Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
12 Cards in this Set
- Front
- Back
|
multiple bond |
Ifthere are not enough electrons for the central atom to attain an octet, a multiple bondis present |
|
|
resonance hybrid |
canbe depicted by more than one valid Lewis structure; havethe same relative placement of atomsbut different locations of bonding and lone electron pairs; the weighted average of the resonance structures is the correct one |
|
|
fractional bond order |
bond order by resonance hybrids # electron pairs / # bonded-atom pairs |
|
|
formal charge |
the charge an atom would have if all its electrons were shared equally = # valence electrons - (# of unshared valence electrons + 1/2 shared valence electrons) must sum to the actual charge on the species for all resonance forms |
|
|
free radical |
molecule with an odd number of electrons |
|
|
expanded valence shell |
only possible for nonmetals period 3 or higher because these elements have available d orbitals |
|
|
group of electrons |
any number of electrons that occupies a localized region around the atom |
|
|
molecular shape |
three dimensional arrangement of nuclei joined by the bonding groups. classified using the designation AXsubmEsubn where m and n are integers, X= surrounding atom, E= nonbonding valence-electron group, A= central atom |
|
|
bond angle |
the angle formed by the nuclei of two surrounding atoms with the nucleus of the central atom |
|
|
molecular polarity |
depends on both shape and bond polarity |
|
|
dipole moment (u) |
given the unit debye (d), it measures the polarity of a molecule |
|
|
a molecule is polar if |
it contains one or more polar bonds and the individual bond dipoles do not cancel |
