1. Chapter 5 Periodic Table H Li Na K Rb Cs Fr Be Mg Ca Sr Ra Ba F Cl Br I Uus At O S Se Te Uuh Po N P As Sb Uup Bi C Si Ge Sn Uuq Pb B Al Ga In Uut Tl ScTiVCrMnFeCoNiCuZn YZrNbMoTcRuRhPdAgCd LuHfTaWReOsIrPtAuHg He Ne Ar Kr Xe Rn Uuo LaCePrNdPmSmEuGdTb AcThPaUNpPuAmCmBk Dy Cf Ho Es Er Fm Tm Md Yb No H Li Na K Rb Cs Fr Be Mg Ca Sr Ra Ba B Al Ga In Uut Tl Lr Rf DbSgBhHsMt UunUuuUub ScTiVCrMnFeCoNiCuZn YZrNbMoTcRuRhPdAgCd LuHfTaWReOsIrPtAuHg Lr Rf DbSgBhHsMt UunUuuUub C Si Ge Sn Uuq Pb N P As Sb Uup Bi O S Se Te Uuh Po F Cl Br I Uus At He Ne Ar Kr Xe Rn Uuo LaCePrNdPmSmEuGdTb AcThPaUNpPuAm CmCm Bk Dy Cf Ho Es Er Fm Tm Md Yb No

2. The Greeks It was Empedocles (490 – 430 BC) who established four ultimate elements which make up all the objects in the world - fire, air, water, earth. Different objects are produced according to the different proportions in which these four indestructible and unchangeable elements are combined with each other. elementsfireair waterearthelementsfireair waterearth AristotleAristotle added aether as the divine substance, reasoning that whereas fire, earth, air, and water were earthly and corruptible and no changes had been perceived in the heavenly regions, the stars cannot be made out of any of the four elements but must be made of a different, unchangeable, heavenly substance. aetherstars Aristotleaetherstars One classic diagram (above) has one square inscribed in the other, with the corners of one being the classical elements, and the corners of the other being the properties. The opposite corner is the opposite of these properties, "hot - cold" and "dry - wet".inscribed

3. Elements Science has come along way since Empedocles’ theory of Air, Water, Fire, and Earth. Science has come along way since Empedocles’ theory of Air, Water, Fire, and Earth. Scientists have identified 90 naturally occurring elements, and created about 28 others. Scientists have identified 90 naturally occurring elements, and created about 28 others.

5. Organizing the Elements Elements Mendeleev (1869) Mendeleev (1869) Arranged the elements into rows in order of increasing mass so that the elements with similar properties were in the same column Arranged the elements into rows in order of increasing mass so that the elements with similar properties were in the same column Periodic Table Periodic Table Periodic Table Periodic Table Arrangement of elements in columns Arrangement of elements in columns based on a set of properties that repeat from row to row.

6. Mendeleev’s Periodic Table Put elements in rows by increasing atomic mass. Put elements in columns by the way they reacted He broke the pattern of increasing atomic mass to keep similar reacting elements together.

7. Elements known at his time

8. Spaces left for elements not discovered yet. Spaces left for elements not discovered yet. Eka-aluminum– similar properties to aluminum Eka-aluminum– similar properties to aluminum Predicted to have a low melting point, soft and density of 5.9 g/cm 3 Predicted to have a low melting point, soft and density of 5.9 g/cm 3 Gallium later discovered which has a low melting point and density of 5.91 g/cm 3 Gallium later discovered which has a low melting point and density of 5.91 g/cm 3 Gallium, Scandium, Germanium discovered later but spaces in Mendeleev’s table predicted the properties of these elements before discovery. Gallium, Scandium, Germanium discovered later but spaces in Mendeleev’s table predicted the properties of these elements before discovery. Gallium Gallium Gallium Gallium

9. By looking at our modern periodic table, can you identify what problems might have caused chemists a headache? Ar and K Co and Ni Te and I Th and Pa

10. The Periodic Law Elements listed in order of increasing number of protons (atomic number) Elements listed in order of increasing number of protons (atomic number) When you do this the properties of the elements repeat. When you do this the properties of the elements repeat. Periodic Law- when the elements are arranged in order of increasing number of protons, the properties tend to repeat in a pattern Periodic Law- when the elements are arranged in order of increasing number of protons, the properties tend to repeat in a pattern

11. Henry Moseley 1887 - 1915 In 1913, through his work with X-rays, he determined the actual nuclear charge (atomic number) of the elements*. He rearranged the elements in order of increasing atomic number. * “ There is in the atom a fundamental quantity which increases by regular steps as we pass from each element to the next. This quantity can only be the charge on the central positive nucleus. ”

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

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

14. What’s in a square? Periodic tables can include various bits of information. Some are: Periodic tables can include various bits of information. Some are:  symbol  name  atomic number  atomic mass  oxidation number  state of matter at room temperature

16. The Periodic Table Rows are called periods Rows are called periods Number of elements in each period varies due to the number of available orbitals at each energy level. Number of elements in each period varies due to the number of available orbitals at each energy level. Number of orbitals increases from energy level to energy level. Number of orbitals increases from energy level to energy level. Period 1 – 2 elements Period 1 – 2 elements Periods 2/3 – 8 elements Periods 2/3 – 8 elements Periods 4/5 – 18 elements Periods 4/5 – 18 elements Periods 6/7 – 32 elements Periods 6/7 – 32 elements

17. Valence Electrons Electron that is in the highest occupied energy level of an atom. (outermost) Electron that is in the highest occupied energy level of an atom. (outermost) Number of valence electrons determines chemical properties. Number of valence electrons determines chemical properties. Elements in a group have similar properties because they have the same number of valence electrons. Elements in a group have similar properties because they have the same number of valence electrons. These are the electrons that are transferred or shared when atoms bond together. These are the electrons that are transferred or shared when atoms bond together. For Groups 1, 2, 3A – 8A (Equal to group number) For Groups 1, 2, 3A – 8A (Equal to group number)

18. Group 1 all have one electron in their outside s orbital Group 1 all have one electron in their outside s orbital Group 2 all have two electrons in their outside s orbital Group 2 all have two electrons in their outside s orbital

19. On the right hand side Group 13 -18 the s orbitals are full, and the p orbitals are filling On the right hand side Group 13 -18 the s orbitals are full, and the p orbitals are filling Group 13 s has 2 e - p has 1 e - Group 13 s has 2 e - p has 1 e - Group 14 s has 2 e - p has 2 e - Group 14 s has 2 e - p has 2 e - Group 18 s has 2 e - p has 6 e - Group 18 s has 2 e - p has 6 e - p and s both full p and s both full

20. Electron Configuration Electron Configuration

22. Variation Across a Period Across a period from left to right, the elements become less metallic and more nonmetallic in their properties. Across a period from left to right, the elements become less metallic and more nonmetallic in their properties. In fact, the properties change greatly across every given row. In fact, the properties change greatly across every given row. The first element in a period is always an extremely active solid. The last element in a period, is always an inactive gas. The first element in a period is always an extremely active solid. The last element in a period, is always an inactive gas.

24. Columns are called groups or families Columns are called groups or families Elements in the same group have similar chemical and physical properties!! Elements in the same group have similar chemical and physical properties!! Elements in groups have similar properties because of similar electron configurations. Elements in groups have similar properties because of similar electron configurations. Electron configuration determines an element’s chemical properties. Electron configuration determines an element’s chemical properties. Why?? They have the same number of valence electrons.They have the same number of valence electrons. They will form the same kinds of ions.They will form the same kinds of ions.

25. Families Periods Families Periods Columns of elements are called groups or families. Columns of elements are called groups or families. Elements in each family have similar but not identical properties. 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. 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. 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 of the elements change in a similar pattern across the rows. For instance, the first element in a period is always an extremely active solid. The last element in a period, is always an inactive gas.

27. Properties of Metals Left Side of Periodic Table Left Side of Periodic Table Metals are good conductors of heat and electricity. Metals are good conductors of heat and electricity. Metals are shiny. Metals are shiny. Metals are ductile (can be stretched into thin wires). Metals are ductile (can be stretched into thin wires). Metals are malleable (can be pounded into thin sheets). Metals are malleable (can be pounded into thin sheets). A chemical property of metal is its reaction with water which results in corrosion. A chemical property of metal is its reaction with water which results in corrosion. Metals will lose electrons when bonding (Cation) Metals will lose electrons when bonding (Cation) Solid at room temperature (Except Mercury) Solid at room temperature (Except Mercury)

28. Properties of Non-Metals Right Side of Periodic Table Non-metals are poor conductors of heat and electricity (Insulators). Non-metals are not ductile or malleable. Solid non-metals are brittle and break easily. They are dull. Will gain or share electrons when bonding (anions) Many non-metals are gases. Sulfur

29. Properties of Metalloids In between metals and nonmetals. 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. B, Si, Ge, As, Sb, Te, At Silicon

30. Families Elements on the periodic table can be grouped into families based on their chemical properties. Elements on the periodic table can be grouped into families based on their chemical properties. Each family has a specific name to differentiate it from the other families in the periodic table. Each family has a specific name to differentiate it from the other families in the periodic table. Elements in each family Elements in each family react differently with other elements.

31. Periodic Table of Elements

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

34. What does it mean to be reactive? Elements that are reactive bond easily with other elements to make compounds. Elements that are reactive bond easily with other elements to make compounds.

35. ALKALI METALS ALKALI METALS Group 1 1 valence electron 1 valence electron Soft and silvery metals Soft and silvery metals Can be cut with a knife Can be cut with a knife Very reactive Very reactive Not found in nature alone, only in compounds (NaCl) Not found in nature alone, only in compounds (NaCl) Reactivity increases as you proceed down a group Reactivity increases as you proceed down a group

36. ALKALINE EARTH METALS Group 2 2 valence electrons 2 valence electrons Harder metals Harder metals Usually found in compounds in nature. Usually found in compounds in nature. Reactive, but less than Alkali metals Reactive, but less than Alkali metals

37. TRANSITION METALS Groups in the middle (B) These are the metals you are probably most familiar with. They have the properties that you recognize as metallic These are the metals you are probably most familiar with. They have the properties that you recognize as metallic Usually has 1 or two valance electrons Usually has 1 or two valance electrons Form compounds with distinct colors (Paints, dyes) Form compounds with distinct colors (Paints, dyes) Less reactive Less reactive

38. BORON FAMILY Group 3A 3 valence electrons. 3 valence electrons. Most are metals Most are metals Boron is a metalloid Boron is a metalloid This family includes the most abundant metal in the earth’s crust (aluminum). This family includes the most abundant metal in the earth’s crust (aluminum).

39. CARBON FAMILY Group 4A 4 valence electrons 4 valence electrons Contains metals, metalloids, and a non-metal Carbon (C) Contains metals, metalloids, and a non-metal Carbon (C) The element carbon is called the “basis of life.” There is an entire branch of chemistry devoted to carbon compounds called organic chemistry. The element carbon is called the “basis of life.” There is an entire branch of chemistry devoted to carbon compounds called organic chemistry. Metallic properties increases as you down a group. In Group 14 you start with Carbon (a nonmetal) and end with Lead ( a metal)

40. NITROGEN FAMILY Group 5 5 valence electrons 5 valence electrons Tend to share electrons when they form compounds. Tend to share electrons when they form compounds. Contains metals, metalloids, and non-metals Contains metals, metalloids, and non-metals The nitrogen family is named after the element that makes up 78% of our atmosphere. The nitrogen family is named after the element that makes up 78% of our atmosphere.

41. OXYGEN FAMILY Group 6 6 valence electrons 6 valence electrons Contains 2 metalloids, and non-metals Contains 2 metalloids, and non-metals Reactive Reactive Oxygen is the most abundant element in the earth’s crust. It is extremely active and combines with almost all elements. Oxygen is the most abundant element in the earth’s crust. It is extremely active and combines with almost all elements.

42. Halogens Group 7 7 valence electrons 7 valence electrons All are non-metals All are non-metals Very reactive are often bonded with elements from Group 1 Very reactive are often bonded with elements from Group 1 They react with alkali metals to form salts. They react with alkali metals to form salts. Most active non- metals. They are never found free in nature. Most active non- metals. They are never found free in nature.

43. Noble Gases Group 8 Exist as gases Exist as gases 8 valence electrons besides He (2 electrons) 8 valence electrons besides He (2 electrons) Colorless, odorless gases Colorless, odorless gases Non-metals Non-metals Extremely unreactive (inert) Extremely unreactive (inert) Full valence energy level Full valence energy level

44. Rare Earth Metals Inner Transition Metals Inner Transition Metals The rare earths are silver, silvery- white, or gray metals. The rare earths are silver, silvery- white, or gray metals. 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. 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. They are very similar to each other in their chemical and physical properties which explains why it took chemists a long time to find them.

45. 1 A – alkali metals 2A – alkaline earth Transition metals Noble gases halogens Rare Earth metals 3A 4A 5A

46. The Periodic Law When arranged by increasing atomic number, the chemical elements display a regular and repeating pattern of chemical and physical properties. When arranged by increasing atomic number, the chemical elements display a regular and repeating pattern of chemical and physical properties.

47. Reactivity Trends Group of metals (lose electrons when bonding)  Reactivity increases down a group Group of metals (lose electrons when bonding)  Reactivity increases down a group Less hold on electrons (larger atomic radius) Less hold on electrons (larger atomic radius) Francium (Group 1)  Most reactive metal Francium (Group 1)  Most reactive metal

48. Reactivity Group of Nonmetals (gain electrons when bonding) Group of Nonmetals (gain electrons when bonding) Reactivity increases up a group Reactivity increases up a group Smaller atomic radius  More hold on electrons (less electron repulsion) Smaller atomic radius  More hold on electrons (less electron repulsion) Fluorine (Group 7A)  Most reactive nonmetal Fluorine (Group 7A)  Most reactive nonmetal

49. Reactivity 0

50. Metallic vs. Nonmetallic trends Down a Group – Down a Group – elements increase in metallic properties elements increase in metallic properties Decreases in non metallic properties Decreases in non metallic properties Across a period - Across a period - Elements increase in nonmetallic properties Elements increase in nonmetallic properties Decreases in metallic properties Decreases in metallic properties

51. Other Trends Ionization Energy – energy required to remove an electron Ionization Energy – energy required to remove an electron Electron Affinity – “attraction” for an electron Electron Affinity – “attraction” for an electron Atomic Radius - size of atom Atomic Radius - size of atom

52. General Trends

53. The Periodic Table  