# Chapter 5. Chapter 5. Objectives. Table of Contents. Chapter 5. Chapter 5. Mendeleev and Chemical Periodicity

Save this PDF as:

Size: px
Start display at page:

## Transcription

1 The Periodic Law of Contents and Periodic Properties Objectives Explain the roles of Mendeleev and Moseley in the development of the periodic table. Describe the modern periodic table. Explain how the periodic law can be used to predict the physical and chemical properties of elements. Describe how the elements belonging to a group of the periodic table are interrelated in terms of atomic number. Mendeleev and Chemical Periodicity Mendeleev noticed that when the elements were arranged in order of increasing atomic mass, certain similarities in their chemical properties appeared at regular intervals. Repeating patterns are referred to as periodic. Mendeleev created a table in which elements with similar properties were grouped together a periodic table of the elements. Mendeleev and Chemical Periodicity, After Mendeleev placed all the known elements in his periodic table, several empty spaces were left. In 1871 Mendeleev predicted the existence and properties of elements that would fill three of the spaces. By 1886, all three of these elements had been discovered. Moseley and the Periodic Law Periodicity of Atomic Numbers In 1911, the English scientist Henry Moseley discovered that the elements fit into patterns better when they were arranged according to atomic number, rather than atomic weight. The Periodic Law states that the physical and chemical properties of the elements are periodic functions of their atomic numbers.

2 The Modern Periodic The Periodic is an arrangement of the elements in order of their atomic numbers so that elements with similar properties fall in the same column, or group. Objectives Explain the relationship between electrons in sublevels and the length of each period of the periodic table. Locate and name the four blocks of the periodic table. Explain the reasons for these names. Objectives, Discuss the relationship between group configurations and group numbers. Describe the locations in the periodic table and the general properties of the alkali metals, the alkalineearth metals, the halogens, and the noble gases. Periods and Blocks of the Periodic Elements are arranged vertically in the periodic table in groups that share similar chemical properties. Elements are also organized horizontally in rows, or periods. The length of each period is determined by the number of electrons that can occupy the sublevels being filled in that period. The periodic table is divided into four blocks, the s, p, d, and f blocks. The name of each block is determined by the electron sublevel being filled in that block. The elements of Group 1 of the periodic table are known as the alkali metals. lithium, sodium, potassium, rubidium, cesium, and francium In their pure state, all of the alkali metals have a silvery appearance and are soft enough to cut with a knife. The elements of Group 2 of the periodic table are called the alkaline-earth metals. beryllium, magnesium, calcium, strontium, barium, and radium Group 2 metals are less reactive than the alkali metals, but are still too reactive to be found in nature in pure form. Hydrogen has an electron configuration of 1s 1, but despite the ns 1 configuration, it does not share the same properties as the elements of Group 1. Hydrogen is a unique element. Like the Group 2 elements, helium has an ns 2 group configuration. Yet it is part of Group 18. Because its highest occupied energy level is filled by two electrons, helium possesses special chemical stability.

3 Sample Problem A a. Without looking at the periodic table, identify the group, period, and block in which the element that has the electron configuration [Xe]6s 2 is located. Sample Problem A b. Without looking at the periodic table, write the electron configuration for the Group 1 element in the third period. Is this element likely to be more reactive or less reactive than the element described in (a)? Sample Problem B An element has the electron configuration [Kr]4d 5 5s 1. Without looking at the periodic table, identify the period, block, and group in which this element is located. Then, consult the periodic table to identify this element and the others in its group. The p-block elements consist of all the elements of Groups except helium. The p-block elements together with the s-block elements are called the main-group elements. The properties of elements of the p block vary greatly. At its right-hand end, the p block includes all of the nonmetals except hydrogen and helium. All six of the metalloids are also in the p block. At the left-hand side and bottom of the block, there are eight p-block metals. The elements of Group 17 are known as the halogens. fluorine, chlorine, bromine, iodine, and astatine The halogens are the most reactive nonmetals. They react vigorously with most metals to form examples of the type of compound known as salts. The metalloids, or semiconducting elements, are located between nonmetals and metals in the p block. Sample Problem C Without looking at the periodic table, write the outer electron configuration for the Group 14 element in the second period. Then, name the element, and identify it as a metal, nonmetal, or metalloid. The metals of the p block are generally harder and denser than the s-block alkaline-earth metals, but softer and less dense than the d-block metals.

4 In the periodic table, the f-block elements are wedged between Groups 3 and 4 in the sixth and seventh periods. Their position reflects the fact that they involve the filling of the 4f sublevel. The first row of the f block, the lanthanides, are shiny metals similar in reactivity to the Group 2 alkaline metals. The second row of the f block, the actinides, are between actinium and rutherfordium. The actinides are all radioactive. [Xe]4f 14 5d 9 6s 1 [Ne]3s 2 3p 5 [Ne]3s 2 3p 6 [Xe]4f 6 6s 2 Block Group Name M / NM / Md Reactivity Objectives Define atomic and ionic radii, ionization energy, electron affinity, and electronegativity. Compare the periodic trends of atomic radii, ionization energy, and electronegativity, and state the reasons for these variations. Define valence electrons, and state how many are present in atoms of each main-group element. Compare the atomic radii, ionization energies, and electronegativities of the d-block elements with those of the main-group elements. Atomic Radii The boundaries of an atom are fuzzy, and an atom s radius can vary under different conditions. To compare different atomic radii, they must be measured under specified conditions. Atomic radius may be defined as one-half the distance between the nuclei of identical atoms that are bonded together. Atomic Radii, Atoms tend to be smaller the farther to the right they are found across a period. Periodic Trends of Radii The trend to smaller atoms across a period is caused by the increasing positive charge of the nucleus, which attracts electrons toward the nucleus. Atoms tend to be larger the farther down in a group they are found. The trend to larger atoms down a group is caused by the increasing size of the electron cloud around an atom as the number electron sublevels increases.

5 Atomic Radii, Sample Problem E Of the elements magnesium, Mg, chlorine, Cl, sodium, Na, and phosphorus, P, which has the largest atomic radius? Explain your answer in terms of trends of the periodic table. Ionization Energy An ion is an atom or group of bonded atoms that has a positive or negative charge. Sodium (Na), for example, easily loses an electron to form Na +. Any process that results in the formation of an ion is referred to as ionization. The energy required to remove one electron from a neutral atom of an element is the ionization energy, IE (or first ionization energy, IE 1 ). Ionization Energy, In general, ionization energies of the main-group elements increase across each period. This increase is caused by increasing nuclear charge. A higher charge more strongly attracts electrons in the same energy level. Among the main-group elements, ionization energies generally decrease down the groups. Ionization Energy, Sample Problem F Consider two main-group elements, A and B. Element A has a first ionization energy of 419 kj/mol. Element B has a first ionization energy of 1000 kj/mol. Decide if each element is more likely to be in the s block or p block. Which element is more likely to form a positive ion? Electrons removed from atoms of each succeeding element in a group are in higher energy levels, farther from the nucleus. The electrons are removed more easily. Electron Affinity The energy change that occurs when an electron is acquired by a neutral atom is called the atom s electron affinity. Electron affinity generally increases across periods. Increasing nuclear charge along the same sublevel attracts electrons more strongly Electron affinity generally decreases down groups. The larger an atom s electron cloud is, the farther away its outer electrons are from its nucleus. Ionic Radii A positive ion is known as a cation. The formation of a cation by the loss of one or more electrons always leads to a decrease in atomic radius. The electron cloud becomes smaller. The remaining electrons are drawn closer to the nucleus by its unbalanced positive charge. A negative ion is known as an anion. The formation of an anion by the addition of one or more electrons always leads to an increase in atomic radius.

6 Ionic Radii, Cationic and anionic radii decrease across a period. Periodic Trends of Radii The electron cloud shrinks due to the increasing nuclear charge acting on the electrons in the same main energy level. The outer electrons in both cations and anions are in higher energy levels as one reads down a group. There is a gradual increase of ionic radii down a group. Valence Electrons Chemical compounds form because electrons are lost, gained, or shared between atoms. The electrons that interact in this manner are those in the highest energy levels. The electrons available to be lost, gained, or shared in the formation of chemical compounds are referred to as valence electrons. Valence electrons are often located in incompletely filled main-energy levels. example: the electron lost from the 3s sublevel of Na to form Na + is a valence electron. Electronegativity Valence electrons hold atoms together in chemical compounds. In many compounds, the negative charge of the valence electrons is concentrated closer to one atom than to another. Electronegativity is a measure of the ability of an atom in a chemical compound to attract electrons from another atom in the compound. Electronegativities tend to increase across periods, and decrease or remain about the same down a group. Electronegativity, Sample Problem G Of the elements gallium, Ga, bromine, Br, and calcium, Ca, which has the highest electronegativity? Explain your answer in terms of periodic trends.

### Chapter 5. Chapter 5. Table of Contents. Objectives. Chapter 5. Chapter 5. Mendeleev and Chemical Periodicity

The Periodic Law of Contents and Periodic Properties Objectives Explain the roles of Mendeleev and Moseley in the development of the periodic table. Describe the modern periodic table. Explain how the

### Chapter 5, Section 5.1 History of the Periodic Table

i) Objectives Chapter 5, Section 5.1 History of the Periodic Table ii) Mendeleev and Chemical Periodicity iii) Moseley and the Periodic Law i) The Modern Periodic Table Objectives i) Explain the roles

### The idea of arranging the elements in the periodic table according to their chemical and physical properties is attributed to. d) Ramsay.

Chemistry I PERIODIC TABLE PRACTICE QUIZ Mr. Scott Select the best answer. 1) The idea of arranging the elements in the periodic table according to their chemical and physical properties is attributed

### The Periodic Table; Chapter 5: Section 1 - History of the Periodic Table Objectives: Explain the roles of Mendeleev and Moseley in the development of

The Periodic Table; Chapter 5: Section 1 - History of the Periodic Table Objectives: Explain the roles of Mendeleev and Moseley in the development of the periodic table. Describe the modern periodic table.

### Unit 2 Periodic Behavior and Ionic Bonding

Unit 2 Periodic Behavior and Ionic Bonding 6.1 Organizing the Elements I. The Periodic Law A. The physical and chemical properties of the elements are periodic functions of their atomic numbers B. Elements

### The Periodic Table. Name: Class: Date: ID: A. Multiple Choice Identify the choice that best completes the statement or answers the question:

Name: Class: Date:, ID: A The Periodic Table Multiple Choice Identify the choice that best completes the statement or answers the question: 1. What are the elements with atomic numbers from 58 to 71 called?

### Unit 3.2: The Periodic Table and Periodic Trends Notes

Unit 3.2: The Periodic Table and Periodic Trends Notes The Organization of the Periodic Table Dmitri Mendeleev was the first to organize the elements by their periodic properties. In 1871 he arranged the

### Periodic Table Instructional Background Patterns in Element Properties (History): Elements vary widely in their properties, but in an orderly way.

Periodic Table Instructional Background Patterns in Element Properties (History): Elements vary widely in their properties, but in an orderly way. In 1869, the Russian chemist Dmitri Mendeleev produced

### Chapter 5: The Periodic Law

Chapter 5: The Periodic Law Section 5.1: The History of the Periodic Table Dmitri Mendeleev (1869) first person to organize the elements in a chart Organized about 70 elements by increasing atomic mass

### Chapter 6 The Periodic Table

Chapter 6 The Periodic Table Organizing the Periodic Table In a grocery store, the products are grouped according to similar characteristics. With a logical classification system, finding and comparing

### Chapter 6: The Periodic Table Study Guide

Chapter 6: The Periodic Table Study Guide I. General organization of table A. Modern periodic table 1. Increasing atomic number B. 3 major blocks 1. Metals a. Mostly solids at room temperature b. Conduct

### Chapter 4. Section 1 How Are Elements Organized? Section 2 Tour of the Periodic Table. Section 3 Trends in the Periodic Table

The Periodic Table Section 1 How Are Elements Organized? Section 2 Tour of the Periodic Table Section 3 Trends in the Periodic Table Section 4 Where Did the Elements Come From? Section 1 How Are Elements

### Chapter Test. Teacher Notes and Answers 5 The Periodic Law TEST A 1. b 2. d 3. b 4. b 5. d 6. a 7. b 8. b 9. b 10. a 11. c 12. a.

Assessment Chapter Test A Teacher Notes and Answers 5 The Periodic Law TEST A 1. b 2. d 3. b 4. b 5. d 6. a 7. b 8. b 9. b 10. a 11. c 12. a 13. c 14. d 15. c 16. b 17. d 18. a 19. d 20. c 21. d 22. a

### SCPS Chemistry Worksheet Periodicity A. Periodic table 1. Which are metals? Circle your answers: C, Na, F, Cs, Ba, Ni

SCPS Chemistry Worksheet Periodicity A. Periodic table 1. Which are metals? Circle your answers: C, Na, F, Cs, Ba, Ni Which metal in the list above has the most metallic character? Explain. Cesium as the

### Periodic Table & Periodic Trends I. Importance of Classification II. History & Development law of octaves III. Periodic Law

Periodic Table & Periodic Trends I. Importance of Classification A. Makes large sums of information manageable. B. In chemistry, it reduces the number of reactions that need to be studied. II. History

### Unit 6 The periodic table

Unit 6 The periodic table How to group elements together? Elements of similar properties would be group together for convenience. The periodic table Chemists group elements with similar chemical properties

### Directions: Multiple Choice For each of the following questions, choose the answer that best answers the question and place it on your answer sheet.

CHEMISTRY TEST: THE PERIODIC TABLE Directions: Multiple Choice For each of the following questions, choose the answer that best answers the question and place it on your answer sheet. 1. Which of the following

### Horizontal Rows are called Periods. Elements in the same period have the same number of energy levels for ground state electron configurations.

The Periodic Table Horizontal Rows are called Periods. Elements in the same period have the same number of energy levels for ground state electron configurations. Vertical Rows are called Families or Groups.

### Chapter 5 TEST: The Periodic Table name

Chapter 5 TEST: The Periodic Table name HPS # date: Multiple Choice Identify the choice that best completes the statement or answers the question. 1. The order of elements in the periodic table is based

### Question Bank Periodic Table and Periodic Properties

Question Bank Periodic Table and Periodic Properties 1. Name the following with reference to the elements of Modern Periodic Table. (1 26) (a) An alkali metal in period 2. Ans. Lithium (b) A halogen in

### Name Class Date ELECTRONS AND THE STRUCTURE OF ATOMS

Name Class Date The Periodic Table ELECTRONS AND THE STRUCTURE OF ATOMS 6.1 Organizing the Elements Essential Understanding Although Dmitri Mendeleev is often credited as the father of the periodic table,

### The Periodic Table of The Elements

The Periodic Table of The Elements Elements are like a collection As more and more elements were discovered it became more important to organize and classify them Between the late 1700 s and mid 1800 s

### Development of the Periodic Table

Father of the Periodic Table Dmitri Mendeleev put the elements in order by atomic mass. He noticed similar properties of atoms at regular intervals. His first periodic table was published in 869. Mendeleev

### Name Date Class THE PERIODIC TABLE. SECTION 6.1 ORGANIZING THE ELEMENTS (pages )

6 THE PERIODIC TABLE SECTION 6.1 ORGANIZING THE ELEMENTS (pages 155 160) This section describes the development of the periodic table and explains the periodic law. It also describes the classification

### Chemistry: The Periodic Table and Periodicity

Chemistry: The Periodic Table and Periodicity Name: Hour: Date: Directions: Answer each of the following questions. You need not use complete sentences. 1. Who first published the classification of the

### Lesson Outline for Teaching

Lesson Outline for Teaching Lesson 1: Using the Periodic Table A. What is the periodic table? 1. The periodic table is a chart of the elements arranged into rows and columns according to their chemical

### Chemistry: The Periodic Table and Periodicity

Chemistry: The Periodic Table and Periodicity Name: per: Date:. 1. By what property did Mendeleev arrange the elements? 2. By what property did Moseley suggest that the periodic table be arranged? 3. What

### The Periodic Table: Chapter Problems Periodic Table Class Work Homework Special Groups Class Work Homework Periodic Families Class Work

The Periodic Table: Chapter Problems Periodic Table 1. As you move from left to right across the periodic table, how does atomic number change? 2. What element is located in period 3, group 13? 3. What

### CHAPTER 6: THE PERIODIC TABLE

CHAPTER 6: THE PERIODIC TABLE Problems to try in the textbook. Answers in Appendix I: 5,9,13,15,17,19,21,25,27,29,31,33,35,41,43,45,47,49,55abcde,57,59,61,63,65,67,69,71,73,75,89,91 6.1 CLASSIFICATION

### The Periodic Table - Grade 10 [CAPS]

OpenStax-CNX module: m38133 1 The Periodic Table - Grade 10 [CAPS] Free High School Science Texts Project This work is produced by OpenStax-CNX and licensed under the Creative Commons Attribution License

### UNIT-3 Classification of elements and periodicity in properties

UNIT-3 Classification of elements and periodicity in properties One mark questions:. For the triad of elements A, B and C if the atomic weights of A and C are 7 and 39. Predict the atomic weight of B..

### Organizing the Elements

The Periodic Table Organizing the Elements A few elements, such as gold and copper, have been known for thousands of years - since ancient times Yet, only about 13 had been identified by the year 1700.

### Key Idea questions > How did Mendeleev arrange the elements in his periodic table? > How are elements arranged in the modern periodic table?

CHAPTER OUTLINE Section 1 Organizing the Elements Key Idea questions > How did Mendeleev arrange the elements in his periodic table? > How are elements arranged in the modern periodic table? Recognizing

### Unit 5 Elements and their Properties

Unit 5 Elements and their Properties 1. In 1871, Russian chemist Mendeleev created the forerunner of the modern periodic table. 2. The elements in Mendeleev's table were arranged in order of increasing

### SAI. Protons Electrons Neutrons Isotope Name. Isotope Symbol 131i S3 1. Atomic Number. Mass Number

ATOMIC STRUCTURE AND THE PERIODIC TABLE CHAPTER 4 WORKSHEET PART A Given the following isotopes, determine the atomic number, the mass number, the number of protons, electrons and neutrons. Isotope Symbol

### Ch. 14 The Periodic Table p. 390-406

Name Period PRE-AP 14-1 Development of the Periodic Table Ch. 14 The Periodic Table p. 390-406 Dmitri Mendeleev published the first periodic table in 1869. He organized the elements by atomic mass. He

### P. Table & E Configuration Practice TEST

P. Table & E Configuration Practice TEST Multiple Choice Identify the choice that best completes the statement or answers the question. 1. A line spectrum is produced when an electron moves from one energy

### Families and Periods of the Periodic Table

Families and Periods of the Periodic Table CK12 Editor Say Thanks to the Authors Click http://www.ck12.org/saythanks (No sign in required) To access a customizable version of this book, as well as other

### Unit 7 Review. Name: Class: Date: Multiple Choice Identify the choice that best completes the statement or answers the question.

Name: Class: Date: ID: A Unit 7 Review Multiple Choice Identify the choice that best completes the statement or answers the question. 1) In which set of elements would all members be expected to have very

### Chapter 5 Periodic Table. Dmitri Mendeleev: Russian Chemist credited with the discovery of the periodic table.

Chapter 5 Periodic Table Dmitri Mendeleev: Russian Chemist credited with the discovery of the periodic table. How did he organize the elements? According to similarities in their chemical and physical

### Look at a periodic table to answer the following questions:

Look at a periodic table to answer the following questions: 1. What is the name of group 1? 2. What is the name of group 2? 3. What is the name of group 17? 4. What is the name of group 18? 5. What is

### 1) is credited with developing the concept of atomic numbers.

Chemistry Chapter 14 Review Name answer key General Concept Questions 1) is credited with developing the concept of atomic numbers. A) Dmitri Mendeleev B) Lothar Meyer C) Henry Moseley D) Ernest Rutherford

### CHM1 Review for Exam Which of the following elements has the highest electronegativity

The following are topics and sample questions for the first exam. Topics 1. Mendeleev and the first periodic Table 2. Information in the Periodic Table a. Groups (families) i. Alkali (group 1) ii. Alkaline

### Chemistry I. (Materials) Unit Five: The Periodic Table. Part 2: Reading the Periodic table. Part 1: Development of the Periodic Table

Chemistry I (Materials) Unit Five: The Periodic Table Part 1: Development of the Periodic Table Part 2: Reading the Periodic table Part 3: Periodic Trends Big Idea (December): How is the periodic table

### Chapter 7 Periodic Properties of the Elements

Chapter 7 Periodic Properties of the Elements 1. Elements in the modern version of the periodic table are arranged in order of increasing. (a). oxidation number (b). atomic mass (c). average atomic mass

### 5.4 Trends in the Periodic Table

5.4 Trends in the Periodic Table Think about all the things that change over time or in a predictable way. For example, the size of the computer has continually decreased over time. You may become more

### Name. Worksheet: Periodic Trends. 11. Which sequence of elements is arranged in order of decreasing atomic radii?

1. Which statement best describes Group 2 elements as they are considered in order from top to bottom of the Periodic Table? (A) The number of principal energy levels increases, and the number of valence

### Periodicity. The Periodic Table. Dmitri Mendeleev. and the Periodic Table. Periods. Metals vs. Non-Metals. Groups

Periodicity and the Periodic Table the result Dmitri Mendeleev arranged elements in order of their atomic numbers, such that elements with similar properties fell into the same column or group. The Periodic

### Periodic Table Questions

Periodic Table Questions 1. The elements characterized as nonmetals are located in the periodic table at the (1) far left; (2) bottom; (3) center; (4) top right. 2. An element that is a liquid at STP is

### THE PERIODIC TABLE AND PERIODIC TRENDS IN ATOM

THE PERIODIC TABLE AND PERIODIC TRENDS IN ATOM The aufbau process is a set of rules that allows us to predict the electronic configuration of an atom if we know how many electrons there are in the atom.

### Periodic Table Study Guide

Chemistry Periodic Table Name: Period: 1 2 3 4 5 6 7 8 Periodic Table Study Guide Directions: Please use this packet as practice and review. DO NOT try to answer these questions during presentations, take

### Patterns of Behavior of Main Group Elements (Groups 1, 2, and 13-18)

Reading Guide - Chapter 8.1 Periodic Properties of the Elements Section 1 - Main Group Elements Patterns of Behavior of Main Group Elements (Groups 1, 2, and 13-18) 1. Elements in the same group have the

### Packet 3b: The Periodic Table

Click: http://www.pbs.org/wgbh/nova/physics/hunting-elements.html Periodic Table: Organizes and classifying the elements Dmitri Mendeleev: Russian chemist who arranged according to their increasing atomic.

### 47374_04_p25-32.qxd 2/9/07 7:50 AM Page 25. 4 Atoms and Elements

47374_04_p25-32.qxd 2/9/07 7:50 AM Page 25 4 Atoms and Elements 4.1 a. Cu b. Si c. K d. N e. Fe f. Ba g. Pb h. Sr 4.2 a. O b. Li c. S d. Al e. H f. Ne g. Sn h. Au 4.3 a. carbon b. chlorine c. iodine d.

### Page WHO CREATED THE PERIODIC TABLE? https://www.youtube.com/watch?v=fpnwbitsmgu DMITRI MENDELEEV

5.1-5.3 Page 125-155 WHO CREATED THE PERIODIC TABLE? https://www.youtube.com/watch?v=fpnwbitsmgu DMITRI MENDELEEV 1834-1907 Russian chemistry professor Wrote name of element & properties on separate cards

### Review Topic 3: Elements, Radioactivity, and the Periodic Table

Name: Score: 19 / 19 points (100%) Review Topic 3: Elements, Radioactivity, and the Periodic Table Multiple Choice Identify the choice that best completes the statement or answers the question. 1. The

### 2. What happens to the number of protons and electrons in atoms across a period on the periodic table?

Name Period Date Honors Chemistry - Periodic Trends Check Your Understanding Answer the following, formulating responses in your own words. (This helps you better understand the concepts) 1. Define shielding

### Periodic Table Trends in Element Properties Ron Robertson

Periodic Table Trends in Element Properties Ron Robertson r2 n:\files\courses\1110-20\2010 possible slides for web\ch9trans2.doc The Periodic Table Quick Historical Review Mendeleev in 1850 put together

### EXPERIMENT 4: Electron Configuration of elements

Material: laboratory display of the elements and a wall periodic table is required. Objective: To learn the use of periodic table for writing electron configuration of elements. INTRODUCTION Basic building

### Review- The Periodic Table

Review- The Periodic Table Name Date Block Matching: Match the description in with the correct term in. Write the letter in the blank provided. Each term matches with only one description, so be sure to

### Periodic Table & Periodic Law

Periodic Table & Periodic Law Organizing the Elements A few elements, such as gold and copper, have been known for thousands of years - since ancient times Yet, only about 13 had been identified by the

### Periodic Table of Elements

Periodic Table of Elements Periodic Table: The periodic table is a tabular arrangement of the chemical elements, organized on the basis of their atomic numbers, electron configurations (electron shell

### Chapter 3, Elements, Atoms, Ions, and the Periodic Table

1. Which two scientists in 1869 arranged the elements in order of increasing atomic masses to form a precursor of the modern periodic table of elements? Ans. Mendeleev and Meyer 2. Who stated that the

### Periodic Table of the Elements

Periodic Table of the Elements Where did it come from? 1869 Demitri Mendeleev Russian chemist who discovered a pattern to the elements Wrote properties on cards Arranged cards according to properties

### 6.5 Periodic Variations in Element Properties

324 Chapter 6 Electronic Structure and Periodic Properties of Elements 6.5 Periodic Variations in Element Properties By the end of this section, you will be able to: Describe and explain the observed trends

### TRENDS IN THE PERIODIC TABLE

Noble gases Period alogens Alkaline earth metals Alkali metals TRENDS IN TE PERIDI TABLE Usual charge +1 + +3-3 - -1 Number of Valence e - s 1 3 4 5 6 7 Electron dot diagram X X X X X X X X X 8 Group 1

### Development of Periodic Table

Chapter 7 Periodic Properties of the Elements Learning Outcomes: Explain the meaning of effective nuclear charge, Z eff, and how Z eff depends on nuclear charge and electron configuration. Predict the

### Chapter 6 : The Periodic Table and Periodic Law. Section 1 Notes

Chapter 6 : The Periodic Table and Periodic Law Section 1 Notes Section 6-1 Development of the Periodic Table In the 1700s, Lavoisier compiled a list of all the known elements of the time. Development

### Coincidence? I Think Not! 0 As you have realized, the Periodic Table provides a great deal more information than just atomic number and atomic mass!

Coincidence? I Think Not! 0 As you have realized, the Periodic Table provides a great deal more information than just atomic number and atomic mass! 0 Each period (row) corresponds to an energy level 0

### IPS Unit 8 Periodic Table Review Worksheet

Name: Period: IPS Unit 8 Periodic Table Review Worksheet Directions: Use the terms below to correctly complete the statements. Write the terms in the blanks to the left. Then find and circle each term

### Worksheet 11 - Periodic Trends

Worksheet 11 - Periodic Trends A number of physical and chemical properties of elements can be predicted from their position in the Periodic Table. Among these properties are Ionization Energy, Electron

### Copyrighted by Gabriel Tang B.Ed., B.Sc.

Chapter 8: The Periodic Table 8.1: Development of the Periodic Table Johann Dobereiner: - first to discover a pattern of a group of elements like Cl, Br, and I (called triads). John Newland: - suggested

### PERIODIC TABLE OF ELEMENTS., a Russian scientist is credited with creating the periodic table.

PERIODIC TABLE OF ELEMENTS, a Russian scientist is credited with creating the periodic table. Periods tell us how many are in the atoms of each element. Groups help us to know how many electrons are in

### Page Which element is a noble gas? (1) krypton (3) antimony (2) chlorine (4) manganese

1. Which characteristics describe most nonmetals in the solid phase? (1) They are malleable and have metallic luster. (2) They are malleable and lack metallic luster. (3) They are brittle and have metallic

### Chapter -9. Classification of Elements The periodic Table

Chapter -9 Classification of Elements The periodic Table SYNOPSIS From the earliest times, scientists have been trying to classify the available elements on the basis of their properties. Dobereiner proposed

### CHAPTER REVIEW. 3. What category do most of the elements of the periodic table fall under?

CHAPTER REVIEW EVIEW ANSWERS 1. alkaline-earth metals 2. halogens 3. metals. electron affinity 5. actinides 6. answers should involve the transmutation of one element to another by a change in the number

### 3. What would you predict for the intensity and binding energy for the 3p orbital for that of sulfur?

PSI AP Chemistry Periodic Trends MC Review Name Periodic Law and the Quantum Model Use the PES spectrum of Phosphorus below to answer questions 1-3. 1. Which peak corresponds to the 1s orbital? (A) 1.06

### Unit 6 Particles with Internal Structure 3-1

Unit 6 Particles with Internal Structure 3-1 The Elements Remember, elements are combined to form molecules the way letters are combined to form words. Presently there are about 115 known elements. Only

### PSI AP Chemistry Unit 2: Free Response CW/HW. The Periodic Law and Ionic Charge Classwork: 1. The PES spectrum for an element can be found below:

PSI AP Chemistry Unit 2: Free Response CW/HW Name The Periodic Law and Ionic Charge Classwork: 1. The PES spectrum for an element can be found below: Intensity 0.63 0.77 3.24 5.44 39.2 48.5 433 Binding

### Class Notes Standards Addressed: 8.3.11

Name: Period #: Class Notes Standards Addressed: 8.3.11 History of the Periodic Table: Demitri Mendeleev = Russian chemist who discovered a pattern to the in 1869. o How did he discovery a pattern to the

### Find a pair of elements in the periodic table with atomic numbers less than 20 that are an exception to the original periodic law.

Example Exercise 6.1 Periodic Law Find the two elements in the fifth row of the periodic table that violate the original periodic law proposed by Mendeleev. Mendeleev proposed that elements be arranged

### THE PERIODIC TABLE O F T H E E L E M E N T S. The Academic Support Center @ Daytona State College (Science 117, Page 1 of 27)

THE PERIODIC TABLE O F T H E E L E M E N T S The Academic Support Center @ Daytona State College (Science 117, Page 1 of 27) THE PERIODIC TABLE In 1872, Dmitri Mendeleev created the periodic table arranged

### Unit 3 Study Guide: Electron Configuration & The Periodic Table

Name: Teacher s Name: Class: Block: Date: Unit 3 Study Guide: Electron Configuration & The Periodic Table 1. For each of the following elements, state whether the element is radioactive, synthetic or both.

### The Periodic Table: Periodic trends

Unit 1 The Periodic Table: Periodic trends There are over one hundred different chemical elements. Some of these elements are familiar to you such as hydrogen, oxygen, nitrogen and carbon. Each one has

### The Periodic Table and Chemical Properties

2.2 The Periodic Table and Chemical Properties The periodic table organizes the elements according to their properties. Elements are listed in rows by increasing order of atomic number. Rows are arranged

### Explain 'Dobereiner's Triads and its drawback.

CLASS: X NCERT (CBSE) Chemistry: For Class 10 Page : 1 Question 1: Explain 'Dobereiner's Triads and its drawback. Dobereiner classified elements into groups of three where the atomic weight of the middle

### Chapter 3 Atoms and Elements

Chapter 3 Atoms and Elements 1 Elements Elements are pure substances that cannot be separated into simpler substances by ordinary laboratory processes the building blocks of matter listed on the inside

### The Periodic Table and Periodic Law

The Periodic Table and Periodic Law Section 6.1 Development of the Modern Periodic Table In your textbook, reads about the history of the periodic table s development. Use each of the terms below just

### Electrons in Atoms & Periodic Table Chapter 13 & 14 Assignment & Problem Set

Electrons in Atoms & Periodic Table Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Electrons in Atoms & Periodic Table 2 Study Guide: Things You

### Name: Period: Date: Unit 3 Practice Review (the questions on the test are NOT the same as the review questions)

Name: Period: Date: Unit 3 Review: things you will need to know 1. Atomic Theories: Know all the scientists in order. What did they discover? What experiment did they use? 2. Development of the periodic

### 6. Each column of the periodic table is

1. Atoms of elements that are in the same group have the same number of 5. Mendeleev left gaps in his periodic table because A. Protons B. Valence Electrons A. the table was too full B. no known elements

### 3 Classification of Elements and Periodicity in Properties

3 Classification of Elements and Periodicity in Properties 1. Which of the following statement is not correct for the element having electronic configuration 1s 2 2s 2 2p 6 3s 2 (a) It is a divalent electropositive

### Test 7: Periodic Table Review Questions

Name: Wednesday, January 16, 2008 Test 7: Periodic Table Review Questions 1. Which halogen is a solid at STP? 1. fluorine 3. bromine 2. chlorine 4. iodine 2. Element M is a metal and its chloride has the

### Chapter 2 Atoms, Ions, and the Periodic Table

Chapter 2 Atoms, Ions, and the Periodic Table 2.1 (a) neutron; (b) law of conservation of mass; (c) proton; (d) main-group element; (e) relative atomic mass; (f) mass number; (g) isotope; (h) cation; (i)

### A. Wanted to organize elements according to their. B. When elements were arranged in order of increasing atomic mass*, similarities in

Chemistry Unit 5- Periodic Table and Periodic Law Name: History of the Periodic Table I. Mendeleev and Chemical Periodicity A. Wanted to organize elements according to their B. When elements were arranged

### Electron Configurations continued:

Electron Configurations continued: Electrons in the outermost shell are called valence electrons. It is the valence electrons determine an atom s chemical properties. Electrons in the inner shells are

### Periodic Table Extra Practice

Periodic Table Extra Practice 1. Which of the following elements in Period 3 has the greatest metallic character? 1) Ar 3) Mg 2) Si 4) S 2. Which sequence of atomic numbers represents elements which have

### Key: Periodic Table Blocks. s block p block d block f block

Name Chemistry / / Periodic Table Today you will learn about the organization of the elements of the periodic table into groups (or families) and periods and the properties of these groups. Groups (or