The Periodic Table (Your new best friend!!)

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.

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.

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)

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

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

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

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

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

Period The Periodic Table Group or Family Group or family Period

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

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.

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: http://www.learner.org/interactives/periodic/groups2.html

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

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.

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

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

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

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

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

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

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

Period The Periodic Table Group or Family Group or family Period

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

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.

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

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.

Atomic Structure

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

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

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

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.

Draw a Diagram of an Atom

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

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.

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

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.

Some show the mass number and atomic number in nuclear symbol form 23 Na atomic number 11 Atomic Symbols

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

Describe Isotope Example: http://education.jlab.org/glossary/isotope.html

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 13C 14C 6 6 6 #p+ _______ _______ _______ #no _______ _______ _______ #e- _______ _______ _______

Answers 12C 13C 14C 6 6 6 #p+ 6 6 6 #no 6 7 8 #e- 6 6 6

Some quick questions An atom has 14 protons and 20 neutrons. A. Its atomic number is 1) 14 2) 16 3) 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 16 14 14

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

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

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 --> Mg2+ + 2 e-

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

Learning Check – Counting State the number of protons, neutrons, and electrons in each of these ions. 39 K+ 16O -2 41Ca +2 19 8 20 #p+ ______ ______ _______ #no ______ ______ _______ #e- ______ ______ _______

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