Download Unit 3-The Big Picture

CHEMISTRY
UNIT THREE: ATOMIC STRUCTURE AND PERIODICITY
Overview
During this unit, students will explore the historical events leading to our understanding of atomic structure and
the quantum mechanical model of the atom for electron structure and the periodic table. They will learn about the
three fundamental particles of all atoms (the proton, neutron, and electron) and be able to identify the number of
subatomic particles in any atom using a Periodic Table. (The teacher should supply specific isotope data for neutron
counts.) Students will study the structural differences of isotopes and be able to calculate average mass of an element
given specific isotopic data. In addition, they will be introduced to nuclear chemistry.
The development of the quantum mechanical model of the atom will be discussed and students will study the
use of quantum numbers to describe probability regions for electron motion. Students should be able to write electron
configurations and draw orbital notations for all elements up to Z = 36 (using either the Aufbau diagram or the Periodic
Table). The orbital diagrams should address Hund’s Rule and the Pauli Exclusion Principle. Upon completion of this unit,
students should understand valence electrons of atoms and ions, and the pattern of valence electrons in the Periodic
Table. Dot notations for representative elements may be introduced here (or in the next unit).
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 families or groups, series and periods,
and trends (including atomic radii, electronegativity, shielding effect, and ionization energy).
Suggested Time Allotment
12 Blocks (4 1/2 weeks)
Conceptual Framework
Atomic Structure & Periodicity
History/Development
Periodic Table
Model of the Atom
Periodic Table
Nucleus
Trends
Partide Characteristics
Mendeleev
Protons
Moseley
Neutrons
Group
Electron Config.
Whole Table
Isotopes
Atomic Theory
Democritus
Dalton
Thomson
Atomic Radii
Atomic #
Electonegativity
Mass #
Ionization Energy
Isotope Symbols
Shielding Effect
Classification
Average Atomic Mass
Nuclear Chem
Periods
Groups
Particles
Rutherford
Millikan
Half-life
Alkali
Equations
Alkaline Earth
Halogen
Radioisotopes
Bohr
Electrons
Planck
Heisenberg
deBroglie
Noble Gases
Characteristics
Regions
Loss/Gain
Metals
Position (Quantum Theory)
Main Group
Levels (Aufbau)
Transition
Sublevels
Inner Transition
Orbitals (Hund)
Nonmetals
Spin (Pauli)
Metalloids
Notation
Representative Elements
Configurations (atoms/ions)
Orbital Diagrams
Dots (valence electrons)
Ground/Excited State
Spectroscopy
s, p, d, f sublevels
Related VA Standards of Learning
SOL 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
a.
b.
c.
d.
e.
f.
g.
average atomic mass, mass number, and atomic number;
isotopes, half lives, and radioactive decay;
mass and charge characteristics of subatomic particles;
families or groups;
series and periods;
trends including atomic radii, electronegativity, shielding effect, and ionization energy;
electron configurations, valence electrons, (and oxidation numbers – not covered at this time); and
i.
historical and quantum models.
Instructional Objectives
3.1
Modern atomic theory and its continuing development
3.1.1
Describe historical models of the atom as modified by current evidence, to include:
Democritus, Dalton, Thomson, Rutherford, Millikan, and Bohr.
3.1.2
Prepare models of the atoms showing the location and arrangement of protons, neutrons
and electrons (including their masses and charges).
3.1.3
Identify and define the following: mass number, atomic number, average atomic mass, and
isotopes, half-lives and radioactive decay.
3.2
Arrangement of electrons within the atom
3.2.1
Develop the quantum mechanical model of the atom showing the arrangement of electrons
into levels, sublevels, orbitals and spin, to include the contributions of the following: Planck,
Heisenberg and deBroglie; and relate the model to spectroscopy.
3.2.2
Write the ground state electron configuration for any atom or ion.
3.2.3
Identify the valence electrons for any atom or ion.
3.2.4
Write orbital notations using the following: Aufbau Principle, Pauli Exclusion Principle and
Hund’s Rule.
3.3
Periodicity
3.3.1
Explain the historical development of the periodic table and the periodic law, including the
contributions of the following: Mendeleev and Moseley.
3.3.2
Identify periods/series and groups/families by names, location on the periodic table and
characteristics to include: alkali metals, alkaline earth metals, transition metals, halogens,
noble gases, representative elements and metals, nonmetals and metalloids.
3.3.3
Using the periodic table, investigate the following and make predictions:
a.
b.
c.
d.
e.
electron configuration
atomic radii
electronegativity
shielding effect
ionization energy.
Enduring Understanding
 Atomic structure is fundamental to understanding matter.
Essential Questions
 How are the characteristics of atoms determined?
 How is the periodic table an important tool for understanding matter?
Guiding Questions
 How has the model of the atom evolved?
 How do electron configurations show similarities and differences between groups and periods?
 How can the periodic table be used to make predictions?
What Students Should Know
 Discoveries and insights related to its structure have changed the model of the atom over time.
 Major insights regarding the atomic model of the atom and principal scientists include:
 particles – Democritus
 first atomic theory of matter – John Dalton
 discovery of the electron – J.J. Thomson
 discovery of the nucleus – Ernest Rutherford
 discovery of charge of electron – Robert Millikan
 planetary model of atom – Niels Bohr
 periodic table by atomic mass – Dmitri Mendeleev
 periodic table by atomic number – Henry Moseley
 quantum nature of energy – Max Planck
 uncertainty principle – Werner Heisenberg
 wave theory – Louis deBroglie
 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 its mass.
 All atoms of the same element have the same number of protons.
 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.


















In a neutral atom, the number of electrons is the same as the number of protons.
The atomic number of an element is the same as the number of protons.
The periodic table is arranged by increasing atomic numbers.
The atomic mass for each element is the weighted average of that element’s naturally occurring isotopes.
The modern atomic theory is called the Quantum Mechanical Model.
Electron configuration is the arrangement of electrons around the nucleus of an atom based on their energy level.
Atoms can gain or lose electrons within the outer energy level. Discoveries and insights related to its structure have
changed the model of the atom over time.
The Periodic Law states that when elements are arranged in order of increasing atomic numbers, their physical and
chemical properties show a periodic pattern.
Vertical columns called groups have similar properties because of their similar valence electron configurations.
Horizontal rows called periods have predictable properties based on an increasing number of electrons in the outer
orbitals.
The names of groups and periods on the periodic chart are alkali metals, alkaline earth metals, transition metals,
halogens, noble gases, and metalloids.
Periods and groups are named by numbering columns and rows.
Some elements such as oxygen, hydrogen, fluorine, chlorine, bromine and nitrogen, naturally occur as diatomic
molecules.
Periodicity is regularly repeating patterns or trends in the chemical and physical properties of the elements arranged
in the periodic table.
Atomic radius decreases from left to right and increases from top to bottom within given groups.
Electronegativity increases from left to right within a period and decreases from top to bottom within a group.
Shielding effect is constant within a given period and increases within given groups from top to bottom.
Ionization energies generally increase from left to right and decrease from top to bottom of a given group.
What Students Should Be Able To Do
 Using a periodic table, determine the atomic number, atomic mass, the number of protons, and the number of
electrons of an atom of a particular element.
 Using specific isotopic data, determine the numbers of neutrons in a specific isotope of an element.
 Use an element’s electron configuration to determine the number of valence electrons and possible oxidation
numbers.
Instructional Resources
Text: Modern Chemistry, pp. 68-95, pp. 97-131, pp. 132-165.
Chemistry Unit 3 Activities: Atomic Structure, Atomic Theorists and Their Contributions, Beanium Lab, Isotopes of
Pennies Lab, Calculating the Atomic Mass of Vabeachium, Isotopes and Average Atomic Mass, Electron Configurations,
Orbital Diagrams and Valence Electrons, Flame Test Lab, License Plate Element Project, Adopt-An-Element, Periodic
Trends of the Elements, Periodic Table Worksheet, Periodic Trends, Laboratory Investigation: Determining Trends in a
Group, Lab: Trends on the Periodic Table, Electrons in Atoms, Chem Activity: Bohr Models and Periodic Relationships,
and Museum of Recognition.
Suggested Assessment Evidence
Pre-Assessment
 Produce a “square” from the periodic table representing an element with questions about the information from the
square (atomic mass, atomic number, number of protons, symbol, etc.)
 Ask students to draw a model of the atom, labeling the parts.
 Label a blank periodic table with information such as groups, periods, metals, and nonmetals.
On-going Assessment
 Use frequent questioning strategies ranging from basic to upper level thinking skills. Suggestions include:






What is the charge of the nucleus of the atom? Why?
Which part of the atom is responsible for its mass? Which part of the atom is responsible for its volume?
Compare and contrast nuclide symbols of various isotopes.
What is the process for finding the average atomic mass of an element?
How does average atomic mass differ from mass number?
In terms of electron configurations, what do elements in the same group have in common? What do elements in
the same period have in common?
 Describe how electrons fill energy levels, sublevels, and orbitals.
 What are the properties of the different groups on the periodic table and how do they relate to reactivity?
 What effect does shielding have on atomic radius, ionization energy, and electronegativity?
 Use the VA SOL Released Test Items on Atomic Structure and Periodicity as daily warm-up exercises.
Unit 3 Atoms - Lessons
Objectives
AB 12 Thur-Fri Oct 7-8
START UNIT 3 – ATOMIC STRUCTURE &
PERIODICITY
1.Identify key ideas in UNIT 3
2.Critique Unit 2 Test
3.Review Sci notation, sig figs, conversions
factors, Si conversions
AB 13 - Mon-Tues Oct 11-12 UNIT 3
ATOMIC STRUCTURE & PERIODICITY
Chapter 3.1 ATOMS – The idea
1. Explain the LAW OF DEFINITE
PROPORTIONS
2. Explain the LAW OF MULTIPLE
PROPORTIONS
3. Summarize DALTON’S ATOMIC THEORY
4. Explain the relationship between Dalton’s
Theory and the LAWs OF: CONSERVATION
OF MASS, DEFINITE PROPORTIONS,
MULTIPLE PROPORTIONS
Procedures
START UNIT 3 – ATOMIC STRUCTURE &
PERIODICITY
1.Identify key ideas in UNIT 3
2.Critique Unit 2 Test
3.Review Sci notation, sig figs, conversions
factors, Si conversions
1.Critique MC part of Unit 2 TEST
2.Q/A Sections 1&2 of Chapter 3
3.Online Textbook Videos
4.QUIZ, Chapter 3.1 (CPS)
HW-Materials
Unit 2 TEST
Textbook
HW
Read – STUDY Chapter 3.1
Review SI Conversions
Textbook
Unit 2 TEST
CPS
HW: Chapter 3
Ready / Study Sections 1&2, Chapter 3,
complete Section Review questions, p.
71 and p.76
A/B 14 Wed-Thur Oct 13-14
Chapter 3.2 ATOMS – The Structure &
Models
UNIT 3 – ATOMIC STRUCTURE &
PERIODICITY
1.Summarize the Cathode Ray Tube
experiment leading to the identification of
the electron.
2. Describe Rutherford’s experiment,
leading to the discovery of the nucleus.
3.List the properties of the subatomic
particles; proton, neutron, electron
4. Define ATOM
A/B 15 Fri-Mon Oct 15 & 18
Chapter 3.2 and 3.3 ATOMS – The Structure
& Models
1.Show Cathode Ray video
2.Show PHet video
http://phet.colorado.edu.simulations
3. complete “1st 18 Elements Chart”
4.Chp 3-2 QUIZ
Complete all of Sections 1 & 2 in Chp 3
Complete Rutherford Lab
1. Define: Mole
Avogadro’s Number
Molar mass
2. Calculate Average Atomic Mass given
relative abundance of isotopes
3.Convert among moles, atoms and grams
for any gram formula unit
A/B 17 Thur-Fri Oct 21-22
Prepare for Chapter 3 TEST
Textbook etc.
1. Complete Rutherford Lab QZ (10 min)
Section 3, Chapter 3
Complete 1st 18 Elements Chart
Describe Tables 2 & 3
Describe / Sample Problem and Practice
Problems, p. 80, 84, 85, 86, 87
2.Complete Chp3-3QUIZ
Textbook
1.Review Chapter 3
2.Work problems in Chapter 3-3
Textbook, Calculator, pencil etc
A/B 18 Mon-Tue Oct 25-26
CHAPTER 3 TEST
Demonstrate mastery of objectives from Oct
16 – Oct 23
Complete Chapter 3 TEST
A/B 19 Wed-Thur Oct 27-28
Chapter 4.1 ELECTRONS – New Atomic
Model
1. Discuss Section 1 & 2, Chapter 4
2. Complete Section Review questions, p.
103
1.Explain the relationship among speed,
wavelength and frequency of
HW
Answer all section review questions,
p.76
Focus on Table 1, p. 76
HW
1. Read/Study Chapter 3, Section 3
2.Complete Section Review p.87
1. Describe Isotopes
2.Define atomic number and mass number
and explain how the relate to isotopes
3. Identify number of subatomic particles in
any identified nucleus
4.Define Mole, Avogadro’s #, Molar Mass
5.Calculate Average Atomic Mass given
abundance
6.Convert moles, atoms, mass for any gram
formula unit
A/B 16 Tue-Wed Oct 19-20
Chapter 3.3 ATOMS – Mole
United Streaming videos
PHet video
1st Element Chart
Begin reading – Studying Chapter 4
Rutherford Quiz
HW:
1.Section Review, p. 87
2. Problems, p. 80, 84, 85, 86, 87
3.Complete Chp3-3QUIZ
HW:
Prepare for Chapter 3 TEST
Chapter 3 TEST
Textbook
HW:
Read/Study Sections 1 & 2 of Chapter
4
Textbook
HW:
Review Section 1, Chapter 4
Read / study Section 2, Chapter 4
electromagnetic radiation
2.Describe the dual “wave-particle” nature
of light
3. Explain how the photoelectric effect and
the Hydrogen emission spectrum contribute
to the modern atomic model.
4. Relate Bohr’s model of the atom to the
Hydrogen emission spectrum
A/B 20 Fri & Mon Oct 29-Nov 1
Chapter 4.2 – QUANTUM MODEL
LAB – Emission Spectrum
Discuss Section 2, Chapter 4, The
Quantum Model of the Atom
Text book
1.Draw 5 atomic models
2.Illustrate the quantum model of the
atom through the 3s orbital
3.Complete Section Review Questions.
P.110
Textbook
Discuss Section 3, Chapter 4
Complete Practice Problems, 1 & 2, p.113
Complete Practice Problems 1-4, p. 121
Complete Practice Problems 1 & 2, p.122
Complete Section Review Ques. p. 122
Materials = Textbook
1.Demonstrate Bright Line Emission
Spectrum
2.Calculate wavelength given frequency;
frequency given wavelength
A/B 21 Wed-Thur Nov 3-4
Chapter 4.2, QUANTUM MODEL P.104
1.Discuss de Broglie’s role in the
development of the quantum model of the
atom
2.Compare the Bohr model and the
quantum model of the atom
3.Explain how Heisenberg’s and
Schrodinger’s work led to the idea of atomic
orbitals
4. Describe the four QUANTUM NUMBERS.
A/B 22 Fri & Mon Nov 5-8
Chapter 4.3 ELECTRON CONFIGURATION
1.List the number of electrons needed to
occupy each main energy level
2.State the 3 major principles governing
electron configurations: Aufbau Principle,
Pauli Exclusion Principle and Hund’s Rule
3.Describe electron configurations of any
element with ELECTRON CONFIGURATION,
ORBITAL NOTATION & NOBLE GAS
NOTATION
Final Review for Quarter 1 EXAM
AB 23 Tue-Wed Nov 9-10
1st Quarter EXAM
Thursday Nov 11
HW
Complete Emission Spectrum Exercise
Prepare for spectrum Quiz
HW
1.Complete the “Models of the Atom”
exercise
2. Complete the Section Review
3. Questions, p. 110
4. Read / Study Section 3, Chap 4
HW
Complete all class work
Practice Pblms, 1 & 2, p.113
Practice Pblms 1-4, p. 121
Practice Pblms 1 & 2, p.122
Complete Sec Review Ques. p. 122
Study for Quarter 1 EXAM
SCHOOL CLOSED
Friday Nov 12 – Teacher WORK DAY
Materials: Textbook
A / B 24 Mon - Tues Nov 15 & 16
CHAPTER 5, SECTION 1 – History of the
Periodic Table
1.Explain the roles of Mendeleev and
Return / Critique 1st Quarter EXAM
Discuss Objectives 1- 4
Define Section 1 Terms p. 165
Discuss Section 1, Chp 5
HW
Complete all class assignments for
Chapter 4
Read / Study Sections 1 & 2, Chapter 5
Moseley in developing the PERIODIC TABLE
2.Describe the modern PERIODIC TABLE
3.Explain how the modern PERIODIC TABLE
and the periodic law can predict physical
and chemical properties
4.Describe how elements of a group are
interrelated in terms of atomic number
Answer Section Review Questions, p.137
A/B 25 Wed-Thurs Nov 17-18
Discuss Objectives 1-4
Define Section 2 Terms, p. 165
Discuss Section 2, Chp 5
CHAPTER 5, SECTION 2 – Electron
Configurations & the Periodic Table
1. Describe the relationship between
electrons in sublevels and the length of each
period in the table.
2. Locate, name and explain the names of
the four blocks of the periodic table.
3. Explain the relationship between group
configurations and group numbers.
4. Describe the locations in the periodic
table and the general properties of the alkali
metals, the alkaline-earth metals, the
halogens, and the noble gases.
A/B 26 Fri & Mon Nov 19 & 22
CHAPTER 5, SECTION 3 – PERIODIC TRENDS
1.Define atomic radii, ionic radii, ionization
energy, electron affinity, and
electronegativity
2.Compare the periodic trends of atomic
radii, ionization energy, and
electronegativity and state reasons for the
variations.
3.Define valence electrons and state how
many are present in atoms of each maingroup element.
4.Compare the atomic radii, ionization
energies, and electronegativities of the dblock elements with those of the maingroup elements
A/B 27 Tues-Wed Nov 23-24
TEST – CHAPTER 5
Complete Class assignments
Read / Study Section 2, Chp 5
Begin reading / studying Section 2, Chp 5
Complete Practice Problems 1 & 2, p. 143
Complete Practice Problems 1 & 2, p. 146
Complete Practice Problems 1 & 2, p. 148
Complete Practice Problem1, p. 149
Answer Section Review Questions, p. 149
1.Discuss Objectives
2. Define Section 3 Terms, p. 165
3. Complete Practice Problems 1-3, p. 152
4.Complete Practice Problem 1, p. 156
5. Complete Section Review Ques., p. 164
Materials: Textbook
HW
Complete Class Assignments
Read / Study Section 3, Chp 5
Materials: Textbook
HW
Complete all class assignments
1. Define Section 3 Terms, p. 165
2. Complete Practice Pblms 1-3, p. 152
3.Complete Practice Pblm 1, p. 156
4. Complete Sec Review Ques., p. 164
5. Answer EOC # 39 – 49, p. 168
6. Study “Standardized Test Prep”,
p.171
7. Study online CHAPTER 5 STUDY
GUIDE
Materials:
Complete Chapter 5 TEST
Chapter 5 TEST
HW:
Read/Study Section 1, Chapter 6
A/B 28 Mon-Tues Nov 29-30
1.Crituque Chapter 5 TEST
2.Prepare for UNIT 3 TEST
CHAPTER 6, SECTION 1 – CHEMICAL
BONDING
1.Define: Chemical Bond
Ionic Bond
PROCEDURES
1. Return Chapter 5 TEST, Q/A
2. Q/A on all Chapters 3,4 and 5
assignments
3. Preview UNIT 3 TEST
4. Introduce Section 1, Chapter 6
MATERIALS
Textbook
Chapter 5 Test
HW
Prepare for UNIT 3 TEST
Study online UNIT 3 STUDY GUIDE
Covalent Bond
2.Explain how atomic stability changes with
chemical bonding
3.Explain the relationship between
electronegativity and bonding type
A/B 29 Wed-Thurs Dec 1-2
PROCEDURES
UNIT 3 TEST
Take UNIT 3 TEST
Read / Study Sections 1 & 2, Chp 6
A/B 30 Fri & Mon Dec 3 & 6
Start UNIT 4 – BONDING & NAMING
Chapter 6.1, 6.2 PRACTICE WRITING LEWIS DOT STRUCTURES
PRACTICE DETERMING MOLECULAR SHAPES
A/B 31 Wed Thurs Dec 9-10
SECTION 2, CHAPTER 6 – IONIC BONDING
MATERIALS
UNIT 3 TEST
Textbook
HW
Read / Study Sections 1 & 2, Chp 6
Complete all Practice Problems and
Section Review Questions p. 177
Complete Practice Problems p. 184,
186 188
Complete Section Review Questions p.
189