IDNLearn.com: Your one-stop destination for reliable answers to diverse questions. Join our community to receive timely and reliable responses to your questions from knowledgeable professionals.

Write the empirical formula for at least four ionic compounds that could be formed from the following ions:

[tex]\[ \text{Pb}^{4+}, \text{CN}^-, \text{CO}_3^{2-}, \text{Fe}^{2+} \][/tex]


Sagot :

Let's find the empirical formulas for the ionic compounds formed from the given ions: [tex]\( \text{Pb}^{4+} \)[/tex], [tex]\( \text{CN}^{-} \)[/tex], [tex]\( \text{CO}_3^{2-} \)[/tex], and [tex]\( \text{Fe}^{2+} \)[/tex].

### Compound 1: [tex]\( \text{Pb}^{4+} \)[/tex] and [tex]\( \text{CN}^{-} \)[/tex]
1. [tex]\( \text{Pb}^{4+} \)[/tex] has a charge of [tex]\( +4 \)[/tex].
2. [tex]\( \text{CN}^{-} \)[/tex] has a charge of [tex]\( -1 \)[/tex].
3. To balance the charges, we need 4 [tex]\( \text{CN}^{-} \)[/tex] ions to balance the single [tex]\( \text{Pb}^{4+} \)[/tex] ion.

[tex]\[ \text{Pb}^{4+} + 4(\text{CN}^{-}) \rightarrow \text{Pb(CN)}_4 \][/tex]

So, the empirical formula for this compound is [tex]\( \text{Pb(CN)}_4 \)[/tex].

### Compound 2: [tex]\( \text{Pb}^{4+} \)[/tex] and [tex]\( \text{CO}_3^{2-} \)[/tex]
1. [tex]\( \text{Pb}^{4+} \)[/tex] has a charge of [tex]\( +4 \)[/tex].
2. [tex]\( \text{CO}_3^{2-} \)[/tex] has a charge of [tex]\( -2 \)[/tex].
3. To balance the charges, we need 2 [tex]\( \text{CO}_3^{2-} \)[/tex] ions to balance the single [tex]\( \text{Pb}^{4+} \)[/tex] ion.

[tex]\[ \text{Pb}^{4+} + 2(\text{CO}_3^{2-}) \rightarrow \text{Pb(CO}_3\text{)}_2 \][/tex]

So, the empirical formula for this compound is [tex]\( \text{Pb(CO}_3\text{)}_2 \)[/tex].

### Compound 3: [tex]\( \text{Fe}^{2+} \)[/tex] and [tex]\( \text{CN}^{-} \)[/tex]
1. [tex]\( \text{Fe}^{2+} \)[/tex] has a charge of [tex]\( +2 \)[/tex].
2. [tex]\( \text{CN}^{-} \)[/tex] has a charge of [tex]\( -1 \)[/tex].
3. To balance the charges, we need 2 [tex]\( \text{CN}^{-} \)[/tex] ions to balance the single [tex]\( \text{Fe}^{2+} \)[/tex] ion.

[tex]\[ \text{Fe}^{2+} + 2(\text{CN}^{-}) \rightarrow \text{Fe(CN)}_2 \][/tex]

So, the empirical formula for this compound is [tex]\( \text{Fe(CN)}_2 \)[/tex].

### Compound 4: [tex]\( \text{Fe}^{2+} \)[/tex] and [tex]\( \text{CO}_3^{2-} \)[/tex]
1. [tex]\( \text{Fe}^{2+} \)[/tex] has a charge of [tex]\( +2 \)[/tex].
2. [tex]\( \text{CO}_3^{2-} \)[/tex] has a charge of [tex]\( -2 \)[/tex].
3. To balance the charges, 1 [tex]\( \text{Fe}^{2+} \)[/tex] ion matches perfectly with 1 [tex]\( \text{CO}_3^{2-} \)[/tex] ion.

[tex]\[ \text{Fe}^{2+} + \text{CO}_3^{2-} \rightarrow \text{FeCO}_3 \][/tex]

So, the empirical formula for this compound is [tex]\( \text{FeCO}_3 \)[/tex].

Putting it all together, the empirical formulas for the four ionic compounds are:
1. [tex]\( \text{Pb(CN)}_4 \)[/tex]
2. [tex]\( \text{Pb(CO}_3\text{)}_2 \)[/tex]
3. [tex]\( \text{Fe(CN)}_2 \)[/tex]
4. [tex]\( \text{FeCO}_3 \)[/tex]