Electronegativity: bond character/bond type: electronegativity difference and predicting bond type

[@josiemoreau7049]

to everyone watching this to study for their chem test, good luck

[@elmtutch1992]

Veryy great video! Covered a lot of stuff and was a step by step guide to electronegativity! I ended up learning more than I thought I would! Thank you

[@aesarahypatia3482]

This is great. Thank you so much for posting. I love your channel!

[@ser3nity6]

great video my teacher didnt go over this too much. thank you!

[@whirrrl3349]

Nice! Beautifully illustrated to drive home the concept. Thanks!

[@chemistrymattersgetit4161]

still doing brilliant work! (keep it up)

[@CrashChemistryAcademy]

Am trying! Thanks much for the comment.

[@msjanktk4882]

Nice and informative video.

[@alam9756]

U should be famous sir

[@CrashChemistryAcademy]

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[@user-hk1wl4qr3m]

nicely done! kudos! thanks so much.

[@bubbahotep6316]

Great lesson. Thanks!

[@bahschemistry1111]

Posted just in perfect timing for my class this week.

[@CrashChemistryAcademy]

😊👍

[@ramachandrakiranaddala3337]

Thanks for making the concept clear.

[@st_nickelouse9219]

abolutely AMAZING video

[@CrashChemistryAcademy]

Thanks!

[@lumpyppp]

soooo excellent

[@ReassuringSmile]

My mind is blown....

[@CrashChemistryAcademy]

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[@jsjsjjsshw]

How does the electronegativity difference between atoms dictate how polar the bond formed is?

[@CrashChemistryAcademy]

polarity is an uneven distribution of electrons in an otherwise neutral molecule (total # protons = total # electrons), making one side more negative, the other side more positive. Electronegativity gives the relative "pull" an atom has for electrons, so a more electronegative atom bonded to a less electronegative atom will have a greater amount of electrons around it, giving it a negative character, while the other atom, with less electrons, is more positive. The bigger the difference between that positive and negative, the more polar it is, and so the bigger the difference in electronegativity, the polar it is. You may want to see my video on polarity in molecules for more detail: kzbin.info/www/bejne/bWOmgphjlLV9i5Y

[@jsjsjjsshw]

@@CrashChemistryAcademy thank you so much!

[@JacobAbiola-ej4gr]

Amazing

[@CrashChemistryAcademy]

Thanks!

[@justtryna4318]

Thanks a lot sir..

[@fairycore7140]

I love it!

[@mnadeemferoz-ow7xp]

Electronegativity differences between hydrogen and fluorine is 1.8 . But why the bond between hydrogen fluoride is considered to be covalent not ionic?

[@CrashChemistryAcademy]

Great question! The 1.7 boundary between covalent and ionic is ambiguous at best, the two bonding types transition from one to the other, without a concrete boundary. The determination of ionic or covalent becomes more of an empirical exercise depending on the conditions & environment the compound is in, and what aspect of the bonding you are interested in. So let's look at the conditions in which HF exists: Most significantly it is a gas at room temperature, the HF molecule is isolated and therefore little influenced by its environment, and so the sharing allowed by their electronegativities is fairly consistent. Hydrogen's electron does spend the majority of its time closer to the fluorine atom, but a significant amount of the electron's time is also spent around hydrogen. That is because at any given moment that the electron is lost to fluorine, the hydrogen atom is a completely unshielded proton-- there are no other electrons in the hydrogen atom to repel that lone valence electron, and so the hydrogen exists as a naked positive charge and is easily able to momentarily grab back its lost electron. If you were to freeze HF into a solid, the bond would likely exhibit more ionic behavior. The multiple fluorine atoms close by would exert a larger attractive force, likely keeping hydrogen's valence electron away from the hydrogen atom for longer moments of time. Conversely, when solid ionic compounds are vaporized, they normally exist in the gaseous state as their empirical formula. For example, vaporized sodium chloride exists as individual NaCl "molecules" and in fact the NaCl bond takes on a more slightly covalent character in that gaseous diatomic state. I hope that answers your question!

[@miencyfratgyueev3]

sick man

[@CrashChemistryAcademy]

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[@zoomrusher9598]

very cool

[@alam9756]

What’s the difference/Relation between polarity and conductivity

[@CrashChemistryAcademy]

polarity refers to a distribution of charge within a molecule, whereas conductivity refers to the movement of charge. They are not quite related, but one connection would be bonded atoms with a large electronegativity difference (metal - non-metal) will often dissociate (split apart) when dissolved in water, creating positive and negative ions (charged particles) that can move in the water, which would allow them to carry an electric current through the water, and these are called electrolytes. It may help to watch my video on molecular polarity: kzbin.info/www/bejne/bWOmgphjlLV9i5Y

[@alam9756]

@@CrashChemistryAcademy bless you.. I already watched it

[@thea-kl1rz]

hi primez

[@fukpoeslaw3613]

so, what exactly is the macro property of polarity

[@CrashChemistryAcademy]

For example water is polar. At the macro (every day) level, we see water attract to a variety of substances that have any kind of charge distribution, either large or small. However, C-H bonds, even though polar (non-zero electronegativity difference of 0.3), appear to manifest non-polar behavior, such as lipids--there are certainly other factors to account for, such as what other atoms are bonding as well as molecular shape, but that is basically what I was getting at.

[@fukpoeslaw3613]

@@CrashChemistryAcademy aha, I understand it now, thanks!

[@returnofthemomos]

first

[@CrashChemistryAcademy]

OWEN! I thought you left. Glad you're back.