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Lewis Structure

Chemistry

TermDefinition
Linear Either two atoms with no unshared electrons or 2 atoms with 3 unshared pairs of electrons; 180* between atoms
Trigonal Planar No lone pairs of electrons and 3 atoms around central atom; 120* between atoms
Tetrahedral 109.5* between atoms; No lone pairs of electrons, 4 atoms around central atom
Triangular Bipyramidal no lone pairs of electrons; 5 atoms around central atom, some 90* from each other and some 120*
Bent 2 pairs unshared electrons, 2 atoms around central atom
Trigonal Pyramidal 3 atoms around central atom, one lone pair of electrons on central atom
See Saw 4 bonded pairs, one unbonded pair of electrons
T-Shaped 2 lone pairs of electrons, 3 atoms around central atom
Square Pyramidal 5 bonded, 1 unbonded pair of electrons around central atom
Square Planar 2 lone pairs of electrons, 4 bonded
Octet rule all atoms want to achieve a full valence shell of electrons
To Break Octet Rule an atom must contain an electron level with an empty d block
Resonance a phenomenon that occurs when double/triple bonds can move to multiple locations in a molecule (MUST SHOW ALL OF THE DIFFERENT SETUPS FOR THE MOLECULE ON TEST)
Electronegativity the ability of an atom to attract electrons to itself; type of bond made depends on this. Less strong in metals bc they have more electrons
Ionic bond one atom takes from another
Covalent two atoms share evenly
Polar Covalent two atoms share unequally (Most bonds are this)
Polar Molecules molecules that have a distinct positive and negative pole. POLAR IFF it contains polar bonds & bonds don't cancel out
Atom is polar if central atom is surrounded by things that are not the same. Polar bond = nonpolar atom
Nonpolar shapes are square planar, tetrahedral, linear, trigonal planar
Created by: 25pollijul
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