
Thai: 
เรามี เขียนตรงนี้ --
เรารู้ว่าคาร์บอน 12 เป็นไอโซโทปคาร์บอน
ที่ทั่วไปที่สุดบนโลก
98.89% ของคาร์บอนบนโลกเป็นคาร์บอน 12
และเรารู้ว่า ตามนิยามแล้ว
มวลของมันเป็น 12 หน่วยมวลอะตอมพอดี
ทีนี้ มันไม่ใช่ไอโซโทปเดียว
ของคาร์บอนบนโลก
มันมีไอโซโทปอื่นๆ
อันที่พบบ่อยที่สุดอันต่อไปคือคาร์บอน 13
1.11% ของคาร์บอนบนโลกคือคาร์บอน 13
และเราพบโดยการทดลองว่า
มวลของมันเท่ากับ 13.0034 หน่วยมวลอะตอม
เลขเหล่านี้ที่เรามี
ทวนหน่อย พวกมันคือมวลอะตอม
นี่คือมวลอะตอม
และ สิ่งที่เราจะคิด ในวิดีโอนี้
คือเราจะหาเลขน้ำหนักอะตอม
ที่เขาให้คุณบนตารางธาตุอย่างนั้นได้อย่างไร?
น้ำหนักอะตอม

German: 
 
C12 (Kohlenstoff) ist das häufigste Isotop des Kohlenstoffs auf der Welt.
98,89% des Kohlenstoffs der Erde ist C12.
Definitionsgemäß wissen wir, dass seine Masse exakt 12 atomare Masseneinheiten umfasst (12u).
Das ist nicht das einzige Kohlenstoffisotop auf der Erde.
Das nächst häufigste ist C13.
1,11% des Kohlenstoffs der Erde ist C13.
Experimentell findet man heraus, dass
seine atomare Masse 13,0034u beträgt
Diese Zahlen, die wir hier haben, geben die Atommasse eines Elements an
Worüber wir in diesem Video sprechen wollen ist, wie die atomare Masse entwickelt wurde,
die im Periodensystem steht wie hier?

Hungarian: 
Felírtuk ide, hogy - amint ismeretes -
a szén-12 a leggyakoribb szénizotóp a Földön.
A Földön levő szén 98,89%-a  szén-12.
És tudjuk, hogy definíció szerint
a tömege pontosan 12 atomi tömegegység.
Ez nem az egyetlen szénizotóp a Földön,
léteznek más izotópjai is.
A második leggyakoribb a szén-13.
A Földön levő szén 1,11%-a szén-13.
És kísérletileg meghatározható, hogy
a tömege 13,0034 atomi tömegegység.
Ezek a számok itt tehát az atomtömeget jelentik.
Ezek atomtömegek.
Ebben a videóban azt tekintjük át,
miképpen jutottak el a relatív atomtömeghez,
amely a periódusos rendszerben található.

English: 
- [Instructor] We have, listed here...
We know that carbon 12 is the most common
isotope of carbon on Earth.
98.89% of the carbon
on Earth in carbon 12.
And we know that, by definition,
its mass is exactly 12 atomic mass units.
Now that's not the only
isotope of carbon on Earth.
There are other isotopes.
The next most frequent one is carbon 13.
1.11% of the carbon on Earth is carbon 13.
And we can experimentally find that
its mass is 13.0034 atomic mass units.
So, these numbers that we have here,
just as a review, these are atomic mass.
These are atomic mass.
And so, what we're gonna
think about, in this video,
is how do they come up with
the atomic weight number
that they'll give you on a
periodic table like that?
So, atomic weight.

Romanian: 
 
Știm că izotopul Carbon 12 este cel mai cunoscut
izotop de carbon de pe Pământ.
98.89% din carbonul de pe Pământ este carbon 12.
Și știm că, prin definiție,
masa lui este de exact 12 unități atomice de masă.
Acesta nu este singurul izotop de carbon de pe Pământ.
Mai sunt și alți izotopi.
Următorul cel mai frecvent este carbon 13.
1,11% din carbonul de pe Pământ este carbon 13.
Și putem găsi experimental că
masa lui este 13,0034 unități atomice de masă.
Așa că, aceste numere pe care le avem aici
să ne reamintim, sunt masele atomice.
Acestea sunt masele atomice.
Așadar, în acest videoclip ne vom gândi
cum se ajunge la masa atomică relativă
care este dată în tabelul periodic?
Deci, masa atomică relativă.

Korean: 
나열된 것을 봅시다
우리는 12번 원소가
지구에서 가장 흔한
탄소의 동위원소임을 알고 있습니다
지구에 있는 탄소의 98.89%는
12번 탄소입니다
그리고 그 정의를 통해
질량이 정확히 12amu
(원자질량단위)임을 알 수 있습니다
그것만이 지구에 존재하는
탄소의 유일한 동위원소는 아닙니다
다른 동위원소들도 있습니다
그다음으로 흔한 것이 13번 탄소입니다
지구의 탄소 1.11%가
13번 탄소입니다
실험적으로 그 질량이
13.0034amu 임을
알 수 있습니다
지금 여기에 있는 숫자들은
원자 질량입니다
원자 질량입니다
그리고 이 영상에서 생각해볼 것은
주기율표에 나와 있는 것처럼
어떻게 원자량을 얻어낼 수 있을까
하는 것입니다

Bulgarian: 
Тук сме изброили...
Знаем, че въглерод-12 е най-често
срещаният изотоп въглерод на Земята.
98,89% от въглерода на Земята е въглерод-12.
Знаем, че по определение
масата му е точно 12 единици атомна маса.
Обаче това не е единственият въглероден изотоп на Земята.
Има и други.
Вторият най-често срещан е въглерод-13.
1,11% от въглерода на Земята е въглерод-13.
Експериментално можем да намерим, че
масата му е 13,0034 единици атомна маса.
Така, тези числа тук,
за преговор - те представляват атомна маса на изотопите.
Атомна маса.
В това видео ще си помислим
как се получава относителната атомна маса,
която се пише ето така в периодичната таблица.

Bulgarian: 
Така... Относителна атомна маса (ОАМ).
Откъде идва?
Във видеото за ОАМ и атомна маса на изотоп,
виждаме, че ОАМ е среднопретеглената стойност
на атомните маси
на различните изотопи на даден елемент.
Така, за да намерим това 12,01,
взимаме среднопретеглената стойност на тези двете.
Спрямо какво претегляме?
Спрямо това колко често се среща даденият изотоп.
Това, което искаме да направим, е
да вземем 98.89% и да го умножим по 12.
Ще напиша процентното число като десетична дроб.
Ще бъде 0,9889 * 12.
И към това ще прибавим...
Ще прибавим 1,11% * 13,0034.

Thai: 
มันมาจากไหน?
ในวิดีโอเรื่องน้ำหนักอะตอม กับมวลอะตอม
เราเห็นว่า น้ำหนักอะตอม 
คือค่าเฉลี่ยถ่วงน้ำหนัก
ของมวลอะตอม
ของไอโซโทปต่างๆ ของธาตุนั้น
เพื่อหาค่านี้ ประมาณ 12.01
เราหาค่าเฉลี่ยถ่วงน้ำหนักของสองอย่างนี้
แล้วเราถ่วงมันด้วยอะไร?
เราถ่วงด้วยความถี่ที่เราพบไอโซโทป
สิ่งที่เราอยากทำก็คือ
เรานำ 98.89% มาคูณด้วย 12
และผมจะเขียนเปอร์เซ็นต์นี้เป็นทศนิยม
มันจะเท่ากับ 0.9889 คูณ 12
แล้วจากนั้น เราจะบวก --
เราจะบวก 1.11% คูณ 13.0034
เป็นทศนิยม มันจะเท่ากับ 0.011

Romanian: 
De unde vine ea?
Ei bine, în videoclipul cu masa atomică și masa atomică relativă
vedem că masa atomică relativă este media ponderată
a maselor atomice ale
diferiților izotopi ai acelui element.
Deci, ca să găsim aproximativ 12,01,
luăm media ponderată a acestor două lucruri.
Și cu cât facem ponderarea?
Ponderea fiecărui izotop va fi procentul care ne arată cât de comun este izotopul.
Ceea ce vom face este
să luăm 98,89% și să îl înmulțim cu 12.
Și voi rescrie acest procentaj, zecimal.
Va fi 0.9889 înmulțit cu 12.
Și, aici, adunăm...
1,11% înmulțit cu 13,0034.
Ca număr zecimal, va fi 0,011.

Hungarian: 
Tehát a relatív atomtömeg.
Vajon honnan származik?
A "Relatív atomtömeg és atomtömeg" című videóban láthattuk,
hogy a relatív atomtömeg
az egyes izotópok atomtömegének súlyozott átlaga.
Szóval, úgy kapjuk meg ezt a nagyjából 12,01-t, hogy
ennek a kettőnek vesszük a súlyozott átlagát.
És mivel súlyozzuk?
Azzal, hogy milyen gyakoriságú az adott izotóp.
Szóval  ehhez azt csináljuk, hogy
a 98,89%-ot szorozzuk 12-vel.
Átírjuk a százalékot tizedestört formába.
Így ez 0,9889-szer 12 lesz.
Ehhez pedig hozzáadunk...
1,11%-szor 13,0034-et.
Ez tizedestört alakban 0,011 lesz.

Korean: 
원자량은 어디에서
나온 것일까요?
원자량과 원자 질량을 다룬
이 영상에서
원자량이 그 원소의 다양한
동위원소들의 원자 질량의
평균이라는 것을 알 수 있습니다
그래서 12.01이라는 값을 찾기 위해
이 두 물체의 가중평균을 구합니다
이것을 무엇으로 잴까요?
동위원소가 흔한 정도를 이용해 잽니다
그래서 98.89%에
가중치 12를 곱할 수 있습니다
이 퍼센트 비율을
소수로 바꿔보겠습니다
그러면 0.9889×12가 됩니다
그리고 여기에
1.11% 곱하기 13.0034를
더할 것입니다
소수로 바꾸면 그 값은
0.011이 될 것입니다

English: 
Where does that come from?
Well, in the video on atomic
weight and on atomic mass,
we see that the atomic weight
is the weighted average
of the atomic masses of
the various isotopes of that element.
So, to find this roughly 12.01,
we take the weighted
average of these two things.
And what do we weight it by?
We weight it by how common
that isotope actually is.
So, what we wanna do is,
we could take 98.89%
and multiply it by 12.
And I'll rewrite this
percentage as a decimal.
So it'll be 0.9889 times 12.
And, to that, we are going to add...
We are going to add 1.11% times 13.0034.
So, as a decimal, that's
going to be 0.011.

German: 
Atomgewicht. Woher kommt das?
In dem Video zu Atomgewicht und Atommasse
sehen wir, dass das Atomgewicht der gewichtete Durchschnitt
der Atommasse der verschiedenen Isotope dieses Elements ist
Um diese genäherten 12,01u zu erhalten,
nimmt man den gewichteten Durchschnitt dieser zwei Stoffe
Wie gewichtet man das?
Man gewichtet es danach, wie häufig das Isotop vorkommt.
Was wir machen werden ist:
Wir nehmen 98,89% und multiplizieren es mit 12.
Ich werde die Prozentzahl als Dezimalzahl schreiben
Also 0,9889 mal 12
Und dazu addieren wir 1,11% mal 13,0034.

English: 
That's 1.11% is 0.011, oh, 111.
And I'm gonna multiply that
times 13.0034 atomic mass units.
So, what does that give us?
Let's get our calculator out here.
So, we are going to have 0.9889
times 12 is equal to 11.8668.
And, to that, we are going to add...
We are going to add 0.0111 times 13.0034.
And I know it's going to do
this multiplication first
because it's a calculator knows
about order of operations.
And so, that's all going to be,
as you can see, 12.01113774,
which, if you were to round
to the hundredths place,

German: 
Als Dezimalzahl wären das 0,0111.
Wir multiplitzieren 0,0111 mit 13,0034u.
Was ergibt das mit dem Taschenrechner?
Wir haben also 0,9889 x 12 = 11,8668
Und wir addieren mit 0,0111 x 13,0034.
Zuerst wird multipliziert, da der Taschenrechner die Rechenregeln kennt
Und das ergibt 12,01113774

Korean: 
그러면 0.0111
방금 그 값에 13.0034amu를
곱할 것입니다
그것이 어떤 의미일까요?
계산기를 꺼내봅시다
0.9889 곱하기
12는 11.8668입니다
그리고 거기에
0.0111 곱하기 13.0034를 
더할 것입니다
그리고 사칙연산 순서를 따르니까
이 곱셈부분을 먼저 하겠지요
그래서 이 결과는 보다시피
12.01113774이고
소수점 둘째 자리까지 반올림하면

Romanian: 
1,11% este 0,0111.
O să înmulțesc asta cu 13.0034 unități atomice de masă.
Deci, cât ne dă ?
Să ne folosim de calculator.
Deci vom avea 0.9889
înmulțit cu 12, care dă 11.8668
Iar la asta vom aduna...
vom aduna 0.0111 înmulțit cu 13.0034.
Și știm că întâi se face această înmulțire,
datorită ordinii operațiilor.
Așadar, totalul va fi 12.01113774,
care, dacă este rotunjit la sutimi,

Bulgarian: 
Като десетична дроб: 0,011...
...с още една единица -  0,0111.
И ще умножа това с 13,0034 единици атомна маса.
Така, това колко прави?
Ето го нашият калкулатор.
Имаме 0,9889
по 12 е равно на 11,8668.
И към това ще прибавим...
ще прибавим 0,0111 * 13,0034.
Знам, че ще сметне първо умножението,
защото калкулаторът знае за приоритета на операциите.
И така, това всичкото, както виждаме, е равно на 12,01113774,
което, ако закръглим до стотната,

Thai: 
นั่นคือ 1.11% คือ 0.0111 โอ้ 111
ผมจะคูณมันด้วย 13.0034 หน่วยมวลอะตอม
แล้วมันจะให้อะไร?
ลองเอาเครื่องคิดเลขออกมา
เราจะได้ 0.9889
คูณ 12 เท่ากับ 11.8668
แล้วจากนั้น เราจะบวก --
เราจะบวก 0.0111 คูณ 13.0034
และผมรู้ว่า มันจะคูณก่อน
เพราะมันเป็นเครื่องคิดเลข
ที่รู้ลำดับการดำเนินการ
แล้ว ทั้งหมดนั้นจะเท่ากับ อย่างที่เห็น
12.0113774
ซึ่ง ถ้าคุณปัดเป็นทศนิยมสองตำแหน่ง

Hungarian: 
1,11% az 0,011. Jaj, vagyis 111.
Ezt szorzom 13,0034 atomi tömegegységgel.
Mit kapunk így?
Nyissuk meg a számológépet.
0,9889-szer 12  egyenlő 11,8668-cal.
És ehhez hozzáadunk...
hozzáadunk 0,0111-szer 13,0034-et.
Először a szorzást végzi el,
mivel a számológép ismeri a műveletek sorrendjét.
És a végén 12,01113774-et kapunk,
melyet ha századra kerekítünk,

Hungarian: 
megkapjuk a relatív atomtömeget.
Ennyi az egész.
Így számoljuk ki a relatív atomtömeget.
Tehát felírhatom, hogy körülbelül 12,01,
ez az atomtömegek súlyozott átlaga.
Még valami, amit érdemes megfigyelned:
mi a különbség a szén-12 és a szén-13 között?
A szén-12-nek 6 protonja van.
A 6 proton teszi szénné,
ezért mindkettőnek 6 van.
A különbség a neutronokban van.
Ennek itt 6 neutronja van.
Ennek pedig eggyel több neutronja, 7.
Így ha megnézed az atomtömegek különbségét,
észreveszed, hogy az eltérés
plusz 1,0034 atomi tömegegység.
Ebből arra következtethetsz: " Hé, nézd csak,
ha hozzáadok 1 neutront,
1 neutront...
akkor ez nagyjából 1 atomi tömegegységet jelent.

German: 
Gerundet auf die zweite Nachkommastelle erhält man die 12,01 u
So errechnet man das Atomgewicht.
Genähert also 12,01 u
Das ist der gewichtete Durchschnitt der Atommassen
Eine weitere Sache, die zu notieren ist, ist der Unterschied zwischen C12 und C13.
C12, das hier oben, hat 6 Protonen
Die 6 Protonen machen den Kohlenstoff aus,
weswegen beide 6 Protonen haben
Der Unterschied liegt in den Neutronen
C12 hat 6 Neutronen
und C13 hat eins mehr also 7 Neutronen.
Wenn man sich den Unterschied der Atommassen anschaut, erkennt man,
dass 1,0034 u hinzugekommen sind.
So kann man sagen:
wenn ich ein Neutron addiere

Bulgarian: 
ще получим тази ОАМ.
Това е.
Ето го.
Така изчисляваме ОАМ.
Мога да го напиша като приблизително 12,01
- среднопретеглената стойност на атомните маси на изотопите.
Друго нещо, което може би си струва да отбележим, е
каква е разликата между въглерод-12 и въглерод-13?
Въглерод-12, този тук, има 6 протона.
Те го определят като въглерод,
така че и двата ще имат по 6 протона.
Разликата е в неутроните.
Този тук има 6 неутрона,
а другият
ще има един неутрон повече - 7 неутрона.
Като се вгледаме в разликата на атомните маси,
ще забележим, че промяната...
...изглежда да е +1,0034 единици атомна маса.
Оттук може би ще си кажеш:
"Ако добавя неутрон"
"той е приблизително равен на една единица атомна маса."

English: 
is how this atomic weight was gotten.
So that's that.
There you go.
That's how we calculate atomic weight.
So, I can write this
as approximately 12.01.
It's the weighted average
of the atomic masses.
Now, another thing that
you might want to note is,
what's the difference between
carbon 12 and carbon 13?
Carbon 12, this right
over here, is six protons.
The six protons are what make it carbon,
so both of these will have six protons.
And the difference is in the neutrons.
This right over here has
six neutrons, six neutrons.
And this, right over here,
is gonna have one more
neutron, seven neutrons.
So, when you look at the
difference in atomic mass,
notice the change is...
Looks like it's plus
1.0034 atomic mass units.
So, from this, you can say, "Hey, look,
if I add a neutron...
Plus one neutron.
Plus one neutron.
It's roughly equal to
an atomic mass unit."

Romanian: 
ne conduce la masa atomică relativă din tabel.
Deci asta este.
Chiar aici.
Așa calculezi masa atomică relativă.
Deci, pot scrie asta aproximativ 12.01.
Este media ponderată a maselor atomice ale izotopilor.
Acum, un alt lucru de notat:
Care-i diferența dintre carbon 12 și carbon 13?
Carbon 12, este chiar aici, cu 6 protoni.
Cei 6 protoni sunt cei care îl diferențiază ca fiind carbon.
Deci aceștia doi vor avea 6 protoni.
Și diferența este la numărul neutronilor.
Acesta de aici are 6 neutroni, șase.
Iar acesta de aici
va avea încă un neutron, deci 7 neutroni.
Deci, când ne uităm la diferența dintre masele atomice
observăm diferența...
Pare că este + 1.0034 unități atomice de masă (uam).
Deci, de aici, poți spune: "Hei, uite!
Dacă adun un neutron...
plus un neutron,
plus un neutron,
este aproximativ egal cu o unitate atomică de masă.

Korean: 
이 원자량이 나옵니다
그렇게 하시면 되겠습니다
됐습니다
이렇게 원자량을 계산합니다
그래서 이건 대략 12.01로
쓸 수 있습니다
이것은 원자 질량들의 가중평균입니다
여기서 여러분이 눈여겨볼 사실은
12번 탄소와 13번 탄소의 차이가
무엇이냐는 겁니다
여기 12번 탄소는 6개의 양성자로
이루어져 있습니다
이 6개의 양성자가
탄소의 성질을 만듭니다
그래서 둘 다 6개의 양성자를 가집니다
차이점은 중성자에 있습니다
이건 6개의 중성자를 가집니다
그리고 이건 7개의
중성자를 가집니다
그래서 원자 질량의 차이를 보면
값의 차이가
1.0034amu쯤 되는 것 같네요
이 결과를 보고 아마 당신은
중성자를 더하고
하나 더 더하고
하나 더 더하면
amu와 거의 비슷하다고 
생각할 수도 있습니다

Thai: 
คือค่าของน้ำหนักอะตอม
แค่นั้นแหละ
ได้แล้ว
นั่นคือวิธีที่เราคำนวณน้ำหนักอะตอม
ผมเขียนค่านี้ได้ว่าประมาณ 12.01
มันคือค่าเฉลี่ยถ่วงน้ำหนักของมวลอะตอม
ทีนี้ อีกอย่างที่คุณอาจสังเกต
คือว่า คาร์บอน 12 กับคาร์บอน 13 
ต่างกันอย่างไร?
คาร์บอน 12 ค่าตรงนี้ มีโปรตอน 6 ตัว
โปรตอน 6 ตัวคือสิ่งที่ทำให้เป็นคาร์บอน
ทั้งคู่จึงมีโปรตอน 6 ตัว
และสิ่งที่ต่างคือนิวตรอน
ค่านี้ตรงนี้มีนิวตรอน 6 ตัว นิวตรอน 6 ตัว
และตรงนี้
จะมีนิวตรอนมากขึ้นหนึ่งตัว
เป็นนิวตรอน 7 ตัว
เมื่อคุณดูผลต่างของมวลอะตอม
สังเกตว่าการเปลี่ยนแปลง --
ดูเหมือนจะเพิ่ม 1.0034 หน่วยมวลอะตอม
จากตรงนี้ คุณบอกได้ว่า เฮ้ ดูสิ
ถ้าฉันเพิ่มนิวตรอน --
เพิ่มนิวตรอนหนึ่งตัว
บวกนิวตรอนหนึ่งตัว
มันจะประมาณเท่ากับหนึ่งหน่วยมวลอะตอม

German: 
Entspricht das ungefähr 1 u, nicht genau, aber gerundet kommt es 1 u sehr nahe.
Das trifft auch auf Protonen zu.
Hoffentlich hast du jetzt eine Vorstellung von dem Unterschied der Atommassen,
die Masse und das Atomgewicht, welche der gewichtete Durchschnitt der verschiedenen Isotope der Elemente ist
und wie man es berechnet
und was die ungefähre Masse eines Neutrons ist, bekommen

Hungarian: 
Nem pontosan 1 atomi tömegegységet,
de tekintheted körülbelül 1 atomi tömegegységnek.
Ez szintúgy igaz a protonokra.
A lényeg, hogy remélhetőleg már
érted, mi a különbség az atomtömeg, amely egy atom tömege
és a relatív atomtömeg között, amely
a Földön levő különböző izotópok tömegének súlyozott átlaga.
Most már a kiszámításának módját
és egy neutron körülbelüli tömegét is ismered.

Romanian: 
Nu este exact o unitate atomică de masă,
dar, aproximând,
o putem vedea, într-un fel,
ca fiind foarte aproape de o unitate atomică de masă.
Același lucru este valabil pentru protoni.
Oricum, sper că acum poți aprecia
diferența dintre masa atomică, cea care este masa propriu-zisă,
și masa atomică relativă, care este media ponderată
a izotopilor unui element de pe Pământ.
Sper că ai înțeles cum se calculează
și cum se aproximează masa unui neutron.

Korean: 
이것은 정확히 amu는 아니지만
대략적으로 아주 광범위하고
높은 수준으로 말하자면
1amu에 굉장히 가깝다고 
볼 수 있습니다
양성자의 경우에도 마찬가지입니다
어쨌든 아마 당신은 이제
질량인 원자 질량과
한 원소의 다양한 동위원소의
가중평균인 원자량을 
구분할 수 있을 것입니다
그리고 그것을 계산하는 방법과
중성자의 질량의 
대략적인 크기도 알 수 있습니다
커넥트 번역 봉사단 | 주영은

Bulgarian: 
Не е точно една единица атомна маса,
но, грубо казано, в широк аспект,
можем да го разглеждаме като един вид
близък до единица атомна маса.
Същото е вярно и за протоните.
И така, надявам се, че сега имаш представа
относно разликата между атомната маса, която е масата,
и ОАМ, която е среднопретеглената стойност
на различките изотопи на даден елемент на Земята,
как да я изчисляваш,
и приблизително каква е масата на неутрона.

Thai: 
มันไม่เท่ากับหนึ่งหน่วยมวลอะตอมพอดี
แต่โดยประมาณแล้ว คิดอย่างคร่าวๆ
คุณมองมัน
ว่าใกล้กับ 1 หน่วยมวลอะตอมมาก
มันเป็นจริงสำหรับโปรตอนด้วย
เอาล่ะ หวังว่าคุณคงเข้าใจ
ความแตกต่างระหว่างมวลอะตอม ซึ่งก็คือมวล
และน้ำหนักอะตอม ซึ่งก็คือค่าเฉลี่ยถ่วงน้ำหนัก
ของไอโซโทปต่างๆ ของธาตุนั้นบนโลกแล้ว
ว่าคำนวณอย่างไร
และมวลของนิวตรอนโดยประมาณเป็นเท่าใด

English: 
It's not exactly an atomic mass unit,
but, roughly speaking,
in a lot of very broad,
high-level terms, you can kind of view it
as being very close to
one atomic mass unit.
And the same thing is true of protons.
Anyway, hopefully you now
have an appreciation for
the difference between atomic
mass, which is the mass,
and atomic weight, which
is the weighted average
of the various isotopes
of that element on Earth,
how to calculate it,
and roughly what the mass of a neutron is.
