![]() ![]() $ Which of the 2$p$ orbitals can actually make a bond with a 1$s$ orbital, assuming that the atoms lie on the z-axis? (d) In the most accepted picture of HF, all the other atomic orbitals on fluorine move over at the same energy into the molecular orbital energy-level diagram for HF. Draw pictures showing the proper orientation of all three 2$p$ orbitals on Finteracting with a 15 orbital on $\mathrm. The 5 electron group consists of the trigonal bypyramidal, see-saw, T. The 1 s orbital of hydrogen will mix only with one 2$p$ orbital of fluorine. A common example of a bent molecule is the water molecule (left). The four electron groups are the 2 single bonds to Hydrogen and the 2 lone pairs of Oxygen. (a) Using only the valence atomic orbitals of a hydrogen atom and a fluorine atom, and following the model of Figure 9.46, how many MOs would you expect for the HF molecule? (b) How many of the MOs from part (a) would be occupied by electrons? (c) It turns out that the difference inĮnergies between the valence atomic orbitals of H and F are sufficiently different that we can neglect the interaction of the 1 s orbital of hydrogen with the 2$s$ orbital of fluorine. Water has four electron groups so it falls under tetrahedral for the electron-group geometry. (Mulliken was mentioned earlier because he proposed a definition of electronegativity, and Hund because of Hunds Rule. It was developed about the same time Valence Bond Theory was developed, primarily by Mulliken and Hund. The ammonia molecule has polar NH bonds, utilizes sp3 hybrid orbitals for bonding, and has HNH bond angles greater than 109.5 degrees. Molecular Orbital (MO) Theory is another theory to explain chemical bonding using orbitals. The hybridization of the carbon atom in the CH4 ion is sp3. The CO2 molecule has 2 double bonds and 2 single bonds. The polar molecule among the options given is CO. The molecular geometry and polarity of the O=C=S molecule is linear and nonpolar. Bonding the water molecule can be explained by the valence bond theory in terms of an overlap between the 1s orbital of the hydrogen and the 2s orbital of the oxygen. ![]()
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