The Periodic Table final.pptx for chemistry

The Periodic Table Presentation

1. Three States of Matter Substances are made up of particles. The state of the substance depends on the arrangement of the particles. Solid Particles held tightly Very close together Regular arrangement Vibrate Can’t move from place to place Liquid Particles held weakly Very close together Random arrangement Vibrate Constantly move past each other Gas No attraction between particles Far apart Random arrangement Vibrate Move quickly in all directions The Three States of Matter

2. What is an ELEMENT? A substance composed of a single kind of atom. Cannot be broken down into another substance by chemical or physical means.

3. What is a COMPOUND? A substance in which two or more different elements are CHEMICALLY bonded together.

4. What is a MIXTURE? Two or more substances that are mixed together but are NOT chemically bonded.

5. Element, Compound or Mixture?

6. Element, Compound or Mixture?

7. Element, Compound or Mixture?

8. Element, Compound or Mixture?

9. Element, Compound or Mixture?

10. Element, Compound or Mixture?

11. What are Atoms? Atoms are the simplest and smallest particle composed of protons , electrons , and neutrons . The number of protons in the nucleus of an atom is equal to its atomic number. Normally, the number of protons equals the number of electrons. The Atom’s Family

12. Protons, Neutrons and Electrons A proton is a positively charged particle inside the nucleus. A neutron is a neutral particle also inside the nucleus. An electron is a negatively charged particle that orbits the nucleus.

13. Periodic Table of Elements

14. History of the Periodic Table Johann Dobereiner grouped three elements with similar properties -40 known elements -First scientist to observe an important trend -Noticed certain groups of three elements had similar physical and chemical properties but different masses Called them TRIADS Ex. Li,Na,K Cl,Br,I Cu,Ag,Au Be,Mg,Ca

15. John Newlands arranged the known elements in order of atomic weights and observed similarities between some elements (Law of Octaves). -mid 1800’s -45 @ known elements -Noted connection of properties and mass were a repeating pattern in order of increasing mass -Every 8 th element had similar properties( Dobereiner’s Triads) -Didn’t know about Noble gases -Called it Law of Octaves -Problems occurred as more elements were discovered and did not fit pattern

16. Mendel e ev 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.

17. Mendeleev 1860’s @ 60+ known elements -Father of Periodic Table (P.T.) -Developed table that showed relationship between properties of elements and atomic masses Remember: the only thing known about atoms is? Dalton’s Theories -No e- or p+ -Carefully planned and in great detail -Avoided earlier mistakes of forcing elements to fit into 8 pattern like Newland

18. Proposed properties were a function of increasing atomic mass Believed similar properties occurred after periods that could vary in length by specific patterns Left blank spaces on table were an element did not fit ( did not force elements in) properties Predicted that spaces were undiscovered elements Predicted masses and properties of unknowns Elements discovered were very close to predictions Elements properties repeated in an orderly way

19. Not all elements fit pattern Ex. Te -I and Co-Ni Mendeleev switched elements around even though masses were not in pattern Believed properties were more important factor to consider Predicted a new theory or discovery would explain this 1 st Periodic Law: properties of the elements are a periodic function of their increasing atomic masses

20. Henry Moseley determined the atomic number of each of the elements and modified the Periodic Law. Modern Periodic Law: properties of the elements are a periodic function of their increasing atomic number

21. Henry Moseley (1887-1915) Made improvements to Mendeleev’s Periodic Table Arranged elements by atomic number instead of mass Realized that there were undiscovered elements

22. Learning The Periodic Table of Elements

23. What is the Periodic Table of Elements? Elements are substances that cannot be broken down any further by chemical means. They are the building blocks of matter. There are over 100! The Periodic Table is the arrangement of these elements by increasing atomic number and similar properties. It holds all the chemical elements found on Earth.

24. What are elements made of? Each element is made up of one type of atom, which is different to the atoms in any other element. Gold is an element made up of only gold atoms . Carbon is an element made up of only carbon atoms . Oxygen is an element made up of only oxygen atoms .

25. Elements Each element on the Periodic Table has an atomic number , symbol , name and average atomic mass . Atomic number – the number of protons found in the nucleus of an atom. Average atomic mass – the mass of an atom including the protons, neutrons and electrons.

26. What is the atomic number? Every element has a unique atomic number . This is the number of protons in the nucleus of each atom. What is the atomic number of this helium atom? A neutral atom must have equal numbers of protons and electrons, so the atomic number of an element also gives the number of electrons . Helium has 2 protons, so its atomic number is 2. Atoms are neutrally charged, so what links atomic number and the number of electrons? electron proton neutron

27. What are the properties of elements? A property is any characteristic feature of a substance. Properties of sodium include: The chemical properties of an element are determined by its atomic number . Are there any patterns in the properties of the elements? highly reactive solid but melts easily feels light (low density). Can you name any properties of the element sodium ? A property is any characteristic feature of a substance.

28. Elements and atoms – true or false?

29. How do you read the PERIODIC TABLE?

30. g o l d helium silver me r cu r y oxygen hydr o g e n sodium nitrogen ni o bium neodymium chlorine carbon

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

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

33. Abundant Elements

34. Periodic Table The periodic table organizes the elements in a particular way. A great deal of information about an element can be gathered from its position in the period table. For example, you can predict with reasonably good accuracy the physical and chemical properties of the element. You can also predict what other elements a particular element will react with chemically. Understanding the organization and plan of the periodic table will help you obtain basic information about each of the 118 known elements.

35. Key to the Periodic Table Elements are organized on the table according to their atomic number, usually found near the top of the square. 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.

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

37. Atomic Number This refers to how many protons an atom of that element has. No two elements, have the same number of protons. Bohr Model of Hydrogen Atom Wave Model

38. 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 H ma s s i s 4 (p r o t on s plu s n e ut r on s ). What is its atomic number?

39. 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.

40. Atomic Mass Unit (AMU) The unit of measurement for an atom is an AMU. It stands for atomic mass unit. One AMU is equal to the mass of one proton.

41. Symbols 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. Carbon C Cu Copper

42. Common Elements and Symbols

43. Valence Electrons The number of valence electrons an atom has may also appear in a square. 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.

44. Patterns: metals and non-metals on the right (except hydrogen) Where are these different types of elements grouped together in the periodic table? metals non-metals between metals and non-metals semi-metals on the left and centre Can you name a semi-metal element? Semi-metals have some properties similar to metals and other properties similar to non-metals.

45. Metals, Nonmetals and Metalloids The major categories of elements are the metals, non-metals, and metalloids. Metals are lustrous, malleable, and are good conductors of heat and electricity. Non-metals are elements that do not share the properties of metals. Metalloids are elements that share some, but not all the properties of metals.

46. Metals - Lustrous, Malleable, and Good Conductors? These are physical properties of metals Lustrous means shiny or reflective of light. Coins and jewelry are shiny and reflective . Malleable means capable of being shaped. Aluminum foil is shaped or molded around food items to keep them fresh. Being a Good Conductor means being able to allow electricity and heat to flow through. When you think about the wires we use for electrical devices, they are mostly made of copper and other metals.

47. Properties of Metals Metals are good conductors of heat and electricity. Metals are shiny. 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.

48. 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

49. Properties of Metalloids 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

50. antimony (Sb) Is this element a or a ? H Li Na K Rb Cs Fr Be Sc Ti Mg V Cr Mn Fe Co Ni Cu Zn Ga Ge Se Br Ca Kr Y Zr Nb Mo Tc Ru Pd Ag Cd In Sn Sb Sr Te Rh Ba Hf Ta W Re Os Ir Au Hg Tl Pb Bi Po La At Pt Ra Rf Db Sg Bh Hs Mt ? ? Ac ? Al P N O S Cl F Ne Ar Rn I Si Xe He B C As Fe Fe Mg S P Mg S P Cu Cu metal non-metal I I Sb Hard to say! Sb Metal or non-metal? iodine (I) iron (Fe) copper (Cu) phosphorus (P) sulfur (S) magnesium (Mg)

51. Metals and non-metals in the periodic table The periodic table is a list of all the known elements which are arranged according to the similarities in their properties. Non-metals are mostly on the right. Metals are on the left and in the centre. What type of elements are between metals and non-metals? Xe

52. Metal, non-metal or metalloid? H Li Na K Rb Cs Fr Be Sc Ti Mg V Cr Mn Fe Co Ni Cu Zn Ga Ge Se Br Ca Kr Y Zr Nb Mo Tc Ru Pd Ag Cd In Sn Sb Sr Te Rh Ba Hf Ta W Re Os Ir Au Hg Tl Pb Bi Po La At Pt Ra Rf Db Sg Bh Hs Mt ? ? Ac ? Al P N O S Cl F Ne Ar Rn I Si Xe He B C As silicon (Si) metalloid francium (Fr) metal scandium (Sc) metal kryPeriodic Tableon (Kr) non-metal cobalt (Co) metal What are metalloids? Which side are the non-metals on? Which side are the metals on? Metalloids sometimes behave like metals and sometimes like non-metals. Metals are on the left and in the center . Non-metals are mostly on the right.

53. Patterns: physical state Only two elements are liquids at room temperature. What are they? liquids Where are these elements of different states grouped together in the periodic table? in the middle and on the right solids on the far right (except hydrogen) gases on the left, in the centre and on the right bromine and mercury

54. The different columns of elements are called groups or families Elements in the same family have similar properties , just like family members have similar characteristics.

55. Columns of elements What are columns of elements called? groups 1 2 4 3 5 6 7

56. Rows of elements periods What are rows of elements called? 1 2 3 4 5 6 7

57. How is it Arranged? The elements are put into rows by increasing ATOMIC NUMBER . The horizontal rows are called periods and are labeled 1 to 7. The vertical rows are called groups and are labeled 1 to 18 The red lines show the different periods and the green lines show the groups.

58. Fa m ilies 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. Periods Each horizontal row of elements is called a period. The elements in a period are not alike in properties. In fact, the properties change greatly across even 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. All elements of the same period have the same number of electron shells.

59. Grouped Elements Have Similarities Elements in the same group have similar properties. Remember, groups are columns. Chemical Property - a property used to characterize materials in reactions that change their identity. Ex: burning something. Physical Property - a characteristic of a substance that can be observed without changing the substance into something else. Ex: measuring something’s length, color, mass or volume.

60. Hydrogen The hydrogen square sits atop Family AI, 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.

61. Hydrogen – is not part of the Alkali metals

62. 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.

63. Alkali metals

64. Alkali Metals Elements in Group 1 (not including Hydrogen). Very reactive metals. Always combine with something else in nature. Salt – an Alkali Metal, Sodium , and another element, Chlorine , combined.

65. 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.

66. 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.) A t oms bond until this le v el is complete. A t oms with f ew valence ele c trons lose them du r ing bon d ing. A t oms with 6, 7, or 8 valence electrons gain electrons during bonding.

67. 5

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

69. Alkaline earth metals

70. Alkaline Earth Metals Elements in Group 2 . Reactive Metals that are always combined with non-metals in nature. Several of these elements are important mineral nutrients, like Calcium.

71. 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.

72. Transition metals

73. Transition Metals Elements in Groups 3-12 . Less reactive, harder metals. Includes metals used in jewelry, money and construction.

74. 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.

75. Transition Elements Transition elements have properties similar to one another and to other metals, but their properties do not fit in with those of any other family. Many transition metals combine chemically with oxygen to form compounds called oxides.

76. Boron Family The Boron Family is named after the first element in the family. Atoms in this family have 3 valence electrons. This family includes a metalloid (boron), and the rest are metals. This family includes the most abundant metal in the earth’s crust (aluminum).

77. Boron Group

78. Boron Family Elements in Group 13 . Boron has properties of both metals and non-metals. The rest of the elements in this group are metals.

79. Carbon Family Atoms of this family have 4 valence electrons. This family includes a non-metal (carbon), metalloids, and metals. The element carbon is called the “basis of life.” There is an entire branch of chemistry devoted to carbon compounds called organic chemistry.

80. Carbon Group

81. Carbon Family Elements in Group 14 . Contains elements important to life and computers. Carbon is the basic element in all organic compounds. Silicon and Germanium are important semiconductors.

82. Nitrogen Family The nitrogen family is named after the element that makes up 78% of our atmosphere. This family includes non- metals, metalloids, and metals. Atoms in the nitrogen family have 5 valence electrons. They tend to share electrons when they bond. Other elements in this family are phosphorus, arsenic, antimony, and bismuth.

83. Nitrogen Group

84. Nitrogen Family Elements in Group 15 . Nitrogen makes up more than ¾ of our atmosphere. The red tip of matches is made of phosphorous.

85. Oxygen Family Atoms of this family have 6 valence electrons. Most elements in this family share electrons when forming compounds. Oxygen is the most abundant element in the earth’s crust. It is extremely active and combines with almost all elements.

86. Oxygen Group

87. Oxygen Family or Chalcogens Elements in Group 16 . Oxygen is necessary for respiration. Many things that have a bad odor contain sulfur.

88. Halogen Family The elements in this family are fluorine, chlorine, bromine, iodine, and astatine. 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. They react with alkali metals to form salts.

89. Halogens

90. Halogens Elements in Group 17 . Very reactive, diatomic non-metals. Always found combined with other elements in nature. Chlorine is used to keep bacteria out of swimming pools.

91. Noble Gases Noble Gases are colorless gases that are extremely un-reactive. One important property of the noble gases is their inactivity. 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. The family of noble gases includes helium, neon, argon, krypton, xenon, and radon. All the noble gases are found in small amounts in the earth's atmosphere.

92. Noble Gases

93. Noble Gases Elements in Group 18 . VERY reactive gases. Used in lighted neon signs. Helium is used to make party balloons float.

94. 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.

95. Lanthanides Actinides Inner Transition Metals

96. Elements Used Everyday Can you think of any elements you use every day?

97. Trends in the Periodic Table Valence electrons – outermost electrons Group (New ) 1 2 13 14 15 16 17 18 Group (Old) IA IIA IIIA IVA VA VIA VIIA VIIIA Element Na Mg Al Si P S Cl Ar Number of Valence electrons 1 2 3 4 5 6 7 8

98. Prerequisite Content: Trends in the Periodic Table Octet Rule – states that elements gain or lose electrons to attain an electron configuration of the nearest noble gas, to become stable.

99. Prerequisite Content: Trends in the Periodic Table Octet Rule – states that elements gain or lose electrons to attain an electron configuration of the nearest noble gas, to become stable. Group (New ) 1 2 13 14 15 16 17 18 Group (Old) IA IIA IIIA IVA VA VIA VIIA VIIIA Element Na Mg Al Si P S Cl Ar Number of Valence electrons 1 2 3 4 5 6 7 8 Lose or gain electron? Loses 1e Loses 2e Loses 3e Loses 4e or gains 4e Gains 3e Gains 2e Gains 1e n/a (stable)

100. Patterns: reactivity of metals Fr Ra Ac Rf Db Sg Bh Hs Mt Ds Rg Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Na Mg Al Li Be What happens to the reactivity of metals down a group ? Which is the most reactive metal ? increase in reactivity increase in reactivity What happens to the reactivity of metals along a period ?

101. Which metal is more reactive?

102. Patterns: reactivity of non-metals increase in reactivity Group 0 elements are the most unreactive of all elements. For the remaining non-metals and semi-metals, reactivity increases up a group and along a period from left to right. Which is the most reactive non-metal/semi-metal? At Rn Sb Te I Xe Ge As Se Br Kr Si P S Cl Ar B C N O F Ne He increase in reactivity unreactive

103. Which non-metal is more reactive?

104. Critical Content: Trends in the Periodic Table

105. Critical Content: Trend in Atomic Radius Across a period (left to right): decreasing, due to the effective nuclear charge Down a group (top to bottom): increasing due to increasing energy levels

106. Patterns, atomic number and electrons What links atomic number and the properties of elements? The periodic table shows that patterns in the properties of elements are linked to atomic number. atomic number = number of protons atomic number = number of electrons number of protons = number of electrons Electrons! As atomic number increases by one, the number of electrons also increases by one. This means that the elements in the periodic table are also arranged in order of the number of electrons.

107. How are electrons arranged? Electrons are arranged in shells around an atom’s nucleus. (The shells can also be called energy levels). This electron arrangement is written as 2,8,8. 1 st shell holds a maximum of 2 electrons 2 nd shell holds a maximum of 8 electrons 3 rd shell holds a maximum of 8 electrons Each shell has a maximum number of electrons that it can hold. Electrons will fill the shells nearest the nucleus first.

108. Electrons in period 1 Elements in period 1 only have electrons in the first shell . Why are there only two elements in period 1? The first shell can only hold a maximum of two electrons, so period 1 only includes the elements hydrogen and helium . What is special about the outer shell of helium? 1 2 H He 1 2 4 3 5 6 7 1

109. Electrons in period 2 Elements in period 2 all have a complete first shell. The second shell is completed one electron at a time going across the period from left to right. What is special about the outer shell of neon? 2, 1 2, 2 2, 3 2, 4 2, 5 2, 6 2, 7 2, 8 Li Be B C N O F Ne 1 2 4 3 5 6 7 What happens to electrons in the second shell in period 2? 2

110. Electrons in period 3 2,8, 1 2,8, 2 2,8, 3 2,8, 4 2,8, 5 2,8, 6 2,8, 7 2,8, 8 Elements in period 3 have complete first and second shells. The third shell is completed one electron at a time going across the period from left to right. What happens to electrons in the third shell in period 3? Na Mg Al Si P S Cl Ar 1 2 4 3 5 6 7 What is special about the outer shell of argon? 3

111. What are the patterns of electron arrangement? Consider the electron arrangements of the first 20 elements in the periodic table. What is the pattern of outer shell electrons in a group? 2,8,1 2,8,2 2,8,3 2,8,4 2,8,5 2,8,6 2,8,7 2,8,8 1 2 4 3 5 6 7 1 2 3 4 2,1 2,2 2,3 2,4 2,5 2,6 2,7 2,8 1 2 2,8,8,1 2,8,8,2 What is the pattern of outer shell electrons across a period? What is the pattern of full electron shells in a group?

112. Electron trends in the periodic table Trends down a group: The point at which a new period starts is the point at which electrons begin to fill a new shell. The number of a group is the same as the number of electrons in the outer shell of elements in that group, except for group 0. the number of outer shell electrons is the same; the number of complete electron shells increases by one. the number of outer shell electrons increases by one; Trends across a period: the number of complete electron shells stays the same.

113. What’s the electron arrangement?

114. Periodic table and electron structure

115. Glossary atomic number – The number of protons in an atom. Sometimes called the proton number. electron arrangement – A shorthand way of writing the number of electrons in an atom’s electron shells. element – A substance made up of only one type of atom. group – A column in the periodic table containing elements with the same number of outer shell electrons and similar chemical properties. period – A row in the periodic table containing elements with the same number of full electron shells. periodic table – The table that lists all the elements in order of increasing atomic number, arranged into groups and periods. property – Any characteristic of an element.

116. Critical Content: Trends in the Periodic Table Summary

117. Critical Content: Periodic Table Arrangement of Elements in the Periodic Table The modern periodic law states that the properties of elements are a periodic function of their atomic numbers.

118. Critical Content: Periodic Table Arrangement of Elements in the Periodic Table Groups and Periods Elements may be classified into groups . Members of the same group exhibit similar properties .

119. Critical Content: Periodic Table Arrangement of Elements in the Periodic Table Groups and Periods The modern periodic table is divided into groups or families , which are the columns and periods , which are the rows There are two sets of groups (families): the representative elements and the transition elements.