Bond Enthalpies
Sophie Anderson
7 min read
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Study Guide Overview
This study guide covers bond energetics, focusing on how energy changes during chemical reactions. It explains that breaking bonds requires energy (endothermic) and forming bonds releases energy (exothermic). The guide defines bond dissociation energy (BDE), describes BDE trends related to bond strength and length, and shows how to calculate the enthalpy of reaction (ΔH) using BDEs with the formula: ΔH = ΣH(reactants) - ΣH(products). It includes example problems, practice questions, and exam tips.
#AP Chemistry Study Guide: Bond Energetics
Hey there, future AP Chem master! Let's break down bond energetics – it's all about energy in reactions, and you've got this! 💪
#Introduction to Bond Energy
#The Basics
- Bonds aren't just lines on paper; they're packed with energy! 😲
- Key Concept: Reactions happen because bonds break and form. This is the heart of why reactions are exothermic or endothermic.
Breaking bonds ALWAYS requires energy (endothermic), while forming bonds ALWAYS releases energy (exothermic).
BARF: Breaking Absorbs, Releasing Forms. This helps you remember the energy flow during bond changes.
#Breaking Bonds: Energy In
- Think of it like snapping a twig 💥: you have to put in energy to break it.
- Breaking a bond requires energy input into the system.
Caption: Energy is required to break the bond between two atoms.
#Forming Bonds: Energy Out
- When bonds form, energy is released.
- This happens because the system goes to a lower potential energy state.
Caption: Potential energy decreases as atoms form a bond, releasing energy.
#Bond Dissociation Energy (BDE)
#What is BDE?
- Definition: The energy needed to brea...
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