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Additional resources for Building Stone Walls (Storey's Country Wisdom Bulletin A-217)
1-15. The 2p y orbitals, one on each carbon atom, will have maximum overlap if they are in the same plane. The 2p y orbitals can overlap in a side-toside manner as shown in Fig. 1-15. The resulting bond is called a pi () bond. The orbital overlap in a bond is not as great as the overlap in a sigma bond, and thus a bond is usually weaker than a sigma bond. Most drawings easily show the head-to-head p orbital overlap forming a sigma bond. In these drawings, it appears that the p orbitals are too far apart py py px px py p orbitals overlapping forming a pi (π) bond py p orbitals overlapping forming a sigma (σ) bond Fig.
Highly symmetrical molecules tend to be nonpolar. The electrons in the carbon-oxygen bond in CO2 (Structure 1-25b) are not shared equally. An oxygen atom is more electronegative than a carbon atom, and thus one would expect the electrons to spend more time closer to the CHAPTER 1 34 Structure and Bonding oxygen atom. The electrons are still shared (as compared to an ionic bond where electrons are transferred), but not equally. This is an example of a polar covalent bond. The polarity of a covalent bond is shown by an arrow pointing in the direction of greater electron density.
A single bond is one electron domain. A double or triple bond is considered one electron domain. An sp3 hybridized carbon atom has four electron domains and a tetrahedral electron-domain geometry. The structures of ammonia and water molecules are shown in Fig. 1-20. The nitrogen atom in ammonia has eight valence electrons, six from the three bonds to hydrogen atoms and one pair of nonbonding electrons. 5° Fig. 1-20. 3-D structures of ammonia and water. 25 CHAPTER 1 26 Structure and Bonding atoms and two pairs of nonbonding electrons.