" science and everyday life cannot and should not be separated." - Rosalind Franklin, Biochemist, Co-discoverer of the Structure of DNA

10-3 Academic 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, 5 (not 5.8)

Question:  What exactly is chemistry and what are some tools that chemists use to do thier jobs? 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 Chapters 2, 3 (except 3.10,    

                                                                                               3.11), 5.8, 13.1 - 13.3, 13.5,

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

Properties of Matter, Density (10/2)  

Properties of Matter, Boyle's Law (10/16)

Charles and Gay-Lussac's Law (10/17)

Combined Gas Law (10/23)

Ideal Gas Law 10/29

Types of changes and substances 11/3

Separating Mixtures 11/5

Isotopes and Atomic Mass 11/13, 11/14

The Periodic Table 11/18

  • 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 Chapters 3.10, 3.11, 4

Question:  What is the language of chemistry?

All unit 3 Notes

  • 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 6

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

  • 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 

Unit 5 – Chemical Reactions Chapter 7, 10.1 - 10.3

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 9

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
  • Define limiting reagent and theoretical yield
  • 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
  • Evaluating laboratory technique

 

Unit 7 – Single and Double Displacement Reactions (solution chemistry) Chapter 8

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

                   eachother as a whole?

  • Use the solubility table
  • 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
  • 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 11, 12

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

Unit 9 – Acids and Bases Chapter 16

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

Unit 10 – Nuclear Chemistry Chapter 19

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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