ATOMIC STRUCTURE : ORBITALS

According to the quantum mechanical model of the atom, and behavior of particular, specific electron described by mathematical model or expression called a wave function. The same types of expression used to described the motion of the waves in a fluid. The solution to a waves, wave equation called wave function. This is denoted by the Greek letter psi (ψ).

           The square of wave function, (ψ²) is by plotted in three dimensional space or structure and orbitals describes the volume of the space and around the nucleus that an electron is most likely to occupy. Orbitals as looking like a photograph of the electron taken at a slow shutter speed. This orbital would appear as a blurry cloud indicating the region of space where the electron. The electron clouds doesn't have a sharp boundary but for practical purposes we can setting the limits by saying that an orbital represents the space where an electron spends 90 percentage to 95 percentage of it's time.

                There's four different types of orbitals, denoted s, p, d, and f, each orbitals have a with different shape. All of the 4 will be concerned primarily with s and p orbitals because these are more common in organic chemistry. And s orbital shape is spherical, with the nucleus and its center, and p orbitals is dumbbell shapes, and five d orbitals are cloverleaf shapes and fifth d orbitals is shapes elongated dumbbell with a doughnut around it's middle. 

                    This orbitals atom organized into different types of electron shells. The centered around the nucleus have successively large size and energy. The different types of shells contains different numbers and types of orbitals. And all each orbitals within a shell can be occupied by two electrons. The first shell contains only one single s orbital, it's denoted 1s, orbital and thus holds only two electrons. The second shells contains one 2s orbital and three 2p orbitals and it's hold a total number of eight electrons, The 3rd shell contains 3s orbital, and 3 p orbitals and five 3 d orbitals for a total capacity of eighteen electrons.

All the energy levels of electrons in atom. The 1st shell holds maximum of two electrons in one1s orbital and second shell holds maximum eight electrons in 2s and three 2p orbital and third shell maximum hold 18 elecyrons. In one 3s three p and five 3d orbitals the two electrons in each orbitals up and down the energy level of the 4s orbitals falling between 3p and 3d

This orbital groups and their energy levels are 3 different p orbitals within a given shell are oriented in the space along mutually perpendicular directions and it's denoted Px, Py, Pz orbitals. The two lobes of each p orbitals are separated by the region of zero electron density called a node. And the 2 type of region separated by the node having different types of algebraic signs, +  and - in the wave function as represented by the different types of colors. The mathematical signs of different orbitals lobes having important consequences with respect to the chemical bonding and chemical reactivity. 

1) 2px                    2)2py            3)2pz

.            1s            1s              H₂ molecule

                    

                    The overlapping between the H₂ molecular orbitals elongated egg shapes by pressing two sphere together. If that plane were to pass through the middle of the bond, intersection of that plane and overlapping orbitals would be a circle shape. In other term H-H bond is cylindrically symmetricals, such bonds which is formed by the head-on overlapping of two atomic orbitals along the line drawn between the nuclei, it's called sigma (σ) bonds.