Review Sheet for Chemistry Final Exam

Review Sheet for Chemistry Final Exam Exam is 25% of your final grade

You will be given a periodic table, and an Ionic Bonds additional sheet with reference Formula writing based on balance of information. (See back of this page for an charge Physical properties of ionic compounds example) high melting point, etc. CH 2 Matter and Energy CH 6 Covalent Compounds Significant figures (uses and determining Structural formulas in a calculation) Bonding tendencies of certain elements/families (Ex. Carbon bonds 4 places, Nitrogen bonds 3 and CH 3 Atoms and Moles usually has a lone pair) Historic models of the atom: Dalton, Bohr  Single bonds Subatomic particles and their charge  Double Bonds Rutherford’s nucleus experiment Atomic Number, Mass, and determining  Triples Bonds protons and neutrons in a neutral atom. Drawing Lewis dot structure to account Isotopes and mass number for all valence electrons Quantum mechanical model of electrons Octet rule Atomic Orbitals VSEPR and bond angles of methane, water, Principle energy levels (n=1, n=2, n=3) ammonia, and analogous compounds. Orbitals s, p, d, f Polar covalent bonding (unequal sharing) Number of electrons per quantum Hydrogen bonding in water sublevel and per orbital Physical Properties of covalent Electron configurations: complete, and using a (molecular)compounds “noble gas base” low melting and boiling points, etc. Filling orbitals using Aufbau, Pauli, Molecular and Ionic compound names Hund Anions/Cations Light and atomic spectra, spectral lines Ionic charges based on family or group Parts of a wave Amplitude, crest, trough, wavelength… CH 7 The mole and chemical composition Electromagnetic Radiation The mole UV, visible, IR, Radio etc. Avagadro’s Number Calculating atomic mass from isotopes CH 4 The periodic Table (Weighted average) Group/Family names Molar conversions: Periodic law 1 step: mass   mole Development of PT: Mendeleev particles   mole s-block, p-block, d-block, f-block 2 step: mass mole  particle Relation of electron configuration to Particles  mole  periodicity (periodic trends) Labs: Periodic Trends:  Periodic Properties -Atomic radius o Trends within families -Ionization energy  Flame test of Metals -Electronegativity o Nature of light emitted Metals/Non Metals Transition metals  Identification of Cations and Anions o Determine in an unknown CH 5 Ions and Ionic Compounds solution contains a Valence Electrons particular ion How does the electron configuration change when an atom becomes an ion?