315199
Oxidation number of cobalt in \(\mathrm{\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right] \mathrm{Cl}_{2} \mathrm{Br}}\) is
1 +6
2 Zero
3 \( + 3\)
4 \({\rm{ + 2}}\)
Explanation:
Let the O.N. of Co be \(\mathrm{x}\) O.N. of \(\mathrm{\mathrm{NH}_{3}}\) is zero O.N. of \(\mathrm{\mathrm{Cl}}\) is \({\rm{ - 1}}\) O.N. of \(\mathrm{\mathrm{Br}}\) is \({\rm{ - 1}}\) Hence, \(\mathrm{x+6(0)-1 \times 2-1=0}\) \(\mathrm{\therefore \quad x=+3}\) so, the oxidation number of cobalt in the given complex compound is +3 .
CHXI08:REDOX REACTIONS
315200
The compound formed in the brown ring test has the formula \(\mathrm{\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{NO}^{+}\right] \mathrm{SO}_{4}}\). The oxidation state of iron in it is
1 +1
2 +2
3 +3
4 Zero
Explanation:
Let, O. N. of \({\rm{Fe = x}}\) \({\rm{x + 5}}\left( {\rm{0}} \right){\rm{ + }}\left( {{\rm{ + 1}}} \right){\rm{ - }}\left( {{\rm{ - 2}}} \right){\rm{ = 0}}\) \({\rm{x = + 1}}\)
CHXI08:REDOX REACTIONS
315201
Assertion : In some cases oxygen shows positive oxidation number though it is an electronegative elements. Reason : Fluorine is more electronegative than oxygen.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
Despite being highly electronegative and typically exhibiting negative oxidation states, oxygen can display positive oxidation states, such as \({\text{ + 2}}\) in oxygen difluoride \(\left(\mathrm{OF}_{2}\right)\), when bonded to more electronegative elements like fluorine. So the option (1) is correct.
CHXI08:REDOX REACTIONS
315202
Which of the following has least oxidation state of \(\mathrm{\mathrm{Fe}}\) ?
315199
Oxidation number of cobalt in \(\mathrm{\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right] \mathrm{Cl}_{2} \mathrm{Br}}\) is
1 +6
2 Zero
3 \( + 3\)
4 \({\rm{ + 2}}\)
Explanation:
Let the O.N. of Co be \(\mathrm{x}\) O.N. of \(\mathrm{\mathrm{NH}_{3}}\) is zero O.N. of \(\mathrm{\mathrm{Cl}}\) is \({\rm{ - 1}}\) O.N. of \(\mathrm{\mathrm{Br}}\) is \({\rm{ - 1}}\) Hence, \(\mathrm{x+6(0)-1 \times 2-1=0}\) \(\mathrm{\therefore \quad x=+3}\) so, the oxidation number of cobalt in the given complex compound is +3 .
CHXI08:REDOX REACTIONS
315200
The compound formed in the brown ring test has the formula \(\mathrm{\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{NO}^{+}\right] \mathrm{SO}_{4}}\). The oxidation state of iron in it is
1 +1
2 +2
3 +3
4 Zero
Explanation:
Let, O. N. of \({\rm{Fe = x}}\) \({\rm{x + 5}}\left( {\rm{0}} \right){\rm{ + }}\left( {{\rm{ + 1}}} \right){\rm{ - }}\left( {{\rm{ - 2}}} \right){\rm{ = 0}}\) \({\rm{x = + 1}}\)
CHXI08:REDOX REACTIONS
315201
Assertion : In some cases oxygen shows positive oxidation number though it is an electronegative elements. Reason : Fluorine is more electronegative than oxygen.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
Despite being highly electronegative and typically exhibiting negative oxidation states, oxygen can display positive oxidation states, such as \({\text{ + 2}}\) in oxygen difluoride \(\left(\mathrm{OF}_{2}\right)\), when bonded to more electronegative elements like fluorine. So the option (1) is correct.
CHXI08:REDOX REACTIONS
315202
Which of the following has least oxidation state of \(\mathrm{\mathrm{Fe}}\) ?
315199
Oxidation number of cobalt in \(\mathrm{\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right] \mathrm{Cl}_{2} \mathrm{Br}}\) is
1 +6
2 Zero
3 \( + 3\)
4 \({\rm{ + 2}}\)
Explanation:
Let the O.N. of Co be \(\mathrm{x}\) O.N. of \(\mathrm{\mathrm{NH}_{3}}\) is zero O.N. of \(\mathrm{\mathrm{Cl}}\) is \({\rm{ - 1}}\) O.N. of \(\mathrm{\mathrm{Br}}\) is \({\rm{ - 1}}\) Hence, \(\mathrm{x+6(0)-1 \times 2-1=0}\) \(\mathrm{\therefore \quad x=+3}\) so, the oxidation number of cobalt in the given complex compound is +3 .
CHXI08:REDOX REACTIONS
315200
The compound formed in the brown ring test has the formula \(\mathrm{\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{NO}^{+}\right] \mathrm{SO}_{4}}\). The oxidation state of iron in it is
1 +1
2 +2
3 +3
4 Zero
Explanation:
Let, O. N. of \({\rm{Fe = x}}\) \({\rm{x + 5}}\left( {\rm{0}} \right){\rm{ + }}\left( {{\rm{ + 1}}} \right){\rm{ - }}\left( {{\rm{ - 2}}} \right){\rm{ = 0}}\) \({\rm{x = + 1}}\)
CHXI08:REDOX REACTIONS
315201
Assertion : In some cases oxygen shows positive oxidation number though it is an electronegative elements. Reason : Fluorine is more electronegative than oxygen.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
Despite being highly electronegative and typically exhibiting negative oxidation states, oxygen can display positive oxidation states, such as \({\text{ + 2}}\) in oxygen difluoride \(\left(\mathrm{OF}_{2}\right)\), when bonded to more electronegative elements like fluorine. So the option (1) is correct.
CHXI08:REDOX REACTIONS
315202
Which of the following has least oxidation state of \(\mathrm{\mathrm{Fe}}\) ?
NEET Test Series from KOTA - 10 Papers In MS WORD
WhatsApp Here
CHXI08:REDOX REACTIONS
315199
Oxidation number of cobalt in \(\mathrm{\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right] \mathrm{Cl}_{2} \mathrm{Br}}\) is
1 +6
2 Zero
3 \( + 3\)
4 \({\rm{ + 2}}\)
Explanation:
Let the O.N. of Co be \(\mathrm{x}\) O.N. of \(\mathrm{\mathrm{NH}_{3}}\) is zero O.N. of \(\mathrm{\mathrm{Cl}}\) is \({\rm{ - 1}}\) O.N. of \(\mathrm{\mathrm{Br}}\) is \({\rm{ - 1}}\) Hence, \(\mathrm{x+6(0)-1 \times 2-1=0}\) \(\mathrm{\therefore \quad x=+3}\) so, the oxidation number of cobalt in the given complex compound is +3 .
CHXI08:REDOX REACTIONS
315200
The compound formed in the brown ring test has the formula \(\mathrm{\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{NO}^{+}\right] \mathrm{SO}_{4}}\). The oxidation state of iron in it is
1 +1
2 +2
3 +3
4 Zero
Explanation:
Let, O. N. of \({\rm{Fe = x}}\) \({\rm{x + 5}}\left( {\rm{0}} \right){\rm{ + }}\left( {{\rm{ + 1}}} \right){\rm{ - }}\left( {{\rm{ - 2}}} \right){\rm{ = 0}}\) \({\rm{x = + 1}}\)
CHXI08:REDOX REACTIONS
315201
Assertion : In some cases oxygen shows positive oxidation number though it is an electronegative elements. Reason : Fluorine is more electronegative than oxygen.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
Despite being highly electronegative and typically exhibiting negative oxidation states, oxygen can display positive oxidation states, such as \({\text{ + 2}}\) in oxygen difluoride \(\left(\mathrm{OF}_{2}\right)\), when bonded to more electronegative elements like fluorine. So the option (1) is correct.
CHXI08:REDOX REACTIONS
315202
Which of the following has least oxidation state of \(\mathrm{\mathrm{Fe}}\) ?
