The formula of zinc nitrate is:

(A) Zn(NO2)3

(B) Zn(NO2)2

(C) Zn(NO3)3

(D) Zn(NO3)2

The correct formula for zinc nitrate is (D) Zn(NO3)2. Let’s break down why this is the case and understand the components involved in forming this compound.

Understanding Zinc Nitrate

Zinc nitrate is an inorganic compound that consists of zinc ions and nitrate ions. To grasp the formula, we need to look at the charges of these ions and how they combine to form a neutral compound.

Components of Zinc Nitrate

• Zinc Ion (Zn²⁺): Zinc typically has a +2 charge when it forms ionic compounds.
• Nitrate Ion (NO3⁻): The nitrate ion carries a -1 charge. Each nitrate ion consists of one nitrogen atom bonded to three oxygen atoms.

Combining the Ions

To create a neutral compound, the total positive charge must balance the total negative charge. Since the zinc ion has a +2 charge, it will need two nitrate ions, each with a -1 charge, to achieve neutrality. This leads us to the following combination:

• 1 Zinc ion (Zn²⁺) = +2 charge
• 2 Nitrate ions (2 x NO3⁻) = -2 charge

When you combine these, the charges balance out perfectly, resulting in the formula Zn(NO3)2.

Why the Other Options are Incorrect

Let’s briefly examine the other options to clarify why they do not represent zinc nitrate:

• (A) Zn(NO2)3: This formula suggests three nitrite ions (NO2⁻), which is not the correct ion for zinc nitrate.
• (B) Zn(NO2)2: Similar to option A, this involves nitrite ions instead of nitrate ions.
• (C) Zn(NO3)3: This would imply three nitrate ions, which would require a +3 charge from zinc, which is not typical for zinc.

Real-World Applications

Zinc nitrate is used in various applications, including fertilizers, as a mordant in dyeing, and in the production of other zinc compounds. Understanding its correct formula is essential for anyone working in chemistry or related fields.

In summary, the correct formula for zinc nitrate is Zn(NO3)2, as it accurately reflects the balance of charges between zinc and nitrate ions. This knowledge is fundamental in both academic and practical chemistry settings.