Lewis Diagrams

Ethan Taylor
8 min read
Listen to this study note
Study Guide Overview
This study guide covers Lewis diagrams, focusing on how to draw them for both ionic and covalent compounds. It explains the octet rule, lone pairs, and bonding pairs of electrons. The guide also details exceptions to the octet rule, including incomplete and expanded octets. Several examples are provided, along with practice questions and a scoring rubric.
#Molecular Structures: Lewis Diagrams
Hey there, future AP Chem pro! š Let's dive into Lewis diagrams ā your key to visualizing molecules and predicting their behavior. This is a major topic, so let's get it down!
#What are Lewis Diagrams?
Lewis diagrams (or Lewis structures) are visual tools that show how atoms bond together. They display valence electrons and bonds, helping us understand molecular shapes and reactivity. Think of them as the blueprints of molecules! āļø
- Based on the octet rule: Atoms want a full valence shell (usually 8 electrons).
- Localized electron model: Electrons stay put (no free roaming).
- Electrons are either:
- Lone pairs: Electrons around a single atom, not shared.
- Bonding pairs: Electrons shared between atoms (represented by a dash).
#Drawing Lewis Dot Structures (LDS)
#Ionic LDSs
Ionic LDSs are straightforward because electrons are transferred from one atom to another. š
- Write the empirical formula to identify elements and their quantities.
- Draw each atom with its valence electrons.
- Transfer electrons from the metal to the nonmetal to achieve full octets.
- Use brackets around each ion with charges outside.
#Example: NaBr
- Formula: NaBr (one Na and one Br).
- Na has 1 valence electron; Br has 7. 3. Transfer 1 electron from Na to Br.
- Show charges: [Na]+ [Br]-
Ionic bonds transfer electrons! Think of it like giving away a gift. Metals give, nonmetals receive.
Try it: Draw the LDS for magnesium chloride (MgCl2). Answer at the end!
#Covalent LDSs
Covalent bonds involve sharing electrons, making their LDSs a bit more involved.
- Count the **total vale...

How are we doing?
Give us your feedback and let us know how we can improve