Compounds of copper(II) are generally colored, but compounds of copper(I) are not. Explain. The electron configuration for is ; the electron configuration for is . Color is a result of the electron transfer between orbitals. This cannot occur for the completely filled orbitals in

copper I ion has a completely filed d-orbital.

Explanation:

The electron configuration of copper is

29Cu-[Ar] 3d10 4s1

The formation of Cu+ involves the loss of one 4s electron leaving a completely filled d subshell. Colour in transition metal complexes is generally attributed mostly to d-d transition. When bonded to ligands, the d-orbitals are no longer degenerate. They split into sets of orbitals depending on the nature of the crystal field. d-d transition is not possible when the d-orbitals are full hence Cu+ compounds are not coloured.

nacl or sodium chloride is an ionic compound. this is because an ionic compound pertains to a compound that consists of positively and negatively charged ions. in this case, na (sodium) has a tendency to lose one electron when it reacts with with other atoms, so the resulting sodium ion contains 11 protons and 10 electrons, thus making it positively charged (na+), when chlorine reacts, it usually gains one electron to form an ion called chloride, thus making it negatively charged ( since the ions are oppositely charged, they attract.

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