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BioChem 1100.tri-c
Chapt. 5-Timberlake
| Question | Answer |
|---|---|
| Chemical Changes | Occurs when atoms of initial substance rearrange to form new substances. |
| Mole | 6.02 x 10 23 power - Avagadro's number |
| Actual yield | Actual amount of product produced by a reaction |
| Coefficients | Whole number placed in front of the formulas to balance the # of atoms/moles/elemnts of both sides of the equation |
| combination reaction | A reaction in which reactants combine to form a single product |
| decomposition reaction | A reaction in whcih a single reactant splits into two or more simpler substances |
| Double replacement reaction | A reaction in which parts of the two different reactants exchange places |
| Excess Reactant | The reactant that remains when the limiting reactant is used up in a reaction |
| formula unit | The group of ions represented by the formula of an ionic compound Ex. 1 mole of CO2, a covalent compound, contains one mole of the "formula unit" or atoms of this compound |
| limiting reactant | The reactant used up during a chemical reaction, which limits the amount of product that can form |
| Molar mass | The mass in grams of 1 mole of an element--EQUAL NUMERICALLY to atomic mass |
| Oxidation | The loss of electrons by a substance. |
| Biological oxidation | May involve the addition of oxygen, or the loss of hydrogen |
| LEO the lion goes GER | Loss of Electrons is Oxidation - Gain of Electrons is a reduction |
| Percent yield | The ratio of the ACTUAL yield a reaction to the THEORETICAL yield possible for the reaction - multiplied by 100 |
| REDUCTION (the contra-intuitive chemical definition) | Means a GAIN of electrons |
| Single replacement reaction | An element replaces a different element in a compoun |
| + Delta sign (triangle) arrow -what do these mean in chemical equations | + means "added to" Delta - means heat used - Arrow--means "reacts to form products" |
| Balance equations-4 steps | 1. Write correct formulas for reactants and products 2. COUNT atoms of each element in reactants and products 3. Use coefficients to balance each element 4. CHECK equation |
| Write/count/co-efficients/CHECK | Remember 4 steps for balancing equation: write correct formulas, COUNT atoms, BALANCE coefficients, Write a "check" -your atomic bank account is balanced!!! |
| How to Calculate # of Atoms/Moleculas in substance (4 steps) | 1.) Determine given number of moles 2. Write plan to convert moles to atoms/molecules 3. Use Avogadro's number to write conversion factors 4 set up problem |
| MOLES under/over 4 steps | 1. # moles 2. Moles under or over (moles under when needed to cance, over when needed to multiply 3. Use 6.02 x 10 - 23rd power 4. Do the math |
| Molar mass - where do you find? | Atomic weight is numerically equal to molar mass Ex. Carbon has atomic weight of 12.01 g; therefore 6.02 x 10 23rd power of C atoms has a molar mass of 12.01 grams |
| Calculate molar mass of compound | Don't "whack-a-mole" just "add-a-mole" 1 Determine # of grams/moles for each elements 2.write grams over moles 3. multiply # of grams times atomic weight 4. add together for molar mass/atomic weight of compound Ex. 1 mole NaF weighs 42 grams |
| Convert mass of a compound to moles Ex. 737 grams NaCL to moles | Remember: molar mass of NaCl is the sum of the masses of each element; one mole NaCl =58.5 g 3. Multiply 737 g NaCl by 1 moleNaCl/58.5 g NaCL - answer: 12.6 moles NaCl |
| Law of Conservation of Mass | There is no change in the total mass of substances reacting in a chemical mass |
| Mole-Mole Factors | A ratio of the moles for any two substances in an equation |
| Percent Yield (equation) | Percent Yield = actual yield(g)/theoretical yield (g) x 100 |
| Percent Yield (cookie example) | Theoretical yield: 60 cookies, but 12 cookies burned; therefore actual yield was 48 cookies. 48 cookies x100/divided by 60 cookies = 80% yield |
| Limiting Reactant | In chemical reaction, limiting reactant gets used up first, stops reactant |
| Limiting Reactant Ex. peanut butter/bread | Sandwiches--if you run out of bread, then it is "limiting factor" |
| Polyatomic Ions for Carbon (4) | 1. Carbonate - CO3 (2- charge); 2. Hydrogen carbonate (or bicarbonate) HCO3 (- charge) 3. Cyanide CN(- charge) 4. acetate C2H3O2(- charge) |
| Sulfur Polyatomic Ions (4) | Sulfate - SO4(2- charge) 2.Hydrogen sulfate (or bisulfate) HSO4(- charge) 3. Sulfite SO3(-2 charge) 4. HSO3(-charge) |
| Phosphorus Polyatomic Ions | 1. Phosphate PO4(3-) 2. Hydrogen phosphate HPO4(-2) 3. DiHydrogen phosphate H2PO4(- charge) 4. Phosphite PO3(-3charge) |
| Chlorine Polyatomic Ions-2 | Chlorate ClO3(-charge) 2. Chlorite ClO2(-charge) |
| Nitrogen Polyatomic Ions-3 | 1. Nitrate NO3(-charge) 2. Ammonium NH4(+ charge) 3. Nitrite NO2(- charge) |
| What is ending for most polyatomic ions | ATE |
| What polyatomic ion has a positive charge? | Ammonium - NH4(-charge) |
| Polyatomic ions - general characteristics | Most a.) are nonmetals bonded to oxygen atoms 2. have -1,-2 or -3 charge because electrons were added to complete octets ONly one has a positive charge (ammonium NH4) |
| Polyatomic ion with sulfur (given by Dr. Belle) | Thiocyanate SCN(-charge) |
| How to calculate charges for polyatomic ions formulas | |
| Which is most electronegative element? | Fluorine (in group 7A - 1 valence electron) |
| Do metals or nonmetals have higher electronegativity?? | Nonmetals - because they have a greater attraction for electrons than metals. |
| Do larger or smaller atoms tend to have higher electronegativity values? | SMALLER - because the valence electrons they share are closer to nuclei 2. this is why electronegativity values INCREASE on the top rows & going across the right side of the Periodic Table |
| Nonpolar covalent bond | No-polar-bears so electrons free to share - equal sharing of electrons |
| Polar covalent bonds | Polar bears are there-electrons afraid to share (stay away from smaller atom) |
| Data | Observations based on measurements |
| Hypothesis | States a possible interpretation of the observations - must be stated so that it can be proved by experiments |
| Hypothesis - Greek origin | hypo "under-beneath-down" Gr. thesis "to put down" begining of argument in Classical Greek rhetoric |
| Experiments | Tests that determine the validity of the hypothesis. |
| Theory | When experiments can be repeated with consistent results that confirm the hypothesis, then it becomes a theory |
| meter-How many inches? | 39.4 inches |
| centimeter - How many to a meter | 100 cm = 1 m |
| How many meters to the inch? | 2.54 cm = 1 inch |
| volume (def) | the amount of space a substance Occupies |
| Liter (L) used to measure what? | VOLUME (slightly larger than a quart) |
| 1 Liter compares to what US measurement | Quart - 1 liter = 1.06 qt. |
| Mass | mass of an object is the measure of the quantity of material it contains - does not depend on gravity |
Created by:
walterina4327
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