Download chemistry review sheet

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