Question

identify the charge of the ions in each compound, then type the formula below: silver (ii) oxide silver (i) chloride (type final formula) (type final formula) answer key

Explanation:

Step1: Determine the charge of silver in Silver (II) oxide

In Silver (II) oxide, the Roman numeral (II) indicates the charge of silver. So, the charge of \( Ag \) is \( 2+ \).

Step2: Determine the charge of oxygen

Oxygen typically has a charge of \( 2 - \) in compounds.

Step3: Determine the formula of Silver (II) oxide

Using the criss - cross method (swap the absolute values of the charges as subscripts), for \( Ag^{2+} \) and \( O^{2 -} \), the formula is \( AgO \) (since \(\frac{2}{2}=1\) for both sub - scripts).

Step4: Determine the charge of silver in Silver (I) chloride

In Silver (I) chloride, the Roman numeral (I) indicates the charge of silver. So, the charge of \( Ag \) is \( 1+ \).

Step5: Determine the charge of chlorine

Chlorine typically has a charge of \( 1 - \) in compounds.

Step6: Determine the formula of Silver (I) chloride

Using the criss - cross method (swap the absolute values of the charges as subscripts), for \( Ag^{1+} \) and \( Cl^{1 -} \), the formula is \( AgCl \) (since \(\frac{1}{1}=1\) for both sub - scripts).

Answer:

For Silver (II) oxide: \( Ag \) charge is \( 2+ \), \( O \) charge is \( 2 - \), formula is \( AgO \).
For Silver (I) chloride: \( Ag \) charge is \( 1+ \), \( Cl \) charge is \( 1 - \), formula is \( AgCl \).