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Home Acid Base CO₂ in Ocean Electronegetivity Electron affinity Ionic charge Ionisation energy N₂ cycle Metal Extracting Molecular geometry Photographic Chem. Polyatomic ions Practical Ptable Reactivity series Reactions Std Re Potential Strange Reac. Titration

H (o-o)
Hydride H^-

Li
⁺

Be
²⁺
Beryl

B
^{3+, 3-}
Borax

N (o-o)
Nitride
^3-

O (o-o)
Oxide
^2-

F (o-o)
Fluoride
^1-

Na
⁺

Mg
²⁺
Dolomite

Al
³⁺
Bauxite

Si
⁴⁺
Quartz

P
Phosphide
^3-

S
Sulfide
^2-

Cl (o-o)
Chloride
^1-

Ca
²⁺
Limestone

Sc
⁺⁺⁺

Ti
⁴⁺

V
^{3+, 4+, 5+}

Cr
^{2+, 3+}

Mn
^{2+, 3+}

Fe
^{2+, 3+}
Bog ore

Co
^{2+, 3+}

Ni
^2+,3+

Cu
^{+, 2+}
Malachite

Zn
⁺⁺

Ga
³⁺

As
^{3-, 3+, 5+}

Se
Selenide
^2-

Br (o-o)
Bromide
^1-

Rb
⁺

Sr
²⁺

Y
⁺⁺⁺

Ag
⁺

Cd
⁺⁺

In
³⁺

Sn
^{2+, 4+}
Cassiterite

Te
^{2-, 2+, 4+, 6+}

I (o-o)
Iodide
^1-

Cs
⁺

Ba
²⁺

Au
^{+, 3+}

Hg
²⁺

Pb
^{2+, 4+}
Cerussite

Bi
³⁺

Oxygen (O)

Potassium Chlorate (KClO₃) and Manganese Dioxide (MnO₂) is heated together to
produce Oxygen in labs.

2KClO₃ + MnO₂ ---> 2KCl + 3O₂

Without MnO₂, potassium chlorate requires heating to around 400�500�C to decompose. With MnO₂, this temperature drops significantly, sometimes to below 200�C, making the process faster and more energy-efficient.