I want to know how to find the formula for the compound formed by the NH
4
+
cation and the F
−
anion.
The Correct Answer and Explanation is :
To determine the formula for the compound formed by the ammonium cation ((\text{NH}_4^+)) and the fluoride anion ((\text{F}^-)), we need to consider the charges of the ions involved.
Step 1: Identify the Ions and Their Charges
- The ammonium ion ((\text{NH}_4^+)) has a charge of (+1).
- The fluoride ion ((\text{F}^-)) has a charge of (-1).
Step 2: Combine the Ions
When combining ions to form a neutral compound, the total positive charge must equal the total negative charge. In this case:
- The (+) charge from the ammonium ion balances the (-) charge from the fluoride ion. Therefore, one ammonium ion can combine with one fluoride ion to form a neutral compound.
Step 3: Write the Chemical Formula
Since we have one ammonium ion and one fluoride ion, we can write the formula as follows:
[
\text{NH}_4^+ + \text{F}^- \rightarrow \text{NH}_4\text{F}
]
Thus, the formula for the compound formed is (\text{NH}_4\text{F}), known as ammonium fluoride.
Explanation
The formation of ionic compounds involves the transfer of electrons and the attraction between positively and negatively charged ions. The ammonium ion, which is a polyatomic ion, acts like a single unit that carries a (+1) charge. Fluoride ions are monatomic and carry a (-1) charge.
When these ions combine, they do so in a 1:1 ratio, meaning that for every ammonium ion, there is one fluoride ion. This combination results in the neutral compound ammonium fluoride. Ionic compounds are typically solid at room temperature and have high melting and boiling points due to the strong electrostatic forces between the ions.
Ammonium fluoride is often used in various applications, including as a reagent in chemistry and in the production of certain types of glass and ceramics. Understanding how to derive formulas for ionic compounds is fundamental in chemistry, as it helps predict the behavior of substances in reactions and their properties in various environments.