characterize the types of orbitals

TYPES OF ORBITAL

Atoms are composed of a heavy nucleus surrounded by light electrons. The behavior of electrons is governed by the rules of quantum mechanics. These rules allow electrons occupy specific regions called orbitals. The interactions of atoms are almost exclusively by their outermost electrons, so that the shapes of these orbitals becomes very important. For example, when atoms approach each other, if their outermost orbital overlap, create a strong chemical bond; then, some knowledge of the shape of the orbit is important to understand the atomic interactions

• And orbital quantum numbers

Physicists have found it convenient to use abbreviations to describe the characteristics of electrons in an atom. The abbreviation is in terms of quantum numbers; these numbers can only be integers, no fractions. The principal quantum number, n, it is related to the electron energy; then, is the orbital quantum number, l, and the angular momentum quantum number, m. Other quantum numbers, but not relate directly to the shape of the orbital. Orbital orbits are not, in the sense of being routes around cores; instead, they represent the positions where it is more likely that the electron will be found.

• Orbital lower order

For each value of n, there is an orbital where m are zero. These orbitals are spheres. The higher the, largest value of n will be the sphere; that is, it is more likely that the electron is farthest from the core. The spheres are not equally dense throughout; It is more likely to be nested shells. For historical reasons, this is called orbital s. Because the rules of quantum mechanics, electrons less energy, with n = 1 and m must be zero, so the only orbital that exists for n = 1 is the s orbital. The orbital s also exists for each different value of n.

• P orbitals

When n is greater than one, more possibilities open. The orbital quantum number, l, may have any value up to n-1. When l equals one, the called orbital p orbital. P orbitals are seen as weights. For each l, m ranges from positive to negative in steps of one. Then for n = 2, l = 1, m can equal 1, 0 or -1. This means that there are three versions of the orbital one with the weight up and down, one with the weight from left to right and one with the weight at right angles to each other. P orbitals exist for all principal quantum number greater than one, but have an additional structure as n increases.

• D orbitals

When n = 3, L may be equal to 2, and when l = 2, m may amount to 2, 1, 0, -1 and -2. Orbital l = 2 are called orbitals, and there are five different types corresponding to different values ​​of m. The orbital n = 3, l = 2, m = 0 is also seen as a weight, but with a donut around the middle. The other four d orbitals look like four eggs stacked one end in a square pattern. The various versions have eggs just pointing in different directions.

• F orbitals

Orbital n = 4, L = 3 is called f orbitals are difficult to describe. They have many complex features. For example, the orbital n = 4, l = 3, m = 0, m = 1 and m = -1 also shaped weights, but now there are two donuts between the ends of the barbell. The other values ​​of m are as a group of eight balloons, with all knots tied together in the middle.