" The most all penetrating spirit before which will open the possibility of tilting not tables, but planets, is the spirit of free human inquiry. Believe only in that." -
Dmitri Mendeleev

10-2 Intensive - Chemistry

Course Outline

please note that this outline may change throughout the year

LAB REPORT OUTLINE               LAB REPORT RUBRIC

Unit 1 – Activities in Science and Measurement Chapter 1-1, 1-2, 2-2, 2-3

Question:  What exactly is chemistry and what are some tools that chemists use to do thier jobs? ALL Unit 1 Notes

  • Distinguish between the different subfields of biological and physical sciences and the different subfields of chemistry
  • The scientific method
  • Laws vs. theories, facts vs. inferences
  • Qualitative vs. qualitative observations
  • Analyzing data using graphs and tables
  • Drawing conclusions about hypotheses and experiments using data and observations
  • Accuracy vs. precision
  • Chemistry lab equiptment
  • Scientific notation
  • Metrics System
  • Conversion factors and dimensional analysis
  • Significant figures

 

Unit 2 – Matter and Its Properties, Periodic Table 1-2 – 1-4, 2-2, 12, 3-1, 3-2, 4-1, 4-2, 4-4

Question: What are the different forms that matter can exist and how are they classified?  All Unit 2 Notes

  • Matter's basic states and properties
  • Density and its units
  • Boyle’s, Charles’, Gay-Lussac’s, and Combined gas laws
  • Physical vs. chemical properties, physical vs. chemical changes
  • Distinguishing elements, compounds, mixtures, homogenous, and heterogeneous mixtures
  • Solubility, solvent, solute, pure substance and mixture
  • Techniques for separating mixtures
  • Dalton’s atomic theory
  • The law of constant composition and the law of conservation of matter
  • Chemical formula, atomic mass, atomic number
  • Finding protons, neutrons, and electrons and their place in the atom
  • Properties of the groups and families on the periodic table
  • Distinguishing a metal, nonmetal, and metalloid
  • Calculate the number of protons, neutrons, and electrons in an atom
  • Isotopes
  • Atomic mass vs. mass number

 

Unit 3 - Compounds, and Nomenclature 5-1 from 162, 5-3

Question:  What is the language of chemistry?

Ions 11/5

Classifying Compounds 11/6

All Naming

  • Determine which atoms become cations and anions
  • Predict the ratios of atoms that may want to combine based on charge
  • Identify the characteristics of the 5 different types of compounds
  • Name binary ionic and binary molecular compounds
  • Name  binary molecular acids and oxyacids
  • Name tertiary compounds

  

Unit 4 – The Mole Chapter 8

Question: How can chemists measure atoms even though they are so tiny?

All unit 4 notes

  • Define an atomic mass unit (amu)
  • Find the formula molecular mass of compounds in amu
  • Use average masses to determine the number of atoms present in a sample
  • Define a mole, Avogadro’s number, and calculate the molar mass of elements
  • Use dimensional analysis to determine the mass, number of moles, and number of atoms present in a sample
  • Analyze the difference between molar and molecular mass
  • Calculate the percent composition
  • Calculate the empirical and molecular formulas

 

Unit 5 – Chemical Reactions Chapter 9 – 1 to 9 – 3

Question: How are chemical reactions used to syntheize the things we see around us every day?

  • Identify reactants, products, and coefficients
  • Use the law of conservation of matter to explain why reactions need to be balanced
  • Identify if a reaction is balanced or not and explain why
  • Use Coefficients to balance reactions
  • Distinguish between the 5 types of reactions
  • Distinguish between exothermic and endothermic reactions
  • Identify mole to mole ratios in balanced equations
  • Identify and perform simple calculations using mole to mole ratios

 

Unit 6 – Stiochiometry  Chapter 10 (content), Chapter 9 pages   321 - 324

Question:  Why is chemistry a lot like cooking?

  • Calculate the number of grams of a product produced in a reaction using a starting amount of 1 to 2 reactants
  • Calculate the number of grams of a reactant needed in a reaction
  • Mathematically identify the limiting reagent of a reaction
  • Mathematically identify the theoretical yield of a reaction
  • Define and calculate the % yield and explain why the % yield is not always 100%
  • Describe the techniques used to obtain the actual yield of an experiment
  • Use the ideal gas law along with Stoichiometry to predict the amount of gas produced in a reaction
  • Evaluating laboratory technique
  • Identify stoichiometric relationships with energy

 

Unit 7 – Single and Double Displacement Reactions (solution chemistry) Chapters 9-4, 10 (application)

Question:  How does everything we have learned so far fit together and relate to

                   eachother as a whole?

  • Use the activity series of metals
  • Predict the products of single replacement reactions
  • Determine the theoretical yield of a single replacement reaction
  • Perform a simple single replacement reaction
  • Determine if the reaction happened using observations and temperature readings
  • Determine the actual yield for a single replacement lab
  • Evaluate experimental technique
  • Use the solubility table
  • Predict the products of a double displacement reaction
  • Describe the experimental technique used to isolate the different products
  • Predict the products of a double displacement reaction
  • Determine the theoretical yield for a  Double displacement lab
  • Successfully perform a double displacement reaction
  • Determine the actual yield for a  Double displacement lab
  • Evaluate experimental technique

 

Unit 8 – Bonding Chapter 3-3, 4-3, 5-1 to 161, 5-2, 6

Question:  Why do molecules and compounds form they way they do?  Why do they

                    not form in some other way?

  • Distinguish between the different theories of atomic structure
  • Define a valance electron
  • Determine the number of valance electrons for an element
  • Recall the differences between the different energies in frequencies of visible light.
  • Explain how and why atoms emit energy
  • Describe the quantum theory of the atom
  • Define the 5 different quantum numbers
  • Sketch the 5 different types of electron orbitals
  • Explain how the principal energy levels fill with electrons
  • Compose an electronic configuration for any given element
  • Label a periodic table with the appropriate quantum numbers
  • Differentiate between valance and core electrons
  • List the quantum numbers for the valance electrons for any given element
  • Determine the electronic configuration of ions
  • Explain why elements adopt an ionic configuration using quantum theory
  • List the quantum numbers for the valance electrons for any given element
  • Compare and contrast the reactivity of different elements in the periodic table using the atomic radius, ionization energy, and electronegativity trends
  • Distinguish between the different periodic trends
  • Use electronegativity to determine the bond type
  • Use an atom’s valance configuration to draw Lewis dot symbols of elements on the periodic table
  • Use an atom’s valance configuration to draw Lewis dot structures of molecular and ionic compounds
  • Use electronegativity to label dipoles in polar covalent molecules
  • Calculate the formal charge of a Lewis structure
  • Determine the molecular geometry using the VSEPR system

Unit 9 – Acids and Bases Chapter 15

Question:  What kind of chemistry can I experience on a daily basis?

  • Define a Bronsted-Lowry acid and base
  • Describe the properties of acids and bases
  • Determine if a substance is an acid or base based on its taste (bitter or sour)
  • Define a Bronsted-Lowry conjugate acid and base
  • Determine the conjugate acid or base
  • Define an acid-base indicator
  • Use the numerical pH scale to identify acids and bases
  • Differentiate between the different acid/base indicators
  • Explain how pH relates to acidity and alkalinity
  • Predict the products of an acid-base reaction
  • Calculate molarity
  • Perform an Acid-base titration

Unit 10 – Nuclear Chemistry Chapter 18

Question:  How can nuclear chemistry be so helpful yet so harmful to humanity at

                    the same time?

  • Define mass number
  • Explain the process of nuclear decay
  • Define radiation
  • Explain where radiation comes from and why it is harmful
  • Differentiate between alpha, beta, and gamma reactions
  • Define half-life
  • Explain how half life is used to determine the age of objects
  • Explain how a substance’s half-life influences the rate of radiation
  • Solve problems using half-life
  • Differentiate between nuclear fusion and fission
  • Perform alpha, beta, gamma, fission, and fusion reactions
  • Summarize the process of obtaining power from nuclear energy
  • Evaluate the use of nuclear energy
  • Summarize the influence of nuclear chemistry on science and our culture.

                                                          

 
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