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[交流] 【咨询】(ACS) Standardized Exams 是什么已有1人参与

American Chemical Society (ACS) Standardized Exams是什么啊？
我去休斯顿大学但是他们要我们一入学就考这一系列的试。问一下，这是一个什么考试啊？我们该怎么准备啊？

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yuhuidavid(金币+2):谢谢参与~ 2010-06-20 08:41:34
flyingcp(金币+1): 2010-06-23 16:49:58
flyingcp(金币+2): 2010-07-09 22:47:14

你中奖了。感觉很不容易考啊，下面的从网上找的
Study Guide for the American Chemical Society Standardized Final Exam
for First Semester of General Chemistry
CHM 115 Dr. Tremain
This comprehensive exam consists of 70 multiple-choice questions. It is a two -hour exam scheduled
for Wednesday December 18th from 8:00 am to 10:00 am. Arrive about 10 minutes early. Bring 2-3 #2
pencils, an eraser, and a calculator. Scratch paper and Scantron sheets will be provided.
If you see any question on the exam that we have not covered in class (or you don’t remember right
away how to answer it), skip that question and go on to the next one. Come back to those questions
only after you have answered all the others. There is no penalty for guessing.
Good luck on all your other finals as well !
Chapter 1
Definition of Chemistry
States of matter
Matter: Elements, Compounds, Mixtures (Homogeneous and Heterogeneous) Examples
*Intensive and Extensive properties (see Chapter 11 Lecture Notes)
SI Prefixes
Conversion: kg to pounds, Temperature
Difference between accuracy and precision
Chapter 2
Postulates of Dalton’s Atomic Theory
J.J. Thompson’s Cathode Ray Tube experiment (know the experiment and result)
Millikan’s Oil Drop experiment (know the experiment and result)
Rutherford’s Gold foil experiment (know the experiment and result)
Definition of isotopes and examples of three elements with isotopes
Names and formulas of Inorganic (Ionic) compounds
Names and formulas of Cations and Anions including Polyatomic Ions (Tables 2.4, 2.5, 2.6, 2.7, & 2.8). See
my lecture notes.
Names and formula of molecular compounds
Writing and balancing chemical equations
Chapter 3
Relationship between mole, molar mass, and Avagadro's number (Calculations)
Calculations of empirical and molecular formula (percentage composition)
Everything dealing with Stoichiometry (amounts of reactants and products)
Determination of a limiting reagent in a reaction and using it properly in a calculation
Calculation of percent yield in a reaction
Chapter 4
Definition of an electrolyte
Examples of compounds that are strong electrolytes, weak electrolytes or non-electrolytes
Net Ionic Equations (know how to predict products of precipitation reactions and the solubility rules)
Definition of an acid and examples of mono-, di- and tri-protic acids
Definition of a base
Example of a neutralization reaction
Oxidation-Reduction reactions (OIL RIG or LEO goes GER). Know oxidizing agent and reducing agent
Balancing Oxidation-Reduction reactions
Calculation of molarity and using molarity to find yield of a product in a reaction
Definition and an example each for combustion, decomposition, combination reactions
Chapter 5
Conversion of Pressure units between atmosphere, torr, mmHg and Pascals
Boyle’s Law, Charles’ Law and Avogadro’s Law and the Ideal gas equation
Calculations based on Ideal gas equation
Dalton’s Law of Partial pressures
Kinetic Theory of Gases and molecular speed of a gas
Why do real gases do not follow the Ideal gas equation? Nonideal behavior
Chapter 6
Potential and Kinetic Energy
System and Surrounding - Internal Energy (U)
First Law of Thermodynamics (Law of Conservation of Energy)
Endothermic and Exothermic Processes
Enthalpy, Enthaplies of Reactions, State Functions, Path Functions
Heat Capacity and Specific heat
Constant-Pressure and Constant-Volume Calorimetery (what you did in Lab Expt. 14 in SWM)
Hess’s Law and Standard Enthalpies of Formation
Chapter 7
Definition of wavelength and frequency
Electromagnetic radiation (spectrum)
Calculations relating wavele ngth, frequency, and speed of light
Calculations relating energy to frequency using Planck’s constant
Calculation of wavelength and/or frequency for a transition of an electron (absorption or emission)
Bohr’s Theory of the Hydrogen Atom
Definition Heisenberg’s Uncertainty Principle and the de Broglie relation
Quantum Numbers n, l, ml and ms; Pauli Exclusion Principle; and shapes of atomic orbitals
Chapter 8
Determination of electron configuration (Aufbau Principle) of atoms and ions
Break up Periodic Table in s, p, d and f block orbitals
Paramagnetic and Diamagnetic substances
Identifying metals, non- metals and metalloids in a Periodic Table of the Elements (know their properties)
Names of different groups in a Periodic Table of the Elements
Periodic Trends in effective nuclear charge, atomic radius, ionic radius, ionization energy, electron affinity,
electronegativity
Classification of metal oxides as basic and non- metal oxides as acidic oxides
Chapter 9
Ionic and covalent bonding and Lewis electron-dot symbols
Writing Lewis structures: Octet rule, expanded octets, resonance structures, formal charges
Bond length, Bond strength, DH and bond energy
Chapter 10
VSEPR and Molecular Geometry; Dipole Moment and Polarity
Valence Bond theory, sigma and pi bonds, multiple bonds
Molecular Orbital theory and bond orders
Chapter 11
Gases, Liquids, and Solids; phase transitions, amount of heat required to convert ice into steam
Vapor pressure, boiling point, and melting point
Phase diagrams, critical temperature, critical pressure, triple point
Surface tension and viscosity
Intermolecular forces: van der Waals, dipole-dipole, ion-dipole, induced dipole, London (dispersion),
hydrogen bonding
Types of solids: molecular, metallic, ionic, covalent network and their properties
Crystalline solids, crystal lattice, simple cubic, body-centered cubic, face-centered cubic
Hexagonal close-packed structure, cubic close-packed structure, coordination number