An aluminum ion has a charge of +3, and an oxide has a charge of -2. What would be the product of a reaction between these two elements

The product of the reaction between  aluminium ion with a charge of +3, and an oxide with a charge of -2 is Al₂O₃ .

The aluminium ion has a charge of +3 and the oxide has a charge of -2. The product of there reaction can be explained below.

The simple technique use here is exchanging the charges. The aluminium is a cation(positive charge) and it has a positive charge of 3.  The oxygen is an anions(negative charge) and it has a negative charge of negative 2.

For the combined product to be electronically neutral, the 2 aluminium atom has to donate 3 of its outer electrons to the 3 oxygen atoms. This kind of bonding is called ionic or electrovalent bonding

Therefore, the product formed will be as follows:

Al³⁺ + 0²⁻ → Al₂O₃

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The product of a reaction between these two elements is .

Explanation:

The oxidation state of an ion in a compound is equal to its charge.

The aluminum having a charge of +3 because oxidation state is +3

The oxide is having charge of -2

The product of these reactants will produce a chemical compound.

The compound formed is  i.e Aluminium oxide. The compound while getting formed will share the charge and cation A+ will have the charge of anion and anion will have the charge of cation. This will result in a compound as there should be a neutral charge on the compound formed.

The +3 charge of the cation Al+ will go to anion oxide O2- and the charge of anion -2 will go with cation Al+.

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in 1783 cavendish was working with his hydrogen gas and found that when he burned it and condensed the vapor it was water. this was very significant since it disproved the greek theory of elements completely since water was not a simple substance but the product of two gases. it was lavoisier who hearing of the experiment gave cavendish's gas the name hydrogen ("water-producer") and added that hydrogen burned by combining with oxygen and that water was a hydrogen-oxygen combination.

explanation: