To understand the complexity of the copper atom, you must first understand the basic structure of a general atom. Atoms are considered the simplest matter; impossible to cut into smaller pieces. There are, however, subatomic particles that are the building blocks of the countless atoms that make up the earth: protons, neutrons and electrons. Positively charged particles (protons) and neutrally charged particles (neutrons) make up the nucleus, electrons surround the nucleus in a cloud. The configuration and number of electrons are crucial to composing and distinguishing elements. This brings us to the analysis of the element copper. There are different ways that electrons are around a copper atom, and all atoms, for that matter. The first aspect of an electronic configuration is the energy level (number n, or principal quantum number) reached by the electrons. Each period of the periodic table represents an energy level. The number of electrons (equal to the number of protons) an element has, for the most part, determines the highest energy level of an atom. Copper has atomic number 29 and is in the fourth period, so its electrons reach the fourth energy level. The energy level determines the size of the orbital. Within each energy level there is a sublevel that represents the shape of the path taken by the electron. The number of possible forms within an energy level is equal to the number of the energy level. In the copper atom the electrons reach the fourth energy level, so there are four “l” values: l=0(s orbital), l=1(p orbital), l=2(d orbital), l=3( f orbital). Then there is another sublevel called magnetic quantum number. This value determines the orientation of the orbit... at the center of the card... the diamagnetic species is slightly repelled by an external field. The way the copper atom fills its orbitals is only one factor that contributes to the distinctness of its character; isotopes are another. There is even more uniqueness and variety in an atom of an element because of isotopes. An isotope is a derivation of an element: it maintains the same quantity of protons (and therefore electrons) but has a different number of neutrons. Isotopes are present in different abundances. For the element copper there are 29 isotopes, of which only two are stable and non-radioactive: 63Cu and 65Cu with abundances of 69.15% and 30.85% respectively. Each element has a distinct composition due to its electronic configuration, the number of protons (and therefore electrons), naturally occurring isotopes, and many other factors. It is this innate uniqueness of the elements that makes up almost every corner of the earth.