Chemistry: Matter and Change

Section 3: How Atoms Differ

Self Check Quizzes

1
Why are all atomic masses not nearly whole numbers?

<a onClick="window.open('/olcweb/cgi/pluginpop.cgi?it=jpg::::/sites/dl/free/007874637x/514737/fig4_18.jpg','popWin', 'width=NaN,height=NaN,resizable,scrollbars');" href="#"><img valign="absmiddle" height="16" width="16" border="0" src="/olcweb/styles/shared/linkicons/image.gif"> (40.0K)</a>
A)This is due to the mass of all the electrons in the atom.
B)This is because of experimental error.
C)This is because atomic masses are the weighted average of the masses of all naturally-occurring isotopes.
D)This is due to binding energy of the atoms.
2
The atomic number of an element is defined by its number of ________.
A)protons
B)neutrons
C)electrons
D)nuclei
3
The sum of the protons and neutrons in a nucleus is __________.
A)the atomic number
B)the mass number
C)Avogadro's number
D)the element number
4
Which of the following is true for any atom?
A)atomic number = number of protons = number of electrons
B)atomic number = number of neutrons = number of electrons
C)mass number = number of protons = number of electrons
D)mass number = number of protons = number of neutrons
5
How is the atomic mass unit (amu) defined?
A)1/12 the mass of a carbon-12 atom
B)1/14 the mass of a nitrogen-14 atom
C)1/13 the mass of a carbon-13 atom
D)1/16 the mass of an oxygen-16 atom
Glencoe Online Learning CenterScience HomeProduct InfoSite MapContact Us

The McGraw-Hill CompaniesGlencoe

Please read our Terms of Use and Privacy Policy before you explore our Web site. To report a technical problem with this Web site, please contact the Web Producer.