
Korean: 
VSEPR 이론을 통해 메테인의 구조를 알아볼게요.
가장 먼저 할 일은 최외각전자로 전자점식을 나타내는 것입니다.
메테인의 경우 4개의 최외각 전자를 가지고
수소는 1족이기 때문에 한 개의 최외각 전자를 갖습니다.
또한 4개의 수소원자이기 때문에 1X4이고 탄소의 전자 4개를 더하면
8개의 최외각 전자를 갖고 전자점식으로 나타냅니다.
탄소가 중심원소가 되고, 4개의 수소와 결합합니다.
4개의 수소를 이렇게 표시할게요.
그러면 가장 간단한 구조식이 되겠네요.
8개의 최외각전자가 모두 나타나겠네요.
2, 4, 6, 8 / 여덟개 입니다.
탄소는 옥텟을 만족하게 됩니다.
다음으로 할 일은 중심원자 주변의 '전자구름'을 세는 것입니다.
전자구름은 전자의 밀도를 나타내주는 것으로서
이 결합을 전자구름으로 본다면

English: 
Let's figure out the shape
of the methane molecule
using VSEPR theory.
So the first thing that you
do is draw a dot structure
to show it the
valence electrons.
So for methane, carbon
is in group four.
So 4 valence electrons.
Hydrogen is in group one, and I
have four of them, so 1 times 4
is 4, plus 4 is 8
valence electrons
that we need to show
in our dot structure.
Carbon goes in the
center and carbon
is bonded to 4 hydrogens,
so I can go ahead and put
my hydrogens in there like that.
And this is a very
simple dot structure.
We've already shown all 8
of our valence electrons.
Let me go ahead and
highlight those here.
2, 4, six, and 8.
So carbon has an
octet and we are done.
The next thing we need
to do is count the number
of electron clouds that
surround our central atom.
So remember, electron clouds
are regions of electron density,
all right?
So we can think about
these bonding electrons
here as being electron clouds.
So that's one electron cloud.

Thai: 
 
ลองหารูปร่างของโมเลกุลเมธเธน
โดยใช้ VSEPR กัน
อย่างแรกที่คุณต้องทำคือวาดโครงสร้างจุด
เพื่อแสดงวาเลนซ์อิเล็กตรอน
สำหรับเมธเธน คาร์บอนอยู่ในหมู่ 4
มีวาเลนซ์อิเล็กตรอน 4 ตัว
ไฮโดรเจนอยู่ในหมู่ 1 
และผมมีอยู่ 4 ตัว 1 คูณ 4
ได้ 4, บวก 4 เป็นวาเลนซ์อิเล็กตรอน 8 ตัว
ที่เราต้องแสดงในโครงสร้างจุด
คาร์บอนอยู่ตรงกลาง และคาร์บอน
ทำพันธะกับไฮโดรเจน 4 ตัว ผมก็ลงมือใส่
ไฮโดรเจนลงไปอย่างนั้น
และนี่คือโครงสร้างจุดที่ง่ายมาก
เราได้แสดงวาเลนซ์อิเล็กตรอน
ทั้งหมด 8 ตัวแล้ว
ขอผมลงมือเน้นพวกมันตรงนี้นะ
2, 4, 6 แล้วก็ 8
คาร์บอนมีออกเตท เราก็เสร็จแล้ว
สิ่งต่อไปที่เราต้องทำ คือนับจำนวน
เมฆอิเล็กตรอนที่ล้อมรอบอะตอมตรงกลาง
นึกดู เมฆอิเล็กตรอน 
คือเขตของความหนาแน่นอิเล็กตรอน
จริงไหม?
เราคิดถึงอิเล็กตรอนที่ทำพันธะเหล่านี้
ว่าเป็นเมฆอิเล็กตรอนได้
นั่นคือเมฆอิเล็กตรอนหนึ่งอัน

Bulgarian: 
Нека намерим формата на молекулата метан,
като използваме теорията VSERP за отблъскване на електронните двойки във валентния слой.
Първото нещо, което правиш, е да начертаеш точкова структура,
за да покажеш валентните електрони.
За метана въглеродът е в четвърта група.
4 валентни електрона.
Водородът е в първа група и имам 4 такива,
тоест 1*4 е 4, +4 е 8 валентни електрона,
които трябва да покажем в точковата си структура.
Въглеродът отива в центъра
и въглеродът е свързан с 4 водородни атома.
Тоест мога да поставя въглеродните си атоми тук, ето така.
И това е много проста точкова структура.
Вече показахме всички 8 от валентните си електрони.
Нека ги подчертая.
2, 4, 6 и 8.
Въглеродът има един октет и сме готови.
Следващото нещо, което правим,
е да преброим броя облаци, които ограждат централния атом.
Помни, електронните облаци са области електронна плътност.
Можем да помислим за тези свързващи електрони
като електронни облаци.
Това е един електронен облак.

Bulgarian: 
Това тук долу е друг.
И тук има още един.
И, после, накрая, тук има още един.
Имаме 4 електронни облаци, които ограждат централния атом.
Следващата стъпка е да прогнозираме геометрията
на електронните облаци около централния атом.
Теорията VSEPR ни казва,
че тези валентни електронни ще се отблъснат взаимно,
след като са отрицателно заредени.
И, следователно, те ще опитат да се отдалечат колкото е възможно повече един от друг.
Когато имаш 4 електронни облаци,
електронните облаци са колкото е възможно по-отдалечени един от друг,
ако сочат към, разбира се, един четиристен,
което е четиристранна фигура.
Нека начертая молекулата тук.
Да начертая молекулата метан.
Ще опитам да я покажа в четиристенна геометрия.
И ще ти покажа как изглежда един четиристен.
Това е бърза скица как изглежда молекулата.
Нека нарисувам четиристена ето тук,
за да разбереш формата му малко по-добре.
Четиристранна фигура.
Готово.
Нещо такова.

Thai: 
นี่คืออีกอันข้างล่าง
แล้วนี่คืออันหนึ่ง
แล้วสุดท้าย นี่คืออีกอัน
เรามีเมฆอิเล็กตรอน 4 ตัว
ล้อมรอบอะตอมกลางของเรา
ขั้นต่อไปคือทำนายเรขาคณิตของเมฆ
อิเล็กตรอนล้อมรอบอะตอมตรงกลาง
แล้วทฤษฎี VSEPR บอกเราว่า
วาเลนซ์อิเล็กตรอนเหล่านั้น
จะผลักกันเพราะพวกมันมีประจุ
เป็นลบ
เพราะฉะนั้น พวกมันจะพยายาม
ห่างกันให้มากที่สุดเท่าที่ทำได้ในสเปซ
และเมื่อคุณเมฆอิเล็กตรอน 4 ก้อน
เมฆอิเล็กตรอนห่างกันมากที่สุด
ถ้าพวกมันชี้หามุมของ tetrahedron
ซึ่งก็คือรูปสี่หน้า
ขอผมลงมือวาดโมเลกุลตรงนี้
วาดโมเลกุลเมธเธน
ผมจะพยายามแสดงมันเป็นรูปทรงสี่หน้า
ผมจะแสดงให้คุณดูว่า
ทรงสี่หน้าเป็นอย่างไร
นี่คือภาพร่างโมเลกุลว่ามันมีหน้าตาอย่างไร
 
ขอผมลงมือวาดทรงสี่หน้า
ตรงนี้ คุณจะได้เข้าใจรูปร่างมากขึ้น
ดีไหม?
ทรงสี่หน้า
ได้แล้ว
ประมาณนั้น

Korean: 
이 밑에도 있고, 여기도 있고, 저기도 있습니다.
그러면 4개의 전자구름을 갖습니다.
중심원소 주위에 4개의 전자구름을 갖는다고 할 수 있습니다.
다음은 중심원소 주변 전자구름의 기하구조를 예측하는 것입니다.
VSEPR 이론에 따르면 최외각전자는 (-)로 대전되어 서로 반발하므로
최대한 공간상에서 서로 멀어지려고 합니다.
4개의 전자구름이 있다면 정사면체의 꼭지점으로 배열될 것 입니다.
분자를 하나 그려보겠습니다.
정사면체를 그려보면 이렇게 생겼을 것입니다.
빠르게 그리면 이렇게 그릴 수 있겠습니다.
이해를 돕기위해 정사면체를 그려보면
네개의 면이 존재하고, 이렇게 생겼습니다.

English: 
Here's another one down here.
And then here's one.
And then finally,
here's another one.
So we have four electron clouds
surrounding our central atom.
The next step is to predict
the geometry of your electron
clouds around your central atom.
And so VSEPR theory tells us
that those valence electrons
are going to repel each other
since they are negatively
charged.
And therefore,
they're going to try
to get as far away from each
other as they can in space.
And when you have
four electron clouds,
the electron clouds are
farthest away from each other
if they point towards the
course of a tetrahedron, which
is a four sided figure.
So let me go ahead and
draw the molecule here,
draw the methane molecule.
I'm going to attempt to show
it in a tetrahedral geometry.
And then I'll
actually show you what
a tetrahedron looks like here.
So here's a quick sketch of
what the molecule sort of looks
like.
And let me go ahead and
draw tetrahedron over
here so you can get a little
bit better idea of the shape,
all right?
So four sided figure.
And so there you go.
Something like that.

English: 
So you could think about the
corners of your tetrahedron
as being approximately
where your hydrogens are
and that just gives you a
little bit better visual picture
of that tetrahedron, that
four sided figure here.
And so we've created the
geometry of the electron clouds
around our central atom.
And in step four, we
ignore any lone pairs
around our central atom,
which we have none this time.
And so therefore, the
geometry the molecule
is the same as the geometry
of our electron pairs.
So we can say that methane is a
tetrahedral molecule like that.
All right, in terms
of bond angles.
So our goal now is to figure
out what the bond angles are
in a tetrahedral molecule.
Turns out to be 109.5
degrees in space.
So that's having those
bonding electrons
as far away from each
other as they possibly
can using VSEPR theory.
So 109.5 degrees turns
out to be the ideal bond
angle for a
tetrahedral molecule.
Let's go ahead and
do another one.

Thai: 
คุณคิดถึงมุมของทรงสี่หน้า
ว่าเป็นตำแหน่งของไฮโดรเจน
และมันให้ภาพทรงสี่หน้า
ชัดขึ้น รูปสี่หน้าตรงนี้
และเราได้สร้างเรขาคณิตของเมฆอิเล็กตรอน
รอบอะตอมศูนย์กลางได้แล้ว
ในขั้นที่ 4 เราไม่สนใจคู่โดดเดี่ยว
รอบอะตอมตรงกลาง ซึ่งเราไม่มีในที่นี้
เพราะฉะนั้น เรขาคณิตของโมเลกุล
ก็คือเรขาคณิตของคู่อิเล็กตรอน
เราจึงบอกได้ว่า เมธเธนคือ
โมเลกุลทรงสี่่หน้าอย่างนั้น
เอาล่ะ ในแง่ของมุมพันธะ
เป้าหมายของเราตอนนี้คือหาว่ามุมพันธะ
ในโมเลกุลทรงสี่หน้าเป็นเท่าใด
ปรากฎว่ามันเท่ากับ 109.5 องศา
นั่นคือการให้อิเล็กตรอนที่ทำพันธะ
ห่างกันที่สุดเท่าที่จะเป็นได้
โดยใช้ทฤษฎี VSEPR
109.5 องศาปรากฏว่าเป็นมุมพันธะในอุดมคติ
สำหรับโมเลกุลทรงสี่หน้า
ลองลงมือทำอีกข้อกัน

Bulgarian: 
И можеш да помислиш за ъглите на четиристена
като приблизително местата, където се намират водородните атоми,
а това ти дава малко по-добра нагледна картина
за този четиристен, тази четиристранна фигура.
И създадохме геометрията на електронните облаци около централния атом.
В стъпка 4 игнорираме всички свободни двойки около централния атом,
като тук нямаме николко такива.
И следователно геометрията на молекулата
е същата като геометрията на електронните двойки.
Можем да кажем, че метанът е четиристенна молекула.
А що се отнася до ъгли на връзката...
Целта ни е да намерим какви са ъглите на връзката
в една четиристенна молекула.
Оказва се, че са 109,5 градуса в пространството.
Така тези свързващи електрони са колкото е възможно по-отдалечени един от друг,
чрез използване на теорията за отблъскване на електронните двойки.
109,5 градуса е идеалният ъгъл на връзката за една четиристенна молекула.
Нека направим друг пример.

Korean: 
정사면체의 꼭지점을 보면, 수소가 위치하게 됩니다.
그러면 전자구름의 기하적인 구조를 예측하고
네번째로는 비공유 전자쌍은 기하구조에서 무시하게 됩니다.
비공유 전자쌍이 없다면 그대로 일 것입니다.
메테인의 경우는 정사면체 구조를 갖습니다.
그러면 이제 사면체의 결합각을 알아보겠습니다.
109.5도 정도가 됩니다.
VSEPR 이론에 따라 각각의 결합이 최대한 멀어지려고 하면
109.5도 가 정사면체 구조에서 가장 이상적인 결합각이라고 할 수 있습니다.
다른 구조를 봐봅시다.

Bulgarian: 
Нека разгледаме амоняка.
Имаме NH3.
Първо трябва да начертаем точковата структура.
Започваме като откриваме валентните електрони.
Азотът е в пета група.
5 валентни електрона.
Водородът е в първа група и имам три такива.
1*3 + 5 е 8.
Отново, имаме 8 валентни електрона, за които трябва да помислим.
Поставяме азота в центъра и знаем,
че азотът е свързан с 3 водородни атома,
поставяме трите водородни атома тук, ето така.
Да видим колко валентни електрона сме използвали дотук.
2, 4 и 6.
8 - 6 е 2 останали валентни електрона.
Не можем да ги поставим към крайните атоми,
понеже водородните атоми вече са оградени от 2 електрона.
Поставяме тези два валентни електрона към централния атом,
който е азот, ето така.
И сега представихме тези два валентни електрона.
В точковата си структура показахме всички 8 валентни електрона.
Връщаме се обратно към стъпките си,
за да си припомним какво правим, след като сме начертали точковата си структура.

English: 
Let's look at ammonia.
So we have NH3.
First thing we need to do
is draw the dot structure.
So we start by finding our
valence electrons, nitrogen
in group five.
So 5 valence electrons.
Hydrogen in group one,
and I have three of them.
So 1 times 3 plus 5 is 8.
So once again, we have 8 valence
electrons to worry about.
We put nitrogen in
the center and we
know nitrogen has
bonded to 3 hydrogens,
so we go ahead and put our 3
hydrogens in there like that.
Let's see how many valence
electrons we've used up so far.
2, 4, and 6.
So 8 minus 6 is 2
valence electrons left.
We can't put them on
our terminal atoms,
because the
hydrogens are already
surrounded by two electrons.
So we go ahead and put
those two valence electrons
on our central atom, which
is our nitrogen like that.
And so now we've gone ahead and
represented those two valence
electrons.
So we have all eight
valence electrons
shown for our dot structure.
All right, we go back
up here to our steps
to remind us what to do after
we've drawn our dot structure.

Korean: 
암모니아를 봐보면,
NH3 입니다.
전자점식을 그려보면, 최외각전자수 부터 봐보죠.
질소는 15족이므로 5개를 갖고,
수소는 1족이므로 1개이고 3개의 원자가 있으므로
1X3=3개 입니다. 다 더하면 8개의 전자를 갖습니다.
8개의 전자를 고려해야 합니다 .
질소를 중심에 두고 세개의 수소와 결합하고 있습니다.
수소를 하나씩 그려주게 되고,
지금까지 몇개의 전자를 썼는지 보면, 2,4,6 / 6개의 전자를 사용했씁니다.
8-6=2 / 두개의 전자가 남았습니다.
이 전자를 말단 원자에 줄순 없습니다.
수소는 이미 두개의 전자가 있기 때문이죠.
그러면 중심원소에 전자 2개를 주겠습니다 .
이제 8개 전자 모두 배열 했습니다.
두번째 단계로 넘어가면,

Thai: 
ลองดูแอมโมเนีย
เรามี NH3
อย่างแรกที่เราต้องทำ คือวาดโครงสร้างจุด
เราเริ่มโดยหาวาเลนซ์อิเล็กตรอน ไนโตรเจน
ในหมู่ 5
วาเลนซ์อิเล็กตรอน 5 ตัว
ไฮโดรเจนในหมู่ 1 และผมมีอยู่ 3 ตัว
1 คูณ 3 บวก 5 ได้ 8
เหมือนเดิม เรามีวาเลนซ์อิเล็กตรอน 8 ตัวให้คิด
เราใส่ไนโตรเจนไว้ตรงกลาง และเรา
รู้ว่าไนโตรเจนทำพันธะกับไฮโดรเจน 3 ตัว
เราก็ลงมือใส่ไฮโดรเจน 3 ตัวลงไปอย่างนั้น
ลองดูว่าเราใช้วาเลนซ์อิเล็กตรอนไปแล้วกี่ตัว
2, 4 และ 6
8 ลบ 6 เหลือวาเลนซ์อิเล็กตรอน 2 ตัว
เราใส่พวกมันในอะตอมปลายไม่ได้
เพราะไฮโดรเจน
ล้อมรอบด้วยอิเล็กตรอน 2 ตัวแล้ว
เราจึงลงมือใส่วาเลนซ์อิเล็กตรอน 2 ตัวนั้น
ลงในอะตอมกลางของเรา 
ซึ่งก็คือไนโตรเจนอย่างนั้น
และตอนนี้ เราก็ลงมือแสดงวาเลนซ์อิเล็กตรอน
2 ตัวได้
เราจึงมีวาเลนซ์อิเล็กตรอน 8 ตัว
แสดงในโครงสร้างจุดของเราแล้ว
เอาล่ะ เรากลับขึ้นไปดูขั้นตอน
ทบทวนสิ่งที่ต้องทำ
หลังจากวาดโครงสร้างจุดแล้ว

Thai: 
เราเห็นได้ว่า ตอนนี้เราจะ
คิดถึงเมฆอิเล็กตรอน
ที่ล้อมรอบอะตอมกลาง
เขตของความหนาแน่นอิเล็กตรอน
ลองลงมือหากัน
ผมเห็นได้ว่า ผมมีอิเล็กตรอนที่ทำพันธะเหล่านี้
นั่นคือเขตของความหนาแน่นอิเล็กตรอน
นั่นคือเมฆอิเล็กตรอน
นี่คืออีกก้อน
นั่นคือ 2
นี่คืออีกก้อน
นั่นคือ 3
และอิเล็กตรอนคู่โดดเดี่ยวนี้ อิเล็กตรอนคู่ที่
ไม่ได้ทำพันธะจะนับเป็นเมฆอิเล็กตรอนเช่นกัน
มันคือเขตของความหนาแน่นอิเล็กตรอนเช่นกัน
เหมือนเดิม เรามีเขต
ความหนาแน่นอิเล็กตรอน 4 เขต
เมื่อคุณคิดถึงเรขาคณิตของ
เมฆอิเล็กตรอนเหล่านั้น
เมฆอิเล็กตรอน 4 ตัวนั้น
จะ เหมือนเดิม พยายามชี้
ไปยังมุมของทรงสี่หน้า
เราก็วาดโมเลกุลแอมโมเนียได้
และเราวาดฐานแบบเดียวกับที่ทำตอนหน้าได้
โดยมีไฮโดรเจน 3 ตัวตรงนี้
แล้วเราจะลงมือใส่
อิเล็กตรอนคู่โดดเดี่ยวตรงนี้

Bulgarian: 
И можем да видим,
че сега ще помислим за електронните облаци,
които ограждат централния атом.
Области електронна плътност.
И нека ги намерим.
Мога да видя, че имам тези свързващи електрони.
Това е една област на електронна плътност,
така че това е един електронен облак.
Тук има още един.
Това са два.
Тук е още един.
Това са три.
И тази свободна двойка електрони, тази несвързваща двойка електрони,
също ще е преброена като електронен облак.
Тя също е една област електронна плътност.
И отново имаме 4 области електронна плътност.
Когато мислиш за геометрията на тези електрони облаци,
тези четири електронни облака,
отново, те ще опитат да сочат към ъглите на един четиристен.
Можем да скицираме молекулата амоняк.
И можем да начертаем основата така, както направихме преди,
като имаме три водородни атома ето тук.
И после ще поставим една свободна двойка електрони ето тук.

Korean: 
이제 중심원소 주변의 전자구름을 고려해야 합니다.
이 결합한 전자들은 하나의 전자구름을 형성하고
여기도 하나가 있고, 하나가 더있습니다. 총 3개가 존재합니다.
그리고 비공유 전자쌍 또한 하나의 전자구름이라고 세야합니다.
전자밀도가 높은 영역이기 때문이죠.
그러면 4개의 전자밀도가 높은 영역이 존재합니다.
기하구조를 본다면 4개가 다시 정사면체의 꼭지점을 향하면 됩니다.
암모니아 분자를 그려본다면,
세개의 수소를 먼저그리고,

English: 
And we can see that
now we're going
to think about the
electron clouds that
surrounded the central atom.
So regions of electron density.
And let's go ahead
and find those.
So I can see that I have
these bonding electrons.
That's a region of
electron density,
so that's an electron cloud.
Here's another one.
So that's two.
Here's another one.
So that's three.
And this lone pair of
electrons, this non-bonding pair
of electrons is also going to
be counted as an electron cloud.
It's a region of
electron density too.
And so once again we have four
regions of electron density.
When you're thinking about
the geometry of those electron
clouds, those four
electron clouds
are going to, once
again, try to point
towards the corners
of a tetrahedron.
So we can kind of sketch
out the ammonia molecule.
And we can draw the base
the same way we did before,
with our three
hydrogens right here.
And then we're going
to go ahead and put
our lone pair of
electrons right up here.

English: 
And so again, it's an attempt
to show the electron clouds
in a tetrahedral geometry.
Let's go back up here and
look at our steps again.
So in step three, we predicted
the geometry electron clouds
are going to attempt to
be in a tetrahedron shape
around our central atom.
But when we're actually talking
about the geometry or shape
of the molecule, we're going
to ignore any lone pairs when
we predict the geometry
of the molecule.
So when we look at
the ammonia molecule,
we're going to ignore that
lone pair of electrons
on top of the nitrogen
and we're just
going to focus in on the
bottom part for the shape here.
And so when we do
that, we get something
that looks like a little
squat pyramid here.
So if I'm [? ignoring ?]
that lone pair of electrons
up there at the top, it's
going to look something
like that for the shape.
And we call this
trigonal pyramidal.
So this is a trigonal
pyramidal shape.

Thai: 
เหมือนเดิม ผมพยายามแสดงเมฆอิเล็กตรอน
ในรูปทรงสี่หน้า
ลองกลับขึ้นมาตรงนี้ ดูขั้นตอนของเราอีกครั้ง
ในขั้นที่ 3 เราทำนายรูปร่างของเมฆอิเล็กตรอน
ว่าจะพยายามเป็นรูปทรงสี่หน้า
รอบอะตอมศูนย์กลาง
แต่เมื่อเราคิดถึงเรขาคณิตหรือรูปทรง
ของโมเลกุลจริงๆ 
เราจะไม่สนใจคู่โดดเดี่ยวเมื่อ
เราทำนายเรขาคณิตของโมเลกุล
เมื่อเราดูโมเลกุลแอมโมเนีย
เราจะไม่สนใจอิเล็กตรอนคู่โดดเดี่ยว
ของไนโตรเจนข้างบน และเรา
จะสนใจแต่รูปส่วนล่างตรงนี้
แล้วเมื่อเราทำอย่างนั้น เราจะได้
สิ่งที่เป็นเหมือนพีระมิดเล็กๆ
ถ้าผมไม่สนใจอิเล็กตรอนคู่โดดเดี่ยว
ข้างบน มันจะมีรูปร่าง
เป็นแบบนี้
และเราเรียกรูปนี้ว่า trigonal pyramidal
นี่คือรูปทรงพีระมิดสามเหลี่ยม

Bulgarian: 
И, отново, това е опит да покажем електронните облаци в четиристенна геометрия.
Нека се върнем тук горе и отново да погледнем стъпките си.
В стъпка 3 прогнозирахме геометрията на електронните облаци
като четиристенна форма около централния атом.
Но когато говорим за геометрията, или формата, на молекулата,
ще игнорираме всички свободни двойки,
когато прогнозираме геометрията на молекулата.
Когато погледнем молекулата на амоняка,
ще игнорираме тази свободна двойка електрони,
която е отгоре на азота
и просто ще се фокусираме върху долната част за тази форма.
И когато направим това, получаваме нещо,
което изглежда като пирамида.
Ако ще игнорирам тази свободна двойка електрони тук горе,
това ще изглежда с подобна форма.
Наричаме това тристенна пирамидална форма.
Това е тристенна пирамидална форма.

Korean: 
비공유전자쌍을 여기에 그릴게요.
그러면 정사면체 구조가 나타납니다.
다시 3번째 단계를 확인해보면, 정사면체 구조라고 예측이 됩니다.
분자의 기하구조를 이야기 한다면, 비공유전자쌍을 무시해야합니다.
암모니아 분자를 보면, 질소위에 있는 비공유전자쌍을 무시해야합니다.
그 아래부분에 초점을 맞추는 것이지요.
그러면 피라미드 형태를 띠게 됩니다.
이 구조를 삼각뿔이라고 부릅니다.
이 구조는 삼각뿔(Trigonal Pyramid)형 이라고 부릅니다.

Bulgarian: 
Въпреки че електронните облаци опитват да са в четиристенен модел,
формата е по-скоро тристенно пирамидална,
понеже игнорираме всички свободни двойки електрони.
Що се отнася до ъгъл на връзката,
тази свободна двойка електрони на азота заема повече пространство.
Тези несвързващи електрони заемат малко повече място,
отколкото свързващите електрони.
И поради това, тези несвързващи електрони
ще отблъснат тези свързващи електрони.
Ще ги поставя в синьо тук, просто като пример.
Отблъскват тези малко повече,
отколкото предишния пример, който видяхме.
И това ще направи ъгъла на връзката малко по-малък
от идеалния свързващ ъгъл, който видяхме, 109,5 за четиристенно подреждане
на електронните облаци.
И се оказва, че този ъгъл на връзката между атомите,
ъгълът на връзката водород-азот-водород,
става малко по-малък от 109,5.
Всъщност става по-малък до приблизително 107 градуса

English: 
So even though the
electron clouds
are attempting to be in
a tetrahedron fashion,
the shape is more
trigonal pyramidal
because we ignore any
lone pairs of electrons.
In terms of a bond
angle, this lone pair
of electrons on the nitrogen
actually occupies more space.
These non-bonding electrons
occupy a little more space
than bonding electrons.
And because of that, those
non-bonding electrons
are going to repel
these bonding electrons.
I'm going to go
ahead and put them
in blue here just as an example.
Repel these a little bit more
than in the previous example
that we saw.
And that's actually
going to make the bond
angle a little bit smaller
than the ideal bonding angle
we saw before for 109.5 for
a tetrahedral arrangement
of electron clouds.
And so it turns out that this
bond angle between the atoms,
the hydrogen nitrogen
hydrogen bond angle
gets a little bit
smaller than 109.5.
So it actually gets smaller
to approximately 107 degrees

Thai: 
ถึงแม้ว่าเมฆอิเล็กตรอน
พยายามทำตัวเป็นทรงสี่หน้า
รูปร่างโมเลกุลจะเป็น
พีระมิดสามเหลี่ยมมากกว่า
เพราะเราไม่สนใจอิเล็กตรอนคู่โดดเดี่ยว
ในแง่ของมุมพันธะ คู่โดดเดี่ยวนี้
บนไนโตรเจนจะกินพื้นที่มากกว่า
อิเล็กตรอนที่ไม่ทำพันธะกินพื้นที่มากกว่า
อิเล็กตรอนที่ทำพันธะเล็กน้อย
ด้วยเหตุนั้น อิเล็กตรอนที่ไม่ทำพันธะเหล่านั้น
จะผลักอิเล็กตรอนที่ทำพันธะเหล่านี้
ผมจะลงมือเขียนพวกมัน
ด้วยสีฟ้าเป็นตัวอย่าง
ผลักพวกนี้มากกว่าตัวอย่างก่อน
ที่เราเห็นหน่อย
และมันจะทำให้มุมพันธะ
น้อยกว่ามุมพันธะในอุดมคติ
ที่เราเห็นก่อนหน้านี้ 109.5 
สำหรับเมฆอิเล็กตรอน
รูปทรงสี่หน้า
และปรากฏว่ามุมพันธะระหว่างอะตอมนี้
มุมพันธะไฮโดรเจน-ไนโตรเจน-ไฮโดรเจน
จะน้อยกว่า 109.5 เล็กน้อย
มันจะน้อยลง กลายเป็นประมาณ 107 องศา

Korean: 
비록 정사면체와 비슷한 모양이지만,
비공유전자쌍을 무시하게되면 삼각뿔형이 됩니다.
결합각은 질소의 비공유전자쌍이 공간을 더 차지하게 됩니다.
공유전자쌍보다 비공유전자쌍이 더 많이 차지하기 때문에
비공유전자쌍은 공유전자쌍과 더 많이 반발하게 됩니다.
이게 결합각을 조금더 작게 만드는 요인입니다.
정사면체의 109.5도인 이상적인 각도에서 멀어지게 하는 것이지요.
그러면 수소-질소-수소 간의 각도는 109.5도보다 살짝 작은 값을 갖습니다.

English: 
here for a trigonal
pyramidal situation.
All right, let's do one more.
Let's go ahead and do
the water molecule.
All right, so we have H2O.
And to follow our steps, we know
that hydrogen's in group one.
I have two of them.
And we know that
oxygen is in group six.
So 6 plus 2 is once
again 8 valence electrons
to represent for
our dot structure.
And we put oxygen in the center.
Oxygen is bonded
to two hydrogens,
so we go ahead and
draw those in there.
And let's see, how many
valence electrons have
we represented so far?
That's 2, that's 4.
So 8 minus 4 is 4
valence electrons left.
We first think about putting
them on our terminal atoms,
but those are our hydrogens,
so they're already
happy with two electrons.
So we go ahead and put
those four valence electrons
on our central atom,
which is our oxygen.
And four valence electrons means
two lone pairs of electrons
now.
And so now we've represented
all eight valence electrons
for water.

Korean: 
실제로 삼각뿔의 경우 약 107도의 각도를 갖습니다.
하나 더 해봅시다.
물분자 입니다. H2O겠지요.
수소는 1족이고 두개입니다.
산소는 16족이고 6+2=8
또 8개의 전자를 갖습니다.
산소를 중심에 두고 두개의 수소와 결합합니다.
이렇게 그릴 수 있고,
두개 결합이니까 4개의 전자를 썼고,
8-4=4 / 네개의 전자가 남습니다.
수소에 주려고 했지만, 수소는 이미 두개의 전자로 만족해있습니다.
그러면 4개의 전자를 중심원소인 산소에게 줍니다.
4개의 전자는 2개의 비공유전자쌍이 되겠지요.
그러면 8개의 전자를 모두 나타냈습니다.

Bulgarian: 
за тристенно пирамидална ситуация.
Нека направим още един пример.
Нека се заемем с една молекула вода.
Имаме Н2О.
И, за да следваме стъпките си, знаем, че водородът е в първа група.
Имам два такива.
И знаем, че кислородът е в шеста група.
6 + 2 е, отново, 8 валентни електрона,
които трябва да представим в тази точкова структура.
И поставяме кислородния атом в центъра.
Кислородният атом е свързан с два водородни атома,
така че ги чертаем тук.
И, да видим, колко валентни електрона сме представили дотук?
Това са 2, това са 4.
8 - 4 са 4 останали валентни електрона.
Първо мислим да ги поставим върху крайните атоми,
но това са водородните атоми,
които вече са доволни с два електрона.
Така че поставяме тези четири валентни електрона
върху централния атом, който е кислород.
И четири валентни електрона означава две свободни двойки електрони.
И представихме всички 8 валентни електрона за водата.

Thai: 
ตรงนี้ในกรณีของพีระมิดสามเหลี่ยม
เอาล่ะ ลองทำอีกอันหนึ่ง
ลองลงมือดูโมเลกุลน้ำกัน
เอาล่ะ เรามี H2O
ทำตามขั้นตอน เรารู้ว่าไฮโดรเจนอยู่ในหมู่ 1
ผมมี 2 ตัว
และเรารู้ว่าออกซิเจนอยู่ในหมู่ 6
6 บวก 2 ได้วาเลนซ์อิเล็กตรอน 
8 ตัวเหมือนเดิม
เพื่อแสดงโครงสร้างจุด
และเราใส่ออกซิเจนไว้ตรงกลาง
ออกซิเจนทำพันธะกับไฮโดรเจน 2 ตัว
เราก็ลงมือวาดพวกมันลงไปได้
ลองดู เราแสดงวาเลนซ์อิเล็กตรอน
ไปแล้วกี่ตัว?
นั่นคือ 2 นั่นคือ 4
8 ลบ 4 จึงเหลือวาเลนซ์อิเล็กตรอน 4 ตัว
ก่อนอื่น เราใส่พวกมันในอะตอมตรงกลาง
แต่พวกมันคือไฮโดรเจน พวกมันจึง
มีความสุขกับอิเล็กตรอน 2 ตัวแล้ว
เราจึงใส่วาเลนซ์อิเล็กตรอน 4 ตัวนั้น
ลงในอะตอมตรงกลาง ซึ่งก็คือออกซิเจน
และวาเลนซ์อิเล็กตรอน 4 ตัวหมายถึง
อิเล็กตรอนคู่โดดเดี่ยว 2 คู่
 
ตอนนี้เราได้แสดงวาเลนซ์อิเล็กตรอน 8 ตัว
สำหรับน้ำแล้ว

Bulgarian: 
Следващата ни стъпка е, разбира се, да преброим колко електронни облака има
около централния атом.
Отново, можем да помислим за тези свързващи електрони
като за един електронен облак.
Тези свързващи електрони са електронен облак,
тези несвързващи електрони, като свободни двойки в един електронен облак
и същото нещо важи за тези несвързващи електрони,
електронен облак и тук.
И отново имаме 4 електронни облака.
И тези четири електронни облака
ще опитат да са в четиристенно подреждане около централния атом.
Като използваме теорията VSEPR, знаем, че ще се отблъснат взаимно
и ще се отдалечат колкото е възможно повече един от друг.
Нека начертая молекулата отново.
Нека продължим.
Имаме нашата молекула вода
и имаме свободните двойки електрони.
И в този случай имаме две свободни двойки електрони.
Помни, свободните двойки или несвързващите електрони
ще заемат малко повече пространство от свързващите електрони.

Thai: 
ขั้นต่อไปคือ แน่นอน นับว่าเรามีเมฆอิเล็กตรอน
รอบล้อมอะตอมกลางกี่ก้อน
เหมือนเดิม เราคิดถึง
อิเล็กตรอนที่ทำพันธะเหล่านี้
เป็นเมฆอิเล็กตรอนหนึ่งก้อน
พันธะที่ทำพันธะเหล่านี้เป็นเมฆอิเล็กตรอน
อิเล็กตรอนที่ไม่ทำพันธะเหล่านี้ เป็น
อิเล็กตรอนคู่โดดเดี่ยว
เช่นเดียวกับอิเล็กตรอนที่ไม่ทำพันธะเหล่านี้
เป็นเมฆอิเล็กตรอนตรงนี้เช่นกัน
เหมือนเดิม เรามีเมฆอิเล็กตรอน 4 ก้อน
และเมฆอิเล็กตรอน 4 ก้อนนั้น
พยายามเรียงตัวเป็นทรงสี่หน้า
รอบอะตอมศูนย์กลาง
เมื่อใช้ทฤษฎี VSEPR พวกมันจะผลักกัน
และห่างกันที่สุดเท่าที่ทำได้
 
ขอผมวาดโมเลกุลใหม่ตรงนี้นะ
ลองลงมือ
เรามีโมเลกุลน้ำ และเรา
มีอิเล็กตรอนคู่โดดเดี่ยวอย่างนั้น
ในกรณีนี้ เรามีอิเล็กตรอนคู่โดดเดี่ยว 2 คู่
นึกดู คู่โดดเดี่ยว หรืออิเล็กตรอนที่ไม่ทำพันธะ
จะใช้พื้นที่มากกว่า
อิเล็กตรอนที่ทำพันธะเล็กน้อย
เพราะฉะนั้น พวกมันจะผลักอิเล็กตรอนเหล่านี้

English: 
Our next step is, of course, to
count how many electron clouds
we have around our central atom.
So once again, we could think
about these bonding electrons
as being an electron cloud.
These bonding electrons
as being electron cloud,
these non-bonding electrons
as lone pairs in an electron
cloud, and same thing for
these non-bonding electrons,
electron cloud
over there as well.
And so once again we have
four electron clouds.
And those four
electron clouds are
going to attempt to be in
a tetrahedral arrangement
around that central atom.
Using VSEPR theory, they're
going to repel each other
and get as far away from each
other as they possibly can.
Let me go and redraw
the molecule here.
So let's go ahead.
And we have our
water molecule and we
have our lone pairs of
electrons like that.
And in this case we have
two lone pairs of electrons.
Remember, lone pairs or
non-bonding electrons take up
a little bit more space
than bonding electrons.
And therefore, they're going
to repel these electrons right

Korean: 
다음 단계는 전자구름을 세는 것인데요.
다시, 결합이 하나의 전자구름이고, 여기도 마찬가지이고,
이 비공유전자쌍들도 마찬가지로 전자구름으로 셉니다.
4개의 전자구름이 있게 되고, 정사면체라는 것을 알 수 있습니다.
산소를 중심으로 하여 VSEPR 이론에 따르면
반발하여 최대한 멀어지려는 구조를 갖게되고,
그러나 이 경우에는
다시 물분자를 그려보면,
비공유전자쌍들이 존재합니다.
두개의 비공유전자쌍이 존재합니다.
비공유전자쌍은 공간을 조금더 차지한다는 것을 기억하세요.

Korean: 
그러므로 여기 공유전자쌍과 반발이 더 존재하겠지요.
그러면 전보다 결합각이 줄어들게 됩니다.
107도 보다도 줄어들게 됩니다.
이 각도는 약 104.5도를 이루고 있습니다.
이 전자구름의 기하구조는 정사면체를 이루지만,
분자의 기하구조는 다릅니다.
분자구조는 비공유전자쌍을 무시하기 때문이죠.
그래서 모양을 살펴보면, 이렇게 생겼습니다.
이 구조는 전에 한번 본구조 입니다.
굽은형이라고 합니다 .
그러므로 물분자의 기하구조는 굽은형이라고 합니다.
약 104.5도의 결합각을 이루고 있습니다.
이 예시들로 4개의 전자구름을 가질때

English: 
in here a little bit more.
And that's going to make
our bond angle even smaller
than before.
So it's going to be even
smaller than 107 degrees.
And so this bond
angle right here,
you'll see it listed as
approximately 104.5 degrees,
or some textbooks
will say 105 degrees.
So that's approximately
what it is for this.
In terms of the geometry
of the molecule.
So the geometry of the electron
clouds are attempting to be,
once again, a
tetrahedral fashion,
but the geometry of the
molecule is different
because you ignore lone
pairs of electrons.
And so when you
look at the shape,
if you look at the
shape of this--
I'll go ahead and draw
the shape over here.
If you're ignoring lone pairs of
electrons, it looks like that.
And we've seen
that shape before.
That's bent or angular.
So we say that the geometry
of the water molecule
is bent or angular with an
approximately 104.5 degree
bond angle.
So those are a couple examples
of four electron clouds

Bulgarian: 
И следователно ще отблъснат тези електрони ето тук малко повече.
И това ще направи ъгъла на връзката още по-малък,
отколкото преди.
Тоест той ще е дори по-малък от 107 градуса.
И този ъгъл на връзката тук...
ще го видиш записан като приблизително 104,5 градуса,
или някои учебници ще го дават 105 градуса.
Това са приблизителните градуси.
Що се отнася до геометрията на молекулата...
Геометрията на електронните облаци се е, отново, четиристенна,
но геометрията на молекулата е различна,
понеже игнорираш свободните двойки електрони.
И когато погледнеш формата,
ако гледаш формата на това –
ще начертая формата ето тук.
Ако игнорираш свободните двойки електрони, тя изглежда ето така.
И сме виждали тази форма преди.
Това е извита или ъглова.
Казваме, че геометрията на молекулата на водата
е извита или ъглова с приблизително 104,5-градусов ъгъл на връзката.
Това са няколко примера за четири електронни облака
и как да намерим геометрията,

Thai: 
มากกว่าเล็กน้อย
และมันจะทำให้มุมพันธะ
เล็กลงเล็กน้อย
มันจะน้อยกว่า 107 องศาอีก
มุมพันธะนี่ตรงนี้
คุณจะเห็นคนเขียนว่าประมาณ 104.5 องศา
หรือหนังสือบางเล่มจะบอกว่า 105 องศา
นั่นคือค่าประมาณของมุมนี้
ในแง่ของเรขาคณิตของโมเลกุล
เรขาคณิตของเมฆอิเล็กตรอนพยายามจะ
เหมือนเดิม เป็นทรงสี่หน้า
แต่เรขาคณิตของโมเลกุลนี้ต่างออกไป
เพราะคุณจะไม่คิดอิเล็กตรอนคู่โดดเดี่ยว
เมื่อคุณดูรูปร่างนี้
ถ้าคุณดูรูปนี้ --
ผมจะวาดรูปทรงตรงนี้
ถ้าคุณไม่คิดอิเล็กตรอนคู่โดดเดี่ยว 
มันจะเป็นอย่างนั้น
เราเห็นรูปนั้นมาก่อน
มันจะรูปงอ หรือมุม
เราบอกได้ว่าเรขาคณิตของโมเลกุลน้ำ
เป็นรูปงอ หรือมุม ซึ่งประมาณได้เป็นมุมพันธะ
104.5 องศา
นั่นคือตัวอย่างเมฆอิเล็กตรอน 4 ก้อน

Bulgarian: 
докато същевременно мислим за ъглите на връзката.

Thai: 
วิธีหาเรขาคณิต
รวมทั้งคิดมุมพันธะด้วย

Korean: 
기하구조를 예측할 수 있었습니다.
그리고 결합각도 생각해보았습니다.

English: 
and how to figure out
the geometry while also
thinking about the bond angles.
