13 - Chemistry 1000 Lecture 13 Enthalpy of lattice...

Info iconThis preview shows pages 1–5. Sign up to view the full content.

View Full Document Right Arrow Icon

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: Chemistry 1000 Lecture 13: Enthalpy of lattice formation Marc R. Roussel Enthalpy of lattice formation Definition: enthalpy change when an ionic compound is formed from the corresponding gaseous ions . Symbol: Δ lf H Example: For NaCl, Δ lf H is Δ H for the reaction Na + (g) + Cl- (g) → NaCl (s) What is this for? This is a measure of the strength of ionic bonding in the solid state. Enthalpy of lattice formation Notes 1. Enthalpy of lattice formation is not directly measurable. 2. Your textbook deals with lattice energy instead of an enthalpy. Either is legitimate, and quantitatively the two are very similar (differences of a few kJ/mol out of several hundred). The small differences are insignificant given the uses made of these numbers. 3. The enthalpy of lattice formation is somewhat more commonly calculated than the lattice energy. 4. Confusingly, most textbooks that calculate an enthalpy incorrectly call it a lattice energy. Review of thermochemistry I Standard enthalpy of formation (Δ...
View Full Document

This note was uploaded on 03/03/2012 for the course CHEM 1000 taught by Professor Marc during the Fall '06 term at Lethbridge College.

Page1 / 9

13 - Chemistry 1000 Lecture 13 Enthalpy of lattice...

This preview shows document pages 1 - 5. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online