1. Created by Carol J Breaux, College of the Ozarks, cbreaux@cofo.edu and posted on VIPEr (www.ionicviper.org) on July 16, 2012, Copyright Carol J. Breaux, 2012. This work is licensed under the Creative Commons Non-Commercial Share Alike License. To view a copy of this license visit http://creativecommons.org/about/license/cbreaux@cofo.edu(www.ionicviper.org

2. Calculate the number of valence electrons available in an ion of CO 3 2-. 26 18 22 20 24 Carbon has 4 valence electrons, each oxygen has 6 valence electrons, and there are two for the charge.

3. Which of the following species is NOT isoelectronic with the others? BF 3 SO 3 NO 3 - CO 3 2- SiF 2 All have 24 valence electrons, except SiF 4 which has 18 (Si has 4 and each F has 7)

4. How many sigma and how many pi bonds in a molecule of HCN? 2 sigma, 1 pi 3 sigma, 1 pi 4 sigma, 0 pi 3 sigma, 0 pi 2 sigma, 2 pi The CH bond is a sigma bond, one of the bonds from the CN triple bond is a sigma bond and the other two are pi bonds

5. What type of hybridization would exist around the central atom in NCl 3 ? s sp 3 d sp sp 2 sp 3 There are three bonding pairs and one nonbonding pair on the nitrogen which will hybridize into 4 sp 3 hybrid orbitals

6. The electron geometry of nitrogen trichloride is linear bent Trigonal planar Trigonal pyramid tetrahedral Electron geometry includes the lone pair. There are four pairs of electrons around the central nitrogen giving a tetrahedral electron geometry

7. The expanded shell around the chlorine in ClF 3 contains how many electrons? 14 12 11 8 10 There are 28 valence electrons in this compound. The central Cl atom will have three bonding pairs of electrons to the fluorines and two lone pairs of electrons to accommodate all of the valence electrons

8. TRUE or FALSE? Increasing numbers of lone pairs on a central atom cause bond angles to decrease. Electron pairs will repulse each other and will go as far apart from each other as they can. Lone pair-bonding pair repulsion is greater than bonding pair-bonding pair repulsion.

9. The molecular geometry of PCl 6 - using VSEPR theory is Trigonal planar Trigonal pyramidal tetrahedral linear octahedral There are 48 valence electrons that can be accommodated by a central P atom and 6 Cl atoms bonded octahedrally around the central atom. There are no lone pairs around the central P.

10. For which of the following compounds will the electron geometry and molecular geometry be the same? XeF 2 NH 3 SF 4 H2OH2O CO 2 The electron geometry and the molecular geometry will be the same For CO 2 because it is the only one that does not have any lone pairs on the central atom

11. A compound of type AX 4 E 2 will have which molecular geometry? octahedral Trigonal bipyramid Trigonal pyramid tetrahedral Square planar A stands for the central atom, X 4 is the number of bonds around the central atom, and E 2 is the number of lone pairs around the central atom. The lone pairs would occupy the axial positions and the 4 bonds would occupy the equatorial positions giving a square planar molecular geometry

12. The formal charge on the central atom in XeO 3 is 0 +2 +1 +3 There are 26 valence electrons available for this compound. Xe is the central atom. There are three bonding pairs from the oxygens and one lone pair on the central atom. The free atom of Xe would have 8 valence electrons. Subtract 2 for the lone pair electrons and 3 for each of the bonds from 8 and The formal charge will be +3.

13. What would be the most likely hybridization for a molecule of PCl 5 ? sp 3 sd 3 dsp 2 d 2 sp 3 dsp 3 The 10 electrons in the expanded shell of P will hybridize from an s, 3 p orbitals, and one d orbital.

14. The occupancy or steric number on the central atom in a molecule of SF 4 is 1 2 3 4 5 The steric number or occupancy tells how many bonding pairs and lone pairs are around the central atom. The S has 4 bonding pairs from the 4 fluorines and one lone pair.

15. TRUE or FALSE? The total number of molecular orbitals formed is not equal to the number of atomic orbitals that are initially present. The number of molecular orbitals is always equal to the number of atomic orbitals initially present

16. Which of the following two orbitals would not have sufficient overlap to form a molecular orbital? d zx and p x p x and p x s and p z s and s p y and p x An orbital on the z axis would not overlap with an orbital on the x axis sufficiently

17. Using MO theory how many unpaired electrons would a molecule of B 2 have? 4 3 0 1 2 B 2 has 6 valence electrons: 2 in the σ g orbital, 2 in the σ u *, and 1 (unpaired) in each of the two π u orbitals.

18. What is the bond order for a molecule of F 2 ? 2 1.5 0.5 1 Bond order is ½ (# electrons in bonding orbitals-#electrons in antibonding orbitals). F 2 has 8 electrons in bonding orbitals and 6 electrons in antibonding orbitals.

19. Which of the following is NOT a rule for forming molecular orbitals? The atomic orbitals must have similar symmetry The atomic orbitals must have sufficient overlap The atomic orbitals must have the right symmetry The number of molecular orbitals must equal the number of atomic orbitals Each orbital must contain two electrons. Molecular orbitals do not have to be completely filled

20. TRUE or FALSE? O 2 is diamagnetic. The MO diagram of O 2 shows 2 unpaired electrons in the π g * orbitals. Unpaired electrons will make a molecule paramagnetic