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All stable copper isotopes—atoms of the same element but with different masses--need to be considered before coming up with an average atomic mass for the element. There are two such isotopes, copper-63 and copper-65 (“Isotopes of Copper”). Copper has an atomic number of 29. This means it has 29 protons. All stable isotopes are electrically neutral. Therefore, there must be the same number of electrons as protons. In the case of copper, there are 29 electrons.
However, to account for the fact that they are isotopes, they have different numbers of neutrons. Protons have a relative mass (on the carbon-12 scale) of about one, and electrons 1/1836 (almost no mass). Neutrons, with a mass also of about one, account for the difference in masses of different isotopes (“Electron Structure Discussion”). Therefore, copper-63 has 34 neutrons, and copper-65 has 36 neutrons. The natural abundance of copper-63 is 69.17%, and the abundance of copper-65 is 30.83% (“Isotopes of Copper”).
As for the electrons themselves, they completely fill the first, second, and third shells. In addition, one electron enters the fourth shell. Within the subshells, they are distributed in the electron configuration 1s2 2s2 2p6 3s2 3p6 4s1 3d10. The “s,” “p,” and “d” are labels of types of subshells. S subshells can hold up to two electrons, p subshells can hold up to six, and d subshells up to ten (“Electron Structure Discussion”). So, the electron configuration indicates that the s subshell in the first, second, and third shells are completely filled. Also, the p subshells in shells two and three and the d subshell in shell three are completely filled. However, the s subshell in shell four is only half-filled.
But, only two electrons can fit in an orbital (“Electron Structure Discussion).
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