Difference between revisions of "Ionic Compound"

Latest revision as of 16:17, 13 December 2019

Key Stage 4

Meaning

An ionic compound is a molecule formed from 2 or more elements which have transferred electrons to become ions.

About Ionic Compounds

Ionic compounds form when atoms lose one or more electrons to become a positive ions and other atoms gain electrons to become negative ions. The electrostatic force of attraction between these ions is a strong chemical bond.

Metal elements form positive ions because it is easier for them lose electrons than gain electrons to get a full outer shell. Metals are on the left hand side of the Periodic Table and usually have either 1, 2, 3 or 4 electrons in the Outer Shell.

Group 1 Elements all form +1 ions; Li⁺¹, Na⁺¹, K⁺¹

Group 2 Elements all form +2 ions; Be⁺², Mg⁺², Ca⁺²

Group 3 Elements all form +3 ions; Al⁺³

Transition Metal Elements can form different ions which are shown by Roman Numerals; Iron can form Fe(II) which is Fe⁺² or Fe(III) is Fe⁺³,

Manganese can form Mn (II) which is Mn⁺² or Mn (IV) which is Mn ⁺⁴

Non-metal elements form negative ions because it is easier for them to gain electrons than lose electrons to get a full outer shell. Non-metals are on the right hand side of the Periodic Table and usually have 4, 5, 6, 7 or 8 electrons in their outer shell.

Group 5 Elements all form -3 ions; N^-3, P^-3

Group 6 Elements all form -2 ions; O^-2, S^-2

Group 7 Elements all form -1 ions; F^-1, Cl^-1

Some covalent compounds can form negative ions; Carbonate forms -2 ions CO₃^-2, Sulphate forms -2 ions SO₄^-2, Nitrate forms -1 ions NO₃^-1

Examples


Lithium forms +1 ions.	Magnesium forms +2 ions.	Aluminium forms +3 ions.

Chlorine forms -1 ions.	Oxygen forms -2 ions.	Nitrogen forms -3 ions.

Bulk Properties

In their solid state ionic compounds are poor electrical conductors because the ions are not free to move.

In their liquid state ionic compounds are good electrical conductors because the electrically charged ions are free to move.

Most ionic compounds are soluble in water.

When dissolved in solution ionic compounds are good electrical conductors because the electrically charged ions are free to move.

Ionic compounds form giant ionic structures which have high melting points due to the strong electrostatic force between the ions.

State	Electrical Conductivity	Reason
Solid	Poor	Ions are in fixed positions and not free to move.
Liquid (Molten)	Good	Ions are free to move in the liquid.
Dissolved in Solution (Aqueous)	Good	Ions are free to move through solution.

References

Edexcel

Ionic compounds, page 180, GCSE Combined Science, Pearson Edexcel

Ionic compounds, page 36, GCSE Chemistry, Pearson, Edexcel

Ionic compounds, pages 20-22, GCSE Chemistry; The Revision Guide, CGP, Edexcel

Ionic compounds, pages 49-55, GCSE Chemistry, CGP, Edexcel

Ionic compounds, pages 83-85, GCSE Combined Science; The Revision Guide, CGP, Edexcel

Ionic compounds; properties, pages 38-39, GCSE Chemistry, Pearson, Edexcel

OCR

Ionic compounds, pages 19, 25, 35, Gateway GCSE Chemistry; The Revision Guide, CGP, OCR

Ionic compounds, pages 58-59, 77, 79, 88-89, 122, Gateway GCSE Chemistry, Oxford, OCR

Ionic compounds, pages 90, 91, 97, 108, Gateway GCSE Combined Science; The Revision Guide, CGP, OCR

@@ Line 9: / Line 9: @@
 : [[Group 2]] [[Element]]s all form +2 [[ion]]s; Be<sup>+2</sup>, Mg<sup>+2</sup>, Ca<sup>+2</sup>
 : [[Group 3]] [[Element]]s all form +3 [[ion]]s; Al<sup>+3</sup>
-: [[Transition Metal]] [[Element]]s can form different [[ion]]s which are shown by [[Roman Numeral]]s; Iron can form [[Fe]](II) which is [[Fe]]<sup>+2</sup> or [[Fe]](III) is [[Fe]]<sup>+3</sup>,
+: [[Transition Metal]] [[Element]]s can form different [[ion]]s which are shown by Roman Numerals; [[Iron]] can form [[Iron|Fe(II)]] which is [[Iron|Fe<sup>+2</sup>]] or [[Iron|Fe(III)]] is [[Iron|Fe<sup>+3</sup>]],
-Manganese can form [[Mn]](II) which is [[Mn]]<sup>+2</sup> or [[Mn]](IV) which is [[Mn]]<sup>+4</sup>
+[[Manganese]] can form [[Manganese|Mn (II)]] which is [[Manganese|Mn<sup>+2</sup>]] or [[Manganese|Mn (IV)]] which is [[Manganese|Mn <sup>+4</sup>]]
 : [[Non-metal]] [[element]]s form [[Negative Ion|negative ions]] because it is easier for them to gain [[electron]]s than lose [[electron]]s to get a full [[Outer Shell|outer shell]]. [[Non-metal]]s are on the right hand side of the [[Periodic Table]] and usually have 4, 5, 6, 7 or 8 [[electron]]s in their [[Outer Shell|outer shell]].
@@ Line 41: / Line 41: @@
 ===Bulk Properties===
 : In their [[solid]] [[State of Matter|state]] '''ionic compounds''' are poor [[Electrical Conductor|electrical conductors]] because the [[ion]]s are not free to move.
-: In their [[liquid]] [[State of Matter|state]] '''ionic compounds''' are good [[Electrical Conductor|electrical conductors]] because the [[Charge|electrically charged]] [[ion]]s are free to move.
+: In their [[liquid]] [[State of Matter|state]] '''ionic compounds''' are good [[Electrical Conductor|electrical conductors]] because the [[Electrical Charge|electrically charged]] [[ion]]s are free to move.
 : Most '''ionic compounds''' are [[soluble]] in [[water]].
-: When [[dissolve]]d in [[solution]] '''ionic compounds''' are good [[Electrical Conductor|electrical conductors]] because the [[Charge|electrically charged]] [[ion]]s are free to move.
+: When [[dissolve]]d in [[solution]] '''ionic compounds''' are good [[Electrical Conductor|electrical conductors]] because the [[Electrical Charge|electrically charged]] [[ion]]s are free to move.
 : '''Ionic compounds''' form [[Giant Ionic Structure|giant ionic structures]] which have high [[Melting Point|melting points]] due to the strong [[Electrostatic Force|electrostatic force]] between the [[ion]]s.
+{| class="wikitable"
+|-
+| style="height:20px; width:200px; text-align:center;" |'''State'''
+| style="height:20px; width:200px; text-align:center;" |'''Electrical Conductivity'''
+| style="height:20px; width:200px; text-align:center;" |'''Reason'''
+|-
+| style="height:20px; width:200px; text-align:center;" |Solid
+| style="height:20px; width:200px; text-align:center;" |Poor
+| style="height:20px; width:200px; text-align:center;" |[[Ion]]s are in fixed positions and not free to move.
+|-
+| style="height:20px; width:200px; text-align:center;" |Liquid (Molten)
+| style="height:20px; width:200px; text-align:center;" |Good
+| style="height:20px; width:200px; text-align:center;" |[[Ion]]s are free to move in the [[liquid]].
+|-
+| style="height:20px; width:200px; text-align:center;" |Dissolved in Solution (Aqueous)
+| style="height:20px; width:200px; text-align:center;" |Good
+| style="height:20px; width:200px; text-align:center;" |[[Ion]]s are free to move through [[solution]].
+|}
+===References===
+====Edexcel====
+:[https://www.amazon.co.uk/gp/product/1292120193/ref=as_li_tl?ie=UTF8&camp=1634&creative=6738&creativeASIN=1292120193&linkCode=as2&tag=nrjc-21&linkId=572df39392fb4200db8391d98ae6314e ''Ionic compounds, page 180, GCSE Combined Science, Pearson Edexcel '']
+:[https://www.amazon.co.uk/gp/product/1292120215/ref=as_li_tl?ie=UTF8&camp=1634&creative=6738&creativeASIN=1292120215&linkCode=as2&tag=nrjc-21&linkId=8f96ddb76196848bafdb124354e4cf77 ''Ionic compounds, page 36, GCSE Chemistry, Pearson, Edexcel '']
+:[https://www.amazon.co.uk/gp/product/1782945725/ref=as_li_tl?ie=UTF8&camp=1634&creative=6738&creativeASIN=1782945725&linkCode=as2&tag=nrjc-21&linkId=694be7494de75af3349537d34e13f7f0 ''Ionic compounds, pages 20-22, GCSE Chemistry; The Revision Guide, CGP, Edexcel '']
+:[https://www.amazon.co.uk/gp/product/1782948147/ref=as_li_tl?ie=UTF8&camp=1634&creative=6738&creativeASIN=1782948147&linkCode=as2&tag=nrjc-21&linkId=f63dcd8345f4e49c717b39a228a36c7c ''Ionic compounds, pages 49-55, GCSE Chemistry, CGP, Edexcel '']
+:[https://www.amazon.co.uk/gp/product/1782945741/ref=as_li_tl?ie=UTF8&camp=1634&creative=6738&creativeASIN=1782945741&linkCode=as2&tag=nrjc-21&linkId=30da4f2178da182547b62a7329d13b57 ''Ionic compounds, pages 83-85, GCSE Combined Science; The Revision Guide, CGP, Edexcel '']
+:[https://www.amazon.co.uk/gp/product/1292120215/ref=as_li_tl?ie=UTF8&camp=1634&creative=6738&creativeASIN=1292120215&linkCode=as2&tag=nrjc-21&linkId=8f96ddb76196848bafdb124354e4cf77 ''Ionic compounds; properties, pages 38-39, GCSE Chemistry, Pearson, Edexcel '']
+====OCR====
+:[https://www.amazon.co.uk/gp/product/1782945679/ref=as_li_tl?ie=UTF8&camp=1634&creative=6738&creativeASIN=1782945679&linkCode=as2&tag=nrjc-21&linkId=a2db42f7b4bdf10cafaafa3bb9120940 ''Ionic compounds, pages 19, 25, 35, Gateway GCSE Chemistry; The Revision Guide, CGP, OCR '']
+:[https://www.amazon.co.uk/gp/product/0198359829/ref=as_li_tl?ie=UTF8&camp=1634&creative=6738&creativeASIN=0198359829&linkCode=as2&tag=nrjc-21&linkId=90e8d7b4f039d53035238fa0320fe00b ''Ionic compounds, pages 58-59, 77, 79, 88-89, 122, Gateway GCSE Chemistry, Oxford, OCR '']
+:[https://www.amazon.co.uk/gp/product/1782945695/ref=as_li_tl?ie=UTF8&camp=1634&creative=6738&creativeASIN=1782945695&linkCode=as2&tag=nrjc-21&linkId=ceafcc80bcad6b6754ee97a0c7ceea53 ''Ionic compounds, pages 90, 91, 97, 108, Gateway GCSE Combined Science; The Revision Guide, CGP, OCR '']