Callbacks of chemistry
1) Equation of Schroedinger:
It defines the wave function y whose module picture represents the probability to find an
electron in one determined region of the space and in a determined 
moment where H is the Hamiltoniana of the system that
it holds account is of the energy upgrades them that of the kinetic
energy of the same one.
2) Energy of electrons in the hydrogen atom:
draft of a quantizzata energy, in fact the electrons cannot assume all the levels of energy.
3) quantici Numbers:
The quantici numbers are the following four:
n main quantico number, characterizes the energy of the orbital one
l secondary quantico number, characterizes the shape of the orbital one
m magnetic quantico number
s quantico number of spin
4) Principle of exclusion of Pauli:
It asserts that the same quantici numbers cannot exist two having atoms, in particular two atomic elements that find neighbors distinguish themselves for the quantico number of spin that it can only assume two values therefore in every orbital can it are us to the maximum two electrons.
5) Orbital and they typology :
The orbital ones s are spherical, the p are 3 orbital ones to shape of 8 having the same energy, the d are orbital to shape of quadripallide, also degenerate they.
6) Principle of Hund:
It asserts that orbital the degenerate ones come filled up all with an electron before and subsequently it is passed to insert in everyone of they according to electron with spin opposite to the previous one.
7) Aufbau:
It is the rule that has rendered the construction of the periodic table possible, is based on leaving from the having hydrogen atom a single electron around to the nucleus and adding 2 electrons on the orbital one s, then 6 electrons in the p and therefore via.
8) Hybridization:
When two atoms come joined from a tie the configuration to minimal orbital energy pu² to preview that nobody of the atomic ones coincides with orbital the molecular one that turns out to be a hybrid of the two orbital ones of departure.
9) Hybridization sp:
It is the hybridization between orbital s and an orbital one p, that is between one sphere and 8,
10) Hybridization sp2 :
It is the hybridization between orbital s and two orbital ones p.
11) Hybridization sp3 :
It is the hybridization between orbital s and three orbital ones p.
12) Energy of tie:
Draft of the energy necessary in order to break off the tie between two atoms.
13) Rule of the octet :
The rule of the octet establishes that the stabler configuration that is that one to minimal energy is that one in which on the energetic level more outside there are a minimum of 8 electrons that is we have 2 electrons in the orbital one s and 6 electrons in the 3 p.
14) Energy of ionization:
It is the energy necessary in order to extract an electron from an atom to the temperature of 0K and carrying it in state of quiet in a at a distance infinite point.
15) Affinity for electron:
Atom size is the variation of energy of one isolates to you to 0K for the purchase of one electron size.
16) Elettronegatività:
It is the ability to an atom to recall to if the electrons that come puttinges in common in a tie.
17) Method of the valence tie:
Every electron comes considered pertaining to the nucleus of an orbital described atom and from an atomic one.
18) orbital Method of the molecular one:
Every electron comes considered pertaining to obtained the orbital described molecule and from a molecular one for linear combination of the orbital functions of wave of the atomic ones.
19) Tie to omeopolare and ties s and p :
It is a tie between two atoms of the same element, of it derives that the permanent molecule does not introduce polarity in how much note the two constituent atoms is characterizes to you from the same elettronegatività. If the tie is along combining the nuclei it speaks otherwise about tie tie s p. A simple tie, that it is always of type s, inthe case everyone of two atoms is had puts to disposition of the tie only an electron, otherwise a double or triple tie can be had. The type ties p come form to you from the orbital ones of type p that they are not found along the axis of the two nuclei.
20) Covalent bond and electrostatic tie:
The covalent bond happens between various atoms characterizes to you from a various elettronegatività, of it it derives that the electrons mainly will be attracted to one of two atoms and therefore the formation of a dipole is had. It is therefore a mixed tie, is atomic that electrostatic.
21) Tie of coordination:
It is a tie in which an atom giver puts to disposition of the tie an orbital suit that is an electron brace, in the atom accepter an empty one to corresponding energy must be had orbital.
22) delocalizzati Electrons:
They are electrons that are common to all the molecule, is the case of the benzene.
23) ionic Ties:
It is the tie that is established when strong elettronegatività between two atoms is one, comes therefore less the attraction between electrons to share same the orbital one and prevails the electrostatic attraction.
24) reticular Energy:
It is the energy that free when Ionian denied to you and Ionian positi to you leaving from infinite distance is coupled in order to form one ionic crystal size.
25) dipolar Tie:
They are electrostatic ties who had us to interactions between dipoles, have had to the forces of van der Waals or of London.
26) Tie hydrogen:
Alloy with a elettronegativo atom is an electrostatic tie in which hydrogen forming therefore a dipole, that it electrostatically attracts an other elettronegativo atom of the same molecule or also of an other.
27) metallic Tie:
The metallic elements are approximately 75% of those present ones in nature, they have tendency to lose electrons therefore in a metallic crystal all the electrons of atom valence every distribute themselves on orbital extended to all the crystal.
