| Sections | |||
|---|---|---|---|
| Molecular vs Electron Geometry | 27 mins | 0 completed | Learn |
| Bond Angles | 10 mins | 0 completed | Learn Summary |
| Hybridization | 20 mins | 0 completed | Learn |
| Molecular Orbital Theory | 19 mins | 0 completed | Learn |
| Heteronuclear Diatomic Molecules | 10 mins | 0 completed | Learn |
| Additional Practice |
|---|
| Sigma and Pi Bonds |
| Electronegativity |
| Benzene |
| Orbital Overlap |
| Bond Order |
| Delocalized Electrons |
| Homonuclear Diatomic Molecules |
| Additional Guides |
|---|
| Molecular Geometry |
| VSEPR Theory |
Consider a molecule of PCl5.
Indicate whether the statements below are true or false.
Cl has a larger atomic radius than P.
When the preferred Lewis structure is drawn, no lone pairs appear on P.
PCl5 is a polar molecule.
Its molecular geometry is trigonal bipyramidal.
Its electron configuration is 1s22s22p63s23p64s23d104p65s24d2
Cl has higher first ionization energy than P.
The molecule has sp3 hybridization.
PCl5 is phosphorus pentachloride.
The bond between P and Cl is polar.
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