Chapter 6 THE PERIODIC TABLE 1 Introduction Activity

Chapter 6 THE PERIODIC TABLE 1

Introduction Activity 2

Label the GROUPS & PERIODS (on BOTH sides) 1 1 18 2 13 14 15 16 17 2 3 3 4 5 6 7 8 9 10 11 12 4 5 6 7 Make Yourself a KEY! 3

Pick a side to start on. 4

Metals 5

Transition Metals 6

Metalloids 7

Hydrogen (the ODD 1) Non Metals Make Yourself a KEY! 8

Flip the Paper Over 9

Representative Elements 1 1 18 2 13 14 15 16 17 2 3 3 4 5 6 7 8 9 10 11 12 4 5 6 7 Make Yourself a KEY! 10

Hydrogen 11

Alkali Metals 12

Alkaline-Earth Metals 13

Boron Group 14

Carbon Group 15

Nitrogen Group 16

Oxygen Group 17

Halogens 18

Noble Gases 19

Lanthanides 20

Actinides 21

All Together! Make Yourself a KEY! 22

Chapter 6 Vocabulary 1. Alkali metals 10. Ionization energy 2. Alkaline earth metals 11. Metalloids 3. Anion 12. Metals 4. Atomic radius 13. Noble gases 5. Cation 14. Nonmetals 6. Electronegativity 15. Periodic law 7. Halogens 16. Representative elements 8. Inner transition metal 17. Transition metal 9. Ion Define all of them for 3 EC points! 23

And Again… 24

Review from yesterday! Complete the chart: Element Symbol Group Number Period Number Group Name Metal, Nonmetal, or Metalloid? Nitrogen N 15 2 Nitrogen Group Nonmetal Platinum Pt 10 6 Transition Metals Metal Tin Sn 14 5 Carbon Group Metal Antimony Sb 15 5 Nitrogen Group Metalloid Potassium K 1 4 Alkali Metals Metal Br 17 4 Halogens Nonmetal Bromine 25

Section 6. 1 Notes Organizing the Elements READ PAGES 155 -160 26

How did chemists begin to organize the known elements? Chemists used the properties of elements to sort them into GROUPS 27 .

1700 13 elements were identified Included: - Copper - Silver - Gold - Carbon 28

1765 -1775 5 new elements were identified Included: - Hydrogen - Nitrogen - Oxygen 29

1829 J. W. Döbereiner (Johann Wolfgang) ◦ German chemist ◦ Grouped some elements into triads ◦ Set of three elements with similar properties 30

Cl, Br, I have very similar chemical properties. Can you find them on the Periodic Table? 31

1869 Dmitri Mendeleev ◦Russian chemist ◦Published the first table of elements ◦ Arranged the elements in order of increasing atomic mass 32

Mendeleev was amazing because he • left spaces in his table for elements not yet discovered • predicted properties for these undiscovered elements correctly 33

Mendeleev’s st 1 Periodic Table In this early version of Mendeleev’s periodic table, the rows contain elements with similar properties. 34

What was wrong with Mendeleev’s Periodic Table? Let’s look at your Periodic Table What did Mendeleev’s Periodic Table go by? ◦ Atomic Mass Any discrepancies? What does yours go by? ◦ Atomic Number 35

1913 Henry Moseley ◦ British physicist ◦ Determined the atomic number for elements ◦ Arranged the elements in order of increasing atomic number ◦ Today’s Periodic Table 36

Today’s Periodic Table 37

Periodic Law when elements are arranged by increasing atomic number, properties of the elements tend to repeat 38

Metals • to the left of the stair-step line • most of the elements (80%) • Properties ◦ Good conductors of heat and electricity ◦ Shiny (luster) ◦ Solid at room temperature ◦ Except liquid mercury ◦ Ductile ◦ Drawn into wires like copper wire ◦ Malleable ◦ Hammer into thin sheets like aluminum foil 39

Metals 40

Of all the elements that make up the world in which we live – solids, liquids, gases – most are metals. • There are metals such as aluminum, zinc, gold, copper, tin, and nickel – and ones you might not think of as metals, such as calcium, which is present in bones and teeth. Did you know that the average human body contains more than 2 lbs of calcium? Ni Ca Zn Sn Al. Au Cu 41

Some metals are dangerous. • Potassium reacts violently with water creating hydrogen gas. Cesium and rubidium will explode if they touch water. K Cs https: //www. youtube. com/watch? v=uixx. Jt. JPVXk Rb 42

Mercury is poisonous. • In fact, the phrase “mad as a hatter” arose because in past centuries, fumes from the mercury used in the hat making process affected the mental health of workers in that industry! 43

• The high density of • Platinum, Pt, is one of osmium, Os, – a metal the rarest and most in the same period as valuable of all metals. It platinum – means that a is used to make jewelry brick of the metal can and used extensively in weigh as much as a industry. small car. Osmium is used in fountain pen nibs and surgical needles. 44

Can you find element names hidden in these sentences? 1. 2. 3. 4. 5. Nick, elbows off the table please! Grandpa is looking older. Your feet are a little stinky. Do you care about the environment? I placed a simple ad in the paper. 45

Nonmetals to the right of the stair-step line most are gases, few solids ◦ except liquid bromine Properties: ◦ poor conductors of heat and electricity ◦ solids tend to be brittle 46

Nonmetals Hydrogen (the ODD 1) 47

Diatomic Elements Br. INCl HOF LABEL THEM ON YOUR P. T. 48

Metalloids Touch the stair-step line ◦ Except aluminum and polonium Have properties of both metals and nonmetals Si 49

Metalloids 50

Metals / Metalloids / Nonmetals Just like Intro Activity 51

Metals, Nonmetals, and Metalloids Inferring: What is the purpose for the black stair-step line? 52

Quick Quiz SECTION 6. 1 53

1. The modern periodic table has elements arranged in order of a. colors. b. melting and boiling points. c. increasing atomic mass. d. increasing atomic number. 54

2. Mendeleev arranged the elements in his periodic table in order of increasing a. atomic mass. b. number of protons. c. number of electrons. d. atomic number. 55

3. Which one of the following is NOT a general property of metals? a. ductility b. malleability c. having a high luster d. poor conductor of heat and electricity 56

What’s Next? Book Work: ◦Page 160 #’s 1 -7 57

Page 160 #1 -7 1. 2. 3. 4. 5. How did chemists begin the process of organizing elements? What property did Mendeleev use to organize his periodic table? How are elements arranged in the modern periodic table? Name three broad classes of elements. Which of the sets of elements have similar physical and chemical properties? a. b. c. 6. Identify each element as a metal, metalloid, or non-metal. a. b. c. d. 7. Oxygen, nitrogen, carbon, boron Strontium, magnesium, calcium, beryllium Nitrogen, neon, nickel, niobium Gold Silicon Sulfur Barium Name two elements that have properties similar to those of the element sodium. 58

1. How did chemists begin the process of organizing elements? Chemists used the properties of elements to sort them into groups, or triads.

2. What property did Mendeleev use to organize his periodic table? Increasing atomic mass

3. How are elements arranged in the modern periodic table? Increasing atomic number

4. Name three broad classes of elements. Metals, Non-Metals, and Metalloids

5. Which of the sets of elements have similar physical and chemical properties? (B) strontium, magnesium, calcium, beryllium

6. Identify each element as a metal, metalloid, or non-metal. A) Metal (Au) B) Metalloid (Si) C) Non Metal (S) D) Metal (Ba)

7. Name two elements that have properties similar to those of the element sodium. Li, K, Rb, Cs, Fr

Section 6. 2 Notes Classifying the Elements READ PAGES 161 -167 66

Representative Elements Groups 1 A through 8 A ◦ Groups 1, 2, 13 -18 67

Representative Elements 68

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Transition Elements Transition metals ◦ Group B ◦ Groups 3 -12 Inner transition metals ◦ Last 2 rows on the periodic table 70

Transition Elements Inner Transition Elements 71

Similar to your colored Periodic Table 72

Periodic Table Key The periodic table displays the symbols and names of the elements, along with information about the structure of their atoms. 73

Quick Quiz SECTION 6. 2 74

1. Which one of the following is incorrectly labeled? a. Ne, noble gas b. Cu, transition metal c. Ga, transition metal d. Cl, halogen 75

What’s Next? Book Work: ◦Page 167 #’s 10, 12, 14 76

10. What information can be included in a periodic table? Symbols and names. Structure. Properties.

12. Why do the elements potassium and sodium have similar chemical properties? K and Na are in the same group. (Alkali Metals)

14. Which of the following elements are transition metals? Cu, Sr, Cd, Au, Al, Ge, Co

Section 6. 3 Notes Periodic Trends READ PAGES 170 -178 80

What does the word periodic mean to you? Periodic ◦ Happens in intervals What are some examples of things that happen periodically? ◦ Birthdays, holidays, periodicals 81

Why is the periodic table called “The Periodic Table”? the properties of elements repeat 82

Trend ◦A predictable change Periodic Trend ◦ Properties of the elements repeat and form patterns ◦ Allows us to make predictions about the chemical behavior of elements ◦ How elements will react with other elements ◦ Many trends exist in the periodic table 83

Atomic Radius Half the distance between two nuclei of the same atom Describes the size of the atom 84

Atomic Radius Trend DOWN A GROUP Increases Why? ◦ Number of energy levels increases ◦ Period 1 = 1 e. l. , ◦ Period 2 = 2 e. l. , ◦ Etc… H Li Na K Rb 85 85

Atomic Radius Trend Na Mg Al Si P S Cl Ar ACROSS A PERIOD Decreases Why? ◦ Electron / proton attraction increases ◦ Opposite of tug of war! 86

Trends in Atomic Size Predicting: If a halogen and an alkali metal are in the same period, which one will have the larger radius? alkali metal 87

Shielding Effect “shielding” is the nuclear pull on electrons Valence electrons are “shielded” from the pull / charge of the nucleus by all the electrons in between. 88

Ions An atom with a charge Cation ◦ Positively charged ion ◦ Formed by metals ◦ Lost electrons Anion ◦ Negatively charged ion ◦ Formed by nonmetals ◦ Gained electrons 89

How do ions form? Positive and negative ions form when electrons are transferred between atoms. 90

Positive Ions When a sodium atom loses an electron, it becomes a positively charged ion. Interpreting Diagrams: What happens to the protons and neutrons during these changes? NOTHING!!! 91

Negative Ions When a chlorine atom gains an electron, it becomes a negatively charged ion. Interpreting Diagrams: What happens to the protons and neutrons during these changes? NOTHING!!! 92

Cation Metals Anion Nonmetals 93

This diagram compares the relative sizes of atoms and ions for selected alkali metals and halogens. The data are given in picometers. Comparing and Contrasting: ◦ What happens to the radius when an atom forms a cation? ◦ When an atom forms an anion? 94

Ionic Size of the ion compared to the parent atom Cations ◦ Positive ions are smaller than the atom it comes from ◦ Why? ◦ It lost electrons Anions ◦ Negative ions are larger than the atom it comes from ◦ Why? ◦ It gained electrons 95

Ionic Radius Increases Trends in Ionic Size Ionic Radius Decreases 96

First Ionization Energy energy needed to remove an electron from an atom 97

First Ionization Energy Trend DOWN A GROUP Decreases Why? ◦ Valence electrons are farther away from the nucleus ACROSS A PERIOD Increases Why? ◦ The atom becomes more stable with more valence electrons 98

Multiple Ionization Energies What would the 2 nd Ionization Energy mean? Energy needed to remove the second electron What would the 3 rd Ionization Energy mean? Energy needed to remove third electron Why are elements such as H and He missing some ionization energy values? 99

Trends in Ionization Energy Predicting: Which element would have the larger first ionization energy, an alkali metal in period 2 or an alkali metal in period 4? Period 2 alkali metal 100

Electronegativity The ability of an atom to attract electrons to itself when bonded to another atom 101

Electronegativity Trend DOWN A GROUP ACROSS A PERIOD Decreases Increases Why? ◦ Valence electrons are farther away from the nucleus ◦ Same reason as ionization energy ◦ Atom becomes more stable with more valence electrons ◦ Same reason as ionization energy ◦ Don’t count noble gases 102

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Most Active Elements Most active metal Most active nonmetal ◦ Fr (Francium) ◦ F (Fluorine) Why? ◦ Lowest electronegativity ◦ Highest electronegativity 104

Summary of Trends RECAP 105

Decreases Increases Atomic Size 106

Increases Decreases Ionization energy 107

Increases Decreases Electronegativity 108

Page 178: Draw arrows to show periodic trends below. 109

Quick Quiz SECTION 6. 3 110

1. Which of the following sequences is correct for atomic size? a. Mg > Al > S b. Li > Na > K c. F > N > B d. F > Cl > Br 111

2. Metals tend to a. b. c. d. gain electrons to form cations. gain electrons to form anions. lose electrons to form cations. 112

3. Which of the following is the most electronegative element? a. Cl b. Se c. Na d. I 113

What’s Next? Book Work: ◦Page 178 #’s 16 -23 114

16. How does atomic size change within groups and across periods? In general, atomic size increases from top to bottom within a group and decreases from left to right across a period.

17. When do ions form? Positive and negative ions form when electrons are transferred between atoms.

18. What happens to first ionization energy within groups and across periods? First ionization energy tends to decrease from top to bottom within a group and increase from left to right across a period.

19. Compare the size of ions to the size of atoms from which they form. Cations (+) are always smaller than the atoms from which they form. Anions (-) are always larger than the atoms from which they form.

20. How does electronegativity vary within groups and across periods? In general, electronegativity values decrease from top to bottom within a group. For representative elements, the values tend to increase from left to right across a period.

21. In general, how can the periodic trends displayed by the elements be explained? The trends that exist among these properties can be explained by variations in atomic structure.

22. Arrange the elements in order of decreasing atomic size: Sulfur, Chlorine, Aluminum, Sodium > Aluminum > Sulfur > Chlorine

23. Which element in each pair has the larger first ionization energy? a) Sodium, Potassium b) Magnesium, Phosphorus

You need to know the NAME (Spelling Counts) and SYMBOL of the following elements (not the location) H He Li Be B C N O F Ne Na Mg Al Si P S Cl Ar K Ca Ti Cr Mn Fe Co Ni Rb Cu Zn Ag Ba Pt Au As Br Sn Hg I Pb Fr 123

The Periodic Law A PUZZLE ACTIVITY 124

Introduction The present organization of the elements is a product of the first periodic table published by Dmitri Mendeleev in 1869. The amazing accuracy of his predictions has been very important to chemists in this century. However, the basis of his arrangement was the atomic masses of the elements. This approach proved incorrect as it would have placed some elements in a group with dissimilar properties. Henry Moseley rearranged the table on the basis of the atomic numbers of the elements. In accordance with Moseley’s revision, the periodic law states: the properties of the elements are periodic functions of their atomic numbers. Each of the 100+ known elements has its own set of characteristic properties. These range from solid to gas, lustrous to dull, low to high melting points, various colors, and so on. The elements are arranged within the periodic table into groups (vertical columns) and periods (horizontal rows). This arrangement reflects the periodic or repeating nature of the properties of the elements. 125

Purpose In this activity, you will use your knowledge of periodic properties and a list of clues to correctly arrange the elements from a scrambled periodic table. 126

Procedure / Clues The following sets of elements belong together in groups: ◦ PSIF, JXBE, ZRD, LHT, QKA, WOV, GUN, YMC Letter clues: J has an atomic number three times that of T U has a total of six electrons I 2 A is the simple formula of an oxide P is less dense than S S is an alkali metal E is a noble gas W is a liquid Z has the smallest atomic mass in its group B has ten protons O has an atomic number larger than V D has the largest atomic mass of its group C has five electrons its outer energy level F is a gas X has an atomic number one higher than F L is an alkaline earth element with atomic mass of 40 Y is a metalloid O is a halogen The atomic mass of T is more than that of H Q has an atomic mass 2 times A Atoms of I are larger than those of S M has an atomic number one less than that of A The atomic radius of K is the largest of the group The electrons of atom N are distributed over three energy levels. 127

Place the correct letter below in their appropriate spot according to the Periodic Table! 1 2 13 14 15 16 17 18 Then you know that GUN are in this group U Let’s do one together… J has an atomic number three times that of T U has a total of six electrons 128

Have Fun EXTRA CREDIT – DUE TOMORROW 129

Answers 1 2 13 14 15 16 17 F 18 X P H Z U M A V B S T R N C Q O E I L D G Y K W J 130