Tutorial:Basic Chemistry Topics: Difference between revisions
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An ionic bond is an attraction between two molecules of opposite charge. The opposite charges are a positive (+) and a negative charge (-). A positively charged atom is referred to as a cation, and a negatively charged atom is referred to as an anion. In this representation the pink represents the negatively charged (acidic) portion of the molecule and the yellow represents the positively charged (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, forming ionic interactions. | An ionic bond is an attraction between two molecules of opposite charge. The opposite charges are a positive (+) and a negative charge (-). A positively charged atom is referred to as a cation, and a negatively charged atom is referred to as an anion. In this representation the pink represents the negatively charged (acidic) portion of the molecule and the yellow represents the positively charged (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, forming ionic interactions. | ||
Hydrogen Bonds, the weakest of bonds, are attractive interactions (dipole-dipole) 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. | Hydrogen Bonds, the weakest of bonds, are attractive interactions (dipole-dipole) 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. | ||
