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Ionic compound
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Ionic compound
In chemistry, an ionic compound is a chemical compound in
which ions are held together in a lattice structure by ionic bonds.
Usually, the positively charged portion consists of metal cations
and the negatively charged portion is an anion or polyatomic ion.
Ions in ionic compounds are held together by the electrostatic
force between oppositely charged bodies. Ionic compounds have a
high melting and boiling point, and they are hard and very brittle.
They are also called salts .
Ions can be single atoms, as the sodium and chloride in common
table salt sodium chloride, or more complex groups such as the
carbonate in calcium carbonate. But to be considered an ion, they
must carry a positive or negative charge. Thus, in an ionic bond,
one 'bonder' must have a positive charge and the other a negative
one. By sticking to each other, they resolve, or partially resolve,
their separate charge imbalances. Positive to positive and negative
to negative ionic bonds do not occur. (For an easily visible
analogy, experiment with a pair of bar magnets.)
The crystal structure of sodium chloride, NaCl, a
typical ionic compound. The purple spheres are sodium
cations, Na+, and the green spheres are chloride anions,
Cl−.
Chemical compounds are never strictly ionic. Even the most electronegative/electropositive pairs such as caesium
fluoride exhibit a degree of covalency. Similarly, covalent compounds often exhibit charge separations. See also
HSAB theory.
Physical properties
Physical Properties
Ionic Compounds
States(at room temperature)
Solid
Electrical conductivity
Solid: No Liquid: Yes Aqueous: Yes (if soluble)
Boiling point and Melting Point High
Solubility in water
Often high
Thermal conductivity
Low
Characteristics
Ionic compounds have strong electrostatic bonds between particles. As a result, they generally have very high
melting and boiling points. They also have good electrical conductivity when molten or in aqueous solution. While
ionic inorganic compounds are solids at room temperature and usually form crystals, organic ionic liquids are of
increasing interest.
The ions produced by electron transfer attract each other by electrostatic attraction and this creates an ionic bond.
Ionic compound
Solubility
Following the aphorism, "like dissolves like", ionic compounds dissolve in polar solvents, especially those that
ionize, such as water and ionic liquids. They are usually appreciably soluble in other polar solvents such as alcohols,
acetone and dimethyl sulfoxide as well. Ionic compounds tend not to dissolve in nonpolar solvents such as diethyl
ether or petrol.
When the oppositely charged ions in the solid ionic lattice are surrounded by the opposite pole of a polar molecule,
the solid ions are pulled out of the lattice and into the liquid. When this force is more than the electrostatic attraction
of the lattice, the ions become dissolved in the liquid.
Electricity conductivity
Solid ionic compounds cannot conduct electricity because there are no mobile ions or electrons present in the lattice.
When the ionic compounds are dissolved in a liquid or molten, they can conduct electricity with the mobile ions.
Name
According to the IUPAC, an ionic compound's common name is written using two words. The name of the cation
comes first (when using stock nomenclature with the oxidation number written in parentheses, followed by the name
of the anion.[1] For example, Fe2(SO4)3 is named as iron(III) sulfate. If the Classical naming system is being used,
some ionic compounds have special "old" names, such as ferric (iron(III)), ferrous (iron(II)), cupric (copper(II)), and
cuprous (copper(I)).
References
[1] Kotz, John C.; Weaver, Paul M (2006). Chemistry and Chemical Reactivity (Sixth ed.). Belmont, CA: Thomson Brooks/Cole. p. 111.
ISBN 0-534-99766-X.
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Image Sources, Licenses and Contributors
Image:Sodium-chloride-3D-ionic.png Source: http://en.wikipedia.org/w/index.php?title=File:Sodium-chloride-3D-ionic.png License: Public Domain Contributors: Benjah-bmm27
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