1. Nuclear Energy - Day One

2. TODAY’S WARM-UP: Answer these questions:
 Atoms of the same element will have the same number of ______________.
 An atom that gains one or more electrons will have a ______________ charge.
 An atom that loses one or more electrons will have a _______________ charge.
 An atom that gains or loses one or more electrons is called an ____________.
 A positive ion is called a ___________ and a negative ion is called an _________________.
 Atoms of the same element that have different numbers of neutrons are called ________________.

3. Answer these questions:
 Atoms of the same element will have the same number of PROTONS.
 An atom that gains one or more electrons will have a NEGATIVE charge.
 An atom that loses one or more electrons will have a POSTIVE charge.
 An atom that gains or loses one or more electrons is called an ION.
 A positive ion is called a CATION and a negative ion is called an ANION.
 Atoms of the same element that have different numbers of neutrons are called ISOTOPES.

4. Elements, Compounds, and Mixtures

5. 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.

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

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

8. Element, Compound or Mixture?

9. Element, Compound or Mixture?

10. Review of the Periodic Table
Atomic Number ● Symbol ● Atomic Weight
Element ● Compound ● Mixture

11. 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.

12. What is the PERIODIC TABLE?
Shows all known elements in the universe.
Organizes the elements by chemical properties.

13. I made the PERIODIC TABLE !
I am Dmitri Mendeleev!
I made the PERIODIC TABLE !

14. 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. 

15. How do you read the PERIODIC TABLE?

16. How do I find the number of protons, electrons, and neutrons in an element using the periodic table?
# of PROTONS = ATOMIC NUMBER
# of ELECTRONS = ATOMIC NUMBER
# of NEUTRONS = ATOMIC _ ATOMIC
WEIGHT NUMBER

17. 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.

18. 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.

19. 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.

21. 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.

22. 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

23. 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

26. Families Periods Each horizontal row of elements is called a period.
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.

27. Families

29. 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.

30. 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.

31. 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.

32. 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.

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

34. 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.

35. 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.

36. 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.

37. 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).

38. 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.

39. 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.

40. 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.

41. 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.

42. 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.

43. 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.

44. 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.

45. Periodic Table Practice
For each element below, give the chemical symbol, # of protons, # of electrons, # of neutrons, # of electron orbits, # of valence electrons and family. In addition, identify the element as a metal, nonmetal, or metalloid.
Calcium
Galium
Bromine

46. COMPLETE - What is an ionic bond?
 Atoms will transfer one or more __________ to another to form the bond.
 Each atom is left with a _________ outer shell.
 An ionic bond forms between a ________ ion with a positive charge and a _____________ ion with a negative charge
 Bonding forms following the _________. Atoms are stable when they have __ valence electrons

47. What is an ionic bond?
 Atoms will transfer one or more electrons to another to form the bond.
 Each atom is left with a complete outer shell.
 An ionic bond forms between a metal ion with a positive charge and a nonmetal ion with a negative charge
 Bonding forms following the Octet rule. Atoms are stable when they have 8 valence electrons

48. Complete the bonding practice diagrams.
Use your Periodic Table.
Draw Lewis Dot diagrams for each element.
Use arrows to electron movement.
Write a balanced chemical equation to represent each reaction.
Give the name of the product.

49. Product is sodium chloride
Na + Cl NaCl
Product is sodium chloride

50. The product is Magnesium Iodide
Mg I MgI2
The product is Magnesium Iodide

51. The product is sodium oxide
BALANCE THE
EQUATION!
Na + O Na2O
The product is sodium oxide 4 2

52. The product is aluminum chloride
Balance the
Equation!
Al Cl AlCl3
The product is aluminum chloride 2 3 2

53. What is a covalent bond?
 Atoms share one or more ______________ with each other to form the bond.
 Each atom is left with a _________________.
 A covalent bond forms between two _______________.
 Bonding will follow the __________ Rule.

54. What is a covalent bond?
 Atoms share one or more electrons with each other to form the bond.
 Each atom is left with a complete outer shell.
 A covalent bond forms between two nonmetals.
 Bonding will follow the Octet Rule.

55. Complete the bonding practice diagrams.
Use your Periodic Table.
Draw Lewis Dot diagrams for each element.
Group electrons using circles.
Write a balanced chemical equation to represent each reaction.
Give the name of the product.

56. Hydrogen molecule

57. The product is dihydrogen oxide
Show how water is formed.
H O H2O
The product is dihydrogen oxide 2 2

58. The product is carbon dioxide
C + O CO2
The product is carbon dioxide

59. The product is carbon tetrahydride
C H CH4 2