1)To determine the oxidation state of a monoatomic ion, firstdetermine the charge of the ion. The oxidation state will be thesame as the charge. For example, I forms the monoatomic ion I−;therefore, the oxidation state of the monoatomic ion for I is−1.

What is the oxidation number of the monoatomic ions ofthe following elements?

Drag each item to the appropriate bin.

Ca, Cs, F, Rb, Mg, Po, S, B, K, N, I

[Bins] +3, +2, +1, -1, -2, -3

2)For the following reaction, calculate ΔH∘rxn,ΔS∘rxn, and ΔG∘rxn at 25 ∘C.

NH4Cl(s)→HCl(g)+NH3(g)

3) For each reaction, identify the substance being oxidized andthe substance being reduced.

Ni2+(aq)+Mg(s)→Mg2+(aq)+Ni(s)

4)In acidic solution, the nitrate ion can be used to react witha number of metal ions. One such reaction is

NO3−(aq)+Sn2+(aq)→NO2(aq)+Sn4+(aq)

Since this reaction takes place in acidic solution, H2O(l) andH+(aq) will be involved in the reaction. Places for these speciesare indicated by the blanks in the following restatement of theequation:

NO3−(aq)+Sn2+(aq)+     −−−→NO2(aq)+Sn4+(aq)+

What are the coefficients of the reactants and products in thebalanced equation above? Remember to include H2O(l) and H+(aq) inthe appropriate blanks. Your answer should have six terms.

Enter the equation coefficients in order separated by commas(e.g., 2,2,1,4,4,3). Include coefficients of 1, as required, forgrading purposes.

5) Classify each half-reaction occurring in acidic aqueoussolution as an oxidation or a reduction and balance thehalf-reaction.

S(s)→H2S(g)

S2O8^2−(aq)→2SO4^2−(aq)

Cr2O7^2−(aq)→Cr3+(aq)

NO(g)→NO3−(aq)

6) Balance each redox reaction occurring in basic aqueoussolution.

Express your answer as a chemical equation. Identify allof the phases in your answer.

H2O2(aq)+ClO2(aq)→ClO−2(aq)+O2(g)

Al(s)+MnO−4(aq)→MnO2(s)+Al(OH)−4(aq)

Cl2(g)→Cl−(aq)+ClO−(aq)

7) Classify each reaction as spontaneous or nonspontaneous.

Cr(s) + 3Ag^+(aq)>Cr^3+(aq)+3Ag(s)

Cu(s)+Ca^2+(aq)>Cu^2+(aq) + Ca(s)

Ca(s)+Ni^2+(aq)>Ca^2+(aq)+Ni(s)

Mg(s)+2K^+(aq)>Mg^2+(aq)+2K(s)

Cu(s)2Ag^+(aq)>Cu^2+(aq)+2Ag(2)

Sn(s)+Ni^2+(aq)>Sn^2+(aq)+Ni(s)