1. Atomic Theory

2. the electron may be in a p orbital
1. Which of the following statements is correct for an electron that has the quantum numbers n = 4 and ml = -2?
  the electron may be in a p orbital
the electron must have a spin quantum number ms = + ½
the electron may be in a d orbital
the electron is in the second principal shell
none of the above applies to this electron

3. 2. Identify the orbital in which electrons with the quantum number n = 5, l = 3 are found.5p 3d

4. 3. Which of the following statements is false?
There are seven f orbitals per energy level starting with the fourth energy level.
There are five d orbitals in every energy level
A set of d orbitals can have a maximum of 10 electrons.
the three p orbitals in a p subshell are mutually perpendicular.
The d orbitals in an energy level are always filled after the p orbitals in the same energy level.

5. 4.Which of the following sets of quantum numbers cannot exist in an excited hydrogen atom?
  n = 3, l = 2, ml = 0, ms = -1/2
n = 27, l = 14, ml = -8, ms = -1/2
n = 4, l = 1, ml = -2, ms = +1/2
  n = 2, l = 1, ml = -1, ms = +1/2

6. 5.Which of the following electron configurations is for an atom in the ground state?
a)   1s12s1 b)   1s22s22p3 c)   [Ne]3s23p64f4 d)   1s22s22p43s2 e)   [Ne]3s23p34s1 

7. 6.What types of hybrid orbitals are involved in bonding of XeF4?
a)   sp2 b)   sp3 c)   sp d)   sp3d2 e)   sp3d 

8. 7. What types of hybrid orbitals are involved in bonding of IF2+?
a)   sp3d2 b)   sp3d c)   sp2 d)   sp e)   sp3 

9. 8. What types of hybrid orbitals are involved in bonding of BH4-?
a)   sp3d2 b)   sp3d c)   sp2 d)   sp e)   sp3 

10. 9. Which of the species in the following list is pyramidal?
ClF3 2) BF3 3) ClO3- 4) SiCl3+ 5) SiH3-
a)   3 only
b)  1 and 3
c)   2 and 4
d)   1 only
e)   3 and 5 

11. 10. Which of the species in the following list is tetrahedral?
BF4- 2) SF4 3) XeF4 4) SiF4 5) PCl4-
a)   3 only b)   1 and 3 c)   2 and 3 d)   1 only e)   1 and 4 

12. 11. Which of the species in the following list is see-saw shaped?
1) BF ) SF4 3) XeF4 4) SiF4 5) PCl4-
a)   3 only b)   1 and 3 c)   1 and 4 d)   1 only e)   2 and 5 

13. a) two b) four c) three d) zero e) one
12. Draw the Lewis formula for ICl2-. How many lone pair(s) of electrons are there in the valence shell of the central atom?
a)   two b)   four c)   three d)   zero e)   one 

14. 13. Consider the following molecules and select those that are nonpolar.
1) SF ) SF ) SF6
a)   1 and 3 b)   3 only c)   1 and 2 d)   1 only e)   2 only 

15. 14. Which of the following does not have a dipole moment?
a)   SO2 b)   SeF6 c)   CH2Cl2 d)   H2S e)   NO 

16. a) 7s & 5d b) only 4f c) only 1p d) 5d & 4f e) 1p & 2d
15. Which in the following list of atomic orbital designations is impossible?
7s 1p 5d 2d 4f
a)   7s & 5d b)   only 4f c)   only 1p d)   5d & 4f e)   1p & 2d 

17. 16. Which of the following has the highest normal boiling point?
a)   H2Se b)   H2S c)   H2O d)   H2Te 

18. 17. Which of the following has the lowest normal boiling point?
a)   GeH4 b)   SiH4 c)   CH4 d)   SnH4 

19. 18. Which element has the highest electron affinity?
b) Na
c) I
d) Kr
e) Cs 

20. 19. What structural units make up solids such as sodium chloride?
polar molecules
atoms
non-polar molecules
a lattice structures
ions. 

21. 20. Which term is given to a substance, which conducts an electric current, and has luster?
a) metallic
b) ionic crystal
network solid
group IA elements
e) molecular solids 

22. 2 sp 180o linear Hg2,BeCl2 3 1 sp2 120o <120o Trigonal Planar/
Valance
Shell
Electron
Pairs
Bonding Electron Pairs(VSEPR) or
Bonding
Orbitals(VB)
Nonboding electron(VSEPR) Nonbonding Orbitals(VB)
Hybrid-
ization
Bond Angle
Geometric Shapes
example 2 sp
180o
linear
Hg2,BeCl2 3 1
sp2
120o
<120o
Trigonal
Planar/
V-shaped
BF3,In(CH3)3
SnCl2,PbBr2 4
sp3
109.5o
<109.5o
Tetrahedral
trigonal
Pyramidal
CH4,SnCl4
NH3,PCl3
H3O+
H2O,OF2,
SCl2 5
sp3d
90o/
<120
<90o
Bipyramidal
See-saw
T-shaped
Linear
PCl5,NbCl5
SF4,TeCl4
ClF3
ICl2-,XeF2 6
sp3d2
90o
>90o
Octalhedral
Square
planar
SF6
BrF5
IC4-,XeF4