Answer :
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]
### 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]
