Memorize For SOL. Ionization Energy = lose or remove electrons

Transcription

1 Memorize For SOL Understanding The Periodic Table: Ionization Energy = lose or remove electrons Electronegativity = attract or steal electrons Atomic radius = Size Electron affinity = gain electrons Charge of Ions is equal to number of valence electrons needed to satisfy octet rule (lose or gain) Charge of ion is also called the oxidation number Cations Positively charged ion - groups 1-14 Group 3-12 (Transition elements) have a roman numeral to indicate charge (Three transition do not have roman numerals, because they never change = Zn+2, Cd+2, Ag+1) Anions Negatively Charged Ion - groups All Metals are left of the Stair-steps / All Nonmetals are to the right of the Stair-steps Alkali = Group 1 Alkaline Earth = Group 2 Transition = Group 3-12 Boron Group = Group 13 Carbon Group = Group 14 Nitrogen Group = Group 15 Oxygen Group = Group 16 Halogens = Group 17 Noble Gases = Group 18 Rare Earth Elements Lanthanides & Actinides

2 Atomic Number = Protons Atomic number = Electrons in neutral atom Mass number = Protons + Neutrons People: Dalton Atomic Theory (Elements are composed of like atoms) Rutherford Discovered atom is empty space (Gold foil experiment) Thompson Discovered electron (Cathode ray tube) Millikan Discovered mass of electron (oil drop experiment) Bohr Planetary model Chadwick Discovered neutron Bonding: Covalent = share electrons Ionic = Steal electrons = charged ions Polar = uneven distribution of electrons = hydrogen bonding in water Metallic = sea of electrons

3 Naming Compounds: These are the polyatomic ions you should remember You need to remember the base ions and you can figure out the other three columns if needed. The charge of the common ions don t change from column to column Per ate = 1 more oxygen Base ite = 1 less oxygen Hypo ite = 2 less oxygen Perchlorate = (ClO 4 ) -1 Chlorate = (ClO 3 ) -1 Chlorite = (ClO 2 ) -1 Hypochlorite = (ClO) -1 Carbonate = (CO 3 ) -2 Nitrate = (NO 3 ) -1 Phosphate = (PO 4 ) -3 Sulfate = (SO 4 ) -2 Hydroxide = (OH) -1 Ammonium = (NH 4 ) Two nonmetals together = covalent = use prefixes NO 2 = nitrogen dioxide 2. Acids = Ionic = Hydrogen plus something else = you must use charges Hydro ic acid = hydrogen plus one other element H +1 S -2 = switch numbers H 2 S = hydrosulfuric acid 3. Acids (non hydro) = Ionic = hydrogen plus polyatomic ion = you must use charges ate = ic acid Hydrogen + Sulfate ite = ous acid Hydrogen + Sulfite H +1 (SO 4 ) -2 = switch numbers H +1 (SO 3 ) -2 = switch numbers H 2 (SO 4 ) = sulfuric acid H 2 (SO 3 ) = sulfurous acid 4. Everything else = Metal + something else = ionic = you must use charges Metal + nonmetal = metal + ide Calcium + Chlorine Metal + polyatomic = Metal + ion name Calcium + Chlorate Ca +2 Cl -1 = switch numbers Ca +2 (ClO 3 ) -1 = switch numbers CaCl 2 = calcium chloride Ca(ClO 3 ) 2 = calcium chloride 5. Organic Acids Anything with a Carboxyl group attached (COOH)

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5 Molecular Geometry Linear = 1 atom attached to one atom (NaCl) OR 2 atoms attached with no lone pairs (CO 2 ) Bent = 2 atoms attached with no lone pairs on center (H 2 O) Trigonal Planer = 3 atoms attached to center with no lone pairs on center (COF 2 ) Pyramidal = 3 atoms attached to center with one lone pair on center (NH 3 ) Tetrahedral = 4 atoms attached to center (CH 4 ) Le Chatelier s Principle (Liquid + Heat Vapor) Add something to the left, reaction shifts right Add something to the right, reaction shifts left Remove something from the right, reaction shifts right Remove something from the left, reaction shifts left If heat is on the left side = Endothermic = positive increase in heat If heat is on the right side = Exothermic = negative change in heat High Entropy = more randomness = Positive change Low Entropy = less random and more stable = Negative change Rules For Significant Figures: 1) Zeros between nonzero digits are significant 2) Zeros in front of all nonzero are NOT significant 3) Zeros at the end of a number that has a decimal point are significant 4) Zeros at the end of a number without a decimal point are NOT significant Types of Reactions: 1) Synthesis A + B AB 2) Decomposition AB A + B 3) Single Replacement AB + C AC + B 4) Double Replacement AB + CD AD + CB 5) Combustion CxHy + O 2 CO 2 + H 2 O

6 Equations and Constants to Remember Density = mass ( grams) volume (milliliters) Molarity (M) = amount of substance (moles) volume of solution (liters) Molality (m) = Half-Life = amount of substance (moles) mass of solution (kilog rams) amount of original mass 2^(number of half lives) Percent Yield = experimental yield actual yield X 100 Percent Error = actual experimental actual X 100 Heat/Energy = Mass x Change In Temperature x Specific Heat (Q = m c ΔT) Specific Heat of Liquid Water = J g C Heat of Fusion = H f (Q = m H f ) Heat of Vaporization = H v (Q = m H v ) Gas Laws = Temperature must be in Kelvin Kelvin = Celcius Boyle s Law: P 1 V 1 = P 2 V 2 Charles Law: V1 = V 2 T1 T2 Gay-Lussac s Law: P1 T1 = P2 T2 Combined Gas Law: P1 V1 T1 = P2 V 2 T2 Avogadro s Gas Constant = 22.4 L = 1 mol Ideal Gas Law: PV = nrt (n = number of moles) (R = Gas Constant) Standard Temperature = 0 C Standard Pressure = 1 atm = 760 mmhg = 760 torr = kpa = 14.7 psi

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