If you complete and balance the following oxidation-reduction reaction in basic solutionno2−(aq) + al(s) → nh3(aq) + al(oh)4−(aq)how many hydroxide ions are there in the balanced equation (for the reaction balanced with the smallest whole-number coefficients)?

There is one 1 hydroxide ion in the balanced equation.

Explanation:

Oxidation reaction is defined as the chemical reaction in which an atom looses its electrons. The oxidation number of the atom gets increased during this reaction.

Reduction reaction is defined as the chemical reaction in which an atom gains electrons. The oxidation number of the atom gets reduced during this reaction.

For the given chemical reaction:

The half cell reactions for the above reaction follows:

Reduction half reaction:  

Oxidation half reaction:  

Multiplying the Oxidation half reaction by 2 and we get that:-

Adding the half reactions, we get that:-

There is one 1 hydroxide ion in the balanced equation.

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"among the transition metal elements, manganese and zinc have a slight lowering of electronegativities. the reason behind this is that the nuclear charges of these elements are slightly weaker than the other transition metal elements due to the way their valence electrons are filled up. both manganese and zinc have their valence electrons filled up to the 4th shell with 1 pair of electrons (4s2) completely occupying it. although the electrons in the 3rd shell (3d) are yet to be paired since the outer most shell is filled up, the ability of the nucleus to attract electrons is lessened. hence,   the electronegativity (or the ability to attract electrons) is lessened."