
Bulgarian: 
В това видео ще приложим теорията за отблъскване на електронните двойки във валентния слой (VSEPR)
към 6 електронни облака.
Ако целта ни е да намерим формата на молекулата на серния хексафлуорид,
отново започваме с точковата структура.
Сярата е в група 6 на периодичната таблица,
тоест 6 валентни електрона.
Флуорът е в седма група, седем валентни електрона,
но имам 6 такива.
7 по 6 ми дава 42
и 42 плюс 6 ми дава 48 валентни електрона,
които трябва да покажем в точковата си структура.
Сярата отива в центъра, поставяме сярата тук.
И ограждаме сярата с 6 флуорни атома.
Нека поставя тези 6 флуорни атома,
които ограждат нашата сяра.
Следващата стъпка е да видим колко валентни електрона
сме показали дотук.
Ще ги подчертая – 2, 4, 6, 8, 10 и 12.
48 минус 12 ми дава 36 останали валентни електрони,

English: 
In this video, we're going
to apply VSEPR theory
to 6 electron clouds.
So if our goal is to find
the shape of the sulfur
hexafluoride
molecule, once again
we start with our dot structure.
So sulfur is in group 6
on the periodic table,
so 6 valence electrons.
Fluorine is in group 7,
so 7 valence electrons,
but I have 6 of them.
So 7 times 6 gives
me 42, and 42 plus 6
gives me 48 valence
electrons that we
need to show in
our dot structure.
Sulfur goes in the center, so we
go ahead and put sulfur there.
And we surround sulfur
with 6 fluorines.
So let me go ahead and put in
those 6 fluorines surrounding
our sulfur.
Our next step is to
see how many valence
electrons that
we've shown so far.
So I go and highlight those--
2, 4, 6, 8, 10, and 12.
So 48 minus 12 gives me 36
valence electrons left over,

Korean: 
 
6개의 전자구름을 가진 분자에 
VSEPR 이론을 적용해보려고 합니다
6개의 전자구름을 가진 분자에 
VSEPR 이론을 적용해보려고 합니다
만약 목표가 육플루오린화황 분자의
모양을 알아내는 것이라면
만약 목표가 육플루오린화황 분자의
모양을 알아내는 것이라면
루이스 전자점식에서 시작해야 합니다
황은 주기율표 상에서 16족에 있고
6개의 원자가 전자가 있습니다
황은 주기율표 상에서 16족에 있고
6개의 원자가 전자가 있습니다
플루오린은 17족이고
7개의 원자가 전자가 있지만
그 중 6개가 있습니다
7 X 6 = 42 이고 42 +6 = 48
루이스 전자점식에 나타내야 하는
원자가 48개입니다
루이스 전자점식에 나타내야 하는
원자가 48개입니다
황은 가운데로 들어가므로 먼저 황을 넣습니다
6개의 플루오린으로 황을 둘러쌉니다
황 주변에 6개의 플루오린을 넣습니다
황 주변에 6개의 플루오린을 넣습니다
다음 단계는 지금까지 원자가 전자를
몇 개 나타냈는지 살펴보는 것입니다
전자를 색칠하겠습니다
2, 4, 6, 8, 10, 12
48-12=36
남은 원자가 전자의 수입니다

Thai: 
 
ในวิดีโอนี้ เราจะใช้ทฤษฎี VSEPR
กับเมฆอิเล็กตรอน 6 ก้อน
ถ้าเป้าหมายของเราคือหารูปร่างของซัลเฟอร์
เฮกซะฟลูออไรด์โมเลกุล เหมือนเดิม
เราเริ่มด้วยโครงสร้างจุด
ซัลเฟอร์อยู่ในหมู่ 6 ของตารางธาตุ
วาเลนซ์อิเล็กตรอน 6 ตัว
ฟลูออรีนอยู่ในหมู่ 7 มีวาเลนซ์อิเล็กตรอน 7 ตัว
แต่ผมมี 6 ตัว
7 คูณ 6 ได้ค่าเป็น 42 แล้ว 42 บวก 6
ให้วาเลนซ์อิเล็กตรอน 48 ตัวที่เรา
ต้องแสดงในโครงสร้างจุด
ซัลเฟอร์อยู่ตรงกลาง 
เราก็ลงมือใส่ซัลเฟอร์ตรงนี้
และเราล้อมรอบซัลเฟอร์ด้วยฟลูออรีน 6 ตัว
ขอผมลงมือใส่ฟลูออรีน 6 ตัวนั้นล้อมรอบ
ซัลเฟอร์
ขั้นต่อไปคือดูว่าเราแสดงวาเลนซ์
อิเล็กตรอนไปแล้วกี่ตัว
ผมจะเน้นพวกมัน -- 2, 4, 6, 8, 10 และ 12
48 ลบ 12 เหลือวาเลนซ์อิเล็กตรอน 36 ตัว

Korean: 
이는 말단 원자인 플루오린 원자들에 놓습니다
플루오린은 옥텟규칙을 따릅니다
각각의 플루오린이 이미
2개의 전자를 가지고 있기 때문에
플루오린 1개당
6개의 전자를 더 넣게 됩니다
각 플루오린에 6개씩 더해주므로
각 플루오린은 8개의 전자를 가지게 됩니다
각 플루오린에 6개씩 더해주므로
각 플루오린은 8개의 전자를 가지게 됩니다
만약 6개의 전자를 6개의 원자에 더하면
6×6=36입니다
이로써 모든 원자가전자를 나타냈습니다
이로써 모든 원자가전자를 나타냈습니다
루이스 전자점식을 완성했습니다
다음 단계로 넘어가서
중심 원자 주변의 전자 구름
즉 전자 밀도를 파악합니다
여기 결합이 있는 부분도
전자 밀도가 존재하는 부분입니다
여기 결합이 있는 부분도
전자 밀도가 존재하는 부분입니다
이런 식으로 계속 진행할 수 있습니다
황을 둘러싸고 있는 이 결합들은
모두 전자 밀도가 있는 부분입니다
황을 둘러싸고 있는 이 결합들은
모두 전자 밀도가 있는 부분입니다
그 부분이 전자구름으로 치는 부분입니다
VSEPR 이론에 따르면
원자가 전자는 모두 음전하를 띠기 때문에
서로서로 밀어내서
공간상에서 가능한한 멀리 위치합니다
공간상에서 가능한한 멀리 위치합니다

Bulgarian: 
които поставяме към крайните атоми, които са флуорните.
Флуорът ще следва октетното правило.
След като всеки флуорен атом вече е ограден от 2 електрона,
ще дадем на всеки флуорен атом още по 6.
Като дадем на всеки флуорен атом по още 6,
сега всеки флуорен атом има един октет електрони около себе си.
Ако добавям 6 електрона към 6 атома, 6 по 6 е 36.
Следователно сега представих всички валентни електрони.
И сме готови с точковата си структура.
Можем да преминем към втора стъпка
и да преброим електронните облаци, които ограждат централния атом.
Области електронна плътност.
Тези свързващи се електрони тук,
това е една област електронна плътност.
И мога да продължа чак дотук.
Всички тези свързващи електрони, които ограждат сярата,
са области електронна плътност.
Следователно ги приемаме за електронни облаци.
Теорията VSEPR ни казва, че тези валентни електрони са отрицателно заредени
и следователно ще се отблъснат
и ще опитат да се отдалечат колкото е възможно повече.

Thai: 
ซึ่งเราใส่มันในอะตอมปลาย คือฟลูออรีน
ฟลูออรีนจะทำตามกฎออกเตท
และเนื่องจากฟลูออรีนมี
อิเล็กตรอนล้อมรอบแล้ว 2 ตัว เราจะ
ให้ฟลูออรีนแต่ละตัวอีก 6 ตัว
เมื่อให้อิเล็กตรอน 6 ตัวแก่ฟลูอออรีนแต่ละตัว
ฟลูออรีนจะมีอิเล็กตรอนตามออกเตท
ถ้าผมใส่อิเล็กตรอน 6 ตัวให้อะตอม 6 ตัว
6 คูณ 6 ได้ 36
เพราะฉะนั้น ผมได้แสดง
วาเลนซ์อิเล็กตรอนทั้งหมดแล้ว
และเราทำโครงสร้างจุดเสร็จแล้ว
เราเลื่อนไปยังขั้นที่ 2 แล้วนับ
จำนวนเมฆอิเล็กตรอน
ที่ล้อมรอบอะตอมตรงกลาง
เขตของความหนาแน่นอิเล็กตรอน
อิเล็กตรอนที่ทำพันธะตรงนี้ 
มันคือเขตของความหนาแน่น
อิเล็กตรอน
และผมทำต่อไปได้
อิเล็กตรอนที่ทำพันธะทั้งหมดที่ล้อมรอบ
ซัลเฟอร์ คือเขตความหนาแน่นอิเล็กตรอน
เพราะฉะนั้น เรานับพวกมันเป็นเมฆอิเล็กตรอน
ทฤษฎี VSEPR บอกว่า
วาเลนซ์อิเล็กตรอนเหล่านี้เป็น
ประจุลบหมด เพราะฉะนั้น พวกมัน
จะผลักกันและพยายาม
อยู่ให้ห่างกันมากที่สุดในสเปซ
เท่าที่จะทำได้

English: 
which we put on our terminal
atoms, which are our fluorines.
So fluorine is going to
follow the octet rule.
And since each
fluorine is already
surrounded by 2
electrons, we're going
to give each fluorine 6 more.
So by giving each
fluorine 6 more, now
each fluorine has an octet
of electrons around it.
So if I'm adding 6 electrons
to 6 atoms, 6 times 6 is 36.
And so therefore, I
have now represented
of all my valence electrons.
And we're done with
our dot structure.
We can move on to
step two and count
the number of electron clouds
surrounding our central atom,
so regions of electron density.
So these bonding electrons here,
that's a region of electron
density.
And I can just keep on
going all the way around.
So all of these bonding
electrons surrounding
our sulfur are regions
of electron density.
Therefore, we consider
them to be electron clouds.
VSEPR theory says that these
valence electrons are all
negatively charged,
and therefore, they're
all going to repel
each other and try
to get as far away from
each other in space
as they possibly can.

English: 
And so when you have
6 electron clouds,
they're going to point
towards the corners
of a regular octahedron
to try to get as far
away from each
other as they can.
So an octahedron
with 8 faces on it.
So let me see if I can
sketch in an octahedron here.
So let's see if we can do it.
It's a little bit
tricky to draw.
So if we consider our sulfur to
be at the center right here--
let's go ahead and
put a point up here
and then start
connecting some lines.
So this is sort of
what it looks like.
So let's do that and then
a point down here as well.
And so we connect those lines.
And once again, this is just a
rough sketch of an octahedron.
Something like that.
So if you think about where your
fluorines are-- right there.
Here's a fluorine right here.
There's a fluorine right here.
So at these corners,
you could think
about a fluorine
being there like that.

Thai: 
และเมื่อคุณมีเมฆอิเล็กตรอน 6 ก้อน
พวกมันจะชี้หามุม
ของทรงแปดหน้าด้านเท่าเพื่อให้ห่างกัน
มากที่สุดเท่าที่จะทำได้
ทรงแปดหน้ามีอยู่ 8 หน้า
ขอผมลองดูว่าจะวาดรูปทรงแปดหน้าได้ไหม
ลองดูว่าเราทำได้ไหม
มันวาดยากหน่อย
 
ถ้าเราพิจารณาซัลเฟอร์อยู่ตรงกลางตรงนี้ --
ลองลงมือใส่จุดบนนี้
แล้วเริ่มเชื่อมเส้น
นี่คือหน้าตาของมัน
ลองทำดู แล้วจุดข้างล่างนี้ด้วย
เราเชื่อมเส้นเหล่านั้น
ย้ำอีกครั้ง นี่คือภาพวาดคร่าวๆ 
ของทรงแปดหน้า
เป็นแบบนั้น
ถ้าคุณคิดว่าฟลูออรีนอยู่ตรงไหน -- ตรงนั้น
นี่คือฟลูออรีนตรงนี้
มีฟลูออรีนตรงนี้
ที่มุมเหล่านี้ คุณคิด
ว่าฟลูออรีนอยู่ตรงนั้นอย่างน้้นได้

Bulgarian: 
Когато имаш 6 електронни облака,
те ще сочат към ъглите на един правилен осмостен,
за да опитат да се отдалечат колкото е възможно повече.
Осмостен с 8 страни.
Нека видя дали мога да скицирам един осмостен.
Да видим дали мога да направя това.
Малко е сложно за чертане.
Ако приемем, че сярата е в центъра,
нека поставим една точка тук
и да започнем да свързваме правите.
Изглежда подобно на това.
Нека направим това и да поставим точка тук долу.
И свързваме тези прави.
Отново, това е просто приблизителна скица на един осмостен.
Нещо подобно.
Ако помислиш къде са флуорните атоми – ето тук.
Това тук е един флуорен атом.
Това тук е един флуорен атом.
В тези ъгли, можеш да помислиш, че тук има един флуорен атом.
Това е нашият осмостен.

Korean: 
6개의 전자구름을 가지고 있을 때는
서로에게서 가능한 멀리 떨어지기 위해
서로에게서 가능한 멀리 떨어지기 위해
정팔면체의 꼭짓점 방향에 위치하게 됩니다
8개의 면을 가진 정팔면체가 됩니다
정팔면체를 그려보도록 합니다
한번 그릴 수 있는지 보겠습니다
그리기가 약간 까다롭습니다
그리기가 약간 까다롭습니다
황이 중심에 있다고 생각합시다
여기에 점을 찍은 후 선을 연결해봅시다
여기에 점을 찍은 후 선을 연결해봅시다
대략적으로 이렇게 생겼습니다
여기에도 점을 찍읍시다
그리고 선들을 연결합시다
팔면체를 대략적으로 그린 것입니다
팔면체를 대략적으로 그린 것입니다
플루오린이 어딨는지를 한번 생각해본다면
바로 여기입니다
여기에 플루오린 하나가 있고
여기에도 플루오린이 있습니다
꼭짓점 부분에 불소가 있다고
생각하면 됩니다

English: 
So that's our octahedron.
So that's step three.
The geometry of the electron
clouds around the central atom,
they occupy an
octahedral geometry.
Step four, ignore any lone
pairs in your central atom
and predict the geometry
of the molecule.
Well, since we have no lone
pairs on our central sulfur,
the geometry of the
molecule is the same
as the geometry of
the electron clouds.
And so therefore, we can
say that sulfur hexafluoride
is an octahedral molecule.
So let's go ahead and
write octahedral here.
In terms of bond angles,
let's analyze our drawing
a little bit more here.
So if I look at
this top fluorine
and I go straight down like an
axis to that other fluorine,
we would expect one of
the ideal bond angles
to be 180 degrees for
this octahedron here.
And the other ideal bond
angles would be 90 degrees.
So if I think about the angle
that the axis I just drew
makes with this one right here,
so that's 90 degrees as well.
And again, anywhere
you look, you're
also going to get 90 degrees.

Bulgarian: 
Това е стъпка 3.
Електронните облаци около централния атом
обитават осмостенна геометрия.
Стъпка 4, игнорирай всички свободни двойки около централния атом
и прогнозирай геометрията на молекулата.
След като нямаме свободни двойки на централната сяра,
геометрията на молекулата е същата като геометрията на електронните облаци.
Следователно можем да кажем, че серният хексафлуорид
е осмостенна молекула.
Нека запишем осмостенна тук.
Що се отнася до ъгли на връзката,
нека анализираме чертежа си.
Ако погледна горния флуорен атом
и продължа право на долу като една ос до този друг флуорен атом,
очакваме един от идеалните ъгли на връзката
да е 180 градуса за този осмостен тук.
И другите идеални ъгли на връзката ще са 90 градуса.
Ако помисля за оста, която току-що начертах, и ъгъла, който
прави с тази тук, това е също 90 градуса.
И, отново, навсякъде, където погледнеш,
също ще получиш 90 градуса.

Korean: 
8면체입니다
3단계입니다
중심원자 주위의 전자구름은 8면체 모양입니다
중심원자 주위의 전자구름은 8면체 모양입니다
4단계인데요, 중심원자의 고립전자쌍들을 무시하고
분자의 모양을 예측해봅니다
중심원자인 황에는 고립전자쌍이 없기 때문에
전자구름의 모양과 분자의 모양이 같습니다
전자구름의 모양과 분자의 모양이 같습니다
육플루오린화황은 8면체 분자라고 할 수 있습니다
육플루오린화황은 8면체 분자라고 할 수 있습니다
8면체를 여기 한번 써보겠습니다
결합각 측면에서 그림을 조금 더 분석해봅시다
결합각 측면에서 그림을 조금 더 분석해봅시다
위쪽의 플루오린에서
아래쪽의 플루오린으로 이어지는 선을 그어보면
이 팔면체에 대한 이론적인 결합각은
180°임을 알 수 있습니다
그리고 다른 이론적인 결합각은 90도일 겁니다
금방 그린 축과 바로 여기있는 축 사이의
각도에 대해서 생각해보면
마찬가지로 90도라는 걸 생각해볼 수 있습니다
어딜 보더라도 90도 결합각을 찾을 수 있습니다
어딜 보더라도 90도 결합각을 찾을 수 있습니다

Thai: 
นั่นคือทรงแปดหน้าของเรา
นั่นคือขั้นที่ 3
เรขาคณิตของเมฆอิเล็กตรอน
รอบอะตอมตรงกลาง
พวกมันมีรูปเรขาคณิตทรงแปดหน้า
ขั้นที่ 4 ไม่สนใจคู่โดดเดี่ยวในอะตอมตรงกลาง
แล้วทำนายเรขาคณิตของโมเลกุล
เนื่องจากเราไม่มีคู่โดดเดี่ยว
ในซัลเฟอร์ตรงกลาง
เรขาคณิตของโมเลกุลจะเหมือนกับ
เรขาคณิตของเมฆอิเล็กตรอน
เพราะฉะนั้น เราบอกได้ว่า
ซัลเฟอร์เฮกซะฟลูออไรด์
คือโมเลกุลทรงแปดหน้า
ลองลงมือเขียนทรงแปดหน้าตรงนี้
ในแง่ของมุมพันธะ ลองวิเคราะห์ภาพวาด
อีกหน่อยตรงนี้
ถ้าผมดูฟลูออรีนด้านบนนี้
ผมลงมาตรงๆ เหมือนแกนไปยังฟลูออรีนอีกตัว
เราคาดว่ามุมพันธะในอุดมคติค่าหนึ่ง
จะเป็น 180 องศาสำหรับทรงแปดหน้านี่ตรงนี้
และมุมพันธะในอุดมคติอีกมุมจะเป็น 90 องศา
ถ้าผมคิดถึงมุมที่แกนที่ผมเพิ่งวาด
ทำกับเส้นนี่ตรงนี้ มันจะเท่ากับ 90 องศาเช่นกัน
เหมือนเดิม ไม่ว่าคุณดูตรงไหน คุณ
จะได้มุม 90 องศา

Korean: 
이 지점의 색깔을 바꿔보고
이 지점에서 결합각을 볼 수도 있습니다
이 결합각은 마찬가지로 90°입니다
8면체에서 각 위치를 차지하는
6개의 플루오린이 모두 같습니다
8면체에서 각 위치를 차지하는
6개의 플루오린이 모두 같습니다
8면체에서 각 위치를 차지하는
6개의 플루오린이 모두 같습니다
8면체 배치에서는 축 위치나 적도 위치가
따로 없고, 모두 동일합니다
8면체 배치에서는 축 위치나 적도 위치가
따로 없고, 모두 동일합니다
이전 동영상에서 5개의 전자구름을 가진
분자에서는 축 위치나 적도 위치를
고려해야 했으므로
지금이 훨씬 간단합니다
오플루오린화브로민을 살펴봅시다
브로민은 7개의 원자가전가를 가졌습니다
17족입니다
플루오린도 17족인데
지금 5개의 플루오린이 있습니다
7×5=35
35+7=42개의 원자가 전자가 나옵니다
브로민은 중앙에 위치하고
5개의 불소와 결합합니다
브로민은 중앙에 위치하고
5개의 불소와 결합합니다
중심원자 주변에 5개의 플루오린을 놓아봅시다

Bulgarian: 
Нека сменя цветовете
и можем да разгледаме друг ъгъл на връзката тук.
Този ъгъл на връзката също ще е 90 градуса.
За един осмостен всички 6 позиции –
имаме 6 флуорни атома, които заемат 6-те позиции –
са еквивалентни.
Те са идентични, което означава, че при осмостенното подреждане
нямаме напречни или екваториални групи.
Това прави живота ни по-лесен,
понеже във видеата с 5-те електронни облака
трябваше да помислим за напречните и екваториалните групи.
Нека направим пример за бромиден пентафлуорид, BrF5.
Бромът има 7 валентни електрони.
Той е в седма група.
Флуорът също е в 7 група и имам 5 флуорни атома.
7 по 5 ми дава 35.
35 плюс 7 ми дава 42 валентни електрона.
Бромът отива в центъра
и е свързан с 5 флуорни атома.

English: 
Let me go ahead and
change colors here,
and we can look at another
bond angle in here.
So this bond angle, that
would also be 90 degrees.
So for an octahedral,
all 6 positions--
we have 6 fluorines
occupying the 6 positions--
are equivalents.
They are identical, which means
no axial or equatorial groups
in an octahedral arrangement.
And that makes our
life much easier,
because in the videos
on 5 electron clouds,
we had to think about the
axial and equatorial groups.
Let's do one for bromine
pentafluoride here, so BrF5.
So valence electrons,
bromine has 7.
It's in group 7.
Fluorine is also in group
7, and I have 5 fluorine.
So 7 times 5 gives me 35.
35 plus 7 gives me
42 valence electrons.
Bromine goes in the
center, and bromine
is bonded to 5 fluorines.
So I can go ahead and
put those 5 fluorines

Thai: 
ขอผมลงมือเปลี่ยนสีตรงนี้
เราเห็นมุมพันธะอีกมุมในนี้
มุมพันธะนี้ มันจะเท่ากับ 90 องศาเช่นกัน
สำหรับทรงแปดหน้า ตำแหน่ง 6 แห่ง --
เรามีฟลูออรีน 6 ตัว จับจอง 6 ตำแหน่ง --
เทียบเท่ากัน
พวกมันเหมือนกัน ซึ่งหมายความว่า 
ไม่มีกลุ่มตามแกนหรือตามแนวศูนย์สูตร
สำหรับทรงแปดหน้า
นั่นทำให้ชีวิตเราง่ายขึ้น
เพราะในวิดีโอเรื่องเมฆอิเล็กตรอน 5 ตัว
เราต้องคิดถึงกลุ่มตามแกน
และตามแนวศูนย์สูตร
ลองทำสำหรับโบรมีน เพนตะฟลูออรีน กัน BrF5
วาเลนซ์อิเล็กตรอน โบรมีนมี 7
มันอยู่ในหมู่ 7
ฟลูออรีนอยู่ในหมู่ 7 เช่นกัน 
และผมมีฟลูออรีน 5 ตัว
7 คูณ 5 ให้ค่า 35
35 บวก 7 ให้วาเลนซ์อิเล็กตรอน 42 ตัว
โบรมีนอยู่ตรงกลาง และโบรมีน
ทำพันธะกับฟลูออรีน 5 ตัว
ผมก็ลงมือใส่ฟลูออรีน 5 ตัวนั้น

English: 
around our central atom.
We have represented, let's
see, 2, 4, 6, 8, and 10 valence
electrons so far.
42 minus 10 is, of course,
32 valence electrons.
And we're going to start
putting those leftover electrons
on our terminal atoms,
which are our fluorines.
So once again, we're going to
give each fluorine an octet.
So we're going to put 6 more
valence electrons around each
of our fluorine atoms.
And so we're putting 6 more
electrons around 5 atoms.
So 6 times 5 is 30.
So 32 minus 30 gives me 2
valence electrons left over.
And whenever you have
valence electrons left over
after assigning them
to your terminal atoms,
you put them on
your central atom.
And so there's going to be
a lone pair of electrons
on our central
bromine like that.
So we've drawn
our dot structure.
Let's go back up here and
look at our steps again.
So after drawing
our dot structure,

Bulgarian: 
Мога да поставя тези 5 флуорни атома около централния атом.
Представихме, да видим, 2, 4, 6, 8 и 10 валентни електрона дотук.
42 минус 10 е 32 валентни електрона.
И ще започнем да поставяме тези останали електрони
към крайните атоми, които са флуорните атоми.
Отново ще дадем на всеки флуорен атом един октет.
И ще поставим още 6 валентни електрона около всеки флуорен атом.
И поставяме още 6 електрона около 5 атома.
6 по 5 е 30.
32 минус 30 ми дава 2 останали валентни електрона.
И когато имаш останали валентни електрона,
след като ги поставиш към крайните атоми,
поставяш ги около централния атом.
И ще има една свободна двойка електрони
около централния атом бром, ето така.
Начертахме точковата си структура.
Нека се върнем тук горе и отново да погледнем стъпките си.
Начертахме точковата си структура,

Thai: 
รอบอะตอมตรงกลางได้
เราได้แสดง ลองดู วาเลนซ์อิเล็กตรอน
2, 4, 6, 8 และ 10 ตัว
ไปแล้ว
42 ลบ 10 แน่นอน 
เหลือวาเลนซ์อิเล็กตรอน 32 ตัว
เราจะเริ่มใส่อิเล็กตรอนที่เหลือพวกนั้น
ในอะตอมปลาย ซึ่งก็คือฟลูออรีน
เหมือนเดิม เราจะทำให้ฟลูออรีน
แต่ละตัวเป็นออกเตท
เราจะใส่วาเลนซ์อิเล็กตรอนอีก 6 ตัวรอบๆ
อะตอมฟลูออรีนแต่ละตัว
เราจะใส่อิเล็กตรอนอีก 6 ตัวรอบอะตอม 5 ตัว
6 คูณ 5 ได้ 30
32 ลบ 30 เหลือวาเลนซ์อิเล็กตรอน 2 ตัว
และเมื่อใดก็ตาม
ที่คุณมีวาเลนซ์อิเล็กตรอนเหลือ
หลังจากใส่ลงในอะตอมปลายแล้ว
คุณก็ใส่พวกมันลงในอะตอมกลาง
และมันจะะเป็นอิเล็กตรอนคู่โดดเดี่ยว
บนโบรมีนตรงกลางอย่างนั้น
เราวาดโครงสร้างจุดไปแล้ว
ลองกลับไปตรงนี้ และดูขั้นตอนอีกที
หลังจากวาดโครงสร้างจุด

Korean: 
중심원자 주변에 5개의 플루오린을 놓아봅시다
우리는 지금까지 2, 4, 6, 8, 10개의 원자가전자를
표현했습니다
42-10=32 이므로 32개의 원자가 전자입니다
남은 전자를 말단 원자인 플루오린에 놓읍시다
남은 전자를 말단 원자인 플루오린에 놓읍시다
각 플루오린의 옥텟을 완성시킵니다
각 플루오린 원자에 6개의
원자가 전자를 더 넣을 예정입니다
각 플루오린 원자에 6개의
원자가 전자를 더 넣을 예정입니다
5 개의 원자들에 각각 6개의
원자가 전자를 더 넣게 됩니다
6×5=30이 됩니다
남은 원자가 전자는 32-30=2 개가 됩니다
말단 원자에 배분한 후
남는 원자가 전자가 있으면
중앙 원자에 배치합니다
중심 원자에 비공유 전자쌍 하나가 있을 것입니다
중심 원자에 비공유 전자쌍 하나가 있을 것입니다
지금까지 루이스 전자점식을 그렸습니다
이 부분으로 돌아가서
지금까지의 단계를 다시 살펴봅시다
루이스 전자점식을 완성하고

Thai: 
เราก็นับจำนวนเมฆอิเล็กตรอน
ที่ล้อมรอบอะตอมตรงกลางต่อ แล้วทำนาย
เรขาคณิตของเมฆอิเล็กตรอนเหล่านั้น
ถ้าเราดูโบรมีนตรงกลางตรงนี้
ลองดูว่ามีเมฆอิเล็กตรอนกี่ก้อน
เรามีอิเล็กตรอนที่ทำพันธะเหล่านี้
เขตของความหนาแน่นอิเล็กตรอน
อิเล็กตรอนที่ทำพันธะ
อิเล็กตรอนที่ทำพันธะเหล่านี้
และเราไปรอบๆ ตรงนี้
พวกนี้คือเมฆอิเล็กตรอนทั้งนั้น
นั่นคือ 5
แล้วนึกดู อิเล็กตรอนที่ไม่ทำพันธะเหล่านี้
อิเล็กตรอนคู่โดดเดี่ยวนี้
เป็นเขตความหนาแน่นอิเล็กตรอนเช่นกัน
เราจึงได้เมฆอิเล็กตรอน 6 ตัว
และเราเพิ่งเห็นในตัวอย่างที่แล้ว เมื่อ
คุณมีเมฆอิเล็กตรอน 6 ก้อน เมฆอิเล็กตรอน
จะอยากชี้หามุม
ของทรงแปดหน้าด้านเท่า
คุณจะได้เรขาคณิตเป็นทรงแปดหน้า
สำหรับเมฆอิเล็กตรอน
ลองคิดถึงอันนี้ดู
เราจะใส่อิเล็กตรอนคู่โดดเดี่ยว
ไว้ตรงไหนในทรงแปดหน้า
เนื่องจาก 6 ตำแหน่งนี้เหมือนกันหมด

English: 
we next count the number
of electron clouds
that surround our central
atom and then predict
the geometry of those
electron clouds.
And so if we look at our
central bromine here,
let's see how many
electron clouds.
Well, we would have
these bonding electrons,
a region of electron density,
these bonding electrons,
these bonding electrons.
And we keep on
going around here.
So those are all
electron clouds.
So that's 5.
And then remember, these
non-bonding electrons,
this lone pair of
electrons, is also
a region of electron density.
And so we have 6
electron clouds.
And so we just saw in the
previous example, when
you have 6 electron
clouds, the electron clouds
are going to want to
point towards the corners
of a regular octahedron.
So you're going to get
an octahedral geometry
for your electron clouds.
Let's think about
this one, though.
Where will we put
those that lone pair
of electrons in an octahedron.
Well, since all 6
positions are identical,

Korean: 
중앙 원자를 둘러싼 전자구름의 개수를 세어보고
중앙 원자를 둘러싼 전자구름의 개수를 세어보고
전자구름의 구조를 예측합니다
중앙 브로민에 전자 구름이
몇 개 있는지 보겠습니다
중앙 브로민에 전자 구름이
몇 개 있는지 보겠습니다
이 결합 전자들이 있는 곳이
전자 밀도가 있는 곳입니다
전자 밀도가 있는 곳입니다
이런 식으로 계속합니다
모두 전자구름입니다
총 5개입니다
기억해야 할 점은, 비공유 전자쌍도
전자 밀도가 존재하는 영역이란 것입니다
전자 밀도가 존재하는 영역이란 것입니다
6개의 전자구름이 있습니다
이전 예시에서 보았듯이
6개의 전자구름이 있으면
정팔면체의 꼭짓점 방향에 위치합니다
정팔면체의 꼭짓점 방향에 위치합니다
전자구름은 정팔면체 구조를 이루게 됩니다
전자구름은 정팔면체 구조를 이루게 됩니다
이 부분에 대해서 생각해봅시다
팔면체의 어느 부분에
비공유 전자쌍을 놓아야 할까요?
6 자리가 사실 다 동일하기 때문에
어디다가 고립전자쌍을 넣을지는 중요하지 않습니다

Bulgarian: 
след което броим електронните облаци,
които ограждат централния атом.
После трябва да прогнозираме геометрията на тези електронни облаци.
Да разгледаме централния бромен атом тук
и да видим колко електронни облака имаме.
Ще имаме тези свързващи електрони, една област електронна плътност,
тези свързващи електрони, тези свързващи електрони.
И продължаваме.
Всички тези са електронни облаци.
Общо 5.
И после, помни, тези несвързващи електрони,
тази свободна двойка електрони,
също са област електронна плътност.
Тоест имаме 6 електронни облаци.
Видяхме в предишния пример, че,
когато имаш 6 електронни облака,
електронните облаци ще искат да сочат към ъглите
на един правоъгълен осмостен.
Ще имаш осмостенна геометрия
за електронните си облаци.
Но нека да помислим за това.
Къде ще поставим тази свободна двойка електрони
в един осмостен?
След като всички 6 позиции са идентични,

Thai: 
มันไม่เกี่ยวว่า
คุณจะใส่อิเล็กตรอนคู่โดดเดี่ยวไว้ตรงไหน
พอผมดูหน่อยว่าผมลงมือวาด
รูปร่างอย่างรวดเร็วได้ไหม
ถ้าผมวาดโบรมีนตรงนี้
ผมจะใส่ฟลูออรีน
ในทิศนี้ ฟลูออรีนอีกตัวไปข้างหลัง
อันนี้ออกมาหน่อย อันนี้ออกไป
แล้วผมจะใส่ฟลูออรีนไปทางนี้
แล้วผมจะใส่อิเล็กตรอนคู่โดดเดี่ยว
ข้างล่างตรงนี้
เหมือนเดิม มันไม่เกี่ยวว่าผมจะเลือก
ตัวไหนเพราะพวกมันเหมือนกันหมด
ผมเลือกมันแบบนี้เพราะมันเห็นเรขาคณิต
ได้ง่ายกว่าหน่อย
เพราะเมื่อคุณดูเรขาคณิตของโมเลกุล
คุณไม่สนอิเล็กตรอนคู่โดดเดี่ยว
ของอะตอมตรงกลาง
ถ้าเราไม่สนอิเล็กตรอนคู่โดดเดี่ยวแล้ว
และเราดูรูปร่าง -- ลอง
ดูว่าเราต่อจุดเหล่านี้ได้ไหม
เราจะเชื่อมจุดนี้เป็นรูปร่าง
เราได้ฐานสี่เหลี่ยมจัตุรัสตรงนี้
และถ้าเราเชื่อมข้างบนนี้กับฟลูออรีนข้างบน
มันเป็นเหมือนพีระมิด
เราจึงได้พีระมิดฐานสี่เหลี่ยมจัตุรัส

Korean: 
6 자리가 사실 다 동일하기 때문에
어디다가 고립전자쌍을 넣을지는 중요하지 않습니다
6 자리가 사실 다 동일하기 때문에
어디다가 고립전자쌍을 넣을지는 중요하지 않습니다
정말 빠르게 그림을 그려보도록 하겠습니다
정말 빠르게 그림을 그려보도록 하겠습니다
여기에 브로민을 그린다면
플루오린 하나는 이 방향으로 그리고
다른 플루오린은 뒤쪽으로 그립니다
하나는 튀어나오고 하나는 들어갑니다
이쪽으로 플루오린 하나를 그리고
비공유 전자쌍을 여기에 넣을 것입니다
비공유 전자쌍을 여기에 넣을 것입니다
사실 모두가 동일하기 때문에
어느 것을 선택할지는 중요하지 않습니다
사실 모두가 동일하기 때문에
어느 것을 선택할지는 중요하지 않습니다
단지 모양을 알아보기가 더 쉽기 때문에
이것을 선택했습니다
왜냐하면 분자의 모양을 따질 때는
중앙원자의 비공유 전자쌍은 무시하기 때문입니다
지금은 비공유 전자쌍을 무시하고
분자의 모양을 따져봅시다
이 점들을 연결해서
모양을 봅시다
여기에는 사각형 바닥이 있습니다
이 위쪽의 플루오린과 연결시키면
일종의 피라미드 모양입니다
바닥이 사각형인 피라미드 구조입니다

English: 
it doesn't really
matter which one
you put that lone
pair of electrons in.
And so let me see if I can
just go ahead and sketch out
the shape really fast.
So if I were to draw
a bromine right here,
I'm going to put
a fluorine going
in this direction, another
fluorine going back,
this one coming out a little
bit, and this one going away.
And then I'm going to put
a fluorine going this way,
and then I'm going to put
the lone pair of electrons
right down here.
Again, it didn't
really matter which one
I chose since they're
all identical.
I just chose it this way
because it's a little bit easier
to see the geometry.
Because when you're looking at
the geometry of the molecule,
you ignore any lone pairs of
electrons on your central atom.
And so if we ignore that
lone pair of electrons now,
and we look at the
shape-- so let's
see if we can connect
these dots here.
So we're just going to connect
this to look at a shape.
So we have a square base here.
And if we connect up here
to this top fluorine, well,
that's kind of a pyramid.
So we have a pyramid
with a square base.

Bulgarian: 
няма значение къде ще поставиш свободната двойка електрони.
И да видим дали мога набързо да скицирам формата.
Ако начертая един атом бром тук,
ще поставя един флуорен атом в тази посока,
друг флуорен атом назад,
този, излизащ малко насам, и още един, преминаващ настрани.
И после ще поставя един флуорен атом насам,
а после ще поставя свободната двойка електрони тук долу.
Отново, няма значение коя позиция ще избера,
след като всички те са идентични.
Избрах тази, понеже е малко по-лесно
да се види геометрията.
Понеже когато гледаш геометрията на молекулата,
игнорираш всички свободни двойки електрони около централния атом.
И ако сега игнорираме тази двойка свободни електрони
и разгледаме формата –
да видим дали можем да свържем точките.
Ще свържем това в една форма.
Тук имаме квадратна основа.
И ако я свържем с този горен флуорен атом,
това е един вид пирамида.
Имаме пирамида с квадратна основа.

Korean: 
이를 사각 피라미드형이라고 부릅니다
사각 피라미드형이라고 적겠습니다
이 모양은 사각 피라미드형이라고 부릅니다
결합각 측면에서 살펴보면
이론적인 결합각은 90도입니다
이론적인 결합각은 90도입니다
바로 전에 이야기한 것과 같습니다
결합각이 90도입니다
여기 결합각은 90도 입니다
사각 피라미드형에서
전자구름이 6개인 예를 한 가지 더 살펴봅시다
전자구름이 6개인 예를 한 가지 더 살펴봅시다
사플루오르화 크세논입니다
원자가 전자를 찾아야 합니다
크세논은 18족이므로 8개의 원자가 전자를 가집니다
플루오린은 17족에 속해있습니다
그럼 원자가 전자는 7×4+8=36개입니다
그럼 원자가 전자는 7×4+8=36개입니다
크세논을 여기 중앙에 놓습니다

English: 
And so we call this
square pyramidal.
So let's go ahead
and write that.
This shape is referred to
as a square pyramidal shape.
And in terms of
bond angles, we know
our ideal bond angles are
going to be 90 degrees.
So if we look at that,
let's use this green here.
So it's just like we
talked about before.
So that bond angle
is 90 degrees.
This bond angle in
here is 90 degrees.
So our ideal bond angles
are all 90 degrees
for our square
pyramidal geometry.
Let's do one more example
of 6 electron clouds.
And this is xenon tetrafluoride.
So we need to find
our valence electrons.
So xenon is in group
8, 8 valence electrons.
Fluorine is in group 7.
So 7 valence electrons
times 4 gives me 28.
28 plus 8 gives me
36 valence electrons.
Xenon goes in the center.

Bulgarian: 
Наричаме това квадратно пирамидална форма.
Нека запиша това.
Формата се нарича квадратно пирамидална.
Що се отнася до ъгли на връзката, знаем, че
идеалните ъгли на връзката ще са 90 градуса.
Ако погледнем това – нека използваме зелено.
Точно както говорихме преди.
Този ъгъл на връзката е 90 градуса.
Този ъгъл на връзката тук е 90 градуса.
Всички идеални ъгли на връзката за квадратно пирамидална геометрия са 90 градуса.
Нека направим още един пример за 6 електронни облака.
Това е ксенонен тетрафлуорид.
Трябва да намерим валентните си електрони.
Ксенонът е в осма група, 8 валентни електрони.
Флуорът е в седма група.
7 валентни електрона по 4 дава 28.
28 плюс 8 прави 36 валентни електрони.
Ксенонът отива в центъра.

Thai: 
และเราเรียกรูปนี้ว่าพีระมิดสี่เหลี่ยมจัตุรัส
ลองลงมือเขียนลงไป
รูปนี้เรียกว่า รูปพีระมิดสี่เหลี่ยมจัตุรัส
และในแง่ของมุมพันธะ เรารู้
ว่ามุมพันธะในอุดมคติจะเท่ากับ 90 องศา
ถ้าเราดูมัน ลองใช้สีเขียวตรงนี้
มันเหมือนกับที่เราพูดไปก่อนหน้านี้
มุมพันธะนั้นเท่ากับ 90 องศา
มุมพันธะนี่ตรงนี้คือ 90 องศา
มุมพันธะในอุดมคติของเราเป็น 90 องศาหมด
สำหรับเรขาคณิตของพีระมิดสี่เหลี่ยมจัตุรัส
ลองทำตัวอย่างเมฆอิเล็กตรอน 6 ก้อนอีกอัน
และอันนี้คือซีนอนเตตระฟลูออไรด์
เราต้องหาวาเลนซ์อิเล็กตรอนก่อน
ซีนอนอยู่ในหมู่ 8 วาเลนซ์อิเล็กตรอน 8 ตัว
ฟลูออรีนอยู่ในหมู่ 7
วาเลนซ์อิเล็กตรอน 7 ตัวคูณ 4 ให้ค่าเป็น 28
28 บวก 8 ให้วาเลนซ์อิเล็กตรอน 36 ตัว
ซีนอนอยู่ตรงกลาง

Korean: 
크세논을 여기 중앙에 놓습니다
크세논은 4개의 플루오린과 결합합니다
크세논을 둘러싸는 4개의 플루오린을 넣습니다
크세논을 둘러싸는 4개의 플루오린을 넣습니다
2, 4, 6, 8개의 원자가 전자를 표현했습니다
2, 4, 6, 8개의 원자가 전자를 표현했습니다
그러면 원자가 전자가 36-8=28개 남고
이들은 말단 플루오린에 놓습니다
그러면 각 플루오린은 옥텟을 이루게 됩니다
각각의 플루오린 원자에 원자가 전자를
6개씩 더 넣어야 합니다
4개의 원자에 전자 6개씩을 더 넣으니까
6×4=24
28-24=4개의 원자가 전자가 남게 됩니다
남는 것을 중앙 원자인 크세논에다가 넣습니다
남는 것을 중앙 원자인 크세논에다가 넣습니다
중앙 원자에 4개의 전자를 추가합니다

Bulgarian: 
Поставяме ксенона в центъра.
И ксенонът е свързан с 4 флуорни атома.
Поставяме нашите 4 флуорни атома
около ксенона.
Да видим, представихме 2, 4, 6 и 8 валентни електрона.
36 минус 8 ще ми даде 28 останали валентни електрона,
които ще поставим към крайните флуорни атоми.
Всеки флуорен атом ще получи един октет.
Трябва да поставим 6 валентни електрона
към всеки от флуорните ни атоми.
Ще представим още 6 електрона на 4 атома.
6 по 4 е 24.
28 минус 24 ни дава 4 останали валентни електрона.
И ще поставим тези към централния атом тук,
тоест ще ги поставим към ксенона.
Добавяме тези 4 електрона

Thai: 
เราก็ลงมือใส่ซีนอนตรงกลาง
และซีนอนมีพันธะกับฟลูออรีน 4 ตัว
เราก็ลงมือใส่ฟลูออรีน 4 ตัว
ล้อมรอบซีนอน
ลองดู เราได้แสดงวาเลนซ์อิเล็กตรอน 2, 4, 6
8 ตัว
36 ลบ 8 จะเหลือวาเลนซ์อิเล็กตรอน 28 ตัว
ซึ่งเราจะใส่ให้ปลายฟลูออรีนตรงนี้
ฟลูออรีนแต่ละตัวจะได้ออกเตท
และเราต้องใส่วาเลนซ์อิเล็กตรอน 6 ตัว
ในอะตอมฟลูออรีนแต่ละตัว
เราจะแสงวาเลนซ์อิเล็กตรอนอีก 6 ตัว
ในอะตอม 4 ตัว
6 คูณ 4 ได้ 24
28 ลบ 24 เหลือวาเลนซ์อิเล็กตรอน 4 ตัว
และเราจะใส่อิเล็กตรอนเหล่านั้น
ในอะตอมตรงกลางตรงนี้
เราจะใส่พวกมันลงในซีนอน
เราก็ลงมือใส่อิเล็กตรอน 4 ตัวนั้น

English: 
So we go ahead and put
xenon in the center here.
And xenon is bonded
to 4 fluorines.
So we go ahead and
put in our 4 fluorines
surrounding our xenon.
And let's see, we have
represented 2, 4, 6,
and 8 valence electrons.
So 36 minus 8, that would
give me 28 valence electrons
left over, which we will put
on our terminal fluorines here.
So each fluorine is
going to get an octet.
And so we need to put
6 valence electrons
on each one of our
fluorine atoms.
So we are representing 6
more electrons on 4 atoms.
So 6 times 4 is 24.
So 28 minus 24 gives us 4
valence electrons left over.
And we're going to put those
on our central atom here,
so we're going to put
those on the xenon.
So we go ahead and add
in those 4 electrons

Korean: 
즉, 비공유 전자쌍 2개를 넣습니다
좋습니다
되돌아가서 루이스 전자점식을 그리고 나서
무엇을 해야 하는지에  대해서 한번 정리를 해봅시다
루이스 전자점식을 그리고 나면
전자구름의 개수를 셉니다
루이스 전자점식을 그리고 나면 전자구름의 개수를 셉니다
그러고 나서 전자구름들의 배치 모양을 예측합니다
이것의 전자구름 개수를 세어봅시다
전자 밀도 영역의 개수를 세는 것입니다
이 결합전자들은 전자구름이고
이 결합전자들도 마찬가지이고
이것들도 마찬가지입니다
이 예에서는 2개의  비공유 전자쌍이 있고
이것들도 각각 전자 밀도 영역입니다
이 예시에서는 총 6개의 전자구름이 있습니다
이 예시에서는 총 6개의 전자구름이 있습니다
이 6개의 전자구름들은
서로에게서 가능한한 멀리 떨어지려고 합니다
서로에게서 가능한한 멀리 떨어지려고 합니다
전자구름들은 팔면체를 이룰 것이고
이 분자를 그려봅시다
만약  비공유 전자쌍들이 서로
최대한 멀리 떨어지려고 한다면

Bulgarian: 
под формата на две свободни двойки към централния атом.
Добре.
Нека се върнем и да освежим паметта си
по отношение на какво правим, след като начертаем точковата структура.
След като начертаеш точковата структура,
броиш електронните облаци.
И после прогнозираш геометрията на тези електронни облаци.
Нека преброим електронните облаци.
Области електронна плътност.
Можем да видим, че тези свързващи електрони са един електронен облак
и същото важи за тези свързващи електрони,
както и за тези тук.
И в този пример имаме 2 свободни двойки електрони
и всяка от тях е една област електронна плътност.
И в този пример имаме общо 6 електронни облака.
Отново, 6 електронни облака,
те ще искат да се отдалечат възможно най-много.
Те ще са в осмостенно подреждане.
Да видим дали можем отново да скицираме тази молекула.

English: 
in the form of two lone
pairs to our central atom.
All right.
Let's go back up and
refresh our memory
about what we do after we
draw our dot structure.
So after you draw
your dot structure,
you count the number
of electron clouds.
And then you predict the
geometry of those electron
clouds, and so let's count our
electron clouds for this one.
So our regions of
electron density,
so we can see that
these bonding electrons
are an electron cloud, same
with these bonding electrons,
and these over here as well.
And in this example, we have
2 lone pairs of electrons,
and each one of those is a
region of electron density.
And so we have a
total of 6 electron
clouds for this example.
So once again, 6
electron clouds,
they are going to want to get
as far away from each other
as they can.
So they are going to be in
an octahedral arrangement,
and so let's see if we can
sketch out this molecule again.
So if the lone
pairs of electrons

Thai: 
ในรูปของคู่โดดเดี่ยว 2 คู่ให้อะตอมตรงกลาง
เอาล่ะ
ลองกลับไปทบทวนความจำ
เกี่ยวกับสิ่งที่เราทำ
หลังจากวาดโครงสร้างจุดกัน
หลังจากที่คุณวาดโครงสร้างจุด
คุณก็นับจำนวนเมฆอิเล็กตรอน
แล้วคุณก็ทำนาย
รูปร่างของเมฆอิเล็กตรอนเหล่านั้น
ลองนับจำนวนเมฆอิเล็กตรอน
สำหรับโมเลกุลนี้กัน
เขตของความหนาแน่นอิเล็กตรอน
เราเห็นได้ว่าอิเล็กตรอนที่ทำพันธะเหล่านี้
เป็นเมฆอิเล็กตรอน เหมือนกับ
อิเล็กตรอนที่ทำพันธะเหล่านี้
และตรงนี้เช่นกัน
และในตัวอย่างนี้ 
เรามีอิเล็กตรอนคู่โดดเดี่ยว 2 คู่
แต่ละตัวเป็นเขตความหนาแน่นอิเล็กตรอน
เราจึงมีเมฆอิเล็กตรอนทั้งหมด 6 ก้อน
ในตัวอย่างนี้
เหมือนเดิม เมฆอิเล็กตรอน 6 ก้อน
พวกมันพยายามอยู่ห่างกันให้มากที่สุด
ที่เท่าทำได้
พวกมันจะเรียงตัวแบบทรงแปดหน้า
ลองดูว่าเราวาดภาพโมเลกุลนี้คร่าวๆ ได้ไหม
ถ้าอิเล็กตรอนคู่โดดเดี่ยว

Thai: 
อยากอยู่ให้ห่างกันมากที่สุด
เท่าที่จะทำได้ เราจะ
ใส่คู่โดดเดี่ยวเหล่านั้นให้ห่างกัน 180 องศา
นี่คือคู่โดดเดี่ยวคู่หนึ่ง และนี่คือ
คู่โดดเดี่ยวอีกคู่หนึ่ง
มันห่างกันเท่าที่จะเป็นไปได้
แล้วเราจะใส่ฟลูออรีนลงไปในนี้
นี่คือฟลูออรีนของเรา
นี่คือฟลูออรีนอีกตัวหนึ่ง
แล้วเรามีอีกสองตัวข้างหลัง
เมื่อเราดูรูปร่างของซีนอนเตตระฟลูออไรด์
ลองดูว่าเราวาดภาพ
รูปร่างที่มันควรเป็นได้ไหม
นึกดู เมื่อคุณทำนาย
รูปร่างของโมเลกุล คุณ
จะไม่สนอิเล็กตรอนคู่โดดเดี่ยว
เห็นได้ง่ายขึ้น
ว่าเรามีสี่เหลี่ยมจัตุรัสบนระนาบ
เราเรียกรูปนี้ว่า square planar
รูปเรขาคณิตคือสี่เหลี่ยมจัตุรัสบนระนาบ
ในแง่ของมุมพันธะอุดมคติ
มันจะเท่ากับ 90 องศา
ขอผมลงมือแสดงอย่างรวดเร็วนะ

Korean: 
만약  비공유 전자쌍들이 서로
최대한 멀리 떨어지려고 한다면
서로 180도를 이룰 것입니다
서로 180도를 이룰 것입니다
이곳과 이곳에 비공유전자쌍이 있습니다
이곳과 이곳에 비공유전자쌍이 있습니다
서로 가능한한 멀리 떨어지려고 합니다
플루오린은 여기 넣습니다
플로오린 하나는 여기에 넣고
여기 다른 플루오린을 넣고
그리고 뒤에 2개의 플루오린을 더 넣습니다
사플루오르화 크세논은
어떤 모양이 될지 한번 그려보도록 하겠습니다
어떤 모양이 될지 한번 그려보도록 하겠습니다
분자의 모양을 예측할 때는
비공유전자쌍은 무시해야 합니다
분자의 모양을 예측할 때는
비공유전자쌍은 무시해야 합니다
분자의 모양을 예측할 때는
비공유전자쌍은 무시해야 합니다
그러면 평면 사각형임이 쉽게 보입니다
그러면 평면 사각형임이 쉽게 보입니다
이 모양은 평면 사각형이라고 부릅니다
이 모양은 평면 사각형이라고 부릅니다
이론적 결합각은 90도입니다
이론적 결합각은 90도입니다
정말 빠르게 보여드리겠습니다

English: 
want to get as far
away from each other
as they possibly
can, we're going
to put those lone pairs 180
degrees from each other.
So here's one lone
pair, and then here's
our other lone pair.
That's as far away from
each other as they can get.
And then we're going to
put our fluorines in here.
So here's one fluorine.
Here would be another fluorine.
And then we would have
two more back here.
So when we look at the shape
of xenon tetrafluoride,
let's see if we
can sketch in what
the shape would look like here.
So remember, when
you're predicting
the geometry of
the molecule, you
ignore the lone
pairs of electrons.
And so that makes it
much easier to see
that we have a square
that is planar.
So we call this square planar.
So the geometry
is square planar.
And in terms of
ideal bond angles,
that would be 90 degrees.
So let me go ahead and
show that real fast.

Bulgarian: 
Ако свободните двойки електрони
искат да се отдалечат възможно най-много,
ще поставим тези свободни двойки на 180 градуса една от друга.
Това е една свободна двойка,
а това е другата свободна двойка.
Толкова могат да се отдалечат.
И ще поставим флуорните атоми тук.
Това е един флуорен атом.
Това ще е друг флуорен атом.
и после тук ще имаме още два.
Ще пробвам да скицирам формата на ксенонен тетрафлуорид.
Помни, когато прогнозираш геометрията на молекулата,
игнорираш свободните двойки електрони.
И така е много по-лесно да видим,
че имаме един квадрат, който е равнинен.
Наричаме това квадратно равнинна форма.
Геометрията е квадратно равнинна.
А идеалните ъгли на връзката са по 90 градуса.
Нека покажа това набързо.
Що се отнася до ъгли на връзката,

Korean: 
결합각 측면에서 본다면 여기있는 모든 각이
90도라서 평면 사각형을 이룹니다
지금까지 전자구름이 6개인
경우에 대해 알아보았습니다
첫 번째 예시는 중앙원자에
0개의 비공유 전자쌍을 가졌습니다
첫 번째 예시는 중앙원자에
0개의 비공유 전자쌍을 가졌습니다
2번째 예시는 1개의 비공유 전자쌍을 가졌고
3번째 예시는 2개의 비공유 전자쌍을 가졌습니다
전자구름의 기하학적 구조는 같지만
실제 분자는 서로 다른 모양을
갖는다고 보는데
이는 중앙원자의 비공유 전자쌍을
무시하기 때문입니다
이는 중앙원자의 비공유 전자쌍을
무시하기 때문입니다

Bulgarian: 
всичко тук за квадратно равнинната връзка ще е 90 градуса.
Така подхождаме към 6 електронни облака.
И първият ни пример имаше 0 свободни двойки електрони
около централния атом.
Вторият ни пример имаше 1 свободна двойка.
И третият пример имаше 2 свободни двойки.
И въпреки че електронните облаци имат същата геометрия,
реалната молекула има различна форма,
понеже игнорираш свободните двойки електрони
на централния атом.

Thai: 
ในแง่ของมุมพันธะ ทุกอย่างตรงนี้
จะเท่ากับ 90 องศาสำหรับสี่เหลี่ยมจัตุรัสระนาบ
นั่นคือวิธีคิดถึงเมฆอิเล็กตรอน 6 ก้อน
ตัวอย่างแรกของเรามีคู่โดดเดี่ยว 0 คู่
รอบล้อมอะตอมตรงกลาง
ตัวอย่างที่สองของเรามีคู่โดดเดี่ยว 1 คู่
และตัวอย่างที่สามมีคู่โดดเดี่ยว 2 คู่
และถึงแม้ว่าเมฆอิเล็กตรอน
มีเรขาคณิตเหมือนกัน
แต่โมเลกุลจริงนั้นมีรูปร่างต่างกัน
เพราะคุณไม่คิดอิเล็กตรอนคู่โดดเดี่ยว
ของอะตอมตรงกลาง

English: 
So in terms of bond
angles, everything here
would be 90 degrees
for our square planar.
And so that's how to
approach 6 electron clouds.
And our first example
had 0 lone pairs
of electrons around
the central atom.
Our second example
had 1 lone pair.
And our third example
had 2 lone pairs.
And so even though the electron
clouds have the same geometry,
the actual molecule is said
to have a different shape,
because you ignore the
lone pairs of electrons
on your central atom.
