Limits of Partial Charges in Dipoles

AI Thread Summary
In the discussion, the focus is on the nature of partial charges in dipoles, particularly in the context of double and triple bonds. It is emphasized that partial charges are always less than the unit electronic charge (1.6×10−19 C), which raises the question of whether electronegative atoms can pull shared electron clouds to create charges exceeding this limit. The consensus is that this is not possible because anions, despite their electronegativity, cannot exert enough influence to surpass the unit charge. The concept of zwitterions is mentioned, likely to illustrate the behavior of charged species, but the primary argument centers on the limitations of charge distribution in covalent bonding scenarios.
tbn032
Messages
34
Reaction score
7
In my book it is written "Ends of dipole possesses partial charges. Partial charges are always less than the unit electronic charge (1.6×10−19 C)".
Suppose in a double bond(two electron is shared by each atom) or triple bond(three electrons are shared by each atom), can the electronegative atom pull the shared electron cloud to the extent that the charges at the end of the dipole exceed 1.6×10−19 C.why is that not possible? Is it because the anions are not electronegative to that extent, hence they cannot pull the electron cloud to the extent that the charges at the end of the dipole exceed 1.6×10−19 C?
 
Chemistry news on Phys.org
I want to test a humidity sensor with one or more saturated salt solutions. The table salt that I have on hand contains one of two anticaking agents, calcium silicate or sodium aluminosilicate. Will the presence of either of these additives (or iodine for that matter) significantly affect the equilibrium humidity? I searched and all the how-to-do-it guides did not address this question. One research paper I found reported that at 1.5% w/w calcium silicate increased the deliquescent point by...
I was introduced to the Octet Rule recently and make me wonder, why does 8 valence electrons or a full p orbital always make an element inert? What is so special with a full p orbital? Like take Calcium for an example, its outer orbital is filled but its only the s orbital thats filled so its still reactive not so much as the Alkaline metals but still pretty reactive. Can someone explain it to me? Thanks!!
I'm trying to find a cheap DIY method to etch holes of various shapes through 0.3mm Aluminium sheet using 5-10% Sodium Hydroxide. The idea is to apply a resist to the Aluminium then selectively ablate it off using a diode laser cutter and then dissolve away the Aluminium using Sodium Hydroxide. By cheap I mean resists costing say £20 in small quantities. The Internet has suggested various resists to try including... Enamel paint (only survived seconds in the NaOH!) Acrylic paint (only...
Back
Top