
Bulgarian: 
Вече разгледахме електронните конфигурации за калий и калций,
но нека много бързо да го направим отново,
понеже те ще повлияят на начина ни на мислене за d орбиталите.
Намираме калия, който е в четвъртия период на периодичната таблица.
Ако използваме обозначението с благороден газ, за да спестим малко време,
работим назад и първият благороден газ, на който попадаме,
е аргон и затова пишем аргон в скоби.
Знаем, че аргонът има 18 електрона, а калият има 19 електрона.
Калият има с един повече електрон от аргона
и поставяме допълнителния електрон в 4s орбитала,
понеже за калия 4s орбиталата е с по-ниска енергия от 3d орбиталите.
Имаме увеличаваща се енергия
и този електрон влиза в 4s орбитала,
така че пълната електронна конфигурация за калия,
като използваме обозначение с благороден газ,
е аргон в скоби 4s1.
Всъщност трябва да кажа за калция.

English: 
- [Voiceover] We've already looked at the
electron configurations for
potassium and for calcium
but let's do it again really quickly
because it's going to
affect how we think about
the d orbitals and so we find potassium
which is in the fourth
period on the periodic table.
If we do noble gas
notation to save some time,
we work backwards and the
first noble gas we hit
is argon, so we write argon in brackets.
We know argon has 18 electrons
and potassium has 19 electrons.
Potassium has one more electron than argon
and so we put that extra
electron into a 4s orbital
because for potassium the 4s orbital
is lower energy than the 3d orbitals here.
We have increasing energy
and that electron goes into a 4s orbital
so the complete electron configuration
using noble gas notation for potassium
is argon in brackets 4s 1.
For calcium I should say.

Korean: 
우리는 이미
K 와 Ca 의 전자배치를 알아보았지만
다시 간단하게 복습해봅시다
d 오비탈에 관해
생각할 때 필요하기 때문입니다
4주기에 속한 K 의 전자배치를
알아봅시다
K 보다 원자번호가 작은 원소 중
원자번호가 가장 큰 비활성기체는
Ar 이므로 [Ar] 을 우선 적습니다
Ar은 18개의 전자를 가지고
K는 19개의 전자를 가집니다
K 가 Ar 보다 전자를 하나 더 가지고
이 전자를 4s 오비탈 칸에 채워 넣습니다
이것은 K에서 4s 오비탈이 3d 오비탈보다
더 낮은 에너지 준위를 갖기 때문입니다
이것이 에너지가 증가하는 방향이므로
전자는 4s 오비탈에 채워집니다
따라서 비활성 기체 표기법을 이용한
K 의 전자배치는
[Ar]4s1 입니다
그리고 Ca 의 경우

Thai: 
เราได้ดู
การจัดอิเล็กตรอนของ
โพแทสเซียมและแคลเซียมไปแล้ว
แต่ลองทำอีกครั้งเร็วๆ
เพราะมันจะมีผลต่อวิธีคิดเกี่ยวกับ
d ออร์บิทัล เราเจอโพแทสเซียม
ซึ่งก็คือคาบที่ 4 ของตารางธาตุ
ถ้าเราเขียนสัญลักษณ์แก๊สเฉื่อย
เพื่อประหยัดเวลา
เราทำย้อนกลับ แก๊สเฉื่อยตัวแรกที่เราเจอ
คืออาร์กอน เราก็เขียนอาร์กอนในวงเล็บ
เรารู้ว่าอาร์กอนมีอิเล็กตรอน 18 ตัว
และโพแทสเซียมมีอิเล็กตรอน 19 ตัว
โพแทสเซียมมีอิเล็กตรอน
มากกว่าอาร์กอน 1 ตัว
เราก็ใส่อิเล็กตรอนที่เกินมาลงใน 4s ออร์บิทัล
เพราะสำหรับโพแทสเซียม 4s ออร์บิทัล
มีพลังงานต่ำกว่า 3d ออร์บิทัลตรงนี้
เรามีพลังงานที่เพิ่มขึ้น
และอิเล็กตรอนนั้นไปอยู่ใน 4s ออร์บิทัล
การจัดอิเล็กตรอนสมบูรณ์
โดยใช้สัญลักษณ์แก๊สเฉื่อยของโพแทสเซียม
และอาร์กอนในวงเล็บคือ 4s1
สำหรับแคลเซียม

Thai: 
เอาล่ะ เรามีอิเล็กตรอน
มากกว่าโพแทสเซียมหนึ่งตัว
อิเล็กตรอนนั้นจะอยู่ใน 4s ออร์บิทัล
เช่นกัน และเราจับคู่สปินของเรา
เราก็เขียนการจัดอิเล็กตรอน
ของแคลเซียม เป็นอาร์กอนในวงเล็บ 4s2
สำหรับแคลเซียม 2 บวกไอออน
ถ้าคุณจะคิดถึงการเกิดไอออนตรงนี้
เรากำลังพูดถึงการจัดอิเล็กตรอน
สำหรับอะตอมที่เป็นกลาง
หมายความว่าจำนวนโปรตอน
และอิเล็กตรอนเท่ากัน
ที่มีเลขอะตอมเป็น 20
โปรตอน 20 ตัวและอิเล็กตรอน 20 ตัว
ถ้าเราเสียอิเล็กตรอน 2 ตัว
เรามีประจุลัพธ์เป็นบวก 2
เราทำให้แคลเซียมเป็นไอออน
อิเล็กตรอน 2 ตัวที่เราเสียไป
เกิดเป็นแคลเซียม 2 บวกไอออนคือสองตัวนี้
อิเล็กตรอนสองตัวนี้ตรงนี้อยู่ใน 4s ออร์บิทัล
การจัดอิเล็กตรอนของแคลเซียม 2 บวก
จะเท่ากับการจัดอิเล็กตรอน
ของแก๊สเฉื่อย อาร์กอน ตรงนี้
เอาล่ะ สำหรับโพแทสเซียม
เมื่อเรานับอาร์กอนเข้ามา

English: 
All right, we have one more
electron then potassium
and so that electron's going
to go into the 4s orbital
as well and so we pair our spins
and we write the electron configuration
for calcium as argon in brackets 4s 2.
For the calcium two plus ion,
so if you're thinking
about forming an ion here,
we're talking about the
electron configurations
for a neutral atom
meaning equal numbers of
protons and electrons.
With the atomic number of 20,
20 protons and 20 electrons.
If we lose two electrons,
we have a net deposited two charge.
We form the calcium to ion.
The two electrons that we would lose
to form the calcium
two plus ion are these.
These two electrons right
here in the 4s orbital.
The electron configuration
for calcium two plus
would be the same as the
electron configuration
for the noble gas argon here.
All right, so for potassium,
once we accounted for argon,

Bulgarian: 
Имаме още един електрон, отколкото при калия
и този електрон също влиза в 4s орбиталата.
Съчетаваме спиновете
и пишем електронната конфигурация за калция като
аргон в скоби 4s2.
За калциевия 2+ йон,
ако мислиш за създаване на йон тук,
говорим за електронните конфигурации за неутрален атом,
което означава равен брой протони и електрони.
С атомно число от 20 – 20 протона и 20 електрона.
Ако загубим 2 електрона,
тогава имаме заряд от +2.
Превръщаме калция в йон.
Двата електрона, които ще загубим, за да създадем калциевия 2+ йон, са тези.
Тези два електрона тук в 4s орбиталата.
Електронната конфигурация за калций 2+
ще е същата като електронната конфигурация за благородния газ аргон.
За калия, след като отбелязахме аргона,

Korean: 
K 보다 전자의 수가 하나 많습니다
이 전자는 4s 오비탈로 들어가고
서로 반대 스핀을 가집니다
Ca 의 전자배치는
[Ar]4s2 라고 쓸 수 있습니다
이제 Ca 2+ 에 대해
생각해봅시다
여기서는 이온을 형성하는 경우를
생각해야 합니다
우리는 이제까지
중성 원자의 경우만 
생각해왔습니다
양성자 수와 전자 수가 같은 경우 말입니다
원자번호 20의 원자는
20개의 양성자와 20개의 전자를 갖습니다
두 개의 전자를 잃으면
2+ 를 띠게 되고
Ca은 2가 양이온을 형성합니다
이 두 개의 전자를 잃으면
Ca2+ 를 형성합니다
이 두 개의 전자들은
4s 오비탈에서 빠져나가고
Ca2+ 의 전자배치는
비활성 기체인 아르곤과
같게 됩니다
K 는
Ar 에 비해

Bulgarian: 
имахме един електрон, за който да помислим.
За калция, след като преброихме аргона,
имахме 2 електрона, за които да помислим.
Да преминем към следващия елемент на периодичната таблица,
това е скандий.
Това е с един електрон повече от калция.
Имаме три електрона, за които да се тревожим,
след като поставим аргона тук.
Тук нещата стават странни.
Сега трябва да помислим за d орбиталите
и, отново, тези неща са много сложни,
след като стигнеш до скандия, понеже енергиите се променят.
Когато стигнеш до скандия,
въпреки че това са много малки енергийни разлики,
сега енергията на 4s орбиталата
е по-висока от енергията на 3d орбиталите.
Говорим отново за увеличаване на енергията
и това е доста странно.
Ако помислиш за тези три електрона,
къде ще ги поставим?
Първото ти предположение,
ако разбираш тези енергийни разлики,
може да е "Е, ще следвам правилото на Хунд.
Ще поставя тези електрони във възможно най-ниското енергийно ниво
и няма да съчетавам спиновете,

English: 
we had one electron to think about.
For calcium, once we counted for argon
we had two electrons to think about.
If we go to the next element
on the periodic table,
that's scandium.
That's one more electron and calcium.
We have three electrons to worry about
once we put argon in here like that.
This is where things get weird.
Now we have to think about the d orbitals
and once again things are very complicated
once you hit scandium
because the energies change.
When you hit scandium
even though these are very
small energy differences,
now the energy of the 4s orbital
is actually higher than the
energy of the 3d orbitals.
We're talking about once
again increasing energy
and so that's pretty weird.
All right, so if you think
about these three electrons,
where are we gonna put them?
Well your first guess,
if you understand these energy differences
might be, okay, well I'm
gonna follow Hund's rule.
I'm gonna put those
electrons in the lowest
energy level possible here
and I'm going to not pair my spins

Thai: 
เรามีอิเล็กตรอนหนึ่งตัวให้คิด
สำหรับแคลเซียม เมื่อเรานับของอาร์กอนแล้ว
เรามีอิเล็กตรอน 2 ตัวให้คิด
ถ้าเราไปยังธาตุต่อไปในตารางธาตุ
นั่นคือสแกนเดียม
มันมีอิเล็กตรอนมากกว่าแคลเซียมหนึ่งตัว
เรามีอิเล็กตรอน 3 ตัวให้คิด
โดยเราใส่อาร์กอนลงไปตรงนี้อย่างนั้น
นี่คือจุดที่เริ่มประหลาด
ตอนนี้เราต้องคิดถึง d ออร์บิทัล
ย้ำอีกครั้ง สิ่งต่างๆ ดูซับซ้อนมาก
เมื่อคุณเจอสแกนเดียม 
เพราะพลังงานเปลี่ยนไป
เมื่อคุณถึงสแกนเดียม
ถึงแม้ว่าพลังงานจะต่างกันน้อยมาก
ตอนนี้พลังงานของ 4s ออร์บิทัล
จริงๆ แล้วสูงกว่าพลังงานของ 3d ออร์บิทัล
เรากำลังพูดถึงพลังงานที่เพิ่มขึ้น
มันแปลกทีเดียว
เอาล่ะ ถ้าคุณคิดถึงอิเล็กตรอนสามตัวนี้
เราจะใส่พวกมันที่ไหน?
สิ่งแรกที่คุณเดาได้
ถ้าคุณเข้าใจความแตกต่างของพลังงาน
คุณก็อาจบอกว่า 
โอเค ฉันจะทำตามกฎของฮุนด์
ฉันจะใส่อิเล็กตรอนเหล่านี้ลงในชั้น
พลังงานที่ต่ำสุดที่เป็นไปได้ตรงนี้
และฉันจะไม่จับคู่สปิน

Korean: 
하나의 전자가 더 많습니다
또한 Ca 는 아르곤에 비해
전자가 2개 더 많습니다
주기율표에서 다음 원소는
Sc 입니다
Sc 는 Ca 보다 전자가 하나 더 많습니다
아르곤보다 3개의 전자가
많다고 표시할 수 있습니다
여기서부터 예외가 생깁니다
d 오비탈에 관해서 생각해야 되기 때문에
다시 복잡한 사고를 거쳐야 합니다
Sc 의 전자배치에서
아주 작은 에너지 차이임에도 불구하고
에너지 준위가 뒤바뀌게 됩니다
4s 오비탈의 에너지 준위가
3d 오비탈의 에너지 준위보다
높아집니다
에너지의 증가에 대해 이야기하고 있지만
이상한 현상입니다
그러면 이 세 전자들을
어디에 배치해야 할까요?
여러분이 에너지 차이에 대해 이해했다면
아마도 이 문제에 대한 답을
훈트 규칙으로 구하려고 할 것입니다
가장 에너지 준위가 낮은 3d 에
전자들을 배치하겠습니다
전자들은 짝짓지 않고 배치합니다

Bulgarian: 
и ще запиша моята електронна конфигурация за скандия ето така."
Може да мислиш, че ще е аргон 3d3,
но не наблюдаваме това при електронната конфигурация на скандия.
Всъщност два от тези електрона
ще се преместят до орбитала с по-висока орбитала.
Два от тези електрона се преместват нагоре
към 4s орбиталата – ето така.
Оказва се, че електронната конфигурация е 4s2 3d1.
Всъщност е 4s2 3d1 или, ако предпочиташ, 3d1 4s2.
Като отново имаме аргон отпред.
Всяко от тези е приемливо.
Това е странно, понеже защо тези електрони,
защо тези два електрона отиват към орбитала с по-висока енергия?
Няма просто обяснение за това.
Въпреки че енергията за тези два електрона може да е по-висока,
като цяло за целият атом скандий тя трябва да не е по-висока.
Има много други фактори, които трябва да вземем предвид,
неща като увеличаването на заряда на ядрото.

Thai: 
ฉันจะเขียนการจัดอิเล็กตรอน
อย่างนั้นสำหรับสแกนเดียม
คุณอาจคิดว่ามันเป็นอาร์กอน 3d3
แต่นั่นไม่ใช่สิ่งที่เราสังเกตเห็น
การจัดอิเล็กตรอนของสแกนเดียม
ที่จริง อิเล็กตรอนสองตัวนี้
เลื่อนขึ้นไปยังออร์บิทัลที่มีพลังงานสูงกว่า
อิเล็กตรอนสองตัวนั้นเลื่อนขึ้น
ไปยัง 4s ออร์บิทัลอย่างนั้น
การจัดอิเล็กตรอน
ปรากฏว่าเป็น 4s2, 3d1
จริงๆ แล้วมันคือ 4s2, 3d1
หรือถ้าคุณชอบ เป็น 3d1, 4s2 ก็ได้
มีอาร์กอนอยู่ข้างหน้าเหมือนเดิม
ตัวไหนก็ถือว่าถูก
มันแปลก ทำไมอิเล็กตรอนพวกนั้น
ทำไมอิเล็กตรอนสองตัวนี้ไปยังออร์บิทัล
ที่มีพลังงานสูง?
มันไม่มีคำอธิบายง่ายๆ ในเรื่องนี้
เอาล่ะ ถึงแม้ว่าอิเล็กตรอนสองตัวนั้น
อาจมีพลังงานสูงขึ้น
แต่อะตอมสแกนเดียมโดยรวม
ต้องไม่มีพลังงานสุงขึ้น
มันมีปัจจัยอื่นหลายอย่างให้คิด
อย่างเช่น การเพิ่มประจุนิวเคลียร์

English: 
and so I'm going to write
my electron configuration
like that for scandium.
You might think it would be argon 3d 3
but that's not what we observed
for the electron
configuration for scandium.
Actually two of these electrons
actually move up to the
higher energy orbital
so two of those electrons move up
to the 4s orbital here like that.
The electron configuration
turns out to be 4s 2, 3d 1.
It's actually 4s 2, 3d 1
or if you prefer 3d 1, 4s 2
once again with argon in front of it.
Either one of these is acceptable.
This is weird so like
why did those electrons,
why did those two
electrons go to an orbital
of higher energy?
There's no simple explanation for this.
All right, so even though
it might be higher in energy
for those two electrons,
it must not be higher energy overall
for the entire scandium atom.
There are many other factors to consider
so things like increasing nuclear charge.

Korean: 
이제 Sc 의 전자배치를
써보겠습니다
이를 [Ar]3d3 이라고 생각할 수 있지만
이것은 Sc 의 실제 전자배치라고
할 수 없습니다
사실 이 두 전자들은
더 높은 에너지를 가진
오비탈로 이동합니다
두 전자들은
4s 오비탈로 올라가면서
전자배치는
[Ar]4s2 3d1 이 됩니다
[Ar]4s2 3d1 이 됩니다
아니면 [Ar]3d1 4s2
라고도 쓸 수 있습니다
이 중 하나를 쓰면 됩니다
왜 이 두 전자는
더 높은 에너지 준위의 오비탈로
이동하는 것일까요?
간단하게 설명할 수는 없습니다
이 두 전자가 더 높은 에너지를
가진다고 하더라도
Sc 원자 전체의 에너지가
높아지지는 않았을 것입니다
핵전하의 증가 등
다양한 요인이 있을 수 있습니다

English: 
The scandium has an extra
proton compared to calcium
and then there are once
again many more factors
and far too much to
get into in this video.
Unfortunately there is no
easy explanation for this
but this is the observed
electron configuration
for scandium.
How do we know this is true?
How do we know that the 4s orbital
is actually higher energy
than the 3d orbitals?
We know this from ionization experiments.
For example if you form
the scandium plus one ion,
the electron configuration
for the scandium plus one ion,
so we're losing an electron
from a neutral scandium atom.
This turns out to be argon 4s 1,
3d 1 or once again you could write argon,
3d 1, 4s 1.
Where did we lose that
electron to form our ion?
We lost that electron from the 4s orbital.
We had 4s 2 here and here we have 4s 1.
We lost this electron
and that only makes
sense if the 4s orbital

Thai: 
สแกนเดียมมีโปรตอนเกินมา 
เทียบกับแคลเซียม
แล้วมันมีปัจจัยอื่นอีก
มากเกินไปที่จะพูดถึงในวิดีโอนี้
โชคร้าย มันไม่มีคำอธิบายง่ายๆ ในเรื่องนี้
แต่นี่คือการจัดอิเล็กตรอนที่พบ
ของสแกนเดียม
เรารู้ได้อย่างไรว่ามันเป็นจริง?
เราเรารู้ได้อย่างไรว่า 4s ออร์บิทัล
จริงๆ แล้วมีพลังงานมากกว่า 3d ออร์บิทัล?
เรารู้ได้จากการทดลองไอออเนเซชัน
ตัวอย่างเช่น ถ้าคุณสร้าง
สแกนเดียม บวก 1 ไอออน
การจัดอิเล็กตรอน
สำหรับสแกนเดียม บวก 1 ไอออน
เราจะเสียอิเล็กตรอนหนึ่งตัว
จากอะตอมสแกนเดียมที่เป็นกลาง
อันนี้ปรากฏว่าเป็นอาร์กอน 4s1
3d1 หรือ คุณเขียนอาร์กอน
3d1, 4s1
เราเสียอิเล็กตรอนตรงไหนเพื่อให้เกิดไอออน?
เราใส่อิเล็กตรอนนั้นจาก 4s ออร์บิทัล
เรามี 4s2 ตรงนี้ และตรงนี้เรามี 4s1
เราเสียอิเล็กตรอนนี้
และมันสมเหตุสมผลถ้า 4s ออร์บิทัล

Bulgarian: 
Скандият има един допълнителен протон в сравнение с калция,
а също така има и много други фактори,
и са твърде много, че да навлизаме в тях в това видео.
За нещастие няма лесно обяснение за това,
но това е наблюдаваната електронна конфигурация за скандия.
Откъде знаем, че е вярна?
Откъде знаем, че 4s орбиталата
наистина е с по-висока енергия от 3d орбиталите?
Знаем това от йонизационни експерименти.
Например ако създадеш скандий 1+ йон,
електронната конфигурация за скандиевия 1+ йон –
губим един електрон от неутралния атом на скандия.
Оказва се, че това е аргон 4s1 3d1
или, отново, можеш да запишеш аргон 3d1 4s1.
Откъде загубихме този електрон, за да създадем нашия йон?
Изгубихме този електрон от 4s орбиталата.
Имахме 4s2, а тук имаме 4s1.
Загубихме този електрон

Korean: 
Sc 는 Ca 에 비해 
양성자를 하나 더 갖습니다
이 동영상에서 설명하기에는
너무 많은 요인들이 있습니다
불행히도 Sc 의 전자배치를
설명할 수 있는 쉬운 방법은
없습니다
이것이 사실이라는 것을 어떻게 알 수 있을까요?
4s 오비탈의 에너지 준위가
3d 오비탈보다 높다는 것을 
어떻게 증명할까요?
이를 이온화 실험을 통해 
알 수 있습니다
예를 들어서 Sc+ 을 형성하면
Sc+ 의 전자배치는
중성 Sc 원자에서
전자를 하나 잃게 되므로
[Ar]4s1 3d1
다르게 쓰면
[Ar]3d1 4s1 이라고 할 수도 있습니다
이온을 형성할 때
어떤 전자를 잃게 될까요?
전자는 4s 오비탈에서 잃게 됩니다
Sc 는 4s2 Sc+는 4s1 을 갖습니다
4s 오비탈의 에너지 준위가
가장 높아야만 여기서 전자를 잃는 것이

English: 
is the highest in energy
because when you lose an
electron for ionization,
you lose the electron
that's highest in energy.
That's the one that's easiest to remove
to form the ion.
The 4s orbital is
actually higher in energy
than the 3d orbitals.
You don't see this a lot in text books
and I think the main reason for that
is because of the fact
that if you're trying
to think about just writing
electron configurations.
Your goal is to write,
let's say you're taking a test
and your goal is to write
the electron configuration
for scandium.
The easiest way to do that ...
Let me go ahead and use red here.
The easiest way to do that
if you want to write the
electron configuration
for scandium, you look
at the periodic table
and if you're doing noble gas notation,
the noble gas that precedes it
is of course argon right here.
That takes care of the argon portion
and then looking at the
periodic table you would say
this could be 4s 1, 4s 2, 3d 1.
That gives you the correct
electron configuration,

Bulgarian: 
и това е логично, само ако 4s орбиталата е най-висока по енергия,
понеже когато губиш електрон при йонизация,
губиш електрона, който е с най-висока енергия.
Той е този, който е най-лесно да се премахне,
за да се създаде йон.
4s орбиталата всъщност е с по-висока енергия
от 3d орбиталите.
Не виждаш това в много учебници
и мисля, че основната причина за това е
поради факта, че ако опитваш да помислиш само за записването на електронните конфигурации,
целта ти е да запишеш...
Да кажем, че правиш тест
и целта ти е да запишеш електронната конфигурация за скандий.
Най-лесният начин да направиш това...
Нека използвам червено тук.
Най-лесният начин да направиш това,
ако искаш да запишеш електронната конфигурация за скандия,
е да погледнеш периодичната таблица
и, ако използваш обозначението за благородния газ,
непосредствено предшестващият благороден газ е, разбира се, аргон.
Това обозначава частта с аргона
и после, като гледаш периодичната таблица, можеш да кажеш,
че това ще е 4s1, 4s2 3d1.
Това ти дава правилната електронна конфигурация,

Korean: 
말이 됩니다
이온화될 때 전자를 잃으면
가장 높은 에너지 준위의 오비탈에서
전자를 잃기 때문입니다
그것이 이온을 생성할 때
가장 제거하기 쉬운 전자이기 때문입니다
4s 오비탈이
3d 오비탈보다
에너지 준위가 높습니다
책에서 쉽게 볼 수는 없는 내용입니다
저는 그 이유가
여러분이 그저 전자 배치만을
알아내려고 하고 있기
때문이라고 생각합니다
알아내려고 하고 있기
때문이라고 생각합니다
여러분이 시험을 보고 있다고 가정하고
Sc 의 전자 배치를 써야 한다고
생각해봅시다
가장 쉬운 방법은
빨간색으로 표시해봅시다
Sc 의 전자 배치를 쓸 때
가장 쉬운 방법은
주기율표를 보고
비활성 기체 표기법을
이용하는 것입니다
Sc보다 원자번호가
작은 비활성 기체는
Ar 입니다
Ar 을 기준으로 하면
주기율표를 보면 그 다음 전자들은
4s1, 4s2, 3d1 에 채워집니다
그러면 Sc 의 정확한 전자배치를
알아낼 수 있습니다

Thai: 
มีพลังงานสูงสุด
เพราะถ้าคุณเสียอิเล็กตรอนในไอออไนเซชัน
คุณจะเสียอิเล็กตรอนที่มีพลังงานสูงสุด
นั่นคืออันที่เอาออกง่ายที่สุด
เกิดเป็นไอออน
4s ออร์บิทัลจริงๆ แล้วมีพลังงานสูงกว่า
3d ออร์บิทัล
คุณไม่เห็นเรื่องนี้บ่อยนักในหนังสือ
ผมว่า สาเหตุหลักคือว่า
ถ้าคุณพยายาม
คิดถึงการเขียนการจัดอิเล็กตรอน
เป้าหมายของคุณคือเขียน
สมมุุติว่าคุณกำลังสอบ
และเป้าหมายคือเขียนการจัดอิเล็กตรอน
ของสแกนเดียม
วิธีทำที่ง่ายที่สุด --
ขอผมลงมือใช้สีแดงตรงนี้นะ
วิธีทำที่ง่ายที่สุด
ถ้าคุณอยากเขียนการจัดอิเล็กตรอน
ของสแกนเดียม คุณก็ดูตารางธาตุ
และถ้าคุณใช้สัญลักษณ์แก๊สเฉื่อย
แก๊สเฉื่อยที่อยู่ก่อนหน้า
แน่นอน คืออาร์กอนตรงนี้
มันจัดการส่วนที่เป็นอาร์กอนแล้ว
เมื่อดูตารางธาตุ คุณก็บอกว่า
อันนี้เป็น 4s1, 4s2, 3d1
มันจะให้การจัดอิเล็กตรอน

Bulgarian: 
аргон 4s2 3d1.
Но това намеква, че d орбиталите,
3d орбиталите се запълват след 4d орбиталите
и, следователно, са с по-висока енергия,
а това всъщност не е вярно.
Това ти помага да предположиш, че това е така,
ако записваш електронна конфигурация,
но в реалността не се случва това.
Тук трябва да помислим за другите елементи.
Току-що се справихме със скандия.
След това нека преминем към титан.
Да помислим за титана.
Следващият елемент в периодичната таблица,
ако въпросът ти на теста беше да напишеш електронната конфигурация за титания,
най-лесният начин да направиш това, отново,
е да помислиш за аргона.
Поставяш аргон в скоби и после си мислиш:
"Това ще е 4s1, това ще е 4s2, това ще е 3d1 и това ще е 3d2."
Можеш да запишеш 4s2 и после 3d2
или, отново, можеш да промениш местата на 3d2 и 4s2.

Korean: 
[Ar]4s2 3d1 말입니다
그러나 d 오비탈의 경우
3d 오비탈이 4s 오비탈 
다음으로 채워지고
따라서 더 높은 에너지를 가진다고
암시하고 있습니다
그러나 이것은 사실이 아닙니다
그저 전자 배치만 쓰는
경우에는 대충 이렇게
가정할 수 있습니다
사실상 일어나지는 않는다는 말입니다
방금 Sc 의 경우에서는 했으나
다른 원소들의 경우에서도 해봅시다
Ti 을 해봅시다
Ti 는 주기율표에서
Sc 다음으로 있는 원소입니다
Ti 의 전자배치를 쓰는 것이
시험에서 출제된다면
가장 쉬운 방법은
Ar 의 전자배치를 이용하는 것입니다
[Ar] 을 쓰고 생각해봅니다
[Ar] 보다 4s1, 4s2
3d1, 3d2 가 더 채워지므로
[Ar]4s2 3d2 라고
쓸 수 있습니다
아니면 3d2 와 4s2 의 위치를
바꿀 수도 있습니다

Thai: 
อาร์กอน 4s2, 3d1
แต่มันสื่อว่า d ออร์บิทัล
3d ออร์บิทัลเติมหลังจาก 4s ออร์บิทัล
และมีพลังานมากกว่า
จริงๆ แล้วมันไม่จริง
การสมมุติว่ามันเป็นจริงช่วยให้
คุณเขียนการจัดอิเล็กตรอนได้
แต่มันไม่ใช่สิ่งที่เกิดขึ้นในความเป็นจริง
เราต้องคิดถึงธาตุอื่นๆ ตรงนี้
เราเพิ่งจัดการสแกนเดียมไป
ลองไปยังไทเทเนียมกัน
คิดถึงไทเทเนียม
ธาตุต่อไปในตารางธาตุ
ถ้าคำถามคุณในข้อสอบ
คือให้เขียนการจัดอิเล็กตรอนของไทเทเนียม
วิธีทำที่ง่ายที่สุดก็เหมือนเดิม
คิดถึงอาร์กอนก่อน
ใส่อาร์กอนในวงเล็บ แล้วคิดเอง
อันนี้จะเป็น 4s1 อันนี้จะเป็น 4s2
อันนี้จะเป็น 3d1 และอันนี้จะเป็น 3d2
คุณก็เขียน 4s2
แล้วก็ 3d2
หรือคุณสลับ 3d2 กับ 4s2 ได้

English: 
argon 4s 2, 3d 1.
But it's implying that the d orbitals,
the 3d orbitals fill after the 4s orbital
and is therefore a higher energy
and that's not true actually.
It does help you to just
assume that's the case
if you're writing an
electron configuration
but that's not what's
happening in reality.
We need to think about
the other elements here.
We just did scandium.
Next let's move on to titanium.
Thinking about titanium,
so the next element in the periodic table
if your question on the test
was write the electron
configuration for titanium,
the easiest way to do
it is just once again
to think about argon.
Put argon in brackets and
then think to yourself,
this would be 4s 1, this would be 4s 2,
this would be 3d 1 and this would be 3d 2.
You could write 4s 2
and then 3d 2
or once again you could
switch 3d 2 and 4s 2.

Thai: 
เหมือนเดิม อันนี้สื่อว่า d ออร์บิทัลเติม
หลัง 4s ออร์บิทัล ซึ่งไม่เป็นจริง
แต่มันให้คำตอบที่ถูกต้อง
การคิดทั้งสองแบบมีประโยชน์
การคิดถึงชั้นพลังงานให้ถูกต้องนั้นมีประโยชน์
แต่ในขณะเดียวกัน 
ถ้าเป้าหมายคุณคือหาคำตอบ
ให้เร็วที่สุดเท่าที่เป็นไปได้
การดูตารางธาตุ
และไล่การจัดอิเล็กตรอน
อาจเป็นวิธีทำข้อสอบที่ดีที่สุด
ลองดูธาตุอื่นๆ บ้างตรงนี้
เราได้พูดถึงสแกนเดียมและไทเทเนียมไป
เอาล่ะ ลองลงมาข้างล่างตรงนี้
ลองดูที่ตั้งไว้ตรงนี้
เอาล่ะ เราทำสแกนเดียมกับไทเทเนียมไป
สแกนเดียมคืออาร์กอน 4s2, 3d1
เราพูดถึงอิเล็กตรอนสองตัวใน 4s ออร์บิทัลไป
อิเล็กตรอน 1 ตัวใน 3d ออร์บิทัล
เราเพิ่งทำไทเทเนียม 4s2, 3d2 ไป
คุณสลับลำดับพวกนี้ได้เหมือนเดิม
เมื่อคุณใช้สัญลักษณ์ออร์บิทัล
เพิ่มอิเล็กตรอนตัวที่ 2 ให้กับ d ออร์บิทัล
นี่คืออิเล็กตรอนที่เราเพิ่ม
เราไม่ได้จับคู่สปิน
เราแค่ทำตามกฎของฮุนด์ตรงนี้

Bulgarian: 
И това намеква, че d орбиталите се запълват след 4s орбиталата,
което не е вярно, но ти дава верния отговор.
Полезно е да мислим за това и по двата начина.
Полезно е да мислим правилно за енергийните нива,
но в същото време, ако целта ти е да стигнеш до отговора по най-бързия възможен начин,
като гледаш периодичната таблица,
създаването на електронната конфигурация може да е най-добрият начин за теста.
Нека разгледаме някои от тези други елементи тук.
Току-що говорихме за скандий и титан.
Нека слезем тук долу.
Нека разгледаме тази малка група тук.
Току-що направихме скандий и титан.
Скандият беше аргон 4s2 3d1.
Говорихме за два електрона в 4s орбиталата, един електрон в 3d орбиталата.
Направихме и титания, 4s2 3d2
като можеш да смениш местата им.
Когато използваш орбиталното обозначение,
добавяйки този втори електрон към d орбитала...
Това е електронът, който добавихме.
Не съчетахме спиновете.
Следваме правилото на Хунд.

Korean: 
이것은 4s 오비탈 다음으로 
d 오비탈을 채운다고 암시하고 있으며
이는 사실이 아니지만
여러분께 올바른 답을 주기는 합니다
두 방법 모두 유용합니다
올바른 에너지 준위를 
구해내는 것은 좋지만
가장 빠른 방법으로
답을 알아내는 것을
목적으로 한다면
주기율표를 보고
전자배치를 알아내는 것이
시험에서는 가장 적합한
방법일 것입니다
다른 원소들에 대해서도 살펴봅시다
방금은 Sc 와 Ti 의 경우에 대해
알아보았습니다
아래로 내려가서
이 그림을 봅시다
방금 Sc 와 Ti 의 전자배치를
살펴보았습니다
Sc 의 전자배치는 [Ar]4s2 3d1 이었고
4s 오비탈에는 두 개의 전자가
3d 오비탈에는 1개의 전자가
채워져 있습니다
Ti 의 전자배치는 [Ar]4s2 3d2 이고
다시 말하지만 4s 와 3d 의
위치를 바꿔 쓸 수 있습니다
전자 표기법에서
d 오비탈의 두 번째 전자를 채울 때
전자를 짝짓지 않고
따로 적습니다
훈트 규칙을 따르는 것입니다

English: 
Once again this is implying
the d orbitals fill
after the 4s orbital which isn't true
but it does get you the right answer.
It's useful to think about it both ways.
It's useful to think about
the energy levels properly
but the same time if your
goal is to get the answer
the fastest way possible,
looking at the periodic table
and running through the
electron configuration
might be the best way to do it on test.
Let's look at some of
these other elements here
so we've just talked about
scandium and titanium.
All right, so let's go down here.
Let's look at this little setup here.
All right, so we just did
scandium and titanium.
All right, so scandium
was argon 4s 2, 3d 1.
We talked about two
electrons in the 4s orbital,
one electron in the 3d orbital.
We just did titanium 4s 2, 3d 2
or once again you could
switch any of these.
When you're doing orbital notation,
adding that second
electron to a d orbital.
Here's the electron that we added
so we didn't pair up our spins.
We're following Hund's rule here.

English: 
Next element is vanadium
so we do the same thing.
One more electron, we add
that electron to a d orbital
but we add it to, we don't
add it to one of the ones
that we've already started the fill here,
we add that electron to another d orbital,
so once again following Hund's rule.
Things get weird when you get to chromium.
Let me use a different
color here for chromium.
If you're just thinking about
what might happen for chromium,
chromium one more electron
to think about than vanadium.
You might think, let's
just add that one electron
to a 3d orbital like that
and then be done with it.
If you think about it, you might guess
4s 2, 3d 4.
Let's go ahead and write that.
4s 2, 3d 4, so question mark
but that's not actually what we get.
We get 4s 1, 3d 5.
That electron, this electron here,
let me go ahead and use red.
So you could think about this electron.
We expect it to be there,
we expect it to be 4s 2, 3d 4.
It's like that electron
has moved over here

Bulgarian: 
Следващият елемент е ванадий.
Още един електрон, добавяме този електрон към d орбитала,
но не го добавяме към една от орбиталите, които вече започнахме да запълваме,
добавяме електрона към друга d орбитала.
И пак следваме правилото на Хунд.
Нещата стават странни, когато стигнеш до хром.
Нека използвам друг цвят за хром.
И така, хромът има с един електрон повече от ванадия.
Може да помислиш, че просто ще добавиш този един електрон
към една 3d орбитала ето така и готово.
Ако помислиш за това,
може да сметнеш, че това е 4s2 3d4.
Нека запишем това.
4s2 3d4, въпросителен.
Но всъщност не получаваме точно това.
Получаваме 4s1 3d5.
Този електрон тук – нека използвам червено.
Можеш да помислиш за този електрон.
Очакваме той да е тук,
очакваме да е 4s2 3d4.
Сякаш този електрон се е преместил ето тук,

Korean: 
다음 원소는 V 이고
같은 규칙을 반복합니다
하나의 전자가 더 있으면 
d 오비탈에 하나의 전자를 더 채웁니다
그러나 이전에 채웠던 칸에
채우지 않고
다른 d 오비탈에 채웁니다
훈트 규칙을 따르는 것입니다
Cr 에서는 조금 다릅니다
다른 색으로 Cr 을 표시해봅시다
Cr 의 경우에 대해
생각해봅시다
Cr는 V 보다 전자가 하나 더 많습니다
단순히 3d 오비탈의 전자가
하나 더 늘 것이라고 생각할 수 있습니다
이렇게 생각하면 전자배치는
[Ar]4s2 3d4 가 됩니다
이를 써보면
[Ar]4s2 3d4 ?
그러나 Cr 의 전자배치는 사실
[Ar]4s1 3d5 입니다
이 전자를
빨간색으로 표시해 봅시다
이 전자를 생각해보면
여기에 위치해 있어야
[Ar]4s2 3d4 가 됩니다
이 전자가 비어있는 3d 오비탈 쪽으로

Thai: 
ธาตุต่อไปคือเวเนเดียม เราก็ทำเหมือนเดิม
อิเล็กตรอนอีกหนึ่งตัว เราเพิ่มอิเล็กตรอนนั้น
ลงใน d ออร์บิทัล
แต่เราเพิ่มมัน เราไม่ได้เพิ่มมันลงใน
อันที่เราเริ่มเติมไปแล้วตรงนี้
เราใส่อิเล็กตรอนนั้นให้ d ออร์บิทัลอีกตัว
เหมือนเดิม ตามกฎของฮุนด์
สิ่งต่างๆ เริ่มแปลกเมื่อคุณไปถึงโครเมียม
ขอผมใช้อีกสีแทนโครเมียมนะ
ถ้าคุณคิดถึง
สิ่งที่อาจเกิดขึ้นกับโครเมียม
โครเมียม มีอิเล็กตรอนมากกว่า
วานาเดียมหนึ่งตัว
คุณอาจคิดว่า ลองเพิ่มอิเล็กตรอนหนึ่งตัวนั้น
ลงใน 3d ออร์บิทัลอย่างนั้น แล้วก็จบ
ถ้าคุณคิดอย่างนั้น คุณอาจเดาว่า
4s2, 3d4
ลองลงมือเขียนดู
4s2, 3d4 เครื่องหมายคำถาม
แต่นั่นไม่ใช่สิ่งที่เราได้จริงๆ
เราได้ 4s1, 3d5
อิเล็กตรอนนั้น อิเล็กตรอนนี่ตรงนี้
ขอผมลงมือใช้สีแดงนะ
คุณคิดถึงอิเล็กตรอนนี้ได้
เราคาดว่ามันจะอยู่ตรงนั้น
เราคาดว่ามันเป็น 4s2, 3d4
มันเหมือนกับว่าอิเล็กตรอนได้เลื่อนไปตรงนี้

English: 
to this empty orbital to give
you this orbital notation.
All right, so that's just an easy way
of thinking about it and in reality
that's not what's happening
if you're building up the atom here
because of the different energy levels.
But just to make things easier
when you're writing
electron configurations,
you can think about moving an
electron from the 4s orbital
over to the last empty d orbital here.
Some people say that this
half filled d subshell,
let me go and circle it here.
This half filled d subshell
is extra stable and that might
be true for the chromium atom
but it's not always true
so it's not really the best explanation.
The real explanation is
extremely complicated
and actually just way too much to get into
for a general chemistry course.
Next element is manganese.
All right, let me go ahead
and stick with blue here.
Manganese, one more
electron than chromium here.
Chromium we had six electrons here,
and manganese we need to
worry about seven electrons.

Bulgarian: 
в тази празна орбитала, за да ти даде това орбитално обозначение.
Това беше просто един лесен начин да помислим за това,
а в реалността не се случва това,
ако надграждаш един атом тук,
поради различните енергийни нива.
Но за да улесним нещата,
когато пишеш електронните конфигурации,
можеш да помислиш за преместване на един електрон от 4s орбиталата
към последната празна d орбитала тук.
Някои хора казват, че това е полузапълнен d подслой.
Нека заградя това.
Този полузапълнен d подслой
е супер стабилен и това може да е вярно за хромния атом,
но не е винаги вярно,
така че не е най-доброто обяснение.
Реалното обяснение е супер сложно
и е твърде трудно, че да навлизаме в него в курс по обща химия.
Следващият елемент е манган.
Нека се придържам към синия цвят.
Манган – има с един електрон повече от хрома.
Хромът имаше шест електрона,
а при мангана трябва да помислим за седем електрона.

Korean: 
이동한 것처럼 보입니다
이것은 단순히 쉽게 생각하기 위한
방법일 뿐이고
원자에서 사실상 일어나는 일은 아닙니다
원자에서 사실상 일어나는 일은 아닙니다
에너지 준위가 다르기 때문입니다
그러나 전자배치를
쉽게 쓰기 위해서는
4s 오비탈에 있는 전자가
비어있는 d 오비탈로 이동했다고
생각할 수 있습니다
몇몇 사람들은 이 반 채워진
d 오비탈이
이를 표시해 봅시다
이 반 채워진 d 오비탈이 보통의
경우보다 안정하다고 말합니다
이는 Cr 의 경우에는 맞을 수도 있지만
모든 경우에서 사실인 것은 아닙니다
최선의 설명은 아니라는 이야기입니다
정확한 설명은 너무 복잡해서
일반 화학의 과정으로 설명하기에는
어렵습니다
다음 원소는 Mn 입니다
파란색으로 표시해봅시다
Mn 은 Cr 보다 전자가 하나 많습니다
Cr 은 여섯 개의 전자가 있으나
Mn 은 고려해야 하는 전자가
7개 입니다

Thai: 
ในออร์บิทัลว่างนี้ 
ได้สัญลักษณ์ออร์บิทัลอย่างนี้
เอาล่ะ นั่นคือวิธี
คิดง่ายๆ และในความเป็นจริง
มันไม่ใช่่สิ่งที่เกิดขึ้น
ถ้าคุณสร้างอะตอมขึ้นมาตรงนี้
เนื่องจากชั้นพลังงานต่างกัน
เพื่อให้สิ่งต่างๆ ง่ายขึ้น
เมื่อคูณเขียนการจัดอิเล็กตรอน
คุณก็คิดถึงการเลื่อนอิเล็กตรอน
จาก 4s ออร์บิทัล
ไปยัง d ออร์บิทัลสุดท้ายที่ว่างอยู่ตรงนี้ได้
บางคนบอกว่า ชั้นย่อย d ที่เติมไว้ครึ่งหนึ่งนี้
ขอผมวงกลมมันตรงนี้นะ
ชั้นย่อย d ที่เต็มไปครึ่งหนึ่งนี้
มีความเสถียรเป็นพิเศษ และมันอาจ
เป็นจริงสำหรับอะตอมโครเมียม
แต่มันไม่จริงเสมอไป
มันจึงไม่ใช่คำอธิบายที่ดีที่สุด
คำอธิบายจริงๆ นั้นซับซ้อนมาก
และมันมากเกินไปที่จะใส่
ลงในวิชาเคมีทั่วไป
ธาตุต่อไปคือแมงกานีส
เอาล่ะ ขอผมใช้สีฟ้านี่ตรงนี้
แมงกานีส อิเล็กตรอนมากกว่า
โครเมียมหนึ่งตัวตรงนี้
โครเมียม เรามีอิเล็กตรอน 6 ตัวตรงนี้
และแมงกานีส เราต้องคิดถึงอิเล็กตรอน 7 ตัว

Korean: 
이것은 우리가 주기율표에서
기대하는 것과 배치가 일치합니다
Mn 의 경우를 살펴봅시다
초록색으로 표시해 봅시다
각각 추가되는 전자들은
4s1, 4s2 에 채워지고
그 다음은 3d1, 3d2, 3d3
3d4, 3d5
이는 [Ar]4s2 3d5 입니다
우리가 예상했던 것과 같습니다
Fe 도 같은 방법으로 하면
[Ar]4s2 3d6 의 전자배치를 갖습니다
그리고 Fe 의 경우
전자가 3d 에서 짝지어집니다
이전의 전자배치에서도 봤듯이 말입니다
다음은 Co 로 하나의 전자를
더 고려해야 합니다
Co 의 전자배치는 [Ar]4s2 3d7 이고
추가한 전자는
하나의 스핀을 또 짝지었습니다
Ni 도 같은 경향입니다
하나의 전자를 추가하면 3d8 의
전자배치를 갖습니다
이는 사실과 일치하고 여기에
추가한 전자가 위치합니다
그리고 하나 더 이상한 경우가 있습니다

English: 
This is kind of what we expect,
just going across the periodic table.
Let me go ahead and do this for manganese.
Let me use green here.
You might say okay,
that's 4s 1, that's 4s 2
and then 3d 1, 3d 2, 3d 3,
3d 4, 3d 5.
You might say to yourself 4s 2, 3d 5.
This precedes how we would expect it to.
All right, and the same thing with iron,
so 4s 2, 3d 6.
All right, so that takes care of iron
and once again now you can
start to pair up your spins.
We've seen that in earlier
electron configurations.
Next cobalt, one more
electron to worry about.
All right, so 4s 2, 3d 7 makes sense
and you can see here would
be the electron that we added
and we paired up our spins again.
Nickel, same trends.
We add one more electron, 3d 8.
That makes sense, here's
the electron that we added
and once again we got a weird one.

Bulgarian: 
Това очакваме, като преминаваме през периодичната таблица.
Нека се заема с мангана.
Нека използвам зелено.
Може да си кажеш, че това е 4s1, това е 4s2,
а после 3d1, 3d2, 3d3, 3d4, 3d5.
Може да си кажеш – 4s2 3d5.
И това предхожда отговора ни, както очакваме.
Същото нещо е с желязото.
4s2 3d6.
Готови сме с желязото
и отново можеш да започваш да съчетаваш спиновете.
Виждали сме това в предишни електронни конфигурации.
Следва кобалт – още един допълнителен електрон.
Добре 4s2 3d7, логично е.
И можеш да видиш, че тук ще е електронът, който добавихме,
и отново съчетахме спиновете.
Никел – същият модел.
Добавяме още един електрон, 3d8.
Това е логично, ето го електрона, който добавихме.
И ето че пак стигнахме до едно по-странно.

Thai: 
นี่เป็นสิ่งที่เราคาด
เวลาข้ามตารางธาตุ
ขอผมลงมือทำสำหหับแมงกานีสนะ
ขอผมใช้สีเขียวตรงนี้
คุณอาจบอกว่า โอเค นั่นคือ 4s1 นั่นคือ 4s2
แล้ว 3d1, 3d2, 3d3
3d4, 3d5
คุณอาจบอกกับตัวเองว่า 4s2, 3d5
อันนี้เป็นไปตามที่เราคาดไว้
เอาล่ะ เช่นเดียวกัน เหล็ก
4s2, 3d6
มันจัดการเหล็กไป
แล้วคุณก็เริ่มจับคู่สปินได้
เราเห็นเช่นนั้นในการจัดอิเล็กตรอนก่อนหน้านี้
ต่อไป โคบอลต์ มีอิเล็กตรอนให้คิดอีก 1 ตัว
เอาล่ะ 4s2, 3d7 สมเหตุสมผล
และคุณเห็นตรงนี้ อิเล้กตรอนที่เราเพิ่ม
เราจับคู่สปินเหมือนเดิม
นิกเกิ้ล เหมือนกัน
เราเพิ่มอิเล็กตรอนอีกตัว 3d8
และมันสมเหตุสมผล 
ตรงนี้คืออิเล็กตรอนที่เราเพิ่ม
และเราเจออันที่แปลก

Thai: 
เอาล่ะ เมื่อเราไปยังทองแดง
ทองแดง คุณอาจคิดว่า
ขอผมใช้สีแดงแทนทองแดงนะ
เรารู้ว่าทองแดงสีแดง
เราคิดว่า เขียนอิเล็กตรอนเพิ่มอีกตัว
ถ้าเรานำการจัดอิเล็กตรอนของนิกเกิ้ลมาตรงนี้
เราเพิ่มอิเล็กตรอนอีกหนึ่งตัว
คุณคงเดาว่านั่นคือ
สัญลักษณ์ออร์บิทัลของทองแดง
แต่นั่นไม่ใช่สิ่งที่เราเห็น
เรานำอิเล็กตรอนนี่ตรงนี้มา
แล้วย้ายมันไปตรงนี้ อย่างนั้น
มันให้ชั้นย่อย d
เต็มตรงนี้
เหมือนเดิม คำอธิบายคือว่า
มันทำให้ทองแดงเสถียรมาก
มันเป็นจริงสำหรับทองแดง
เอาล่ะ มันปล่อยให้มีอิเล็กตรอนแค่ตัวเดียว
ใน 4s ออร์บิทัล
การจัดอิเล็กตรอนคือ 4s1, 3d10
แต่คำอธิบายในเคมีทั่วไปทั้งหลาย
นั้นง่ายเกินไปที่จะอธิบายความจริง
แต่ถ้าคุณเพิ่งเริ่ม
มันก็คือวิธีเป็นวิธีคิดที่ดี
แล้วสุดท้าย สังกะสี สังกะสีมันถูกต้องดี
เราเพิ่มอีกตัว
อิเล็กตรอนเพิ่มอีก 1 ตัว

English: 
All right, so when we get to copper.
So copper you might think ...
Let me use red for copper
so we know copper's red.
We think about it,
writing one more electron.
If we took the electron
configuration here for nickel,
we added one more electron.
You might guess that would be
the orbital notation for copper
but that's not what we see.
We've taken this electron here
and moved it over to here, like that.
This gives us a filled
d subshell here.
Once again one explanational see for that
is extremely stable for copper
and that might be true for copper.
All right, and that leaves
us only one electron here
in our 4s orbital.
The electron configuration is 4s 1, 3d 10
but all these general
chemistry explanations
are just a little bit
too simple for reality
but if you're just starting out,
they're pretty good way to think about it.
Then finally zinc, zinc makes sense.
We're adding one more,
writing one more electrons.

Bulgarian: 
Стигаме до мед.
За медта може да помислиш...
Нека използвам червено за мед.
Знаем, че медта е червена.
Записваме още един електрон.
Ако вземем електронната конфигурация тук – за никел –
добавяме още един електрон.
Може да предположиш, че това ще е
орбиталното обозначение за медта,
но всъщност не е така.
Взели сме този електрон тук
и сме го преместили насам, ето така.
Това ни дава запълнен d подслой тук.
Още един начин да обясним това е,
че така се получава изключително стабилна конфигурация за атома на медта.
Това ни оставя само един електрон тук в нашата 4s орбитала.
Електронната конфигурация е 4s1 3d10,
но всички тези обяснения от общата химия
са малко прекалено опростени за реалността.
Ако тепърва започваш с химията,
те са доста добър начин да помислим за нещата.
Последно, цинк – при цинка виждаме логиката.
Добавяме още един,
записваме още един електрон.

Korean: 
Cu 의 경우입니다
Cu 의 경우에는
빨간색으로 표시해봅시다
Cu 는 빨간색으로 표시합니다
하나의 전자가 추가됩니다
Ni 의 전자배치에서
하나의 전자를 추가해보겠습니다
이것이 Cu 의 전자 표기법이라고
생각할 수도 있습니다
그러나 이는 사실이 아닙니다
4s 의 전자는 이동하여
이와 같이 3d 오비탈에 채워집니다
그러면 완전히 차있는
d 오비탈이 됩니다
이에 대한 한 가지 설명은
이것이 Cu 에 대해 매우
안정적이라는 것이며
이는 Cu 의 경우 올바른 설명입니다
따라서 4s 오비탈에는
전자가 하나 남았기 때문에
전자배치는 [Ar]4s1 3d10 이 됩니다
이러한 일반화학 수준의 설명은
사실을 상당히 간단하게 설명한 것입니다
그러나 시작하는 단계에 있다면
생각하기에는 꽤나 괜찮은 방법입니다
마지막으로 Zn 입니다
하나의 전자를 추가해서
써보면

English: 
We just took care of copper.
For zinc we have one more electron
and so you could think about this being
4s 2 right here and then we have 3d 10,
one, two, three four, five, six,
seven, eight, nine, 10.
4s 2, 3d 10 or 3d 10, 4s 2
with argon in front of it
gives you the complete
electron configuration
and you can see, you've
now filled your 4s orbital
and your 3d orbitals like that.
Once again pretty complicated topic
and hopefully this just gives you an idea
about what's going on.

Korean: 
방금은 Cu 의 경우를 살펴보았으나
Zn 은 하나의 전자가 더 있고
전자배치는
[Ar]4s2 3d10 이 됩니다
하나 둘 셋 넷 다섯 여섯
일곱 여덟 아홉 열
[Ar] 4s2 3d10 또는 [Ar] 3d10 4s2 가
완전한 전자배치 입니다
그리고 이제 4s 오비탈과 3d 오비탈이
완전히 꽉 차있는 모습을 볼 수 있습니다
꽤나 복잡한 주제였지만
여러분이 이해할 수 있었으면
좋겠습니다
커넥트 번역 봉사단 | 고지우

Bulgarian: 
Погрижихме се за медта,
а за цинка имаме още един допълнителен електрон
и можеш да помислиш за това като за
4s2 ето тук и после имаме 3d10.
1, 2, 3, 4, 5, 6, 7, 8, 9, 10.
4s2 3d10 или 3d10 4s2, като отпред имаме аргон.
Това ти дава пълната електронна конфигурация
и можеш да видиш, че сега 4s орбиталата е запълнена
и 3d орбиталата е запълнена.
Отново, това е доста сложна тема
и се надявам, че това ти дава представа за онова, което се случва.

Thai: 
เราจัดการทองแดงไป
สำหรับสังกะสี เรามีอิเล็กตรอนมากขึ้นหนึ่งตัว
แล้วคุณก็คิดว่าอันนี้เป็น
4s2 ตรงนี้ แล้วเรามี 3d10
1, 2, 3, 4, 5, 6
7, 8, 9, 10
4s2, 3d10 หรือ 3d10, 4s2 
มีอาร์กอนอยู่ข้างหน้า
จะให้การจัดอิเล็กตรอนสมบูรณ์
และคุณเห็นได้ว่า
 ตอนนี้คุณเติม 4s ออร์บิทัลเต็ม
และ 3d ออร์บิทัลเต็มอย่างนั้น
ย้ำอีกครั้ง มันซับซ้อนทีเดียว
และหวังว่าคุณคงเข้าใจแนวคิด
ว่าเกิดอะไรขึ้นบ้างนะ
