Draw the Lewis structure for the following ions. Be sure to calculate the formal charge of each atom to confirm that your structure is correct. (d) AlCl⁻₄

Verified step by step guidance

1. Step 1: Determine the total number of valence electrons.
2. Step 2: Identify the central atom and arrange the other atoms around it.
3. Step 3: Draw single bonds between the central atom and surrounding atoms.
4. Step 4: Distribute remaining electrons to satisfy the octet rule for each atom.
5. Step 5: Calculate the formal charge for each atom to ensure the structure is correct.

Key Concepts

Lewis Structures

Lewis structures are diagrams that represent the bonding between atoms in a molecule and the lone pairs of electrons that may exist. They use dots to represent valence electrons and lines to represent bonds between atoms. Understanding how to draw Lewis structures is essential for visualizing molecular geometry and predicting reactivity.

Formal Charge

Formal charge is a theoretical charge assigned to an atom in a molecule, calculated based on the number of valence electrons, the number of non-bonding electrons, and half the number of bonding electrons. It helps in assessing the stability of a Lewis structure; ideally, the formal charges should be minimized and should reflect the actual charge distribution in the molecule.

Ionic Compounds

Ionic compounds are formed when atoms transfer electrons, resulting in the formation of charged ions. In the case of AlCl₄⁻, aluminum (Al) donates electrons to chlorine (Cl) atoms, leading to a negatively charged ion. Understanding the nature of ionic bonding is crucial for predicting the behavior and properties of such compounds.