Chapter 5 The Periodic Table

Chapter 5 Note Guide

5.1 Organizing the Elements

Links on Periodic Table (5.1)

5.1.1 Describe how Mendeleev arranged the elements in his table

5.1.2 Explain how the predictions Mendeleev made and the discovery of new elements demonstrated the usefulness of his periodic table

• Mendeleev arranged the elements into rows in order of increasing mass so that elements with similar properties were in the same column.
• The close match between Mendeleev’s predictions and the actual properties of new elements showed how useful his periodic table could be.

Day 1

• Chapter 5 Summary: Talking to the Text
• 5.1 PowerPoint (19 slides) & Note Guide
• Element Song
• Names Proposed for New Elements
• 5.1 Reading & Study Workbook

5.2 The Modern Periodic Table

Active Art – Periodic Table (5.2)

Links on Periodic Law (5.2)

5.2.1 Describe the arrangement of elements in the modern periodic table

5.2.2 Explain how the atomic mass of an element is determined and how atomic mass units are defined

5.2.3 Identify general properties of metals, nonmetals, and metalloids

5.2.4 Describe how properties of elements change across a period in the periodic table

• In the modern periodic table, elements are arranged by increasing atomic number (number of protons). Each row on the table is a period. Each column is a group.
• Properties of elements repeat in a predicable way when atomic numbers are used to arrange elements in a group.
• Atomic mass is a value that depends on the distribution of an element’s isotopes in nature and the mass of those isotopes.
• Elements are classified as metals, nonmetals, and metalloids. Metals are elements that are good conductors of electric current and heat. Nonmetals are poor conductors of electric current and heat. Metalloids are elements with properties that fall between those of metals and nonmetals.

Day 2 & 3

• Collect & Correct 5.1 RSW
• 5.2 PowerPoint (39 slides) & Note Guide
• 5.2 Reading & Study Workbook – due Day 4
• Worksheet: Calculating Average Atomic Mass   
• Brightstorm The Periodic Table Periodic Table Overview (4:31)

The periodic table is a chart which arranges all of the known elements according to their atomic numbers. The columns in the periodic table are called families or groups. The rows are called periods. The elements to left of the periodic table are metals while the elements in the top right are non metals. All metals are solid at normal temperatures while non-metals are liquid or gaseous. Metalloids have properties of both metals and non-metals.

5.3 Representative Groups

Articles on Elements (5.3)

5.3.1 Relate the number of valence electrons to groups in the periodic table and to properties of elements in those groups

5.3.2 Predict the reactivity of some elements based on their locations within a group

5.3.3 Identify some properties of common A group elements

• Elements in a group have similar properties because they have the same number of valence electrons.
• The alkali metals in Group 1A are extremely reactive. The reactivity of these metals increases from the top of the group to the bottom.
• Differences in reactivity among the alkaline earth metals in Group 2A are shown by the ways they react with water.
• Group 3A contains the most abundant metal in Earth’s crust – aluminum. The energy needed to recycle aluminum is 5 percent of the energy needed to extract aluminum from bauxite.
• Group 4A contains the nonmetal carbon. Most compounds in your body contain carbon. Carbon compounds control reactions that occur in cells.
• Fertilizers usually contain the Group 5A elements nitrogen and phosphorus.
• Oxygen, in Group 6A, is the most abundant element in Earth’s crust.
• Despite their physical differences, the halogens in group 7A are all highly reactive nonmetals.
• The noble gases, in Group 8A, are colorless, odorless, and extremely unreactive.

Day 4 & 5

• ES PowerPoint: Matter & It’s Changes – The Periodic Table – slides 22-40
• 5.3 PowerPoint & Note Guide (35 slides)

• 5.3 Reading & Study Workbook
• Brightstorm The Periodic Table (25 minutes total)

Brightstorm The Periodic Table s-Block Elements (5:00)

The s-block elements share electron configurations. s-block elements are the elements found in Group 1 and Group 2 on the periodic table. Group 1 are the alkali metals which have one valence electron. They have low ionization energies which makes them very reactive. Group 2 is the alkali earth metals which have two valence electrons, filling their s sublevel. Because they have 2 valence electrons they are less reactive than group 1. Hydrogen is a nonmetal grouped with the alkali metals because it has one electron in its valence shell.

Brightstorm The Periodic Table p-Block Elements (1:13)

The p-block elements are found on the right side of the periodic table. They include the boron, carbon, nitrogen, oxygen and florine families in addition to the noble gases. The noble gases have full p-orbital's and are nonreactive.

Brightstorm The Periodic Table d-Block Elements - f-Block Elements (2:06)

The d-block elements are found in the middle of the period table. The d-block elements are called transition metals and have valence electrons in d orbital's. The f-block elements,found in the two rows at the bottom of the periodic table, are called inner transition metals and have valence electrons in the f-orbital's.

Transition Metals - Inner Transition Metals (4:01)

Transition metals are in the d-block and have valence electrons in the d-orbital's. They can form multiple oxidation states and form different ions. Iron, Cobalt and Nickel are ferromagnetic. Inner transition metals are in the f-block and have valence electrons in the f-orbital's. They consist of the Lanthanides and the Actinides. The Actinides are radioactive and mostly synthetic.

Boron Family - Carbon Family - Nitrogen Family (3:49)

The Nitrogen family, the Carbon family and the Boron family are found in the p-block of the Periodic Table. The Nitrogen family is group 13, while the Carbon family is group 14 and the Boron family is group 15. All of the elements in the Nitrogen, Carbon and Boron families have unique characteristics and are of great chemical importance.

Oxygen Family (2:36)

The Oxygen family, sometimes also known as chalcogens, is group 16 on the periodic table and consisted of oxygen, sulfur, selenium, tellurium, polonium and ununhexium. The elements in this group show patterns in its electron configuration, especially in the outermost shells.

Halogens (2:57)

Halogens are nonmetal elements located on the right side of the periodic table in Group 7. Halogens include the elements of florine, chlorine, bromine, iodine and astatine. Halogens have a negative 1 charge and are considered very reactive.

Noble Gases (2:43)

The noble gases are located in the last column on the right side of the periodic table and are some of the most stable elements in the periodic table. The noble gases include helium, neon, argon, krypton, xenon and radon.

Day 6

• Element Crosswords
• Element Word Search
• Element Code
• Who Am I

Day 7

Investigation 5A Using Clues to Identify Elements

Day 8 – Review

• Chapter 5 Word Wise & Cross a Clue
• Revisit Chapter 5 Summary – Talking to the Text part 2
• Chapter 5 Self-Grading Assessment

Day 9 – Chapter 5 Test

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More Brightstorm:

Electronegativity (4:26)

Electronegativity is a quantitative measure of how tightly an atom holds onto its electrons. Bond polarity results from imbalanced electronegativities of the atoms involved in bonding. Electronegativity is a periodic trend which increases as you go up and to the right along the periodic table.

Ionization Energy - Periodic Trends (2:37)

Ionization energy is the minimum energy required to remove an electron from the ground state of an atom. Ionization energy is a periodic trend which increases going from top to bottom and left to right across the periodic table.

Atomic Radii - Ionic Radii (3:38)

Atomic and ionic radii are distances away from the nucleus or central atom that have different periodic trends. Atomic is the distance away from the nucleus. Atomic radius increases going from top to bottom and decreases going across the periodic table. Ionic radius is the distance away from the central atom. Ionic radius increases going from top to bottom and decreases across the periodic table.

 

Virtual Lab: How is an Element’s Structure Related to its Position of the Periodic Table