Assertion -Statement - 1 - The direction of dipole moment in CO is from - O- to - C- Reason- Statement - 2 - The contribution of co - ordinated - - bond is more compared to electronegativity factor in the overall polarity of the molecule-

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Assertion :St...

Question

Assertion :Statement $-$ 1 : The direction of dipole moment in $C O$ is from ' $O$ ' to ' $C$ '. Reason: Statement $-$ 2 : The contribution of co $-$ ordinated $π -$ bond is more compared to electronegativity factor in the overall polarity of the molecule.

Statement

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1 is true, Statement

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2 is true and Statement

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2 is correct explanation for Statement

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Statement

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1 is true, Statement

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2 is true and Statement

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2 is NOT the correct explanation for Statement

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Statement

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1 is true, Statement

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2 is false.

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Statement

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1 is false, Statement

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2 is true.

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Solution

The correct option is D Statement $-$ 1 is false, Statement $-$ 2 is true.
$: C = O ::$
There is a resonance structure that gives carbon a negative formal charge and oxygen a positive formal charge. It creates separation of charge and adds formal charges for a complete octet on carbon.
But at the same time, oxygen is more electronegative than carbon meaning electron density is going to be pulled in the direction of oxygen, away from carbon.
But as contribution of co $-$ ordinated $π -$ bond is more compared to electronegativity factor in the overall polarity of the molecule so direction of dipole moment in $C O$ is from ' $O$ ' to ' $C$ '.

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Assertion :Statement − 1 : The direction of dipole moment in CO is from 'O' to 'C'. Reason: Statement − 2 : The contribution of co − ordinated π− bond is more compared to electronegativity factor in the overall polarity of the molecule.

Assertion :Statement $-$ 1 : The direction of dipole moment in $C O$ is from ' $O$ ' to ' $C$ '. Reason: Statement $-$ 2 : The contribution of co $-$ ordinated $π -$ bond is more compared to electronegativity factor in the overall polarity of the molecule.