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| − | An '''ionic bond''' can be formed after two or more [[atoms]] lose or gain [[electron]]s to form an [[ion]]. Ionic bonds occur between [[metal]]s, losing electrons, and [[non-metal]]s, gaining electrons. Ions with opposite [[charge]]s will attract one another creating an ionic bond. Such bonds are stronger than [[hydrogen bond]]s, but similar in strength to [[covalent bond]]s.
| + | #Redirect[[Chemical_bond#The_Ionic_Bond]] |
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| − | <!-- The \,\! are to keep the formulae rendered as PNG instead of HTML. Please don't remove them.—>
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| − | : <math>Li + F\ \ \ \to\ \ \ Li^+F^-\,\!</math>
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| − | : <math>3Na + P\ \ \ \to\ \ \ Na^+_3P^{3-}</math>
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| − | It only occurs if the overall energy change for the reaction is favourable (the bonded atoms have a lower energy than the free ones). The larger the energy change the stronger the bond.
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| − | ''Pure'' ionic bonding doesn't actually happen with real atoms. All bonds have a small amount of [[covalent bond|covalency]]. The larger the difference in [[electronegativity]] the more ionic the bond.
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| − | <table align="right" width="70%" cellpadding ="10" border="1">
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| − | <tr><td>[[Image:Ionic bonding.png]]</td> <td align="middle">[[image:ionicbond.JPG]]</td></tr>
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| − | <tr><td> <font face="Arial" size=1>
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| − | The diagram above shows the electron configurations of lithium and fluorine. Note that lithium has one electron in its outer shell. This electron is held rather loosely (''because the ionisation energy is very different in the two ions''). Note also that fluorine has 7 electrons in its outer shell. If the electron moves from lithium to fluorine each ion acquires the configuration of a [[noble gas]]. The bonding energy (from the [[electrostatic attraction]] of the two oppositely charged ions) is large enough (negative value) that the overall bonded state energy is lower than the unbonded state.
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| − | </font></td>
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| − | <td><font face="Arial" size=1>
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| − | Impression of two ions (for example [Na]<sup>+</sup> and [Cl]<sup>-</sup>) forming an ionic bond. [[Electron orbital]]s generally do not overlap (ie. [[molecular orbital]]s are not formed), because each of the ions reached the lowest [[energy state]], and the bond is based only (ideally) on the electrostatic interactions between positive and negative ions.
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| − | </font></td></tr>
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| − | </table>
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| − | ==Difference between ionic and covalent bonds==
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| − | 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 geometry around each atom is determined by [[VSEPR]] rules, whereas in ionic materials, the geometry follows maximum packing rules. Thus, a compound can be classified as ionic or covalent based on the geometry of the atoms.
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| − | {{chem-stub}}
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| − | [[de:Ionische Bindung]]
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| − | [[et:Iooniline side]]
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| − | [[es:Enlace iónico]]
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| − | [[fr:Liaison ionique]]
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| − | [[it:Legame ionico]]
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| − | [[he:קשר יוני]]
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| − | [[nl:Ionaire binding]]
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| − | [[ja:イオン結合]]
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| − | [[nn:Ionebinding]]
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| − | [[pt:Ligação iônica]]
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| − | [[sl:Ionska vez]]
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| − | [[fi:Ionisidos]]
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| − | [[th:พันธะไอออน]]
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| − | [[zh:离子键]]
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| − | {{Natural sciences-footer}}
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| − | {{Credit|24707153}}
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