Search results
Results from the WOW.Com Content Network
Bent's rule addresses disparities between the observed and idealized geometries. [3] According to Bent's rule, a central atom bonded to multiple groups will rehybridize so that orbitals with more s character are directed towards electropositive groups, and orbitals with more p character will be directed towards groups that are more electronegative.
A central atom is defined in this theory as an atom which is bonded to two or more other atoms, while a terminal atom is bonded to only one other atom. [1]: 398 For example in the molecule methyl isocyanate (H 3 C-N=C=O), the two carbons and one nitrogen are central atoms, and the three hydrogens and one oxygen are terminal atoms.
2 O) is a simple triatomic bent molecule with C 2v molecular symmetry and bond angle of 104.5° between the central oxygen atom and the hydrogen atoms. Despite being one of the simplest triatomic molecules, its chemical bonding scheme is nonetheless complex as many of its bonding properties such as bond angle, ionization energy, and electronic ...
AX 2 E 1 molecules, such as SnCl 2, have only one lone pair and the central angle about 120° (the centre and two vertices of an equilateral triangle). They have three sp 2 orbitals. There exist also sd-hybridised AX 2 compounds of transition metals without lone pairs: they have the central angle about 90° and are also classified as bent.
For example, in carbon dioxide (CO 2), which does not have a lone pair, the oxygen atoms are on opposite sides of the carbon atom (linear molecular geometry), whereas in water (H 2 O) which has two lone pairs, the angle between the hydrogen atoms is 104.5° (bent molecular geometry).
This is because according to Bent's rule, the C–F bond gains p-orbital character leading to high s-character in the C–H bonds, and H–C–H bond angles approaching those of sp 2 orbitals – e.g. 120° – leaving less for the F–C–H bond angle. The difference is again explained in terms of bent bonds. [3]
For premium support please call: 800-290-4726 more ways to reach us
Many rules in chemistry rely on electron-counting: Octet rule is used with Lewis structures for main group elements, especially the lighter ones such as carbon, nitrogen, and oxygen, 18-electron rule [2] in inorganic chemistry and organometallic chemistry of transition metals, Hückel's rule for the π-electrons of aromatic compounds,