Electron Configurations Using the Periodic Table

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A crash course on using the periodic table to find electron configurations.
Other CC Academy videos for step by step Chemistry help on your chemistry homework, problems, and experiments:
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- Quantum Numbers
- Rutherford's Gold Foil Experiment, Explained
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- Effective Nuclear Charge, Shielding, and Periodic Properties
- Electron Configuration Tutorial + How to Derive Configurations from Periodic Table
- Orbitals, the Basics: Atomic Orbital Tutorial - probability, shapes, energy
- Metric Prefix Conversions Tutorial
- Gas Law Practice Problems: Boyle's Law, Charles Law, Gay Lussac's, Combined Gas Law
-More on Electron Configuration: Wikipedia-
"In atomic physics and quantum chemistry, the electron configuration is the distribution of electrons of an atom or molecule (or other physical structure) in atomic or molecular orbitals.[1] For example, the electron configuration of the neon atom is 1s2 2s2 2p6.
Electronic configurations describe electrons as each moving independently in an orbital, in an average field created by all other orbitals. Mathematically, configurations are described by Slater determinants or configuration state functions.
According to the laws of quantum mechanics, for systems with only one electron, an energy is associated with each electron configuration and, upon certain conditions, electrons are able to move from one configuration to another by the emission or absorption of a quantum of energy, in the form of a photon.
Knowledge of the electron configuration of different atoms is useful in understanding the structure of the periodic table of elements. The concept is also useful for describing the chemical bonds that hold atoms together. In bulk materials, this same idea helps explain the peculiar properties of lasers and semiconductors."
Wikipedia contributors. "Electron configuration." Wikipedia, The Free Encyclopedia. Wikipedia, The Free Encyclopedia, 5 Jan. 2016. Web. 27 May. 2016.

Опубликовано:

7 окт 2011

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Комментарии : 50

@icyylemur 4 года назад

This is amazing. I’ve been so confused and asking people for help. Everyone is so confusing. But I watch this confused. And pause at a certain point. And after a quick look, it is glued to my head. You helped me so much for my test. You deserve way more on this video

@DogLover1o144Three4 8 месяцев назад

THANK YOU SO MUCH!!! Ive been stuck on this concept for nearly a month, and within FIVE MINUTES you helped me figure out this concept that i couldt learn for 23 days. Thank you so much!

@katherinnegarcia2165 9 месяцев назад

From someone who didn’t understand this at all, this is AMAZING! THANKYOU !!!

@mehdialikermally 2 года назад

thank you for successfully explaining an entire subchapter of the MCAT Chem Review in

@goatwhisperer6502 2 года назад

I was also stuck on this exact subchapter lmao

@1superNORRIS 10 лет назад

I have a chemistry test over quantum's and electron configuration tomorrow and I missed the class where the teacher taught us this and she didn't teach me it so thank you so much for making this easier to understand!!!!

@blissfulfragrance2511 6 лет назад

It's weird how the person who made this is so *straightforward & clear* but when my school chemistry teacher attempts to explain stuff its *mind-numblingly confusing* 😕

@maggiemurphy4739 7 месяцев назад

Omg same my teacher was a long term substitute who never taught chemistry and when she started to teach this she said I didn’t know if I’m doing this right

@maxymtaras2464 9 месяцев назад

THANK YOU, this is exactly what I was looking for. I went through a few videos before this one, and they were not covering this specific concept. I appreciate it!!!

@karladelmoral3955 Год назад

This was the best explanation I have ever seen of Electron configuration using the periodic table!! I have studied this so many times, and I could never fully grasp it until now. Thank you so so much!

@CrashChemistryAcademy Год назад

Thanks!

@WharfRat44 11 лет назад

Thank you very much! This helped me so much. It's an easy concept and I was giving it too much thought.

@aspektn.5066 4 года назад

Seen once, shall be seen again. Good vid.

@mandisamkhize4475 9 лет назад

another epic video thank you!

@yamsang0__0 5 лет назад

Aye I’m pretty happy you included noble gas configuration lol

@lmshan11 10 лет назад

incredibly helpful, thanks!

@chiefkeefsson9979 7 лет назад

holy crap this man is a genius

@Chem5724 Год назад

Wonderful and impressive way to make the concept very clear

@ronaldinho031003 11 лет назад

Thank you!

@mituot4746 2 года назад

I spent an hr looking at my book without understanding what it said and this awesome man explain it in not even 5mins and i got it!!!!

@joelweiner4156 2 года назад

😊

@catalinadelafuenteordaz4535 4 месяца назад

Thank youuuu for this

@charlie13albert 10 лет назад

What tool or app did you use to show to demonstrate this?

@Lutopian 7 месяцев назад

my god you you saved my skin with this video

@Jdklajfl 9 месяцев назад

Very easy to understand, thank you so much! This saved me

@CrashChemistryAcademy 9 месяцев назад

Great!

@nickatinaaa 3 года назад

wow thank you sooo much! im excited for my exam now lol

@mumbabig4l552 7 месяцев назад

U the goat bro

@milanadela7781 2 года назад

Oooooh so the vertical column is how many layers there are and the horizontal one is how many there are on the last layer. Thanks a lot!

@ace0415 11 лет назад

if i had just watched this before my mid term today..... oh god

@Rebeccatriplet 11 лет назад

this was really helpful, but at the beginning you switched the positions of the d block and p block

@aspektn.5066 4 года назад

The last you said, about d-block being one less than the row, what was that about?

@CrashChemistryAcademy 4 года назад

The rows (periods) are numbered, and that number is equal to the prinsiple energy level of the s and p electrons (4s and 4p are in period 4) however the d electrons are one less than the period number (3d is in period 4). Hope that helps!

@aspektn.5066 4 года назад

@@CrashChemistryAcademy Appreciated. Haven't noticed that. Is all of this 'cause elements fill their s-subshell of a higher orbital before getting to the d-subshell?

@CrashChemistryAcademy 4 года назад

@@aspektn.5066 Yes, although we'd have to look at Schrodinger's equation to find the real answer, which is beyond me.

@imverymentallystable7609 2 года назад

Thanks for saving my life

@joelweiner5877 2 года назад

anytime!

@monicawai3125 6 лет назад

tankyou

@wehaadkhamo9619 9 лет назад

Don't you have to use the Aufbau Diagram when you reach the 4th period in the periodic table?

@wehaadkhamo9619 9 лет назад

Oh ok, thank you. You explained it way better than my chemistry teacher. Thanks for the video!

@CrashChemistryAcademy 11 лет назад

The f-filling elements (inner transition elements) do not conform well to rules of electron configurations. For example, #64 is [Xe]4f7 5d1 6s2 while #65 is [Xe]4f9 6s2. just do an internet search for the electron configuration of any element, you'll get lots of links.

@Martin_Z555 4 года назад

you mixed the D's and P's at the beginning! you can make a little annotation to fix it in post!

@ayshaanwar5643 9 лет назад

0n 0.15 when you show the s,p,d,f in colour you kinda made a mistake by writing p instead of d and viceverca

@kisho2679 Месяц назад

Since for the electron configiration of the d-bock periods you have to subtract -1, so why are those d-block periods not just depicted one row abowe in the periodic table of elements (then it would be easier to directly read instead of conducting this subtraction as exeption)?

@CrashChemistryAcademy Месяц назад

The periodic table was originally organized according to properties and weight (1869), the weight was replaced by #protons (1917), but that did not change the organization. That organization was later found to fit perfectly with electron organization (late 1920s). So the answer to your question lies in electron organization and Schrodinger's original quantum mathematics from 1926. The mathematics gives a simple formula for how many electrons will occupy a given energy level (principle quantum number, n), which is 2n^2. Another organizing principle is that when going from one block to another on the periodic table, the added electron will go to the next higher energy level in the very specific order given in electron configurations. This is the aufbau principle. OK, so what happens when going from 4s to 3d? The issue here is that 1) the 3d orbital has a slightly higher energy than the 4s orbital, and so 3d has to be filled after 4s. 2) This also allows for the fullfilment of the 2n^2 rule. The reason 3d has more energy than 4s is due to angular momentum. The shape of the 3d orbital is far more convuluted than the simple sphere of 4s, which in turn requires that the 3d electron have a much greater angular momentum (which translates to more energy) than a 4s electron. The same explanation tells us why 4f comes after 6s, and why 5d comes after 4f. I hope that makes sense!

@kisho2679 Месяц назад

Thx