Question

What is the empirical formula for magnesium oxide?

Answer 1

Hint: We need to know that empirical formula for any molecule is used to represent the number of atoms present and the type of atom in the molecule. There are generally two types of formula used to identify a molecule. One is Empirical Formula and one is Molecular Formula.

 Complete answer:
We also remember that the empirical Formula is defined as the simplest form of representing a compound. It is calculated using weight percentages of elements present in the compound. It represents the simplest ratio for the atoms present in the molecule. Molecular formula is also calculated using empirical formula itself for a compound. Thus, molecular formula is a multiple of empirical formula.
Molecular formula is related to the total weight of the molecular entity.
An oxide is formed when an element reacts with oxygen. Oxide is the dianion of oxygen. They are called binary compounds of oxygen. Oxygen has a valency $ - 2$ hence the element present will get a subscript $2$ making it a binary compound.
Magnesium oxide is formed when Magnesium reacts with oxygen.
The word equation can be written as,
Magnesium +Oxygen → Magnesium oxide
By using the cross method of valency we can calculate the empirical formula
As we know Magnesium is a metal so it has a \[ + 2\] valency whereas oxygen has $ - 2$ valency.
Hence we have

$M{g^{2 + }} + {O^{2 - }} \to MgO$
The subscript of oxygen and magnesium gets cancelled by each other and the formula becomes $MgO$.

 Note:
We must have to know that the oxygen forms oxides with metals and non-metals. The oxides can be acidic, basic or amphoteric in nature. Generally metallic oxides are basic in nature whereas non-metallic oxides are acidic in nature. Amphoteric oxides are those oxides which are basic as well acidic in nature.