Electrons have fixed energies. Electrons move around the nucleus in shells (or energy levels) - the further away a shell is from the nucleus the higher its energy.
There are sub-shells that have slightly differing energies.
Each sub-shell consists of a different number of orbitals (the bit of space where an electron moves).
Each orbital can hold up to 2 electrons, if there are 2 then they spin in opposite directions (spin-pairing).
Electrons fill shells singularly before pairing up.
Cu and Cr will donate one of their 4s electrons to the 3d sub-shell as they are happier to have a full or half full 3d block as they are more stable.
Electronic structure can be used to determine the properties of an element. Eg s block elements losing their electrons in their outer shell to become a positive ion.
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