NaF is an ionic compound. This is because Na gives up an electron to F. The elements in a covalent bond share electrons — one of the elements doesn’t give up its electron(s).

The ionic bond between ions results from the electrostatic attraction of opposite charges. The final formula of sodium fluoride is NaF. An ionic compound is formed by the complete transfer of electrons from a metal to a nonmetal and the resulting ions have achieved an octet.

Chemical structure Sodium fluoride is an inorganic ionic compound, dissolving in water to give separated Na+ and F− ions.

Molecular Meanings As you can see, the three polar N-F bonds are all pointing in the same direction. Because the side of the molecule containing the fluorine atoms has three partial negative charges and the side of the molecule containing the nitrogen atom has a partial positive charge, the whole molecule is polar.

Covalent bond

Bond order and bond length indicate the type and strength of covalent bonds between atoms. Bond order and length are inversely proportional to each other: when bond order is increased, bond length is decreased.

So , carbon – carbon triple bonds are strongest . More is the overlapping , more stronger a bond is. Hence, carbon – carbon triple bond is strongest then double bond then single bond.

Thus an H–F bond is stronger than an H–I bond, H–C is stronger than H–Si, H–N is stronger than H–P, H–O is stronger than H–S, and so forth….The Relationship between Bond Order and Bond Energy.

Of course C-C. N, Cl, F and O all have higher eletronegativities than C, so C-N, C-Cl, C-F and C-O are polar. But C-C is non-polar. C-C bond is the least polar because both carbon have the same electronegativity and both carbon attract the shared electron pair equally..

The COCl2 molecule has 3 areas of electron repulsion around the central C atom, so the shape is trigonal planar. Both C–Cl bonds are polar, due to the difference in electronegativity of C and Cl. The C=O bond is also polar, due to the difference in electronegativity of C and O.