
English: 
Voiceover: The video on SP3 hybridization,
we saw a carbon is bonded to four atoms
and in the video in SP2 hybridization,
we saw that carbon
is bonded to three atoms
and in this video,
we're gonna look at the
type of hybridization
that's present when carbon
is bonded to two atoms.
If I look at this carbon right here
and the ethyne or the acetylene molecule.
This carbon is bonded to a hydrogen
and it's also bonded to another carbon.
We have carbon bonded to only two atoms
and the shape of the acetylene molecule
has been determined to be linear.
We have a linear geometry.
We also have a bond angle here.
These bond angles are 180 degrees
and so we must have a
different hybridization
for this carbon.
We have a different geometry,
a different bond angle
and a different number
of atoms that this carbon is bonded to.
To find our new type of hybridization,
we look at our electronic configuration
already in the excited stage.
We have carbons, four valence electrons
represented here in the excited stage.

Thai: 
ในวิดีโอเรื่อง sp3 ไฮบริดไดเซชัน
เราเห็นคาร์บอนทำพันธะกับอะตอม 4 ตัว
และในวิดีโอเรื่อง sp2 ไฮบริดไดเซชัน
เราเห็นว่าคาร์บอนทำพันธะกับอะตอม 3 ตัว
และในวิดีโอนี้
เราจะดูไฮบริดไดเซชันอีกแบบ
ที่เกิดขึ้นเมื่อคาร์บอนทำพันธะกับอะตอม 2 ตัว
ถ้าผมดูคาร์บอนนี่ตรงนี้
และเอธธีน หรืออเซธิลีนโมเลกุล
คาร์บอนนี้ทำพันธะกับไฮโดรเจน
และมันยังทำพันธะกับคาร์บอนอีกตัวด้วย
เรามีคาร์บอนทำพันธะกับอะตอมแค่ 2 ตัว
และรูปร่างของโมเลกุลอเซธิลีน
นั้นมีรูปร่างเป็นเส้นตรง
เรามีเรขาคณิตแบบเส้นตรง
เรายังมีมุมงอตรงนี้
มุมงอเหล่านี้เท่ากับ 180 องศา
และเราต้องมีไฮบริดไดเซชันต่างออกไป
สำหรับคาร์บอนนี้
เรามีเรขาคณิตที่ต่างออกไป
มุมพันธะต่างออกไป และจำนวน
อะตอมที่คาร์บอนทำพันธะด้วยต่างออกไป
เวลาหาไฮบริดไดเซชันแบบใหม่
เราดูการจัดอิเล็กตรอน
ที่อยู่ในสถานะกระตุ้นแล้ว
เรามีคาร์บอน วาเลนซ์อิเล็กตรอน 4 ตัว
อยู่ตรงนี้ในสถานะกระตุ้น

Portuguese: 
No vídeo sobre hibridização SP3,
vimos um carbono ligado a quatro átomos,
e no vídeo sobre hibridização SP2,
vimos o carbono ligado a três átomos
e neste vídeo,
veremos o tipo de hidbridização
presente quando o carbono está
ligado a dois átomos.
Se eu olhar este carbono aqui
e a molécula de etino ou acetileno.
Este carbono está ligado a um hidrogênio
e a outro carbono.
Nós temos carbono ligado a apenas dois 
átomos
e a geometria da molécula de acetileno
foi determinada como sendo linear.
Temos uma geometria linear.
Também temos um ângulo de ligação aqui.
Estes ângulos de ligação são 180 graus
então a hibridização tem que ser diferente
para este carbono.
A geometria é diferente,
o ângulo de ligação é diferente,
o número de átomos a que este carbono
está ligado é diferente.
Para determinar o novo tipo de 
hibridização,
olhamos a configuração eletrônica
no estado excitado.
Temos carbonos, quatro elétrons de 
valência
respresentado no estado excitado.

Bulgarian: 
Във видеото
за sp³-хибридизацията
видяхме въглероден атом,
който е свързан с 4 други атома,
а във видеото
за sp²-хибридизацията
видяхме въглероден атом,
свързан с 3 други атома.
В това видео ще говорим
за типа хибридизация,
който се получава,
когато въглеродният атом
е свързан с 2 други атома.
Да погледнем този
въглероден атом
от молекулата на етина
(или ацетилена).
Този въглерод е свързан с водород
и освен това е свързан
само с още един въглероден атом.
Тук имаме въглероден атом,
свързан само с два атома.
Формата на молекулата
на ацетилена
е определена
като линейна.
Имаме линейна геометрия.
Тук също има
ъгли на връзките:
те са по 180 градуса.
Това изисква
различен тип хибридизация
за този въглероден атом.
Геометрията е различна:
различен ъгъл на връзката
и различен брой атоми,
свързани с въглерода.
За да намерим новия
тип хибридизация,
ще погледнем
електронната конфигурация
във вече
възбудено състояние.
Тук са показани
четирите валентни електрона
на въглерода
във възбудено състояние.

Thai: 
1, 2, 3 และ 4
เรากำลังหาไฮบริดออร์บิทัล 2 ตัว
เพราะคาร์บอนทำพันธะกับ 2 ตัว
เราจะนำ s ออร์บิทัล
เราจะยกระดับ s ออร์บิทัล
ในแง่ของพลังงาน และเราจะลดระดับ
p ออร์บิทัล p ออร์บิทัลแค่ตัวเดียวคราวนี้
เรามี s ออร์บิทัลที่มีอิเล็กตรอนแค่ 1 ตัว
p ออร์บิทัลที่มีอิเล็กตรอน 1 ตัว
มันจะเหลือ p ออร์บิทัลแค่ 2 ตัว
p ออร์บิทัลแต่ละตัวมีอิเล็กตรอน 1 ตัวในนั้น
เรามีคาร์บอน วาเลนซ์อิเล็กตรอน 4 ตัว
แต่อันนี้ไม่ใช่ s ออร์บิทัลอีกต่อไป
เพราะเราได้ผสมมัน
กับ p ออร์บิทัล กลายเป็น sp ไฮบริดออร์บิทัล
อันนี้ไม่ใช่ p ออร์บิทัลอีกต่อไป
เพราะเราจะผสมมัน
เกิดเป็น sp ไฮบริดออร์บิทัล
อันนี้เรียกว่า sp ไฮบริดไดเซชัน
นี่คือ sp ไฮบริดไดเซชัน
เพราะไฮบริดออร์บิทัลของเรา
มาจาก s ออร์บิทัลหนึ่งตัว
กับ p ออร์บิทัลหนึ่งตัวอย่างนั้น
คาร์บอนนี่ตรงนี้คือ sp ไฮบริด

English: 
One, two, three and four
and we're looking for two hybrid orbitals
since carbon is bonded to two atoms.
We're going to take an S orbital.
We're gonna promote an S orbital
in terms of energy and
we're going to demote
a P orbital, only one P orbital this time.
We have an S orbital with one electron.
A P orbital with one electron.
That's gonna leave behind two P orbitals.
Each one of those P orbitals
has one electron in it.
We have carbons, four valence electrons
but this is no longer an S orbital
because we're going to hybridized it
with a P orbital to make
an SP hybrid orbital.
This is no longer a P orbital
because we're going to hybridize it
to form our SP hybrid orbital.
This is called SP hybridization.
This is SP hybridization
because our new hybrid orbitals
came from one S orbital
and one P orbital like that.
This carbon right here is SP hybridized

Bulgarian: 
един, два, три, четири.
Искаме да получим
две хибридни орбитали,
тъй като въглеродът е свързан
с два атома.
ще вземем s-орбиталата
и ще увеличим
нейната енергия,
а отгоре ще смъкнем
този път само една
p–орбитала.
Имаме s-орбитала
с един електрон.
Също и p-орбитала
с един електрон.
Остават още две
p-орбитали.
Всяка от тях също
има по един електрон.
Запазихме четирите
валентни електрона на въглерода,
но вече нямаме s-орбитала,
защото ще я хибридизираме
с една p-орбитала,
за да получим sp-хибридна орбитала.
Това вече няма да е p-орбитала,
защото ще бъде хибридизирана,
за да образува
sp-хибридна орбитала.
Това се нарича
sp-хибридизация.
Името идва от комбинирането
в новите хибридни орбитали
на една s-орбитала
и една p-орбитала.
Този въглероден атом
е sp-хибридизиран,

Portuguese: 
Um, dois, três e quatro
e estamos olhando por dois orbitais híbridos
porque este carbono está ligado a dois 
átomos.
Vamos pegar um orbital S.
Vamos promover o orbital S
em termos de energia e vamos reduzir
um orbital P, somente um orbital P 
desta vez.
Temos um orbital S com um elétron.
Um orbital P com um elétron.
Isso vai deixar para trás dois orbitais P.
Cada um destes orbitais P tem um elétron.
Temos carbonos, quatro elétrons de 
valência
mas isto não é mais um orbital S
porque vamos hibridizar ele
com um orbital P para fazer um orbital SP.
Isto não é mais um orbital P
porque vamos hibridizar ele
formar um orbital híbrido SP.
Isso é chamado hibridização SP.
Isto é hibridização SP
porque nosos novos orbitais
vieram de um orbital S
e um orbital P, assim.
Este carbono aqui tem hibridização SP

Bulgarian: 
тъй като е свързан с два атома,
другият въглероден атом
също е sp-хибридизиран.
Сега да помислим за формата
на новите sp-хибридни орбитали.
Трябва ми място за рисуване.
Да повторим: знаем, че
s-орбиталата има форма
на сфера.
Комбинираме една s-орбитала
с една p-орбитала,
която има форма на гиричка.
Хибридизираме тези две
орбитали,
за да получим две нови
хибридни орбитали.
Две sp-хибридни орбитали.
Сега ще нарисувам
sp-хибридна орбитала.
И тук, когато я изобразяваме,
ще пропускаме малката издутина.
Когато я използваме
за чертежа,
ще ни е достатъчна
по-голямата фронтална издутина.
Сега да намерим процентите
на s-характера.
Използвали сме една
s-орбитала и една p-орбитала.
Това означава, че имаме
50% s-характер
и 50% p-характер.
Тук s-характерът
е повече,
отколкото при предишните
хибридизации.
Във видеото за
sp³-хибридизацията

Thai: 
เพราะมันทำพันธะกับอะตอม 2 ตัว
คาร์บอนนี่ตรงนี้เป็น sp ไฮบริดเช่นกัน
ลองคิดถึงรูปร่างของ sp ไฮบริดออร์บิทัลกัน
ลองหาที่ว่างข้างล่างนี้
เหมือนเดิม เรารู้ว่า s ออร์บิทัลมีรูปร่าง
เหมือนทรงกลม
เรานำ s ออร์บิทัลมาหนึ่งตัว 
และเรานำ p ออร์บิทัลมาหนึ่งตัว
ซึ่งมีรูปร่างเหมือนดัมเบล
และเราผสมออร์บิทัล 2 ตัวนี้เข้าด้วยกัน
ได้เป็นไฮบริดออร์บิทัลใหม่ 2 ตัว
sp ไฮบริดออร์บิทัล 2 ตัว
ขอผมลงมือวาด 
sp ไฮบริดออร์บิทัลลงไปตรงนี้
เหมือนเดิม เราจะไม่สนใจก้อนเล็ก
เราจะไม่สนก้อนเล็ก
เมื่อเราวาดภาพ
คิดถึงแค่ก้อนใหญ่ข้างหน้าตรงนี้
เมื่อเราคิดถึงเปอร์เซ็นต์ของ s
เราใช้ s ออร์บิทัล 1 ตัวกับ p ออร์บิทัล 1 ตัว
นั่นหมายความว่ามันมีสมบัติ s อยู่ 50%
และ p อยู่ 50%
ตัวนี้มีความเป็น s
มากกว่าในวิดีโอก่อนๆ
ในวิดีโอเรื่อง sp3 ไฮบริดไดเซชัน

Portuguese: 
desde que ele está ligado a dois carbonos
e este carbono aqui também tem
hibridização SP.
Vamso pensar sobre a forma do nosso novo
orbital híbrido SP.
Vamos arrumar um pouco mais de espaço.
Mais uma vez, sabemos que o 
orbital S tem a forma
de uma esfera.
Pegamos um orbital S e um orbital P,
quem forma de lóbulos,
e nós hibridizamos esses dois orbitais
para formar novos orbitais híbridos.
Dois orbitais hibridizados SP.
Vou desenhar um orbital híbrido SP aqui
e mais uma vez vamos ignorar o lóbulo
menor.
Vamos ignorar o lóbulo menor.
Quando desenharmos,
pense somente no lóbulo frontal maior 
aqui.
Quando eu penso sobre a porcentagem de 
caráter S.
Usamos um orbital S e um orbital P.
Isso significa 50% de caráter S
e 50% de caráter P
e esse tem mais caráter S
que em vídeos anteriores.
No vídeo sobre hibridização SP3,

English: 
since it bonded to two atoms
and this carbon right here
is also SP hybridized.
Let's think about the shape
of our new SP hybrid orbitals.
Let's get a little bit of room down here.
Once again, we know an S orbital shaped
like a sphere.
We took one S orbital and
we took one P orbital,
which is shaped like a dumbbell
and we hybridized these
two orbitals together
to give us two new hybrid orbitals.
Two SP hybrid orbitals.
Let me go ahead and draw in
an SP hybrid orbital here
and once again, we're going
to ignore the small lobe.
We're going to ignore the small lobe.
When we draw our picture,
only think about this
bigger frontal lobe here.
When I think about the
percentage of S character.
We use one S orbital and one P orbital.
That means it's 50% S character
and 50% P character
and this is more S character
than in the previous videos.
On the video on SP3 hybridization,

Bulgarian: 
говорехме за 25% s-характер,
при sp²-хибридизацията
имахме около 33% s-характер,
а в тези хибридни орбитали тук
имаме още повече
s-характер,
достигащ до 50%
и тъй като електронната плътност
на една s-орбитала
е с по-голяма плътност
в по-голяма близост до ядрото,
отколкото при
p–орбиталата,
това означава, че тази издутина
има по-голяма
електронна плътност
по-близо до ядрото,
което обяснява защо
атомните връзки
стават все по-къси,
когато се увеличава s-характерът.
Общото правило гласи,
че с увеличаване на s-характера
се получават по-близки връзки,
тъй като хибридните орбитали
стават по-малки.
Да се върнем на формулата
на етина (ацетилена).
Да опитаме да начертаем
формата му.
Знаем, че и двата
въглеродни атома
в ацетилена са
sp-хибридизирани.
Да се върнем тук долу
и да начертаем набързо
структурната формула.
Имаме ацетилен.
Два атома въглерод,
свързани чрез тройна връзка.

Portuguese: 
falamos de 25% de caráter S.
No vídeo sobre hibridização SP2,
falamos de 33% de caráter S
e para estes orbitais híbridos,
o cáráter S é ainda maior,
até 50% e desde que a densidade eletrônica
do orbital S é maior
do que a de um orbital P
perto do núcleo,
isso significa que esse lóbulo aqui tem 
uma
densidade eletrônica maior perto do 
núcleo,
que é uma maneira de pensar sobre porque
estas ligações
ficam menor a medida que o caráter S a
umenta.
Em geral, a medida que o caráter S aumenta,
você obtêm ligações menores
porque você tem orbitais híbridos menores.
Vamos votar à figura do acetileno.
kkk
Quero desenhá-la.
Sabemos como estes dois carbonos
no acetileno são hibridizados SP.
Vamos voltar aqui,
e eu vou desenhar uma estrutura de Lewis 
rapidamente.
Temos acetileno aqui.
Temos carbono triplamente ligado a outro
carbono.

Thai: 
เราพูดถึงความเป็น s 25%
วิดีโอเรื่อง sp2 ไฮบริดไดเซชัน
เราพูดถึงความเป็น s 33%
แล้วสำหรับไฮบริดออร์บิทัลนี้
เรามีความเป็น s มากกว่าเดิมอีก
มากถึง 50% และเนื่องจาก
ความหนาแน่นอิเล็กตรอน
สำหรับ s ออร์บิทัลเพิ่มขึ้น 
ความหนาแน่นอิเล็กตรอน
จะเข้าใกล้นิวเคลียสยิ่งขึ้น สำหรับ s ออร์บิทัล
เทียบกับ p ออร์บิทัล
นั่นหมายความว่า ก้อนนี้มีความหนาแน่น
ใกล้นิวเคลียสยิ่งขึ้น
ซึ่งก็คือวิธีคิดอย่างหนึ่งว่าทำไมพันธะเหล่านี้
จึงสั้นลงเมื่อคุณเพิ่มลักษณะของ s
โดยทั่วไป เมื่อคุณเพิ่มความเป็น s
คุณจะได้พันธะที่สั้นลง
เพราะคุณมีไฮบริดออร์บิทัลที่เล็กลงตรงนี้
ลองกลับไปดูภาพ
อเซธิลีนกัน
ผมอยากลองดูว่าจะวาดได้ไหม
ตอนนี้เรารู้ว่าคาร์บอนทั้งสองตัว
ในอเซธิลีนเป็น sp ไฮบริด
ลองไปข้างล่างตรงนี้
ขอผมวาดโครงสร้างจุดเร็วๆ นะ
เรามีอเซธิลีนตรงนี้
เรามีคาร์บอนทำพันธะสามกับคาร์บอนอีกตัว

English: 
we're talking about 25% S character
The video on SP2 hybridization,
we talked about 33% S character
and then for these hybrid orbitals,
we have even more S character,
up to 50% and since the electron density
for an S orbital is
increased electron density
closer to the nucleus for an S orbital
than for a P orbital,
that means that this lobe
here has an increased
electron density closer to the nucleus,
which is one way to think
about why these bonds
get shorter as you
increase in S character.
In general, as you
increase in S character,
you're going to get shorter bonds
because you have smaller
hybrid orbitals here.
Let's go back up here to this picture
of acetylene.
I wanna see if we can draw it.
We now know that both of these carbons
in a acetylene are SP hybridized.
Let's go back down here
and let me draw up a dot
structure really fast.
We have acetylene here.
We have carbon triple
bonded to another carbon.

Thai: 
เรารู้ว่าคาร์บอนแต่ละตัวเป็น sp ไฮบริด
ถ้าคาร์บอนแต่ละตัวเป็น sp ไฮบริด
คาร์บอนแต่ละตัวจะมี sp ไฮบริดออร์บิทัล 2 ตัว
เราก็ลงมือวาด sp ไฮบริดออร์บิทัล 1 อันได้
เหมือนเดิม ผมจะไม่คิดก้อนหลังอันเล็ก
นี่คือ sp ไฮบริดออร์บิทัลอีกตัวของคาร์บอนนี้
ขอผมกลับไปดูแผนภาพของเราอีกครั้ง
คาร์บอนแต่ละตัว เราใช้สีแดงสำหรับตัวนี้
คาร์บอนแบบ sp ไฮบริดแต่ละตัว
มี sp ออร์บิทัล
ที่มีอิเล็กตรอนหนึ่งตัวในนั้น
และเราใส่มันตรงนี้
แล้วมันมีอีกตัว
มี sp ไฮบริดออร์บิทัลอีกตัว
ที่มีวาเลนซ์อิเล็กตรอนหนึ่งตัวในนั้น
ผมจะใส่อิเล็กตรอนอีกตัวตรงนี้
ในไฮบริดออร์บิทัลนี้
แล้ว สังเกตว่า ถ้าคุณคิดคาร์บอน sp ไฮบริด
คุณจะมี p ออร์บิทัล 2 อันด้วย
p ออร์บิทัลที่ไม่ใช่ไฮบริด 2 อัน
p ออร์บิทัลแต่ละอัน
มีวาเลนซ์อิเล็กตรอนหนึ่งตัว
ขอผมไปข้างล่างตรงนี้
และผมจะวาด

English: 
We know each of those
carbons as SP hybridized.
If each of those carbons is SP hybridized,
each carbon has two SP hybrid orbitals.
We go ahead and draw in
one SP hybrid orbital.
Again, I'm ignoring the smaller back lobe
and here's our other SP
hybrid orbital on this carbon.
Let me go back and look
at our diagram again.
Each carbon, we use red for this.
Each SP hybridized
carbon has an SP orbital
with one valence electron in it
and we put that in here
and then there's another one.
There's another SP hybrid orbital
with one valence electron in it.
I'm gonna go ahead and put
the other electron over here
in this hybrid orbital.
Also, notice, if you're
dealing with an SP hybridized
carbon, you also have two P orbitals.
Two unhybridized P orbitals.
Each P orbital with a valence electron.
Let me go back down here
and I'm gonna draw in.

Bulgarian: 
Знаем, че всеки от тях
е в sp-хибридно състояние.
Тъй като всеки въглерод
е sp-хибридизиран,
то всеки има по две
sp-хибридни орбитали.
Ще нарисувам първата
sp-хибридна орбитала.
Пропускам по-малката
издутина.
Ето и другата sp-хибридна
орбитала на този въглерод.
Да погледнем отново
графиката.
Всеки въглероден атом,
ще отбелязвам с червено,
в sp-хибридно състояние
има тази sp-орбитала
с един валентен електрон
в нея,
нарисували сме я,
после има още
една такава:
втора sp-хибридна орбитала
с един валентен електрон
в нея.
Ще отбележа и другия електрон
в неговата хибридна орбитала.
Забележи също, че в случая
на sp-хибридизиран
въглероден атом
остават и две p-орбитали.
Две нехибридни
p-орбитали.
Всяка p-орбитала е с по един
валентен електрон.
Сега ще начертая
и тях.

Portuguese: 
Sabemos cada carbono tem hibridização SP.
Se cada um destes carbono tem hibridização
SP,
cada carbono tem dois orbitais híbridos 
SP.
Vamos desenhar um orbital híbrido SP.
Novamente, estou ignorando o lóbulo menor 
de trás
e aqui está outro orbital híbrido neste 
carbono.
Vou olhar no nosso diagrama de novo.
Cada carbono, usamos vermelho para isto.
Cada carbono hibridizado SP tem um 
orbital SP
com um elétron de valência
e nós colocamos aquilo aqui,
e então tem outro.
Tem orbital híbrido SP
com um elétron de valência.
Vou colocar os outros elétrons aqui
neste orbital híbrido.
Note que se você está mexendo com um 
orbital de carbono
hibridizado SP, você também tem dois 
orbitais P.
Dois orbitais P não hibridizados.
Cada orbital P com um elétron de valência.
Vou voltar aqui
e vou desenhar.

Portuguese: 
Aqui está um orbital P.
Alí está um orbital P com um elétrons de
valência
e alí tem outro orbital P
com o outro elétron de valência.
Agora temos nossa figura de um carbono
hibridizado SP.
Vamos dizer que isso é este carbono
a esquerda.
Agora vamos desenhar este carbono
a direita.
Este carbono a direita também tem 
hibridização SP.
Então, este carbono a direita
tem um orbital híbrido SP
com um elétron de valência aqui
e então outro orbital híbrido SP
com um elétron de valência aqui.
Este carbono, é hibridizado SP.
Mais uma vez, vamos voltar aqui para este
diagrama.
Este carbono também vai ter
um orbital P com um eléron de valência
e outro orbital P com outro elétron de
valência.
Vamos voltar aqui
e desenhar aquele orbitais P.
Aqui está outro orbital P.
Aqui está outro orbital P com um elétron
de valência
e alí está outro orbital P
com um elétron aqui assim.

English: 
here's one P orbital.
There's one P orbital
with one valence electron
and there here's another
P orbital right here
with another one of
those valence electrons.
Now, we have our picture
of an SP hybridized carbon.
Let's say that was this carbon over here
on the left.
Now, let's go ahead
and draw in this carbon
on the right.
This carbon on the right
is also SP hybridized.
Therefore, this carbon on the right
has an SP hybrid orbital
with one valence electron in here
and then another SP hybrid orbital
with one valence electron here.
This carbon, it's SP hybridized.
Once again, go back up
here to this diagram.
This carbon is also going to have
a P orbital with a valence electron
and another P orbital with
another electron in it.
Go back down to here
and we draw in those P orbital.
Here is one P orbital.
Here is one P orbital
with one valence electron
and there here's another P orbital
with an electron in here like that.

Thai: 
นี่คือ p ออร์บิทัล
มี p ออร์บิทัลหนึ่งอัน
ที่มีวาเลนซ์อิเล็กตรอนหนึ่งตัว
และมี p ออร์บิทัลอีกตัวตรงนี้
ที่มีวาเลนซ์อิเล็กตรอนอีกตัวหนึ่ง
ทีนี้ เรามีภาพคาร์บอน sp ไฮบริดแล้ว
สมมุติว่านั่นคือคาร์บอนนี่ตรงนี้
ทางซ้าย
ทีนี้ ลองวาดคาร์บอนนี้
ทางขวา
คาร์บอนทางขวานี้เป็น sp ไฮบริดเช่นกัน
เพราะฉะนั้น คาร์บอนนี้ทางขวา
มี sp ไฮบริดออร์บิทัล
และวาเลนซ์อิเล็กตรอนหนึ่งตัวในนั้น
แล้ว sp ไฮบริดออร์บิทัลอีกอัน
มีวาเลนซ์อิเล็กตรอนหนึ่งตัวตรงนี้
คาร์บอนนี้ มันคือ sp ไฮบริด
เหมือนเดิม กลับไปที่แผนภาพนี้
คาร์บอนจะมี
p ออร์บิทัลกับวาเลนซ์อิเล็กตรอนหนึ่งตัว
แล้วก็ p ออร์บิทัลพร้อม
วาเลนซ์อิเล็กตรอนหนึ่งตัวในนั้นอีกอัน
ไปข้างล่างตรงนี้
เราวาด p ออร์บิทัลพวกนั้น
นี่คือ p ออร์บิทัลหนึ่งอัน
นี่คือ p ออร์บิทัลหนึ่งอันที่มี
วาเลนซ์อิเล็กตรอนหนึ่งตัว
และนี่คือ p ออร์บิทัลอีกตัว
ที่มีอิเล็กตรอนในนั้นอย่างนั้น

Bulgarian: 
Ето една p-орбитала.
Тя има един
валентен електрон;
ето и другата
p-орбитала
с още един
валентен електрон.
Това е илюстрация
на sp-хибридизиран въглерод.
Да речем, че това е
левият въглероден атом
от формулата.
Сега да нарисуваме
и десният въглероден
атом.
Той също е
sp-хибридизиран.
Следователно и той има
sp-хибридна орбитала
с един валентен електрон,
после още една
sp-хибридна орбитала
с един валентен електрон.
Все пак, този въглерод
е sp-хибридизиран.
Да си припомним
графиката:
този атом ще има също и
p-орбитала
с валентен електрон
и още една p-орбитала
с още един електрон в нея.
Сега да нарисуваме
и тези p-орбитали.
Това е едната,
с нейния електрон,
а това е другата p-орбитала
с един електрон в нея.

Thai: 
สุดท้าย เราต้องเพิ่มไฮโดรเจน
เรามีไฮโดรเจนแต่ละด้านตรงนี้
เรารู้ว่าไฮโดรเจนมีวาเลนซ์อิเล็กตรอนหนึ่งตัว
ใน s ออร์บิทัลที่ไม่ใช่ไฮบริด
ตรงนี้ เรามีไฮโดรเจน
ที่มีวาเลนซ์อิเล็กตรอนหนึ่งตัว
ใน s ออร์บิทัลที่ไม่ใช่ไฮบริด
ตอนนี้ เราวิเคราะห์พันธะ
ที่มีอยู่ได้ในที่สุด
เรารู้ว่าถ้าเรามีการซ้อนทับของออร์บิทัลตรงๆ
อย่างตรงนี้
นั่นคือพันธะซิกม่า
มันมีพันธะซิกม่าหนึ่งอัน
นี่คือการซ้อนทับตรงหน้าของออร์บิทัล
ระหว่างคาร์บอนสองตัว
นั่นคือพันธะซิกม่า
แล้วสุดท้าย เรามีการซ้อนทับตรงๆ
ของออร์บิทัลตรงนี้
นั่นคือพันธะซิกม่าอีกตัว
มีพันธะซิกม่าทั้งหมด 3 ตัว
ในอเซธีลีนโมเลกุล
วิดีโอเรื่อง sp2 ไฮบริดไดเซชัน
เราเห็นวิธีสร้างพันธะพายไป
เรามีการซ้อนทับของออร์บิทัลข้างๆ
ตรงนี้เรามีพันธะพาย 1 อัน
เรามีอันตรกิริยาข้างบนและข้างล่าง
นั่นคือพันธะพายหนึ่งอัน
แล้วเรามีพันธะพายอีกหนึ่งอันตรงนี้

Bulgarian: 
И накрая остана
да добавим водорода.
Имаме по един водороден
атом от двете страни.
Знаем, че водородът
има един валентен електрон
в нехибридна s-орбитала.
Отбелязвам и втория
водороден атом
с един валентен електрон
в нехибридната му s-орбитала.
Вече можем да анализираме
връзките.
Знаем, че когато
орбиталите се срещат челно,
както е тук,
това е сигма-връзка.
Тук имаме една
сигма-връзка.
Тук също има челно
припокриване на орбитали
между двата
въглеродни атома.
Това също е сигма-връзка.
И тук също има
челно припокриване
на орбитали.
Това е още една
сигма-връзка.
Общо има
три сигма-връзки
в молекулата на ацетилена
(етина).
Във видеото за sp²-хибридизацията
видяхме как се образува
пи-връзка.
При нея орбиталите
се припокриват странично.
Тук имаме една пи-връзка.
Имаме взаимодействия
отгоре и отдолу.
Това е едната пи-връзка,
а това е другата по-връзка.

Portuguese: 
Finalmente, temos que adicionar 
hidrogênio.
Temos que adicionar hidrogênio em ambos
os lados.
Sabemos que hidrogênio te um elétron de
valência
e um orbital S não hibridizado.
Aqui, temos um hidrogênio
com um elétron de valência em um orbital S
não hibridizado.
Agora, podemos finalmente analizar a 
ligação
que está presente.
Sabemos que se os orbitais se sobrepõe
frontalmente
como aqui.
Isso é uma ligação sigma.
Alí está uma ligação sigma.
Aqui ocorre a sobreposição dos
orbitais dos dois carbonos.
Isso é uma ligação sigma.
E ocorre outra sobreposição frontal
dos orbitais aqui.
Aquela é outra ligação sigma.
Dando um total de três ligações sigmas
na molécula de acetileno.
No vídeo sobre hibridização SP2,
vimos como formar uma ligação pi.
Nós temos esta sobreposição lateral 
de orbitais.
Aqui temos uma ligação pi.
Temos interação acima e abaixo.
Esta é uma ligação pi
e então temos outra ligação pi aqui.

English: 
Finally, we have to add in hydrogen.
We have a hydrogen on either side here.
We know that hydrogen
has one valence electron
in an unhybridized S orbital.
Over here, we have a hydrogen
with one valence electron
in unhybridized S orbital.
Now, we can finally analyze the bonding
that's present.
We know that if we have
head on overlap of orbitals
like right in here.
That's a sigma bond.
There's one sigma bond.
Here's a head on overlap of orbitals
between our two carbons.
That's a sigma bond.
Then finally, we have a head on overlap
of orbitals here.
That's another sigma bond.
With a total of three sigma bonds
in the acetylene molecule.
The video on SP2 hybridization,
we saw how to make a pi bond.
We had this side by side
overlap of orbitals.
Here we have one pi bond.
We have interaction above and below.
That's one pi bonds
and then we have another pi bond here.

Portuguese: 
Temos sobreposição lateral dos orbitais 
aqui
também e então temos duas ligações pi
presentes.
Temos duas ligações pi presentes
na molécula de acetileno.
Vamos olhar nossa esturura de Lewis de 
novo.
Nós vimos que a ligação entre este carbono
e este hidrogênio era uma ligação sigma.
Vimos que havia uma ligação sigma
entre os dois carbonos.
Vou pegar a do meio aqui.
Isso é uma ligação sigma
e essa ligação aqui
também é uma ligação sigma.
Essas são nossas três ligações sigmas
e nós temos uma ligaçãos tripa presente.
Também havia duas ligações pi presentes.
Duas dessas são ligações pi aqui.
Um total de duas ligações pi
e três ligações sigma
para a molécula de acetileno aqui.
Lembre-se que ligação pi impede a rotação.
Não podemos rotacionar em volta da ligação
sigma
entre esses dois carbonos por causa da 
ligação pi.
Não tem rotação
na nossa ligação tripla.
Temos uma forma linear.
Vou desenhar aquela linha aqui.

English: 
We have side by side
overlap of orbitals here
as well and so we have
two pi bonds present.
We have two pi bonds present
in the acetylene molecules.
Let's look at our dot structure again.
We saw the bond between this carbon
and this hydrogen was a sigma bond.
We saw there was one sigma bond
between our two carbons.
I'm just gonna pick the
one on the middle here.
Say that's a signal bond
and then this bond over here
we said was a sigma bond.
There's our three sigma bonds
and then we have a triple bond presence.
There were two pi bonds also present.
Two of these are pi bonds here.
A total of two pi bonds
and three sigma bonds
for the acetylene molecule here.
Remember pi bonds prevent free rotation.
We can't rotate about the sigma bond
between the two carbons
because of the pi bonds.
There's no free rotation
for our triple bond.
We have a linear shape.
Let me go ahead and
draw that line in here.

Bulgarian: 
Тук има странично
припокриване на орбитали,
стават общо 2
пи-връзки.
В молекулата на ацетилена
има две пи-връзки.
Да погледнем отново
структурната формула.
Видяхме, че връзката
между този въглероден атом
и този водороден атом
е сигма-връзка.
Видяхме още една сигма връзка
между двата въглеродни атома.
Ще отбележа
чертичката по средата
като сигма-връзка.
И накрая и тази връзка тук
също е сигма-връзка.
Това са нашите три
сигма-връзки.
Но тук имаме
тройна връзка.
В нея са и двете
пи-връзки.
Две от тези три
са пи-връзки.
Общо имаме две
пи-връзки
и три
сигма-връзки
в молекулата на ацетилена.
Помни, че пи-връзките
пречат на свободното въртене.
Не можем да завъртим
около тройната връзка
двата въглеродни атома
поради пи-връзките.
Тройната връзка
не позволява въртене.
Имаме линейна геометрия.
Ще начертая права линия,

Thai: 
เรามีการซ้อนทับด้านข้างของออร์บิทัลตรงนี้
เช่นกัน เราจึงมีพันธะพาย 2 อัน
เรามีพันธะพาย 2 อัน
ในโมเลกุลอเซธิลีน
ลองดูโครงสร้างจุดอีกครั้ง
เราเห็นพันธะระหว่างคาร์บอนนี้
กับไฮโดรเจนนี้ว่าเป็นพันธะซิกม่า
เราเห็นว่ามีพันธะซิกม่าหนึ่งอัน
ระหว่างคาร์บอนสองตัว
ผมแค่เลือกอันตรงกลางนี้
บอกว่ามันคือพันธะซิกม่า
และพันธะนี่ตรงนี้
เราบอกว่ามันคือพันธะซิกม่า
มีพันธะซิกม่า 3 อัน
แล้วเรามีพันธะสามอยู่
มีพันธะพาย 2  อัน
2 ตัวนั้นเป็นพันธะพาย
พันธพายทั้งหมด 2 อัน
และพันธะซิกม่า 3 อัน
สำหรับโมเลกุลอเซธิลีนตรงนี้
นึกดู พันธะพายป้องกันการหมุนอิสระ
เราหมุนรอบพันธะซิกม่า
ระหว่างคาร์บอนสองตัวไม่ได้เพราะพันธะบาย
มันไม่มีการหมุนอิสระ
ในพันธะสาม
เรามีรูปร่างแบบเส้นตรง
ขอผมวาดเส้นตรงในนี้

Bulgarian: 
за да изразя
линейната геометрия
на молекулата.
Сега да видим
дължинитие на връзките.
Разстоянието между
тези два въглеродни атома,
ще ги отбележа
с очертаване;
Разстоянието между
двата въглеродни атома
възлиза на приблизително
1,20 ангстрьома.
Това е по-близка връзка,
отколкото в предишните видеа.
Това се дължи на по-големия
s-характер.
По-големият s-характер
води до по-малки орбитали,
така можем да си представим
и по-малкото
разстояние
на връзката
при тройната връзка
в сравнение с двойната
или с единичната връзка.
Дотук покрихме доста материал.
Сега можем да начертаем
структурната формула
още веднъж и да я анализираме
чрез стеричното число.
Имаме тройна връзка.
Ще използваме стеричното число
за намиране
на типа хибридизирано
състояние.
Знаем как се намира
стеричното число:
взимаме броя сигма-връзки,

English: 
You see there's linear geometry
for this molecule like that.
Also in terms of bond length.
The distance between these two carbons.
The distance between this carbon
and this carbon, let me circle them.
The distance between these two carbons
turns out to be
approximately 1.20 angstroms.
An even shorter bond length
than in our previous videos.
Once again, that's due to
the increased S character.
Increased S character gives
you these smaller orbitals
and that's one way to think
about the shorter bond distance
and the triple bond
compared to a double bond
or a single bond.
That's a lot that we've covered here.
Let's go ahead and draw the dot structure
one more time and analyze
it using steric number.
We have our triple bonds.
If we're doing steric number to find out
the hybridization state,
we know to do steric number,
you take the number of sigma bonds.

Thai: 
คุณเห็นว่าเรขาคณิตเป็นเชิงเส้น
สำหรับโมเลกุลอย่างนั้น
แล้วในแง่ของความยาวพันธะ
ระยะระหว่างคาร์บอนสองตัวนี้
ระยะระหว่างคาร์บอนตัวนี้
กับคาร์บอนตัวนี้ ขอผมวงกลมมันนะ
ระยะระหว่างคาร์บอนสองตัวนี้
ปรากฏว่าประมาณเท่ากับ 1.20 อังสตรอม
ความยาวพันธะสั้นกว่าในวิดีโอที่แล้วอีก
ย้ำอีกครั้ง มันเป็นเพราะความเป็น s เพิ่มขึ้น
ลักษณะของ s มากขึ้น ทำให้คุณได้
ออร์บิทัลเล็กลง
นั่นคือวิธีคิด
ถึงระยะพันธะที่สั้นลงอย่างหนึ่ง
พันธะสามเทียบกับพันธะคู่
หรือพันธะเดี่ยว
เราพูดถึงเรื่องต่างๆ มากมาย
ลองวาดโครงสร้างจุด
อีกครั้ง และวิเคราะห์โดยใช้เลขสเตอริกกัน
เรามีพันธะสาม
ถ้าเราคิดเลขสเตอริกเพื่อหา
สถานะไฮบริดไดเซชัน
เรารู้เลขสเตอริก
คุณนำจำนวนพันธะซิกม่ามา

Portuguese: 
Você vê uma geometria linear
para esta molécual assim
Em termos de comprimento de ligação.
A distância entre esses dois carbonos.
A distância entre este carbono
e este carbono, vou circular eles.
A distância entre estes dois carbonos
é aproximadamente 1,20 angstroms.
Um comprimento de ligação ainda menor que 
nos vídeos anteriores.
Mais uma vez isso é devido ao maior 
caráter S.
Elevado caráter S dá orbitias menores
este é um jeito de pensar
em comprimento de ligações menores
da ligação tripla comparado com a 
ligação dupla
ou a ligação simples.
Cobrimos muita coisa aqui.
Vamos desenhar a estrutura de Lewis
mais uma vez e analizar usando número
estérico.
Temos nossa ligação tripla.
Se vamos usar número estérico para
descobrir
o estado de hibridização,
para calcular número estérico,
você pega o número de ligações sigmas.

Thai: 
สมมุติว่าเป้าหมายของเราคือหา
เลขสเตอริกของคาร์บอนตัวนี้
จำนวนพันธะซิกม่า
ผมรู้ว่านี่คือพันธะซิกม่า
ผมรู้ว่าพันธะสาม
ผมมีพันธะซิกม่า 1 ตัวกับพันธะพาย 2 ตัว
มีพันธะซิกม่า 2 ตัวตรงนี้
และอิเล็กตรอนคู่โดดเดี่ยว 0 คู่
2 บวก 0 ให้ค่าเป็น 2
ผมต้องมีไฮบริดออร์บิทัล 2 ตัว
ซึ่งคุณสร้างจาก s ออร์บิทัลหนึ่งตัว
กับ p ออร์บิทัลหนึ่งตัว
ถ้าคุณได้เลขสเตอริกเป็น 2
คุณก็คิดถึง sp ไฮบริดไดเซชัน
คาร์บอนนี้เป็น sp ไฮบริด
คาร์บอนตัวนี้ก็เช่นกัน
นั่นคือวิธีคิดโดยใช้เลขสเตอริก
เหมือนเดิม เรขาคณิตเชิงเส้นที่มีมุมพันธะ
เป็น 180 องศา
ลองทำตัวอย่างการใช้เลขสเตอริก
เพื่อวิเคราะห์โมเลกุลอีกกัน
ลองคาร์บอนไดออกไซด์บ้าง
ถ้าเราอยากหาไฮบริดไดเซชัน
ของคาร์บอนตรงนั้น
ลองลงมือทำกัน
โดยใช้เลขสเตอริก
ไฮบริดไดเซชันของคาร์บอนนี้

Bulgarian: 
ще направим примера
с първия въглероден атом,
броят на неговите
сигма-връзки
е една от тук,
още една
от тройната връзка,
където има и две
пи-връзки.
Имаме общо две
сигма-връзки
и никакви свободни
електронни двойки.
Две плюс нула прави две.
Значи нужните
хибридни орбитали са две.
Те се състоят от една
s-орбитала
и една p-орбитала.
Когато се получи
стерично число, равно на 2,
това говори за
sp-хибридизация.
Този въглероден атом
е sp-хибридизиран.
Също и другият
въглероден атом.
Така прилагаме
стеричното число.
Геометрията е линейна
с ъгъл на връзката
180 градуса.
Да направим още един пример
със стерично число
за анализ на молекулата.
Да вземем молекулата
на въглеродния диоксид.
Да определим
типа хибридизация
на въглерода в нея.
Като използваме
стеричното число,
ще разберем типа хибридизация
на този въглероден атом.

Portuguese: 
Digamos que o objetivo é descobrir
o número estérico deste carbono.
O número de ligações sigmas.
Sei que isto é uma ligação sigma.
Sei que em uma ligação tripla,
eu tenho uma ligação pi e duas 
ligações pi.
Tem duas ligações sigmas aqui
e nenhum par isolado de elétrons.
Dois mais zero dá dois.
Eu preciso de dois orbitais híbridos.
Os quais você faz de um orbital S
e um orbital P.
Se obter um número estérico dois,
você pensa hibridização SP.
Este carbono é hibridizado SP,
e este carbono também.
Isso é como pensar sobre isso usando
número estérico.
Mais uma vez, uma geometria linear com
ângulo de ligação
de 180 graus.
Vamos fazer mais um exemplo usando número
estérico
para analizar a molécula.
Vamos fazer dióxido de carbono.
Nós queremos descobrir a hibriização
daquele carbono.
Vamos fazer isso.
Usando número estérico.
A hibridização deste carbono.

English: 
Let's say our goal was to figure out
the steric number for this carbon.
The number of sigma bonds.
I know this is a sigma bond.
I know on a triple bond,
I have one sigma bond and two pi bonds.
There are two sigma bonds here
and zero lone pairs of electrons.
Two plus zero gives me two.
I need two hybrid orbitals.
Which you make from one S orbital
and one P orbital.
If you get a steric number of two,
you think SP hybridization.
This carbon is SP hybridized
and so is this carbon as well.
That's how to think about
it using steric number.
Once again, a linear
geometry with a bond angles
of 180 degrees.
Let's do one more example
using steric number
to analyze the molecule.
Let's do carbon dioxide.
If we wanted to figure
out the hybridization
of the carbon there.
Let's go ahead and do that.
Using steric number.
The hybridization of this carbon.

Czech: 
Až se toto vvideo přeloží, je třeba ho přidat na KŠ místo tohoto: https://khanovaskola.cz/video-editor/?videoId=1704

Portuguese: 
O número estérico é igual ao número
de ligações sigmas.
Se eu focar na ligação dupla
entre estes oxigênios e este carbono,
eu sei que um destas ligações é uma
ligação sigma
do vídeos anterior.
Eu tenho uma ligação sigma aqui
e então para esta outra ligação dupla a
direita,
eu sei que uma dela é uma ligação sigma.
Eu tenho duas ligações sigmas aqui
e nenhum par isolado de elétrons
em volta do carbono.
Dois mais zero dá um número estérico dois.
Eu preciso de dois orbitais híbridos para
aquele carbono
e isto significar que este carbono
tem hibridização SP.
Este carbono aqui tem hibridização SP 
também
e então sabemos que isso é uma molécula
linear
com um ângulo de ligação de 180 graus.
Mais uma vez, o número estérico é apenas
um jeito
de analizar a hibridização
e também a geometria da molécula.
No próximo vídeo vamos ver alguns
exemplos de moléculas orgânicas
em diferentes estados de hibridização.
[Legendado por: Daniela Dering]

Thai: 
เลขสเตอริกเท่ากับจำนวน
พันธะซิกม่า
ถ้าผมสนใจพันธะคู่
ระหว่างออกซิเจนตัวหนึ่งกับคาร์บอนนี้
ผมรู้ว่าพันธะตัวหนึ่งจะเป็นพันธะซิกม่า
จากวิดีโอที่แล้ว
ผมมีพันธะซิกม่าหนึ่งตัวตรงนี้
แล้วสำหรับพันธะคู่อีกตัวทางขวานี้
ผมรู้ว่าตัวหนึ่งเป็นพันธะซิกม่า
ผมมีพันธะซิกม่า 2 ตัวตรงนี้
และอิเล็กตรอนคู่โดดเดี่ยว 0 คู่
รอบคาร์บอน
2 บวก 0 ให้เลขสเตอริกเป็น 2
ผมต้องการไฮบริดออร์บิทัล 2 ตัว
จากคาร์บอนนั้น
และแน่นอน มันหมายความว่าคาร์บอนนี้
เป็น sp ไฮบริด
คาร์บอนนี่ตรงนี้เป็น sp ไฮบริดเช่นกัน
เพราะฉะนั้น เรารู้ว่านี่คือโมเลกุลเชิงเส้น
ที่มีมุมพันธะ 180 องศา
ย้ำอีกครั้ง เลขสเตอริกเป็นวิธีที่ดี
เพื่อวิเคราะห์ไฮบริดไดเซชัน
และเรขาคณิตของโมเลกุล
ในวิดีโอหน้า เราจะดู
ตัวอย่างโมเลกุลอินทรีย์
ที่มีสถานะไฮบริดไดเซชันต่างๆ กัน

English: 
The steric number is equal to the number
of sigma bonds.
If I focus in on the double bond
between one of these
oxygens in this carbon,
I know that one of these
bonds is a sigma bond.
from our previous video.
I have one sigma bond here
and then for this other
double bond on the right,
I know that one of them is a sigma bond.
I have two sigma bonds here
and zero lone pairs of electrons
around the carbon.
Two plus zero gives me
a steric number of two.
I need two hybrid orbitals for that carbon
and of course, that must mean this carbon
is SP hybridized.
This carbon here is SP hybridized as well
and therefore, we know that
this is a linear molecule
with a bond angle of 180 degrees.
Once again, steric
number is just a nice way
of analyzing the hybridization
and also the geometry of the molecule.
In the next video, we'll look at a couple
of examples of organic molecules
in different hybridization states.

Bulgarian: 
Стеричното число
е равно на броя на сигма-връзките
плюс този на свободните
електронни двойки.
Да погледнем двойната връзка
между единия кислороден
и въглеродния атом.
Знаем, че едната от тези връзки
е сигма-връзка,
видяхме в предното видео.
И така, оттук имам
една сигма-връзка
и от другата двойна връзка
имам още една сигма-връзка.
Общо стават две
сигма-връзки.
Свободните електронни двойки
около въглеродния атом
са нула.
Две плюс нула дава
стерично число, равно на 2.
Ще са нужни две
хибридни орбитали за въглерода.
Това, разбира се, означава,
че този въглероден атом
е sp-хибридизиран.
Означавам и него
като sp-хибридизиран.
От това следва,
че тази молекула е линейна
с ъгъл на връзката
от 180 градуса.
Да обобщим: стеричното число
е един удобен начин
за анализ
както на хибридизацията,
така и на геометрията
на молекулата.
В следващото видео
ще видим няколко примера
за органични молекули
в различни състояния
на хибридизация.
