Chapter 3: Chemical Foundations: Elements, Atoms, and Ions
Chapter 19: Radioactivity and Nuclear Energy
Purpose
All matter is made from atoms and all matter can be broken down chemically into elements. Our understanding of
the elements has evolved through time with several important scientists making major contributions to our
current understanding.
In this Topic, we will study the elements, the history of the atom, and the modern concept of the atom. We will
also understand how an element can exist as different isotopes and as an ion.
A and B
10/1 and 10/2
In-Class
 Combined Element quiz
 Chapter 3 and 19 Notes
 Assign Polyatomic Ion Quiz
(Symbol – name 10/15 for
B day and 10/16 for A day)
(Name – symbol 10/21 for
B day and 10/22 for A day)
 Go over Atomic
Structure/Ion Worksheet
 CCC – Atomic Structure
 Explain Graphing Activity
 Radioactivity of Pennium
Lab*
10/7 and 10/8
 Go over Ch 3 and 19: Wk #1
 Unknown Liquid Lab*
 CCC- Radioactivity
10/9 and 10/13  Go over Ch 3 and 19 Review
Sheet
 Chapter 3 and 19 Test
10/14
 PSAT
10/15 and
 Polyatomic Ion Quiz
10/16
Symbol – name
 Introduce One to the World
Atomic Theory
10/19 and
 Research Atomic Theory
10/20
* These labs require appropriate lab attire!!
HW Assignments
 Atomic Structure/Ion
Worksheet
 Chapter 3 and 19:
Worksheet #1
 Finish Graphing Activity
10/5 and 10/6
 Chapter 3 and 19 Review
Sheet
 Study for Test!!
 Color periodic table
 Study for Polyatomic Ion
Quiz Symbol-name



Study for Polyatomic Ion
Quiz Name-symbol
Vocabulary
atom
atomic mass
atomic number
proton
neutron
electron
isotope
half-life
α (alpha) radiation
β (beta) radiation
γ (gamma) radiation
Democritus
Dalton
Thomson
Millikan
Rutherford
By the end of these Topics, you should be able to demonstrate proficiency in the following areas:
Essential Understandings
The concepts developed in this standard include the following:

The atomic number of an element is the same as the number of protons. In a neutral atom, the number
of electrons is the same as the number of protons. All atoms of an element have the same number of
protons.

The average atomic mass for each element is the weighted average of that element’s naturally occurring
isotopes.

The mass number of an element is the sum of the number of protons and neutrons. It is different for
each element’s isotopes.

An isotope is an atom that has the same number of protons as another atom of the same element but
has a different number of neutrons. Some isotopes are radioactive; many are not.

Half-life is the length of time required for half of a given sample of a radioactive isotope to decay.

Electrons have little mass and a negative (–) charge. They are located in electron clouds or probability
clouds outside the nucleus.

Protons have a positive (+) charge. Neutrons have no charge. Protons and neutrons are located in the
nucleus of the atom and comprise most of its mass. Quarks are also located in the nucleus of the atom.
Knowledge, and Skills
In order to meet this standard, it is expected that students will

determine the atomic number, atomic mass, the number of protons, and the number of electrons of any
atom of a particular element using a periodic table.

determine the number of neutrons in an isotope given its mass number.

perform calculations involving the half-life of a radioactive substance.

differentiate between alpha, beta, and gamma radiation with respect to penetrating power, shielding,
and composition.

differentiate between the major atom components (proton, neutron and electron) in terms of location,
size, and charge.

identify key contributions of principal scientists including: Democritus, Dalton, Thomson, Rutherford,
Millikan

differentiate between the historical and quantum models of the atom.
SOL Standard
CH.2 The student will investigate and understand that the placement of elements on the periodic table is a
function of their atomic structure. The periodic table is a tool used for the investigations of
b) isotopes, half lives, and radioactive decay;
c) mass and charge characteristics of subatomic particles;
i) historical and quantum models.