1. Determine the INTRAmolecular force for the following compounds: (nonpolar covalent, polar covalent ionic) CH4 ,CF4,CO2, NH3,NaCl, HI. 2. How did you determine the intramolecular force for these compounds?

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Explanation:

What you need to know.

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A polar bond is when atoms have unequal attractions for electrons and so the sharing is unequal.

Electromagnetivity is the ability of an atom to attract electrons when atoms are in a compound.

To determine the electromagnetivity of an atom:

< 0.5 - Non-Polar

0.5 - 1.7 - Polar

Therefore, unequal sharing results in either a hydrogen or dipole bond.

Hydrogen bonding is just a special case of dipole-dipole interactions as hydrogen is partially positive in the molecule. When covalently bonded to a highly electronegative element, the hydrogen atom becomes so highly partial positive while the other so partial negative that a higher amount of interaction is obtain.However, keep in mind that hydrogen bonding can ONLY occur when hydrogen is covalently bonded to fluorine, oxygen and nitrogen.

A dipole-dipole interaction occurs between opposite partial charges in polar molecules. These attractions are generally weaker than hydrogen bonding.

London dispersion forces occurs in all bonds, as it's a temperorary attraction force when electrons in an atom occupy positions that form temporary dipoles. It's notable particularly in noble gases and it's the weakest of the intermolecular forces.

the answer is c.the valence of the atoms combine .