
French: 
l;kk
lo

Bulgarian: 
В тази поредица от видеа ще прогнозираме формите на молекулите и йоните,
като използваме VSEPR, което е акроним за
отблъскване на електронните двойки във валентния слой.
И това означава, че електроните,
тъй като са отрицателно заредени, ще се отблъскват взаимно.
Еднаквите заряди се отблъскват
и когато тези електрони около един централен атом се отблъснат,
те ще доведат до определена форма на молекулата или йона.
Първата стъпка за прогнозиране
на формата на една молекула или един йон
е да начертаем точковата структура, за да покажем валентните електрони.
И нека начертаем точковата структура за BeCl2.
Намираш берилия на периодичната таблица.
Той е в група 2, тоест два валентни електрона.
Хлорът е в седма група и имаме два хлорни атома.
2*7 е 14.
И 14 + 2 ни дава общо 16 валентни електрона,
които трябва да отчетем в точковата си структура.
Поставяш най-слабо електроотрицателния атом в центъра.
Берилият отива в центъра.

English: 
This next set of
videos, we're going
to predict the shapes
of molecules and ions
by using VSEPR, which is an
acronym for valence shell
electron pair repulsion.
And really all this
means is that electrons,
being negatively charged,
will repel each other.
Like charges repel, and
so when those electrons
around a central atom
repel each other,
they're going to
force the molecule
or ion into a particular shape.
And so the first
step for predicting
the shape of a
molecule or ion is
to draw the dot structure to
show your valence electrons.
And so let's go ahead and draw
a dot structure for BeCl2.
So you find beryllium
on the periodic table.
It's in group 2, so
two valence electrons.
Chlorine is in group 7,
and we have two of them.
So 2 times 7 is 14.
And 14 plus 2 gives us a
total of 16 valence electrons
that we need to account
for in our dot structure.
So you put the less
electronegative atom
in the center.
So beryllium goes in the center.

Korean: 
 
다음 비디오에서
우리는 분자와 이온의 모양을 알아 보겠습니다
"원자가껍질 전자쌍 반발' 의 머리글자인
VSEPR 을 이용하여
즉 ,음전하를 띤 전자들은 서로서로
밀어낸다는 의미입니다
전하들이 밀어내듯이,중심원자를 둘러싸고 있는
전자들은 서로를 밀어냅니다
전자들은 분자나 이온이
특정한 모습이 되도록 힘을 가할 것입니다
그래서 분자나 이온의 모양을 알아보는 처음 단계는
원자가 전자를 보여주기 위하여
전자점식을 그리는 것입니다
자 이제, BeCl2 를 위한 점자식을 그려봅시다
주기율표에서 베릴률을 찾아보면
그것은, 2 군에있어서
2원자가전자를 갖고 있고
염소는 7군에 속하고 
우리는 2개의 염소를 갖고 있습니다
그래서 2 곱하기 7은 14 겠죠
그리고 14 플러스 2는 총 16개의 원자가전자를 갖습니다
저는  점자식에서 이것들을 설명해보겠습니다
전기음성도가 작은 원자를
중앙에 배치합니다
그래서 베릴륨은 중앙으로 배치하고

Thai: 
 
ในวิดีโอชุดต่อไปนี้ เราจะ
ทำนายรูปร่างของโมเลกุลและไอออน
โดยใช้ VSEPR ย่อมาจาก Valence Shell
Electron Pair Repulsion
จริงๆ แล้วมันหมายความว่า อิเล็กตรอน
มีประจุลบ จะผลักกัน
ประจุเหมือนกันผลักกัน เมื่ออิเล็กตรอน
รอบอะตอมกลางผลักกัน
พวกมันจะบังคับให้โมเลกุล
หรือไอออนมีรูปร่างเจาะจง
และขั้นตอนแรกของการทำนาย
รูปร่างโมเลกุลหรือไอออนคือ
วาดโครงสร้างจุดเพื่อแสดงวาเลนซ์อิเล็ตกรอน
ลองลงมือวาดโครงสร้างจุดสำหรับ BeCl2 กัน
คุณหาแบริเลียมในตารางธาตุ
มันอยู่ในหมู่ 2 วาเลนซ์อิเล็กตรอน 2 ตัว
คลอรีนอยู่ในหมู่ 7 และเรามี 2 ตัว
2 คูณ 7 เป็น 14
และ 14 บวก 2 ให้
วาเลนซ์อิเล็กตรอนทั้งหมด 16 ตัว
ที่เราต้องนับสำหรับโครงสร้างจุด
คุณก็ใส่อะตอมที่อิเล็กโตรเนกาทีฟน้อยกว่า
ไว้ตรงกลาง
แบริเลียมไปอยู่ตรงกลาง

English: 
We know it is surrounded
by two chlorines,
so we show beryllium bonded
to two chlorines here.
And we just represented
four valence electrons.
So here's two valence electrons.
And here's another two
for a total of four.
So, instead of 16,
we just showed four.
So now we're down to
12 valence electrons
that we need to account for.
So 16 minus 4 is 12.
We're going to put those left
over electrons on our terminal
atoms, which are our chlorines.
And chlorine is going to
follow the octet rule.
Each chlorine is
already surrounded
by two valence electrons, so
each chlorine needs six more.
So go ahead and put six
more valence electrons
on each chlorine.
And, since I just represented
12 more electrons there,
now we're down to
0 valence electron.
So this dot structure has
all of our electrons in it.
And some of you might think,
well, why don't you keep going?
Why don't you show some of
those lone pairs of electrons
in chlorine moving in to
share them with the beryllium
to give it an
octet of electrons?
And the reason you don't is
because of formal charge.

Korean: 
베릴륨은 두 염소에 의해 둘러싸이게 되니
우리는 두 염소에 둘러싸인 베릴륨을 보게 됩니다
방금 원자가 전자 4개를 표시했습니다
여기 원자가전자 2개가 있습니다
그리고 여기 또 다른 2개로 총 4개
그래서 16개 대신 오직 4개만 보였습니다
이제 지금은 12개 원자가 전자가 남았습니다
저는 그것을설명해 보겠습니다
16 빼기 4는 12입니다
이제 이 남은 전자를 말단부분에 몰아줍니다
그리고 염소는 옥텟 규칙을 따르겠죠
각 염소는 이미
두 원자가 전자가 있어서
각각 여섯개 더 필요합니다
그래서 원자가 전자를
각각의 염소에 6개씩 줍니다
그리고  12 개의 전자를 표현했기에
원자가 전자가 0개 남았습니다
따라서 전자점식이  모든 전자를 가지고 있습니다
그리고 여러분 중 몇몇은 
그과정을 계속 진행하기를 바랄것입니다
염소에 있는 몇몇의 비공유전자쌍들을
베릴률과 공유하기 위하여 이동시켜서
옥텟규칙을 만족시켜 주면 어떨까요?
그럴 필요가 없는 이유는 형식전하 때문입니다

Thai: 
เรารู้ว่ามีคลอรีนสองตัวล้อมรอบ
เราแสดงแบริเลียม
มีพันธะกับคลอรีนสองตัวตรงนี้
และเราแสดงวาเลนซ์อิเล็กตรอนไป 4 ตัว
นี่คือวาเลนซ์อิเล็กตรอน 2 ตัว
นี่คืออีก 2 ตัวรวมเป็น 4
แทนที่จะเป็น 16 เราเพิ่งแสดงไป 4
ตอนนี้เราเหลือวาเลนซ์อิเล็กตรอน 12 ตัว
ที่เราต้องจัดการ
16 ลบ 4 ได้ 12
เราจะใส่อิเล็กตรอนที่เหลือลงใน
อะตอมปลาย ซึ่งก็คือคลอรีน
คลอรีนจะทำตามกฎออกเตท
คลอรีนแต่ละตัวถูกล้อมด้วย
วาเลนซ์อิเล็กตรอน 2 ตัว
คลอรีนแต่ละตัวจึงต้องการอีก 6
ลงมือใส่วาเลนซ์อิเล็กตรอนอีก 6 ตัว
ให้คลอรีนแต่ละตัว
เนื่องจากผมใส่อิเล็กตรอนอีก 12 ตัวตรงนี้
ตอนนี้เราเหลือวาเลนซ์อิเล็กตรอน 0 ตัว
โครงสร้างจุดนี้มีอิเล็กตรอนครบแล้ว
คุณอาจคิดว่า ทำไมไม่ทำต่อล่ะ?
คุณไม่ต้องเอาอิเล็กตรอนคู่โดดเดี่ยว
ในคลอรีนมาแบ่งกับแบริเลียม
ให้ได้อิเล็กตรอนเป็นออกเตทเหรอ?
สาเหตุที่คุณไม่ต้องทำ คือประจุทางการ

Bulgarian: 
Знаем, че е ограден от два хлорни атома,
така че показваме берилия, свързан с два хлорни атома.
И току-що представихме четири валентни електрона.
Това са два валентни електрона.
И това са още два за общо 4.
Вместо 16, току-що показахме 4.
Сега слязохме до 12 валентни електрона,
които трябва да отчетем.
16 минус 4 е 12.
Ще поставим останалите електрони към крайните атоми, които са хлорните атоми.
И хлорът ще следва октетното правило.
Всеки хлорен атом вече е ограден от два валентни електрона,
така че на всеки хлорен атом му трябват още 6.
Поставяме още 6 валентни електрона
към всеки хлорен атом.
И след като току-що представих още 12 електрона тук,
сега слязохме до 0 валентни електрона.
Тази точкова структура има всички наши електрони.
И може да си помислиш защо просто не продължа.
Защо не покажа някои от тези свободни двойки електрони в хлора,
които се придвижват, за да бъдат споделени с берилия,
за да му дам един октет електрони?
И причината да не направя това е поради формалния заряд.

Thai: 
ลองลงมือกำหนดประจุทางการ
ให้อะตอมแบริเลียมตรงกลางกัน
นึกดู พันธะโควาเลนต์แต่ละตัว
ประกอบด้วยอิเล็กตรอน 2 ตัว
ผมก็ลงมือใส่มันลงไป
และถ้าผมอยากหาประจุทางการ
ก่อนอื่น ผมจะคิดถึงจำนวนวาเลนซ์อิเล็กตรอน
ในอะตอมอิสระ
มันจะเท่ากับ 2 -- สำหรับแบริเลียม
เรามีอิเล็กตรอน 2 ตัวในอะตอมอิสระ
แล้วเราก็คิดถึงอะตอมที่มีพันธะตรงนี้
เมื่อผมดูพันธะโควาเลนต์
ผมจะให้อิเล็กตรอนหนึ่งตัวกับคลอรีน 
และอิเล็กตรอนอีกตัว
ให้กับแบริเลียม
ผมทำแบบเดียวกันกับพันธะนี่ตรงนี้
คุณเห็นได้ว่ามันล้อมรอบ
ด้วยวาเลนซ์อิเล็กตรอน 2 ตัว
2 ลบ 2 ให้ค่าประจุทางการเป็น 0
นั่นคือวิธีคิดวิธีหนึ่งว่าทำไมคุณถึงหยุดตรงนี้
เวลาหาโครงสร้างจุด
มันมีวาเลนซ์อิเล็กตรอนแค่ 2 ตัว
ถึงแม้ว่ามันอยู่ในคาบที่ 2 แต่มันไม่จำเป็น
ต้องทำตามกฎออกเตท
มันมีอิเล็กตรอนน้อยกว่า 8 ตัวได้
ย้ำอีกครั้ง ประจุทางการช่วย

English: 
So let's go ahead and
assign a formal charge
to the central
beryllium atom here.
So remember each of
our covalent bonds
consists of two electrons.
So I go ahead and put that in.
And if I want to
find formal charge,
I first think about the number
of the valence electrons
in the free atom.
And that would be two,
four-- four berylliums.
So we have two electrons
in the free atom.
And then we think about
the bonded atom here,
so when I look at
the covalent bond,
I give one of those electrons
to chlorine and one of those
electrons to beryllium.
And I did the same thing
for this bond over here,
and so you can see
that it is surrounded
by two valence electrons.
2 minus 2 gives us a
formal charge of 0.
And so that's one way to think
about why you would stop here
for the dot structure.
So it has only two
valence electrons,
so even though it's in period
2, it doesn't necessarily
have to follow the octet rule.
It just has to have less
than eight electrons.
And so, again,
formal charge helps

Bulgarian: 
Нека поставим формалния заряд
към централния атом берилий тук.
Помни, всяка от ковалентните ни връзки се състои от два електрона.
Поставям това.
Ако искам да намеря формалния заряд,
първо мисля за броя валентни електрони в свободния атом.
И това ще са 2, 4 – 4 атома берилий.
Имаме два електрона в свободния атом.
И после мислим за свързания атом.
Когато погледна ковалентната връзка,
давам един електрон на хлора
и един от тези електрони на берилий.
И направих същото нещо за тази връзка ето тук.
И можеш да видиш, че това е оградено от два валентни електрона.
2 минус 2 ни дава формален заряд от 0.
И това е един начин да помислим защо ще спреш тук
за точковата структура.
Има само два валентни електрона,
въпреки че е в период 2,
не е задължително да следва октетното правило.
Просто трябва да има по-малко от 8 електрона.
И, отново, формалният заряд помага

Korean: 
여기 중앙에 있는 베릴륨 원자에
형식전하를 배정해 보겠습니다.
기억해야 할것은
공유결합은
2개의 전자들로 구성되어 있다는 것입니다
그래서 저는 그것을 넣고
그리고 제가 만약 형식전하를 찾기를 원한다면
자유원자 안에서 원자가전자의
수에대해서 먼저 생각해봐야 합니다
그것은 2쌍 ,즉 4개입니다
그래서 우리는 자유원자안에서 2개의 전자들을 가지고  있습니다
그리고 우리는 여기서 결합한 원자들에 대해 생각해봅니다
우리가 공유결합을 생각해볼때
하나는 염소에 전자들중 하나를 주고
또 다른 하나는 베릴륨에 줍니다
그리고 저는  이 쪽 결합에도 같은 작업을 해줍니다
그래서 여러분들은 2개의 원자가 전자들에 의해서
그것이 둘러싸여 있는 것을 보게 됩니다
"2-2=0" 의 형식전하가 되므로
우리가 전자점식 을 위한
과정을 완료했습니다
그래서 그것은 단지 두개의 원자가 전자를 가지고 있습니다
그러므로 그것이 2번 주기에 해당된다할지라도
반드시 옥텟규칙을 따라야할 필요는 없습니다
그것은 8개의 전자보다 더 적게 가져야하고
또 게다가 형식전하 측면에서도 여기서 전자점식을 위한

English: 
you understand why you can stop
here for your dot structure.
Let me go ahead and
redraw our molecule
so we can see it a
little bit better.
And we'll go ahead and
move on to the next step.
So let me go ahead and
put in my lone pairs
of electrons around
my chlorine here.
So we have our dot structure.
Next, we're going to count
the number of electron clouds
that surround the central atom.
And I like to use the
term electron cloud.
You'll see many
different terms for this
in different textbooks.
You'll see charge clouds,
electron groups, electron
domains, and they have
slightly different definitions
depending on which
textbook you look in.
And really the term
of electron cloud
helps describe the idea
of valence electrons
in bonds and in lone
pairs of electrons
occupying these electron clouds.
And you could think about them
as regions of electron density.
And, since electrons
repel each other,
those regions of electron
density, those clouds,
want to be as far
apart from each other
as they possibly can.

Korean: 
단계는 멈춰도 되는 이유가 될수 있습니다
이 쯤에서 조금더 잘 이해할수 있도록
분자를 다시 그려보겠습니다
그리고 그 다음 단계도 설명해 보겠습니다
자, 여기에 염소주변에
비공유전자쌍을 그려넣겠습니다
그래서 여기에  우리의 전자점식이 있습니다
이제 다음단계로 중심원자를 둘러싸고 있는
전자구름의 수를 세어보겠습니다
저는  "전자구름"이라는 용어를 사용하기를 좋아합니다만
여러분들은 각각의 다른 교재마다
다르게 표현하는 단어를 접할수도 있습니다
여러분이 사용하시는 교재의 종류에 따라
"하전운모형" , "전자그룹', '전자영역"
이란 용어를 사용하기도 합니다
그리고  "전자구름' 이야말로
전자구름을 포함하고 있는 비공유전자쌍이나 원자가전자에 대한
개념을 설명하는데
가장 적합하다고 생각합니다
그리고 여러분은 전자구름을 전자들의 밀도의 영역으로 생각하셔도 됩니다
왜냐하면 전자들은 서로서로 밀어내려하기 때문에
그러한 전자밀도는  (전자구름들)
그들이 가능한한  서로서로
떨어져있기를 원합니다

Bulgarian: 
да разбереш защо можеш да спреш точковата структура дотук.
Нека начертая отново нашата молекула,
така че да можем да я видим малко по-добре.
И ще преминем към следващата стъпка.
Нека поставя свободните двойки електрони около хлора.
Имаме точковата си структура.
След това ще преброим колко са електронните облаци,
които ограждат централния атом.
Харесва ми да използвам термина електронен облак.
Ще видиш много различни термини за това в различните учебници.
Ще видиш облаци на заряда, електронни групи, електронни множества
и всички те имат леко по-различни определения,
в зависимост от това кой учебник имаш.
И терминът електронен облак ти помага да опишеш идеята за валентни електрони във връзки
и в свободни двойки електрони,
които обитават тези електронни облаци.
И можеш да помислиш за тях като за области с електронна плътност.
И след като електроните се отблъскват взаимно,
тези области на електронна плътност, тези облаци,
искат да са колкото е възможно по-отдалечени един от друг.

Thai: 
ให้คุณเข้าใจสาเหตุที่คุณหยุดหา
โครงสร้าจุดตรงนี้
ขอผมลงมือวาดโมเลกุลใหม่
เราจะได้เห็นชัดขึ้น
และเราก็ไปยังขั้นต่อไป
ขอผมลงมือใส่อิเล็กตรอนคู่โดดเดี่ยว
รอบคลอรีนตรงนี้
เรามีโครงสร้างจุด
ต่อไป เราจะนับจำนวนเมฆอิเล็กตรอน
ที่ล้อมรอบอะตอมกลาง
ผมชอบใช้คำว่าเมฆอิเล็กตรอน
คุณจะเห็นคำเรียกหลายแบบ
ในหนังสือเรียน
คุณจะเห็นคำว่า เมฆประจุ กลุ่มอิเล็กตรอน
อิเล็กตรอนโดเมน และพวกมันมีนิยามต่างกัน
เล็กน้อยขึ้นอยู่กับหนังสือที่คุณดู
และจริงๆ แล้ว คำว่าเมฆอิเล็กตรอน
ช่วยบรรยายแนวคิดเรื่องวาเลนซ์อิเล็กตรอน
ในพันธะและในคู่โดดเดี่ยว
ซึ่งกินพื้นที่เป็นเมฆอิเล็กตรอนพวกนี้
และคุณคิดถึงมันเป็นขอบเขตของ
ความหนาแน่นอิเล็กตรอนก็ได้
และเนื่องจากอิเล็กตรอนผลักกัน
เขตความหนาแน่นอิเล็กตรอนเหล่านั้น 
เมฆเหล่านั้น
อยากห่างจากกัน
ให้มากที่สุดเท่าที่ทำได้

Korean: 
자, 이제 여기있는 우리의 분자를 분석해 보겠습니다
우리는 여기서 중심 원자를
둘러싼 결합전자를
볼수 있습니다
그래서 우리는 그것들을 전자구름으로서 여길수 있습니다
여기에 또하나의 전자구름이 형성되고
그래서 결국 우리는 이 분자에서 2개의 전자구름을 갖게 됩니다
그리고 그 2개의 전자구름들은 서로 떨어져 있으며
또한 그것들이 서로 반대방향에 있으며
동시에 중심원자를 둘러싼
구름의 모양과 형태가
여기에서 보듯이
'직선형"이 됨을 알수 있습니다
우리는 비공유 전자쌍은 고려하지
않으므로 이 분자는 직선형이 됩니다
그래서 우리는 이 분자의 형태를
선형분자라고 예측할수 있습니다
그리고 선형분자의 경우 결합각은
다시말해서, 베릴륨과 염소 사이의 각은
180 도가 되겠습니다
단지 직선의 형태가 된다는 의미입니다
자 ,이제
이것이 분자의 구조를 예측하기 위하여 VSEPR를  사용하는 방법입니다

Thai: 
ลองลงมือวิเคราะห์โมเลกุลของเราตรงนี้
ล้อมรอบอะตอมตรงกลาง
เราเห็นได้ว่าตรงนี้คืออิเล็กตรอนที่มีพันธะตรงนี้
ล้อมรอบอะตอมกลางของเรา
เราก็คิดถึงพวกมันเป็นเมฆอิเล็กตรอนได้
แล้วตรงนี้ เรามีเมฆอิเล็กตรอนอีกอัน
เรามีเมฆอิเล็กตรอนสองตัวสำหรับโมเลกุลนี้
และเมฆอิเล็กตรอนเหล่านี้ห่างกันที่สุด
เมื่อพวกมันอยู่ในทิศตรงกันข้าม
เรขาคณิตหรือรูปร่างของเมฆอิเล็กตรอน
รอบอะตอมกลาง ถ้าพวกมัน
ชี้ในทิศตรงข้าม
มันจะได้รูปร่างเป็นเส้นตรงตรงนี้
โมเลกุลนี้จริงๆ แล้วเป็นเส้นตรง
เพราะเราไม่มีคู่โดดเดี่ยวให้คิดตรงนี้
เราก็ลงมือทำนาย
เรขาคณิตของโมเลกุลนี้ว่าเป็นเส้นตรงได้
และถ้ามันเป็นเส้นตรง เราก็บอกได้ว่ามุมพันธะ --
มุมระหว่างคลอรีน แบริเลียม
และคลอรีนอีกตัว -- เท่ากับ 180 องศา
แค่เส้นตรง
เอาล่ะ
นั่นนคือวิธีใช้ VSEPR เพื่อทำนายรูปร่าง

English: 
And so let's go ahead and
analyze our molecule here.
So surrounding the central atom.
So we can see that here are some
bonding electrons right here
surrounding our central atom.
So we could think about those
as being an electron cloud.
And then over here we have
another electron cloud.
So we have two electron
clouds for this molecule,
and those electron
clouds are furthest apart
when they point in
opposite directions.
And so the geometry or
the shape of the electron
clouds around the
central atom, if they're
pointing in opposite
directions, it's
going to give you a
linear shape here.
So this molecule
is actually linear
because we don't have any lone
pairs to worry about here.
So we're going to
go ahead and predict
the geometry of the
molecule as being linear.
And if that's linear, then
we can say the bond angle--
so the angle between the
chlorine, the beryllium,
and the other chlorine--
is 180 degrees.
So just a straight line.
All right.
So that's how to use VSEPR
to predict the shape.

Bulgarian: 
Нека анализираме молекулата си.
Ограждащи централния атом.
Можем да видим, че има няколко свързващи електрона тук,
които ограждат централния атом.
Можем да ги приемем за един електронен облак.
И ето тук имаме друг електронен облак.
Имаме два електронни облака за тази молекула,
а тези електронни облаци са най-отдалечени,
когато сочат в противоположни посоки.
И геометрията, или формата на електронните облаци около централния атом...
ако те сочат в противоположни посоки,
това ще ти даде линейна форма.
Тази молекула е линейна,
понеже не трябва да се притесняваме за свободни електронни двойки.
Ще продължим нататък и ще прогнозираме
геометрията на молекулата като линейна.
И ако тя е линейна, тогава можем да кажем, че ъгълът на свързване –
ъгълът между хлора, берилия и другия хлорен атом – е 180 градуса.
Просто права линия.
Добре.
Ето така използваш теорията за отблъскване на електронните двойки (VSEPR),
за да прогнозираш формата.

English: 
Let's do another example.
So CO2-- so carbon dioxide.
So we start off by drawing
the dot structure for CO2.
Carbon has four
valence electrons.
Oxygen has six.
And we have two of them.
So 6 times 2 gives us 12.
12 plus 4 gives us
16 valence electrons
to deal with for
our dot structure.
The less electronegative
atom goes in the center,
so carbon is bonded to oxygen,
so two oxygens like that.
We just represented
four valence electrons.
Right?
So two here and two
here, so that's four.
So 16 minus 4 gives us 12
valence electrons left.
Those electrons are going to
go on our terminal atoms, which
are oxygens if we are going
to follow the octet rule.
So each oxygen is
surrounded by two electrons.
So, therefore, each oxygen needs
six more valence electrons.
I'll go ahead and put in
six more valence electrons
on our oxygen.
Now you might think we're
done, but, of course, we're
not because carbon is going
to follow the octet rule.
Carbon does not have
a formal charge of 0
in this dot structure,
so even though we've

Thai: 
ลองทำตัวอย่างอีกอันกัน
CO2 -- คาร์บอนไดออกไซด์
เราเริ่มด้วยการวาดโครงสร้างจุดของ CO2
คาร์บอนมีวาเลนซ์อิเล็กตรอน 4 ตัว
ออกซิเจนมี 6
และเรามีออกซิเจน 2 ตัว
6 คูณ 2 ให้ค่าเป็น 12
12 บวก 4 ให้ค่าเป็นวาเลนซ์อิเล็กตรอน 16 ตัว
ที่ต้องคิดโครงสร้างจุด
อะตอมที่อิเล็กโตรเนกาทีฟน้อยกว่า
อยู่ตรงกลาง
คาร์บอนจึงทำพันธะกับออกซิเจน
ออกซิเจน 2 ตัวอย่างนั้น
เราเพิ่งแสดงวาเลนซ์อิเล็กตรอนไป 4 ตัว
จริงไหม?
2 ตัวตรงนี้ กับ 2 ตรงนี้ นั่นคือ 4
16 ลบ 4 ให้ค่าเหลือวาเลนซ์อิเล็กตรอน 12 ตัว
อิเล็กตรอนเหล่านั้น
จะไปอยู่ในอะตอมปลาย
ซึ่งก็คือออกซิเจน ถ้าเราทำตามกฎออกเตท
ออกซิเจนแต่ละตัวถูกล้อมด้วยอิเล็กตรอน 2 ตัว
เพราะฉะนั้น ออกซิเจนแต่ละตัวต้องการ
วาเลนซ์อิเล็กตรอนอีก 6 ตัว
ผมจะลงมือใส่วาเลนซ์อิเล็กตรอนอีก 6 ตัว
ให้กับออกซิเจน
ทีนี้ คุณอาจคิดว่าเราเสร็จแล้ว แต่แน่นอน
เรายังไม่เสร็จ 
เพราะคาร์บอนจะทำตามกฎออกเตท
คาร์บอนไม่ได้มีประจุทางการเป็น 0
ในโครงสร้างจุดนี้ ถึงแม้ว่าเรา

Korean: 
또 다른 예를 들어 보겠습니다
CO2( 이산화탄소)를 예로 들겠습니다
이산화탄소의 전자점식을 먼저 그리겠습니다
탄소는 4개의 원자가전자를 가지고 있고
산소는 6개의 원자가전자를 가지고 있고
그런데 우리는 산소를 2개 가지고 있으니
6곱하기 2를 하니 12가 되어
거기에 4를 더하여 16개의 원자가전자를 가지고
전자점식을 그려보겠습니다
더 작은 전기음성도의 전자를 중앙에 위치시키면
탄소는 2개의 산소에 의해 결합되어
우리는 4개의 원자가전자를 나타낼수 있습니다
맞죠?
그래서 여기에 2개 그리고 또 다른2개 하여 4개가 되었습니다
즉,"16-4=12"가 되어 12개가 남습니다
이 여분의 전자들은 말단의 원자들로 분배됩니다
이 경우 산소들이 이 전자들을 받아 옥텟규칙을  따르게 됩니다
그래서 각각의 산소는 2 전자들에 의해 둘러싸이고
그러므로 각각의 산소는 6개의 원자가전자들이 필요로 합니다
그러므로 저는 산소에
원자가전자 6개를 더 그립니다
또한 탄소는 옥텟규칙을 따라야하므로
우리는 다음단계를 실행하겠습니다
비록 우리가 모든 원자가전자를  여기에 나타냈다할지라도
이 점자식에서 탄소는 '0'의 형식전하를

Bulgarian: 
Нека направим друг пример.
СО2 – въглероден диоксид.
Започваме, като чертаем точковата структура за СО2.
Въглеродът има 4 валентни електрона.
Кислородът има 6.
И имаме два такива.
6*2 ни дава 12.
12 + 4 ни дава 16 валентни електрона,
с които трябва да се занимаем в нашата точкова структура.
Най-слабо електроотрицателният атом отива в центъра,
тоест въглеродът е свързан с кислорода, с двата кислородни атома, ето така.
Представихме 4 валентни електрона.
Нали така?
2 тук и 2 тук, това са 4.
16 минус 4 ни дава останали 12 валентни електрона.
Тези електрони ще преминат към крайните ни атоми,
които са кислородните, ако следваме октетното правило.
Всеки кислороден атом е ограден от два електрона.
Следователно всеки кислороден атом има нужда от още 6 валентни електрона.
Ще поставя още 6 валентни електрона към нашия кислороден атом.
Сега можеш да помислиш, че сме готови,
но, разбира се, не сме, понеже въглеродът ще следва октетното правило.
Въглеродът няма формален заряд от 0 в тази точкова структура.

Korean: 
갖고 있지 않기 때문에
우리는 탄소에 옥텟규칙을 적용해야합니다
우리는 탄소에 형식전하 "0"을 주어야합니다
우리는 비공유전자쌍에 있는것을  탄소와 산소사이에 둘이 공유할수 있도록
이렇게 옮겨줌으로써
또한 같은 방법으로
이쪽에 있는 전자도 탄소와 산소사이에 놓아줍니다
이제 우리는 탄소가 2개의 산소에 의해
결합되어 있는 전자점식을 보게 됩니다
그래서 각각의 산소는 3개의 비공유 전자쌍을 갖는 대신에
이제는 단지 2개의
비공유 전자쌍을 갖는 모습을 볼수 있습니다
결과적으로 이것이 우리가 원하던 전자점식이 완성되었습니다
이 분자의 구조를 예측하기 위해 행했던 과정을
다시한번 살펴보겠습니다
첫단계로 원자가전자를 보여주는
전자점식을 그립니다
다음으로,중심원자를 둘러 싸고 있는
전자구름의 수를 세어봅니다
물론 이산화탄소에서는 탄소가
중심원자가 됩니다
그리고 우리는 중심원자를 둘러산
전자들의 영역에 대해 생각해보아야합니다
우리는  전자 밀도영역에 전자의 수에 대해서는 고려하지 않아도 되므로

Thai: 
จะแสดงวาเลนซ์อิเล็กตรอนทั้งหมดไปแล้ว
แต่เรายังต้องการให้คาร์บอนเป็นออกเตท
เราต้องการให้คาร์บอนมีประจุทางการเป็น 0
และเราทำได้โดยเลื่อนอิเล็กตรอนคู่โดดเดี่ยว
ในนี้ไปแบ่งกับอิเล็กตรอนเหล่านั้น
ระหว่างคาร์บอน
กับออกซิเจน และอิเล็กตรอนคู่โดดเดี่ยวนี้ด้วย
เราเลื่อนพวกมันไปอย่างนั้น
และตอนนี้เราเห็นได้ว่าคาร์บอน
ทำพันธะคู่กับออกซิเจน
ตอนนี้ โครงสร้างจุดของเราเป็นแบบนี้
และออกซิเจนแต่ละตัว แทนที่จะมีอิเล็กตรอนคู่
โดดเดี่ยว 3 คู่ ตอนนี้ออกซิเจนแต่ละตัว
มีแค่ 2 คู่อย่างนั้น
นี่่คือโครงสร้างจุด
ลองกลับมาตรงนี้ ดูขั้นตอน
การทำนายรูปร่างของโมเลกุลกัน
ขั้น 1 เสร็จแล้ว วาดโครงสร้าง
เพื่อแสดงวาเลนซ์อิเล็กตรอน
ต่อไป เราจะนับจำนวนเมฆอิเล็กตรอน
ที่ล้อมรอบอะตอมตรงกลาง
เราจะลงมาข้างล่างตรงนี้ 
และเราหาอะตอมตรงกลาง
ซึ่งก็คือคาร์บอน
และเราคิดถึงเขตความหนาแน่นอิเล็กตรอน
ที่ล้อมรอบมัน
เรานับพันธะคู่นี้เป็น
เขตความหนาแน่นอิเล็กตรอนหนึ่งอัน

Bulgarian: 
Затова, въпреки че представихме всички валентни електрони,
трябва да дадем на въглерода един октет.
Трябва да дадем на въглерода формален заряд от 0.
И можем да направим това, като преместим тази свободна двойка електрони ето тук,
за да споделим тези електрони между въглерода и кислорода,
и същото е с тази свободна двойка електрони.
Преместваме ги, ето така.
И сега виждаме, че въглеродът е двойно свързан с кислорода.
Нашата точкова структура изглежда ето така.
Всеки кислороден атом, вместо да има три свободни двойки електрони,
сега всеки кислороден атом има само две свободни двойки, ето така.
Това е точковата ни структура.
Нека се върнем нагоре и да разгледаме стъпките си
за прогнозиране на формата на тази молекула.
Стъпка 1 е готова – "начертай точкова структура,
за да покажеш валентните електрони".
След това ще преброим електронните облаци,
които ограждат централния атом.
Връщаме се тук долу и намираме централния атом,
който е въглерод.
И мислим за областите на електронна плътност,
които го ограждат.
Можем да преброим тази двойна връзка като една област електронна плътност,

English: 
represented all of our
valence electrons now,
we need to give carbon an octet.
We need to give carbon
a formal charge of 0.
And we can do that by moving
in this lone pair of electrons
into here to share those
electrons between the carbon
and the oxygen, and also with
this lone pair of electrons.
So we move those in like that.
And now we can see that carbon
is double bonded to our oxygen.
So now our dot structure
looks like this.
And each oxygen, instead
of having three lone pairs
of electrons, now
each oxygen only
has two lone pairs like that.
So there is our dot structure.
So let's go back up here
to look at our steps
for predicting the
shape of this molecule.
So step 1 is done,
draw dot structure
to show the valence electrons.
Next, we're going to count
the number of electron clouds
surrounding our central atom.
So we go back down here, and
we find our central atom,
which is our carbon.
And we think about the
regions of electron density
that surround that.
So we can count this double bond
as a region of electron density

Bulgarian: 
понеже не се тревожим колко електрона има.
Интересува ни само фактът,
че има област на електронна плътност.
Това е един електронен облак.
И тук имаме друг електронен облак.
Имаме две области на електронна плътност.
Имаме два електронни облака тук,
които ще се отблъскват взаимно.
Когато разгледаме стъпка 3 –
"прогнозирай геометрията на електронните облаци" –
прогнозирай геометрията на електронните облаци
около централния атом.
Тези електронни облаци ще са противоположни един на друг.
Те ще сочат в обратни посоки.
Отново, те ще накарат тази молекула да заеме линейна форма.
Тази молекула въглероден диоксид
също ще е линейна със 180-градусов ъгъл на свързване.
Отново, нямаме свободни двойки електрони на централния атом,
така че не трябва да се притесняваме за това.
И можем да прогнозираме геометрията като линейна.
Така подхождаме към това.
Чертаем точковата структура.
Мислим за електронните облаци
и мислим за формата на молекулите.
В следващото видео ще видим

Korean: 
이식에서 2개의 결합선을  찾을수 있습니다
우리는 전자밀도영역이 있다는
사실만 고려하면 되므로
전자구름은 하나가 있게됩니다
그리고 여기에 또 다른 하나의 전자구름이 있어서
우리는 2개의 전자밀집영역을 갖습니다
최종적으로 우리는 서로서로 밀쳐내고 있는
2개의 전자구름이 여기에 있습니다
그래서
3번째 스텝인
중심원자를 둘러싼
전자구름의 형태는
물런 ,그 전자구름들은
서로서로 반대방향에서
위치되어  있겠고,
그래서 또 다시 언급하자면 이 분자들은 선형상으로
그려지게 되겠습니다
그러므로 이산화탄소는 180도의 결합각을
가진 직선형이 됩니다
우리는 우리의 중앙 원자위에
어떠한 다른 비공유전자쌍도 가지고 있지 않기 때문에
우리는 그점에 대해 걱정할 필요가 없습니다
그리고 이분자는 직선형이라  말할수 있습니다
지금까지 분자의 구조를 어떻게 예측하는지 방법을 알아보았습니다
요약하자면,전자점식을 그리고
전자구름에 대해 생각해본뒤
분자의 모양에 대해 고려해보면 됩니다
이제 다음 비디오에서는 우리는

English: 
because we're not worried about
how many electrons are there.
We're just worried
about the fact
that there is a region
of electron density.
So that's one electron cloud.
And then over here we have
another electron cloud.
So we have two regions
of electron density.
We have two electron
clouds here,
which are going to
repel each other.
So when we look at
step 3-- predict
the geometry of the
electron clouds--
predict the geometry
of the electron
clouds around the central atom.
Well, those electron
clouds are going
to be opposite to each other.
They're going to point
in opposite directions.
So, once again, they're
going to force this molecule
into a linear shape.
So this carbon dioxide
molecule is also
linear with 180
degree bond angle.
So, once again, we don't have
any lone pairs of electrons
on our central atom,
so we don't really
have to worry about that.
And we can go ahead and predict
the geometry as being linear.
So that's how to approach it.
Draw the dot structure.
Think about electron
clouds and think
about the shapes
of your molecules.
In the next video,
we will look at how

Thai: 
เพราะเราไม่สนใจว่ามีอิเล็กตรอนกี่ตัว
เราสนใจแค่ว่า
มันมีเขตความหนาแน่นอิเล็กตรอนหนึ่งอัน
นั่นคือเมฆอิเล็กตรอนหนึ่งอัน
แล้วตรงนี้ เรามีเมฆอิเล็กตรอนอีกอัน
เรามีความหนาแน่นอิเล็กตรอน 2 เขต
เรามีเมฆอิเล็กตรอน 2 ก้อนตรงนี้
ซึ่งจะผลักกัน
เมื่อเราดูขั้นที่ 3 -- ทำนาย
รูปร่างของเมฆอิเล็กตรอน --
ทำนายรูปร่างของเมฆ
อิเล็กตรอนรอบอะตอมตรงกลาง
เมฆอิเล็กตรอนเหล่านั้นจะ
ตรงข้ามกัน
พวกมันจะชี้ทิศตรงกันข้าม
เหมือนเดิม พวกมันจะบังคับโมเลกุลนี้
ให้มีรูปร่างเชิงเส้น
โมเลกุลคาร์บอนไดออกไซด์นี้จะ
เป็นเส้นตรง มีมุมพันธะ 180 องศาเช่นกัน
เหมือนเดิม เราไม่มีอิเล็กตรอนคู่โดดเดี่ยว
ในอะตอมตรงกลาง เราจึงไม่ต้อง
กังวลเรื่องนั้น
และเราก็ลงมือทำนายรูปร่างว่าเป็นเส้นตรงได้
นั่นคือวิธีการคิด
วาดโครงสร้างจุด
คิดถึงเมฆอิเล็กตรอน และคิด
ถึงรูปร่างโมเลกุลของคุณ
ในวิดีโอหน้า เราจะดูวิธี

Thai: 
คิดเมฆอิเล็กตรอน 3 ก้อนกัน
 

Korean: 
3개의 전자구름들에 대해서 접근해 보겠습니다
 

English: 
to approach three
electron clouds.

Bulgarian: 
как да подходим към три електронни облака.
