λν = c         E = hν       c = 3.00×108 m/s      h = 6.626×10-34 J·s
λ = h/mu      En = -(B/n2)      B = 2.18×10-18J      NA = 6.022×1023
1/λ = R[(1/n12) - (1/n22)]         R = 1.097×107 m-1      



1.
Who proposed a model that successfully explained the photoelectric effect?
A.
Planck
B.
Einstein
C.
Compton
D.
Rydberg
E.
Bohr


2.
Select the arrangement of electromagnetic radiation which starts with the shortest wavelength and ends with the longest wavelength.
A.
radio, infrared, ultraviolet, gamma rays
B.
radio, ultraviolet, infrared, gamma rays
C.
gamma rays, radio, ultraviolet, infrared
D.
gamma rays, infrared, radio, ultraviolet
E.
gamma rays, ultraviolet, infrared, radio


3.
If the energy of a photon is 1.32×10-18 J, what is its wavelength in nm?
A.
1.51×10-7 nm
B.
151 nm
C.
1.99×1015 nm
D.
1.99×1024 nm
E.
6.64×10-3 nm


4.
Calculate the wavelength of a photon emitted when the hydrogen atom undergoes a transition from the n = 5 to the n = 3 state (one of the Paschen series of emission lines).   R = 1.097×107 m-1
A.
205.1 nm
B.
384.6 nm
C.
683.8 nm
D.
1282 nm
E.
> 1500 nm


5.
The de Broglie equation predicts that the wavelength of a proton with mass 1.673×10-27 kg moving at 1000. m/s is
A.
3.96×10-10 m
B.
3.96×10-7 m
C.
2.52×106 m
D.
2.52×109 m
E.
> 1010 m


6.
The shape of an atomic orbital is associated with
A.
the principal quantum number (n).
B.
the angular momentum quantum number (l).
C.
the magnetic quantum number (ml).
D.
the spin quantum number (ms).
E.
the magnetic and spin quantum numbers, together.


7.
Which of the following is a correct set of quantum numbers for an electron in a 3d orbital?
A.
n = 3, l = 0, ml = -1
B.
n = 3, l = 1, ml = +3
C.
n = 3, l = 2, ml = 3
D.
n = 3, l = 3, ml = +2
E.
n = 3, l = 2, ml = -2


8.
In the quantum mechanical treatment of the hydrogen atom, the energy depends on the principal quantum number n but not on the values of l or ml.
A. True
B. False


9.
The effective nuclear charge for an atom is less than the actual nuclear charge due to
A.
shielding.
B.
penetration.
C.
paramagnetism.
D.
electron-pair repulsion.
E.
relativity.


10.
Select the correct set of quantum numbers (n, l, ml, ms) for the highest energy electron in the ground state of potassium, K.
A.
4, 1, -1, ½
B.
4, 1, 0, ½
C.
4, 0, 1, ½
D.
4, 0, 0, ½
E.
4, 1, 1, ½


11.
Select the correct electron configuration for Te (Z = 52).
A.
[Kr]5s25p64d8
B.
[Kr]5s25d105p4
C.
[Kr]5s24d105p6
D.
[Kr]5s24f14
E.
[Kr]5s24d105p4


12.
Which of the following elements has the largest atomic size?
A.
S
B.
Ca
C.
Ba
D.
Po
E.
Rn


13.
Which of the following elements has the largest first ionization energy?
A.
Na
B.
Cl
C.
Ca
D.
Te
E.
Br


14.
Elements with ________________ first ionization energies and ___________ electron affinities generally form cations.
A.
low; very negative (high)
B.
high; positive or slightly negative (low)
C.
low; positive or slightly negative (low)
D.
high; very negative (high)
E.
None of the above is generally correct.


15.
The most acidic oxides are formed from elements found in the _________________ region of the periodic table.
A.
upper right
B.
upper left
C.
center
D.
lower right
E.
lower left


16.
Select the paramagnetic ion.
A.
Cu+
B.
Ag+
C.
Fe3+
D.
Cd2+
E.
Ca2+


17.
What is the correct order of decreasing size of the following ions?
A.
P3- > Cl- > K+ > Ca2+
B.
Ca2+ > K+ > Cl- > P3-
C.
K+ > Cl- > Ca2+ > P3-
D.
K+ > Cl- > P3- > Ca2+
E.
None of the above is correct.


18.
Which of the following contains covalent bonds?
A.
BaO
B.
IBr
C.
Mg
D.
LiBr
E.
Cu


19.
Select the element whose Lewis symbol is correct.
A.
· Fr ·
B.
· Ra ·
C.
· Pb ·
D.
: Te :
E.
  He ·


20.
Select the compound with the highest (i.e. most negative) lattice energy.
A.
CaS(s)
B.
BaO(s)
C.
NaI(s)
D.
LiBr(s)
E.
MgO(s)


21.
The lattice energy of MgCl2 is the energy change for which one of the following processes?
A.
Mg(s)   +   Cl2(g) →   MgCl2(s)
B.
Mg(g)   +   2Cl(g) →   MgCl2(s)
C.
Mg2+(s)   +   2Cl-(g) →   MgCl2(g)
D.
Mg2+(g)   +   2Cl-(g) →   MgCl2(s)
E.
MgCl2(aq) →   MgCl2(s)


22.
Arrange the following bonds in order of increasing bond strength.
A.
C–I < C–Br < C–Cl < C–F
B.
C–F < C–Cl < C–Br < C–I
C.
C–Br < C–I < C–Cl < C–F
D.
C–I < C–Br < C–F < C–Cl
E.
none of the above orders is correct


23.
Which of the following elements is the least electronegative?
A.
Si
B.
Se
C.
S
D.
Sc
E.
Sr


24.
Based on electronegativity trends in the periodic table, predict which of the following compounds will have the greatest % ionic character in its bonds.
A.
H2O
B.
LiI
C.
CaO
D.
RbF
E.
HCl


25.
Which one of the following properties is least characteristic of typical metals?
A.
moderately high melting point
B.
high boiling point
C.
brittleness
D.
good electrical conductor when solid
E.
good electrical conductor when molten


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