Question

How acid base behaviour of oxides period 3 depend upon structure of oxides(, giant to simple)
???? please i need answer​

Answer 1

Answer:

It continues the trend of the highest oxides of the Period 3 elements towards being stronger acids. Chlorine(VII) oxide reacts with water to give the very strong acid, chloric(VII) acid - also known as perchloric acid. The pH of typical solutions will, like sulphuric acid, be around 0.

Answer 2

In the periodic table the period three contains element in the left hand side that are strong basic oxides and the ones on the right are strong acidic ones and aluminum(amphoteric) oxide are present in the middle.

The amphoteric oxide in the middle shows both acidic and basic properties.

The period three contains the following oxides

• Na2O
• MgO
• Al2O3
• SiO2
• P4O10
• SO3
• Cl2O7
• P4O6
• SO2
• Cl2O

• The strong basic oxides contain oxide ions whereas the acidic ones do not contain them as the electronegativity increases as we move from left to right and it is difficult to form ionic bonds.
• Electronegativity is the tendency of atom to attract the bonding pair of electrons.
• The first three have metallic properties, silicon is a giant covalent and the rest are simple molecules.
• The metallic bonds are strong in nature and the atoms are tightly packed together.
• Silicon is held together by strong covalent bonds.
• The simple molecules contain covalent bonds held together apart from Argon.