Sir i don’t know how to thank u! Nobody could make me understand what this was! I have an exam in 10 days and with ur help i shall pass! Thank u thank u thank u!!!
Good video. Here's a teaching tip for you. In the beginning you say "It's actually very easy". It's only easy for you because you understand it already. When you started chemistry, I am sure it was hard, and then you learned and it became easy. For all beginners watching your video it's complicated, hard stuff. So it's better to start your video with "this is pretty complicated but after watching this video I'm sure you'll understand it better". Also you leave out some stuff that's relevant, like the maximum number of electrons in shells. You should provide a diagram that shows the maximum number per shell, so it becomes obvious. Otherwise people can be confused as to why you suddenly jump to the next shell.
thank you bro. I knew how to do the drawing, but using the period no. and group no. was new to me. thanks for your hep and plssss do keep making such helpful videos.
This is only a doubt. At 4:21, you told that the 3rd shell can hold 8 electrons, but in our chemistry lessons, we have learned the formula 2n^2. Accordingly the 3rd shell should be having a capacity of 18 electrons. Please reply so i can clarify my doubt, because even in other videos, they show it like this and i dont seem to understand which i should cope with. Hope you will reply soon
An excellent question! TL:DR, we're both correct. The order of filling electrons is a little messy - so in senior chemistry we abandon this method (rings) for something that's more precise. But it's still messy though. The third shell does hold a maximum of 18 (obeys the 2n^2 rule), but when filled with 8, it then gets left behind until later on until the 4th shell gets its first 2 electrons. From there onwards, 10 more electrons are added to complete the 3rd shell. I often tell my students that the 3rd shell holds 8... then 10 more later (=18). I suspect that because of this confusion/limitation of the Bohr model (rings), we don't ask students to draw atoms larger than Calcium like I show in the video.
this is so helpfull thank you so much for helping. but there is some partsthat i stil dont understand. you said we need need to see the back of group is the last shell answer but my teacher said it's wrong can you help me ;[ because i have a chemistry test tommorow and i don't rlly understand. if youhelp me i'm gonna be so thankful thank you so much for these videospleasemake more ;]
I'm having trouble understanding how to balance the electrons in the outermost shell. Like if there are two electrons, should the electrons be together at 1 point or opposite one another?
we can find the total number shells that can be accommodated using the equation 2*nsquare. Can we write the electronic configuration using this euation .So K,L,M,N,O shells can accommodate k=2 L=8 M=18 N=32 please answer it quikly
Hi Paul, yes you can determine the maximum number of electrons possible per electron shell using 2n^2 (with n=shell number). And yes, K, L, M, N, O shells do fit 2, 8, 18, 32, and 50 respectively. I think I have seen electron configurations expressed using KLMNO letters but I'm not familiar with that method.
I found this video very helpful, especially the combination of the visual diagram with the verbal explanation. However, in class, our Professor explained the third shell to contain 18 electrons, and the 4th shell to contain 32 electrons. I've concluded this to be correct through other various resources, including our text: Fundamentals of General, Organic, and Biological Chemistry - 7th edition by McMurry, Ballantine, Hoeger, and Peterson. Is your video an explanation of Organic atoms? Or, why does it explain up to 8 electrons in the third shell, and 2 electrons in the fourth shell?
Your professor & textbooks are correct (and so am I). The third shell does indeed hold 18 electrons at maximum - however it won't fill in the remaining 10 (I only cover as far as filling it with 8 in the examples) until you reach the end of the first row of d-block elements (zinc). It's weird, since those elements are in the 4th row but they fill the 3rd shell... this is where the Bohr model of electron configurations breaks down - most people give up and learn the Quantum Mechanical Model (like the example at the end of the video) for electron configurations since it covers this weirdness more accurately.
Why is the group number of O 16? I get that Ca is in column 2 and has 2 valence electrons. I would have said that O was in group 6. How do you figure 16? Where does that initially come from?
Every other video that I watch says something different. Half of the videos say 2-8-8, the other half say 2-8-18. Which is it, it can be both, are we counting the sub shells, or are we not?
The technical limits are 2, 8, 18, and so on. However, the main reason why we're interested in knowing what the limits are per energy level is to determine if the electron configuration is stable or not. Atoms with configurations of 2, or 2,8, or 2,8,8, or 2,8,18 are all stable. Things get weird between that 8--->18 stage of the 3rd energy level which is where this basic 'Bohr' model of the atom reaches its limits and you need to look into the Wave model (aka wave mechanical model, or quantum model, think schrodinger).
They're often listed at the top going from 1 to 18 across horizontally. If you don't see them (it depends on the style of periodic table) you can just count how many columns from the left side. That's the group number.
Hi Henrik. It's a really difficult question to answer: 1. It's difficult to convey in text 2. It requires more advanced chemistry to explain (quantum mechanical model) - so if you're quite early/young in your chemistry journey, I'd only make things more confusing by giving you the answer. I'll try my best, but it comes down to the limitations of the Bohr model of the atom (the illustrations we use with concentric rings with electrons on them). Bohr's model assumes that electrons exist in defined 'energy levels' - you might call them electron shells* but I'll be calling them energy levels from now on because that's important for this explanation. Erwin Schrodinger in more recent history put forth the idea of the Quantum model (or quantum mechanical model), which conveys that electrons exist in one or more sub-shells (orbitals) for each energy level. This helped fix the flaws in Bohr's model (e.g. explaining emission spectra for elements other than hydrogen) This means that when filling in electrons, you need to consider the lowest energy 'orbital' rather than the lowest energy level*. Everything is fine until Argon, 2,8,8 who has filled the 1st and 2nd energy levels* (and its orbitals), but not fully filled its 3rd energy level*. When you proceed to Potassium 2,8,8,1 this is where the 3rd and 4th energy levels* overlap in their orbitals' energy. As you know, electrons will fill up from lowest to highest energy as possible. So after Argon, electrons will fill 2 electrons into the 4th energy level, since one of its orbitals is lower in energy, than the 10 remaining vacant spots in the orbitals of the 3rd energy level. Now after calcium, you'll start finishing off the 10 vacant spaces until you reach Zinc. If you have the benefit of talking with a chemistry teacher, share with them what Iv'e written so they can expand upon it, and note that I've deliberately tried to avoid mentioning s, p, d, and f in my explanation to keep things as simple as I can.
+Demolition Bomer It probably makes sense in another video of mine where I show a picture of the periodic table, such as writing ionic formulas. I drop off the 10 because there are 10 groups (columns) of elements in the 'd-block' of the table that have no elements in them in the top 1/3 of the table. so really, only groups 1-2 and 13-18 are used for the top part of the table (that makes 8 groups left to right, so group 1 has one electron, group 2 has two electrons, group 13 has three electrons, etc)
can you please tell me why the i nermost shell has the lowest energy and outer has the highest energy is it true the angular momentum appeared as energy i cant figure it out please help me and please tell me the way how to find energy of the shells hope you reply soon
I'm sorry but I'll have to admit that your question goes beyond my expertise. In most cases, it's not important for everyday chemistry to understand the maths/physics of the energy levels. If your maths is strong enough, you might find the answers you're after in the Wave Equation, or the Quantum Mechanical Model (Schrodinger). Again, the mathematics of the quantum mechanical model are beyond me.
but why innermost has higher energy and which thing present there in an atom which we are calling energy what is this kinetic potential or what kind of thing there appeared as energy
why the protons are always held together although they have same charge i found answer that the nuclear force hold them together but from where that force comes up
Electrostatic Repulsion works over longer distances, whereas the nuclear force is greater at shorter range, so if the protons are close enough, the nuclear/strong force is much greater than their electrostatic repulsion. Neutrons help too - as charged particles are attracted to neutral particles as well as oppositely charged particles. You're asking physics questions and not chemistry questions I'm afraid you'll need to find someone who specialises in nuclear physics.
i am from pakistan where i am living in a lower class area where things like science obviously not explained well thats why i am asking questions from you was my questions are not right ..............??????? Or these questions have no sense
I'm presuming you're asking about the Group number 16, and remove ten? It's to do with the fact that for the first few rows (periods as they're called) of the table, there aren't any elements sitting in the middle. e.g. there's a gap between Berylium, and Boron. The gap is exactly ten spaces. You'll learn more in-depth about that gap section (the 'd-block' elements sit right under there) when you take a senior chemistry class. Not really necessary to know when you're just starting out.
I would disagree that they always come in pairs... but you are right - it's odd that they are conventionally drawn on opposite sides rather than paired together like you suggest. I think you'll like the Quantum Mechanical Model for electron configurations a lot more :)
Oh my gosh - I hadn't considered the placement of subtitles before. You've made a really good point and I will try to make more space at the bottom in future videos for the subtitles. Some of my students depend on them too if English isn't their first language so thank you for sharing the constructive criticism!
Hi David, I'm just sticking to the simpler bohr-model electron configurations. Subshells weren't part of his theory at the time until Schrodinger came along.
Technically, you would have to put 2 of them into the s-subshell and the 4 remaining in the p-subshell, as per the Aufbau principle and Madelung energy ordering rule en.wikipedia.org/wiki/Aufbau_principle
I'm not sure what you're asking about. In any case, I do wish you good luck with your research. Don't forget that you can ask for help from your teachers/lecturer/professor.
Curious, why would you prefer standing? It would be more challenging in this case because I've got my computer & wacom tablet just below that I'm using to illustrate in real-time.
Hey, don't give up - if this is something that you're passionate about then take a look around - there might be other teachers, or RUclipsrs out there that can explain it in a way that works for you. Also keep in mind that many things take time until they really make sense.
Depends on how old-school your periodic table is, or perhaps it's even been simplified for junior classes. It's group 16 or 6 depending on whether they give group numbers to the d-block elements in the middle of the table (Sc to Zn).
you explain this so much better then my teachers, all they do is yell at use and expect use to understand, then get made that we dont
I was always confused with this subject, but you and the periodic table song have helped immensely. Thanks!
Me too ❣️
I can't believe it took me this long to find your videos. They're amazingly helpful!
:) I'm so glad that these videos have helped you.
Sir i don’t know how to thank u! Nobody could make me understand what this was! I have an exam in 10 days and with ur help i shall pass! Thank u thank u thank u!!!
That's it. I'm subscribing to this guy.
very helpful, and comprehensible! please proceed to making more of these videos! thanks!
Good video. Here's a teaching tip for you. In the beginning you say "It's actually very easy". It's only easy for you because you understand it already. When you started chemistry, I am sure it was hard, and then you learned and it became easy. For all beginners watching your video it's complicated, hard stuff. So it's better to start your video with "this is pretty complicated but after watching this video I'm sure you'll understand it better". Also you leave out some stuff that's relevant, like the maximum number of electrons in shells. You should provide a diagram that shows the maximum number per shell, so it becomes obvious. Otherwise people can be confused as to why you suddenly jump to the next shell.
The best vid on Electron Configuration
Agreed 👍
This 7 minute video made me understand what my chemistry teacher failed to do in a month.
First time I have confused on this topic but now saw i understand suddenly😍
The way you explained this made me understand it faster than my own cram school science teacher
ok i just want you to know that you and you alone helped me to understand electron configuration. thank you so much
Wi3Gamers You're welcome, I'm pleased to hear that it helped you so much : )
Super. Even the quick 2 minute alternative electon config way. Nice job.
Dang I'm in 8th grade and I have to do it the hard way where you write it in a very specific way. Life sucks but you help man.
The video I came from did this wrong! I thought something seemed off, and this video confirmed it. Thank you.
No worries ^_~
thank you bro. I knew how to do the drawing, but using the period no. and group no. was new to me. thanks for your hep and plssss do keep making such helpful videos.
+Rahul Menon yeah the tricks really make it easy don't they?
Angles and Acid yes they do
This is a awesome video on explaining electron configuration and thank you so much sir.keep on doing the great job sir.
thx a lot sir it helped me so much as i had some confusions related to this topic
thx a lot and i hope it is gonna to help in my exams overhead
You're welcome :)
oxygen was straight forward but calcium wasn't just because you jumped a few steps but I figured it out. thankyou.
Aww your so cute! thanx for the help, you made it easy for me to understand.
juanita arbelo I'm glad it helped :)
bruh thanks you for this, helped me remeber your a life saver!!!
nichlous soomaru You're welcome :)
This is only a doubt. At 4:21, you told that the 3rd shell can hold 8 electrons, but in our chemistry lessons, we have learned the formula 2n^2. Accordingly the 3rd shell should be having a capacity of 18 electrons. Please reply so i can clarify my doubt, because even in other videos, they show it like this and i dont seem to understand which i should cope with. Hope you will reply soon
An excellent question! TL:DR, we're both correct. The order of filling electrons is a little messy - so in senior chemistry we abandon this method (rings) for something that's more precise. But it's still messy though. The third shell does hold a maximum of 18 (obeys the 2n^2 rule), but when filled with 8, it then gets left behind until later on until the 4th shell gets its first 2 electrons. From there onwards, 10 more electrons are added to complete the 3rd shell. I often tell my students that the 3rd shell holds 8... then 10 more later (=18). I suspect that because of this confusion/limitation of the Bohr model (rings), we don't ask students to draw atoms larger than Calcium like I show in the video.
sublevels
I saw many videos only for this confusion
this was so helpful I have a bio final coming up tomorrow and I FINALLY understand this!! Thank you so much! :)
Excellent! I'm glad to hear that.
thx a lot!!! this video helped me soooo much!!! I feel more nerdy!
Umanga Ruhunage You're welcome :)
Your awesome man I couldn't figure the electrons confurtion when is searche it up I get the other complex way of writing it thanks dude
simply yet clear!!! thanks for this video.. bravo!
Amazing :-) I just love this video. Its just so simple and easy, it's very very very helpful... thanks alot!
THANKYOU for uploading this video,it was very informative and helpful! :D
Wow thanks for your help
thanks this really helps on my exams
Glad it helped :)
Your really helpful, just earned your self a sub !!!!
Thanks :)
Thnx
Thank for this, I am subscribing you.
This helped me a lot! Thank you so much :)
You're welcome :) glad it was so useful! Check out my chemistry 101 playlist for other odds and things if you want
Not bad, this guy did a good job!
Thanks :)
this is so helpfull thank you so much for helping. but there is some partsthat i stil dont understand. you said we need need to see the back of group is the last shell answer but my teacher said it's wrong can you help me ;[ because i have a chemistry test tommorow and i don't rlly understand. if youhelp me i'm gonna be so thankful thank you so much for these videospleasemake more ;]
I'm having trouble understanding how to balance the electrons in the outermost shell. Like if there are two electrons, should the electrons be together at 1 point or opposite one another?
You explained me everything
hello could you make another video on drawing and writing electron configurations from scandium to strontium
Wow thanks for this mr❤❤❤
we can find the total number shells that can be accommodated using the equation 2*nsquare. Can we write the electronic configuration using this euation .So K,L,M,N,O shells can accommodate k=2 L=8 M=18 N=32 please answer it quikly
Hi Paul, yes you can determine the maximum number of electrons possible per electron shell using 2n^2 (with n=shell number). And yes, K, L, M, N, O shells do fit 2, 8, 18, 32, and 50 respectively. I think I have seen electron configurations expressed using KLMNO letters but I'm not familiar with that method.
I found this video very helpful, especially the combination of the visual diagram with the verbal explanation. However, in class, our Professor explained the third shell to contain 18 electrons, and the 4th shell to contain 32 electrons. I've concluded this to be correct through other various resources, including our text: Fundamentals of General, Organic, and Biological Chemistry - 7th edition by McMurry, Ballantine, Hoeger, and Peterson. Is your video an explanation of Organic atoms? Or, why does it explain up to 8 electrons in the third shell, and 2 electrons in the fourth shell?
Your professor & textbooks are correct (and so am I). The third shell does indeed hold 18 electrons at maximum - however it won't fill in the remaining 10 (I only cover as far as filling it with 8 in the examples) until you reach the end of the first row of d-block elements (zinc). It's weird, since those elements are in the 4th row but they fill the 3rd shell... this is where the Bohr model of electron configurations breaks down - most people give up and learn the Quantum Mechanical Model (like the example at the end of the video) for electron configurations since it covers this weirdness more accurately.
thx sir it was my doubt also
thanks so much!this really helped me!
Thanks! This really helped 😊.
Why is the group number of O 16? I get that Ca is in column 2 and has 2 valence electrons. I would have said that O was in group 6. How do you figure 16? Where does that initially come from?
+Brian Merritt Nevermind, I get it, the transition metal groups were included, but since there are 10 groups of those, it work out.
+Brian Merritt I'm glad you found the answer for yourself :)
+Brian Merritt the answer to this question
is solving the groups of 10
+Angles and Acid are the solving experiments
But isn't the 3rd energy level able to contain 18 electrons?
Thx sir u r the best
thanx it helped:) and u r very good at explaining :)
Doreen Baraka You're welcome and thank you :)
completely great helped a lot!
Do you happen to have any videos that show electron orbitals?
Jorge Padua Sorry, not at this time.
thank you very helpful information and easy to understand! :-)
+Marixza Ortiz Thank you :)
Very helpful. Thanks.
Devika Sood You're welcome :)
good job bro from:batticaloa srilanka
Every other video that I watch says something different. Half of the videos say 2-8-8, the other half say 2-8-18. Which is it, it can be both, are we counting the sub shells, or are we not?
The technical limits are 2, 8, 18, and so on. However, the main reason why we're interested in knowing what the limits are per energy level is to determine if the electron configuration is stable or not. Atoms with configurations of 2, or 2,8, or 2,8,8, or 2,8,18 are all stable. Things get weird between that 8--->18 stage of the 3rd energy level which is where this basic 'Bohr' model of the atom reaches its limits and you need to look into the Wave model (aka wave mechanical model, or quantum model, think schrodinger).
I'm sorry but I'm really confused where did you get the group numbers?
They're often listed at the top going from 1 to 18 across horizontally. If you don't see them (it depends on the style of periodic table) you can just count how many columns from the left side. That's the group number.
You have a really nice voice or accent , anyway you sound good 😊
Thanks!
if the period is 6 so 6 shells? i just started to learn chemistry
Good
How intersting
Namaste sir i am from india
That is so helpful
You're welcome :) I'm glad you liked it
What about things like gold (Au) which has 32 electrons in one of its shells
may I ask why calcium is 2,8,8,2 but not 2,8,10 as I have learnt that the third electron shells has a maximum number of 18 electrons
Hi Henrik. It's a really difficult question to answer:
1. It's difficult to convey in text
2. It requires more advanced chemistry to explain (quantum mechanical model) - so if you're quite early/young in your chemistry journey, I'd only make things more confusing by giving you the answer.
I'll try my best, but it comes down to the limitations of the Bohr model of the atom (the illustrations we use with concentric rings with electrons on them). Bohr's model assumes that electrons exist in defined 'energy levels' - you might call them electron shells* but I'll be calling them energy levels from now on because that's important for this explanation. Erwin Schrodinger in more recent history put forth the idea of the Quantum model (or quantum mechanical model), which conveys that electrons exist in one or more sub-shells (orbitals) for each energy level. This helped fix the flaws in Bohr's model (e.g. explaining emission spectra for elements other than hydrogen)
This means that when filling in electrons, you need to consider the lowest energy 'orbital' rather than the lowest energy level*. Everything is fine until Argon, 2,8,8 who has filled the 1st and 2nd energy levels* (and its orbitals), but not fully filled its 3rd energy level*. When you proceed to Potassium 2,8,8,1 this is where the 3rd and 4th energy levels* overlap in their orbitals' energy.
As you know, electrons will fill up from lowest to highest energy as possible. So after Argon, electrons will fill 2 electrons into the 4th energy level, since one of its orbitals is lower in energy, than the 10 remaining vacant spots in the orbitals of the 3rd energy level. Now after calcium, you'll start finishing off the 10 vacant spaces until you reach Zinc.
If you have the benefit of talking with a chemistry teacher, share with them what Iv'e written so they can expand upon it, and note that I've deliberately tried to avoid mentioning s, p, d, and f in my explanation to keep things as simple as I can.
How do you know Calcium needs 8 for some of the shells?
+Bioshock Infinite ah, that's one of the rules we follow with filling electron shells. Just got to remember them I'm afraid.
* you swoosh your hair majestically showing your manliness as a alpha male , showing your dominance to every Beta male*
Helpful. Thank you.
You're welcome :)
How do you know the groups
the best !!!!!!
Thank you 😊
This is confusing. The oxygen in the periodic table is on the 6th period not the 2nd period
That would imply you're seeing the symbol 'O' in the 6th row of the periodic table. It's in the 2nd row, hence, 2nd period.
❤ it thank u mr
angels and acids with the group number can you eplain why you only pull out six instead of ten
+Demolition Bomer It probably makes sense in another video of mine where I show a picture of the periodic table, such as writing ionic formulas. I drop off the 10 because there are 10 groups (columns) of elements in the 'd-block' of the table that have no elements in them in the top 1/3 of the table. so really, only groups 1-2 and 13-18 are used for the top part of the table (that makes 8 groups left to right, so group 1 has one electron, group 2 has two electrons, group 13 has three electrons, etc)
can you please tell me why the i nermost shell has the lowest energy and outer has the highest energy is it true the angular momentum appeared as energy i cant figure it out please help me and please tell me the way how to find energy of the shells hope you reply soon
I'm sorry but I'll have to admit that your question goes beyond my expertise. In most cases, it's not important for everyday chemistry to understand the maths/physics of the energy levels. If your maths is strong enough, you might find the answers you're after in the Wave Equation, or the Quantum Mechanical Model (Schrodinger). Again, the mathematics of the quantum mechanical model are beyond me.
but why innermost has higher energy and which thing present there in an atom which we are calling energy what is this kinetic potential or what kind of thing there appeared as energy
why the protons are always held together although they have same charge
i found answer that the nuclear force hold them together but from where that force comes up
Electrostatic Repulsion works over longer distances, whereas the nuclear force is greater at shorter range, so if the protons are close enough, the nuclear/strong force is much greater than their electrostatic repulsion. Neutrons help too - as charged particles are attracted to neutral particles as well as oppositely charged particles. You're asking physics questions and not chemistry questions I'm afraid you'll need to find someone who specialises in nuclear physics.
i am from pakistan where i am living in a lower class area where things like science obviously not explained well thats why i am asking questions from you was my questions are not right ..............??????? Or these questions have no sense
Why did you remove the ten on 16?
I'm presuming you're asking about the Group number 16, and remove ten? It's to do with the fact that for the first few rows (periods as they're called) of the table, there aren't any elements sitting in the middle. e.g. there's a gap between Berylium, and Boron. The gap is exactly ten spaces. You'll learn more in-depth about that gap section (the 'd-block' elements sit right under there) when you take a senior chemistry class. Not really necessary to know when you're just starting out.
thank you sir
electrons come in pairs so in the first orbit they shouldve been next to eachother, coming in a pair
I would disagree that they always come in pairs... but you are right - it's odd that they are conventionally drawn on opposite sides rather than paired together like you suggest. I think you'll like the Quantum Mechanical Model for electron configurations a lot more :)
Angles and Acid i'll check it out :D
The subtitle blocks the contents so cannot see important bits, I think contents are more important than subtitle if can only chose to have one.
Oh my gosh - I hadn't considered the placement of subtitles before. You've made a really good point and I will try to make more space at the bottom in future videos for the subtitles. Some of my students depend on them too if English isn't their first language so thank you for sharing the constructive criticism!
If there were 6 left on the outer shell how come he didn't put all of them into the p subshell?
Hi David, I'm just sticking to the simpler bohr-model electron configurations. Subshells weren't part of his theory at the time until Schrodinger came along.
+Angles and Acid oh ok but can you just put them all in the p subshell if you wanted to
Technically, you would have to put 2 of them into the s-subshell and the 4 remaining in the p-subshell, as per the Aufbau principle and Madelung energy ordering rule en.wikipedia.org/wiki/Aufbau_principle
+Angles and Acid ok thank you your video was really helpful
I love you already.
Ugh I wanna know how I could prepare my chemistry research about electron configuration
I'm not sure what you're asking about. In any case, I do wish you good luck with your research. Don't forget that you can ask for help from your teachers/lecturer/professor.
Thank you
You're welcome!
But we're is group 2 for oxygen
👏
because in my book they have written like this
thanks
Thanks
You're welcome :)
now I get it
Dionatan Miguel Thanks!
this is a good video but i just will never understand this stuff
+Kinzygirl Never give up on yourself :) Some things take time until they click.
The occasional YOI.
No!!!! The website is not working!
after he said done 😂😂
Pardon?
Angles and Acid 4:37
Pls stand and explain properly
Curious, why would you prefer standing? It would be more challenging in this case because I've got my computer & wacom tablet just below that I'm using to illustrate in real-time.
Pls punjabi
my brain explode too hard can't understand lit af -.-
Hey, don't give up - if this is something that you're passionate about then take a look around - there might be other teachers, or RUclipsrs out there that can explain it in a way that works for you. Also keep in mind that many things take time until they really make sense.
ok thank you
o is 6 in group u r wrong
Depends on how old-school your periodic table is, or perhaps it's even been simplified for junior classes. It's group 16 or 6 depending on whether they give group numbers to the d-block elements in the middle of the table (Sc to Zn).
Which is 10 elements across, which gives the number 16 or 6 depending on whether you count them or not.
Waste
Thank you