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Name the seven fundamental units of measurements and their symbols
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Chemistry 1211 UGA
Final UGA
| Question | Answer |
|---|---|
| What is chemistry? | the science that describes matter--its properties, the changes it undergoes and the energy change that accompany those processes |
| Name the seven fundamental units of measurements and their symbols | 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 |
| Give abbreviation and meaning for following prefixes: 1) mega- 2) kilo- 3) deci- 4)centi- 5) milli- 6)micro- 7) nano- 8)pico- | 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 |
| Convert these lengths: 1 ft = ? in 1 yd = ? ft 1 mile = ? ft ? cm = 1 in 1 mL = ? cm 1 gal = ? qt 1 L = ? qt 1 lb = ? oz | 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 |
| Formula: Percent by mass | Mass A / Mass Mixture |
| 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? | 1.46g zinc |
| Formula: Density | density = mass/volume |
| Formula: Specific Gravity | Sp. Gr. = D substance / D water |
| Formula: Celsius to Kelvin | K = C + 273.15 |
| Formula: Fahrenheit to Celcius | C = 5/9 (F - 32) |
| Formula: Specific Heat | amount of heat (J)/ (mass (g) x change in temperature (C)) |
| Solve: How much heat in joules, is required to raise the temperature of 205g of water from 21.2C to 91.4C? | 6.02 x 10^4 J |
| Accuracy | how closely a measure value agrees with the correct value |
| Calorie | 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 |
| Chemical Change | A change in which one or more new substances are formed |
| Endothermic | Describes processes that absorb heat |
| Energy | The capacity to do work or transfer heat |
| Exothermic | Describes processes that release heat energy |
| Law of Conservation of Energy | Energy cannot be created or destroyed in a chemical reaction or in a physical change; it may be changed from one form to another. |
| Law of Conservation of Matter | No detectable change occurs in the total quantity of matter during a chemical reaction or during a physical change |
| Law of Conservation of Energy and Matter | The combined amount of matter and energy in the universe is fixed |
| Law of Constant Composition or Law of Definite Proportion | Different samples of any pure compound contain the same elements in the same proportions by mass. |
| Precision | How closely repeated measurements of the same quantity agree with one another. |
| Scientific (natural) law | A general statement based on the observed behavior of matter to which no exceptions are known |
| Which of the following processes are exothermic? endothermic? a. burning gasoline b. freezing ice cream c. melting chocolate d. cooling hot water e. condensing water vapor f. burning a match | a. exothermic b. exothermic c. endothermic d. exothermic e. exothermic f. exothermic |
| Which illustrate the concept of potential energy? Kinetic energy? a. a car moving at 55mph b. a rubber band stretched around a paper c. frozen ice cream d. a comet moving through space e. a basketball dropping through a net f. the roof of a house | a. kinetic b. potential c. potential d. kinetic e. kinetic f. potential |
| Molecular Compound : H20 | Water |
| Molecular Compound : H2O2 | Hydrogen Peroxide |
| Molecular Compound : HCl | Hydrogen Chloride Hydrochloric acid |
| Molecular Compound :H2SO4 | sulfuric acid |
| Molecular Compound : HNO3 | Nitric Acid |
| Molecular Compound : CH3COOH | Acetic Acid |
| Molecular Compound : NH3 | Ammonia |
| Molecular Compound : SO2 | Sulfur dioxide |
| Molecular Compound : SO3 | Sulfur trioxide |
| Molecular Compound : CO | Carbon monoxide |
| Molecular Compound : CO2 | Carbon dioxide |
| Molecular Compound : methane | CH4 |
| Molecular Compound : ethane | C2H6 |
| Molecular Compound : propane | C3H8 |
| Molecular Compound : butane | C4H10 |
| Molecular Compound : pentane | C5H12 |
| Molecular Compound : C6H6 | benzene |
| Molecular Compound : methanol | CH3OH |
| Molecular Compound : ethanol | CH3CH2OH |
| Molecular Compound : CH3COCH | Acetone |
| Molecular Compound : diethyl ether | CH3CH2OCH2CH3 |
| Moles | 6.022 x 10^23 |
| Solve : How many moles of atoms does 136.9g of iron metal contain? | 2.451 mol Fe atoms |
| 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. | %C : 39.99% %H : 6.72% %O : 53.2% |
| Solve : Calculate the masses of NaOH and impurities in 45.2 g of 98.2% pure NaOH. | 44.4 g NaOH 0.81 g impurities |
| Allotropic Modifications (allotropes) | Different forms of the same element in the same physical state |
| Law of Multiple Proportions | When two elements, A and B, form more than one compound, the ration of the masses of element B that combine with a given mass of element A in each of the compounds can be expressed by small whole numbers |
| Solve : Name each of the following compounds: a)MgCl2 b)Fe(NO3)2 c)Na2SO4 d)Ca(OH)2 e)FeSO4 | a)magnesium chloride b)iron(II)nitrate c)sodium sulfate d)Calcium hydroxide e)sodium(III)sulfate |
| Solve : Testosterone contains only C, H and O. 79.12%C and 9.79%H by mass. Each molecule contains two O atoms. What are a)the molecular weight and b) the molecular formula for testosterone? | a) 288.5amu b) C19H28O2 |
| 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? | 1.35 x 10^3 g/mol vitamin B12 |
| Solve : What mass of oxygen is required to react completely 1.20 mol of CH4? CH4 + 2 O2 --->CO2 + 2 H2O | 76.8g O2 |
| Formula : percent yield | actual yield / theoretical yield x 100% |
| Formula : Molarity | number of moles of solute / number liters of solution V1M1 = V2M2 (for dilution only) |
| Solve : Commercially available concentrated sulfuric acid is 18.0 M H2SO4. Calculate the volume of concentrated sulfuric acid required to prepare 2.00L of 1.50Molarity H2SO4 solution. | 14.7 M H3PO4 |
| 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? | 0.40L |
| Formula : mass number | Number of protons + number of neutrons Atomic Number + number of neutrons |
| 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 | x(68.9257) + (1-x)(70.9249) = 69.72 amu 60.0% 69Ga 40.0% 71Ga |
| Formula : Speed of Light or waves | (Wavelength)(velocity) |
| The longer the wavelength, the ______ the amplitude | Lower |
| Formula : Energy of Light | E = (plank's constant)(velocity) E = (Plank's constant)(speed of light) / (wavelength) |
| Formula : Plank's Constant | 6.626 x 10^-34 J |
| Formula : Speed of Light | 3.00 x 10^8 m/s |
| 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. | 4.09 x 10^-19 J/photon |
| Formula : de Broglie Wavelength | (plank's constant) / (mass x velocity) |
| Solve : a) Calculate the wavelength in meters of an electron traveling at 1.24 x 10 ^7 m/s. The mass of an electron is 9.11 x 10^-28 g. B) Calculate the wavelength of a baseball of mass 5.25 oz traveling at 92.5 mph. Recall that 1 J = 1 kg x m^2/s^2. | a) 5.87 x 10^-11 m b) 1.08 x 10^-34 m |
| Formula : principal quantum number | n = 1, 2, 3, 4... main energy level or shell than an electron occupies |
| Formula : momentum quantum number | l = 0, 1, 2, ...(n-1) Shape of orbital |
| Formula : magnetic quantum number | ml = (-l)...,0,...,(l) which atomic orbital |
| Formula : spin quantum number | ms = positive or negative 1/2 spin of the electron |
| Absorption Spectrum | the spectrum associated with absorption of electromagnetic radiation by atoms resulting from transitions from lower to higher electronic energy states |
| Aufbau Principle | A guide to predicting the order in which electrons fill subshells and shells in atoms |
| Continuous Spectrum | A spectrum that contains all wavelengths in a specified region of the electromagnetic spectrum |
| Electromagnetic radiation | energy that is propagated by means of electric and magnetic fields that oscillate in directions perpendicular to the direction of travel of the energy. |
| Emission Spectrum | The spectrum associated with emission of electromagnetic radiation by atoms resulting from electron transitions from higher to lower energy states |
| Ferromagnetism | the property that allos a substance to become permanently magnetized when placed in a magnetic field; exhibited by iron, cobalt, and nickel and some of their alloys |
| frequency | the number of crests of a wave that pass a given point per unit time |
| Heisenberg Uncertainty Principle | It is impossible to determine accurately both the momentum and position of an electron simultaneously |
| Hund's Rule | Each orbital of a given subshell is occupied by a single electron before pairing begins |
| Isotopes | To or more forms of atoms of the same element with different masses; atoms containing the same number of protons but different neutrons |
| Paramagnetism | Attraction toward a magnetic field, strong than diamagnetism, but still very weak compared with ferromagnetism; due to presence of unpaired electrons |
| Pauli Exclusion Principle | No two electrons in the same atom may have identical sets of quantum numbers |
| Photoelectric effect | emission of an electron from the surface of a metal, caused by impinging electromagnetic radiation of certain minimum energy; the resulting current increases with increasing intensity of radiation. |
| Trends : Atomic Radii | Decreases Across Periodic Table Increase Down Periodic Table |
| Trends : Ionization Energy | General Trend with Many Exceptions Increasing Across Periodic Table Decreases Down A periodic Table |
| Trends : Electron Affinity | Generally Increases Across Periodic Table Decreases down a periodic table Exceptions: For Rows 2-5 Column V will always be lower than IV and VI. For Rows 2-5 Column III will always be lower than I and for all rows Column II will be the lowest. |
| Trends : Ionic Radii | General Rules Decreases Across Periodic Table Increases Down Periodic Table The more positive an elements valence shell, the smaller it will be. |
| Trends : Electronegativity | Increase across periodic table Decrease down periodic table |
| Electrolytes | substances whose acqeous solutions conduct electric currents. Strong Electrolytes Weak Electrolytes Nonelectrolytes |
| A) Common strong acids B) Common weak acids | A) HCl; HBr; HI; HNO3; HClO4; HClO3; H2SO4 B) HF; CH3COOH; HCN; HNO2; H2CO3; H2SO3; H3PO4; (COOH)2 - oxalic acid |
| A) Common Strong Bases B) Common Weak Bases | A) LiOH; NaOH; KOH; RbOH; CsOH, Ca(OH)2, Sr(OH)2, Ba(OH)2 B) NH3 |
| Naming : HClO, HClO4, HNO2, HNO3, H3PO2 | Hypochlorous acid, perchloric acid, nitrious acid, nitric acid, hypophosphorous acid |
| Naming : Rules | 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 |
| Oxidation and Reduction | 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 |
| Oxidizing and Reducing Agents | OA - 1) oxidize other substances 2)contain atoms that are reduced 3)gained electrons RA - 1)reduce other substances 2)contain atoms that are oxidized 3)lose electrons |
| Disproportionation reaction | redox reaction in which the same element is oxidized or reduced |
| Redox Reactions | Where reducing and oxidizing occur REDOX |
| Combination Reactions | Reactions in which two or more substances combine to form a compound. REDOX |
| Decomposition Reactions | in which a compound decomposes to produce (1) two elements, (2) one or more elements and one or more compounds, (3) two or more compounds REDOX |
| Displacement Reactions | Reactions in which one element displaces another from a compound REDOX |
| Matathesis Reaction | In many reactions between two compounds in aqueous solution, the positive and negative ions appear to "change partners" to form two new compounds, with no change in oxidation numbers. NOT REDOX |
| Gas Formation Reaction | Products include an insoluble or slightly soluble gas, which escapes from solution |
| Bond Lengths and Strengths A) Single Bond B) Double Bond C) Triple Bond | A) Longest and weakest B) Medium and Medium C) Shortest and strongest |
| Electronic and Molecular Geometry : Linear | 180(deg) angles AB2 No Lone Pairs Hybridization = sp |
| Electronic and Molecular Geometry : Trigonal Planar | 120(deg) angles AB3 AB2U - bent Hybridization - sp2 |
| Electronic and Molecular Geometry : Tetrahedral | 109.5 (deg) angles AB4 AB3U - Trigonal pyramidal AB2U2 - Bent Hybridization - sp3 |
| Electronic and Molecular Geometry : Trigonal Bipyramidal | 90(deg), 120(deg), 180(deg) angles AB5 AB4U - seesaw AB3U2 - t-shaped AB2U3 - linear Hybridization - sp3d |
| Electronic and Molecular Geometry : Octahedral | 90(deg) and 180(deg) angles AB6 AB5U - square pyramidal AB4U2 - square planar Hybridization - sp3d2 |
| Sigma Bond | a bond resulting from head on overlap of atomic orbitals single bonds, double and triple bonds have one sigma bond |
| Pi Bond | bond resulting from side-on overlap of atmoic orbitals double bonds - one pi bond triple bond - two pi bonds |
| Formula : Bond Order | (number of bonding electrons) - (number of antibonding electrons / 2 |
| Properties of Aqueous Solutions of Acids | sour taste, change colors of indicators, Nonoxidizing acids react with metal above hydrogen to liberate hydrogen gas, acids react with metal oxides and hydroxides to form salts and water, acids react with salts of weaker acids and form weaker acids |
| Properties of Aqueous Solutions of Bases | 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 |
| Arrhenius Theory | 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 |
| Bronsted-Lowry Theory | An acid is defined as a proton donor (H+) and a base is defined as a proton acceptor. The stronger the acid, the weaker is its conjugate base. Water can act as either acid or base |
| Lewis Theory | An acid is any species that can accept a share in an electron pair. A abse is any species that can donate or share one or more lone pairs of electrons. |
| Boyle's Law | At a given temperature, the product of pressure and volume of a definite mass of gas is constant |
| Formula : Boyle's law | PV = k P1V1 = P2V2 |
| Charles Laws | At constant pressure, the volume occupied by a definite mass of a gas is directly proportional to its absolute temperature |
| Formula : Charles Law | V = kT (temperature K) V1/T1 = V2/T2 |
| Standard Temperature and Pressure | One atmosphere, 273 Kelvin |
| Formula : Combined Gas Law | |
| Standard Molar Volume | 22.414 L at STP |
| Formula : The Ideal Gas Equation | PV=nRT (Pressure)(Volume)=(Moles)(Ideal Gas Constant)(Temperature) |
| Formula : Ideal Gas Constant | 0.0821 (L)(atm)/(mol)(K) 8.314 (J)/(mol)(K) 8.314 (kPa)(dm^3)/(mol)(K) |
| Dalton's Law of Pressure | The total pressure exerted by a mixture or ideal gases is the sum of the partial pressures of those gases |
| Formula : Dalton's Law of Pressure | Ptotal = n1RT/V + n2RT/V + n3RT/V .... Ptotal = P1 + P2 + P3.... |
| Kinetic Molecular Theory | 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 |
| Formula : Kinetic Molecular Theory | Average molecular speed = Sqr.root(T/molecular weight) |
| Formula : Molecular Speed | Sqare.Root (3RT/molecular weight) |
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