Question

Assertion: Statement-1: The direction of dipole moment in $CO$ is from $O$ to $C$.
Reason: Statement-2: The contribution of coordinate $\pi$-bond is more compared to electronegativity factor in the overall polarity of the molecule.
A. Statement-1 is true, Statement-2 is true and Statement-2 is the correct explanation for statement-1.
B. Statement-1 is true, Statement-2 is true and Statement-2 is not the correct explanation for Statement-1.
C. Statement-1 is true, Statement-2 is false.
D. Statement-1 is false, Statement-2 is true.

Answer 1

Hint: We need to remember that the dipole moments happen when there is a division of charge. They could take place between two particles present in an ionic bond or between atoms present in a covalent bond; dipole moments emerge from contrasts in electronegativity. The bigger the distinction in electronegativity, the bigger the dipole moment.

Complete step by step answer:
We must have to remember that at the point when particles in an atom share electrons inconsistent, they make what is known as a dipole moment. This happens when one iota is more electronegative than another, subsequent in that molecule pulling all the more firmly on the shared pair of electrons, or when one particle has a solitary pair of electrons and the distinction of electronegativity vector focuses similarly.
We must know that a nonpolar molecule that contains polar bonds is carbon dioxide (Figure 3a). This is a direct particle and each $C=O$ bond is, indeed, polar. The central carbon will have a net positive charge and the two external oxygen atoms a net negative charge. In any case, since the particle is straight, these two bond dipoles counterbalance one another (for example the vector expansion of the dipoles approaches zero) and the general atom has a zero dipole second $\left(\mu =0\right)$.
There is a reverberation structure that gives carbon a negative proper charge and oxygen a positive conventional charge. It makes partition of charge and adds formal charges for a total octet on carbon.
And yet, oxygen is more electronegative than carbon meaning electron thickness will be pulled toward oxygen, away from carbon.
However, as commitment of coordinated $\pi$− bond is more contrasted with electronegativity factor in the general extremity of the atom so heading of dipole second in $CO$ is from $O$ to $C$. Based on the explanation, Statement-1 is false and statement-2 is true.

So, the correct answer is Option D.

Note: We need to know that an atom has a dipole moment when there is a generally inconsistent appropriation of electrons across the whole molecule. Dipole moments are represented with a massive arrow pointing from the incompletely positive region of the molecule to the somewhat negative zone of the atom. $C{O}_2$ has the structure as $$O=C=O$$in which there is a bond dipole moment ($$C-O$$bond). Yet, as the dipole snapshot of one bond is dropped by another, the structure of $C{O}_2$ is straight. Thus, $C{O}_2$ has zero dipole moment since it is a straight molecule.