Pergunta

Write the empirical formula for at least four ionic compounds that could be formed from the following ions: ClO_(3)^-,Pb^4+,CN^-,Fe^3+ square
Solução

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FelipeAvançado · Tutor por 1 anos
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1. \(Pb(ClO_{3})_{4}\) 2. \(Pb(CN)_{4}\) 3. \(Fe(ClO_{3})_{3}\) 4. \(Fe(CN)_{3}\)
Explicação
To write the empirical formula for ionic compounds, we need to combine the cations (positively charged ions) with the anions (negatively charged ions) in such a way that the overall charge of the compound is neutral. This is achieved by balancing the charges of the ions so that the total positive charge equals the total negative charge.<br /><br />1. For the compound formed from \(ClO_{3}^{-}\) and \(Pb^{4+}\), we need four \(ClO_{3}^{-}\) ions to balance one \(Pb^{4+}\) ion, resulting in the formula \(Pb(ClO_{3})_{4}\).<br /><br />2. For the compound formed from \(CN^{-}\) and \(Pb^{4+}\), we need four \(CN^{-}\) ions to balance one \(Pb^{4+}\) ion, resulting in the formula \(Pb(CN)_{4}\).<br /><br />3. For the compound formed from \(ClO_{3}^{-}\) and \(Fe^{3+}\), we need three \(ClO_{3}^{-}\) ions to balance one \(Fe^{3+}\) ion, resulting in the formula \(Fe(ClO_{3})_{3}\).<br /><br />4. For the compound formed from \(CN^{-}\) and \(Fe^{3+}\), we need three \(CN^{-}\) ions to balance one \(Fe^{3+}\) ion, resulting in the formula \(Fe(CN)_{3}\).<br /><br />In each case, the empirical formula is written by placing the cation first, followed by the anion, with the appropriate subscripts to indicate the number of each ion needed to balance the charges.
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