Question

fill in the name and empirical formula of each ionic compound that could be formed from the ions in this table:

some ionic compounds
$ce{k^+}$	$ce{so_4^{2-}}$	$ce{k2so4}$	potassium sulfate
$ce{zn^{2+}}$	$ce{oh^-}$	$ce{zn(oh)2}$	zinc hydroxide
$ce{pb^{4+}}$	$ce{bro_3^-}$	$ce{pb(bro3)4}$	lead(iv)bromate

Explanation:

To determine the empirical formula and name of ionic compounds, we use the principle of charge balance (the total positive charge equals the total negative charge) and follow naming conventions for ionic compounds.

For \( \boldsymbol{\ce{K^+}} \) and \( \boldsymbol{\ce{SO_4^{2-}}} \):

Step 1: Balance Charges

The charge of \( \ce{K^+} \) is \( +1 \), and the charge of \( \ce{SO_4^{2-}} \) is \( -2 \). To balance the charges, we need 2 \( \ce{K^+} \) ions (total positive charge \( 2 \times (+1) = +2 \)) to balance 1 \( \ce{SO_4^{2-}} \) ion (total negative charge \( -2 \)).
Empirical formula: \( \ce{K_2SO_4} \) (Note: The original "K2SO4" in the table should be formatted as \( \ce{K_2SO_4} \) for clarity.)

Step 2: Name the Compound

For ionic compounds with monatomic cations (like \( \ce{K^+} \)) and polyatomic anions (like \( \ce{SO_4^{2-}} \)), we use the cation name (potassium) and the anion name (sulfate).
Name: potassium sulfate

For \( \boldsymbol{\ce{Zn^{2+}}} \) and \( \boldsymbol{\ce{OH^-}} \):

Step 1: Balance Charges

The charge of \( \ce{Zn^{2+}} \) is \( +2 \), and the charge of \( \ce{OH^-} \) is \( -1 \). To balance the charges, we need 2 \( \ce{OH^-} \) ions (total negative charge \( 2 \times (-1) = -2 \)) to balance 1 \( \ce{Zn^{2+}} \) ion (total positive charge \( +2 \)).
Empirical formula: \( \ce{Zn(OH)_2} \) (Note: The original "Zn(OH)2" in the table should be formatted as \( \ce{Zn(OH)_2} \) for clarity.)

Step 2: Name the Compound

For ionic compounds with a metal cation (like \( \ce{Zn^{2+}} \)) and a polyatomic anion (like \( \ce{OH^-} \)), we use the cation name (zinc, a metal with a fixed charge) and the anion name (hydroxide).
Name: zinc hydroxide

For \( \boldsymbol{\ce{Pb^{4+}}} \) and \( \boldsymbol{\ce{BrO_3^-}} \):

Step 1: Balance Charges

The charge of \( \ce{Pb^{4+}} \) is \( +4 \), and the charge of \( \ce{BrO_3^-} \) is \( -1 \). To balance the charges, we need 4 \( \ce{BrO_3^-} \) ions (total negative charge \( 4 \times (-1) = -4 \)) to balance 1 \( \ce{Pb^{4+}} \) ion (total positive charge \( +4 \)).
Empirical formula: \( \ce{Pb(BrO_3)_4} \) (Note: The original "Pb(BrO3)4" in the table should be formatted as \( \ce{Pb(BrO_3)_4} \) for clarity.)

Step 2: Name the Compound

For ionic compounds with a metal cation (like \( \ce{Pb^{4+}} \)) that can have multiple charges, we use a Roman numeral to indicate the charge of the cation (IV for \( +4 \)) and the anion name (bromate).
Name: lead(IV) bromate

Final Table (Corrected Formatting):

cation	anion	empirical formula	name of compound
\( \ce{Zn^{2+}} \)	\( \ce{OH^-} \)	\( \ce{Zn(OH)_2} \)	zinc hydroxide
\( \ce{Pb^{4+}} \)	\( \ce{BrO_3^-} \)	\( \ce{Pb(BrO_3)_4} \)	lead(IV) bromate

Answer:

To determine the empirical formula and name of ionic compounds, we use the principle of charge balance (the total positive charge equals the total negative charge) and follow naming conventions for ionic compounds.

For \( \boldsymbol{\ce{K^+}} \) and \( \boldsymbol{\ce{SO_4^{2-}}} \):

Step 1: Balance Charges

The charge of \( \ce{K^+} \) is \( +1 \), and the charge of \( \ce{SO_4^{2-}} \) is \( -2 \). To balance the charges, we need 2 \( \ce{K^+} \) ions (total positive charge \( 2 \times (+1) = +2 \)) to balance 1 \( \ce{SO_4^{2-}} \) ion (total negative charge \( -2 \)).
Empirical formula: \( \ce{K_2SO_4} \) (Note: The original "K2SO4" in the table should be formatted as \( \ce{K_2SO_4} \) for clarity.)

Step 2: Name the Compound

For ionic compounds with monatomic cations (like \( \ce{K^+} \)) and polyatomic anions (like \( \ce{SO_4^{2-}} \)), we use the cation name (potassium) and the anion name (sulfate).
Name: potassium sulfate

For \( \boldsymbol{\ce{Zn^{2+}}} \) and \( \boldsymbol{\ce{OH^-}} \):

Step 1: Balance Charges

The charge of \( \ce{Zn^{2+}} \) is \( +2 \), and the charge of \( \ce{OH^-} \) is \( -1 \). To balance the charges, we need 2 \( \ce{OH^-} \) ions (total negative charge \( 2 \times (-1) = -2 \)) to balance 1 \( \ce{Zn^{2+}} \) ion (total positive charge \( +2 \)).
Empirical formula: \( \ce{Zn(OH)_2} \) (Note: The original "Zn(OH)2" in the table should be formatted as \( \ce{Zn(OH)_2} \) for clarity.)

Step 2: Name the Compound

For ionic compounds with a metal cation (like \( \ce{Zn^{2+}} \)) and a polyatomic anion (like \( \ce{OH^-} \)), we use the cation name (zinc, a metal with a fixed charge) and the anion name (hydroxide).
Name: zinc hydroxide

For \( \boldsymbol{\ce{Pb^{4+}}} \) and \( \boldsymbol{\ce{BrO_3^-}} \):

Step 1: Balance Charges

The charge of \( \ce{Pb^{4+}} \) is \( +4 \), and the charge of \( \ce{BrO_3^-} \) is \( -1 \). To balance the charges, we need 4 \( \ce{BrO_3^-} \) ions (total negative charge \( 4 \times (-1) = -4 \)) to balance 1 \( \ce{Pb^{4+}} \) ion (total positive charge \( +4 \)).
Empirical formula: \( \ce{Pb(BrO_3)_4} \) (Note: The original "Pb(BrO3)4" in the table should be formatted as \( \ce{Pb(BrO_3)_4} \) for clarity.)

Step 2: Name the Compound

For ionic compounds with a metal cation (like \( \ce{Pb^{4+}} \)) that can have multiple charges, we use a Roman numeral to indicate the charge of the cation (IV for \( +4 \)) and the anion name (bromate).
Name: lead(IV) bromate

Final Table (Corrected Formatting):

cation	anion	empirical formula	name of compound
\( \ce{Zn^{2+}} \)	\( \ce{OH^-} \)	\( \ce{Zn(OH)_2} \)	zinc hydroxide
\( \ce{Pb^{4+}} \)	\( \ce{BrO_3^-} \)	\( \ce{Pb(BrO_3)_4} \)	lead(IV) bromate