Question

silver oxide is a chemical compound.

a. is this an ionic or covalent compound?
explain how you can tell based on the types of elements it contains.

b. how do you determine the chemical formula of this compound?
describe the steps you used and write the correct formula.

Explanation:

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<reasoning>

Identify compound type

Silver oxide contains silver (a metal) and oxygen (a nonmetal).
Using Chemical Nomenclature rules, a metal combined with a nonmetal forms an ionic compound.

Determine ionic charges

Silver forms a \(1+\) cation, written as \(\text{Ag}^+\).
Oxygen forms a \(2-\) anion, written as \(\text{O}^{2-}\).

Balance the charges

To balance the charges, two \(\text{Ag}^+\) ions are needed for every one \(\text{O}^{2-}\) ion.
This makes the overall compound neutral: \(2(+1) + 1(-2) = 0\).

Write final formula

Combining the balanced ions gives the chemical formula \(\text{Ag}_2\text{O}\).
</reasoning>

<answer>

Question A

Silver oxide is an ionic compound. It consists of silver, which is a metal, and oxygen, which is a nonmetal.

Question B

To determine the formula, identify the charges of the ions: silver is \(\text{Ag}^+\) and oxide is \(\text{O}^{2-}\). Balance the charges to make the compound neutral, requiring two silver ions for every one oxide ion, which gives the formula \(\text{Ag}_2\text{O}\).
</answer>

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Answer:

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<reasoning>

Identify compound type

Silver oxide contains silver (a metal) and oxygen (a nonmetal).
Using Chemical Nomenclature rules, a metal combined with a nonmetal forms an ionic compound.

Determine ionic charges

Silver forms a \(1+\) cation, written as \(\text{Ag}^+\).
Oxygen forms a \(2-\) anion, written as \(\text{O}^{2-}\).

Balance the charges

To balance the charges, two \(\text{Ag}^+\) ions are needed for every one \(\text{O}^{2-}\) ion.
This makes the overall compound neutral: \(2(+1) + 1(-2) = 0\).

Write final formula

Combining the balanced ions gives the chemical formula \(\text{Ag}_2\text{O}\).
</reasoning>

<answer>

Question A

Silver oxide is an ionic compound. It consists of silver, which is a metal, and oxygen, which is a nonmetal.

Question B

To determine the formula, identify the charges of the ions: silver is \(\text{Ag}^+\) and oxide is \(\text{O}^{2-}\). Balance the charges to make the compound neutral, requiring two silver ions for every one oxide ion, which gives the formula \(\text{Ag}_2\text{O}\).
</answer>

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