Chapter 6 The Periodic Table and Periodic Law. National Standards for Chapter 5 – UCP.1 Systems,...

Chapter 6

The Periodic Table and Periodic Law

National Standards for Chapter 5– UCP.1 Systems, order, and organization– UCP.2 Evidence, models, and explanation– UCP.5 Evolution and equilibrium– A.1 Abilities necessary to do scientific inquiry– A.2 Understandings about scientific inquiry– B.1 Structure of atoms– B.2 Structure and properties of matter– B.6 Interactions of energy and matter– E.1 Abilities of technological design– E.2 Understandings about science and technology– G.1 Science as a human endeavor– G.2 Nature of scientific knowledge– G.3 Historical perspectives

Vocabulary/Study Guide

• Define each term using the Glossary• Either write on the handout, or use your own

paper• This is due on Test Day (tentatively, Thursday,

November 21)

Section 1: Development of the Modern Periodic Table

• National Standards:– UCP.1 Systems, order, and organization– UCP.2 Evidence, models, and explanation– UCP.5 Evolution and equilibrium– A.1 Abilities necessary to do scientific inquiry– A.2 Understandings about scientific inquiry– B.1 Structure of atoms– B.2 Structure and properties of matter– E.2 Understandings about science and technology– G.1 Science as a human endeavor– G.2 Nature of scientific knowledge– G.3 Historical perspectives

Objectives – Section 1

• Trace the development of the periodic table.

• Identify key features of the periodic table.REVIEW VOCABULARY:

atomic number: the number of protons in an atom

• The periodic table evolved over time as scientists discovered more useful ways to compare and organize the elements.

New Vocabularyperiodic lawgroupperiodrepresentative elementstransition elementsmetalalkali metalsalkaline earth metals

transition metalinner transition metallanthanide seriesactinide seriesnonmetalshalogennoble gasmetalloid

Lab: How Can You Recognize Trends?

• OBJECTIVE: To use the organization of everyday items to help visualize the periodic trends on the table of elements.

• PRE-LAB/PREDICTIONS:– As you sort items, how does this help you to

predict physical and chemical properties?• DATA:– Create a periodic table of household fasteners in a

4x3 grid

Development of the Periodic Table

• In the 1700s, Lavoisier compiled a list of all the known elements of the time.


• The 1800s brought large amounts of information and scientists needed a way to organize knowledge about elements.

• John Newlands proposed an arrangement where elements were ordered by increasing atomic mass.


• Newlands noticed when the elements were arranged by increasing atomic mass, their properties repeated every eighth element.


• Meyer and Mendeleev both demonstrated a connection between atomic mass and elemental properties.

• Moseley rearranged the table by increasing atomic number, and resulted in a clear periodic pattern.

• Periodic repetition of chemical and physical properties of the elements when they are arranged by increasing atomic number is called periodic law.

The Modern Periodic Table

• The modern periodic table contains boxes which contain the element's name, symbol, atomic number, and atomic mass.


• Columns of elements are called groups.• Rows of elements are called periods.• Elements in groups 1,2, and 13-18 possess a

wide variety of chemical and physical properties and are called the representative elements.

• Elements in groups 3-12 are known as the transition metals.


• Elements are classified as metals, non-metals, and metalloids.

• Metals are elements that are generally shiny when smooth and clean, solid at room temperature, and good conductors of heat and electricity.

• Alkali metals are all the elements in group 1 except hydrogen, and are very reactive.

• Alkaline earth metals are in group 2, and are also highly reactive.


• The transition elements are divided into transition metals and inner transition metals

• The two sets of inner transition metals are called the lanthanide series and actinide series and are located at the bottom of the periodic table.


• Non-metals are elements that are generally gases or brittle, dull-looking solids, and poor conductors of heat and electricity.

• Group 17 is composed of highly reactive elements called halogens.

• Group 18 gases are extremely unreactive and commonly called noble gases.


• Metalloids have physical and chemical properties of both metals and non-metals, such as silicon and germanium.

Transparency 18: The Modern Periodic Table

Lab: Analyze Trends, page 180

Lab: Investigate Descriptive Chemistry, page 196

Homework, Section 1

• SECTION 1 REVIEW, Page 181• Questions #1,2,4-7• Answer with complete sentences• Due tomorrow

Section 2: Classification of Elements

• National Standards:– UCP.1 Systems, order, and organization– UCP.2 Evidence, models, and explanation– UCP.5 Evolution and equilibrium– A.1 Abilities necessary to do scientific inquiry– B.1 Structure of atoms– B.2 Structure and properties of matter


• Explain why elements in the same group have similar properties.

• Identify the four blocks of the periodic table based on their electron configuration.

• Identify the relationships among a hydrogen atom's energy levels, sublevels, and atomic orbitals.

Review Vocabulary:valence electron: electron in an atom's outermost orbitals;

determines the chemical properties of an atom


Elements are organized into different blocks in the periodic table according to their electron configurations.

Organizing the Elements by Electron Configuration

• Recall electrons in the highest principal energy level are called valence electrons.

• All group 1 elements have one valence electron.


• The energy level of an element’s valence electrons indicates the period on the periodic table in which it is found.

• The number of valence electrons for elements in groups 13-18 is ten less than their group number.

The s-, p-, d-, and f-Block Elements

• The shape of the periodic table becomes clear if it is divided into blocks representing the atom’s energy sublevel being filled with valence electrons.


• s-block elements consist of group 1 and 2, and the element helium.

• Group 1 elements have a partially filled s orbital with one electron.

• Group 2 elements have a completely filled s orbital with two electrons.


• After the s-orbital is filled, valence electrons occupy the p-orbital.

• Groups 13-18 contain elements with completely or partially filled p-orbitals.


• The d-block contains the transition metals and is the largest block.

• There are exceptions, but d-block elements usually have filled outermost s-orbital, and filled or partially filled d orbital.

• The five d-orbitals can hold 10 electrons, so the d-block spans ten groups on the periodic table.


• The f-block contains the inner transition metals.

• f-block elements have filled or partially filled outermost s orbitals and filled or partially filled 4f and 5f orbitals.

• The 7 f-orbitals hold 14 electrons, and the inner transition metals span 14 groups.

Transparency 19: The s-,p-,d-, and f-Block Elements

Math Skills Transparency 6: Using the Periodic Table

Homework, Section 2

• PRACTICE PROBLEMS #8-10 on page 186• Write the problem, then the answer• SECTION 2 REVIEW, Page 186• Questions #11-15• Answer with complete sentences• Due tomorrow

Section 3: Electron Configuration• National Standards:

– UCP.1 Systems, order, and organization– UCP.2 Evidence, models, and explanation– UCP.5 Evolution and equilibrium– A.1 Abilities necessary to do scientific inquiry– A.2 Understandings about scientific inquiry– B.1 Structure of atoms– B.2 Structure and properties of matter– B.6 Interactions of energy and matter– E.1 Abilities of technological design– E.2 Understandings about science and technology– G.2 Nature of scientific knowledge– G.3 Historical perspectives


• Compare period and group trends of several properties.

• Relate period and group trends in atomic radii to electron configuration.

Review Vocabulary:principal energy level: the major energy level of an atom

New Vocabulary

ionionization energyoctet ruleelectronegativity

Trends among elements in the periodic table include their size and their ability to lose or attract electrons

Atomic Radius

• Atomic size is a periodic trend influenced by electron configuration.

• For metals, atomic radius is half the distance between adjacent nuclei in a crystal of the element.

Atomic Radius

• For elements that occur as molecules, the atomic radius is half the distance between nuclei of identical atoms.

Atomic Radius

• There is a general decrease in atomic radius from left to right, caused by increasing positive charge in the nucleus.

• Valence electrons are not shielded from the increasing nuclear charge because no additional electrons come between the nucleus and the valence electrons.

Atomic Radius

Atomic Radius

• Atomic radius generally increases as you move down a group.

• The outermost orbital size increases down a group, making the atom larger.

Atomic Radius

• Practice Problems #16-19, page 189

Ionic Radius

• An ion is an atom or bonded group of atoms with a positive or negative charge.

• When atoms lose electrons and form positively charged ions, they always become smaller for two reasons:

1. The loss of a valence electron can leave an empty outer orbital resulting in a small radius.

2. Electrostatic repulsion decreases allowing the electrons to be pulled closer to the radius.

Ionic Radius

• When atoms gain electrons, they can become larger, because the addition of an electron increases electrostatic repulsion.

Ionic Radius

• The ionic radii of positive ions generally decrease from left to right.

• The ionic radii of negative ions generally decrease from left to right, beginning with group 15 or 16.

Transparency 20: Atomic and Ionic Radius

• Both positive and negative ions increase in size moving down a group.

Ionization Energy

• Ionization energy is defined as the energy required to remove an electron from a gaseous atom.

• The energy required to remove the first electron is called the first ionization energy.

Ionization Energy

Ionization Energy

• Removing the second electron requires more energy, and is called the second ionization energy.

• Each successive ionization requires more energy, but it is not a steady increase.

Transparency 21: First Ionization and Successive Ionization Energies

Ionization Energy

• The ionization at which the large increase in energy occurs is related to the number of valence electrons.

• First ionization energy increases from left to right across a period.

• First ionization energy decreases down a group because atomic size increases and less energy is required to remove an electron farther from the nucleus.

Ionization Energy

Lab: Organize Elements, page 193

Ionization Energy

• The octet rule states that atoms tend to gain, lose or share electrons in order to acquire a full set of eight valence electrons.

• The octet rule is useful for predicting what types of ions an element is likely to form.

Ionization Energy

• The electronegativity of an element indicates its relative ability to attract electrons in a chemical bond.

• Electronegativity decreases down a group and increases left to right across a period.

Ionization Energy

Lab: Properties of the Periodic Table

Lab: Periodic Trends in the Periodic Table

Homework, Section 3

• SECTION 3 REVIEW, Page 194 • Questions #20-24• Answer with complete sentences• Due tomorrow

Key Concepts

• The elements were first organized by increasing atomic mass, which led to inconsistencies. Later, they were organized by increasing atomic number.

• The periodic law states that when the elements are arranged by increasing atomic number, there is a periodic repetition of their chemical and physical properties.

• The periodic table organizes the elements into periods (rows) and groups (columns); elements with similar properties are in the same group.

Key Concepts

• Elements are classified as either metals, nonmetals, or metalloids.

Key Concepts

• The periodic table has four blocks (s, p, d, f).

• Elements within a group have similar chemical properties.

• The group number for elements in groups 1 and 2 equals the element’s number of valence electrons.

• The energy level of an atom’s valence electrons equals its period number.

Key Concepts

• Atomic and ionic radii decrease from left to right across a period, and increase as you move down a group.

• Ionization energies generally increase from left to right across a period, and decrease as you move down a group.

• The octet rule states that atoms gain, lose, or share electrons to acquire a full set of eight valence electrons.

• Electronegativity generally increases from left to right across a period, and decreases as you move down a group.

Chapter 6 The Periodic Table and Periodic Law. National Standards for Chapter 5 – UCP.1 Systems,...

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