Certainly! First ionization energy refers to the energy required to remove the first electron from an atom in its gaseous state. Elements with high first ionization energies require a significant amount of energy to remove an electron, while elements with low first ionization energies require relatively less energy. Here are examples of elements with high and low first ionization energies:
High first ionization energy:
- Helium (He): Helium has the highest first ionization energy among all elements. It has a fully filled 1s^2 electron configuration, and removing an electron from the 1s orbital requires a large amount of energy.
- Neon (Ne): Neon is another noble gas with a high first ionization energy. It also has a stable electron configuration (1s^2 2s^2 2p^6), making it difficult to remove an electron.
Low first ionization energy:
- Lithium (Li): Lithium has the lowest first ionization energy among all elements. It has a single valence electron in the 2s orbital, which is relatively far from the nucleus and experiences less electrostatic attraction.
- Francium (Fr): Francium is the element with the lowest first ionization energy among the naturally occurring elements. It has a single valence electron in the 7s orbital, and due to its large atomic size and shielding effect, the electron is easier to remove.
Please note that the first ionization energy can vary depending on factors such as atomic structure, atomic size, and effective nuclear charge. The examples provided above are for general reference and represent extreme cases within the periodic table.