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Which one of the following constitutes a group of the isoelectronic species? [AIEEE-2008]
- a)C22-, O-2, CO, NO
- b)NO+, C22-, CN-, N2
- c)CN-, N2, O22-, C2
- d)N2, O,-2NO+ ,CO
Correct answer is option 'B'. Can you explain this answer?
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Which one of the following constitutes a group of the isoelectronic sp...
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Which one of the following constitutes a group of the isoelectronic sp...
Explanation:
Let's analyze each option to determine which one constitutes a group of isoelectronic species.
Option A: C2^2-, O^-2, CO, NO
- C2^2-: Carbon ion with a charge of 2-. It has 6 electrons.
- O^-2: Oxygen ion with a charge of 2-. It has 10 electrons.
- CO: Carbon monoxide molecule. It has 10 electrons.
- NO: Nitric oxide molecule. It has 11 electrons.
These species have different numbers of electrons, so they are not isoelectronic.
Option B: NO, C2^2-, CN^-, N2
- NO: Nitric oxide molecule. It has 11 electrons.
- C2^2-: Carbon ion with a charge of 2-. It has 6 electrons.
- CN^-: Cyanide ion with a charge of 1-. It has 10 electrons.
- N2: Nitrogen molecule. It has 14 electrons.
All these species have the same number of electrons (11), so they are isoelectronic.
Option C: CN^-, N2, O2^2-, C2
- CN^-: Cyanide ion with a charge of 1-. It has 10 electrons.
- N2: Nitrogen molecule. It has 14 electrons.
- O2^2-: Oxygen ion with a charge of 2-. It has 12 electrons.
- C2: Carbon molecule. It has 12 electrons.
These species have different numbers of electrons, so they are not isoelectronic.
Option D: N2, O^-2, NO, CO
- N2: Nitrogen molecule. It has 14 electrons.
- O^-2: Oxygen ion with a charge of 2-. It has 10 electrons.
- NO: Nitric oxide molecule. It has 11 electrons.
- CO: Carbon monoxide molecule. It has 10 electrons.
These species have different numbers of electrons, so they are not isoelectronic.
Therefore, the correct answer is Option B: NO, C2^2-, CN^-, N2, as all these species have the same number of electrons (11) and are isoelectronic.
Let's analyze each option to determine which one constitutes a group of isoelectronic species.
Option A: C2^2-, O^-2, CO, NO
- C2^2-: Carbon ion with a charge of 2-. It has 6 electrons.
- O^-2: Oxygen ion with a charge of 2-. It has 10 electrons.
- CO: Carbon monoxide molecule. It has 10 electrons.
- NO: Nitric oxide molecule. It has 11 electrons.
These species have different numbers of electrons, so they are not isoelectronic.
Option B: NO, C2^2-, CN^-, N2
- NO: Nitric oxide molecule. It has 11 electrons.
- C2^2-: Carbon ion with a charge of 2-. It has 6 electrons.
- CN^-: Cyanide ion with a charge of 1-. It has 10 electrons.
- N2: Nitrogen molecule. It has 14 electrons.
All these species have the same number of electrons (11), so they are isoelectronic.
Option C: CN^-, N2, O2^2-, C2
- CN^-: Cyanide ion with a charge of 1-. It has 10 electrons.
- N2: Nitrogen molecule. It has 14 electrons.
- O2^2-: Oxygen ion with a charge of 2-. It has 12 electrons.
- C2: Carbon molecule. It has 12 electrons.
These species have different numbers of electrons, so they are not isoelectronic.
Option D: N2, O^-2, NO, CO
- N2: Nitrogen molecule. It has 14 electrons.
- O^-2: Oxygen ion with a charge of 2-. It has 10 electrons.
- NO: Nitric oxide molecule. It has 11 electrons.
- CO: Carbon monoxide molecule. It has 10 electrons.
These species have different numbers of electrons, so they are not isoelectronic.
Therefore, the correct answer is Option B: NO, C2^2-, CN^-, N2, as all these species have the same number of electrons (11) and are isoelectronic.
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Which one of the following constitutes a group of the isoelectronic sp...
They all should have same no. of electrons NO+ = 7+8-1= 14C2-2= 2×6+2=14CN-= 6+7+1= 14 N2= 7+7= 14
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Which one of the following constitutes a group of the isoelectronic species? [AIEEE-2008]a)C22-, O-2,CO, NOb)NO+, C22-, CN-, N2c)CN-, N2, O22-, C2d)N2, O,-2NO+,COCorrect answer is option 'B'. Can you explain this answer?
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