1. gold silver helium oxygen mercury hydrogen sodium nitrogen niobium neodymium chlori ne carbon

2. Elements The elements, alone or in combinations, make up our bodies, our world, our sun, and in fact, the entire universe. Elements are the simplest pure substances that cannot be broken down into any other substances.

3. Matter may consist of elements, compounds, or mixtures.

4. 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.

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

6. What is the simplest form of an Element? Example of piece of copper

7. An Atom (Draw what you think an atom would look like.) Include the following labeled in your diagram (An atom has a nucleus, protons, neutrons and electrons)

8.  An element contains one kind of atom!!  An atom, still has properties of that element  If you could line up 100,000,000 copper atoms in a single file, they would be approximately 1 cm long  Despite their small size, individual atoms are observable with instruments such as scanning tunneling (electron) microscopes

9. The Atom The smallest particle of an element The nucleus of the atom contains Protons and Neutrons The atom is surrounded by ELECTRONS.

10. The Atom Protons have a Charge of + 1. Protons are located in the nucleus Protons have a Mass of 1 amu

11. The Atom Neutrons have a Charge of 0 (No charge/neutral charge) Neutrons are located in the nucleus Neutrons have a Mass of 1 amu

12. The Atom Electrons have a Charge of -1 Electrons surround the nucleus making the electron cloud. Electrons have a Mass of almost ZERO.

13. 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. H This is a helium atom. Its atomic mass is 4 (protons plus neutrons). What is its atomic number?

14. 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.

15. Atomic Mass Unit (AMU) There are 6 X 10 23 or 600,000,000,000,000,00 0,000,000 amus in one gram.

16. 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.

17. Mass Number Mass number is the number of protons and neutrons in the nucleus of an isotope: Mass # = p + + n 0 Nuclide p+p+p+p+ n0n0n0n0 e-e-e-e- Mass # Oxygen - 10 -3342 - 31 - 3115 8 8 18 Arsenic 7533 75 Phosphorus 15 31 16

18. Atomic Mass Unit (AMU) Electrons are 2000 times smaller than one amu). WOW!!!!!! They have a mass of almost nothing!!!

19. Electron If your nucleus of an atom were the size of a dime. An electron in this model atom could be more than 1,700 meters away!!!!! As you can see an atom is mostly empty space!

20. A more realistic picture of the electrons would look like this, a cloud surrounding the nucleus of the atom. + - + -

21. Electron The electrons in an atom are found in energy levels as they scatter around the nucleus. The first level can only contain two electrons. The other levels can contain up to eight! The electrons in the outermost shell are called Valence Electrons!! The greatest number of valence electrons an atom can have is eight!! In a stable atom the number of positively charged PROTONS and negatively charged ELECTRONS are the same + + + + + + + + + + - - - - --- - - - + -- ---

22. Valence Electrons Valence electrons are the electrons in the outer energy level of an atom. Valence electrons are the electrons involved in bonding between atoms. We will talk about these A LOT More in the next packet!

23. Counting Valence Electrons

24. Revisit The Atom –The atom is mostly empty space –All the positive charge, and almost all the mass is concentrated in a small area in the center. Called the nucleus –The nucleus is composed of protons and neutrons (they make the nucleus!) –The electrons distributed around the nucleus, and occupy most of the volume

25. - Elements and Atoms Atomic Theory and Models Dalton thought that atoms were like smooth, hard balls that could not be broken into smaller pieces.

26. Thomson’s Atomic Model Thomson believed that the electrons were like plums embedded in a positively charged “pudding,” thus it was called the “plum pudding” model. J. J. Thomson

27. - Elements and Atoms Atomic Theory and Models Thomson suggested that atoms had negatively charged electrons embedded in a positive sphere.

28. Ernest Rutherford’s Gold Foil Experiment - 1911  The alpha particles were fired at a thin sheet of gold foil  Particles that hit on the detecting screen (film) are recorded

29. Rutherford’s problem: In the following pictures, there is a target hidden by a cloud. To figure out the shape of the target, we shot some beams into the cloud and recorded where the beams came out. Can you figure out the shape of the target? Target #1 Target #2

30. The Answers: Target #1 Target #2

31. Rutherford’s Findings Rutherford concluded that an atom’s positive charge must be clustered in a tiny region in its center, called the nucleus.  Most of the particles passed right through  A few particles were deflected  VERY FEW were greatly deflected “Like howitzer shells bouncing off of tissue paper!” Conclusion:

33. Pre-Periodic Table Chemistry … …was a mess!!! No organization of elements. Imagine going to a grocery store with no organization!! Hot dogs next to the candy??? Difficult to find information. Chemistry didn’t make sense.

34. 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.

35. Dmitri Mendeleev: Father of the Table HOW HIS WORKED… Put elements in rows by increasing atomic weight. Put elements in columns by the way they reacted. SOME PROBLEMS… He left blank spaces for what he said were undiscovered elements. (Turned out he was right!) He broke the pattern of increasing atomic weight to keep similar reacting elements together.

36. The Current Periodic Table Mendeleev wasn’t too far off. Now the elements are put in rows by increasing ATOMIC NUMBER!! The horizontal rows are called periods and are labeled from 1 to 7. The vertical columns are called groups or families and are labeled from 1 to 18.

38. 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.

40. Symbols All elements have their own unique symbol. It can consist of a single capital letter, or a capital letter and a lower case letter. Put down a few examples C Carbon Cu Copper

41. Common Elements and Symbols

42. Atomic Number Elements are organized on the table according to their atomic number, usually found near the top of the square. – The atomic number refers the number of protons in the nucleus of that atom. – 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.

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

44. Notice the similarity between atomic number and atomic mass

45. Groups…Here’s Where the Periodic Table Gets Useful!! Elements in the same group or family have similar chemical and physical properties!! (Mendeleev did that on purpose.) Why?? They have the same number of valence electrons.

46. Groups/Families on the Periodic Table Each group/family on the periodic table has its own characteristic properties based on the number of valence electrons!! Just like us elements in the same family are very similar!!

47. 18 Families ( Groups ) 1 2 3 45678 9 ETC

48. How can you tell how many valence electrons each group has and why does that tell us characteristics and properties of the elements? * Atoms want to have a full outer shell!! This is how bonding takes place!! * If an atom has 7 valence electrons and only needs one more for a full eight it is very reactive!!

49. Family/Group 1 elements have how many valence electrons? Family/Group 2 elements have how many valence electrons? Family/Group 15 elements have how many valence electrons?

51. 7 Periods 12345671234567

53. 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.

54. 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

55. 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

57. Hydrogen The hydrogen square sits atop Group 1, but it is not a member of that Group. 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.

58. Hydrogen Hydrogen belongs to a family of its own. Hydrogen is a diatomic, reactive gas. Hydrogen was involved in the explosion of the Hindenberg. Hydrogen is promising as an alternative fuel source for automobiles

59. Periodic Table Packet

60. Halogens Elements in group 17 Very reactive, volatile, diatomic, nonmetals The most reactive nonmetals!! Always found combined with other element in nature. Used as disinfectants and to strengthen teeth.

61. Oxygen Family Elements in group 16 Oxygen is necessary for respiration. Many things that stink, contain sulfur (rotten eggs, garlic, skunks,etc.)

63. Nitrogen Family Elements in group 15 Nitrogen makes up over ¾ of the atmosphere. Nitrogen and phosphorus are both important in living things. Most of the world’s nitrogen is not available to living things. The red stuff on the tip of matches is phosphorus.

65. 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

66. Carbon Family Elements in group 14 Contains elements important to life and computers. Carbon is the basis for an entire branch of chemistry. Silicon and Germanium are important semiconductors.

68. Periodic Table Packet page

70. The Noble Gases

71. 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.

72. The Noble Gases Elements in group 18 VERY unreactive, monatomic gases Used in lighted “neon” signs Used in blimps to fix the Hindenberg problem. Have a full valence shell.

73. Periodic Table Packet page

75. Alkali Metals 1 st column on the periodic table (Group 1) not including hydrogen. Very reactive metals, always combined with something else in nature (like in salt). Soft enough to cut with a butter knife

76. Alkaline Earth Metals Second column on the periodic table. (Group 2) * Reactive metals that are always combined with nonmetals in nature. Examples include Be, Mg, Ca, Sr, Ba, Ra Several of these elements are important mineral nutrients (such as Mg and Ca

77. 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.

78. 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.

79. Periodic Table Packet page

80. Boron Family Elements in group 13 Aluminum metal was once rare and expensive, not a “disposable metal.”

81. Periodic Table Packet page

83. 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.

84. Transition Metals Elements in groups 3- 12 Less reactive harder metals Includes metals used in jewelry and construction. Metals used “as metal.”

85. 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.

86. 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.

87. 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.

88. 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.

89. Electron Dot Diagrams 1)Find your element on the periodic table. 2)Determine the number of valence electrons. 3)This is how many electrons you will draw.

90. Lewis Structures Find out which group (column) your element is in. This will tell you the number of valence electrons your element has. You will only draw the valence electrons. www.chem 4kids.com

91. Groups - Review Each element in a group has the same number of electrons in their outer orbital, called “Valence Electrons” Except for He, it has 2 valence electrons www.chem 4kids.com

92. Lewis Structures 1)Write the element symbol. 2)Carbon is in the 4 th group, so it has 4 valence electrons. 3)Starting at the right, draw 4 electrons, or dots, counter- clockwise around the element symbol.

93. Lewis Structures 1)Check your work. 2)Using your periodic table, check that Carbon is in the 4 th group. 3)You should have 4 total electrons, or dots, drawn in for Carbon.

94. Lewis Structures On your worksheet, try these elements on your own: a)H b)P c)Ca d)Ar e)Cl f)Al

95. Lewis Structures On your worksheet, try these elements on your own: a)H b)P c)Ca d)Ar e)Cl f)Al

96. Lewis Structures On your worksheet, try these elements on your own: a)H b)P c)Ca d)Ar e)Cl f)Al

97. Lewis Structures On your worksheet, try these elements on your own: a)H b)P c)Ca d)Ar e)Cl f)Al

98. Lewis Structures On your worksheet, try these elements on your own: a)H b)P c)Ca d)Ar e)Cl f)Al

99. Lewis Structures On your worksheet, try these elements on your own: a)H b)P c)Ca d)Ar e)Cl f)Al

100. Lewis Structures On your worksheet, try these elements on your own: a)H b)P c)Ca d)Ar e)Cl f)Al