Chemistry 1
Unit 4, Beginning Atomic Theory and the Periodic Table
Guiding Questions:
1. How can the properties of atoms be predicted by the number of each of its
subatomic particles?
2. What is the relationship to the subatomic particles and ions?
3. What is the relationship to the subatomic particles and isotopes?
4. What are some of the ways that subatomic particles can be represented?
5. How can the periodic table be used to get information about electrons in
an atom?
6. How do trends develop throughout the periodic table?
Key Vocabulary Terms:
Subatomic particles
Neutrons
Nonmetals
Family
Atomic radius
Ionic compounds
electrons
energy levels
metalloids
period
electronegativity
covalent compounds
protons
metals
group
periodicity
ionization energy
Questions for Review
1. Describe the atomic theory of each of the following people in history:
a. Democritus
b. Aristotle
c. John Dalton
d. J.J. Thomson
e. Ernest Rutherford
2. Describe the three laws that Dalton used to create his atomic theory:
a. Law of conservation of mass
b. Law of Definite Proportion (or Composition)
c. Law of Multiple Proportion
3. Compare the three subatomic particles:
Particle
Symbol Charge Relative Mass
Proton
Neutron
Electron
Location
4. For each of the following neutral isotopes, provide the missing
information.
Isotope Name
Helium-4
Atomic number
53
Number of Protons
Number of Neutrons
74
143
Number of Electrons
92
5. Which subatomic particle identifies an atom as that of a particular
element? How is this particle related to the atom’s atomic number?
6. What is the difference between an isotope and an ion?
7. How is the charge of an ion determined? What can be said about the
attraction between ions?
8. Calculate the average atomic mass of uranium. Relative abundances of
the isotopes are shown below.
Isotope Mass
Relative Abundance
Uranium-234
0.005%
Uranium-235
0.720%
Uranium-238
99.275%
9. Calculate the average atomic mass of nickel. Relative abundances of
the isotopes are shown below:
Isotope Mass
Relative Abundance
Nickel-58
68.27%
Nickel-60
26.10%
Nickel-61
1.13%
Nickel-62
3.59%
Nickel-64
0.91%
10. Explain how the existence of isotopes is related to atomic masses not
being whole numbers.
11. What is the difference between a covalent bond and an ionic bond?
12. Name the representative particle for each of the following substances: a
monatomic element, an ionic compound, a covalent compound, and a
diatomic element.
13. List the diatomic molecules, also known as the stupendous seven.
14. Which elements are gases under standard conditions? Which elements
are liquids under standard conditions? Which elements are manmade?
15. Provide the element name or chemical symbol as specified below. Then
classify each as a metal, nonmetal, or metalloid.
Element Name
Chemical
Metallic Nature
Symbol
sodium
Fe
fluorine
Mg
silicon
S
16. Distinguish between a group and a period on the periodic table.
17. State the element name, atomic number, and/or atomic mass as
specified below:
Element Name
Atomic Number
Atomic Mass (amu)
phosphorus
38
238.029
Copper
10
26.9815
18. Describe the contributions of the following to the modern periodic table.
a. John Newlands
b. Lothar Meyer
c. Dmitri Mendeleev
d. Henry Moseley
19. What is the difference between Mendeleev’s period law and Moseley’s
modern periodic law?
20. Show the location of a family or group, period, halogens, noble gases,
alkali metals, alkaline earth metals, transition metals, inner transition
metals, nonmetals, metalloids, representative elements, and metals.