ln = c

E = hn

c = 3.0 x 108 m/s

l = h/mv

h = 6.6 x 10-34 J.s

(1/l) = Rh[(1/na2) - (1/nb2)]

Rh = 1.1 x 107 m-1






1. Calculate the frequency of light whose wavelength is 4.2 x 10-7 meters.
A.6.2 x 1013 s-1
B.7.1 x 1014 s-1
C.8.3 x 1013 s-1
D.1.8 x 1014 s-1
E.none of these


2. What is the energy of a photon of light that has a frequency of 2.3 x 1014 s-1 (h = 6.6 x 10-34 J·s)?
A.2.8 x 10-18 J
B.1.5 x 10-19 J
C.2.9 x 10-48 J
D.6.4 x 10-22 J
E.none of these


3. Calculate the wavelength of light emitted when an electron in the hydrogen atom goes from the n = 4 shell to the n = 2 shell.
A.2.0 x 106 m
B.4.8 x 10-7 m
C.3.6 x 10-7 m
D.4.0 x 10-19 m
E.none of these


4. Given the three statements below, which answer is best?
(a) Although the wavelength of light and the frequency of light can change, the energy remains constant.
(b) An important consequence of quantum theory is that the energy of various electronic states for atoms are at fixed discrete levels.
(c) The energy of an electronic state for a hydrogen atom is dependent only on the principal quantum number n.
A.a and b are true, c is false
B.b and c are true, a is false
C.a and c are true, b is false
D.all are true
E.all are false


5. Three sets of quantum numbers are given below. Choose the best answer.
(a) n = 3, l = 3, ml = 0, ms = 1/2
(b) n = 2, l = 1, ml = 1, ms = 3/2
(c) n = 4, l = 2, ml = 3, ms = -1/2
A.a and b are allowed sets, c is not
B.a and c are allowed sets, b is not
C.only a is allowed
D.only b is allowed
E.none of these are allowed


6. The quantum number l for a 3d electron is:
A.1
B.2
C.3
D.4
E.none of these


7. How many electrons can be placed in the subshell described by the quantum numbers n = 3, l = 2?
A.none
B.2
C.6
D.10
E.none of these


8. The element with a ground state electron configuration of 1s22s22p4 is
A.B
B.C
C.O
D.F
E.Ne


9. The three quantum numbers that describe the state labeled F are:

A.n = 2, l = 0, ml = 0
B.n = 3, l = 1, ml = 1
C.n = 2, l = 1, ml = 1
D.n = 3, l = 0, ml = 0
E.none of these


10. If all the boxes shown contain as many electrons as possible, what neutral element has that energy level diagram?

A.Ca
B.Ar
C.Mg
D.K
E.none of these


11. The ground state of which species below has the most unpaired electrons?
A.P
B.O
C.Se
D.Fe
E.N


12. The ground state electron configuration of Se is:
A.[Ar]3s23d103p4
B.[Ar]4s24d104p4
C.[Ar]4s23d104p4
D.[Ar]4s23d104p5
E.none of these


13. The ground state electron configuration of the ion, P+, may be represented as:
A.[Ne]3s23p2
B.[Ne]3s23p4
C.1s22s22p63s23p3
D.[Ne]3s23p6
E.none of these


14. What is the ground state electron configuration of Cr2+?
A.[Ar]4s13d3
B.[Ar]4s23d2
C.[Ar]3d4
D.[Ar]3d3
E.none of these


15. Which element has the valence electrons 4s23d2?
A.Ca
B.Sc
C.Ti
D.V
E.none of these


16. Of the three species, which would be isoelectronic with O?
(a) N- (b) F- (c) Ne2-
A.a and b are isoelectronic, c is not isoelectronic with O
B.only a is isoelectronic with O
C.only b is isoelectronic with O
D.all are isoelectronic with O
E.none are isoelectronic with O


17. Which species shown below is the largest?
A.O
B.O2-
C.F
D.F-
E.N3-


18. Which species shown below is the largest?
A.P
B.S
C.Cl
D.N
E.O


19. Which answer below correctly lists the atoms shown in order of increasing first ionization energy?
A.B < N < Be
B.C < Be < Li
C.B < N < F
D.C < Be < N
E.none of these


20. Which element listed below has the most exothermic electron affinity?
A.Se
B.Sn
C.As
D.Cl
E.none of these



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