Chapt. 5-Timberlake
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
Help!
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| Chemical Changes | Occurs when atoms of initial substance rearrange to form new substances.
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| Mole | 6.02 x 10 23 power - Avagadro's number
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| Actual yield | Actual amount of product produced by a reaction
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| Coefficients | Whole number placed in front of the formulas to balance the # of atoms/moles/elemnts of both sides of the equation
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| combination reaction | A reaction in which reactants combine to form a single product
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| decomposition reaction | A reaction in whcih a single reactant splits into two or more simpler substances
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| Double replacement reaction | A reaction in which parts of the two different reactants exchange places
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| Excess Reactant | The reactant that remains when the limiting reactant is used up in a reaction
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| 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
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| limiting reactant | The reactant used up during a chemical reaction, which limits the amount of product that can form
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| Molar mass | The mass in grams of 1 mole of an element--EQUAL NUMERICALLY to atomic mass
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| Oxidation | The loss of electrons by a substance.
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| Biological oxidation | May involve the addition of oxygen, or the loss of hydrogen
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| LEO the lion goes GER | Loss of Electrons is Oxidation - Gain of Electrons is a reduction
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| Percent yield | The ratio of the ACTUAL yield a reaction to the THEORETICAL yield possible for the reaction - multiplied by 100
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| REDUCTION (the contra-intuitive chemical definition) | Means a GAIN of electrons
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| Single replacement reaction | An element replaces a different element in a compoun
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| + Delta sign (triangle) arrow -what do these mean in chemical equations | + means "added to" Delta - means heat used - Arrow--means "reacts to form products"
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| 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
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| 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!!!
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| 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
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| 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
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| 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
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| 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
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| 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
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| Law of Conservation of Mass | There is no change in the total mass of substances reacting in a chemical mass
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| Mole-Mole Factors | A ratio of the moles for any two substances in an equation
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| Percent Yield (equation) | Percent Yield = actual yield(g)/theoretical yield (g) x 100
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| 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
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| Limiting Reactant | In chemical reaction, limiting reactant gets used up first, stops reactant
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| Limiting Reactant Ex. peanut butter/bread | Sandwiches--if you run out of bread, then it is "limiting factor"
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| 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)
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| Sulfur Polyatomic Ions (4) | Sulfate - SO4(2- charge)
2.Hydrogen sulfate (or bisulfate) HSO4(- charge) 3. Sulfite SO3(-2 charge)
4. HSO3(-charge)
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| Phosphorus Polyatomic Ions | 1. Phosphate PO4(3-)
2. Hydrogen phosphate HPO4(-2)
3. DiHydrogen phosphate H2PO4(- charge)
4. Phosphite PO3(-3charge)
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| Chlorine Polyatomic Ions-2 | Chlorate ClO3(-charge) 2. Chlorite ClO2(-charge)
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| Nitrogen Polyatomic Ions-3 | 1. Nitrate NO3(-charge) 2. Ammonium NH4(+ charge) 3. Nitrite NO2(- charge)
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| What is ending for most polyatomic ions | ATE
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| What polyatomic ion has a positive charge? | Ammonium - NH4(-charge)
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| 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)
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| Polyatomic ion with sulfur (given by Dr. Belle) | Thiocyanate SCN(-charge)
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| How to calculate charges for polyatomic ions formulas |
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| Which is most electronegative element? | Fluorine (in group 7A - 1 valence electron)
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| Do metals or nonmetals have higher electronegativity?? | Nonmetals - because they have a greater attraction for electrons than metals.
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| 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
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| Nonpolar covalent bond | No-polar-bears so electrons free to share - equal sharing of electrons
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| Polar covalent bonds | Polar bears are there-electrons afraid to share (stay away from smaller atom)
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| Data | Observations based on measurements
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| Hypothesis | States a possible interpretation of the observations - must be stated so that it can be proved by experiments
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| Hypothesis - Greek origin | hypo "under-beneath-down" Gr. thesis "to put down" begining of argument in Classical Greek rhetoric
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| Experiments | Tests that determine the validity of the hypothesis.
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| Theory | When experiments can be repeated with consistent results that confirm the hypothesis, then it becomes a theory
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| meter-How many inches? | 39.4 inches
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| centimeter - How many to a meter | 100 cm = 1 m
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| How many meters to the inch? | 2.54 cm = 1 inch
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| volume (def) | the amount of space a substance Occupies
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| Liter (L) used to measure what? | VOLUME (slightly larger than a quart)
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| 1 Liter compares to what US measurement | Quart - 1 liter = 1.06 qt.
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| Mass | mass of an object is the measure of the quantity of material it contains - does not depend on gravity
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