Wednesday, August 17, 2011

Patterns of Chemical Bonding

Only a few elements on the periodic table are satisfied with their arrangement of electrons. This is due to an imbalance between the perceived positive and negative forces of attraction involved in the atom. Collage may be seen as a form of atoms undergo correction, resulting from the electronic configuration as stable as possible a full shell. This pattern is known Asthe octet rule. It is so called because the second row elements, and who need to fill eight valence electron shells. This is a golden rule, and there are many exceptions to this, but generally the elements combine in a way that results in that there are 8 valence electrons in their shells. An important exception is the closest orbital electron to the nucleus, this orbit requires only two electrons to fill it.

The electrons necessary for this purpose are not free, must come from somewhere. This is where the atomic bond This occurs when two atoms, dissatisfied with their electronic configurations meet to share / exchange of electrons to obtain a more stable configuration. There are two main types of atomic bonds:

A covalent bond where electrons are shared.

Bond ionic bonding that occurs after the transfer of electrons.

When you think of covalent bonds, always, always think about sharing. Atoms together and share electrons with each other in a sort of meshing model. This is the most common bond, and is completely non-metals.

Ionic bonds, however, occur when the attraction of one atom to another is sufficient to tear an electron-atom valence shell and make it part of them. Reception, or steal, the atom is the atom charge more positive than that, it takes between when the electron with negative charge more attractive the atom, was part of the first.

This change causes ionization, charge exchange of neutral atoms, both atoms. Exchange leads to a more stable configuration of the second atom, but what about the atom the electron has been taken in the first place? After that, and will deionize restabalize. Ionic bond forms when the positive charge (electron-deficient), the atom by atom is attracted to, the more negative charge (electron-rich). This attraction is not just the transfer of electrons. Thus the term "ionic bond" is a somewhat 'misleading. A more appropriate term would be "ionic attraction '

A "real life" alongside the covalent vs ionic dynamics of a pair of hand in front of a person being robbed, respectively. The couple shares a mutual attraction and covalent bonds are more stable than single, and there is a common link between them. A person who is being stolen and the thief closing (atom) and robbery (electrons) are more closely parallel the dynamics of ionic bond, because there is a common bond between the atoms, rather than an attraction.

You can ask how an ionic bond prefer a more stable configuration for the two atoms when one of them gets much the tree? For that, you believe that the elements are more attractive than others to electrons, called electro negativity, and it generally increases with the atom approaches a more stable configuration. If an atom with low electronegativity (such as sodium, which has an "extra" electrons), to something that has a high electronegativity (such as fluorine, which needs a more electrons to satisfy the byte), fluoride, sodium steal its electron to obtain a more stable configuration. Sodium is now slightly unfortunate, because now a more positive effect of the nucleus of a negative force of its electrons. It will have an equally mild attraction for the electron has been lost. This creates a situation that is lower in energy and more stable.

The molecule formed by this bond, in particular, is known as sodium fluoride, and is an excellent example of a salt. A salt is an ionic compound formed by bonds.Given the nature of their duties, the salts are very low and usually very soluble. Acids and bases are usually found in salt form (HCl and NaOH) for hydrogen (H) and hydronium (OH-) easily dissociate chlorine and sodium, respectively, in aqueous solution. All salts are called in this way, the first metal, nonmetal second and adds the suffix "IDE".


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