iiiiii molecular polarity covalent bonding. covalent bonds involve sharing electrons but just like...
TRANSCRIPT
/Electronegativity
Electronegativity is the ability of an atom to Attract electrons to itself in a covalent bond
Large Electronegavity Small Electronegativity
The atom that “wins” will be the one that is more electronegative.
Because this atom gets the electrons more of the time, it becomes slightly negative
The atom that “loses” becomes slightly positive
A. Dipole Moment Means the direction of the polar bond in a
molecule. Arrow points toward the more
electronegative atom. (The direction the electrons will flow
H Cl+ -
B. Determining Molecular Polarity Depends on:
Electronegativity differences dipole moments molecular shape
B. Determining Molecular Polarity Polar Molecules
Dipole moments are asymmetrical and don’t cancel .
netdipolemoment
H2OH H
O
B. Determining Molecular Polarity Nonpolar Molecules
Dipole moments are symmetrical and cancel out.
BF3
F
F F
B
CHCl3
H
Cl ClCl
B. Determining Molecular Polarity Therefore, polar molecules have...
asymmetrical shape (lone pairs) or asymmetrical atoms
netdipolemoment
Example: CO2
Example: HCN
Linear molecules can be nonpolar . . .
Or Nonpolar.
What makes the difference?
No Net Dipole Moment
Net Dipole Moment Towards N
Trigonal Planar molecules are usually nonpolar
But, what makes this one polar?
Example: BF3
Example: BF2Cl
Can a Molecule be Both Polar and NonPolar?
Non Polar EndPolar End
Tetrahedral with symmetric atoms
Trigonal planar withAsymmetric atoms
So, polarity can be more of a spectrum than a black and white determination
Polar------------------------------------------------------nonpolar
More Nonpolar Molecules
•Share electrons the “best”
•Have the closest electronegativities (or smallest differences)
•Have lower boiling and melting points
•. . .so More likely to be gases at room temperature
•Like dissolves like . . . • Use a nonpolar solvent to dissolve a nonpolar solute
More Polar Molecules•Do not share well at all!
•Their electronegativity differences are great
•Are more like ionic compounds
•Have higher melting and boiling points
•Most likely to be liquids at room temperature
•Like dissolves like . . .
•Use a polar/ionic solvent to dissolve a polar/ionic solute