Quiz on molecular bonds defintions Flashcards
Formal charge
a calculation for choosing which structure is most correct
what are delocalized electrons
electrons spread themselves out for greater stability to a molecule or ion
Resonance structure
any molecule in which a double bond can be moved into multiple locations
when are covalent bonds formed
when two orbitals overlap to produce a new combined orbital containing 2 electrons with opposite spin
why do we hybridize
so two orbitals can have same shape and energy in order to make a certain shape ex (tetrahedral) and so there will not be unequal bonds on each side in terms of energy .
how do double bonds occur
when two p orbitals overlap sideways
when you hybridize and orbitals become completely filled out what does that mean?
it means that the ones that are filled out are lone pairs
what is a dipole
a molecule with a partial positve side ( s+ symbol) and a partial negative side ( s - symbol)
what do you call a bond less or equal than 1.6 EN
polar covalent
what do you call a bond more than 1.6 EN
ionic
what do you call a bond with 0 EN
pure covalent bond
what is diff between a polar bond and a polar molecule
a molecule can have polar bonds but be a non polar molecule because the polar bonds cancel out. Bond polarity refers to the polarity of a bond while molecule polarity reflects the overall molecule
structures that have ____ for formal charge are most stable
0
what is a dative bond(important)
a dative bond is a donation of a pair of electrons to a covalent bond!
