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 |
