Final UGA
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| show | the science that describes matter--its properties, the changes it undergoes and the energy change that accompany those processes
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| show | 1)length: meter - m 2)mass: kilogram - kg 3)time: second - s 4)electric current: ampere - A 5)temperature: kelvin - K 6)luminous intensity: candela - cd 7)amount of substance: mole - mol
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| show | 1)M 1000000 2)k 1000 3)d 0.1 4)c 0.01 5)m 0.001 6)meu 0.000001 7)n 0.000000001 8)p 0.000000000001
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| show | 1 ft = 12 in
1 yd = 3 ft
1 mile = 5280 ft
2.54 cm = 1 in
1 mL = 1 cm (cubed)
1 gal = 4 qt
1 L = 1.057 qt
1 lb = 16 oz
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| Formula: Percent by mass | show 🗑
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| Solve: Us pennies made since 1982 consist of 97.6% zinc and 2.4% copper. The mass of a particular penny is measured to be 1.494g. How many grams of zinc does this penny contain? | show 🗑
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| show | density = mass/volume
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| show | Sp. Gr. = D substance / D water
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| show | K = C + 273.15
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| Formula: Fahrenheit to Celcius | show 🗑
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| Formula: Specific Heat | show 🗑
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| Solve: How much heat in joules, is required to raise the temperature of 205g of water from 21.2C to 91.4C? | show 🗑
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| Accuracy | show 🗑
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| show | Defined as exactly 4.184 J. Originally defined as the amount of heat required to raise the temperature of one gram of water from 14.5 degrees Celsius to 15.5 degrees celsius
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| Chemical Change | show 🗑
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| Endothermic | show 🗑
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| Energy | show 🗑
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| Exothermic | show 🗑
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| show | Energy cannot be created or destroyed in a chemical reaction or in a physical change; it may be changed from one form to another.
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| show | No detectable change occurs in the total quantity of matter during a chemical reaction or during a physical change
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| Law of Conservation of Energy and Matter | show 🗑
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| show | Different samples of any pure compound contain the same elements in the same proportions by mass.
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| show | How closely repeated measurements of the same quantity agree with one another.
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| show | A general statement based on the observed behavior of matter to which no exceptions are known
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| show | a. exothermic
b. exothermic
c. endothermic
d. exothermic
e. exothermic
f. exothermic
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| show | a. kinetic
b. potential
c. potential
d. kinetic
e. kinetic
f. potential
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| Molecular Compound : H20 | show 🗑
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| Molecular Compound : H2O2 | show 🗑
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| show | Hydrogen Chloride
Hydrochloric acid
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| show | sulfuric acid
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| show | Nitric Acid
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| show | Acetic Acid
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| Molecular Compound : NH3 | show 🗑
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| Molecular Compound : SO2 | show 🗑
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| Molecular Compound : SO3 | show 🗑
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| show | Carbon monoxide
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| Molecular Compound : CO2 | show 🗑
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| Molecular Compound : methane | show 🗑
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| show | C2H6
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| Molecular Compound : propane | show 🗑
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| Molecular Compound : butane | show 🗑
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| Molecular Compound : pentane | show 🗑
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| Molecular Compound : C6H6 | show 🗑
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| Molecular Compound : methanol | show 🗑
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| Molecular Compound : ethanol | show 🗑
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| Molecular Compound : CH3COCH | show 🗑
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| show | CH3CH2OCH2CH3
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| Moles | show 🗑
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| Solve : How many moles of atoms does 136.9g of iron metal contain? | show 🗑
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| Solve : A 0.1014-g sample of purified glucose was burned in a C-H combustion train toproduce 0.1486 g sample of CO2 and 0.0609 g of H2O. Determine the masses of C,H and O in the sample and the percentages of these elements in glucose. | show 🗑
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| show | 44.4 g NaOH
0.81 g impurities
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| Allotropic Modifications (allotropes) | show 🗑
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| Law of Multiple Proportions | show 🗑
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| Solve : Name each of the following compounds: a)MgCl2 b)Fe(NO3)2 c)Na2SO4 d)Ca(OH)2 e)FeSO4 | show 🗑
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| show | a) 288.5amu
b) C19H28O2
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| Vegetarians sometimes suffer from the lack of vitamin B12. Each molecule of vitamin B12 contains a single atom of cobalt and is 4.35% cobalt by mass. What is the molecular weight of B12? | show 🗑
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| show | 76.8g O2
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| Formula : percent yield | show 🗑
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| Formula : Molarity | show 🗑
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| show | 14.7 M H3PO4
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| Solve : to what volume must a student dilute 50 mL of a solution containing 25mg of AlCl3/mL so that the Al concentrate in the new solution is 0.024Molarity? | show 🗑
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| show | Number of protons + number of neutrons
Atomic Number + number of neutrons
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| Solve : The atomic weight of gallium is 69.72 amu. The masses of the naturally occurring isotopes are 68.9257 amu for 69Ga and 70.9249 amu for 71Ga. Calculate the percent abundance of each isotope | show 🗑
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| show | (Wavelength)(velocity)
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| The longer the wavelength, the ______ the amplitude | show 🗑
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| Formula : Energy of Light | show 🗑
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| Formula : Plank's Constant | show 🗑
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| show | 3.00 x 10^8 m/s
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| Solve : A green line of wavelength 4.86 x 10^-7 m is observed in the emission spectrum of hydrogen. Calculate the energy of one photon of this green light. | show 🗑
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| show | (plank's constant) / (mass x velocity)
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| show | a) 5.87 x 10^-11 m
b) 1.08 x 10^-34 m
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| Formula : principal quantum number | show 🗑
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| Formula : momentum quantum number | show 🗑
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| show | ml = (-l)...,0,...,(l)
which atomic orbital
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| Formula : spin quantum number | show 🗑
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| Absorption Spectrum | show 🗑
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| show | A guide to predicting the order in which electrons fill subshells and shells in atoms
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| show | A spectrum that contains all wavelengths in a specified region of the electromagnetic spectrum
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| Electromagnetic radiation | show 🗑
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| show | The spectrum associated with emission of electromagnetic radiation by atoms resulting from electron transitions from higher to lower energy states
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| Ferromagnetism | show 🗑
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| frequency | show 🗑
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| Heisenberg Uncertainty Principle | show 🗑
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| show | Each orbital of a given subshell is occupied by a single electron before pairing begins
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| Isotopes | show 🗑
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| Paramagnetism | show 🗑
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| show | No two electrons in the same atom may have identical sets of quantum numbers
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| Photoelectric effect | show 🗑
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| show | Decreases Across Periodic Table
Increase Down Periodic Table
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| show | General Trend with Many Exceptions
Increasing Across Periodic Table
Decreases Down A periodic Table
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| Trends : Electron Affinity | show 🗑
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| Trends : Ionic Radii | show 🗑
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| Trends : Electronegativity | show 🗑
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| show | substances whose acqeous solutions conduct electric currents.
Strong Electrolytes
Weak Electrolytes
Nonelectrolytes
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| A) Common strong acids B) Common weak acids | show 🗑
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| A) Common Strong Bases B) Common Weak Bases | show 🗑
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| show | Hypochlorous acid, perchloric acid, nitrious acid, nitric acid, hypophosphorous acid
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| show | 1. Hypo- -ous/-ite, -ous/-ite, -ic/-ate, per- -ic/-ate
2. When two nonmetals are bonded together, use greek and latin number prefixes one through ten
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| show | Oxidation : increase in oxidation state and corresponds to the loss or apparent loss of electrons
Reduction - decrease in oxidation state and corresponds to a gain or apparent gain in electrons
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| Oxidizing and Reducing Agents | show 🗑
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| show | redox reaction in which the same element is oxidized or reduced
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| show | Where reducing and oxidizing occur
REDOX
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| show | Reactions in which two or more substances combine to form a compound.
REDOX
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| Decomposition Reactions | show 🗑
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| Displacement Reactions | show 🗑
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| Matathesis Reaction | show 🗑
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| show | Products include an insoluble or slightly soluble gas, which escapes from solution
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| show | A) Longest and weakest
B) Medium and Medium
C) Shortest and strongest
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| Electronic and Molecular Geometry : Linear | show 🗑
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| Electronic and Molecular Geometry : Trigonal Planar | show 🗑
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| Electronic and Molecular Geometry : Tetrahedral | show 🗑
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| show | 90(deg), 120(deg), 180(deg) angles
AB5
AB4U - seesaw
AB3U2 - t-shaped
AB2U3 - linear
Hybridization - sp3d
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| Electronic and Molecular Geometry : Octahedral | show 🗑
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| Sigma Bond | show 🗑
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| Pi Bond | show 🗑
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| show | (number of bonding electrons) - (number of antibonding electrons / 2
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| Properties of Aqueous Solutions of Acids | show 🗑
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| show | Bitter taster, slippery feeling, change color of indicators from red to blue and yellow to blue, reacts with acids to form salts and water, conduct an electric current
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| show | an acid is a substance that contains hydrogen and produces H+ in aqueous solution. a base is a substance that contains the OH group and produces OH- in aqueous solution
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| Bronsted-Lowry Theory | show 🗑
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| Lewis Theory | show 🗑
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| Boyle's Law | show 🗑
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| show | PV = k
P1V1 = P2V2
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| Charles Laws | show 🗑
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| show | V = kT (temperature K)
V1/T1 = V2/T2
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| Standard Temperature and Pressure | show 🗑
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| show |
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| Standard Molar Volume | show 🗑
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| Formula : The Ideal Gas Equation | show 🗑
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| show | 0.0821 (L)(atm)/(mol)(K)
8.314 (J)/(mol)(K)
8.314 (kPa)(dm^3)/(mol)(K)
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| show | The total pressure exerted by a mixture or ideal gases is the sum of the partial pressures of those gases
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| Formula : Dalton's Law of Pressure | show 🗑
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| show | the average kinetic energy of gaseous molecules is directly proportional to the absolute temperature of the sample. The average kinetic energies of molecules of different gases are equal at a given temperature
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| Formula : Kinetic Molecular Theory | show 🗑
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| show | Sqare.Root (3RT/molecular weight)
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Created by:
ems693
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