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Adv. chem unit 3

TermDefinition
covalent bonding nonmetal to nonmetal, shared electrons, low melting and room temperature boiling points, liquids and gases at room temp, weak bonds, does not conduct electricity, insoluble in water, electron orbitals overlap
formation of cations lose electrons, makes positive ion, metals like to be cations
formation of anions gain electrons, makes negative ion, name typically ends with ide
formation of ionic compounds must be neutral, charge is zero, positive charge cancels negative charge, opposites attract, force of attraction is electrostatic force
properties of ionic compounds crystalline solids, high melting points, brittle, made of metal and nonmetal, conductive
metallic bond attraction between metal cations and the surrounding sea of electrons, empty p and d orbitals allow electrons to move freely, valence electrons do not belong to any one atom,
Ionic bonding metal bonded to nonmetal, metal bonded to poly atomic ion, total transfer of electrons, high melting and boiling point, solids at room temp, strong bonds, electrically reactive, soluble in water, electron orbitals are seperate
VESPR (valence shell electron repulsion) electrons will arrange themselves to minimize repulsion, bond angle: angle between the bonds connecting atoms in a molecule
dipoles and molecular polarity net dipole:polar, dipoles cancel: nonpolar,
IMF (general) ((intermolecular force)) force of attraction, holds groups of molecules together, also known as van der Waal's forces
states of matter determined by forces weak forces=gas low boiling point, strong= solid or liquid, high BP
Dispersion force all molecules have it, more electrons=more dispersion, weakest force
dipole-dipole stronger than dispersion, all polar molecules
hydrogen bonds not a bond, polar molecules with H and N, O, or F
Created by: claughlin
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