Chemical Bonding

strong bonds, salts, electronegativity difference greater than 1.7

formed when a metallic atom transfers an electron to a nonmetallic atom

which are repeating units with strong intermolecular attractive forces

1.solids at room temperature 2.conductors in the molten (liquid) sate 3.non-conductors in solid state 4.electrolytes in aqueous state

when electron pairs are shared between two atoms; group 6 nonmetals and group 7 nonmetals, N, P, C, Si, and H

1.single bond (sigma bond) 2.double bond (pi bond) 3.triple bond (sigma bond and 2 pi bonds)

1.low m.p. 2.non-electrolytes (except for acids) 3.do not dissociate (except acids) 4.mostly liquids at room temp

valance shell electrons pair repulsion theory: affect the molecular geometry of a molecule

180 degrees

120 degrees

109.5 degrees

107 degrees

104.5 degrees

exists when there is an uneven distribution of electrons about the central atom, lack symmetry

determined though electronegativity differences; < or = to 0.3 then non covalent, 0.3-1.7 polar covalent, > or = to 1.7 then ionic

hydrogen bonding, dipole-dipole, london dispersion forces

hydrogen to F, O, N

between polar covalent molecules

exists between non-polar covalent