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- 1. Multiple ChoiceA lone pair is defined asA pair of bonding electronsOne non-bonding electronA pair of non-bonding electronsA pair of electrons on the central atom
- 2. Multiple ChoiceWhat is the VSEPR theory used to predict?Bond StrengthPolarityMolecular ShapeElectronegativity
- 3. Multiple ChoiceWhich of the following shapes has an unshared pairs of electrons on the central atom?BipyramidalBentTrigonal PlanarTetrahedral
- 4. Multiple Choice
Which molecule would have this molecular geometry?BF3CH4PCl5CO2 - 5. Multiple ChoiceWhat molecule could this be?BF3CH4H2OCO2
- 6. Multiple ChoiceWhat molecule could this be?H2OCCl4PCl5NaCl
- 7. Multiple ChoiceWho could this molecule be?CH4CO2PCl5BF3
- 8. Multiple ChoiceWho could this be?CO2NH3H2SCH4
- 9. Multiple ChoiceWho could this be?H2ONH3CO2CH4
- 10. Multiple Choice
What molecular geometry would PH3 have?
Trigonal Pyramidal
Trigonal Bipyramidal
Bent
Linear
- 11. Multiple ChoiceA molecule with a lone pair on the central atom would have the same electron and molecular geometryTrueFalse
- 12. Multiple ChoiceHow many lone pairs of electrons are on the P atom in PF3?1230
- 13. Multiple ChoiceDetermine the electron geometry (eg) and molecular geometry (mg) of XeF4 (Lewis structure is shown) .eg = tetrahedral, mg = tetrahedraleg = linear, mg = lineareg = octahedral, mg = square planareg = trigonal bipyramidal, mg = tetrahedral
- 14. Multiple ChoiceConsider the molecule below. Determine the molecular geometry at each of the 2 labeled carbons.C1 = tetrahedral, C2 = linearC1 = trigonal planar, C2 = bentC1 = bent, C2 = trigonal planarC1 = trigonal planar, C2 = tetrahedral
- 15. Multiple Choice
Is this molecule polar?
Yes
No
- 16. Multiple Choice
Is this molecule polar?
No
Yes
- 17. Multiple ChoiceAccording to VSEPR, molecules adjust their shapes to keep which of the following as far away as possible?Pairs of valence electronsInner shell electronsMobile ElectronsElectrons closest to the nucleus
- 18. Multiple ChoiceWhat is the measure of a tetrahedral bond angle?90 Degrees109.5 Degrees120 Degrees180 Degrees
- 19. Multiple ChoiceWhich of the following shapes has unshared pairs of electrons on the central atom?BipyramidalBentTrigonal PlanarTetrahedral
- 20. Multiple ChoiceWhich molecule would have this shape?BF3CH4PCl5CO2
- 21. Multiple ChoiceWhich of the following molecular shapes would have a bond angle of 180 Degrees?BentTrigonal PlanarTetrahedralLinear
- 22. Multiple ChoiceWhat molecule could this be?BF3CH4H2OCO2
- 23. Multiple ChoiceThe bond angle for a trigonal planar molecule is90 Degrees109.5 Degrees120 Degrees180 Degrees
- 24. Multiple ChoiceWhich shapes are altered by unshared pairs of electrons?Bent and PyramidalTrigonal Planar and BentTetrahedram and BipyramidalPyramidal and Linear
- 25. Multiple Choice
How many unshared pairs of electrons will a bent molecule have?
0
2
3
4
- 26. Multiple ChoiceHow many unshared pairs of electrons will a pyramidal molecule have?1234
- 27. Multiple Choice
What is the bond angle for a trigonal pyramidal molecule?
90
107
109.5
120
- 28. Multiple Choice
What is the bond angle in a bent molecule?
90
109.5
107
180
- 29. Multiple ChoiceWho could this molecule be?CH4CO2PCl5BF3
- 30. Multiple Choice
What shape would PH3 have?
Trigonal Planar
Trigonal pyramidal
Bent
Linear
- 31. Multiple ChoiceHow many unshared pairs of electrons will a pyramidal molecule have?1234
- 32. Multiple ChoiceWhat is the bond angle for this molecule?109.512010790
- 33. Multiple ChoiceWill this molecule be polar or nonpolar? PH3polarnonpolar
- 34. Multiple ChoiceWill this molecule be polar or nonpolar? CS2polarnonpolar
- 35. Multiple ChoiceCalculate the Formal Charge for the Oxygen Labeled 1-1+10-2
- 36. Multiple ChoiceCalculate the Formal Charge for the Oxygen Labeled 2-1+10-2
- 37. Multiple ChoiceCalculate the Formal Charge for the Nitrogen-1+10-2
- 38. Multiple ChoiceWhat is the formal charge for each of the Fluorine atoms-1+10+2
- 39. Multiple ChoiceWhat is the formal charge for Xenon-1+10+2
- 40. Multiple ChoiceWhat is the formal charge for Oxygen+1-10-2
- 41. Multiple ChoiceWhat is the formal charge for Phosphorus+1-10-2
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