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MCAT Gen. Chem Ch. 2

TermDefinition
Periodic Table Of The Elements Organizes the elements according to their atomic numbers and reveals a pattern of similar chemical and physical properties among elements
Periods Rows on the Periodic Table, and are based on the principal energy level, n
Groups Columns on the Periodic Table. Elements in the same group have the same valence shell electron configuration.
Metals Are: Shiny (lustrous), conduct electricity well, and are malleable and ductile. Metals are found on the left side and the middle of the Periodic Table.
Nonmetals Dull, poor conductors of electricity and are brittle. Nonmetals are found on the right side of the Periodic Table.
Metalloids Possess characteristics of both metals and nonmetals. They are found in a stair-step pattern starting with Boron (B).
Effective Nuclear Charge (Zeff) Net positive charge experienced by electrons in the valence shell and forms the foundation for all periodic trends
Zeff Increases From: Left to right across a period with little change in value from top to bottom in a group.
As The Principle Energy Level, n, Increases From Top To Bottom In A Group: Valence electrons become increasingly separated from the nucleus
Atomic Radius Decreases from left to right across a period, and increases from top to bottom in a group.
Ionic Radius Size of a charged species. The largest nonmetallic ionic radii and the smallest metallic ionic radii exist at the metalloid boundary.
Cations Are Generally: Smaller than their corresponding neutral atom.
Anions Are Generally: Larger than their corresponding neutral atom.
Ionization Energy The Amount of energy needed to remove an electron from the valence shell of a gaseous species.
Ionization Increases From: Left to right across a period, and decreases from top to bottom in a group.
Electron Affinity Amount of energy released when a gaseous species gains an electron in its valence shell.
Electron Affinity Increases From: Left to right across a period and decreases from top to bottom in a group
Electronegativity Measure of the attractive force of the nucleus for electrons within a bond.
Electronegativity Increases From: Left to right across a period, and decreases from top to bottom in a group.
Alkali Metals Take on an oxidation state of +1 and prefer to lose an electron to achieve a noble gas-like config.
Alkali Metals And Alkaline Earth Metals Are: The most reactive of all metals.
Alkaline Earth Metals Take on an oxidation state of +2 and can lose two electrons to achieve noble gas-like configurations.
Chalcogens Take on oxidation states of -2 or +6 (depending on whether they are nonmetals or metals respectively) in order to achieve noble gas configuration. They are very biologically important.
Halogens Take on an oxidation state of -1 and prefer to gain an electron to achieve noble gas-like configurations. .
Halogens Have The: Highest electronegativities.
Noble Gases Have a fully filled valence shell in their standard state and prefer to not give up or take on additional electrons. They have very high ionization energies.
Noble Gase Such As He, Ne, And Ar: Have virtually nonexistent electronegativities and electron affinities
Transition Metals Unique because they take on multiple oxidation states, which explains their ability to form colorful complexes with nonmetals in solution and their utility in certain biological systems.
Created by: SamB91
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