Unit 1 Day 1
All students will feel welcomed to the class. Students will use Think, Pair, Share to discuss prior knowledge regarding Scientific method. Make observations regarding a chemical change
Unit 1 Day 10
Understand that matter can be categorized.
Explain how the 3 states of matter are different
Know that physical properties describe matter and give examples of different physical properties.
Students will know which graph to use for comparing densities of different metals and liquids.
Students can explain what type of property of matter density is physical/chemical, intrinsic/extrinsic.
Students can explain and demonstrate the proper way to measure and calculate in chemistry.
Unit 2 :Atomic Structure and Nuclear Chemistry -November 3:
Day 1 Students will understand John Dalton’s atomic theory and be able to summarize the four main ideas and evaluate them based on current knowledge.
Day 1 Students will be able to describe the size of the atom.
Day 2 Students will understand Thomson’s discovery of electrons and the atomic model based on the discovery, (Plum Pudding model) and replicate the model.
Day 2 Students will understand the defining characteristics of an atom and distinguish between protons, neutrons and electrons by comparing size, mass, charge and location.
Day 2 Students will understand Rutherford’s “gold foil experiment” and explain why the plum pudding model would require updating.
Day 4 Students will construct the atomic models through time and replicate the Rutherford experiment to understand the next progression of the theory development.
Day 3 Students will understand how the atomic number identifies an element and give examples of different elements and their atomic numbers.
Day 4 Students will determine the number of protons, neutrons and electrons in different atoms.
Day 6 Students will explain what makes atoms and isotopes different from each other.
Day 7 Students will calculate the atomic mass of an element and explain what atomic mass means.
Sept 29 Day 8 Students will recognize the nucleus of an unstable isotope and will write an equation to describe alpha decay.
Sept 30 Day 9 Students will recognize that the nucleus of an unstable isotope can decay by Beta radiation and write the equation describing the change.
Day 10 Students will be able to classify gamma radiation as a type of high energy electromagnetic emission with no mass and no charge. Students will be able to show examples of nuclear equations and how gamma radiation is sometimes produced at the same time as alpha and beta radiation.
Day 11 Students will understand a proton to neutron “belt of stability” graph and use it to predict the type of decay that an isotope will undergo.
Day 12 Students will use (and sketch) half-life graphs to determine the half-life of a radioisotope. Students will understand how to use the graphs and the half-life equations to determine how much of a substance will remain following a certain period of time. Students will also use the information to solve real-life problems and determine original amounts of radioactive material.
Students will infer that transmutation reactions are the conversion of one atom to another atom of a different element. Students will recognize that transmutation can happen spontaneously or artificially by bombarding fragments at targeted nuclei.
Students will be able to compare and contrast nuclear fusion and fission reactions and recognize each by the reactants and products of each.
Students will investigate a real-life application of nuclear chemistry and create a presentation that will inform other members of the class about the pros and cons, history and future of this application of radiation.
Unit 2 Oct 10-29th Electrons in Atoms:
Understand how an electron’s position determines the properties and bonding behavior of atoms.
Students will summarize the development of the atomic theory. Identify new idea of the atomic model (Bohr) and use it to explain how electrons exist in specific energy levels within atoms.
Students will describe energies and positions of electrons in atoms.
Apply the aufbau principle, the Pauli exclusion principle, and Hund’s rule in writing the electron configurations of elements.
Explain why the electron configurations for some elements differ from those assignmed using the aufbau principle. (Exceptions to the rule)
Describe electromagnetic radiation in terms of wavelength, frequency and energy of quanta and photons.
Calculate the warvelength, frequencey or energy of light, given any two of these values.
Explain the origin of the atomic emission spectrum of an element.
Unit 3 Week 12 (October 29th) Chemical Periodicity
Day One: Explain how Mendeleev organized the elements in the periodic table. Compare the periodic table proposed by Mendeleev with that described by Moseley.
Describe the three major classes of elements on the periodic table.
Relate an atom’s electron configuration to it’s atomic radius. Describe a relationship between electron configuration and atomic radius.
Use the electron configuration of various elements to classify elements as noble gases, halogens, alkali metals, alkaline earth metals, representative elements, transition metals or inner transition metals.
Construct a graph to show GROUP and Period trends in atomic radii; compare with ionic radii, ionization energy, and electronegativity graphs.
Unit 4 Bonding Week November 13th
Day 1 Describe the properties of ionic compounds.
State two ways an atom can become an ion.
Define the octet rule and predict how elements will seek to follow it.
Describe the differences between anions and cations and be able to describe both.
Given any element, infer it’s oxidation state from it’s lewis dot structure
Write formulas for ionic compounds
Calculate percent composition of ionic compounds.
Name ionic compounds and acids
Predict ionic bonding using electronegativity differences.
We will test a variety of unknowns and identify them (ionically bonded or covalently bonded) based on their physical and chemical properties.
Unit 5 Math of Chemistry (MOLES)
Understand how to measure substances in chemistry (Volume is measured in Liters for gases, atoms are counted using the unit “mole”, and solids and liquids are massed in grams) Convert mass to moles, Convert mass to volume
Determine the percent composition of a given substance.
Determine the empirical formula given a percent composition or given samples of a substance.