1. The Periodic Table (Your new best friend!!)

2. The Periodic Table
The Periodic Table is a list of all the known elements.
It is organized by increasing atomic number.
As you move from the left to the right, the elements become less metallic with the far right side of the table consisting of nonmetals.

3. The Periodic Table
Elements in the middle of the table are called “transition” elements because they are changed from metallic properties to nonmetallic properties.
Elements who touch the “zigzag” line are called metalloids because they have both metallic and nonmetallic properties.

5. Properties of Metals
Metals are good conductors of heat and electricity
Metals are malleable (can be hammered into thin sheets)
Metals are ductile (can be pulled into wires)
Metals have luster (shiny)

6. Examples of Metals
Potassium, K reacts with water and must be stored in kerosene or oil
Copper, Cu, is a relatively soft metal, and a very good electrical conductor.
Zinc, Zn, is more stable than potassium
Mercury, Hg, is the only metal that exists as a liquid at room temperature

7. Properties of Nonmetals
Carbon, the graphite in “pencil lead” is a great example of a nonmetallic element.
Nonmetals are poor conductors of heat and
electricity
Nonmetals tend to be brittle
Nonmetals do not have luster
Many nonmetals are gases at room temperature

8. Examples of Nonmetals
Microspheres of phosphorus, P, a reactive nonmetal
Sulfur, S, was once known as “brimstone”
Graphite is not the only pure form of carbon, C. Diamond is also carbon; the color comes from impurities caught within the crystal structure

9. Properties of Metalloids
Metalloids straddle the border between metals and nonmetals on the periodic table.
They have properties of both metals and nonmetals.
Metalloids are more brittle than metals, less brittle than most nonmetallic solids
Metalloids are semiconductors of electricity
Some metalloids possess metallic luster

10. Silicon, Si – A Metalloid
Silicon has metallic luster
Silicon is brittle like a nonmetal
Silicon is a semiconductor of electricity
Other metalloids include:
Boron, B
Germanium, Ge
Arsenic, As
Antimony, Sb
Tellurium, Te

11. Period
The Periodic Table
Group or Family
Group or family
Period

12. Families on the Periodic Table
The table is arranged in vertical columns called “groups” or “families”
The horizontal rows are called “periods.”
Elements in each vertical column or group have similar properties

13. 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.

14. ALKALI METALS Group 1 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
Image:

15. ALKALINE EARTH METALS Group 2 2 electrons in the outer shell
White and malleable
Reactive, but less than Alkali metals
Conduct electricity

16. 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.

17. BORON FAMILY Group 3 3 electrons in the outer shell Most are metals
Boron is a metalloid

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

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

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

21. Halogens Group 7 7 electrons in the outer shell All are non-metals
Very reactive are often bonded with elements from Group 1

22. Noble Gases Group 8 Exist as gases Non-metals
8 electrons in the outer shell = Full
Helium (He) has only 2 electrons in the outer shell = Full
Not reactive with other elements

23. Rare Earth Metals Some are Radioactive
The rare earths are silver, silvery-white, or gray metals.
Top row are lanthanides
Bottom row are actinides

24. Period
The Periodic Table
Group or Family
Group or family
Period

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

26. Describe how to read the periodic table:
Atomic Symbol:
One or two letters chosen to represent an element.
These symbols are used every where in the world
Usually, abbreviation of the element or the abbreviated Latin name of the element.

27. Describe how to read the periodic table:
Atomic Number
The number of protons in an atom identifies the element. 

28. Describe how to read the periodic table:
Atomic Mass:
The average mass of an element
Measured in atomic mass units ("amu”)
Is an average of all the isotopes of an element.
Mass Number:
protons + neutrons = Mass Number
Is always a whole number.

29. Atomic Structure

30. What are the 3 major parts of an atom?
Proton
Neutron
Electron

31. Protons Positively charged particles found in the atomic nucleus.
Have a mass of 1 AMU
Are made from other particles called quarks.

32. Neutrons Uncharged particles found in the atomic nucleus
Have a mass of 1 AMU
Made from other particles called quarks.

33. Electron
Negatively charged particles that surround the atom's nucleus.
Have no mass??
Determine properties of the atom.
Chemical reactions involve sharing or exchanging electrons.

34. Draw a Diagram of an Atom

35. A diagram showing the location of each part of the atom.

36. The Quark One of the basic building blocks of matter
Discovered in experiments done in the late 1960’s
There are Three families of quarks
Each family contains two quarks.

37. The Quark He Three Families: Consists of Up and Down quarks,
these quarks join together to form protons and neutrons.
Consists of Strange and Charm quarks
Exist only at high energies.
Consists of Top and Bottom quarks He

38. The Nucleus The central part of an atom
Composed of protons and neutrons
Contains most of an atom's mass
Discovered by Ernest Rutherford in 1911.

39. Some show the mass number and atomic number in nuclear symbol form
23 Na
atomic number
Atomic Symbols

40. Isotopes
Atoms that have the same number of protons but different numbers of neutrons

41. Describe Isotope Example:

42. Naturally occurring carbon consists of three isotopes, 12C, 13C, and 14C. State the number of protons, neutrons, and electrons in each of these carbon atoms.
12C C 14C
#p+ _______ _______ _______
#no _______ _______ _______
#e- _______ _______ _______

43. Answers
12C C 14C #p
#no #e

44. Some quick questions An atom has 14 protons and 20 neutrons.
A. Its atomic number is
1) ) ) 34
B. Its mass number is
C. The element is
1) Si 2) Ca 3) Se
D. Another isotope of this element is
1) 34X 2) 34X 3) 36X

45. 7 DIATOMIC MOLECULES
Elements that only exist as PAIRS.
Note: when they combine to make compounds, they are no longer elements so they are no longer in pairs!
Hydrogen, Nitrogen, oxygen, fluorine, chlorine, bromine, iodine

46. IONS
IONS are atoms or groups of atoms with a positive or negative charge.
Taking away an electron from an atom gives a CATION with a positive charge
Adding an electron to an atom gives an ANION with a negative charge.
To tell the difference between an atom and an ion, look to see if there is a charge in the superscript! Examples: Na+ Ca+2 I- O-2
Na Ca I O

47. Forming Cations & Anions
A CATION forms when an atom loses one or more electrons.
An ANION forms when an atom gains one or more electrons
F + e- --> F-
Mg --> Mg e-

48. PREDICTING ION CHARGES
In general
metals (Mg) lose electrons ---> cations
nonmetals (F) gain electrons ---> anions

49. Learning Check – Counting
State the number of protons, neutrons, and electrons in each of these ions.
39 K O Ca +2
#p+ ______ ______ _______
#no ______ ______ _______
#e- ______ ______ _______

50. A diagram showing the location of each part of the atom.