1. Chapter 6 The Periodic Table
Stylish Shoes

2. What is in common with all the pictures below?

3. Which one does not belong?

4. Which one does not belong?

5. Which one does not belong?

6. Which one does not belong?

8. History of the Periodic Table
Mendeleev published a classification scheme of all the currently known elements
Organized elements based on similar characteristics.
Left blank spaces in table for undiscovered elements.

9. Mendeleev’s Periodic Table (1869)
Mendeleev arranged the elements on his table in order of increasing atomic mass.

10. Many scientist suggested other periodic tables.
Albert Tarantola’s
Orbital Table
                                                                           

11. Timothy Stowe – Table for Physicists
                                                     

12. Theodor Benfey
                                                                           

13. Emil Zmaczynski
                                                       

14. Vocational Exile Periodic Table

15. The Periodic Law
In the modern periodic table, elements are arranged in order of increasing atomic number

16. Periodic Law – when elements are arranged in order of increasing atomic number, there is a trend in their physical and chemical properties

17. Metals, Metalloids and Nonmetals
Elements can be grouped into three broad classes based on their general properties
Metals
Nonmetals
Metalloids

18. Metals:
Generally solid at room temp.
Ductile – drawn into wires.
Malleable – hammered into sheets
Shiny surface
Conduct heat and electricity

19. Metals

20. Nonmetals:
Varying properties, but are generally poor conductors of heat and electricity
Brittle

21. Non-metals
Nonconductors

22. Metalloids:
some properties of metals and nonmetals
Intermediate

23. Metalloids or Semimetals
Properties of both

25. Practice Tell me all you can about the following elements:
Titanium (Ti)
Germanium (Ge)
Calcium (Ca)
Fluorine (F)
1- Ti – metal,
2 – Ge – metalloid,
3 – Ca – metal,
4 – F – nonmetal,

26. Section 6.2 - Classifying the Elements
The periodic table displays the symbols and names of the elements, along with information about the structure of their atoms (# of protons, neutrons, and electrons)

27. Black symbol = solid
Green = gas
Blue = liquid

28. Electron Configurations in Groups
Elements can be sorted into 4 different groupings based on their electron configurations:
Noble gases
Representative elements
Transition metals
Inner transition metals *

29. Transition
Representative
Inner Trans.
Noble Gases

30. Electron Configurations in Groups
Noble gases elements in Group 8A
Very stable = do not react
Noble gases have an electron configuration that has the outer s and p sublevels completely full *

31. Ci
Circle the Noble Gases

32. Electron Configurations in Groups
Representative Elements are in Groups 1A through 7A
Display wide range of properties, thus a good “representative”
Include metals, nonmetals, metalloids, solids, gases, or liquids
Their outer s and p electron configurations are NOT filled *

33. Circle the Representative Elements

34. Electron Configurations in Groups
Transition metals are in the “B” columns of the periodic table
Electron configuration has outer s sublevel full
Elements in the “d” sublevel
A “transition” between the metal area and the nonmetal area *

35. Circle the Transition Metals

36. Electron Configurations in Groups
Inner Transition Metals are located below the main body of the table, in two horizontal rows
Electron configuration has the outer s sublevel full
Elements in the f sublevel *

37. Circle the Inner Transition Metals

38. Elements in the 1A-7A groups are called the representative elements
outer s or p filling 1A 8A 2A 3A 4A 5A 6A 7A *

39. The group B are called the transition elements
These are called the inner transition elements, and they belong here *

40. Groups of elements - family names
Group 1A – alkali metals
Forms a “base” (or alkali) when reacting with water
Exception is Hydrogen
Group 2A – alkaline earth metals
Also form bases with water; do not dissolve well, hence “earth metals”
Group 7A – halogens
Means “salt-forming” *

41. Group 1A - alkali metals (but NOT H) Group 2A - alkaline earth metals*

42. Group 8A are the noble gases Group 7A is called the halogens*

43. The Groups of the Periodic Table
Representative Elements
Noble Gases
Transition Metals
Inner Transition Metals
Family names:
Alkali metals
Alkaline earth metals
Halogens

44. Practice Tell me all you can about the following elements:
Titanium (Ti)
Germanium (Ge)
Calcium (Ca)
Fluorine (F)
1- Ti – metal, inner trans.
2 – Ge – metalloid, representative
3 – Ca – metal, representative, alkaline earth metal
4 – F – nonmetal, rep, halogen

46. Section 6.3 – Periodic Trends
Properties of elements are related to their location on the periodic table
We will be studying 3 periodic trends:
Atomic Radius
Ionization Energy
Electronegativity

47. 1. Atomic Radius or Atomic Size
One-half the distance from center to center of two atoms
Atomic Radius

48. Atomic Radius or Atomic Size
What do you notice about the atomic radii of the elements on the periodic table?
Atomic Radius increases towards the bottom left corner of the PT

49. Atomic Radius/Size Practice
Which element has a greater atomic radius?
F or Cs
Ga or K
Kr or Rb
Ba or Si
Fr or W
O or Ag

50. Ions
Normally, atoms are neutral because they have the same number of protons and electrons
When elements combine in compounds, they transfer electrons.
Ions are atoms that have a positive or negative charge.

51. Transfer of an electron forms two ions: a cation and anion

52. Cations Circle the cation
Cation – an ion with a positive charge (lost electrons)
Circle the cation
Na+

53. Anions Circle the anion
Anion – an ion with a negative charge gained electrons)
Circle the anion
Na+

55. Ionic Size
Cations are always smaller than the atoms from which they form
Anions are always larger than the atoms from which they form

56. Before
After

57. Does this make sense?
Where are electrons located in the atom?
Around the nucleus
The more electrons around the nucleus, the larger the atom will be.

58. Practice Which of the following is larger? Na or Na+ Al or Al3+
I or I-
Ca2+ or Ca
S or S2-
O2- or O

59. 2. Ionization Energy
The energy required to remove an electron from an atom

60. Ionization Energy
What trend do you notice about the ionization energy of the elements on the periodic table?
Ionization Energy increases towards the top right corner of the PT

61. Does this make sense?
Which elements are the most stable?
Elements with full orbitals
The more stable the elements is, the harder it will be to remove an electron.

62. Ionization Energy Practice
Which of these elements has a greater ionization energy?
Kr or Ar
Al or Na
S or Rb
Si or Cs
He or Ca
P or O

63. 3. Electronegativity (EN)
The ability of an atom to attract electrons to itself when in a compound

64. Electronegativity
What trend do you notice about the electronegativity of the elements on the periodic table?
Electronegativity increases towards the top right corner of the PT

65. Does this make sense?
Which elements want electrons?
Elements closest to filling their orbitals
The closer the elements is to filling its orbital, the more it will attract electrons.

66. Electronegativity Practice
Which element has greater electronegativity?
Na or F
Ca or C
Al or Mg
Sr or Al
Ca or K
Cl or F

68. Draw a diagonal arrow showing increasing atomic size

69. Draw a diagonal arrow showing increasing ionization energy

70. Draw a diagonal arrow showing increasing electronegativity