Question

Question #41f77

Answer 1

The most common oxide of aluminum is `Al_2O_3`.

Explanation:

An oxide is a binary compound with oxygen and another element (in this case, aluminum).

Oxygen typically has a charge of `-2` since it likes to gain `2` electrons to fill its valence shell. Aluminum commonly has a charge of `+3` since it likes to lose `3` electrons to reach noble gas configuration.

In order for the compound to form, there needs to be the same amount of electrons gained and lost, so there needs to be a common multiple of electrons either gained or lost on each side: `6`.

Since oxygen has a `-2` charge, it will be denoted as `O_3`, showing that there are `3` oxygen atoms total, which will gain `6` electrons in all. Aluminum's `+3` charge means it will be in the compound in the form `Al_2`, since the `2` aluminum atoms will donate `3` electrons each, `6` total.

The two elements in the compound will be written together, starting with the more metallic element, or the element further left on the periodic table: `Al_2O_3`.

Because `Al` sometimes forms `+1` ions so that it will still have a full `2s` subshell, and for other exceptions, aluminum(`I`) oxide (`AlO`) and aluminum(`II`) oxide (`Al_2O`) also form, but they only do so very rarely.

Answer 2

Al2O3

Explanation:

Al has oxidation state +3 and Oxygen has -2 i.e `Al^+3 , O^-2`. By combining the oxidation state are cross multiplied.