General Help – Flashcards
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| NH4+ |
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| Ammonium/ Cation |
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| H3O+ |
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| Hydronium/ Cation |
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| Hg22+ |
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| Mercury(I)/ Cation |
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| OH- |
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| Hydroxide/ Diatomic Anion |
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| CH3CO2- |
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| Acetate/ Anion with Carbon |
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| CO32- |
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| Carbonate/ Anion with Carbon |
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| CN- |
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| Cyanide/ Diatomic Anion |
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| C2O42- |
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| Oxalate/ Anion with Carbon |
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| SO4- |
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| Sulfate/ Oxoanions |
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| SO32- |
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| Sulfite/ Oxoanions |
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| NO3- |
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| Nitrate/ Oxoanion |
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| NO2- |
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| Nitrite/ Oxoanion |
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| PO43- |
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| Phosphate/ Oxoanions |
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| MnO4- |
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| Permanganate/ Oxoanion |
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| CrO42- |
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| Chromate/ Oxoanion |
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| Cr2O72- |
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| Dichromate/ Oxoanion |
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| ClO4- |
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| Perchlorate |
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| ClO3- |
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| Chlorate |
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| ClO2- |
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| Chlorite/ Oxanions |
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| ClO- |
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| Hypochlorite/ Oxoanions |
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| Hydrogen 1 (alkali) |
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| H / 1.008 (+1) |
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| Helium 2 (Noble Gas) |
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| He/ 4.003 |
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| Lithium 3 (Alkali) |
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| Li/ 6.941 (+1) |
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| Beryllium 4 (Alkaline Earth) |
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| Be/ 9.012 (+2) |
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| Boron 5 (Metalloid) |
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| B/ 10.81 (+3) |
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| Carbon 6 (Non metal) |
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| C/ 12.01 (+-4) |
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| Nitrogen 7 (Non metal) |
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| N/ 14.01 (-3) |
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| Oxygen 8 (Non metal) |
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| O/ 16.00 (-2) |
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| Fluorine 9 (Non metal) (diatomic) |
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| F / 19.00 (-1) |
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| Neon 10 (Noble Gas) |
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| Ne/ 20.18 |
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| Sodium 11 (Alkali) |
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| Na/ 22.99 (+1) |
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| Magnesium 12 (Alkaline Earth Metal) |
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| Mg/ 24.31 (+2) |
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| Aluminum 13 (Metalloid) |
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| Al/ 26. 98 (+3) |
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| Silicon 14 (Metalloid) |
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| Si/ 28.09 (+-4) |
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| Phosphorous 15 (Non metal) |
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| P/ 30.97 (-3) |
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| Sulfur 16 (non metal) |
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| S/ 32.07 (-2) |
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| Chlorine 17 (non metal) |
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| Cl/ 35.45 (-1) |
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| Argon 18 (noble) |
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| Ar/ 39.95 |
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| Potassium 19 (Alkali) |
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| K /39.10 (+1) |
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| Calcium 20 (Alkaline)) |
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| Ca 40.08 (+2) |
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| Scandium 21 Transition |
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| Sc/ 44.96 |
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| Titanium 22 Transition |
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| Ti/ 47.88 |
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| Vanadium 23 Transition |
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| V/ 50.94 |
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| Chromium 24 Transition |
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| Cr/ 51.99 |
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| Manganese 25 Transition |
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| Mn/ 54.94 |
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| Iron 26 Transition |
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| Fe/ 55.85 (+2, +3) |
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| Cobalt 27 Transition |
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| Co/ 58.93 |
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| Nickel 28 Transition |
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| Ni/ 58.69 |
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| Copper 29 Transition |
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| Cu/ 63.55 (+1, +2) |
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| Zinc 30 Transition |
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| Zn/ 65.39 (+2) |
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| Gallium 31 |
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| Ga/ 69.72 (+3) |
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| Germanium 32 Metalloid |
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| Ge/ 72.61 (+-4) |
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| Arsenic 32 Metalloid |
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| As/ 74.92 (-3) |
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| Selenium 33 Metalloid |
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| Se/ 78.96 (-2) |
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| Bromine 35 Halogen |
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| Br/ 79.90 (-1) |
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| Krypton 36 Noble |
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| Kr/ 83.80 |
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| Rubidium 37 Alkali |
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| Rb/ 85.47 (+1) |
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| Strontium 38 Alkaline |
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| Sr/ 87.62 (+2) |
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| yttrium 39 Transition |
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| Y/ 88.91 |
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| zirconium 40 Transition |
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| Zr/ 91.22 |
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| Niobium 41 Transition |
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| Nb/ 92.91 |
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| Molybdenum 42 Transition |
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| Mo/ 95.94 |
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| Technetium 43 Transition |
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| Tc/ 98 |
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| Ruthenium 44 Transition |
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| Ru/ 101.07 |
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| Rhodium 45 Transition |
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| Rh/ 102.91 |
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| Palladium 46 Transition |
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| Pd/ 106.42 |
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| Silver 47 Transition |
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| Ag/ 107.87 (+1) |
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| Cadmium 48 Transition |
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| Cd/ 112.41 |
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| Indium 49 |
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| In/ 114.82 (+3) |
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| Tin 50 Metalloid |
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| Sn/ 118.71 (+2, +4) |
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| Sig Fig Rules |
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| 1. All non-zero digits are significant 2. Zeros between 2 sig figs are significant 3. Zeros at the beginning are NEVER significant. 4. Zeros at the end of a number are significant only if a decimal point is written in the number. |
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| Addition + Subtraction Rule with Sig Figs |
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| Round to the least significant decimal place (farthest to the left) |
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| Division and Multiplication with Sig Fig |
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| Round to the least number and the sig fig it has. 32cm-> 3.2E1cm |
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| Sig Figs with Scientific Notation |
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| Round first to sig figs, then put in notation form. |
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| Hydrates |
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| Compounds that have water trapped in the crystal lattice. |
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| Empirical Formula |
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| The atom ratio is the simplest possible whole number ratio. |
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| Molecular Formula |
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| True number of atoms of each kind in a molecule. Obtained by multiplying the empirical number by a whole number. Only molecules have molecular. |
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| Stoicheometry Coefficients |
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| Give the relative number of molecules or moles involved in a reaction. |
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| Rules for writing net ionic equations |
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| 1. Write balanced molecular equation. 2. Dissociate all ions 3. check for precipitates 4. Cross out all spectator ions 5. Write the net ionic equation with the species remaining. |
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| Arrhenius Acids |
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| Substances that give up protons in aqueous solutions |
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| Bronsted Lowry Acids |
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| Proton Donors |
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| Oxidation Rules |
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| 1. Elements in their most stable form =0 2. the oxidation # of a monotamic ion is the same as its charge. 3. Oxygen has an oxidation number of -2 except in peroxides. 4. hydrogen is -1 with a metal, +1 with a nonmetal. 5. Halogens have an oxidation number of -1 in binary compounds (F is always -1) 6. Halogens have varying oxidation numbers in polyatomic anions (e.g. in oxyanions, they can have a positive charge). |
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| The sum of the oxidation numbers |
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| Equal 0 in a neutral compound |
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| Displacement Reactions |
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| Often involve metal solids that react with acid or metal salt. A(s)+BX(aq)->AX(aq)+B |
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| Dissociate completely |
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| Strong Acids |
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| Partially Dissociate in Water |
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| Weak Acids |
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| Arrhenius Base |
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| Substances that increase OH- when dissolved |
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| Bronsted Lowry Base |
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| Proton acceptors |
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| Some Strong Bases |
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| All Alkali Metals Calcium Hydroxide Strontium Hydroxide Barium Hydroxide |
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| Titration |
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| Analytical technique used to calculate the concentration of a solute in a solution. |
