Bonding And Structure
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Created by:
failing123 on March 15, 2012
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35 terms
Terms | Definitions |
|---|---|
 Chemical Bond | is *ANY* force of attraction between atoms or molecules |
| intramolecular bonding | bonds that hold the atoms within the molecule together. |
| intermolecular bonding | bonds that hold molecules between molecules together. |
| IMFs | are strong intermolecular forces, which give off a substance cohesion |
| In solids and liquids cohesion is.... | strong force |
| in gases cohesion is... | lacking |
| Electronegativity | an atom's attraction for nearby electrons in a compound. It can not be measured |
| Electronegativity in Metals | very low can't hold on to electrons very well electrons are often lost when they interact with other elements. |
| Electronegativity in Non-Metals | compared to metals have high level hold on to electrons very well they often steal electrons from other elements that they interact with. |
| Charge Transfer | Metal to the Non-Metal |
| Effect of Charge Transfer | Metals electrons are stolen by the non-metals, making the metals cation. this leaves the non-metals as anions |
| Anions are? | negative, more electrons |
| Cations are? | positive, less electrons |
| Ionic Bonding | is the charge transfer which takes place ONLY between NON-METALS and METALS |
| Covalent Bonding | Electron Sharing between NON-METAL AND NON-METAL they share their electrons, because they both refuse to loss any electrons, so instead they share them. they use these shared electrons to fill their valence shell. (Octet Rule) |
| Metallic Bonding | Between METAL AND METAL since the metals want to lose their electrons, the electrons drift in the Sea of Electrons. |
| Sea of Electrons | is what holds the positive nuclei together. |
| Lewis Dot Structures of atoms | a simple diagram showing how that valence electrons of that atom are arranged. With a LDS you can predict the bonding behavior of that element. |
| Valence Bond Number | equal to the number of unpaired electron dots in the LDS.??? |
| Unpaired Electrons | the amount of them is equal to the valence bond number |
| Lone Pairs | electrons that are paired on an atom are both tied up with each other; so they can be shared with electrson on other atoms. |
| Monatomic Ion LDS | if the charge is negative, then add that number to the number of electrons the ion has. if the charge is positive, then subtract that number from the number of electrons the ion has. |
| Free Radicals | are the unpaired electrons in a molecule. they are highly unstable. |
| Bonding Order | is the number of COVALENT BONDS between two atoms. |
| Single bond, Double Bond, Triple Bond | 2 electrons, 4 electrons, 6 electrons |
| VSEPR Structures | are to predict the 3D shapes of the molecules |
| The shape of the molecule... | is very important because it determines many important qualities of the molecule. |
| Geometric Center (GC) | the center atom of the molecule (A) |
| Ligands | atoms surrounding the central atom or the GC. (B) |
| ABx | A is the geometric center B os the ligands x is the number of ligands around the central atom |
| AB₂ No LONE PAIRS | linear Shape |
| AB₂ One or two LONE PAIRS | Bent Shape |
| AB₃ No LONE PAIRS | trigonal Planar |
| AB₃ ONE OR TWO LONE PAIRS | Trigonal Pyramid |
| AB₄ | Tetrahedral |
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