1.6 Intermolecular Forces | Organic Chemistry

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Chad, you have re-ignated all of the semantic networks in my brain from O-chem and all of GenChem that I was reluctant to re-learn for a huge test. I cant thank you enough for your talent for teaching. I feel like im back at office hours.

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Excellent - thanks for sharing and good luck on your test!

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Chad, I just wanted to take a moment to tell you how appreciated you are. Your lectures completely blow away those of most instructors as far as in how well you are able to explain the material in a way that makes sense to us. Thank you for your time and hard work you've put into providing us all with supplementary material for helping us better understand the concepts that we may have been confused about in class.

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There is a lot of content of KZbin but I have a methodical way that I prefer to learn. Your channel is laid out in a way that builds up and makes sense of one thing at a time. I study part time and my study guides are not helpful at all with the way I like to learn. Thank you for creating these videos and also the playlists that take us through the chapters and concepts one by one. Really neatly laid out and well explained. The gift of education surpasses any other. God bless brother.

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I am so glad i found this channel. My prof could not explain this in a week. You made it so clear, thanks Chad!

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Best examples for solubility and ranking boiling points! Chad you're the BEST!

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Thanks Gabrielle! I do my best to choose examples to cover the different types of questions students are likely to encounter on exams. Glad you found this helpful!

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[@sciencenerd7639]

I think it's just kind of nice to know that melting point trends don't always match boiling point trends, even though exact nuances aren't always very predictable. Great lecture, thanks so much.

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Literally this video saved me before my chem exam!! You explain things so well!! THANK YOUUU

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was having trouble with this topic. have my acs on monday - tysm!!

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Great lecture

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[@meenashivapuram6920]

Thx a lot Chad! This was a beautiful lecture. But why does the compound having more number of carbons are more soluble in a polar substance? Tho bigger non polar region decreases hydrogen bonding between a few compounds in the solution

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fantastic video

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[@mayarise4242]

Hydrogen Bonding Definition: The strongest type of dipole-dipole interaction. Criteria: Occurs when hydrogen is bonded to highly electronegative atoms such as fluorine, oxygen, or nitrogen. Example: Water (H₂O) molecules, where hydrogen bonds form between the hydrogen of one molecule and the oxygen of another. Dipole-Dipole Forces Definition: Attractive forces between polar molecules. Example: Hydrogen chloride (HCl) molecules, where the partial positive charge of hydrogen is attracted to the partial negative charge of chlorine in adjacent molecules. London Dispersion Forces (Van der Waals Forces) Definition: The weakest intermolecular force, present in all molecules. Mechanism: Temporary dipoles caused by momentary distributions of electron density. Example: Present in all molecules, but especially noticeable in nonpolar molecules like methane (CH₄). Ion-Dipole Forces Definition: Attractive forces between an ion and a polar molecule. Example: Sodium chloride (NaCl) dissolved in water, where the Na⁺ ions interact with the partial negative charge on water's oxygen atoms, and Cl⁻ ions interact with the partial positive charge on water's hydrogen atoms. Importance of Intermolecular Forces Properties Affected: Boiling and Melting Points: Higher intermolecular forces result in higher boiling and melting points. Viscosity: Stronger intermolecular forces lead to higher viscosity. Surface Tension: Higher intermolecular forces result in higher surface tension. Vapor Pressure: Higher intermolecular forces lead to lower vapor pressure. Examples and Applications Hydrogen Bonding: Example: Water (H₂O) exhibits strong hydrogen bonding, leading to its high boiling point relative to its molecular weight. Dipole-Dipole Forces: Example: HCl exhibits dipole-dipole interactions due to its polar nature. London Dispersion Forces: Example: Methane (CH₄) only has London dispersion forces but they increase with larger molecules. Ion-Dipole Forces: Example: NaCl in water demonstrates strong ion-dipole interactions, which are significant in dissolving salts. Ranking Boiling Points Network Covalent Solids: (e.g., diamond, SiO₂) have the highest boiling points. Ionic Compounds: (e.g., NaCl) also have high boiling points. Molecular Compounds with Hydrogen Bonding: (e.g., water, NH₃) have lower boiling points than ionic compounds but higher than those with only dipole-dipole or dispersion forces. Molecular Compounds with Dipole-Dipole Forces: Lower boiling points than hydrogen-bonded compounds. Molecular Compounds with London Dispersion Forces: Typically have the lowest boiling points among molecular compounds. Branching and Boiling Points Effect of Branching: More Branched Molecules: Lower boiling points due to reduced surface area and weaker dispersion forces. Example: Isomers of pentane show different boiling points based on branching. Solubility Principle: Like dissolves like. Polar Solvents: Dissolve polar solutes (e.g., water dissolves salt). Non-Polar Solvents: Dissolve non-polar solutes (e.g., hexane dissolves oils).

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