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Understanding Molecular Shapes and Intermolecular Forces

This review covers fundamental concepts in molecular geometry, including shapes like linear, trigonal planar, bent, tetrahedral, and more. It explores hybridization, explaining how sub-orbitals mix, and discusses polarity, detailing how differences in electronegativity create negative and positive dipoles. The principles of miscibility and immiscibility are outlined, emphasizing the importance of polarity. Additionally, it delves into intermolecular forces, including London dispersion forces, dipole-dipole interactions, and hydrogen bonds, providing a comprehensive view of how molecules interact and behave in various phases.

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Understanding Molecular Shapes and Intermolecular Forces

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  1. Bonding and Solution Review

  2. Shapes • Linear • Trigonal Planer • Bent • Tetrahedral • Trigonal Pyramidal • Trigonal Bipyramidal • See-Saw • T-shaped • Octahedral

  3. Hybridization • Tells you the mix of sub orbitals • s- 1, p-3, d-5, f-7 • Flower petal method

  4. Polarity • Polarity occurs when there is a disturbance (unequal sharing) of the electrons caused by a large difference in electronegativity's. • Atoms that pull the electrons towards themselves are called negative dipoles (-δ). • Atoms that do not have the electrons close to them are called positive dipoles (+δ).

  5. Miscible- “like dissolves like” same polarity (polar or nonpolar). • Immiscible – will not mix, different polarity.

  6. IMFs • Forces holding molecules to other molecules (inter…between) • London Dispersion Force (LDF)- every molecules has this. As the molecules size/ mass/ # of e- increases so to do the LDFs. • Dipole-Dipole- only polar molecules have this…attraction between opposite dipoles of other molecules. The more polar the molecule is the stronger the force. • Hydrogen bond- a type of dip-dip seen when H is bonded with a N, O, or F. The smaller the molecule the stronger the H-bond is.

  7. Phase Diagram

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