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Have a basic knowledge of the development of the atomic model (Dalton, Thomson, Millikan, Rutherford)

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Distinguish between protons, neutrons, and electrons and be able to describe the composition of an atom of any particular element in terms of these subatomic particles. Know the difference between an atom, an ion, and a molecule.

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Have a basic knowledge of the periodic table, which includes being able to predict whether an element is a metal, nonmetal, or metalloid. Locate alkali metals, alkaline earth metals, halogens, noble gases, transition metals, actinides and lanthanides on the periodic table. Be familiar with basic properties of these groups.

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Be able to write the correct name of an inorganic compound from its formula and vice versa.

Be able to write, balance, and predict the products of nuclear reactions.

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Understand the meaning of half-life. Understand the nature and applications of radioactive dating. Perform calculations involving radioactive decay.

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Be able to balance chemical equations and write balanced chemical equations from word descriptions.

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Calculate moles of solute, volume of solution, or Molarity of the solution from the other two.

Recognize and work dilution problems.

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Calculate the volume of a certain molarity solution required to react with another solution of known molarity. Calculate the mass of a substance that would be required to react with a given volume of a solution of known molarity.

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Predict the products and write balanced equations for reactions of the following reaction types: double replacement, synthesis, decomposition, neutralization, and combustion reactions.

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Predict to some extent whether a substance will be a strong electrolyte, weak electrolyte, or nonelectrolyte. Predict the ions that an electrolyte dissociates into. Identify substances as acids, bases, and salts.

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After constructing molecular reactions for double displacement reactions, be able to identify spectator ions and write the net ionic equations. Using solubility rules, predict if a precipitate forms in a double replacement reaction.

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Be able to assign oxidation numbers to the atoms in a compound. Identify species that are oxidized and reduced in a redox reaction.

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Use the activity series (reduction potentials table) to predict whether a Single Displacement reaction will occur and be able to write the molecular and net ionic equations if it does.

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Resources

Reaction type Summary Table

In-class Reaction WS    (key)

In Class Redox WS 

Solution Stoichiometry  (key)

Solution Limiting Reactant WS   (key)

Solubility Table

PRACTICE FOR CHAPTER 4 QUIZ

Predicting Products WS  (key)

molecular, ionic and net ionic equations for double replacement reactions   (WS)   (key)

Understand what the First Law of Thermodynamics means. Understand what the system, the surroundings, and the universe mean. Be familiar with how the internal energy of a system is affected by exchanges of heat and work between the system and the surroundings.

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Understand the concept of enthalpy. Know what the sign of the enthalpy indicates about the reaction. Be able to calculate the amount of heat released or absorbed by a reaction knowing the quantity of the reactants and the enthalpy of the reaction on a mole basis.

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Define Heat Capacity and Specific Heat (Capacity). Be able to work problems involving Calorimetry.

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State and apply Hess's Law of Constant Heat

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Define and illustrate what Standard Enthalpy of Formation means. Know what the Standard State of an element or compound is. Calculate the enthalpy change of a reaction using a table of standard enthalpies of formation.

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Resources

Specific Heat WS

Enthalpy Calorimetry WS   (key)

Thermochemistry Practice

Describe properties of gases compared to other physical states. Understand the kinetic molecular theory.

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Describe how gases respond to changes in V, n, P, and T. Be able to work problems using combined and ideal gas equations. Define and use common units of gas pressure in calculations.

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Describe how the relative rates of diffusion and effusion of gases depend on their molar masses.

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Understand that real gases deviate from ideal gases, especially at high pressure and/or low temperature. Know the existence of the real gas equation with corrections for particle attraction and size.

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Be able to calculate molar mass from gas density and vice versa.

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Perform calculations involving mixtures of gases. Calculate partial pressure / mole fraction of any gas from the composition of its mixture. Understand the process and calculation of the pressure of a gas collected over water.  

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Identify key scientists and explain how their discoveries contributed to development of the model of the atom. Have a basic knowledge of the development of electron theory (Planck, Einstein, DeBroglie, Bohr, Schrodinger)

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Understand the concept of quantized atom and its relationship to line spectra of atoms. Understand the relationships c = λν and

E = hν.

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Perform calculations releated to electron energy and energy levels using equations developed by Planck, Bohr, and DeBroglie

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Describe the quantum numbers as to how they define electron orbitals and their value limitations. Describe the Uncertainty Principle and its effect on atomic theory. Describe the shapes of the orbital types. Understand the concept of electron spin and what it has to do with electron configuration.

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Write the electron configuration both symbolically and as orbital diagram for any element.

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Be able to write electron configurations, especially valence configurations for any element using the periodic table with the knowledge of the s, p, d, f blocks.

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Describe the variations of atomic radii in the groups and periods on the periodic table and the underlying reasons for the variations.

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Describe the variations in first ionization energies in the groups and periods on the periodic table and the underlying reasons for the variations. Describe and explain the observed changes in successive ionization energies for a given atom.

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Describe the variations of electron affinity in the groups and periods on the periodic table

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Describe what happens to radius when an atom forms an ion. Be able to explain the variation in size of an isoelectronic series. Be able to write the electron configuration of an ion.

Resources

Good summary and practice problems
Periodic Trends WS     (key)

Compare and contrast covalent, ionic, and metallic bonds.

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Understand the energies involved in the formation of ionic bonds—ionization energy, electron affinity, and lattice energy.

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Qualitatively compare lattice energies for ionic compounds

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Predict the formula of an ionic compound between representative elements using the octet rule, and predict an atom's probable valence, using the periodic table. Be able to write the Lewis symbol for any atom.

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Be able to show covalent bond formation using Lewis symbols. Write correct Lewis structures for any simple molecule or ion even when there is an exception to the octet rule.

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Be able to write resonance structures when no one structure is adequate. Use formal charges to determine the most plausible Lewis structure for a molecule.

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Explain electonegativity, how it varies on the periodic table, and its relationship to the nature of the bond between two atoms.

Predict the relative polarities of bonds between any two atoms from their electonegativities or their positions on the periodic table.

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Relate the number of electron domains in the valence shell of an atom to the geometric arrangement of electrons around the atom.

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Predict the molecular shape of a molecule or ion from its Lewis structure. Understand that the relative degree of repulsion between nonbonding pairs is greater than between bonding pairs of electrons.

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Predict, from its molecular shape and the electonegativities of the atoms involved, whether a molecule is polar (has a dipole).

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Explain the types of hybridization. Assign the type of hybridization on the basis of the electron geometry of the valence shell of an atom.

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Describe the bonding between atoms in a molecule as σ or . Explain the concept of delocalization in bonds.