Download Hon Chem Year Outline

Into to Chemistry
 What is chemistry and how is it part of everyday life?
 What is matter and how does it interact?
 What is energy and how is it related to matter?
 What are the basic units of measurement in chemistry?
Chem Equations and Reactions
 Write, balance and classify chemical reactions.
 Predict properties of elements based upon location on the periodic table.
 Be able to recognize compounds as ionic, molecular, acidic, basic, etc.
Stoich
1. What is a mol and how is it used in chemistry?
2. What is molarity?
3. What is stoichiometry?
4. How do you determine the theoretical amount of products that should be made in a chemical
reaction?
5. How do you determine the % yield of product in a chemical reaction?
ThermoChem
 How do we define heat? (not temperature) & main unit
 What is a system, and what are the surroundings, and how these are needed to describe heat
transfer?
 How is calorimetry used to determine heat?
 To describe heat transfer as exothermic or endothermic and calculate transfer using specific heat
values
 Understand how to use a calorimeter and solve a heat transfer problem, using calorimetry and q1
= -q2
 To calculate heat released/absorbed during a substance phase change
Structure of the Atom
 What are protons, neutrons, and electrons?
 How did scientists build on the atomic theory to provide more detail of the atom?
 How is wavelength, frequency, and energy of waves determined?
 What are some common forms of electromagnetic radiation?
 Calculate wavelength, frequency, and energy of waves
 Describe a basic time line of the development of the atomic model
 State possible quantum number values for some lighter elements
 Write out basic electron configurations ad orbital diagrams of certain elements.
Electron Configuration & the Periodic Table
 What s a period in the periodic table?
 What is a group in the periodic table?
 What are the names of certain families/groups?
 What are valence electrons?
 What are some trends predicted in the periodic table?
 write an electron configuration
 identify certain areas of the periodic table, eg transition metals, alkali metals, alkaline
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earth metals, halogens, noble gases, etc.
define atomic radius, electronegativity, ionization energy, and electron affinity
identify and explain periodic trends of above terms
determine number of valence electrons in an atom
predict certain properties of elements based on the location on the periodic table
Chemical Bonding
 will recognize “cations” and “anions” in binary compounds.
 will draw Lewis structures for atoms.
 will relate Roman numerals on the periodic table to valence electrons and Lewis structures.
 will relate Lewis structures to auf bau notation.
 will relate valence electrons to oxidation number.
 will draw Lewis structures for ionic compounds.
 will draw Lewis structures for covalent compounds
 will recognize structures that are isoelectric.
 will describe the difference between single, double, and triple bonds.
 will recognize which elements are able to form double and triple bonds.
 will differentiate between ions with a noble gas configuration, a pseudonoble gas configuration
and ions having neither.
 will draw Lewis structures for compounds that do not follow the octet rule.
 will describe a coordinate covalent or dative bond.
Molecular Structure, Hybridization, and Orbitals
 How /why are hybrid orbitals formed?
 How do multiple bonds play in the shape of the molecule?
 How are lone pairs of electrons different/ the same in determining the molecular geometry?
 How do we determine if a bond is stable or not?
 How does bond order suggest if a bond is stable or not?
 To recognize or determine the shape of a molecule by studying the Lewis Dot Structure
 To determine the bond angles of a given molecular model
 To identify the hybrid orbitals present in a molecule, including multiple bonds
 Recognize the difference between bonding and anti-bonding molecular orbitals.
 Identify orbitals represented as σs, σp, πp, σs*, σp* πp* orbitals.
 Draw energy diagrams for diatomic molecules
 Calculate the bond order of a diatomic molecule
Gases
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describe the physical make-up of gases.
define gas pressure.
convert gas pressures.
Mm of Hg -> torr -> atm -> kPa
describe the relationship expressed in Boyle’s Law
describe the relationship expressed in Charles’s Law
solve problems involving changes in pressure and volume.
solve problems involving changes in temperature and pressure.
solve problems involving changes in temperature pressure and volume
define absolute zero.
convert celsius -> kelvin
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describe the relationship expressed in Gay-Lussac’s Law and Avogadro’s law
solve problems illustrating Gay-Lussac’s Law.
write the ideal gas equation and define the terms.
solve problems using the ideal gas equation.
define STP.
define molar volume of a gas.
solve problems using the molar volume of a gas.
describe Dalton’s Law of partial pressures.
solve problems involving Dalton’s Law of partial pressures.
describe the relationship expressed in Graham’s Law.
solve problems involving Graham’s Law.
describe Kinetic-molecular theory.
Intermolecular Forces
 Learn the different types of intermolecular forces
 be able to determine the intermolecular forces when given a molecular structure
 learn the properties of different types of solid structures
 learn the properties of liquids
 interpret a basic phase diagram
Solutions
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explain Henry’s Law.
describe the effect of temperature on solubility.
predict the solubilities of metal compounds using rules of solubility.
calculate the % composition by mass of a solution.
calculate molarity.
calculate molality.
calculate mol fraction.
define colligative properties.
solve boiling point elevation problems.
memorize the molal boiling point elevation constant for water.
solve freezing point depression problems.
memorize the molal freezing point depression constant for water.
Kinetics
 What are the factors that determine the speed of reaction?
 How do you describe the rate of a reaction using the collision theory?
 What is the difference between the Rate Law and Integrated Rate Law?
 What are the differences in the three rate orders (0, 1, 2)
 What are the mathematical equations for these orders?
 How do we determine a half life of a reaction?
 How do you describe activation energy
Equilibrium
 to write out a mass action expression, and to calculate the equilibrium constant
 to calculate the final equilibrium concentrations using the MAE
 to predict a reaction shift whn a stress is applied
 to describe these reaction shifts on the molecular level
Acides & Bases
 identify acids and bases when given the chemical formula
 identify bronsted acids and bases, and their conjugates
 write dissociation reactions of acids and bases
 identify Lewis acids
 calculate concentration in terms of molarity, molality, and normality
Aqueous Equilibria
 Calculate pH, pOH, H+ and OH- of a weak acid or base when given the Ka or Kb
 perform a titration, and calculate the pH at certain points in the titration
 prepare an effective buffer for a specific pH
 identify which combination of chemicals would produce an effective buffer
 Be able to work with and ICE chart to determine concentrations
KSP
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define Ksp and relate it to equilibrium
write the mathematical expression for the Ksp for a saturated solution
given concentrations in a saturated solution, Calculate the Ksp
given the Ksp calculate concentrations in a saturated solution i.e. solubilities
given concentrations and the Ksp, predict if precipitation will occur.
Thermodynamics
 determine if a reaction/ physical change is exothermic or endothermic
 determine if a reaction/ physical change increases or decreases in disorder
 calculate changes in enthalpy and entropy using standard thermodynamic data
 use Gibb's free energy calculations to determine a reactions spontaneity
Electrochemistry
 Sketch a basic galvanic cell, labeling all basic parts
 determine anode and cathodes based on cell potentials
 calculate cell potentials with cells of different concentrations
 electrolysis calculations
Nuclear Chemistry
 distinguish between different types of nuclear decay
 "balance" a nuclear decay equation
 predict the stability of an isotope
 calculate the mass defect and energy produced
 state some effects of nuclear radiation exposure
 identify key components of a nuclear reactor