Chapter 4 Notes: The Periodic Table Mostly memorization no math involve

How would you organize the following items? 1) Organize, closet, computer and grocery store. If you are working at a hardware store (ACE, do it center, Lowes, Home depot) figure this task out (dairy, meat, cans etc..) Work with your table partner and ready to present to the class 2) How is the periodic table arranged? (students go to the board and write their lay out)

Chp 4-1 Periodic Law Periodic law - periodic table is organized based on the atomic #, chemical & physical properties of the elements Mendeleev is the creator of the periodic table used atomic mass 1st periodic table in 1869 arranged by mass

The Periodic Table Group Period A vertical columns Elements in a group share the same chemical properties Period A horizontal rows Elements in the same period have the same number of energy levels

The Periodic Table Elements’ chemical properties are determined by the number of valence electrons Valence electrons are electrons that are in the outermost energy level of an atom (in the S and P orbital)

Main Group Elements Transition Elements Inner Transition Elements

Main Group

Metals Properties

Metals Properties Most elements are metals They are good conductors of electricity Most are ductile (can be rolled into wire) and malleable (can be hammered or rolled into sheets) Can form alloys - solid or liquid mixtures of metals Talk about wires (landline, and internet) that are used as conductor – Expensive speakers with gold coating for better sounds (Beats by Dre headphones)

Check-In A = metals B = non metals C = metalloids Classify the following elements: 1.Na 2.H 3.C 4.Ca 5.Si 6.W

Alkali Metals Group 1 Highly reactive (easily combine with other elements) React with water to make alkaline (basic) solutions Will give away 1 valence electron Found in nature as compounds Electrolytes Lithium burns red and use in battery (lithium-ion) Potassium helps muscles contract

Alkaline Earth Metals Group 2 2nd most reactive group Found in nature in compounds Give away 2 v.e. Calcium build bones Magnesium deficient can lead to depression. Cerebral spinal fluid (CSF) magnesium has been found low in treatment-resistant suicidal depression patients

Transition Metals d and f blocks Most lanthanides and actinides (f-block) are radioactive. Generally less reactive than alkali and alkaline earth metals Do not have identical outer electron configurations Common metals that a person will think of (copper, iron, gold, silver, zinc)

Halogens Group 17 Gain 1 electron in reactions React with metals to form salts Halogens are non-metals Seven valence electrons making them highly reactive Halogens are oxidants (elements that grab electrons and mess up the cells in your body)

Noble Gases Group 18 Not reactive at all Eight valence electrons makes them very stable (outermost energy level is full) Also called inert gases because of their low reactivity

Hydrogen Most common element in the universe Found in many organic compounds Fuel source for the sun (nuclear fusion) Unlike all other elements Highly reactive

Chp 4-3 Periodic Trends Atomic radius Ionization energy Electronegativity Electron affinity

Periodic Trends Atomic Radius: The estimated distance from the nucleus to the outer most electrons Increases down a group As electrons energy levels are added, the nucleus becomes larger Decreases across a period # protons increases which pulled the v.e. closer to the nucleus

Atomic Radius Trend Radius decreases Radius Increases Radius decreases Based on the picture what trend do you see? In term of atomic size Radius decreases

Periodic Trends Ionization Energy - The energy required to remove one electron from an atom or ion Decreases down a group Electrons are farther from the nucleus and easier to remove Increases across a period Electrons are closer to the nucleus

Periodic Trends Electronegativity - the ability of an atom to attract electrons to itself Decreases down a group Increases across a period How many like to have a car or an A in chemistry? Decreases down a group because the radius is too big, harder to attract electrons

Periodic Trends Electron Affinity - the energy change that occurs when an electron is added to a neutral atom Decreases down a group Increases across a period

Example Consider the following elements: Na, Al, P, Cl Largest and smallest radius? Highest electronegavity? Largest radius = Na smallest = Cl Highest electronegavity = Cl

Fill in your periodic table Color and label each of these: Main-group metals Transition metals Lanthanides and Actinides Nonmetals Noble Gases Metalloids Label with arrows each of these trends: Atomic Radius Ionization energy Electronegativity Electron affinity Reactivity (this is different on each side of the PT)