Polar covalent molecules

Of course, HF is actually a polar covalent molecule, but from the extent of the polarity, it behaves as if it were composed of the two structures shown above. A similar analysis can be carried out for all of the hydrogen halides, and the results are shown in Table 3.2. 

H20(.s) is a polar covalent molecule. Between the individual molecules would be hydrogen bonds. 

In a polar covalent molecule such as H-Cl, all of the electrons in the bond between the atoms are assigned to the more electronegative atom, thus CP has an oxidation number of —1, leaving the hydrogen atom with an oxidation number of +1. 

Polar covalent bonds are the source of dipoles. Dipole-dipole attractions, including those resulting from hydrogen bonds, hold together liquids composed of polar covalent molecules. But what about molecules with pure covalent bonds Such molecules have no permanent dipoles. So, what intermolecular force holds them together ... 

Carbocations are able to react effectively not only with anions but also with polarized covalent molecules by attacking the negative end of the dipole. Likewise, carbanions are capable of attacking the positive end of a polarized... 

How are the partial charges shown in a polar covalent molecule ... 

Considering the shapes of MO energy level diagrams for nonpolar covalent and polar covalent molecules, what would you predict about MO diagrams, and therefore about overlap of atomic orbitals, for ionic compounds ... 

Permanent dipole-dipole interactions occur between polar covalent molecules because of the attraction of the 5+ atoms of one molecule to the 5— atoms of another molecule (Section 7-9). 

Strong hydrogen bonding occurs among polar covalent molecules containing H and one of the three small, highly electronegative elements—F, O, or N. 

HF is a polar covalent molecule characterized by polar covalent bonding. This implies that the electrons are shared unequally. 

A molecule is polar if its centers of positive and negative charges do not coincide. A polar covalent molecule has at least one polar covalent bond. An imderstanding of the concept of electronegativity, the relative electron-attracting power of atoms in molecules, helps us to assess the polarity of a bond. 

ACs can be calculated from quantum mechanics by partitioning the wave function or on the basis of calculated electron densities. The AC on an atom in a polar covalent molecule Is always Intermediate between its oxidation number (which... 

In the previous chapters, we discussed various models of bonding for covalent and polar covalent molecules (the VSEPR and LCP models, valence bond theory, and molecular orbital theory). We shall now turn our focus to a discussion of models describing metallic bonding. We begin with the free electron model, which assumes that the ionized electrons in a metallic solid have been completely removed from the influence of the atoms in the crystal and exist essentially as an electron gas. Freshman chemistry books typically describe this simplified version of metallic bonding as a sea of electrons that is delocalized over all the metal atoms in the crystalline solid. We shall then progress to the band theory of solids, which results from introducing the periodic potential of the crystalline lattice. 

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