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polar covalent bonds

are formed when two atoms share electrons unequally due to a difference in electronegativity, resulting in a partial positive charge on one atom and a partial negative charge on the other

covalent bond

electrons are equally distribution

ionic bond

electrons completely transfer from one atom to another

difference between polar covalent, covalent and ionic bonds

polar - uneuqally shared electrons

covalent - equally shared electrons

ionic - transfer electrons

electronegativity

intrinsic ability of an atom to attract the shared electrons in a covalent bond

electronegativity trends

increases left to right and decreases from top to bottom

why are the electronegativity tends like this?

increases left to right because atoms have more protons; decreases becasue outer electrons sit farther from nucleas and feel less pull

0.0 to 0.4

nonpolar covalent Δ𝐸𝑁

0.5 to 1.9

polar covalent Δ𝐸𝑁

2.0 or higher

ionic Δ𝐸𝑁

dipole moment

magnitude of the charge Q at either end of the molecular dipole times the distance r between the charges ( μ = Q x r)

formal charge

#of valence electrons - dots - sticks

(dots = nonbonding electrons, sticks = bonds)

resonance forms

multiple lewis structures used to represnt a single molecule or ion (indicated by the double headed arrow between them)