Why is there a difference in the bond angles of H 2S and H 2O? The molecular geometry of H 2S is bent since the central sulfur atom has 2 lone pairs (4 electrons) and 2 bond pairs with hydrogen atoms (2 electrons) around it, for its 6 valence electrons. The ∠HSH bond angle is 92° instead of 120°, with the lone pairs causing more repulsion than the bond pairs. The electron geometry of H 2S is tetrahedral as the central sulfur atom possesses 4 pairs of electrons two of which are lone pairs (4 electrons) and two are bond pairs with hydrogen atoms (2 electrons), for sulfur’s 6 valence electrons. The ∠OSO bond angle is 119° instead of 120°, as the lone pair causes more repulsion (than a bond pair). With a total of 3 electron pairs around sulfur, the electronic geometry of sulfur dioxide, SO 2 is trigonal planar. The remaining two valence electrons act as a lone pair. The central sulfur atom has 6 valence electrons and forms two double bonds with the two oxygen atoms, using 4 of its valence electrons. The oxygen atoms arrange as far apart as possible with a bond angle of 180° between them. The electron geometry of carbon dioxide, CO 2, is linear because the central carbon atom, having 4 valence electrons, forms a double bond with each of the oxygen atoms. A tetrahedral electron geometry results, with an ∠HNH bond angle of 107° rather than 109.5° due to more repulsion from the lone pair as compared to a bond pair. So there are a total of 4 electron pairs around the central nitrogen atom. The electron geometry of ammonia (NH3) is tetrahedral because the central nitrogen atom, having 5 valence electrons, bonds 3 of its electrons with 3 hydrogen atoms, and the remaining 2 electrons act as a single lone pair. This results in a tetrahedral electron geometry vs a bent molecular geometry. The central oxygen atom has 6 valence electrons, 2 of which form two bond pairs with the hydrogen atoms, and the other 4 electrons form two lone pairs. Show H 2O Electron geometry vs molecular geometry. Valence Shell Electron Pair Repulsion (VSEPR) Theoryĭifference between molecular geometry and electron geometryĮlectron geometry can be determined by finding out the number of electron pairs, both bonding and non-bonding pairs around the central atom(s).Lewis Structure (Representation of Valence Electrons in a molecule).Its molecular geometry is trigonal pyramidal while its electron geometry is tetrahedral. With the central atom nitrogen having 5 valence electrons, it possesses 3 bond pairs and a lone pair of electrons. Its molecular, as well as electronic geometry, is tetrahedral.Īn example with differing molecular and electron geometries is that of ammonia, NH 3. An example is a methane molecule, CH 4 with 4 bond pairs and no lone pairs, all 4 of carbon’s valence electrons are bonded with hydrogen atoms. If all of the electron groups are bond pairs (no lone pairs), the molecular geometry and electron geometry are the same. This causes a slight decrease in bond angles (angles between bonds or bond pairs). Under the influence of a single nucleus, a lone pair offers more repulsion than a bond pair which is influenced by two nuclei. This repulsion causes the electron pairs around the central atom to arrange as far apart from each other as possible. It is well known that the electron pairs, being negatively charged, repel each other.
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