# Ch. 14 The Periodic Table p

Save this PDF as:

Size: px
Start display at page:

Download "Ch. 14 The Periodic Table p. 390-406"

## Transcription

1 Name Period PRE-AP 14-1 Development of the Periodic Table Ch. 14 The Periodic Table p Dmitri Mendeleev published the first periodic table in He organized the elements by atomic mass. He even left holes for elements he said were yet to be discovered. One of these holes was below silicon. He named this element Ekasilicon and predicted its properties. Later germanium was discovered and was determined to be Mendeleev s Ekasilicon. Compare the properties that Mendeleev predicted to the actual properties of Germanium with Figure 5-5 on p. 162 of your text. In 1913 H.G.C. Mosley while working in Rutherford s lab, discovered a way to determine the atomic number of each element. He then improved on Mendeleev s periodic table when he reorganized the table by atomic number instead of atomic mass. 1

2 The Periodic Law says that when elements are arranged in increasing atomic number, their chemical and physical properties show a periodic pattern. We have already seen one example of this law in the electron configuration Reading the Periodic Table Groups or families are vertical columns on the periodic table. Periods are horizontal rows on the periodic table. Figure 14-5 on p. 395 shows the long form of the periodic table. The elements of all the "A" groups are called representative elements. (S & P Block) The elements of all the "B" groups are called transition elements. The elements in the bottom two rows (f-block) are the inner transition elements. Figure 14.2 on p identifies some group and section names. 2

3 YOU NEED COLOR PENCILS AND A NEW PERIODIC TABLE FOR THIS SECTION!!!! Group 1A are called the alkali metals. (Note: Hydrogen is its own group.) Group 2A are called the alkaline earth metals. 3

4 Group 3A are called the Boron group. Group 4A are called the Carbon group. Group 5A are called the Nitrogen group. Group 6A are called the Oxygen group. Group 7A are called the halogens. (Halogen means salt forming.) Group 8A are called the Noble Gases. The number of the A group elements is the number of valence electrons in the atom Elements in a group have similar properties because they have the same number and location of valence electrons.. Figure 14.2 on p is a periodic table with phases at room temperature (20 o C) and metallic properties. 4

5 Metals are elements that have high luster (looks shiny), are malleable (can be hammered into sheets), ductile (can be pulled into wire), and are good electrical and heat conductors. Almost all metals are solids at room temperature. Metals are on the left of the zigzag line. Nonmetals are elements that have low luster (looks dull), are NOT malleable or ductile, and poor conductors of heat and electricity. Most nonmetals are gases at room temperature, but several are solids and one is a liquid. Nonmetals are on the right of the zigzag line plus hydrogen. Semimetals (a.k.a. metalloids) are elements that have some characteristics of both metals and nonmetals Semimetals are on the zigzag line except Aluminum and Polonium both of which are metals. 5

6 14-2 Periodic Trends YOU NEED COLOR PENCILS AND A NEW PERIODIC TABLE FOR THIS SECTION!!!! Periodic trends are the properties of the elements that cycle in predictable ways as you move through the periodic table. Atomic radius (a.k.a. atomic size) is the distance from the center of the atom s nucleus to the outermost electron. Atomic radius decreases as you move left to right in any period. Atomic radius increases as you move down in any group. Fig on p The downward trend occurs because as you move down a group you increase the principal quantum number, n. As n increases, so does the size of the orbital s. The horizontal trend occurs because as you move left to right in a period you are increasing the number of protons in the nucleus, which increases the positive charge of the nucleus, which pulls the negatively charged electrons closer to the nucleus, which decreasing the size of the atom. 6

7 Ionic Radii: There are often several different ions each element can make. However, there is typically an ion of a particular charge that is most common. The list of common ion charges is below. Group 1A ions are Group 5A ions are Group 2A ions are Group 6A ions are Group 3A ions are Group 7A ions are Group 4A ions are Group 8A is Please note that each atom gain or loses electrons so that it has the electron configuration of the closest noble gas.. This is because the noble gas configuration is very stable because it has a full s and p outer sublevel also know as a stable octet. The size of these common ions is also periodic. Look at Fig.. Ionic size increases as you move down a group and decreases as you move left to right with a jump up at 5A. The reasons for both the downward and horizontal trends are the same as those for atomic size. However, in ionic size you have a jump because of the increase in the number of energy levels the ion has. How many electrons does C 4+ have? What is its configuration? How many electrons does N 3- have? What is its configuration? Density, Melting point, and boiling point all increase as you go down a group. These do not have significant left to right trends. Metals increase in reactivity as you go down a group. Nonmetals increase in reactivity as you go up a group. Again, these have no significant left to right trends. Ionization Energy: Ionization energy is the energy needed to remove an electron from the atom. Remember the SI unit for energy is the joule (J). The unit for a large number of atoms is the mol, abbreviated mol. So ionization energy is measured in kj/mol. 7

8 Li + energy --> Li + + e - You can think of ionization energy as how strongly the atom holds its outer-most electron. Ionization energy increases as you move left to right in any period. Ionization energy decreases as you move down in any group. See Fig p Please note these trends are opposite of the atomic size trends. The larger the attraction is between the nucleus and the outer-most electron, the smaller the atom will be and the larger the ionization energy will be. The energy needed to remove the first electron is sometimes called the first ionization energy. The energy to remove the second electron is the second ionization energy. Li ---> Li + + e - First ionization energy = 521 kj/mol Li + ---> Li 2+ + e - Second ionization energy = 7,304 kj/mol Li > Li 3+ + e - Third ionization energy = 11, 752 kj/mol Look at Fig on p Notice the large increase in ionization energy for sodium from its first to second. For magnesium the large increase is from second to third. Why do you suppose this is? It is again the idea of a stable octet or a stable noble gas configuration. Electron affinity is the energy change that occurs when an electron is added to an atom. Ne + e - ---> Ne - Electron affinity = 29 kj/mol A positive electron affinity means that amount of energy had to be added to the atom to make it take the electron. A negative electron affinity means that amount of energy was given off by the atom when the electron was added. F + e - --> F - Electron affinity = -328 kj/mol You can think of electron affinity as the amount of attraction an atom has for an extra electron. Remember that a negative electron affinity means the atom has more attraction than a positive one. 8

9 In general, metals have positive (low) electron affinities and nonmetals have negative (high) electron affinities. Again this trend relates to the stable octet rule. Electronegativity is the attraction an atom has for electrons in a bond. Electronegativity increase as you move left to right in any period. Electronegativity decreases as you move down in any group. See Figure 14.2 on p

### 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

### 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

### 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.

### 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

### 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,

### 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 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

### PERIODIC TABLE NOTES (from chapters 5 and 6)

PERIODIC TABLE NOTES (from chapters 5 and 6) I. History of the Periodic Table As the number of elements began to grow, chemists needed a way to all of these elements. [In the 1700 s there were known elements.

### 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

### 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 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 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

### 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

### Periodic Table of the Elements Notes

Periodic Table of the Elements Notes Arrangement of the known elements based on atomic number and chemical and physical properties. Divided into three basic categories: Metals (left side of the table)

### 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.

### Properties of Metals. A chemical property of metal is its reaction with water which results in rust/corrosion.

Properties of Metals Found on the left side of the Periodic Table (except Hydrogen is not) Metals are good conductors of heat and electricity. shiny. ductile (can be stretched into thin wires). malleable

### 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

### 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

### The Periodic Table of The Elements.

The Periodic Table of The Elements http://www.youtube.com/watch?v=fpnwbitsmgu http://www.youtube.com/watch?v=zuddiwtftem Dmitri Mendeleev: Father of the Periodic Table HOW HIS WORKED Put elements in rows

### 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

### 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

### 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

### 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

### The Periodic Table of The Elements

The Periodic Table of The Elements The Periodic Table The periodic table is a chart that organizes all the elements according to different categories Divided into three basic categories: Metals Non-Metals

### HIGH SCHOOL SCIENCE. Physical Science 10: Periodic Table

HIGH SCHOOL SCIENCE Physical Science 10: Periodic Table WILLMAR PUBLIC SCHOOL 2013-2014 EDITION CHAPTER 10 Periodic Table In this chapter you will: 1. Describe how Mendeleev arranged the elements in his

### Mendeleev s s Periodic Table. Dmitri Mendeleev

The Periodic Table History Russian scientist Dmitri Mendeleev taught chemistry in terms of properties. Mid 1800 - molar masses of elements were known. Wrote down the elements in order of increasing mass.

### 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

### An Organized Table Worksheet Due The Periodic Table of Elements. The Periodic Law

Name: Date: Period: An Organized Table Worksheet Due The Periodic Table of Elements In 1871, the first periodic table was developed by Dmitrii Mendeleev. Mendeleev is known as the father of the current

### Trends of the Periodic Table Diary

Trends of the Periodic Table Diary Trends are patterns of behaviors that atoms on the periodic table of elements follow. Trends hold true most of the time, but there are exceptions, or blips, where the

### Chemistry A: Periodic Table Packet Name: Hour: Page 1. Chemistry A Periodic Table

Chemistry A: Periodic Table Packet Name: Hour: Page 1 Chemistry A Periodic Table Chemistry A: Periodic Table Packet Name: Hour: Page 2 Worksheet #1: Periodic Table Inquiry Activity Directions: I know that

### 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

### 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

### 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

### 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

### Chapter 7. Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten

Chemistry, The Central Science, 11th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten Chapter 7 John D. Bookstaver St. Charles Community College Cottleville, MO Development of Table

### 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

### 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

### 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. The periodic table organises the elements in a particular way.

A quick guide... Periodic Table n The periodic table organises the elements in a particular way. n A great deal of information about an element can be gathered from its position in the periodic table.

### 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

### 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

### 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

### 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

### Periodic Table. Science

Periodic Table Science 7 2015 ??? From an elements location in the periodic table, you can predict properties From an elements location in the periodic table, you can predict ??? Most metals are this state

### 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

### 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

### Unit 2 - The Periodic Table

Name Regents Chemistry 2014-15 Unit 2 - The Periodic Table This unit will be both quick and easy, serving as a bridge between two very challenging units. Objectives: At the end of this unit, students will:

### 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

### 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

### Metals and Nonmetals

The Periodic Table and Atomic Properties The periodic table originally came from the observation that when the elements are arranged by atomic mass, properties recur periodically. (Mendeleev) Now we understand

### Unit 3 - The Periodic Table

*STUDENT* Unit 3 - The Periodic Table *STUDENT* VOCABULARY: Ionization energy Electronegativity Atomic Radius Ionic Radius Chemical Reactivity Metallic Character Nonmetallic character Metals Metalloids

### 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

### 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

### Chapter 5. Chapter 5. Objectives. Table of Contents. 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. 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

### 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

### 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?

### Chapter 3 Atoms & the. Chapter 3 Section 2 The Simplest Matter Pages 80-85

Chapter 3 Atoms & the Periodic Table Chapter 3 Section 2 The Simplest Matter Pages 80-85 The Elements There are many different types of atoms. An element is matter made up of only one kind of atom. An

### 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

### 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

### 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

### 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

### NOTES. The Periodic Table

NOTES COMPLETE The Periodic Table Ch. 6 What elements do you already know about that we use everyday AND are, for the most part, known by just about everybody? Silver, Gold, and Copper have been known

### 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

### 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

### 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.

### 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 & ELECTRON CONFIGURATION. Chapters 5 & 6

THE PERIODIC TABLE & ELECTRON CONFIGURATION Chapters 5 & 6 Dimitri Mendeleev Do Not Copy Invented periodic table Organized elements by properties Arranged elements by atomic mass Predicted existence of

### Composition and Structure of the Atom. Protons: Positively charged, high mass particle. Neutrons: Neutral (no) charge, high mass

Composition and Structure of the Atom Atom: basic unit of an element; smallest unit that retains chemical properties of an element Subatomic particles: Small particles that are the building blocks from

### 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

### The Periodic Table of Elements

The Periodic Table of Elements (AKA THE MOST AWESOME THING EVER!) 1 2 The Development of the Periodic Table of Elements In 1869, Dmitri Mendeleev was studying the physical and chemical properties of the

### Matter and the Periodic Table Chemical Families and Periodic Trends

Matter and the Periodic Table Purpose The purpose of this station is to reinforce students understanding of the organization and predictive power of the Periodic Table of the Elements and students ability

### b. How is the modern periodic table arranged? In order of increasing atomic number

Unit 3 Review Chapters 4 (Atomic Structure) & 6 (Periodic Table) Part 1: Answer the following questions. 1. a. Which scientist created the first modern atomic theory? John Dalton b. What was his theory?

### PERIODIC TABLE. reflect

reflect Suppose you wanted to organize your locker at school. How could you separate and arrange everything in an organized way? You could place the books, notebooks, and folders on a shelf that is separate

### 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

### 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

### IONISATION ENERGY CONTENTS

IONISATION ENERGY IONISATION ENERGY CONTENTS What is Ionisation Energy? Definition of t Ionisation Energy What affects Ionisation Energy? General variation across periods Variation down groups Variation

### Section 1: Arranging the Elements Pages 106-112

Study Guide Chapter 5 Periodic Table Section 1: Arranging the Elements Pages 106-112 DISCOVERING A PATTERN 1. How did Mendeleev arrange the elements? a. by increasing density b. by increasing melting point

### 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

### Trends of the Periodic Table Basics

Trends of the Periodic Table Basics Trends are patterns of behaviors that atoms on the periodic table of elements follow. Trends hold true most of the time, but there are exceptions, or blips, where the

### Dalton s s Atomic Theory

Dalton s s Atomic Theory 1. Elements are made of tiny particles called atoms. 2. All atoms of a given element are identical (not exactly; isotopes) 3. The atoms of a given element are different from those

### Atomic Structure & the Periodic Table CHAPTERS 4 & 5

Atomic Structure & the Periodic Table CHAPTERS 4 & 5 Objectives Understandings: Chemical structure determines the properties of matter The identity and properties of individual elements is determined by

### Ch 3 Atomic Structure and the Periodic Table. Figure 3.1 size relationship is not to scale, ratio of average diameters atom/nucleus = 10 5

1 Ch 3 Atomic Structure and the Periodic Table Figure 3.1 size relationship is not to scale, ratio of average diameters atom/nucleus = 10 5 2 Atoms are very small and spherical. Radii Range 0.9 x 10-10

### 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..

### Untitled Document. 1. Which of the following best describes an atom? 4. Which statement best describes the density of an atom s nucleus?

Name: Date: 1. Which of the following best describes an atom? A. protons and electrons grouped together in a random pattern B. protons and electrons grouped together in an alternating pattern C. a core

### 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

### 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

### 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: Class: Date: ID: A

Name: Class: Date: ID: A Chapter 5 Assessment Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Mendeleev arranged the elements in his periodic table in

### 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

### Chemical Building Blocks: Chapter 3: Elements and Periodic Table

Name: Class: Date: Chemical Building Blocks: Chapter 3: Elements and Periodic Table Study Guide Multiple Choice Identify the letter of the choice that best completes the statement or answers the question.

### Pre PeriodicPeriodic Table Chemistry. No organization of elements. Difficult to find information. Chemistry didn t make sense.

Pre PeriodicPeriodic Table Chemistry No organization of elements. Difficult to find information. Chemistry didn t make sense. Why is the Periodic Table important to us? The periodic table is the most useful

### Chapter 4 - Elements and the Periodic Table

Chapter 4 - Elements and the Periodic Table I. Introduction to atoms A. Development of atomic models 1. Atom, smallest particle of an element 2. Parts of atom a. Electrons, negatively charged b. Protons,

### Chapter 17 Assessment Please write you answers on a separate piece of paper.

Chapter 17 Assessment Please write you answers on a separate piece of paper. Multiple Choice Identify the letter of the choice that best completes the statement or answers the question. 1. Mendeleev created

### 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

### 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

### UNIT 6: The Periodic Table. CPChemistry GHS

UNIT 6: The Periodic Table CPChemistry GHS Objectives Explain organiza8on of periodic table in periods and groups. Iden8fy elements as belonging to representa8ve elements, transi8on elements, metals, nonmetals,