Name Chemistry Review

Chemistry Review

Chm.1.1 Matter:Properties and Change 

Chm. 1.1.1	Analyze the structure of atoms, isotopes, and ions.
Chm. 1.1.2	Analyze an atom in terms of the location of electrons.
Chm. 1.1.3	Explain the emission of electromagnetic radiation in spectral form in terms of the Bohr model
Chm. 1.1.4	Explain the process of radioactive decay by the use of nuclear equations and half-life.

Big Ideas

Essential Questions

         Know the location and charge of protons, neutrons, electrons          Determine an element’s number of protons, electrons, and neutrons based off the given isotopic symbols          Differentiate average atomic mass of an element from the actual isotopic mass and mass number of specific isotopes          Analyze electrons in terms of •         Bohr model •         Excited stated vs. ground state •         Emission spectrum (Reference Table) •         electron configurations •         wave/particle duality           Understand the inverse relationship between wavelength and frequency, and the direct relationship between energy and frequency.           Write and balance nuclear equations          Describe nuclear decay          Compare fission and fusion          Understand half-life problems

How can atomic models be used to describe and explain the structure of atoms? In what ways has the theory of the atom changed over time due to technological developments? What is the law of conservation of mass? What is the law of definite proportions/multiple proportions? What were the 5 points to Dalton’s atomic theory? How was the use of cathode rays responsible for the discovery of the electron? How did Rutherford’s experiment lead to the discovery of the atomic nucleus? What are the properties (charge, mass, position) of protons, neutrons, and electrons? What is an isotope? What is the atomic number of an atom equal to? What is the mass number of an atom equal to? Why is the mass number in the periodic table a decimal? How is the wave-particle duality explanation used to explain light and electrons? What is the relationship between the speed, frequency, and wavelength of electromagnetic radiation? What is the significance of the photoelectric effect in describing the behavior of the electron and light? How did the Heisenberg Uncertainty Principle and the Schrödinger Wave equation lead to atomic orbitals? What are the downfalls of the Bohr model of the atom? What are the differences between the Bohr model and the Quantum model of the atom? What is the significance of each of the four quantum numbers? How are the quantum numbers used to describe the position of an electron in an atom? How many electrons fill each energy level and each orbital? What is the significance of the Aufbau principle, the Pauli Exclusion Principle, and Hund’s rule when discussing electron configuration within the atom? Given an element, how do I determine its electron configuration, orbital notation, and electron dot notation? How are nuclear reactions used to describe nuclear decay How do nuclear fission and nuclear fusion reactions differ?

Atom Atomic mass Atomic mass unit Atomic number Electron Ion Isotope Mass number Neutron Nucleus Proton Bohr Model Electron Electron cloud Electron configurations

Emission Spectra Energy level Orbital Sublevel Electromagnetic radiation Emission spectra Energy Energy level Frequency Nucleus Orbital Photon Quanta Sublevel Wavelength Fission Fusion Half life Nuclear Decay Radioactive decay

Student Performance Goals
Learning Targets	Criteria for Success
I will…	I can…
Be able to look at the periodic table and determine the number of protons, electrons and neutrons and elements has Determine number of protons, electrons, and neutrons when given an isotopic symbol Tell the difference between average atomic mass and mass number Draw an elements Bohr Model Be able to determine electron configurations for elements Manipulate and solve C =  Use and understand the electromagnetic spectrum Be able to write and balance nuclear equations use alpha and beta particles Explain nuclear fission and fusion Successfully work through half-life problems	Correctly calculate the number of protons, neutrons and electrons for all elements Describe the difference between average atomic mass and mass number Correctly draw Bohr Models for all elements making sure to include the nucleus and energy levels in which to place the electrons Write the correct electron configurations for all elements making sure to include the s, p, d, f in the appropriate order Use the numbers given to me in word problems to solve the wavelength formula and then use the numbers locate the appropriate area on the electromagnetic spectrum Correctly write and balance nuclear equations using the knowledge that undergoing alpha decay produces an alpha particle and undergoing beta decay produces a beta particle. Correctly describe nuclear fission is the splitting of one nucleus into two or more smaller nuclei and nuclear fusion is the joining of two or more nuclei into one nucleus Use given information to solve radioactive half-life problems

Chm. 1.2 Understand the bonding that occurs in simple compounds in terms of bond type, strength, and properties

Chm. 1.2.1	Compare (qualitatively) the relative strengths of ionic, covalent, and metallic bonds
Chm. 1.2.2	Infer the type of bond and chemical formula formed between atoms
Chm. 1.2.3	Compare inter- and intra- particle forces
Chm. 1.2.4	Interpret the name and formula of compounds using IUPAC convention
Chm. 1.2.5	Compare the properties of ionic, covalent, metallic, and network compounds

Big Ideas

Essential Questions

         Predict bond type based off location of elements on the periodic table          Determine positive and negative charge of element based off location of element on periodic table          Predict chemical formulas          Write and name binary chemical formulas/compounds          Write and name compounds using Polyatomic Ions          Know names and formulas for common acids          Describe intermolecular forces for molecular compounds          Explain the strengths and characteristics of intermolecular forces, ionic, covalent, and metallic bonds          Explain the strengths of hydrogen bonds, dipole-dipole forces, and London Dispersion forces          Apply and explain VSEPR with respect to molecular geometry          Compare/Contrast polarity vs. nonpolarity          Describe macromolecules and network solids

How does the distribution of electrons in atoms affect the formation of a compound? What factors determine the types of chemical bonds that form between particles? How do elements form ionic bonds? How do elements form covalent bonds? Are all electrons shared equally? How are the properties of metals explained through metallic bonding? How are the names of compounds determined (inorganic and acids)? How are the formulas for compounds written? How can I translate between a compound's name and its formula? How can the charges of ions be used to determine balanced formulas involving polyatomic ions? How can we predict the shape, structure and properties of molecules? What is the difference between ionic, covalent, and metallic bonding? How do intramolecular and intermolecular forces affect properties of a compound?

Anion Cation Covalent Bond Electron Dot Structure/Diagram (Lewis Dot Structure/Diagram) Ionic Bond Metallic Bond Valence Electron

Chemical Formula Ionic Bond Lewis Structure Periodic Table Covalent Bond Diatomic Molecule Dipole-Dipole Forces Hydrogen Bond Intermolecular Forces Intramolecular Forces Ionic Bond London Dispersion Forces Metallic Bond Polar Bond

Binary Compound Metal Molecule Nomenclature Nonmetal Polyatomic Ion Covalent Bond Ionic Bond Ionic Compound London Dispersion Forces Metallic Bond Molecular Compound van der Waals Forces VSEPR

Chm. 2.1  Understand the relationship among pressure, temperature, volume, and phase

Big Ideas

Essential Questions

         All chemical and physical changes involve energy transfer          The amount of heat transferred in a chemical/physical change can be predicted (calculated) using a balanced chemical equation. It can also be measured quantitatively through experimental means and graphically represented          Explain why gases are less soluble in warm water than cold water          Investigate the difference in the boiling or freezing point of pure water and a salt solution          Measure, plot, and interpret the graph of a phase diagram of a substance under various conditions          Examine and interpret heating and cooling curves for various closed systems.          Contrast heat and temperature, including temperature as a measure of average kinetic energy          Know that energy is neither created nor destroyed          Explain physical equilibrium          Explain and understand the relationship between pressure, temperature, volume, and amount of gas          Complete calculations of:

How is energy transferred in chemical systems? How does the potential energy and kinetic energy of molecules change during thermodynamic processes? How do heat, temperature and internal energy differ? Why is absolute zero so named? Why can all reactions be classfiied as exothermic and endothermic? How much energy is required to change a substance? How is energy converted between kinetic energy and potential energy in a chemical reaction? How does the motion of particles affect the temperature and phase of a substance? How does pressure affect particle motion and phase change? What is the relationship between molecular motion and thermal energy? What is the nature of energy transfer? How do you calculate heat capacity?          How do gases behave?          How do changes in pressure, volume, and temperature affect a gas? What impact does the world of gases have on your life? What are the key parameters that define a gas? How are pressure and volume related to each other? How are volume and temperature related to each other? How are temperature and pressure related to each other? How does Kinetic Molecular Theory describe the behavior of gases? What is pressure? How does a gas exert pressure? How do we measure pressure?