Name ___________________________
Inorganic Chemistry
Exam 1
Feb. 11, 1997
All work must be shown for any credit to be given.
(6 pts.) 1. Write the electron configuration beyond a noble gas core(for example, F, [He]2s2, 2p6) for an atom of Fe.
(3 pts.) 2. What is the spectroscopic notation for an atom in an energy state in which L = 2 and S = 1.
(6 pts.) 3. Describe and explain the trends in the periodic table for the atomic radius.
(9 pts.) 4. Draw the three Lewis electron dot resonance structures for [CO3 ]-2.
5. For the following compound
SeCl4
(3 pts.) Draw the Lewis electron dot structure.
(3 pts.) Using the VSEPR Theory, predict the shape of the molecule ( specify the number of bond and lone pairs of electrons).
(2 pts.) Specify the type of hybridization present.
______________
(2 pts.) Using your molecular models, determine the principal axis of rotation.
______________
(2 pts.) Determine if there are any non-coincident axes of rotation.
_____________
(2 pts.) Determine which type of mirrors, if any are present.
_____________
(2 pts.) Specify the point group for the molecule.
6. For the following ion
[ICl4]-1
(3 pts.) Draw the Lewis electron dot structure.
(3 pts.) Using the VSEPR Theory, predict the shape of the molecule (specify the number of bond and lone pairs of electrons).
(2 pts.) Specify the type of hybridization present.
______________
(2 pts.) Using your molecular models, determine the principal axis of rotation.
______________
(2 pts.) Determine if there are any non-coincident axes of rotation.
_____________
(2 pts.) Determine which type of mirrors, if any are present.
_____________
(2 pts.) Specify the point group for the molecule.
(3 pts.) 7. Complete the following nuclear reaction.
2 12C ---> 20Ne +
(4 pts.) 8. For the 3d5 electron configuration, specify the principal and secondary quantum numbers and possible values for the magnetic and spin quantum numbers.
(6 pts.) 9. Using Slater’s rules, calculate the effective nuclear charge for a 3d electron in Fe.
(6 pts.) 10. Describe the trend in radius for the iso-electronic series involving S-2 through Ca+2.
(2 pts.) 11. Give an example of orbitals (atomic and/or hybridization) which can be combined to form a sigma bond.
(2 pts.) 12. Give an example of atomic orbitals which can be combined to form a pi bond.
13. For the following compound
SO2
(3 pts.) Draw the Lewis electron dot structure.
(3 pts.) Using the VSEPR Theory, predict the shape of the molecule ( specify the number of bond and lone pairs of electrons).
(2 pts.) Specify the type of hybridization present.
(6 pts.) 14. For SF6, give the energy diagram for ground state S atom, hybrid state S atom without F atoms, and hybrid state S atom showing electrons contributed by F atoms.
Name ___________________________
Inorganic Chemistry
Exam 1
Take-Home Portion
All work must be shown for any credit to be given.
(15 pts.) 15. Derive the spectral terms for the p4 configuration. Show all the micro-states. Identify the ground-state term. Give all J values for the ground-state term and indicate which is lowest in energy.
I neither received nor gave assistance on this take home exam, nor did I see others giving or receiving assistance.
____________________________ _____________
Signature Date
Ideal Geometries
Effect of Unshared Pairs on Geometry
A => central atom
B => surrounding atoms
E => unshared pair electrons
--------------------------------------------------------------------------------------------------------------------------------
AB 1 electron pair
1 bond pair
0 lone pair
linear geometry
linear shape, 180o angle
----------------------------------------------------------
AB2 2 electron pair
2 bond pair
0 lone pair
linear geometry
linear shape, 180o angle
----------------------------------------------------------
ABE only two atoms, therefore, linear
----------------------------------------------------------
AB3 3 bond pairs
0 lone pairs
3 electron pairs
trigonal planar geometry
trigonal planar shape
----------------------------------------------------------
AB2E 2 bond pairs
1 lone pair
3 electron pairs
trigonal planar geometry
bent shape
----------------------------------------------------------
AB4 4 bond pairs
0 lone pairs
4 electon pairs
tetrahedral geometry
tetrahedral shape
----------------------------------------------------------
AB3E 3 bond pairs
1 lone pair
4 electron pairs
tetrahedral geometry
trigonal pyramidal
AB2E2 2 bond pairs
2 lone pairs
4 electron pairs
tetrahedral geometry
bent shape
----------------------------------------------------------
AB5 5 bond pairs
0 lone pairs
5 electon pairs
trigonal bipyramidal geometry
trigonal bipyramidal shape
----------------------------------------------------------
AB4E 4 bond pairs
1 lone pair
5 electron pairs
trigonal bipyramidal geometry
"See-Saw" shape
----------------------------------------------------------
AB3E2 3 bond pairs
2 lone pairs
5 electron pairs
trigonal bipyramidal geometry
"T" shape
----------------------------------------------------------
AB2E3 2 bond pairs
3 lone pairs
5 electron pairs
trigonal bipyramidal geometry
linear shape
--------------------------------------------------------
AB6 6 bond pairs
0 lone pairs
6 electron pairs
octahedral geometry
octahedral shape
AB5E 5 bond pairs
1 lone pair
6 electron pairs
octahedral geometry
square pyramidal shape
-----------------------------------------------------
AB4E2 4 bond pairs
2 lone pairs
6 electron pairs
octahedral geometry
square planar shape
-----------------------------------------------------
AB7 7 bond pairs
0 lone pairs
7 electron pairs
pentagonal bipyramidal geometry
pentagonal bipyramidal symmetry 72o, 90o
----------------------------------------------------
AB8 8 bond pairs
0 lone pairs
8 electron pairs
square antiprismatic geometry
square antiprismatic symmetry 70.5o, 99.6o, 109.5o