Electron-Dot Model of Bonding Lewis Structures

Show the bond polarization in H2O, SCO, SO, IBr, CH4, CHCI3, CH2CI2, and CH3CI by using dipole arrows to indicate separation of charge. (In the last four exarr5)les, place the carbon in the center of the molecule.) 

Ammonia, NH3, is not trigonal but pyramidal, with bond angles of 107.3°. Water, H26, is not linear but bent (104.5°). Why (Hint Consider the effect of the nonbonding electron pairs.) 

In Summary There are two extreme types of bonding, ionic and covalent. Both derive favorable energetics from Coulomb forces and the attainment of noble-gas electronic structures. Most bonds are better described as something between the two types the polar covalent (or covalent ionic) bonds. Polarity in bonds may give rise to polar molecules. The outcome depends on the shape of the molecule, which is determined in a simple manner by arrangement of its bonds and nonbonding electrons to minimize electron repulsion. 

Lewis structures are important for predicting geometry and polarity (hence reactivity) of organic compounds, and we shall use them for that purpose throughout this book. In this section, we provide rules for writing such structures correctly and for keeping track of valence electrons. 

Lewis structures are drawn by following simple rules 

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Electron-Dot Model of Bonding Lewis Structures CHAPTER 1... 

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