Writing Ionic Formulae |
Key Concepts |
- Positively charged ions are called cations
- Negatively charged ions are called anions
- The formula of an ionic compound represents the simplest whole number ratio of ions present.
- The net charge on an ionic compound is zero, so the sum of the positive charges equals the sum of the negative charges.
- A subscript number written to the right of an element's symbol tells us how many of those ions are present in the formula.
for example: potassium sulfide has the formula K2S, 2 potassium ions (K+) and 1 sulfide ion (S2-) are present.
If no number is given, then only one of that ion is present.
for example: sodium hydride has the formula NaH, 1 sodium ion (Na+) and 1 hydride ion (H+) are present.
- If more than one polyatomic ion (ion having more that one element in its formula) is present, round brackets enclose the formula of the polyatomic ion and a subscript number written to the right of the final bracket tells us how many of that polyatomic ion are present in the formula.
for example, the nitrate ion is a polyatomic ion, NO3-, it is an ion containing nitrogen and oxygen atoms. Calcium nitrate has the formula Ca(NO3)2 and it contains 1 calcium ion (Ca2+) and 2 nitrate ions (NO3-).
| Type of Ion |
Charge |
Examples |
|---|
| CATIONS |
+1 |
Group I ions (Li+, Na+, K+, Rb+, Cs+)
Ag+, H+, NH4+[amminium], Cu+[copper (I)], Hg22+[mercury(I)] |
|---|
|
| +2 |
Group II ions (Be2+, Mg2+, Ca2+, Sr2+, Ba2+)
Zn2+, Cu2+[copper (II)], Fe2+[iron (II)], Pb2+[lead (II)], Sn2+[tin (II)], Hg2+[mercury (II)] |
|
| +3 |
Al3+, Fe3+[iron (III)] |
|
| +4 |
Pb4+[lead(IV)], Sn4+[tin(IV)] |
| |
|---|
| ANIONS |
-1 |
Group VII ions (F-[fluoride], Cl-[chloride], Br-[bromide], I-[iodide])
H-[hydride], OH-[hydroxide], NO3-[nitrate], NO2-[nitrite] |
|---|
|
| -2 |
Group VI ions (O2-[oxide], S2-[sulfide])
SO42-[sulfate], SO32-[sulfite], CO32-[carbonate] |
|
| -3 |
N3-[nitride], P3-[phosphide], PO43-[phosphate] |
Examples
Charge on Cation EQUALS Charge on Anion
magnesium oxide
- CATION: magnesium (Group II) charge is +2: Mg2+
- ANION: oxide ion (Group VI) charge is -2: O2-
- 1 Mg2+ cation and 1 O2- anion combine to give a compound with zero net charge,
+2 + -2 = 0
- Formula of magnesium oxide is MgO
ammonium hydroxide
- CATION: ammonium ion, charge is +1: NH4+
- ANION: hydroxide ion, charge is -1: OH-
- 1 NH4+ cation and 1 OH- anion combine to give a compound with zero net charge,
+1 + -1 =0
- Formula of ammonium hydroxide is NH4OH
Charge on Cation DOES NOT EQUAL Charge on Anion
aluminium chloride
- CATION: aluminium (Group III), charge is +3: Al3+
- ANION: chloride (Group VII), charge is -1: Cl-
- 1 Al3+ cation and 3 Cl- anions combine to give a compound with zero net charge:
+3 + (3 x -1) = 0
- Formula of aluminium chloride is AlCl3
sodium oxide
- CATION: sodium (Group I), charge is +1: Na+
- ANION: oxide (Group VI), charge is -2: O2-
- 2 Na+ cations and 1 O2- anion combine to give a compound with zero net charge:
(2 x -1) + -2 = 0
- Formula of sodium oxide is Na2O
ammonium sulfate
- CATION: ammonium, charge is +1: NH4+
- ANION: sulfate, charge is -2: SO42-
- 2 NH4+ cations and 1 SO42- anion combine to give a compound with zero net charge:
(2 x -1) + -2 = 0
- Formula of ammonium sufate is (NH4)2SO4
barium hydroxide
- CATION: barium (Group II), charge is +2: Ba2+
- ANION: hydroxide, charge is -1: OH-
- 1 Ba2+ cation and 2 OH- anions combine to give a compound with zero net charge:
+2 + (2 x -1) = 0
- Formula of barium hydroxide is Ba(OH)2
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