CHEM 1101 Chapter Notes - Chapter 4: Coordinate Covalent Bond, Lone Pair, Valence Electron
13 Aug 2017
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Covalent bond = bond formed by sharing e- between atoms (instead of ionic which involve complete transfer of e-) Attractive forces (nucleus-electron) are stronger than repulsive forces (nucleus-nucleus & electron-electron), resulting in a net attractive force that allows atoms to stay together. Molecule = a group of atoms held together by covalent bonds. Main group elements undergo reactions that leave them with 8 valence e- (or 2 for hydrogen), so that they have a noble gas electron configuration. Nonmetals can achieve an electron octet by sharing an appropriate # of e- in covalent bonds. Spherical 1 s orbitals overlap to give an egg-shaped region. Two electrons between the nuclei, providing 1 s 2 configuration of helium. H-h, h:h and h 2 all represent a hydrogen molecule. The dash between the hydrogens represents two electrons (shared) Bond length = the optimum distance between nuclei in a covalent bond (where net attractive forces are maximized & molecule is most stable.
