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Chem chapters 1-3
Chem
| Question | Answer |
|---|---|
| writing the formula for ionic compounds (polyatomic modifications) | per....ate (evern more O in formula/add 1 O) .....ate (more O in formula- should have these memorized, Polyatomic ions flashcards - Blessed Rectangle 9) .....ite (fewer O in formula/ remove 1 O) hypo.....ite (even fewer O in formula / remove 2 O) |
| hydrate def | a compound in which water molecules are chemically bound to another compound or an element. |
| why are hydrates generally ionic | ionic compounds have both a canion and anion & H2O molecules are polar ionic compound + H2O, = hydration shell (water molecules surround the ions) + ions attract the oxygen end of the water molecules, and the - ions attract the hydrogen ends |
| how to write the formula for hydrates | ionic compound🟢___H20 blank = moles of H2O |
| how to write the names of hydrates | (ionic cmpound name as normal) prefixHYDRATE prefix = the number of moles of water in the compound |
| def oxyacids/oxoacids | a type of acid that conatins hydrogen, oxygen, and at least one other element |
| naming an acid (polyatomic modifications) | (oxyacids) (p. 44) the name of the acid is based on the new (not H or O) element or polyatomic ion ate ending becomes ic and ite becomes ous per and hypo stay the same -put acid after the name (modified-name acid ) |
| HCl (g) VS HCl (aq) | HCl(g) = covalent, not an acid in that state. HCl(aq) = strong acid, fully ionized into H₃O⁺ and Cl⁻. |
| why are acids only acids when aqueous/in water | Arrhenius def: acids must product H+ ions when dissolved in H2O -“acid” is defined by its ability to donate protons (H⁺), and without a solvent to accept the proton, it stays intact. strong acids fully dissociate but weak only parcially |
| limiting reactant | the reactant that runs out first |
| how to find the limiting reacant | 1. balanced equation 2. change reactant g to mol 3. convert mol of each reactant to mol of a product- stoiciometry (all products work, they're all limited by the same reactant) answer: _____ is limiting, ____ is excess |
| after finding the limting reactant, how do you know how many moles are going to be produced | the moles of the limiting reactant is the answer |
| you have a balanced equation and you are given the moles of each reactant. find which is limiting | ?????? |
| after finding the limiting reactant, determine how much excess of the other reactant there will be | start with g of the limiting reactant, change to mol, stoiciometry (mol of limiting ---> mol of other reactant), change other to g, what you found is the amount of the other consumed. Subtract this from the g of other u started w/ and BOOM |
| what is percent yield | A comparison of the accutal amount produced Vs the theoretic amount produced how much product you produce when a reaction occurs VS how much product you were supposed to get (theoretical amount) |
| percent yield formula | actual/theoretical x 100 = ____ % Yield |
| why is percent yield typically less than 100 percent (1) | 1. equalibrium will naturally stop the reactants from makeing the max amount of product becuase the reaction will reverse the reactant will alawys be present |
| why is percent yield typically less than 100 percent (2) | 2. a system can't sit entirely at products cause that would be too ordered. Entropy won't allow it, even if enthalpyf avors the products |
| given the grams of the limiting reactant, the acctual yield of the reaction, and a balanced equation, find the percent yield | start withe grams of the limiting reactant, convert to moles, use stoiciometry (moles of limitng to moles of product), conver moles of product to grams this is the theoretical yield then plug into formula |
| empirical formula def | simplest whole-number ratio of atoms of each element in the compound. It doesn't necessarily represent the actual number of atoms, but rather the simplest ratio. |
| calculating empirical formulas from % | 1. how many grams of each element are in 100g of the compound (take off the % symbol) 2. convert grams into moles of each element 3. divide the moles by the lowest # of moles (mole ratio) 4. round to whole number of write the formula NO DIATOMICS |
| molecular formula | actual formula of a compound -gives the composition of the molescules that are present |
| calculate the molecular formula from the empirical formula | 1. calculate the molar mass of the EF 2. divide the given molar mass by step one (finds a whole number that respresents how many times the EF needs to be increased) 3, multiply the subscripts of EF by the number found in step two |
| solving for the empirical formula | 1. change grams to moles (no diatomics) 2. mole to mole ratio (don't rounf in AP! multiply the decimals until you get all whole numbers, what you do to one do to the rest of them) |
| molar mass VS molecular mass VS atomic mass VS 6.022 x 10^23 | 1. mass of 1 mole of a substance (g/mol) 2. mass of one molecule (no units) 3. mass of a single atom of an element 4. number of particles in 1 mol of a substance |
| beer lambert law def | describes the relationship between the absorption of light by a substance and its properties the amount of light it absorbs is relative to the concentration of the chemical more concentrated ---> more color & less light can pass/ more absorption |
| in a mixture of chemical species, what can determine the structure and concetration in a mixture of chemical species | spectroscopy |
| in a mixture of chmical species, what can spectroscopy determine | the structure and concentration |
| beer-lambert equation | A = ε b c |
| what the beer-lambert equation means | A = absorbence, amount of light absorbed ε = constant for the particular chem. -molar absorbtivity: how well it absorbs that particular color of light b = path length, width of test tube/distance light travels through chem. c = concentration (molarity) |
| beer-lambert equation, patterns | b & c are proportional to the # of absorbing species (particles in solution that absorb light at given wavelength). the more absorbing molecules light encounters (increasing c or b), greater the A. A is directly prop. to b & 𝑐, but b & 𝑐 are not prop. |
| molar absorptivity def | molar absorptivity: how intensly a sample of molecules or ions absorbs light of a specific wavelength. |
| in most expieriments, what is the pattern | the path length and wavelength of light are constant therefore, the absorbance is proportional only to the concentration of absorbing molecules or ions |
| covalent naming memorize prefixes (page 43) | |
| oxide def | a chemical compound that includes at least one oxygen atom and one other element. |
| how to order elements in your answer for organic compounds | C 1st, then H, then the remaining elements in alphabetical order |
| Why cant you solve for g of O using proportions: A 4.000 g sample of a compound containing carbon, hydrogen, and oxygen is combusted. The combustion produces 5.760 g of CO2 and 2.400 g of H2O. Determine the empirical formula of the compound. | the oxygen in the products (H2O and CO2) come from 2 places: the original compound and the O used for combustion you dont usually know how much O2 reacted, |
| REMINDER, when calculating the empirical formula, when you divide, EVERYTHING MUST BE IN MOLES dont divide when everything is in g because elvery compound or element has a different molar mass | |
| when to put hydro----- in the beginging of an acid | "hydro-" is used exclusively for binary acids, which are acids containing hydrogen and only one other element so for oxyacids, this prefix is never used The prefixes "hypo-" and "per" are used for oxyacids |
| how to find the fomrula of a hydrate when given the formula of the anahydrous salt, the grams of the hydrate, and the grams of the anahydrous salt | find grams of water. change grams of anahydrous salt and water into moles. divide by the lowest number, thats the moles of each substance |
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Blessed Rectangle 10