Chemistry Chapter 5B (Prentice)
 
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Chemistry Chapter 5B (Prentice)

Matching
 
 
Match each item with the correct statement below.
a.
atomic emission spectrum
d.
photon
b.
frequency
e.
quantum
c.
wavelength
f.
spectrum
 

 1. 

discrete bundle of electromagnetic energy
 

 2. 

energy needed to move an electron from one energy level to another
 

 3. 

number of wave cycles passing a point per unit of time
 

 4. 

distance between wave crests
 

 5. 

separation of light into different wavelengths
 

 6. 

frequencies of light emitted by an element
 

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

 7. 

In the Bohr model of the atom, an electron in an orbit has a fixed ____.
a.
position
c.
energy
b.
color
d.
size
 

 8. 

The shape (not the size) of an electron cloud is determined by the electron's ____.
a.
energy sublevel
c.
speed
b.
position
d.
principal quantum number
 

 9. 

The letter "p" in the symbol 4pmc009-1.jpg indicates the ____.
a.
spin of an electron
c.
principle energy level
b.
orbital shape
d.
speed of an electron
 

 10. 

What is the electron configuration of potassium?
a.
1smc010-1.jpg2smc010-2.jpg2pmc010-3.jpg3smc010-4.jpg3pmc010-5.jpg4smc010-6.jpg
c.
1smc010-12.jpg2smc010-13.jpg3smc010-14.jpg3pmc010-15.jpg3dmc010-16.jpg
b.
1smc010-7.jpg2smc010-8.jpg2pmc010-9.jpg3smc010-10.jpg3pmc010-11.jpg
d.
1smc010-17.jpg2smc010-18.jpg2pmc010-19.jpg3smc010-20.jpg3pmc010-21.jpg4smc010-22.jpg
 

 11. 

How many unpaired electrons are in a sulfur atom (atomic number 16)?
a.
0
c.
2
b.
1
d.
3
 

 12. 

What is the wavelength of an electromagnetic wave that travels at 3 mc012-1.jpg 10mc012-2.jpg m/s and has a frequency of 60 MHz? (1 MHz = 1,000,000 Hz)
a.
mc012-3.jpg
b.
60 MHz ´ 300,000,000 m/s
c.
mc012-4.jpg
d.
No answer can be determined from the information given.
 

 13. 

The light given off by an electric discharge through sodium vapor is ____.
a.
a continuous spectrum
c.
of a single wavelength
b.
an emission spectrum
d.
white light
 

 14. 

Emission of light from an atom occurs when an electron ____.
a.
drops from a higher to a lower energy level
b.
jumps from a lower to a higher energy level
c.
moves within its atomic orbital
d.
falls into the nucleus
 

 15. 

As changes in energy levels of electrons increase, the frequencies of atomic line spectra they emit ____.
a.
increase
c.
remain the same
b.
decrease
d.
cannot be determined
 

 16. 

The atomic emission spectra of a sodium atom on Earth and of a sodium atom in the sun would be ____.
a.
the same
b.
different from each other
c.
the same as those of several other elements
d.
the same as each other only in the ultraviolet range
 

 17. 

What is the approximate energy of a photon having a frequency of 4 mc017-1.jpg 10mc017-2.jpg Hz? (h = 6.6 mc017-3.jpg 10mc017-4.jpg Jmc017-5.jpgs)
a.
3 mc017-6.jpg 10mc017-7.jpg J
c.
2 mc017-10.jpg 10mc017-11.jpg J
b.
3 mc017-8.jpg 10mc017-9.jpg J
d.
3 mc017-12.jpg 10mc017-13.jpg J
 

 18. 

What is the approximate frequency of a photon having an energy 5 mc018-1.jpg 10mc018-2.jpg J? (h = 6.6 mc018-3.jpg 10mc018-4.jpg Jmc018-5.jpgs)
a.
8 mc018-6.jpg 10mc018-7.jpg Hz
c.
3 mc018-10.jpg 10mc018-11.jpg Hz
b.
3 mc018-8.jpg 10mc018-9.jpg Hz
d.
1 mc018-12.jpg 10mc018-13.jpg Hz
 

 19. 

Which of the following quantum leaps would be associated with the greatest energy of emitted light?
a.
n = 5 to n = 1
c.
n = 2 to n = 5
b.
n = 4 to n = 5
d.
n = 5 to n = 4
 

 20. 

Which variable is directly proportional to frequency?
a.
wavelength
c.
position
b.
velocity
d.
energy
 

 21. 

How do the energy differences between the higher energy levels of an atom compare with the energy differences between the lower energy levels of the atom?
a.
They are greater in magnitude than those between lower energy levels.
b.
They are smaller in magnitude than those between lower energy levels.
c.
There is no significant difference in the magnitudes of these differences.
d.
No answer can be determined from the information given.
 

 22. 

What are quanta of light called?
a.
charms
c.
muons
b.
excitons
d.
photons
 

 23. 

Which scientist developed the quantum mechanical model of the atom?
a.
Albert Einstein
c.
Niels Bohr
b.
Erwin Schrodinger
d.
Ernest Rutherford
 

 24. 

Bohr's model could only explain the spectra of which type of atoms?
a.
single atoms with one electron
b.
bonded atoms with one electron
c.
single atoms with more than one electron
d.
bonded atoms with more than one electron
 

 25. 

The quantum mechanical model of the atom ____.
a.
defines the exact path of an electron around the nucleus
b.
was proposed by Niels Bohr
c.
involves the probability of finding an electron in a certain position
d.
has many analogies in the visible world
 

 26. 

Who predicted that all matter can behave as waves as well as particles?
a.
Albert Einstein
c.
Max Planck
b.
Erwin Schrodinger
d.
Louis de Broglie
 

 27. 

According to the Heisenberg uncertainty principle, if the position of a moving particle is known, what other quantity CANNOT be known?
a.
mass
c.
spin
b.
charge
d.
velocity
 

 28. 

How can the position of a particle be determined?
a.
by analyzing its interactions with another particle
b.
by measuring its velocity
c.
by measuring its mass
d.
by determining its charge
 

 29. 

The wavelike properties of electrons are useful in ____.
a.
defining photons
b.
writing electron configurations
c.
magnifying objects
d.
determining the velocity and position of a particle
 

 30. 

In an s orbital, the probability of finding an electron a particular distance from the nucleus does NOT depend on ____.
a.
a quantum mechanical model
c.
the Schrodinger equation
b.
direction with respect to the nucleus
d.
the electron energy sublevel
 



 
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