Write The Empirical Formula Of At Least Four Binary Ionic Compounds That Could Be Formed From The Following Ions:${ Ca^{2+}, Au^{3+}, Cl^{-}, S^{2-} }$1. { CaCl_2 $}$2. { CaS $}$3. { AuCl_3 $} 4. \[ 4. \[ 4. \[

Introduction

In chemistry, binary ionic compounds are formed when two different elements combine to form a compound. These compounds are typically composed of a metal cation and a nonmetal anion. The empirical formula of a binary ionic compound is a representation of the simplest whole-number ratio of atoms of each element present in the compound. In this article, we will explore the empirical formula of at least four binary ionic compounds that could be formed from the following ions: $Ca^{2+}, Au^{3+}, Cl^{-}, S^{2-}$.

Empirical Formula of Binary Ionic Compounds

To determine the empirical formula of a binary ionic compound, we need to consider the charges of the ions involved. The charges of the ions are as follows:

• $Ca^{2+}$: +2
• $Au^{3+}$: +3
• $Cl^{-}$: -1
• $S^{2-}$: -2

1. Empirical Formula of $CaCl_2$

The empirical formula of $CaCl_2$ can be determined by considering the charges of the ions involved. Since $Ca^{2+}$ has a charge of +2 and $Cl^{-}$ has a charge of -1, we need two $Cl^{-}$ ions to balance the charge of one $Ca^{2+}$ ion. Therefore, the empirical formula of $CaCl_2$ is:

${ CaCl_2 }$

2. Empirical Formula of $CaS$

The empirical formula of $CaS$ can be determined by considering the charges of the ions involved. Since $Ca^{2+}$ has a charge of +2 and $S^{2-}$ has a charge of -2, we need one $S^{2-}$ ion to balance the charge of one $Ca^{2+}$ ion. Therefore, the empirical formula of $CaS$ is:

${ CaS }$

3. Empirical Formula of $AuCl_3$

The empirical formula of $AuCl_3$ can be determined by considering the charges of the ions involved. Since $Au^{3+}$ has a charge of +3 and $Cl^{-}$ has a charge of -1, we need three $Cl^{-}$ ions to balance the charge of one $Au^{3+}$ ion. Therefore, the empirical formula of $AuCl_3$ is:

${ AuCl_3 }$

4. Empirical Formula of $Au_2S_3$

The empirical formula of $Au_2S_3$ can be determined by considering the charges of the ions involved. Since $Au^{3+}$ has a charge of +3 and $S^{2-}$ has a charge of -2, we need three $S^{2-}$ ions to balance the charge of two $Au^{3+}$ ions. Therefore, the empirical formula of $Au_2S_3$ is:

${ Au_2S_3 }$

5. Empirical Formula of $Ca_2S$

The empirical formula of $Ca_2S$ can be determined by considering the charges of the ions involved. Since $Ca^{2+}$ has a charge of +2 and $S^{2-}$ has a charge of -2, we need one $S^{2-}$ ion to balance the charge of two $Ca^{2+}$ ions. Therefore, the empirical formula of $Ca_2S$ is:

${ Ca_2S }$

Conclusion

In conclusion, the empirical formula of at least four binary ionic compounds that could be formed from the following ions: $Ca^{2+}, Au^{3+}, Cl^{-}, S^{2-}$ are:

• $CaCl_2$
• $CaS$
• $AuCl_3$
• $Au_2S_3$
• $Ca_2S$

Introduction

In our previous article, we explored the empirical formula of at least four binary ionic compounds that could be formed from the following ions: $Ca^{2+}, Au^{3+}, Cl^{-}, S^{2-}$. In this article, we will answer some frequently asked questions related to the empirical formula of binary ionic compounds.

Q: What is the empirical formula of a binary ionic compound?

A: The empirical formula of a binary ionic compound is a representation of the simplest whole-number ratio of atoms of each element present in the compound.

Q: How do you determine the empirical formula of a binary ionic compound?

A: To determine the empirical formula of a binary ionic compound, you need to consider the charges of the ions involved. The charges of the ions are as follows:

• $Ca^{2+}$: +2
• $Au^{3+}$: +3
• $Cl^{-}$: -1
• $S^{2-}$: -2

Q: What is the empirical formula of $CaCl_2$?

A: The empirical formula of $CaCl_2$ is $CaCl_2$. This is because $Ca^{2+}$ has a charge of +2 and $Cl^{-}$ has a charge of -1, so we need two $Cl^{-}$ ions to balance the charge of one $Ca^{2+}$ ion.

Q: What is the empirical formula of $CaS$?

A: The empirical formula of $CaS$ is $CaS$. This is because $Ca^{2+}$ has a charge of +2 and $S^{2-}$ has a charge of -2, so we need one $S^{2-}$ ion to balance the charge of one $Ca^{2+}$ ion.

Q: What is the empirical formula of $AuCl_3$?

A: The empirical formula of $AuCl_3$ is $AuCl_3$. This is because $Au^{3+}$ has a charge of +3 and $Cl^{-}$ has a charge of -1, so we need three $Cl^{-}$ ions to balance the charge of one $Au^{3+}$ ion.

Q: What is the empirical formula of $Au_2S_3$?

A: The empirical formula of $Au_2S_3$ is $Au_2S_3$. This is because $Au^{3+}$ has a charge of +3 and $S^{2-}$ has a charge of -2, so we need three $S^{2-}$ ions to balance the charge of two $Au^{3+}$ ions.

Q: What is the empirical formula of $Ca_2S$?

A: The empirical formula of $Ca_2S$ is $Ca_2S$. This is because $Ca^{2+}$ has a charge of +2 and $S^{2-}$ has a charge of -2, so we need one $S^{2-}$ ion to balance the charge of two $Ca^{2+}$ ions.

Q: How do you write the empirical formula of a binary ionic compound?

A: To write the empirical formula of a binary ionic compound, you need to follow these steps:

1. Determine the charges of the ions involved.
2. Balance the charges of the ions by adding or subtracting ions.
3. Write the empirical formula by listing the ions in the correct ratio.

Conclusion

In conclusion, the empirical formula of at least four binary ionic compounds that could be formed from the following ions: $Ca^{2+}, Au^{3+}, Cl^{-}, S^{2-}$ are:

• $CaCl_2$
• $CaS$
• $AuCl_3$
• $Au_2S_3$
• $Ca_2S$

We hope this article has helped you understand the empirical formula of binary ionic compounds and how to determine it. If you have any further questions, please don't hesitate to ask.