Chemical Bonding and Molecular Structure Test - 3

The bond length depends on the strength of the bond. The stronger the bond is, the shorter it will be. The triple bonds are the strongest and hence the shortest. Then comes double bonds which are of intermediate strength between the triple and single bonds. And finally the single bonds are weaker than the other two. This way, Triple bonds are the shortest. Then comes double bonds. Finally, single bonds are the longest among the three.

The order of bond lengths is given as, Triple bond < Double bond < Single bond

Na lose its one electron forming Na⁺ while Cl gains the electron formimg Cl^-

A dipole moment is a measurement of the separation of two opposite electrical charges. Dipole moments are a vector quantity. The magnitude is equal to the charge multiplied by the distance between the charges and the direction is from negative charge to positive charge:

µ=q x r

CO₂ is linear, so even though the C−O bonds have individual dipole moments, the overall dipole moment is zero as these cancel out (they point in opposite directions, as shown in the diagram below).
On the other hand, H₂O is "bent", which means that the individual dipole moments of the bond are at an angle to each other and because of Presence of lp on head of O atom in H₂O therefore it has max dipole moment.

overlapping of atomic orbitals having electrons of opposite spin take place in the formation of molecule to cancel the dipole moment.