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General Chemistry: Chemical Bonding
Terms in this set (28)
bond length: double bonds v. triple bonds
shorter bond length between triple bonds than double bonds, shorter bond length between double bonds than single bonds
how do we define bond energy
the energy required to separate 2 bonded atoms
the strength of a bond (and therefore the bond energy) increases as the number of ______________ increases
shared electron pairs
unshared electron pairs are also known as
lone electron pairs
what is it called when more than one lewis structure can be drawn for a molecule
what is the equation we use to find the formal charge of an atom
Formal Charge = (Valence electrons) - (number of bonds aka half number of bonding electrons + number of nonbonding electrons)
a lewis structure in which negative formal charges are placed on more electronegative atoms are more or less stable than one in which formal charges are placed on less EN atoms?
exceptions to octet rule? why?
atoms found in or beyond the 3rd period can hav emore than eight valence electrons, since some of the valence electrons occupy d orbitals (they can have more than 4 bonds in Lewis structures)
value of polar covalent bonds
0.3 to 1.7
the dipole points to where
the atom that is more electronegative
the dipole moment has a vector quantity (u) measured in Debye units (coulumb meters). what is the equation?
lewis acid in terms of electrons
accepts electron pair to form covalent bond
a lewis base
donates an electron pair
VSEPR theory predicts what
molecular geometry of covalently bonded molecs
3 electron pairs
4 electron pairs
4 electron pairs (one of the pairs is nonbonding)
4 electron pairs (2 nonbonding)
5 electron pairs
6 electron pairs
if the signs of 2 atomic orbitals are the same, what is formed
a bonding orbital
if the signs of 2 atomic orbitals are different, then what is formed
an antibodning orbital
when 2 orbitals of different atoms overlap head-to head, what is the resulting bond
when parallel p orbitals interact,what is formed?
a pi bond
intermolecular forces: lowest to highest
LDF --> dipole-dipole --> H-BONDING --> dipole-ion
dipole-dipole and LDF forces are also called
van der Waals forces
hydrogen bonding is a strong type of...
H with F, O, or N
larger molecules have greater or smaller LDF?
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