Questions: Identify the name of Pb(ClO3)4. lead(IV) tetrachlorate lead tetrachlorate lead(II) chlorate lead(IV) chlorate lead chlorate

Identify the name of Pb(ClO3)4. lead(IV) tetrachlorate lead tetrachlorate lead(II) chlorate lead(IV) chlorate lead chlorate
Transcript text: Identify the name of $\mathrm{Pb}\left(\mathrm{ClO}_{3}\right)_{4}$. lead(IV) tetrachlorate lead tetrachlorate lead(II) chlorate lead(IV) chlorate lead chlorate
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Solution

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Solution Steps

Step 1: Identify the Cation and Its Oxidation State

The chemical formula $\mathrm{Pb}\left(\mathrm{ClO}_{3}\right)_{4}$ contains lead (Pb) as the cation. The subscript 4 indicates that there are four chlorate ions ($\mathrm{ClO}_{3}^{-}$) associated with one lead ion. Each chlorate ion has a charge of -1.

Step 2: Determine the Total Charge of the Anions

Since there are four chlorate ions, the total negative charge contributed by the chlorate ions is: \[ 4 \times (-1) = -4 \]

Step 3: Determine the Oxidation State of Lead

To balance the -4 charge from the chlorate ions, the lead ion must have a +4 charge. Therefore, the oxidation state of lead in this compound is +4.

Step 4: Name the Compound

The name of the compound is derived from the cation (lead) and the anion (chlorate). Since the lead ion has an oxidation state of +4, it is specified as lead(IV). The anion is chlorate.

Final Answer

\[ \boxed{\text{lead(IV) chlorate}} \]

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