Answered

Explore Westonci.ca, the leading Q&A site where experts provide accurate and helpful answers to all your questions. Explore comprehensive solutions to your questions from a wide range of professionals on our user-friendly platform. Connect with a community of professionals ready to provide precise solutions to your questions quickly and accurately.

Which are possible equations for an ionic compound with calcium?

A. \( \text{CaO}, \text{CaMg}, \text{or CaF}_2 \)

B. \( \text{Ca}_2\text{Cl}, \text{CaNa}, \text{or CaP} \)

C. \( \text{CaF}, \text{CaMg}, \text{or CaNa} \)

D. [tex]\( \text{CaO}, \text{CaF}_2, \text{or CaCl}_2 \)[/tex]

Sagot :

GinnyAnswer
To determine which combinations are possible ionic compounds with calcium, we should analyze the chemical properties and valences of each element involved.

### Step 1: Understand Calcium's Ionic Nature
- Calcium (Ca) typically forms a +2 ion (Ca²⁺).

### Step 2: Evaluate the Given Combinations

1. First Option: \( \text{CaO}, \text{CaMg}, \text{CaF}_2 \)
- \( \text{CaO} \): Calcium forms a +2 ion, and oxygen typically forms a -2 ion. Therefore, \( \text{CaO} \) is a valid ionic compound because the charges balance.
- \( \text{CaMg} \): Both calcium and magnesium form positive ions. Since both are cations, they cannot form an ionic compound together.
- \( \text{CaF}_2 \): Calcium forms a +2 ion, and fluorine forms a -1 ion. Two fluorine ions (-1 each) will balance with one calcium ion (+2), making \( \text{CaF}_2 \) a valid ionic compound.

2. Second Option: \( \text{Ca}_2 \text{Cl}, \text{CaNa}, \text{CaP} \)
- \( \text{Ca}_2 \text{Cl} \): This formula does not make sense because each calcium is +2 and chlorine is -1. The proper formula with these charges balanced would be \( \text{CaCl}_2 \).
- \( \text{CaNa} \): Both calcium and sodium are metals and form positive ions (cations). They cannot form an ionic compound together.
- \( \text{CaP} \): Phosphorus typically forms a -3 ion (P³⁻). The correct formula for a compound with calcium and phosphorus (to balance the charges) would be \( \text{Ca}_3 \text{P}_2 \).

3. Third Option: \( \text{CaF}, \text{CaMg}, \text{CaNa} \)
- \( \text{CaF} \): This does not balance correctly; one calcium ion requires two fluorine ions to balance (thus \( \text{CaF}_2 \)).
- \( \text{CaMg} \): As previously explained, both are cations and cannot form an ionic compound together.
- \( \text{CaNa} \): Again, both are cations and cannot form an ionic compound together.

4. Fourth Option: \( \text{CaO}, \text{CaF}_2, \text{CaCl}_2 \)
- \( \text{CaO} \): As explained, this is a valid ionic compound.
- \( \text{CaF}_2 \): As explained, this is a valid ionic compound.
- \( \text{CaCl}_2 \): Calcium forms a +2 ion and chlorine forms a -1 ion. Two chlorine ions will balance with one calcium ion (+2), making \( \text{CaCl}_2 \) a valid ionic compound.

### Conclusion
Considering the detailed analysis of the ion formation and charge balance:
- The fourth option \( \text{CaO}, \text{CaF}_2, \text{CaCl}_2 \) contains all valid ionic compounds with calcium.

Therefore, the correct answer is:
[tex]\[ \text{CaO}, \text{CaF}_2, \text{CaCl}_2 \][/tex]
Thanks for using our platform. We're always here to provide accurate and up-to-date answers to all your queries. We hope this was helpful. Please come back whenever you need more information or answers to your queries. Thank you for visiting Westonci.ca, your go-to source for reliable answers. Come back soon for more expert insights.