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Molecular Models

Quiz yourself by thinking what should be in each of the black spaces below before clicking on it to display the answer.
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Question
Answer
Ionic Bond   Transfer of electrons so that both have an octet EN greater than or equal to 1.67  
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Covalent Bond   Share electrons so they both have an octet EN less than 1.67  
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Metallic Bond   Dipole, polar, alloys, protons in sea of electrons, good conductors of heat and electricity  
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Dipole   Polar, covalent bond, net pull  
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Vander Waals Forces   Weak, intermolecular, attractive forces  
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London Dispersion Forces   DD (strongest), DN (intermediate), or NN (weakest)  
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Molecule   Two or more atoms  
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Lewis Structure   Number of valence electrons for all atoms in a molecule, organized, complete octets  
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Sigma Bond   End-to-end single, covalent bonds  
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Pi Bond   Covalent, sideways/parallel bonds  
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Single Bond   Covalent, 2 shared electrons (1 sigma)  
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Double Bond   Covalent, 4 shared electrons (1 sigma, 1 pi)  
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Triple Bond   Covalent, 3 shared electron pairs (1 sigma, 2 pi)  
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Resonance   The average of all Lewis structures for a molecule  
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VSEPR   Determines shape and angle from orbital position  
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Hybridized Orbital   The blending of two or more orbitals  
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Molecular Orbitals   New orbitals -> new molecule Bonding and anti-bonding  
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Bond Order   Bond strength (B-A)/2  
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Paramagnetic   1 or more unpaired electrons Attracted to magnetic field  
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Diamagnetic   No unpaired electrons Not attracted to magnetic field  
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Coordinate Covalent Bond   Shared, come from the same atom  
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Bonding Orbital   Molecular orbital, constructive interference, less energy, more stable  
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Anti-bonding Orbital   Molecular orbital, destructive interference, more energy, less stable *  
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Created by: archergirl
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