1. Periodic Table of Elements

2. Mendeleev
In 1869, Dmitri Ivanovitch Mendeléev created the first accepted version of the periodic table.
He grouped elements according to their atomic mass, and as he did, he found that the families had similar chemical properties. 
Blank spaces were left open to add the new elements he predicted would occur. 

4. Elements
The elements, alone or in combinations, make up our bodies, our world, our sun, and in fact, the entire universe.

5. The most abundant element in the earth’s crust is oxygen.

6. Modern Periodic Table
Modern periodic law : PROPERTIES OF THE ELEMENTS ARE PERIODIC FUNCTIONS OF THEIR ATOMIC NUMBER.
The modern table is organized according to the ATOMIC NUMBER

7. Key to the Periodic Table
Elements are organized according to their atomic number.
The atomic number refers to how many protons an atom of that element has.
For instance, hydrogen has 1 proton, so it’s atomic number is 1.
The atomic number is unique to that element. No two elements have the same atomic number.

8. What’s in a square?
Different periodic tables can include various bits of information, but usually:
atomic number
symbol
atomic mass
electron configuration
state of matter at room temperature.

9. Atomic Mass Atomic Mass refers to the “weight” of the atom.
It is derived at by adding the number of protons with the number of neutrons.
This is a helium atom. Its atomic mass is 4 (protons plus neutrons).
What is its atomic number? H

10. Atomic Mass and Isotopes
While most atoms have the same number of protons and neutrons, some don’t.
Some atoms have more or less neutrons than protons. These are called isotopes.
An atomic mass number with a decimal is the total of the number of protons plus the average number of neutrons.

11. C Cu Symbols Carbon Copper All elements have their own unique symbol.
It can consist of a single capital letter, or a capital letter and one or two lower case letters. C
Carbon Cu
Copper

12. Common Elements and Symbols

13. Valence Electrons
Valence electrons are the electrons in the outer energy level of an atom.
These are the electrons that are transferred or shared when atoms bond together.
In our table the valence electrons are the last electrons or the electron configuration Na

15. Properties of Metals
Metals are good conductors of heat and electricity.
Metals are shiny- metallic lustet.
Metals are ductile (can be stretched into thin wires).
Metals are malleable (can be pounded into thin sheets).
A chemical property of metal is its reaction with water which results in corrosion.

16. Properties of Non-Metals
Non-metals are poor conductors of heat and electricity.
Non-metals are not ductile or malleable.
Solid non-metals are brittle and break easily.
They are dull.
Many non-metals are gases.
Sulfur

17. Properties of Metalloids B, Si, Ge, As, Sb, Te
Metalloids (metal-like) have properties of both metals and non-metals.
They are solids that can be shiny or dull.
They conduct heat and electricity better than non-metals but not as well as metals.
They are ductile and malleable.
Silicon

18. METALLOIDS (locate them in the periodic table!)Si Ge As Sb Te

20. Periodic Table Organization------ Groups or Families
Vertical columns in the periodic table are known as groups or families The elements in a group have similar electron configurations (same number of valence electrons)

21. Periodic Table Organization ---- Periods
Horizontal Rows in the periodic table are known as Periods The Elements in a period undergo a gradual change in properties as one proceeds from left to right. SAME NUMBER OF SHELLS

22. Families Periods Columns of elements are called groups or families.
Elements in each family have similar but not identical properties.
For example, lithium (Li), sodium (Na), potassium (K), and other members of family IA are all soft, white, shiny metals.
All elements in a family have the same number of valence electrons.
Each horizontal row of elements is called a period.
The elements in a period are not alike in properties.
the properties change greatly across a row.
The first element in a period is always an extremely active solid. The last element in a period, is always an inactive gas.
SAME NUMBER OF SHELLS

23. January 5 Families or groups of elements ALLOTROPES
Trends in the periodic table
Hw – review book – topic 5
Questions 1 to 29 page 83

24. Families

25. Hydrogen
The hydrogen square sits atop Family but it is not a member of that family. Hydrogen is in a class of its own.
It’s a gas at room temperature.
It has one proton and one electron in its one and only energy level.
Hydrogen only needs 2 electrons to fill up its valence shell.

26. Alkali Metals
The alkali family is found in the first column of the periodic table.
Atoms of the alkali metals have a single electron in their outermost level, in other words, 1 valence electron.
They are shiny, have the consistency of clay, and are easily cut with a knife.

27. Alkali Metals They are the most reactive metals.
They react violently with water.
Alkali metals are never found as free elements in nature. They are always bonded with another element.

28. Alkaline Earth Metals They are never found uncombined in nature.
They have two valence electrons.
Alkaline earth metals include magnesium and calcium, among others.

29. Transition Metals
Transition Elements include those elements in the B families.
These are the metals you are probably most familiar: copper, tin, zinc, iron, nickel, gold, and silver.
They are good conductors of heat and electricity.

30. Transition Metals
The compounds of transition metals are usually brightly colored and are often used to color paints.
Transition elements have 1 or 2 valence electrons, which they lose when they form bonds with other atoms. Some transition elements can lose electrons in their next-to-outermost level.

31. Transition Elements
Transition elements have COLORED IONS

32. Halogen Family
Halogens have 7 valence electrons, which explains why they are the most active non-metals. They are never found free in nature.
Halogen atoms only need to gain 1 electron to fill their outermost energy level.

33. Noble Gases
Noble Gases are colorless gases that are extremely un-reactive. They are inactive because their outermost energy level is full.
Because they do not readily combine with other elements to form compounds, the noble gases are called inert.
All the noble gases are found in small amounts in the earth's atmosphere.

34. Rare Earth Elements
The thirty rare earth elements are composed of the lanthanide and actinide series.
One element of the lanthanide series and most of the elements in the actinide series are called trans-uranium, which means synthetic or man-made.

35. TRENDS IN THE PERIODIC TABLE
-- Ionization Energy
-- Electronegativity
-- Ionic Radius
-- Metallic Character
-- Activity - reactivity

36. Periodic Properties
Elements show gradual changes in certain physical properties as one moves across a period or down a group in the periodic table. These properties repeat after certain intervals. In other words they are PERIODIC
Periodic properties include:
-- Ionization Energy
-- Electronegativity
-- Electron Affinity
-- Atomic Radius
-- Ionic Radius

37. Atomic Radius The radius increases on going down a group.
Each additional energy level “shields” the electrons from being pulled in toward the nucleus.
The radius decreases on going across a period.

38. Atomic Radius
The radius decreases across a period because the nuclear charge is increasing and the last electrons are in the same shell. Each added electron feels a greater and greater positive charge.
Large
Small

39. Atomic Radius

40. JANUARY 6 MORE ON PERIODIC TRENDS IONIC RADIUS IONIZATION ENERGY
ELECTRONEGATIVITY
METALLIC CHARACTER

41. ION FORMATION Metals lose electrons and become positive ions
Non-metals gain electrons and become negative ions

42. REVIEW BOOK PAGE 83 1 2 4 3 1 4 3

43. REVIEW BOOK P 84 3 1 2 4

44. IONIC RADIUS
METALLIC Cations (positive ions) are smaller than their corresponding atoms because the ions have less electrons than the atom

45. Ionic Radius CATIONS are SMALLER than the atoms from which they come.Li +
, 78 pm
2e and 3 p
Forming a cation.
Li,152 pm
3e and 3p
CATIONS are SMALLER than the atoms from which they come. .

46. Ionic Radius for Cations (METALLIC I ONS
Positive ions or cations are smaller than the corresponding atoms.

47. Anions (NON-METALLIC IONS)
Anions (negative ions) are larger than their corresponding atoms

48. Ionic Radius-Anions F -
, 133 pm
10 e- and 9 p+
F pm
9e- and 9p+
Forming an anion.
ANIONS are LARGER than the atoms from which they come.

49. January 9
More trends
Ionization energy
Electronegativity
Allotropes

50. Trends in Ionization Energy
Ionization energy is the energy required to
Remove an electron from an atom
Ionization energy increases across a period because the nuclear charge increases.
Metals lose electrons more easily than nonmetals. Metals have low ionization energy
Nonmetals lose electrons with difficulty (they like to GAIN electrons). They have high ionization energy

51. Trends in Ionization Energy
The ionization energy decreases DOWN a group because going down a group the atoms have extra shells and it is easier to remove an electron from a larger atom

52. Electronegativity
Electronegativity is a measure of the ability of an atom in a molecule to attract electrons to itself.
This concept was first proposed by Linus Pauling ( ). He later won the Nobel Prize for his efforts

53. Periodic Trends: Electronegativity
In a group: Atoms with fewer energy levels can attract electrons better (less shielding). So, electronegativity increases UP a group of elements.
In a period: More protons, while the energy levels are the same, means atoms can better attract electrons. So, electronegativity increases RIGHT in a period of elements.

54. Summary of Periodic Trends

55. METALLIC CHARACTER Metals react by losing electrons.
The metallic character increases as we move down a group and to the left of the table.
Francium is the most metallic element
Metals have low ionization energy and low electronegativities

56. What does it mean to be reactive?
We will be describing elements according to their reactivity.
Elements that are reactive bond easily with other elements to make compounds.
Some elements are only found in nature bonded with other elements.
What makes an element reactive?
An incomplete valence electron level.
All atoms (except hydrogen) want to have 8 electrons in their very outermost energy level (This is called the rule of octet.)
Atoms bond until this level is complete. Atoms with few valence electrons lose them during bonding. Atoms with 6, 7, or 8 valence electrons gain electrons during bonding.

57. 5

60. ALLOTROPES Some elements exist in nature in different forms.
Oxygen exist as O2 (g) and O3 (g)- Ozone

61. Carbon allotropic forms
Graphite
Diamond
Buckminsterfullerene

62. Phosphorous Allotropes
White
Red
Black

63. PAGE 90 1 4 3 2 4 1 2 3 4 1 3 2

66. Set 1 Metals-Metalloids-Non Metals3 4 2 1
A. solid
b. conductivity, luster, malleability
Set 2 1 2 3 4
A Very reactive metals. Lose 1 electron easily
b It is a metal