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Redox Reactions - Class 11 Medical Chemistry - Extra Questions

Arrange the following in the order of increasing oxidation number of chlorine: Cl2O7,Cl2O,HCl,ClF3,Cl2.



Write oxidation. no of chromium in CrO5.



Complete the following chemical reactions.
(i) PbS(s)+H2O2(aq)
(ii) MnO4(aq)+H2O2(aq)
(iii) CaO(s)+H2O(g)
(Iv) AlCl3(g)+H2O(l)
(v) Ca3N2(s)+H2O(l)
Classify the above into 
(a) hydrolysis, 
(b) redox and 
(c) hydration reaction.



The sum of the oxidation numbers of both the nitrogen atoms in NH4NO3 is :



Mention the oxidation number of Oxygen in Superoxides.



Find oxidation number of boron in NaBH4.



Is the following reaction is a redox reaction?
BaO2+H2SO4BaSO4+H2O2



The oxidation number of Mn in the product of alkaline oxidative fusion of MnO2 is



Find the oxidation numbers to the underlined species in the following compounds or ions.
C2H5OH
H3PO3



Calculate the oxidation number of 
S in Na2S4O6



Calculate the oxidation number of 
Fe in Fe3O4



Oxidation number of O in H2O2 is: 



What is oxidation number of nickel in [Ni(CO)4]?



Calculate oxidation number of S in H2SO4 and C in C3O2



Calculate the oxidation number of 
Pb in Pb3O4



What is an oxidation number or oxidation state ? how is it useful to  identify  redox reactions, oxidant and reductant ?



Solve;-
Oxidation state of Cr. in Cr2(SO4)3 



Oxidation states of nitrogen in the explosive formed by reaction of ammonia iodine is          .



How has this black coloured substance formed ?



Match the List I with List II.



In the following reactions, find the sum of x+y+z:

(i) xNa+O2yNa2O
(ii) H2SO4+2NaOHNa2SO4+yH2O
(iii) yH2O22H2O+O2
(iv) 2Al+2H3PO42AlPO4+zH2
(v) Ca(OH)2+2HClCaCl2+yH2O



SO2 reduces Cr2O72 to Cr2+. The change in oxidation number of Cr is: 



When SO2 gas is passed into aqueous K2Cr2O7 solution (orange), it changes to green coloured solution. What is the oxidation number of the species that has this green color?



The oxidation state of "C" in diamond is :



What is the oxidation number of Mg in magnesium nitride?



The brown ring complex [Fe(H2O)5NO+]SO4 has oxidation number of Fe as :



On combustion of CH4 to CO2 and H2, the oxidation number of carbon changes by :



Number of peroxy linkage in K3Cr(O2)x having oxidation number of Cr as +5 is :



Oxidation number of Cr in (NH3)2Cr(O2)2 is:



The oxidation state of I in H4IO6 is :



The oxidation number of chlorine is NaClO3 is :



The oxidation state of N in NaNO3 is +x. Here, x is :



Find the sum of oxidation state of phosphorus in H3PO4 and H3PO3.



What is the oxidation number of underlined element?

       S_2 



Among the compounds given, what is the total number of compounds having +5 oxidation state of the underlined elements?
a.  K4P2_O7
b.  NaAu_Cl4
c.  Rb4Na[HV10_O28]
d.  I_Cl
e.  Ba2Xe_O6
f.  O_F2
g.  Ca(Cl_O2)2
h.  N_O2



Among the following, what is the total number of compounds having +3 oxidation state of the underlined elements?
a.  K4P2_O7
b.  NaAu_Cl4
c.  Rb4Na[HV10_O28]
d.  I_Cl
e.  Ba2Xe_O6
f.  O_F2
g.  Ca(Cl_O2)2
h.  N_O2



Among the following, what is the total number of compounds having zero oxidation state of the underlined elements?
a.  S_O23
b.  H2C_O
c.  C_H2Cl2
d.  Na2Cr2_O7
e.  O3_



The oxidation number of Ni in K4[Ni(CN)4] is :



The oxidation states of sulphur in SO23 is :



Oxidation number of iodine in IF3 is:



The oxidation number of sulphur in the sulphur molecule (S8) is :



The oxidation states of sulphur in S2O24 is :



The oxidation number of phosphorus in P2O47 is



The oxidation state of sulphur in S2O26 is :



Justify that the following reactions are redox reactions:

CuO(s)+H2(g)Cu(s)+H2O(g)



For a titration of 100cm3 of 0.1 M Sn2+ to Sn4+, 50 cm3 of 0.40 M Ce4+ solution was required. The oxidation state of cerium in the reduction product is :



Consider the reactions:
Why it is more appropriate to write these reactions as: 6CO2(g)+12H2O(l)C6H12O6(aq)+6O2(g)+6H2O(l)
Also suggest a technique to investigate the path of the above (a) and (b) redox  reactions.
6CO2(g)+6H2O(l)C6H12O6(aq)+6O2(g)



What are the oxidation number of the underlined elements in each of the following and how do you rationalise your results?
KI_3



Assign oxidation numbers to each atom of the following reaction equation:
2Fe(s)+O2(g)+2H2O(l)2Fe(OH)2(s)



NaOH+H2SO4Na2SO4+H2O. Balance the given chemical equation



What is the oxidation state of sulphur in the following.
a) SF6    b) Na2S2O3



A greenish yellow gas burns in a rotten egg smelling gas giving an acidic gas and a yellow coloured non metal. Write the balanced chemical equation of the reaction.



Explain how Zn+2AgNO32Ag+Zn(NO3)2 is a redox reaction.



Give two examples for oxidation-reduction reaction.



Read the redox reaction given below and answer the questions:
CuO+H2Cu+H2O
(a) Conversion of CuO into Cu is called _______.
(b) Conversion of H2 into H2O is called _______.



What is the oxidation number of Mn in KMnO4 and of S in Na2S2O3?



Find the oxidation number of S in HSO3 ion.



Find the oxidation number of Mn in [MnO4] ion.



Which compound amongst the following has the highest oxidation number for Mn? KMnO4,K2MnO4,MnO2 and Mn2O3.



Find the oxidation number of Pt in [PtCl6]2 ion.



Balance the following equation by oxidation number method.
PbS+H2O2PbSO4+H2O.



Find the oxidation number of P in NaH2PO4.



Find the oxidation number of Fe in [Fe(CN)6]4.



Find the oxidation number of Ni in [Ni(CN)6]4.



Find the oxidation number of P in PH+4.



Find the oxidation number of Pt in [PtCl6]2.



Find the oxidation number of C in C12H22O11.



Find the oxidation number of S in H2S2O8.



Find the oxidation number of P in Mg2P2O7.



Find the oxidation number of Cr in K2Cr2O7.



Find the oxidation number of Mn in MnO4.



Find the oxidation number of N in NO3.



Find the oxidation number of S in S2Cl2.



Find the oxidation number of Fe in Na2[Fe(CN)5NO].



Which compound among the following has the lowest oxidation number of Mn?
KMnO4,K2MnO4,MnO2 and Mn2O3.



Which compound among the following has the highest oxidation number of P?
PH3,H3PO2,PCl3 and H3PO4.



Which compound among the following has the lowest oxidation number of chlorine?
HClO4,HOCl,ClF3,HClO3 and HCl.



Find the oxidation number of Cr in (NH4)2Cr2O7.



Find the oxidation number of Ni in Ni(CO)4.



Find the oxidation number of Cl in Ca(ClO2)2.



Give the oxidation state of underlined.
CaOCl2_.



Give the oxidation state of underlined.
Fe3_O4.



Give the oxidation state of underlined.
N_H4N_O3.



Give the oxidation state of underlined.
N_H4N_O2.



Give the oxidation state of underlined.
Na2S4_O6.



Give the oxidation state of underlined.
H2S_O5.



Give the oxidation state of underlined.
(CH3)2S_O.



Give the oxidation state of underlined.
KO2_.



Give the oxidation state of underlined.
Cr_O5.



Give the oxidation state of underlined.
Co_SeO4.



What is the value of n in the molecular formula BenAl2Si6O18?



Write balanced chemical equation for the following.
Action of ozone on hydrogen peroxide.



What is redox reaction? Explain with one example.



What is an oxidizing agent in Cl2+2I12Cl+I2?



Name a reducing agent that can be used to obtain manganese from manganese dioxide. Write the balanced chemical equation for the reaction.



State the characteristic of chemical reaction which takes place when:
1) Lead reacts with KI
2) Zinc reacts with HCI
3) Reaction of candle wax



In basic medium +2Na2+4S26O3+2Na2+6S3O4.
Write the balanced chemical equation.



Calculate the oxidation number of oxygen in the following : OF2,O2,Na2O2 and CH3COOH



Calculate the oxidation number of C in the following: C2H6,C4H10,CO,CO2 and HCO3



Give one example each of displacement, decomposition and combination reaction with explaination.



Consider the reactions :
2S2O23(aq)+I2(s)S4O26(aq)+2I(aq)
S2O23(aq)+2Br2(l)+5H2O(l)2SO24(aq)+4Br(aq)+10H+(aq)
Why does the same reductant, thiosulphate react differently with iodine and bromine ?



Oxidation number of iron in Na2[Fe(CN)5NO+] is?



After balancing the equation,
K2Cr2O7+xH2SO4+ySO2K2SO4+Cr2(SO4)3+zH2O
The values X,Y and Z obtained will be respectively



Give one example each of the componds of chlorine which show +1, +3, +4 and +6 oxidation states.



O||CH|HCOH|H
Write oxidation No. of each C atom.



LiAlH4
Find oxidation no.of Al.



Explain the term reduction reaction with an example involving the reaction of hydrogen sulphide with chlorine .



Find oxidation number of Fe in K3[Fe(CN)6].



What is the reaction called when oxidation and reduction take place simultaneously? Explain with one example.



Balance the following equations and write sown the stoichiometric proportions.
a) CaCO3+HClCaCl2+H2O+CO2
b) MnO2+HClMnCl2+H2O+Cl2
c) Mg(OH)2+HClMgCl2+H2O
d) KI+H2SO4KHSO4+I2+SO2



Oxidation no. of Fe in K3[Fe(CN)6]



What is the oxidation number of Cl in HClO and HClO2?



Calculate the oxidation number of the metal in following
(i) K4[Fe(CN)6]
(ii) KAg(CN)2



Find the oxidation number of carbon in HCOOH.



Find oxidation number of S in PbSO4.



Find oxidation number of Sulphur in H2S2O7.



Find oxidation number of oxygen in CaO2.



Find oxidation number of Sulphur in KAl(SO4)2.12H2O.



Find oxidation number of Magnese in K2MnO4.



Find the oxidation number of carbon in HCHO.



Find oxidation number:-
Br3O8 [Br]



Find oxidation number of Sulphur in H2SO5.



Find the oxidation number of carbon in CH3OH.



Consider the reactions:
2S2O23(aq)+I2(s)S4O26(aq)+2I(aq)
S2O23(aq)+2Br2(l)+5H2O(l)2SO24(aq)+4Br(aq)+10H+(aq)
Why does the same reductant thiosulphate react differently with iodine and bromine?



Cr2O27+H2O+3SO22Cr+3+2OH+3SO24
write down to oxidation and reduction reaction



It requires 40mL of 0.5MCe4+ to titrate 10mL of 1M Sn4+. What is the oxidation state of the cerium in the product?



Balance the following redox reaction.
(Cr2O7)2(aq)+Fe2+(aq)Cr3+(aq)+Fe3+(aq)    (acidic medium)



Write the oxidation number of K and B in the given species:
K2MnO4 and NaBH4



Calculate the oxidation number of Xe in XeF4 and XeO2.



Calculate oxidation number of central atom in [K4[Fe(CN)6].



Write balanced net ionic equation for the following reaction in acidic solution.
HSO_4(aq)+As_4(s)+Pb_3O_4(s)\rightarrow PbSO_4(s)+H_2AsO_4^-(aq)



Calculate oxidation number of central atom in [Fe(CO)_5].



Write balanced net ionic equation for the following reaction in acidic solution.
HNO_2(aq) \rightarrow NO_3^-+NO(g)



What is the oxidation number of Cu in [Cu(NH_{3})_{4}]^{2+}?



What is the oxidation number of V in { K }_{ 4 }Na[{ HV }_{ 10 }{ O }_{ 28 }]?



(CH_3)_2 \underline {  S} O \Longrightarrow oxd^n number of S _____



The oxidation state (integer) of chlorine in perchlorie acid (HClO_{4}) is:



Find the Oxidation number of Fe in {K}_{2}Fe{O}_{4}.



Define Redox reactions. Identify oxidising and reducing agents in following reactions:
{I}_{2(aq)}+2{S}_{2}{O}_{3}^{2-}(aq)\rightarrow {S}_{4}{O}_{6}^{2-}(aq)+2{I}^{-}(aq)



Write the oxidation reaction of diphenyl amine indicator :



What is the atomic number of the following elements 
Potassium iodide, Iodine is 



Arrange the following in increasing order of oxidation states of Mn,
K_2MnO_4, MnO_2, KMnO_4



Find the oxidation numbers to the underlined species in the following compounds or ions.
V_2O_7^{4-}
H_5P_3O_{10}



Which of the following is the strongest oxidising agent : CrO_{4}^{2-}MoO_{4}^{2-}, WO_{4}^{2-}.



Find the oxidation numbers to the underlined species in the following compounds or ions.
VO_4^{3-}
Ni_2O_3



Find the oxidation numbers to the underlined species in the following compounds or ions.
Mn(OH)_3
I_3^-



Find the oxidation numbers to the underlined species in the following compounds or ions.
CuSO_4
BiO_3^-



Find the oxidation numbers to the underlined species in the following compounds or ions.
K_3[Fe(CN)_6]



Find the oxidation numbers to the underlined species in the following compounds or ions.
Na_2CO_3
IO_4^-



Find the oxidation numbers to the underlined species in the following compounds or ions.
PF_6^-
NaIO_3



Hydrogen is a good reducing agent.
What do you understand by the above statement? Explain with the help of copper oxide as an example . 



Balance the equation in basic medium Al+NO_3^-\rightarrow Al(OH)^-_4+NH_3



Write the following equation redox reation in the oxidation and reduction half reaction 
2K_{(s)}+Cl_{2(g)}----- \to 2KCL_{(s)}.



Answer the following question : Complete the equation Cr2O7^{2-}+14\,H^++6e : \rightarrow



Oxidation states of nitrogen in the explosive formed by reaction of ammonia iodine is      



Complete the reaction : 
I^- + IO_3^- \rightarrow I_2^ +



The reaction Cl_{2}(g) + 2OH^{-} (aq) \rightarrow ClO^{-}(aq) + Cl^{-1} (aq) + H_{2}O(l)
represents the process of bleaching. Identify and name the species that bleaches the
substances due to its oxidising  action.



Calculate the oxidation number of 
N in (NH_{4})_{2}SO_{4}



explain the reaction
1346785_8454ff0d1ef04ea6926ec4b9f0f6ce52.png



Three oxides of nitrogen, NO, NO_{2} and N_{2}O, can be formed under different conditions.
Complete the table to give the oxidation numbers of nitrogen in NO and NO_{2}.
CompoundNONO_{2}
Oxidation number of N



Calculate the oxidation number of Mn in KMnO_{4}   and Cr in K_{2}Cr_{2}O_{7}



Assign ON to atoms of only those elements which undergo ON change in the following redox reaction and then balance the Kl+H_{2}SO_{4} \to KHSO_{4}+SO_{2}+l_{2}+H_{2}O .



Assign ON to atoms of only those elements which undergo ON change in the following redox reactions and then balance the reaction:

C_{2}H_{5}OH +MnO_{4}^{-}+ OH^{-} \to C_{2}H_{3}O^{-} + MnO_{2}+H_{2}O



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the equation:

H_{2}S+Cr_{2}O_{7}^{2-}+ H^{+}\to Cr^{3+}+S_{8}+H_{2}O  



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the equation:

KNO_{3}+FeSO_{4}+H_{2}SO_{4} \to K_2SO_{4}+Fe_{2}(SO_{4})_{3}+ NO+H_{2}O



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the equation: 

H_{2}S+K_{2}Cr_{2}O_{7}+H_{2}SO_{4}\to KHSO_{4}+ Cr_{2}(SO_{4})_{3}+S+H_{2}O



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the equation:

ZnS+O_{2}\to ZnO+SO_{2}



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the reaction: 

Fe_{3}O_{4}+ MnO_{4}^{-} + H_{2}O \to Fe_{2}O_{3}+MnO_{2}+OH^{-}



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the   Cr_{2}O_{7}^{2-}+SO_{3}^{2-}+ H^{+} \to Cr^{3+}+ SO_{4}^{2-}+H_{2}O .



Assign ON to atoms of only those elements which undergo ON change in the following redox reactions and then balance the   I_{2}+SO_{2}+H_{2}O \to SO_{4}^{2-}+ I^{-}+ H^{+}.



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the MnO_{4}^{-} + SO_{2} + H_{2}O \to Mn^{2+}+SO_{4}^{2-} +H^{+}.



Assign ON to atoms of only those elements which undergo ON change in the following redox reactions and then balance the MnO_{4}^{-}+SO_{3}^{2-}+H_{2}O \to MnO_{2} +SO_{4}^{2-}+OH^{-}.



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the K_{2}Cr_{2}O_{7} +H_{2}O + S \to SO_{2}+KOH+ Cr_{2}O_{3}.



Assign ON to atoms of only those elements which undergo ON change in the following redox reactions and then balance the  MnO_{4}^{-}+SO_{3}^{2-} +OH^{-}  \to MnO_{4}^{2-}+H_{2}O .



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the MnO_{4}^{-} + SO_{2} + H_{2}O \to Mn^{2+}+SO_{4}^{2-} +H^{+}.



Assign ON to atoms of only those elements which undergo ON change in the following redox reaction and then balance the reaction:

Al +KMnO_{4}+H_{2}SO_{4} \to KHSO_{4}+Al_{2}(SO_{4})_{3}+MnSO_{4}+H_{2}O



Assign ON to atoms of only those elements which undergo ON change in the following redox reactions and then balance the Sn +NO_{3}^{-}+H^{+} \to SnO_{2}+NO_{2}+ H_{2}O .



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the ClO^{-} +Br^{-} \to BrO_{3}^{-}+Cl^{-}



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the equation:

KMnO_{4}+H_{2}O_{2}+H_{2}SO_{4}\to MnSO_{4}+K_{2}SO_{4}+O_{2}+H_{2}O



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the equation:

Cl_{2}+IO_{3}^{-}+OH^{-}\to Cl^{-}+IO_{4}^{-}+H_{2}O



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the equation:

KMnO_{4}+HCl\to Cl_{2}+KCl+MnCl_{2}+H_{2}O



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the Zn+NO_{3}^{-}+OH^{-} = NH_{3}+ZnO_{2}^{2-}+H_{2}O



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the equation:

Zn+ NO_3^{-}+H^{+}\to Zn^{2+}+NH_{4}^{+}+H_{2}O



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the ClO+SbO_{2}^{-}+OH^{-}\to ClO_{2}^{-}+Sb (OH)_{6}^{-}+H_{2}O



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the equation:

H_{2}O_{2}+PbS\to PbSO_{4}+H_{2}O



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the H_{2}SO_{3}+Cr_{2}O_{7}^{2-}+H^{+}=HSO_{4}^{-}+Cr^{3+}+H_{2}O



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the equation:

BaCrO_{4}+KI+HCl\to BaCl_{2}+I_{2}+KCl+CrCl_{3}+H_{2}O



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the reaction:

Cl_{2}+SeO_{3}^{2-}+ H_{2}O \to SeO_{4}^{2-}+Cl^{-}+H^{+}



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the  CuO +NH_{3} \to Cu+N_{2}+H_{2}O .



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the equation:

Cu_{3}P+H^{+}+Cr_{2}O_{7}^{2-}\to Cu^{2+}+H_{3}PO_{4}+Cr^{3+}+H_{2}O



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the equation:

H_{2}O+SbCl_{3}\to SbOCl+2HCl



Assign ON to atoms of only those elements which undergo ON change in the following redox reactions and then balance the K_{4}Fe(CN)_{6}+Ce(NO_{3})_{4}+KOH \to Ce(OH)_{3}+Fe(OH)_{3}+H_{2}O+K_{2}CO_{3}+KNO_{3} 



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the equation:

HNO_{3}+I_{2}\to HIO_{3}+NO_{2}+H_{2}O



Assign ON to atoms of only those elements which undergo ON change in the following redox reactions and then balance the  As_{2}S_{5}+HNO_{3}=H_{3}AsO_{4}+H_{2}SO_{4}+NO_{2}+H_{2}O .



Assign ON to atoms of only those elements which undergo ON change in the following redox reactions and then balance the  PbS+O_{3} \to PbSO_{4}+O_{2}.



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the equation:

AsO_{3}^{3-}+I_{2}+H_{2}O \to AsO_{4}^{3-}+ H^{+}+I^{-}



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the equation:

K_{2}Cr_{2}O_{7}+H_{2}SO_{4}+KI\to I_{2}+K_{2}SO_{4}+Cr_{2}(SO_{4})_{3}+H_{2}O



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the equation:

(NH_{4})_{2}Cr_{2}O_{7}\to N_{2}+H_{2}O +Cr_{2}O_{3}



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the reaction:

CuSO_{4}+KI\to Cu_{2}I_{2}+I_{2}+K_{2}SO_{4}



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the reaction:

NaOH+Cl_{2}\to NaCl+NaClO+H_{2}O



Point out the oxidation number of C in the following:

{ CH }_{ 4 },\ { C }_{ 3 }{ H }_{ 8 },\ { C }_{ 2 }{ H }_{ 6 },\ { C }_{ 4 }{ H }_{ 10 },\ CO,\ { CO }_{ 2 },\ H{ CO }_{ 3 }^{ - } and { CO }_{ 3 }^{ 2- }



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the reaction: 

As_{2}S_{5}+HNO_{3}\to H_{2}SO_{4}+NO_{2}+H_{3}AsO_{4}+H_{2}O



Assign ON to atoms of only those elements which undergo ON change in the following redox reactions and then balance the equation: 

Zn+HNO_{3} \to Zn(NO_{3})_{2}+N_{2}O+ H_{2}O



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the equation:

MnO_{4}^{2-}+H^{+}\to  MnO_{4}^{-} + MnO_{2} +H_{2}O     



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the equation:

H_{3}PO_{3}\to H_{3}PO_{4} + PH_{3}  



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the reaction: 

Br_{2}+OH^{-}\to BrO^{-}+Br^{-}+H_{2}O



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the reaction: 

Cr_{2}O_{7}^{2-}+SO_{2}+H^{+}\to Cr^{3+}+HSO_{4}^{-}+H_{2}O



Fill in the blanks:

(a) Hydrogen is ______ than air.
(b) Hydrogen is ______soluble in water.
(c) Hydrogen burns with a ___________ flame and _____ sound is heard.
(d) A metal _______ hydrogen in the reactivity series gives hydrogen with ______.
(e) Hydrogen reacts with metal oxides to form ______ and ______.
(f) Oxidation is the removal of ________ and addition of _______. 
(g) In redox reaction oxidation and reduction occur ___________.



Write a balanced chemical equation for each of the following reactions and also classify them.
(c) Iron (III) oxide on heating with carbon monoxide gas reacts to form solid iron and liberates carbon dioxide gas.



Name the following:
(a) Two metals which give hydrogen with cold water.
(b) A metal which liberates hydrogen only when steam is passed over red hot metal.
(c) The process in which oxygen is added or hydrogen is removed.
(d) A metallic oxide which can be reduced into metal by hydrogen.



Give reasons:
Carbon cannot reduce the oxides of Na or Mg.



Write a balanced chemical equation for the following reaction and also classify them.
Hydrogen sulphide gas reacts with oxygen gas to form solid Sulphur and liquid water.



What do you mean by redox reaction? Explain with the help of an example.



Balance the following chemical equation and identify the type of chemical reaction.

H g O(s) \stackrel{H e a t}{\longrightarrow} H g(l)+O_{2}(g)



Give two examples each of:
Redox reactions



Define:
(a) catalytic hydrogenation
(b) oxidation
(c) reduction
(d) redox reaction



Calculate the oxidation number of the element underline in each of the following cases

Al in Al_2O_3



Calculate the oxidation number of the element underline in each of the following cases

Na_2PdCl_4



Balance Fe^{2+} + Cr_2O^{2-}_7 \rightarrow Fe^{3+} Cr^{3+} is acid media.



Calculate the oxidation number of the element underline in each of the following cases

S in Na_2S_2O_3



Calculate the oxidation number of the element underline in each of the following cases

HA_4Cl_4



Calculate the oxidation number of the element underline in each of the following cases

Mn in KMnO_4



Calculate the oxidation number of the element underline in each of the following cases

P in P_2O_5



What do you understand by redox reactions?



What do you understand redox reactions? Explain oxidation and reduction in terms of loss or gain of electrons.



What does (II) in lead (II) nitrate indicate?



Calculate the oxidation number of the element underline in each of the following cases

H\underline{S}O^-_3



Find the oxidation number of the underlined atoms.
H\underline{P}O^-_2



Calculate the oxidation number of the element underline in each of the following cases

 \underline {Cl}O^-



Find the oxidation number of the underlined atoms.
Na_2\underline{B}_4O_7



Find the oxidation number of the underlined atoms.
 \underline {C}H_4



Find the oxidation number of the underlined atoms.
\underline{C}Cl_4



Find the oxidation number of the underlined atoms.
\underline {C}IO^-_3



What is oxidation number of sulphur in the following molecules / ions $$ (n) (i) H_2S (ii) SO^{2-}_4 (iii) H_2SO_4 $$



Calculate the oxidation number of the element underline in each of the following cases

\underline{Cr_2}O_7^{-2}



Calculate the oxidation number of the element underline in each of the following cases

\underline{Si}0_3^{- 2}



What is the oxidation number of Li in LiAlH_{4}?



In the given structure, the electronegativity of Y is more then Z. Find the oxidation number of Z.
1829978_9019aa57a5c449579ce3da744ac5583c.png



Calculate the oxidation number of Ni in [Ni(CN)_{4}]^{2-}.



Calculate the oxidation number of Mo in (NH_{4})_{2} Mo O_{4}.



What is the oxidation number of oxygen in KO_{2}?



Find the oxidation number of the underlined atoms.
Fe_3O_4



Calculate the oxidation state of Na in Na_2O_2 .



Observe the following chemical equation
Cu +2H_2SO_4\to CuSO_4 +SO_2 +2H_2O
Which one has oxidation state as 0?



Find the oxidation number of Mn in KMnO_4 (oxidation number of K is +1, oxidation number of O is -2)



Observe the following chemical equation
Cu +2H_2SO_4\to CuSO_4 +SO_2 +2H_2O
What is its oxidation state of Cu after the chemical reaction?



\displaystyle \overset{0}{H_2} + \overset{0}{Cl_2} \longrightarrow \overset{+1}{2H} \overset{-1}{Cl}  
In the formation of hydrogen chloride does the oxidation number of hydrogen increase or decrease ?
Whether the oxidation number of chlorine decrease or increase ?
Based on oxidation number which is the oxidizing agent and reducing agent ?



How do you determine the oxidation number of sulfur in H_2SO_4 ?



Find the oxidation number of Mn in MnO_2 , Mn_2O_3 and Mn_2O_7



Analyze the following equation, fill-up the blanks.
\overset{0}{Zn} + 2 \overset{+1}{H} \overset{-1}{Cl} \rightarrow \overset{+2}{Zn} \overset{-1}{Cl_2} + \overset{0}{H_2}  
The oxidation number of hydrogen increases/decreases from ............. to ........



Consider the equation H_2 + Cl_2 \rightarrow 2 HCl What is the oxidation number of hydrogen in H_2
What is the oxidation number of chlorine in Cl_2 ?
In this reaction , does the oxidation number of hydrogen increase or decrease ?
What change takes place in the oxidation number of chlorine ? 



Analyze the following equation and fill-up the blanks.
\overset{0}{Zn} + 2 \overset{+1}{H} \overset{-1}{Cl} \rightarrow \overset{+2}{Zn} \overset{-1}{Cl_2} + \overset{0}{H_2}  
The oxidation number of zinc increases/decreases from ............to ........ 



Find the oxidation number of the ions in ionic compound ?



In the following chemical reactions which is the oxidizing agent which is the reducing agent ? Analyze the oxidation number and find out ?
\overset{0}{C} + 2 \overset{0}{Cl_2} \longrightarrow \overset{+4}{C} \overset{-1}{Cl_4}



Given below is the equation of the reaction between zinc and hydrochloric acid also indicating the oxidation number.
\overset{0}{Zn} + 2 \overset{+1}{H} \overset{-1}{Cl} \rightarrow \overset{+2}{Zn} \overset{-1}{Cl_2} + \overset{0}{H}  
Analyze and find the following:



The oxidation number of \mathrm{N} in \mathrm{NI}_{3} is \dots



Sone chemical equations are given below.
C + O_2 \rightarrow CO_2
CH_4 + 2O_2 \rightarrow CO_2 + 2H_2O  
N_2 + O_2 \rightarrow NO  
CaCO_2 \rightarrow CaO + CO_2  
H_2 + I_2 \rightarrow HI  
Fe + HCl \rightarrow FeCl_2 + H_2  
CO_2 + C \rightarrow CO  

Which among these are redox reactions ?



Match list-I (compounds) with list-II (oxidation states of nitrogen).



{ { H }_{ 2 }O }_{ 2 }(aq) reduces Cl{ O }_{ 4 }^{ - }(aq) in acidic medium. If 1 mole of { { H }_{ 2 }O }_{ 2 } reduces 0.5 mole of Cl{ O }_{ 4 }^{ - }(aq). What is the oxidation number of reduced species?
(Answer is the modulus of the oxidation number)



Nitrogen forms five different compounds with oxygen. Match appropriate formulae for these compounds if the oxidation state of N in them is +1,+2,+3,+4 and +5.



Match the compounds in Column I with the matter in Column II.



The number of redox reactions from the following equations are:
a.  { H }_{ 2 }S + { Fe }^{ 3+ } \longrightarrow { Fe }^{ 2+ } + S\downarrow + { H }^{ \oplus  }
b.  { I }^{ \ominus  } + I{ O }_{ 3 }^{ \ominus  } + { H }^{ \oplus  } \longrightarrow { I }_{ 2 } + { H }_{ 2 }O
c.  Bi\left( s \right) + N{ O }_{ 3 }^{ \ominus  } + { H }^{ \oplus  } \longrightarrow N{ O }_{ 2 } + { Bi }^{ 3+ } + { H }_{ 2 }O
d.  { I }^{ \ominus  } + { O }_{ 2 }\left( g \right) + { H }_{ 2 }O \longrightarrow { I }_{ 2 } + \overset { \ominus  }{ O } H
e.  Cu\left( s \right) + { Au }^{ \oplus  } \longrightarrow Au\left( s \right) + { Cu }^{ 2+ }



6 mol of Cl_2 undergo a loss and gain of 10 mol of electrons to form two oxidation states of Cl. Write down the oxidation number of Cl having positive charge.



Match the following with their minimum and maximum oxidation number if any as well as with their respective variable oxidation number if any.



Match the reactions in column I with the molar ratio of their respective oxidants and reductant in column II.



Among the following elements, what is the total number of elements having the lowest oxidation state of zero?
a.  Ta
b.  Te
c.  Tc
d.  Ti
e.  Tl



Match the reactions given in column I with average oxidation numbers given in column II.



Reactlon                                                             Oxidation state



What is the magnitude of summation of oxidation states of all oxygen in CrO_5?



Assign oxidation number to the underlined element in NaH_2\underline{P}O_4.



Arrange the following in the order of increasing oxidation number of nitrogen: NH_3, N_3H, N_2O, NO, N_2O_5.



Can the reaction Cr_{2} O_{7}^{2-} + H_{2}O \rightarrow 2CrO_{4}^{2-} + 2H^{+} be regarded as a redox reaction?



Complete and rewrite the balanced chemical equation.
Butanone+2, 4 dinitro-phenyl hydrazine \overset{H^+}{\rightarrow}?



In the following redox reaction { Cr }_{ 2 }{ O }_{ 7 }^{ 2- }\ +\ { Fe }^{ 2+ }\quad \longrightarrow { Fe }^{ 3+ }\ +{ Cr }^{ 3+ } 1 mol of Cr_2O_7^{2-} oxidizes x mol of { Fe }^{ +2 }. Find x.



Dvide the following redox equations into oxidation half equation and reduction half equation.
a)P_{ (s) }+P{ O }_{ 4(aq) }^{ 3 }HP{ O }_{ 3(aq) }^{ 2 }\\ b)HNO_{ 2(aq) }\longrightarrow N{ O }_{ 3(aq) }^{ - }+NO_{ (g) }\\ c)I{ O }_{ 3(aq) }^{ - }+{ Re }_{ (s) }\longrightarrow { Re }{ O }_{ 4(aq) }^{ }+{ I }_{ (aq) }



AI{ F }_{ 3 } is insoluble in a hydrous HF but when little KF is added to the compound it becomes soluble. On addition of { BF }_{ 3 }, AI{ F }_{ 3 } is precipitated. Write the balanced chemical equations.



Why can MnO_2 be reduced by 'Al' and not by carbon?



Give a clear idea about how { MnO }_{ 4 }^{ - }{ ,CrO }_{ 4 }^{ 2- },{ Cr }_{ 2 }{ O }_{ 7 }^{ 2- } changes its oxidation state when it is in the acidic, basic and neutral medium.



What is oxidation state of manganese in manganate form?



When KMnO_4 acts as an oxidising agent and ultimately forms [MnO_4]^{-1}, MnO_2, Mn_2O_3, and Mn_2O^+, then the number of electrons transferred in each case respectfully is 



Zinc oxide is white but it turns yellow on heating . Explain.



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the equation:

S+OH^{-}\to S^{2-}+S_{2}O_{3}^{2-}+H_{2}O



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the equation:

MnO_{4}^{-}+C_{2}O_{4}^{2-}+H^{+}\to Mn^{2+}+CO_{2}+H_{2}O



Assign ON to atoms of only those elements which undergo ON change in the following redox reactions and then balance the reaction:

FeSO_{4}\to Fe_{2}O_{3}+SO_{2}+SO_{3}.



Find the oxidation number of carbon in the following compounds:

{ CH }_{ 3 }OH,\quad { CH }_{ 2 }O,\quad HCOOH,\quad { C }_{ 2 }{ H }_{ 2 }.



Assign ON to atoms of only those elements which undergo ON change in the following redox  reactions and then balance the equation:

Na_{2}SnO_{2}+Bi(OH)_{3}\to Bi+Na_{2}SnO_{3}+H_{2}O



Determine the ox. no of underlined atom in each of the following:
(a) K\underline { Cr } { O }_{ 3 }Cl
(b) { K }_{ 2 }\underline { Fe } { O }_{ 4 }
(c) Ba{ \left( { H }_{ 2 }{ \underline { P } O }_{ 2 } \right)  }_{ 2 }
(d) { Rb }_{ 4 }Na\left[ H{ \underline { V }  }_{ 10 }{ O }_{ 28 } \right]
(e) { Ba }_{ 2 }\underline { Xe } { O }_{ 6 }
(f) { Na }_{ 2 }{ \underline { S }  }_{ 2 }
(g) { K }_{ 2 }\underline { Mn } { O }_{ 4 }
(h) { K }_{ 2 }{ \underline { Cr }  }_{ 2 }{ O }_{ 7 }
(i) \underline { Mn } { O }_{ 4 }^{ - }
(j) \underline { S } { O }_{ 4 }^{ 2- }
(k) \underline { P } { O }_{ 4 }^{ 3- }
(l) \underline { C } { O }_{ 3 }^{ 2- }
(m) [\underline { Cu } { \left( { NH }_{ 3 } \right)  }_{ 4 }]^{ 2+ }
(n) \underline { Ni } { \left( CO \right)  }_{ 4 }
(o) \underline { C } { S }_{ 2 }
(p) { \left( { NH }_{ 4 } \right)  }_{ 6 }{ \underline { Mo }  }_{ 7 }{ O }_{ 24 }
(q) { \left[ \underline { Co } { F }_{ 4 } \right]  }^{ - }
(r) \underline { Os } { O }_{ 4 }
(s) { Na }_{ 4 }\underline { Xe } { O }_{ 6 }
(t) K\underline { Cr } { O }_{ 3 }Cl
(u) { \underline { F }  }_{ 2 }{ H }_{ 2 }



Arrange the following in order of:
(a) Increasing oxidation no. of Mn:Mn{ Cl }_{ 2 },Mn{ O }_{ 2 },Mn{ \left( OH \right)  }_{ 3 },KMn{ O }_{ 4 }
(b) Decreasing oxidtaion no. X:HX{ O }_{ 4 },HX{ O }_{ 3 },HX{ O }_{ 2 },HXO
(c) Increasing oxidation no. I:{ I }_{ 2 },HI,HI{ O }_{ 4 },ICl,I{ F }_{ 3 },I{ F }_{ 5 }
(d) Increasing oxidation no. of N:{ N }_{ 2 },{ NH }_{ 3 },{ N }_{ 3 }H,{ NH }_{ 2 }{ NH }_{ 2 },{ NH }_{ 2 }OH,K{ NO }_{ 2 },K{ NO }_{ 3 },{ N }_{ 2 }O



What is the name of the reaction ?
2 CH_3 CH_2 CH_2SH \rightarrow CH_3CH_2CH_2 -S -S- CH_2CH_2CH_3
whether condensation , oxidation reduction or polymerization ? 



Select the nature or type of redox change in the following reactions:

(a) 2{ Cu }^{ 2+ }\longrightarrow { Cu }^{ 2+ }+{ Cu }^{ 0 }\quad

(b) { Cl }_{ 2 }\longrightarrow Cl{ O }^{ - }+{ Cl }^{ - }\quad

(c) 2KCl{ O }_{ 3 }\xrightarrow [  ]{ \Delta  } 2KCl+3{ O }_{ 2 }

(d) { \left( { NH }_{ 4 } \right)  }_{ 2 }{ Cr }_{ 2 }{ O }_{ 7 }\longrightarrow { N }_{ 2 }+{ Cr }_{ 2 }{ O }_{ 3 }+4{ H }_{ 2 }O

(e) 10Fe{ SO }_{ 4 }+2KMn{ O }_{ 4 }+8{ H }_{ 2 }{ SO }_{ 4 }\longrightarrow 2Mn{ SO }_{ 4 }+5{ Fe }_{ 2 }{ \left( { SO }_{ 4 } \right)  }_{ 3 }+{ K }_{ 2 }{ SO }_{ 4 }+{ 8H }_{ 2 }O

(f) 5{ H }_{ 2 }{ C}_{ 2 }{ O }_{ 4 }+2KMn{ O }_{ 4 }+3{ H }_{ 2 }{ SO }_{ 4 }\longrightarrow { K }_{ 2 }{ SO }_{ 4 }+2Mn{ SO }_{ 4 }+10{ CO }_{ 2 }+8{ H }_{ 2 }O\quad



Some chemical reactions are given below 
Zn+2HCl \rightarrow ZnCl_2+H_2
2Mg+O_2 \rightarrow 2MgO
NH_4Cl \leftrightharpoons NH_3+HCl
What type of reactions are they all represent?



Class 11 Medical Chemistry Extra Questions