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Basic Algebra
-addition, subtraction, multiplication, division, taking the square root, taking the reciprocal
-solving simultaneous equations
-re-writing equations to solve for any variable
-calculating and using logarithms, including natural logarithms
-using scientific notation
-order of operations
-finding and using the slope of a line/tangent line
-constructing and using clear, well-labeled, correct graphs
-using the quadratic formula
-what sigma (the summation sign) means and how to use it
-finding and using percentages
-solving word problems effectively
Basic Knowledge
-taking clear, comprehensive notes from lecture and reading
-taking prior knowledge and applying it in new ways
-taking prior knowledge and combining it to be used in more complex ways
-using an index and a glossary
-being organized
-knowing and using the metric system
-completing and turning assignments in on time
-following all school and class/laboratory rules
-participating appropriately in class, including in a laboratory setting
-persevering!!
Tools to help you succeed in Chemistry
-a scientific (NON-GRAPHING) calculator with square root, nth root, y to the x, exponent (EXP or EE), logarithm and natural logarithm (10 to the x AND e to the x), reciprocal (1/x or x to the -1)
-study groups--work only with other motivated students who wish to succeed
-an open, well-fed, well-rested brain
-a willingness to learn and the ability to keep trying NO MATTER WHAT!
***When you finish each chapter in Chemistry you should know***
Chapter 2
-mass is measured in grams (or a unit containing grams, like kilograms)
-volume is measured in liters (or a unit containing liters) REMEMBER: 1 cubic centimeter = 1 milliliter
-length, distance, etc are measured in meters (or a unit containing meters)
-significant figures (sig figs) are used to provide appropriate accuracy for calculations; know how to count them and use them
-dimensional analysis (canceling units); this method will be used for virtually all work done all year
-temperature can be measured in oC or K REMEMBER: TK = toC + 273.15
-density = mass/volume, usually expressed in g/ml or g/cm3; know how to solve for d, m or V
-physical and chemical (changes and properties), mixture, solution, hetero-/homo-geneous, substance, element, compound
Chapter 3 (VERY IMPORTANT CHAPTER)
-average atomic mass; calculate it from both the periodic table and from individual molar masses with percent abundance
-moles/atoms/molecules/grams using molar mass, chemical formulas, masses, etc
-convert grams to moles to atoms, milliliters to grams to moles to molecules, etc (relate any two or more of these units)
-mass percent; how to find it and how to use it
-molecular/empirical formula
-product/reactant/coefficient/subscript
-balance chemical equations
-use balanced equations for stoichiometric problems
-limiting/excess reactant
-theorectical and percent yield
-M = m/n
-Avagadro's number = 6.022 x 10 23rd; usually used for atoms or molecules per mole
-know what a mole represents in terms of mass, atoms, and molecules
Chapter 3/4
-law of conservation of mass (big lie to be revealed later)
-law of definite proportion
-law of multiple proportions (H2O is water, H2O2 is hydrogen peroxide; same elements in different proportions make different compounds)
-Dalton's Atomic Theory and the common flaw to this theory according to what we know now
-cathode ray tube and gold foil experiments; basic parts of experiments, what part of the atom was found and how
-diagram of an atom--include all parts of the structure
-structural/empirical/molecular formula
-atomic number and mass number, find numers of protons, neutrons, and electrons for any ion or atom
-ion/atom/cation/anion/polyatomic ion
-families/groups/periods; where are they and what is each called?
-formulas and names of compounds from periodic table, list of polyatomic ions (p. 66), charge on ions, making compounds from any of these
Chapter 5
-common units of pressure, convert from one kind to another
-Absolute Zero and what it actually means (theoretically)
-Ideal Gas Law (all forms), Dalton's Law of Partial Pressures, Graham's Law
-molar mass and density of a gas
-diffusion/effusion
-real gases don't actually behave as ideal gases do
-how do temperature, pressure, volume and number of moles affect each other
Chapter 7
-parts of a wave, parts of the electromagnetic spectrum
-electrons have energy and can gain more; if they gain enough they can leave the ground state and move to an excited state or even leave the atom altogether: know how to calculate this energy amount
-duality of light
-quantom mechanics; 4 quantum numbers for an individual electron, meaning of each number
-Heisenberg Uncertainty/Pauli Exclusion/Aufbau Principles
-electron configuration for atoms and ions (include abbreviated)
-periodic trends of ionization energy, ionic/atomic radius, electronegativity (some of these are in Chapter 8)
- lambda x nu = c, E = h x nu
-change in E = -2.178 x 10 -18th J [(1/n1 squared) - (1/n2 squared)]
-flame tests; what actually causes the colors to be seen and what causes different colors for different atoms
-what is shielding
Chapter 8/9
-ionic/covalent bonding; know how to tell the difference mathematically and from the placement on the periodic table
-Lewis structures of molecules and polyatomic ions; shapes, names, polarity, hybridization, resonance, single/double/triple bonding
-octet rule and exceptions
Chapter 10
-relative strengths of intermolecular forces; dipole forces, hydrogen bonding, dispersion/London/Van der Waal forces
-surface tension, capillary action, attraction based on polarity
-unit cells; 2r = s, 4r = s square root of 2, 4r = s square root of 3
-metallic, polar/nonpolar covalent, network covalent, ionic
-phase changes, phase diagram, enthalpy of fusion/vaporization
-normal melting/boiling point, critical temperature/pressure