Tutorial:Basic Chemistry Topics: Difference between revisions
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==Ionic Bonds== | ==Ionic Bonds== | ||
[[Image:Ionic bond.png| thumb | right | 300px | Ionic Bonding | [[Image:Ionic bond.png| thumb | right | 300px | Ionic Bonding]] | ||
An ionic bond is an attraction between two molecules of opposite charge. The opposite charges are positive (+) and negative (-). A positively charged atom is referred to as a cation, and a negatively charged atom is referred to as an anion. To the image to the right, you can see a negatively charged Fluorine (F) and the cation Sodium (Na). These two atoms are attracted to each other due to there opposite charges. The double-sided arrow between them is representation of there attractive force. | An ionic bond is an attraction between two molecules of opposite charge. The opposite charges are positive (+) and negative (-). A positively charged atom is referred to as a cation, and a negatively charged atom is referred to as an anion. To the image to the right, you can see a negatively charged Fluorine (F) and the cation Sodium (Na). These two atoms are attracted to each other due to there opposite charges. The double-sided arrow between them is representation of there attractive force. | ||
In this representation the pink depicts the negatively charged (anionic/acidic) portion of the molecule and the yellow represents the positively charged (cationic/basic) portion of the molecule. Through this representation you will notice that the charges are evenly distributed. They are evenly distributed because the positive and negative charges are attracted to one and other, while the positive-positive and negative-negative charges repel each other. The repulsion of common charges and the attraction of oppositely charged atoms/molecules is what causes them to distribute evenly. <scene name='Tutorial:Basic_Chemistry_Topics/Ionic_bond/3'>positive and negative charges</scene> | In this representation the pink depicts the negatively charged (anionic/acidic) portion of the molecule and the yellow represents the positively charged (cationic/basic) portion of the molecule. Through this representation you will notice that the charges are evenly distributed. They are evenly distributed because the positive and negative charges are attracted to one and other, while the positive-positive and negative-negative charges repel each other. The repulsion of common charges and the attraction of oppositely charged atoms/molecules is what causes them to distribute evenly. <scene name='Tutorial:Basic_Chemistry_Topics/Ionic_bond/3'>positive and negative charges</scene> | ||
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==Hydrogen Bonds== | ==Hydrogen Bonds== | ||
[[Image:3D hydrogen Bonding.jpg | thumb | left | 200px | Hydrogen Bonding | [[Image:3D hydrogen Bonding.jpg | thumb | left | 200px | Hydrogen Bonding]] | ||
Hydrogen Bonds, the weakest of bonds, are attractive interactions between an electronegative atom and hydrogen. Electronegative atoms are atoms that have high electron density. They are strong atoms that pull electrons towards them from weaker/low electron density atoms, such as hydrogen. When the electronegative atom pulls the electrons, it leaves the other atom with a slightly positive charge. Water is the most common example of hydrogen bonding. The water molecule chemical formula is H2O. The highly electronegative oxygen pulls the hydrogen closer by attracting hydrogen’s electrons and allowing the formation of a water droplet. The electronegative atoms allow for the droplet to be held together instead of spreading. In this representation the hydrogen bonds are represented as yellow-dashed lines. The hydrogen bonds are important to the stability of the secondary structures. <scene name='Tutorial:Basic_Chemistry_Topics/Hydrogen_bonds/2'>Hydrogen Bonds</scene> | Hydrogen Bonds, the weakest of bonds, are attractive interactions between an electronegative atom and hydrogen. Electronegative atoms are atoms that have high electron density. They are strong atoms that pull electrons towards them from weaker/low electron density atoms, such as hydrogen. When the electronegative atom pulls the electrons, it leaves the other atom with a slightly positive charge. Water is the most common example of hydrogen bonding. The water molecule chemical formula is H2O. The highly electronegative oxygen pulls the hydrogen closer by attracting hydrogen’s electrons and allowing the formation of a water droplet. The electronegative atoms allow for the droplet to be held together instead of spreading. In this representation the hydrogen bonds are represented as yellow-dashed lines. The hydrogen bonds are important to the stability of the secondary structures. <scene name='Tutorial:Basic_Chemistry_Topics/Hydrogen_bonds/2'>Hydrogen Bonds</scene> | ||
