Topic II: Atomic Structure (Chapter 6 in Your Text Book)

AP CHEMISTRY MIDTERM REVIEW

Topic I: Based on your summer assignment covered in the chapters 1 – 4 in your text-book. Understand and be able to use scientific notation (standard form), Recall and use SI units and prefixes ,Be able to convert between units , Understand the concept of derived units and use relationships relating to density , Know the meaning of uncertainty and understand and be able to use the rules for determining significant figures and rounding off. Basic information related to three states of matter, their general properties, Separation of matter, Understand and recall definitions for physical and chemical change , Know the difference between elements, mixtures and compounds including the difference between heterogeneous and homogeneous mixtures.

Extension: Brief history of Atomic theory, contributions of scientists, five main aspects of Dalton's Atomic Theory, Identification of sub-atomic particles, Rutherford’s gold foil experiment, Atoms, molecules, Isotopes, relative atomic masses, Ions, Locate approx. position of metals, non-metals and metalloids on the periodic table , List of strong acids, strong bases, polyatomic ions.

Stoic problems:Write chemical equations using chemical formulae and chemical symbols;understand the concept of percentage by mass, Empirical formula, Molecular formula using molar mass. Mole concept: Mass, volume, # of particles, Mass-mass, Volume-volume problems, Limiting reagent, percent yield.

Topic II: Atomic structure (Chapter 6 in your text book):

Electromagnetic spectrum, Wave variables, relation between speed, frequency and wavelength. Atomic spectrum, line, band, emission, absorption spectrums, Neils bohr model, Photoelectric effect, max-Planck quantum theory, De Broglie wave equation, Heisenberg’s uncertainty principle, Dual nature of an electron. Problems based on the Energy, frequency, speed and wavelength of waves including the Rydberg equation, Knowledge of quantum numbers, Atomic orbitals- s, p, d and f and their use in orbital notation, understand the rules for filling orbitals and determining electronic configuration, including the Pauli exclusion principle, Hund's rule of maximum multiplicity and notable exceptions, To write electronic configuration of the elements using the s, p and d and f notation, describe electronic configurations using the electrons in boxes notation, Recall the meanings of the terms paramagnetic, diamagnetic and isoelectronic , hydrated salts.

Topic III: Periodic classification of elements:

History Doberiniers triad, Newland octave, Mendeleev contributions, Mosley, Blocks of elements, Trends atomic size, ionization energy, electro negativity, Electron affinity, notable exceptions with reasons.

Topic IV: Chemical Bonding: Chapters 8 & 9 in text book;

Understand that when forming chemical bonds atoms are attempting to form more stable electronic configurations, types of bonds: Ionic, Covalent, properties of different types of bonds, Understand the concept of covalent bonding and nature of the covalent bond, Draw Lewis structures, Understand the concept of resonance related to Lewis structures, Understand the concept of formal charge related to Lewis structures, Be able to predict the shape and bond angles in molecules and ions using VSEPR theory , Understand that ionic bonding and covalent bonding are at two ends of a sliding scale of bond type, Understand the concept of electro negativity, Understand that polarization caused by small highly charged cations leads to ionic compounds exhibiting some covalent character, Understand that differences in electro negativity in covalent molecules causes dipoles and some ionic character in covalent compounds, Understand when molecules exhibit polarity, Be able to predict the shapes of simple molecules and ions using Lewis structures, atomic orbital theory, sigma and Pi bonds, Hybridization.

Topic V: Gases Measurable variables of gases, Gas laws and calculations based on them: Boyle's law, Charles' law, Gay-Lussac's law, Avogadro's law,the Combined gas law, the Ideal gas law, the van der Waals equation (modified ideal gas law) in calculations, Dalton's law of partial pressures in calculations, Graham law of diffusion, The Kinetic theory, the terms effusion and diffusion

Topic VI: Solids and Liquids Difference between intra, inter particle attractions, factors that change due to these forces, L.D, hydrogen, dipole-dipole, viscosity, surface tension, must be in a position to identify these forces, must be in a position to pick the molecule with maximum change in physical property like boiling point, melting point etc. Types of solids (ionic, networking, molecular, metallic) properties, solid crystal lattice structures, s.c.c, b.c.c, f.c.c problems based on length and volume of edge. Phase changes, phase diagram, triple point. Clausis-claypron equation, vapor pressure.

Topic VII: Solutions: Types of solutions, concentration methods mass %, molarity, molality, mole fraction, Normality, problems using density. Colligative properties, Henrys law, Raoults law, understand the concept of vapor pressure, Ideal solution, quantitative treatments of Boiling Point Elevation, Freezing Point Depression, Osmotic Pressure and the van't Hoff factor

Topic VIII: Chemical kinetics: Understand Collision Theory, understand how temperature, concentration, surface area and catalysts affect a rate of reaction, Interpret an energy profile plot, activation energy, Deduce orders, rate equations and rate constants (including units) from initial rate data, Understand the link between the rate determining (slow step) in a reaction mechanism and the rate equation, Understand AND be able to interpret graphical data relating to rates.

Topic IX: Chemical equilibrium: Understand the concept of dynamic equilibrium, Write an expression in terms of concentrations for the equilibrium constant Kc given a chemical equation, Calculate values for Kc and associated data from initial concentrations, Write an expression in terms of partial pressures for the equilibrium constant Kp given a chemical equation, Calculate values for Kp and associated data from pressure data , Reaction Quotient , Le Chatelier's Principle , predict shift using of Le Chatelier's Principle, Apply the relationship of Kc to Kp, the different formats of Kc (reciprocals and roots) and the relationships in simultaneous equilibria.