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Chemistry-IMF

semester 2 chemistry

TermDefinition
inside forces intramolecular- ionic, metallic and covalent
between molecule intermolecular forces(IMF)- properties eg boiling point
homoatomic molecules share electrons equally -NOT polar
Heteroatomic molecules one element is more electronegative than the other-polar bond
can covalent bond be non-polar yes- they can balance out
Linear will only have up to two bonds with M
Trigonal Planar 3 bonds with no lone pair so its flat (plane)
V-Shaped will have lone pair so its bent- two bonds and one lone pair
Tetrahedral 4 bonds no lone pairs
Trigonal Pyramidal three bonds and a lone pair so its not flat
octahedral 6 bonds to make 8 sides
-hedral Describes number f faces
polar molecules when electron density is not evenly distributed (electrons pull in direction of net diploe)
when does a bond become polar when electronegativity is >0.4(greater than 0.4)
what is a Dipole-dipole -Between two polar molecules -molecules line up s+ and s-
ion-dipole -ions and dipole -s+ attracted to anion -s- attracted to cation
hydrogen bonding the bond between a hydrogen atom covalently bonded to an atom of F, O or N and another molecule that also contains an atom of H, F, O or N
non-polar covalent bond bond formed between atoms with the same electronegativity
non-polar molecule molecule that does not have permanent dipoles or is symmetrical
polar covalent bond bond formed when two atoms that have different electronegativities share electrons
dipole–dipole interactions weak bonding caused by the positive end of one dipole attracting the negative end of another dipole- IMF occurs between two polar molecules
dispersion force Non-polar molecules that cant form dipoles electrons move- instantaneous dipoles forming- momentary dipoles
Created by: cIsbel
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