Periodic Table Charges Review - Video Tutorials & Practice Problems
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1
concept
Periodic Table: Charges
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Now the elements of the periodic table will either lose or gain electrons to become just like the noble gases. Now, remember, your noble gases are the elements that are found in group 8 a or group 18. K. So remember, 2 different ways to describe the same column of the periodic table. The reason these elements want to become the noble gas is because noble gases themselves have the optimal number of outer shell electrons. What that means specifically, we'll talk about several chapters from now, but just realize when it comes to the elements, they'll either lose or gain electrons so so that their number of electron matches one of the nearest noble gases. Now we're going to say here when it comes to metals, metals tend to lose electrons to become positively charged ions called cations. Here, just think of it like this, cations at t could represent the positive charge that the ion gains. And it makes sense because if you're losing negatively charged subatomic particles in the form of electrons, you're gonna become more positively charged. Now metals themselves, metals can have either one type of positive charge or multiple types of positive charges. When a metal possesses one charge, we refer to them as type 1 metals. When metals have multiple charges, then they're referred to as type 2 metals. We'll go in greater detail on what types of metals are type 1 metals and what other types of metals are type 2 metals. Now if metals lose electrons, then nonmetals must be gaining electrons. So nonmetals tend to gain electrons to become negatively charged ions called anions. Remember, again, this makes sense. I'm gaining negatively charged electrons, so I'm gonna become more negative as a result. So just remember, the whole reason elements gain and lose electrons is to become just like the noble gases. In the next video, we'll see exactly how many electron will we lose or gain for any particular element.
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Periodic Table Charges Review Example
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So for this example question it says, from what you know about ion formation in the periodic table, which ion would be unlikely to occur? So before we look at this question, remember, we're gonna say that metals, they tend to lose electrons. So if they're gonna lose electrons, they're gonna become positively charged and remember, non metals tend to gain electrons and therefore become negatively charged. So if we take a look here, we have r b. Looking on a periodic table, we know that r b is a metal, and therefore, it makes sense that it would have a positive charge. So this is a likely, setup for RB ion. Next, oxygen. Oh, oxygen is a nonmetal. Nonmetals tend to gain electrons and become negatively charged. So this is reasonable. M n. M n is a metal. Again, metals tend to lose electrons to become positively charged, so that positive charge is a possibility. A l. A l is aluminum. Aluminum is a metal. Again, metals tend to lose electrons to become positively charged. So it doesn't make sense that a l would have a negative 3 charge here. So this is unlikely. So this would be our answer. Then if we look at the last one, cl chlorine, chlorine is a nonmetal, so it makes sense it could gain electrons to become negatively charged. So just remember remember, metals tend to lose electrons to become positively charged, nonmetals tend to gain electrons to become negatively charged. K. Now that we know this fundamental idea, let's move on to our next video where we go into how many electrons do they gain, how many electrons do they lose, and in that way know what type of ions are possible for certain types of elements.
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Main Group Elements
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So let's talk about first our main group elements. Remember, your main group elements are the elements found in group 1 a or group 1, 2 a or group 2, and then from 3 a to 8 a, or what we call groups 13 to 18. The elements here in the grayed out box, those are our transition metals. We'll talk about those later on. But for right now, let's just focus on our main group elements. Now recall that the atomic number which uses the variable z of an atom equals the number of protons within its nucleus. For example, we'd say that beryllium has an atomic number 4 so it has 4 protons. For a neutral element, its number of electrons is equal to its number of protons. So beryllium here has an atomic number of 4 which means it has 4 protons, and here, if we're dealing with a neutral element, it'll have the same number of electrons, so it'll also have 4 electrons. Now, we said that all these elements of the periodic table are all trying to become just like our noble gases, our group 8 a elements. They have the optimal number of electrons. Helium has 2, neon has 10, argon has 18, and as we go down, these are all their atomic numbers, which gives us the number of electrons they have. Now elements try to gain or lose electrons to match each number of electrons for the noble gases. So noble gases, since they're perfect, their their charge is 0. So they don't have a charge. They don't need to gain or lose electrons. Let's look at group 7 a, all the elements in group 7 a. Fluorine, let's look at f. Fluorine has 9 electrons when it's neutral. If it wants to have 10 electrons like neon, it would have to gain 1 electron. Chlorine has 17 electrons with neutral. To have 18 like argon, again, it would have to gain 1 electron. So each element in this column would have to gain 1 electron to become like the noble gas next to it. By gaining that one electron, they would get an a charge now of minus 1, because, remember, gaining electrons gives us a negative charge. Oxygen oxygen when neutral has 8 electrons, to have 10 electrons like neon, how many electrons would it need to gain? If you said 2, you'd be right. So same thing with sulfur, it has 16. It'd have to gain 2 electrons to become just like argon. So this group 6 a, its charge is normally negative 2. Nitrogen has 7, so to get to 10 it'd have to gain 3 electrons. So this char the charge of this group is normally minus 3. Now, of course, some of these groups it gets tricky because in group 5, we see that we have nonmetals here, so they have a negative 3 charge, but then we have metalloids and then we run into metals. Metals don't wanna have a negative charge. They wanna have a positive charge. So these negative charges, when we're referring to them, is predominantly with the nonmetal, the blue species, the elements that are in the blue boxes. Group 4 is a little bit tricky. So group 4 is equal distance, either way. What What I mean by that is carbon could try to gain 4 electrons to become like neon or it could try to lose 4 electrons so that it has 2 like helium. So it's kind of in a special situation. So as a result of this, we kinda just say non applicable to group 4 based on the location in the periodic table. Now, though, we do have an exception that that's around, exception 1, and this pertains to lead and tin. Lead and tin are here, s n and p b. Okay? Because of where they're located, how far down they are, they kinda have characteristics similar to transition metals. They can either be plus 2 or plus 4 for their charges. So just remember when it comes to tenant lend, they can be plus 2 or plus 4. They're, interesting situation when it comes to the periodic table and charges. Now let's look at boron and the other elements that are within this group. Boron is a metalloid. Metalloids, they have characteristics of both metals and nonmetals, so it's a bit tricky with them. So we won't be talking about boron, but we can talk about the elements below boron, aluminum all the way down to n h. They're all metals, so they all wanna lose electrons to become like a noble gas. Now aluminum here, its atomic number is 13. So when it's neutral, it has 13 electrons. It has 2 choices. It can either try to gain 7 electrons to get to okay. I mean, not 7. It could try to gain 5 electrons to have 18 electrons just like argon, or it could do something easier than that. Instead of trying to gain 5 electrons, it could just try to lose 3 electrons, so that it has 10 electrons like neon. And when it comes to chemistry, we chemistry, we always go in the path that's easiest and fastest. Okay. So it's easier for aluminum to lose 3 electrons than to loop to gain 5 electrons, okay, because it's more spaces that you have to jump to become a noble gas this way. Easier just to let go of your 3 electrons. So because of this, this group tends to be plus 3 for its charge. Beryllium. Let's look at Beryllium. Beryllium has an atomic number of 4, so it has two choices. It can either try to what? Gain 6 electrons, 1, 2, 3, 4, 5, 6, to become like neon or do something easier. Just lose 2 electrons so that it has 2 electrons just like helium. So the easier and shorter path is to lose electrons. So it's this this group tends to be plus 2. Then finally, again, we're talking about the metals. They're the ones who wanna lose electrons to become positive. Hydrogen is not an a metal, so we don't talk about hydrogen in this regard, but we'd say that lithium could try to gain 7 electrons to get to 10 like helium, which is a long distance to cover, or the easier thing would be just to lose 1 electron and become like helium. So this group tends to be plus 1. So these are the charges that you need to commit to memory when it comes to these different groups. Group 1 a plus 1, group 2 a plus 2, then plus 3. 4th group is not applicable. Group 5 a is minus 3, then minus 2, then minus 1. Noble gases are perfect, so they don't wanna gain a charge. Now exception 2, we're gonna say this pertains to our heavy metals of bismuth, polonium, and those that have atomic numbers from 114 to 118. Because of their position on the periodic table, they're a little bit weird and they have multiple types of charges, so we tend not to talk about them. But when it comes to main group elements, just keep in mind the major charges that we've listed, plus 1, plus 2, plus 3, minus 3, minus 2, minus 1, and then, of course, your exception 1. This is what you need to take away from the main group elements and their various charges.
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example
Periodic Table Charges Review Example
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So for this example question, it says predict a charge that a gallium ion would possess. So we know it has a charge because it's using the term ion. Now gallium, remember, gallium is element symbol is Ga. Gallium itself is in group 3 a, or what we known as group 13. Now remember, in this group, it's easier to lose electrons because most of the elements in this group are metals, and it's easier for them to lose 3 electrons in order to be like the nearest noble gas. So here, this group 3 a normally tends to be plus 3 in terms of charge. Because of this, option c would be our correct answer.
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Problem
Problem
Which element possesses a -2 charge when it combines with other elements?
A
Ca
B
Mn
C
P
D
Se
E
F
6
concept
Transition Metals (Type II Metals)
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2m
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So remember, type 2 metals are metals that possess multiple charges. Now we're gonna say most transition metals have varying positive charges because of their electron arrangements around the nucleus. Now, there's gonna be more advanced explanations for this later on, but we'll discuss them in much later chapters. So just remember, when it comes to type 2 metals, a majority of them are the transition metals. They have multiple charges. So here if we take a look, we have some of the most common types of transition metals, and what we need to realize is that although many of them have multiple charges, there are quite a few that do possess only one charge. So, for example, scandium, which is in group 3 or 3 b, it's plus 3, and there's some similar chemical properties going on for elements within that group. Because scandium is plus 3, that means the other metals that are in this group with it are also plus 3. But then, of course, when you look at other transition metals, you're gonna see a bunch of charges like, manganese, for example, could be plus 2, plus 3, plus 4, plus 5, or even plus 7. Now the way we're able to tell which one of these charges manganese will have will be dependent on the other element it's connected to. We'll learn about that later on. But just realize here that these transition metals are called transition metals because they have a bunch of possible charges. Now besides the elements in group 3b or 3, we also have silver, cadmium, and zinc. Although they're transition metals as well, they also have only one particular charge. So silver when it's an ion, it's going to be plus 1. Cadmium and zinc, they're both in the same group again, so so they're going to be similar to each other. Both of them will be plus 2 when they do have a charge. So again, transition metals, a lot of them have multiple possible charges, and because of that they're characterized as being type 2 metals. Some of the transition metals, the ones in red, they possess only one charge. They are transition metals, but they're not type 2 metals because they don't have multiple charges. So keep this in mind when we're confronting different types of transition metals. Some have the potential to have multiple charges.
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example
Periodic Table Charges Review Example
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1m
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So if we look at this example question, it says predict the major charge of an ion if it were discovered to be in period 10, group 3 b. Alright. So something that might jump out at you when you look at this question is the fact that we're talking about a period 10 element. But we know that when we look at a periodic table, there's only 7 rows. So our periodic tables only go up to period 7. So where is this period 10 coming from? Well, remember, I discussed earlier that the periodic table is dynamic. It changes over time because we are either going to discover new elements or create new elements. The number of roles will over time increase, so there is a chance that we will create an element, or maybe there's an element that already exists that is located in period 10. But that's not the important part of this question. The important part is the group that it's in. It's in group 3 b. So remember we talked about this up above, group 3 b, this contains the element scandium, and it has a charge of plus 3. And we said that there's something special about that group 3 b. The other metals in that group would also possess a charge of plus 3. So here, that would mean that option e would be my correct choice. So remember, a lot of the transition metals have multiple charges, but there are some patterns that we can observe when looking at different transition metals, one of them being elements from group 3 b having a charge of plus 3.
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Problem
Problem
What is the likely charge of the element with an atomic number of 47?
A
+4
B
+3
C
-1
D
+1
E
+2
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Problem
Problem
How many electrons would the cadmium ion possess?
A
50
B
48
C
46
D
52
E
30
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