ and calcium $[\text{ar}] 4 s^{2}$ . the s orbital of a main shell holds a maximum of two electrons. the next element would thus have the electron configuration $[\text{ar}] 4 s^{2} \; 3d^{1}$ and satisfy the requirements.

a neutral atom of the element contains three electrons on top of the most recent noble gas element. it should thus be placed in the third column of the periodic table. both scandium and yttrium would satisfy the conditions. an aufbau diagram indicates that the 4f orbital is filled before the 5d. however, it appears that exceptions exists for both lanthanum and actinium. neutral atoms of the two d-block elements also demonstrate the $ns^{2} \; (n-1) p^{1}$ and should be highlighted as well.

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What is the cathode in mg(s) | mg2+(aq) || au+(aq) | au(s) mg2+ + 2 e − → mg e ◦ red = −2.36 au+ + e...

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