In the electron dot structure of ammonia, the nitrogen atom shares one electron each from three hydrogen atoms, resulting in three shared pairs of electrons (single bonds). This allows nitrogen to achieve a stable octet configuration, while each hydrogen atom attains a duet configuration.
How do all four atoms in a molecule of ammonia (NH₃) achieve noble gas configuration?
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In a molecule of ammonia (NH₃), each hydrogen atom achieves a stable, noble gas configuration by sharing its single electron with the nitrogen atom. Nitrogen has five valence electrons and shares one electron with each of the three hydrogen atoms. This sharing forms three covalent bonds, and the resulting molecule has a tetrahedral shape. Through this arrangement, nitrogen attains a stable configuration with a total of eight electrons in its outer shell, simulating the noble gas configuration of neon. Meanwhile, each hydrogen atom achieves a duet (two electrons) in its outer shell, mimicking the noble gas configuration of helium.