1. Atoms, Elements and the periodic table

2. Matter
All matter is composed of atoms and groups of atoms bonded together, called molecules.
Substances that are made from one type of atom only are called pure substances.
Substances that are made from more than one type of atom bonded together are called compounds.
Compounds that are combined physically, but not chemically, are called mixtures.

3. Creation of a pamphlet about the models of atomic structure
In each section you must include:
Their theory about atomic structure
The technology they used to support their idea
A diagram of the model
The reason for the downfall of their theory
John Dalton
JJ Thomson
Ernest Rutherford
Neils Bohr

4. Atomic structure of an atom-what we know now…
Nucleus Proton Neutron Electron

5. n

6. What is an atom?
The smallest part of an atom.
Made up of a nucleus surrounded by electrons.

7. What is the nucleus?
The core part of the atom.
Made up of protons and neutrons.
99.99% of the mass of the atom.

8. What is a proton?
A positively charged particle.
Found in the nucleus.

9. What is a neutron?
A neutral particle(no charge)
Found in the nucleus.

10. What is an electron?
A negatively charged particle.
Found in orbit around the nucleus.

11. helium carbon nitrogen sodium silver oxygen mercury neodymium chlorine
gold
mercury
oxygen
hydrogen
helium
sodium
niobium
neodymium
carbon

12. 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.

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

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

15. 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.

16. Why is the Periodic Table important to me?
The periodic table is the most useful tool to a chemist.
You get to use it on every test.
It organizes lots of information about all the known elements.

17. Pre-Periodic Table Chemistry …
…was a mess!!!
No organization of elements.
Imagine going to a grocery store with no organization!!
Difficult to find information.
Chemistry didn’t make sense.

18. 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. 

19. Dmitri Mendeléev : Father of the Table
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.

20. 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 are labeled from 1 to 18.

22. 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

23. Elements and Symbols
Many symbols are the first letter of the element…carbon
others are the first two letters, like calcium
others use two prominent letters like cadmium…Cd
still others use latin, greek or other language roots, like copper Cu (cuprium)
Scientists have devised a ‘short hand’ way of naming elements
these are called chemical symbols
hydrogen = H
carbon = C
calcium = Ca

24. Elements and Symbols
Whatever the reason for naming an element, the same rules apply
only one capital letter
if the symbol is two letters, it must be one upper and one lower case letter
The newest of the synthetic elements have three letters, Uub for example
eventually when element 112 is named it will be given a two letter symbol

25. Describe how to read the periodic table:
Atomic Symbol: The atomic symbol is one or two letters chosen to represent an element ("H" for "hydrogen," etc.). 
These symbols are used every where in the world
  Usually, a symbol is the abbreviation of the element or the abbreviated Latin name of the element.

26. Compounds and formula
Compounds also have a short hand way of naming them
these are called chemical formula
H2O is a familiar example
CO2 = carbon dioxide
C6H12O6 = glucose
H2O2 = hydrogen peroxide
CuSO4 = copper sulfate

27. Chemical formula For example: H2O tells us many things about water…
the fact that it is made up of hydrogen and Oxygen
the fact that there are 2x as many hydrogen atoms as oxygen atoms
Like symbols, formula have certain rules for their use.
They always contain the elements found in the compounds
they always show the relative number of atoms of each element

28. 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.

29. Common Elements and Symbols

30. 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.

32. Describe the Periodic Table

33. 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.

34. 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

35. 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

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

39. Families on the Periodic Table
Columns are also grouped into families.
Families may be one column, or several columns put together.
Families have names rather than numbers. (Just like your family has a common last name.)

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

41. 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

42. 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.

43. ALKALI METALS
Group 1
The alkali family is found in the first column of the periodic table.
Hydrogen is not a member, it is a non-metal
1 electron in the outer shell
Soft and silvery metals
Very reactive, esp. with water
Conduct electricity
Soft enough to cut with a butter knife

44. 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.

45. 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.

46. 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.

47. 5

50. ALKALINE EARTH METALS Group 2 2 electrons in the outer shell
White and malleable
Reactive, but less than Alkali metals
Conduct electricity
Several of these elements are important mineral nutrients (such as Mg and Ca

51. TRANSITION METALS Groups in the middle
Good conductors of heat and electricity.
Some are used for jewelry.
The transition metals are able to put up to 32 electrons in their second to last shell.
Can bond with many elements in a variety of shapes.

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

53. 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.

54. 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.

55. 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.

56. BORON FAMILY Group 3 3 electrons in the outer shell Most are metals
Boron is a metalloid
Elements in group 13
Aluminum metal was once rare and expensive, not a “disposable metal”.

57. 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).

58. 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.

59. CARBON FAMILY Group 4 4 electrons in the outer shell
Contains metals, metalloids, and a non-metal Carbon (C)

60. 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.

61. 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.

62. 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.

63. NITROGEN FAMILY Group 5 5 electrons in the outer shell
Can share electrons to form compounds
Contains metals, metalloids, and non-metals

64. 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.

65. OXYGEN FAMILY Group 6 6 electrons in the outer shell
Contains metals, metalloids, and non-metals
Reactive

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

67. 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.

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

69. 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.

70. 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.

71. 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.

72. The Noble Gases
Also known as rare gases or inert gases

73. Rare Earth Metals Some are Radioactive
The rare earths are silver, silvery-white, or gray metals.
Conduct electricity

74. 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

75. 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

76. 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.
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.

77. Name that family!

89. Describe how to read the periodic table:
Every table has:

90. Describe how to read the periodic table:
Atomic Number
The number of protons in an atom identifies the element. 
  The number of protons in an atom is referred to as the atomic number of that element.

91. 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.

92. 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.

93. Atomic Mass Unit (AMU) There are
6 X 1023 or 600,000,000,000,000,000,000,000 amus in one gram.
(Remember that electrons are 2000 times smaller than one amu).

94. Describe how to read the periodic table:
Atomic Mass: The atomic mass is the average mass of an element in atomic mass units ("amu"). 
Though individual atoms always have a whole number of amus, the atomic mass on the periodic table is shown as a decimal number because it is an average of all the isotopes of an element.

95. 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.

96. Elements, Compounds, Mixtures
Sodium is an element.
Chlorine is an element.
When sodium and chlorine bond they make the compound sodium chloride, commonly known as table salt.
Compounds have different properties than the elements that make them up.
Table salt has different properties than sodium, an explosive metal, and chlorine, a poisonous gas.

97. Elements, Compounds, Mixtures
Hydrogen is an element.
Oxygen is an element.
When hydrogen and oxygen bond they make the compound water.
When salt and water are combined, a mixture is created. Compounds in mixtures retain their individual properties.
The ocean is a mixture.

98. Elements, compounds, and mixtures
Mixtures can be separated by physical means.
Compounds can only be separated by chemical means.
Elements are pure substances. When the subatomic particles of an element are separated from its atom, it no longer retains the properties of that element.