Elements with low ionization energies generally form cations. Explain.

Answer

To explain why elements with low ionization energies generally form cations, we can break down the explanation into a series of logical steps:

### Step-by-Step Solution:

1. **Definition of Ionization Energy**:
- Ionization energy is defined as the amount of energy required to remove an electron from the outermost shell of an atom.

2. **Understanding Low Ionization Energy**:
- Elements with low ionization energies require less energy to remove an electron. This means that it is easier for these elements to lose an electron compared to elements with high ionization energies.

3. **Formation of Cations**:
- When an atom loses one or more electrons, it becomes positively charged. This positively charged species is known as a cation.

4. **Ease of Electron Removal**:
- Since elements with low ionization energies can lose their outermost electrons easily, they tend to form cations readily. For example, sodium (Na) has one electron in its outermost shell.

5. **Example of Sodium**:
- When sodium loses its one outermost electron, it forms a Na⁺ cation. The energy required to remove this electron is relatively low due to its low ionization energy, making the formation of the cation favorable.

6. **Conclusion**:
- Therefore, elements with low ionization energies tend to form cations because they can easily lose electrons, resulting in a stable positively charged ion.