Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu The Periodic Table Table of Contents Section 1 Arranging the Elements Section 2 Grouping the Elements Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 1 Arranging the Elements Objectives Describe how Mendeleev arranged elements in the first periodic table. Explain how elements are arranged in the modern periodic table. Compare metals, nonmetals, and metalloids based on their properties and on their location in the periodic table. Describe the difference between a period and a group. Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 1 Arranging the Elements Discovering a Pattern In 1869, Russian chemist Dmitri Mendeleev arranged the elements in order of increasing atomic mass. Periodic Properties of the Elements When the elements are arranged in order of increasing atomic mass, those that had similar properties occurred in a repeating pattern. These repeating patterns are periodic, meaning that they happen at regular intervals. Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 1 Arranging the Elements Discovering a Pattern, continued Predicting Properties of Missing Elements Mendeleev’s arrangement had gaps in its pattern. Mendeleev predicted that elements yet to be found would fill these gaps. He also predicted the properties of the missing elements. By 1886, all of the gaps had been filled and Mendeleev’s predictions were right. Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 1 Arranging the Elements Changing the Arrangement A few elements’ properties did not fit in the pattern of Mendeleev’s table. In 1914, British scientist Henry Moseley found the number of protons—the atomic number—in an atom. When the elements were arranged by atomic number, they fit the pattern in Mendeleev’s table. Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 1 Arranging the Elements Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 1 Arranging the Elements The Periodic Table and Classes of Elements Elements are classified as metals, nonmetals, and metalloids, according to their properties. The number of electrons in the outer energy level of an atom is one characteristic that helps determine which category an element belongs in. The zigzag line on the periodic table can help you recognize which elements belong in which category. Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 1 Arranging the Elements The Periodic Table and Classes of Elements, continued Metals are found to the left of the zigzag line. Atoms of most metals have few electrons in their outer energy level. Most metals are shiny, ductile, malleable, and are good conductors of electric current and thermal energy. Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 1 Arranging the Elements The Periodic Table and Classes of Elements, continued Nonmetals are found to the right of the zigzag line. Atoms of most nonmetals have an almost complete set of electrons in their outer energy level. Nonmetals are not shiny, ductile, or malleable, and are poor conductors of electric current and thermal energy. Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 1 Arranging the Elements The Periodic Table and Classes of Elements, continued Metalloids are the elements that border the zigzag line. Atoms of metalloids have about half of a complete set of electrons in their outer energy level. Metalloids have some properties of metals and some properties of nonmetals. Metalloids are also called semiconductors. Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 1 Arranging the Elements Decoding the Periodic Table Each Element is Identified by a Chemical Symbol Each square on the periodic table includes an element’s name, chemical symbol, atomic number, and atomic mass. For most elements, the chemical symbol has one or two letters. The newest elements have temporary three-letter symbols. Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 1 Arranging the Elements Decoding the Periodic Table, continued Rows Are Called Periods Each horizontal row of elements is called a period. The chemical and physical properties of elements in a row follow a repeating pattern as you move across the period. Columns Are Called Groups Each vertical column of elements is called a group. Elements in the same group often have similar chemical and physical properties. Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Periodic Table Overview Chapter 5 Section 1 Arranging the Elements

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 2 Grouping the Elements Bellringer Think about the following: How do you know that a bird is a bird? A kangaroo is a kangaroo? A shark is a shark? What characteristics of each animal help you to tell them apart? How does this apply to elements? Record your answers in your science journal. Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 2 Grouping the Elements Objectives Explain why elements in a group often have similar properties. Describe the properties of the elements in the groups of the periodic table. Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 2 Grouping the Elements Group 1: Alkali Metals Alkali metals are elements in Group 1 of the periodic table. Alkali metal properties: group contains metals 1 electron in the outer level very reactive softness, color of silver, shininess, low density Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 2 Grouping the Elements Group 2: Alkaline-Earth Metals Alkaline-earth metals are elements in Group 2. Alkaline-earth metal properties: group contains metals 2 electrons in the outer level very reactive, but less reactive than alkali metals color of silver, higher densities than alkali metals Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 2 Grouping the Elements Group 3–12: Transition Metals Transition metals are in Groups 3–12. Some of the transition metals are shown below. Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 2 Grouping the Elements Group 3–12: Transition Metals, continued Properties of Transition Metals vary widely but include: groups contains metals 1 or 2 electrons in the outer level less reactive than alkaline-earth metals shininess, good conductors of electric current and thermal energy Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 2 Grouping the Elements Group 3–12: Transition Metals, continued Lanthanides and Actinides Some transition metals from Periods 6 and 7 appear in two rows at the bottom of the periodic table. Elements in the first row are called lanthanides and elements in the second row are called actinides. Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 2 Grouping the Elements Group 13: Boron Group Aluminum is the most common element from Group 13. Group 13 properties: group contains one metalloid and four metals 3 electrons in the outer level reactive solids at room temperature Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 2 Grouping the Elements Group 14: Carbon Group Group 14 properties: group contains one nonmetal, two metalloids, and two metals 4 electrons in the outer level reactivity varies among the elements solids at room temperature Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 2 Grouping the Elements Group 15: Nitrogen Group Group 15 properties: group contains two nonmetals, two metalloids, and one metal 5 electrons in the outer level reactivity varies among the elements solids at room temperature (except for nitrogen, which is a gas) Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 2 Grouping the Elements Group 16: Oxygen Group Group 16 properties: group contains three nonmetals, one metalloids, and one metal 6 electrons in the outer level reactive solids at room temperature (except for oxygen, which is a gas) Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 2 Grouping the Elements Group 17: Halogens Halogens are the elements in Group 17. Group 17 properties: group contains nonmetals 7 electrons in the outer level very reactive poor conductors of electric current, never in uncombined form in nature Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 2 Grouping the Elements Group 18: Noble Gases Noble gases are the elements in Group 18. Group 18 properties: group contains nonmetals 8 electrons in the outer level (except helium, which has 2) unreactive colorless, odorless gases at room temperature Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 2 Grouping the Elements Hydrogen The properties of hydrogen do not match the properties of any single group, so hydrogen is set apart. a nonmetal 1 electron in the outer level reactive colorless, odorless gas at room temperature, low density Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Use the terms below to complete the concept map on the next slide. Concept Mapping elements periods metals electrons nonmetals periodic table groups (families) Chapter 5 The Periodic Table

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu The Periodic Table Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu The Periodic Table Chapter 5

End of Chapter 5 Show ResourcesChapter menu

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu The graph below shows the densities in kilograms per cubic meter (kg/m3) of the elements in Period 2 of the periodic table. The densities of the elements of Period 3 follow this trend. Chapter 5 Standardized Test Preparation

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 1. Which of the following elements is most likely to have a lower density than calcium (Ca) has? A.gallium (Ga) B.germanium (Ge) C.potassium (K) D.selenium (Se) Chapter 5 Standardized Test Preparation

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu 1. Which of the following elements is most likely to have a lower density than calcium (Ca) has? A.gallium (Ga) B.germanium (Ge) C.potassium (K) D.selenium (Se) Chapter 5 Standardized Test Preparation

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 5 Standardized Test Preparation 2. In Mendeleev’s periodic table, the element iodine (I) came before tellurium (Te). He arranged the elements by atomic weight. Later, Henry Moseley revised the table to place iodine after tellurium. Moseley’s version of the periodic table is still in use today. Explain the basis for Moseley’s revision to the periodic table.

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 5 Standardized Test Preparation 2. Explain the basis for Moseley’s revision to the periodic table. Full-credit answers should include the following points: Moseley’s version of the periodic table is based on atomic number. Some elements have higher atomic weights than neighboring elements that have higher atomic numbers. Therefore, some elements were rearranged when atomic numbers were discovered and used to organize the periodic table.

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 5 Standardized Test Preparation The diagram below is an enlargement of a section of the periodic table.

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 5 Standardized Test Preparation 3. What is the biggest difference between cobalt (Co) and nickel (Ni) as shown in the periodic table entries? F.Nickel has more protons. G.Cobalt has more electrons. H.Cobalt has a lower number of neutrons. I.Nickel has a higher value for atomic mass.

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 5 Standardized Test Preparation 3. What is the biggest difference between cobalt (Co) and nickel (Ni) as shown in the periodic table entries? F.Nickel has more protons. G.Cobalt has more electrons. H.Cobalt has a lower number of neutrons. I.Nickel has a higher value for atomic mass.

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 5 Standardized Test Preparation The table below shows some properties of copper and tungsten. In the table, the density of the elements are given in grams per cubic centimeter (g/cm3). When making coins, a large machine squashes the metal into the coin shape.

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 5 Standardized Test Preparation 4.Which property of copper makes copper easier to form into coins than tungsten? A.lower density B.lower hardness C.higher reflectivity D.higher heat conductivity

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Chapter 5 Standardized Test Preparation 4.Which property of copper makes copper easier to form into coins than tungsten? A.lower density B.lower hardness C.higher reflectivity D.higher heat conductivity

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 2 Grouping the Elements Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 2 Grouping the Elements Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 2 Grouping the Elements Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 2 Grouping the Elements Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 2 Grouping the Elements Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 2 Grouping the Elements Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 2 Grouping the Elements Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 2 Grouping the Elements Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 2 Grouping the Elements Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 2 Grouping the Elements Chapter 5

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu Section 2 Grouping the Elements Chapter 5