To determine which periodic trend is larger for lithium (Li) compared to potassium (K), let's analyze each trend:
1. Ionization energy: Lithium (Li) has a larger ionization energy than potassium (K). Ionization energy is the energy required to remove an electron from an atom. Since lithium has a smaller atomic radius than potassium, it holds its electrons more tightly, making it more difficult to remove an electron from a lithium atom compared to a potassium atom.
2. Atomic radius: Potassium (K) has a larger atomic radius than lithium (Li). Atomic radius refers to the size of an atom. Moving down a group in the periodic table, atomic radius increases. Therefore, potassium, which is located below lithium in the periodic table, has a larger atomic radius.
3. Number of protons: Both lithium (Li) and potassium (K) have the same number of protons. The number of protons in an atom determines its element identity. Since lithium has 3 protons and potassium has 19 protons, they do not have the same number of protons.
4. Ionic radius: Potassium (K) has a larger ionic radius than lithium (Li). Ionic radius refers to the size of an ion. When lithium forms an ion by losing an electron, it becomes smaller due to increased nuclear attraction. In contrast, when potassium forms an ion, it becomes larger as it gains an electron and the electron-electron repulsion increases its size.
In summary, lithium (Li) has a larger value for ionization energy compared to potassium (K), while potassium has a larger atomic radius and ionic radius than lithium. Both elements do not have the same number of protons.
