By the end of the class period today, I will be able to…. Describe the structure of periods and groups on the periodic table Identify the location of chemical families, metals, nonmetals, and states of matter on the periodic table

Quick Review!

Rows (periods): elements are put in rows by increasing atomic number Columns (groups): elements are put into columns (groups) based on how they react (chemical properties)

Metals ◦Metals are elements found on the left side of the “steps” of the Periodic Table (except for Hydrogen). ◦Metals are shiny, ductile, malleable, good conductors, and have high melting points. Ductile – Ability to be drawn into wire Malleability – ability to be hammered into a thin sheet

Nonmetals ◦Nonmetals are elements found on the right of the “steps” of the Periodic Table. ◦Nonmetals are brittle, lackluster, and poor conductors.

Metalloids ◦Metalloids share characteristics of both metals and non-metals giving them special properties ◦These elements are located along the “steps” of the Periodic Table (except for Aluminum). ◦Often make good semi-conductors.

Noble Gases

We are Family… Take three minutes and think about your immediate family (mom, dad, brothers, sisters) On one side of a T chart write 2 characteristics that everyone in your family shares On the other side of a T chart write 2 characteristics that you do not share with any other member of your family

Column = Group = Family Elements in a group are like members of a family-each is different, but all are related by common characteristics. Knowing an element’s group can help us predict its properties and how it will react. Is like….

Keep in mind: the Periodic Table is arranged by trends

Alkali Metals Physical Properties: solids, silvery appearance, soft, shiny Chemical Properties: undergo chemical changes easily and sometimes violently (especially water) MOST important fact: the most reactive metal group on the periodic table don’t occur in nature in their elemental form

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Alkaline Earth Metals Physical Properties: solids, metallic, harder, denser, and stronger than alkali metals Chemical Properties: second most reactive metal group MOST important fact: less reactive than alkali metals, but too reactive to be found as free elements

Transition Metals Physical Properties: very hard, high boiling point, high electrical conductivity, malleable Chemical Properties: less reactive than group 1 and 2 metals MOST important fact: occur in nature in elemental form

Halogens Physical Properties: nonmetals, diatomic molecules Chemical Properties: very reactive, especially with alkali metals and alkaline earth metals MOST important fact: most reactive group of nonmetals

Noble Gases Physical Properties: gases at room temperature, when excited many of the noble gases give off light How do they react: Do not naturally react MOST important fact: the most stable group on the periodic table (exist in elemental form)

Row Races I will display an element symbol on the board. You will pass an answer sheet around your group.

I

Mg

Ar

Valence Electron The electrons in the outermost shell of an atom The electrons in the outermost shell of an atom The electrons that are available to be lost, gained, or shared in the formation of chemical compounds The electrons that are available to be lost, gained, or shared in the formation of chemical compounds Valence Electrons determine the chemical properties of elements

Noble Gases

Quick Check! Write the number of valence electrons for the following elements: NPoNeCa Write the outer shell number of the following elements: NPoNeCa

Quick Check! Write the number of valence electrons for the following elements: N5Po6Ne8Ca2 Write the outer shell number of the following elements: N2Po6Ne2Ca4

Quick Check! Write the number of valence electrons for the following elements: KRuSeBe Write the outer shell number of the following elements: KRuSeBe

Quick Check! Write the number of valence electrons for the following elements: K1Ru1Se6Be2 Write the outer shell number of the following elements: K4Ru5Se4Be2

Octet Rule Chemical compounds tend to form so that each atom, by gaining, losing, or sharing electrons, has an octet of electrons in its highest occupied energy level