Term
|
Definition
Bonding electrons attracted
more strongly by one atom than
by the other |
|
|
Term
|
Definition
| intrinsic ability of an atom to attract the shared electrons in a covalent bond |
|
|
Term
|
Definition
|
|
Term
|
Definition
| Difference in EN of atoms < 2 |
|
|
Term
|
Definition
|
|
Term
|
Definition
| shifting of electrons in a bond in response to EN of nearby atoms |
|
|
Term
Electrostatic potential maps |
|
Definition
show calculated charge distributions
Colors indicate electron-rich (red) and electron-poor (blue) regions
|
|
|
Term
|
Definition
- Net molecular polarity, due to difference in summed charges
|
|
|
Term
|
Definition
|
|
Term
|
Definition
|
|
Term
|
Definition
In symmetrical molecules, what happens when the dipole moments of each bond has one in the opposite direction? |
|
|
Term
|
Definition
If the atom has one more electron in
the molecule |
|
|
Term
|
Definition
If the atom has one less electron |
|
|
Term
|
Definition
Neutral molecules with both a “+” and a “-”
|
|
|
Term
|
Definition
nSome molecules are have structures that cannot be shown with a single representation
nIn these cases we draw structures that contribute to the final structure but which differ in the position of the p bond(s) or lone pair(s) |
|
|
Term
|
Definition
A structure with resonance forms does
not alternate between the forms
Instead, it is a hybrid of [BLANK] |
|
|
Term
|
Definition
| Structural formula of benzene |
|
|
Term
|
Definition
|
|
Term
|
Definition
is a substance that donates a hydrogen ion (H+) |
|
|
Term
|
Definition
|
|
Term
|
Definition
| is a substance that accepts the H+ |
|
|
Term
|
Definition
Stronger acids have
[blank] Keq... larger or smaller? |
|
|
Term
|
Definition
| characterized by the presence of positively polarized hydrogen atom |
|
|
Term
|
Definition
Have an atom with a lone pair of electrons that can bond to H+ |
|
|
Term
| Nitrogen-containing compounds derived from ammonia |
|
Definition
| most common organic bases |
|
|
Term
Lewis acids are electron pair
acceptors and Lewis bases are
electron pair donors |
|
Definition
Lewis acids are electron pair
[BLANK] and Lewis bases are
electron pair [BLANK]
|
|
|
Term
|
Definition
The Lewis definition of acidity includes
metal cations, such as?? |
|
|
Term
|
Definition
| Lewis bases cannot accept protons as well as Lewis acids, true or false?? |
|
|
Term
|
Definition
Molecular shape is critical in determining
the chemistry a compound undergoes in the
lab, and in living organisms, and thus they
use?? |
|
|
Term
dipole dipole forces
dispersion forces
hydrogen bonds
|
|
Definition
| types of Noncovalent interactions |
|
|
Term
|
Definition
Occur between polar molecules as a result of electrostatic interactions
|
|
|
Term
|
Definition
Occur between all neighboring molecules and arise because the electron distribution within molecules that are constantly changing |
|
|
Term
|
Definition
• Most important noncovalent interaction in biological molecules
• Forces are result of attractive interaction between a hydrogen bonded to an electronegative O or N atom and an unshared electron pair on another O or N atom |
|
|
Term
|
Definition
| The polarity of a molecule is measured by its?? |
|
|
Term
|
Definition
| (+) and (-) indicate [blank] on atoms in molecules to keep track of valence electrons around an atom |
|
|
Term
polar covalent bonds *first blank*
electronegativity *2nd* |
|
Definition
Organic molecules often have
[blank] as a result of unsymmetrical
electron sharing caused by differences in
the [blank] of atoms |
|
|
Term
FALSE
A Brønsted(–Lowry) acid donates
a proton
A Brønsted(–Lowry) base accepts a
proton |
|
Definition
bronsted lowry acid and base both donate a proton *true or
false?* |
|
|
Term
|
Definition
| weaker pka's have stronger acids *true or false?* |
|
|
Term
|
Definition
In condensed structures [blank] and
[blank]
are implied |
|
|
Term
|
Definition
are useful for representing structures for study
|
|
|
