UNIT 2
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unit_1a_atomic_theory_review_worksheet.docx | |
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chemistry_average_atomic_mass_wksht.pdf | |
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Unit 3
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unit_1b_electronic_structure_review_worksheet.docx | |
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wave_formula_and_plancks_equation.docx | |
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Unit 4
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unit_2_test_review_p1.docx | |
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unit_2_test_review_p2.docx | |
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You need to know:
- Identify the principal types of chemical bonds (ionic & covalent), how they are formed and examples of substances that contain these bonds.
- Write Lewis dot structures of elements molecules and compounds, applying the octet rule
- Describe the formation of positive and negative ions and relate formation to the octet rule and electron configuration.
- Generalize about the strength and physical properties of ionic and covalent bonds: polarity, melting point, boiling point, hardness, conductivity
- Recognize and define monoatomic ions
- Recognize ionic substance begin with metal ions
- Use Roman numerals to indicate the charge of common transition metal ions.
- Know the process of combining cations and anions into neutral ionic formulas
- Name ionic compounds from the ion names or ionic formula
- Recognize nonmetal-nonmetal compounds as molecular (covalent)
- Recognize the seven diatomic elements
- Utilize numerical prefixes in naming and writing formulas of covalent compounds
- Compare and contrast intramolecular and intermolecular forces
- Recognize that only polar molecules can form hydrogen bonds and all molecules have potentail of Van der Waals forces
- All material from previous unit as tests are comprehensive.
You need to know:
- Relate the mole to common counting units such as dozens and pairs.
- Recognize one mole equals 6.02 x10^23 particles (atoms or molecules).
- Understand the mole is the number of particles required to have the same mass in grams as the atom has in amu’s.
- Identify the representative particles of elemental, ionic, and covalent substances.
- Gain an appreciation for the immense size of Avogadro’s number.
- Determine the mass of a mole of substance and see the mole as a convenient amount of a substance.
- Determine the mass of one mole of a compound (molar mass).
- Use dimensional analysis to convert between grams, moles, atoms, and molecules.
- Calculate the percent by mass of individual elements within a compound.
- Determine the empirical formula of a compound given percent by mass of individual elements within a compound.
- Determine the molecular formula of a compound given percent by mass of individual elements within a compound and molar mass.
- All material from previous units as tests are comprehensive
- Differentiate between physical and chemical properties of matter.
- physical: volume, compressibility, density, conductivity, malleability, states of matter, color, texture, etc.
- chemical: reactivity with acids/bases, flammability, reactivity with oxygen, etc.
- Describe the formation of mixtures as physical change.
- Describe simple laboratory techniques that can be used to separate homogeneous and heterogeneous mixtures (e.g. filtration, distillation, chromatography, and evaporation).
- Recognize evidence of a chemical change including:
- formation of a gas
- formation of a precipitate
- production of heat or light
- formation of a new substance
- Describe a chemical reaction in terms of collision theory:
- reacting substances must collide
- reacting substances must be correctly oriented in space
- reacting substances must have sufficient energy to form a new stable arrangement (bond)
- Predict how a change in concentration, temperature, and surface area will affect reaction rate.
- Apply the law of conservation of mass to balance chemical equations.
- Relate coefficients in balanced chemical equations to number of moles and/or particles.
- Classify and distinguish the main types of chemical reactions:
- synthesis, decomposition, single replacement and double replacement
- combustion and acid-base
- All material from previous units as tests are comprehensive
Unit 6 Stoichiometry Test Study Guide
Test Date: Thursday March 2, 2017
Concept: Stoichiometry
SC.912.P.8.9 Apply the mole concept and the law of conservation of mass to calculate quantities of chemicals participating in reactions.
How does a balanced chemical equation show relationships between the reactants and products of a chemical reaction?
Test Date: Thursday March 2, 2017
Concept: Stoichiometry
SC.912.P.8.9 Apply the mole concept and the law of conservation of mass to calculate quantities of chemicals participating in reactions.
How does a balanced chemical equation show relationships between the reactants and products of a chemical reaction?
- Apply the law of conservation of mass to calculate the initial and final masses of reactants and products.
- Identify coefficients as relating to moles of reactants used.
- Determine the ratio of moles of products used or formed.
- Convert the mass of one material into mass of another material using a balanced equation.
- Perform mole to mole conversions
- Perform mass to mass conversions
- Know that reactions stop when the limiting reactant is gone and that some of the excess reactant remains
Unit 6 Thermochemistry Test Study Guide
Test Date: Thursday, March 30th 2017
What are the characteristics of each state of matter?
· Identify the properties of gases, liquids and solids: particle arrangement, compressibility, fluidity
· Define and give an example of plasma.
Note: currently five states of matter are known (Bose-Einstein Condensate).
What is the relationship between temperature and average molecular kinetic energy?
· Know that temperature and average kinetic energy are directly related.
· Convert temperature units from Kelvin to degrees Celsius and vice versa. (K = C +273 will be provided).
How does the average kinetic energy of a substance change during a phase change?
· Recognize changes of state require molecules to gain or lose energy
The addition of energy causes endothermic phase changes: Melting, Vaporization, Sublimation
· The removal of energy causes exothermic phase changes: Freezing, Condensation, Deposition
· Recognize that intermolecular forces determine the phase of a material.
· Use phase diagrams of a substance with regard to changes in temperature, pressure and energy.
How does a phase change reach dynamic equilibrium?
· Explain that equilibrium is established when forward and reverse-reaction rates are equal.
o e.g. Know that the rate of vaporization will equal the rate of condensation in a sealed container.
What are examples in chemistry of how energy can be transformed from one form into another?
· Describe chemical bonds also as stored chemical potential energy.
o Energy is absorbed to break bonds and released when bonds form.
· Recognize that virtually every chemical reaction is accompanied by a change and subsequent transfer in energy.
How do endothermic and exothermic chemical processes compare?
· Recognize that virtually every chemical reaction is accompanied by a transfer in energy.
· Recognize that exothermic reactions release heat and endothermic reactions absorb heat.
· Know that enthalpy is negative for exothermic reactions and positive for endothermic reactions.
· Understand that changes in energy accompany chemical reactions.
Chemical reactions result in the release or absorption of energy.
How can potential energy diagrams help us distinguish between exothermic and endothermic reactions?
· Create and identify the parts of a potential energy diagram of a chemical reaction from provided information, such as the energy of reactants, activation energy, and the absorbing or releasing of heat.
· Justify a chemical process as either endothermic or exothermic from a potential energy diagram.
· Conceptually relate enthalpy to endothermic and exothermic reactions through thermochemical equations and potential energy diagrams.
Test Date: Thursday, March 30th 2017
What are the characteristics of each state of matter?
· Identify the properties of gases, liquids and solids: particle arrangement, compressibility, fluidity
· Define and give an example of plasma.
Note: currently five states of matter are known (Bose-Einstein Condensate).
What is the relationship between temperature and average molecular kinetic energy?
· Know that temperature and average kinetic energy are directly related.
· Convert temperature units from Kelvin to degrees Celsius and vice versa. (K = C +273 will be provided).
How does the average kinetic energy of a substance change during a phase change?
· Recognize changes of state require molecules to gain or lose energy
The addition of energy causes endothermic phase changes: Melting, Vaporization, Sublimation
· The removal of energy causes exothermic phase changes: Freezing, Condensation, Deposition
· Recognize that intermolecular forces determine the phase of a material.
· Use phase diagrams of a substance with regard to changes in temperature, pressure and energy.
How does a phase change reach dynamic equilibrium?
· Explain that equilibrium is established when forward and reverse-reaction rates are equal.
o e.g. Know that the rate of vaporization will equal the rate of condensation in a sealed container.
What are examples in chemistry of how energy can be transformed from one form into another?
· Describe chemical bonds also as stored chemical potential energy.
o Energy is absorbed to break bonds and released when bonds form.
· Recognize that virtually every chemical reaction is accompanied by a change and subsequent transfer in energy.
How do endothermic and exothermic chemical processes compare?
· Recognize that virtually every chemical reaction is accompanied by a transfer in energy.
· Recognize that exothermic reactions release heat and endothermic reactions absorb heat.
· Know that enthalpy is negative for exothermic reactions and positive for endothermic reactions.
· Understand that changes in energy accompany chemical reactions.
Chemical reactions result in the release or absorption of energy.
How can potential energy diagrams help us distinguish between exothermic and endothermic reactions?
· Create and identify the parts of a potential energy diagram of a chemical reaction from provided information, such as the energy of reactants, activation energy, and the absorbing or releasing of heat.
· Justify a chemical process as either endothermic or exothermic from a potential energy diagram.
· Conceptually relate enthalpy to endothermic and exothermic reactions through thermochemical equations and potential energy diagrams.
Unit 8 Gases Study Guide
Test Thursday April 27th, 2017
What is absolute zero?
How does kinetic molecular theory explain the behavior of gases?
How are temperature, pressure, and volume of a gas related?
How does Avogadro’s Law demonstrate the relationship between mole ratios and gas volumes in a balanced chemical equation?
Why are the Ideal Gas Laws “laws?”
Test Thursday April 27th, 2017
What is absolute zero?
- Understand that all movement of particles inside of a substance stopped when absolute zero is reached.
How does kinetic molecular theory explain the behavior of gases?
- Have small particles with large, empty spaces between them.
- Gas particles are in constant, random motion.
- Gas particles have elastic collisions.
- Temperature is a measure of the average kinetic energy of the gas particles.
How are temperature, pressure, and volume of a gas related?
- Predict how gas behavior and pressure will change using the gas laws, including:
- pressure
- volume
- temperature (including at absolute zero)
- number of particles
- Solve Combined Gas Law problems.
How does Avogadro’s Law demonstrate the relationship between mole ratios and gas volumes in a balanced chemical equation?
- Relate molar volume to stoichiometric relationships.
- Solve Ideal Gas Law problems.
Why are the Ideal Gas Laws “laws?”
- Explain that laws describe specific relationships under given conditions, but do not offer explanations.
unit_8_gases_study_guide.docx | |
File Size: | 14 kb |
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