Transcription
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We decided on a chemical bond as the set of electrostatic and magnetic forces that hold atoms and molecules together to achieve stability. That is, if we know that in a free state they have a lot of energy, then it is very good that through the formation of the bond, that level of energy is lowered. In this way, much more stable compound structures or molecules are obtained.
We can differentiate three types of biological chemical bonds, such as the law of pymetal and CCOO, to be able to know which of these three cases it is going to be about if we see a compound or a molecule. That's why we're making this video; we're going to learn to differentiate in a reasoned way.
As you know, it's the ionic, metallic, and covalent bonds. Welcome to the Arantza Education channel and this chemistry video that I invite you to watch here. We're going to finish with a super final that you will love, and if you like it, you can leave me a comment, you can share it on the networks, and now we begin.
We will also explain the characteristics of each of these types. The ionic bond occurs from a metal and a non-metal, and it also goes to produce an electron management of an atom. The covalent bond occurs in a metal and non-metal and involves sharing electrons. In the metallic bond, it will occur between a single element, and they have to be metallic. That is, it will occur between metal and metal.
To be able to understand what we are talking about when we talk about metals and non-metals, we have the periodic table here. We are going to learn first of all how to differentiate which areas are occupied by metals and which by non-metals.
In this area that I have marked here in orange are the metals. They reveal themselves periodically, except for this first box, which is occupied by hydrogen and is a non-metal element. In addition, this area I have marked here in blue is occupied by the non-metals, and here are the semi-metals.
So for these links, the key that we need is to know which elements are metallic and non-metallic. We are going to base this exercise on that today, in which we are given several compounds. We are going to see several compounds, molecules, or elements, and we are going to see what type of bond is going to be involved in each case.
So we are going to go with the first one, which is magnesium chloride. The first thing we are going to do is identify the position of each of the elements that make it up on the periodic table. This compound, and we are going to see what type of bond it is going to be about.
Then we are going to see the magnesium. Magnesium occupies this group 2, the alkaline earth metals. It is one of the alkaline metals. Then we are going to be talking about that it is a metal. Chlorine is in this group 7, the halogens. Chlorine is going to be a non-metal.
We are going to have the metal plus non-metal. We are going to notice here that the ionic action is between the most metallic metal. Then we are going to be talking in this case about ionic bonding.
We are going to see what these ionic bonds are based on. We have said that there is a management of electrons from one socket to another. Why does this happen? Well, because it occurs between two elements that are going to have very different electronegativities.
That is to say, non-metals such as chlorine have a great tendency to attract electrons since it has 7 electrons in its last layer. Chlorine is a halogen and has 7 electrons, so to obtain the noble gas configuration, it only needs 1.
Then it has a great tendency to capture this electron, while magnesium has only 2 electrons in its last layer. To get the stable electronic configuration and stay with 8 in the last one, what it will have a tendency to do is to lose those electrons.
In this way, both would already have a stable electron configuration with 8 electrons in the last shell and would comply with the octet rule. We will see it graphically. Magnesium would have two valence electrons; it is in group 2, which means that it has 2 valence electrons.
The valence electrons are represented with some points according to the Lewis structures. On the other hand, we would have two chlorine atoms. That is to say, we will have chlorine and chlorine. The chlorine atom has 7 valence electrons, represented as 2, 3, 4, 5, 6, and 7.
The other chlorine will also have 7 because it is going to bond with magnesium. These magnesium electrons are going to go one with this chlorine and the other one goes with this chlorine so that the magnesium will remain with a stable configuration.
Giving them to chlorine, chlorine will also have it since it will have 8 electrons. As the unit, magnesium, when losing the electrons, will remain positively charged.
That is, it will be the cation. The chlorine, when receiving each one of these electrons, will remain negatively charged. That is to say, they will receive electrons and they will be the anions.
We are going to learn now that chlorine with its 8 electrons will have three branches charged negatively. That is to say, both chlorines will have a negative charge.
In this way, we already know that it is the ionic bond and that it has been due to a transfer of electrons. That is to say, magnesium has given up the electrons; it has transferred them to the chlorine.
In this way, what we are going to be left with are positive ions and negative ions, which is what causes the bond to form because opposite charges attract.
We are going to talk about the following compound that we have here, which is ammonia. In this case, we are going to see where hydrogen and nitrogen are. Nitrogen is in group 5, so it is a non-metal.
We have also said that hydrogen, which is in this position, occupies the first box of the table, is also a non-metal. So, being non-metal plus non-metal, we are in this case, that is, it will be covalent bonds.
In this case, what will happen is that there will not be a transfer, as in the previous ionic bond, but rather there will be a sharing of electrons to achieve that stable electronic configuration with 8 electrons in the last layer for nitrogen and with 2 electrons in the last layer for hydrogen.
Hydrogen, as if only with one electron, will need to share to have the complete layer with two. It would be then symbolized in the following way. We will have that nitrogen has, in total, 5 valence electrons.
The valence electrons are represented with dots around the element symbol. For hydrogen, we will place a hydrogen, a hydrogen, and a hydrogen, and they will share an electron. Nitrogen will have its 8 electrons; it will have the noble gas configuration.
In this way, the link can also be represented, achieving by sharing electrons a very stable electronic configuration. Then we have said that in this case it is about a covalent bond in which electrons have been shared.
There has been no transfer, as in the ionic case. Let's go with this last example, the metallic bond. We have metal plus metal. In this case, we are going to have a single metallic element.
If we have copper atoms here, the copper atoms will remain positively charged because the electrons that are in the valence shell are going to be delocalized around the atoms. They are not going to be lost; they are not going to be shared.
In this case, in the metallic bond, the valence electrons are going to leave that last shell and are going to be placed forming an electronic cloud between all the nuclei of those metal atoms, which will form the metallic structure.
It is a very stable structure, and then a metallic bond will be formed. Well, let's work now on these examples to identify in a reasoned way the type of bond.
You can try to solve it, and if not, now below yours, I will explain the solution. Well, let's look at the first case. Here we have zinc oxide.
First of all, we have to look at the position occupied by each of these elements. We will know that oxygen is here in group 6, and it is a non-metal. Zinc is in this zone of the transition elements, so it is a metal.
This whole zone is occupied by metals. That is, a metal plus non-metal will result in an ionic bond.
In the second example, we have sulfur, which occupies the following position. It is in this area, and in that area, there are also non-metals. We are going to have non-metal plus non-metal, so it will be a covalent bond.
Here we have bromine. Bromine occupies this group of halogens. We will have two bromine atoms, which is a molecule.
So it will be non-metal plus non-metal, and this is also going to be a covalent bond. Now we are going to see potassium iodide. Iodine, which is in group 7, is a non-metal element.
On the other hand, lithium, which belongs to group 1, is also a metallic element. So we have metal plus non-metal, which will result in an ionic bond.
We have silver plus silver. Silver is one of the transition elements, and being in this group, we all know that silver is a metal.
Then, because it is metal plus metal, it will be a metallic bond. In this last one, we have magnesium, which is a metal, and we have oxygen, which is a non-metal.
So we are not going to have metal anymore.
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Chemical bond introduction to the chemical bond: ionic, covalent, and metallic. We define chemical bond as the set of electrostatic and magnetic forces that hold atoms together in molecules to achieve stability.
There are three types of chemical bonds: ionic, covalent, and metallic. [Music]
We must know where non-metals and metals are placed in the periodic table to identify these types of bonds. Metals occupy the orange-colored area in this table, and the non-metals occupy the blue area.
In addition, hydrogen occupies the first box of the periodic table and is also a non-metal. In the ionic bond, the main characteristic is that there is a transfer of electrons, and a unique crystalline network is formed.
For example, in sodium chloride, when the transfer of electrons occurs from the metal to the non-metal, two positive sodium ions and negative chloride ions are formed.
In the covalent bond, or metal plus non-metal, electrons are shared, and molecules or crystals are formed. For example, in hydrochloric acid, where there is a simple covalent bond, a molecule is formed.
The metallic elements, such as silver, copper, gold, and iron, form a metal network.
Until this video arrived, in which we have learned to differentiate the type of bond. If you liked it, you can leave a like or a comment, and you can share it on the networks.
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