Covelant bonds:why dont the electrons(+) repel eachother?

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    Electrons Repel
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Electrons are negatively charged, which explains why they do not repel each other despite their proximity. Instead of pairing, electrons occupy available spaces in atomic orbitals, influenced by the attractive force of the positively charged nucleus. This attraction keeps electrons stable within their orbitals, preventing repulsion. Understanding electron behavior in this context clarifies misconceptions about their interactions in covalent bonds. Overall, the dynamics of electron distribution and nuclear attraction are key to their arrangement in molecules.
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what is the explanation for electron pairing in molecules since the electrons are all positively charged? Shouldn't they repel each other?
Any help would be appreciated:) sorry for the newb question :)
 
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First, electrons are negatively charged.

Second, the electrons don't really pair with each other, they fill open wells in the orbital space of an atom, and are held in place by attraction to the dense positive charge in the nucleus of the atom.
 
Thread 'Motional EMF in Faraday disc, co-rotating magnet axial mean flux'

Thread 'Motional EMF in Faraday disc, co-rotating magnet axial mean flux'

So here is the motional EMF formula. Now I understand the standard Faraday paradox that an axis symmetric field source (like a speaker motor ring magnet) has a magnetic field that is frame invariant under rotation around axis of symmetry. The field is static whether you rotate the magnet or not. So far so good. What puzzles me is this , there is a term average magnetic flux or "azimuthal mean" , this term describes the average magnetic field through the area swept by the rotating Faraday...
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