Which of the following ions are likely to form? Explain.a. Li^2+b. K-c. Mn^3+d. Zn^4+e. Ne+

Verified step by step guidance

1. Step 1: Understand the concept of ion formation. Ions are formed when atoms gain or lose electrons to achieve a stable electron configuration, often resembling the nearest noble gas.
2. Step 2: Analyze each ion option. Consider the electron configuration of the neutral atom and how gaining or losing electrons affects stability.
3. Step 3: Evaluate Li^2+. Lithium (Li) has an electron configuration of 1s^2 2s^1. Losing one electron forms Li^+, achieving a stable configuration like helium. Losing two electrons to form Li^2+ would result in an unstable configuration.
4. Step 4: Evaluate K-. Potassium (K) has an electron configuration of [Ar] 4s^1. Gaining an electron to form K- would result in an unstable configuration, as it would not resemble a noble gas.
5. Step 5: Evaluate Mn^3+, Zn^4+, and Ne+. Consider the electron configurations and stability of these ions. Mn^3+ is common due to its stable half-filled d-orbital configuration. Zn^4+ and Ne+ are unlikely due to instability and noble gas configuration, respectively.

Key Concepts

Ionic Charge and Stability

Ionic charge refers to the electrical charge an atom or molecule carries due to the loss or gain of electrons. Atoms tend to form ions to achieve a stable electron configuration, often resembling the nearest noble gas. For example, metals typically lose electrons to form positive ions, while nonmetals gain electrons to form negative ions.

Common Ion Formation

Certain ions are more likely to form based on their position in the periodic table and their electron configurations. For instance, alkali metals like potassium (K) usually form +1 ions, while transition metals can have multiple oxidation states. Understanding these trends helps predict which ions are stable and likely to exist.

Electron Configuration and Valence Electrons

Electron configuration describes the distribution of electrons in an atom's orbitals. Valence electrons, the outermost electrons, play a crucial role in chemical bonding and ion formation. Analyzing the electron configuration of an element helps determine its tendency to gain or lose electrons, influencing its ability to form stable ions.