Lewis Dot Structures help?
What would lewis dot structures look like for the following molecules or polyatomic ions:
PH3, phosphine
BF3, boron trifluoride
SO3/2 silfite ion
SeF4, selenium tetrafluoride
Please be detailed. Thank you :]
What would lewis dot structures look like for the following molecules or polyatomic ions:
PH3, phosphine
BF3, boron trifluoride
SO3/2 silfite ion
SeF4, selenium tetrafluoride
Please be detailed. Thank you :]
Comments
PH3 - three single bonds, all P-H. One unshared pair on the P
BF3 - three single bonds, all B-F. Note: only 6 electrons in valence shell of B. Each F has three unshared pairs.
SO3^2-
The S is central to the three oxygens. One oxygen has a db to the S and also has two unshared pairs. The other two oxygens each have a single bond to the S and also have three unshared pairs. Each of these last two oxygens bears a negative charge. The sulfur has an additional unshared pair of electrons.
There are three resonance forms to the above structure. The bond order for each S-O bond is 1.33.
SeF4 - I'll take a different tack here. The molecular geometry is disphenoidal and is given the generic formula of AX4E. There are 4 single bonds and one unshared pair on the Se.
Best wishes on the Lewis structure.