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21 Cards in this Set
- Front
- Back
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Chemical bond
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Positive nucleus attracted to negative valence electrons of different atoms that bond them together
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Ionic bonding
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Bond between cations and anions where atoms completely give up electrons to other atoms
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Covalent bonding
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Sharing of electron pairs between 2 atoms
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Molecule
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Neutral group of covalently bonded atoms
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Molecular compound
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Chemical compound whose simplest units are molecules
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Diatomic molecule
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Molecule containing 2 atoms
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Bond length
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Distance between nucleus if two atoms
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Bond energy
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Energy it takes to break a bond between atoms
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Molecular polarity
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Uneven distribution of molecular charges
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VSEPR
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Causes electrons to be as far away from eachother as possible
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Resonance
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Things that can't be represented by a single Lewis structure
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Poly atomic ions
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Negative ions with a charge/ many ions with a charge
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Charge
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Excess or shortage of electrons
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Intermolecular forces
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Forces of attraction between molecules
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Intramolecular forces
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Stronger than intermolecular
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London dispersion force
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Weakest; instantaneous dipoles. Attraction resulting from electron motions
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Dipole-dipole forces
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Middle strength; between polar molecules
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Hydrogen bonding
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Strongest; between H and N, O, or F.
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Ionic compounds
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Anions from crystal lattice structures
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Volatile
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How quickly things evaporate
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Metallic bonding
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Chemical bonding that results from attraction
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