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

write the empirical formula for at least four ionic compounds that could be formed from the following ions: $nh_{4}^{+}, pb^{4 + }, c_{2}h_{3}o_{2}^{-}, bro_{3}^{-}$

write the empirical formula for at least four ionic compounds that could be formed from the following ions: $nh_{4}^{+}, pb^{4 + }, c_{2}h_{3}o_{2}^{-}, bro_{3}^{-}$

Answer

Answer:

  1. $(NH_4)_2C_2H_3O_2$
  2. $(NH_4)BrO_3$
  3. $Pb(C_2H_3O_2)_4$
  4. $Pb(BrO_3)_4$

Explanation:

Step1: Recall ionic - compound formation

Ionic compounds are formed by the combination of cations and anions. The overall charge of the compound must be zero.

Step2: Combine $NH_4^+$ with $C_2H_3O_2^-$

The charge on $NH_4^+$ is + 1 and on $C_2H_3O_2^-$ is - 1. So, the formula is $(NH_4)C_2H_3O_2$.

Step3: Combine $NH_4^+$ with $BrO_3^-$

The charge on $NH_4^+$ is + 1 and on $BrO_3^-$ is - 1. So, the formula is $(NH_4)BrO_3$.

Step4: Combine $Pb^{4 + }$ with $C_2H_3O_2^-$

The charge on $Pb^{4+}$ is + 4 and on $C_2H_3O_2^-$ is - 1. To balance the charge, we need 4 $C_2H_3O_2^-$ ions. So, the formula is $Pb(C_2H_3O_2)_4$.

Step5: Combine $Pb^{4 + }$ with $BrO_3^-$

The charge on $Pb^{4+}$ is + 4 and on $BrO_3^-$ is - 1. To balance the charge, we need 4 $BrO_3^-$ ions. So, the formula is $Pb(BrO_3)_4$.