Question #41f77

2 Answers
Nov 15, 2015

Answer:

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.

Nov 15, 2015

Answer:

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.