Sodium and chlorine bonding ionically to form sodium chloride. Sodium loses its outer electron endothermically to give it a noble gas electron configuration, and this electron enters the chlorine atom exothermically. The oppositely charged ions are then attracted to each other, and their bonding releases energy. The net transfer of energy is that energy leaves the atoms, so the reaction is able to take place.

An ionic bond (or electrovalent bond) is a type of chemical bond that can often form between metal and non-metal ions (or polyatomic ions such as ammonium) through electrostatic attraction. Image File history File links No higher resolution available. ... Image File history File links No higher resolution available. ... This article is about the chemical series. ... A chemical bond is the physical process responsible for the attractive interactions between atoms and molecules, and that which confers stability to diatomic and polyatomic chemical compounds. ... This article is about metallic materials. ... Together with the metals and metalloids, a nonmetal is one of three categories of chemical elements as distinguished by ionization and bonding properties. ... This article is about the electrically charged particle. ... A polyatomic ion or molecule ion is an ion consisting of covalently bonded atoms that can be considered as acting as a single unit in the context of acid/base chemistry or in the formation of salts. ... A ball-and-stick model of the ammonium cation Ammonium is also an old name for the Siwa Oasis in western Egypt. ... Electrostatics is the branch of physics that deals with the force exerted by a static (i. ...

The metal donates one or more electrons, forming a positively charged ion or cation with a stable electron configuration. These electrons then enter the non metal, causing it to form a negatively charged ion or anion which also has a stable electron configuration. The electrostatic attraction between the oppositely charged ions causes them to come together and form a bond. For other uses, see Electron (disambiguation). ... A cation is an ion with positive charge. ... Electron atomic and molecular orbitals In atomic physics and quantum chemistry, the electron configuration is the arrangement of electrons in an atom, molecule, or other physical structure (, a crystal). ... An anion is an ion with negative charge. ...

For example, common table salt is made of sodium chloride. In the ionic bonding, the sodium (Na) loses one electron, forming a cation, and the chlorine (Cl) gains an electron to form an anion. These ions are then attracted to each other in a 1:1 ratio to form sodium chloride (NaCl). Edible salt is a mineral, one of the few rocks people eat. ... R-phrases 36 S-phrases none Flash point Non-flammable Related Compounds Other anions NaF, NaBr, NaI Other cations LiCl, KCl, RbCl, CsCl, MgCl2, CaCl2 Related salts Sodium acetate Supplementary data page Structure and properties n, εr, etc. ... For sodium in the diet, see Edible salt. ... General Name, symbol, number chlorine, Cl, 17 Chemical series halogens Group, period, block 17, 3, p Appearance yellowish green Standard atomic weight 35. ...

2Na⁺ + Cl^-₂ → 2NaCl

Electron configurations of lithium and fluorine. Lithium has one electron in its outer shell, held rather loosely because the ionization energy is low. Fluorine carries 7 electrons in its outer shell. When one electron moves from lithium to fluorine, each ion acquires the noble gas configuration. The bonding energy from the electrostatic attraction of the two oppositely-charged ions has a large enough negative value that the overall bonded state energy is lower than the unbonded state

The removal of electrons from the atoms is endothermic and causes the ions to have a higher energy. There may also be energy changes associated with breaking of existing bonds or the addition of more than one electron to form anions. However, the attraction of the ions to each other lowers their energy. Image File history File links Diagram of electron transfer. ... Image File history File links Diagram of electron transfer. ... Electron atomic and molecular orbitals In atomic physics and quantum chemistry, the electron configuration is the arrangement of electrons in an atom, molecule, or other physical structure (, a crystal). ... This article is about the chemical element named Lithium. ... Distinguished from fluorene and fluorone. ... The ionization energy (IE) of an atom or of a molecule is the energy required to strip it of an electron. ... This article is about the electrically charged particle. ... This article is about the chemical series. ... It has been suggested that Coulombs law be merged into this article or section. ...

Ionic bonding will occur only if the overall energy change for the reaction is favourable – when the bonded atoms have a lower energy than the free ones. The larger the resulting energy change the stronger the bond. The low electronegativity of metals and high electronegativity of non-metals means that the energy change of the reaction is most favorable when metals lose electrons and non-metals gain electrons. Electronegativity is a measure of the ability of an atom or molecule to attract electrons in the context of a chemical bond. ...

Pure ionic bonding is not known to exist. All ionic bonds have a degree of covalent bonding or metallic bonding. The larger the difference in electronegativity between two atoms, the more ionic the bond. Ionic compounds conduct electricity when molten or in solution. They generally have a high melting point and tend to be soluble in water. Covalent redirects here. ... Metallic bonds are found in metals like copper. ... Electronegativity is a measure of the ability of an atom or molecule to attract electrons in the context of a chemical bond. ... Electricity (from New Latin Ä“lectricus, amberlike) is a general term for a variety of phenomena resulting from the presence and flow of electric charge. ... The melting point of a crystalline solid is the temperature range at which it changes state from solid to liquid. ...

Polarization effects

Ions in crystal lattices of purely ionic compounds are spherical; however, if the positive ion is small and/or highly charged, it will distort the electron cloud of the negative ion. This polarization of the negative ion leads to a build-up of extra charge density between the two nuclei, i.e., to partial covalency. Larger negative ions are more easily polarized, but the effect is usually only important when positive ions with charges of 3+ (e.g., Al³⁺) are involved (e.g., pure AlCl₃ is a covalent molecule). However, 2+ ions (Be²⁺) or even 1+ (Li⁺) show some polarizing power because their sizes are so small (e.g., LiI is ionic but has some covalent bonding present). ally i lalalalove u haha This article is about the electrically charged particle. ... In mineralogy and crystallography, a crystal structure is a unique arrangement of atoms in a crystal. ... For other uses, see Sphere (disambiguation). ... In electrostatics, the polarization is the vector field that results from permanent or induced electric dipole moments in a dielectric material. ... The nucleus of an atom is the very small dense region, of positive charge, in its centre consisting of nucleons (protons and neutrons). ... Electric charge is a fundamental property of some subatomic particles, which determines their electromagnetic interactions. ...

Ionic structure

Ionic compounds in the solid state form a continuous ionic lattice structure in an ionic crystal. The simplest form of ionic crystal is a simple cubic. This is as if all the atoms were placed at the corners of a cube. This unit cell has a weight that is the same as 1 of the atoms involved. When all the ions are approximately the same size, they can form a different structure called a face-centered cubic (where the weight is 4 * atomic weight), but, when the ions are different sizes, the structure is often body-centered cubic (2 times the weight). In ionic lattices the coordination number refers to the number of connected ions. The crystal structure of sodium chloride, NaCl, a typical ionic compound. ... An ionic crystal is a crystal consisting of ions bound together by their electrostatic attraction. ... In mineralogy and crystallography, a crystal structure is a unique arrangement of atoms in a crystal. ... In crystallography, the cubic crystal system (or isometric crystal system) is the most symmetric of the 7 crystal systems. ... In crystallography, the cubic crystal system (or isometric crystal system) is the most symmetric of the 7 crystal systems. ... In chemistry coordination number (c. ...

Ionic versus covalent bonds

In an ionic bond, the atoms are bound by attraction of opposite ions, whereas, in a covalent bond, atoms are bound by sharing electrons. In covalent bonding, the molecular geometry around each atom is determined by VSEPR rules, whereas, in ionic materials, the geometry follows maximum packing rules. Covalent redirects here. ... Geometry of the water molecule Molecular geometry or molecular structure is the three-dimensional arrangement of the atoms that constitute a molecule, inferred from the spectroscopic studies of the compound. ... Geometry of the water molecule Molecules have fixed equilibrium geometries--bond lengths and angles--that are dictated by the laws of quantum mechanics. ... Close-packing of spheres refers to arranging an infinite lattice of spheres so that they take up the greatest possible fraction of an infinite 3-dimensional space. ...

Electrical conductivity

Main article: Electrolyte

Ionic substances in solution conduct electricity because the ions are free to move and carry the electrical charge from the anode to the cathode. Ionic substances conduct electricity when molten because atoms (and thus the electrons) are mobilised. Electrons can flow directly through the ionic substance in a molten state. An electrolyte is a substance containing free ions that behaves as an electrically conductive medium. ...

Substances in ionic form

See also

• Chemical bond
• Covalent bond
• Linear combination of atomic orbitals
• Metallic bonding
• Hybridisation
• Hydrogen bond
• Noncovalent bonding
• Disulfide bond
• Chemical polarity
• Polyatomic ion

A chemical bond is the physical process responsible for the attractive interactions between atoms and molecules, and that which confers stability to diatomic and polyatomic chemical compounds. ... Covalent redirects here. ... The linear combination of atomic orbitals molecular orbital method (usually called the LCAO MO method) is a technique for calculating molecular orbitals in quantum chemistry. ... Metallic bonding is intramolecular bonding within metals. ... four sp³ orbitals three sp² orbitals In chemistry, hybridisation or hybridization (see also spelling differences) is the concept of mixing atomic orbitals to form new hybrid orbitals suitable for the qualitative description of atomic bonding properties. ... An example of a quadruple hydrogen bond between a self-assembled dimer complex reported by Meijer and coworkers. ... This article needs to be wikified. ... In chemistry, a disulfide bond is a single covalent bond derived from the coupling of thiol groups. ... A commonly-used example of a polar compound is water (H2O). ... An electrostatic potential map of the nitrate ion (NO3−). Areas coloured red are lower in energy than areas coloured yellow A polyatomic ion is a molecule that bears ionic groups, that is, a molecule with a charge. ...

External links

• ionic bonding tutorial I
• ionic bonding tutorial II
• ionic bonding tutorial III