Question

Arrange the oxides Al2O3, B2O3, CO2, Cl2O7, SO3 in order from the most acidic through amphoteric to most basic. Give explanation also.

Answer 1

Answer:

Explanation:

if you see this all are non metals

so acidic oxides are formed

i list some amphoteric oxides

sno,pbo,zno,al2o3,cuo,be2o

and by oxidation number you can find remaining

if you see b2o3

oxidation number is 3

so basic oxide

if you see

co2

oxidation number is 4

so amphoteric

if you see cl2o7

oxidation no. is 7

so acidic oxide

if you see so3

oxidation number is 6

so acidic oxide

Answer 2

Answer:

Most acidic oxides:  SO₃, Cl₂O₇,

Amphoteric oxides: Al₂O₃

Slightly acidic oxides: B₂O₃, CO₂

Explanation:

• Al₂O₃ is amphoteric in nature. It can react with both with acids as well as bases.

                  $Al_{2}O_{3} + 6HCl$   →   $2AlCl_{3} + 3H_{2}O$

                $Al_{2}O_{3} + 2NaOH + 3H_{2}O$  → $2Na[Al(OH)_{4}]$

• B₂O₃ is weakly acidic in nature. They react with alkalies:

                 $B_{2}O_{3}+2NaOH$  →  $2NaBO_{2}$  + $H_{2}O$

• CO₂ behaves as weak acid. It dissolves in water gives carbonic acid.

              $CO_{2}+H_{2}O$  ⇄  $H_{2}CO_{3}$

• Cl₂O₇ is very strongly acidic. It reacts with water forming perchloric acid.

                $Cl_{2}O_{7}+H_{2}O$   →  $2HClO_{4}$

• SO₃ is strongly acidic. It dissolves readily and exothermically in water to form sulphuric acid.

                 $SO_{3}+H_{2}O$    →  $H_{2}SO_{4}$ + Heat