To determine which of the given compounds is most likely to exhibit covalent bonding, we need to understand the nature of covalent bonding. Covalent bonding typically occurs between non-metal atoms that share electrons to achieve stability.
1. NaF (Sodium Fluoride):
- Sodium (Na) is a metal.
- Fluorine (F) is a non-metal.
- The bond between a metal and a non-metal is ionic.
2. CaCl₂ (Calcium Chloride):
- Calcium (Ca) is a metal.
- Chlorine (Cl) is a non-metal.
- The bond between a metal and a non-metal is ionic.
3. Cs₂O (Cesium Oxide):
- Cesium (Cs) is a metal.
- Oxygen (O) is a non-metal.
- The bond between a metal and a non-metal is ionic.
4. CO₂ (Carbon Dioxide):
- Carbon (C) is a non-metal.
- Oxygen (O) is a non-metal.
- The bond between non-metal atoms tends to be covalent, as they share electrons to achieve stability.
5. NaCl (Sodium Chloride):
- Sodium (Na) is a metal.
- Chlorine (Cl) is a non-metal.
- The bond between a metal and a non-metal is ionic.
From the above analysis, we can determine that CO₂ (Carbon Dioxide) involves bonding between two non-metals (carbon and oxygen), which is indicative of covalent bonding. Therefore, among the given choices, CO₂ (Carbon Dioxide) is the compound most likely to exhibit covalent bonding.
The position of CO₂ within the list of options (0-indexed) is 3. Thus, CO₂ is the compound most likely to exhibit covalent bonding.
