Bent molecular geometry

{{Short description|Molecular geometry}} {{Infobox molecular geometry | Image_File=Bent-3D-balls.png| Symmetry_group= C_2v | Atom_direction=2 | Bond_angle=90° to 120° | mu=>0 | Examples= H₂O, SO₂ }} [[Image:Oxygen-difluoride-3D-vdW.png|thumb|left|200px|Oxygen difluoride, an example of a molecule with the bent coordination geometry.]] In chemistry, molecules with a non-collinear arrangement of two adjacent bonds have '''bent molecular geometry''', also known as '''angular''' or '''V-shaped'''. Certain atoms, such as oxygen, will almost always set their two (or more) covalent bonds in non-collinear directions due to their electron configuration. Water (H₂O) is an example of a bent molecule, as well as its analogues. The bond angle between the two hydrogen atoms is approximately 104.45°.<ref>{{cite book|first1=G. L.|last1=Miessler|first2=D. A.|last2=Tarr|title=Inorganic Chemistry|year=2004|edition=3rd|publisher=Pearson/Prentice Hall|isbn=0-13-035471-6|url-access=registration|url=https://archive.org/details/inorganicchemist03edmies}}</ref> Nonlinear geometry is commonly observed for other triatomic molecules and ions containing only main group elements, prominent examples being nitrogen dioxide (NO₂), sulfur dichloride (SCl₂), and methylene (CH₂).

This geometry is almost always consistent with VSEPR theory, which usually explains non-collinearity of atoms with a presence of lone pairs. There are several variants of bending, where the most common is AX₂E₂ where two covalent bonds and two lone pairs of the central atom (A) form a complete 8-electron shell. They have central angles from 104° to 109.5°, where the latter is consistent with a simplistic theory which predicts the tetrahedral symmetry of four sp³ hybridised orbitals. The most common actual angles are 105°, 107°, and 109°: they vary because of the different properties of the peripheral atoms (X).

Other cases also experience orbital hybridisation, but in different degrees. AX₂E₁ molecules, such as SnCl₂, have only one lone pair and the central angle about 120° (the centre and two vertices of an equilateral triangle). They have three sp² orbitals. There exist also sd-hybridised AX₂ compounds of transition metals without lone pairs: they have the central angle about 90° and are also classified as bent.{{Citation needed|date=August 2022}} {{Crossreference|(See further discussion at {{section link|VSEPR theory#Complexes with strong d-contribution}}.)}}

==See also== *AXE method

==References== {{reflist}}

== External links == *[http://www.3dchem.com/ 3D Chem: Chemistry, Structures, and 3D Molecules] *[http://arquivo.pt/wayback/20160523113736/http://www.iumsc.indiana.edu/ Indiana University Molecular Structure Center] * [https://web.archive.org/web/20181129012854/https://www.staff.ncl.ac.uk/j.p.goss/symmetry/Molecules_l3d.html Interactive molecular examples for point groups] *[https://web.archive.org/web/20080120023822/http://chemlab.truman.edu/CHEM121Labs/MolecularModeling1.htm Molecular Modeling] *[http://intro.chem.okstate.edu/1314F97/Chapter9/3BP.html Animated Trigonal Planar Visual]

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Category:Stereochemistry Category:Molecular geometry