NOTETAKING GUIDE: ATOMIC STRUCTURE UNIT
Use your book (and other sources if necessary) to take THOROUGH two-column notes in the first section of your spiral
notebook that address the concepts below! This is your FOUNDATION for knowledge in this unit – so DO YOUR BEST
WORK! This information is found in Chapters 3, 4, and 21 of your textbook.
PARTICLES IN THE ATOM
 For each of the subatomic particles (proton, neutron, electron) summarize the following:
o Location in the atom
o Charge
o RELATIVE mass (not the actual mass of a VERY SMALL number of grams, but rather the mass that is
designated to them in atomic mass units – amu’s). Sometimes this is also called their “mass number”
o Which scientist is credited with the discovery of that particle
 Draw a picture of an atom that shows the relative size (volume) of the nucleus compared to the whole atom.
Label the nucleus and the electron cloud.
 Define atomic number as it relates to an atom of an element. How will you determine the atomic number if you
know the number of each of the subatomic particles? What letter is used to represent it?
 Define mass number as it relates to an atom of an element. How will you determine the mass number if you
know the number of each of the subatomic particles?
 What is the OVERALL charge of an atom of ANY element? Which subatomic particles must be equal in number
for this to be the case?
 An element’s name can be written as the name-#. (example: hydrogen-1, hydrogen-2) What is meant by the
number
 The nuclear (also called nuclide) symbol for an element shows the element’s symbol with the mass number and
atomic number (see the chart on page 79 for examples.) Rewrite this for element X (a fake element) so that it
looks like: 𝐴𝑍𝑋, and label “A” and “Z” as atomic number and mass number.
 Copy the chart below in your notes and complete it. We will check this together – but you should be ok to fill it
out yourself using what you have written above!
Nuclear
symbol
125
52𝑇𝑒
Element
name-#
Atomic
number
Mass
number
6
13
Number of
protons
Number of
electrons
Number of
neutrons
nickel-62
74
107
40
32___
hydrogen-1
HISTORY OF THE ATOMIC MODEL
Study of the chemical reactions of matter gave rise to several “laws” related to them. Summarize and give examples of
each of the following:
o
o
o
Law of Conservation of Mass
Law of Definite Proportions (also called Law of Constant Composition)
Law of Multiple Proportions
A list of scientists is given below. Describe each of these scientists’ contributions to the model of the atom. Be sure to
include the general information listed for each, as well as any specific things mentioned for individual scientists. It may
be helpful for you to use a chart format to summarize the basics!
Scientist/Philosopher (the list is not in chronological order!)
Antoine Lavoisier
James Chadwick*
Max Planck
Albert Einstein
JJ Thomson*
Niels Bohr*
Democritus
John Dalton*
Robert Millikan
Ernest Rutherford*
Louis De Broglie
Werner Heisenberg
Erwin Schrodinger
Marie Curie
For all, provide:
 When/where they lived/worked
 Their MAJOR contribution to ATOMIC THEORY (many worked on other things also – focus on how they changed
our knowledge of the atom)… For JOHN DALTON, include the basic ideas of his atomic theory!
 The experiments they did that led them to their contribution (both what they are “called” and what was
involved)
 Interesting facts – other accomplishments, personal information, famous historical events at the time, etc.
 For those with a * next to their name, draw a MODEL of what ONE atom looked like according to their work
 AFTER you’ve looked all of this up, place them in order according to the progression of atomic theory, especially
the ones with the stars and Millikan!
ISOTOPES, AVERAGE ATOMIC MASS, AND AVOGADRO
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Define “isotope.” What causes the difference between isotopes? What is the same about isotopes (give several
similarities)?
Which element is the relative atomic mass system based on? Explain how it works, defining an atomic mass unit
as you explain.
Define “average atomic mass.” Where can you easily look up the average atomic mass of an element?
Write a formula for calculating the average atomic mass of an element if you know the masses of each of its
isotopes and their abundance. LEAVE SPACE for some examples in class!
Define “mole” as it is used in chemistry. What is Avogadro’s number and how does it relate to a mole?
Define “molar mass.” How does molar mass relate to average atomic mass?
Write the equalities that can be used to form conversion factors between these:
_______ mole = ________ atoms of an element
_______ mole = ________ grams (explain where you will find this number!)
Leave space for some example conversions between mass, moles, and atoms!
NUCLEAR CHEMISTRY
Define “nucleon” as it applies to the atom.
Define “radioactive decay”, and write the nuclide symbol for the particles produced by radioactive decay: alpha, beta,
positron, and gamma. Leave some space beside each of these particle symbols to write examples of these nuclear
reactions together in class.
Define “half-life.” Give example UNITS for half-lives of substances.
Make a space for example problems involving half-life. We will work several together in class.
Compare and contrast nuclear fission and nuclear fusion. Pay attention to the processes that occur, the amount of
energy released, and give some examples of each.