
Thai: 
ลองหาการจัดอิเล็กตรอน
สำหรับคาบที่สองกัน
เราหาคาบที่สอง
ในตารางธาตุ และเราไล่ไป
ธาตุแรกที่เราเจอ
คือลิเธียมมีอิเล็กตรอน 3 ตัว
มี 3 ตัวให้คิดสำหรับลิเธียม
ลองคิดถึงอิเล็กตรอน
สองตัวแรกสำหรับลิเธียม
อิเล็กตรอนสองตัวแรกสำหรับลิเธียม
จะอยู่ในชั้นแรก
เราได้พูดถึงเรื่องนี้ในวิดีโอก่อนแล้ว
ชั้นแรกเมื่อ n เท่ากับ 1
ค่า l เดียวที่เป็นไปได้คือ 0
เราจึงพูดถึง s ออร์บิทัล
มันมี s ออร์บิทัลตัวเดียว
ในชั้นแรก ผมก็วาดได้
ขอผมลงมือวาดออร์บิทัลนะ
ตรงนี้คือ 1s ออร์บิทัลในชั้นแรก
ลิเธียมมีอิเล็กตรอน 3 ตัว
อิเล็กตรอน 2 ตัวแรกสำหรับลิเธียม
จะไปอยู่ใน 1s ออร์บิทัลนี้
เราจับคู่สปินอย่างนั้น
เขียนการจัดอิเล็กตรอนสำหรับลิเธียม
ขอผมลงมือเริ่ม
เขียนตรงนี้

Bulgarian: 
Нека преминем към електронните конфигурации за втория период.
Ето го втория период от периодичната таблица.
Първият елемент, който виждаме, е Литий с 3 електрона.
При лития трябва да мислим за 3 електрона.
Нека помислим за първите 2 електрона за лития.
Първите 2 електрона за лития влизат в първата електронна обвивка.
Говорихме за това в предишното видео.
Първата обвивка е, когато n=1.
Единствената възможна стойност за l е 0.
Говорим за s орбитала.
И има само 1 s орбитала в първата обвивка и мога да я начертая.
Нека начертая тази орбитала.
В първата обвивка има една s орбитала.
Литият има 3 електрона.
Първите два електрона на лития ще са в тази една s орбитала.
Съчетаваме спиновете ето така.
Пишем електронната конфигурация за лития.
Ще започнем да я записваме ето тук.

English: 
- Let's do electron configurations
for the second period.
So we find the second period
on the periodic table and we go across
and the first element we see
is Lithium with three electrons.
So three electrons to
worry about for Lithium.
Let's think about the first two
electrons for Lithium.
The first two electrons for Lithium
are going to go into the first shell.
So we talked about this in the last video.
The first shell when n is equal to one,
the only possible value for l is zero.
So we're talking about an s orbital.
And there's only one s orbital
in the first shell here so I can draw in,
let me go ahead and draw that orbital in.
So here's the one s
orbital in the first shell.
So Lithium has three electrons.
The first two electrons for Lithium
are going to go into this one s orbital.
So we pair up our spins like that.
So writing the electron
configuration for Lithium,
let me go ahead and we'll start
writing it right here.

Korean: 
주기율표의 2주기 원소에 대한
전자 배치를 해봅시다
주기율표의 2주기 원소에 대한
전자 배치를 해봅시다
주기율표의 2주기를 보니
주기율표의 2주기를 보니
1족에 3개의 전자를 가지고 있는
리튬(Li)이 있습니다
리튬(Li)에 있는 3개의
전자를 살펴봅시다
먼저 리튬(Li)의 전자 중
앞쪽 두 전자를 봅시다
제일 처음 두 전자는
첫 번째 전자 껍질에 갈 것입니다
이 내용은 지난번
동영상에서 설명했습니다
첫 번째 전자 껍질에서 n=1일 때
l에 가능한 값은 0밖에 없습니다
그래서 s오비탈입니다
그리고 첫 번째 전자 껍질에는
s오비탈이 하나만 있을 수 있습니다
s오비탈이 하나만 있을 수 있습니다
첫 번째 전자 껍질에는
s오비탈이 하나가 있습니다
리튬(Li)은 3개의 전자를
가지고 있습니다
리튬(Li)의 전자 중 두 개는
이 s오비탈에 가게 됩니다
이렇게 스핀을 짝지읍시다
리튬(Li)의 전자 배치를
리튬(Li)의 전자 배치를
여기에 적겠습니다

Thai: 
ถึงตอนนี้เรามี 1s2
ลิเธียมมีอิเล็กตรอน 3 ตัว
แต่ชั้นแรกเต็ม มันปิดแล้ว
เราต้องไปยังชั้นที่สอง
เพื่อใส่อิเล็กตรอนตัวที่ 3 ของลิเธียม
ในชั้นที่สอง n เท่ากับ 2
ค่าที่ยอมได้สำหรับ l มีอะไรบ้าง?
l เท่ากับ 0
หรือ l เท่ากับ 1 ได้
เราได้พูดถึงแล้ว
ในวิดีโอเรื่องเลขควอนตัม
เมื่อ l เท่ากับ 0
เรากำลังพูดถึง s ออร์บิทัล
ในชั้นที่สอง
ในชั้นพลังงานที่สอง
เรามี s ออร์บิทัล
และเรามีตัวหนึ่ง
เราต้องคิดถึง
l เท่ากับ 1 มันจะพูดถึง p ออร์บิทัล
ค่าที่ยอมได้สำหรับ ml ได้แก่
ลบ 1, 0 และบวก 1
ค่าที่เป็นไปได้สามอย่างนี้หมายถึง
p ออร์บิทัล 3 ตัวตรงนี้
เราจึงมี p ออร์บิทัล 3 ตัว
ในชั้นพลังงานที่สองเช่นกัน
ลองวาดภาพโดยใช้แผนภาพออร์บิทัลตรงนี้

English: 
So we have one s two so far.
Well Lithium has three electrons
but the first shell is full, it's closed.
So we have to move on to the second shell
to add in Lithium's third electron.
So in the second shell, n is equal to two.
What are the allowed values for l?
L could be equal to zero
or l could be equal to one.
So we talked about that again
in the videos on quantum numbers.
So when l is equal to zero,
we're talking about an s orbital.
So in the second shell,
in the second energy level,
we also have an s orbital
and we also have one of them
and we also have to think about
l is equal to one, that's
talking about a p orbital.
The allowed values for ml would be
negative one, zero and positive one.
So three possible values means
three p orbitals here.
So we have three p orbitals
in the second energy level as well.
So let's draw those in on our
orbital diagram over here.

Bulgarian: 
Дотук имаме 1s2.
Литият има 3 електрона, но първата обвивка е пълна, затворена.
Трябва да преминем към втората обвивка,
за да добавим третия електрон на лития.
Във втората обвивка n=2.
Какви са позволените стойности за l?
l може да е 0 или l може да е равно на 1.
Вече говорихме за това във видеата за квантовите числа.
Когато l=0, говорим за s орбитала.
Във втората обвивка, във второто енергийно ниво също имаме една s орбитала.
Имаме една s орбитала
и също трябва да помислим за l=1, това е р орбитала.
Позволените стойности за ml ще са -1, 0 и +1.
Три възможни стойности означава три р орбитали.
Имаме 3 р орбитали във второто енергийно ниво.
Нека начертаем тези в орбиталната си диаграма.

Korean: 
지금까지 1s2가 있습니다
리튬(Li)은 전자 3개가 있는데
첫 번째 전자 껍질은 다 차서
전자를 더 받을 수 없습니다
그래서 리튬(Li)의
세 번째 전자를 더하기 위해
두 번째 전자 껍질로 넘어갑시다
두 번째 전자 껍질에서는
 n=2입니다
그러면 가능한 l의 값은 무엇일까요?
l=0이나 l=1이 가능하겠습니다
l=0이나 l=1이 가능하겠습니다
이것은 양자수 동영상에서도
다뤘습니다
이것은 양자수 동영상에서도
다뤘니다"
l=0인 경우에는
s오비탈입니다
두 번째 전자 껍질에서는
즉 두 번째 에너지 준위에서는
s오비탈이 있는데
역시 하나가 있습니다
l=1일 경우도 생각해야 하는데
이는 p오비탈입니다
ml에 가능한 값은 -1, 0, 1입니다
ml에 가능한 값은 -1, 0, 1입니다
여기에서 가능한 값이 3개라는 것은
3개의 p오비탈을 뜻합니다
그러므로 두 번째 에너지 준위에는
3개의 p오비탈도 있습니다
여기 오비탈 다이어그램에 그려봅시다

Korean: 
이미 첫 번째 전자 껍질에
s오비탈을 그렸습니다
이미 첫 번째 전자 껍질에
s오비탈을 그렸습니다
이 s오비탈을 두 번째 전자 껍질
즉 두 번째 에너지 준위에 그립시다
더 높은 에너지를 
가지고 있으므로 여기에 그립시다
더 높은 에너지를 
가지고 있으므로 여기에 그립시다
이것은 2s오비탈입니다
두 번째 에너지 준위에
p오비탈도
총 3개가 있습니다
두 번째 에너지 준위에
p오비탈을 그려넣읍시다
더 높은 에너지를 가지고 있습니다
2p오비탈이 3개가 있습니다
그 중 하나는 2px가 될 것이고
하나는 2py가 될 것이고
다른 하나는 2pz가 될 것입니다
뭐가 뭔지는 크게 상관은 없습니다
여기에 그것들을 그릴 것입니다
리튬(Li)의 3개의 전자 중에서
리튬(Li)의 3개의 전자 중에서
두 개를 다뤘습니다
그럼 세 번째 전자는
그 다음으로 에너지가 높은
오비탈에 들어가야 합니다
그러니 2s오비탈이 됩니다
에너지가 이 방향으로
갈수록 커지므로
점점 높아질수록 에너지는 커집니다
그래서 리튬(Li)의 전자를 쌓을 때

Bulgarian: 
Вече начертахме тази s орбитала в първата обвивка.
Сега нека начертаем s орбиталата във втората обвивка, второто енергийно ниво.
Тя има по-висока енергия.
Чертаем я ето тук.
Това са двете s орбитали.
После, във второто енергийно ниво имаме и p орбитали – имаме 3 такива.
Чертаем р орбиталите във второто енергийно ниво.
Те са с по-висока енергия.
Ето ги двете р орбитали, а после има 3 от тях.
Първата ще е 2рх, една ще е 2ру,
а другата ще е 2рz.
Няма значение коя коя е.
Просто ще ги начертаем ето така.
Литий.
Погрижихме се за два от трите му електрона.
Третият електрон трябва да влезе в най-високата орбитала, що се отнася до енергия,
така че това ще е орбиталата 2s.
Имаме енергия, която преминава нагоре, ето така.
Колкото по-нависоко отиваш, толкова повече се увеличава енергията ти.
Следващият електрон на лития, докато надграждаш литиевия атом,

Thai: 
เราได้วาดดออร์บิทัล s นี้
ในชั้นแรก
ต่อไป ลองวาดใน s ออร์บิทัลนี้กัน
ในชั้นที่สอง ชั้นพลังงานที่สอง
มันมีพลังงานสูง
เราวาดมันในนี้
นี่คือ 2s ออร์บิทัล
แล้วเรามี p ออร์บิทัลเหมือนเดิม
ในชั้นพลังงานที่สอง
เรามีอิเล็กตรอน 3 ตัว
เราวาดใน p ออร์บิทัล
ในชั้นพลังงานที่สอง
พวกมันมีพลังงานสูงขึ้น ตรงนี้มี
2p ออร์บิทัล มีอยู่ 3 ตัว
ตัวหนึ่ง มันจะเป็น 2px
ตัวหนึ่งจะเป็น 2py
และตัวหนึ่งจะเป็น 2pz
ตัวไหนเป็นตัวไหนไม่สำคัญ
เราจะวาดมันลงไปแบบนั้น
เอาล่ะ ลิเธียม
เราจัดการอิเล็กตรอน
สองตัวจากสามตัวแล้ว
อิเล็กตรอนตัวที่สามต้องไปอยู่
ออร์บิทัลสูงสุดในแง่ของพลังงานอันต่อไป
มันจะเป็น 2s ออร์บิทัล
เรามีพลังงานขึ้นไปแบบนี้
เมื่อคุณอยู่สูงขึ้นไปเรื่อยๆ พลังงานจะเพิ่มขึ้น
อิเล็กตรอนตัวต่อไปของลิเธียม 
เมื่อคุณสร้างขึ้นไป

English: 
So we already drew in this s orbital
in the first shell.
Next let's draw in this s orbital
in the second shell,
the second energy level.
It's of higher energy.
So we draw it in here.
This is the two s orbital.
Then we also have p orbitals
in the second energy level,
we have three of them.
So we draw in our p orbitals
in the second energy level.
They're of higher energy so here are
the two p orbitals and
there are three of them.
So one of them is, it would be two px,
one of them would be two py
and one of them would be two pz.
Doesn't really matter which one is which.
We'll just draw them in
there like that so far.
All right, so Lithium.
We've taken care of the two
of it's three electrons.
It's third electron has to go into
this next highest orbital
in terms of energy,
so that would be the two s orbitals.
We have energy going up this way.
So as you get higher and
higher, energy increases.
So Lithium's next
electron, as you build up

Korean: 
리튬(Li)의 다음 전자는
여기 이 오비탈에 들어가야 합니다
2s오비탈에 들어가야 합니다
그러므로 리튬(Li)의 전자 배치는
1s2 2s1이 되는데
이 숫자들이 의미하는 바를 기억해냅시다
이 숫자는 1개의 전자와 s오비탈 하나가
두 번째 에너지 준위에 있다는 뜻입니다
그러니 리튬(Li)의 전자 배치는
1s2 2s1입니다
다음 원소를 해봅시다
베릴륨(Be)입니다
베릴륨(Be)은 다룰 전자가 4개입니다
베릴륨(Be)의 다이어그램을 봅시다
베릴륨(Be)의 다이어그램을 봅시다
베릴륨(Be)은 빨간색으로 합시다
전자 1개가 더 있습니다
그러니 베릴륨(Be)의 네 번째 전자를
이 오비탈에 배치하고
스핀을 짝지읍시다
베릴륨(Be)의 전자 배치를 써 봅시다
1s2를 썼고 2개의 전자와
2개의 s오비탈이 있으니까
여기 이렇게 2s2도 씁시다
이제 2s오비탈을 채웠습니다
각각의 오비탈에는 최대 2개의

Thai: 
อะตอมลิเธียมต้องไปยังออร์บิทัลนี่ตรงนี้
2s ออร์บิทัล
เพราะฉะนั้น การจัดอิเล็กตรอนของลิเธียม
คือ 1s2, 2s1 และนึกดู
ว่าเลขเหล่านี้หมายถึงอะไร
นี่หมายความว่า มีอิเล็กตรอนหนึ่งตัว
และ s ออร์บิทัลในชั้นพลังงานที่สอง
เรามี 1s2, 2s1
สำหรับการจัดอิเล็กตรอนของลิเธียม
ลองทำธาตุต่อไปกัน
นั่นคือแบริเลียม
แบริเลียมมีอิเล็กตรอน 4 ตัวให้คิด
สำหรับแบริเลียม ถ้าคุณดูแนผนภาพ
ลองดูว่าเราใช้อีกสีแทน
แบริเลียมได้ไหม 
ลองให้แบริเลียมเป็นสีแดงตรงนี้
อิเล็กตรอนอีกหนึ่งตัว
เราใส่อิเล็กตรอนตัวที่ 4 ของแบริเลียม
ในออร์บิทัลนี้ และจับคู่สปินได้
ลองเขียนการจัดอิเล็กตรอน
สำหรับแบริเลียมกัน
มันจะเป็น 1s2 แล้วเรามี
อิเล็กตรอน 2 ตัว แล้วก็ 2s ออร์บิทัล
เราก็เขียน 2s อย่างนั้นได้ตรงนี้
ทีนี้ เราเติม 2s ออร์บิทัลหมดแล้ว
นึกดู แต่ละออร์บิทัลใส่

English: 
the Lithium atom must go
into this orbital here.
The two s orbital.
So therefore, Lithium's
electron configuration
is one s two, two s one and remember
what these numbers mean.
So this means that there is one electron
and an s orbital in the
second energy level.
So we have one s two, two s one
for Lithium's electron configuration.
Let's do the next element.
So that's Beryllium.
Beryllium has four
electrons to worry about.
So for Beryllium, if
you look at the diagram,
Let's see if we can just
make a different color
here for Beryllium, so let's
make Beryllium red here.
So one more electron.
So we can put Beryllium's fourth electron
into this orbital and pair up our spins.
So let's write the electron
configuration for Beryllium.
So it would be one s two and then we have
two electrons and then two s orbitals,
so we would write two
s two here like that.
Now, we've filled the two s orbitals.
Remember, each orbital can hold

Bulgarian: 
трябва да влезе в тази орбитала ето тук.
Орбиталата 2s.
Следователно конфигурацията на лития е 1s2 2s1 и помни какво означават тези числа.
Това означава, че има един електрон и една s орбитала във второто енергийно ниво.
Конфигурацията на лития е 1s2 2s1.
Нека се заемем със следващия елемент.
Това е Берилий.
Берилият има четири електрона, за които трябва да помислим.
Така че за берилия, ако погледнеш диаграмата...
Да видим дали можем да направим берилия в различен цвят – нека е червено.
Още един електрон.
Можем да поставим четвъртия електрон на берилия
в тази орбитала и да съчетаем спиновете.
Нека запишем електронната конфигурация за берилия.
Това ще е 1s2 и после имаме два електрона и две s орбитали.
Ще запишем 2s2 ето така.
Сега запълнихме двете s орбитали.

Korean: 
전자를 채울 수 있습니다
2s오비탈까지 채웠으니
다음 원소인 붕소(B)로 넘어갑시다
다음 원소인 붕소(B)로 넘어갑시다
붕소(B)는 5개의 전자를
가지고 있습니다
붕소(B)의 전자 배치를
써 보도록 합시다
지금 1s2 2s2까지 배치했습니다
5개의 전자를 배치해야 하는데
이것들은 4개밖에
배치하지 못합니다
그럼 다섯 번째 전자는
어디로 갈까요?
다섯 번째 전자는 다음으로 가능한
오비탈에 갈 것입니다
따라서 붕소(B)의 다섯 번째 전자는
2p오비탈로 가게 됩니다
그러니 다섯 번째 전자가
두 번째 에너지 준위의
p오비탈에 갔다는 뜻으로
2p1을 쓸 것입니다
그러니 1s2 2s2 2p1이 되고
이것은 붕소(B)의 전체 전자 배치입니다
다음으로 탄소(C)로 해봅시다
다음으로 탄소(C)로 해봅시다
탄소(C)는 파란색으로 씁시다
탄소(C)는 총 6개의 전자를
가지고 있습니다
전자 한 개를 더 생각해야 합니다

English: 
a maximum of two electrons.
We filled the two s orbitals
so when we move on to the next element,
which is Boron over here.
So Boron has five electrons.
So let's write the electron
configuration for Boron.
Well so far we have one s two,
two s two but that only takes care
of four electrons, we need five.
So where does the fifth one go?
The fifth one goes into the next
available orbital here so we're going
to put the electron in, the fifth electron
for Boron goes into a two p orbital.
So we would write two p one indicating
that the fifth electron for Boron
went into a p orbital in
the second energy level.
So one s two, two s two, two p one,
is the full electron
configuration for Boron.
All right, so let's do Carbon.
So next we have Carbon.
Let's use blue for Carbon here.
So Carbon has a total of six electrons.
We have one more to think about.

Bulgarian: 
Помни, всяка орбитала може да съдържа максимум 2 електрона.
Запълнихме двете s орбитали,
така че преминаваме към следващия елемент, който е борон.
Боронът има 5 електрона.
Нека запишем електронната конфигурация за борона.
Дотук имаме 1s2 2s2,
но това включва само 4 електрона, а на нас ни трябват 5.
Къде отива петият?
Петият влиза в следващата налична орбитала,
така че ще поставим петия електрон на борона  2р орбитала.
Ще запишем 2р1, което означава,
че петият електрон на борона е в р орбитала във второто енергийно ниво.
1s2 2s2 2р1 е пълната електронна конфигурация за борона.
Нека преминем към въглерода.
След това е ред на въглерода.
Нека използваме синьо за въглерода.
Въглеродът има общо 6 електрона.
Имаме още 1, за който да помислим.

Thai: 
อิเล็กตรอนได้มากสุด 2 ตัว
เราเติม 2s ออร์บิทัลครบแล้ว
เมื่อเราไปยังธาตุต่อไป
ซึ่งก็คือโบรอนตรงนี้
โบรอนมีอิเล็กตรอน 5 ตัว
ลองเขียนการจัดอิเล็กตรอนสำหรับโบรอนกัน
ถึงตอนนี้ เรามี 1s2
2s2 แต่มันจัดการอิเล็กตรอน
แค่ 4 ตัว เราต้องการ 5
แล้วตัวที่ 5 จะไปอยู่ไหน?
ตัวที่ 5 จะไปยังออร์บิทัล
ที่ว่างอันต่อไป เราจะ
ใส่อิเล็กตรอนลงไป อิเล็กตรอนตัวที่ 5
สำหรับโบรอน ไปอยู่ใน 2p ออร์บิทัล
เราก็เขียน 2p1 แสดงถึง
อิเล็กตรอนตัวที่ 5 สำหรับโบรอน
ไปยัง p ออร์บิทัลในชั้นพลังงานที่ 2
1s2, 2s2, 2p1
คือการจัดอิเล็กตรอนของโบรอน
เอาล่ะ ลองไปยังคาร์บอนกัน
ต่อไป เรามีคาร์บอน
ลองใช้สีฟ้าแทนคาร์บอนกันตรงนี้นะ
คาร์บอนมีอิเล็กตรอนทั้งหมด 6 ตัว
เรามีอิเล็กตรอนอีกตัวให้คิด

English: 
So we know it's going
to go into a p orbital,
a p orbital in the second energy level.
The question is which
one of these p orbitals
do we put this next electron for Carbon?
So we have to think about
something called Hund's rule.
I'm never going to pronounce the German
properly so Hund's rule tells us
that our goal is to minimize
electron repulsion here.
So let's think about...
Let me just go ahead and draw
the p orbitals down here.
So we already have one
electron right here.
Well it doesn't make any sense to put
an electron into the same orbital here
because that puts the
electrons really close
together in space.
So if you're thinking about a p orbital,
remember a p orbital is shaped
like a dumbbell so I'm just saying
we have a p orbital on
this axis let's say.
So we all ready have, let me use,
I'll just use blue here.
So we already have one electron in there,
it doesn't make any sense to add
an electron to that exact same p orbital.
That puts them really close together
in space and electrons repel.
So that doesn't make any sense

Bulgarian: 
Знаем, че той ще влезе в р орбитала,
р орбитала във второто енергийно ниво.
Въпросът е в коя от тези р орбитали поставяме този следващ електрон на въглерода.
Трябва да помислим за нещо, наречено правило на Хунд.
Никога няма да успея да произнеса немските думи правилно.
Правилото на Хунд ни казва,
че целта ни е да минимизираме електронното отблъскване.
Нека помислим за...
Нека начертая р орбиталите тук долу.
Вече имаме един електрон ето тук.
Не е логично да поставим електрон в същата орбитала тук,
понеже това поставя електроните много близо един до друг в пространството.
Ако мислиш за р орбитала,
помни, че една р орбитала е с форма на камбанка,
така че просто казвам, че имаме р орбитала на тази ос.
Вече имаме – нека използвам синьо тук.
Вече имаме 1 електрон тук,
не е логично да добавим един електрон в същата тази р орбитала.
Това ги поставя много близо един до друг в пространството
и електроните ще се отблъснат.

Korean: 
이 한 개가
두 번째 에너지 준위에 있는
p오비탈에 간다는 점을
알고 있습니다
이 p오비탈 중 어느 것에
탄소(C)의 다음 전자를
넣을 것인지가 문제입니다
훈트 규칙에 대해 생각해봐야 합니다
훈트 규칙에 대해 생각해봐야 합니다
저는 독일어를
바르게 발음하지 못합니다
훈트 규칙에 따르면
여기서 전자 반발력을
최소화해야 합니다
여기에 p오비탈을 그리겠습니다
여기에 p오비탈을 그리겠습니다
여기에 p오비탈을 그리겠습니다
이미 전자 1개가 여기 있습니다
같은 오비탈에 전자를 두는 것은
말이 안됩니다
같은 오비탈에 전자를 두는 것은
말이 안됩니다
공간상에서 전자들을 서로 매우
가깝게 놓는 것이기 때문입니다
공간상에서 전자들을 서로 매우
가깝게 놓는 것이기 때문입니다
p오비탈을 떠올려본다면
p오비탈은 아령 모양으로 생겼습니다
p오비탈은 아령 모양으로 생겼습니다
이 축에 p오비탈이 있다고 해봅시다
파란색을 쓰겠습니다
파란색을 쓰겠습니다
이미 전자 1개가 있어서
완전히 같은 p오비탈에
전자를 더하는 것은
말이 되지 않습니다
이렇게 하면 전자들을 공간상에
서로 아주 가깝게 두게 되는데
전자들 사이에는
반발력이 작용하기 때문입니다
그러니 말이 전혀 되지 않는 것이고

Thai: 
เรารู้ว่ามันจะอยู่ใน p ออร์บิทัล
p ออร์บิทัลในชั้นพลังงานที่สอง
คำถามคือว่าเราจะใส่อิเล็กตรอนตัวต่อไป
ของคาร์บอนไว้ที่ p ออร์บิทัลอันไหน?
เราต้องคิดถึง
สิ่งที่เรียกว่ากฎของฮุนด์ (Hund's rule)
ผมไม่เคยออกเสียงภาษาเยอรมันถูกเลย
กฎของฮุนด์บอกเราว่า
เป้าหมายของเราคือทำให้
การผลักกันของอิเล็กตรอนน้อยที่สุด
ลองคิด --
ขอผมลงมือวาด
p ออร์บิทัลข้างล่างตรงนี้
เรามีอิเล็กตรอนหนึ่งตัวแล้วตรงนี้
มันไม่สมเหตุสมผลถ้าเรา
ใส่อิเล็กตรอนในออร์บิทัลเดียวกันตรงนี้
เพราะมันทำให้อิเล็กตรอนอยู่
ใกล้กันในสเปซมากขึ้น
ถ้าคุณคิดถึง p ออร์บิทัล
นึกดู p ออร์บิทัลมีรูปร่าง
เหมือนดัมเบล ผมจึงบอกว่า
เรามี p ออร์บิทัล สมมุติว่า บนแกนนี้
เรามี ขอผมใช้
ผมจะใช้สีฟ้าตรงนี้นะ
เรามีอิเล็กตรอน 1 ตัวในนี้แล้ว
มันไม่ดีถ้าเราใส่
อิเล็กตรอนใน p ออร์บิทัลเดียวกันเลย
มันอยู่ใกล้กัน
ในสเปซ อิเล็กตรอจะผลักกัน
มันจึงไม่สมเหตุสมผล

English: 
so we need to take that
electron out of there.
That doesn't make any sense.
We need to add an electron
to another p orbital.
So we'll take this electron
out of there like that.
So remember, there are other p orbitals
on these other axis here.
So here's another p orbital
and then here's another p orbital.
So we need to add an electron
to another one of these.
Whichever one, it doesn't really matter.
Let's just say we're adding one here.
So we're adding an electron to
a different p orbital,
whichever one it is,
px, py, or pz.
And it turns out that keeping the spins
parallel helps to minimize
the electron repulsion
for pretty complicated reasons
and I think they might still be doing
research on this and
so we put the electron
in a different orbital and
we keep the spins parallel
which helps to lower
energy for the atom here.
And so that's where we're going
to put Carbon's sixth electron.
We're going to put it into
a different p orbital and we're going
to keep the spins parallel like that.

Bulgarian: 
Така че не е логично, тоест трябва да извадим този електрон оттук.
Това не е логично.
Трябва да добавим един електрон в друга р орбитала.
Ще извадим този електрон оттук ето така.
Помни, има други р орбитали на тези оси тук.
Ето още една р орбитала,
а после тук има друга р орбитала.
Трябва да добавим един електрон към друга от тези орбитали.
Няма значение коя.
Да кажем, че добавим един тук.
Добавяме един електрон към различна р орбитала, която и да е,
рх, ру или pz.
И се оказва, че поддържането на успоредни спинове помага
за минимизиране на електронното отблъскване,
поради доста сложни причини.
Мисля, че все още правят проучвания върху това.
Поставяме електрона в различна орбитала и поддържаме спиновете успоредни,
което помага да се намали енергията за атома тук.
И сега ще поставим шестия електрон на водорода.
Ще го поставим в различна р орбитала
и ще поддържаме спиновете успоредни.

Korean: 
전자를 그곳에서 빼내야 합니다
말이 전혀 안 됩니다
그러면 이 전자를
다른 p오비탈에 넣어야 합니다
그러니 이렇게 전자를 빼내겠습니다
다른 축에도
다른 p오비탈이 있습니다
다른 축에도
다른 p오비탈이 있습니다
여기 다른 p오비탈이 있고
여기 또 다른 p오비탈이 있습니다
그러니 이 중 하나에
전자를 더해야 합니다
둘 중에 무엇을 고르든 별로 상관은 없습니다
여기에 더한다고 생각해 봅시다
그것이 px, py, pz 중 무엇이든지
그것이 px, py, pz 중 무엇이든지
전자를 다른 p오비탈에 더합니다
또 스핀을 평행하게 유지하는 것은
꽤 복잡한 이유에 의해
전자 사이의 반발력을 최소화 하도록 
도와줍니다
아마 이 이유에 대해 아직 연구하고
있을 수도 있습니다
여기 이 원자의 에너지를 낮추기 위해
전자를 다른 오비탈에 넣고
스핀을 평행하게 유지합니다
그리고 그것이 탄소(C)의
여섯 번째 전자가 들어갈 자리입니다
전자를 다른 p오비탈에 넣어서
이런 식으로 스핀을 평행하게
유지할 것입니다
이런 식으로 스핀을 평행하게
유지할 것입니다

Thai: 
เราต้องเอาอิเล็กตรอนออกไปจากตรงนี้
มันไม่สมเหตุสมผล
เราต้องเพิ่มอิเล็กตรอนที่ p ออร์บิทัลอื่น
เราจะนำอิเล็กตรอนนี้ออกมาอย่างนั้น
นึกดู มี p ออร์บิทัลอื่นๆ
บนแกนอื่นๆ ตรงนี้
นี่คือ p ออร์บิทัลอีกอัน
และนี่คือ p ออร์บิทัลอีกอัน
เราต้องเพิ่มอิเล็กตรอน
ที่ออร์บิทัลหนึ่งในนี้ที่เหลือ
อันไหนก็ได้ ไม่สำคัญ
สมมุติว่าเราเพิ่มอันหนึ่งตรงนี้
เราจะเพิ่มอิเล็กตรอน
ใน p ออร์บิทัลอีกอัน อันไหนก็ได้
px, py หรือ pz
และปรากฏว่า การให้สปินชี้
ขนานกันช่วยลดแรงผลักของอิเล็กตรอน
ด้วยเหตุผลที่ซับซ้อน
ผมคิดว่ายังมีคนทำวิจัย
เรื่องนี้อยู่ เราใส่อิเล็กตรอน
คนละออร์บิทัล และเราให้สปินชี้ขนานกัน
ช่วยให้พลังงานของอะตอมลดลงตรงนี้
นั่นก็คือตำแหน่งที่เราจะ
ใส่อิเล็กตรอนตัวที่ 6 ของคาร์บอนลงไป
เราจะใส่มันลงใน
p ออร์บิทัลอีกตัว และเราจะ
ให้สปินชี้คู่กันไปอย่างนั้น

Thai: 
เราก็ลงมือ
เขียนการจัดอิเล็กตรอนของคาร์บอนได้
ลองอ่านทุกอย่างที่เรามี
ในสัญลักษณ์ออร์บิทัลตรงนี้
เรามี 1s2, เรามี 2s2
และเรามี 2p2 ตรงนี้
อิเล็กตรอน 2 ตัวใน p ออร์บิทัล
ในชั้นพลังงานที่สองของคาร์บอน
ต่อไป เรามีไนโตรเจน ลองใช้สีเขียว
แทนไนโตรเจนกัน
ไนโตรเจนมีอิเล็กตรอน 7 ตัว
มีอิเล็กตรอนอีกตัวให้คิด
ลองใส่ไนโตรเจนตรงนี้
ถึงตอนนี้เรามี 1s2, 2s2
ทีนี้ลองคิดถึงไนโตรเจนกัน
เราต้องใส่อิเล็กตรอนอีกตัวในแผนภาพ
เหมือนเดิม เราจะทำตามกฎของฮุนด์
เราจะไม่ใส่อิเล็กตรอน
เพิ่มในออร์บิทัลที่เต็มแล้ว
เราจะใส่อิเล็กตรอนนี้ของไนโตรเจน
ลงในออร์บิทัลที่ยังไม่เต็ม และเราจะ
ให้สปินชี้ไปในทิศเดียวกัน
เพื่อให้พลังงานรวมลดลง
เราจึงมีอิเล็กตรอน 3 ตัวสำหรับไนโตรเจน

Bulgarian: 
Можем да запишем електронната конфигурация на въглерода.
Просто прочитаме всичко, което имаме в орбиталното обозначение тук.
Имаме 1s2, имаме 2s2 и после имаме 2р2.
За въглерода имаме 2 електрона в р орбиталите във второто енергийно ниво.
След това имаме азот.
Нека за азота да използвам зелено.
Азотът има седем електрона,
тоест трябва да помислим за още един електрон.
Нека поставим азота тук.
Дотук имаме 1s2 2s2.
А сега нека помислим за азота.
Трябва да добавим още един електрон към диаграмата си.
Отново ще следваме правилото на Хунд.
Няма да добавяме електрона
към една от вече заетите орбитали.
Този азотен електрон ще добавим към незаета орбитала.
Ще задържим спиновете успоредни,
за да може всичко да е с по-ниска енергия.

Korean: 
한 발 더 가서 탄소(C)의
전자 배치를 쓸 것입니다
한 발 더 가서 탄소(C)의
전자 배치를 쓸 것입니다
그냥 여기 있는 오비탈 표기를
읽어내면 됩니다
여기 1s2 2s2 2p2가 있습니다
여기 1s2 2s2 2p2가 있습니다
탄소(C)는 두 번째 에너지 준위에 있는
p오비탈에 2개의 전자가 있습니다
다음으로 질소(N)가 있습니다
초록색을 쓰겠습니다
질소(N)는 7개의 전자를 가지고 있으니
전자 1개를 더 생각해봐야 합니다
질소(N)는 여기에 놓읍시다
지금까지 1s2, 2s2를 했습니다
이제는 질소(N)에 대해 생각해 봅시다
다이어그램에 전자 1개를 더해야 합니다
여기서 훈트 규칙을 다시 한번 따라야 합니다
이미 전자가 들어있는 오비탈에는
전자를 더하지 않고
이미 전자가 들어있는 오비탈에는
전자를 더하지 않고
전자가 없는 오비탈에
질소(N)의 전자를 더할 것이고
모든 것의 에너지를 낮추기 위해
스핀을 평행하게 유지할 것입니다
스핀을 평행하게 유지할 것입니다
2p오비탈에는

English: 
So we can go ahead
and write Carbon's electron configuration.
Just read off everything we have
on our orbital notation here.
So we have one s two, we have two s two
and we have two p two here.
So two electrons in the p orbitals
in the second energy level for Carbon.
Next we have Nitrogen so let's use green
here for Nitrogen.
So Nitrogen has seven electrons,
so one more electron to think about.
Let's put Nitrogen right here.
So we have so far, one s two, two s two.
Now let's think about Nitrogen.
So we need to add one more
electron to our diagram.
Once again, we're going to
follow Hund's rule here.
We're not going to add the electron
to one of the already occupied orbitals,
we're going to add this
electron for Nitrogen
to an unoccupied orbital and we're going
to keep the spins parallel to keep
everything lower in energy.
And so we have three
electrons for Nitrogen,

English: 
in the two p orbitals.
So we write two p three.
So we have one, two, three.
So we have one s two,
two s two, two p three,
would be the full electronic
configuration for Nitrogen.
Let's move on to Oxygen.
So let's pick, let's see here,
what color should we pick for that?
Let's use orange here for Oxygen.
So we have eight, eight total electrons.
So for Oxygen, let's see,
let's put Oxygen right here.
So so far we have, one s two, two s two.
So how many more electrons
do we need for Oxygen?
Oxygen has a total of eight electrons,
we all ready represented four,
so we need to represent four more.
Oxygen's eighth electron, now that all
of our orbitals are occupied,
we can start to pair our spins.
So we put Oxygen's
eighth electron in there.
So we can start to pair up our spins.
We have four electrons
in the two p orbitals

Bulgarian: 
За азота имаме три електрона в двете р орбитали.
Пишем 2р3.
Имаме 1, 2, 3.
Имаме 1s2 2s2 2р3
и това ще е пълната електронна конфигурация за азота.
Нека преминем към кислорода.
Да видим, какъв цвят трябва да изберем за това?
Нека за кислорода да използваме оранжево.
Имаме общо 8 електрона.
Да видим, нека поставим кислорода ето тук.
Дотук имаме 1s2 2s2.
Колко още електрона ни трябват за кислорода?
Кислородът има общо 8 електрона,
вече представихме 4, така че трябва да представим още 4.
Осмият електрон на кислорода –
сега всички орбитали са заети
и можем да започнем да съчетаваме спиновете.
Поставяме осмия електрона на кислорода ето тук.
Можем да започнем да съчетаваме спиновете.
Имаме 4 електрона в двете р орбитали.

Korean: 
3개의 전자가 있습니다
그래서 2p3를 씁니다
1, 2, 3개가 있습니다
1s2 2s2 2p3가
1s2 2s2 2p3가
질소(N)의 전체 전자 배치입니다
산소(O)로 넘어갑시다
여길 봅시다
무슨 색을 써야 할까요?
여기에서 산소(O)는 주황색을 씁시다
총 8개의 전자가 있습니다
산소(O)를 여기 둡시다
이 시점까지 1s2, 2s2를 했습니다
그러니 산소(O)는
몇 개의 전자가 더 필요할까요?
산소(O)는 총 8개의 전자가 있는데
이미 4개는 나타냈으니
4개를 더 나타내면 됩니다
오비탈이 다 찼으니
산소(O)의 여덟 번째 전자는
스핀을 짝짓기 시작할 수 있습니다
그러니 산소(O)의
여덟 번째 전자를 저기 둡니다
스핀을 짝짓기 시작할 수 있습니다
2p오비탈에 산소(O)의 4개의 전자가 있어서

Thai: 
ใน 2p ออร์บิทัล
เราก็เขียน 2p3
เรามี 1, 2, 3
เรามี 1s2, 2s2, 2p3
เป็นการจัดอิเล็กตรอน
สำหรับไนโตรเจน
ลองไปยังออกซิเจนกัน
ลองเลือก ลองดูตรงนี้
เราเลือกสีอะไรดี?
ลองใช้สีส้มแทนออกซิเจนแล้วกัน
เรามี 8 อิเล็กตรอนทั้งหมด 8 ตัว
ออกซิเจน ลองดู ลองใส่ออกซิเจนตรงนี้
ถึงตอนนี้เรามี 1s2, 2s2
เราต้องการอิเล็กตรอน
อีกกี่ตัวสำหรับออกซิเจน?
ออกซิเจนมีอิเล็กตรอนทั้งหมด 8 ตัว
เราแสดงไป 4 ตัวแล้ว
เราจึงต้องเขียนอีก 4 ตัว
อิเล็กตรอนตัวที่ 8 ของออกซิเจน ตอนนี้
ออร์บิทัลทั้งหมดมีอิเล็กตรอนอยู่
เราก็เริ่มจับคู่สปินได้
เราใส่อิเล็กตรอนตัวที่ 8 ของออกซิเจนในนี้ได้
เราก็เริ่มจับคู่สปินของเรา
เรามีอิเล็กตรอน 4 ตัวใน 2p ออร์บิทัล

Korean: 
2p4를 씁니다
그래서 1s2 2s2 2p4가 됩니다
2+2+4를 하면
산소(O)의 전자 배치에서 나타내야 될
산소(O)의 전자 배치에서 나타내야 될
전자의 총 개수인 8이 나옵니다
전자의 총 개수인 8이 나옵니다
플루오린(F)으로 넘어갑시다
플루오린(F)은 다른 초록색을 씁시다
플루오린(F)을 보면
총 9개의 전자가 있습니다
다시 한번 스핀을 짝지어 봅니다
그래서 플루오린(F)의
아홉 번째 전자를 저기 더하고
여기에 씁시다
플루오린(F)에는
1s2, 2s2를 쓰고 5개의 전자가
있다는 것을 고려해야 합니다
그러니까 플루오린(F)은 2p5도 가집니다
그리고 마지막으로 네온(Ne)를 해봅시다
네온은 10개의 전자를 가지고 있습니다
그래서 처리해야 할 전자가 1개 더 있습니다

Thai: 
สำหรับออกซิเจน เราก็เขียน 2p4
1s2, 2s2, 2p4
สังเกตว่าถ้าคุณบวกเลขเหล่านี้เข้าด้วยกัน
2 กับ 2 กับ 4 คุณจะได้ 8
ซึ่งก็คือจำนวนอิเล็กตรอนทั้งหมด
ที่เรามีเพื่อแทนการจัด
อิเล็กตรอนของออกซิเจน
ลองไปยังฟลูออรีนกัน
ลองใช้สีเขียวอีกแบบสำหรับฟลูออรีนกัน
สมมุติว่าฟลูออรีนอยู่ตรงนี้
อิเล็กตรอนทั้งหมด 9 ตัว
เหมือนเดิม เราจับคู่สปิน
เราใส่อิเล็กตรอนตัวที่ 9 ของฟลูออรีนลงในนี้
เราลงมือเขียนมันตรงนี้ได้
สำหรับฟลูออรีน เราจะเขียน
1s2, 2s2, และสังเกตว่า
ตอนนี้เรามีอิเล็กตรอน 5 ตัว
2p5 สำหรับฟลูออรีน
แล้วสุดท้าย ลองไปดูนีออนกัน
นีออนมีอิเล็กตรอน 10 ตัว
เรามีอิเล็กตรอนอีกตัวที่ต้องคิด

English: 
for Oxygen, so we write two p four.
So one s two, two s two, two p four.
Notice if you add these together,
two and two and four then you get eight
which is the total number of electrons
that we had to represent for the electron
configuration for Oxygen.
Let's move on to Fluorine.
So let's use a different
green here for Fluorine.
So let's say Fluorine right here.
Nine total electrons.
So once again, we're pairing up our spins.
So we add Fluorine's
ninth electron to there
and we can go ahead and
write it right here.
So for Fluorine we would write
one s two, two s two, and notice
we have five electrons now.
So two p five would be for Fluorine.
And then finally, let's
go ahead and do Neon.
So Neon has ten electrons.
So we have one more
electron to account for.

Bulgarian: 
Така че пишем 2р4.
1s2 2s2 2р4.
Забележи, ако събереш тези,
2 и 2 и 4, тогава получаваш 8,
което е общият брой електрони,
които трябваше да представим за електронната конфигурация за кислорода.
Нека преминем към флуорът.
Нека използваме различно зелено за флуора.
Да кажем, флуор – ето тук.
Общо 9 електрона.
Отново, съчетаваме спиновете.
Добавяме деветия електрон на флоура ето тук
и можем да го запишем.
За флуора ще запишем 1s2 2s2
и, забележи, сега имаме 5 електрона.
Тоест за флуора ще е 2р5.
И последно, нека преминем към неона.
Неонът има 10 електрона.
Имаме още един електрон, който трябва да запишем.

Thai: 
เรามีที่ว่างอีกหนึ่งที่ จริงไหม?
อิเล็กตรอนตัวสุดท้ายของนีออนจะไป
ยัง 2p ออร์บิทัลตรงนี้
สำหรับนีออน เราจะเขียน
1s2, 2s2, 2p6
สังเกตว่าเราไม่มีที่ให้ใส่อิเล็กตรอนแล้ว
ในชั้นพลังงานที่ 1 และ 2
เราเต็มแล้ว
ชั้นที่สองตอนนี้ก็เต็ม
และถ้าคุณอยากเพิ่มอิเล็กตรอนอีกตัว
คุณต้องเปิดชั้นใหม่
คุณต้องไปยังชั้นพลังงานที่สาม
และคุณสังเกตรูปแบบตรงนี้
ในตารางธาตุได้
เราบอกว่าการจัดอิเล็กตรอน
ของไฮโดรเจนตรงนี้คือ 1s1
แล้วเราไปตรงนี้ ฮีเลียมคือ 1s2
แล้วเราไปยังชั้นพลังงงานที่ 2
นี่คือลิเธียม อยู่ที่ 2s1
และแบริเลียมอยู่ที่ 2s2

English: 
We have one more space right?
The last electron for Neon would go
into a two p orbital here.
So for Neon we would write,
one s two, two s two, two p six.
Notice we have no more
places to put electrons,
in the first or the second energy levels.
We are completely full.
So the second shell is now full
and if you wanted to add another electron,
you would have to open up a new shell.
You would have to go to
the third energy level.
And so you notice a pattern here
emerging on the periodic table.
So we said that Hydrogen's electronic
configuration over here was one s one.
Then we went over here
to Helium was one s two.
And then we moved on to
the second energy level.
So this was Lithium
here ended in two s one.
And Beryllium ended in two s two.

Bulgarian: 
Имаме още едно пространство.
Последният електрон за неона
ще влезе в една 2р орбитала.
За неона ще запишем 1s2 2s2 2р6.
Забележи, нямаме повече места, в които да поставяме електрони,
в първото или във второто енергийно ниво.
Напълно сме запълнили местата.
Втората обвивка сега е запълнена
и ако искаш да добавиш друг електрон,
тогава ще трябва да отвориш нова обвивка.
Трябва да преминеш към третото енергийно ниво.
И забелязваш модел тук,
който виждаме от периодичната таблица.
Казахме, че електронната конфигурация за водорода беше 1s1.
После преминахме към хелий, който беше 1s2.
И после преминахме към второто енергийно ниво.
Това беше литият, който приключваше с 2s1.
И берилият приключваше с 2s2.

Korean: 
자리가 하나 더 있죠?
네온(Ne)의 마지막 전자는
여기 이 2p오비탈에 갈 것입니다
네온(Ne)에서는
1s2 2s2 2p6를 쓸 것입니다
네온(Ne)에서는
1s2 2s2 2p6를 쓸 것입니다
첫 번째와 두 번째 에너지 준위에는
더 이상 전자를 놓을 자리가 없습니다
완전히 찼습니다
두 번째 전자 껍질이 이제 다 찼고
다른 전자를 더하고 싶다면
새로운 전자 껍질이 필요할 것입니다
세 번째 에너지
준위로 가야 할 것입니다
주기율표에서 드러나는
패턴을 볼 수 있습니다
수소(H)의 전자 배치는
1s1이었습니다
수소(H)의 전자 배치는
1s1이었습니다
그 다음 헬륨(He)은 1s2였습니다
그리고 두 번째 에너지 준위로
옮겨갔습니다
그리고 리튬(Li)은
2s1에서 끝났습니다
그 다음 붕소(B)는 2s2에서 끝났습니다

English: 
And then we filled the s orbital
and moved on to the p orbitals.
And notice we have over here,
Boron's last electron was two p one,
Carbon's two p two,
Nitrogen's two p three,
Oxygen's two p four, Flourine's two p five
and Neon is two p six.
So notice we have these
six boxes over here
on the periodic table.
Those represent our p orbitals.
And then over here on the left
we have these two boxes representing
our s orbital.
And so that's the idea.
The s orbital, we have one of them,
holds a maximum of two electrons.
We have these two boxes
on the periodic table.
Over here on the right,
we had these six boxes
which is the maximum number of electrons
we can put into the p orbitals
because we have three p orbitals,
each one can hold two.
So noticing these patterns on
the periodic table helps you
when you are writing
electron configurations.
You can just sit down and look at
the periodic table and write them out
after you've had enough practice.

Thai: 
แล้วเราก็เติม s ออร์บิทัล
แล้วเลื่อนไปยัง p ออร์บิทัล
สังเกตสิ่งที่เรามีตรงนี้
อิเล็กตรอนตัวสุดท้ายของโบรอนคือ 2p1
คาร์บอนคือ 2p2 ไนโตรเจนคือ 2p3
ออกซิเจนคือ 2p4 ฟลูออรีนคือ 2p5
และนีออนคือ 2p6
สังเกตว่าเรามี 6 กล่องตรงนี้
บนตารางธาตุ
พวกมันแสดง p ออร์บิทัล
แล้วตรงนี้ทางซ้าย
เรามี 2 กล่องแสดง
s ออร์บิทัล
และนั่นคือแนวคิด
s ออร์บิทัล เรามีหนึ่งอันตรงนี้
มีอิเล็กตรอนสูงสุด 2 ตัว
เรามีกล่อง 2 อันนี้บนตารางธาตุ
ตรงนี้ทางขวา เรามี 6 กล่องนี้
ซึ่งเป็นจำนวนอิเล็กตรอนสูงสุด
ที่เราใส่ลงใน p ออร์บิทัลได้
เพราะเรามี p ออร์บิทัล 3 อัน
แต่ละอันใส่ได้ 2 ตัว
การสังเกตรูปแบบเหล่านี้
บนตารางธาตุ ช่วยคุณ
เวลาเขียนการจัดอิเล็กตรอน
คุณนั่งลงดู
ตารางธาตุ และเขียนออกมาได้
หลังจากที่คุณฝึกมากพอ

Korean: 
s오비탈을 다 채운 다음
p오비탈로 넘어갔습니다
붕소(B)의 마지막 전자는 2p1이었습니다
붕소(B)의 마지막 전자는 2p1이었습니다
탄소(C)는 2p2이고 질소(N)는 2p3이며
산소(O)는 2p4, 플루오린(F)은 2p5이고
네온은 2p6입니다
여기 주기율표상에
6개의 박스들이 있습니다
여기 주기율표상에
6개의 박스들이 있습니다
저것들은 p오비탈을 나타냅니다
그리고 왼쪽 여기에 있는 두 박스는
s오비탈을 나타냅니다
s오비탈을 나타냅니다
여기서 생각해볼 수 있습니다
하나 있는 s오비탈은
최대 2개의 전자를 가질 수 있습니다
주기율표상에 이 두 박스가 있습니다
여기 이 오른쪽에는
박스가 6개 있는데
이것은 p오비탈에 넣을 수 있는
최대 전자 개수에 해당됩니다
3개의 p오비탈은 각각
전자 두 개씩을 가질 수 있기 때문입니다
주기율표상의 이 패턴을
알아내는 것은
주기율표상의 이 패턴을
알아내는 것은
전자 배치를 쓸 때 도움을 줍니다
충분한 연습을 한 뒤에는
그냥 앉아서 주기율표를 보고도
전자 배치를 쓸 수 있게 될 것입니다

Bulgarian: 
И после запълнихме s орбиталата,
и преминахме към р орбиталите.
Забележи, боронът беше 2p1.
Въглеродът беше 2р2, азотът – 2р3.
Кислородът е 2р4, флуорът – 2р5.
А неонът е 2р6.
Забележи, тук в периодичната таблица имаме тези шест квадратчета.
Тези представляват р орбиталите.
И тук вляво имаме 2 квадратчета,
които представляват s орбиталата.
Това е идеята.
s орбиталата – имаме една от тях –
съдържа максимум два електрона.
Имаме тези две квадратчета на периодичната таблица.
Тук вдясно имаме тези шест квадратчета,
което е максималният брой електрони,
които можем да поставим в р орбиталите,
понеже имаме 3 р орбитали,
а всяка от тях може да съдържа 2 електрона.
Забелязването на тези модели на периодичната таблица ти помага,
когато записваш електронните конфигурации.
Можеш да седнеш и да погледнеш периодичната таблица, и да ги запишеш,
след като се поупражняваш достатъчно.

Bulgarian: 
Реши всички тези отново и помисли за електронните конфигурации,
къде поставяш електроните и как това се свързва със структурата на периодичната таблица.

English: 
So make sure to do all of these again
and think about electron configurations.
Where you're putting your electrons
and think about how it relates
to the structure of the periodic table.

Thai: 
อย่าลืมลองทำเองอีกครั้ง
คิดถึงการจัดอิเล็กตรอนนี้ดู
โดยคุณใส่อิเล็กตรอน
และคิดว่ามันเกี่ยวข้อง
กับโครงสร้างของตารางธาตุอย่างไร

Korean: 
반드시 이 모든 것을 다시 해보고
전자 배치를 할 때
전자를 어디에 놓을지
생각해보시기 바랍니다
그리고 그것이 주기율표의 구조와 어떤
연관이 있는지도 생각해보길 바랍니다
그리고 그것이 주기율표의 구조와 어떤
연관이 있는지도 생각해보길 바랍니다
