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[1] [2] [3] Introduced by Gilbert N. Lewis in his 1916 article The Atom and the Molecule, a Lewis structure can be drawn for any covalently bonded molecule, as well as coordination compounds. [4] Lewis structures extend the concept of the electron dot diagram by adding lines between atoms to represent shared pairs in a chemical bond.
Ball-and-stick model of a sulfamic acid zwitterion as it occurs in the crystal state. [4]The compound is well described by the formula H 3 NSO 3, not the tautomer H 2 NSO 2 (OH). The relevant bond distances are 1.44 Å for the S=O and 1.77 Å for the S–N.
Indeed, the estimated N−N and N−O bond orders are 2.76 and 1.9, respectively, [7] approaching the formula of integer bond orders that would include the ionic contribution explicitly as a bond (in green): Conversely, formal charges against electronegativities in a Lewis structure decrease the bond order of the corresponding bond.
The connection of atoms in the hydrogen disulfide molecule is H−S−S−H. The structure of hydrogen disulfide is similar to that of hydrogen peroxide, with C 2 point group symmetry. Both molecules are distinctly nonplanar. The dihedral angle between the H a −S−S and S−S−H b planes is 90.6°, compared with 111.5° in H 2 O 2.
Another example is O(SiH 3) 2 with an Si–O–Si angle of 144.1°, which compares to the angles in Cl 2 O (110.9°), (CH 3) 2 O (111.7°), and N(CH 3) 3 (110.9°). [24] Gillespie and Robinson rationalize the Si–O–Si bond angle based on the observed ability of a ligand's lone pair to most greatly repel other electron pairs when the ligand ...
[9] [10] G. N. Lewis was born in 1875 in Weymouth, Massachusetts . After receiving his PhD in chemistry from Harvard University and studying abroad in Germany and the Philippines , Lewis moved to California in 1912 to teach chemistry at the University of California, Berkeley, where he became the dean of the college of chemistry and spent the ...
(a) The LDQ structure of the B 2 H 7 − molecule. The nuclei are as indicated and the electrons are denoted by either dots or crosses, depending on their relative spins. The thick lines denote coincident electron pairs. (b) The traditional valence bond theory structure for the B 2 H 7 − molecule. The horizontal bar stretching across the ...
Below pH = 9.6 the hydrated electron reacts with the hydronium ion giving atomic hydrogen, which in turn can react with the hydrated electron giving hydroxide ion and usual molecular hydrogen H 2. [11] Solvated electrons can be found even in the gas phase.