Name: 
 

Chemistry 12 - Chapter 3 Quiz



True/False
Indicate whether the sentence or statement is true or false.
 

1. 

The region in space where an electron is most likely to be found is called an energy level.
 

2. 

Electron configurations are often condensed by writing them using the previous noble gas core as a starting point. In this system, [Ar] 3d34s2 would represent calcium.
 

3. 

The f sublevel is thought to have five orbitals.
 

4. 

Orbital diagrams generally include the region of space in which the electron may be found most of the time.
 

5. 

For some alpha particles to be reflected backward by a gold nucleus in Rutherford’s experiment, the gold nucleus had to be both very massive and strongly positive.
 

6. 

Rutherford knew the nucleus had to be very small because most alpha particles were deflected when fired through a layer of gold atoms.
 

7. 

Electrons shifting to higher levels, according to Bohr, would account for emission spectra.
 

8. 

Elements with atomic electron configurations ending in np5, where n is an integer from 2 to 6, are called the halogens.
 

9. 

Photon is the term used to refer to a quantum of electromagnetic energy.
 

10. 

The serious shortcoming of Bohr’s theory was failure to predict spectra for atoms other than hydrogen.
 

11. 

The Pauli exclusion principle states that two electrons may not occupy the same energy level.
 

Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
 

12. 

Rutherford’s classic experiment produced evidence for a nuclear atom model when atoms in a thin metal foil scattered a beam of
a.
cathode rays.
b.
alpha particles.
c.
X rays.
d.
electrons.
e.
protons.
 

13. 

Max Planck’s mathematical explanation of blackbody radiation required that he assume that, for atoms
a.
most of the mass is in a tiny part of the volume.
b.
electrons orbit the nucleus as planets orbit a star.
c.
electrons have several different energy levels.
d.
the energy of the vibrating atoms was quantized.
e.
all of the positive charge is located in the nucleus.
 

14. 

Niels Bohr assumed that when a photon is released from an atom to produce a bright line in the spectrum,
a.
an electron has dropped from a higher energy level to a lower one.
b.
the atom must have returned to its ground state.
c.
an electron has been converted into emitted energy.
d.
the electron has both wave and particle properties.
e.
the energy of the atom has increased one quantum.
 

15. 

If the ground-state electron configuration of an atom is [Ne] 3s2 3p4, the atom is
a.
magnesium.
b.
silicon.
c.
sulfur.
d.
argon.
e.
selenium.
 

16. 

Which of the following will not have an electron configuration ending with 3s2 3p6?
a.
chloride ion
b.
sulfide ion
c.
aluminum ion
d.
calcium ion
e.
potassium ion.
 

17. 

Which of the following is not used to determine an electron configuration for an atom?
a.
Hund’s rule
b.
Heisenberg’s uncertainty principle
c.
Pauli’s exclusion principle
d.
the aufbau principle
e.
the periodic table
 

18. 

Which of the following statements is false, based upon your knowledge of electron configurations?
a.
Iron is ferromagnetic; copper is paramagnetic.
b.
The sodium ion is formed by the sodium atom losing one s electron.
c.
The silver atom has an electron promoted from the 5s to a 4d orbital.
d.
The manganese atom has one electron in each 3d orbital.
e.
The tin (IV) ion is formed by the tin atom losing two p electrons and two d electrons.
 

19. 

The contribution of Erwin Schrödinger to the quantum mechanical atomic model was
a.
a theoretical prediction that particles should exhibit wave properties.
b.
a theoretical principle that precision of measurement has an ultimate limit.
c.
an explanation of the photoelectric effect utilizing an energy quantum.
d.
a mathematical description that treats electrons as standing waves.
e.
experimental verification of the quantization of charge.
 



 
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