A Wisdom Archive on Ion

A chemical bond is the physical phenomenon of chemical substances being held together by electrons or by electrostatic forces. Classically, strong chemical bonds are found in molecules, crystals or in solid metal and they organize the atoms in ordered structures. Weak chemical bonds are classically explained to be effects of polarity, or the lack of it, of strong bonds. In theory, all bonds can be explained by quantum theory, but in practice, chemical bonds are divided in several categories. Simplifications of quantum theory ha ... Including:

• Chemical bond - Bonds in chemical formulas
• Chemical bond - Strong chemical bonds
• Chemical bond - Ionic bond
• Chemical bond - Polar covalent bond
• Chemical bond - Covalent bond
• Chemical bond - Other strong bonds
• Chemical bond - Coordinate covalent bond
• Chemical bond - Polyatomic ions
• Chemical bond - Banana bond
• Chemical bond - Chemical bonds involving more than two atoms
• Chemical bond - Aromatic bond
• Chemical bond - Metallic bond
• Chemical bond - Weak chemical bonds
• Chemical bond - Dipole-dipole interactions
• Chemical bond - Hydrogen bond
• Chemical bond - Induced dipole interactions
• Chemical bond - Van der Waals forces
• Chemical bond - Electrons in chemical bonds
• Chemical bond - Limitations of valence bond theory

Read more here: » Chemical bond: Encyclopedia - Chemical bond

Generally speaking, atomic ionization energies decrease down a group of the periodic table, and increase left-to-right across a period. Ionization energy exhibits a strong negative correlation with atomic radius. Successive ionization energies of any given element increase markedly. Particularly dramatic increases occur after any given block of atomic orbitals is exhausted. This is because, after all the electrons are removed from an orbital, the next ionization energy involves removing an electron from a closer orbital to the nucle ...

Read more here: » Ionization potential: Encyclopedia II - Ionization potential - Values and trends

N and the O+ ion are isoelectronic because each has one atom and 5 electrons in the outer electronic shell. CO, N2 and NO+ are isoelectronic because each has 2 nuclei and 10 valence electrons (4+6, 5+5, and 5+5, respectively). CH2=C=O and CH2=N=N are isoelectronic. CH3COCH3 and CH3N2CH3 are not isoelectronic. They do have the same number of nuclei and the same number of valence electrons, but the atoms' co ...

Read more here: » Isoelectronic: Encyclopedia II - Isoelectronic - Examples

Weak chemical bonds are mostly intermolecular (between two molecules), or can be considered as such, since they are the first to break when conditions change. In some organic molecules, and especially in biomolecules, correct organisation of weak chemical bonds, sometimes even the Van der Waals forces, is essential for the proper function of the molecule, f.e. for the catalytic activity of a protein. Chemical bond - Dipole-dipole interactions. Main articles

Read more here: » Chemical bond: Encyclopedia II - Chemical bond - Weak chemical bonds

Chemical bond - Aromatic bond. Main articles: Aromaticity, and [[{{{2}}}]], and [[{{{3}}}]], and [[{{{ ...

Read more here: » Chemical bond: Encyclopedia II - Chemical bond - Chemical bonds involving more than two atoms

Chemical bond - Coordinate covalent bond. Main articles: Coordinate covalent bond, and [[{{{2}}}]], and [[{{{3}}}]], and [[{{{4}}}]]

Read more here: » Chemical bond: Encyclopedia II - Chemical bond - Other strong bonds

Many simple compounds involve covalent bonds. These molecules have structures that can be predicted using valence bond theory, and the properties of atoms involved can be understood using concepts such as oxidation number. Other compounds that involve ionic structures can be understood using theories from classical physics. In the case of ionic bonding, electrons are mainly localized on the individual atoms, and electrons do not travel between the atoms very much. Each atom is assigned an overall electric charge to help concept ...

Read more here: » Chemical bond: Encyclopedia II - Chemical bond - Electrons in chemical bonds

However, more complicated compounds such as metal complexes, or electron deficient compounds, cannot be described by valence bond theory alone, and quantum chemistry (based on quantum mechanics) has to be used. Intermolecular forces cause molecules to be attracted or repulsed by each other. Often, these define some of the physical characters (f.e.melting point) of a substance. These forces include ionic interactions, hydrogen bonds, dipole-dipole interactions, and induced dipole interactions. Linus Pauling's book The Nature of the Chemical Bond

Read more here: » Chemical bond: Encyclopedia II - Chemical bond - Limitations of valence bond theory

These chemical bonds are intramolecular forces, that keep atoms held together in molecules and in solids. All these bonds may be single, double or triple, by which it is meant that the amount of electrons participating in a bond (or located in a bonding orbital) is two, four or six, respectively. Quadruple bonds are not unheard of, but they are extremely rare. Chemical bond - Ionic bond. Main articles: Ionic bond,

Read more here: » Chemical bond: Encyclopedia II - Chemical bond - Strong chemical bonds