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SCH4U- Kapica
Name:________________
Section A- Multiple Choice ( K/ U)
Please transfer your answers to your test sheet.
1.
Which of the following did the Bohr model of the atom help explain
a) Nuclear Structure
c) Atomic Spectra
b) Structure of the electron
d) Wave property of the Atom
e) Structure of the alpha particle
2.
Which of the following electron configurations is impossible for an atom, regardless of whether it is in the ground state or
an excited state?
a) 1s22s22p3
c) 1s32s12p4
b) 1s22s12p1
d) 1s22s12p3
2 2
6
e) 1s 2s 2p
3.
Which of the following electron configurations shows a transition metal atom?
a) 1S22s22p5
b) 1s22s22p63s23p64s23d104p3
2 2
6 2
1
b) 1s 2s 2p 3s 3p
e) 1s22s22p63s23p64s23d3
2 2
6 2
6 2
10 2
1
e) 1 s 2s 2p 3s 3p 4s 3d 4s 4p
4.
Who postulated that electrons must fill the lowest available energy level ?
a) Schrodinger
c) Heisenberg
b) Bohr
d) Einstein
e) Aufbau
5.
What experimental evidence led Bohr to believe that electrons can possess only specific amounts of energy?
a) most alpha particles went straight through the gold foil
b) some alpha particles were deflected by the gold foil
c) the line spectra produced by excited atoms
d) atoms are electrically neutral
e) none of the above
6.
Which atoms could have the electron configuration shown below:
____
s
___ ___ ___
p
a) N3c) O2e) All of the above
b) Cl 1d) Ar
7.
Which of the following is true of electron orbitals?
a) They are three-dimensional
b) They can contain maximum of two electrons
c) Their shapes are predicted by Schrödinger’s equation
d) all of the above
e) none of the above
8.
Which of the following sets of quantum numbers (written in the following order, n, l, ml, ms) would represent the 23rd
electron of lead ?
a) 4, 2, 3, - ½
c) 3, 2, 1, - ½
b) 3, 2, 0, ½
d) 4, 2, -1, ½
e) Two of the above are possible
SCH4U- Kapica
9.
Name:________________
The total number of orbitals in the energy levels, n=4, is
a) 16
c) 32
b) 7
d) 9
e) 8
10. Which one of the following quantum numbers would not be found for a valence electrons of phosphorus
a) ml = 0
c) l = 2
b) l = 0
d) ml = -1
d) n = 3
11. What was Planck’s contribution to the quantum mechanical model of the atom
a) the uncertainty principle
b) the concept of quanta of energy
c) the idea that every mass has a wave with which it is associated
d) the wave equation
e) a relationship between energy and mass
12. Which situation must be true for two electrons to occupy the same orbital
a) the electrons must have the same principle quantum number, but the other quantum numbers must be different
b) the electrons must have the same spin
c) the electrons must have identical sets of quantum numbers
d) the electrons must have low energy
e) the electrons must have the opposite spin
13. What did Heisenberg contribute to the quantum mechanical model of the atom?
a) The uncertainty principle
b) the concept of quanta of energy
c) the idea that every mass has a wave with which it is associated
d) the wave equation
e) a relationship between energy and mass
14. The lines of the emission spectrum of an atom results in
a) energy absorbed by electrons dropping back down to a lower energy level
b) energy absorbed by electrons jumping to a higher energy level
c) energy released by electrons jumping to a higher energy level
d) energy released by electrons dropping back down to a lower energy level
e) none of the above