Grade 9 Chemistry, Lesson 8 - Bohr diagrams - By Lumos Learning
Transcript
00:00 | Hey there . And welcome to Mr Lee Han teaches | |
00:02 | you stuff . This is grade nine chemistry lesson eight | |
00:05 | board diagrams . So if you're looking to make a | |
00:08 | board diagram of an element , the first thing you | |
00:10 | need to do is draw a circle , and this | |
00:12 | circle represents the nucleus in that circle . You're going | |
00:16 | to write the number of protons and neutrons that that | |
00:18 | element has . So let's choose an element . We're | |
00:22 | gonna take sulfur . So here's the box for sulfur | |
00:26 | and up at the top . Left says it has | |
00:29 | an atomic number of 16 , which means it has | |
00:32 | 16 protons , so we'll write 16 p in our | |
00:36 | circle . Next , we need to figure out the | |
00:38 | neutrons , so we'll take our big number . Subtract | |
00:42 | our little number . We get 30 to minus 16 | |
00:45 | is 16 neutrons , so he put 16 n . | |
00:50 | So the next thing we need to do is add | |
00:52 | the electrons . Now you need to remember that the | |
00:55 | number of electrons is equal to the number of protons | |
00:58 | . So since sulfur has 16 protons , we're gonna | |
01:01 | have to draw in 16 electrons and we put them | |
01:06 | in orbits or shells , and the first three shells | |
01:08 | can hold 28 and eight electrons and each shell must | |
01:15 | be filled before another shell can be started . So | |
01:19 | we need to start with the first two in the | |
01:21 | first shell and then at eight in the next shell | |
01:24 | , etcetera , and one last point . When we | |
01:27 | add electrons , we have to pair them up after | |
01:29 | half filling the shell . So let's get started . | |
01:33 | The first one can hold two , and we pair | |
01:36 | them up because it's more than half full . So | |
01:39 | we've got two electrons out of the way . The | |
01:40 | next shell can hold eight . So we put eight | |
01:45 | in the second orbit there and notice that they're all | |
01:49 | paired up because it's more than half full , mhm | |
01:53 | and then the third orbit we're already at . What | |
01:55 | is that ? 10 electrons . We need six more | |
01:57 | to make 16 . So we add six more electrons | |
02:02 | to that third orbit or that third shell and two | |
02:06 | of which are paired up . And then we have | |
02:07 | to before I guess , are paired up and then | |
02:10 | to sort of lonely , uncared electrons over there . | |
02:14 | So that's it . That's the board diagram for sulfur | |
02:18 | . So let's try a couple more . So now | |
02:20 | let's do a board diagram of lithium . So first | |
02:23 | we draw the nucleus , figure out how many protons | |
02:26 | and neutrons lithium has so little has got an atomic | |
02:30 | number of three . So we know it has three | |
02:31 | protons . We can write that in and next we | |
02:35 | need to figure out how many neutrons it has . | |
02:38 | It has an atomic mass , which is protons plus | |
02:41 | neutrons 6.94 So we round that up to seven . | |
02:46 | So it has seven minus three new drug seven minus | |
02:49 | three new drones , which is four . So long | |
02:52 | story short . Take the big number . Subtract a | |
02:54 | small number . You get the number of neutrons . | |
02:58 | Four . So next up is the electrons . How | |
03:03 | many electrons is gonna have ? It's gonna have the | |
03:04 | exact same number of electrons protons , so it's gonna | |
03:07 | have three electrons . So first we add up the | |
03:12 | first shell , and then we add more to the | |
03:14 | second . The first one can only hold too . | |
03:16 | So we put two in there , and then we | |
03:19 | only need one more . So we add one more | |
03:21 | in the powder shell and we are done . And | |
03:26 | remember , when we add electrons , we have to | |
03:27 | pair them up after half filling the shell But we | |
03:31 | don't need to do that yet because there was only | |
03:33 | one in that outer outer shell . So that's it | |
03:36 | for the board diagram of lithium . It's done . | |
03:39 | So now I want to show you a few tricks | |
03:40 | that you can use with the periodic table to help | |
03:44 | you create board diagrams . Um , so first off | |
03:49 | , the period the element is in will correspond to | |
03:51 | the number of orbits the board diagram will have . | |
03:55 | So if your element that you're creating is in the | |
03:59 | first period right here , it will have one orbit | |
04:05 | . If it is in the second period , anywhere | |
04:08 | in this highlighted yellow area , it will have two | |
04:12 | orbits or two shells . If it's in the third | |
04:17 | period , it will have three orbits and if it | |
04:21 | is in the fourth shell , and I only highlighted | |
04:24 | the first two because we were only doing board diagrams | |
04:27 | for the 1st 20 elements . But if it's in | |
04:30 | this fourth period , it will have four orbits , | |
04:35 | so that's just a quick little way to figure out | |
04:37 | how many orbits it's going to have . You can | |
04:39 | draw them in . Another fun fact is that if | |
04:42 | you count the number of elements in each period , | |
04:45 | it will match how many electrons are in that shell | |
04:49 | , so the first period has two elements in it | |
04:54 | , so there's only two electrons that will fill up | |
04:57 | that shell . For the second one . There's eight | |
05:02 | . So to fill up that shells you used eight | |
05:04 | electrons . The third one is also ate , so | |
05:08 | the third shell there has eight electrons in it . | |
05:12 | And then the fourth one I mentioned before , we're | |
05:15 | only doing the first two elements , so you don't | |
05:18 | ever have to put in two electrons in that fourth | |
05:22 | shell . So we'll give a demonstration of how this | |
05:26 | works . We're going to choose an element , and | |
05:29 | then we'll figure out what the board diagram would look | |
05:30 | like for that element . But unlike before , we're | |
05:33 | not going to use any information . We're just going | |
05:35 | to use its location on the periodic table to create | |
05:39 | a board diagram . So here we go . We're | |
05:41 | gonna pick this element , not even going to say | |
05:44 | what this element is . It doesn't matter . So | |
05:47 | let's figure out how to draw this element . It | |
05:51 | is in the third period , right ? It's three | |
05:54 | rows down , so we already know it has three | |
05:58 | shells or three orbits . Now in the first shell | |
06:05 | , it's going to have to electrons , so we'll | |
06:08 | put those in two electrons in the second shell . | |
06:12 | It has eight electrons , so we dry in eight | |
06:15 | electrons , and then in the third shell it has | |
06:20 | 12345 And then we stopped there because that's the element | |
06:24 | we're at . So we dry in five electrons , | |
06:30 | and if we count up all the electrons here , | |
06:33 | we'll see that there is 15 of them . So | |
06:36 | we know that it must have 15 protons as well | |
06:39 | . Um , now , without the periodic table , | |
06:41 | Uh , and the atomic mass . We can't really | |
06:45 | say how many neutrons are in here , but we | |
06:47 | got fairly far with this four diagram by just looking | |
06:52 | at a location on the periodic table . So I | |
06:55 | just wanted to show you how helpful it can be | |
06:56 | to have a periodic table around when you're creating board | |
07:00 | diagrams . So let's do a board diagram of oxygen | |
07:07 | . Oxygen has an atomic number of eight , so | |
07:09 | it has eight protons and electrons , and it has | |
07:13 | an atomic mass of 16 . So it has 16 | |
07:16 | minus eight , which is eight new tribes . So | |
07:20 | here's our nucleus eight p . Eight n If we | |
07:24 | look at our periodic table , there's oxygen . It's | |
07:27 | in the second row , which means , well , | |
07:31 | the second period . Rather so it has two orbits | |
07:35 | , two shells . The first shell is going to | |
07:40 | have two electrons in it , and we need to | |
07:42 | add up to eight . So we need six more | |
07:45 | , and we add those extra six in the next | |
07:48 | orbit and we are done . There is a board | |
07:50 | diagram of oxygen now . Valence shells and valence electrons | |
07:57 | are very important in chemistry . The outermost shell , | |
08:00 | or orbit of an atom is called the Valence shell | |
08:04 | , and the electrons in it are called valence electrons | |
08:07 | . So this right here is the valence shell , | |
08:09 | the outer shell or the outer orbit . I've been | |
08:11 | calling them orbits . That's the valence shell , and | |
08:15 | any electrons in that shell are valence electrons . And | |
08:20 | they're important because these are the ones that react with | |
08:23 | other atoms . So when there's a chemical reaction of | |
08:27 | some sort , the reason that chemical reaction is happening | |
08:30 | is because the valid shells of an atom are interacting | |
08:35 | . Now let's take a look at the patterns of | |
08:38 | the valence electrons in the periodic table . So if | |
08:41 | we look at the board diagrams of a period on | |
08:44 | the periodic table . We can see that the number | |
08:46 | of Valence electrons increases by one each step to the | |
08:50 | right . So in the first row are the first | |
08:55 | period we have one and then two Valence electrons . | |
08:58 | In the second period we have one and then two | |
09:02 | and then 345678 electrons in the Valence shell . And | |
09:10 | then in the next period we have 12345678 electrons in | |
09:16 | the valence shell . And then in the fourth period | |
09:20 | , we only have one and then two . And | |
09:22 | then we stopped there because we stop at 20 . | |
09:25 | So we can also see from looking at these board | |
09:28 | diagrams that the number of Valence electrons is the same | |
09:32 | for every element in a group or column . So | |
09:36 | for the first column there , the first group , | |
09:38 | those are the alkali metals . There is one Valence | |
09:43 | electron for the second group , the alkaline earth metals | |
09:49 | there is too failing to electrons , and that's the | |
09:52 | same for that whole group . And the pattern keeps | |
09:55 | going from there goes 34567 and then a full valence | |
10:01 | shell . We say it's eight , but that top | |
10:04 | one there only has to , uh , but that's | |
10:07 | a full valence shell for the last column there . | |
10:11 | Now It's important because the number of valence electrons determines | |
10:16 | the way the elements combined to create compounds . And | |
10:19 | remember that each one of the columns in the periodic | |
10:22 | table all have elements that behave very similarly chemically , | |
10:27 | and those two things are linked . So the reason | |
10:29 | why they behave similarly in a chemical reaction is because | |
10:33 | they have the same number of valence electrons . Now | |
10:37 | , if we take a look at the noble gases | |
10:39 | on the far right of the table , each of | |
10:43 | these noble gases has the maximum number of electrons in | |
10:46 | their valence shell , and this is what makes them | |
10:48 | very un reactive . So if you take a look | |
10:52 | , they can't fit any more electrons into their outer | |
10:54 | shell , and this is why they don't react with | |
10:59 | anything . The whole reason elements react with each other | |
11:02 | is so that they can fill up their valence shell | |
11:06 | . These guys already have full valence shells , so | |
11:09 | they have no interest in interacting with any other elements | |
11:12 | at all . So that's why they run reactive . | |
11:16 | All right , so that's it for this video . | |
11:18 | Tune in for the next video on isotopes and ions |
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