Chemical Bonds - Video Tutorials & Practice Problems
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A chemical bond is the connection of different elements through the sharing, transferring or pooling of electrons.
Chemical Bond Classifications
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concept
Chemical Bonds
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Chemical bonds can be seen as the attractive force that holds atoms or ions together in a chemical compound. Now, the driving force of these types of chemical bonds, We're going to say when elements bond, they're either trying to lose, gain, or share electrons to attain a filled outer shell like the noble gases. Remember, the noble gases are perfect. All the elements that are not noble gases will do things in order to achieve the same type of electron arrangements as these noble gases. This is the driving force behind chemical bonds. In the next series of videos we'll see the different types of chemical bonds exist and see do they lose, gain or share electrons to obtain the same kind of configuration as our noble gases.
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concept
Chemical Bonds
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Now ionic bonding represents a type of chemical bonding. Here, the attractive force is between the opposing charges of a cation, which is positive, and an anion which is negative. We're gonna say here, recall that metals tend to lose their valence electrons and nonmetals tend to gain electrons. We're going to say here that ionic bonding itself, the ionic bond formation helps to lower the potential energies of the cation and the anion. This lowering of energy basically entails them releasing their excess energy. This releasing of energy can be thought of as an exothermic reaction. So when we talk about thermochemistry and we're talking about the releasing of energy, we use the term exothermic. So if we take a look here, we have sodium and we have chlorine. Sodium is a metal, sodium will want to give away its electron so that it becomes plus 1 and becomes more like a noble gas. So it gave up its electrons so now it's plus 1. Chlorine has its 7 original electrons and it just gained that electron from sodium. So now it has one additional electron and that gives it a minus one charge. It's their opposing charges. Remember, opposites attract. Their opposing charges is what makes them attracted to one another. So because of this, they will combine together to give me sodium chloride as my ionic solid. So just remember, when it comes to my ionic bond, we first have to have the transferring of the electron from the metal to the nonmetal to create opposing charges. Those opposite charges cause the ions to combine together to form my ionic compound at the end.
Ionic bond occurs through a transfer of an electron from a metal to a non-metal in order to create opposing charges.
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example
Chemical Bonds Example 1
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Here we're asked which of the following species has bonds with the most ionic character? So think about it. When we talk about ionic bonding, we said it's the opposing charges of a cation and an anion. Remember, the cation, which is positive, is usually a metal. It can also be the ammonium ion, and then remember our anion, our negative ion will be a nonmetal. These are the fundamental definitions we talked about way back when we first covered covered ionic compounds versus covalent compounds. So if you don't remember that, good idea to write this down. So basically the multi ionic character will be the one that fits this definition of a cation bonded to an anion. So we're looking for an example that has either a metal connected to a nonmetal or the ammonium ion connected to a nonmetal. And if we look at our choices present, we see that the only choice has to be option c because here it has tin, which is s n, a metal, connected to oxygen, a nonmetal. So we have in this example a metal to a nonmetal. All the others don't fit the criteria to be an ionic compound because they're just nonmetals connected together. They themselves would just represent covalent compounds.
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Problem
Problem
The strength of an ionic bond comes principally from:
a) The converting of atoms into compounds.
b) The movement of electrons from cations to anions.
c) The mutual attraction of opposite electrical charges.
d) The sharing of electrons.
A
The converting of atoms into compounds.
B
The movement of electrons from cations to anions.
C
The mutual attraction of opposite electrical charges.
D
The sharing of electrons.
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concept
Chemical Bonds
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Covalent bonding represents a type of chemical bonding. Here we have molecular bonds involving the sharing of valence electrons between nonmetals. Now if we take a look here, we have 2 chlorine atoms and 2 oxygen atoms. Chlorine is in group 7 a. It just needs one more electron to become just like argon, the noble gas next to it. So how can it gain that one electron? What it does is it teams up with another chlorine or another element and it's going to share one of the electrons from its neighbor. So here, the 2 chlorines, they're both gonna share an electron with each other. So here are our chlorines and they're sharing one electron with each other. Neither one has sole possession of both electrons, they're sharing the electrons together. So in essence, they both have reached the same number of electrons as argon. They're they're fulfilling filling out their outer shell and being like a noble gas. Oxygen. Oxygen is in group 6 a, so it needs 2 more electrons to become just like neon. What does it do? It decides to share its 2 electrons with another oxygen. So here are our oxygens and they're sharing their electrons with one another, And in that way, they've achieved in a filled outer shell just like neon, the noble gas closest to them. And notice here that these elements are forming single bond between each other with the chlorines and a double bond between the oxygens. As we delve deeper and deeper into different types of chemical compounds, we'll learn about the bonding preferences found between different elements. But remember, it's always trying to form the optimal number of electrons to help fill out their outer shell and become just like a noble gas, at least when we're talking about covalent bonding. So just remember, covalent bonding involves nonmetals sharing electrons with one another.
Covalent bond involves sharing of the valence electrons between two non-metals, giving both a filled outer shell like a noble gas closest to them.
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example
Chemical Bonds Example 2
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Which of these elements is unlikely to form covalent bonds? So we have here sulfur, we have hydrogen, we have potassium, we have argon, and we have silicon. So remember, covalent bonds are the sharing of electrons between nonmetals between nonmetals. So if we take a look here, sulfur is a nonmetal so sulfur could form covalent bonds. Hydrogen is a nonmetal. Potassium is a metal. We said that it's between nonmetals. So this can't ever form covalent bonds. Let's look at the other options. We have argon and then we have silicon. Argon is a non metal. Silicon is a metalloid. Now technically remember metalloids share characteristics of both metals and nonmetals, and we'll see that because it's a metalloid and shares some nonmetal characteristics, there is the potential to form covalent bonds. Alright. So e has the potential. C can't ever have the potential in forming covalent bonds because it's strictly a metal. So just remember, when it comes to covalent bonding, it's the sharing of electrons between elements that have nonmetallic characteristics.
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concept
Chemical Bonds
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Metallic bonding represents another type of chemical bonding, but the name is a little bit deceiving. It's not really metals bonding together. What it is, it's the attractive force between free floating valence electrons and positively charged ions on metal surface. Now metallic bonding is important because it's responsible for the unique physical properties of metals such as their malleability or their conductivity. If we take a look here at this image of metallic bonding, we have our positive ions on the surface of the metal and moving freely around are these negative electrons in green. Now these electrons are not confined to each other metal or, positively charged ions. They can actually move to the other ones. They're moving around freely. So metallic bonding is a little bit different from the chemical bonding we're accustomed to seeing.
Metallic bond occurs through attractive force between free flowing valence electrons and positively charged ions on metal's surface.
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example
Chemical Bonds Example 3
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Which of the following is the best description of the free flowing electrons and metallic bonding? So here a, core electrons that can move freely between metal ions. Remember, we said it's valence electrons. The electrons that are found on the outer shell in terms of the element or ion. So this doesn't make sense. So a is out. B would also be out because again it's including core electrons. Valence electrons that can move freely between metal ions, that's what we showed in the picture. Those, valence electrons are not confined to each one of their those positive ions. They can move around between them. So c is a good description. D, valence electrons are bond to metal ions. They're not bound, they can freely move around. And then e, again core electrons are bond to the metal ions, yes, but metallic bonding has to do more with the free flowing of valence electrons between positive ions. So c is the best description of metallic bonding.
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Problem
Problem
Which of the following is not a physical property attributed to metallic bonding?