1st Test, Keller, Chem 105, UAF – Flashcards
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Acetate |
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CH_3_COO- |
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Ammonia |
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NH_3_, not an Ion |
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Ammonium |
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NH_4_^+ |
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Carbonate |
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CO_3_^2- |
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Chlorate |
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ClO_3_^- |
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Chlorite |
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ClO_2_^- |
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Chromate |
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CrO_4_^2- |
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Coulombic attraction |
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opposite charges attract hold atoms together |
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Cyanide |
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CN^- |
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Dihydrogen phosphate |
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H_2_PO_4_^- |
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G (Giga) |
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10(9) (1,000,000,000) |
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Heterogenous |
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all different |
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Homogenous |
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all the same |
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Hydrogen Carbonate |
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HCO_3_^- |
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Hydrogen phosphate |
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HPO_4_^2-PO43- |
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Hydrogen sulfate or Bisulfate |
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HSO_4_^- |
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Hydroxide |
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OH^- |
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Intensive properties |
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independent of the amount |
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Ions |
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different number of electrons |
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Isotopes |
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different number of neutrons |
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M (mega) |
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10(6) 1,000,000 |
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Metals with More Than One Oxidation State |
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If you are naming a metal cation that has more than one oxidation state, use a Roman numeral in the name. |
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Nitrate |
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NO_3_^- |
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Nitrite |
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NO_2_^- |
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Nomenclature of Binary Ionic Compounds |
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Cation name = name of element. Anion name = element name with the ending replaced by the suffix "ide". Compound name = cation name + anion name Compound Charge = 0 |
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Nomenclature of Ionic Compounds with Oxo Anions |
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Ionic compounds are named by stating the cation name and then the anion name. Oxo anions always have the suffix 'ate' or 'ite'. |
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Number Prefix 1 |
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mono |
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Number prefix 10 |
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deca |
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Number prefix 2 |
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di |
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Number prefix 4 |
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tetra |
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Number prefix 5 |
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penta |
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Number prefix 6 |
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hexa |
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Number prefix 7 |
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hepta |
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Number prefix 8 |
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octa |
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Number prefix 9 |
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nona |
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Phosphite |
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PO_3_^3- |
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Standard Deviation |
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Find average, find difference from each number from the average, average those, and take the square roots |
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T (Tera) |
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10(12) (1,000,000,000,000) |
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centi |
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1/100 |
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deci |
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1/10 |
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density |
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Mass divided by volume M/V |
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extensive properties |
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depends on the amount |
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femto |
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10^-15 |
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k (kilo) |
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10(3) 1000 |
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kilo |
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10^3, 1000 |
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m (milli) |
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10(-3) |
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micro (u) |
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10^-6 |
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milli |
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10^-3 |
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n (nano) |
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10(-9) |
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nano meters nm |
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10^-9 |
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number prefix 3 |
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tri |
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p (pico) |
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10(-12) |
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phosphate |
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PO_4_^3- |
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pico |
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10^-12 |
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sulfate |
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SO_4_^2− |
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sulfite |
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SO_3_^2- |
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µ (micro) |
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10(-6) |
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sodium (Na+) salts |
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Soluble |
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Potassium (K+) salts |
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Soluble |
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Ammonium (NH4+) salts |
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Soluble |
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Nitrate (NO3-) salts |
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SOLUBLE. |
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Acetate (CH3CO2-) salts |
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SOLUBLE. |
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Chlorate (ClO3- ), and perchlorate (ClO4-) salts |
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SOLUBLE. |
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chloride (Cl-) salts |
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SOLUBLE -- EXCEPT those also containing: lead, silver, or mercury (I) (Pb2+,Ag+, Hg22+) which are NOT soluble. |
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bromide (Br-)salts |
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SOLUBLE -- EXCEPT those also containing: lead, silver, or mercury (I) (Pb2+,Ag+, Hg22+) which are NOT soluble. |
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iodide (I-) salts |
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SOLUBLE -- EXCEPT those also containing: lead, silver, or mercury (I) (Pb2+,Ag+, Hg22+) which are NOT soluble. |
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Sulfate (SO4^2-) salts |
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SOLUBLE - - EXCEPT those also containing: hydrogen, calcium, silver, mercury (I), strontium, barium, or lead (Ca2+, Ag+, Hg22+, Sr2+, Ba2+, Pb2+) which are NOT soluble. |
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Hydroxide (OH-) compounds |
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NOT SOLUBLE -- EXCEPT those also containing: sodium, potassium, or barium (Na+, K+, Ba2+) which are soluble. |
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oxide (O2-) compounds |
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NOT SOLUBLE -- EXCEPT those also containing: sodium, potassium, or barium (Na+, K+, Ba2+) which are soluble. |
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Sulfide (S2-) salts |
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NOT SOLUBLE -- EXCEPT those also containing: sodium, potassium, ammonium, or barium (Na+, K+, NH4+, Ba2+) which are soluble. |
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Carbonate (CO32-) salts |
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NOT SOLUBLE -- EXCEPT those also containing: sodium, potassium, or ammonium (Na+, K+, NH4+) which are soluble. |
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phosphate (PO43-) salts |
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NOT SOLUBLE -- EXCEPT those also containing: sodium, potassium, or ammonium (Na+, K+, NH4+) which are soluble. |
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Writing Net Ionic Equations |
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1. Write reactants. 2. Write products by exchanging cations. 3. Dissociate (write as ions) ALL soluble salts, strong acids, and strong bases (except Ca(OH)2) Reminder: Do not break up polyatomic ions i.e.) K_2_SO_4_ --> 2 K^+ + SO4^2- NOT S2- + 4 O2- 4. Balance. 5. Cross out identical (spectator) ions on both sides of the equation. 6. Rewrite NET IONIC EQUATION. CHECK atom and charge balance. |
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Binary Acid Nomenclature |
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There are two ways to name these compounds: 1. Molecular Name : Hydrogen + anion name 2. Acid Name : Hydro ____ ic acid. Used for aqueous solutions of the compound. |
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HCN |
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hydrocyanic acid or hydrogen cyanide |
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HCl |
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hydrogen chloride |
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HCl (aq) |
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hydrochloric acid |
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HBr |
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hydrogen bromide |
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HI |
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hydrogen iodide |
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HBr (aq) |
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hydrobromic acid |
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HI (aq) |
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hydroiodic acid |
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Strong Binary Acids |
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HCl, HBr, HI |
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HF |
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hydrogen fluoride |
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HF (aq) |
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hydrofluoric acid |
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H_2_S |
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hydrogen sulfide |
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H_2_S |
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hydrosulfuric acid |
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Weak Binary Acids |
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HF, H_2_S, HCN |
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Oxo Acid Nomenclature |
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ate anions form ic acids. HNO3 = nitric acid ite anions form ous acids. HNO2 = nitrous acid |
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Ate acid |
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ic |
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Ite acid |
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ous |
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6 strong acids |
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HCl, HBr, HI, HNO3, HClO4, H2SO4 |
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Strong Acids and Strong Bases in aqueous solution |
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ionize 100% |
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Assigning Oxidation Numbers Atoms in their elemental state |
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Percent Yield |
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real/theoretical * 100 |
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Strong Bases |
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LiOH, NaOH, KOH, Ca(OH)2 slightly soluble, Ba(OH)2, Sr(OH)2 |
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"Filling up" or Aufbau Principle |
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Electrons go into the lowest energy orbitals first. |
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Pauli Principle |
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A maximum of 2 electrons can occupy an orbital. When 2 electrons occupy the same orbital, they must have paired spins, (or "ud" using our notation). |
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Hund's Rule |
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When filling p or d orbitals with the same energy, electrons go into separate orbitals with parallel spins until all of the orbitals are occupied by one electron. Then they are paired. |
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Drawing Lewis Structures 1 |
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Write the skeletal structure (the arrangement of atoms within the molecule): Central atom = the atom with the lowest electronegativity (usually). Hydrogen is always a terminal atom (on the end). |
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Drawing Lewis Structures 2 |
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Count the total number of valence electrons: Group number for each element = # valence electrons. Add electrons for negatively charged ions. Subtract electrons for positively charged ions. |
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Drawing Lewis Structures 3 |
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Draw a bond between the central atom and each surrounding atom. Single bond = 1 pair of electrons |
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Drawing Lewis Structures 4 |
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Place lone pairs of electrons about each terminal atom to complete their octets. Octet = 4 electrons pairs around an atom (eight electrons) Hydrogen can only have 2 electrons. |
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Drawing Lewis Structures 5 |
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If there are more electrons left, place them as lone pairs on the central atom. This will sometimes lead to an "expanded octet" around the central atom. Expanded octet = five or six electron pairs around an atom. Only central atoms from the third period and above can have expanded octets. |
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Drawing Lewis Structures 6 |
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If the central atom has an incomplete octet, use the electrons from surrounding atoms to make double or triple bonds. Do not add electrons. "Borrow" them from surrounding atoms. Double bond = 2 pairs of electrons Triple bond = 3 pairs of electrons Only C, N, O, P, and S form multiple bonds. F and Cl do not form multiple bonds. |
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Drawing Lewis Structures 7 |
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Sometimes you just can't complete the octet for a central atom. If there is an odd number of electrons, give the central atom 7 electrons instead of 8. Boron and Beryllium just don't have enough electrons to go around and often have incomplete octets. |
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Aromatic hydrocarbons |
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characterized by having ring systems in which the bonding can be described as alternating single and double bonds. |
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aliphatic hydrocarbons |
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subdivided into alkanes, alkenes and alkynes. |
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Hydrocarbons |
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compounds that contain only the elements H and C. They can be divided into two classes: aliphatic and aromatic. |
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alkanes |
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each C atom is bonded to four other atoms and all bonds are single bonds. |
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alkene |
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contains a carbon-carbon double bond. |
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Alkyne |
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carbon-carbon triple bond. |
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sodium (Na+) salts |
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Soluble |
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Potassium (K+) salts |
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Soluble |
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Ammonium (NH4+) salts |
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Soluble |
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Nitrate (NO3-) salts |
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SOLUBLE. |
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Acetate (CH3CO2-) salts |
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SOLUBLE. |
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Chlorate (ClO3- ), and perchlorate (ClO4-) salts |
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SOLUBLE. |
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chloride (Cl-) salts |
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SOLUBLE -- EXCEPT those also containing: lead, silver, or mercury (I) (Pb2+,Ag+, Hg22+) which are NOT soluble. |
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bromide (Br-)salts |
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SOLUBLE -- EXCEPT those also containing: lead, silver, or mercury (I) (Pb2+,Ag+, Hg22+) which are NOT soluble. |
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iodide (I-) salts |
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SOLUBLE -- EXCEPT those also containing: lead, silver, or mercury (I) (Pb2+,Ag+, Hg22+) which are NOT soluble. |
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Sulfate (SO4^2-) salts |
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SOLUBLE - - EXCEPT those also containing: hydrogen, calcium, silver, mercury (I), strontium, barium, or lead (Ca2+, Ag+, Hg22+, Sr2+, Ba2+, Pb2+) which are NOT soluble. |
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Hydroxide (OH-) compounds |
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NOT SOLUBLE -- EXCEPT those also containing: sodium, potassium, or barium (Na+, K+, Ba2+) which are soluble. |
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oxide (O2-) compounds |
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NOT SOLUBLE -- EXCEPT those also containing: sodium, potassium, or barium (Na+, K+, Ba2+) which are soluble. |
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Sulfide (S2-) salts |
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NOT SOLUBLE -- EXCEPT those also containing: sodium, potassium, ammonium, or barium (Na+, K+, NH4+, Ba2+) which are soluble. |
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Carbonate (CO32-) salts |
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NOT SOLUBLE -- EXCEPT those also containing: sodium, potassium, or ammonium (Na+, K+, NH4+) which are soluble. |
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phosphate (PO43-) salts |
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NOT SOLUBLE -- EXCEPT those also containing: sodium, potassium, or ammonium (Na+, K+, NH4+) which are soluble. |
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Writing Net Ionic Equations |
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1. Write reactants. 2. Write products by exchanging cations. 3. Dissociate (write as ions) ALL soluble salts, strong acids, and strong bases (except Ca(OH)2) Reminder: Do not break up polyatomic ions i.e.) K_2_SO_4_ --> 2 K^+ + SO4^2- NOT S2- + 4 O2- 4. Balance. 5. Cross out identical (spectator) ions on both sides of the equation. 6. Rewrite NET IONIC EQUATION. CHECK atom and charge balance. |
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Binary Acid Nomenclature |
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There are two ways to name these compounds: 1. Molecular Name : Hydrogen + anion name 2. Acid Name : Hydro ____ ic acid. Used for aqueous solutions of the compound. |
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HCN |
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hydrocyanic acid or hydrogen cyanide |
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HCl |
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hydrogen chloride |
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HCl (aq) |
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hydrochloric acid |
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HBr |
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hydrogen bromide |
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HI |
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hydrogen iodide |
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HBr (aq) |
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hydrobromic acid |
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HI (aq) |
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hydroiodic acid |
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Strong Binary Acids |
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HCl, HBr, HI |
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HF |
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hydrogen fluoride |
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HF (aq) |
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hydrofluoric acid |
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H_2_S |
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hydrogen sulfide |
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H_2_S |
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hydrosulfuric acid |
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Weak Binary Acids |
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HF, H_2_S, HCN |
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Oxo Acid Nomenclature |
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ate anions form ic acids. HNO3 = nitric acid ite anions form ous acids. HNO2 = nitrous acid |
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Ate acid |
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ic |
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Ite acid |
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ous |
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6 strong acids |
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HCl, HBr, HI, HNO3, HClO4, H2SO4 |
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Strong Acids and Strong Bases in aqueous solution |
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ionize 100% |
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Assigning Oxidation Numbers Atoms in their elemental state |
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Percent Yield |
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real/theoretical * 100 |
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Strong Bases |
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LiOH, NaOH, KOH, Ca(OH)2 slightly soluble, Ba(OH)2, Sr(OH)2 |
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Gases (ie methane) in order |
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methane, ethane, propane, butane, pentane hexane, heptane, octane, nonane, decane |
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Linear |
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180? 0 or 3 extra sets |
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Triangular Planar |
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120? BF3 |
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Bent |
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<120? SO2 extra set |
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Tetrahedron |
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109.5? CH4 |
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Triangular Pyramidal |
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extra pair <109.5? NH3 |
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Bent |
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2 extra pair <109.5? H2O |
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Triangular Bipyramidal |
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90?, 120?, 180? PF5 |
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See-Saw |
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1 extra set 90?, 120?, 180? SF4 |
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T-shaped |
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2 extra set 90?, 180? ClF3 |
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Octahedral |
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90?, 180? SF6 |
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Square Pyramidal |
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extra pair 90?, 180? ClF5 |
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Square Planar |
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2 extra pairs 90?, 180? XeF4 |