Question

1)To determine the oxidation state of a monoatomic ion, first determine the charge of the ion. The oxidation state will be the same 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 of the 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 and the substance being reduced.

Ni2+(aq)+Mg(s)→Mg2+(aq)+Ni(s)

4)In acidic solution, the nitrate ion can be used to react with a 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) and H+(aq) will be involved in the reaction. Places for these species are indicated by the blanks in the following restatement of the equation:

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

What are the coefficients of the reactants and products in the balanced equation above? Remember to include H2O(l) and H+(aq) in the 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, for grading purposes.

5) Classify each half-reaction occurring in acidic aqueous solution as an oxidation or a reduction and balance the half-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 aqueous solution.

Express your answer as a chemical equation. Identify all of 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)

Answer 1

Question 1)

To determine the oxidation state of a monoatomic ion, first determine the charge of the ion. The oxidation state will be the same 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 of the following elements?

Drag each item to the appropriate bin.

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

Ca is in the 2nd family, so it will have a +2 oxidation state

Cs is in the 1st fmaily, so it should have +1 oxidation state

F is in the VIIA family, it has 7 valence electrons, so it will charge with -1, for a total of 8 electrons

Rb is in the 1st family, so it should have +1 oxidation state

Mg is in the 2nd family, so it will have a +2 oxidation state

S is in family 6, it has 6 electrons, so it needs 2 more, it will have -2 oxidation state

B is in the family 3, it will oxidize as +3

Po is in family 6, it has 6 electrons, so it needs 2 more, it will have -2 oxidation state

K is in the 1st fmaily, so it should have +1 oxidation state

N. is in family 5, will typically gain 3 electrons to form octet, so -3

I is in the VIIA family, it has 7 valence electrons, so it will charge with -1, for a total of 8 electrons