Oxidation number of Fe in K₃[Fe(CN)₆] is:

(a) +2

(b) +3

(c) +4

(d) +1

The correct order of reducing power of halide ions is:

(1) Cl^- > Br^- > I^- > F^-

(2) Cl^- >  I^- > Br^- > F^-

(3)  Br^- > Cl^- > I^- > F^-

(4)  I^- > Br^- > Cl^- > F^-

In which of the following processes nitrogen is oxidised?

(a) N${\mathrm{H}}_4^{+}$ $\to$N₂

(b) N${\mathrm{O}}_3^{-}<mspace\; width="1em"></mspace>\to$NO

(c) NO₂ $\to$N${\mathrm{O}}_2^{-}$

(d) NO₃ $\to$N${\mathrm{H}}_4^{+}$ 

Fluorine is a strong oxidising agent because:

(1) it has several isotopes

(2) it is very small and has 7 electrons in valency shell

(3) its valency is one

(4) it is the first member of the halogen series

The oxidation state of Ni in Ni(CO)₄ is:

(a) zero

(b) +4

(c) +8 

(d) +2

When SO₂ is passed through acidified solution of potassium dichromate, then chromium sulphate is formed. The change in oxidation number of chromium is:

(1) +4 to+2 

(2) +5 to+3

(3) +6 to+3

(4) +7 to+2

In the reaction;

2Ag + 2H₂SO₄ $\to$Ag₂SO₄ + 2H₂O + SO₂,H₂SO₄ acts as:

(1) oxidising agent

(2) reducing agent

(3) dehydrating agent

(4) none of these

In the equation,

N${\mathrm{O}}_2^{-}$ +  H₂O $\to$N${\mathrm{O}}_3^{-}$ + 2H⁺ + ne^-

n stands for:

(a) H⁺

(b) e^-

(c) 2e^-

(d) 3e^-

In the reaction between acidified K₂Cr₂O₇ and iron (II) ions shown by the equation:

Cr₂${\mathrm{O}}_7^{2-}$(aq) + 6Fe²⁺(aq) +14H⁺(aq)$\to$2Cr³⁺(aq) + 7H₂O(l) + 6Fe³⁺(aq)

(a) the colour of the solution changes from green to blue

(b) the iron (II) ions are reduced 

(c) the dichromate ions are reduced 

(d) hydrogen ions are reduced

Which metal exhibits more than one oxidation states?

(1) Na

(2) Mg

(3) Al

(4) Fe