1. The Periodic Table
And the Periodic Law

4. Chapter 6: The Periodic Table and Periodic Law
Section 6.1 Development of the Modern Periodic Table
Antoine Lavoisier
( )
Composed a list in 1790
of the 23 elements
known at the time.

5. The advent of electricity (used to break down compounds into their component elements- electrolysis) and the development of the spectrometer, used to identify elements lead to the discovery of many new elements (70 total by 1870)

6. Nuclear Magnetic Resonance
(NMR) spectrometer

7. John Newlands
Noticed that when elements were arranged by increasing atomic mass their properties repeated every eight element.

8. John Newlands
This type of pattern is called periodic because it repeats in a specific manner.
Newlands called this relationship the Law of Octaves.

9. Dmitri Ivanovich Mendeleev (1834-1907)
Organized elements increasing atomic mass
Noticed that there was a repetition or periodic pattern in their properties.

10. Dmitri Mendeleev
Elements with similar properties were arranged in columns- this was the first periodic table

11. Dmitri Mendeleev
Mendelev predicted the existence and properties of undiscovered elements and left spaces where they should go.

14. Henry Moseley
Arranging the elements by mass resulted in several elements being placed in groups of elements with different properties.

15. Henry Moseley ( )
Discovered that atoms of each element contained a unique number of protons in their nuclei, the number of protons being equal to the atom’s atomic number.

17. Henry Moseley
By arranging elements by increasing atomic number, the problems with the order of the elements in the periodic table were solved.

18. The Periodic Law
When elements are arranged by increasing atomic number, there is a periodic repetition of their chemical and physical properties.

19. The Modern Periodic Table
Consists of boxes that contain the elements name, symbol, atomic number and atomic mass.

20. The Modern Periodic Table Groups
The boxes are arranged in order of increasing atomic number in a series of columns called groups or families.

21. The Modern Periodic Table Groups
Each group is numbered 1 through 18.

22. The Modern Periodic Table Groups
Each group is numbered 1 through 8, followed by the letter A or B.

23. Periods
The boxes are arranged in order of increasing atomic number in a series of rows called periods.
Beginning with hydrogen in period 1, there are 7 periods.

24. Main Group Elements
Groups 1,2,and are referred to as the main group (or representative) elements because they possess a wide range of chemical and physical properties.

25. Transition elements
Transition elements
Groups 3-12

26. Classifying the Elements
Metals
All elements to the left side (except H) of the stair-step line from B to At

27. Metals good conductor of heat and electricity shiny luster
solid at room temperature (except Hg)
Malleable and ductile
high boiling and melting points
High densities

28. Metals (continued) large atomic radius low ionization energy
low electronegativity

29. Alkali Metals The group 1 elements (except for H)
Most reactive group of metals !!!

30. Alkaline Earth Metals The group 2 elements
Second most reactive group of metals 

31.  Transition Elements
These are the group B elements (all are metals)

32. Transition Metals
Transition Metals
Also known as the d-block elements

33. Inner transition Metals
Located along the bottom of the periodic table
Known as the lanthanide- actinide series
Lanthanides are also called rare earth elements
Many are radioactive
Also know as the f- block elements

34. Non- Metals Occupy the upper right side of the periodic table
(right of the stair-step line from B to At)

35. Non-Metals (Characteristics)
Generally gasses at room temperature
Poor conductors of heat and electricity
Brittle dull-looking when solids
lower boiling and melting points than metals (except carbon)
usually have lower densities than metals

36. Non-Metals ( Other Characteristics)
high electronegativity
Small atomic radius
higher ionization energy than metals

37. Halogens Group 17 elements
Most highly reactive group of the non-metals
Diatomic (Mr. BrINClHOF)

38. Nobel gases Group 18 elements Extreamly unreactive
also called Inert gases

39. Metalloids Elements border the stair-step line from B to At
Physical and chemical properties of both metals and non-metals

45. Section review 6.1 Laviosier,- Composed a list in 1790
of the 23 known elements.
Newlands: Noticed that when elements were arranged by increasing atomic mass their properties repeated every eight element Law of Octaves.
Mendeleev : Organized elements increasing atomic mass
Elements with similar properties were arranged in columns- this was the first periodic table
predicted the existence and properties of undiscovered elements and left spaces where they should go
Moseley:By arranging elements by increasing atomic number, the problems with the order of the elements in the periodic table were solved.

50. .

51. Classification of the Elements
By noting an atoms position on the periodic table, you can determine an its electron configuration and number of valence electrons

52. Valence Electrons electrons in an atoms highest principle energy level
elements have similar chemical properties because they have the same number of valence electrons

53. Valence Electrons and Period
The energy level of an elements valence electrons indicates the period on the periodic table in which it is found
Ex. Li - found in period 2; valence electrons found in second energy level
Ex. Gallium (Ga) found in period 4; valence electrons found in fourth energy level

54. Valence electrons and group number
A main group (representative) element and the number of valence electrons it contains are related.
Group 1 has one valence electron, Group 2 has 2 valence electrons and so on. ( Exception He is in group 18, but only has 2 valence electrons

55. Lewis electron dot structures illustrate this connection.

56. The s- p- d- and f- block elements
The periodic table is divided into sections, or blocks representing the atoms energy sub levels being filled with valence electrons.

57. s- block elements
Consist of groups 1 and 2, H and He

58. s- block elements Valence electrons occupy only s orbitals
group 1 elements have partially filled s orbitals s1
group 2 elements have partially filled s orbitals s2

59. s- block elements Group 1 elements have partially filled s orbitals s1
Group 2 elements have filled s orbitals s2

60. p- block elements
After the s sublevel is full, the valence electrons next occupy the p sublevel with its three p orbitals.

61. p- block elements
The p-block is comprised of groups 13 through 18, with filled or partially filled p orbitals

62. p- block elements
There are no p block elements in the period 1, the first p-block element B is in period 2

63. p- block elements
Together the s- and p- blocks compromise the main group elements.

64. p- block elements
Group 18 are the Nobel gases that are unreactive with any other elements.

65. p- block elements
Nobel gases have their highest PEL completely full, this is a very stable electron configuration.

66. d- block elements
Largest of the blocks
Contains the transition metals

67. d- block elements
Characterized by a filled outermost s orbital and filled or partially filled d orbitals
d- block spans
10 groups on
the periodic table

68. f- block elements
Contains the inner transition metals (lanthanide-actinide series)

69. f- block elements
Have filled or partially filled outermost s orbital, and filled or partially filled 4f and 5f orbitals

70. F- block
Electrons do not fill their orbitals in a predictable manner.

71. F- block http://freezeray.com/flashFiles/discoveryDates.htm
There are 7 seven f orbitals that hold a maximum of 14 electrons, so the f-block spans 14 columns of the periodic table.

72. Period 1: s-block elements only
Period 1: s-block elements only
Periods 2 and 3: s- and p- block elements
Periods 4 and 5: s-, p-, and d- block elements
Periods 6 and 7: s-, p-, d- and f- block elements

73. Section 6.3 Periodic Trends
As you move across a period or down a group elements tend to change in a predictable way, this is known as a periodic trend.

74. Atomic Radius
Defined as half the distance between adjacent nuclei in a crystal of the element
For diatomic atoms AR is defined as half the distance between nuclei of identical atoms that are chemically bonded together.

75. Trends within periods
In general there is a decrease in atomic radii as you move left-to-right across a period

76. Trends within periods
In general there is a decrease in atomic radii as you move left-to-right across a period

77.
The result is that the increased nuclear charge pulls the outermost electrons closer to the nucleus.

78. Trends within groups
Atomic radii generally increase as you move down a group.
Electrons are added to higher PELs, so the outermost orbitals increase the size of the atom.
The valence electrons are also farther from the nucleus

79. Largest: Na Smallest: S Largest: Xe Smallest: He
No, with only this information, you will be unable to determine the specific groups and periods That the elements are in; so you can’t apply the periodic in atomic size to determine which element has the larger atomic radius.

80. No, with only this information, you will be unable to determine the soecific groups and periods That the elements are in; so you can’t apply the periodic in atomic size to determine which element has the larger atomic radius.

81. Ionic Radius
When atoms lose electrons they form positively charged ions, they always become smaller.  

82. Ionic Radius
This is due to the loss of electrons that are always valence electrons, thus the outer orbital is empty resulting in a smaller radius.

83. Ionic Radius
Atoms can gain or lose one or more electrons to form ions and gain a net charge.  

84. Ionic Radius
Atoms can gain or lose one or more electrons to form ions and gain a net charge. An ion is an atom or bonded group of atoms that has a positive or negative charge. 

85. Ionic Radius
When atoms gain electrons, they have a negative charge resulting in a larger radius.

86. Trends within periods Ionic Radius
As you move left to right across the period the ionic radius decreases, then when you get to group 5A or 6A, the size of the larger negative ions also decreases.

87. Trends within groups
As you move down a group, an ion’s outer electrons are in a higher PEL resulting in a gradual increase in size.

88. Ionic radius
Atoms can gain or lose one or more electrons to form ions and gain a net charge. An ion is an atom or bonded group of atoms that has a positive or negative charge.

89. Ionic radius
When atoms lose electrons they form positively charged ions, they always become smaller. This is due to the loss of electrons that are always valence electrons, Thus the outer orbital is empty resulting in a smaller radius.

90. Ionic radius
 When atoms gain electrons, they have a negative charge resulting in a smaller radius.

91. Ionic radius Trends within periods
As you move left to right across the period the ionic radius decreases, then when you get to group 5A or 6A, the size of the larger negative ions also decreases.

92. Ionic radius Trends within groups
As you move down a group, an ion’s outer electrons are in a higher PEL resulting in a gradual increase in size.

94. Ionization energy
To form a positive ion, an electron must be removed from a neutral atom.
Ionization energy is defined as the energy required to remove an electron (from the gaseous state).
The energy required to remove the first electron is called the first ionization energy (energy required to remove the second electron, is called the second ionization energy)

95. Ionization energy
A high ionization energy value indicates that an atom has a strong hold on electrons.
IE is a measure of how strongly an atom’s nucleus will hold onto valence electrons.
Atoms with large IE are less likely to form positive ions than atoms with low IE.

96. Ionization energy Trends within periods
First ionization energies generally increase as you move l to r across a period.

97. Ionization energy Trends within groups
First ionization energies generally decrease as you move down a group.
With the valence electrons farther away from the nucleus, less energy is required to remove them.

98. Octet Rule
Atoms tend to gain, lose or share electrons in order to acquire a full set of eight valence electron, (noble gas configuration).

99. Octet Rule
This is a very stable electron configuration. Elements to the right of the periodic table tend to gain electrons (form negative ions)
Elements to the left of the periodic table tend to lose electrons (form positive ions to attain this configuration.

100. Electronegativity
The relative ability of an atom to attract elements in a chemical bond.
Expressed in terms of a numerical value of 3.98 or less.
Units called Paulings (see Linus Pauling )

101. Electronegativity
The relative ability of an atom to attract elements in a chemical bond.

102. Electronegativity Noble gases have been left out
F is the most electronegative element (3.98); Cs and Fr are the least electronegative (.79 and .7)
In a chemical bond the atoms with the greater electronegativity more strongly attract the bond’s electrons

103. Electronegativity Trends within groups and periods
Electronegativity generally decreases as you move down a group and increases as you move left to right across a period.

104. Electronegativity Trends within groups and periods
Elements with the higher electronegativity are at the upper right and elements with the lower electronegativity are at the bottom left of the periodic table.

107. AR increase down a group as the electrons are added to higher energy levels and inner core electrons shields the valence electrons from the increased nuclear charge. AR decrease across a period as increased nuclear charge coupled with unchanging shielding by inner core electrons pulls the valence electrons (being added to the same energy level) closer to the nucleus.
Largest: antimony (Sb) Smallest: (nitrogen (N)

108. a. F c. Br
b. Br d. F
Lithium’s second removed electron is an inner core electron, not a valence electron. Carbon’s fourth removed electron is still a valence electron.