Which Lewis Structure for BeCl2 is more commonly seen? Ask Question Asked 11 years, 1 month ago Modified 11 years, 1 month ago
AlCl3 + RCl β AlCl4 (-) indicating that AlCl3 is a Lewis Acid but SiCl4 + RCl β SiCl5 (-) ?????? So, this tells me that AlCl3 > SiCl4 in terms of electron accepting behavior. Now, don't get me wrong: pentacoordinated Si is well known. One of the failures of the Lewis Acid concept is that, as far as I know, there is no unambiguous way to measure it. It is much more qualitative than ...
Now for BeCl2 Usually, we only show the bond and lone pair of the central atom but if you want, just for your information, each chlorine atom in the reaction has got 3 lone pairs (the red dots.)
In the vapour phase, beryllium chloride exists in its dimeric state, wherein one beryllium atom is bound to two chlorine atoms via covalent bonds and to one chlorine atom via a coordinate bond with
What can be the order of acidity of aqueous solutions of following Lewis acids: FeClX3, AlClX3, BeClX2, NiClX2 F e C l X 3, A l C l X 3, B e C l X 2, N i C l X 2
It is to be noted that, in case of group- 13 elements, the strength of Lewis acidity order is: BClX3>AlClX3>GaClX3 B C l X 3> A l C l X 3> G a C l X 3 This is due to difference in electronegativity and size of central atoms.
Consider the bent shape of $\\ce{H2O}$ with a bond angle of $104Β°$. From my understanding, this is due to the lone pair repulsion between the 2 pairs of lone pair electrons. Hence, it adopts a tetra...
Lewis acidity is a function of electron deficiency on the acceptor atom, which in this case is B B and Al A l respectively. Back donation is better as is the case of B B, due to better 2p overlap compared to 3p overlap, then the electron deficiency on the B B atom should be lesser, as it's deficiency is getting filled better; but then how is BClX3 B C l X 3 β stronger acid than AlClX3 A l C ...
Beryllium chloride's geometric structure is linear, with a bond angle of 180 degrees. Drawing the Lewis dot structure for this covalent compound, one can see that the compound is electron deficient...
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