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Chapter 13 and 14 REVIEW TEST


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

 1. 
The distance between two successive peaks on a wave is its
a.
frequency.
c.
quantum number.
b.
wavelength.
d.
velocity.
 

 2. 
Max Planck proposed that a hot object radiated energy in small, specific amounts called
a.
quanta.
c.
hertz.
b.
waves.
d.
electrons.
 

 3. 
Bohr's theory helped explain why
a.
electrons have negative charge.
b.
most of the mass of the atom is in the nucleus.
c.
excited hydrogen gas gives off certain colors of light.
d.
atoms combine to form molecules.
 

 4. 
The change of an atom from an excited state to the ground state always requires
a.
absorption of energy.
c.
release of visible light.
b.
emission of electromagnetic radiation.
d.
an increase in electron energy.
 
 
ch13-14review_test_files/i0060000.jpg
 

 5. 
According to Bohr, electrons cannot reside at ____ in the figure above.
a.
point A
c.
point C
b.
point B
d.
point D
 

 6. 
The region outside the nucleus where an electron can most probably be found is the
a.
electron configuration.
c.
s sublevel.
b.
quantum.
d.
electron cloud.
 

 7. 
The quantum number that indicates the position of an orbital about the three axes in space is the
a.
principal quantum number.
c.
magnetic quantum number.
b.
angular momentum quantum number.
d.
spin quantum number.
 

 8. 
The spin quantum number of an electron can be thought of as describing
a.
the direction of electron spin.
b.
whether the electron's charge is positive or negative.
c.
the electron's exact location in orbit.
d.
the number of revolutions the electron makes about the nucleus per second.
 

 9. 
Because of the property described by the spin quantum number, an electron behaves as though it
a.
were positively charged.
c.
oscillated in one position.
b.
were a magnet.
d.
were spiraling toward the nucleus.
 

 10. 
The set of orbitals that are dumbbell-shaped and directed along the x, y, and z axes are called
a.
d orbitals.
c.
f orbitals.
b.
p orbitals.
d.
s orbitals.
 

 11. 
The p orbitals are shaped like
a.
electrons.
c.
dumbbells.
b.
circles.
d.
spheres.
 

 12. 
For the f sublevel, the number of orbitals is
a.
5.
c.
9.
b.
7.
d.
18.
 

 13. 
How many orientations can an s orbital have about the nucleus?
a.
1
c.
3
b.
2
d.
5
 

 14. 
If 8 electrons completely fill a main energy level, what is n?
a.
2
c.
8
b.
4
d.
32
 

 15. 
If the third main energy level contains 15 electrons, how many more could it possibly hold?
a.
0
c.
3
b.
1
d.
17
 

 16. 
The statement that no two electrons in the same atom can have the same four quantum numbers is
a.
the Pauli exclusion principle.
c.
Bohr's law.
b.
Hund's rule.
d.
the Aufbau principle.
 

 17. 
Both copper (atomic number 29) and chromium (atomic number 24) appear to break the pattern in the order of filling the 3d and 4s orbitals. This change in pattern is expressed by
a.
an increase in the number of electrons in both the 3d and 4s orbitals.
b.
a reduction in the number of electrons in both the 3d and 4s orbitals.
c.
a reduction in the number of electrons in the 3d orbital and an increase in the 4s orbital.
d.
a reduction in the number of electrons in the 4s orbital and an increase in the 3d orbital.
 

 18. 
The electron configuration for the carbon atom (C) is 1s2 2s2 2p2. The atomic number of carbon is
a.
3.
c.
11.
b.
6.
d.
12.
 

 19. 
What are the elements whose discovery added an entirely new row to Mendeleev's periodic table?
a.
noble gases
c.
transition elements
b.
radioactive elements
d.
metalloids
 

 20. 
What are the elements with atomic numbers from 58 to 71 in the periodic table called?
a.
the lanthanide elements
c.
the actinide elements
b.
the noble gases
d.
the alkali metals
 

 21. 
The periodic law states that the properties of elements are periodic functions of their atomic numbers. This means that the ____ determines the position of each element in the periodic table.
a.
mass number
c.
number of protons
b.
number of neutrons
d.
number of nucleons
 

 22. 
The period of an element can be determined from its
a.
reactivity.
c.
symbol.
b.
density.
d.
electron configuration.
 

 23. 
Magnesium, atomic number 12, has the electron configuration [Ne] 3s2. To what group does magnesium belong?
a.
Group 2
c.
Group 5
b.
Group 3
d.
Group 12
 

 24. 
The most reactive group of the nonmetals are the
a.
lanthanides.
c.
halogens.
b.
transition elements.
d.
rare-earth elements.
 

 25. 
A measure of the ability of an atom in a chemical compound to attract electrons is called
a.
electron affinity.
c.
electronegativity.
b.
electron configuration.
d.
ionization potential.
 

 26. 
In the alkaline-earth group, atoms with the smallest radii
a.
are the most reactive.
c.
are all gases.
b.
have the largest volume.
d.
have the highest ionization energies.
 

 27. 
As the atomic number of the metals of Group 1 increases, the ionic radius
a.
increases.
c.
remains the same.
b.
decreases.
d.
cannot be determined.
 

 28. 
The ionization energies for removing successive electrons from sodium are 496 kJ/mol, 4562 kJ/mol, 6912 kJ/mol, and 9544 kJ/mol. The great jump in ionization energy after the first electron is removed indicates that
a.
sodium has four or five electrons.
b.
the atomic radius has increased.
c.
a d-electron has been removed.
d.
the noble gas configuration has been reached.
 

 29. 
As you move down the periodic table from carbon through lead, atomic radii
a.
generally increase.
c.
do not change.
b.
generally decrease.
d.
vary unpredictably.
 

 30. 
In Groups 13 through 18, valence electrons may be in sublevels
a.
s and d.
c.
d and f.
b.
s and p.
d.
p and d.
 



 
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