NEET Test Series from KOTA - 10 Papers In MS WORD
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CHXI08:REDOX REACTIONS
315450
Which of the acid possesses oxidizing, reducing and complex forming properties?
1 \(\mathrm{HNO}_{3}\)
2 \(\mathrm{H}_{2} \mathrm{SO}_{4}\)
3 HCl
4 \(\mathrm{HNO}_{2}\)
Explanation:
An element in its intermediate oxidation state acts as reducing, oxidizing and complex forming agent. Here, in \(\mathrm{HNO}_{2}\), ' N ' is in +3 state (Intermediate oxidation state).
CHXI08:REDOX REACTIONS
315451
Which of the following reaction is an example of redox reaction?
2 \(\mathrm{\mathrm{NaOH}(}\) aq \(\mathrm{)+\mathrm{HCl}(}\) aq \(\mathrm{) \rightarrow \mathrm{NaCl}(}\) aq \(\mathrm{)}\) \(\mathrm{+\mathrm{H}_{2} \mathrm{O}(1)}\)
The type of redox reactions in which same substance undergoes both oxidation and reduction are called disproportionation reactions.
CHXI08:REDOX REACTIONS
315452
Which of the following elements does not show disproportionation tendency?
1 \(\mathrm{\mathrm{Cl}}\)
2 \(\mathrm{\mathrm{Br}}\)
3 \(\mathrm{\mathrm{F}}\)
4 I
Explanation:
Being the most electronegative element, \(\mathrm{\mathrm{F}}\) can only be reduced and hence it always shows an oxidation number of\({\rm{ - 1}}\). Further, due to the absence of \(\mathrm{d}\) - orbitals, it cannot be oxidised and hence it does not show +ve oxidation numbers. In other words, F cannot be simultaneously oxidised as well as reduced and hence does not show disproportionation reactions.
315450
Which of the acid possesses oxidizing, reducing and complex forming properties?
1 \(\mathrm{HNO}_{3}\)
2 \(\mathrm{H}_{2} \mathrm{SO}_{4}\)
3 HCl
4 \(\mathrm{HNO}_{2}\)
Explanation:
An element in its intermediate oxidation state acts as reducing, oxidizing and complex forming agent. Here, in \(\mathrm{HNO}_{2}\), ' N ' is in +3 state (Intermediate oxidation state).
CHXI08:REDOX REACTIONS
315451
Which of the following reaction is an example of redox reaction?
2 \(\mathrm{\mathrm{NaOH}(}\) aq \(\mathrm{)+\mathrm{HCl}(}\) aq \(\mathrm{) \rightarrow \mathrm{NaCl}(}\) aq \(\mathrm{)}\) \(\mathrm{+\mathrm{H}_{2} \mathrm{O}(1)}\)
The type of redox reactions in which same substance undergoes both oxidation and reduction are called disproportionation reactions.
CHXI08:REDOX REACTIONS
315452
Which of the following elements does not show disproportionation tendency?
1 \(\mathrm{\mathrm{Cl}}\)
2 \(\mathrm{\mathrm{Br}}\)
3 \(\mathrm{\mathrm{F}}\)
4 I
Explanation:
Being the most electronegative element, \(\mathrm{\mathrm{F}}\) can only be reduced and hence it always shows an oxidation number of\({\rm{ - 1}}\). Further, due to the absence of \(\mathrm{d}\) - orbitals, it cannot be oxidised and hence it does not show +ve oxidation numbers. In other words, F cannot be simultaneously oxidised as well as reduced and hence does not show disproportionation reactions.
315450
Which of the acid possesses oxidizing, reducing and complex forming properties?
1 \(\mathrm{HNO}_{3}\)
2 \(\mathrm{H}_{2} \mathrm{SO}_{4}\)
3 HCl
4 \(\mathrm{HNO}_{2}\)
Explanation:
An element in its intermediate oxidation state acts as reducing, oxidizing and complex forming agent. Here, in \(\mathrm{HNO}_{2}\), ' N ' is in +3 state (Intermediate oxidation state).
CHXI08:REDOX REACTIONS
315451
Which of the following reaction is an example of redox reaction?
2 \(\mathrm{\mathrm{NaOH}(}\) aq \(\mathrm{)+\mathrm{HCl}(}\) aq \(\mathrm{) \rightarrow \mathrm{NaCl}(}\) aq \(\mathrm{)}\) \(\mathrm{+\mathrm{H}_{2} \mathrm{O}(1)}\)
The type of redox reactions in which same substance undergoes both oxidation and reduction are called disproportionation reactions.
CHXI08:REDOX REACTIONS
315452
Which of the following elements does not show disproportionation tendency?
1 \(\mathrm{\mathrm{Cl}}\)
2 \(\mathrm{\mathrm{Br}}\)
3 \(\mathrm{\mathrm{F}}\)
4 I
Explanation:
Being the most electronegative element, \(\mathrm{\mathrm{F}}\) can only be reduced and hence it always shows an oxidation number of\({\rm{ - 1}}\). Further, due to the absence of \(\mathrm{d}\) - orbitals, it cannot be oxidised and hence it does not show +ve oxidation numbers. In other words, F cannot be simultaneously oxidised as well as reduced and hence does not show disproportionation reactions.
315450
Which of the acid possesses oxidizing, reducing and complex forming properties?
1 \(\mathrm{HNO}_{3}\)
2 \(\mathrm{H}_{2} \mathrm{SO}_{4}\)
3 HCl
4 \(\mathrm{HNO}_{2}\)
Explanation:
An element in its intermediate oxidation state acts as reducing, oxidizing and complex forming agent. Here, in \(\mathrm{HNO}_{2}\), ' N ' is in +3 state (Intermediate oxidation state).
CHXI08:REDOX REACTIONS
315451
Which of the following reaction is an example of redox reaction?
2 \(\mathrm{\mathrm{NaOH}(}\) aq \(\mathrm{)+\mathrm{HCl}(}\) aq \(\mathrm{) \rightarrow \mathrm{NaCl}(}\) aq \(\mathrm{)}\) \(\mathrm{+\mathrm{H}_{2} \mathrm{O}(1)}\)
The type of redox reactions in which same substance undergoes both oxidation and reduction are called disproportionation reactions.
CHXI08:REDOX REACTIONS
315452
Which of the following elements does not show disproportionation tendency?
1 \(\mathrm{\mathrm{Cl}}\)
2 \(\mathrm{\mathrm{Br}}\)
3 \(\mathrm{\mathrm{F}}\)
4 I
Explanation:
Being the most electronegative element, \(\mathrm{\mathrm{F}}\) can only be reduced and hence it always shows an oxidation number of\({\rm{ - 1}}\). Further, due to the absence of \(\mathrm{d}\) - orbitals, it cannot be oxidised and hence it does not show +ve oxidation numbers. In other words, F cannot be simultaneously oxidised as well as reduced and hence does not show disproportionation reactions.
