Write equations for the loss of an electron by a K atom and the gain of an electron by a K+ ion.

Verified step by step guidance

1. Identify the initial species involved in each process: a neutral potassium atom (K) and a potassium ion (K⁺).
2. For the loss of an electron by a K atom, write the equation: K → K⁺ + e⁻. This represents the ionization of potassium, where a neutral potassium atom loses one electron to form a positively charged ion.
3. For the gain of an electron by a K⁺ ion, write the equation: K⁺ + e⁻ → K. This represents the reduction process, where a potassium ion gains an electron to become a neutral potassium atom.
4. Understand that these processes are examples of oxidation and reduction. The loss of an electron (K to K⁺) is oxidation, and the gain of an electron (K⁺ to K) is reduction.
5. Review the concept of oxidation states: In the first equation, the oxidation state of K changes from 0 to +1, and in the second equation, it changes from +1 to 0.

Key Concepts

Ionization Energy

Ionization energy is the energy required to remove an electron from an atom in its gaseous state. For potassium (K), this process involves overcoming the attraction between the negatively charged electron and the positively charged nucleus. The equation for the loss of an electron from a K atom can be represented as K(g) → K⁺(g) + e⁻, indicating that an electron is removed, resulting in a positively charged ion.

Electron Affinity

Electron affinity refers to the energy change that occurs when an electron is added to a neutral atom in the gaseous state. For a potassium ion (K⁺), gaining an electron results in the formation of a neutral potassium atom. The equation for this process is K⁺(g) + e⁻ → K(g), which shows that the addition of an electron to K⁺ releases energy, making the process exothermic.

Atomic Structure

The atomic structure of an element defines the arrangement of protons, neutrons, and electrons within an atom. Potassium has 19 electrons, with its outermost electron in the fourth energy level. Understanding atomic structure is crucial for predicting how potassium will interact with electrons, including its tendency to lose an electron to form K⁺ and its ability to gain an electron to revert to a neutral state.