Modern Atomic theory
The actual model for the atom is the Electron Cloud Model, which is the result is the result of quantum mechanics. The atom consists in a nucleus formed by Protons and Neutrons (p++n0) where the Proton gives the identity of the element. The electrons are arranged within a cloud, called that way because the atom must be in some place of that cloud, that is called Heisenberg's uncertainty. The electrons are arranged in four type of orbitals (clouds), the s, p, d, f blocks. Each block accept certain mount of electrons per period. For instance, s accepts only 2 electrons. p accepts 6, d accepts 10, f accepts 14.
With the discover of Planck's constant & Photoelectric effect. The view for the atoms changed radically.
The electron plays an important role in the object of making compounds. They have the job of sharing or giving up themselves. As every compound needs to be stable (8 electrons per element, except for hydrogen) they need to be shared or gifted according to their number of valence electrons.
Quantum Numbers
The Bohr model was a one-dimensional model that used one quantum number to describe the distribution of electrons in the atom. The only information that was important was the size of the orbit, which was described by the n quantum number. Schrödinger's model allowed the electron to occupy three-dimensional space. It therefore required three coordinates, or three quantum numbers, to describe the orbitals in which electrons can be found. (Chemed, 2015)
The three coordinates that come from Schr�dinger's wave equations are the principal (n), angular (l), and magnetic (m) quantum numbers. These quantum numbers describe the size, shape, and orientation in space of the orbitals on an atom.
The principal quantum number (n) describes the size of the orbital. Orbitals for which n = 2 are larger than those for which n = 1, for example. Because they have opposite electrical charges, electrons are attracted to the nucleus of the atom. Energy must therefore be absorbed to excite an electron from an orbital in which the electron is close to the nucleus (n = 1) into an orbital in which it is further from the nucleus (n = 2). The principal quantum number therefore indirectly describes the energy of an orbital.
The angular quantum number (l) describes the shape of the orbital. Orbitals have shapes that are best described as spherical (l = 0), polar (l = 1), or cloverleaf (l = 2). They can even take on more complex shapes as the value of the angular quantum number becomes larger.
4 iMagazine / April, 2013