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Bonding

Regents Chem Bonding

QuestionAnswer
molecular compound compound with covalent bonds contains nonmetals and/or semimetals
ionic compound compound with ionic bonds; usually between metals and nonmetals and/or table E ions
ionic bonds formed by a TRANSFER of electrons
covalent bonds formed by SHARING of electrons
coordinant covalent bonds covalent bonds where the 2 shared electrons come from the same atom. Hydronium (H3O+) and ammonium (NH4+) contain this special type of bond.
polar molecules molecule with an uneven distribution of electrons. Positive and negative regions exist
nonpolar molecules molecule with even distribution of electrons due to its SYMMETRY.
Dipoles another name for the charged regions in a polar molecule
network bonding/network solid strongest intermolecular force. Covalent bonds continue in all directions. Ex. Diamond, graphite and silicon dioxide, silicon carbide
metallic bonding nuclei surrounded by a “sea of moving electrons’ – this is why metals conduct.
intermolecular forces attractive forces between molecules, the stronger they are, the higher the boiling and melting points will be
dipole-dipole forces attraction between polar molecules. Positive regions attraction to negative regions.
hydrogen bonding strong attraction between certain polar molecules containing hydrogen bonded to small, highly electronegative elements like N, O and F
dispersion forces/van der Waals forces attractions between nonpolar molecules, due to a temporary shifting of electrons
molecule ion attractions polar molecules are attracted to ionic compounds. This is how water dissolves salts, by attacking and surrounding the ions
octet rule all elements want 8 valence electrons to become stable. H and He only require 2 electrons (duet rule)
ion a charged element or compound, formed by a gain or loss of electrons
cation "MEOW" the special name for a positive ion
anion A-Negative ION
formula unit a single piece of an ionic compound
molecule atoms held together by covalent bonds, traveling around together (ex. H2O)
formula represents a compound, using element symbols and their subscripts
electronegativity ability to attract electrons
polar covalent bond unequal sharing of electrons; END is 0.3-2.0
nonpolar covalent bond equal sharing of electrons, usually in diatomic molecules; END 0-0.3
diatomic element 7 elements that cannot exist alone in nature. They bond to themselves (F2, Cl2, Br2, I2, O2, N2, H2)
structural formula represents a compound, showing bonding e's, non-bonded e's, element symbols, and the geometry
unshared (lone) electron pair non-bonded electrons. These repel all bonded e's and change the bond angles in the molecule
symmetry when a molecule looks the same on all sides and has evenly balanced e's
VESPR theory Valence shell electrons repel eachother and spead out, creating molecular geometries.
linear molecular geometry with 180* bond angles. can be polar or nonpolar
Bent/V-shaped molecuar geometry with 105* bond angles. Is polar, ex. H2O
Pyramidal molecular geometry with 107* bond angle. Is olar, ex. NH3
Tetrahedral molecular geometry with 109.5* bond angle. Can be polar or nonpolar. Ex. CH4, CH3Cl
Has both ionic and covalent bonds Any ionic compound that has a table E ion in it. (the polyatomic ion contains covalent bonds, but the overall bonding is ionic)
Created by: etucci