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Chapter 4 Notes: The Periodic Table How would you organize the following items? 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 The Periodic Table Group 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 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 Alkaline Earth Metals Group 2 2nd most reactive group Found in nature in compounds Give away 2 v.e. Transition Metals d and f blocks Most lanthanides and actinides (f-block) are radioactive. Generally less reactive than alkali and alkaline earth metals 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 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 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 Increases Radius decreases 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 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? 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)