The empirical formula for copper(II) nitrite is O Cu(NO2)2 CUNO2 O CO(NO2)2 CO2NO2
The Correct Answer and Explanation is :
The correct empirical formula for copper(II) nitrite is Cu(NO₂)₂.
Explanation
- Understanding the Components:
- Copper(II) indicates that copper has a charge of +2.
- Nitrite is a polyatomic ion with the formula NO₂⁻ and a charge of -1.
- Balancing Charges:
- Since copper has a +2 charge and each nitrite ion has a -1 charge, two nitrite ions are needed to balance the charge of one copper ion.
- This results in the compound Cu(NO₂)₂, where the charges balance to zero.
- Empirical Formula:
- The empirical formula represents the simplest whole-number ratio of atoms in a compound.
- In this case, the ratio of copper to nitrite is already in its simplest form: 1:2.
- Therefore, the empirical formula is Cu(NO₂)₂.
- Why Other Options Are Incorrect:
- O Cu(NO₂)₂: The “O” at the beginning is redundant and incorrect.
- CUNO₂: This implies a different chemical composition, which does not reflect the presence of two nitrite ions.
- CO(NO₂)₂: This suggests carbon monoxide bonded to two nitrite ions, which is incorrect for copper(II) nitrite.
- CO₂NO₂: This represents a different compound entirely, not related to copper(II) nitrite.
- Key Chemical Characteristics:
- Copper(II) nitrite is typically a coordination compound where the copper ion is surrounded by nitrite ions.
- It is an ionic compound, consisting of positively charged copper(II) cations and negatively charged nitrite anions.
Understanding the empirical formula requires analyzing the charges and ensuring the total charge of the compound equals zero. Cu(NO₂)₂ satisfies this requirement and accurately reflects the composition of copper(II) nitrite.