Chapter 6 true or false

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A molecule with polar bonds must itself be polar

Covalent compounds are network solids

If two of more atoms are covalently bonded together, a molecule of a compound results

To attain a noble gas structure, a nitrogen atom must lose its five valence electrons

A hydrogen bond must involve a hydrogen atom that is covalently bonded to a very electronegative atom

In general the electronegativity values of nonmetallic elements are greater than the electronegavity values of metallic elements

Unshared pairs of electrons affect the shape of molecules

The modern interpretation of resonance is that electron pairs rapidly flip back and forth between the various electron dot structures

In a polar covalent bond the more electronegative atom has a slight positive charge

The compound OF2 contains two double covalent bonds

The tendency of carbon to form four bonds to other atoms can be explained by the four p electrons in its outer shell

1.2 Levels of Structural Organization