To determine which pair of elements would form an ionic bond, we need to understand the nature of ionic bonding. Ionic bonds typically form between metals and non-metals. In this bond, one atom donates electrons and becomes a positively charged ion (cation), while the other atom gains electrons and becomes a negatively charged ion (anion).
Let's analyze each pair of elements:
1. Carbon (C) and Oxygen (O):
- Carbon is a non-metal.
- Oxygen is a non-metal.
- Both are non-metals, and non-metal pairs typically form covalent bonds rather than ionic bonds.
2. Strontium (Sr) and Chlorine (Cl):
- Strontium is a metal.
- Chlorine is a non-metal.
- Metals tend to lose electrons and become cations, while non-metals tend to gain electrons and become anions.
- Thus, strontium can donate electrons to chlorine, forming an ionic bond.
3. Cesium (Cs) and Germanium (Ge):
- Cesium is a metal.
- Germanium is a metalloid.
- While cesium can donate electrons, germanium typically does not gain electrons to form an ionic bond. Hence, this pair is less likely to form a strong ionic bond.
4. Magnesium (Mg) and Aluminum (Al):
- Magnesium is a metal.
- Aluminum is also a metal.
- Metals generally do not form ionic bonds with each other, as they both tend to lose electrons rather than gain them.
Considering these analyses, the pair of elements that would form an ionic bond is:
Strontium (Sr) and Chlorine (Cl).
