Atomic Theory

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

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

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.

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

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 

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

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

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

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 

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 

11. Which of the species in the following list is see-saw shaped? 1) BF4- 2) 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 

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 

13. Consider the following molecules and select those that are nonpolar. 1) SF2 2) SF4 3) SF6 a)   1 and 3 b)   3 only c)   1 and 2 d)   1 only e)   2 only 

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

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 

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

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

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

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

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 

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