Ncert Solutions Chemistry Class 11th
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The largest oxidation number exhibited by an element depends on its outer electronic configuration. With which of the following outer electronic configurations the element will exhibit largest oxidation number?
(i) 3d1 4s2
(ii) 3d3 4s2
(iii) 3d5 4s1
(iv) 3d5 4s2
The largest oxidation number exhibited by an element depends on its outer electronic configuration. With which of the following outer electronic configurations the element will exhibit largest oxidation number?
(i) 3d1 4s2
(ii) 3d3 4s2
(iii) 3d5 4s1
(iv) 3d5 4s2
This is a Multiple Choice Questions as classified in NCERT Exemplar
Option (iv) is the correct answer
For 3d1 4s2 can exhibit the highest oxidation state as 2+1 = +3,
For 3d34s2can exhibit the highest oxidation state as 2+3 = +5
For 3d54s1can exhibit the highest oxidation state as 1+5 =&
Upvote 
Which of the following arrangements represent increasing oxidation number of the central atom?
(i) CrO2 – , ClO3 – , CrO4 2– , MnO4 –
(ii) ClO3 – , CrO42– , MnO4 – , CrO2
(iii) CrO2 – , ClO3 – , MnO4 – , CrO4 2–
(iv) CrO4 2– , MnO4 – , CrO2 – , ClO3–
Which of the following arrangements represent increasing oxidation number of the central atom?
(i) CrO2 – , ClO3 – , CrO4 2– , MnO4 –
(ii) ClO3 – , CrO42– , MnO4 – , CrO2
(iii) CrO2 – , ClO3 – , MnO4 – , CrO4 2–
(iv) CrO4 2– , MnO4 – , CrO2 – , ClO3–
This is a Multiple Choice Questions as classified in NCERT Exemplar
Option (i) is the correct answer
Let the oxidation number of central atom be 'y'.
Oxidation number of O = −2
CrO2−: y + 2 × (−2) = −1
y − 4 = −1 or y = +3
CrO42−? : y + 4 × (−2) = −2
y − 8 = −2 or y = +6
C
Upvote In which of the following compounds, an element exhibits two different oxidation states.
(i) NH2OH
(ii) NH4NO3
(iii) N2H4
(iv) N3H
In which of the following compounds, an element exhibits two different oxidation states.
(i) NH2OH
(ii) NH4NO3
(iii) N2H4
(iv) N3H
This is a Multiple Choice Questions as classified in NCERT Exemplar
Option (ii) is the correct answer.
The oxidation states are given below-
In NH2OH oxidation of N is -1.
NH4NO3 exists as NH4+.NO3-,
Thus, the oxidation state of N in NH4+ is -3 while in NO3? is +5.
In N2H4 oxidation of
Upvote The oxidation number of an element in a compound is evaluated on the basis of certain rules. Which of the following rules is not correct in this respect?
(i) The oxidation number of hydrogen is always +1.
(ii) The algebraic sum of all the oxidation numbers in a compound is zero.
(iii) An element in the free or the uncombined state bears oxidation number zero.
(iv) In all its compounds, the oxidation number of fluorine is – 1
The oxidation number of an element in a compound is evaluated on the basis of certain rules. Which of the following rules is not correct in this respect?
(i) The oxidation number of hydrogen is always +1.
(ii) The algebraic sum of all the oxidation numbers in a compound is zero.
(iii) An element in the free or the uncombined state bears oxidation number zero.
(iv) In all its compounds, the oxidation number of fluorine is – 1
This is a Multiple Choice Questions as classified in NCERT Exemplar
Option (i) is the correct answer
In ionic hydrides hydrogen exists in -1 oxidation state because the hydrogen acquires negative charge in the presence of its companion.
Upvote Thiosulphate reacts differently with iodine and bromine in the reactions given below:
2S2O32– + I2 → S4O62– + 2I– S2O32–+ 2Br2 + 5H2O → 2SO42– + 2Br– + 10H
Which of the following statements justifies the above dual behaviour of thiosulphate?
(i) Bromine is a stronger oxidant than iodine.
(ii) Bromine is a weaker oxidant than iodine.
(iii) Thiosulphate undergoes oxidation by bromine and reduction by iodine in these reactions.
(iv) Bromine undergoes oxidation and iodine undergoes reduction in these reactions.
Thiosulphate reacts differently with iodine and bromine in the reactions given below:
2S2O32– + I2 → S4O62– + 2I– S2O32–+ 2Br2 + 5H2O → 2SO42– + 2Br– + 10H
Which of the following statements justifies the above dual behaviour of thiosulphate?
(i) Bromine is a stronger oxidant than iodine.
(ii) Bromine is a weaker oxidant than iodine.
(iii) Thiosulphate undergoes oxidation by bromine and reduction by iodine in these reactions.
(iv) Bromine undergoes oxidation and iodine undergoes reduction in these reactions.
This is a Multiple Choice Questions as classified in NCERT Exemplar
Option (i) is the correct answer.
Standard reduction potential of bromine is higher than Iodine, hence Bromine is a stronger oxidant than iodine.
Upvote Using the standard electrode potential, find out the pair between which redox reaction is not feasible.
EᶱV values : Fe3+/Fe2+ = + 0.77; I2 /I– = + 0.54
Cu2+/Cu = + 0.34; Ag+ /Ag = + 0.80 V
(i) Fe3+ and I–
(ii) Ag+ and Cu
(iii) Fe3+ and Cu
(iv) Ag and Fe3+
Using the standard electrode potential, find out the pair between which redox reaction is not feasible.
EᶱV values : Fe3+/Fe2+ = + 0.77; I2 /I– = + 0.54
Cu2+/Cu = + 0.34; Ag+ /Ag = + 0.80 V
(i) Fe3+ and I–
(ii) Ag+ and Cu
(iii) Fe3+ and Cu
(iv) Ag and Fe3+
This is a Multiple Choice Questions as classified in NCERT Exemplar
Option (iv) is the correct answer.
E? will be negative for the pair Ag and Fe3+. Hence the reaction is not feasible.
Upvote EᶱV values of some redox couples are given below. On the basis of these values choose the correct option.
EᶱV values : Br2 /Br– = + 1.90; Ag+ /Ag(s) = +0.80
Cu2+/Cu(s) = + 0.34; I2 (s)/I– = + 0.54
(i) Cu will reduce Br–
(ii) Cu will reduce Ag
(iii) Cu will reduce I–
(iv) Cu will reduce Br2
EᶱV values of some redox couples are given below. On the basis of these values choose the correct option.
EᶱV values : Br2 /Br– = + 1.90; Ag+ /Ag(s) = +0.80
Cu2+/Cu(s) = + 0.34; I2 (s)/I– = + 0.54
(i) Cu will reduce Br–
(ii) Cu will reduce Ag
(iii) Cu will reduce I–
(iv) Cu will reduce Br2
This is a Multiple Choice Questions as classified in NCERT Exemplar
Option (iv) is the correct answer
Reduction potential is defined as the tendency of the specie to get reduced. More positive the value of E® , greater is the tendency of the species to get reduced and stronger is the oxidisi
Upvote The more positive the value of EV , the greater is the tendency of the species to get reduced. Using the standard electrode potential of redox couples given below find out which of the following is the strongest oxidising agent.
EV values: Fe3+/Fe2+ = + 0.77; I2 (s)/I– = + 0.54;
Cu2+/Cu = + 0.34; Ag+/Ag = + 0.80V
(i) Fe3+
(ii) I2 (s)
(iii) Cu2+
(iv) Ag+
The more positive the value of EV , the greater is the tendency of the species to get reduced. Using the standard electrode potential of redox couples given below find out which of the following is the strongest oxidising agent.
EV values: Fe3+/Fe2+ = + 0.77; I2 (s)/I– = + 0.54;
Cu2+/Cu = + 0.34; Ag+/Ag = + 0.80V
(i) Fe3+
(ii) I2 (s)
(iii) Cu2+
(iv) Ag+
This is a Multiple Choice Questions as classified in NCERT Exemplar
Option (iv) is the correct answer
The strongest oxidising agent means it has greater tendency to oxidise other species and itself gets easily reduced. So higher the E? values, stronger is the oxidising agent it is. Thus, Ag
Upvote Which of the following is not an example of redox reaction?
(i) CuO + H2 → Cu + H2O
(ii) Fe2O3 + 3CO → 2Fe + 3CO2
(iii) 2K + F2 → 2KF
(iv) BaCl2 + H2 SO4 → BaSO4 + 2HCl
Which of the following is not an example of redox reaction?
(i) CuO + H2 → Cu + H2O
(ii) Fe2O3 + 3CO → 2Fe + 3CO2
(iii) 2K + F2 → 2KF
(iv) BaCl2 + H2 SO4 → BaSO4 + 2HCl
This is a Multiple Choice Questions as classified in NCERT Exemplar
option (iv) is the correct answer.
Redox reaction is defined as the simultaneous oxidation and reduction of reacting species. Thus, change in oxidation state will decide whether a reaction is redox or not. Thus, assigning the oxidatio
Upvote Balance the following ionic equations
(i) Cr2 O72– + H+ + I– → Cr3+ + I2 + H2O
(ii) Cr2 O72– + Fe2+ + H+ → Cr3+ + Fe3+ + H2O
(iii) MnO4– + SO32– + H+ → Mn2+ + SO42– + H2O
(iv) MnO4– + H+ + Br– → Mn2+ + Br2 + H2O
Balance the following ionic equations
(i) Cr2 O72– + H+ + I– → Cr3+ + I2 + H2O
(ii) Cr2 O72– + Fe2+ + H+ → Cr3+ + Fe3+ + H2O
(iii) MnO4– + SO32– + H+ → Mn2+ + SO42– + H2O
(iv) MnO4– + H+ + Br– → Mn2+ + Br2 + H2O
This is a Short answer type question as classified in NCERT Exemplar
(i) The balanced chemical is given as –
(ii) The balanced chemical is given as –
(iii) The balanced chemical is given as –
(iv) The balanced chemical is given as –
Upvote