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CHEMISTRY REVIEW SHEET - UNIT 3 Define period and family/group as it pertains to the periodic table Know the way to number periods and the 2 ways to number groups Know how many elements exist total, as well as how many exist naturally Describe the creation of the periodic table and know the scientists who are credited with it Based on what property or properties is our current periodic table assembled? Describe periodic trends (electronegativity, atomic radius, ionization energy, etc.) Know what the trends are and be able to explain WHY the most important ones exist Know relative mass and charge of electrons, protons, and neutrons (sub-atomic particles) – Which two account for almost all the mass in an atom? Do they have the exact same mass? What are the relative charges of each sub-atomic particle? Know the general structure of an atom and the location of sub-atomic particles in an atom – Which are found in the nucleus? Which are found outside of the nucleus? Isotopes – What similarities and differences do isotopes have? Realize that the mass listed on the periodic table is an average atomic mass including isotopes and know how to calculate it when given percent abundance Know how to find mass number, atomic number, number of protons, neutrons, and electrons for an atom of any element Classify elements as metals, nonmetals, and metalloids Know the names, locations, and general properties of different groups on the periodic table (alkali metals, alkaline earth metals, halogens, noble gases, transition metals, rare earth metals, lanthanides, actinides, main group elements, etc) Know the 4 physical properties of metals Describe properties of non-metals and metalloids Which elements exist naturally as liquids? As gases? As solids? Which elements exist as diatomic molecules? Triatomic? Tetratomic? Octatomic? Determine the number of valence electrons in a main group (A group) element’s atoms Why are noble gases so unreactive? Explain electron configuration, including principal quantum numbers (aka principal energy levels), sublevels, orbitals, and spin Know the primary rules or principles that affect and determine electron configurations or orbital Notations (Aufbau principle, Pauli exclusions principle, Hund’s rule) Be able to correctly write both unabbreviated and abbreviated electron configurations Predict what type of bond will be formed between atoms Know how to write formulas for and name ionic compounds – always criss-cross charges Simple or binary ionic compounds - a metal and a non-metal Ionic compounds containing a transition metal - a transition metal and a nonmetal – use Roman numerals for charge of cation when writing the name Ionic compounds containing a polyatomic ion – use parentheses around polyatomic ion after criss-crossing if the subscript is more than 1 Know how to go from “per ate” to “ ate” to “ ite” to “hypo ite” as the polyatomic anion loses one O atom Know how to write formulas for and name covalent compounds – use prefixes – no criss-crossing because the atoms are not ions Know how to write formulas for and name acids – three rules (“-ate””-ic acid”, “-ite””-ous acid”, “-ide” or binary acid ”hydro ic acid”) Classify a compound as ionic or covalent – ionic always has a cation and an anion and involves an exchange of electrons, covalent is always two non-metals or a metal and a non-metal that share electrons Classify a compound as an acid or base – acids start with one or more H’s (hydrogen ion), bases end in OH (hydroxide ion) Compare and contrast the properties of covalent and ionic compounds Classify a compound as nonpolar covalent, polar covalent, or ionic based on electronegativity differences