INTRODUCTION: The building block of all matter is the atom. The word atomos means “indivisible” and was first used by Democritus in the 4th century B.C. This concept of the atom later returned in the atomic theory of John Dalton over 2200 years later. In the past 200 years atomic theory has dramatically changed. Today we have a predominantly mathematical model of the atom called the Quantum Mechanical Model. Atomic structure is foundational to the study of Chemistry. In particular, the organization and behavior of electrons in the “electron cloud” provides the basis of the phenomena in Chemistry as well as the reason for the organization of the Periodic Table. Because of similarities between electron configurations in the atoms there are similarities in the properties of some elements. In addition to similarities in properties there are also predictable trends in these properties of elements based on the position of the element in the periodic table. In this unit we will review simple atomic structure, learn about the importance of electron configurations, and see the effect of these arrangements of electrons on the properties of elements and groups of elements.
OBJECTIVES:
As you study this unit, you should be able to do the following:
Summarize the development of the Modern Atomic Theory
incorporating the contributions of Dalton, Thomson, Rutherford, Bohr and
Schrodinger. (3-2, 3-2, 4-2,
4-3, 4-4)
Distinguish among protons, electrons, and neutrons in
terms of their relative masses, charges and location in the atom.
(3-3)
Infer the number of protons, electrons, and neutrons
using the atomic number and mass number of an element. (3-3)
Explain how an element can become an ion in terms of
sub atomic particles. Also
infer the number of protons, electrons, and neutrons using the atomic
number, mass number and charge of an ion.
(3-3)
Describe changes that occur in the nucleus of an atom when it undergoes radioactive decay. Write a nuclear equation for a and b particle decay. (3-4)
Explain the significance of quantized energies of the
Quantum Mechanical Model. (4-2
& 4-3)
Describe atomic orbitals in terms of shape, size and
relative energy. (4-4)
Apply the Aufbau principal, Pauli exclusion principal
and Hund’s Rule to write electron configurations and orbital diagrams for
elements. (4-5)
LEARNING ACTIVITIES:
These activities are to be completed and handed in parts.
The components of Chapter 3 and 4 are due by
To learn about objectives 1-5:
READ Chapter 3-1 to 3-4; pp. 90 - 117. See objectives for specific section.
WRITE answers to end of the chapter questions 1-5, 8-10, 12, 15-18, 22-24, 27, 30; pp. 122-123 AND Unit Review questions: 30, 31 p. 221.
WRITE worksheet: ChemActivity 1: The Nuclear Atom (hand out)
READ and PERFORM Lab Exploration “Ions and Atoms.”
WRITE answers to questions for “Ions and
Atoms.”
Quiz on objectives 1-5 Day 2 of Week of Oct. 11. [C & D blocks on Tues Oct. 12; E & F blocks on Thur. Oct. 14] Chapter 3 homework problems are due by 4 pm the day of your quiz.
To learn about objectives 1, 6-8:
READ all of Chapter 4 , pp. 124-153.
EXPLORE Discovering Science database on the computers to learn more about Dalton, Thomson, Rutherford, Bohr, Schrodinger and their atomic theories. (Optional)
WRITE answers to end of the chapter questions 3-10, 12-15, 18, 20, 22, 23, 26-28; pp. 156-157.
To make sure you understand the objectives for this unit:
ASK me, the teacher, any lingering QUESTIONS
TAKE the Unit’s Self-Test
TEST ON CHAPTERS 3-4
on
