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THANK YOU ALL THE FROM ZAMBIA.

how about c-c triple bonds sir?

I will most definitely consider a like and share !

i was in my second year along with 28K subs. now u got 100K Chad! woohoo 🥳

I think I am in love with you in an academical way, sir.

I would like to mention that another major difficulty of fusion power plants (which is very little talked about) is the difficulty of producing tritium, which is not found in nature and is currently recovered by nuclear fission power plants

what i wanna know is, who are the 18 people that dislike this video.

I'm taking Ochem 1 in the summer, which is super fast-paced. Your videos help so much. Thank you.

Thank you for making higher education syllabus available freely for inaccessible students!

Thank you Chad, you're the best teacher on YT!!!

Thanks Mr.Chad...From Sri Lanka

The golden rule is to like before you watch 😊😊

You deserve more subscribers

Well explained

wonderful lesson as always. But shouldn't oxygen 16/8 + alpha particle give carbon 12/6?

I recommend you to all my classmates!

thank you! could you please explain if C is always obligated to undergo promotion in order to get hybridized?

congrats on 100K. well deserved

Yes i am preparing for jee can you help by doing a separate Playlist for that or it is ok

Nice explanation

OMG THANK YOU THESE VIDEOS ARE THE BESTTTTT!!!!!!!! :)))))))))))))

u r a herooooo!!!!!!!!

Talks too fast😢

24:49 So if normal force is 490 N and positive as you annotated, does the weight now become negative?

u look like the guy on the speedboat who faceplanted

Me running 🏃‍♂️ to call all the chemistry students to come and watch this wonderful explanation

I think it will be more understandable if he wrote the carbon bonds rather than drawing those lines

Thanks

that explanation about oxidation state was superb. i finally understand it. thanks so much. congrats for 100K subscribers!

Would love to learn more!

thank you❤❤

Thank you, Chad, God Bless.

Congrats on 100k

thank you ❤❤

thanks for simplifying this. when it comes down to it the math and the logic aren't that difficult, but i appreciate the clarity of your lecture (like all ur others)

Congratulations on 100K! YOU DESERVE IT!!! I can't thank you enough for helping me with most of my classes! You are doing many great things with assisting so many students. May God bless you and may He be with you always ☦

thank you.♥♥

Sir I now understand it after ur explaination

3:15 we call that the PP orbital LOL sorry couldn't help myself

hey man, I've passed Chemistry 1 and 2 with you. Thanks.

Best professor ever

Man i love u so much, i tried varity of youtube channnel nothing helped me the way u did , thank you so much

You Break it down

please write a textbook, I will pre-order right now. ;) Got a 91 on exam

GOD BLESS YOU!

can't LiAlH4 lead to a 3° alcohols?

our assignment also had water along with the hydrohalic acid and i'm kind of thrown off. do i get an alcohol from reacting that water with the resulting alkyl halide?

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).

Electronegativity and Polarity Electronegativity: A measure of an atom’s ability to attract electrons in a bond. Polarity Rules: Non-Polar Bonds: Identical atoms (e.g., H₂) have no difference in electronegativity. Polar Covalent Bonds: Differences in electronegativity between 0.5 and 1.7. Ionic Bonds: Differences in electronegativity greater than 1.7. Key Bonds and Their Polarities Carbon-Hydrogen Bond: Non-polar (difference in electronegativity = 0.4). Carbon-Nitrogen Bond: Polar covalent (difference = 0.5). Carbon-Oxygen Bond: Polar covalent (difference = 1.0). Carbon-Fluorine Bond: Polar covalent (difference = 1.5, approaching ionic character). Sodium-Chloride Bond: Ionic (difference = 2.1). Exceptions Carbon-Magnesium Bond: Despite being a metal and a non-metal, this bond is polar covalent (difference = 1.3), not ionic. Identifying Polar Molecules Step 1: Look for polar bonds within the molecule. Step 2: Check the orientation of these polar bonds: If the vector sum of bond dipoles cancels out, the molecule is non-polar. If the vector sum does not cancel out, the molecule is polar. Examples of Molecular Polarity Carbon Dioxide (CO₂): Non-polar because the bond dipoles cancel out (linear shape, bond angles of 180°). Carbonyl Sulfide (COS): Polar because the bond dipoles do not cancel out (due to different electronegativities of oxygen and sulfur). Methane (CH₄): Non-polar with no polar bonds. Chloromethane (CH₃Cl): Polar with a dipole moment of 1.87 D. Dichloromethane (CH₂Cl₂): Less polar than CH₃Cl (dipole moment of 1.6 D) due to the bond angles causing partial cancellation. Trichloromethane (CHCl₃): Even less polar (dipole moment of 1.01 D). Tetrachloromethane (CCl₄): Non-polar as the four polar bonds cancel out. Dipole Moments Definition: A measure of the polarity of a molecule, represented by the symbol μ. Calculation: Depends on the difference in partial charges and the distance of separation.