Ions and its classification

 

IONS

 

1.Ions are charged atoms or molecules. (or)

2.Ions are charged chemical species.(or)

3.Atom or group of atoms which are having charge on it are called as Ions.

4.Basically ionic compounds are made up of ions.

5.Ionic compounds are dissolved in polar or ionic liquids(solvents).

6.Ionic compounds are crystalline solids in nature.

7.The melting and boiling points of ionic compounds are very high.

8.Attracted to oppositely charged ions, repelled by similar charges.

9.Conduct electricity in solutions or molten states (electrolytes).

 

Examples:

table salt-sodium chloride-NaCl will form sodium Na⁺ ion and Cl⁻ chloride ion in water.

 

Formation of ions:

Ions are formed due to the unequal number of protons and electrons in an atom of an element or a chemical species.It is happening

1.by the loss of electrons

2.by the gain of electrons

Due to loss of electrons, an atom is forming positively charged chemical species(cations).

Example:

Na element has 11electrons(-11)= 11protons (11+)so that the total charge on it is “0(zero)”.

But when it loose it's 1 electron from the last shell,it has 10electrons(-10)= 11protons (11+) due to unequal number of electrons and protons the Na element gets Na¹⁺ ion.

Due to gain of electrons, an atom is forming negatively charged chemical species (anions).

Example:

Cl element has 17electrons(-17)= 17protons (17+)so that the total charge on it is “0(zero)”.

But when it gains 1 electron from other element,it has 18electrons(-18)= 17protons (17+) due to unequal number of electrons and protons the Cl element gets Cl⁻anion.

 

Reason for formation of ions:

1.Noble gases are the elements which are present in 18th group(vertical column) in periodic table.

2.These elements are always having 8 electrons in their valency shell.(except Helium -1S²)And this ns²np⁶ (8 electrons in their valency shell) is called as "octet configuration".So that these elements are stable in nature(not reactive-lazy-inert gases).

3.To get this stability all the other elements are ready to lose or gain or share their valency electrons.

5.In the case of ions, some elements will lose or gain electrons to form cations or anions.

Classification of Ions:

I.Based on type of charge:

Ions are classified into 2 types:

1. Positive ions(cations):

The atom or group of atoms which is having positive charge on it.

The ions which are having positive charge on them.

The positive ions are also called as Cations.

 

2. Negative ions(anions):

The atom or group of atoms which is having Negative charge on it.

The ions which are having Negative charge on them.

The Negative ions are also called as anions.

 

II.Based on number of atoms in them:

Ions are classified into 2 types:

 

1. Simple ions:

Simple ions are charged particles formed from a single atom that has gained or lost electrons.

Single atom which is having charge on it.

Examples:

Sodium ion (Na⁺),

potassium ion(K⁺)

calcium ion (Ca²⁺),

magnesium ion (Mg²⁺),

Aluminium ion(Al⁺³)

Stannic ion(Sn⁴⁺)

chloride ion(Cl⁻),

Oxide ion(O⁻²),

Phosphide ion(P⁻³)

 etc.

2. Compound ions:

A compound ion is a group of two or more atoms that are having charge on it.

The ions which are having 2 or more number of atoms in them.

Examples:

ammonium (NH₄⁺),

sulfate (SO₄²⁻),

nitrate (NO₃⁻),

hydroxide (OH⁻),

carbonate (CO₃²⁻) etc

 

III.Based on number of unit of charge on them:

Ions are classified into 4 types:

 

1.Monovalent positive/negative ions:

The ions which are having 1 unit of positive or negative charge on it.

Example:

ammonium (NH₄⁺),

Sodium ion (Na⁺),

potassium ion(K⁺) etc

 

nitrate (NO₃⁻),

hydroxide (OH⁻), etc

 

 

 

2.Di/Bivalent positive/negative ions:

The ions which are having 2 units of positive or negative charge on it.

Examples:

calcium ion (Ca²⁺),

magnesium ion (Mg²⁺),

Zinc ion(Zn⁺²) etc

 

sulfate (SO₄²⁻),

carbonate (CO₃²⁻) etc

 

3.Trivalent positive/negative ions:

The ions which are having 3 units of positive or negative charge on it.

Examples:

Aluminium ion(Al⁺³)

Chromic ion(Cr⁺³)

Cobaltous ion(Co⁺³) etc

Phosphate (PO₄³⁻)

Nitride (N³⁻)

Borate (BO₃³⁻) etc

 

 

4.Polyvalent positive/negative ions:

The ions which are having more than 3 units of positive or negative charge (+4 to +8) or (-4 to -8)on it.

Examples:

Stannic ion(Sn⁴⁺)

Antimonous ion(Sb⁺⁵)

Arsenous ion(As⁺⁵) etc

 

Carbide ion(C⁻⁴)

[Fe(CN)6]⁴⁻ etc

List of IONS

 

 

1.CATIONS(POSITIVE IONS)

        name of cation-   symbol/formula

 

1. Hydrogen ion - H⁺
2. Lithium ion -     Li⁺
3. Sodium cation -    Na⁺
4. Potassium cation -K⁺
5. Rubidium -            Rb⁺
6. Cesium -               Cs⁺
7. Magnesium ion -  Mg²⁺
8. Calcium ion -        Ca²⁺
9. Zinc ion -              Zn²⁺
10. Barium ion-          Ba²⁺
11. Cadmium ion-      Cd²⁺
12. Nickel ion-            Ni²⁺
13. Aluminium ion-.    Al⁺³
14. Ferrous ion -        Fe²⁺
15. Ferric ion -           Fe³⁺
16. Cuprous ion-       Cu⁺
17. Cupric ion-          Cu²⁺
18. (Silver)Argentous ion-Ag⁺
19. Argentic ion-        Ag⁺²
20. Stannous ion -    Sn²⁺
21. Stannic ion-         Sn⁴⁺
22. (Gold)Aurous ion-Au⁺
23. Auric ion-            Au³⁺
24. Ammonium ion-  NH₄⁺
25. Nitronium ion-     NO₂⁺
26. Hydronium ion-   H₃O⁺
27. Platinnous ion-    Pt²⁺
28. Platinnic ion-       Pt⁴⁺
29. Plumbous ion-     Pb⁺²
30. Plumbic ion-        Pb⁺⁴
31. Mangannous ion-Mn²⁺
32. Mangannic ion-  Mn⁺³
33. Chromous ion-   Cr²⁺
34. Chromic ion-      Cr⁺³
35. Cobaltous ion-   Co²⁺
36. Cobaltic ion-      Co⁺³
37. Antimonous ion-Sb⁺³
38. Antimonic ion-  Sb⁺⁵
39. Arsenious ion-  As⁺³
40. Arsenic ion-      As⁺⁵
41. Beryllium ion-   Be²⁺
42. Carbon ion-      C⁺⁴
43. Mercurous ion- Hg⁺¹
44. Mercuric ion-    Hg²⁺

 

2.ANIONS(NEGATIVE IONS)

        name of anion-   symbol/formula

1. Hydride ion - H⁻
2. Fluoride ion -         F⁻
3. Cloride ion  -         Cl⁻
4. Bromide ion-          Br⁻
5. Iodide ion   -           I⁻
6. Oxide ion-              O²⁻
7. Peroxide ion  -       O₂²⁻
8. Superoxide ion -    O₂⁻
9. Ozonide ion-          O₃⁻
10. Hydroxide ion -     OH⁻
11. Sulfide ion  -          S²⁻
12. Sulfate  ion  -        SO₄²⁻
13. BiSulfate ion -       HSO₄⁻
14. Sulfite ion -            SO₃²⁻
15. Biulfite ion-           HSO₃⁻
16. Nitride ion-             N³⁻
17. Nitrate ion-             NO₃⁻
18. Nitrite ion-              NO₂⁻
19. Phosphide ion-          P³⁻
20. Phosphate ion-       PO₄³⁻
21. Biphosphate ion-   HPO₄²⁻
22. Phosphite ion -        PO₃³⁻
23. Bihosphite ion -     HPO₃²⁻
24. Carbide ion-              C⁴⁻
25. Cyanide ion-            CN⁻
26. Thiocyanate ion-     SCN⁻
27. Cyanate ion-           CNO⁻
28. Carbonate ion-        CO₃²⁻
29. Bicarbonate ion-     HCO₃⁻
30. Chromate ion-        CrO₄²⁻
31. Dichromate ion-     Cr₂O₇²⁻
32. Permanganate ion-MnO₄⁻
33. Manganate ion-     MnO₄⁻²
34. Acetate ion-         CH₃COO⁻
35. Formate ion-         HCOO⁻
36. Oxalate ion-           C₂O₄²⁻
37. Iodate ion-               IO₃⁻
38. Borate ion-             BO₃³⁻
39. Chlorate ion-          ClO₃⁻
40. Perchlorate ion-     ClO₄⁻
41. Hypochlorite ion-    ClO⁻
42. Silicate ion-            SiO₃⁻²
43. Ferrocynide ion-   [Fe(CN)₆]⁴⁻
44. Ferricynide ion-   [Fe(CN)₆]³⁻