1. Which of the following sets of quantum numbers are allowed for an electron in an atom?
n l ml ms 1) 2 1 0 +1/2 2) 3 0 +1 -1/2 3) 3 2 -2 -1/2 4) 1 1 0 +1/2 5) 2 1 0 0
a) 2, 4, 5
b) 2, 4
c) 1, 2, 3
d) 1, 3
e) 3, 4
2. Which of the following sets of quantum numbers is not allowed?
a) n = 2, l = 0, ml = 0
b) n = 3, l = 2, ml = -3
c) n = 3, l = 1, ml = -1
d) n = 2, l = l, ml = 0
3. Which of the following sets of quantum numbers is not allowed?
a) n = 3, l = 0, ml = 0
b) n = 2, l = l, ml = 0
c) n = 2, l = 2, ml = -1
d) n = 3, l = 1, ml = -1
4. What is the energy content per photon (J) for light of frequency 4.2 x 1014?
a) 2.5 x 10-18
b) 3.4 x 10-19
c) 2.5 x 10-19
d) 2.8 x 10-19
e) 4.1 x 10-19
5. Which of the following represents the shortest wavelength?
a) 3.5 x 10-6 m
b) 735 nm
c) 6.3 x 10-5 cm
6. A blue line in the spectrum of mercury occurs at 4.36 x 10-7 m. What is this wavelength in Å?
a) 4.36 x 104
b) 2.29 x 10-4
c) 2.29 x 10-3
d) 4.36 x 102
e) 4.36 x 103
7. Give the corresponding atomic orbital designations for electrons with the following quantum numbers.
n l ml ms 1) 2 1 0 -1/2 2) 5 3 -1 -1/2 3) 3 2 +1 -1/2
a) 2s,5d,3p
b) 2p,5f,3f
c) 2p,5f,3d
d) 2p,5d,3p
e) 2p,5f,3p
8. Identify the sub-shell in which electrons with the quantum numbers n = 3, l = 2 may be found.
a) 4d
b) 2f
c) 3p
d) 4f
e) 3d
9. What type of orbital is occupied by an electron with the quantum numbers n = 3, l = 2. How many orbitals of this type are found in a multi electron atom?
a) 3s, 1
b) 3p, 3
c) 3d, 5
d) 2d, 5
e) 2p, 3
10. Consider the argon atom. For how many electrons does this atom have ml = 1 and ms = + 1/2 ?
a) 0
b) 1
c) 6
d) 2
e) 4
11. Consider the argon atom. For how many electrons does this atom have ml = 1?
a) 0
b) 6
c) 1
d) 2
e) 4
12. Consider the chlorine atom (atomic number 17). For how many electrons does this atom have l = 0?
a) 12
b) 2
c) 10
d) 6
e) 8
13. Which of the following sets of quantum numbers describes the most easily removed electron in a copper atom in its ground state?
a) n = 3, l = 1, ml = -1, ms = -1/2
b) n= 4, l = 2, ml = 0, ms = +1/2
c) n= 3, l = 0, ml = 0, ms = -1/2
d) n= 4, l = 0, ml = 0, ms = +1/2
e) n= 3, l = 1, ml = 0, ms = -1/2
14. Which of the following sets of quantum numbers cannot exist in an excited hydrogen atom?
a) n = 27, l = 14, ml = -8, ms = -1/2
b) n = 4, l = 1, ml = -2, ms = +1/2
c) n = 2, l = 1, ml = -1, ms = +1/2
d) n = 3, l = 2, ml = 0, ms = -1/2
15. Which of the following sets of quantum numbers describes the most easily removed electron in an potassium atom in its ground state?
a) n = 4, l = 0, ml = 1, ms = +1/2
b) n = 4, l = 0, ml = 0, ms = +1/2
c) n = 3, l = 1, ml = 1, ms = -1/2
d) n = 2, l = 1, ml = 0, ms = -1/2
e) n = 2, l = 0, ml = 0, ms = -1/2
16. Elements with atomic numbers 58 through 71 are placed separately at the bottom of the periodic table because:
a) they are radioactive.
b) they are all very dense.
c) they have large atomic weights.
d) they were discovered recently.
e) the table is made more compact.
17. Elements with similar chemical properties are located ______ the periodic table.
a) in the center of along zig-zag lines in
b) in vertical columns in
c) in groups of five in
d) in horizontal rows in
18. The modern periodic table has the elements arranged in order of:
a) number of isotopes.
b) increasing number of neutrons.
c) their date of discovery.
d) increasing radii of the atoms.
e) increasing number of protons.
19. What alkali metal is located in period 4?
a) Sr
b) Na
c) Ca
d) K
e) Mg
20. Consider the following elements and select those that are metalloids.
Pb P Ge Co Hg
a) only Co
b) only P
c) Pb, Co and Hg
d) Pb and Hg
e) Ge
21. Consider the following elements and select those that are metals.
Se Ti Ba Br O
a) only Ba
b) Ti and Ba
c) only Se
d) Se, Br and O
e) Br and O
22. After the 5s subshell of an atom is filled the next electron is located in the ______ subshell.
a) 4d
b) 4f
c) 4p
d) 5d
e) 5p
23. In what group of the periodic table is an element with [Ar]4s23d10 electron configuration located?
a) IIB
b) VIIB
c) IIA
d) IIIA
e) VIIA
24. Identify the group that has a ns2(n-1)d5 electron configuration.
a) VIIB
b) VB
c) VA
d) VIIA
e) IIA
25. Which of the following electron configurations is correct for antimony, (atomic number 51)?
a) [Ar]4s23d104p3
b) [Ar]4s24d104p3
c) [Kr]5s24d105p3
d) [Kr]4s23d104p3
e) [Ar]5s23d105p3
26. Which of the following electron configurations is correct for niobium, (atomic number 41)?
a) [Kr]4s23d5
b) [Ar]5s24d3
c) [Kr]5s24d3
d) [Kr]4s23d3
e) [Ar]5s24d5
27. Which of the following electron configurations is correct for zirconium, (atomic number 40)?
a) [Kr]4d45s2
b) [Ar]3d24s2
c) [Ar]3d103f2
d) [Kr]4d25s1
e) [Kr]4d25s2
