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s 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
An
ionic bond (or
electrovalent bond) is a type of chemical bond based on electrostatic forces between two oppositely-charged
ions. In ionic bond formation, a metal donates an electron, due to a low electronegativity, to form a positive ion or cation. In ordinary table salt (NaCl), the bonds between the sodium and
chloride ions are ionic bonds. Often ionic bonds form between
metals and non-metals. The non-metal atom has an electron configuration just short of a noble gas structure. They have high electronegativity, and so readily gain electrons to form negative ions or anions. The two or more ions are then attracted to each other by electrostatics.
\mathrm{Li + F}\ \ \ \to\ \ \ \mathrm{Li^+F^-}\,\!
\mathrm{3Na + P}\ \ \ \to\ \ \ \mathrm{(Na^+)_3P^{3--->
Ionic bonding occurs 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.
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.
Polarization effects
Ions in crystal lattices of purely ionic compounds are sphere; however, if the positive ion is small and/or highly charged, it will distort the electron cloud of the negative ion. This
Polarization (electrostatics) of the negative ion leads to a build-up of extra charge density between the two
atomic nucleus, i.e., to partial covalency. Larger negative ions are more easily polarized, but the effect is usually only important when positive ions with electrical charge 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).
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 Cubic (crystal system) (where the weight is 4*atomic weight), but, when the ions are different sizes, the structure is often
Cubic (crystal system) (2 times the weight). In ionic lattices the
coordination number refers to the number of connected ions.
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
close-packing rules.
Electrical conductivity
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.
Substances in ionic form
{||valign="top"|{|class="wikitable"|+Common
Cations|-!style="text-align: left"|Stock System Name!style="text-align: left"|Formula!style="text-align: left"|Historic Name|-!colspan="3" style="background-color: aliceblue"|
Simple Cations|-|Aluminum||Al3+|||-|Barium||Ba2+|||-|Beryllium||Be2+|||-|Caesium||Cs+|||-|Calcium||Ca2+|||-|Chromium(II)||Cr2+||Chromous|-|Chromium(III)||Cr3+||Chromic|-|Chromium(VI)||Cr6+||Chromyl|-|Cobalt(II)||Co2+||Cobaltous|-|Cobalt(III)||Co3+||Cobaltic|-|Copper(I)||Cu+||Cuprous|-|Copper(II)||Cu2+||Cupric|-|Copper(III)||Cu3+|||-|Gallium ||Ga3+|||-|Gold(I)||Au+|||-|Gold(III)||Au3+|||-|Helium||He2+||(Alpha particle)|-|Hydrogen||H+||(Proton)|-|Iron(II)||Fe2+||Ferrous|-|Iron(III)||Fe3+||Ferric|-|Lead(II)||Pb2+||Plumbous|-|Lead(IV)||Pb4+||Plumbic|-|Lithium||Li+|||-|Magnesium||Mg2+|||-|Manganese(II)||Mn2+||Manganous|-|Manganese(III)||Mn3+||Manganic|-|Manganese(IV)||Mn4+||Manganyl|-|Manganese(VII)||Mn7+|||-|Mercury(II)||Hg2+||Mercuric|-|Nickel(II)||Ni2+||Nickelous|-|Nickel(III)||Ni3+||Nickelic|-|Potassium||K+|||-|Silver||Ag+|||-|Sodium||Na+|||-|Strontium||Sr2+|||-|Tin(II)||Sn2+||Stannous|-|Tin(IV)||Sn4+||Stannic|-|Zinc||Zn2+|||-!colspan="3" style="background-color: aliceblue"|
Polyatomic Cations|-|Ammonium||NH4+|||-|Hydronium||H3O+|||-|Nitronium||NO2+|||-|Mercury(I)||Hg22+||Mercurous|}|valign="top"|{|class="wikitable"|+Common
Anions|-!style="text-align: left"|Formal Name!style="text-align: left"|Formula!style="text-align: left"|Alt. Name|-!colspan="3" style="background-color: aliceblue"|
Simple Anions|-|Arsenide||As3−|||-|Azide||N3−|||-|Bromide||Br−|||-|Chloride||Cl−|||-|Fluoride||F−|||-|Hydride||H−|||-|Iodide||I−|||-|Nitride||N3−|||-|Oxide||O2−|||-|Phosphide||P3−|||-|Sulphide||S2−|||-
|Peroxide||O22−|||-!colspan="3" style="background-color: aliceblue"|
Oxoanions|-|Arsenate||AsO43−|||-|Arsenite||AsO33−|||-|Borate||BO33−|||-|Bromate||BrO3−|||-|Hypobromite||BrO−|||-|Carbonate||CO32−|||-|Hydrogen Carbonate||HCO3−||Bicarbonate|-|Chlorate||ClO3−|||-|Perchlorate||ClO4−|||-|Chlorite||ClO2−|||-|Hypochlorite||ClO−|||-|Chromate||CrO42−|||-|Dichromate||Cr2O72−|||-|Iodate||IO3−|||-|Nitrate||NO3−|||-|Nitrite||NO2−|||-|Phosphate||PO43−|||-|Hydrogen Phosphate||HPO42−|||-|Dihydrogen Phosphate||H2PO4−|||-|Permanganate||MnO4−|||-|Phosphite||PO33−|||-|Sulphate||SO42−|||-|Thiosulphate||S2O32−|||-|Hydrogen Sulphate||HSO4−||Bisulphate|-|Sulphite||SO32−|||-|Hydrogen Sulphite||HSO3−||Bisulphite|-!colspan="3" style="background-color: aliceblue"|
Anions from Organic Acids|-|Acetate||C2H3O2−|||-|Formate||HCO2−|||-|Oxalate||C2O42−|||-|Hydrogen Oxalate||HC2O4−||Bioxalate|-!colspan="3" style="background-color: aliceblue"|
Other Anions|-|Hydrogen Sulphide||HS−||Bisulphide|-|Telluride||Te2−|||-|Amide||NH2−|||-|Cyanate||OCN−|||-|Thiocyanate||SCN−|||-|Cyanide||CN−||
|-|}
|}
See also
External links
- ionic bonding tutorial I
- ionic bonding tutorial II
- ionic bonding tutorial III
s 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
An
ionic bond (or
electrovalent bond) is a type of chemical bond based on electrostatic forces between two oppositely-charged ions. In ionic bond formation, a metal donates an electron, due to a low
electronegativity, to form a positive ion or cation. In ordinary table salt (NaCl), the bonds between the sodium and
chloride ions are ionic bonds. Often ionic bonds form between
metals and non-metals. The non-metal atom has an electron configuration just short of a noble gas structure. They have high electronegativity, and so readily gain electrons to form negative ions or
anions. The two or more ions are then attracted to each other by
electrostatics.
\mathrm{Li + F}\ \ \ \to\ \ \ \mathrm{Li^+F^-}\,\!
\mathrm{3Na + P}\ \ \ \to\ \ \ \mathrm{(Na^+)_3P^{3--->
Ionic bonding occurs 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.
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.
Polarization effects
Ions in
crystal lattices of purely ionic compounds are sphere; however, if the positive ion is small and/or highly charged, it will distort the electron cloud of the negative ion. This Polarization (electrostatics) of the negative ion leads to a build-up of extra charge density between the two atomic nucleus, i.e., to partial covalency. Larger negative ions are more easily polarized, but the effect is usually only important when positive ions with
electrical charge 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).
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 Cubic (crystal system) (where the weight is 4*atomic weight), but, when the ions are different sizes, the structure is often Cubic (crystal system) (2 times the weight). In ionic lattices the coordination number refers to the number of connected ions.
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 close-packing rules.
Electrical conductivity
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.
Substances in ionic form
{||valign="top"|{|class="wikitable"|+Common
Cations|-!style="text-align: left"|Stock System Name!style="text-align: left"|Formula!style="text-align: left"|Historic Name|-!colspan="3" style="background-color: aliceblue"|
Simple Cations|-|Aluminum||Al3+|||-|Barium||Ba2+|||-|Beryllium||Be2+|||-|Caesium||Cs+|||-|Calcium||Ca2+|||-|Chromium(II)||Cr2+||Chromous|-|Chromium(III)||Cr3+||Chromic|-|Chromium(VI)||Cr6+||Chromyl|-|Cobalt(II)||Co2+||Cobaltous|-|Cobalt(III)||Co3+||Cobaltic|-|Copper(I)||Cu+||Cuprous|-|Copper(II)||Cu2+||Cupric|-|Copper(III)||Cu3+|||-|Gallium ||Ga3+|||-|Gold(I)||Au+|||-|Gold(III)||Au3+|||-|Helium||He2+||(Alpha particle)|-|Hydrogen||H+||(Proton)|-|Iron(II)||Fe2+||Ferrous|-|Iron(III)||Fe3+||Ferric|-|Lead(II)||Pb2+||Plumbous|-|Lead(IV)||Pb4+||Plumbic|-|Lithium||Li+|||-|Magnesium||Mg2+|||-|Manganese(II)||Mn2+||Manganous|-|Manganese(III)||Mn3+||Manganic|-|Manganese(IV)||Mn4+||Manganyl|-|Manganese(VII)||Mn7+|||-|Mercury(II)||Hg2+||Mercuric|-|Nickel(II)||Ni2+||Nickelous|-|Nickel(III)||Ni3+||Nickelic|-|Potassium||K+|||-|Silver||Ag+|||-|Sodium||Na+|||-|Strontium||Sr2+|||-|Tin(II)||Sn2+||Stannous|-|Tin(IV)||Sn4+||Stannic|-|Zinc||Zn2+|||-!colspan="3" style="background-color: aliceblue"|
Polyatomic Cations|-|Ammonium||NH4+|||-|Hydronium||H3O+|||-|Nitronium||NO2+|||-|Mercury(I)||Hg22+||Mercurous|}|valign="top"|{|class="wikitable"|+Common
Anions|-!style="text-align: left"|Formal Name!style="text-align: left"|Formula!style="text-align: left"|Alt. Name|-!colspan="3" style="background-color: aliceblue"|
Simple Anions|-|Arsenide||As3−|||-|Azide||N3−|||-|Bromide||Br−|||-|Chloride||Cl−|||-|Fluoride||F−|||-|Hydride||H−|||-|Iodide||I−|||-|Nitride||N3−|||-|Oxide||O2−|||-|Phosphide||P3−|||-|Sulphide||S2−|||-
|Peroxide||O22−|||-!colspan="3" style="background-color: aliceblue"|
Oxoanions|-|Arsenate||AsO43−|||-|Arsenite||AsO33−|||-|Borate||BO33−|||-|Bromate||BrO3−|||-|Hypobromite||BrO−|||-|Carbonate||CO32−|||-|Hydrogen Carbonate||HCO3−||Bicarbonate|-|Chlorate||ClO3−|||-|Perchlorate||ClO4−|||-|Chlorite||ClO2−|||-|Hypochlorite||ClO−|||-|Chromate||CrO42−|||-|Dichromate||Cr2O72−|||-|Iodate||IO3−|||-|Nitrate||NO3−|||-|Nitrite||NO2−|||-|Phosphate||PO43−|||-|Hydrogen Phosphate||HPO42−|||-|Dihydrogen Phosphate||H2PO4−|||-|Permanganate||MnO4−|||-|Phosphite||PO33−|||-|Sulphate||SO42−|||-|Thiosulphate||S2O32−|||-|Hydrogen Sulphate||HSO4−||Bisulphate|-|Sulphite||SO32−|||-|Hydrogen Sulphite||HSO3−||Bisulphite|-!colspan="3" style="background-color: aliceblue"|
Anions from Organic Acids|-|Acetate||C2H3O2−|||-|Formate||HCO2−|||-|Oxalate||C2O42−|||-|Hydrogen Oxalate||HC2O4−||Bioxalate|-!colspan="3" style="background-color: aliceblue"|
Other Anions|-|Hydrogen Sulphide||HS−||Bisulphide|-|Telluride||Te2−|||-|Amide||NH2−|||-|Cyanate||OCN−|||-|Thiocyanate||SCN−|||-|Cyanide||CN−||
|-|}
|}
See also
External links
- ionic bonding tutorial I
- ionic bonding tutorial II
- ionic bonding tutorial III
Ionic Bond
Simple explanation of ionic bond in the framework of the history of the Universe ... Physical Environment > Ionic Bond This site tells the story of the history of the universe
BBC - GCSE Bitesize - Chemistry | Classifying Materials | Ionic ...
Ions are electrically-charged particles formed when atoms lose or gain electrons, and they have the same electronic structures as noble gases. Metal atoms form positive ions and ...
BBC - GCSE Bitesize - Chemistry | Classifying Materials | Ionic ...
When metals react with non-metals, electrons are transferred from the metal atoms to the non-metal atoms, forming ions. The resulting compound is called an ionic compound.
ionic (electrovalent) bonding
Explains how ionic (electrovalent) bonds are formed, starting with a simple view and then extending it for A'level.
Ionic bonding
P rices : Biology (450 slides) : £199, Chemistry (280 slides) : £149, Physics (370 slides) : £179, All 3 CD-ROMS : £449 Order form
Ionic bond - Wikipedia, the free encyclopedia
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 ...
Structure and Bonding: Ionic Bonds
Elements in the first few columns of the periodic table have a few more electrons than predicted by the octet rule: they therefore lose the electrons in the outermost shells fairly ...
Chemistry: Ionic Bonding
Chemistry Learning Resources ... As we have already learned, ionic bonding occurs between metals and non-metals.
1. Classification of Solids
This leads to a direct electrostatic attraction between the ions and is known as ionic bonding. These different forms of bonding are largely responsible for the different thermal ...
Ionic and covalent bonding
Information on ionic and covalent bonding and properties of each and when they occur ... GCSE Chemistry > Ionic and covalent bonding Bonding is the attraction between atoms.
