What is the simplest formula for copper (II) nitride
The Correct Answer and Explanation is:
The simplest formula for copper (II) nitride is Cu₃N₂.
Explanation:
To understand how we arrive at the formula Cu₃N₂ for copper (II) nitride, we need to consider the oxidation states of copper and nitrogen, and how they combine to form a neutral compound.
- Oxidation State of Copper:
Copper (II) nitride contains copper in the +2 oxidation state. This means each copper (Cu) atom has lost two electrons, resulting in a charge of +2. This is denoted as Cu²⁺. - Oxidation State of Nitrogen:
Nitrogen typically forms nitride (N³⁻) in ionic compounds. In nitride, nitrogen has an oxidation state of -3. - Balancing Charges:
In an ionic compound, the total positive charge must balance the total negative charge to make the compound neutral. Therefore, we need to determine the ratio of copper (Cu²⁺) ions to nitride (N³⁻) ions.
- Each Cu²⁺ ion has a charge of +2.
- Each N³⁻ ion has a charge of -3. To balance these charges, we need multiples of copper and nitrogen such that their total charges equal zero.
- Let’s say we have 3 copper ions (each with a +2 charge) and 2 nitrogen ions (each with a -3 charge):
- 3 copper ions × (+2 charge) = +6
- 2 nitrogen ions × (-3 charge) = -6
- Final Formula:
The simplest formula, reflecting this charge balance, is Cu₃N₂, meaning 3 copper ions for every 2 nitrogen ions.
Thus, the simplest formula for copper (II) nitride is Cu₃N₂, which adheres to the charge balance rule for ionic compounds.