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 first developed an empirical equation from which the wavelengths of the lines in the hydrogen atomic emission spectrum can be calculated?
A.
Planck
B.
Einstein
C.
Rydberg
D.
Heisenberg
E.
de Broglie


2.
Arrange the following types of electromagnetic radiation in order of decreasing wavelength starting with the longest wavelength and ending with the shortest wavelength.
A.
microwave, infrared, ultraviolet, gamma ray
B.
infrared, ultraviolet, gamma ray, microwave
C.
ultraviolet, gamma ray, microwave, infrared
D.
gamma ray, microwave, infrared, ultraviolet
E.
microwave, gamma ray, infrared, ultraviolet


3.
What is the wavelength of a photon with energy 7.34×10-11 J?
A.
3.44×10–9 m
B.
5.32×10–25 m
C.
2.71×10–10 m
D.
5.32×10–16 m
E.
2.71×10–15 m


4.
Calculate the wavelength of the photon emitted when the hydrogen atom undergoes a transition from n = 7 to n = 3. (R = 1.096776×107 m-1)
A.
478.7 nm
B.
291.4 nm
C.
741.9 nm
D.
1005.2 nm
E.
829.7 nm


5.
The de Broglie equation predicts that the wavelength of a neutron with a mass of 1.675×10-27 kg moving at a speed of 5.76×105 m/s is
A.
6.87×10-13 m
B.
5.01×10-15 m
C.
3.93 ×10-9 m
D.
6.87×10-20 m
E.
5.01×10-5 m


6.
Consider the principal (n), angular momentum (l), and magnetic (ml) quantum numbers describing the orbitals of the H atom. The size of an atomic orbital is associated with
A.
the angular momentum quantum number
B.
the magnetic quantum number
C.
the principal and angular momentum quantum numbers
D.
the angular momentum and magnetic quantum numbers
E.
the principal quantum number


7.
Which of the following is a correct set of quantum numbers for an electron in a 7d orbital?
A.
n = 8, l = 2, ml = –3
B.
n = 8, l = 7, ml = –1
C.
n = 7, l = 7, ml = 3
D.
n = 6, l = –2, ml = –3
E.
n = 7, l = 2, ml = –1


8.
Which of the following statements is correct?
A.
In the Bohr model of the hydrogen atom the electron moves around the nucleus in elliptical orbits.
B.
In the quantum mechanical treatment of the hydrogen atom the probability to find the electron at a given point is proportional to the square of the wave function at that point.
C.
Emission spectra of atoms in the gas phase are continuous and consist of all wavelengths in a given spectral range.
D.
Solid objects heated to incandescence produce line spectra which consist of discrete wavelengths called spectral lines.
E.
The ejection of electrons from metal surfaces by irradiation with light occurs at all frequencies of the light as long as the light is intense enough.


9.
'No two electrons in the same atom can have the same four quantum numbers' is a statement of
A.
Hund's rule.
B.
the Pauli exclusion principle.
C.
Heisenberg's uncertainty principle.
D.
the aufbau principle.
E.
the periodic law.


10.
Select the correct set of quantum numbers (n, l, ml, ms) for the highest energy electron in the ground state of silicon, Si.
A.
2, 0, 0, ½
B.
2, 1, 2, -½
C.
3, 0, 2, ½
D.
3, 1, 0, ½
E.
2, 0, 2, -½


11.
Select the correct electron configuration for Co (Z = 27).
A.
[Ar]4s13d8
B.
[Ar]4s23d7
C.
[Ar]4s24d7
D.
[Ar]3d9
E.
[Kr]4f143d9


12.
Which of the following elements has the smallest atomic size?
A.
Br
B.
F
C.
As
D.
In
E.
Cs


13.
Which of the following elements has the largest first ionization energy?
A.
Br
B.
Ne
C.
Se
D.
Sn
E.
Ra


14.
Select the element that most readily becomes an anion (i.e., accepts an electron most readily).
A.
He
B.
As
C.
Pb
D.
S
E.
Ga


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.
In+
B.
Ca2+
C.
Ni2+
D.
Cd2+
E.
Au+


17.
What is the correct order of decreasing size of the following ions (from left to right)?
A.
Se2- > S2- > Cl- > K+
B.
S2- > Se2- > K+ > Cl-
C.
Se2- > Cl- > S2- > K+
D.
K+ > Cl- > S2- > Se2-
E.
Cl- > K+ > Se2- > S2-


18.
In which of these substances are the atoms held together by ionic bonding?
A.
ClF
B.
Al
C.
CsCl
D.
HBr
E.
Ag


19.
The Lewis symbol is valid for
A.
Sb
B.
Sn
C.
B
D.
Te
E.
Cl


20.
Arrange the following four ionic compounds in order of increasing lattice energy (from left to right).
A.
RbBr < KCl < CaS < MgS
B.
KCl < RbBr < CaS < MgS
C.
RbBr < KCl < MgS < CaS
D.
KCl < RbBr < MgS < CaS
E.
MgS < CaS < KCl < RbBr


21.
The lattice energy of CaCl2 is the energy change for which one of the following processes?
A.
CaCl2(g)    →    Ca2+(s)   +   2Cl-(s)
B.
CaCl2(s)    →    Ca(s)   +   2Cl(g)
C.
CaCl2(s)    →    Ca(s)   +   Cl2(g)
D.
CaCl2(s)    →    Ca2+(g)   +   2Cl-(g)
E.
CaCl2(aq)    →    CaCl2(s)


22.
Arrange the following bonds in order of increasing bond strength (from left to right).
A.
Si–I < Si–Br < Si–Cl < Si=O
B.
Si–Cl < Si–Br < Si–I < Si=O
C.
Si=O < Si–I < Si–Br < Si–Cl
D.
Si=O < Si–Cl < Si–Br < Si–I
E.
Si–Cl < Si=O < Si–Br < Si–I


23.
Arrange the following elements in order of increasing electronegativity (from left to right).
A.
S < Si < K < Fr
B.
K < Fr < S < Si
C.
Fr < K < S < Si
D.
K < Fr < Si < S
E.
Fr < K < Si < S


24.
Select the most polar bond amongst the following.
A.
F–O
B.
F–Sn
C.
Se–Se
D.
F–Se
E.
Se–Sn


25.
Which one of the following properties is least characteristic of a typical metal?
A.
moderately high melting point
B.
high boiling point
C.
poor heat conductivity
D.
good electrical conductivity
E.
malleability and ductility


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