1. Chapter 6
The Periodic Table

2. Introduction Activity

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

4. Pick a side to start on.

5. Metals

6. Transition Metals

7. Metalloids

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

9. Flip the
Paper Over

10. Representative Elements1 18 2 13 14 15 16 17 3 4 5 6 7 8 9 10 11 12
Make Yourself a KEY!

11. Hydrogen

12. Alkali Metals

13. Alkaline-Earth Metals

14. Boron Group

15. Carbon Group

16. Nitrogen Group

17. Oxygen Group

18. Halogens

19. Noble Gases

20. Lanthanides

21. Actinides

22. All Together!
Make Yourself a KEY!

23. Define all of them for 3 EC points!
Chapter 6 Vocabulary
Alkali metals
Alkaline earth metals
Anion
Atomic radius
Cation
Electronegativity
Halogens
Inner transition metal
Ion
Ionization energy
Metalloids
Metals
Noble gases
Nonmetals
Periodic law
Representative elements
Transition metal
Define all of them for 3 EC points!

24. And Again…

25. 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 Sn 5
Potassium 17 4 Pt 10 6
Transition Metals
Metal
Tin 14 5
Carbon Group
Metal
Antimony Sb
Nitrogen Group
Metalloid K 1 4
Alkali Metals
Metal
Bromine Br
Halogens
Nonmetal

26. Section 6.1 Notes Organizing the Elements
Read pages

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

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

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

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

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

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

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

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

35. 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

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

37. Today’s Periodic Table

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

39. 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

40. Metals

41. Of all the elements that make up the world in which we live – solids, liquids, gases – most are metals. Al Cu Zn
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? Ca Ni Sn Au

42. Some metals are dangerous.
Potassium reacts violently with water creating hydrogen gas. Cesium and rubidium will explode if they touch water. Cs Rb K

43. 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!

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

45. Can you find element names hidden in these sentences?
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.

46. 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

47. Hydrogen
(the ODD 1)
Nonmetals

48. Diatomic Elements
BrINCl HOF
LABEL THEM ON YOUR P.T.

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

50. Metalloids

51. Metals / Metalloids / Nonmetals Just like Intro Activity

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

53. Quick Quiz
Section 6.1

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

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

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

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

58. Page 160 #1-7
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 the three broad classes of elements.
Which of the sets of elements have similar physical and chemical properties?
Oxygen, nitrogen, carbon, boron
Strontium, magnesium, calcium, beryllium
Nitrogen, neon, nickel, niobium
Identify each element as a metal, metalloid, or non-metal.
Gold
Silicon
Sulfur
Barium
Name two elements that have properties similar to those of the element sodium.

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

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

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

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

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

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

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

66. Section 6.2 Notes Classifying the Elements
Read pages

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

68. Representative Elements

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

71. Transition Elements Inner Transition Elements

72. Similar to your colored Periodic Table

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

74. Quick Quiz
Section 6.2

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

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

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

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

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

80. Section 6.3 Notes Periodic Trends
Read pages

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

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

83. 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

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

85. Rb K Atomic Radius Trend Na Down a group Increases Why?Li Na
Down a group
Increases
Why?
Number of energy levels increases
Period 1 = 1 e. l.,
Period 2 = 2 e. l.,
Etc… K Rb 85

86. Na Mg Atomic Radius Trend Al Si P Across a period S Cl Decreases Why?Ar
Across a period
Decreases
Why?
Electron / proton attraction increases
Opposite of tug of war!

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

88. 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.

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

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

91. 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!!!

92. 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!!!

93. Cation
Metals
Anion
Nonmetals

94. Comparing and Contrasting:
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?

95. Ionic Size 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
It gained electrons

96. Trends in Ionic Size
Ionic Radius Increases
Ionic Radius Decreases

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

98. First Ionization Energy Trend
Down a group
Across a period
Decreases
Why?
Valence electrons are farther away from the nucleus
Increases
Why?
The atom becomes more stable with more valence electrons

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

100. 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

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

102. Electronegativity Trend
Down a group
Across a period
Decreases
Why?
Valence electrons are farther away from the nucleus
Same reason as ionization energy
Increases
Why?
Atom becomes more stable with more valence electrons
Same reason as ionization energy
Don’t count noble gases

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

105. Summary of Trends
Recap

106. Atomic Size
Decreases
Increases

107. Ionization energy
Increases
Decreases

108. Electronegativity
Increases
Decreases

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

110. Quick Quiz
Section 6.3

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

112. 2. Metals tend to gain electrons to form cations.
gain electrons to form anions.
lose electrons to form anions.
lose electrons to form cations.

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

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

115. 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.

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

117. 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.

118. 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.

119. 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.

120. 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.

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

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

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

124. The Periodic Law
A Puzzle Activity

125. Introduction
The present organization of the elements is a product of the first periodic table published by Dmitri Mendeleev in 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.

126. 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.

127. Procedure / Clues
The following sets of elements belong together in groups:
PSIF, JXBE, ZRD, LHT, QKA, WOV, GUN, YMC
Letter clues:
The electrons of atom N are distributed over three energy levels.
J has an atomic number three times that of T
U has a total of six electrons
I2A 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

128. Then you know that GUN are in this group
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

129. Have Fun
Extra Credit – Due Tomorrow

130. Answers F 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 1 2 13 1415 16 17 18 F 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